課程名稱︰普通化學丙
課程性質︰必修(大一)
課程教師︰鄭淑芬
開課系所︰機械系
考試時間︰95年04月06日
試題 :
General Chemistry,1st Mid-term Exam
Single Choice Questions(40%,2 points per question)
1. What answer should be reported if 4.560 is added to 2.6×10^-3 ?
(a) 4.6 (b) 4.56 (c) 4.563 (d) 435626
2.The systematic (IUPAC) name of MgI2 is:
(a)manganese iodide (b)magnesium diiodide
(c)magnesium iodide (d)magnesium(Π) iodide
3.How many electrons are present in a Ca^2+ species ?
(a) 40 (b) 38 (c) 20 (d) 18
4.Common desired characteristics of explosives include ?
(a)relatively large quantities of released energy
(b)creation of small , gaseous molecules as products
(c)a rapid rate of reaction
(d)all of the above
5. given that : CaCl2(aq)+NaHCO3(aq)→CaCO3(s)+NaCl(aq)+HCl(aq), which of the
following species is classified as a spector ion ?
(a) Na^1+ (b) CO3¯ (c) OH¯ (d) Ca^2+
6. Complete and balance the following redox equation.What is the coefficient of
H2O when the equation is balanced with the set of smallest whole numbers ?
MnO4¯+SO3^2¯→Mn^2+ +SO4^2¯(acidic solution)
(a) 3 (b) 4 (c) 5 (d) 8
7. Which of the following equations best illustrate the net ionic equation for
reaction of radium chloride with potassium sulfate ?
(a)RaCl2 +K2SO4 →RaSO4 + 2 KCl
(b)Ra^2+(aq)+2 Cl¯(aq)+2 K^+(aq)+SO4^2¯(aq)→RaSO4(s) +2 C1¯(aq) +2 K^+(aq)
(c)Ra^2+(aq) +SO4^2¯(aq) →RaSO4(s)
(d)Ra^2+(aq)+2 Cl¯(aq)+2 K^+(aq)+SO4^2¯(aq)→RaSO4(s) +2 KCl(s)
8.Which of the following substances is an example of a strong electrolyte ?
(a)C6H12O6 (b)KNO3 (c) Ag2SO4 (d)C4H10
9.What volume of a 1.00M HCl solution is required to create 300mL of a
0.250M HCl solution ?
(a) 30.0 mL (b)25.0 mL (c)60.0 mL (d) 75.0 mL
10. Consider the reaction between KI and Pb(NO3)2 to form lead iodide
precipitate. How much of the insoluble precipitate will be recovered
if 582.4 grams of Pb(NO3)2 reacts with 596.8 grams of KI ?
(a) 1.353kg (b) 641.0g (c)257.3g (d)810.6g
11. A sample of a hydrocarbon is combusted completely in O2(g) to produce
21.83g CO2(g) and 8.95g H2O. Which of the following can be the molecular
formula of the hydrocarbon ?
(a) CH4 (b) C2H6 (c) C3H6 (d) C4H6
12.A fertilizer manufacturer uses the reaction between hydrogen and nitrogen to
create ammonia (assume no other reactants or products). If 9.5×10^3 moles
of hydrogen and 1.7×10^3 moles of nitrogen react at 277 K and 1.25atm, what
volume of ammonia is produced ?
(a)2.1×10^4L (b)3.0×10^4L (c)6.2×10^4L (d)1.9×10^5L
13.In quantum mechanics, an "l" value of 2 corresponds to a letter designation
of orbital:
(a) s (b) p (c) d (d) f
14.The "ml" value of the quantum number assigned to an atom best describes the
orbital's:
(a) shape (b) size (c) orientation (d)electron spin
15.How many orbitals are in n=4 shell of H-like atom ?
(a) 4 (b) 8 (c) 16 (d) 18
16. Which of the following has the largest radius ?
(a) Na (b) K^+ (c) Rb (d) Cs^+
17. Which of the following compounds illustrates sp2 hybridization?
(a) NCl3 (b) CF2Cl2 (c) C6H6 (d) SnCl2
↑ ↑ ↑ ↑
18.What is the molecular geometry of PCl3
(a)trigonal pyramidal (b) see-saw
(c)tetrahe dral (d) T-shape
19.Which of the following molecules is most polar ?
