Download Ionic Bonding

Ionic Bonding
1. What properties of ionic compounds suggest that ionic bonds are strong?
2. What types of elements form ionic bonds with each other?
3. Which of the representative elements tend to form positive ions? Which tend to form negative ions?
4. What is the minimum number of different ions in the formula of an ionic compound? Explain.
5. Predict the charge on the most stable ion formed by each of the following
elements. Indicate the ion by writing the symbol complete
with charge.
(a) sulfur
(b) barium
(c) bromine
(d) chlorine
(e) calcium
(f) potassium
(g) phosphorus
(h) rubidium
(i) beryllium
8. (a) How do the electron dot diagrams of metal ions differ from those of nonmetal ions?
(b) How are the electron dot diagrams of metal ions similar to those of nonmetal ions?
9. Use electron dot diagrams to illustrate the formation of
(a) lithium iodide
(b) barium chloride
(c) potassium oxide
(d) calcium fluoride
10. Represent each of the following elements using electron dot diagrams:
(a) nitrogen
(b) sulfur
(c) argon
(d) iodine
(e) lithium
(f) cesium
(g) calcium
(h) sodium
11. Use electron dot diagrams to determine the ratio in which oxygen will combine with each of the
following elements to form an ionic compound. Label each diagram with the chemical formula of the
compound.
(a) calcium
(b) rubidium
(c) strontium
(d) aluminum
12. Represent the five halogens, using electron dot diagrams. How are these diagrams consistent with the
concept of a chemical family?
13. Explain, referring to stable octets, how the following ionic compounds are formed from pairs of
elements; illustrate the formation of each compound with electron dot diagrams; and predict the formula
of each compound.
(a) magnesium chloride
(b) sodium sulfide
(c) aluminum oxide (bauxite)
(d) barium chloride
(e) calcium fluoride (fluorite)
(f) sodium iodide
(g) potassium chloride (a substitute for table salt)
14. Give the common names for the following chemicals:
(a) sodium bicarbonate
(b) NaCl
(c) calcium carbonate
(d) Ca(OH)2
Covalent Bonding
1. Draw a Lewis structure and write the molecular formula for each of the following:
(a) F2(g)
(b) H2O(l)
(c) CH4(g)
(d) PCl3(s)
(e) H2S(g)
(f) SiO2(s)
2. Draw Lewis structures and structural formulas for each of the following molecules:
(a) H2(g) (d) NF3(g)
(b) O3(g) (e) N2H2(g)
(c) OF2(g) (f) P2H4(g)
3. Draw Lewis structures and structural formulas for each of the following polyatomic ions:
(a) PO3–4(aq)
(c) BrO–3(aq)
(b) OH–(aq)
(d) ClO –4(aq)
4. Which of the Lewis structures in questions 2 and 3 include coordinate covalent bonds?
5. Distinguish between bonding electrons and lone pairs.
6. Are the following pairs of atoms more likely to form ionic or covalent bonds?
(a) sulfur and oxygen
(b) iodine and iodine
(c) calcium and chlorine
(d) potassium and bromine
7. (a) List six examples of molecular elements and compounds and six examples of ionic compounds.
(b) Compare the two lists, referring to bond types to explain the contrasting physical properties.
8. (a) How does the bonding capacity of nitrogen differ from that of chlorine?
(b) Give a theoretical explanation for your answer to (a).
9. How are coordinate covalent bonds similar to covalent bonds? How are they different?
10. (a) Use an electron dot diagram to explain the formula for nitrogen, N2.
(b) Draw the Lewis structure for nitrogen.
(c) Nitrogen is a fairly inert (unreactive) gas. Explain this, referring to the bonds involved.
11. Illustrate the formation of each of the following molecular compounds, using electron dot diagrams and
Lewis structures:
(a) HCl (c) H2S
(b) NH3 (d) CO2
12. Use the octet rule to develop a table that lists the bonding capacities for carbon, nitrogen, oxygen,
hydrogen, fluorine, chlorine, bromine, and iodine.
13. Use bonding capacities (Table 1, page 77) to draw the structural formula of each of the following
molecules.
(a) O2
(b) Br2
(c) H2O2
(d) C2H4
(e) HCN
(f) C2H5OH
(g) CH3OCH3
(h) CH3NH2
14. (a) Illustrate the structure of a hydronium ion (H3O+) by drawing its Lewis structure.
(b) Name the bonds within the hydronium ion.
(c) What kinds of bonds is this ion likely to form with other entities?
15. Is it correct for the structural formula of H2S to be written as H—H—S? Explain, using a diagram.
Electronegativity, Polar Bonds,
and Polar Molecules
1. Describe how we can use electronegativity values to predict the types
of bonds that will form within a compound.
2. Which type of bond—ionic or covalent—will form between each of the following pairs of atoms? Of the
covalent bonds, indicate which would be the most polar.
