This document discusses the properties and states of matter. It defines matter as anything that has mass and takes up space, and explains that matter is made up of atoms. It then describes the three main states of matter - solids, liquids, and gases - and how their properties differ based on factors like the arrangement and movement of particles. The document also briefly introduces plasma and Bose-Einstein condensates as more advanced states of matter. It concludes by contrasting physical and chemical properties and changes in matter.
The document discusses the three states of matter: solids, liquids, and gases. It provides examples of each state and describes their key properties - solids maintain their shape, liquids take the shape of their container, and gases spread out to fill their space. The document includes a short quiz to test the reader's understanding of states of matter.
States of Matter for highschool, solid, liquid, gas, freezing point, melting point, characteristic properties, physical properties, chemical properties.
The document discusses physical and chemical changes. Physical changes alter the state of a substance but do not create a new substance, such as melting, freezing, or breaking something into smaller pieces. Chemical changes form an entirely new substance, evidenced by a change in color, gas release, or new solid forming. Examples of physical changes include shattering a plate or melting wax, while examples of chemical changes include burning wood or rusting metal.
The document discusses several physical properties of matter including thermal conductivity, state, malleability, ductility, solubility, density, and how density relates to whether an object will float or sink in water. It provides definitions and examples for each property. Density is defined as mass per unit volume and most substances have a unique density value expressed in grams per milliliter or grams per cubic centimeter.
The document discusses the composition of matter. It states that matter is anything that occupies space and has mass, and is composed of molecules which are made up of even smaller units called atoms.
This document discusses the physical and chemical properties of substances. Physical properties can be observed without changing the substance's identity and include properties like state, colour, odour, and hardness. Chemical properties describe a substance's ability to change into new substances through chemical reactions like combustibility, solubility, and reaction with acids. Both qualitative properties observable by the senses and quantitative properties measured with numbers are discussed.
The document defines key vocabulary terms related to matter including matter, mass, volume, and the Law of Conservation of Matter. It provides definitions and examples of solid, liquid, and gas matter. Mass is defined as how much matter makes up an item, while volume refers to how much space an item takes up. The Law of Conservation of Matter states that matter can change forms but cannot be created or destroyed.
Chemical properties describe how a substance reacts or changes during a chemical reaction. Some key chemical properties include flammability, reactivity, and the ability to undergo chemical changes that alter the composition of the substance. Common signs that a chemical change has occurred include a change in color, production of a gas, or formation of a precipitate. However, physical changes can sometimes exhibit similar signs, so the only definitive way to identify a chemical change is if the composition of the substance changes to form new substances.
The document discusses the three states of matter: solids, liquids, and gases. It provides examples of each state and describes their key properties - solids maintain their shape, liquids take the shape of their container, and gases spread out to fill their space. The document includes a short quiz to test the reader's understanding of states of matter.
States of Matter for highschool, solid, liquid, gas, freezing point, melting point, characteristic properties, physical properties, chemical properties.
The document discusses physical and chemical changes. Physical changes alter the state of a substance but do not create a new substance, such as melting, freezing, or breaking something into smaller pieces. Chemical changes form an entirely new substance, evidenced by a change in color, gas release, or new solid forming. Examples of physical changes include shattering a plate or melting wax, while examples of chemical changes include burning wood or rusting metal.
The document discusses several physical properties of matter including thermal conductivity, state, malleability, ductility, solubility, density, and how density relates to whether an object will float or sink in water. It provides definitions and examples for each property. Density is defined as mass per unit volume and most substances have a unique density value expressed in grams per milliliter or grams per cubic centimeter.
The document discusses the composition of matter. It states that matter is anything that occupies space and has mass, and is composed of molecules which are made up of even smaller units called atoms.
This document discusses the physical and chemical properties of substances. Physical properties can be observed without changing the substance's identity and include properties like state, colour, odour, and hardness. Chemical properties describe a substance's ability to change into new substances through chemical reactions like combustibility, solubility, and reaction with acids. Both qualitative properties observable by the senses and quantitative properties measured with numbers are discussed.
The document defines key vocabulary terms related to matter including matter, mass, volume, and the Law of Conservation of Matter. It provides definitions and examples of solid, liquid, and gas matter. Mass is defined as how much matter makes up an item, while volume refers to how much space an item takes up. The Law of Conservation of Matter states that matter can change forms but cannot be created or destroyed.
Chemical properties describe how a substance reacts or changes during a chemical reaction. Some key chemical properties include flammability, reactivity, and the ability to undergo chemical changes that alter the composition of the substance. Common signs that a chemical change has occurred include a change in color, production of a gas, or formation of a precipitate. However, physical changes can sometimes exhibit similar signs, so the only definitive way to identify a chemical change is if the composition of the substance changes to form new substances.
An element is a pure substance that cannot be separated into simpler substances. Elements have unique characteristic properties like melting point and reactivity that can be used to identify them. Elements are grouped into metals, nonmetals, and metalloids based on shared properties. Compounds are formed when two or more elements chemically combine to form a new substance with different properties. Mixtures are combinations of substances that do not chemically combine and can be separated physically.
This document discusses the fundamental concepts of matter including atoms, elements, compounds, and mixtures. It defines chemistry as the study of matter and its properties. Properties can be physical, describing observable characteristics without changes in composition, or chemical, involving changes in what substances are present. Physical properties include things like color, texture, and boiling point while chemical properties relate to reactivity and changes in substances. The document also discusses the classification of matter as pure substances or mixtures and the differences between homogeneous and heterogeneous mixtures.
Matter can exist in three states - solid, liquid, and gas. The state depends on how closely packed the molecules are and how freely they can move. In solids, molecules are tightly packed and can only vibrate. In liquids, molecules have some space between them and move more freely. Gas molecules are most spaced out and move freely in any direction. Increases in temperature cause molecules to move faster and spread out more, potentially changing the state from solid to liquid to gas. Decreases in temperature have the opposite effect, causing molecules to slow down, pack closer together, and potentially change the state from gas to liquid to solid.
The document discusses the three phases of matter - solid, liquid, and gas. It defines evaporation and condensation, explaining that evaporation occurs when molecules break away from the surface of a liquid and enter the gas phase, while condensation is the reverse process where gas molecules become liquid. It also describes the differences between boiling and evaporation, and explains that phase changes involve absorption or release of heat energy as molecules change their arrangement and movement between solid, liquid, and gas states. Common phase changes like melting, freezing, vaporization, and condensation are defined.
The document discusses the definition and classification of matter. It defines matter as anything that has mass and takes up space, and discusses its physical and chemical properties. Matter can exist in different states such as solid, liquid, gas, and plasma. It also discusses the differences between physical and chemical changes, and how matter can be classified based on its composition, such as elements, compounds, mixtures, alloys and colloids.
Grade 8 Integrated Science Chapter 9 Lesson 1 on understanding chemical reactions. An introduction to reactants, products, and reading chemical equations.
The document discusses the benefits of exercise for mental health. Regular physical activity can help reduce anxiety and depression and improve mood and cognitive functioning. Exercise causes chemical changes in the brain that may help boost feelings of calmness, happiness and focus.
This document discusses the three main states of matter - solids, liquids, and gases. It provides definitions and comparisons of their properties, including that gases are well-separated particles that move freely, liquids have particles close together that can slide past one another, and solids have tightly packed, ordered particles that vibrate in place. The document also examines physical changes between states of matter caused by temperature and pressure changes.
Physical changes alter the state or form of a substance without changing its chemical identity, and are reversible. Chemical changes transform one or more substances into new substances with different properties, are indicated by color changes, formation of precipitates or gas bubbles, production of heat or light, and are not easily reversible. Physical and chemical changes can be distinguished by whether the identity of the substance is conserved and if the change is reversible.
