Nelson Science Perspectives 10
Nelson Science Perspectives 10
1st Edition
Christy C. Hayhoe, Doug Hayhoe, Jeff Major, Maurice DiGiuseppe
ISBN: 9780176355289
Table of contents
Textbook solutions

All Solutions

Section 5-9: Polyatomic Ions

Exercise 1
Step 1
1 of 9
a.

The polyatomic ion in KNO$_3$ is the nitrate ion; NO$_3^{-}$.

Step 2
2 of 9
b.

The polyatomic ion in Ca(OH)$_2$ is the hydroxide ion; OH$^{-}$.

Step 3
3 of 9
c.

The polyatomic ion in CaCO$_3$ is the carbonate ion; CO$_3^{-2}$.

Step 4
4 of 9
d.

The polyatomic ion in CuSO$_4$ is the sulfate ion; SO$_4^{-2}$.

Step 5
5 of 9
e.

The polyatomic ion in KOH is the hydroxide ion; OH$^{-}$.

Step 6
6 of 9
f.

The polyatomic ion in Fe(NO$_3$)$_3$ is the nitrate ion; NO$_3^{-}$.

Step 7
7 of 9
g.

The polyatomic ion in Cu(ClO$_3)_2$ is the chlorate ion; ClO$_3^{-}$.

Step 8
8 of 9
h.

The polyatomic ion in (NH$_4)_3$PO$_4$ is the phosphate ion; PO$_4^{-3}$.

Result
9 of 9
Click to see answer.
Exercise 2
Step 1
1 of 9
a.

The ionic charge on potassium (K) is $+1$ while that on the polyatomic ion nitrate is $-1$, therefore the chemical formula of potassium nitrate is KNO$_3$.

Step 2
2 of 9
b.

The ionic charge on barium (Ba) is $+2$ while that on the polyatomic ion sulfate is $-2$, therefore the chemical formula of barium sulfate is BaSO$_4$.

Step 3
3 of 9
c.

The ionic charge on the polyatomic ion ammonium (NH$_4$) is $+1$ while that on the polyatomic ion nitrate is $-1$, therefore the chemical formula of ammonium nitrate is NH$_4$NO$_3$.

Step 4
4 of 9
d.

The ionic charge on aluminum (Al) is $+3$ while that on the polyatomic ion sulfate is $-2$, therefore the chemical formula of aluminum sulfate is Al$_2$(SO$_4)_3$.

Step 5
5 of 9
e.

The ionic charge on potassium (K) is $+1$ while that on the polyatomic ion chlorate is $-1$, therefore the chemical formula of potassium chlorate is KClO$_3$.

Step 6
6 of 9
f.

The ionic charge on copper II (Cu) is $+2$ while that on the polyatomic ion nitrate is $-1$, therefore the chemical formula of copper(II) nitrate is Cu(NO$_3)_2$.

Step 7
7 of 9
g.

The ionic charge on lead II (Pb) is $+2$ while that on the polyatomic ion sulfate is $-2$, therefore the chemical formula of lead(II) sulfate is PbSO$_4$.

Step 8
8 of 9
h.

The ionic charge on tin II (Sn) is $+2$ while that on the polyatomic ion phosphate is $-3$, therefore the chemical formula of tin(II) phosphate is Sn$_3$(PO$_4)_2$.

Result
9 of 9
Click to see answer.
Exercise 3
Step 1
1 of 3
a.

The names of all polyatomic anions end with the suffix $color{#c34632}text{-ate}$. For example; sulf$color{#c34632}text{ate}$, nitr$color{#c34632}text{ate}$, phosph$color{#c34632}text{ate}$, etc.

Step 2
2 of 3
b.

The names of all anions made up of one element end with the suffix $color{#c34632}text{-ide}$. For example; sulf$color{#c34632}text{ide}$, nitr$color{#c34632}text{ide}$, phosph$color{#c34632}text{ide}$, etc.

Result
3 of 3
Click to see answers.
Exercise 4
Step 1
1 of 2
Nitrates form an essential part of fertilizers used to increase crop yield in agricultural lands. Some of these nitrates can become dissolved in groundwater and travel to wells.
Result
2 of 2
Nitrates in fertilizers can cause nitrate pollution.
Exercise 5
Step 1
1 of 9
a.

