Which of the following molecule/ion has all the three types of bonds, electrovalent, covalent and co-ordinate :

Options

A. HCl
B. `NH_(4)^(+)`
C. `Cl^(-)`
D. `H_(2)O_(2)`

Answer

To determine which molecule or ion has all three types of bonds—electrovalent (ionic), covalent, and coordinate—we need to analyze each option provided in the question.

### Step-by-Step Solution:

1. **Understanding the Types of Bonds**:
- **Electrovalent (Ionic) Bond**: Formed when one atom donates an electron to another, resulting in oppositely charged ions that attract each other.
- **Covalent Bond**: Formed when two atoms share electrons.
- **Coordinate Bond**: A type of covalent bond where one atom donates both electrons to the bond, while the other atom accepts them.

2. **Analyzing Each Option**:
- **HCl**:
- Contains a covalent bond (H shares an electron with Cl).
- No ionic or coordinate bonds present.
- **NH4⁺ (Ammonium Ion)**:
- Contains covalent bonds between nitrogen and three hydrogen atoms.
- The fourth bond is a coordinate bond where nitrogen donates a pair of electrons to bond with an H⁺ ion.
- No ionic bond present.
- **Cl⁻ (Chloride Ion)**:
- A single ion with no bonds present.
- **H2O2 (Hydrogen Peroxide)**:
- Contains covalent bonds (O shares electrons with H and O).
- No ionic or coordinate bonds present.

3. **Conclusion**:
- After analyzing all the options, we find that none of the provided molecules or ions contain all three types of bonds (ionic, covalent, and coordinate).
- The only candidate with two types of bonds (covalent and coordinate) is NH4⁺, but it lacks an ionic bond.

### Final Answer:
None of the options have all three types of bonds (electrovalent, covalent, and coordinate).