This document provides an introduction to chemistry, including defining chemistry and matter. It discusses classifying pure substances as elements or compounds and distinguishing pure substances from mixtures. Key topics covered include the five states of matter (solid, liquid, gas, plasma, Bose-Einstein condensate), kinetic theory, and gas laws including Boyle's law, Charles' law, and the combined gas law. Examples are provided to illustrate concepts such as physical and chemical properties, physical and chemical changes, phase changes, and factors that affect gas pressure.
This document summarizes key concepts about matter and its properties from a chemistry textbook chapter. It defines matter, mass, and weight. It describes the different states of matter and properties of substances and mixtures. It explains physical and chemical changes and how to classify them. It also outlines the concepts of elements, compounds, mixtures, and the periodic table.
This document defines key concepts about the properties of matter. It explains that matter is anything that has mass and takes up space, and can exist in solid, liquid, or gas states. Physical properties can be observed without changing a substance's identity, while chemical properties involve chemical changes forming new substances. Matter can also be classified as pure substances like elements and compounds, or mixtures that are either homogeneous solutions or heterogeneous mixtures of different phases.
Chemistry - Chapter 2 matter and changeMr. Walajtys
This document provides an overview of chapter 2 which covers properties of matter, states of matter, mixtures, elements and compounds, and chemical reactions. It defines key terms including physical and chemical properties, extensive and intensive properties, elements, compounds, mixtures, homogeneous and heterogeneous mixtures, physical and chemical changes, reactants and products. It also outlines the key objectives covered in each section and provides examples to illustrate important concepts such as the three states of matter, separating mixtures, symbols and formulas of elements, and the law of conservation of mass.
The document defines matter and describes its three common states: solid, liquid, and gas. It distinguishes between physical and chemical properties of matter, and between physical and chemical changes. It defines mixtures and pure substances, and classifies matter as homogeneous or heterogeneous. Key terms include the various states of matter, physical and chemical properties, and the classification of matter.
- Matter can exist in three main states: solid, liquid, and gas. The kinetic theory of matter explains the behavior of each state in terms of molecular motion.
- In solids, molecules are tightly packed in a fixed pattern, giving the material a definite shape and volume. In liquids, molecules can flow but have no definite shape. Gases have neither definite shape nor volume as molecules move freely.
- Changes between states are physical changes governed by temperature. Heating provides energy to overcome molecular attractions in solids (melting) and liquids (boiling), turning them to liquids and gases with increased motion. Cooling reverses these changes.
Matter is anything that has mass and takes up space. It is composed of atoms, which contain protons, neutrons, and electrons. Elements are pure substances made of only one type of atom, while compounds are made of two or more elements chemically bonded together. Mixtures contain different substances mixed together but not chemically combined. The three main states of matter are solids, liquids, and gases. Chemical and physical properties can be used to describe and identify matter.
Matter is anything that has mass and takes up space. There are three states of matter: solids have a definite shape and volume with particles close together and fixed; liquids have an indefinite shape but definite volume, taking the shape of their container with mobile but close particles; gases have an indefinite shape and volume, taking the shape and volume of their container with particles far apart and moving. Properties of matter include physical properties which are observed without changing the substance like color, shape, or boiling point, and chemical properties which are only observed when a substance interacts with another like flammability or rusting. Basic kinds of matter are elements, compounds, and mixtures.
This document discusses the properties and changes of matter. It defines matter as anything that has mass and takes up space. It distinguishes between physical and chemical properties and changes. Physical changes do not alter the chemical identity of a substance, while chemical changes produce new substances. The three common states of matter are solids, liquids, and gases. Pure substances have a uniform composition and properties, while mixtures maintain the identities of their components but are not uniform throughout.
This document summarizes key concepts about matter and its properties from a chemistry textbook chapter. It defines matter, mass, and weight. It describes the different states of matter and properties of substances and mixtures. It explains physical and chemical changes and how to classify them. It also outlines the concepts of elements, compounds, mixtures, and the periodic table.
This document defines key concepts about the properties of matter. It explains that matter is anything that has mass and takes up space, and can exist in solid, liquid, or gas states. Physical properties can be observed without changing a substance's identity, while chemical properties involve chemical changes forming new substances. Matter can also be classified as pure substances like elements and compounds, or mixtures that are either homogeneous solutions or heterogeneous mixtures of different phases.
Chemistry - Chapter 2 matter and changeMr. Walajtys
This document provides an overview of chapter 2 which covers properties of matter, states of matter, mixtures, elements and compounds, and chemical reactions. It defines key terms including physical and chemical properties, extensive and intensive properties, elements, compounds, mixtures, homogeneous and heterogeneous mixtures, physical and chemical changes, reactants and products. It also outlines the key objectives covered in each section and provides examples to illustrate important concepts such as the three states of matter, separating mixtures, symbols and formulas of elements, and the law of conservation of mass.
The document defines matter and describes its three common states: solid, liquid, and gas. It distinguishes between physical and chemical properties of matter, and between physical and chemical changes. It defines mixtures and pure substances, and classifies matter as homogeneous or heterogeneous. Key terms include the various states of matter, physical and chemical properties, and the classification of matter.
- Matter can exist in three main states: solid, liquid, and gas. The kinetic theory of matter explains the behavior of each state in terms of molecular motion.
- In solids, molecules are tightly packed in a fixed pattern, giving the material a definite shape and volume. In liquids, molecules can flow but have no definite shape. Gases have neither definite shape nor volume as molecules move freely.
- Changes between states are physical changes governed by temperature. Heating provides energy to overcome molecular attractions in solids (melting) and liquids (boiling), turning them to liquids and gases with increased motion. Cooling reverses these changes.
