Pakistan MCQs

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

Use v=u+at.
V=5+2×6 = 17 m/s.

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.

The octet rule is a useful main-group bonding guideline.
Hydrogen, boron, and expanded-valence species are exceptions.

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

Lewis structures use lines and dots for bonds and lone pairs.
They help predict connectivity and formal charge.

Halogens have seven valence electrons.
They commonly form -1 ions.

Lone pairs influence shape and reactivity.
They repel bonding pairs strongly in VSEPR theory.