Name: Date: Physical Science Period: Chapter 2: Properties of Matter Student Outline GA Performance Standards SPS1. Students will investigate our current understanding of the atom. SPS2. Students will explore the nature of matter, its classifications, and its system for naming types of matter. SPS6. Students will investigate the properties of solutions. 2.1 Classifying Matter is the study of what things are made of and how things change. is anything that has mass and takes up space. Matter is made up of., sound and are NOT matter. A. Pure Substances is matter that always has exactly the same composition, or simply a substance. Examples of pure substances:, Every sample of a given substance has the same properties because a substance has a, uniform. Substances can be classified into two categories elements and compounds. B. Elements is a substance that be broken down into simpler substances. is the smallest particle of an element. An element has a composition because it contains only type of atom. Examples of Elements,, C. Compounds is a substance that is made from two or more simpler substances and can be broken down into those simpler substances. The properties of a compound differ from those of the substance from which it is made. A always contains two or more elements joined in a fixed Example: = + D. Mixtures Mixtures tend to retain some of the of their individual substances. The properties of a mixture can because the composition of a mixture is not fixed. Mixtures can be classified by how well the parts of the mixture are throughout the mixture. Can be or. 1. Heterogeneous Mixture o Parts of the mixture are noticeably from one another. Ex: 2. Homogeneous Mixture o The substances are distributed and it is difficult to distinguish one substance in the mixture from another. Ex:
E. Solutions, Suspensions, and Colloids The size of the particles in a mixture has an effect on the properties of the mixture. Based on the size of its largest particles, a mixture can be classified as a solution, a suspension, or a colloid. 1. Solutions o Placing a spoonful of sugar in a glass of hot water and stirring will dissolve the sugar and make a homogeneous mixture. o forms when a substance dissolves and forms a homogeneous mixture. o Example: or tea 2. Suspensions o is a heterogeneous mixture that separates into layers over time. o Examples: salad dressing, and o Because larger particles can light in all direction suspensions are. 3. Colloids o contains some particles that are intermediate in size between the small particles in a solution and the larger particles in a suspension. o Milk is a mixture of substances including water, sugar, proteins and fats. o Colloids do separate into. o is a colloid of water droplets in air. Summary:
2.2 Physical Properties A. Examples of Physical Properties is any characteristic of a material that can be observed or measured without changing the composition of the substances in the material. Viscosity, conductivity, malleability, hardness, melting point, boiling point, and density are examples of physical properties. 1. Viscosity o is the tendency of a liquid to keep from flowing (its resistance to flowing). o The the viscosity, the the liquid moves. o Viscosity will when it is. o Ex: honey and corn syrup have viscosity and vinegar has viscosity. 2. Conductivity o is a material s ability to allow heat to flow. o Metals have high conductivity and are o will not conduct heat and it makes a great spoon. 3. Malleability o is the ability of a solid to be hammered into sheets (or shapes) without shattering. o Most are malleable. o Solids that when struck are. 4. Hardness o One way to compare the hardness of two materials is to see which of the materials can the other. o is the hardest known material. 5. Melting and Boiling Points o is the temperature at which a substance changes from solid to liquid. o Ex: Melting point of water is 0C o is the temperature at which a substance boils o Ex: Boiling point of water is 100C 6. Density o is the ratio of the mass of a substance to its volume. o Density can be used to test the of a substance. Physicals properties are used to a material, to choose a material for a specific purpose or to the substances in a mixture. B. Using Properties to Separate Mixtures Filtration and distillation are two common separation methods. 1. Filtration o is a process that separates materials based on the size of their particles. o Ex: tea leaves caught in a strainer when making tea 2. Distillation o is a process that separates the substances in a solution based on their boiling points. o Ex: A practical use of distillation is to provide freshwater for submarines.
