Finals

1. 0 Finals REVIEW CHAPTERS 1 through 16 Finals in Room T123 at 9:30 am Dec 19th (Monday) Bring a scantron 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. Mass # 35 Cl 17 At. # • 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 14C 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 0

4. 0 • 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 (NO3)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 : Acid; 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 0

7. 0 • 6.023x1023ATOMS = 1 mole OF ATOMS • weighs At. Mass in g • 6.023x1023MOLECULES = 1 mole OF MOLECULES • weighs Molar mass in g • Suppose the molecule has formula A2B • then • 1 mole of A2B consists of 6.023x1023MOLECULES of A2B and • 2 X 6.023x1023ATOMS of A • weighs 2 X At. Mass of A in g • 1 X 6.023x1023ATOMS of B • weighs 1 X At. Mass of B in g

8. 0 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 MaVa = MbVb