天津大学
- The photoelectric effect is __________.
- A combination of sand, salt, and water is an example of a __________.
- Which isoelectronic series is correctly arranged in order of increasing radius?
- The 4d subshell in the ground state of atomic xenon contains __________ electrons.
- Which of the following reactions is a redox reaction? (a) K2CrO4 + BaCl2 → BaCrO4 + 2KCl; (b) Pb22+ + 2Br- → PbBr; (c) Cu + S → CuS
- CO2 from hydrocarbon combustion creates a major environmental problem that is described as __________.
- When the following equation is balanced, the coefficients are __________. Al(NO3)3 + Na2S → Al2S3 + NaNO3
- Of the following statements, __________ is not true for oxygen.
- Of the following transitions in the Bohr hydrogen atom, the __________ transition results in the emission of the highest-energy photon.
- Metals can be __________ at room temperature.
- The most common and stable allotrope of sulfur is __________.
- __________ is the chemical symbol for elemental sodium.
- The atomic number indicates __________.
- There are __________ orbitals in the third shell.
- The correct name for SrO is __________.
- Which of the following is not a colloid?
- A closed-end manometer was attached to a vessel containing argon. The difference in the mercury levels in the two arms of the manometer was 12.2 cm. Atmospheric pressure was 783 mm Hg. The pressure of the argon in the container was __________ mm Hg.
- The electron configuration of a ground-state Ag atom is __________.
- __________ solids consist of atoms or molecules held together by dipole-dipole forces, London dispersion forces, and/or hydrogen bonds.
- The average kinetic energy of the particles of a gas is directly proportional to __________.
- Which group 16 element is a metal?
- Classify the following compounds as weak bases (W) or strong bases (S): ammonia, fluoride ion and sodium hydroxide.
- Cl2 (g) + H2O (l) → ________
- Which of the following liquids will have the lowest freezing point?
- The reaction used to inflate automobile airbags __________.
- The Lewis structure of HCN (H bonded to C) shows that __________ has __________ nonbonding electron pairs.
- An electron cannot have the quantum numbers n = __________, l = __________, ml = __________.
- Of the following, __________ is a valid statement of Charles' law.
- Of the hydrogen halides, only __________ is a weak acid.
- As the concentration of a solute in a solution increases, the freezing point of the solution __________ and the vapour pressure of the solution __________.
- The mass % of C in methane (CH4) is __________.
- When solutions of strong electrolytes in water are formed, the ions are surrounded by water molecules. These interactions are best described as a case of __________.
- Of the following gases, __________ will have the greatest rate of effusion at a given temperature.
- Which one of the following reactions is a redox reaction?
- An ideal gas differs from a real gas in that the molecules of an ideal gas __________.
- The initial or tentative explanation of an observation is called a(n) __________.
- The chloride of which of the following metals should have the greatest lattice energy?
- In the nitrite ion (NO2-), __________.
- Which hydroxides are strong bases?
- Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN3 (s) → 2Na (s) + 3N2 (g) How many moles of N2 are produced by the decomposition of 2.88 mol of sodium azide?
- Methane and ethane are both made up of carbon and hydrogen. In methane, there are 12.0 g of carbon for every 4.00 g of hydrogen, a ratio of 3:1 by mass. In ethane, there are 24.0 g of carbon for every 6.00 g of hydrogen, a ratio of 4:1 by mass. This is a statement of the law of __________.
- Which two bonds are most similar in polarity?
- In which of the following atoms is the 3s orbital closest to the nucleus?
- How many oxygen atoms are contained in 2.74 g of Al2(SO4)3?
- The solubility of lead (II) chloride (PbCl2) is 1.6 × 10-2 M. What is the Ksp of PbCl2
- When gases are treated as real, via use of the van der Waals equation, the actual volume occupied by gas molecules __________ the pressure exerted and the attractive forces between gas molecules __________ the pressure exerted, as compared to an ideal gas.
- The recommended adult dose of Elixophyllin , a drug used to treat asthma, is 6.0 mg/kg of body mass. Calculate the dose in milligrams for a 115-lb person. 1 lb = 453.59 g.
- A 0.100 m solution of which one of the following solutes will have the lowest vapour pressure?
- A mixture of two gases was allowed to effuse from a container. One of the gases escaped from the container 1.43 times as fast as the other one. The two gases could have been __________.
- Colligative properties of solutions include all of the following except __________.
- How many molecules of CH4 are in 48.2 g of this compound?
- The van der Waals equation for real gases recognizes that __________.
- The concentration of iodide ions in a saturated solution of lead (II) iodide is __________ M. The solubility product constant of PbI2 is 1.4 × 10-8.
- The number of monkeys in a boat is how many?
- Which one of the following concentration units varies with temperature?
- At 333 K, which of the pairs of gases below would have the most nearly identical rates of effusion?
- What is the coefficient of O2 when the following equation is completed and balanced? C4H8O2 + O2 → ________
- The concentration of chloride ion in a solution that contains 35.0 ppm chloride is __________% by mass.
- The acid-dissociation constant for chlorous acid, HClO2, at 25.0 °C is 1.0 × 10-2. Calculate the concentration of H+ if the initial concentration of acid is 0.10 M.
