This document describes a lesson on the phases of matter. It includes objectives, definitions of matter and the three phases (solid, liquid, gas), an activity to classify materials as solid, liquid or gas, comparisons of the different phases, descriptions of phase changes like melting, freezing, evaporation and condensation, and questions about a video on phase changes.
Matter can exist in three states - solid, liquid, and gas. Examples of solids are ice and diamonds; examples of liquids are water and mercury. Gases include water vapor and oxygen. Characteristic properties like boiling point and melting point are used to identify substances and do not change, even if the substance changes state. Physical changes alter the substance's form through processes like melting or crushing, but do not change its chemical makeup. Chemical changes form new substances through chemical reactions.
Matter is anything that can take up space and exists in three main states: solids, liquids, and gases. Solids have a definite shape and volume, with particles tightly packed together. Liquids have no definite shape but a definite volume, with particles close together but able to move past one another. Gases have neither a definite shape nor volume, with particles very spread out and able to move freely past one another.
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.
This document discusses different types of motion including up and down, straight line, round and round, and zigzag motion. It describes how to measure motion through distance, time, and speed. Forces that affect motion include the strength and direction of applied forces, the mass of an object, and friction. Gravity is also identified as a force that pulls objects down toward Earth.
Matter exists in three states: solids, liquids, and gases. Solids have a definite shape and volume, while liquids take the shape of their container but have a definite volume. Gases fill their container completely and do not have a definite shape or volume. The particles that make up solids, liquids and gases, called molecules, behave differently in each state - in solids they are close together and don't move much, in liquids they are loosely tied and flow freely, and in gases they are far apart and move freely.
There are four fundamental forms of matter: solids, liquids, gases, and plasma. Solids have a definite shape and volume due to their rigid molecular structure. Liquids also have a definite volume but cannot maintain a definite shape as their molecules are drawn together weakly, allowing liquids to flow and take the shape of their container. Gases have neither a definite shape nor volume as their molecules are very weakly bonded and spread out to fill their container. Plasma differs from solids, liquids, and gases in that its molecules are ionized, meaning they are positively or negatively charged, and thus exhibit electromagnetic properties.
The document discusses the different phases of matter (solid, liquid, gas) and the phase changes between them. When energy is added to a solid, its bonds break and it melts into a liquid where particles can move freely. Adding more energy turns the liquid into a gas where particles move randomly. The phase changes - melting/freezing, vaporization/condensation, sublimation/deposition - describe the changes in particle arrangement that occur when energy is added or removed. Phase changes are classified as endothermic, where energy is absorbed during the change, or exothermic, where energy is released.
Matter can exist in three states - solid, liquid, and gas. Examples of solids are ice and diamonds; examples of liquids are water and mercury. Gases include water vapor and oxygen. Characteristic properties like boiling point and melting point are used to identify substances and do not change, even if the substance changes state. Physical changes alter the substance's form through processes like melting or crushing, but do not change its chemical makeup. Chemical changes form new substances through chemical reactions.
Matter is anything that can take up space and exists in three main states: solids, liquids, and gases. Solids have a definite shape and volume, with particles tightly packed together. Liquids have no definite shape but a definite volume, with particles close together but able to move past one another. Gases have neither a definite shape nor volume, with particles very spread out and able to move freely past one another.
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.
This document discusses different types of motion including up and down, straight line, round and round, and zigzag motion. It describes how to measure motion through distance, time, and speed. Forces that affect motion include the strength and direction of applied forces, the mass of an object, and friction. Gravity is also identified as a force that pulls objects down toward Earth.
Matter exists in three states: solids, liquids, and gases. Solids have a definite shape and volume, while liquids take the shape of their container but have a definite volume. Gases fill their container completely and do not have a definite shape or volume. The particles that make up solids, liquids and gases, called molecules, behave differently in each state - in solids they are close together and don't move much, in liquids they are loosely tied and flow freely, and in gases they are far apart and move freely.
There are four fundamental forms of matter: solids, liquids, gases, and plasma. Solids have a definite shape and volume due to their rigid molecular structure. Liquids also have a definite volume but cannot maintain a definite shape as their molecules are drawn together weakly, allowing liquids to flow and take the shape of their container. Gases have neither a definite shape nor volume as their molecules are very weakly bonded and spread out to fill their container. Plasma differs from solids, liquids, and gases in that its molecules are ionized, meaning they are positively or negatively charged, and thus exhibit electromagnetic properties.
The document discusses the different phases of matter (solid, liquid, gas) and the phase changes between them. When energy is added to a solid, its bonds break and it melts into a liquid where particles can move freely. Adding more energy turns the liquid into a gas where particles move randomly. The phase changes - melting/freezing, vaporization/condensation, sublimation/deposition - describe the changes in particle arrangement that occur when energy is added or removed. Phase changes are classified as endothermic, where energy is absorbed during the change, or exothermic, where energy is released.
