CLASSIFICATION of MATTER Unit 2 -- Matter Chapter 3 CHEMISTRY
Matter Anything that has both mass AND volume –MASS A measure of the amount of matter contained in an object –VOLUME A measure of the amount of space an object takes up Substances –Matter that has a uniform and unchanging chemical composition –EX. Water (H2O); Table salt (NaCl) SECTION 3.1 – Properties of Matter
Physical Properties of Matter A characteristic that can be observed or measured without changing the sample’s composition –Also used to describe pure substances There are two types of physical properties –EXTENSIVE PROPERTIES dependent on the amount of the substance present –INTENSIVE PROPERTIES NOT dependent on the amount of the substance present SECTION 3.1 – Properties of Matter
Chemical Properties of Matter Ability OR inability of a substance to combine with or change into one or more other substances SECTION 3.1 – Properties of Matter
Identify Properties Classify each of the properties below into either PHYSICAL or CHEMICAL SECTION 3.1 – Properties of Matter
States of Matter Solid –Form of matter that has its own definite shape and volume –Particles within a solid are tightly packed When heated, it will expand only slightly Cannot be compressed Low Kinetic Energy (KE) SECTION 3.1 – Properties of Matter
States of Matter Liquid –Form of matter that flows, has a constant volume, and takes the shape of its container Less tightly packed –When heated, it will expand –Is virtually incompressible –Moderate Kinetic Energy (KE) SECTION 3.1 – Properties of Matter
States of Matter Gas –Form of matter that flows to conform to the shape of its container and fills the entire volume of its container Very loosely packed –When heated, it will expand and sometimes escape –Easily compressed –High Kinetic Energy (KE) Gas vs. Vapor –Gas = the state of matter –Vapor = gaseous state of a substance that is either a liquid or gas at room temperature BOTH liquids and gases are “fluids” because they flow SECTION 3.1 – Properties of Matter
Physical Changes Changes that DO NOT alter the composition of a substance –Physical changes are those that are causing a change in a physical property –Examples: Cutting paper Breaking a crystal SECTION 3.2 – Properties of Matter
Changes in States of MatterStates of Matter Changes in the state of matter are all PHYSICAL CHANGES as they do NOT alter the arrangement of the substance Deposition SECTION 3.2 – Properties of Matter
Chemical Changes Process that involves one or more substances changing into new substances a.k.a. Chemical reaction –Reactants – Starting substances –Products – Resulting substances Newly formed substances will have different compositions and properties than the original substances SECTION 3.2 – Changes in Matter
Four Indications of a Chemical Change 1.release of a gas 2.release of heat, light or sparks 3.formation of a precipitate 4.color change SECTION 3.2 – Changes in Matter
Law of Conservation of Mass Mass is neither created nor destroyed, it is only rearranged. –The total mass you have in the beginning of a reaction must be present at the end of the reaction Mercury + Oxygen Mercury Oxide If there are 200g of mercury and 16g of oxygen, what mass of mercury oxide is produced. Mercury + Oxygen Mercury Oxide 200g 16g ? 216g SECTION 3.2 – Changes in Matter
Law of Conservation of Mass: Lavoisier Total mass of substances doesn’t change during chemical rxn. Matter can’t be created/destroyed. reactant 1 + reactant 2 product total mass = calcium oxide + carbon dioxidecalcium carbonate CaO + CO 2 CaCO g g100.08g Observations leading to Atomic view of matter
32.5g g =60.3g -43.8g 16.5g Conservation of Mass Problem Solutions 1). What is the mass of iron oxide produced if 9.9g of iron reacts with 3.4g of oxygen? Iron (Fe) + Oxygen (O) Iron oxide 9.9g + 3.4g _____ 13.3g 2). 32.5g of magnesium reacts with 27.8g of zinc nitrate to produce 43.8g of magnesium nitrate and zinc. What is the mass of zinc produced? Mg + Zn(NO 3 ) 2 Mg(NO 3 ) 2 + Zn 32.5g g 43.8g + _____ 9.9g + 3.4g 13.3g 16.5g SECTION 3.1– Changes in Matter