- A fixed amount of gas at 25.0 °C occupies a volume of 10.0 L when the pressure is 629 torr. Use Charles's law to calculate the volume (L) the gas will occupy when the temperature is increased to 121 °C while maintaining the pressure at 629 torr.
- A fixed amount of gas at 25.0 °C occupies a volume of 10.0 L when the pressure is 667 torr. Use Boyle's law to calculate the pressure (torr) when the volume is reduced to 7.88 L at a constant temperature of 25.0 °C.
- On a clear day at sea level, with a temperature of 25 °C, the partial pressure of N2 in air is 0.78 atm and the concentration of nitrogen in water is 5.3 × 10-4 M. When the partial pressure of N2 is __________ atm, the concentration in water is 1.1 × 10-3 M.
- The volume of a sample of gas (2.49 g) was 752 mL at 1.98 atm and 62 °C. The gas is __________.
- An aqueous solution of a soluble compound (a nonelectrolyte) is prepared by dissolving 33.2 g of the compound in enough water to form 250 mL of solution. The solution has an osmotic pressure of 1.2 atm at 25.0 °C What is the molar mass (g/mL) of the compound?
- Which of the following is an illustration of the law of constant composition?
- How much faster does 235UF6 effuse than 238UF6?
- A solution is prepared by dissolving 0.60 g of nicotine (a nonelectrolyte) in water to make 12 mL of solution. The osmotic pressure of the solution is 7.55 atm at 25 °C. The molecular weight of nicotine is ________ g/mol.
A:the ejection of electrons by a metal when struck with light of sufficient energy B:the darkening of photographic film when exposed to an electric field C:the production of current by silicon solar cells when exposed to sunlight D:the total reflection of light by metals giving them their typical luster E:a relativistic effect
答案:the ejection of electrons by a metal when struck with light of sufficient energy
A:pure substance B:solid C:homogeneous mixture D:heterogeneous mixture E:compound
答案:heterogeneous mixture
A:Ca2+ < K+ < Cl- < Ar B:Ca2+ < K+ < Ar < Cl- C:Cl- < Ar < K+ < Ca2+ D:Ca2+ < Ar < K+ < Cl- E:K+ < Ca2+ < Ar < Cl-
答案:Ca2+ < K+ < Ar < Cl-
A:6 B:8 C:10 D:36 E:2
答案:10
A:(b) only B:(c) only C:(b) and (c) D:(a) and (c) E:(a) only
答案:(c) only
A:acid rain B:photochemical smog C:the greenhouse effect D:all of the above E:stratospheric ozone depletion
答案:the greenhouse effect
A:4, 6, 3, 2 B:2, 1, 3, 2 C:2, 3, 2, 3 D:2, 3, 1, 6 E:1, 1, 1, 1
答案:2, 3, 1, 6
A:Oxygen forms peroxide and superoxide anions. B:Oxygen is a colourless gas at room temperature. C:The chemical formula of ozone is O3. D:Dry air is about 79 % oxygen. E:The most stable allotrope of oxygen is O2.
答案:Dry air is about 79 % oxygen.
A:n = 1 → n = 4 B:n = 6 → n = 3 C:n = 3 → n = 6 D:n = 1 → n = 6 E:n = 6 → n = 1
答案:n = 6 → n = 1
A:solid, liquid, or gas B:liquid or gas C:solid or liquid D:liquid only E:solid only
A:S4 B:S8 C:S D:Sulfur does not form allotropes E:S2
A:S B:W C:Sn D:So E:Na
A:the number of atoms in 1 g of an element B:the total number of neutrons and protons in a nucleus C:the number of neutrons in a nucleus D:the number of protons or electrons in a neutral atom E:the number of different isotopes of an element
A:25 B:9 C:1 D:4 E:16
A:strontium peroxide B:strontium oxide C:strontium hydroxide D:strontium monoxide E:strontium dioxide
A:whipped cream B:smoke C:homogenized milk D:air E:fog
A:795 B:771 C:882 D:122 E:661
A:[Ar]4s2 4d9 B:[Ar]4s14d10 C: [Kr]5s14d10 D:[Kr]5s23d9 E:[Kr]5s2 4d10
A:Molecular B:Metallic and covalent-network C:Metallic D:Covalent-network E:Ionic
A:the rms speed B:the square of the rms speed C:the square of the particle mass D:the square root of the rms speed E:the particle mass
A:selenium B:polonium C:tellurium D:sulfur E:tellurium and polonium
A:S S S B:S W W C:W S W D:W S S E:W W S
A:2 HCl (aq) + O2 (g) B:HCl (aq) + HOCl (aq) C:Cl2 (aq) + H2O (l) D:2 HCl (aq) + O2- (g) E:2Cl- (aq) + H2O (l)
A:aqueous NaI (0.030 m) B:aqueous FeI3 (0.030 m) C:aqueous glucose (0.050 m) D:pure H2O E:aqueous CoI2 (0.030 m)
