Bonding and Ions Review

Flashcards covering key vocabulary related to chemical bonding, ions, naming conventions, and electronegativity from Chapters 3 and 4 of the lecture.

BONDING

The joining of two atoms in a stable arrangement.

IONIC bonds

Bonds that result from the transfer of electrons from one element to another.

COVALENT bonds

Bonds that result from the sharing of electrons between two atoms.

Ionic Bonds (Formation)

Form between a metal (left side of the periodic table) and a non-metal (right side of the periodic table).

Covalent Bonds (Formation)

Formed between two nonmetals or between a metalloid and a nonmetal.

Molecule

A compound or element containing two or more atoms joined together with covalent bonds.

Ions

Charged species in which the number of protons and electrons in an atom is unequal.

Ionic compounds

Consist of oppositely charged ions that have a strong electrostatic attraction for each other.

Cations

Positively charged ions, having fewer electrons than protons, formed by losing one, two, or three electrons.

Anions

Negatively charged ions, having more electrons than protons, formed by gaining one, two, or three electrons.

Octet rule

A main group element is especially stable when it possesses an octet of electrons (8 valence electrons) in its outer shell.

Ionic Charge (Groups 1A, 2A, 3A metals)

The group number equals the charge on the cation.

Ionic Charge (Groups 6A, 7A nonmetals)

The anion charge equals 8 minus the group number.

Naming Main Group Cations

Named for the element from which they are formed (e.g., Calcium, Potassium).

Naming Anions

Named by replacing the ending of the element name by the suffix "-ide" (e.g., Chloride, Oxide).

Naming Ionic Compounds (Variable Charge Metals)

The charge on the cation is indicated by a Roman numeral in parentheses after the metal's name (e.g., copper(II) chloride).

Unshared electron pairs

Also called nonbonded electron pairs or lone pairs.

Lewis structures

Electron-dot structures for molecules that show the location of all valence electrons.

Electronegativity

A measure of an atom's attraction for electrons in a bond, indicating how much a particular atom "wants" electrons.

Nonpolar bond

A bond with an electronegativity difference less than 0.5 units, where electrons are equally shared.

Polar covalent bond

A bond with an electronegativity difference of 0.5 to 1.9 units, where electrons are unequally shared and pulled towards the more electronegative element.

Ionic bond (Electronegativity)

A bond with an electronegativity difference greater than 1.9 units, where electrons are transferred from the less electronegative element to the more electronegative element.