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Basic review questions for the CLEP chemistry

1. The correctly balanced equation for the reaction of gaseous octane with oxygen to give carbon dioxide and water vapor is

A. 2C8H18(g) + 25O2(g) ---> 16CO2(g) + 18H2O(l)

B. 2C8H18(g) + 25O2(g) ---> 16CO2(g) + 18H2O(g)

C. 2C8H18(g) + 50O(g) ---> 16CO2(g) + 18H2O(g)

D. C7H16(g) + 11O2(g) ---> 7CO2(g) + 8H2O(g)

2. Which process illustrates Boyle's law?

A. heating a filled balloon

B. squeezing a balloon

C. using a pressure cooker

D. blowing up a balloon

E. filling propane gas tank

3. Which highlighted element has the smallest atomic radius?

A. O

B.In

C.P

D. Ge

4. Which subshell is highlighted in the periodic table below?

A.5d

B.4p

C.5p

D.5s

5. The correct IUPAC name for CH3CH (CH3) CH (CH3) C (CH3)2CH3 is (Any branches (chains or atoms) are shown in parentheses after the carbon to which the branch is attached.)

A. 1, 1, 1, 2, 3-pentamethylbutane

B. 2, 3, 4, 4-tetramethylpentane

C. 2, 2, 3, 4-tetramethylnonane

D. 2, 3, 4-tetramethylpentane

E. 3-ethyl-4-isopropylhexane

6. For l = 2, what are the possible values of ml?

A. 2

B. 2, 1, 0, -1, -2

C. 1, 0, -1

D. 2, 1, 0

E. 1, 0

7. For n = 4, how many values of l are possible?

A.1

B.2

C.3

D.4

E.5

8. For the hydrogen atom, which is highest in energy - the 2s, the 3s, or 2p orbital?

A. 2s

B.3s

C.2p

D.2f

9. How many photons of frequency 1.50 x 1014 s-1 are needed to give 30.1 J of energy?

A. 9.94 x 1020 photons

B. 0.450 photons

C. 9.94 x 10-20 photons

D. 1.01 x 1019 photons

E. 3.03 x 1020 photons

10. Identify the specific element that corresponds to the electron configuration [Kr]5s24d105p4.

A. Te

B.Sn

C.In

D.Sb

11. Identify the specific element that corresponds to the electron configuration [Ar]4s23d104p4.

A. Br

B. Se

C. Ge

D.Cr

E. S

12. The distance between two atoms in a certain metal is 2.62 Å. What is the atomic radius of an atom?

A. 2.62Å

B. 1.31Å

C. 5.24Å

D. 1Å

13. What is the frequency of radiation that has a wavelength of 0.589 pm?

A. 5.09 s-1

B. 5.09 x 108 s-1

C. 5.09 x 1020 s-1

D.1 .96 x 10-21 s-1

E. 5.09 x 1022 s-1

14. What is the frequency of radiation that has a wavelength of 1.15 angstroms?

A. 2.90 x 101 s-1

B. 3.45 x 10-2 s-1

C. 2.61 x 1018 s-1

D.3 .83 x 10-19 s-1

E. 2.61 x 1016 s-1

15. What is the maximum number of electrons that can occupy the subshell 3d?

A.1

B.2

C.3

D.5

E.6

F.10

16. Which is an incorrect electron configuration for the given element?

A. 1s2 2s2 2p1 -- B

B. 1s2 2s2 2p4 -- N

C. [Ne] 3s2 3p5 -- Cl

D. [Ne] 3s2 3p3 – P

E. [Ne] 3s2 – Mg

17. Which Bohr orbit has the lowest energy?

A. n = 5

B. n = 4

C. n = 2

D. n = 3

E. n = 7

18. Which values of n, l, and ml are possible for a 4d orbital?

A. n = 4, l = 4, ml = 2

B. n = 4, l = 2, ml = 4

C. n = 3, l = 1, ml = 0

D. n = 4, l = 3, ml = 2

E. n = 4, l = 2, ml = 2

19. Write the electron configuration for the atom Zn, using the appropriate noble gas inner core for abbreviation.

A. [Ar]4s23d10

B. [Ar]4s24d10

C. [Ar]4s13d10

D. [Kr]4s24d10

E. [Kr]4s23d10

20. Which set is not an acceptable set of quantum numbers?

A. n = 7, l = 3, ml = +3

B. n = 1, l = 0, ml = 0

C. n = 2, l = 1, ml = +1

D. n = 3, l = 1, ml = -3

E. n = 2, 1 = 1, ml = -1

21. Which is a possible set of quantum numbers for a 4f electron?

