Ionic Or Electrovalent Bond

According to VSEPR (Valence Shell Electron Pair Repulsion) theory, when a molecule has 4 bond pairs and no lone pairs, the electron pairs repel each other equally in 3D space. This results in a tetrahedral geometry where the bond angles are approximately 109.5°. A classic example is methane (CH₄), where the central carbon forms four single bonds with hydrogen atoms and has no lone pairs.

The correct answer is option (A): tetrahedron

A sigma (σ) bond is the strongest type of covalent bond and is formed by the direct overlapping of orbitals along the internuclear axis. This overlap can occur in two ways:

End-to-end overlap (also called linear overlap)
Head-on overlap (essentially the same concept as end-to-end, just a different description)

Thus, both descriptions (1) and (2) refer to the same fundamental bonding mechanism that forms sigma bonds.

The correct option is (C): Both (1) and (2)

Element A forms a tripositive ion, meaning its charge is . Element B forms a dinegative ion, meaning its charge is . To balance charges in a neutral compound, the total positive and negative charges must be equal. Let the number of A atoms be , and B atoms be : The smallest whole number solution is: So the chemical formula is , balancing positive and negative charges.

The correct option is (C):

Correct answer: lose electrons

Explanation:
When a metal atom forms an ionic bond with a non-metal atom, the metal atom tends to lose electrons to achieve a stable electronic configuration (usually resembling the nearest noble gas). This results in the formation of a positively charged ion (cation).

The non-metal atom gains the electrons lost by the metal, forming a negatively charged ion (anion). The electrostatic attraction between these oppositely charged ions leads to the formation of an ionic bond.

Correct answer: Both (1) and (2)

Explanation:
An ionic bond is formed by:
1. Transfer of electrons from one atom (usually a metal) to another atom (usually a non-metal).
2. The resulting ions (a positively charged cation and a negatively charged anion) are then held together by the electrostatic force of attraction.
For example, in sodium chloride (NaCl):
Sodium donates one electron to chlorine → Na⁺ and Cl⁻
These oppositely charged ions are attracted to each other forming an ionic bond.

Therefore, both transfer of electrons and electrostatic attraction are involved.