NAT Chemistry MCQs

Forming Na+ removes the outer 3s electron.
The cation is smaller than the neutral atom.

Adding an electron increases electron-electron repulsion.
The anion is larger than the neutral atom.

Ionic bonding follows electron transfer and ion formation.
The resulting cations and anions attract in a lattice.

Covalent bonds commonly form between nonmetal atoms.
Shared electrons are attracted to both nuclei.

Metallic bonding explains conductivity and malleability.
Valence electrons move through the metal lattice.

Bond polarity arises from electronegativity differences.
The more electronegative atom gains partial negative charge.

Identical atoms form nonpolar covalent bonds.
Small electronegativity differences also give nearly nonpolar bonds.

After formation, a coordinate bond behaves like an ordinary covalent bond.
The electron-pair donor provides both bonding electrons.

Thomson's cathode-ray experiments revealed negatively charged particles.
He proposed an early model with electrons in positive matter.

Periodic trends arise from repeating valence-shell patterns.
The periodic table organizes these regularities.

Chadwick identified the neutral nuclear particle in 1932.
Neutrons explain isotopic mass differences.

Alkali metals have one valence electron.
They commonly form +1 ions and are highly reactive.