Atomic Bonding Lecture Notes

Flashcards about Atomic Bonding

Matter

Anything that has mass and occupies space.

Solid

Particles are closely packed in a regular pattern, and they vibrate/oscillate around fixed positions, having a definite shape and volume.

Liquid

Particles are still closely packed but are not in a fixed position, having a definite volume but no fixed shape.

Gas

Particles are far apart and have high kinetic energy, having neither a definite shape nor a definite volume.

Plasma

Particles are charged entities such as electrons and ions and their interactions are governed by electromagnetic forces; shape and volume can be controlled by electromagnetic forces.

Atom

The smallest units of an element that retain the chemical properties of that element, consisting of a nucleus (composed of protons + neutrons), surrounded by electrons.

Mass number (A)

Number of protons + neutrons in an atom's nucleus.

Atomic number (Z)

Number of protons in an atom's nucleus.

Isotopes

Atoms with the same number of protons but different numbers of neutrons.

Atomic weight

The weighted average mass of an element’s atoms, considering the natural abundances of its isotopes, expressed in atomic mass units (amu or u).

Principal quantum number (n)

Defines the shell energy level of an electron (K, L, M, N, O or 1, 2, 3, etc.).

Sub-shell quantum number ()

Defines the sub-shell or orbitals of an electron (s, p, d, f or 0, 1, 2, 3,…, n-1).

Magnetic quantum number (ml)

Defines the number of electron orbitals (- to +).

Spin moment quantum number (ms)

Defines the spin moment of an electron (+½ (up) or -½ (down)).

Pauli exclusion principle

Each electron state can hold no more than 2 electrons, which must have opposite spins.

FA

Attractive force between atoms.

FR

Repulsive force between atoms.

Ionic bond

Electrostatic attraction between oppositely charged ions.

Covalent bonding

Forms when two atoms share one or more pairs of electrons to achieve a stable electron configuration.

Metallic bonding

Strong electrostatic attraction between positively charged ions and a “sea” of delocalized electrons in a metal.

Van der Waals bonds

Weak intermolecular forces that arise due to temporary or permanent dipoles in atoms or molecules.

London dispersion forces

Temporary dipoles due to momentary electron shifts.

Dipole-dipole interactions

Attractions between permanent dipoles in polar molecules.

H-bonding

Strong dipole-dipole force when H bonds with N, O, or F.