Question

Consider an ion with the symbol $Y^{3-}$formed from a representative element.

a. What is the group number of the element?

b. What is the Lewis symbol of the element?

c. If $Y$is in Period $3$, what is the element?

d. What is the formula of the compound formed from $Y$and

the barium ion?

Short answer

a. Group number of the element will be $15$,

b. Lewis symbol is given below.

c. The element will be phosphide.

d. The formula of the compound formed from $Y$and barium ion is $B{a}_3{Y}_2$.

Step-by-step solution

Part(a) Step 1: Given information

We need to find the group number of respective element.

Part(a) Step 2: Explanation

As the element lacks three electrons in outermost shell to achieve noble gas configuration so the group number will be$15$.

Part(b) Step 1: Given information

We need to find the Lewis symbol for the given element.

Part(b) Step 2: Explanation

As it has achieved noble gas configuration so it has $8$electrons in outermost shell so the Lewis symbol will be

Part(c) Step 1: Given information

We need to find the element with period number $3$and group number $15$.

Part(c) Step 2: Explanation

The element with group number $15$and period $3$is magnesium with symbol $P^{3-}$.

Part(d) Step 1: Given information

We need to find the formula of the compound formed between $Y$and Barium.

Part(d) Step 2: Explanation

Oxidation state of $Y$is $3-$.

Oxidation state of Barium is $+2$.

So the formula of compound will be$B{a}_3{Y}_{2_{}}$.