This document discusses the properties of solids, liquids, and gases. It defines a material as anything made up of tiny particles and explains that a material's properties tell us something about what it is like. Solids have tightly packed particles that hold their shape, while liquids have less tightly packed particles that flow and take the shape of their container. Gases have particles with lots of room to move that spread out and fill all available space. An example given is water, which can be a solid (ice), liquid (water), or gas (steam) depending on temperature.
The document discusses various physical and chemical properties of matter. It defines physical properties as those that can be determined without changing the composition of a substance, such as texture, color, and boiling point. Chemical properties describe how a substance can change to form another substance through a chemical reaction. The document also defines physical and chemical changes, and discusses the phases of matter, forms of matter such as elements and compounds, properties of metals and acids/bases, and types of mixtures like solutions, suspensions and colloids.
During a change of state, the motion and arrangement of a substance's particles change as it gains or loses energy from its surroundings. The three main states of matter - solid, liquid, and gas - can change between each other. Freezing and melting occur between solids and liquids as particles slow down or speed up. Evaporation, boiling, condensation change between liquids and gases as particles escape or are attracted together. Sublimation and deposition change directly between solids and gases. Mass and identity are conserved during state changes.
This document discusses various physical separation techniques for mixtures. It describes 12 different methods: hand picking, winnowing, threshing, magnetic attraction, sifting/sieving, filtration, sedimentation, decantation, sublimation, evaporation, distillation, and boiling. Common examples are provided for each technique to separate mixtures like grains from husks, solids from liquids, or soluble and insoluble components.
This document discusses the three states of matter - solids, liquids, and gases. It explains that in solids, particles are tightly packed and vibrating in a fixed position. In liquids, particles are tightly packed but can slide over one another. In gases, particles are very far apart and move freely. The document also discusses physical changes like melting, freezing, boiling, evaporating, and condensing. During these phase changes, heat is either absorbed or released by the matter. Finally, it explains that chemical changes occur when new substances are formed through rearrangement of atoms.
A chemical change is a change where one or more new types of matter form as the original materials react and combine in new ways. Some signs that a chemical change has occurred include a change in color, gases being given off, or a change in temperature without external heating or cooling. Common examples of chemical changes provided are burning, rusting, wood ash being left after burning, and fruits or metals oxidizing and changing color when exposed to air.
Matter is anything that has mass and occupies space. It exists in three main states: solid, liquid, and gas. The state depends on how tightly or loosely the particles are packed. Solids have a fixed shape and volume as particles are tightly packed and vibrate in place. Liquids take the shape of their container but maintain a fixed volume as particles can move past one another. Gases have no definite shape or volume as particles are very far apart and move freely. Water can change states by adding or removing heat, going from solid ice to liquid to gas vapor.
5th grade chapter 14 section 2 - what is sound energyhinsz
Sound is a wave of vibrations that spreads from its source. The vibration is a back-and-forth motion, and sound waves have areas where particles are close together called crests. The number of crests that pass per second is the frequency, with a higher frequency creating a higher pitch. Louder sounds come from sources that vibrate more and have more energy, while loudness can be measured in decibels. Your vocal cords vibrate when talking, caused by air rushing past them, making air particles around them vibrate and travel as sound waves. Sound can travel through solids, liquids and gases but not vacuums, and its speed depends on the material. For sound to be heard, an object
This document discusses the different states of matter - solids, liquids, gases, and plasma. It explains that in solids, particles are close together and vibrate in place. In liquids, particles can slide past each other but the substance takes the shape of its container. Gases have particles that are far apart and expand to fill their container. Changes between these states require the addition or removal of energy. The document provides examples like melting, freezing, evaporation, and condensation to illustrate changes between solid, liquid, and gas states.
This document discusses methods for separating mixtures into their pure components. It describes techniques like filtration, crystallization, distillation, and paper chromatography. Filtration can separate insoluble solids from liquids. Crystallization involves evaporating a solution to leave behind crystals of the solute. Distillation separates liquids based on their boiling points. Paper chromatography uses a solvent to separate mixtures on a paper strip based on how far different substances travel up the paper. The document emphasizes that pure substances have fixed melting and boiling points, while mixtures can be separated into pure components using these techniques.
The document discusses magnetism and electricity concepts including:
- Iron, nickel, and cobalt have the greatest magnetic permeability.
- Permanent magnet examples include ceramic bars, fridge magnets, and neodymium discs.
- Temporary magnets include induced paper clips and electromagnets.
- Earth's magnetic field is generated by a dynamo effect in its solid iron inner core.
- Moving a magnet near a wire or changing the magnetic field around a wire induces electric current in the wire.
An element is a pure substance that cannot be separated into simpler substances. Elements have unique characteristic properties like melting point and reactivity that can be used to identify them. Elements are grouped into metals, nonmetals, and metalloids based on shared properties. Compounds are formed when two or more elements chemically combine to form a new substance with different properties. Mixtures are combinations of substances that do not chemically combine and can be separated physically.
This document discusses the fundamental concepts of matter including atoms, elements, compounds, and mixtures. It defines chemistry as the study of matter and its properties. Properties can be physical, describing observable characteristics without changes in composition, or chemical, involving changes in what substances are present. Physical properties include things like color, texture, and boiling point while chemical properties relate to reactivity and changes in substances. The document also discusses the classification of matter as pure substances or mixtures and the differences between homogeneous and heterogeneous mixtures.
Matter can exist in three states - solid, liquid, and gas. The state depends on how closely packed the molecules are and how freely they can move. In solids, molecules are tightly packed and can only vibrate. In liquids, molecules have some space between them and move more freely. Gas molecules are most spaced out and move freely in any direction. Increases in temperature cause molecules to move faster and spread out more, potentially changing the state from solid to liquid to gas. Decreases in temperature have the opposite effect, causing molecules to slow down, pack closer together, and potentially change the state from gas to liquid to solid.
The document discusses the three phases of matter - solid, liquid, and gas. It defines evaporation and condensation, explaining that evaporation occurs when molecules break away from the surface of a liquid and enter the gas phase, while condensation is the reverse process where gas molecules become liquid. It also describes the differences between boiling and evaporation, and explains that phase changes involve absorption or release of heat energy as molecules change their arrangement and movement between solid, liquid, and gas states. Common phase changes like melting, freezing, vaporization, and condensation are defined.
The document discusses the definition and classification of matter. It defines matter as anything that has mass and takes up space, and discusses its physical and chemical properties. Matter can exist in different states such as solid, liquid, gas, and plasma. It also discusses the differences between physical and chemical changes, and how matter can be classified based on its composition, such as elements, compounds, mixtures, alloys and colloids.
Grade 8 Integrated Science Chapter 9 Lesson 1 on understanding chemical reactions. An introduction to reactants, products, and reading chemical equations.
The document discusses the benefits of exercise for mental health. Regular physical activity can help reduce anxiety and depression and improve mood and cognitive functioning. Exercise causes chemical changes in the brain that may help boost feelings of calmness, happiness and focus.
This document discusses the three main states of matter - solids, liquids, and gases. It provides definitions and comparisons of their properties, including that gases are well-separated particles that move freely, liquids have particles close together that can slide past one another, and solids have tightly packed, ordered particles that vibrate in place. The document also examines physical changes between states of matter caused by temperature and pressure changes.