Matter can change states between solid, liquid, and gas. Water is used as an example, changing between ice, liquid water, and water vapor through the processes of melting, evaporation, and condensation. Evaporation occurs when liquid water is heated and changes into gas water vapor, while condensation is when water vapor cools and changes back into liquid water.
This document provides information about the particle nature of matter. It includes standards and objectives about demonstrating an understanding of the particle nature of matter and its properties. It discusses the key concepts of explaining the properties of solids, liquids, and gases based on how the particles are arranged and move. It also explains physical changes in these states in terms of particle arrangement and motion, and how this can be used to explain processes like melting, freezing, evaporating, and condensing.
This document summarizes the differences between physical and chemical changes in matter. It defines matter as anything that occupies space and has mass. A physical change alters the form of matter but does not create a new substance, and may be reversible. A chemical change produces a new substance that cannot be changed back to the original by ordinary means. Examples of each type of change are provided for classification exercises.
4th grade unit c ch. 11 lesson 1 what is matterhinsz
The document defines matter as anything that has mass and takes up space. It explains that matter exists in three states - solid, liquid, and gas - which are distinguished by the arrangement of their particles and how they behave. Solids have a definite shape and volume from tightly packed particles, while liquids take the shape of their container but maintain a constant volume, and gases fill their container and have particles far apart.
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 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.
This document describes the differences between freezing, melting, and evaporation. It defines these terms and explains factors that influence their rates. Freezing is a change from liquid to solid, melting is solid to liquid, and evaporation is liquid to gas below the boiling point. Temperature, size/shape, conduction, humidity, and composition affect rates. Higher temperatures speed melting and evaporation, while lower temperatures speed freezing. Smaller pieces melt/freeze faster due to more surface area. Good conductors transfer heat/cold faster. Evaporation is slowest in high humidity.
Phase changes occur when matter transitions between solid, liquid, and gas states. During a phase change, molecules either absorb or release heat energy as they speed up or slow down. There are several types of phase changes, including melting (solid to liquid), freezing (liquid to solid), vaporization/boiling (liquid to gas), evaporation, condensation, and sublimation. A key characteristic of phase changes is that the temperature remains constant despite an exchange of heat energy, as the molecules rearrange their structure.
This document discusses the three states of matter - solids, liquids, and gases. It defines each state and explains how their particle arrangements differ. Solids have a definite shape and volume, while liquids have a definite volume but not shape, and gases fill their container. The document also covers physical changes like melting, freezing, and evaporation which alter a substance's state without changing its chemical makeup. Finally, it defines mixtures as combinations of materials that retain their individual properties, and solutions as mixtures where one material disseminates evenly throughout another.
The document discusses different types of mixtures including homogeneous and heterogeneous mixtures, solution-based mixtures, and solid mixtures. Homogeneous mixtures have a uniform composition while heterogeneous mixtures have a non-uniform composition. Solution-based mixtures can be classified as true solutions, colloidal solutions, or suspensions depending on the particle size of the solute. Solid mixtures include alloys, which are homogeneous solid solutions of metals that are difficult to separate. An example given is brass, which is a homogeneous mixture of copper and zinc that takes on properties between the two metals.
If iced tea mix is stirred into water, it would form a homogeneous solution. The tea mix particles would be too small to separate out or filter from the water. Over several days, the drink would not separate into distinct layers. Solutions like this form a single phase because the solute particles are small enough to dissolve uniformly throughout the solvent.
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.
Energy is a property of objects that can be transferred or converted into different forms. There are two main types of energy: potential energy, which is the stored energy of position, and kinetic energy, which is the energy of motion. Mechanical energy is the sum of potential and kinetic energy and represents the energy from an object's motion and position. Energy can be transformed from one form to another, such as mechanical energy transforming to other forms like thermal, radiant, or electrical energy, which then become useful sources of energy for applications.
This document discusses different methods for separating mixtures: evaporation/heating, filtration, sieving, sifting, straining, and winnowing. It provides examples of each method and a matching exercise to test understanding of the various separation techniques.
This document defines and describes mixtures and solutions. It states that a mixture is made of two or more substances that are not chemically combined and can exist as solids, liquids, gases, or combinations. Mixtures are either heterogeneous, where the phases can be seen, or homogeneous, where they cannot. A solution is a special type of homogeneous mixture containing a solute dissolved in a solvent. It discusses how to make solutions by dissolving a solute in a solvent, and defines concepts like solubility, dilute vs concentrated solutions, saturated solutions, and super-saturated solutions.
The document discusses the 5Rs approach to waste management: reduce, reuse, recycle, repair, recover. It defines each of the 5Rs. Reduce means lessening unnecessary use of materials. Reuse means using items again, either by oneself or others. Recycle means processing waste materials to make new products. Repair means fixing broken items to reuse them. Recover means extracting energy or materials from wastes that can no longer be used. The 5Rs promote a clean environment by transforming wastes into useful materials through these various strategies.
This document provides an overview of stoichiometry concepts in chemistry. It defines stoichiometry as calculations with chemical formulas and equations. Key concepts covered include the law of conservation of mass, types of chemical reactions, anatomy of chemical equations, formula weights and molecular weights, moles, mole ratios, empirical formulas, combustion analysis, stoichiometric calculations, limiting reactants, theoretical yield, and percent yield.