(a) NaCl (b) C2F6 (c) HF (d) H2S
20.Which of the following species is non-ploar?
(a) NF3 (b) IF3 (c) SF4 (d) PF5
Prblems:
21.Write the correct chemical formulas to distinguish between
(a) sodium carbonate and sodium hydrogen carbonate
(b) aluminum nitride and aluminum nitrite
(c) potassium phosphate and potassium phosphite
(d) iron(Π)hydroxide and iron(Π) peroxide
(e) hydrogen sulfide and hydrosulfuric acid (10%)
22.What is the maximum number of electrons that can have following quantum
numbers: (5%)
(a) n=0, l=1
(b) n=3, l=1
(c) n=2, l=2, ml=-1
(d) n=3, l=2, ml=0
(e) n=1, l=2, ml=-1, ms=1/2
23.Write the chemical formula of the following compounds: (10%)
(a) PVC
(b) Teflon
(c) pyridine
(d) 2-ethyl-6-methylphenol
(e)圖(抱歉，不會畫)
24. Naturally occurring strontium consists of the following four isotopes.
The atomic mass of strontium is 87.62. Calculate the percent abundance
of Strontium-87 and Strontium-88. (5%)
--------------------------------------------------------------------------
Isotope Atomic mass,u Percent abundance(%)
--------------------------------------------------------------------------
Strontium-84 83.913 0.56
Strontium-86 85.909 9.86
Strontium-87 86.909 x
Strontium-88 87.906 y
--------------------------------------------------------------------------
25.A 2.50L flask contains carbon dioxide at 25'C and 646.0 Torr. After 25.8% of
the gas is allowed to escaped, the flask is heated to 100'C. What is the
expected pressure in the flask ? (5%)
26.NO, NO2, N2O and NO3¯all contain N—O bond.
(a)Draw the Lewis structures of these species, including all the possible
resonance forms.
(b)Rank the four species in order of increasing N—O bond strength. (10%)
27.In 2.00 min, 150mL of Ne at 100'C effuses through a small hole. At the same
temperature, it take 3.19 min for the same volume of a hydro carbon compound
to effuse through the hole. (5%)
(a)What is the molecular mass of the compound ?
(b)When the temperature is lowered to 10'C, how long does it take for this
hydrocarbon gas to diffuse through the hold?
28.The van der Waals equation is used to describe the actual behavior of real
gases. ( P + an^2/V^2 )(V-nb) = nRT (10%)
(a)What do the empirical constants "a" and "b" mean?
(b)Put the following gases in order of {increasing} in "a" and "b" values,
respectively, and briefly explain your answers: He, O2, CO2, H2O, CCl4 (10%)
29.It requires 186 kj/mol to eject electrons from sodium metal.
(a)What is the minimum frequency of light necessary to emit electrons from
sodium via the photoelectric effect?
(b)If sodium is irradiated with light of 212 nm, what is the maximum velocity
of the emitted electron?
(c)What is the wavelength of the matter wave of this emitted electron? (8%)
30. Describe the contribution of the following scientists and give the
representative equations in understanding the atomic structure. (6%)
(a) Louis de Broglie (b) Werner Heisenberg
(c) Erwin Schrodinger
31.
(a) Show the molecular orbial energy-level diagram of H2, indicating the
bonding and anti-bonding orbitals. (2%)
(b) Write the valence-shell electron configurations and bond orders of H2,
H2^- and H2^+ . Put the above three species in order of increasing bond
length. (5%)
(c) Indicate the above three species to be "paramagnetic" or "diamagnetic" ?
(3%)
_________________
Useful informations:
gas constant, R=0.08206 atm L /(mol K)
Avogadro constant N = 6.022×10^23 /mol
Planck's constant, h=6.626×10^-34 J.s =6.626×10^-27 erg.s
1 atm = 760mmHg = 760Torr
Speed of light, c =2.9979×10^8
Mass of electron =9.109×10^-31 kg
Atomic mass: H = 1.00 He = 4.00 C = 12.01
N = 14.01 O = 16.00 Ne = 20.18
Na = 22.99 Mg = 24.31 Cl = 35.45
K = 39.10 I = 126.90 Pb = 207.19
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