Fundamentals of Inorganic Chemistry - The Periodic Table

These flashcards cover key concepts from the lecture on the periodic table and various properties of elements.

Atomic Weight

The total number of protons and neutrons in an atom.

Atomic Number

The number of protons in the nucleus of an atom, unique to each element.

Electron Configuration

The distribution of electrons in atomic orbitals.

Quantum Numbers

A set of four numbers that describe the state of an electron in an atom.

Hund’s Rule

Electrons will occupy degenerate orbitals singly before pairing begins.

Halogens

Group 17 elements: F, Cl, Br, I, At.

Chalcogens

Group 16 elements: O, S, Se, Te, Po.

Pnictogens

Group 15 elements: N, P, As, Sb, Bi.

Alkali Metals

Group 1 elements: Li, Na, K, Rb, Cs, Fr.

Alkali Earth Metals

Group 2 elements.

Ionization Potential (IP)

The energy required to remove an electron from an isolated atom in the gas phase.

Shielding Effect

The reduction in effective nuclear charge on the electrons from the attraction of other electrons.

Covalent Radius

Half the distance between two atoms bonded covalently.

Atomic Radius

Overall size of an atom, which includes covalent and metallic radii.

Electronegativity

A measure of the tendency of an atom to attract a bonding pair of electrons.

Oxidation State

The charge of an atom in a molecule, determined by the number of electrons lost or gained.

Diagonal Relationships

Similar properties of elements located diagonally across the periodic table from each other.

Metallic Character

A measure of how easily an element can lose an electron; increases down a group.

Lanthanide Contraction

The decrease in ionic radii caused by poor shielding by f-electrons.

Transition Metals

Elements that have partially filled d orbitals.

Noble Gases

Group 18 elements, known for their lack of reactivity.

Catenation

The ability of an element to form bonds with itself.