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Dinitrogen monoxide (nitrous oxide, N2O) is:
- a) a brown poisonous gass that is one of the chemicals involved in the production of photochemical smog.
- b) a colorless gas that decomposes into nitrogen and oxygen upon heating.
- c) a colorless gas used in the production of nitric acid.
- d) the product of nitrogen fixation in the atmosphere.
- e) a colorless gas used in the manufacture of explosives.
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Which of the following contains a tetrahedral arrangement of phosphorus atoms?
- a) P4O6
- b) P4
- c) P4O10
- d) A and C
- e) All of the above
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Nitric acid and sulfuric acid are both powerful oxidizing agents because:
- a) the central elements (N and S) are in high oxidation states.
- b) the central elements (N and S) have low oxidation states.
- c) the elements nitrogen and sulfur are very stable.
- d) both compounds can be obtained in highly concentrated forms.
- e) more information would have to be given to answer the question.
-
The chemical formula for the superoxide ion is:
- a) O-
- b) O22-
- c) O2-
- d) O3-
- e) O2-
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The halogens are:
- a) strong acids
- b) oxidizing agents
- c) reducing agents
- d) strong bases
- e) not very reactive
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Which of the nitrogen oxides has the lowest oxidation number?
- a) nitrous oxide
- b) nitric oxide
- c) nitrogen dioxide
- d) none of the above
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Which of the halogens is important to living organisms and cooking utensils?
- a) iodine
- b) bromine
- c) chlorine
- d) fluorine
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What do nitrogen and phosphorus not have in common?
- a) as gaseous compounds, both are used as anesthetics.
- b) both are found in organic molecules such as DNA and RNA.
- c) both are used for explosives.
- d) none of the above.
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Which of the following elements is a liquid at atmospheric temperature and pressure?
- a) iodine
- b) carbon
- c) surfur
- d) bromine
- e) fluorine
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When copper is treated with dilute nitric acid, the nitric acid is reduce to:
-
The reaction of PCl3 with water produces:
- a) Cl2
- b) H3PO3
- c) H3PO4
- d) PCl5
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Which of the following are allotropes of phosphorous?
I) P4
II) P4O6
III) P4O10
IV) (P4)n
- a) I and III
- b) II and III
- c) I and II
- d) III and IV
- e) I and IV
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Which of the following is the world's most important industrial chemical?
- a) H2SO4
- b) H3PO4
- c) HClO3
- d) H2SO3
- e) HNO3
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Sodium hypochlorite is used:
- a) as an oxidizer in rocket fuels.
- b) in the manufacture of steel.
- c) as a bleaching agent.
- d) in the chemical analysis of agricultural pesticides.
- e) as an insecticide.
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The chlor-alkali process produces chlorine, Cl2 (g), in large quantities. What other industrially important substances are also produced in the chlor-alkali process?
- a) NaOH and O2
- b) Na and H2
- c) H2 and O2
- d) NaOH and H2
- e) Na and O2
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Arsenic trichloride with water
AsCl3(l) + 3H2O(l) ----> H3AsO3(aq) + 3HCl(g)
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Magnesium with dinitrogen
3Mg(s) + N2(g) ----> Mg3N2(s)
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Ammonia with excess chlorine
NH3(g) + 3Cl2(g) ----> NCl3(l) + 3HCl(g)
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Methane with stream
CH4(g) + H2O(g) ----> CO(g) +3H2(g)
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Hydrazine and oxygen
N2H4(l) + O2(g) ----> N2(g) + 2H2O(g)
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Heating a solution of ammonium nitrate
NH4NO3(aq) ----> N2O(g) + 2H2O (l)
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Sodium hydroxide solution with dinitrogen trioxide
2NaOH(aq) + N2O3(aq) ----> 2NaNO2(aq) + H2O(l)
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Heating sodium nitrate
2NaNO3(s) ----> 2NaNO2(s) + O2(g)