Physical changes alter the state or form of a substance without changing its chemical identity, and are reversible. Chemical changes transform one or more substances into new substances with different properties, are indicated by color changes, formation of precipitates or gas bubbles, production of heat or light, and are not easily reversible. Physical and chemical changes can be distinguished by whether the identity of the substance is conserved and if the change is reversible.
This document discusses the properties of solids, liquids, and gases. It defines a material as anything made up of tiny particles and explains that a material's properties tell us something about what it is like. Solids have tightly packed particles that hold their shape, while liquids have less tightly packed particles that flow and take the shape of their container. Gases have particles with lots of room to move that spread out and fill all available space. An example given is water, which can be a solid (ice), liquid (water), or gas (steam) depending on temperature.
The document discusses various physical and chemical properties of matter. It defines physical properties as those that can be determined without changing the composition of a substance, such as texture, color, and boiling point. Chemical properties describe how a substance can change to form another substance through a chemical reaction. The document also defines physical and chemical changes, and discusses the phases of matter, forms of matter such as elements and compounds, properties of metals and acids/bases, and types of mixtures like solutions, suspensions and colloids.
During a change of state, the motion and arrangement of a substance's particles change as it gains or loses energy from its surroundings. The three main states of matter - solid, liquid, and gas - can change between each other. Freezing and melting occur between solids and liquids as particles slow down or speed up. Evaporation, boiling, condensation change between liquids and gases as particles escape or are attracted together. Sublimation and deposition change directly between solids and gases. Mass and identity are conserved during state changes.
This document discusses various physical separation techniques for mixtures. It describes 12 different methods: hand picking, winnowing, threshing, magnetic attraction, sifting/sieving, filtration, sedimentation, decantation, sublimation, evaporation, distillation, and boiling. Common examples are provided for each technique to separate mixtures like grains from husks, solids from liquids, or soluble and insoluble components.
This document discusses the three states of matter - solids, liquids, and gases. It explains that in solids, particles are tightly packed and vibrating in a fixed position. In liquids, particles are tightly packed but can slide over one another. In gases, particles are very far apart and move freely. The document also discusses physical changes like melting, freezing, boiling, evaporating, and condensing. During these phase changes, heat is either absorbed or released by the matter. Finally, it explains that chemical changes occur when new substances are formed through rearrangement of atoms.
A chemical change is a change where one or more new types of matter form as the original materials react and combine in new ways. Some signs that a chemical change has occurred include a change in color, gases being given off, or a change in temperature without external heating or cooling. Common examples of chemical changes provided are burning, rusting, wood ash being left after burning, and fruits or metals oxidizing and changing color when exposed to air.
Matter is anything that has mass and occupies space. It exists in three main states: solid, liquid, and gas. The state depends on how tightly or loosely the particles are packed. Solids have a fixed shape and volume as particles are tightly packed and vibrate in place. Liquids take the shape of their container but maintain a fixed volume as particles can move past one another. Gases have no definite shape or volume as particles are very far apart and move freely. Water can change states by adding or removing heat, going from solid ice to liquid to gas vapor.
5th grade chapter 14 section 2 - what is sound energyhinsz
Sound is a wave of vibrations that spreads from its source. The vibration is a back-and-forth motion, and sound waves have areas where particles are close together called crests. The number of crests that pass per second is the frequency, with a higher frequency creating a higher pitch. Louder sounds come from sources that vibrate more and have more energy, while loudness can be measured in decibels. Your vocal cords vibrate when talking, caused by air rushing past them, making air particles around them vibrate and travel as sound waves. Sound can travel through solids, liquids and gases but not vacuums, and its speed depends on the material. For sound to be heard, an object
This document discusses the different states of matter - solids, liquids, gases, and plasma. It explains that in solids, particles are close together and vibrate in place. In liquids, particles can slide past each other but the substance takes the shape of its container. Gases have particles that are far apart and expand to fill their container. Changes between these states require the addition or removal of energy. The document provides examples like melting, freezing, evaporation, and condensation to illustrate changes between solid, liquid, and gas states.
This document discusses methods for separating mixtures into their pure components. It describes techniques like filtration, crystallization, distillation, and paper chromatography. Filtration can separate insoluble solids from liquids. Crystallization involves evaporating a solution to leave behind crystals of the solute. Distillation separates liquids based on their boiling points. Paper chromatography uses a solvent to separate mixtures on a paper strip based on how far different substances travel up the paper. The document emphasizes that pure substances have fixed melting and boiling points, while mixtures can be separated into pure components using these techniques.
The document discusses magnetism and electricity concepts including:
- Iron, nickel, and cobalt have the greatest magnetic permeability.
- Permanent magnet examples include ceramic bars, fridge magnets, and neodymium discs.
- Temporary magnets include induced paper clips and electromagnets.
- Earth's magnetic field is generated by a dynamo effect in its solid iron inner core.
- Moving a magnet near a wire or changing the magnetic field around a wire induces electric current in the wire.
This document provides an overview of physical science concepts related to matter. It defines matter as anything that has mass and takes up space. All matter is made up of atoms, which are the smallest units comprising over 100 different elements. The document discusses the structure of atoms including protons, neutrons, and electrons. It also defines key terms like elements, compounds, mixtures, solutions, and homogeneous and heterogeneous mixtures. Students are provided guidance on setting up their lab notebooks and navigating the class wiki page to access course resources and assignments.
The document outlines the key steps of the scientific method including observation, hypothesis, experiment, and conclusion. It emphasizes the importance of recording specific procedures so experiments can be performed by others. The conclusion should state whether the data supports or contradicts the original hypothesis. Errors should be noted to improve future experiments, and plans for further investigation should be proposed.
The document outlines the key steps of the scientific method: observation, hypothesis, experiment, and conclusion. It discusses performing experiments, including developing procedures, collecting data, and analyzing results to determine if the hypothesis is supported or needs revision. Potential sources of bias are addressed, as well as the importance of collaboration and replication in scientific research. Safety protocols for the laboratory are also covered.
This document provides an overview of current electricity, including:
- Current electricity involves a continuous flow of charged particles through a conductor, measured in amperes.
- Electric circuits form a closed loop through which current can flow. A difference in electric potential provides the incentive for current to flow.
- Voltage is a measure of the difference in electric potential and provides the force for current to flow. Batteries use chemical reactions to produce electricity between two electrodes.
- Resistance opposes the flow of current and is affected by the material, length, and diameter of a conductor. Ohm's law describes the relationship between voltage, current, and resistance in a circuit.
This document discusses magnetism and magnetic fields. It begins by defining a magnet and different types of magnets. It then explains magnetic materials, domains, and magnetic field lines. The document discusses how cutting a magnet in half would affect its poles. It also covers permanent and temporary magnets, as well as how magnetism can be induced using electricity or electromagnets. The final section provides a sample lab experiment to test magnetic fields and determine which magnet has the strongest field.
This document provides an overview of the periodic table of elements and key information about each group. It discusses the physical and chemical properties of elements in groups 1-18, including alkali metals, alkaline earth metals, transition metals, and noble gases. Diagrams showing atomic structure (Bohr models and Lewis dot structures) are provided for many elements, along with examples of common compounds and reactions. The periodic trends of atomic radius, ionization energy, and reactivity across periods and down groups are also covered.
This document provides an overview of several key concepts in chemistry including:
- The structure of atoms and how they interact through ionic bonds by transferring electrons or covalent bonds by sharing electrons.
- How the periodic table organizes elements based on their atomic structure and valence electrons.
- The formation of ions when atoms gain or lose electrons to achieve full energy levels. Ionic bonds are formed when oppositely charged ions attract.
- Covalent bonds form when atoms share valence electrons to achieve full energy levels.