C. Recognizing Physical Changes occurs when some of the properties of a material change, but the substances in the material remain the same. Ex: Heating butter until it melts, crumpling a piece of paper, slicing a tomato Some physical changes can be ; & Some physical changes be reversed: re-forming a whole tomato from its slices 2.3 Chemical Properties A. Observing Chemical Properties is any ability to produce a change in the composition of matter. Chemical properties can be observed only when the substances is a sample of matter are into substances 1. Flammability o is a material s ability to burn in the presence of oxygen. o Example: burning newspapers to start a fire 2. Reactivity o describes how readily a substance combines with other substances o Oxygen is highly reactive element and reacts easily with most other elements. o Oxygen reacts with iron and water to form rust. o Nitrogen has low reactivity and can be used inside tanks to limit rust formation. B. Recognizing Chemical Changes occur when a substance reacts and forms one or more new substances. Three (3) common types of evidence for a chemical change are: a change in color, the production of a gas, and the formation of a precipitate. 1. A change in o a change in color is a clue that a chemical change has at least one new substance. o Ex: silver that over time; copper roof changing from red to green when exposed to water 2. Production of a o of gas forming when you mix vinegar and baking soda is a sign that a chemical change occurred. 3. Formation of a Precipitate o is a solid that forms and separates from a liquid mixture. o Adding lemon juice to milk will form a white C. Is a Change Chemical or Physical? Ask yourself: are different substances present after the changes take place? NO = physical change, YES = Chemical change When matter undergoes a chemical change the composition of the matter changes. When mater undergoes a physical change the composition of the matter remains the same.
Chapter 3: States of Matter Student Notes GA Performance Standards SPS5. Students will compare and contrast the phases of matter as they relate to atomic and molecular motion. a. compare and contrast the atomic/molecular motion of solids, liquids, gasses and plasmas. b. relate temperature, pressure, and volume of gases to the behavior of gasses SPS7. Students will relate transformations and flow of energy within a system. d. Explain the flow of energy in a phase changes through the use of a phase diagram. 3.1 Solids, Liquids, and Gases A. Describing the States of Matter Materials can be classified as solids, liquids, or gases based on whether their and are definite or variable. Frequently referred to as the of matter or of matter. 1. Solids o is the state of matter in which materials have a shape and volume. o The shape and volume of a solid will change. o Almost all solids have some type of of particles at the atomic level. 2. Liquids o is the stage of matter in which a material has a volume but not a shape. o A liquid always has the same shape as its container and can be poured from one container to another. o The arrangement is more random than in a solid. 3. Gases o is the state of matter in which a material has an shape and an volume. o A gas takes the and volume of its container. o The atoms are arranged in a regular, and they are at random locations throughout the container. 4. Other States of Matter o 99% of all matter in the universe exists in a state that is not as common on Earth. o Plasma is a gas-like substance of charged particles; traveling very fast. o exist at extremely temperatures, such as on the sun or on stars. o Plasma is found on earth during. B. Kinetic Theory is the energy an object has due to its motion. The the object moves, the its kinetic energy is. The kinetic theory of matter says that particles of matter are in motion. These tiny particles are always in motion. The higher the temperature, the faster the particles move. At the same temperature, more massive ( ) particles move than less massive (lighter) particles. C. Explaining the Behavior of Solids Solids have a volume and shape because particles in a solid around locations. Vibration is a repetitive back and forth motion. Each atom vibrates around its location but it does not exchange places with a neighboring atom. D. Explaining the Behavior of Liquids The particles in a liquid are packed than the particles in a gas. The attractions between the particles in a liquid affect the movement of the particles.
A liquid takes the of its container because the particles in a liquid can flow to new locations. The of a liquid is because forces of attraction keep the particles close together. E. Explaining the Behavior of Gases The particles in a gas are at. Particles in a gas are in constant, motion. The constant motion of particles in a gas allows a gas to fill a container of any shape or size. The motion of one particle is by the motion of other particles unless the particles collide. Forces of among particles in a gas can be under ordinary conditions. F. Illustrations and Summary of Phases of Matter Solid Liquid Gas Summary of Phases of Matter Phase Shape Volume Solid Liquid Gas G. Reading Data Table Practice Substance Melting Point Boiling Point Rubbing Alcohol - 89 C 82.5 C Salt 801 C 1413 C Water 0 C 100 C Baking soda 50 C 851 C 1. What phase of matter is alcohol in at 0 C? 2. What phase of matter is Salt in at 900 C? 3. What substances are a gas at 110 C? 4. What is the freezing point of baking soda? 5. At what temperature is salt a gas? 6. At what temperature range is baking soda a liquid?
