Draw a depiction of a gas sample, as described by kinetic molecular theory, containing equal molar amounts of helium, neon, and krypton. Use different color dots to represent each element. Give each atom a "tail" to represent its velocity relative to the others in the mixture.

The lightest gas will have the greatest molecular speed as shown

Explanation:

According to the kinetic theory of gases, gas molecules are in constant motion and frequently collide with each other and the walls of the vessel. Gas molecules have negligible intermolecular forces of attraction between them hence they move at a very high speed.

However, the distribution of molecular velocities in a mixture of gases depends on the relative molecular masses of the gases in the mixture. Given helium, neon and krypton; the order of decreasing masses and increasing molecular velocities is ; krypton<neon<helium. Hence helium being the lightest gas will have the greatest molecular velocity.

The molecular velocities of each gas has been represented using the length of arrows with different colours in the image attached. The colour codes are;

Red- krypton

Blue- neon

Black-helium

It can be seen that helium has the highest molecular velocity followed by neon and lastly, krypton.

c. electrical charges of ionic bonds.

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