- Polar molecules that have unequal sharing of electrons can form hydrogen bonds through weak electrostatic attractions between partially positive and negative regions.
This document provides an overview of basic chemistry concepts including:
- Subatomic particles involved in chemical reactions are valence electrons.
- Covalent bonds involve the sharing of electrons between two or more atoms.
- The periodic table can be used to understand patterns in elements like Bohr diagrams and Lewis dot structures.
- Stable atoms have paired electrons and full energy levels.
- Examples of physical properties of substances like water and how polarity arises in some covalent molecules are discussed.
The document discusses various topics relating to chemistry including chemical reactions, the periodic table, chemical bonding, and reaction rates. It provides definitions and explanations of key terms and concepts. Examples are given to illustrate different types of chemical reactions like synthesis, decomposition, combustion, and displacement reactions. Factors that affect reaction rates like concentration, temperature, surface area, and catalysts are also summarized.
Work is defined as the transfer of energy when a force causes an object to move. Power is the rate at which work is done and is calculated by dividing the work by the time taken. Machines make work easier by changing the direction or magnitude of the applied force, allowing tasks to be completed with less exertion. They do not reduce the total amount of work done.
1. The document discusses concepts related to motion including speed, velocity, acceleration, momentum, and conservation of momentum. It provides definitions and formulas for calculating these values.
2. Examples are given to demonstrate how to calculate speed, relative velocity between two objects, acceleration, and momentum. Factors like mass, velocity, and time are considered.
3. The conservation of momentum is explained as the principle that the total momentum of a system remains constant if no external forces act on it. Collisions are used to illustrate how momentum can be transferred between objects.
Newton's second law states that an object's acceleration depends on the net force acting on it and its mass. Force equals mass times acceleration. Newton's third law states that for every action there is an equal and opposite reaction. Gravity is a force between any two masses that depends on their masses and the distance between them, as described by the law of universal gravitation. In free fall, the only force acting is gravity, so all objects accelerate at the same rate due to gravity.
1) Fluids are substances that can flow and take the shape of their container. Pressure is defined as force per unit area and increases with depth in fluids.
2) Pascal's principle states that pressure increases are transmitted equally throughout a fluid in a closed container. Hydraulic systems use this principle to magnify force.
3) Pressure increases linearly with depth in fluids due to the weight of the fluid above pressing down. Atmospheric and water pressure are greatest at sea level and the deepest point underwater, respectively.
Electrical energy is the movement of charged particles called ions. There are two types of ions: cations with positive charges that have missing electrons, and anions with negative charges that have extra electrons. Ions exert forces on one another, with opposite charges attracting and like charges repelling. The electrical force is directly proportional to the magnitude of the charges and inversely proportional to the distance between objects. Static electricity occurs when electrons are transferred between materials that touch, resulting in an accumulation of charges and forces on nearby objects. Electrical conduction allows the movement of electrons along conductors like metals, while insulators tightly hold electrons in place.
This document discusses measuring systems and converting between units. It covers:
- The English and metric systems, including their base units and scales.
- The metric system is decimal-based while English uses various units.
- Methods for converting between units like meters to centimeters using prefixes and multiplication.
- Examples are provided for converting distances, volumes, and temperatures between English and metric units.
Newton's First Law states that an object at rest stays at rest and an object in motion stays in motion with the same speed and in the same direction unless acted upon by an unbalanced force. Inertia is an object's resistance to changes in motion and is determined by its mass. Friction is a force that opposes the motion between two surfaces in contact and depends on factors such as the roughness of the surfaces and whether the object is moving or stationary. The net force on an object, which is the combination of all individual forces, determines whether its motion will change.
Energy is the ability to do work or cause change and exists in various forms including thermal, chemical, electrical, radiant, and nuclear. It can be converted from one form to another but cannot be created or destroyed based on the law of conservation of energy. Kinetic energy is the energy of movement and depends on an object's mass and velocity, while potential energy is stored energy due to position or state and depends on mass, force, and height or configuration. Renewable energy sources like solar, wind, and hydro can be replenished, while nonrenewable fossil fuels like coal, petroleum, and natural gas are limited and will run out over time.
The document provides information about our solar system and the universe. It describes the major components of the solar system including the sun, planets, moons, comets, asteroids and dwarf planets. It then discusses the history of astronomy from ancient civilizations studying the night sky to modern space exploration. It also explains how gravity and orbits allow the solar system to function and how scientists like Newton contributed to our understanding of motion and orbits. Finally, it summarizes the leading scientific theory of the origins of the universe via the Big Bang over 14 billion years ago.
Matter and energy are the fundamental building blocks of chemistry. The periodic table organizes elements based on atomic structure and properties to help understand relationships between different types of matter. Physical changes alter a substance's state without changing its chemical makeup, while chemical changes form new substances through atomic rearrangements. Scientific models are used to represent unobservable phenomena and further our understanding of how matter behaves.
This chapter introduces key concepts in chemistry including distinguishing science from technology, defining important terms like hypothesis and theory, and classifying types of matter. It outlines learning objectives related to the states and properties of matter, physical and chemical changes, and using units and calculations. Students will learn to differentiate elements, compounds, mixtures and various research types as well as manipulate matter concepts like density, heat, temperature and phases. Critical thinking skills will also be developed.
The document discusses the four states of matter and physical and chemical changes that matter undergoes. It provides details on the kinetic molecular theory explanation for differences between solids, liquids, and gases. Physical changes alter a substance's state or form without changing its chemical makeup, while chemical changes create new substances. The document also discusses plasma as the fourth state of matter and its many applications in manufacturing, medicine, and waste processing.
Ch 1 Matter in Our Surroundings Slide show 3.pptRajveerKaushal1
- Matter exists in solid, liquid, gas, and plasma states and undergoes physical and chemical changes. Physical changes alter a substance's state or form without changing its chemical makeup, while chemical changes create new substances.
- Substances can be elements, compounds, or mixtures. Elements cannot be broken down further, while compounds have a fixed composition and can be decomposed into simpler substances through chemical changes. Mixtures are combinations of substances that are not chemically bonded and have variable compositions.
- Plasma, the fourth state of matter, consists of free-floating ions and electrons. It is created by applying energy to strip electrons from atoms and can be controlled using electric and magnetic fields. Plasma research aids in understanding
This document provides an introduction to general chemistry, including why chemistry is studied, its central role in understanding matter, and learning goals for the course. Chemistry involves understanding the properties and behavior of matter, which exists as elements, compounds, and mixtures. The three states of matter - solid, liquid, and gas - are classified based on molecular motion and energy. Physical and chemical properties help characterize different types of pure substances and mixtures. Changes in matter can involve physical changes of state or chemical reactions that alter chemical identity. Energy also plays a key role in these transformations.
This document discusses physical and chemical changes, pure substances, mixtures, and states of matter. It defines physical changes as changes in a substance's state or form without changing its chemical composition, and chemical changes as the formation of new substances through chemical reactions. Mixtures are combinations of substances that are not chemically bonded and can be separated by physical means. The four common states of matter are solids, liquids, gases, and plasma, which differ in the arrangement and movement of their particles according to the kinetic molecular theory.
G8 Science Q3- Week 3-4- Protons and Atoms.pptxazielcapuyan1
This document discusses the classification of matter and the properties of solids, liquids, and gases. It begins by defining key terms like elements, compounds, mixtures, homogeneous mixtures, and heterogeneous mixtures. It then discusses the particle nature of matter and how the kinetic energy and attractive forces between particles determines a substance's state. It provides examples of physical and chemical properties and changes. It explains the states of matter and phase changes using diagrams of heating/cooling curves and a phase diagram.