(a) H and Cl
(b) Si and O
(c) Mg and Cl
(d) Li and O
(e) N and O
(f) O and O
(g) I and Cl
(h) Cr and O
(i) C and Cl
3. Identify the more polar bond in each of the following pairs.
(a) H—F; H—Cl
(b) N—O; C—O
(c) S—H; O—H
(d) P—Cl; S—Cl
(e) C—H; N—H
(f) S—O; P—O
(g) C—N; N—N
4. Draw Lewis structures for the following substances. In each case, use appropriate notation to indicate
the atoms that are slightly positive and those that are slightly negative.
(a) H2O
(b) Br2
(c) HBr
(d) PCl3
(e) OF2
5. Some molecules contain polar covalent bonds but are not themselves polar. Explain, with diagrams,
how this is possible.
6. Use Lewis structures and electronegativity values to explain why methane, CH4(g), is not a polar
substance.
7. Water is known for its many anomalous properties. Use your knowledge of intermolecular forces and
intramolecular bonding to explain theoretically why lakes freeze from top to bottom.
8. Using Table 3 (page 85), predict whether each of the following moleculeswould be polar or nonpolar.
(a) CH3OH(l)
(d) PCl3(s)
(b) I2(s)
(e) HC2H3O2(aq)
(c) HBr(g)
(f) CCl4(l)
9. Which compound(s) in question 8 were classified as nonpolar but contain polar covalent bonds? Explain
how this is possible.
10. How are hydrogen bonds different from other dipole–dipole forces?
11. Predict the type of intermolecular force that would exist between molecules of the following:
(a) I2(s)
(b) H2O(l)
(c) NH3(g)
12. Explain each of your predictions in question 11 theoretically.
Binary Ionic Compounds
1. How were compounds named before the advent of systematic means of chemical nomenclature?
2. State the common names of each of the following chemicals:
(a) hydrochloric acid
(b) sodium hydrogen carbonate
(c) dinitrogen monoxide
(d) ethanol
3. How many elements are there in each binary compound?
4. Describe the IUPAC system of naming a binary ionic compound.
5. If an element is described as“multivalent,” what characteristic does it
have?
6. Write the formula for each of the following compounds:
(a) calcium fluoride (l) mercury(I) oxide
(b) sodium sulfide (m) nickel(II) bromide
(c) aluminum nitride (n) zinc oxide
(d) aluminum chloride (o) cobalt(III) chloride
(e) potassium oxide (p) strontium bromide
(f) calcium chloride (q) gold(I) fluoride
(g) copper(II) sulfide (r) lithium chloride
(h) lead(II) bromide (s) strontium nitride
(i) silver iodide (t) barium bromide
(j) barium nitride (u) tin(IV) iodide
(k) iron(II) fluoride
7. Write the names of each of the following binary ionic compounds,
using the IUPAC system of chemical nomenclature:
(a) table salt, NaCl(s)
(h) chalcocite, Cu2S(s)
(b) lime, CaO(s)
(i) galena, PbS2(s)
(c) road salt, CaCl2(s)
(j) hematite, Fe2O3(s)
(d) magnesia, MgO(s)
(k) molybdite, MoO3(s)
(e) bauxite, Al2O3(s)
(l) argentite, Ag2S(s)
(f) zinc ore, ZnS(s)
(m) zincite, ZnO(s)
(g) cassiterite, SnO2(s)
8. Write the IUPAC names for the following binary ionic compounds:
(a) Na2O(s)
(g) Ni2O3(s)
(b) SnCl4(s)
(h) Ag2S(s)
(c) ZnI2(s)
(i) FeCl2(s)
(d) SrCl2(s)
(j) KBr(s)
(e) AlBr3(s)
(k) CuI2(s)
(f) PbCl4(s)
(l) NiS(s)
9. Write the chemical formulas and names (using IUPAC chemical nomenclature) for the binary ionic
compounds formed by each of the following pairs of elements:
(a) strontium and oxygen
(b) sodium and sulfur
(c) silver and iodine
(d) barium and fluorine
(e) calcium and bromine
(f) lithium and chlorine
10. Write the chemical formulas for the following ionic compounds:
(a) mercury(II) sulfide, cinnabar ore
(b) molybdenum(IV) sulfide, molybdenite ore
(c) manganese(IV) oxide, pyrolusite ore
(d) nickel(II) bromide
(e) copper(II) chloride
(f) iron(III) iodide
11. Rename each of the following compounds, using the IUPAC system of nomenclature:
(a) ferrous sulfide
(b) plumbic bromide
(c) stannous chloride
Polyatomic Ionic Compounds
13. How many elements are there in a tertiary compound?
14. Use each of the following terms correctly in a sentence about the formation of compounds:
(a) polyatomic ion
(b) oxyanion
(c) hydrate
15. Write the IUPAC name for each of the following ionic compounds:
(a) NaNO3(s) (found in tobacco)
(b) NaNO2(s) (a meat preservative)
(c) Cu(NO3)2(s) (forms a blue solution in water)
(d) CuNO3(s) (forms a green solution in water)
(e) Al2(SO3)3(s) (a food additive in pickles)
(f) Ca(OH)2(s) (firming agent in fruit products)
(g) PbCO3(s) (cerussite, a mineral popular with collectors)
(h) Sn3(PO4)2(s) (use to fix paints to silk)
(i) Fe2(SO4)3(s) (a mineral found on Mars)
16. Write the chemical formula for each of the following ionic compounds:
(a) calcium carbonate (active ingedient in antacids)
(b) sodium bicarbonate (a foaming agent added to foods)
(c) sodium hypochlorite (a component of bleach)
(d) calcium sulfate (plaster of Paris)
(e) ammonium nitrate (used in fertilizers)
(f) ammonium phosphate (a leavening agent added to foods)
(g) copper(II) sulfate (used as a fungicide)
(h) sodium hydroxide (a strong base used as a washing agent)
(i) potassium permanganate (a traditional antiseptic)
17. Use IUPAC chemical nomenclature to name each of the following
ionic compounds containing polyatomic ions:
(a) LiClO3(s)
(n) Ag2SO4(s)
(b) BaSO4(s)
(o) Hg(BrO3)2(s)
(c) Hg2CO3(s)
(p) Fe2(CO3)3(s)
(d) Mg(NO3)2(s) (q) NH4ClO(s)
(e) Fe(BrO3)3(s) (r) Au(NO3)3(s)
(f) Na3PO4(s)
(s) Mg(BrO3)2(s)
(g) NH4IO3(s)
(t) NaIO(s)
(h) AuC2H3O2(s) (u) Zn(ClO2)2(s)
(i) Zn3(PO4)2(s) (v) SnCO3(s)
(j) Sb(ClO3)5(s) (w) SrSO3(s)
(k) MnSO3(s)
(x) NiPO4(s)
(l) KBrO(s)
(y) Cu(C2H3O2)2(s)
(m) AlPO5(s)
(z) Ba3(PO5)2(s)
18. Write the IUPAC name and chemical formula for each of the following
ionic compounds containing polyatomic ions:
(a) cuprous hypophosphite
(b) stannic chlorite
(c) ferrous bromate
(d) ferric chlorite
(e) plumbic sulfate
Hydrates
19. Name each of the following hydrated ionic compounds:
(a) bluestone, CuSO4·5 H2O(s)
(b) Na2SO4·10 H2O(s)
(c) MgSO4·7 H2O(s)
20. Write the chemical formulas for the following ionic hydrates:
(a) iron(III) oxide trihydrate (rust)
(b) aluminum chloride hexahydrate (component of antiperspirant)
(c) sodium thiosulfate pentahydrate (photographic “hypo”)
(d) cadmium(II) nitrate tetrahydrate (photographic emulsion)
(e) lithium chloride tetrahydrate (in fireworks)
(f) calcium chloride dihydrate (deicer)
21. How would you convert a hydrate to an anhydrous compound?
Molecular Compounds
22. Write the chemical formula for each of the following molecules:
(a) nitrogen
(n) sulfur tetrafluoride
(b) carbon dioxide
(o) phosphorus pentachloride
(c) carbon monoxide
(p) disulfur dichloride
(d) nitrogen dioxide
(q) carbon tetrachloride
(e) nitrogen monoxide
(r) sulfur trioxide
(f) dinitrogen oxide
(s) sulfur hexafluoride
(g) dinitrogen tetroxide
(t) chlorine dioxide
(h) sulfur dioxide
(u) dinitrogen pentoxide
(i) diiodine pentoxide
(v) phosphorus trichloride
(j) silicon tetrafluoride
(w) silicon tetrachloride
(k) boron trifluoride
(x) carbon disulfide
(l) phosphorus triiodide
(y) phosphorus pentabromide
(m) diphosphorus pentoxide
(z) carbon tetrafluoride
23. Name the compound indicated by each of the following formulas:
(a) SF6(g)
(f) IF7(g)
(b) N2O3(g)
(g) BF3(g)
(c) NO2(g)
(h) P2S5(s)
(d) PCl3(l)
(i) P2O5(s)
(e) PCl5(s)
Acids and Bases
24. Write the chemical formulas for the following acids:
(a) aqueous hydrogen chloride
(g) aqueous hydrogen nitrite
(b) hydrochloric acid
(h) nitric acid
(c) aqueous hydrogen sulfate
(i) hydrobromic acid
(d) sulfuric acid
(j) hyposulfurous acid
(e) aqueous hydrogen acetate
(k) hydroiodic acid
(f) acetic acid
(l) aqueous hydrogen perchlorate
25. Name each of the following compounds, using both the classical and
the IUPAC nomenclature systems:
(a) H2SO3(aq)
(d) H2CO3(aq)
(g) HCN(aq)
(b) H3PO4(aq)
(e) H2S(aq)
(h) H2SO4(aq)
(c) HCN(aq)
(f) HCl(aq)
(i) H3PO4(aq)
26. Write the names of the following bases:
(a) KOH(aq)
(b) CaOH2(aq)
27. Write the formulas of the following bases:
(a) aqueous magnesium hydroxide
(b) aqueous sodium hydroxide
(c) aqueous aluminum hydroxide