A. 3, 4, 3, +1/2

B. 4, 3, -4, -1/2

C. 4, 2, 2, +1/2

D. 4, 3, 3, +1/2

E. 4, 2, 1, -1/2

22. The valence-shell electron configuration of the halogens is

A. ns1

B. ns2np3

C. ns2np5

D. ns2

E. ns2np6

23. The metal that is most likely to form several different positive ions is

A. Cs.

B. V.

C. Al.

D. Ca.

24. The elements below that are in order of decreasing atomic radius are

A. Mg, Na, P, and Si.

B. Si, P, AR, Na, and Mg.

C. Si, P, Na, and Mg.

D. Na, Mg, Si, and P.

25. In order for a covalent bond to form between 2 atoms,

A. the nucleus-nucleus repulsions must equal the electron-electron repulsions.

B. the nucleus-nucleus and electron-electron repulsions must equal the nucleus-electron attractions.

C. the nucleus-nucleus and electron-electron attractions must be greater than the nucleus-electron repulsions

D. the nucleus-electron attractions must be less than the nucleus-nucleus and electron-electron repulsions.

E. the nucleus-nucleus and electron-electron repulsions must be less than the nucleus-electron attractions.

26. The periodic trend of increasing electronegativity going from left to right across the periodic table is related to

A. more negative electron affinity and decreasing ionization energy.

B. increasing electron affinity but is unrelated to ionization energy.

C. less negative electron affinity and increasing ionization energy.

D. less negative electron affinity and decreasing ionization energy.

E.more negative electron affinity and increasing ionization energy.

27. Which molecule does not have the correct bond distribution given next to its formula?

A. NCCH2CH2CN; 7 single bonds and 2 triple bonds

B. CH2CHCHCH2; 7 single bonds and 2 double bonds

C. Cl2CO; 4 single bonds

D. H2NNH2; 5 single bonds

E. CH3CH3; 7 single bonds

31. Which statement is true regarding the excited-state electron configuration of the C atom [He]2s12px12py12pz1?

A. The extra electron in the 2p orbital was promoted from the 1s orbital.

B. If the 2s and 2p orbitals overlap with other orbitals, they will form nonequivalent bonds.

C. The formation of 4 covalent bonds using the 2s and 2p orbitals would result in a tetrahedral electron-charge cloud arrangement.

D. The bond angle that would result from the formation of covalent bonds by the 2p orbitals would be about 109 degrees.

E. The three 2p orbitals have different energies, since one of the orbitals is occupied by a promoted electron.

32. In the CO molecule the C atom has ____ hybridization and the O atom has ____ hybridization.

A. sp2, sp2

B. sp3, sp3

C. sp, sp

D. sp, sp2

E. sp3, sp2

33. In the molecule CH3CCH there are

A. 6 sigma bonds and 2 pi bonds.

B. 2 sigma bonds and 2 pi bonds.

C. 2 sigma bonds and 6 pi bonds.

D. 8 sigma bonds.

E. 6 sigma bonds.

37. True or false

A. Single bonds are stronger that all bonds

B. Single bonds are weaker than triple bonds which are also weaker than double bonds

C. Triple bonds are the strongest bonds and longest bonds

D. Triple bonds are the strongest bonds and shortest bonds

38. What is the electronegativity value of F?

A.1

B.2

C.3

D.4

39. A sigma (s) bond is a bond in which the shared electron density is concentrated directly along the internuclear axis between the two nuclei involved in bonding. T or F

40.What is the electronic structure of H?