This document outlines a lesson plan for teaching students about the properties of matter. The objective is for students to identify characteristics of solids, liquids, and gases, as well as physical and chemical properties. The lesson includes engaging activities like showing samples of water in different states and having students watch an educational video. Students will explore concepts through a demonstration of states of matter and discussion. They will also conduct a lab experiment with "Oobleck" to investigate its properties. For evaluation, students will complete assignments summarizing their learning.
The document discusses physical and chemical changes of matter. A physical change alters the form of a substance but not its chemical composition, such as melting or freezing. A chemical change produces new substances through rearrangement of atoms, like burning or rusting. The document also covers the states of matter, kinetic molecular theory, changes of state, and temperature scales.
201115985 power point slides ( matter and matterial)musa chauke
This document discusses the classification and states of matter. It begins by defining matter and classifying it into elements, compounds and mixtures. It then describes the three states of matter - solid, liquid and gas. Physical properties and chemical properties are distinguished. Physical properties can be observed without changing the identity of the substance while chemical properties involve changes to its identity. Common phase changes like melting, boiling, evaporation and condensation are also outlined.
This document provides an overview of properties of matter. It begins by defining the three states of matter - solids, liquids, and gases. It describes the properties of each state, such as solids having a fixed shape and volume while gases have no fixed shape or volume. The document then discusses physical and chemical properties and changes, defining the difference between physical and chemical changes. It provides examples of each. Density is also covered, defining concepts such as mass, volume, and density and providing practice problems. The document concludes by discussing elements, compounds, and mixtures.
The document discusses physical and chemical changes of matter. A physical change alters the form of a substance without changing its chemical composition, such as melting or freezing. A chemical change produces new substances through rearrangement of atoms, like burning or rusting. The three main states of matter are solids, liquids, and gases. Changes between these states are physical changes caused by temperature increases that provide kinetic energy to particles. The kinetic molecular theory describes particle behavior in the different states.
The document discusses physical and chemical changes of matter. A physical change alters the form of a substance without changing its chemical composition, such as melting or freezing. A chemical change produces new substances through rearrangement of atoms, like burning or rusting. The three main states of matter are solids, liquids, and gases. Changes between these states are physical changes caused by temperature increases that provide kinetic energy to particles. The kinetic molecular theory describes particle behavior in the different states.
The document discusses physical and chemical changes of matter. A physical change alters the form of a substance without changing its chemical composition, such as melting or freezing. A chemical change produces new substances through rearrangement of atoms, like burning or rusting. The three main states of matter are solids, liquids, and gases. Changes between these states are physical changes driven by temperature and the kinetic energy of particles. Chemical reactions follow the law of conservation of mass and involve energy transfer between systems and their surroundings.
The document discusses physical and chemical changes of matter. A physical change alters the form of a substance without changing its chemical composition, such as melting or freezing. A chemical change produces new substances through rearrangement of atoms, like burning or rusting. The three main states of matter are solids, liquids, and gases. Changes between these states are physical changes driven by temperature and the kinetic energy of particles. Chemical reactions follow the law of conservation of mass and involve energy transfer between systems and their surroundings.
The document discusses physical and chemical changes of matter. A physical change alters the form of a substance without changing its chemical composition, such as melting or freezing. A chemical change produces new substances through rearrangement of atoms, like burning or rusting. The three main states of matter are solids, liquids, and gases. Changes between these states are physical changes driven by temperature and the kinetic energy of particles. Chemical reactions follow the law of conservation of mass and involve energy transfer between systems and their surroundings.
This document provides an introduction to general chemistry concepts. It begins with defining chemistry and discussing its branches, including analytical chemistry, physical chemistry, organic chemistry, and inorganic chemistry. It then discusses the importance of chemistry for nurses, focusing on understanding drug composition and properties, diagnosis, disease mechanisms, and sterilization. The document also defines matter and the three states of matter - solid, liquid, and gas. It provides examples and descriptions of the properties and changes between each state. Finally, it classifies matter as either pure substances like elements and compounds, or impure substances like mixtures, and provides brief definitions of each.
The document describes the key points of the kinetic particle theory. It explains that kinetic particle theory views matter as being made up of tiny particles in constant random motion. It also describes the three states of matter (solid, liquid, gas) in terms of the arrangement and motion of particles. Specifically, it explains how the properties of each state, such as compressibility and ability to change shape, can be understood by considering the forces between particles and how tightly or loosely packed they are.
This document discusses the three common states of matter - solids, liquids, and gases. It describes their characteristic properties, including how the particles move and interact in each state. The document also explains the phase changes between these different states, such as melting, freezing, boiling, evaporation, condensation, and sublimation. Energy must be either absorbed or released for matter to change phases. The behaviors of gases are further explained through gas laws like Boyle's and Charles' Laws.
Unit b matter and chemical change notesRileyAntler
The document discusses matter and chemical change. It defines matter as anything that has mass and takes up space. Matter exists in different states - solid, liquid, and gas - which are determined by the motion and spacing of particles. Changes between states of matter involve adding or removing heat. Chemical and physical properties are also discussed, where chemical changes alter the chemical composition and physical changes do not. The document provides examples of physical and chemical properties and changes. Classifying matter as elements, compounds, or mixtures is also covered.
The document provides information about Earth's spheres, biomes, ecosystems, and natural resources. It discusses the following:
- Earth has four spheres - the geosphere (rocks), hydrosphere (water), atmosphere (air), and biosphere (life).
- Major biomes include aquatic, desert, tundra, grassland, forest (taiga, temperate deciduous, tropical rainforest), and their characteristic climates, soils, plants and animals.
- Ecosystems involve interactions between biotic factors like producers, consumers, decomposers and abiotic factors like the environment. Species interact through food chains, webs and pyramids.
- Natural resources can be
This document provides information about fossils and methods used to date the age of fossils. It discusses the different types of fossils that can form like molds, casts, carbon films, and trace fossils. Living fossils are described as organisms that have survived relatively unchanged for millions of years. Transitional fossils are discussed as evidence of evolution but are noted to be rare. Methods for dating fossils include relative dating based on positioning in rock layers and absolute dating techniques like radiometric dating which provide numeric ages but have assumptions and margins of error.
This document discusses simple machines and how they make work easier. It defines work as a force moving an object over a distance. The six basic simple machines that reduce the force needed for work are the inclined plane, wedge, screw, lever, wheel and axle, and pulley. Each machine works by either changing the size or direction of the applied force. Compound machines combine two or more simple machines to accomplish work.
This document discusses key aspects of scientific inquiry including conclusions and presentations. It provides examples of scientific facts, theories, and laws. Facts are objective observations that can be verified, theories are explanations for how natural phenomena work that can be observed and tested, and laws are descriptions of observable phenomena that always apply under the same conditions. The document also addresses forming hypotheses, collecting and analyzing data, drawing conclusions, and sharing findings.
This document provides instructions for an experiment to test whether eggs can float in water with added salt. The scientific method is followed, beginning with making observations and forming a hypothesis that eggs will float if enough salt is dissolved in water. Materials are listed and procedures described for conducting trials adding increasing amounts of salt to water and recording if the egg sinks or floats. Data is organized in a table and graph showing that eggs begin to float when salt reaches 25-30 ml added to 300 ml water. The conclusion supports the hypothesis and results are shared with the class.
This document provides information about science experiments, including the scientific method, variables, controls, hypotheses, procedures, data collection, analysis, and conclusions. It discusses key parts of an experiment like the independent and dependent variables, controls, developing hypotheses, designing procedures, collecting objective versus subjective data, analyzing results, and drawing conclusions. Examples are provided to illustrate these scientific experiment concepts.
