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Sia

青州's Question
Chemistry
Posted 7 months ago

Unit 6 lonic Bonding Review P...
Practice problems
Draw Lewis structures for the following atoms
1. N\mathrm{N}
2. P\mathrm{P}
3. Mg\mathrm{Mg}
4. Cl\mathrm{Cl}

Draw Lewis structures for the following ionic compounds
5. NaCl\mathrm{NaCl}
6. MgBr2\mathrm{MgBr}_{2}
7. Li2O\mathrm{Li}_{2} \mathrm{O}
8. Fe2O3\mathrm{Fe}_{2} \mathrm{O}_{3}

Write the formula for the following ionic compounds
9. Lead (IV) oxide
10. Sodium sulfate
11. Iron (II) sulfide
12. Magnesium carbonate
13. Potassium hromidn
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Answer from Sia
Posted 7 months ago
Solution
1
Draw Lewis structures for the following atoms: - Nitrogen ($\mathrm{N}$): Nitrogen has 5 valence electrons. The Lewis structure is represented as N\mathrm{N} with 5 dots around it. - Phosphorus ($\mathrm{P}$): Phosphorus has 5 valence electrons. The Lewis structure is represented as P\mathrm{P} with 5 dots around it. - Magnesium ($\mathrm{Mg}$): Magnesium has 2 valence electrons. The Lewis structure is represented as Mg\mathrm{Mg} with 2 dots around it. - Chlorine ($\mathrm{Cl}$): Chlorine has 7 valence electrons. The Lewis structure is represented as Cl\mathrm{Cl} with 7 dots around it
2
Draw Lewis structures for the following ionic compounds: - Sodium chloride ($\mathrm{NaCl}$): Sodium loses one electron to form Na+\mathrm{Na}^+ and chlorine gains one electron to form Cl−\mathrm{Cl}^-. The Lewis structure is Na+[Cl]−\mathrm{Na}^+ [\mathrm{Cl}]^-. - Magnesium bromide ($\mathrm{MgBr}_2$): Magnesium loses two electrons to form Mg2+\mathrm{Mg}^{2+} and each bromine gains one electron to form Br−\mathrm{Br}^-. The Lewis structure is Mg2+[Br]−[Br]−\mathrm{Mg}^{2+} [\mathrm{Br}]^- [\mathrm{Br}]^-. - Lithium oxide ($\mathrm{Li}_2\mathrm{O}$): Each lithium loses one electron to form Li+\mathrm{Li}^+ and oxygen gains two electrons to form O2−\mathrm{O}^{2-}. The Lewis structure is 2Li+[O]2−2\mathrm{Li}^+ [\mathrm{O}]^{2-}. - Iron(III) oxide ($\mathrm{Fe}_2\mathrm{O}_3$): Each iron loses three electrons to form Fe3+\mathrm{Fe}^{3+} and each oxygen gains two electrons to form O2−\mathrm{O}^{2-}. The Lewis structure is 2Fe3+3[O]2−2\mathrm{Fe}^{3+} 3[\mathrm{O}]^{2-}
3
Write the formula for the following ionic compounds: - Lead (IV) oxide: Lead (IV) has a charge of +4+4 and oxide has a charge of −2-2. The formula is PbO2\mathrm{PbO}_2. - Sodium sulfate: Sodium has a charge of +1+1 and sulfate has a charge of −2-2. The formula is Na2SO4\mathrm{Na}_2\mathrm{SO}_4. - Iron (II) sulfide: Iron (II) has a charge of +2+2 and sulfide has a charge of −2-2. The formula is FeS\mathrm{FeS}. - Magnesium carbonate: Magnesium has a charge of +2+2 and carbonate has a charge of −2-2. The formula is MgCO3\mathrm{MgCO}_3. - Potassium bromide: Potassium has a charge of +1+1 and bromide has a charge of −1-1. The formula is KBr\mathrm{KBr}
Answer
1. N\mathrm{N}: N\mathrm{N} with 5 dots 2. P\mathrm{P}: P\mathrm{P} with 5 dots 3. Mg\mathrm{Mg}: Mg\mathrm{Mg} with 2 dots 4. Cl\mathrm{Cl}: Cl\mathrm{Cl} with 7 dots 5. NaCl\mathrm{NaCl}: Na+[Cl]−\mathrm{Na}^+ [\mathrm{Cl}]^- 6. MgBr2\mathrm{MgBr}_2: Mg2+[Br]−[Br]−\mathrm{Mg}^{2+} [\mathrm{Br}]^- [\mathrm{Br}]^- 7. Li2O\mathrm{Li}_2\mathrm{O}: 2Li+[O]2−2\mathrm{Li}^+ [\mathrm{O}]^{2-} 8. Fe2O3\mathrm{Fe}_2\mathrm{O}_3: 2Fe3+3[O]2−2\mathrm{Fe}^{3+} 3[\mathrm{O}]^{2-} 9. PbO2\mathrm{PbO}_2 10. Na2SO4\mathrm{Na}_2\mathrm{SO}_4 11. FeS\mathrm{FeS} 12. MgCO3\mathrm{MgCO}_3 13. KBr\mathrm{KBr}
Key Concept
Lewis structures represent the valence electrons of atoms and ions.
Explanation
Lewis structures help visualize the bonding between atoms in a molecule and the lone pairs of electrons that may exist.

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