Ionic and Covalent Bonding Patterns

Flashcards covering key vocabulary related to ionic and covalent bonding patterns, compound naming, and Lewis structures, based on the provided lecture notes.

Ionic compounds

Compounds in which the particles are ions, and the bond is a result of electrostatic attraction between oppositely charged species.

Covalent compounds

Compounds in which the particles are neutral molecules, discrete groups of atoms connected to each other in a specific arrangement.

Chemical formula

Expresses the composition of a compound using a combination of element symbols and subscripts.

Subscripts

Denotes the relative number of each atom or ion present in a chemical formula.

Ionic Bonding

The simplest form of bonding that results from the electrostatic attraction between a positively charged metal cation and a negatively charged anion (consisting of one or more nonmetals).

Main group metal cations

Positively charged ions formed from main group metals, named by simply adding 'ion' to the corresponding element name.

Nonmetal anions

Negatively charged ions formed from nonmetals, named by combining the first syllable of the corresponding element name with the suffix '-ide'.

Polyatomic ions

Charged species composed of more than one atom.

Roman numeral in transition metal names

Indicates the ionic charge of a transition metal cation in parentheses after the metal name, especially when the metal can form more than one cation.

Covalent bond

A bond formed by the sharing of valence electron pairs between two atoms, typically nonmetals.

Bonding pair

A pair of electrons shared between two atoms, forming a covalent bond.

Single bond

A covalent bond where two atoms share only one bonding pair of electrons.

Double bond

A covalent bond where two atoms are joined by two bonding pairs of electrons.

Triple bond

A covalent bond where two atoms are joined by three bonding pairs of electrons.

Lone pairs

Valence electron pairs on an atom that are not involved in bonding.

Octet rule

States that most atoms react to achieve a configuration with eight electrons in their outer shell.

Lewis structures

Visual representations of atomic arrangements and bonding patterns in covalent compounds, using dots for nonbonding electrons and dashes for bonding pairs.