This document provides an overview of the scientific method process, including:
1) Observation and forming a testable question, which should have one variable and measurable outcomes.
2) Developing a hypothesis in an "if...then...because" format to make an educated guess about what will happen during the experiment.
3) Designing and performing an experiment to test the hypothesis by manipulating the variable and collecting objective data.
4) Analyzing the results to determine if the hypothesis was supported or needs revising, and drawing a conclusion.
The document summarizes several key human body systems and the five senses. It includes review questions about the nervous system and its major divisions of the central nervous system and peripheral nervous system. Experiments are described to test sight, smell, taste, touch and reflexes. Step-by-step instructions for a bovine eye dissection are provided to examine the anatomy of vision.
This document provides information about the human nervous system, including:
- The central nervous system (CNS) which includes the brain and spinal cord.
- The peripheral nervous system (PNS) which includes nerves that connect all body parts to the spinal cord, including somatic nerves (voluntary movement and senses) and autonomic nerves (involuntary functions).
- Key parts of the brain like the cerebrum, cerebellum, and brain stem and their functions.
- How the nervous system uses neurons, synapses, and neural pathways to collect sensory input, integrate it in the brain, and result in motor outputs to the body's muscles and glands.
Here are the major human body systems and some of their key organs:
- Digestive system: mouth, esophagus, stomach, small intestine, large intestine, liver, pancreas, gallbladder
- Circulatory/Cardiovascular system: heart, blood vessels (arteries, veins, capillaries)
- Respiratory system: nose, pharynx, larynx, trachea, lungs, diaphragm
- Urinary system: kidneys, ureters, bladder, urethra
- Integumentary system: skin, hair, nails
- Skeletal system: bones, cartilage, ligaments, tendons
- Muscular system:
This document summarizes key aspects of the respiratory system and the effects of smoking. It describes the major parts of the respiratory system including the nose, larynx, trachea, lungs, bronchi, and alveoli. It explains how gas exchange occurs in the alveoli and the composition of inhaled and exhaled air. It also details the mucus elevator defense system and effects of smoking such as increased risk of various diseases, cancer, and overall shortened lifespan.
The cardiovascular system circulates blood throughout the body via the heart and blood vessels. The heart has four chambers and pumps around 4,000 gallons of blood per day through arteries, veins, and capillaries to deliver oxygen and nutrients to cells and remove carbon dioxide and waste. Blood contains plasma, red blood cells to carry oxygen and carbon dioxide, white blood cells to fight infection, and platelets to help clotting.
This document provides information about the human digestive system and nutrition. It defines the major parts of the digestive system and their functions. It also explains the three main types of nutrients - carbohydrates, lipids (fats), and proteins. For each nutrient, it identifies food sources and describes the digestion process. Additionally, it distinguishes between good and bad types of each nutrient and provides examples. The document aims to educate about nutrition and how the body breaks down and uses different foods.
This document provides information about the human digestive and excretory systems. It describes the major organs involved in digestion, including the mouth, esophagus, stomach, small intestine, large intestine, liver, and pancreas. It explains the physical and chemical processes of digestion that break down food into smaller molecules that can be absorbed and used by the body. These include mechanical and chemical digestion in the mouth, stomach acid and enzymes, and nutrient absorption in the small intestine. The document also covers the role of the kidneys and urinary system in filtering waste from the blood and excreting it from the body as urine.
This document provides information about the human body systems, specifically bones and muscles. It begins with a review quiz about the skin and its layers (epidermis, dermis, hypodermis). It then discusses the chicken wing dissection and homologous features in the human body. The document lists and describes various bones and their functions. It also covers bone cells, tissues, and shapes. Finally, it discusses the three types of muscle tissues and their roles in voluntary and involuntary movement.
The document summarizes the human body systems, beginning from the cellular level up to full organ systems. It describes that cells make up tissues, tissues make up organs, and organs work together in organ systems to carry out functions. As an example, it focuses on the integumentary system and skin, describing the three layers of the skin (epidermis, dermis, hypodermis), their components and functions, as well as common skin problems like acne, dermatitis, skin cancer and burns.
The document discusses several key concepts relating to evolution and the fossil record, including:
- Microevolution involves small changes within a species over short time periods, while macroevolution describes large changes over millions of years that result in new species through speciation events.
- The geologic column provides evidence of evolution through its layered fossil and rock formations arranged from oldest to youngest, though it has gaps and inconsistencies that are puzzling.
- The Cambrian explosion saw a sudden appearance of many animal phyla without clear precursor fossils, challenging gradual evolution theories.
- Comparative anatomy and embryology provide evidence of common ancestry through homologous structures, though their interpretation differs between evolutionary and creationist viewpoints.
This document discusses the classification of living things. It begins by explaining that Carolus Linnaeus developed the first scientific classification system in the 1700s, grouping organisms into three kingdoms: Animal, Vegetable, and Mineral. It then discusses how modern taxonomy further classifies organisms using a hierarchical system of domains, kingdoms, phyla, classes, orders, families, genera, and species. The rest of the document provides details on the six kingdoms of life - Archaea, Bacteria, Protista, Fungi, Plantae, and Animalia - and examples of major groups within each kingdom.
This document discusses basic concepts of genetics and inheritance, including:
- Germ cells undergo meiosis to form gametes like eggs and sperm, which are haploid.
- Gregor Mendel conducted experiments on pea plants in the 1800s and discovered dominant and recessive traits are inherited based on predictable ratios.
- Traits are determined by alleles, or variations of genes. Dominant alleles are expressed over recessive alleles in heterozygotes based on genotypes.
- Meiosis and fertilization allow for genetic variation through independent assortment and recombination of parental chromosomes.
This document discusses key concepts about the water cycle and glaciers. It begins with a review of where glaciers form and icebergs come from. It then covers the water cycle in more detail, explaining processes like precipitation, infiltration, evaporation, transpiration, runoff, and aquifer storage. Glacial movement and erosion are described. The document concludes with a review quiz testing understanding of these hydrologic and glacial concepts.
A Visual Guide to 1 Samuel | A Tale of Two HeartsSteve Thomason
These slides walk through the story of 1 Samuel. Samuel is the last judge of Israel. The people reject God and want a king. Saul is anointed as the first king, but he is not a good king. David, the shepherd boy is anointed and Saul is envious of him. David shows honor while Saul continues to self destruct.
Gender and Mental Health - Counselling and Family Therapy Applications and In...PsychoTech Services
A proprietary approach developed by bringing together the best of learning theories from Psychology, design principles from the world of visualization, and pedagogical methods from over a decade of training experience, that enables you to: Learn better, faster!
This presentation was provided by Rebecca Benner, Ph.D., of the American Society of Anesthesiologists, for the second session of NISO's 2024 Training Series "DEIA in the Scholarly Landscape." Session Two: 'Expanding Pathways to Publishing Careers,' was held June 13, 2024.
Leveraging Generative AI to Drive Nonprofit InnovationTechSoup
In this webinar, participants learned how to utilize Generative AI to streamline operations and elevate member engagement. Amazon Web Service experts provided a customer specific use cases and dived into low/no-code tools that are quick and easy to deploy through Amazon Web Service (AWS.)
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Chapter wise All Notes of First year Basic Civil Engineering.pptxDenish Jangid
Chapter wise All Notes of First year Basic Civil Engineering
Syllabus
Chapter-1
Introduction to objective, scope and outcome the subject
Chapter 2
Introduction: Scope and Specialization of Civil Engineering, Role of civil Engineer in Society, Impact of infrastructural development on economy of country.
