22.E: Chemistry of the Nonmetals (Exercises)
- Page ID
- 68442
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Questions
- The chemistry of the noble gases is largely dictated by a balance between two competing properties. What are these properties? How do they affect the reactivity of these elements?
- Of the group 18 elements, only krypton, xenon, and radon form stable compounds with other atoms and then only with very electronegative elements. Why?
- Give the type of hybrid orbitals used by xenon in each species.
- XeF2
- XeF4
- XeO3
- XeOF4
- XeO4
- XeO64−
- Which element is the least metallic—B, Ga, Tl, Pb, Ne, or Ge?
- Of Br, N, Ar, Bi, Se, He, and S, which would you expect to form positive ions most easily? negative ions most easily?
- Of BCl3, BCl4−, CH4, H3N·BF3, PCl3, PCl5, XeO3, H2O, and F−, which species do you expect to be
- electron donors?
- electron acceptors?
- neither electron donors nor acceptors?
- both electron donors and acceptors?
- Of HCl, HClO4, HBr, H2S, HF, KrF2, and PH3, which is the strongest acid?
- Of CF4, NH3, NF3, H2O, OF2, SiF4, H2S, XeF4, and SiH4, which is the strongest base?
Structure and Reactivity
- Write a balanced chemical equation showing how you would prepare each compound from its elements and other common compounds.
- XeF2
- XeF4
- XeF6
- XeOF4
- XeO3
- Write a balanced chemical equation showing how you would make each compound.
- XeF2 from Xe gas
- NaXeF7 from its elements
- RnO3 from Rn
- In an effort to synthesize XeF6, a chemist passed fluorine gas through a glass tube containing xenon gas. However, the product was not the one expected. What was the actual product?
- Write a balanced chemical equation to describe the reaction of each species with water.
- B2H6
- F2
- C4+
- Using heavy water (D2O) as the source of deuterium, how could you prepare each compound?
- LiAlD4
- D2SO4
- SiD4
- DF
-
Predict the product(s) of each reaction and write a balanced chemical equation for each reaction.
- Al2O3(s) in OH−(aq)
- Ar(g) + F2(g)
- PI3(s) + H2O(l)
- H3PO3(l) + OH−(aq)
- Bi(s) + excess Br2(l)
Answers
- Xe(g) + F2(g) → XeF2(s)
- Xe(g) + 2F2(g) → XeF4(s)
- Xe(g) + 3F2(g) → XeF6(s)
- 2XeF6(s) + SiO2(s) → 2XeOF4(l) + SiF4(l)
- XeF6(s) + 3H2O(l) → XeO3(s) + 6HF(aq)
- SiF4; SiO2(s) + 2F2(g) → SiF4(l) + 2O2(g)
-
- 2Na(s) + 2D2O(l) → D2(g) + 2NaOD(aq)
2Li(s) + D2(g) → 2LiD(s)
4LiD(s) + AlCl3(soln) → LiAlD4(s) + 3LiCl(soln)
- D2O(l) + SO3(g) → D2SO4(l)
- SiCl4(l) + LiAlD4(s) [from part (a)] → SiD4(g) + LiCl(s) + AlCl3(s)
- CaF2(s) + D2SO4(l) [from part (b)] → 2DF(g) + CaSO4(s)
22.4: Group 7A: The Halogens
Questions
- The lightest elements of groups 15, 16, and 17 form unusually weak single bonds. Why are their bonds so weak?
- Fluorine has an anomalously low F–F bond energy. Why? Why does fluorine form compounds only in the −1 oxidation state, whereas the other halogens exist in multiple oxidation states?
- Compare AlI3, InCl3, GaF3, and LaBr3 with respect to the type of M–X bond formed, melting point, and solubility in nonpolar solvents.
- What are the formulas of the interhalogen compounds that will most likely contain the following species in the indicated oxidation states: I (+3), Cl (+3), I (−1), Br (+5)?
- Consider this series of bromides: AlBr3, SiBr4, and PBr5. Does the ionic character of the bond between the Br atoms and the central atom decrease or increase in this series?
