Question

Which of the following are correct statements?

(A) Hydrogen bond is weaker than covalent bond.
(B) CH\(_4\) has covalent bonds.
(C) Covalent compounds do not conduct electricity except diamond.
(D) Graphite is a soft solid and a good conductor of electricity.
Choose the correct answer from the options given below:

• A. (A), (B) and (D) only.
• B. (A), (B) and (C) only.
• C. (A), (B), (C) and (D).
• D. (B), (C) and (D) only.

Hint:

Hydrogen bonds are weaker than covalent bonds. Graphite is soft and conductive, while covalent compounds generally do not conduct electricity.

Answer 1

The Correct Option is A

Step 1: Hydrogen Bonding.
- Hydrogen bonds are weaker than covalent bonds. A hydrogen bond is an attractive force between a hydrogen atom covalently bonded to a more electronegative atom (e.g., oxygen, nitrogen) and another electronegative atom.
Step 2: Covalent Bonding in CH\(_4\).
- CH\(_4\) (methane) has covalent bonds between carbon and hydrogen atoms.
Step 3: Conductivity of Covalent Compounds.
- Covalent compounds generally do not conduct electricity unless they are in molten form or dissolved in water. However, diamond is an exception because it is a covalent network solid that does not conduct electricity.
Step 4: Graphite Properties.
- Graphite is a soft solid and a good conductor of electricity due to the mobility of electrons between layers.
Step 5: Conclusion.
Thus, the correct statements are:
- Hydrogen bond is weaker than covalent bond.
- CH\(_4\) has covalent bonds.
- Graphite is a soft solid and a good conductor of electricity.
Final Answer: \[ \boxed{\text{(A), (B) and (D) only}} \]