Topic 1.1 Matter & Change EI: physical and chemical properties depend on the ways in which different atoms combine. NOS: Making quantitative measurements with replicates to ensure reliability – definite and multiple proportions (3.1)

What is Matter? What is Matter? Anything that takes up space and has mass. Made up of particles (atoms, molecules, ions) Particles are in constant motion

Distance between particles Arrangement of particles A 2. States of Matter State Shape Volume Distance between particles Arrangement of particles Solid (S) Fixed shape Fixed volume Close together regular Liquid (l) No fixed shape Fixed volume Close, but farther than solids random Gas or Vapor (g) No fixed shape Not fixed Far apart random

Switching between states Solid  melting  Liquid Liquid  freezing  Solid Liquid  evaporating (boiling)  Gas Gas  condensing  Liquid

Switching between states Solid  sublimation  Gas Gas  deposition  Solid Heat is required from solid to liquid to gas Heat is removed from gas to liquid to solid

Switching between States

U1: Properties of Matter Physical property A characteristic of a substance that can be measured or observed without changing the substance’s composition Chemical property The ability of a substance to undergo a chemical reaction to form new substances

Examples of Physical Properties Examples of Chemical Properties U1. Properties of Matter Examples of Physical Properties Color Solubility (Dissolving) Odor Hardness Density Melting Point Boiling Point State of matter Thermal capacity Mass Examples of Chemical Properties Reactivity with oxygen Reactivity with acids Reactivity with bases Reactivity with other elements Sodium and Chlorine Reaction

U1. Properties of Matter Sodium is a silver metal at room conditions; combines with chlorine to make table salt; reacts with water to form hydrogen; has a density of 0.93 g/cm3; oxidizes rapidly in air, melts at 97.8oC. Using the above description, list the physical properties of sodium Using the above description, list the chemical properties of sodium

U1. Properties of Matter Sodium is a silver metal at room conditions; combines with chlorine to make table salt; reacts with water to form hydrogen; has a density of 0.93 g/cm3; oxidizes rapidly in air, melts at 97.8oC. Using the above description, list the physical properties of sodium Using the above description, list the chemical properties of sodium

U1. Changes of Matter Physical change An alteration of matter that does not change the chemical composition of the material.

U1. Changes of Matter . Chemical change Results in a change in the chemical composition of the substance(s). This is called a reaction.

U1. Changes of Matter Examples of Physical Changes Examples of Freezing or melting Boiling or condensing Cutting Grinding Bending Blending Dissolving Examples of Chemical Changes Combustion (burning) Reacts with an acid Reacts with a base Rusting Oxidizing Decomposing Digesting

U1. Changes of Matter Copy the statement on your paper and write P for physical or C for chemical Bending of a piece of wire Burning of coal Cooking a steak Cutting grass Sodium reacts with water 6. Iron rusts 7. Silicon is insoluble in water 8. Ice melts 9. Neon boils at -2460C 10. Nitric Acid reacts with Copper

U2. Distinguishing Compounds and Mixtures Elements are composed of just one type of atom. They cannot be separated into simpler substances using chemical means. Stop Here do to the physical/chemical lab 2014

U2. Distinguishing Compounds and Mixtures Compounds are substances composed of two or more different kinds of atoms that have combined chemically. They can be separated by chemical means. Stop Here do to the physical/chemical lab 2014

U2. Distinguishing Compounds and Mixtures Mixtures are a physical blend of two or more substances. They can be separated by physical means. Stop Here do to the physical/chemical lab 2014

U2. Distinguish compounds and mixtures Elements Represented by a chemical symbol (see Periodic Table) Gold (Au), Iron (Fe), Oxygen (O or O2) Start here after physical/chemical change lab

U2. Distinguish compounds and mixtures A fixed ratio of elements, shown using element symbols and a number

U2. Distinguish compounds and mixtures Examples: Water, H2O, contains 2 atoms of hydrogen (H) and one atom of oxygen(O). Salt, NaCl, contains one atom of sodium (Na) for each atom of chlorine (Cl).

U3. Mixtures Mixtures: composition is not fixed Homogeneous mixture- has uniform composition and properties, also called solutions. Ex: pure air, pure water, syrup

U3. Mixtures Mixtures: Heterogeneous mixture – non-uniform composition, properties are not the same, able to see the separate components Ex: soup, concrete, granite

Ways to separate mixtures: U3. Mixtures Ways to separate mixtures: Heterogeneous: sieving, tweezers, skimming Homogeneous: distillation, ion exchange, reverse osmosis, evaporation

Distinguish between elements, compounds, and mixtures Copy the item and indicate if it is an element, compound or mixture 6. Silver 7. Orange juice 8. Neon 9. Sugar (C6H12O6) 10. Lake water Blood Hydrogen Brass (copper and zinc) Ice (H2O) Motor oil Practice Problems: pg. 40 14-18

A& S. 1: Chemical Reactions In a chemical reaction, one or more substances change into new substances by rearranging the atoms Reactants  Products

A& S. 1: Chemical Reactions Reactants  Products Reactants: the substances that are combined together Products: the substances that are formed after the reactants are combined together.

A& S. 1: Chemical Reactions Chemical Reaction Example: Reactants  Products Copper+ nitric acid copper(II) nitrate+ nitrogen dioxide+water Cu + HNO3  Cu(NO3)2 + NO2 + H2O

A& S. 1: Chemical Reactions Reactants  Products Copper+ nitric acid copper(II) nitrate+ nitrogen dioxide+water Cu + HNO3  Cu(NO3)2 + NO2 + H2O

A&S 1. Chemical Reactions A chemical reaction has occurred if: Heat is absorbed or given off (change in temperature) Change in color or odor Production of a gas or solid Not easily reversible

A&S 1. Chemical Reactions Law of Conservation of Mass During any chemical reaction, mass is neither created nor destroyed, it is conserved. The mass of the products will always equal the mass of the reactants. The mass of each element is also unchanged.

A&S 1. Chemical Reactions Law of Conservation of Mass In a reaction where hydrogen reacted with oxygen to produce water, if 4.5 g of hydrogen and 34 g of oxygen were used, how many grams of water were produced? Hydrogen + oxygen = water 4.5 + 34 = 38.5 g water