A. 1s2

B.1s1

C.2s1

D.2s2

41. For l = 2, what are the possible values of ml?

A. 2

B. 2, 1, 0, -1, -2

C. 1, 0, -1

D. 2, 1, 0

E. 1, 0

42. For n = 4, how many values of l are possible?

A.1

B.2

C.3

D.4

E.5

43. For the hydrogen atom, which is highest in energy--the 2s, the 3s, or 2p orbital?

A. 2s

B.3s

C.2p

D.2f

44. How many photons of frequency 1.50 x 1014 s-1 are needed to give 30.1 J of energy?

A. 9.94 x 1020 photons

B. 0.450 photons

C. 9.94 x 10-20 photons

D. 1.01 x 1019 photons

E. 3.03 x 1020 photons

45. Identify the specific element that corresponds to the electron configuration [Kr]5s24d105p4.

A. Te

B.Sn

C.In

D.Sb

46. Identify the specific element that corresponds to the electron configuration [Ar]4s23d104p4.

A. Br

B. Se

C. Ge

D.Cr

E. S

47. The distance between two atoms in a certain metal is 4.62 Å. What is the atomic radius of an atom?

A. 4.62Å

B. 2.31Å

C. 5.24Å

D. 1Å

48. What is the frequency of radiation that has a wavelength of 0.589 pm?

A. 5.09 s-1

B. 5.09 x 108 s-1

C. 5.09 x 1020 s-1

D.1 .96 x 10-21 s-1

E. 5.09 x 1022 s-1

49. What is the frequency of radiation that has a wavelength of 1.15 angstroms?

A. 2.90 x 101 s-1

B. 3.45 x 10-2 s-1

C. 2.61 x 1018 s-1

D.3 .83 x 10-19 s-1

E. 2.61 x 1016 s-1

50. What is the maximum number of electrons that can occupy the subshell 3d?

A.1

B.2

C.3

D.5

E.6

F.10

51. Which is an incorrect electron configuration for the given element?

A. 1s2 2s2 2p1 -- B

B. 1s2 2s2 2p4 -- N

C. [Ne] 3s2 3p5 -- Cl

D. [Ne] 3s2 3p3 – P

E. [Ne] 3s2 -- Mg

52. Which values of n, l, and ml are possible for a 4d orbital?

A. n = 4, l = 4, ml = 2

B. n = 4, l = 2, ml = 4

C. n = 3, l = 1, ml = 0

D. n = 4, l = 3, ml = 2

E. n = 4, l = 2, ml = 2

53. Write the electron configuration for the atom Zn, using the appropriate noble gas inner core for abbreviation.

A. [Ar]4s23d10

B. [Ar]4s24d10

C. [Ar]4s13d10

D. [Kr]4s24d10

E. [Kr]4s23d10

54. Which set is not an acceptable set of quantum numbers?

A. n = 7, l = 3, ml = +3

B. n = 1, l = 0, ml = 0

C. n = 2, l = 1, ml = +1

D. n = 3, l = 1, ml = -3

E. n = 2, 1 = 1, ml = -1

55. Which is a possible set of quantum numbers for a 4f electron?

A. 3, 4, 3, +1/2

B. 4, 3, -4, -1/2

C. 4, 2, 2, +1/2

D. 4, 3, 3, +1/2

E. 4, 2, 1, -1/2

56. The valence-shell electron configuration of the halogens is

A. ns1.

B. ns2np3.

C. ns2np5.

D. ns2.

E. ns2np6.

57. The metal that is most likely to form several different positive ions is

A. Cs.

B. V.

C. Al.

D. Ca.

58. The elements below that are in order of decreasing atomic radius are

A. Mg, Na, P, and Si.

B. Si, P, AR, Na, and Mg.

C. Si, P, Na, and Mg.

D. Na, Mg, Si, and P.

59. The periodic trend of increasing electronegativity going from left to right across the periodic table is related to

A. more negative electron affinity and decreasing ionization energy.

B. increasing electron affinity but is unrelated to ionization energy.

C. less negative electron affinity and increasing ionization energy.

D. less negative electron affinity and decreasing ionization energy.

E.more negative electron affinity and increasing ionization energy.

