# 5.E: Homework Chapter 5 Answers

$$\newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}} }$$ $$\newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash {#1}}}$$$$\newcommand{\id}{\mathrm{id}}$$ $$\newcommand{\Span}{\mathrm{span}}$$ $$\newcommand{\kernel}{\mathrm{null}\,}$$ $$\newcommand{\range}{\mathrm{range}\,}$$ $$\newcommand{\RealPart}{\mathrm{Re}}$$ $$\newcommand{\ImaginaryPart}{\mathrm{Im}}$$ $$\newcommand{\Argument}{\mathrm{Arg}}$$ $$\newcommand{\norm}[1]{\| #1 \|}$$ $$\newcommand{\inner}[2]{\langle #1, #2 \rangle}$$ $$\newcommand{\Span}{\mathrm{span}}$$ $$\newcommand{\id}{\mathrm{id}}$$ $$\newcommand{\Span}{\mathrm{span}}$$ $$\newcommand{\kernel}{\mathrm{null}\,}$$ $$\newcommand{\range}{\mathrm{range}\,}$$ $$\newcommand{\RealPart}{\mathrm{Re}}$$ $$\newcommand{\ImaginaryPart}{\mathrm{Im}}$$ $$\newcommand{\Argument}{\mathrm{Arg}}$$ $$\newcommand{\norm}[1]{\| #1 \|}$$ $$\newcommand{\inner}[2]{\langle #1, #2 \rangle}$$ $$\newcommand{\Span}{\mathrm{span}}$$$$\newcommand{\AA}{\unicode[.8,0]{x212B}}$$

1.      lose; cations

3.      H+ for hydrogen ion; H- for hydride ion

5.

a. Nitrogen,1; Hydrogen,4; Chlorine,1.

b. Sodium,1; Carbon,1; Nitrogen,1.

c. Barium,1; Hydrogen,2; Carbon,2; Oxygen,6.

d. Calcium,1; Nitrogen,2; Oxygen,4.

e. Magnesium,1; Chlorine,2.

7.       a. not a molecule   b. a molecule; four atoms total    c. a molecule; four atoms total

9.

 Formula Number of SO42- Units Number of Sulfur Atoms Number of Oxygen atoms Number of metal atoms CaSO4 1 1 4 1 Al2(SO4)3 3 3 12 2 K2SO4 1 1 4 2

11.  MgO, Magnesium Oxide

13.   a)   covalent b)  ionic    c)    ionic    d)    covalent    e)    covalent

15.  a. ionic   b. ionic   c. molecular    d. ionic

17.  a. atomic   b.  atomic      c. molecular   d. molecular

19.  a. molecular   b. molecular        c. atomic        d. atomic

21.  a. molecular b. molecular c. atomic d. ionic

23.  a. covalent b. ionic c. covalent d. covalent

25.  Name the cation and then the anion but don’t use numerical prefixes.

27.  Ionic compounds in which the cation can have more than one possible charge have two naming systems. FeCl3 is either iron(III) chloride or ferric chloride (answers will vary).

29.

a.       iron(III) bromide or ferric bromide

b.      iron(II) bromide or ferrous bromide

c.       gold(III) sulfide or auric sulfide

d.      gold(I) sulfide or aurous sulfide

31.

a.        ​NaOCl

b.      KOH

c.       NH4NO3

d.      Al2(SO3)3

e.        Fe(CN)3

33.

a.        ​ 1 aluminum ion & 3 hydroxide ions

b.       3 lithium ions & 1 phosphate ion

c.       1 potassium ion & 1 chloride ion

d.       1 zinc ion & 2 fluoride ions

e.       2 sodium ions and 1 oxide ions

35.

a.           mercury(I) sulfide

b.      chromium(III) oxide

c.        potassium sulfae

d.       iorn(III) carbonate

e.       zinc hypochlorite

37.