Matter is anything that has mass and takes up space. It is composed of atoms, which contain protons, neutrons, and electrons. Elements are pure substances made of only one type of atom, while compounds are made of two or more elements chemically bonded together. Mixtures contain different substances mixed together but not chemically combined. The three main states of matter are solids, liquids, and gases. Chemical and physical properties can be used to describe and identify matter.
Matter is anything that has mass and takes up space. There are three states of matter: solids have a definite shape and volume with particles close together and fixed; liquids have an indefinite shape but definite volume, taking the shape of their container with mobile but close particles; gases have an indefinite shape and volume, taking the shape and volume of their container with particles far apart and moving. Properties of matter include physical properties which are observed without changing the substance like color, shape, or boiling point, and chemical properties which are only observed when a substance interacts with another like flammability or rusting. Basic kinds of matter are elements, compounds, and mixtures.
This document discusses the properties and changes of matter. It defines matter as anything that has mass and takes up space. It distinguishes between physical and chemical properties and changes. Physical changes do not alter the chemical identity of a substance, while chemical changes produce new substances. The three common states of matter are solids, liquids, and gases. Pure substances have a uniform composition and properties, while mixtures maintain the identities of their components but are not uniform throughout.
No, you do not need to learn the complete periodic table right away. Focus on learning:
- The names and symbols of the most common elements like H, He, C, N, O, F, Na, Mg, Al, Si, P, S, Cl, K, Ca, etc.
- The overall layout and organization of the periodic table. Pay attention to how elements are grouped based on their properties.
- Key trends as you read across or down the periodic table, such as changes in atomic radius, electronegativity, metallic/non-metallic character.
As you study chemistry concepts involving different elements, you will naturally learn more of the periodic table over time. But it's
This document summarizes key concepts from a chapter on matter, including:
- Distinguishing between physical and chemical properties and changes
- Defining the three physical states of matter
- Explaining conservation of mass in chemical reactions
- Contrasting mixtures and pure substances
- Describing techniques to separate mixtures
- Distinguishing between elements and compounds
- Explaining the organization of the periodic table and laws of definite and multiple proportions governing compounds
1. Matter is classified as either pure substances or mixtures. Pure substances are uniform and consist of elements or compounds, while mixtures contain two or more substances mixed together.
2. Elements are the simplest pure substances made of only one type of atom, while compounds are formed by chemical bonds between different atoms in specific ratios.
3. Mixtures can be either homogeneous, with substances mixed uniformly, or heterogeneous, with distinct parts. Homogeneous mixtures include solutions and colloids, while heterogeneous mixtures have visible parts that settle over time like suspensions.
The document discusses properties of matter. It defines properties as characteristics and behaviors used to describe matter. There are two main types of properties: physical properties which can be observed without changing the substance, and chemical properties which describe a substance's ability to change into another. Matter can exist as pure substances or mixtures, and can be broken down into molecules, compounds, and atoms.
This document discusses the classification of matter. It defines mixtures as combinations of two or more substances that are not chemically bonded and can be separated by mechanical means. Mixtures can be heterogeneous, with visible components, or homogeneous, appearing uniform. Pure substances cannot be broken down and include elements, which cannot be broken down further, and compounds, made of two or more elements joined in a fixed ratio. Elements are found on the periodic table and compounds are named according to the elements present and their ratios. The properties of materials, such as their conductivity, magnetism, and position on the periodic table, determine whether they are classified as metals, nonmetals, or metalloids.
Matter is anything that has mass and takes up space. Mass refers to how heavy an object is based on the amount of particles it contains, while volume refers to the space an object occupies. Mass and volume can be measured using tools like balances and measuring cylinders. The properties of matter depend on how closely packed and attracted the particles are - solids have a fixed shape and volume as particles are tightly packed, liquids have a fixed volume but not shape as particles are moderately attached, and gases have no fixed shape or volume as particles are far apart with weak attraction.
This chapter discusses the fundamental concepts of matter and chemical changes. It defines matter as anything that has mass and takes up space, and describes its three main states as solid, liquid, and gas. Properties of matter are classified as either intensive or extensive. Physical and chemical properties are distinguished. Mixtures and compounds are introduced, where mixtures maintain the properties of the individual components and compounds exhibit new properties. Elements are defined as pure substances made of only one type of atom that cannot be broken down further by chemical means. Chemical changes, in which the reactants are converted into products with different compositions, are described along with clues that indicate a chemical change has occurred. The law of conservation of mass, whereby the mass of the reactants equals the mass
This document provides an overview of key chemistry concepts related to classifying and identifying matter. It defines pure substances, elements, compounds, mixtures and their subcategories. Physical properties like viscosity, conductivity and melting point are described, as well as common separation techniques like filtration and distillation. Chemical properties like reactivity and flammability are also covered. Key differences between physical and chemical changes are outlined. The document concludes with review questions to test understanding of these fundamental chemistry concepts.
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.
This document discusses the classification of matter into elements, compounds, and mixtures. An element consists of only one type of atom and cannot be separated into simpler substances. A compound contains two or more elements chemically bonded together and has distinct properties from its constituent elements. A mixture is not chemically combined and can be separated into its components by physical means alone. Elements, compounds, and mixtures differ in their composition and the ways they can be separated.
This document provides an overview of the classification and properties of matter. It defines pure substances as elements or compounds that contain only one type of matter and cannot be physically separated. Mixtures are physical combinations of substances that can be separated. Homogeneous mixtures appear uniform throughout while heterogeneous mixtures have distinguishable parts. Solutions are homogeneous mixtures where a solute dissolves in a solvent. The document also distinguishes between intensive properties that do not depend on amount and extensive properties that do. It describes physical properties related to physical changes and chemical properties involved in chemical changes, providing examples of each.
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.