The document defines stoichiometry as representing the exact mass or moles of reactants and products in a chemical reaction without waste. Stoichiometry is demonstrated through a balanced chemical equation, where the coefficients indicate the mole ratios of reactants and products. There are four types of stoichiometry problems: mole-mole, mole-mass, mass-mole, and mass-mass, which relate quantities of reactants and products by either moles or mass.
Matter can change states between solid, liquid, and gas. Water is used as an example, changing between ice, liquid water, and water vapor through the processes of melting, evaporation, and condensation. Evaporation occurs when liquid water is heated and changes into gas water vapor, while condensation is when water vapor cools and changes back into liquid water.
This document provides information about the particle nature of matter. It includes standards and objectives about demonstrating an understanding of the particle nature of matter and its properties. It discusses the key concepts of explaining the properties of solids, liquids, and gases based on how the particles are arranged and move. It also explains physical changes in these states in terms of particle arrangement and motion, and how this can be used to explain processes like melting, freezing, evaporating, and condensing.
This document summarizes the differences between physical and chemical changes in matter. It defines matter as anything that occupies space and has mass. A physical change alters the form of matter but does not create a new substance, and may be reversible. A chemical change produces a new substance that cannot be changed back to the original by ordinary means. Examples of each type of change are provided for classification exercises.
4th grade unit c ch. 11 lesson 1 what is matterhinsz
The document defines matter as anything that has mass and takes up space. It explains that matter exists in three states - solid, liquid, and gas - which are distinguished by the arrangement of their particles and how they behave. Solids have a definite shape and volume from tightly packed particles, while liquids take the shape of their container but maintain a constant volume, and gases fill their container and have particles far apart.
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 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.
This document describes the differences between freezing, melting, and evaporation. It defines these terms and explains factors that influence their rates. Freezing is a change from liquid to solid, melting is solid to liquid, and evaporation is liquid to gas below the boiling point. Temperature, size/shape, conduction, humidity, and composition affect rates. Higher temperatures speed melting and evaporation, while lower temperatures speed freezing. Smaller pieces melt/freeze faster due to more surface area. Good conductors transfer heat/cold faster. Evaporation is slowest in high humidity.
Phase changes occur when matter transitions between solid, liquid, and gas states. During a phase change, molecules either absorb or release heat energy as they speed up or slow down. There are several types of phase changes, including melting (solid to liquid), freezing (liquid to solid), vaporization/boiling (liquid to gas), evaporation, condensation, and sublimation. A key characteristic of phase changes is that the temperature remains constant despite an exchange of heat energy, as the molecules rearrange their structure.
This document discusses the three states of matter - solids, liquids, and gases. It defines each state and explains how their particle arrangements differ. Solids have a definite shape and volume, while liquids have a definite volume but not shape, and gases fill their container. The document also covers physical changes like melting, freezing, and evaporation which alter a substance's state without changing its chemical makeup. Finally, it defines mixtures as combinations of materials that retain their individual properties, and solutions as mixtures where one material disseminates evenly throughout another.
The document discusses different types of mixtures including homogeneous and heterogeneous mixtures, solution-based mixtures, and solid mixtures. Homogeneous mixtures have a uniform composition while heterogeneous mixtures have a non-uniform composition. Solution-based mixtures can be classified as true solutions, colloidal solutions, or suspensions depending on the particle size of the solute. Solid mixtures include alloys, which are homogeneous solid solutions of metals that are difficult to separate. An example given is brass, which is a homogeneous mixture of copper and zinc that takes on properties between the two metals.
If iced tea mix is stirred into water, it would form a homogeneous solution. The tea mix particles would be too small to separate out or filter from the water. Over several days, the drink would not separate into distinct layers. Solutions like this form a single phase because the solute particles are small enough to dissolve uniformly throughout the solvent.
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.
Energy is a property of objects that can be transferred or converted into different forms. There are two main types of energy: potential energy, which is the stored energy of position, and kinetic energy, which is the energy of motion. Mechanical energy is the sum of potential and kinetic energy and represents the energy from an object's motion and position. Energy can be transformed from one form to another, such as mechanical energy transforming to other forms like thermal, radiant, or electrical energy, which then become useful sources of energy for applications.
This document discusses different methods for separating mixtures: evaporation/heating, filtration, sieving, sifting, straining, and winnowing. It provides examples of each method and a matching exercise to test understanding of the various separation techniques.
This document defines and describes mixtures and solutions. It states that a mixture is made of two or more substances that are not chemically combined and can exist as solids, liquids, gases, or combinations. Mixtures are either heterogeneous, where the phases can be seen, or homogeneous, where they cannot. A solution is a special type of homogeneous mixture containing a solute dissolved in a solvent. It discusses how to make solutions by dissolving a solute in a solvent, and defines concepts like solubility, dilute vs concentrated solutions, saturated solutions, and super-saturated solutions.