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Heating tetraphosphorus decaoxide with carbon
P4O10(g) + C(s) ----> P4(g) + 10CO (g)
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Finely divided iron with dioxygen
2Fe(s) + 3O2(g) ----> 2Fe2O3(s)
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Solid barium sulfide with trioxygen
BaS(s) + 4O3(s) ----> BaSO4(s) + 4O2(g)
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Solid barium dioxide with water
BaO2(s) + 2H2O(l) ----> Ba(OH)2(aq) + H2O2(aq)
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Potassium hydroxide solution with carbon dioxide
- 2KOH(aq) + CO2(g) ----> K2CO3(aq) + H2O (l)
- K2CO3(aq) + CO2(g) + H2O(l) ----> 2KHCO3(aq)
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Sodium sulfide solution with dilute sulfuric acid
Na2S(aq) + H2SO4(aq) -----> Na2SO4(aq) + H2S(g)
-
Sodium sulfite solution with cyclo-octasulfur
Na2SO3(aq) + H2SO4(aq) -----> Na2SO4(aq) + SO2(g) + H2O (l)
-
Uranium (IV) oxide with hydrogen fluoride
UO2(s) + 4HF(g) ----> UF4(s) + 2H2O(l)
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Calcium fluoride with concentrated sulfuric acid
CaF2(s) + H2SO4(l) ----> 2HF(g) + CaSO4(s)
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Liquid sulfur tetrachloride with water
SCl4(l) + 2H2O(l) -----> SO2(g) + 4HCl(g)
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Aqueous dichlorine and hot sodium hydroxide solution
3Cl2(aq) + 6NaOH(aq) ----> NaClO3(aq) + 5NaCl(s) + 3H2O(l)
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Diiodine with difluorine in a 1:5 mole ratio
I2(s) + 5F2(g) -----> 2IF5(s)
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Bromine trichloride and water
BrCl3(l) + 2H2O(l) ----> 3HCl (aq) + HBrO2(aq)
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Contrast the behavior of nitrogen and carbon by comparing the properties of:
a) methane and ammonia;
b) ethane and hydrazine
Difference in boiling points; different acid-base properties; difference in their combustions.
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Why is dinitrogen very stable?
Yet why is dinitrogen not always the product during redox reactions involving nitrogen compounds.
- a) Nitrogen has a very strong nitrogen-nitrogen triple bond.
- b) Kinetic factors can lead to other products.
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Nitrogen trifluoride boils at -129°C, whereas ammonia oils at -33°C. Account for the difference in these values.
Hydrogen bonding in ammonia molecules.
-
Draw the shape of each of the following molecules:
a) dinitrogen oxide;
b) dinitrogen tetroxide;
c) phosphorus trifluoride;
d) phosphonic acid.
-
Contrast the properties of the two common allotropes of phosphorus.
White phosphorus is a very reactive, white, waxy substance that consists of P4, while red phosphorus is a red powdery solid that consists of long polymer chains.
-
Suggest a structure for the O2F2 molecules, explaining your reasoning. Determine the oxidation number of oxygen in this compound and comment on it.
- The oxidation number of +1 for oxygen is a result of each atom being sandwiched between a more electronegative fluorine atom.

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Summarize the unique features of fluorine chemistry
Fluorine has a very weak fluorine-fluorine bond; its compounds with metals are often ionic when those of the comparable chlorides are covalent; it forms the strongest hydrogen bonds known; it tends to stabilize high oxidation states; the solubility of its metal compounds is often quite different than those of the other halides
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Which of the folowing statements is false?
- a) Chemical properties of group 15 elements are uniform.
- b) Group 15 elements exhibit a wide range of oxidation states.
- c) Group 15 elements form many compounds with oxygen.
-
White and black phosphorus are ___________ forms of the chemical element phosphorus.
- a) isotopic
- b) allotropic
- c) polymorphic
-
Which of the following elements is used as a dopant in solid state devices?
-
Going down the group:
- a. The +3 oxidation state becomes more favorable relative to the +5 one.
- b. The +5 oxidation state becomes more favorable relative to the +3 one.
- c. The +3 oxidation state predominates; the +5 one is rarely manifested.