This document discusses the classification of matter. It defines a pure substance as either an element or compound that has a definite and uniform chemical composition and physical properties. Mixtures can be either heterogeneous or homogeneous. A heterogeneous mixture has an uneven texture that is visible, while a homogeneous mixture, or solution, is completely uniform throughout. There are three main types of mixtures: solutions, suspensions, and colloids. A solution is a mixture where one or more substances are uniformly distributed in another substance. A suspension is a mixture where particles are spread through but settle over time. A colloid is between a solution and suspension, with particles that do not settle over time.
This document defines the classification of matter. There are two main categories: pure substances and mixtures. Pure substances include elements, which are made of only one type of atom, and compounds, which are two or more elements chemically bonded together. Mixtures contain two or more pure substances mixed together without chemical bonding. Mixtures can be either heterogeneous, where the parts can be seen, or homogeneous, where the parts cannot be seen. Heterogeneous mixtures are less pure than homogeneous mixtures.
The document discusses the characteristic properties of matter. It states that matter has physical properties like color, odor, and melting point that can be observed without chemical changes. It also has chemical properties like acidity and reactivity that involve chemical changes. The characteristic properties do not depend on amount or shape of the matter. Some factors like heat, pressure, and nuclear processes can change the properties.
This document provides an overview of chemistry and physics concepts related to matter. It defines matter as anything that occupies space and has mass. Key topics covered include the states of solid, liquid, and gas; chemical and physical changes; elements, compounds, and mixtures; and the composition and properties of matter. Important chemistry concepts like the law of conservation of mass and the law of definite proportions are also summarized.
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.
1. Matter can exist in three main states: solid, liquid, or gas. The state depends on temperature and pressure.
2. Solids have a definite shape and volume, liquids have a definite volume but indefinite shape, and gases have indefinite shape and volume.
3. Changes between states, like melting, freezing, evaporation, and condensation, involve changing the temperature or pressure without altering the substance's chemical properties.
Matter can be classified based on its properties, state, composition, and whether it undergoes physical or chemical changes. There are three main states of matter - solid, liquid, and gas. Matter can also exist as a plasma at very high temperatures or as a Bose-Einstein condensate at very low temperatures. Matter is either a pure substance, which has a definite composition, or a mixture of substances. Pure substances can be elements or compounds. Chemical changes result in new substances forming, while physical changes do not alter the composition of the matter. The law of conservation of mass states that mass is neither created nor destroyed in physical and chemical changes.
This document provides an overview of key concepts in matter and changes of state from a chemistry textbook. It defines matter as anything that has mass and takes up space. Properties of matter are classified as either extensive, depending on amount, or intensive, not depending on amount. The three main states of matter are solids, liquids, and gases. Mixtures can be either heterogeneous, with unevenly distributed components, or homogeneous, with uniformly distributed components. During chemical changes, the composition of reactants changes as they are converted into different products.
This document discusses the basics of matter and chemistry. It defines matter as anything that has mass and volume, and distinguishes elements from compounds. Elements are made of atoms with a specific number of protons, while compounds are formed by two or more elements chemically bonded together. Chemical formulas use symbols to represent elements and subscripts to show the number of atoms in molecules and compounds. The document also categorizes materials as either pure substances like elements and compounds, or mixtures which combine two or more pure substances but retain their individual properties.
No, you do not need to learn the complete periodic table right away. Focus on learning:
- The names and symbols of the most common elements like H, He, C, N, O, F, Na, Mg, Al, Si, P, S, Cl, K, Ca, etc.
- The overall layout and organization of the periodic table. Pay attention to how elements are grouped based on their properties.
- Key trends as you read across or down the periodic table, such as changes in atomic radius, electronegativity, metallic/non-metallic character.
As you study chemistry concepts involving different elements, you will naturally learn more of the periodic table over time. But it's
This document summarizes key concepts from a chapter on matter, including:
- Distinguishing between physical and chemical properties and changes
- Defining the three physical states of matter
- Explaining conservation of mass in chemical reactions
- Contrasting mixtures and pure substances
- Describing techniques to separate mixtures
- Distinguishing between elements and compounds
- Explaining the organization of the periodic table and laws of definite and multiple proportions governing compounds
1. Matter is classified as either pure substances or mixtures. Pure substances are uniform and consist of elements or compounds, while mixtures contain two or more substances mixed together.
2. Elements are the simplest pure substances made of only one type of atom, while compounds are formed by chemical bonds between different atoms in specific ratios.
3. Mixtures can be either homogeneous, with substances mixed uniformly, or heterogeneous, with distinct parts. Homogeneous mixtures include solutions and colloids, while heterogeneous mixtures have visible parts that settle over time like suspensions.
The document discusses properties of matter. It defines properties as characteristics and behaviors used to describe matter. There are two main types of properties: physical properties which can be observed without changing the substance, and chemical properties which describe a substance's ability to change into another. Matter can exist as pure substances or mixtures, and can be broken down into molecules, compounds, and atoms.
This document discusses the classification of matter. It defines mixtures as combinations of two or more substances that are not chemically bonded and can be separated by mechanical means. Mixtures can be heterogeneous, with visible components, or homogeneous, appearing uniform. Pure substances cannot be broken down and include elements, which cannot be broken down further, and compounds, made of two or more elements joined in a fixed ratio. Elements are found on the periodic table and compounds are named according to the elements present and their ratios. The properties of materials, such as their conductivity, magnetism, and position on the periodic table, determine whether they are classified as metals, nonmetals, or metalloids.
Matter is anything that has mass and takes up space. Mass refers to how heavy an object is based on the amount of particles it contains, while volume refers to the space an object occupies. Mass and volume can be measured using tools like balances and measuring cylinders. The properties of matter depend on how closely packed and attracted the particles are - solids have a fixed shape and volume as particles are tightly packed, liquids have a fixed volume but not shape as particles are moderately attached, and gases have no fixed shape or volume as particles are far apart with weak attraction.
