Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 3: Problem 117

Write the formula for each of the following compounds: a. sulfur difluoride b. sulfur hexafluoride c. sodium dihydrogen phosphate d. lithium nitride e. chromium(III) carbonate f. \(\operatorname{tin}(\text { II })\) fluoride g. ammonium acetate h. ammonium hydrogen sulfate i. cobalt(III) nitrate J. mercury(I) chloride k. potassium chlorate 1\. sodium hydride

Short Answer

Expert verified
a. \(SF_2\) b. \(SF_6\) c. \(NaH_2PO_4\) d. \(Li_3N\) e. \(Cr_2(CO_3)_3\) f. \(SnF_2\) g. \((NH_4)CH_3COO\) h. \((NH_4)HSO_4\) i. \(Co(NO_3)_3\) j. \(HgCl\) k. \(KClO_3\) l. \(NaH\)

Step by step solution

01

a. Sulfur difluoride

Sulfur is represented by the symbol S. Fluorine is represented by the symbol F. "Di" means two. Sulfur forms a -2 charge when combined with Fluorine, which forms a -1 charge. To balance the charges, we need one sulfur atom and two fluorine atoms. Thus, the formula for sulfur difluoride is \(SF_2\).
02

b. Sulfur hexafluoride

Similar to sulfur difluoride, sulfur is represented by the symbol S, and fluorine is represented by the symbol F. "Hexa" means six. In this case, sulfur forms a +6 charge and fluorine forms a -1 charge. We need one sulfur atom and six fluorine atoms to balance the charges. So, the formula for sulfur hexafluoride is \(SF_6\).
03

c. Sodium dihydrogen phosphate

Sodium is represented by the symbol Na, hydrogen by the symbol H, and phosphate by the symbol \(PO_4\). Sodium forms a +1 charge, Hydrogen forms a +1 charge and phosphate forms a -3 charge. "Di" means two, referring to two hydrogen atoms. To balance the charges, we need one sodium atom, two hydrogen atoms, and one phosphate atom. Therefore, the formula for sodium dihydrogen phosphate is \(NaH_2PO_4\).
04

d. Lithium nitride

Lithium is represented by the symbol Li and nitrogen by the symbol N. Lithium forms a +1 charge, and nitrogen forms a -3 charge. To balance the charges, we need three lithium atoms and one nitrogen atom. The formula for lithium nitride is \(Li_3N\).
05

e. Chromium(III) carbonate

Chromium is represented by the symbol Cr and carbonate by the symbol \(CO_3\). Chromium(III) refers to a chromium ion with a +3 charge, and carbonate has a -2 charge. To balance the charges, we need two chromium atoms and three carbonate atoms. Therefore, the formula for chromium(III) carbonate is \(Cr_2(CO_3)_3\).
06

f. Tin(II) fluoride

Tin is represented by the symbol Sn and fluorine by the symbol F. Tin(II) refers to a tin ion with a +2 charge, and fluorine forms a -1 charge. To balance the charges, we need one tin atom and two fluorine atoms. The formula for tin(II) fluoride is \(SnF_2\).
07

g. Ammonium acetate

Ammonium is represented by the symbol \(NH_4\), and acetate is represented by the symbol \(CH_3COO\). Ammonium forms a +1 charge and acetate forms a -1 charge. Since the charges are already balanced, the formula for ammonium acetate is \((NH_4)CH_3COO\).
08

h. Ammonium hydrogen sulfate

Ammonium is represented by the symbol \(NH_4\), and hydrogen sulfate is represented by the symbol \(HSO_4\). Ammonium forms a +1 charge and hydrogen sulfate forms a -1 charge. Since the charges are already balanced, the formula for ammonium hydrogen sulfate is \((NH_4)HSO_4\).
09

i. Cobalt(III) nitrate

Cobalt is represented by the symbol Co and nitrate by the symbol \(NO_3\). Cobalt(III) refers to a cobalt ion with a +3 charge, and nitrate has a -1 charge. To balance the charges, we need one cobalt atom and three nitrate atoms. The formula for cobalt(III) nitrate is \(Co(NO_3)_3\).
10

j. Mercury(I) chloride

Mercury is represented by the symbol Hg and chloride by the symbol Cl. Mercury(I) refers to a mercury ion with a +1 charge, and chloride forms a -1 charge. To balance the charges, we need one mercury atom and one chloride atom. The formula for mercury(I) chloride is \(HgCl\).
11

k. Potassium chlorate

Potassium is represented by the symbol K, and chlorate is represented by the symbol \(ClO_3\). Potassium forms a +1 charge, and chlorate forms a -1 charge. Since the charges are already balanced, the formula for potassium chlorate is \(KClO_3\).
12

1. Sodium hydride

Sodium is represented by the symbol Na and hydrogen by the symbol H. Sodium forms a +1 charge, and hydrogen forms a -1 charge. Since the charges are already balanced, the formula for sodium hydride is \(NaH\).

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Give three ions that are isoelectronic with neon. Place these ions in order of increasing size.

Rationalize the following lattice energy values: $$\begin{array}{|lc|} \hline & \text { Lattice Energy } \\ \text { Compound } & \text { (kj/mol) } \\ \hline \text { CaSe } & -2862 \\ \text { Na }_{2} \text { Se } & -2130 \\ \text { CaTe } & -2721 \\ \text { Na }_{2} \text { Te } & -2095 \\ \hline \end{array}$$

Which compound in each of the following pairs of ionic substances has the most negative lattice energy? Justify your answers. a. NaCl, KCl b. LiF, LiCl c. \(\mathrm{Mg}(\mathrm{OH})_{2}, \mathrm{MgO}\) d. \(\mathrm{Fe}(\mathrm{OH})_{2}, \mathrm{Fe}(\mathrm{OH})_{3}\) e. \(\mathrm{NaCl}, \mathrm{Na}_{2} \mathrm{O}\) f. \(\mathrm{MgO}, \mathrm{BaS}\)

Indicate the bond polarity (show the partial positive and partial negative ends) in the following bonds. a. \(C-O\) b. \(P-H\) \(\mathbf{c} . \quad \mathbf{H}-\mathbf{C l}\) d. \(\mathrm{Br}-\mathrm{Te}\) \(\mathbf{e} . \mathbf{S e}-\mathbf{S}\)

Arrange the following in order of increasing radius and increasing ionization energy. a. \(\mathrm{N}^{+}, \mathrm{N}, \mathrm{N}^{-}\) b. \(\mathrm{Se}, \mathrm{Se}^{-}, \mathrm{Cl}, \mathrm{Cl}^{+}\) c. \(\mathrm{Br}^{-}, \mathrm{Rb}^{+}, \mathrm{Sr}^{2+}\)
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemical Reactions

Read Explanation

Nuclear Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Kinetics

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free