Chemical Compounds and Ions

Binary Ionic Compounds

• Naming: The metal is written first, followed by the non-metal. The name ends in "-ide."
• Examples: Sodium chloride (NaCl), Magnesium nitride (Mg₃N₂), Aluminum oxide (Al₂O₃)

Multivalent Elements

• Definition: Elements that can have more than one ionic charge.
• Application: Primarily used for transition metals.
• Examples: Copper (I) (Cu⁺), Copper (II) (Cu²⁺), Iron (II) Chloride (FeCl₂), Chromium (III) Chloride (CrCl₃), Chromium Oxide (Cr₂O₃)

Polyatomic Ions

• Definition: Ions composed of more than one atom.
• Naming: Refer to a chart for names and formulas.
• Examples: Nitrate (NO₃⁻), Bromate (BrO₃⁻), Ammonium (NH₄⁺), Magnesium Carbonate(MgCO₃)

Understanding Salt

• Salt properties: Size (bigger, smaller, same), Attitude (upright or inverted), Location (relative to other points/mirror), Type (real or virtual).

Concave Mirrors

• Shape: Curve inwards (like the inside of a spoon).
• Ray 1: Parallel to the principal axis reflects through the focal point (F).
• Ray 2: Passes through the focal point reflects parallel to the principal axis.
• Ray 3: Passes through the center of curvature (C) reflects along the same path.
• Ray 4: Hits the vertex (V) reflects at the same angle.
• Image characteristics: Smaller, inverted, real.

Convex Mirrors

• Shape: Curve outwards.
• Ray 1: Parallel to the principal axis reflects as if it has passed through F.
• Ray 2: Appears to have passed through F reflects parallel to the principal axis.
• Ray 3: Appears to have passed through C reflects along the same path.
• Ray 4: Hits the vertex reflects at the same angle.
• Image characteristics: Smaller, upright, virtual.

General Terms (Mirrors)

• F: Focal Point
• V: Vertex
• C: Center of Curvature (2F)
• PA: Principal Axis of Symmetry
• Image: Reflected object.

Types of Reactions

• Single Displacement: One element replaces another in a compound (e.g., A + BC → AC + B).
• Double Displacement: Two compounds react, elements exchange places (e.g., AB + CD → AD + CB).
• Synthesis: Two or more substances combine to form a new substance (e.g., A + B → AB).
• Decomposition: A compound breaks down into simpler substances (e.g., AB → A + B).

Types of Molecules

• Mono: One
• Di: Two
• Tri: Three

Bohr-Rutherford/Lewis Dot Diagrams

• Used to represent atoms and their valence electrons.

Covalent/Ionic Bonds

• Ionic: Between a metal and non-metal, electrons are transferred.
• Covalent: Between two non-metals, electrons are shared.

Neutralization Reactions

• Acid + Base → Salt + Water
• Example: HCl + NaOH → H₂O + NaCl

Periodic Table Sections

• Nonmetals: Groups 14-17 (lack characteristics of metals).
• Halogens: Group 17 (form salts reacting with metals).
• Earth Metals: Group 2 (less reactive than alkali metals).
• Alkali Metals: Group 1 (react with water to form alkalis).

Atoms and Changes

• Proton: Positively charged.
• Neutron: Neutral charge.

Osmosis

• Movement of water from high to low concentration.

Organ Systems-Circulatory System

• Function: Transport substances (food, oxygen, wastes) throughout the body using blood.
• Arteries: Carry blood away from the heart.
• Veins: Carry blood towards the heart.
• Capillaries: Exchange oxygen in lungs.
• Key Components: Superior vena cava/vena cava, Right atrium, Tricuspid valve, Right ventricle, Pulmonary valve, Pulmonary artery, Pulmonary veins, Left atrium, Mitral valve, Left ventricle, Aorta.