Review

1. Review Each of you will be assigned a Unit and Number. Number your study guide as I have on the following slides. On your whiteboards, write the Unit and Number. We will go over them as a class!

2. Unit 7 – Elements, Compounds, Mixtures; Physical and Chemical Properties; Physical and Chemical Changes; Mass percent; Conservation of MassConcepts and important formulae:1. The difference between heterogeneous and homogeneous mixture: Heterogeneous has different particle sizes; Homogeneous has uniform composition throughout2. Definition of an element: cannot be broken down, one kind of atom, on the PT, rarest form of matter3. Definition of a compound: two or more elements, can be broken down chemically4. Physical properties of a substance include: density, color, odor, hardness, melting/boiling/freezing pt5. Chemical properties/signs of chem change of a substance include: rusting, fermenting, oxidizing, combustion, corroding, decaying, forming gas, tarnishing, decomposing6. A substance undergoes physical change when: it changes the state of matter (liquid to gas; solid to liquid)7. A substance undergoes chemical change when: it changes its chemical makeup ; new substance formed8. Law of conservation of mass states that: matter cannot be created nor destroyed; atoms are rearranged9. The formula for mass percent or percent composition is:(mass of component) x 100(mass total)

3. Unit 7 – Elements, Compounds, Mixtures; Physical and Chemical Properties; Physical and Chemical Changes; Mass percent; Conservation of MassConcepts and important formulae:1. The difference between heterogeneous and homogeneous mixture: Heterogeneous: multiple compounds that are distinguishable from each other Homogeneous: same appearance throughout2. Definition of an element: On the periodic table; one type of atom; pure & rare substance that cannot be broken down by chemical or physical means3. Definition of a compound: more than one element; every molecule is the same4. Physical properties of a substance include: melting point, boiling point, hardness, conductivity, density, color, odor; physical changes: rupture, tear, puncture5. Chemical properties/changes of a substance include: Oxidization, Rust, Combustion, Rotting, Decay, Burning, ferment, corroding, decomposition6. A substance undergoes physical change when: appearance or state change (liquid to solid); chemical formula does not change7. A substance undergoes chemical change when: chemical formula is changed; a new substance formed8. Law of conservation of mass states that: matter is neither created nor destroyed during a chemical reaction but is conserved or rearranged9. The formula for mass percent or percent composition is: (mass of component) x 100 (mass total)

4. Unit 7 – Elements, Compounds, Mixtures; Physical and Chemical Properties; Physical and Chemical Changes; Mass percent; Conservation of MassConcepts and important formulae:1. The difference between heterogeneous and homogeneous mixture: homogeneous mixture is same appearance throughout; Heterogeneous : particle size is not the same, different appearance2. Definition of an element: Found on the PT, pure substance, rarest form of matter; cannot be broken down3. Definition of a compound: 2 or more element bonded together; chemical name and chemical formula4. Physical properties of a substance include: density, color, odor, hardness, melting pt, boiling pt. , freezing point, rupture 5. Chemical properties/changeof a substance include: rusting, corroding, tarnishing, burning, molding (bread), solubility, forming gas, fermenting, decomposing, decaying, exploding/combusting6. A substance undergoes physical change when: if the state or shape changes, but not the chemical composition7. A substance undergoes chemical change when: chemical make-up is different after the reaction8. Law of conservation of mass states that: matter neither created nor destroyed in reaction; atoms are rearranged9. The formula for mass percent or percent composition is: mass of component) x 100 (mass total)

5. Unit 8 - Naming & Formula Writing, Moles, Balancing, and Predicting ProductsConcepts and important formulae:1. How do you write names from formulas for ionic compounds? Cation (positive ion) is first; anion (or polyatomic) is last with an ending of –ide. Transition metals: The roman numeral is the charge of the metal. E.g. Fe2O3 You know that O 2- so Fe must have a +3 charge. Iron (III) oxide2. How do you write formulas from names for ionic compounds? Criss cross the charges of the elements or PAI. Parentheses indicate there is more than one group. IO3- 1 = iodate Beryllium iodate: Be +2 IO3-  Be(IO3)23. How can you tell if a compound is covalent vs. ionic?Covalent = two nonmetals; contains prefixes Ionic : has cation and anion (metal and a nonmetal) 4. How do you write the name from a formula for covalent compounds? E.g. CO2 subscript becomes prefix; carbon dioxide Mono = one di = two tri = three tetra = four penta = five hexa = six hepta = seven oct- eight nona= nine deca = ten5. What is a mole? # of atoms or molecules; A unit of measurement for the amount of a substance; 6.02x1023 6. What do you use to predict single replacement reactions? Activity series E.g. NaBr + Cl2 NaCl + Br2Cl replaces Br in the activity series because it is above it

