Ionic and Covalent Compounds Flashcards

Vocabulary flashcards covering core concepts of ionic and covalent compounds, ionic charges, nomenclature, periodic trends, Lewis structures, molecular geometry, and bond polarity based on lecture notes.

Bonding

The joining of two atoms in a stable arrangement to attain the electronic configuration of the noble gas closest to them in the periodic table.

Ionic Bond

A chemical bond resulting from the transfer of valence electrons from one element (typically a metal) to another (typically a nonmetal).

Covalent Bond

A chemical bond resulting from the sharing of electrons between two atoms (typically nonmetals or a metalloid and a nonmetal).

Molecule

A discrete group of atoms that share electrons held together by covalent bonds.

Octet Rule

The principle that main group elements adjust their valence electrons to possess an octet of $8$ valence electrons in their outer shell to achieve special stability.

Cation

A positively charged ion formed when an atom (usually a metal) loses valence electrons, leaving it with fewer electrons than protons.

Anion

A negatively charged ion formed when an atom (usually a nonmetal) gains valence electrons, leaving it with more electrons than protons.

Polyatomic Ion

A cation or anion that contains more than one atom carrying an overall net charge.

Systematic Name (Nomenclature)

A method of naming cations with variable charge by following the cation name with a Roman numeral in parentheses to indicate its charge.

Common Name Cation Suffixes

The use of suffix "-ous" for a metal cation with a smaller charge and suffix "-ic" for a cation with a higher charge.

Atomic Radius Trend

The trend where atomic size increases from top to bottom in a group due to added energy levels, and decreases from left to right across a period due to an increase in protons in the nucleus.

Ionization Energy

The amount of energy needed to remove an electron from an atom.

Electronegativity

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

Lewis Structures

Representations of atoms, molecules, or ions that use dots to indicate valence electrons surrounding element symbols.

Lone Pairs (Nonbonded Electron Pairs)

Unshared pairs of valence electrons around an atom in a molecule that are not involved in chemical bonding.

VSEPR Theory

Valence Shell Electron Pair Repulsion Theory; a theory developed to predict molecular geometry by minimizing electrostatic repulsion between bonding and nonbonding electron pairs around a central atom.

Single Bond

A covalent bond in which $1$ pair of electrons ($2$ electrons) is shared between two atoms.

Double Bond

A covalent bond in which $2$ pairs of electrons ($4$ electrons) are shared between two atoms.

Triple Bond

A covalent bond in which $3$ pairs of electrons ($6$ electrons) are shared between two atoms.

Nonpolar Covalent Bond

A bond in which electrons are equally shared because the electronegativity difference between the bonded atoms is less than $0.5$ units.

Polar Covalent Bond

A bond in which electrons are unequally shared because the electronegativity difference between atoms is $0.5$\text{--}$1.9$ units.

Bond Dipole

A separation of partial positive ($\delta+$) and partial negative ($\delta-$) charges resulting from unequal electron sharing in a polar covalent bond.

Carbonate

A polyatomic anion with the formula $\text{CO}_3^{2-}$.

Nitrate

A polyatomic anion with the formula $\text{NO}_3^-$.

Sulfate

A polyatomic anion with the formula $\text{SO}_4^{2-}$.

Phosphate

A polyatomic anion with the formula $\text{PO}_4^{3-}$.

Hydroxide

A polyatomic anion with the formula $\text{OH}^-$.