Ionic and Covalent Bonding, Solutions, and Concentration Concepts

A collection of flashcards summarizing key concepts related to ionic and covalent bonding, as well as solution and concentration terminology.

Ionic bond

Electrostatic attraction between oppositely charged ions.

Lewis electron dot symbol

Element symbol showing valence electrons as dots.

Lattice energy

Energy released when ions form a solid crystal.

Covalent bond

Shared electron pair between two atoms.

Lewis electron dot formula

Diagram showing bonding and lone pairs in molecules.

Bonding pair

Electron pair shared between two atoms.

Nonbonding (lone) pair

Unshared electron pair on an atom.

Octet rule

Atoms tend to gain eight valence electrons.

Single bond

One shared electron pair between atoms.

Double bond

Two shared electron pairs between atoms.

Triple bond

Three shared electron pairs between atoms.

Polar covalent bond

Unequal sharing of electrons between two atoms.

Electronegativity

Atom's ability to attract bonding electrons.

Delocalized bonding

Electrons spread across multiple atoms.

Resonance forms

Multiple valid Lewis structures for one molecule.

Bond (dissociation) energy

Energy needed to break a bond.

Molecular geometry (structure)

Three-dimensional shape of a molecule.

VSEPR

Electron pairs arrange to minimize repulsion.

Dipole moment

Measure of bond or molecular polarity.

Vector

Quantity having both magnitude and direction.

Formal charge

Hypothetical charge assigned to an atom.

Valence bond theory

Bonds form from overlapping atomic orbitals.

Hybrid orbitals

Mixed atomic orbitals creating new equivalent orbitals.

Sigma (σ) bond

Head-on orbital overlap along the bonding axis.

Pi (π) bond

Sideways orbital overlap above and below the bonding axis.

Multiple bonds

Two or three pairs shared between atoms.

Bonding orbital

Orbital that stabilizes and holds atoms together.

Antibonding orbital

Orbital that destabilizes the bond between atoms.

Bond order

Number of bonding pairs between two atoms.

Diamagnetic

All electrons paired, not attracted to magnets.

Paramagnetic

Unpaired electrons, attracted to magnetic fields.

Molecular orbital

Orbital belonging to the entire molecule.

Molecular orbital theory

Electrons occupy orbitals spanning the whole molecule.

Node

Region of zero electron density in orbital.

Overlap

Sharing of orbital space between two atoms.

Aqueous solution

Substance dissolved in water as solvent.

Concentrated

Solution with a relatively large amount of solute.

Concentration

Amount of solute per unit of solution.

Dilute

Solution with a relatively small amount of solute.

Dilution

Reducing concentration by adding more solvent.

Dissolved

Solute uniformly distributed throughout the solvent.

Formula mass

Sum of atomic masses in a formula unit.

Molar mass

Mass of one mole of a substance.

Molarity

Moles of solute per liter of solution.

Mole

6.022 imes 10^{23} units of a substance.

Percent composition

Percentage of each element in a compound.

Mass percentage (percent by mass)

Solute mass divided by solution mass.

Solute

Substance that gets dissolved in a solution.

Solvent

Substance that dissolves the solute.