SCH3U – Exam Review



SCH3U – Exam Review

Chapter 1

• Review of grade 10 (Bohr/Bohr-Rutherford diagrams, info from Periodic table

(eg: protons + neutrons = atomic mass)

• Bohr model

• Modern atomic theory

• Quantum theory

• Electron configuration

• Trends in the periodic table

Chapter 2

• intramolecular forces (within a molecule)

- ionic

- covalent

a) polar covalent bonds use electronegativity table

b) nonpolar covalent bonds

• Lewis dot diagrams (shows valence electrons)

- for ionic compounds (square brackets and charges)

- for nonpolar covalent bonds (use “have”, “want”, “bonds”)

- for polar covalent bonds (use “have”, “want”, “bonds”) – include partial positives and negatives

- for polyatomic ions (square brackets, charge affects your “have”)

- does it include a coordinate covalent bond?

• Shapes of molecules

- is it a polar or nonpolar molecule? (use type of bonds and symmetry)

• Intermolecular forces (between molecules)

- London dispersion forces (all molecules)

- dipole-dipole forces (only in polar molecules)

- hydrogen bonding (only in polar molecules between H and O, F or N)

• Naming compounds

- molecular (use prefixes)

- ionic

a) basic

b) multivalent (only have to know IUPAC names)

c) polyatomic ions (per-ate, -ate, -ite, hypo-ite)

- acids

a) binary (hydro-ic acid)

b) oxyacids (per-ic acid, -ic acid, -ous acid, hypo-ous acid)

Chapter 3

• Types of reactions

- synthesis

- decomposition

- single displacement (look at the activity series to see if reaction occurs)

- double displacement (3 types to have a reaction)

a) precipitate formed (use the solubility table)

b) gas produced

c) neutralization reactions

- combustion

- for each equation, be able to write the:

a) balanced equation

b) total ionic equation

c) net ionic equation

d) identify spectator ions

Chapter 4

• isotopic abundance

• mole concept and molar mass

• calculating number of molecules/atoms/formula units

• percent composition

• empirical and molecular formulas

Chapter 5

• balancing chemical reactions

• stoichiometry (using the mole ratio)

• limiting and excess reagent

• percent yield

• percent difference (percent error)

Chapter 6

• percent concentrations

- percent weight by volume

- percent volume by volume

- percent weight by weight

• very low concentrations (ppm)

• molar concentration

• converting from % concentration to molar concentration and vice versa

• dilutions of solutions

Chapter 7

• qualitative analysis

- flame test

- line spectrum

- sequential qualitative analysis (flow chart – based on solubility)

• total and net ionic equations for single displacement reactions

Chapter 8

• ionization versus dissociation

• weak versus strong acid or base

• Arrhenius theory

• Revised Arrhenius theory

• Bronsted-Lowry concept

- identify the acid, base, conjugate acid, conjugate base, and the conjugate acid/base pairs

• What it means to be amphiprotic

• Calculating pH or hydrogen ion concentration (be careful with significant digits)

• titration experiments

Chapter 9

• converting (pressures, temperatures, etc)

• gas laws

• ideal gas law

Chapter 10

• Dalton’s law of partial pressures

• molar volume

• gas stoichiometry (can use the ratio for volume of gases only)

What to bring to your exam

*there will be no sharing of materials AT ALL – you must bring all of your own items

- scientific calculator (no cell phones/MP3 players, etc)

- pencils, erasers, highlighter

- textbook (to return)

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