60. Hydrogen is the least electronegative element. True or false

A. True

B. False

61. Which molecule does not have the correct bond distribution given next to its formula?

A. NCCH2CH2CN; 7 single bonds and 2 triple bonds

B. CH2CHCHCH2; 7 single bonds and 2 double bonds

C. Cl2CO; 4 single bonds

D. H2NNH2; 5 single bonds

E. CH3CH3; 7 single bonds

62. The formal charge of an atom in a molecule

A. is positive if the atom has more electrons in the molecule than in the free atom.

B. is equal to the number of valence electrons in the free atom minus the sum of the bonding and nonbonding electrons.

C. is the actual charge of an atom.

D. is always equal to zero in a neutral molecule.

E. is equal to the number of valence electrons in the free atom minus the number of valence electrons assigned to the bound atom.

64. Which statement is true regarding the excited-state electron configuration of the C atom [He]2s12px12py12pz1?

A. The extra electron in the 2p orbital was promoted from the 1s orbital.

B. If the 2s and 2p orbitals overlap with other orbitals, they will form nonequivalent bonds.

C. The formation of 4 covalent bonds using the 2s and 2p orbitals would result in a tetrahedral electron-charge cloud arrangement.

D. The bond angle that would result from the formation of covalent bonds by the 2p orbitals would be about 109 degrees.

E. The three 2p orbitals have different energies, since one of the orbitals is occupied by a promoted electron.

65. In the CO molecule the C atom has ____ hybridization and the O atom has ____ hybridization.

A. sp2, sp2

B. sp3, sp3

C. sp, sp

D. sp, sp2

E. sp3, sp2

66. In the molecule CH3CCH there are

A. 6 sigma bonds and 2 pi bonds.

B. 2 sigma bonds and 2 pi bonds.

C. 2 sigma bonds and 6 pi bonds.

D. 8 sigma bonds.

E. 6 sigma bonds.

67. What is the electronegativity value of F?

A.1

B.2

C.3

D.4

68. A sigma (s) bond is a bond in which the shared electron density is concentrated directly along the internuclear axis between the two nuclei involved in bonding. T or F

69.Which of the following represents the range of values possible for the Azimuthal quantum number for an electron with principal quantum number n?

A. 0 to n-1

B. 0 to n

C. –n to n

D. – (n-1) to (n-1)

70. Which of the following is NOT true in general as we move from sodium to chlorine in the periodic table?

A. Electronegativity increases

B. Atomic radius increases

C. Ionization energy increases

D. electron affinity increases

71. Ten electrons have just been placed into 4d orbital. The next electron will be placed in a:

A. 4f orbital

B. 4p orbital

C.5p orbital

D. 5f orbital

72. All of the following are state functions EXCEPT:

A. Volume

B. Entropy

C. Work

D. Enthalpy

73. What is the characteristic valence-electron configuration of the chalcalogen group?

A. ns2

B. ns2np1

C.ns2np4

D.ns1np3

74) What are the quantum numbers associated with the last electron of nitrogen atom?

A) n=2, l=1, ml=+1, ms=+1/2

B) n=2, l=1, ml=+1, ms=-1/2

C) n=2, l=1, ml=-1, ms=+1/2

D) n=2, l=1, ml=-1, ms=-1/2

75) How many electrons can be accommodated in the n=4 quantum level?

A. 4

B. 16

C. 18

D. 32

76) Which ion is the largest?

A. Cl-

B. Na+

C.K+

D. Br-

77. The heat capacity of a certain metal is 0.20 Cal/g.k.How much heat is absorbed when 12g of this metal increases from 25.3C to 45.3C

A.1200 calories

B 480 calories

C. 96calories

D.48 calories

Match the following to

A. no change in temperature

B. no change in volume

C. no change in pressure

D. no change in heat

78. What is an adiabatic process?

A.

B

C.

D.

79. What is an isobaric process?

A.

B.

C.

D.

What is an isochoric process?

A.

B

C.

D.

79. Which of the following is the electronic configuration for an excited state of Na+

A. 1s22s22p53s2

B 1s22s22p63s1

C. 1s22s22p6

D. 1s22s22p53s1

80. Identify the Bronsted acid in the following reaction

H2S04 (aq) + 2NH3 (aq) à (NH4)2S04(aq)

A. H2S04 (aq)

B. 2NH3 (aq)

C. (NH4)2S04(aq)

D. This equation does not contain a Bronsted acid

I will post the answers to the next log. You can also comment re question # and I can provide the answer as well.