As compared to `^12C` atom, `^14C` atoms has

Options

A. two extra protons and two extra electrons
B. two extra protons but no extra electron
C. two extra neutrons and no extra electron
D. two extra neutrons and two extra electrons

Answer

To solve the question regarding the comparison between the `^12C` and `^14C` atoms, we will follow these steps:

### Step 1: Understanding the Notation
The notation `^A_ZX` represents a nucleus where:
- `A` is the mass number (total number of protons and neutrons).
- `Z` is the atomic number (number of protons).
- `X` is the chemical symbol of the element.

For `^12C`, the mass number is 12, and for `^14C`, the mass number is 14.

### Step 2: Identify the Atomic Number
Both `^12C` and `^14C` are isotopes of carbon. The atomic number (Z) of carbon is 6, which means both isotopes have 6 protons.

### Step 3: Calculate the Number of Neutrons
To find the number of neutrons in each isotope, we use the formula:
\[ \text{Number of Neutrons} = \text{Mass Number} - \text{Atomic Number} \]

For `^12C`:
- Mass Number = 12
- Atomic Number = 6
- Number of Neutrons = 12 - 6 = 6

For `^14C`:
- Mass Number = 14
- Atomic Number = 6
- Number of Neutrons = 14 - 6 = 8

### Step 4: Compare the Number of Neutrons
Now we compare the number of neutrons in both isotopes:
- `^12C` has 6 neutrons.
- `^14C` has 8 neutrons.

Thus, `^14C` has 2 more neutrons than `^12C`.

### Step 5: Compare the Number of Protons and Electrons
Since both isotopes are neutral atoms, the number of protons equals the number of electrons:
- Both `^12C` and `^14C` have 6 protons and 6 electrons.

### Conclusion
In summary, as compared to `^12C`, `^14C` has:
- 2 extra neutrons and no extra electrons.

### Final Answer
The correct statement is: `^14C` has 2 extra neutrons and no extra electrons compared to `^12C`.

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