The document discusses the 5Rs approach to waste management: reduce, reuse, recycle, repair, recover. It defines each of the 5Rs. Reduce means lessening unnecessary use of materials. Reuse means using items again, either by oneself or others. Recycle means processing waste materials to make new products. Repair means fixing broken items to reuse them. Recover means extracting energy or materials from wastes that can no longer be used. The 5Rs promote a clean environment by transforming wastes into useful materials through these various strategies.
This document provides an overview of stoichiometry concepts in chemistry. It defines stoichiometry as calculations with chemical formulas and equations. Key concepts covered include the law of conservation of mass, types of chemical reactions, anatomy of chemical equations, formula weights and molecular weights, moles, mole ratios, empirical formulas, combustion analysis, stoichiometric calculations, limiting reactants, theoretical yield, and percent yield.
The document defines stoichiometry as representing the exact mass or moles of reactants and products in a chemical reaction without waste. Stoichiometry is demonstrated through a balanced chemical equation, where the coefficients indicate the mole ratios of reactants and products. There are four types of stoichiometry problems: mole-mole, mole-mass, mass-mole, and mass-mass, which relate quantities of reactants and products by either moles or mass.
This document provides information on various topics in biology including populations, ATP, photosynthesis, respiration, and energy and ecosystems. It begins by defining key terms related to populations such as ecology, ecosystem, habitat, niche, biotic and abiotic factors, and types of competition. It then discusses methods for investigating populations such as quadrats, random sampling, and mark-release-recapture. Subsequent sections cover human populations, birth and death rates, ATP and energy, the light-dependent and light-independent stages of photosynthesis, aerobic and anaerobic respiration including glycolysis, the link reaction, the Krebs cycle, electron transport chain, and coenzymes. The document concludes with a brief section on energy
Stoichiometry allows us to use balanced chemical equations to determine the amounts of reactants and products involved in chemical reactions. It treats the chemical equation like a recipe, using mole ratios derived from the coefficients to solve mole-mole, mole-mass, and mass-mass problems. For example, if 2 moles of hydrogen gas react with 1 mole of oxygen gas to produce 2 moles of water, how many moles of oxygen are needed to produce 4 moles of water? By using the 1:1 mole ratio of oxygen to water given in the balanced equation, we can determine that 4 moles of oxygen are needed.
Stoichiometry is the measurement of elements and compounds involved in a chemical reaction. The document uses the example reaction of 4NH3 + 5O2 → 6H2O + 4NO to explain key stoichiometry concepts. These include: chemical formulas represent numbers of atoms and have molar masses; formulas are balanced with coefficients that represent mole ratios; and stoichiometry problems use mole ratios and molar masses to convert between grams and moles of reactants and products. Several stoichiometry practice problems are worked through as examples.
1. The document outlines key concepts and skills students should master in stoichiometry including calculating moles, mass, atoms, and molecules from balanced chemical equations and using these calculations to determine empirical formulas, molecular formulas, theoretical yields, and percent yields.
2. Example problems are provided to assess students' mastery of calculating moles from mass and vice versa, determining mass of products from reactants, calculating percent yields from experimental data, determining empirical and molecular formulas, and using balanced equations to calculate heat released.
This document discusses stoichiometry, which uses balanced chemical equations to determine amounts of reactants and products in chemical reactions. It provides examples of using mole ratios from chemical equations to solve stoichiometry problems involving moles of substances or conversions between moles and grams. The key aspects are that chemical equations provide mole ratios that can be used as conversion factors, and problems must be worked in moles since equations relate substances in moles.
This is an example of a combustion reaction. Propane (C3H8) is burning in oxygen gas (O2), producing carbon dioxide (CO2) and water vapor (H2O) as products. The balanced chemical equation is:
C3H8 + 5O2 → 3CO2 + 4H2O
This document provides guidance and questions for analyzing pictures that depict different phase changes of matter. It includes questions about observing candles, clothes drying, and identifying phase changes shown in various pictures. Students are asked to define phase changes, identify different types of phase changes like melting, evaporation, condensation, freezing and sublimation/deposition. It also discusses the importance of phase changes in daily life and provides activity directions and questions to have students illustrate and explain the particle behavior and arrangements during phase changes of ice to liquid water.
The document outlines a lesson plan about the states of matter and changes in state, including defining boiling, condensation, freezing, and melting, and explaining these processes using a particle model. It discusses boiling point and melting point, defining them and providing examples, and distinguishes between boiling and evaporation by defining evaporation, explaining it using a particle model, and listing the differences between boiling and evaporation.
This document provides study material for Class IX Science covering topics in Chemistry, Biology, and Physics. It includes key concepts, concept details, question banks, and sample papers for various chapters. The Chemistry section covers chapters on matter and its states, particle nature of matter, atoms and molecules, and structure of atoms. The Biology section addresses chapters on the fundamental unit of life, tissues, diversity in living organisms, why we fall ill, natural resources, and improvement in food resources. The Physics section focuses on chapters involving motion, force, gravitation, work, and sound. The document aims to help students study and prepare for their exams.
