SCH 3U1/3UP June 2025 Exam - Study Notes

Flashcards for SCH 3U1/3UP June 2025 Exam - Study Notes

Metals

Shiny, conductive, malleable, form positive ions (cations)

Non-metals

Dull, brittle, non-conductive, form negative ions (anions)

Alkali Metals (Group 1)

Very reactive, 1 valence e-

Alkaline Earth Metals (Group 2)

Fairly reactive, 2 valence e-

Halogens (Group 17)

Reactive non-metals, form -1 ions

Noble Gases (Group 18)

Inert, full valence shells

Atomic Radius (AR)

Decreases across period, increases down group

Ionization Energy (IE)

Increases across period, decreases down group

Electron Affinity (EA)

More negative across period, less negative down group

Metal Reactivity (MR)

Decreases across period, increases down group

Non-metal Reactivity (NR)

Increases across period, decreases down group

Electronegativity (EN)

Increases across period, decreases down group

Higher AR

Lower IE

Higher MR

Lower IE

Higher NR

Higher EA

Cations

Smaller than atoms

Anions

Larger than atoms

Ionic Bonds

Electron transfer, form between metal & non-metal, crystal lattice

Properties of Ionic Compounds

High melting/boiling points, conduct electricity in solution

Covalent Bonds

Shared electrons between non-metals

Bond Polarity

Use delta (δ) symbols, based on EN difference

Molecular Shapes (VSEPR)

Linear, bent, trigonal planar, tetrahedral, pyramidal

Polarity of Molecules

Depends on symmetry and bond polarity

Properties of Covalent Compounds

Low melting points, poor conductivity

Intermolecular Forces (IMFs)

London Dispersion, Dipole-Dipole, Hydrogen Bonds

Macroscopic Properties

Boiling/melting points depend on strength of IMFs

Reaction Types

Synthesis, Decomposition, Single Displacement, Double Displacement, Combustion

Balancing Equations

Conserve mass, equal atoms on both sides

Mole Calculations

Use molar mass, Avogadro's number

Percent Composition

% = (mass of element / total mass) x 100

Empirical Formula

Simplest ratio

Molecular Formula

Actual ratio, multiple of empirical

Limiting reagent

Fully consumed

Excess reagent

Left over

Key Terms (Solutions)

Solute, solvent, solution, saturated, dilute, concentrated

Solubility Curves

Read temperature vs solubility graphs

Dissolving in Water

Ionic compounds dissociate

Properties of Water

Polar molecule, hydrogen bonding

Factors Affecting Solubility

Temperature, pressure, polarity

Ionic/Net Ionic Equations

Show dissociation and spectator ions

Preparation of Stock Solutions

Dilution formula: C1V1 = C2V2

Quantitative Terms (Solutions)

Molarity (mol/L), Percent concentration

Acids

Sour, pH < 7, donate H+

Bases

Bitter, pH > 7, accept H+

Bronsted-Lowry Theory

Acids donate, bases accept protons

Conjugate Pairs

Differ by one H+

pH Calculations

pH = -log[H+]

Titration

Find unknown concentration

Endpoint

Color change

Equivalence point

Moles acid = moles base

Boyle’s Law

P ↑ V ↓ (inverse)

Charles’ Law

V ↑ T ↑ (direct)

Gay-Lussac’s Law

P ↑ T ↑ (direct)

Avogadro’s Law

V ↑ n ↑

Combined Gas Law

PV/T = constant

Dalton’s Law

Total P = sum of partial pressures

Ideal Gas Law

PV = nRT

Molar Mass

M = mRT/PV

Density

D = PM/RT

Oxidation

Lose electrons

Reduction

Gain electrons

Oxidizing agent

Gets reduced

Reducing agent

Gets oxidized

Assigning Oxidation Numbers

Follow rules (O = -2, H = +1, etc.)

Half-Reactions

Separate into oxidation and reduction parts

Anode

Oxidation

Cathode

Reduction