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Transcript
Chem152
Dr. saidane
Final Exam
1. What is the term for the smallest particle that represents an element?
A) atom
B) entity
C) formula unit
D) molecule
E) none of the above
2. What is the term for the number that identifies a particular element?
A) atomic number
B) element number
C) mass number
D) substance number
E) none of the above
3. Which of the following laws states that the total mass and energy before a chemical reaction is
equal to the total mass and energy after the reaction?
A) law of conservation of energy
B) law of conservation of mass
C) law of conservation of mass and energy
D) law of definite composition
4. What is the term for a compound composed of two or more nonmetal atoms?
A) atom
B) entity
C) formula unit
D) molecule
E) none of the above
5. Which of the following describes a substance in the solid physical state?
A) The substance has a fixed shape.
B) The substance has a fixed volume.
C) The substance compresses negligibly.
D) all of the above
E) none of the above
6. What is the total number of atoms in the chemical formula C17H19NO3?
A) 4
B) 39
C) 40
D) 42
E) none of the above
7. Which of the following observations is evidence for a physical change?
A) decomposing sodium nitrate
B) evaporating ethyl alcohol
C) forming insoluble silver chloride
D) releasing oxygen gas E) none of the above
8. What is the term for the weighted average mass of all the naturally occurring isotopes of an
element?
A) atomic notation
B) atomic number
C) atomic mass
D) mass number
E) none of the above
9. How many neutrons are in the nucleus of an atom of silver-107?
A) 47
B) 60
C) 107
D) 154
E) none of the above
10. What is the term for an atom (or group of atoms) that bears a charge as the result of gaining
or losing valence electrons?
A) anion
B) cation
C) ion
D) polyatomic ion E) none of the above
11. What is the name of the family of elements in Group IIA/2?
A) alkali metals
B) alkaline earth metals
C) halogens
D) noble gases
E) none of the above
12. Which of the following is a general trend in the periodic table for the atomic radius of the
elements? A) increases from left to right, increases from bottom to top
B) increases from left to right, decreases from bottom to top
C) decreases from left to right, increases from bottom to top
D) decreases from left to right, decreases from bottom to top
13. Which element has the following electron configuration: [Kr] 5s2 4d10 5p2?
A) Pb
B) Sn
C) Sr
D) Xe
E) Zr
14. Predict the number of valence electrons for a Group VA/15 element.
A) 2
B) 3
C) 5
D) 8
E) 15
15. Which of the following is the electron dot formula for an atom of potassium?
A)
B)
C)
D)
E)
16. What is the term for a compound containing one metal and one nonmetal?
A) binary acid
B) binary ionic
C) binary molecular
D) ternary ionic
E) ternary molecular
17. What is the chemical formula for cobalt(III) bromide?
A) Co3Br
B) CoBr3
C) Co3Br2
D) Co2Br3
E) Co3Br3
18. What is the ionic charge for the chromium ion in Cr2(SO4)3?
A) zero
B) 1+
C) 2+
D) 3+
E) none of the above
19. What is the systematic name for aqueous HF?
A) hydrogen fluoride
B) hydrofluoric acid
C) fluorous acid
D) fluoric acid
E) hypofluoric acid
20. What is the term for a type of reaction in which an acid and a base react to produce a salt and
water?
A) combination
B) decomposition
C) double replacement
D) neutralization
E) single replacement
21. What term refers to an insoluble solid substance that is produced from a chemical reaction in
aqueous solution?
A) condensate
B) precipitate
C) salt
D) suspension E) none of the above
22. Which of the statements below best describes the following reaction?

Na2CO3(s)  Na2O(s) + CO2(g)
A) Sodium carbonate decomposes with heat.
B) Sodium carbonate decomposes to sodium oxide and carbon dioxide.
C) Sodium carbonate decomposes to sodium oxide and carbon dioxide gas.
D) Sodium carbonate is heated to give sodium oxide and carbon dioxide.
E) Solid sodium carbonate is heated to give solid sodium oxide and carbon dioxide gas.
