1. Finals REVIEW CHAPTERS 1 through 16 Finals in Room T123 at 9:30 am Dec 19 th (Monday) Bring a scantron ItemScoresWeighta ge Exam 4X100 = 400 *1.25 50050% Finals15015% Hws (drop 1 lowest grade) 808% Lab (drop 1 lowest grade) 25025% Attendance/impr ession/quiz 202% Total1000100% Calculation of Final grade SCCC GRADING 60-64 “D”; 65-69 “D+”; 70-74 “C”; 75-79 “C+”; 80-85 “B”; 85-89 “B+”; Above 90 “A”

2. Chapter 1 and 3  Concept of Experiment Hypothesis and Theory  Classification of matter  Physical change? Chemical change?  Pure substance? Mixture? Chapter 2 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 2.3 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 2.8 Density (D= Mass/Volume) Density calculations-check density lab calculations (Lab#2, 3)

3. Chapter 4 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 Periodic Table (section 4.8) 1. Group 1 – alkali metals +1 ion only 2. Group 2 – alkali earth metals +2 ion only 3. Group 7 – halogens usually –1 ion 4. Group 8 – noble gases Elements Chapter 11 electronic configuration of atoms and ions valence electrons orbital, how many electrons can sub-shells have? S-2, p-6, d? etc Filling order 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s-MEMORIZE A. Atomic size 1. Decreases as you move to the right along a row (period) 2. Increases as you go down a column (group) Ionization energy has trends opposite to Atomic Size 35 Cl 17 Mass # At. #

4. Chapter 12 Bonding and shapes- MODELS LAB #7 Correct Lewis structure Molecular geometry –important-2 questions! Type of bonding? Ionic, Polar covalent, non polar covalent etc. Polar- non polar??, Chapter 5 (check review 3) How many atoms in some chemical formula Al (NO 3 ) 3 Ans:13 Correct formulas for chemicals, polyatomics Names of compounds molecular, ionic compounds and Acids Chapter 6 and 7 –Check single/Double lab (#9 and 10) Types of reaction? Displacement, dissociation etc Balancing equation- write the coefficients? Solubility chart(check review 3) Chapter 8 (check review 3) How many moles, number of atoms/molecules ? Empirical formula- easy one Molecular formulas- Ratio Mass %- hey this is easy!!!

5. Chapter 9 Balance equations First!!! Calculations in chemical reaction how much reactant will produce how much product, moles to moles, grams to grams etc- STOICHIOMETRY

6. Chapter 13 – Gases – 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 and P ∞1/V Chapter 14 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 15 Check review 4 in website Mass percentage Molarity and number of moles in solution Titration Chapter 16 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: Weak acid + salt containing anion of weak Acid Basic Buffers: Weak Base + Salt containing cation of weak base

7. 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

8. Important Formulas to memorize Chapter 2 – Density, temperature conversion, powers of 10 Chapter 10– At.#, mass#, protons, neutrons, e-, isotopes, ions Chapter 11 – Valence electrons, electron config. Chapter 5 – Formulas of compounds, Lewis structure rules Chapter 12 – VSEPR shapes of molecules, polarity, dipole Chapter 6, 7 – Balancing chemical equations, Single-double displacement reactions Chapter 8,9 – 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 14 –, Concept of inter-molecular bonding, H-bond Chapter 13 – Gas laws, relation of P vs V, T & n Temp in Kelvin!! Chapter 15 – Molarity = moles/L of solution, % composition = Chapter 16 – pH = -log([H+]), [OH-] = Kw/[H+], pH calculations Titrations 1:1 M a V a = M b V b