Bonding In Metal Carbonyls

To solve the problem, we need to identify which of the given molecules contains a triple covalent bond.

1. Understanding Triple Bonds:
A triple bond consists of one sigma (σ) bond and two pi (π) bonds. It is the strongest and shortest type of covalent bond between two atoms.

2. Analyzing the Given Molecules:
- : Oxygen molecules contain a double bond between the two oxygen atoms.
- : Nitrogen molecules contain a triple bond between the two nitrogen atoms, making them very stable.
- : Hydrogen molecules contain a single bond between the two hydrogen atoms.
- : Chlorine molecules also contain a single bond.

Final Answer:
The molecule that has a triple bond is .

To solve the problem, we need to identify which among the given compounds is not an ionic compound.

1. Understanding Ionic Compounds:
Ionic compounds are formed by the transfer of electrons from a metal to a non-metal, resulting in the formation of positive and negative ions that are held together by strong electrostatic forces.

2. Analyze the Given Compounds:
- : Formed by sodium (metal) and oxygen (non-metal) → Ionic
- : Formed by magnesium (metal) and chlorine (non-metal) → Ionic
- : Formed by sodium (metal) and chlorine (non-metal) → Ionic
- : Although it appears ionic, beryllium has a small size and high charge density, and forms covalent bonds with chlorine due to polarization.

3. Key Concept:
Beryllium chloride ( ) is predominantly covalent due to the polarizing power of the Be²⁺ ion, which distorts the electron cloud of Cl⁻.

Final Answer:
The compound that is not an ionic compound is BeCl₂.

To solve the problem, we need to determine the bond angle in a methane ( ) molecule.

1. Molecular Structure of :
Methane has a tetrahedral molecular geometry. The carbon atom is at the center, with four hydrogen atoms symmetrically arranged around it.

2. VSEPR Theory:
According to the Valence Shell Electron Pair Repulsion (VSEPR) theory, in a tetrahedral geometry, the electron pairs around the central atom repel each other and arrange themselves as far apart as possible. This results in a bond angle of approximately .

3. Common Bond Angles for Comparison:
- : Typical of bent molecules like
- : Tetrahedral geometry (as in ) ✅
- : Trigonal planar geometry
- : Linear geometry

Final Answer:
The bond angle in molecule is .