23. Which of the following elements occurs naturally as diatomic molecules?
A) chlorine gas B) fluorine gas C) iodine vapor D) all of the above E) none of the above
24. What is the coefficient of oxygen gas after balancing the following equation?
___P(s) + ___O2(g) → ___P2O3(s)
A) 1
B) 2
C) 3
D) 5
E) none of the above
25. What are the products from the following single-replacement reaction?
Al(s) + Pb(NO3)2(aq) →
A) Pb and Al(NO3)3
B) Pb and Al(NO2)3
C) PbO and Al(NO3)3
D) PbO and Al(NO2)3
E) no reaction
26. What is the term for a temperature of 0°C and a pressure of 1 atm?
A) atmospheric temperature and pressure
B) experimental temperature and pressure
C) ideal gas temperature and pressure
D) standard temperature and pressure
E) none of the above
27. What is the term for a substance that accepts a proton in an acid-base reaction?
A) Arrhenius acid
B) Arrhenius base
C) Brønsted-Lowry acid
D) Brønsted-Lowry base
E) none of the above
28. What is the term for the stage in an acid-base titration when the indicator changes color?
A) color point
B) endpoint
C) indicator point
D) stoichiometric point
E) none of the above
29. What is the term for a chemical equation that portrays an ionic reaction after spectator ions
have been canceled?
A) dissociation equation
B) ionization equation
C) net ionic equation
D) total ionic equation
E) none of the above
30. What is the term for a solution that is a good conductor of electricity?
A) aqueous electrolyte
B) nonelectrolyte
C) strong electrolyte
D) weak electrolyte
E) none of the above
31. What is the term for a chemical bond characterized by the sharing of one or more pairs of
valence electrons?
A) covalent bond
B) electrovalent bond
C) ionic bond
D) valence bond
E) none of the above
32. What type of bond is characterized by sharing two pairs of electrons?
A) single bond
B) double bond
C) triple bond
D) electrovalent bond
E) none of the above
33. What is the term for a chemical bond characterized by the attraction between a cation and
anion?
A) coordinate covalent bond
B) ionic bond
C) nonpolar bond
D) polar bond
E) none of the above
34. What is the term for the concentration expression that relates the moles of solute dissolved in
each liter of solution?
A) mass/mass percent (m/m %)
B) molarity (M)
C) molality (m)
D) parts per million (ppm)
E) none of the above
35. How many orbitals are in the 4p subshell?
A) 1
B) 3
C) 4
D) 5
E) none of the above
36. What is the systematic name for (NH4)2CO3?
A) ammonium carbonate
B) ammonium dicarbonate C) diammonium carbonate
D) diammonium hydrogen carbonate
E) dinitrogen octahydrogen carbonate
37. Predict the chemical formula for sodium sulfide, given the formula of lithium oxide, Li2O.
A) NaS
B) Na2S
C) NaS2
D) Na2S3
E) Na3S2
38. What is the ionic charge for the manganese ion in MnSO4?
A) zero
B) 1+
C) 2+
D) 3+
E) none of the above
39. What are the products from the following double-replacement reaction?
BaCl2(aq) +K2SO4(aq) →
A) BaS and KClO4
B) BaSO3 and KCl
C) BaSO3 and KClO4
D) BaSO4 and KCl
E) BaSO4 and KClO4
40. What are the products from the complete neutralization of sulfuric acid with aqueous sodium
hydroxide?
A) Na2S(aq) and H2O(l) B) NaHSO3(aq) and H2O(l)
C) NaHSO4(aq) and H2O(l)
D) Na2SO3(aq) and H2O(l)
E) Na2SO4(aq) and H2O(l)
41. A sample of ozone gas occupies 225 mL at 1.00 atm and 0°C. If the volume of the gas is 625
mL at 25°C, what is the pressure?
A) 0.330 atm B) 0.360 atm C) 0.393 atm D) 2.54 atm
E) 3.03 atm
42. If 7.75 L of radon gas is at 1.55 atm and -19°C, what is the volume at STP?
A) 4.65 L
B) 5.37 L
C) 8.33 L
D) 11.2 L
E) 12.9 L
43. How many moles of helium occupy a volume of 5.00 L at 227.0°C and 5.00 atm?
A) 0.609 mol B) 1.64 mol
C) 5.00 mol
D) 25.0 mol
E) 6090 mol
44. What acid and base are neutralized to give lithium fluoride salt?
A) HCl(aq) and LiOH(aq)
B) HF(aq) and LiOH(aq)
C) HF(aq) and LiF(aq)
D) HOH(aq) and LiF(aq)
E) none of the above
45. In the following reaction, which reactant is a Brønsted-Lowry base?
Na2HPO4(aq) + H2CO3(aq) → NaH2PO4(aq) + NaHCO3(aq)
A) Na2HPO4 B) H2CO3
C) NaH2PO4 D) NaHCO3 E) none of the above
46. If a 25.0 mL sample of sulfuric acid is titrated with 50.0 mL of 0.200 M potassium hydroxide
to a phenolphthalein endpoint, what is the molarity of the acid?