3.3 Phase Change A. Characteristics of Phase Changes is the physical change that occurs when a substance changes from one of matter to another. Melting, freezing, vaporization, condensation, sublimation, and deposition are six common phase changes All phase changes share certain characteristics related to and. B. Temperature and Phases Changes One way to recognize a phase change is by measuring the temperature of the substances as it is heated or cooled. The of a substance does change during a phase. Temperature remains during a phase change. 1. Energy and Phase Changes o During a phase change, energy is transferred between a substance and its surroundings. o Energy is either absorbed or released during a phase change. o is when the system absorbs energy from its surroundings. o is when the system releases energy to its surroundings. C. Melting and Freezing o The arrangement of molecules in water becomes less orderly as water melts and more orderly as water freezes. 1. Melting o is when energy is added to a object and it turns into a. o The average kinetic energy of the molecules increase and the temperature rises. o This is ENDOTHERMIC. 2. Freezing o is when energy is removed form an object and it goes from a to a. o As the average kinetic energy decreases, the molecules move more slowly. o This is EXOTHERMIC. D. Vaporization and Condensation 1. Boiling o ( ) is when a substance changes from a into a. o Vaporization is an endothermic process; the substance has to absorb energy to change from a liquid to a gas. o As the temperature increases the molecules move faster and faster. o This is ENDOTHERMIC. 2. Condensation o is the phase change in which a substance changes from a or vapor to a. o Condensation is an EXEOTHERMIC process.
E. Sublimation and Deposition 1. Sublimation o is the phase change in which a substance changes from a to a or vapor without changing to a liquid first o Dry Ice (solid carbon dioxide) at room temperature goes from solid to gas and forms a fog. o Sublimation is ENDOTHERMIC. 2. Deposition o is when a or vapor changes directly into a without first changing to a liquid. o Deposition causes frost to form on windows. o This is EXOTHERMIC. Phase Change Diagram Phase Change Diagram Practice What is occurring at the following points? o Point A o Point B What phases is present at the following points? o Point A o Point B o Point C o Point D o Point E 3.2 The Gas Laws A. Pressure is the result of a force distributed over an. Pressure in a gas is produced by the gas atoms colliding with a wall. between particles of a gas and the walls of the container the in a closed container of gas. The more frequent the collisions, the greater the pressure of the gas. B. Factors that Affect Gas Pressure Factors that affect the pressure of an enclosed gas are its temperature, its volume, and the number of its particles.
1. Temperature As the rises, the average energy of the particles in the air increases. The particles move faster and collide more often. the of a gas will its if the volume of the gas and the number of particles are constant. 2. Volume the volume of a gas its if the temperature of the gas and the number of particles are constant. 3. Number of Particles The particles there are in the same volume, the greater the number of collisions and the the. Increasing the number of particles will the of a gas if the temperature and the volume are constant. C. Charles s Law Jacques Charles showed that the volume of a gas increases at the same rate as the temperature of the gas. states that the of a gas is proportional to its in Kelvin if the pressure is constant. D. Boyle s Law states that the of a gas is proportional to its if the temperature is constant. E. Gay-Lussac s Law According to, for a given amount of gas held at a constant volume, the is to the. If one increases the other will increase. Gas Law Practice P Pressure Temperature Volume Charles Boyle s Gay-Lusaac s Pressure is constant: If temperature increases volume. If temperature decreases volume. Temperature is constant: If pressure increases volume. If pressure decreases volume. Volume is constant: If the temperature decreases pressure. If the temperature increases pressure. T V