To determine which statements are wrong, we will analyze each statement one by one.
### Step 1: Analyze Statement A
**Statement A:** Photons having energy 400 kilojoules will break 4 moles of bond of molecule A where the bond dissociation energy is 100 kilojoules per mole.
**Analysis:**
- The energy required to break 4 moles of bonds is calculated as:
\[
\text{Total energy required} = \text{Bond dissociation energy} \times \text{Number of moles} = 100 \, \text{kJ/mol} \times 4 \, \text{mol} = 400 \, \text{kJ}
\]
- The statement implies that 400 kJ of energy will always break 4 moles of bonds, but it does not specify the number of photons involved. The energy of the photons must match the energy required to break the bonds, and the number of photons must equal the number of moles multiplied by Avogadro's number to ensure all bonds are broken.
- Therefore, this statement is ambiguous and can be considered wrong.
### Step 2: Analyze Statement B
**Statement B:** Two bulbs are emitting light having wavelengths 2000 angstroms and 3000 angstroms respectively. If bulb A and B are 40 Watts and 30 Watts respectively, then the ratio of the number of photons emitted by A and B is 1:2.
**Analysis:**
- The energy of a photon can be calculated using the formula:
\[
E = \frac{1240}{\lambda} \, \text{(in eV)}
\]
where \(\lambda\) is in angstroms.
- For bulb A (2000 angstroms):
\[
E_A = \frac{1240}{2000} \, \text{eV} = 0.62 \, \text{eV}
\]
- For bulb B (3000 angstroms):
\[
E_B = \frac{1240}{3000} \, \text{eV} \approx 0.4133 \, \text{eV}
\]
- The number of photons emitted can be calculated as:
\[
\text{Number of photons} = \frac{\text{Power} \times \text{Time}}{\text{Energy of one photon}}
\]
- For bulb A:
\[
N_A = \frac{40 \times 86400}{0.62 \times 1.6 \times 10^{-19}} \, \text{(in photons)}
\]
- For bulb B:
\[
N_B = \frac{30 \times 86400}{0.4133 \times 1.6 \times 10^{-19}} \, \text{(in photons)}
\]
- The ratio \(N_A:N_B\) does not equal 1:2, hence this statement is also wrong.
### Step 3: Analyze Statement C
**Statement C:** When an electron makes a transition from lower to higher orbit, a photon is emitted.
**Analysis:**
- This statement is incorrect because a photon is emitted when an electron transitions from a higher energy level (excited state) to a lower energy level (ground state). The transition from lower to higher orbit requires energy absorption, not emission.
- Therefore, this statement is wrong.
### Conclusion
The wrong statements are:
- **A**: Ambiguous regarding the number of photons.
- **B**: Incorrect ratio of photons emitted.
- **C**: Incorrect understanding of photon emission during electron transitions.
### Final Answer
The wrong statements are A, B, and C.
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