-
The Haber-Bosch process, which has had a major impact on civilization, produces:
- a. hydrazine, N2H4
- b. ammonia, NH3
- c. hydroxylamine, NHOH
-
PF3 is a ligand that is similar to CO in that:
- a) It is a weak σ-donor and a weak π-acceptor.
- b) It is a strong σ-donor and a strong π-acceptor.
- c) It is a weak σ-donor and a strong π-acceptor.
-
The synthesis of organophosphorus compounds includes:
-
NO is:
- a) rapidly oxidized by O2 to NO2 in the atmosphere.
- b) an odd electron molecule.
- c) not an atmospheric pollutant.
-
When heated above 200°C, phosphoric acid, H3PO4:
- a) forms polyphosphates by condensation
- b) decomposes thermally
- c) releases P2O5
-
Select the correct answer:
- a. Organometallic compounds of group 15 elements in +3 oxidation state become less stable in the order Bi >
- Sb > As. Aryl compounds are more stable than alkyls.
- b. Organometallic compounds of group 15 elements in +3 oxidation state become less stable in the order As >
- Sb > Bi. Aryl compounds are more stable than alkyls.
- c. Organometallic compounds of group 15 elements in +3 oxidation state become less stable in the order As >
- Sb > Bi. Aryl compounds are less stable than alkyls.
-
The electron configuration of group 16 elements is ns2np4. This configuration suggests.
- a. a maximum oxidation number of +6
- b. a maximum oxidation number of +4
- c. a maximum oxidation number of –2
-
Sulfur-containing impurities that are naturally present in crude oil and natural gas are removed by:
- a. fractional distillation
- b. the Frasch process
- c. the Claus process
-
Water can be viewed as a hydride of oxygen. By comparison with the heavier hydrides in the group, water's melting and boiling points are higher than expected because:
- a. The water molecules have the lowest bond length of all group 16 hydrides.
- b. The water molecules form hydrogen bonds to a much higher degree than the remaining group 16 hydrides.
- c. The water molecules have the highest bond angles of all group 16 hydrides.
-
The geometry of the SF4 molecule is:
- a. tetrahedral
- b. triagonal planar
- c. octahedral
-
Identify the free radical chain reaction that produce acid rain in the atmosphere:
-
Select the correct statement about the oxoanions of sulfur:
- a) SO32- is a strong oxidizing agent; SO42- is a strong reducing agent; S2O82- is unreactive.
- b) SO32- is a strong reducing agent; SO42- is a strong oxidizing agent; S2O82- is unreactive.
- c) SO32- is a strong reducing agent; SO42- is unreactive; S2O82- is a strong oxidizing agent.
-
Diatomic oxygen readily removes electrons from metals to form a variety of metal oxides. In general:
- a) Oxides of M2+ ions (MO formula) have a rock salt structure (6:6 coordination).
- b) Oxides of M3+ ions (M2O3 formula) have a fluorite structure (6:3 and 8:4 coordination).
- c) Oxides with an MO4 formula have a 6:4 coordination.
-
S, Se, and Te form polyanions as follows:
- a. S forms chains and bicyclic ring polysulfides.
- b. Se forms chain and ring polyselenides.
- c. Te forms chain polytellurides only.
-
In the case of oxoacids of sulfur:
- a. Sulfuric acid decomposes but forms stable salts.
- b. Thiosulfuric acid is a strong acid.
- c. Sulfurous acid is actually an aqueous solution of SO2.
-
Sulfur/nitrogen compounds:
- a) decompose explosively
- b) are stable
- c) do not exist
-
The halogens have high electron affinity because:
- a. They can accommodate only one electron in their valence shell; therefore the energy required for this process is low.
- b. The incoming electron can occupy an orbital of an incomplete valence shell and thus experience strong nuclear attraction.
- c. The nuclear attraction to the electrons in their atoms is high and tends to draw new electrons in.
-
All group 17 elements:
- a. undergo thermal or photochemical dissociation in the gas phase to form free radicals
- b. are gases at room temperature
- c. sublimate easily
-
Why are aqueous fluoride solutions not used in the production of fluorine by electrolysis?
- a. because fluorides are insoluble in water.
- b. because water is oxidized at a much lower potential than F- and because any F2 produced would react rapidly with the water.