6. Iodate: IO3- Unit 8 - Naming & Formula Writing, Moles, Balancing, and Predicting ProductsConcepts and important formulae:1. How do you write names from formulas for ionic compounds? Metal/cation goes first; nonmetal/anion goes last and has –ide at the end, e.g. Li2S lithium sulfide Li +1 S 2-  transition metals(groups 3-12): find out charge of the transition metal from the charge of the anion , e.g. Fe2O3 Fe 3+ O2- Iron (III) oxide  Roman numeral is the charge on the transition metal2. How do you write formulas from names for ionic compounds? Criss-cross charges to become subscripts; parentheses indicate more than 1 group: e.g. Be2+ IO3-Beryllium iodate  Be(IO3)23. How can you tell if a compound is covalent vs. ionic? Covalent has two non-metals and has prefixes Ionic has cation and anion; can also have roman numerals (for transition metals)4. How do you write the name from a formula for covalent compounds?Use prefixes--- CO2is carbon dioxide. Don’t use mono if the first element has one5. What is a mole? A unit to measure amount of a substance; 6.02x1023Use Avo’s# to make really small #s manageable 6. What do you use to predict single replacement reactions? Activity series If an element is above the element in the compound, it will replace it. e.g. 2NaBr + Cl 2 Cl will replace Br  2NaCl + Br2

7. Unit 8 - Naming & Formula Writing, Moles, Balancing, and Predicting ProductsConcepts and important formulae:1. How do you write names from formulas for ionic compounds? Name of cation (positive ion) goes first; name of anion (negative ion) goes last with ending of –ide • E.g. Li2S : lithium sulfide 2. How do you write formulas from names for ionic compounds? Criss cross charges of elements or polyatomic ions • E.g. Fe2O3 O has a -2 charge; Fe must have a +3 charge ; iron (III) oxide3. How can you tell if a compound is covalent vs. ionic? Covalent: has two nonmetals, has prefixes in the name • Ionic: has a metal (cation)4. How do you write the name from a formula for covalent compounds? Subscripts become prefixes: Example: CO2 is carbon dioxide5. What is a mole? A measurement or unit; 6.02 x 10236. What do you use to predict single replacement reactions? Use the activity series example: NaBr + Cl2Cl is higher than Br and will replace  NaCl + Br2

8. Unit 9 – Stoichiometry and Predicting PrecipitatesConcepts and important formulae:1. What is a Mole ratio : ratio of # of moles between any two substances2. Any given element in a balanced chemical equation must have the same number on both the reactantsand product side.(Unit 9 continued) ---3. What is a precipitate? A solid produced during double replacement reaction in aqueous solution4. What do you use to predict if a double replacement reaction will form a precipitate in aqueous solution? Solubility Rules!5. What do the designations (s), (l), (g), and (aq) mean? S = solid g= gas l= liquid aq= aqueous

9. Answers to Concept Questions • Unit 9 – Stoichiometry and Predicting PrecipitatesConcepts and important formulae:1. What is a Mole ratio : a ratio of the coefficients of a balanced chemical equation2. Any given element in a balanced chemical equation must have the same number on both the ___reactant______ and product side.(Unit 9 continued) ---3. What is a precipitate? Solid product from aqueous double replacement reaction4. What do you use to predict if a double replacement reaction will form a precipitate in aqueous solution? Solubility Rules5. What do the designations (s), (l), (g), and (aq) mean? • Solid, liquid, gas, aqueous

10. Unit 10 – Solutions and Concentrations 1. Molarity = mol solute / L solution 2. Dilution equation = M1V1 = M2V2 where M is molarity and V is volume Unit 11 – Acids and Bases Concepts and important formulae: Your Unit 11 Review sheet should be very helpful to you. 1. Arrhenius acid: substance that produces H3O+ 2. Arrhenius base: substance that produces OH- 3. Bronsted-Lowry acid: substance that donates H+ ions 4. Bronsted-Lowry base: substance that accepts H+ ions 5. Congugateacid: substance produced when B/L base accepts H+ ion; usually looks like the base; positively charged 6.Conjugate base: substance produced when B/L acid donates H+ ion; usually looks like the acid; negatively charged 7. Monoprotic: one H or one proton e.g. HCl 8. Diprotic: two Hs or two protons e.g. H2SO4 9. Triprotic: three Hs or three protons e.g. H3PO4 10. Amphoteric: able to react as a base or an acid e.g. H2O 11. If the pH of a substance is from 0 to < 7.0, the substance is : acidic 12. If the pH of a substance is 7.0, the substance is neutral 13. If the pH of a substance is from > 7.0 to 14.0, the substance is basic 14. Properties of Acids: sour, electrolytes in aq solution, changes color of indicator, reacts with metals 15. Properties of Bases: bitter taste, electrolytes in aq solution, changes color of indicator, slippery

11. Unit 12 – Gas Laws Concepts and important formulae: (refer to your Unit Behavior of Gases Review) 1. Combined Gas Law Formula = on the board 2. Ideal Gas Law Formula = PV = nRT (on the board) 3. R is the universal gas constant. When would you use 8.31? When your pressure is in kPa 4. When would you use 0.0821? When your pressure is in atmospheres (atm)