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Chapter 6: Q. 6.149 (page 210)

Identify the group number in the periodic table of $X$ , a representative element, in each of the following ionic compounds: $(6.2)$
a. $X C l_{3}$
b. $A l_{2} X_{3}$
c. $X C O_{3}$

Short Answer

Expert verified

a. The group number is $3 A (13)$ .

b. The group number is $6 A (16)$ .

c. The group number is $2 A (2)$ .

Step by step solution

01

Part (a) step 1: Given Information

We need to identify the group number of $X C l_{3}$ .

02

Part (a) step 2: Simplify

Consider: $X C l_{3}$

ion of Chlorine $C l^{-}$ change of $X$ is $x$ so by change balance:

$x + 3 (1 -) = 0 x = 3 +$

Therefore, ion of $x 鈥� 鈥� 鈥� X^{3 +}$

Here, three electrons donated to achieve octect so group is $3 A (13)$ .

03

Part (b) step 1: Given Information

We need to identify the group number of $A l_{2} X_{3}$ .

04

Part (b) step 2: Simplify

Consider: $A l_{2} X_{3}$

ion of Aluminium $A l^{3 +}$ change of $X$ is $x$ so by change balance:

$3 x + 2 (3 +) = 0 x = 2 -$

Therefore ion of $x 鈥� 鈥� 鈥� X^{2 -}$

Here, two electrons accepted to achieve octect so the group is $6 A (16)$ .

05

Part (c) step 1: Given Information

We need to identify the group number of $X C O_{3}$ .

06

Part (c) step 2: Simplify

Consider: $X C O_{3}$

ios of Carbonate ${C O}_{3}^{2 -}$ charge of $X$ is $x$ so by charge balance:

$x + (2 -) = 0 x = 2 +$

Therefore, ion of $x 鈥� 鈥� 鈥� X^{2 +}$

Here, two electrons donated to achieve octect so group is $2 A (2)$ .

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Most popular questions from this chapter

Which of the following pairs of elements are likely to form an ionic compound?

a. helium and oxygen

b. magnesium and chlorine

c. chlorine and bromine

d. potassium and sulfur

e. sodium and potassium

f. nitrogen and iodine

Write the correct ionic formula for the compound formed between each of the following pairs of ions:

a. ${Al}^{3 +}$ and ${Cl}^{-}$

b. ${Ca}^{2 +}$ and $S^{2 -}$

c. ${Li}^{+}$ and $S^{2 -}$

d. ${Rb}^{+}$ and $P^{3 -}$

e. ${Cs}^{+}$ and $I^{-}$

State the number of valence electrons, bonding pairs, and lone pairs in each of the following Lewis structures:

6.11 Write the names for each of the following ions:

a. $L i^{+}$ b. $C a^{3 +}$

c. $G a^{3 +}$ d. $P^{3 -}$ localid="1654321115964" $P^{3 -}$ $P^{3 -}$

Write the name for the following:

a. $K^{+}$

b. $N a^{+}$

c. $B a^{2 +}$

d. $C l^{-}$

See all solutions

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