Chem m15 changes that matter undergoesdionesioable
This module discusses various chemical and phase changes that occur in everyday life. It is divided into four lessons: (1) Changing Phases explains the differences between melting, freezing, evaporation, condensation, sublimation and deposition; (2) When Does a Chemical Change Occur? describes the indicators of a chemical change and differentiates chemical from physical changes; (3) Types of Chemical Changes outlines four types of chemical reactions - combination, decomposition, single replacement and double displacement; (4) Chemical Changes Around Us provides examples of changes that happen in the human body during digestion and exercise as well as in cleaning products like soap. The module aims to help students understand and identify different types of changes in their environment.
1. The document outlines a microteaching lesson plan on states of matter for students.
2. It includes warm up activities like hangman to review key terms, matching properties to solids, liquids, and gases.
3. A modeling activity uses balls to demonstrate the movement and bonding of molecules in solids, liquids, and gases.
4. Students then answer questions about the models and watch a video defining additional vocabulary before consolidating their understanding.
pedagogical plan-changes in the states of matterArr Vergara
This pedagogical plan outlines the learning activities for a Science 8 class on the topic of changes in the state of matter over a one week period from November 3-7, 2014. The plan was created by teachers Richard Bon and Richard Magbatoc. It includes the content standards, learning outcomes, assessments, and learning activities for students. The learning outcomes focus on students' knowledge, skills, and affective domain regarding the states of matter. Assessment includes charts, diagrams, role-playing, interviews and a test. Learning activities engage students in simulations, discussions, poster-making and media presentations to explore the states of matter and their importance.
The document provides instructions and materials for a science lesson on phases of matter. Students are asked to complete power notes on phases of matter by answering questions about states of matter, phase changes, and energy. A list of daily assignments is also included, with the power notes and a test on phases of matter due by the end of the week.
Chapt 1 kpt of solids, liquids & gases (1)Danica Balilla
This document describes the kinetic particle theory and the changes of state between solids, liquids, and gases. It explains that all matter is made of particles in constant motion. In solids, particles are packed closely together in a fixed pattern, in liquids they are more loosely packed but still in contact, and in gases they are far apart with little attraction. Changes between these states, like melting, boiling, condensation, and freezing occur when heating or cooling causes particles to gain or lose energy and change their motion and arrangement. The document provides detailed explanations of each state and phase change using the kinetic particle theory model.
This document discusses physical and chemical changes in matter. It begins by outlining key questions about how matter changes and objectives to analyze how matter changes physically and chemically. Examples of physical changes discussed include tearing paper, molding clay, and folding a handkerchief. Chemical changes discussed include rusting iron, souring milk, and ripening fruits. A physical change alters the appearance of matter but does not change its chemical composition, while a chemical change produces new substances. The document seeks to demonstrate the difference between physical and chemical changes in various examples and situations.
PPT FOR CBSE, ICSE BOARD,
CHAPTER 1: MATTER IN OUR SURROUNDING
MATTER, PROPERTIES OF MATTER, CHARACTERISTICS OF MATTER, DIFFUSION, EVAPORATION, SUBLIMATION, KEY OINTS, NOTES.
EXPERIMENTS: PARTICLES OF MATTER ARE VERY SMALL
PARTICLES OF MATTER ARE ALWAYS MOVING
PARTICLES OF MATTER HAVE SPACE BETWEEN THEM.
POTASSIUM PERMANGANATE EXPERIMENT
The document outlines a lesson plan on phase changes of matter. Students will be divided into groups to present on different phase changes through singing, dancing, poetry, or drawing. They will learn about freezing, melting, evaporation, and condensation. The class objectives are to differentiate the four types of phase changes, illustrate how temperature affects particle motion and arrangement, and cite ways to reduce global warming and climate change.
Changes in matter.pptx 20013 2014 ( Physical and chemical change)Shirley Valera
This document discusses physical and chemical changes in matter. It begins by outlining key questions about how matter changes and objectives to analyze how matter changes physically and chemically. It then provides examples of physical changes like tearing paper, folding a handkerchief, and mixtures. Chemical changes form new substances, like rusting iron or souring milk. Finally, it defines physical changes as changes in size, shape or appearance without new substances, while chemical changes result in new substances and altered properties.