SnCO$_3$ is tin(II) carbonate.

Step 2
2 of 9
c.

CaCl$_2$ is calcium chloride.

Step 3
3 of 9
c.

Fe(OH)$_3$ is iron(III) hydroxide.

Step 4
4 of 9
d.

MnO$_2$ is manganese(IV) oxide. We know that this is manganese(IV) because the charge on oxide ion is $-2$, if 2 molecules of oxide ion are needed, then this implies that this is manganese(IV).

Step 5
5 of 9
e.

K$_2$S is potassium sulfide.

Step 6
6 of 9
f.

(NH$_4)_2$SO$_4$ is ammonium sulfate.

Step 7
7 of 9
g.

Mn(ClO$_3)_2$ is manganese(II) chlorate. We know that this is manganese(II) because the charge on chlorate ion is $-1$, if 2 molecules of chlorate ion are needed, then this implies that this is manganese(II).

Step 8
8 of 9
h.

PbI$_2$ is lead(II) iodide.

Result
9 of 9
Click to see answer.
Exercise 6
Step 1
1 of 9
a.

The ionic charge on calcium (Ca) is $+2$ while that on the polyatomic ion sulfate is $-2$, therefore the chemical formula of barium sulfate is CaSO$_4$.

Step 2
2 of 9
b.

The ionic charge on the polyatomic ion ammonium (NH$_4$) is $+1$ while that on chloride is $-1$, therefore the chemical formula of ammonium chloride is NH$_4$Cl.

Step 3
3 of 9
c.

The ionic charge on copper I (Cu) is $+1$ while that on the polyatomic ion carbonate is $-2$, therefore the chemical formula of copper(I) carbonate is Cu$_2$CO$_3$.

Step 4
4 of 9
d.

The ionic charge on barium (Ba) is $+2$ while that on sulfide is $-2$, therefore the chemical formula of barium sulfide is BaS.

Step 5
5 of 9
e.

The ionic charge on calcium (Ca) is $+2$ while that on the polyatomic ion chlorate is $-1$, therefore the chemical formula of calcium chlorate is Ca(ClO$_3)_2$.

Step 6
6 of 9
f.

The ionic charge on tin II (Sn) is $+2$ while that on the polyatomic ion hydroxide is $-1$, therefore the chemical formula of tin(II) hydroxide is Sn(OH)$_2$.

Step 7
7 of 9
h.

The ionic charge on iron II (Fe) is $+2$ while that on the polyatomic ion phosphate is $-3$, therefore the chemical formula of iron(II) phosphate is Fe$_3$(PO$_4)_2$.

Step 8
8 of 9
g.

The ionic charge on aluminum (Al) is $+3$ while that on nitride is $-3$, therefore the chemical formula of aluminum nitride is AlN.

Result
9 of 9
Click to see answer.
Exercise 7
Step 1
1 of 2
The chemical formula of calcium hydroxide is written as Ca(OH)$_2$ because this gives a very vivid representation of the charges of each ion and their combining ratio. Ca(OH)$_2$ implies that 2 hydroxide ions are required per calcium ion in this compound. This piece of information is absent in CaO$_2$H$_2$.
Result
2 of 2
Click to see answer.
Exercise 8
Step 1
1 of 2
The polyatomic ammonium ion NH$_4^+$ is the exception in this rule. It is made up of non-metals but behaves as a cation, and subsequently its compounds are ionic in nature.
Result
2 of 2
Ammonium ion is the exception here.
Exercise 9
Result
1 of 1
The cation or metallic ion is written first followed by the anion while writing the chemical formulas of ionic compounds.
Exercise 10
Step 1
1 of 7
Compound
Cation(s)
Anion(s)
Step 2
2 of 7
Fe(OH)$_3$
1 Fe$^{+3}$
3 OH$^{-}$
Step 3
3 of 7
Cu(NO$_3)_2$
1 Cu$^{+2}$
2 NO$_3^-$
Step 4
4 of 7
Al$_2$(SO$_4)_3$
2 Al$^{+3}$
3 SO$_4^{-2}$
Step 5
5 of 7
(NH$_4)_2$CO$_3$
2 NH$_4^{+}$
1 CO$_3^{-2}$
Step 6
6 of 7
K$_3$PO$_4$
3 K$^{+}$
1 PO$_4^{-3}$
Result
7 of 7
Click to see table.
Exercise 11
Step 1
1 of 4
a.

