Chemical Bonds: Practice Problems - Solutions BCHEM 143

This set of flashcards covers key concepts related to chemical bonds, including definitions and characteristics of covalent bonds, ionic compounds, electronegativity, resonance structures, and others important for understanding molecular interactions.

Covalent bond

A bond formed by the sharing of electrons between atoms.

Bond length

The distance between the nuclei of two bonded atoms.

Bond energy

The amount of energy required to break a bond.

Polarity

The distribution of electrical charge over the atoms joined by the bond.

Electronegativity

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

Resonance structures

Different ways to draw the same molecule that shows delocalized electrons.

Lewis structure

A diagram that shows the bonding between atoms of a molecule and the lone pairs of electrons.

Formal charge

The charge an atom would have if all bonded electrons were shared equally.

Hypervalent

Describes molecules in which one or more atoms have more than eight electrons around them.

Radical

A molecule that contains an unpaired electron.

Ion

An atom or molecule with a net electric charge due to the loss or gain of one or more electrons.

Single bond

A chemical bond in which one pair of electrons is shared between two atoms.

Double bond

A chemical bond in which two pairs of electrons are shared between two atoms.

Triple bond

A chemical bond in which three pairs of electrons are shared between two atoms.

Ionic compound properties

Properties like low electrical conductivity in solid form and high melting/boiling points due to strong ionic bonds.

Bonding patterns in Lewis structures

Indicates how many bonds elements prefer to form based on their valence electrons.

Bond strength

The measure of how much energy is required to break a bond between two atoms.