Scientifically continuous phase apersed phase Speaking Chapter Review or hono- 458 I. How is a mixture determined to be hetere ty What are the phases of matter that form gelst sols? How ndal effect gels and sols different? 3. What property of the liquids in an emulsion would work against their forming any kind of mixture?em to 4. How can you tell that a rock is a heterogeneous clation inty \'s law 5. What property do colloidal dispersions and solutions that other kinds of mixtures do not? is a col. 470 472 472 473 6. What is one property of skim milk indicating that it 31 loidal dispersion? tage by mass ve properties -point depression oint elevation 7. How might you visually tell the difference between a sion and a colloidal dispersion? 474 8. What can happen when metals with very different-sized are mixed in heterogeneous alloys? 9. Which part of a solution is the solvent? How is this inf used to classify the solution? 10. When you mix a solid and a liquid, what are two indication that a solution was formed and not a new compound? 11. What are solutions of different metals called? Why are often preferred to pure metals? 12. Why is it not possible to have a solid-in-gas solution? 13. Why is the water molecule electrically polar? 14. Why is solvation of a solute particle an important step in d 15. What kind of solvent could dissolve a nonpolar solute like sul. 16. Explain the difference between the terms soluble and solubility 18. How can you tell when a solid-in-liquid solution is saturated? solving the solute? What do we call the solution ionic solutes? process for fur? Explain your answer Explain why the solubility of gases normally decreases with ris ing temperature. 17. 19. Where does the solution process take place on a piece of a solid solute? How can you increase the rate of solution in light of this fact? 20. What instrument could be used to measure a mole of solid sol- ute particles? Why can this instrument be used? 21. Which solution would have a lower boiling point, one with 1.0 mol of solute particles or one with 2.0 mol? Explain. DS 0 22. Some conservationists are disturbed by the large amount of brine that is pumped back into the ocean by desalination plants. Why could it be a problem? What could be done to re- duce the effects of returning concentrated brine to the sea?
Solution
in case of multiple questions being posted i am allowed to answer the first question. please post one question at one time.
Answer 1)
A homogeneous mixture has the same appearence and compostion throughout. wheras a heterogenous mixture would consist of visibly different phases or substances like solid-liquid or suspensions
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a draft of a chemistry lesson on the 6- sided crystal structure of snowflakes, as related to water molecule structure and hydrogen bonding. Note that water VAPOR condenses directly into ice crystal snowflakes, with no liquid phase between the vapor and solid phases.
This document discusses physical and chemical changes in matter. It provides examples of physical changes such as melting, freezing, evaporation and condensation. Chemical changes result in new substances forming, like rusting, burning, and cooking. The key questions are how matter changes and the importance of understanding matter's properties and types. The objectives are to analyze how matter changes physically and chemically, and demonstrate ways matter undergoes property changes.
This document is a school project on matter and its states by a 9th grade student named Jyoti Kumari. It defines matter as anything that has mass and takes up space, and discusses the three states of matter - solid, liquid, and gas. It explains the characteristics of each state in terms of intermolecular forces and kinetic energy of particles. The document also covers topics like temperature, the units used to measure it, melting point, boiling point, evaporation, the factors that affect evaporation, and some sample questions related to these concepts.
1.Distinguish the three states of matter in terms of movement of the particles
2.Relate the three states of matter with energy of movement of particles in them
3. Describe the changes of state using kinetic theory
Boiling, Vaporization, Melting, Fusion, Evaporation,
Condensation, Sublimation, Deposition,Freezing
- The document outlines assignments and tasks for students related to the phases of matter. It includes completing power notes on phases of matter that are due the next day, as well as a physical properties lab, interactive reader questions, and a test on the topics.
- It also provides links and instructions for students to access online resources on the phases of matter, including descriptions of solids, liquids, gases, and plasma. A graphic organizer is assigned to illustrate the states of matter.
This document outlines the learning outcomes and content covered in a Year 9 unit on matter and atoms. It includes 10 student learning outcomes related to the particle nature of matter, states of matter, density, diffusion, the atomic model, and distinguishing between elements, compounds, and mixtures. Key concepts covered are the particle theory of matter, the three states of matter and how matter changes between states, density and factors that affect floating and sinking, conduction and convection as methods of heat transfer, the structure of the atom including subatomic particles, and writing chemical formulas.
1. The document discusses states of matter and gas laws. It provides descriptions of solids, liquids, gases and plasmas, focusing on how particle movement differs between each state.
2. Gas laws including Boyle's law and Charles' law are introduced. Boyle's law states that for a fixed amount of gas at constant temperature, volume and pressure are inversely related. Charles' law states that for a fixed amount of gas at constant pressure, volume and temperature are directly related.
3. Examples are given to demonstrate these gas laws, such as how the volume of balloons changes under differing pressures in Boyle's law experiment, and how bicycle tire pressure should be adjusted for temperature changes according to Charles' law.
This document provides information about study resources for exams, including quick study options with over 400 YouTube videos and 200 slideshare presentations covering 11 subjects, as well as comprehensive studying with 250 lessons per subject broken into modules and over 30,000 test items. Users can create an account to access these resources through a Moodle online learning platform by searching courses or topics.
This document outlines the key concepts and examples for matrices including: addition and subtraction of matrices with the same dimensions; scalar multiplication by multiplying each element of the matrix by the scalar; matrix multiplication where the number of columns of the first matrix equals the number of rows of the second matrix; determinants of 2x2 matrices; inverse matrices for non-singular 2x2 matrices; solving systems of equations using matrices; and geometric transformations using matrices including rotation, reflection, translation and examples of applying transformations.
