For the following pairs of ions, predict the formula of the simplest compound that the ions are most likely to form.

a. as3+ and cl-

b. sn2+ and p3-

c. zn2+ and o2-

d. mn4+ and s2-

Explanation:

Formation of compound -

A compound can be formed from its corresponding cation and anion ,

firstly the cation is written which is followed by the anion .

Then the valence of the cationic portion is written next to the anion as lowercase ,

and

The valence of the anionic portion is written next to the cation as lowercase  .

From the question ,

a. As³⁺ and Cl⁻

Here ,

cation = As³⁺

anion = Cl⁻

The compound formed by using the above information as,

compound = AsCl₃

b. Sn²⁺ and P³⁻

cation = Sn²⁺

anion = P³⁻

The compound formed by using the above information as,

compound = Sn₃P₂

c. Zn²⁺ and O²⁻

cation = Zn²⁺

anion = O²⁻

The compound formed by using the above information as,

compound = ZnO

The valence of both cation and anion is same hence , gets cancelled out .

d. Mn⁴⁺ and S²⁻

cation =  Mn⁴⁺

anion = S²⁻

The compound formed by using the above information as,

compound = Mn₂S₄ = MnS₂

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.