Electron affinity for a noble gas is appoximately equal to

Options

A. that of halogens
B. zero
C. that of oxygen family
D. that of nitrogen family

Explanation

To determine the electron affinity of noble gases, we can follow these steps:

### Step 1: Define Electron Affinity
Electron affinity is the amount of energy released when an electron is added to a neutral atom in the gas phase. It indicates the tendency of an atom to accept an electron.

**Hint:** Remember that electron affinity measures how much an atom wants to gain an electron.

### Step 2: Understand Noble Gases
Noble gases, which include helium, neon, argon, krypton, xenon, and radon, have a complete valence shell (octet) of electrons. This means they have a stable electron configuration.

**Hint:** Recall that noble gases are known for their stability and low reactivity due to their filled outer electron shells.

### Step 3: Analyze the Stability of Noble Gases
Since noble gases have completely filled outer shells, they do not have a tendency to gain additional electrons. Gaining an electron would disrupt their stable configuration, making them less stable.

**Hint:** Consider why atoms generally prefer to maintain stability rather than gain electrons.

### Step 4: Conclude the Electron Affinity of Noble Gases
Because noble gases do not favor the addition of electrons due to their stable electron configuration, their electron affinity is effectively zero. This means they do not release energy when an electron is added, as they do not accept electrons.

**Hint:** Think about the relationship between stability and energy changes when electrons are added to atoms.

### Final Answer
The electron affinity for a noble gas is approximately equal to zero.