H2SO4(aq) + 2 KOH(aq) → K2SO4(aq) + 2 H2O(l)
A) 0.100 M
B) 0.150 M
C) 0.200 M
D) 0.300 M
E) 0.400 M
47. If 1.500 g of vanadium metal react with oxygen gas to give 2.679 g of vanadium oxide, what
is the empirical formula of the product?
A) VO
B) V2O3
C) V2O5
D) V3O2
E) V5O2
48. Fructose is a sugar found in fruit and honey. Calculate the empirical formula for fructose
given its percent composition: 40.00% C, 6.72% H, and 53.29% O.
A) CHO
B) CH2O
C) CHO2
D) C3H6O3
E) C6HO8
49. What is the molecular formula for lactic acid if the percent composition is 40.00% C, 6.71%
H, 53.29% O, and the approximate molar mass is 90 g/mol?
A) CHO
B) CH2O
C) CHO2
D) C3H6O3
E) C6HO8
50. How many atoms of nickel equal a mass of 58.69 g?
A) 1
B) 27
C) 58.69
D) 59
E) 6.02 × 1023
51. How many methane molecules are in 0.500 mol of CH4 gas?
A) 1.20 × 1023 molecules
B) 1.20 × 1024 molecules
C) 3.01 × 1022 molecules
D) 3.01 × 1023 molecules
E) 3.01 × 1024 molecules
52. What is the mass of 4.50 × 1022 atoms of gold, Au?
A) 0.0679 g
B) 0.0748 g
C) 13.3 g
D) 14.7 g
E) 2640 g
53. What is the mass of 5.00 liters of oxygen gas, O2, at STP?
A) 0.286 g
B) 3.50 g
C) 6.40 g
D) 7.14 g
E) 112 g
54. How many ethane molecules are in 22.4 liters of C2H6 gas at STP?
A) 1.20 × 1024
B) 1.35 × 1025 C) 1.81 × 1024
D) 6.02 × 1023 E) 2.69 × 1022
55. How many bromine molecules, Br2, have a mass equal to 31.8 g?
A) 1.20 × 1023 molecules
B) 1.51 × 1024 molecules C) 1.91 × 1025 molecules
D) 2.40 × 1023 molecules
E) 3.03 × 1024 molecules
56. How many xenon atoms are in 10.0 L of Xe gas at STP?
A) 1.35 × 1024 atoms
B) 2.69 × 1021 atoms
C) 2.69 × 1023 atoms
22
24
D) 6.02 × 10 atoms
E) 6.02 × 10 atoms
57. What is the volume occupied by 11.0 g of propane gas, C3H8, at STP?
A) 0.250 L
B) 4.00 L
C) 5.59 L
D) 21.6 L
E) 89.6 L
58. How many moles of carbon monoxide react with 0.5 mol of oxygen gas according to the
balanced chemical equation?
2 CO(g) + O2(g)  2 CO2(g)
A) 1 mol
B) 2 mol
C) 3 mol
D) 4 mol
E) none of the above
59. What is the volume of carbon dioxide produced from 20 L of methane (CH4) at STP?
__CH4(g) + __O2(g)  __H2O(l) + __CO2(g)
A) 10 L
B) 20 L
C) 30 L
D) 40 L
E) 4 L
60. What is the volume of carbon monoxide gas reacts with 225 g of iron(III) oxide (159.70
g/mol) at STP?
2 Fe2O3(l) + 6 CO(g)  4 Fe(s) + 6 CO2(g)
A) 31.56 L
B) 189.34 L
C) 378.68
D) 126.22 L
E) 94.67 L
61. What is the mass of silver bromide (187.77 g/mol) precipitated from 2.96 g of iron(III)
bromide (295.55 g/mol)?
__FeBr3(s) + __AgNO3(aq) → __AgBr(s) + __Fe(NO3)3(aq)
A) 0.940 g
B) 0.627 g
C) 1.88 g
D) 5.64 g
E) 3.76 g
62. Considering the limiting reactant, what is the mass of zinc sulfide (97.46 g/mol) produced
from 0.750 g of zinc and 0.750 g of sulfur? Zn(s) + S(s)  ZnS(s)
A) 0.560 g
B) 1.12 g
C) 1.50 g
D) 2.24 g
E) 2.28 g