- Chromium forms compounds in the +6, +3, and +2 oxidation states. Which halogen would you use to produce each oxidation state? Justify your selections.
- Of ClF7, BrF5, IF7, BrF3, ICl3, IF3, and IF5, which one is least likely to exist? Justify your selection.
Answers
- Electrostatic repulsions between lone pairs on adjacent atoms decrease bond strength.
- Ionic character decreases as Δχ decreases from Al to P.
- ClF7
Structure and Reactivity
- SiF4 reacts easily with NaF to form SiF62−. In contrast, CF4 is totally inert and shows no tendency to form CF62− under even extreme conditions. Explain this difference.
- Predict the products of each reaction and then balance each chemical equation.
- Xe(g) + excess F2(g) →
- Se(s) + Cl2(g) →
- SO2(g) + Br2(g) →
- NaBH4(s) + BF3(soln) →
- Write a balanced chemical equation for the reaction of aqueous HF with
- SiO2.
- Na2CO3.
- CaO.
- Oxyhalides of sulfur, such as the thionyl halides (SOX2, where X is F, Cl, or Br), are well known. Because the thionyl halides react vigorously with trace amounts of water, they are used for dehydrating hydrated metal salts. Write a balanced chemical equation to show the products of reaction of SOCl2 with water.
- Write a balanced chemical equation describing each reaction.
- the burning of sulfur in a chlorine atmosphere
- the dissolution of iodine in a potassium iodide solution
- the hydrolysis of PCl3
- the preparation of HF from calcium fluoride and sulfuric acid
- the thermal decomposition of KClO3
- the oxidation of sulfide ion by elemental iodine
- Write the complete Lewis electron structure, the type of hybrid used by the central atom, and the number of lone pair electrons present on the central atom for each compound.
- CF4
- PCl3
- XeF4
Answers
- Carbon has no low energy d orbitals that can be used to form a set of d2sp3 hybrid orbitals. It is also so small that it is impossible for six fluorine atoms to fit around it at a distance that would allow for formation of strong C–F bonds.
- SiO2(s) + 6HF(aq) → SiF62−(aq) + 2H+(aq) + 2H2O(l)
- Na2CO3(s) + 2HF(aq) → CO2(g) + 2NaF(aq) + H2O(l)
- CaO(s) + 2HF(aq) → CaF2(s) + H2O(l)
- S8(s) + 4Cl2(g) → 4S2Cl2(l)
- I2(s) + KI(aq) → I3−(aq) + K+(aq)
- PCl3(l) + 3H2O(l) → H3PO3(aq) + 3HCl(aq)
- CaF2(s) + H2SO4(aq) → 2HF(aq) + CaSO4(s)
- 2KClO3(s) \(\xrightarrow{\Delta}\) 2KCl(s) + 3O2(g)
- 8S2−(aq) + 8I2(aq) → S8(s) + 16I−(aq)
22.7: Nitrogen
Problems
- Complete and balance the following equations
N2 + ___H2→ ___NH_
H2N2O2 → ?
2NH3 + CO2 → ?
__Mg + N2 → Mg_N_
N2H5 + H2O → ?
- What are the different isotopes of Nitrogen?
- List the oxiadation states of various nitrogen oxides: N2O, NO, N2O3, N2O4, N2O5
- List the different elements that Nitrogen will react with to make it basic or acidic....
- Uses of nitrogen
Answers
- Complete and balance the following equations
N2 + 3H2→ 2NH3(Haber process)
H2N2O2 → HNO
2NH3 + CO2 → (NH2)2CO + H2O
2Mg + 3N2 → Mg3N2
N2H5 + H2O → N2+ H+ + H2O
- What are the different isotopes of Nitrogen?
Stable forms include nitrogen-14 and nitrogen-15
- List the oxidation states of various nitrogen oxides: +1, +2, +3, +4, +5 respectively
- List the different elements that Nitrogen will react with to make it basic or acidic :Nitride ion is a strong base when reacted with water, Ammonia is generally a weak acid
- Uses of nitrogen include anesthetic, Refrigerant, metal protector