1. Finals Chapter 1 Concept of Experiment Hypothesis and Theory (5% ) Physical change? Chemical change? Pure substance? Mixture? Chapter 2 ( 12.5% = Approx 5 questions)-Do your % math!! Significant figure –how many in 0.0050 ? Scientific notation in form of exponent of 10 Conversion eg. cm-> meter->kilometer, liters-> ml etc., ºF to ºC Density calculations-check ice cube lab calculations, density lab Finals on Thursday 6:00 Pm-7:25 Pm Room T-109: Dec 19 th 2011 40 multiple choice questions BRING A SCANTRON Good Luck and Happy Holidays!! REVIEW CHAPTERS 1 through 15

2. 2.6 The Basic Units of Measurement (memorize power of 10 table) A. English, metric, SI B. SI Units (Mass – kg; Length – m; Time – sec, volume L) C. Prefix Multipliers  milli (m) 0.001  centi (c) 0.01  kilo (k) 1000  Mega (M) 1,000,000 2.7 Density (D= Mass/Volume) Chapter 3 (7.5%) Symbols for elements (from periodic table) No. protons, no. neutrons, no. electrons, charge problem Atomic Number = Number of protons Mass Number = # of Protons + # of neutrons Isotopes, writing in the 14 C convention Average atomic mass calculation Chapter 4,9,10 (7.5%) electronic configuration of atoms and ions valence electrons orbital, how many electrons can sub-shells have? S-2, p-6, d? etc. 35 Cl 17 Mass # At. #

3. Chapter 5 and 6,11 (25%)- 10 Questions! How many atoms in some chemical formula Al (NO 3 ) 3 Ans:13 Correct formulas for chemicals, polyatomic ions- 4 questions Names of compounds molecular and ionic compounds Correct Lewis structure Molecular geometry –important-2 questions! Type of bonding? Ionic, Polar covalent, non polar covalent etc. Polar- non polar??, Chapter 7 (5%) Types of reaction? Displacement, dissociation etc Balancing equation- write the coefficients? Chapter 8,9 –(15%)- 6 questions! How many moles, number of atoms/molecules ? Empirical formula- easy one Molecular formulas- Ratio Calculations in chemical reaction how much reactant will produce how much product, moles to moles, grams to grams etc (3 questions)- STOICHIOMETRY

4. Chapter 13 (5%) Polar dissolves polar and non polar dissolves non polar Intermolecular forces are strong will result in high boiling point H-bonding INTER molecular bond between H and O or F or N Electrolytes and metallic bonding; London dispersion forces, dipole-dipole forces Chapter 12 – Gases –(5%) Boyle’s law relation of P and V Charles law relation of V and T Avogadro's law relation of V and N combined gas law PV=nRT relationship P ∞T, P ∞n (pressure is directly proportional to T, and n) P ∞1/V (pressure is inversely proportional to V) Chapter 14 (5%) Mass percentage Molarity = moles /Litres solution Molarity and number of moles in solution Titration: M a V a = M b V b; Dilution Chapter 15 (10%) Weak and strong electrolytes (refer to lab): NEED IONS!! Acids produce H + and Bases produce OH - concepts pH 7 bases, pH=7 neutral; Strong acid or strong base Buffers: Maintain pH

5. 6.023x10 23 ATOMS = 1 mole OF ATOMS weighs At. Mass in g 6.023x10 23 MOLECULES = 1 mole OF MOLECULES weighs Molar mass in g Suppose the molecule has formula A 2 B then 1 mole of A 2 B consists of 6.023x10 23 MOLECULES of A 2 B and 2 X 6.023x10 23 ATOMS of A weighs 2 X At. Mass of A in g 1 X 6.023x10 23 ATOMS of B weighs 1 X At. Mass of B in g

6. Important Formulas to memorize Chapter 2 – Density, temperature conversion, powers of 10 Chapter 3,4 – At.#, mass#, protons, neutrons, e-, isotopes, ions Chapter 9,10 – Valence electrons, electron config. Chapter 5,6 – Formulas of compounds, Lewis structure rules Chapter 11 – VSEPR shapes of molecules, polarity, dipole Chapter 7 – Balancing chemical equations, Single-double displacement reactions Chapter 8 – Moles? Avogadro number? Molar mass, Stoichiometry Start from balanced equation, moles of A to moles of B? grams of A to grams of B? etc Chapter 13 –, Concept of inter-molecular bonding, H-bond Chapter 12 – Gas laws, relation of P vs V, T & n Temp in Kelvin!! Chapter 14 – Molarity = moles/L of solution, % composition = Chapter 15 – pH = -log([H+]), [OH-] = Kw/[H+], pH calculations Titrations 1:1 M a V a = M b V b Titrations n a M a V a = n b M b V b;