Essential Chemistry: Bonds, Nomenclature, and Atomic Structure
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Chemical Bonds and Properties
Ionic Bonds
Ionic bonds are characteristic of compounds formed between a metal and a non-metal. Metals form positive ions (cations), and non-metals form ion-accepting negative ions (anions).
Properties of Ionic Compounds
- Soluble in water
- Hard and fragile
- Have an ionic crystal structure
Covalent Bonds
Covalent bonds are seen in particles formed by atoms of non-metals, as is the case of diatomic gas molecules. Atoms share one or more pairs of electrons to complete their outer octet.
Properties of Covalent Compounds
- Do not conduct electric current
- Molecules of simple gases have covalent bonds
- Have atomic or molecular crystalline structure
Types of Covalent Bonds
- Polar Covalent
- Non-Polar Covalent
- Coordinate Covalent: Two electrons are shared, provided by only one of the atoms forming the bond.
Metallic Bonds
Metallic bonds involve metal cations within a negatively charged "sea" or "cloud" of electrons. This union gives metals their characteristic brightness.
Properties of Metallic Compounds
- Permeability
- Electrical conductivity
- Ductility
Key Definitions in Chemical Bonding
- Equation: A representation of a chemical reaction.
- Valence: The combining capacity of a chemical element.
- Electrovalence: The number of electrons an atom gives or gains in an ionic bond.
- Covalence: The number of electrons an atom shares in a covalent bond.
Chemical Nomenclature Systems
Oxide Nomenclature
Traditional System
For metals with a single valence: Oxide of [Metal Name]
For metals with multiple valences: Use suffixes -ous (lower valence) and -ic (higher valence) with the metal name.
Modern (IUPAC) System
Uses prefixes: mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, deca-. Example: monooxide
Stock System
[Name of Metal] (Valence in Roman Numerals)
Hydride and Acid Nomenclature
Non-metal Hydrides
- HF: Hydrogen Fluoride
- HCl: Hydrogen Chloride
- HBr: Hydrogen Bromide
- HI: Hydrogen Iodide
- H2S: Hydrogen Sulfide
Hydrohalic Acids (Aqueous Solutions)
- HF (aq): Hydrofluoric Acid
- HCl (aq): Hydrochloric Acid
- HBr (aq): Hydrobromic Acid
- HI (aq): Hydroiodic Acid
- H2S (aq): Hydrosulfuric Acid
Atomic Structure Fundamentals
Mass Number (A)
The mass number represents the sum of the protons and neutrons present in the atomic nucleus.
Formula: A = p + n (where p = protons, n = neutrons)
Atomic Number (Z)
The atomic number is the positive integer that equals the total number of protons in an atomic nucleus.
Formula: Z = Number of Protons
Quantum Numbers
These numbers describe the properties of electrons in atoms:
- Principal Quantum Number (n): Describes the electron's energy level and distance from the nucleus.
- Azimuthal (Angular Momentum) Quantum Number (l): Describes the shape of the orbital.
- Magnetic Quantum Number (ml): Describes the orientation of the orbital in space.
- Spin Quantum Number (ms): Describes the intrinsic angular momentum (spin) of an electron.