Hydrogen molecule differs from chlorine molecule in the following respect `:`

Options

A. hydrogen molecule is non-polar but chloride molecule is polar.
B. hydrogen molecule is polar while chlorine molecule is non-polar.
C. hydrogen molecule can form intermolecular hydrogen bonds but chloride molecule does not.
D. hydrogen molecule cannot participates in co-ordinate bond formation but chlorine molecule can.

Explanation

To analyze how the hydrogen molecule differs from the chlorine molecule, we will evaluate the provided statements step by step.

### Step 1: Evaluate the Polarity of the Molecules
- **Hydrogen Molecule (H₂)**: The hydrogen molecule consists of two hydrogen atoms bonded together. Since both atoms have the same electronegativity, the shared electrons are equally distributed. Therefore, H₂ is a non-polar molecule.
- **Chlorine Molecule (Cl₂)**: Similarly, the chlorine molecule consists of two chlorine atoms bonded together. Both chlorine atoms have the same electronegativity, leading to an equal sharing of electrons. Thus, Cl₂ is also a non-polar molecule.

**Conclusion**: Both hydrogen and chlorine molecules are non-polar. Therefore, the statement that "hydrogen is non-polar while chlorine is polar" is incorrect.

### Step 2: Analyze the Polarity of the Molecules
- The second statement claims that "hydrogen is polar while chlorine is non-polar." As established in Step 1, both molecules are non-polar. Therefore, this statement is also incorrect.

### Step 3: Examine Hydrogen Bonding
- **Hydrogen Bonding**: Hydrogen bonding occurs when a hydrogen atom is covalently bonded to a highly electronegative atom (like oxygen, nitrogen, or fluorine) and is attracted to another electronegative atom nearby.
- **Hydrogen Molecule (H₂)**: Hydrogen can form intermolecular hydrogen bonds when it is bonded to an electronegative atom.
- **Chlorine Molecule (Cl₂)**: Chlorine does not form hydrogen bonds due to its larger atomic size and lower electron density, which makes it less capable of forming such bonds.

**Conclusion**: The statement that "hydrogen can form intermolecular hydrogen bonds but chlorine cannot" is correct.

### Step 4: Assess Coordinate Bond Formation
- **Coordinate Bonds**: A coordinate bond is formed when one atom donates both electrons to a bond.
- **Hydrogen**: With an atomic number of 1, hydrogen has only one electron and cannot form coordinate bonds because it cannot donate a pair of electrons.
- **Chlorine**: Chlorine, with an atomic number of 17, has several electrons available for bonding. It can donate lone pairs to form coordinate bonds with metals.

**Conclusion**: The statement that "hydrogen cannot participate in coordinate bond formation while chlorine can" is also correct.

### Final Summary
- The correct statements are:
- Hydrogen can form intermolecular hydrogen bonds, but chlorine cannot.
- Hydrogen cannot participate in coordinate bond formation, but chlorine can.