Consider an ion with the symbol X2+ formed from a representative element. (5.2, 5.3)a. What is the group number of the element?b. What is the electron-dot symbol of the element?c. If X is in Period 3, what is the element?d. What is the formula of the compound formed from X and the nitride ion?

a) the element belongs to group 2

b) see image attached

c) Magnesium

d) X3N2

Explanation:

Any ion with the formula X^2+ was derived from group 2 elements. The group two element found in period 3 is magnesium alone.

Since the nitride ion has a valency of -3 and X^2+ has a valency of +2 , then a compound formed between X^2+ and the nitride ion will have the formula X3N2.

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

24