Inert gases such as helium behave like ideal gases over a wide range of temperature .However , they condense into the solid state at very low temperatures. it indicates that at very low temperature there is a

Options

A. weak attractive force between the atoms
B. weak repulsive force between the atoms
C. strong attractive force between the atoms
D. strong repulsive atteractive between the atoms

Explanation

To solve the question regarding the behavior of inert gases like helium at low temperatures, we can break down the explanation into several steps:

### Step 1: Understanding Ideal Gas Behavior
Inert gases, such as helium, behave like ideal gases over a wide range of temperatures. This means that they follow the ideal gas law (PV = nRT) closely, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature.

**Hint:** Recall the characteristics of ideal gases and the conditions under which real gases approximate this behavior.

### Step 2: Behavior at Low Temperatures
However, at very low temperatures, these gases condense into a solid state. This indicates a change in the intermolecular forces acting between the gas atoms.

**Hint:** Think about what happens to gas particles as temperature decreases and how this affects their state.

### Step 3: Intermolecular Forces
At low temperatures, the kinetic energy of the gas particles decreases, allowing intermolecular forces to become significant. For inert gases, these forces are primarily Van der Waals forces, which are weak attractive forces that become more pronounced as the distance between atoms decreases.

**Hint:** Consider the types of intermolecular forces and how they vary with temperature and distance between particles.

### Step 4: Polarizability and Atomic Size
The strength of Van der Waals forces increases with the size of the atoms. Larger atoms have more electrons, which makes them more polarizable. This means that their electron clouds can be distorted more easily, leading to stronger temporary dipoles and thus stronger attractive forces.

**Hint:** Remember the relationship between atomic size, polarizability, and the strength of intermolecular forces.

### Step 5: Ionization Potential
As we move down the group of noble gases, the ionization potential decreases. A lower ionization potential means that it is easier for the atom to become polarizable, further enhancing the attractive forces between them.

**Hint:** Consider how ionization potential affects the stability and interactions of atoms in a gas.

### Conclusion
Thus, at very low temperatures, the strong attractive forces (Van der Waals forces) between the atoms of inert gases lead to their condensation into solid states. Therefore, the correct answer to the question is that at very low temperatures, there are strong attractive forces between the atoms.

**Final Answer:** Strong attractive forces between the atoms.