Group 15 Elements - Properties Quiz

The electrons in the outermost energy level of an atom that are involved in chemical bonding. For group 15 elements, it's ns²np³.

The measure of how easily an atom can lose an electron. It decreases down group 15 due to increasing atomic size.

The distance between the center of an atom and its outermost electron. It increases down the group but shows a smaller increase from As to Bi due to filled d and f orbitals.

Group 15 elements have a higher ionization enthalpy compared to group 14 elements in the same period because of their half-filled p orbital configuration and smaller size.

The energy required to remove successive electrons from an atom. Each subsequent ionization enthalpy is higher than the previous one (∆iH1 < ∆iH2 < ∆iH3).

The outermost energy level of an atom that contains the electrons involved in chemical bonding. For Group 15 elements, it's ns²np³. This configuration makes the elements extra stable.

The distance between the center of two bonded atoms. It generally increases down the group, but there's a smaller increase from As to Bi due to filled d and f orbitals in heavier members.

The energy required to remove one electron from a neutral atom in its gaseous state. It generally decreases down the group due to an increase in atomic size.

Group 15 elements have a higher ionization enthalpy compared to Group 14 elements in the same period because of their half-filled p orbital configuration and smaller size.

The energy required to remove successive electrons from an atom. It generally increases with each successive ionization, following the order ∆ i H 1 < ∆ i H 2 < ∆ i H 3.