Which of the following statements concerning a covalent bond is FALSE ?

Options

A. The electrons are shared between atoms
B. The bond is non-directionsl
C. The strength of the bond depends upon the extent of overlapping
D. The bond formed may or may not be polar

Answer

To determine which statement concerning a covalent bond is false, we can analyze each statement provided.

### Step-by-step Solution:

1. **Understanding Covalent Bonds**:
- Covalent bonds are formed when two atoms share electrons. This sharing allows each atom to attain a stable electron configuration, typically resembling that of noble gases.

2. **Evaluating the First Statement**:
- The first statement claims that "electrons are shared between atoms."
- This statement is **TRUE** as it accurately describes the fundamental nature of covalent bonds.

3. **Evaluating the Second Statement**:
- The second statement claims that "the bond is non-directional."
- This statement is **FALSE**. Covalent bonds are directional due to the overlapping of atomic orbitals. The directionality influences the geometry of the molecule.

4. **Evaluating the Third Statement**:
- The third statement states that "the strength of the bond depends upon the extent of overlapping."
- This statement is **TRUE**. The greater the overlap of orbitals, the stronger the bond formed.

5. **Evaluating the Fourth Statement**:
- The fourth statement claims that "the bond may be polar or may not be polar."
- This statement is **TRUE**. Depending on the electronegativity difference between the bonded atoms, a covalent bond can be polar (like HCl) or non-polar (like H2).

6. **Conclusion**:
- The only statement that is false is the second one: "the bond is non-directional." Covalent bonds are indeed directional due to the nature of orbital overlap.

### Final Answer:
The false statement concerning a covalent bond is: **"the bond is non-directional."**

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