This chapter discusses the fundamental concepts of matter and chemical changes. It defines matter as anything that has mass and takes up space, and describes its three main states as solid, liquid, and gas. Properties of matter are classified as either intensive or extensive. Physical and chemical properties are distinguished. Mixtures and compounds are introduced, where mixtures maintain the properties of the individual components and compounds exhibit new properties. Elements are defined as pure substances made of only one type of atom that cannot be broken down further by chemical means. Chemical changes, in which the reactants are converted into products with different compositions, are described along with clues that indicate a chemical change has occurred. The law of conservation of mass, whereby the mass of the reactants equals the mass
This document provides an overview of key chemistry concepts related to classifying and identifying matter. It defines pure substances, elements, compounds, mixtures and their subcategories. Physical properties like viscosity, conductivity and melting point are described, as well as common separation techniques like filtration and distillation. Chemical properties like reactivity and flammability are also covered. Key differences between physical and chemical changes are outlined. The document concludes with review questions to test understanding of these fundamental chemistry concepts.
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.
This document discusses the classification of matter into elements, compounds, and mixtures. An element consists of only one type of atom and cannot be separated into simpler substances. A compound contains two or more elements chemically bonded together and has distinct properties from its constituent elements. A mixture is not chemically combined and can be separated into its components by physical means alone. Elements, compounds, and mixtures differ in their composition and the ways they can be separated.
This document provides an overview of the classification and properties of matter. It defines pure substances as elements or compounds that contain only one type of matter and cannot be physically separated. Mixtures are physical combinations of substances that can be separated. Homogeneous mixtures appear uniform throughout while heterogeneous mixtures have distinguishable parts. Solutions are homogeneous mixtures where a solute dissolves in a solvent. The document also distinguishes between intensive properties that do not depend on amount and extensive properties that do. It describes physical properties related to physical changes and chemical properties involved in chemical changes, providing examples of each.
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.
This document discusses the classification of matter. It defines a pure substance as either an element or compound that has a definite and uniform chemical composition and physical properties. Mixtures can be either heterogeneous or homogeneous. A heterogeneous mixture has an uneven texture that is visible, while a homogeneous mixture, or solution, is completely uniform throughout. There are three main types of mixtures: solutions, suspensions, and colloids. A solution is a mixture where one or more substances are uniformly distributed in another substance. A suspension is a mixture where particles are spread through but settle over time. A colloid is between a solution and suspension, with particles that do not settle over time.
This document defines the classification of matter. There are two main categories: pure substances and mixtures. Pure substances include elements, which are made of only one type of atom, and compounds, which are two or more elements chemically bonded together. Mixtures contain two or more pure substances mixed together without chemical bonding. Mixtures can be either heterogeneous, where the parts can be seen, or homogeneous, where the parts cannot be seen. Heterogeneous mixtures are less pure than homogeneous mixtures.
The document discusses the characteristic properties of matter. It states that matter has physical properties like color, odor, and melting point that can be observed without chemical changes. It also has chemical properties like acidity and reactivity that involve chemical changes. The characteristic properties do not depend on amount or shape of the matter. Some factors like heat, pressure, and nuclear processes can change the properties.
This document provides an overview of chemistry and physics concepts related to matter. It defines matter as anything that occupies space and has mass. Key topics covered include the states of solid, liquid, and gas; chemical and physical changes; elements, compounds, and mixtures; and the composition and properties of matter. Important chemistry concepts like the law of conservation of mass and the law of definite proportions are also summarized.
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.
1. Matter can exist in three main states: solid, liquid, or gas. The state depends on temperature and pressure.
2. Solids have a definite shape and volume, liquids have a definite volume but indefinite shape, and gases have indefinite shape and volume.
3. Changes between states, like melting, freezing, evaporation, and condensation, involve changing the temperature or pressure without altering the substance's chemical properties.
Matter can be classified based on its properties, state, composition, and whether it undergoes physical or chemical changes. There are three main states of matter - solid, liquid, and gas. Matter can also exist as a plasma at very high temperatures or as a Bose-Einstein condensate at very low temperatures. Matter is either a pure substance, which has a definite composition, or a mixture of substances. Pure substances can be elements or compounds. Chemical changes result in new substances forming, while physical changes do not alter the composition of the matter. The law of conservation of mass states that mass is neither created nor destroyed in physical and chemical changes.
This document provides an overview of key concepts in matter and changes of state from a chemistry textbook. It defines matter as anything that has mass and takes up space. Properties of matter are classified as either extensive, depending on amount, or intensive, not depending on amount. The three main states of matter are solids, liquids, and gases. Mixtures can be either heterogeneous, with unevenly distributed components, or homogeneous, with uniformly distributed components. During chemical changes, the composition of reactants changes as they are converted into different products.
This document discusses the basics of matter and chemistry. It defines matter as anything that has mass and volume, and distinguishes elements from compounds. Elements are made of atoms with a specific number of protons, while compounds are formed by two or more elements chemically bonded together. Chemical formulas use symbols to represent elements and subscripts to show the number of atoms in molecules and compounds. The document also categorizes materials as either pure substances like elements and compounds, or mixtures which combine two or more pure substances but retain their individual properties.
This document is a chapter summary about classifying and identifying the properties of matter. It discusses that matter can be classified as pure substances, which are either elements or compounds, or as mixtures, which can be homogeneous or heterogeneous. Mixtures are further classified as solutions, suspensions, or colloids based on particle size. The chapter also describes various physical properties that are used to identify materials, such as viscosity, conductivity, density, and melting and boiling points. It explains how physical properties are used to separate mixtures using filtration and distillation methods. Finally, it defines chemical properties and chemical changes, noting evidence like color change, gas production, and precipitate formation.