Chapter 3
Surveying: Object Principles & Types of Surveying; Site Plans, Plans & Maps; Scales & Unit of different Measurements.
Linear Measurements: Instruments used. Linear Measurement by Tape, Ranging out Survey Lines and overcoming Obstructions; Measurements on sloping ground; Tape corrections, conventional symbols. Angular Measurements: Instruments used; Introduction to Compass Surveying, Bearings and Longitude & Latitude of a Line, Introduction to total station.
Levelling: Instrument used Object of levelling, Methods of levelling in brief, and Contour maps.
Chapter 4
Buildings: Selection of site for Buildings, Layout of Building Plan, Types of buildings, Plinth area, carpet area, floor space index, Introduction to building byelaws, concept of sun light & ventilation. Components of Buildings & their functions, Basic concept of R.C.C., Introduction to types of foundation
Chapter 5
Transportation: Introduction to Transportation Engineering; Traffic and Road Safety: Types and Characteristics of Various Modes of Transportation; Various Road Traffic Signs, Causes of Accidents and Road Safety Measures.
Chapter 6
Environmental Engineering: Environmental Pollution, Environmental Acts and Regulations, Functional Concepts of Ecology, Basics of Species, Biodiversity, Ecosystem, Hydrological Cycle; Chemical Cycles: Carbon, Nitrogen & Phosphorus; Energy Flow in Ecosystems.
Water Pollution: Water Quality standards, Introduction to Treatment & Disposal of Waste Water. Reuse and Saving of Water, Rain Water Harvesting. Solid Waste Management: Classification of Solid Waste, Collection, Transportation and Disposal of Solid. Recycling of Solid Waste: Energy Recovery, Sanitary Landfill, On-Site Sanitation. Air & Noise Pollution: Primary and Secondary air pollutants, Harmful effects of Air Pollution, Control of Air Pollution. . Noise Pollution Harmful Effects of noise pollution, control of noise pollution, Global warming & Climate Change, Ozone depletion, Greenhouse effect
Text Books:
1. Palancharmy, Basic Civil Engineering, McGraw Hill publishers.
2. Satheesh Gopi, Basic Civil Engineering, Pearson Publishers.
3. Ketki Rangwala Dalal, Essentials of Civil Engineering, Charotar Publishing House.
4. BCP, Surveying volume 1
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Iván Bornacelly, Policy Analyst at the OECD Centre for Skills, OECD, presents at the webinar 'Tackling job market gaps with a skills-first approach' on 12 June 2024
2. Demonstration 2.2
Physical vs. Chemical Descriptions
(a.k.a. Guess What's in the Bag)
• Physical descriptions:
• State of matter
• Temperature
• Size, density, mass, volume
• Texture, color, shape, smell
• Chemical descriptions:
• Flammability, toxicity
• Reactivity, corrosiveness
• chemical composition
• (describe interactions)
3. In your lab notebook, please answer as best you can:
1. What is matter (definition) and what is it made of?
• Matter is anything that has mass and takes up space; it is made up of atoms
1. Name the three sub-atomic particles and their respective charges.
• Proton (+), Electron (-), and Neutron (0)
3. What is a molecule ?
• More than one atom bonded (joined) together.
4. A substance made of molecules with different types of atoms is a...
• Compound
4. A substance made up of only one type of atom is called…
• An element
Bonus Question: What type of mixture is air?
Air is a homogeneous mixture (and also a solution) of different gasses.
Review
Quiz 1
5. All matter is made of atoms
Atoms of the same kind form pure elements
What properties do the different elements possess?
Color, texture, odor?
Melting point, flammability?
Density, reactivity?
What form do the elements
take at normal temperatures?
States of matter:
Solid
Liquid
Gas
Plasma
B-E Condensate
MatterMatter
Interactive Periodic TableInteractive Periodic Table
Review
GoldM
ercury
Helium
Oxyge
n
Alum
inumCoppe
r
Lead
Silver
Neon
Sulfer
6. Common States of MatterCommon States of Matter
• Elements & compounds can exist in different states
• The most common are solid, liquid, and gas
7. Looking CloserLooking Closer
• Arrangement of the particles
what patterns the atoms or molecules form
(due to bonding or attraction)
• Energy of particles
how fast the atoms/molecules are moving
(temperature)
• Distance between particles
how far apart the atoms or molecules are
from each other (density)
States of matter are affected by...
8. Experiment 2.1
Inner Space
How is the cup of marbles like water?
• Are the marbles a good representation of
molecules?
Which aspects of this experiment
• change? (variables)
• stay the same? (controls)
Sugar & Salt Solutions SIM
• Observation:
• What do you know?
• What do you want to
know more about?
• Hypothesis:
• What do you think will
happen (& why)?
• Experiment:
• Record the data
• What happened?
• Conclusion:
• Was your hypothesis
correct?
• What's next?
9. Solids
Particles are tightly packed togetherParticles are tightly packed together
• Crystal lattice structure of moleculesCrystal lattice structure of molecules
Particles vibrate about a fixed positionParticles vibrate about a fixed position
• Do NOT move freely or slide past one anotherDo NOT move freely or slide past one another
They have a definite shape and a definite volume.They have a definite shape and a definite volume.
• Retain their shape regardless of containerRetain their shape regardless of container
• Cannot be compressedCannot be compressed
10. Liquids
Particles are touching, but can slide past one anotherParticles are touching, but can slide past one another
Have an indefinite shapeHave an indefinite shape
• Fit into the bottom of whatever container they are placed inFit into the bottom of whatever container they are placed in
Liquids have a definite volumeLiquids have a definite volume
• Cannot be compressedCannot be compressed
11. Particles are very far apart and move freely and rapidly.Particles are very far apart and move freely and rapidly.
Have an indefinite shapeHave an indefinite shape
• Fill whatever container they are place inFill whatever container they are place in
Have an indefinite volumeHave an indefinite volume
• Can easily be compressedCan easily be compressed
Gases
12. Atomic Speed
• Did you know we can
measure the motion of
atoms and molecules?
• The temperature of a
substance is a measure of
it’s molecular motion
Molecules + Energy = Faster Molecule Movement = Heat
13. • Celsius
• Water based
• Kelvin
• No negatives
• No degrees
• Fahrenheit
• smaller units
of change
Temperature Scales
14. There are predictable temperatures of phase change for water (at sea level):There are predictable temperatures of phase change for water (at sea level):
• Melting/Freezing Point = 0o
C, 32o
F or 273K
• Boiling/Condensing Point = 100o
C, 212o
F or 373 K
Points of Change
0o
C 100o
C
15. A plasma is an ionized gas.
• Superheated over 1,000o
C
• Electrons are stripped away from the protons
A plasma is a very good conductor of electricity
• Affected by magnetic fields
• Has an overall neutral charge
Plasmas, like gases have an indefinite shape and volume.
• Particles move VERY fast.
PlasmaAdvanced
Topic
16. • Atoms no longer move around as individuals.
• They all act the same, as a singular particle
• You can no longer tell them apart!
• Requires quantum physics to understand.
Bose-Einstein Condensate
Super-cooled matter (near absolute zero or - 273o
C) forms another state
Advanced
Topic
BE Condensate
Visualization
17. Changes of StateChanges of State
• What affects a substance’s physical state?
• Temperature
• Adding heat (energy)
excites the
atoms/molecules
• Pressure
• Adding pressure
“immobilizes” the
atoms/molecules
• Atomic Interactions
• Bonding between
atoms/molecules
• Water's H-bonds make
it less susceptible to
state changes
19. Properties of Matter
• Physical properties: observed characteristics that
describe a substance
• State of matter (solid, liquid, gas, plasma, B-E condensate)
• Melting and boiling point
• Size, density, mass, volume
• Temperature, color, texture, etc.