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1) Identifying equivalent and opposite vectors in a diagram
2) Calculating components of vectors
3) Writing vector expressions in terms of other vectors
4) Illustrating vector addition and subtraction on a grid
5) Expressing vectors in terms of other vectors using properties of midpoints
6) Expressing vectors in terms of other vectors and proving collinearity using properties of parallelograms
Math unit36 contructions and enlargementseLearningJa
This document discusses geometric transformations including lines of symmetry, rotational symmetry, enlargements, and finding the scale factor and center of enlargement. Lines of symmetry and orders of rotational symmetry are identified for different shapes. Enlargements are performed using given scale factors and centers. The ratio of areas for different enlargements is calculated. Scale factors and centers of enlargement are determined for shapes.
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Math unit32 angles, circles and tangentseLearningJa
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Math unit29 using graphs to solve equationseLearningJa
This document discusses using graphs to solve equations. It covers solving simultaneous equations by graphing the lines and finding their intersection point. It also discusses graphs of quadratic, cubic, and reciprocal functions, including their key characteristics and shapes. Examples of each type of function are shown. The document concludes by discussing using graphs to find specific values or intervals related to equations.
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2) It further explores functions, mappings, and domains with examples.
3) It provides another example and asks about domain and range.
4) It covers composite functions, finding functions of other functions.
5) It introduces the concept of inverse functions.
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2. Writing coordinates of points and identifying locations
3. Plotting straight lines by connecting points
4. Plotting curves by connecting points in a smooth curve
5. Finding the midpoint of a line segment by averaging the x and y coordinates
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2. Constructing a formula to calculate an engineer's charge based on a fixed fee plus an hourly rate multiplied by hours worked.
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2. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
INTRODUCTION
Demonstration on the
different phases of matter
Procedure:
A.Place the popcorn-butter
mixture (frozen) in a beaker and
heat it until the butter melts.
B.Pour the melted mixture to
and from two beakers.
C.Heat the liquid mixture until
the popcorn begins to pop. (do
not cover the beaker)
Type your responses to each of
these questions on the next five
slides.
1.What does the butter
represent?
2.What do the popcorn kernels
represent?
3.What caused the mixture to
melt?
4.What must be done to the
mixture to cause it to solidify?
5.When the popcorn popped and
exited the beaker, what did it
represent?
2
3. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
Activity 1 – Question 1
What does the butter represent?
3
Forces holding the molecules together.Click here for possible answer.
4. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
Activity 1 – Question 2
What do the popcorn kernels represent?
4
They represent the molecules of a solid.
Click here for possible answer.
5. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
Activity 1 – Question 3
What caused the mixture to melt?
5
The solid popcorn-kernel mixture melted
because HEAT was applied to it.Click here for possible answer.
6. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
Activity 1 – Question 4
What must be done to the melted mixture to cause
it to solidify?
6
The mixture must be COOLED for it to
solidify. Click here for possible answer.
7. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
Activity 1 – Question 5
When the popcorn popped and exited the beaker,
what did it represent?
7
This represented GAS molecules leaving
the mixture.Click here for possible answer.
8. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
Objectives
As a result of this lesson, the student will be able to:
1.appreciate that matter exist in different forms.
2.classify materials into different states.
3.state the different states of matter.
4.explain comparative differences between the
different states of matter.
5.observe and explain changes between the different
states of matter.
8
9. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
What is matter?
Matter is anything that has
mass and takes up space.
9
10. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
Activity2: Classifying materials
Classify materials in the list as solid, liquid or gas.
Type your responses in the boxes below.
Click CHECK to see answers.
10
SOLID LIQUID GAS
LIST: Water, Milk, Ice, copper, Oil, , salt, Kerosene,
nitrogen, Oxygen, Mercury, Cloth, Paper, air
CHECK
11. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
Activity 2: Classifying materials
Answers to Activity: Classify materials in the list as
solid, liquid or gas.
11
SOLID LIQUID GAS
LIST: Water, Milk, Ice, Copper, Oil, , Salt, Kerosene,
Nitrogen, Oxygen, Mercury, Cloth, Paper, Air
Copper
Salt
Cloth
Paper
Ice
Water
Milk
Oil
Kerosene
Mercury
Nitrogen
Oxygen
Air
12. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
What are the different phases or
states of matter?
Matter has three states:
12
Solid
Liquid
Gas
13. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
What are the different phases or
states of matter?
Click the link below to watch a video on the different
phases of matter.http://www.youtube.com/watch?
v=s-KvoVzukHo
1.You should identify the differences between the
solids, liquids and gases in your groups.
2.Click NEXT to check if your answers coincide with
those in the table.
13
14. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
ComparingThe States Of
Matter
SOLID LIQUID GAS
Particles are tightly packed,
usually in a regular pattern.
(high density)
Particles are close together
with no regular
arrangement. (medium
density)
Particles are well separated
with no regular
arrangement.
