Periodic Patterns in the Main-Group Metals

Vocabulary flashcards covering periodic trends, oxide properties, and related energetic concepts from the lecture notes.

Ionization Energy

Energy required to remove an electron; increases left-to-right across a period and up a group, mirroring Zeff.

Effective Nuclear Charge (Zeff)

Net positive charge felt by valence electrons; rises across a period, leading to higher ionization energies.

Electron Affinity

Energy change when an atom gains an electron; becomes more negative up and to the right, highest for nonmetals.

Atomic Size (Atomic Radius)

Distance from nucleus to outermost electrons; decreases across a period and up a group.

Reactivity (Groups 1A & 7A)

Tendency to react; greatest for alkali metals and halogens at opposite ends of the table (excluding noble gases).

Electronegativity

Ability of an atom in a bond to attract electrons; rises across a period and up a group, with F > Cl.

Nonmetallic Character

How much an element behaves like a nonmetal; increases up and to the right on the periodic table.

Metallic Character

Extent to which an element shows metallic properties; increases down and to the left on the periodic table.

Electropositivity

Tendency of an atom to donate electrons; increases down a group.

Covalent Oxides

Oxides whose bonding is largely covalent; more common for elements up and to the right on the periodic table.

Ionic Oxides

Oxides with predominantly ionic bonding; favored for elements down and to the left on the periodic table.

Acidity of Oxides

Acidic behavior of an oxide; increases for oxides of elements up and to the right.

Basicity of Oxides

Basic behavior of an oxide; increases for oxides of elements down and to the left.

Hydration Energy

Energy released when gaseous ions are solvated by water; higher for higher charged ions and, for equal charge, smaller ions.

Lattice Energy

Energy released when gaseous ions form an ionic solid; conceptually similar in magnitude (opposite sign) to hydration energy.

Covalent Character of Oxides

Degree to which an oxide’s bonding is covalent; follows trend SO₃ > P₂O₅ > As₂O₅ > Sn₂O > SrO.