SNC3U1 Chemistry Exam Review

SNC3U1 Exam Review

Titration: A procedure used to determine the concentration of a solution using a standardized solution (known concentration). (Section 10.3)
Dissociation: The separation of ions when an ionic compound dissolves in water.
Ionization: Formation of ions from uncharged molecules (non-electrolytes) when in water (e.g., acids). (Section 10.2)
Spectator Ions: Ions that appear on both sides of a chemical equation, remain unchanged, and can be omitted to simplify the net ionic equation. (Section 9.1)
Standard Solution: A solution with a precisely known concentration, typically prepared using a volumetric flask. (Section 8.6)
Stock Solution: A concentrated solution that is diluted to a lower concentration before use. (Section 8.6)
Polar Bonds: Covalent bonds where electrons are not shared equally due to differences in electronegativity (0.5 < EN < 1.7)
Non-Polar Bonds: Covalent bonds where electrons are shared equally (0 < EN < 0.5)
Ionic Bonds: Very strong bonds resulting from a complete transfer of electrons (EN > 1.7). High melting points.
Precipitate: A solid formed from a chemical reaction in a solution.
Dipole-Dipole Forces: Relatively strong intermolecular forces between polar molecules. The polarity is stronger when the EN difference is greater.
London Dispersion Forces: Weak attractive forces between all molecules (polar or nonpolar). Temporary fluctuations in electron distribution cause temporary dipoles.
Hydrogen Bonding: A type of dipole-dipole force. Strong bond between a hydrogen atom bonded to a highly electronegative atom (N, O, F) and another electronegative atom in a different molecule.
Theoretical Yield: The predicted amount of product based on the balanced chemical equation.
Actual Yield: The amount of product actually obtained in an experiment.
Percentage Yield: (Actual Yield/Theoretical Yield) x 100%
Chemical Change: Observable changes like color change, energy release/absorption, gas production, or precipitate formation.
Unsaturated Solution: A solution that can dissolve more solute at a given temperature.
Saturated Solution: A solution that contains the maximum amount of solute that can be dissolved at a given temperature.
Supersaturated Solution: A solution containing more solute than it can hold at a given temperature. This is unstable, and small changes can lead to crystallization.

Additional Concepts (from page 2)

Periodic Table Groups: Groups (columns) of elements with similar chemical properties are labeled 1-18.
Periodic Table Periods: Periods (rows) show trends in elemental properties.
Charles' Law: The volume of a gas is directly proportional to its temperature (in Kelvin) at constant pressure. (V1/T1 = V2/T2)
How to create Super Saturated Solution: Heat the solution to saturation point (dissolve maximal solute). Cool back slowly, allowing solute to remain in solution beyond the max amount.

Additional Concepts (From page 3)

Boyles' Law: The volume of a gas is inversely proportional to its pressure at constant temperature. (P1V1 = P2V2)
Gay-Lussac's Law: The pressure of a gas is directly proportional to its temperature (in Kelvin) at constant volume. (P1/T1 = P2/T2)
Combined Gas Law: Combines Boyle's, Charles', and Gay-Lussac's laws. (P1V1/T1 = P2V2/T2)
Dalton's Law of Partial Pressures: The total pressure of a mixture of non-reacting gases is the sum of the partial pressures of the individual gases. (Ptotal = P1 + P2 + ... )
Avogadro's Law: Equal volumes of gases at the same temperature and pressure contain the same number of molecules.
Effective Nuclear Charge: The net positive charge experienced by an electron in an atom, taking into account the shielding effect of inner electrons.
Electron Shielding: Inner electrons reduce the attractive force between the nucleus and outer electrons.
Alkali Metals: Group 1 elements, highly reactive, soft metals.
Alkaline Earth Metals: Group 2 elements, reactive metals.
Transition Metals: Elements in groups 3-12 with diverse properties, typically good conductors of electricity and heat, and have high melting/boiling points.
Metalloids: Staircase elements displaying properties of both metals and nonmetals.

Additional Concepts (from page 4)

Oxyanion: A negatively charged polyatomic ion containing oxygen. Examples include carbonate (CO3⁻²) and sulfate (SO₄⁻²).
Electron Configuration: Shows the arrangement of electrons in different orbitals around the nucleus of an atom. Used in predicting chemical behavior.
Lewis Structures: Diagrams showing the arrangement of atoms and valence electrons in a molecule.

Additional Concepts (from page 5)

VSEPR (Valence Shell Electron Pair Repulsion): Theory used to predict the 3D shape of molecules based on the repulsion between electron pairs.
Isotope Calculations: Used to determine average atomic mass (weighted average) of an element.
Electronegativity: The ability of an atom to attract electrons in a chemical bond.
Atomic Size: Atomic size generally increases down a group and decreases across a period of the periodic table.

Additional Concepts (from page 6)

Empirical Formula: The simplest whole-number ratio of atoms in a compound.
Molecular Formula: Represents the actual number of atoms of each element in a molecule of a compound.

Additional Concepts (from page 7)

Calculating Empirical and Molecular Formulas: Steps involved in determining these formulas based on percent composition or mass data. This often includes converting to moles and then using ratios to obtain the lowest common multiple in a whole number ratio.