Chapter 2: Chemical Compounds and Bonding

Chemical Bonding

The electrostatic attraction between two atoms or ions.

Ionic Bond

A type of bond formed by the complete transfer of electrons from one atom to another.

Covalent Bonding

A type of bonding that involves the sharing of electrons between two atoms.

Valence Electrons

Electrons located in the outermost shell of an atom, important for bonding.

Lewis Structure

A diagram that represents the arrangement of valence electrons in a molecule.

Octet Rule

When atoms combine, they transfer or share electrons so that each atom ends up with 8 electrons in their outermost shell.

Cation

A positively charged ion formed when a metal loses electrons.

Anion

A negatively charged ion formed when a non-metal gains electrons.

Electrostatic Attraction

The force that draws oppositely charged ions together.

Crystal Lattice

The ordered structure in which ionic compounds are arranged in a solid state.

Melting Point

The temperature at which a solid becomes a liquid, affected by ionic bonding strength.

Electrolyte

A substance that conducts electricity when dissolved in water or melted.

Molecular Compound

A compound made up of molecules, typically formed by covalent bonds.

Diatomic Molecule

A molecule that contains two atoms, e.g., H2 or O2.

Triatomic Molecule

A molecule that contains three atoms.

Bonding Capacity

The number of bonds an atom can form based on its valence electrons.

Coordinate Covalent Bond

A bond in which one atom donates both electrons to be shared with another atom.

Intermolecular Forces

Attractions between molecules, including van der Waals forces and hydrogen bonds.

Polar Covalent Bond

A type of bond where electrons are shared unequally, resulting in partial charges.

Electronegativity

A measure of the ability of an atom to attract electrons in a bond.

Ionic Compounds

Compounds formed by ionic bonds, typically consisting of metals and non-metals.

Hydrogen Bonding

A strong type of intermolecular force between hydrogen and highly electronegative atoms.

Lone Pair Electrons

Valence electrons that are not involved in bonding.

Nonpolar Covalent Bond

A bond in which electrons are shared equally, typically between identical atoms.

Melting and Boiling Points of Ionic Compounds

Ionic compounds have high melting and boiling points due to strong ionic bonds.

Dipole

A molecule that has a positive end and a negative end due to electronegativity differences.

Lewis Dot Diagram

A visual representation of an atom's valence electrons using dots.

Isoelectronic

Having the same electron configuration as a noble gas.

Ionization Energy (IE)

The energy required to remove an electron from an atom or ion.

Electron Affinity (EA)

The tendency of an atom to gain or lose electrons.

Chemical Formula

A symbolic representation of a chemical compound indicating the elements and their ratios.

Properties of Covalent Compounds

Varies, can be gases, liquids, or solids with lower melting points than ionic compounds.

Electronegativity Difference

The difference in electronegativity values which determines the type of bond formed.

Van der Waals Forces

Weak attractions between molecules, contributing to the properties of covalent compounds.

HOFBrINCl

An acronym used to remember the diatomic molecules: Hydrogen, Oxygen, Fluorine, Bromine, Iodine, Nitrogen, Chlorine.

Melting Point of Water

0 °C, the temperature at which water transitions from solid to liquid.

High Conductivity

Characteristic of ionic compounds when dissolved in water, allowing for electric current to flow.