(low density)
retains a fixed volume and
shape.
assumes the shape of the
part of the container which
it occupies.
assumes the shape and
volume of its container.
vibrate (jiggle) but generally
do not move from place to
place.
vibrate, move about, and
slide past each other.
vibrate and move freely at
high speeds.
not easily compressed. not easily compressed. compressible.
have intermolecular forces
of attraction between the
particles which are very
strong.
have intermolecular forces
of attractions between the
particles which are
relatively strong.
have intermolecular forces
of attractions between.
does not flow easily. flows easily. Flows very easily.
14
15. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
Phase Changes
15
a change from solid to liquid
a change from liquid to solid
a change from liquid to gas
a change from solid to gas or gas to solid.
a change from gas to liquid
MeltingMelting
FreezingFreezing
EvaporationEvaporation
SublimationSublimation
CondensingCondensing
16. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
Phase Changes - What happens to
matter when heated and cooled?
Watch a video on the different phases of matter and
answer corresponding questions on the next ten
slides.
Click on the link below to view the video.
http://mutuslab.cs.uwindsor.ca/schurko/animations/
waterphases/status_water.htm
16
17. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
Phase Changes
Activity 3 – Question 1
What happened to the ice when it was heated and
explain this change with respect to intermolecular
forces between molecules and distance between
molecules?Type your response in the box below
before clicking CHECK to see the answer.
17
The ice started to turn into water . The heat
weakened the intermolecular forces and caused
the molecules to move further apart.
CHECK
18. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
Phase Changes
Activity 3 – Question 2
What is the name given to this phase change?
18
Melting
CHECK
19. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
Phase Changes
Activity 3 – Question 3
What happened to the water when it was heated and
explain this change with respect to Intermolecular
forces between molecules and distance between
molecules?
19
The volume of the water decreased.
The heat weakened the intermolecular forces
and caused them to move further apart.
CHECK
20. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
Phase Changes
Activity 3 – Question 4
What is the name given to this phase change?
20
EvaporationCHECK
21. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
Phase Changes
Activity 3 – Question 5
What would happen to the water if it was cooled and
explain this change with respect to intermolecular
forces between molecules and distance between
molecules?
21
The water turned into ice. Cooling the water
increases the intermolecular forces between
molecules causing them to come closer together.
CHECK
22. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
Phase Changes
Activity 3 – Question 6
What is the name given to this phase change?
22
Freezing
CHECK
23. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
Phase Changes
Activity 3 – Question 7
What would happen to the water vapour if it cooled
and explain this change with respect to
intermolecular forces between molecules and
distance between molecules?
23
The water vapour would turn into water droplets.
Cooling increases the intermolecular forces
between molecules causing them to come closer
together.
CHECK
24. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
Phase Changes
Activity 3 – Question 8
What is the name given to this phase change?
24
Condensation
CHECK
25. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
Phase Changes
Activity 3 – Question 9
What would happened to a solid if it was heated
directly to vapour and explain this change with
respect to intermolecular forces between molecules
and distance between molecules?
25
The ice would turn to gas without passing
through the liquid state. Heating the solid would
cause the intermolecular forces between the
molecules causing them to separate very
rapidly.
CHECK
26. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
Phase Changes
Activity 3 – Question 10
What is the name given to this phase change?
26
SublimationCHECK
27. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
QUIZ
1. There are fifteen statements on the next seven
slides.
2. In Slide Show view, read each statement and
then type words that will correctly complete
each statement. For some statements, you will
need to delete the line before typing your
response.
3. Point and click CHECK below the statement to
see answers.
27
28. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
Quiz
28
1. When a solid changes directly into a gas, it is
called sublimation.
2. When a gas changes into a liquid, it is called
condensation.
CHECK
CHECK
29. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
29
3. States are also known as phases.
4. Matter in a solid state has a fixed volume and
also a fixed shape.
Quiz
CHECK
CHECK
30. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
Quiz
30
6. When a gas reaches condensation point it turns
into a liquid.
5. Matter in a liquid state has a fixed volume but does
not have a fixed shape.CHECK
CHECK
31. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
Quiz
31
8. A solid resists very strongly if you try to change its
shape.
7. A liquid can fit into a container of any size and
shape. CHECK
CHECK
32. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
Quiz
32
10.True or False? Liquids expand in all directions to
take the shape of the container it is in. False
9. The molecules in a gas spread out until they fill
the container no matter how big the container is.CHECK
CHECK
33. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
Quiz
33
12. True or False? Gases are harder to compress
than solids. False
11. True or False? Compression spreads atoms out.
False CHECK
CHECK
34. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
Quiz
34
14. In a gas the atoms are spread out the most.
13. True or False? Liquids are harder to compress
than gases. True
15. In a solid the atoms are packed the closest
together.
CHECK
CHECK
CHECK
35. OBJECTIVES
WHAT IS MATTER?
DIFFERENT PHASES
OF MATTER
COMPARING THE
DIIFERENT PHASES
OF MATTER
PHASE CHANGES
QUIZ
XX
INTRODUCTION
End of Activity
• You have reached the end of the activity.
• If you wish to review other concepts in this lesson,
go to the first slide.
• If you have finished viewing the lesson, click the
Close (X) button.
35