• Chemical properties: characteristics that
describe how a substance's composition can
change (undergo a chemical reaction)
• Flammability, toxicity
• Susceptibility to rust (oxidation state)
• Resistance to decomposition
• Reactivity to other substances
• Chemical composition (what atoms form the substance)
20. Chemical Formulas
• Each element has a symbol
• O for Oxygen, C for Carbon, Cl for Chlorine, etc.
• Periodic Table of the Elements lists these symbols
• A compound's chemical composition can be
written out as a formula showing the ratio of
different elements
Common Compounds
Compound Chemical Formula
Ammonia NH3
Carbon dioxide CO2
Carbon monoxide CO
Glucose C6H12O6
Methane CH4
Sodium Chloride NaCl
Water H2O
• The subscript # refers to
the symbol before it
• Example: Water
• For every one atom of
Oxygen, there are two
Hydrogen atoms
21. Physical vs. Chemical Changes
• When matter undergoes a physical change:
• it alters the state, shape or appearance
• it retains it's chemical composition
• the original matter can be recovered
• i.e. wood is still wood after being cut or shredded into sawdust, but its
size and shape may change
• When matter undergoes a chemical change:
• it changes into a totally different type of matter
• it's chemical composition changes (atoms and
molecules are broken apart or combined
differently to form new substances)
• the original matter cannot be recovered
• i.e. wood that is burned changes into charcoal and
ashes
22. Examples of Physical & Chemical
Changes
Physical Changes Chemical Changes
Wood getting ground into sawdust Wood burned in a campfire.
An aluminum can getting crushed. Rust forming on a leaky pipe.
Cheese melting on tortilla chips. Bread baking in the oven.
A puddle of water evaporating. A silver platter that is tarnishing.
Blueberries becoming frozen in the freezer. Milk turning into cheese.
Rubbing alcohol evaporating on your skin. Butane igniting in a lighter.
A kernel of corn being popped. Decomposing plants or animals.
Gasoline burning in a car engine.
Eggs being scrambled in a hot pan.
Apple slices turning brown.
Drain cleaner removing a hair clog.
23. Indications of a Chemical Change
• Change in color
• Change in temperature
• gets warmer or cooler
• Bubbles or precipitate
• (evidence that a new substance with
a different state of matter is forming)
• Release of energy
• Sound, light, and/or heat
Editor's Notes
Opener: guess what’s in the bag demo
Paper bags with objects: (tennis, ping-pong & bouncy balls, marble and stress ball or orange), (sugar-filled baggie, cotton balls, water-filled balloon & bean), (wooden block, rock, styrofoam, metal box) (inflated balloon, stuffed animal, feather, wad of paper)
Students must use senses other than sight to describe. 1 student describes the object and class (or group) guesses.
- include shape, size/volume, mass, texture
- MUST include what state of matter the object is in
All because of the atoms that form them -
different atoms have different properties that react depending on their number of protons, electrons & neutrons
The different states of matter are categorized by the arrangement and energy of the particles at normal temperatures and pressures. The state of matter can be altered by adding or removing energy and/or pressure which can affect the arrangement and energy of the particles.
These are the three most common - but there are others that we will discuss later.
The different states of matter are categorized by the arrangement and energy of the particles at normal temperatures and pressures. The state of matter can be altered by adding or removing energy and/or pressure which can affect the arrangement and energy of the particles.
SUPPLIES: CLEAR plastic cups, 8-oz. or smaller, water in bottles, marbles, salt, sugar & sand (about ½ cup each), measuring spoons
Plastic plates for collecting water overflow, paper towels, coffee filters, strainer
PROCEDURE
1. Label three cups “marbles,” “sugar water,” and “salt water.”
2. Completely fill the cup labeled “marbles” with marbles.
• How do you know the cup is full?
• Do you think you could add sand to this cup? Where would the sand go if you added it?
3. Add sand to the cup full of marbles.
• How many spoonfuls of sand can you add to the marbles?
• Where did the sand go?
4. Completely fill the cups labeled “sugar water,” and “salt water” with water.
• How do you know the cups are full?
• How are these cups full of water similar to the cup full of marbles?
5. In the next step, you will add salt to the “salt water” cup until the water overflows.
• Predict: How many spoonfuls of salt do you think you can add?
6. Carefully add 1 spoonful of salt to the “salt water” cup. Count and add more spoonfuls of salt.
• How many spoonfuls of salt could you add to the water?
• Where did the salt go?
7. In the next step, you will add sugar to the “sugar water” cup until the water overflows.
• Predict: How many spoonfuls of sugar do you think you can add?
8. Now add one tablespoon of sugar to the “sugar water” cup. Count and add more spoonfuls of sugar.
• How many spoonfuls of sugar could you add to the water?
• Where did the sugar go?
9. Clean up your area.
• Follow your teacher’s directions.
Most of the 100+ elements are solid at room temperature.
Drool - coffee - mercury - bromine?
Mercury and bromine only liquid elements (at room temp).
Kelvin is a temperature scale designed so that zero degrees K is defined as absolute zero (at absolute zero, a hypothetical temperature, all molecular movement stops - all actual temperatures are above absolute zero) and the size of one unit is the same as the size of one degree Celsius.
The Kelvin scale is popular in scientific applications because of the lack of negative numbers. This scale is convenient for recording the very low temperatures of liquid helium and liquid nitrogen, for example. The lack of negative numbers also makes it easier to calculate differences between temperatures, such as saying one temperature is three times another temperature.
In 1848, Kelvin used this as a basis for an absolute temperature scale. He defined "absolute" as the temperature at which molecules would stop moving, or "infinite cold." From absolute zero, he used the same unit as Celsius to determine the increments.
Absolute zero cannot technically be achieved. However, scientists have been able to lower the temperature of matter to just a fraction of a Kelvin above absolute zero through techniques such as slowing down particles using lasers.
Sublimation = going directly from solid to gas (i.e. dry ice)
In a plasma the electrons have been stripped away from the central nucleus. Therefore, a plasma consists of a sea of ions and electrons and is a very good conductor of electricity and is affected by magnetic fields. Electrons are separated from their respective nucleus when enough heat is applied. In controlled thermonuclear fusion research, plasmas are heated to over 100 million degrees.
The negatively charged electrons (yellow) are freely streaming through the positively charged ions (blue).
In February 2003, the Boomerang Nebula was observed to have been releasing gases at a speed of 500,000 km/h (over 300,000 mph) for the last 1,500 years. This has cooled it down to approximately 1 K, as deduced by astronomical observation, which is the lowest natural temperature ever recorded.
Review 5 states of matter: solid, liquid, gas, plasma, BE condensate
Explore ptable.com to see state changes at different temperatures
In 1924 (82 years ago), two scientists, Albert Einstein and Satyendra Bose predicted a 5th state of matter which would occur at very very low temperatures.
Finally, in 1995 (71 years later), Wolfgang Ketterle and his team of graduate students discovered the 5th state of matter for the first time.
Chemical property: the way a substance may change or react to form other substances
isopropyl alcohol = C3H8O
see "Physical & Chemical Changes Lab" document
May use some of the “Stations” as a teacher demo: starch/glue to make a polymer, vinegar & milk, vinegar & chalk (grind chalk first for physical change, then add vinegar for chemical change), steel wool and Kool-Aid, electrolysis, or decomposition of hydrogen peroxide catalyzed by platinum contact-solution neutralizing disc.