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Chapter 2: Problem 90

Write the formula for each of the following compounds: a. ammonium hydrogen phosphate b. mercury(I) 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 l. cesium perchlorate

Short Answer

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

Step by step solution

01

Identify the ions

Ammonium: \(NH_4^+\) and hydrogen phosphate: \(HPO_4^{2-}\).
02

Write the formula

Combine the ions ensuring that the charges cancel out: \( (NH_4)_2HPO_4 \). b. mercury(I) sulfide
03

Identify the ions

Mercury (I): \(Hg_2^{2+}\) and sulfide: \(S^{2-}\).
04

Write the formula

Combine the ions ensuring that the charges cancel out: \(Hg_2S\). c. silicon dioxide
05

Identify the ions

Silicon: \(Si^{4+}\) and oxide: \(O^{2-}\).
06

Write the formula

Combine the ions ensuring that the charges cancel out: \(SiO_2\). d. sodium sulfite
07

Identify the ions

Sodium: \(Na^+\) and sulfite: \(SO_3^{2-}\).
08

Write the formula

Combine the ions ensuring that the charges cancel out: \(Na_2SO_3\). e. aluminum hydrogen sulfate
09

Identify the ions

Aluminum: \(Al^{3+}\) and hydrogen sulfate: \(HSO_4^-\).
10

Write the formula

Combine the ions ensuring that the charges cancel out: \(Al(HSO_4)_3\). f. nitrogen trichloride
11

Identify the atoms

Nitrogen: N and Chlorine: Cl.
12

Write the formula

Combine the atoms according to the given prefixes: \(NCl_3\). g. hydrobromic acid
13

Identify the ions

Hydrogen: \(H^+\) and bromide: \(Br^-\).
14

Write the formula

Combine the ions ensuring that the charges cancel out: \(HBr\). h. bromous acid
15

Identify the ions

Hydrogen: \(H^+\) and bromite: \(BrO_2^-\).
16

Write the formula

Combine the ions ensuring that the charges cancel out: \(HBrO_2\). i. perbromic acid
17

Identify the ions

Hydrogen: \(H^+\) and perbromate: \(BrO_4^-\).
18

Write the formula

Combine the ions ensuring that the charges cancel out: \(HBrO_4\). j. potassium hydrogen sulfide
19

Identify the ions

Potassium: \(K^+\) and hydrogen sulfide: \(HS^-\).
20

Write the formula

Combine the ions ensuring that the charges cancel out: \(KHS\). k. calcium iodide
21

Identify the ions

Calcium: \(Ca^{2+}\) and iodide: \(I^-\).
22

Write the formula

Combine the ions ensuring that the charges cancel out: \(CaI_2\). l. cesium perchlorate
23

Identify the ions

Cesium: \(Cs^+\) and perchlorate: \(ClO_4^-\).
24

Write the formula

Combine the ions ensuring that the charges cancel out: \(CsClO_4\).

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Most popular questions from this chapter

Name the compounds in parts a–d and write the formulas for the compounds in parts e–h. a. \(\operatorname{NaBr}\) b. \(\mathrm{Rb}_{2} \mathrm{O}\) c. \(\mathrm{CaS}\) d. d. \(\mathrm{AlI}_{3}\) e. strontium fluoride f. aluminum selenide g. potassium nitride h. magnesium phosphide

What is the systematic name of \(\mathrm{Ta}_{2} \mathrm{O}_{5} ?\) If the charge on the metal remained constant and then sulfur was substituted for oxygen, how would the formula change? What is the difference in the total number of protons between \(\mathrm{Ta}_{2} \mathrm{O}_{5}\) and its sulfur analog?

Which of the following explain how an ion is formed? Explain your answer. a. adding or subtracting protons to/from an atom b. adding or subtracting neutrons to/from an atom c. adding or subtracting electrons to/from an atom

For each of the following ions, indicate the total number of protons and electrons in the ion. For the positive ions in the list, predict the formula of the simplest compound formed between each positive ion and the oxide ion. Name the compounds. For the negative ions in the list, predict the formula of the simplest compound formed between each negative ion and the aluminum ion. Name the compounds. a. \(\mathrm{Fe}^{2+}\) b. \(\mathrm{Fe}^{3+}\) c. \(\mathrm{Ba}^{2+}\) d. \(\mathrm{Cs}^{+}\) e. \(\mathrm{S}^{2-}\) f. \(\mathrm{P}^{3-}\) g. \(\mathrm{Br}^{-}\) h. \(\mathrm{N}^{3-}\)

In Section 1.1 of the text, the concept of a chemical reaction was introduced with the example of the decomposition of water, represented as follows: Use ideas from Dalton’s atomic theory to explain how the above representation illustrates the law of conservation of mass.
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