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Chapter 2: Problem 86

Write the formula for each of the following compounds: a. ammonium hydrogen phosphate b. mercury(1) sulfide c. silicon dioxide d. sodium sulfite e. aluminum hydrogen sulfate f. nitrogen trichloride g. hydrobromic acid h. bromous acid i. perbromic acid j. potassium hydrogen sulfide k. calcium iodide I, cesium perchlorate

Short Answer

Expert verified
a. \((NH_4)_2HPO_4\) b. \(Hg_2S\) c. \(SiO_2\) d. \(Na_2SO_3\) e. \(Al_2(HSO_4)_3\) f. \(NCl_3\) g. \(HBr\) h. \(HBrO_2\) i. \(HBrO_4\) j. \(KHS\) k. \(CaI_2\) l. \(CsClO_4\)

Step by step solution

01

a. ammonium hydrogen phosphate

Write the formula using the ions ammonium (NH₄⁺), hydrogen (H⁺), and phosphate (PO₄³⁻). The compound contains one phosphate ion, two ammonium ions, and one hydrogen ion to balance the charges, so the formula is (NH₄)₂HPO₄.
02

b. mercury(1) sulfide

Write the formula with mercury(I) ion (Hg₂²⁺) and sulfide ion (S²⁻). In this case, there is one mercury(I) ion and one sulfide ion, giving the formula Hg₂S.
03

c. silicon dioxide

Create a formula using silicon (Si) ions and oxygen ions (O²⁻), remembering that silicon typically has a charge of +4. Since two oxygen ions with a charge of -2 balance the charge of silicon, the formula is SiO₂.
04

d. sodium sulfite

Write the formula using sodium ions (Na⁺) and sulfite ions (SO₃²⁻). The compound contains one sulfite ion and two sodium ions to balance the charges, resulting in the formula Na₂SO₃.
05

e. aluminum hydrogen sulfate

Make a formula considering aluminum ions (Al³⁺), hydrogen ions (H⁺), and sulfate ions (SO₄²⁻). The compound must have two aluminum ions, one hydrogen ion, and three sulfate ions to achieve a neutral charge, leading to the formula Al₂(HSO₄)₃.
06

f. nitrogen trichloride

Combine nitrogen (N) ions (with a typical charge of -3) with chlorine (Cl) ions (with a charge of -1) to form a neutral compound. The formula is NCl₃ due to the 1:3 ratio of nitrogen to chlorine atoms, required to balance the charge.
07

g. hydrobromic acid

Write the formula using hydrogen ions (H⁺) and bromide ions (Br⁻). Hydrobromic acid is a binary acid, so the formula directly reflects the ions involved: HBr.
08

h. bromous acid

Use hydrogen ions (H⁺) and bromite ions (BrO₂⁻) to form the formula. Bromous acid is an oxyacid with the formula HBrO₂.
09

i. perbromic acid

Combine hydrogen ions (H⁺) with perbromate ions (BrO₄⁻) to form the formula. The formula for perbromic acid is HBrO₄.
10

j. potassium hydrogen sulfide

Create a formula using potassium ions (K⁺), hydrogen ions (H⁺), and sulfide ions (S²⁻). For a neutral compound, combine one potassium ion, one hydrogen ion, and one sulfide ion, resulting in the formula KHS.
11

k. calcium iodide

Write the formula using calcium ions (Ca²⁺) and iodide ions (I⁻). The compound consists of one calcium ion and two iodide ions to balance the charges, yielding the formula CaI₂.
12

I. cesium perchlorate

Formulate the compound using cesium ions (Cs⁺) and perchlorate ions (ClO₄⁻). The neutral formula consists of one cesium ion and one perchlorate ion, giving the formula CsClO₄.

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