The chemical formula of sodium chloride is NaCl, while that of sodium chlorate is NaClO$_3$.

Step 2
2 of 4
b.

The chemical formula of the chloride ion is Cl$^-$ while that of the ployatomic chlorate ion is ClO$_3^-$.

Step 3
3 of 4
c.

The chemical formula of calcium chloride is CaCl$_2$, while that of calcium chlorate is Ca(ClO$_3)_2$.

Result
4 of 4
Click to see answers.
Exercise 12
Result
1 of 1
Eat foods that are low-sodium or contain no sodium
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Chapter 1: Living and Working with Science
Chapter 4: Plant Systems
Section 4-1: Systems in Plants
Section 4-2: Plant Tissue Systems
Section 4-4: Tissues Working Together
Section 4-6: Plant Growth
Page 150: Review
Page 152: Self-Quiz
Page 159: Unit Review
Page 164: Self-Quiz
Chapter 5: Chemicals and Their Properties
Section 5-1: Properties and Changes
Section 5-3: Hazardous Products and Workplace Safety
Section 5-4: Patterns and the Periodic Table
Section 5-5: Atoms and Ions
Section 5-6: Ionic Compounds
Section 5-7: Names and Formulas of Ionic Compounds
Section 5-9: Polyatomic Ions
Section 5-10: Molecules and Covalent Bonding
Page 216: Review
Page 218: Self-Quiz
Chapter 6: Chemicals and Their Reactions
Chapter 7: Acids and Bases
Section 7-2: Properties, Names, and Formulas
Section 7-3: The pH Scale
Section 7-5: Neutralization Reactions
Section 7-7: Explore an Issue Critically
Page 294: Review
Page 296: Self-Quiz
Page 303: Unit Review
Page 309: Self-Quiz
Chapter 8: Earth’s Climate System and Natural Change
Section 8-1: Weather and Climate
Section 8-2: Classifying Climate
Section 8-3: The Sun Powers Earth’s Climate System
Section 8-4: Components of Earth’s Climate System
Section 8-6: The Greenhouse Effect
Section 8-8: Energy Transfer within the Climate System: Air and Ocean Circulation
Section 8-9: Long-Term and Short-Term Changes
Section 8-10: Feedback Loops and Climate
Section 8-11: Studying Clues to Past Climates
Page 364: Review
Page 367: Self-Quiz
Chapter 9: Earth’s Climate: Out of Balance
Chapter 10: Assessing and Responding to Climate Change
Section 10-1: Climate Models and Clean Energy
Section 10-2: Global Impacts of Climate Change
Section 10-3: Impacts of Climate Change on Ontario
Section 10-4: Taking Action to Limit Climate Change
Section 10-5: What Can Individuals Do?
Page 438: Review
Page 440: Self-Quiz
Page 446: Unit Review
Page 453: Self-Quiz
Chapter 11: The Production and Reflection of Light
Section 11-1: What is Light?
Section 11-2: How is Light Produced?
Section 11-3: The Laser?A Special Type of Light
Section 11-4: The Ray Model of Light
Section 11-6: The Laws of Reflection
Section 11-7: Images in Plane Mirrors
Section 11-9: Images in Curved Mirrors
Page 506: Review
Page 509: Self-Quiz
Chapter 13: Lenses and Optical Devices
Section 13-1: Writing a Critical Analysis
Section 13-3: Images in Lenses
Section 13-4: The Lens Equations
Section 13-5: Lens Applications
Section 13-6: The Human Eye
Page 582: Review
Page 584: Self-Quiz
Page 590: Unit Review
Page 596: Self-Quiz