- c. because the electrolysis of water solutions of fluorides would require a prohibitively large amount of water and energy.
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Fluorine atoms are small and their electrons are tightly gripped by the nucleus. Therefore, molecular fluorine compounds have:
- a. high polarizabilities and strong dispersion interactions.
- b. low polarizabilities and strong dispersion interactions.
- c. low polarizabilities and weak dispersion interactions.
-
What is the molecular (electron-domain) geometry of ClF3 as predicted by VSEPR?
- a. trigonal bipyramidal
- b. trigonal pyramidal
- c. trigonal planar
-
When I2 is added to a solution containing I-, a deep brown color develops. How can that phenomenon be explained?
- a) I- is oxidized to I2.
- b) I2 is dissolved in the water.
- c) Polyiodides, such as I3- and I5-, are formed.
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Perchlorate is a very weak Brønsted base and a weak Lewis base and is used as a weakly coordinating ion that can be easily displaced from a complex by other ligands. When using the perchlorate ion in this situation, care must be taken because:
- a. The perchlorate ion is a powerful oxidizing agent that can explode unexpectedly and unpredictably.
- b. The perchlorate ion is a powerful oxidizing agent that rapidly oxidizes the ligands before complexes are formed for further study.
- c. The perchlorate ion is a powerful oxidizing agent that rapidly oxidizes the metal acceptors before complexes are formed for further study.
-
Basic solutions of chlorine, bromine, and iodine undergo _____, with the formation of +1 (XO-) and –1 (X-) species:
- a) oxidation
- b) reduction
- c) disproportionation
-
The oxidation of molecules and ions by halogen oxoanions increases in the order:
- a) ClO2-< ClO3-< ClO4-
- b) ClO4-< BrO4-< IO4-
- c) IO3-< IO4-
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Why must care be taken during the high-temperature depolymerization of polytetrafluoroethylene (PTFE)?
- a. because the monomer, tetrafluoroethylene, is highly toxic
- b. because a byproduct, perfluoroisobutylene, is highly toxic
- c. because PTFE decomposes explosively at high temperatures
-
The inert gases possess an electron configuration of ns2np6. Which statement applies to their ionization energy and electron affinity?
- a. low ionization energies and negative electron affinities
- b. high ionization energies and negative electron affinities
- c. low ionization energies and positive electron affinities
-
Which noble gas seems to defy the notion that group 18 elements are chemically inert?
-
Which of the noble gases is classified as an indoor air pollutant?
- a) Ne
- b) Rn
- c) No inert gas is an air pollutant
-
Xe forms _________ with fluorine.
- a) XeF2 and XeF4.
- b) XeF2, XeF4, and XeF6.
- c) no compounds.
-
Xenon fluorides:
- a) are strong reducing agents.
- b) form complexes with F2.
- c) form complexes with F-.
-
Xe fluorides are of interest because:
- a. They can be used to prepare noble gas compounds with elements other than fluorine and oxygen.
- b. The molecular shape of their complexes with fluoride ions is unknown; more research needs to be done.
- c. They are the only compounds of Xe.
-
Xe oxides can be prepared by direct interaction of the element with oxygen.
- a. This statement is correct.
- b. This statement is incorrect.
- c. Only XeO3 can be prepared that way; XeOF2 and XeOF4 cannot.
-
Organoxenon compounds can be prepared by:
- a. direct interaction between an aromatic hydrocarbon and Xe
- b. hydrolysis of phenol in the presence of a Xe fluoride
- c. xenodeborylation
-
The stability of the complexes M(CO)5E (where M = Cr, Mo, or W and E = Ar, Kr, or Xe) decreases in the order:
- a. W > Mo ≈ Cr and Xe > Kr > Ar
- b. Cr > Mo ≈ W and Xe > Kr > Ar
- c. Cr > Mo ≈ W and Ar > Kr > Xe
-
Which statement is correct?
- a. Like Xe, Kr and Rn form fluorides and oxides.
- b. Kr and Rn can form fluorides but in a more limited fashion than Xe.
- c. Kr and Rn do not form fluorides and oxides.
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