Which of the following gives rise to the formation of bond ?

Options

A.
B.
C.
D.

Answer

To determine which of the options gives rise to the formation of a bond, we need to analyze the interactions between the orbitals based on their signs (phases). Here's a step-by-step solution:

### Step 1: Understand Orbital Overlap
- Bonds are formed when atomic orbitals overlap. The nature of this overlap (whether it is constructive or destructive) determines if a bond or an anti-bond is formed.

**Hint:** Remember that constructive interference leads to bonding, while destructive interference leads to anti-bonding.

### Step 2: Identify the Signs of the Orbitals
- Orbitals can have positive (plus) or negative (minus) signs.
- When two orbitals with the same sign overlap, they create a bonding orbital.
- When two orbitals with opposite signs overlap, they create an anti-bonding orbital.

**Hint:** Look for the signs of the orbitals in each option to determine the type of bond formed.

### Step 3: Analyze Each Option
1. **Option 1:** Plus and Plus
- Overlap leads to bonding (constructive interference).
- **Conclusion:** This option forms a bond.

2. **Option 2:** Plus and Plus
- Overlap leads to bonding (constructive interference).
- **Conclusion:** This option forms a bond.

3. **Option 3:** Minus and Plus
- Overlap leads to anti-bonding (destructive interference).
- **Conclusion:** This option does not form a bond.

4. **Option 4:** Minus and Plus
- Overlap leads to anti-bonding (destructive interference).
- **Conclusion:** This option does not form a bond.

**Hint:** Compare the signs in each option to determine if they will lead to bonding or anti-bonding.

### Step 4: Determine the Correct Option
- From the analysis, we see that the second option (Plus and Plus) is the only one that consistently leads to the formation of a bond.

**Final Conclusion:** The correct option that gives rise to the formation of a bond is **Option 2**.