1.7 Covalent Bonds and Properties

Covalent Bonding

The attraction between atoms that results from the sharing of electrons.

Multiple Bonds

Atoms share additional electrons to form filled valence shells when there are not enough valence electrons for two atoms to share one pair of electrons.

Bonding Pair

A pair of electrons shared between two atoms.

Lone Pair

A pair of electrons not involved in bonding.

Polyatomic Ions

Molecular compounds that gain electrons to complete octets on all of their atoms and form a charged ion.

Non-Polar Covalent Bond

Equal sharing of a pair of electrons by two atoms of the same electronegativity.

Polar Covalent Bond

Unequal sharing of a pair of electrons by atoms of slightly different electronegativity, resulting in partial charges.

Dipoles

Molecules with positive and negative ends due to the unequal sharing of electrons in a polar covalent bond.

Various compounds have different _____ and _____ points based on their _____ and _______ ______.

melting, boiling, bonding, molecular structure

High Melting/Boiling Point Compounds

Ionic compounds with strong electrostatic forces between oppositely charged particles.

Intermediate Melting/Boiling Point Compounds

Polar molecular compounds with dipole-dipole forces.

Low Melting/Boiling Point Compounds

Non-polar molecular compounds with weak intermolecular forces.

Intermolecular Forces

Attractive forces that act between molecules, such as dipole-dipole forces and London dispersion forces.

Dipole-Dipole Forces

Attractive forces between the positive end of one dipole and the negative end of another dipole.

Hydrogen Bonds

Stronger dipole-dipole forces between a positive hydrogen atom of one molecule and a highly electronegative atom (e.g., O, N, F) in another molecule.

Solubility in Water

Polar molecular compounds dissolve in water, while non-polar compounds do not.

Electrical Conductivity

Molecular compounds do not conduct electricity, even when dissolved in water, because electrons are shared and do not create positive and negative changes

london dispersion forces

A weak and short-lived attractive force that’s weaker than a dipole due to the movement of electrons