1.    Ba(C2H3O2)2  barium acetate
2.   (NH4)2SO4  ammonium sulfate
3.  Zn(ClO)2  zinc hypochlorite
4.   Al(OH)3  aluminum hydroxide
5. Na2CO sodium carbonate

39.  HgO and Hg2O

41.  a) K3PO4; (b) CuSO4; (c) CaCl2; (d) TiO2; (e) NH4NO3; (f) NaHSO4

43.  (a) cesium chloride; (b) barium oxide; (c) potassium sulfide; (d) beryllium chloride; (e) hydrogen bromide; (f) aluminum fluoride

45.

a.         dinitrogen tetroxide

b.       sulfur hexachloride

c.       carbon tetrabromide

d.       Diphosphorus pentoxide

e.       chlorine heptafluoride

47.   a. Nitrogen trichloride;  b. Carbon tetraiodide;  c. Carbon monoxide;  d. correct

49.   a. Carbon tetrafluoride; b. dichlorine trioxide; c. tetraiodine nonaoxide; d. sulfur hexafluoride

51.  a. Nitrogen tribromide b. Oxygen gas c. Ammonia (nitrogen trihydride) d. methane (carbon tetrahydride)

53.

a.    295.50 amu   b. 215.60 amu    c. 490.30 amu    d. 426.10 amu

55.

a. 158.04 amu      b. 62.03 amu       c. 304.23 amu      d. 262.87 amu

57.

 Ionic compound Cation Symbol and name Anion symbol and name NaC2H3O2 Na+  ; sodium C2H3O2-  ; acetate Cr(NO3)3 Cr3+   ; chromium(III) NO3- ; nitrate PbCl2 Pb2+    ; lead(II) Cl-  ; chlorine Hg3(PO4)2 Hg2+    ; mercury(II) PO43-  ; phosphate Ca(HCO3)2 Ca2+    ; Calcium HCO3-  ; bicarbonate

59.

 Formula Unit Chemical Name MgS Magnesium sulfide Al2O3 Aluminum Oxide Fe(OH)3 Iron(III)hydroxide CuCl2 Copper(II) chloride Pb(CO3)2 Lead(IV) carbonate Zn(HCO3)2 Zinc bicarbonate CaSO4 Calcium sulfate NaC2H3O2 Sodium acetate BaBr2 Barium bromide NH4NO3 Ammonium nitrate

61.

 Ion K+ Fe3+ NH4+ Ba2+ Cl- KCl FeCl3 NH4Cl BaCl2 SO42- K2SO4 Fe2(SO4)3 (NH4)2SO4 BaSO4 PO43- K3PO4 FePO4 (NH4)3PO4 Ba3(PO4)2 NO3- KNO3 Fe(NO3)3 NH4NO3 Ba(NO3)2 OH- KOH Fe(OH)3 NH4OH Ba(OH)2

63.  a. Sulfur tetrafluoride b. Potassium Oxide c. Calcium Iodide   d. Phosphorus pentabromide

65.

1. Sodium Chloride, 58.44 amu
2. Silver Nitrate, 169.88 amu
3. Aluminum Fluoride, 83.98 amu
4. Iodine pentafluoride, 221.90 amu

67.  A. H2O b. NH3     c. CH4       d. CO2

69.

 Formula Type of compound Name K3N ionic Potassium nitride SiCl4 Molecular Silicon tetrachloride CO molecular Carbon monoxide NBr3 molecular Nitrogen tribromide

71.

1. Copper(I) phosphate, 285.62 amu
2. Tetrasulfur dinitride, 156.26 amu
3. Lead (II) sulfide, 239.26 amu
4. Vanadium (IV) oxide, 82.94 amu

73.

1. 639.2 amu
2. 379.7 amu
3. 210.4 amu
4. 188.2 amu
5. 225.8 amu

5.E: Homework Chapter 5 Answers is shared under a not declared license and was authored, remixed, and/or curated by LibreTexts.