1. Matter is anything that occupies space and can be measured. Examples of matter include rocks, water, animals, plants and planets.
2. Properties of matter include extensive properties like mass, volume and length, which depend on the amount of matter present, and intensive properties like density and boiling point, which do not depend on amount.
3. Matter can be measured using units like meters (m) for length, square meters (m2) for area, cubic meters (m3) for volume, liters (L) for capacity, grams (g) and kilograms (kg) for mass, and degrees Celsius (°C) for temperature.
The document discusses the benefits of exercise for mental health. Regular physical activity can help reduce anxiety and depression and improve mood and cognitive function. Exercise causes chemical changes in the brain that may help protect against mental illness and improve symptoms.
The document discusses various topics related to matter and chemical changes. It defines elements and compounds, explains that compounds can undergo chemical changes while elements cannot, and states that the law of conservation of mass means the mass of reactants equals the mass of products in a chemical reaction. It also distinguishes physical and chemical changes, noting that only chemical changes alter the composition of matter.
Matter can be classified as either pure substances or mixtures. Pure substances have a fixed composition and include elements, which contain only one type of atom, and compounds, which contain two or more elements in a fixed ratio. Mixtures have a variable composition and include homogeneous mixtures, which are uniform throughout, and heterogeneous mixtures, where the distinct components can be seen. The document provides examples of elements, compounds, and mixtures to illustrate these classifications.
Here are brief explanations of the key concepts:
- The composition of an element is fixed because elements are pure substances made of only one type of atom.
- The composition of a compound is also fixed, but compounds contain two or more elements combined in a fixed ratio.
- Properties of mixtures can vary because mixtures are combinations of two or more substances that are not chemically combined. Their compositions are not fixed.
- Mixtures can be classified as solutions, suspensions, or colloids based on whether the mixed substances are uniformly dispersed (solutions), settle over time (suspensions), or are dispersed with particles too small to settle but large enough to scatter light (colloids).
- Every sample of
The document discusses the structure of atoms and isotopes. It begins by defining matter and the particle theory of matter. It then explains that atoms are made up of protons, neutrons and electrons. The atomic structure of various elements is discussed through their electron configurations. Isotopes are then introduced as atoms of the same element that have the same number of protons but different numbers of neutrons. Examples of isotopes including hydrogen and oxygen isotopes are provided.
This document provides an overview of introductory chemistry concepts. It begins by defining chemistry and its major areas of study. It then defines matter and classifies pure substances as elements or compounds. Elements are substances that cannot be broken down further, while compounds are formed by combining two or more elements. Mixtures are combinations of pure substances that can be either heterogeneous or homogeneous. The document also discusses physical and chemical properties of matter and how to distinguish between physical and chemical changes. It introduces the five states of matter and uses kinetic theory to explain the behavior of gases, liquids, and solids. Key concepts covered include phase changes, pressure, and gas laws like Boyle's, Charles', and the combined gas law.
The document discusses the key properties and characteristics of matter. It defines matter as anything that has mass and takes up space. It describes the three main states of matter - solids, liquids, and gases - and their properties. It also discusses physical and chemical properties, mixtures and compounds, and how chemical and physical changes can alter matter.
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 key concepts about matter and chemical changes from a chemistry textbook. It defines matter and its three main states (solid, liquid, gas). It describes properties as either extensive (depending on amount) or intensive (depending on type). It differentiates between physical and chemical changes, elements and compounds, and mixtures and pure substances. It outlines clues that indicate a chemical change has occurred and introduces the law of conservation of mass.
This document provides an overview of chemistry, including what it is, different types of chemistry, the scientific method, matter and its properties, energy, and chemical reactions. It defines chemistry as the study of matter, its composition and properties. It describes the major branches of chemistry and explains key concepts like the scientific method, states of matter, physical and chemical properties, and the conservation of mass and energy in chemical changes.
This document provides an overview of chemistry, including what it is, different types of chemistry, the scientific method, matter and its properties, energy, and chemical reactions. It defines chemistry as the study of matter, its composition and properties. It describes the major branches of chemistry and explains key concepts like the scientific method, states of matter, physical and chemical properties, and the conservation of mass and energy in chemical changes.
This document provides an overview of chemistry, including what it is, different types of chemistry, the scientific method, matter and its properties, energy, and chemical reactions. It defines chemistry as the study of matter, its composition and properties. It describes the major branches of chemistry and explains key concepts like the scientific method, states of matter, physical and chemical properties, and the conservation of mass and energy in chemical changes.
This document provides an overview of chemistry, including what it is, different types of chemistry, the scientific method, matter and its properties, energy, and chemical reactions. It defines chemistry as the study of matter, its composition and properties. It describes the major branches of chemistry and explains key concepts like the scientific method, properties of matter, different states of matter, physical and chemical changes, types of energy, and conservation of mass and energy.
This document provides an overview of chemistry, including what it is, different types of chemistry, the scientific method, matter and its properties, energy, and chemical reactions. It defines chemistry as the study of matter, its composition and properties. It describes the major branches of chemistry and explains key concepts like the scientific method, states of matter, physical and chemical properties, and the conservation of mass and energy in chemical changes.
This document provides an overview of chemistry, including what it is, different types of chemistry, the scientific method, matter and its properties, energy, and chemical reactions. It defines chemistry as the study of matter, its composition and properties. It describes the major branches of chemistry and explains key concepts like the scientific method, states of matter, physical and chemical properties, and the conservation of mass and energy in chemical changes.
