Types of Chemical Bonds and Naming Conventions

Type I Naming

For ionic compounds with metals that have a fixed charge (e.g., NaCl).

Type II Naming

For ionic compounds with transition metals that can have multiple charges (e.g., FeCl₃).

Type III Naming

For covalent compounds using prefixes to denote the number of atoms (e.g., CO₂).

Ionic Bond

Electrons are transferred from one atom to another.

Covalent Bond

Electrons are shared between atoms.

Zero Rule

The sum of oxidation states in a neutral molecule is zero.

Usage of Zero Rule

Assign oxidation states to atoms and adjust to satisfy the rule.

Nonpolar Bond

Difference < 0.5.

Polar Bond

Difference 0.5 to 1.7.

Ionic Bond

Difference > 1.7.

Strongest Bond

Ionic bonds (high electrostatic forces).

Weakest Bond

Nonpolar covalent bonds (equal sharing of electrons).

Structure of Ionic Bond

A lattice structure of alternating positive and negative ions.

Breaking Ionic Bonds

Ionic bonds break when dissolved in water or melted (disrupts lattice).

Metallic Bonds

A 'sea' of delocalized electrons shared by metal atoms.

Properties of Metallic Bonds

Conductivity, Malleability, Ductility, Luster.

Covalent Bond Structures

Linear (180°), Trigonal Planar (120°), Tetrahedral (109.5°).

Water Structure

Bent structure with ~104.5° angle due to lone pairs.

Structure of Molecule

Determined by lone pairs and bonded atoms.

Shape/Name of Molecule

Determined by bonded atoms (ignores lone pairs).

Polar + Nonpolar Interaction

Limited interaction due to differences in polarity.

Polar + Ionic Interaction

Polar molecules stabilize ions, often dissolving ionic compounds.

First Question for Naming

Ask: 'Is it ionic or covalent?' (determines Type I, II, or III naming).

Ionic Lewis Dot Structure

Show electron transfer and charges (e.g., Na⁺ and Cl⁻).

Covalent Lewis Dot Structure

Show shared electrons as lines or dots.

Difference in Lewis Dot Structures

Ionic involves charges; covalent involves shared pairs.

Smaller Atom in Bonding

The metal (loses electrons, reducing size).

Reason for Smaller Metal

Loss of electron shells and increased nuclear pull.

Type 1 Ionic Compounds

Metals with fixed charges.

Type 2 Ionic Compounds

Metals with variable charges (transition metals).

Prefixes in Naming

Used in Type III covalent compounds.

Resonance

A situation where a molecule has multiple valid Lewis structures.

Dipole Moment

A measure of charge separation in a polar molecule.

Finding Dipole Moment

Calculate based on bond polarity and molecular geometry.

Steps in Covalent Lewis Dot Structure

SPA!!!!!

Carbonate

CO₃²⁻.

Sulfite

SO₃²⁻.

Sulfate

SO₄²⁻.

Nitrite

NO₂⁻.

Nitrate

NO₃⁻.

Hydroxide

OH⁻.

Exceptions to Lewis Dot Structures

6 exceptions to know and why each is an exception.

Polyatomic Ions Charge

Their charge is a result of the overall electron imbalance, not individual atoms.

Differences between Bonded and Lone Pairs

Bonded Pairs: Shared between atoms, form bonds. Lone Pairs: Unshared, affect geometry but not bonding.

Double/Triple Bond Count

Count as one bonded pair in geometry.