Let's analyze each statement to determine which ones are correct:

Analyzing Statement (A): Hydrogen Bond vs Covalent Bond Strength

Statement (A) claims that a hydrogen bond is weaker than a covalent bond. This is generally true. A hydrogen bond is a type of intermolecular force, meaning it occurs between different molecules or different parts of a large molecule. It is an attraction between a hydrogen atom covalently bonded to a highly electronegative atom (like N, O, or F) and another nearby electronegative atom. In contrast, a covalent bond is an intramolecular force, holding atoms together within a single molecule by sharing electrons. Covalent bonds are significantly stronger than hydrogen bonds. For example, the energy of a covalent bond is typically in the range of 150-1100 kJ/mol, while a hydrogen bond is typically in the range of 5-50 kJ/mol.

Analyzing Statement (B): Methane ($CH_4$) Bonding

Statement (B) states that $CH_4$ has covalent bonds. Methane ($CH_4$) is a molecule where a central carbon atom is bonded to four hydrogen atoms. The bonds are formed by the sharing of electrons between the carbon atom and each hydrogen atom. This sharing of electrons is the definition of a covalent bond. Therefore, statement (B) is correct.

Analyzing Statement (C): Covalent Compounds Conductivity

Statement (C) claims that covalent compounds do not conduct electricity except diamond. Most covalent compounds, like methane or water, exist as discrete neutral molecules and lack free-moving charged particles (ions or electrons), so they do not conduct electricity in any state (solid, liquid, or gas). However, diamond is a covalent network solid where carbon atoms are bonded covalently in a tetrahedral structure. Diamond is an electrical insulator, meaning it does not conduct electricity. The statement implies that diamond *does* conduct electricity ("except diamond"), which is false. Therefore, statement (C) is incorrect.

Analyzing Statement (D): Graphite Properties

Statement (D) states that graphite is a soft solid and a good conductor of electricity. Graphite has a layered structure. Within each layer, carbon atoms are strongly bonded covalently in hexagonal rings. However, the forces between these layers are weak van der Waals forces, making graphite soft and easily cleavable, allowing it to be used as a lubricant and in pencils. Furthermore, due to the delocalization of electrons within the layers (each carbon atom forms three covalent bonds, leaving one valence electron per atom delocalized), graphite is a good conductor of electricity. Therefore, statement (D) is correct.

Conclusion on Correct Statements

Based on the analysis:

• Statement (A) is correct (Hydrogen bonds are weaker than covalent bonds).
• Statement (B) is correct ($CH_4$ has covalent bonds).
• Statement (C) is incorrect (Diamond does not conduct electricity).
• Statement (D) is correct (Graphite is soft and conducts electricity).

Thus, the correct statements are (A), (B), and (D).

Identifying the Correct Option

Comparing our findings with the given options:

• Option 1: (A), (B) and (D) only. - This matches our conclusion.
• Option 2: (A), (B) and (C) only. - Incorrect because (C) is false.
• Option 3: (A), (B), (C) and (D). - Incorrect because (C) is false.
• Option 4: (B), (C) and (D) only. - Incorrect because (A) is true and (C) is false.

The correct option is 1.