This document provides an overview of chemistry, including what it is, different types of chemistry, the scientific method, matter and its properties, energy, and chemical reactions. It defines chemistry as the study of matter, its composition and properties. It describes the major branches of chemistry and explains key concepts like the scientific method, states of matter, physical and chemical properties, and the conservation of mass and energy in chemical changes.
This document provides an overview of chemistry, including what it is, different types of chemistry, the scientific method, matter and its properties, energy, and chemical reactions. Chemistry is the study of matter - its composition, properties, and the changes it undergoes. There are different types including analytical, inorganic, organic, and biochemistry. The scientific method is used to solve problems through observation, hypothesis, experimentation, and developing theories. Matter has mass and takes up space, and can be elements, compounds, or mixtures. Energy powers chemical and physical changes and exists in different forms like potential, kinetic, heat, and chemical. Chemical reactions occur when substances are transformed into new substances.
This document provides an overview of chemistry, including what it is, different types of chemistry, the scientific method, matter and its properties, energy, and chemical reactions. It defines chemistry as the study of matter, its composition and properties. It describes the major branches of chemistry and explains key concepts like the scientific method, states of matter, physical and chemical properties, and the conservation of mass and energy in chemical changes.
This document provides an overview of chemistry, including what it is, different branches of chemistry, the scientific method, states and types of matter, physical and chemical changes, energy, and chemical reactions. It defines chemistry as the study of matter, its composition and properties. It describes the major topics in chemistry including elements, compounds, mixtures, solutions, states of matter, energy, and chemical reactions.
This document provides an overview of chemistry, including what it is, different branches of chemistry, the scientific method, states and types of matter, physical and chemical changes, energy, and chemical reactions. It defines chemistry as the study of matter, its composition and properties. It describes the major topics in chemistry including elements, compounds, mixtures, solutions, states of matter, energy, and chemical reactions.
This document provides an overview of chemistry, including what it is, different types of chemistry, the scientific method, matter and its properties, energy, and chemical reactions. It defines chemistry as the study of matter, its composition and properties. It describes the major branches of chemistry and explains key concepts like the scientific method, states of matter, physical and chemical properties, and the conservation of mass and energy in chemical changes.
This document provides an overview of chemistry, including what it is, different types of chemistry, the scientific method, matter and its properties, energy, and chemical reactions. It defines chemistry as the study of matter, its composition and properties. It describes the major branches of chemistry and explains key concepts like the scientific method, states of matter, physical and chemical properties, and the conservation of mass and energy in chemical changes.
This document provides an overview of chemistry, including what it is, different branches of chemistry, the scientific method, properties and states of matter, mixtures and solutions, energy, and chemical reactions. It defines chemistry as the study of matter, its composition and properties. It describes the major topics in chemistry including elements, compounds, mixtures, physical and chemical properties, phases of matter, and energy transformations.
This document provides an overview of chemistry, including what it is, different types of chemistry, the scientific method, matter and its properties, energy, and chemical reactions. It defines chemistry as the study of matter, its composition and properties. It describes the major branches of chemistry and explains key concepts like the scientific method, states of matter, physical and chemical properties, and the conservation of mass and energy in chemical changes.
This document provides an overview of chemistry, including what it is, different types of chemistry, the scientific method, matter and its properties, energy, and chemical reactions. It defines chemistry as the study of matter, its composition and properties. It describes the major branches of chemistry and explains key concepts like the scientific method, states of matter, physical and chemical properties, and the conservation of mass and energy in chemical changes.
2. ObjectivesObjectives
Define chemistry
Define matter
Classifying pure substances as elements or
compounds
Describe the characteristics of and element and
compound
Distinguish pure substance from mixtures
Classify mixtures as solutions, suspensions, or
colloids
3. Introduction to ChemistryIntroduction to Chemistry
Definition
- study of matter and the changes it undergoes
Divided into five major areas
- Organic: study of essential all substances
containing carbon
- Inorganic: study of substances that do not contain
carbon
- Analytical: study of the composition of
substances
4. Introduction to Chemistry Cont.Introduction to Chemistry Cont.
- Physical: study of theories and experiments that
describe the behavior of chemicals
- Biochemistry: study of the chemistry of living
organisms
6. Pure SubstancesPure Substances
Matter that always has the same composition
ex. table salt, sugar, sulfur,
- fixed, uniform composition: every sample of a
given substance has the same properties
- 2 categories
- elements
ex. H, O, Si, C
- compounds
ex. NaCl, KBr
7. ElementsElements
- a substance that can not be broken down into
simpler substances
- 119 elements
- 88 are found naturally, about 90%
- not equally common
- others are made in laboratories
Why?
- heaviest elements are too unstable to occur
naturally
- elements heavier then hydrogen are manufactured
in stars, enormous temperatures and pressures cause
hydrogen atoms to fuse into more complex elements
8. Elements Cont.Elements Cont.
- exception of hydrogen, and a few other trace
elements are all remnants of stars that exploded long
before our solar system came into existence
- these remnants are the building of all matter
- each element is represented by a symbol
ex.