A:produces sodium gas B:is a decomposition reaction C:is a combustion reaction D:is a combination reaction E:violates the law of conservation of mass
A:C, 2 B:N, 2 C:C, 1 D:N, 1 E:H, 1
A:1, 1, 1 B:2, 0, 0 C:2, 1, -1 D:3, 2, 1 E:3, 1, -1
A:V = constant × n B:PV = constant C:V = constant × P D: V/T = constant E:P/T = constant
A:HCl (aq) B:HF (aq) C:HI (aq) D:They are all weak acids E:HBr (aq)
A:increases, decreases B:increases, increases C:decreases, increases D:decreases, decreases E:decreases, is unaffected
A:25.13 B:7.743 C:133.6 D:74.87 E:92.26
A:solvation B:dehydration C:supersaturation D:hydration E:crystallization
A:CH4 B:HCl C:NH3 D:HBr E:Ar
A:None of the above is a redox reaction. B:NaOH + HCl → NaCl + H2O C:H2O + NaCl → NaOH + HCl D:Pb2+ + 2Cl- → PbCl2 E:AgNO3 + HCl → HNO3 + AgCl
A:have no attraction for one another B:have no kinetic energy C:have appreciable molecular volumes D:have a molecular weight of zero E:have an average molecular mass
A:hypothesis B:experiment C:law D:test E:theory
A:potassium B:sodium C:caesium D:lithium E:rubidium
A:both bonds are double bonds B:both bonds are the same C:there are 20 valence electrons D:one bond is a double bond and the other is a single bond E:both bonds are single bonds
A:None of these is a strong base B:KOH, NaOH, Ba(OH)2 C:KOH, Ba(OH)2 D:KOH, NaOH E:Sr(OH)2 , KOH, NaOH, Ba(OH)2
A:8.64 B:1.92 C:0.96 D:1.44 E:4.32
A:constant composition B:conservation of mass C:conservation of matter D:multiple proportions E:octaves
A:I–Br and Si–Cl B:B–F and Cl–F C:Cl–Cl and Be–Cl D:O–F and Cl–F E:Al–Cl and I–Br
A:Br B:At C:The 3s orbitals are the same distance from the nucleus in all of these atoms. D:I E:Cl
A:12 B:7.22 × 1024 C:8.01 × 10-3 D:5.79 × 1022 E:6.02 × 1023
A:1.6 × 10-5 B:3.1 × 10-7 C:4.1 × 10-6 D:5.0 × 10-4 E:1.6 × 10-2
A:increases, decreases B:does not affect, decreases C:does not affect, increases D:increases, increases E:decreases, increases
A:3.1 × 105 B:313 C:1.5 D:1521 E:24
A:Ca(ClO4)2 B:KClO4 C:NaCl D:Al(ClO4)3 E:sucrose
A:Cl2 and SF6 B:CO and CO2 C:O2 and Cl2 D:CO and SF6 E:O2 and SF6
A:elevation of the boiling point of a solution upon addition of a solute to a solvent B:depression of the freezing point of a solution upon addition of a solute to a solvent C:an increase in the osmotic pressure of a solution upon the addition of more solute D:depression of vapor pressure upon addition of a solute to a solvent E:the increase of reaction rates with increase in temperature
A:4 B:3 C:5.00 × 1024 D:1.81 × 1024 E:2.90 × 1025
A:gas particles have non-zero volumes and interact with each other B:the molecular attractions between particles of gas decreases the pressure exerted by the gas C:molar volumes of gases of different types are different D:all of the above statements are true E:the non-zero volumes of gas particles effectively decrease the amount of "empty space" between them
A:1.4 × 10-8 B:3.8 × 10-4 C:3.5 × 10-9 D:1.5 × 10-3 E:3.0 × 10-3
A:113.7 B:113.73635 C:113.736 D:113.74 E:1.1 × 102
A:mass percent B:molality C:mole fraction D:all of the above E:molarity
A:N2O and NO2 B:CO and CO2 C:N2 and O2 D:CO and N2 E:NO2 and N2O4
A:2 B:6 C:5 D:1 E:3
A:3.50 × 10-3 B:3.50 × 10-6 C:3.50 × 102 D:3.50 × 101 E:3.50 × 10-2
A:3.7 × 10-2 B:1.0 × 10-3 C:1.0 × 10-2 D:2.7 × 10-2 E:3.2 × 10-2
A:7.56 B:48.4 C:10.9 D:13.2 E:2.07
A:846 B:0.118 C:526 D:1.11 E:5.26 × 104
A:1.6 atm B:0.63 atm C:1.0 atm D:0.78 atm E:2.1 atm
A:Ne B:NO2 C:NH3 D:SO2 E:SO3
A:6.8 × 102 B:28 C:2.3 × 102 D:1.0 × 103 E:2.7 × 103
A:Water is 11% hydrogen and 89% oxygen by mass B:Water can be separated into other substances by a chemical process C:Water boils at 100°C at 1 atm pressure D:Water and salt have different boiling points E:Water is a compound
A:1.006 times as fast B:1.018 times as fast C:1.004 times as fast D:1.009 times as fast E:1.013 times as fast
A:28 B:50 C:0.6 D:43 E:160
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