Question

the electronic structures of some atoms and ions are shown.
(a) write the letters, a, b, c, d, e, f, g or h, of the electronic structures which show:
(i) atoms of two different noble gases................................ and................................
2
(ii) an ion of a group i element................................
1
(iii) an ion of a group v element................................
1
(b)
use the periodic table to deduce:
(i) the chemical symbol for ion g................................
1
(ii) the element which forms an ion with a 3+ charge and the same electronic structure as h.
1

Explanation:

Step1: Recall noble - gas electron - configurations

Noble gases have full outer shells. Atom A has 2 electrons (helium configuration) and atom F has 10 electrons (neon configuration).

Step2: Identify Group I ion

Group I elements form + 1 ions by losing one electron. Ion B has a + 1 charge and has a helium - like electron configuration after losing an electron.

Step3: Identify Group V ion

Group V elements gain 3 electrons to form ions with a - 3 charge. Ion D has a - 3 charge.

Step4: Identify ion G

Ion G has a - 1 charge and 2 electrons. It is the hydride ion, $H^-$.

Step5: Identify the element for part (b)(ii)

Ion H has 10 electrons. An element that forms a 3+ ion with 10 electrons has 13 electrons in its neutral state, which is aluminum ($Al$).

Answer:

(a)(i) A, F
(ii) B
(iii) D
(b)(i) $H^-$
(ii) $Al$