9. Elements ContElements Cont……
- majority of the elements are not found in abundance
- some are exceedingly rare
- only a dozen or so make up everyday things
- primarily: carbon, hydrogen, oxygen, nitrogen
10. CompoundsCompounds
Definition
- a substance made of atoms of more than one
element bound together
- unique and different from the elements it contains
ex. Water: (H2O) liquid, clear, non toxic
hydrogen & oxygen
- gas, colorless - gas, colorless
- non toxic - non toxic
- volatile
11. Classifying Matter Cont.Classifying Matter Cont.
Mixtures
- combination of more than one pure substance
ex. salsa, air, salad, pepper
Two types of mixtures
- heterogeneous
- homogenous
12. Classifying Mixtures Cont.Classifying Mixtures Cont.
Heterogeneous
- not uniform in composition
- different components can be seen as individual
substances
ex: Oj: juice & water, pulp
Suspension (Heterogeneous)
- mixtures that separates into layers over time
- suspended particles settle out of solution or are
trapped by filter
- larger particles can scatter light: will be cloudy
ex. O.J., sand/water, muddy water
13. Classifying Matter Cont.Classifying Matter Cont.
Homogenous
- substances are so evenly distributed that it is
difficult to distinguish one substance from another
-appears to contain only one substance
ex. stainless steel: iron, nickel, chromium
- 3 categories
- solutions, and collides
- based upon the size of the largest
particles
14. Classifying Matter Cont.Classifying Matter Cont.
Solutions (Homogenous)
- mixtures that forms when substances dissolve and
form a homogenous solution
- particles are too small to settle, scatter light, or be
trapped
ex. salt water, windshield wiper fluid
Colloids (Homogeneous)
- mixtures that contain some particles that are
intermediate in size between the small particles in a
solution and the larger particles in a suspension
- do not separate into layers
ex. homogenized milk vs. cow’s milk, fog
15. ObjectivesObjectives
Describe the physical and chemical properties of
matter
Describe the clues that indicates that a chemical
change is taking place
Distinguish chemical and physical changes
16. Properties of MatterProperties of Matter
Two types of properties
- chemical and physical
Which ones do you think are physical properties?
Evolution
of a gas : Chemical
Color Change:
Cutting: Chemical
Physical
17. Physical Properties of MatterPhysical Properties of Matter
Definition
- a characteristic of a substance that can be observed
or measured without changing the composition of
the substance
ex. viscosity, conductivity, malleability
melting point, boiling point
- remain the same for all pure substances
ex. water always boils at 100 and freezes at 0
18. Physical Properties of MatterPhysical Properties of Matter
Viscosity
- the tendency of a liquid to keep from flowing
- the greater the viscosity, the slower the liquid
moves
ex. oil vs. honey
- will usually decrease when it is heated
Conductivity
- materials ability to allow heat to flow
ex. metal vs. wood
19. Physical Properties of MatterPhysical Properties of Matter
Malleability
- ability of a solid to be hammered without
shattering
ex. silver vs. glass
Hardness
- can be compared by examining which object
scratched
ex. knife against copper sheet
copper sheet will scratch
20. Physical Properties of MatterPhysical Properties of Matter
Melting/Boiling points
- Melting pt.: temperature at which a substance
changes from a solid to liquid
ex. ice cube at room temperature
- Boiling Pt.: temperature at which a substance boils
ex. water boils at 100o
C
Density
- the ratio of a materials mass to its volume
- D= M/V
21. Physical Properties of MatterPhysical Properties of Matter
What do we use physical properties for?
- identify a material
ex. crime scene, paint chips
- chose a material for a specific purpose
ex. construction worker might wear a titanium
ring instead of a gold ring for scratching
- separate the substances in a mixture
filtration: separates materials based on size
22. Physical Properties of MatterPhysical Properties of Matter
distillation: separates the substances in
a solutions based on the boiling points
When does a physical change occur?
- some of the properties of the material have
changed, but the material remains the same
ex. tearing/crumpling a piece of paper
cutting your hair
**ask yourself is it still the SAME substance**
23. Chemical Properties of MatterChemical Properties of Matter
Definition
- any ability to produce a change in the composition
of matter
- can only be observed when the substances in a
sample of matter are changing into a different
substance
Flammability
- material’s ability to burn in the presence of oxygen
ex. newspaper, gasoline
24. Chemical Properties of MatterChemical Properties of Matter
Cont.Cont. Reactivity
- describes how readily a substance combines
chemically with other substances
ex. iron turns to rust in the presence of
oxygen
25. Chemical Changes of MatterChemical Changes of Matter
Chemical Change
- a change that produces one or more new
substances
ex. ripening fruit: banana
- all chemical changes are accompanied by changes
in energy, hence either endothermic or exothermic
- atoms rearrange during chemical change, forming
and breaking bonds, its new arrangement of atoms
results in a material completely different from the
starting material
26. Chemical Changes Cont.Chemical Changes Cont.
How do you know if a chemical changed occurred?
- look for evidence
Evidence of a chemical change
- the evolution of a gas
- the formation of a precipitate
- the evolution or absorption of heat
- emission of light
- color change in the reaction system
27. Chemical vs. Physical ChangeChemical vs. Physical Change
How do you know if it’s a physical or chemical
change?
- can be very tricky, they will both change some of
the substances attributes
- a chemical change will produce a new substance
ex. burning paper
28. ObjectivesObjectives
Describe the five states of matter
Classify materials as solid, liquids, or gases
Explain the behavior of gases, liquids, and solids,
using kinetic theory
29. States of MatterStates of Matter- one of the most important ways we can describe
matter is by its phase, also known as its state
- 5 states of matter, solid, liquid, gas, plasma, BEC
(Bose-Eistein condensate)
Solid: definite shape and volume and is not readily
deformed
ex. rock
Liquid: definite volume but indefinite shape
ex. milk may take the shape of its carton or the
shape of a bowl, but its volume remains the
same
30. States of Matter Cont.States of Matter Cont.
Gas: a diffuse, having neither definite shape or
volume
ex. compressed air may assume the volume
and shape of a toy balloon or an
automobile
tire
31. States of Matter Cont.States of Matter Cont.
Plasma
- state of matter in which atoms have been striped of
their electrons
- exist at extremely high temperatures
Bose-Einstein condensate (BEC)
- exists at extremely low temperatures –2730
C
- behave as though they were a single particle
32. States of Matter Cont.States of Matter Cont.
Solid matter
- the attractions among the submicroscopic
particles are strong enough to hold them together in
some fixed 3D arrangement
ex.
