Atomic Properties and Chemical Bonds

These flashcards cover the key concepts from the lecture on atomic properties and chemical bonds, including definitions and important principles.

Ionic Bonding

Involves transfer of electrons, usually between metals and nonmetals.

Covalent Bonding

Involves sharing of electrons, typically occurring between nonmetals.

Metallic Bonding

Involves electron pooling when metals bond together.

Lewis Dot Symbols

Represent the valence electrons of main group elements with dots.

Octet Rule

Atoms bond to achieve a full outer shell of 8 electrons (or 2 for hydrogen).

Lattice Energy

Measure of the strength of an ionic bond and the enthalpy change for separating one mole of a solid ionic compound into gaseous ions.

Coulomb's Law

Describes the effect of charge and distance on ionic lattice energy.

Electronegativity

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

Bond Order

The number of shared electron pairs between two atoms; higher bond order indicates shorter and stronger bonds.

Resonance Structures

Structures that depict delocalized electrons within certain molecules that cannot be expressed by a single Lewis structure.

Formal Charge

The charge assigned to an atom in a molecule, calculated by taking the number of valence electrons and subtracting bonds and non-bonding electrons.

Valence Shell Electron Pair Repulsion (VSEPR) Theory

A model used to predict the geometry of individual molecules based on the repulsion of electron pairs.

Bond Angles

The angle formed between three atoms across at least two bonds.

Molecular Polarity

Determined by the shape and distribution of charge within a molecule, affecting its dipole moment.

electrostatic force

proportional to the product of their charges divided by the square of the distance between them (q1*q2/r)

The electrostatic potential energy

proportinal to the product of the charges divided by the distance between them (E = q1 * q2/r)

effects of ionic charge on lattice energy

energy increases as the magnitude of the charge increases

effects of ion size on lattice energy

inverse relationship, as size increases the energy decreases