- particles are able to vibrate about their fixed
positions, but they can not move past one another,
adding heat causes these vibrations to increase
33. States of Matter Cont.States of Matter Cont.
Liquid matter
- once a certain temperature is achieved, (they are
rapid enough to disrupt the fixed arrangement)
particles then slip past one another and tumble
around much like a bunch of marbles held within a
plastic bag --- this is now the liquid phase of matter,
and it is the mobility of submicroscopic particles
that give rise to the liquids fluid character, taking
shape of its container
- can be heated so that it transforms to the gas phase
Gas
- phase in which the submicroscopic particles are
widely separated due to high speeds
34. States of Matter Cont.States of Matter Cont.
- occupies much more volume than it does in its solid
or liquid phase
Why?
- explains how gases are easily compressed
ex. air tanks for scuba diving
- move at high speeds, but they do not drift very far
because they are constantly hitting one another
ex. Baking cookies, BBQ
35. What Will the Subatomic ParticlesWhat Will the Subatomic Particles
Look like at each StateLook like at each State
Solid
Liquid
Gas
36. Characteristics of Phase ChangesCharacteristics of Phase Changes
Phase Change
- the reversible physical change that occurs when a
substances changes from one state of matter to
another
ex. Ice ----- water
- energy is either absorbed or released
- absorbed: endothermic
- released: exothermic
Common phase changes
- freezing, melting, vaporization, condensation,
sublimation, deposition
37. Kinetic TheoryKinetic Theory
Kinetic Theory
- all particles of matter are in constant motion
ex. a pitched baseball
Kinetic Energy (KE)
- the energy an object has due to it’s motion
- faster the object moves the more KE
38. Kinetic Energy RelationshipsKinetic Energy Relationships
Kinetic Energy relationship to
Temperature
- interdependent
- as temperature increases KE increases
Mass
- interdependent
- greater the mass the greater the KE
39. MeltingMelting
Melting
- molecules are becoming less orderly
- subatomic level: molecules gain energy and begin
to vibrate
- when all molecules have enough energy to move
melting is complete
ex. Ice (solid) Water (liquid)
Water molecules keep the molecules in a
fixed position. Heat flows from surrounding
area increasing the KE, therefore the
temperature
40. FreezingFreezing
Freezing
- molecules are becoming more orderly
- subatomic level: molecules lose energy and begin
to slow down
- when all molecules are have been drawn into an
orderly arrangement, freezing is complete
ex. water (liquid) ice (solid)
molecules posses energy and are able
to move, as the temperature decreases
the KE decreases, slowing down molecules
42. Vaporization Cont.Vaporization Cont.
Boiling
- takes place throughout a liquid (boiling pt)
- depends upon the atmospheric pressure
- will differ for all substances
ex. pot of water on the stove In Phoenix vs.
Flagstaff
Evaporation
- takes place at the surface of a liquid, occurs at
temperatures below the boiling pt.
ex. puddles after a rainy day within a few
hours may disappear
43. CondensationCondensation
Definition
- phase change in which a substance changes from a
gas/vapor to a liquid
- exothermic (gives off heat)
ex. morning dew on grass
water on mirror after a shower
44. SublimationSublimation
Definition
- phase change in which a substance changes from a
solid to a gas/vapor without changing into a liquid
first
- endothermic (absorbs heat)
ex. dry ice (solid carbon dioxide) vapors
form clouds
45. DepositionDeposition
Definition
- a gas/vapor changes directly into a solid without
first changing to a liquid
ex. dry ice: solid carbon dioxide
water vapor ice
when cold air hits window
46. PressurePressure
Pressure
- the result of a force distributed over an area
ex. two people of differing weight sit on a
padded booth (imprint left behind)
SI unit
- N/m2
:due to force and area
- pascal (Pa)
Factors
- temperature
- volume
- number of particles
47. Factors Affecting PressureFactors Affecting Pressure
Temperature
- increase in temperature increase in pressure
ex. tires of a car after traveling a distance
* Increase in temperature = increase in KE, the
movement of particles = more collision = more
pressure
Volume
- reducing volume increases pressure
ex. empty water bottled: crush it, unscrew the lid
just enough to let air seep out, cap will shoot off
48. Factors Affecting Pressure Cont.Factors Affecting Pressure Cont.
Number of particles
- increasing the number of particles increases the
pressure
ex. blowing up a balloon: too much air and it
will burst
49. CharlesCharles’’s Laws Law
The volume of a gas is directly proportional to its
temperature in kelvins if the pressure and the
number of particles of the gas are constant
- the volume of gas increases at the same rate as the
temperature of gas
- extended this graph until –273.15o
C, absolute zero
= 0 K
Mathematical Expression
V1
= V2
T1 = T2 Temperature must be in kelvins
50. BoyleBoyle’’s Laws Law
The volume of a gas is inversely proportional to its
pressure if the temperature and the number of
particles are constant.
Mathematically
P1V1 = P2V2
(Before) (After)
51. Combined Gas LawCombined Gas Law
Relationship of Boyle’s and Charles’s Law:
- when the number of particles are constant the
relationship among temperature, volume, pressure
Mathematically
P1V1 = P2V2
T1 T2
52. Gas Law ProblemsGas Law Problems
A cylinder that contains air at a pressure of 100 kPa
has a volume of 0.75 L. The pressure is increased to
300 kPa. The temperature does not change. Find
the new volume of air?
- identify formula: P1V1 = P2V2
T1 T2
- get rid of constant variables (temperature)
P1V1 = P2V2
-solve for V2
- 100 kPa x 0.75 L = 0.25 L