Master CHEM 1311 Test Bank

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1. Which of the following metric relationships is incorrect? (1A)
a) 1 liter = 1000 milliliters
b) 1 kilogram = 103 grams
c) 1 microgram = 106 grams
d) 1 centimeter = 10-2 meters
e) 1 nanometer = 10-9 meters

c) 1 microgram = 106 grams

2. What is the elemental symbol for the isotope
18
40X? (1A)
a) Ti
b) Ar
c) Mg
d) Zr
e) Kr

b) Ar

3. An atom of the isotope sulfur-31 consists of how many protons, neutrons, and electrons?
(p = proton, n = neutron, e = electron) (1A)

a) 15 p, 16 n, 15 e
b) 32 p, 31 n, 32 e
c) 16 p, 15 n, 16 e
d) 16 p, 16 n, 15 e
e) 16 p, 31 n, 16 e

c) 16 p, 15 n, 16 e

4. How many electrons in an atom can have the quantum numbers n = 4, l = 2? (1A)
a) 2
b) 5
c) 10
d) 18
e) 6

c) 10

5. Which of the following combinations of quantum numbers would not be possible for an electron in
an atom? (1A)
n l ml ms
a) 1 0 0 +1/2
b) 3 2 -1 -1/2
c) 2 0 1 +1/2
d) 2 1 1 -1/2
e) 3 1 -1 +1/2

c) 2 0 1 +1/2

6. Which of the following diagrams represents the shape of a "p" orbital?

Draw it (1A)

X O ∞ +

7. Lithium forms compounds which are used in dry cells and storage batteries and in high-temperature
lubricants. It has two naturally occurring isotopes, 6Li (isotopic mass = 6.015121 amu) and 7Li
(isotopic mass = 7.016003 amu).

Lithium has an atomic mass of 6.9409 amu. What is the percent abundance of lithium-6?
(1A)
a) 92.50%
b) 86.66%
c) 46.16%
d) 7.503%
e) 6.080%

d) 7.503%

8. Which of the following atoms has the lowest first ionization energy? (1A)
a) Li b) Na c) F d) O e) C

b) Na

9. Which of the following atoms has the largest atomic radius? (1A)
a) Be b) Sr c) Sn d) Ne e) Xe

b) Sr

10. What is the electron configuration of Fe2+? (1A)
a) [Ar]3d44s2
b) [Ar]3d54s1
c) [Ar]3d6
d) [Ar]3d64s2
e) [Ar]3d64s1

c) [Ar]3d6

11. The radii of the species, Te, Te+, and Te- decrease in the following order: (1A)
a) Te+ > Te > Te-
b) Te+ > Te- > Te
c) Te > Te- > Te+
d) Te > Te+ > Te-
e) Te- > Te > Te+

e) Te- > Te > Te+

15. Atoms X, Y, Z, and R have the following nuclear compositions:
Which two are isotopes? (1A)
a) X & Y
b) X & R
c) Y & R
d) Z & R
e) X & Z

e) X & Z

16. The alkali metal elements are found in _______ of the periodic table. (1A)
a) Group 1A
b) Group 2A
c) Group 3A
d) Period 7
e) Period 1

a) Group 1A

17. Which of these elements is chemically similar to oxygen? (1A)
a) sulfur
b) calcium
c) iron
d) nickel
e) potassium

a) sulfur

18. How many atoms are in 31.3 g of nickel, Ni? (1A)
a) 1.13 × 1024 atoms
b) 1.48 × 1025 atoms
c) 2.44 × 1022 atoms
d) 3.21 × 1023 atoms
e) 6.98 × 1021 atoms

d) 3.21 × 1023 atoms

19. What is defined as the number of waves that pass through a particular point in one second?
a) light
b) amplitude
c) magnitude
d) wavelength
e) frequency

e) frequency

20. What is the frequency of light having a wavelength of 360 nm? (1A)
a) 8.3 × 1014 s-1
b) 108 s-1
c) 1.2 × 10-6 s-1
d) 1.2 × 10-15 s-1
e) 8.3 × 105 s-1

a) 8.3 × 1014 s-1

21. Infrared radiation from the sun has a wavelength of 6200 nm. Calculate the energy of one photon
of that radiation. (1A)
a) 4.l × 10-39 J b) 3.2 × 10-26 J c) 4.l × 10-30 J
d) 3.2 × 10-20 J e) 3.2 × 10-29 J

d) 3.2 × 10-20 J

22. Consider the Bohr model of the hydrogen atom. When an electron moves from the n = 1 orbit to
the n 1 orbit to the n = 6 orbit, which of the following statements is true? (1A)

a) light is emitted
b) energy is absorbed
c) the electron can have a continuous range of energies in between those of the n=1 and 6 orbits
d) all of the above
e) none of the above

b) energy is absorbed

12. A sample of iron weighing 6.09 g contains how many moles of iron atoms? (1A)
a) 0.0480 moles
b) 0.0558 moles
c) 0.109 moles
d) 0.917 moles
e) 9.17 moles

c) 0.109 moles

13. Of the following atoms, which contain(s) ten 3d electrons in the ground state (1A)
a) Zn b) Cu c) Cd d) a and b are correct
e) a and c are correct

ANSWER: COUNTED ALL CORRECT

14. Who is credited with discovering the atomic nucleus? (1A)
a) Dalton and his atomic theory
b) Millikan and the oil drop experiment
c) Thomson and cathode ray tubes
d) Chadwick using beryllium sheets
e) Rutherford and the gold foil experiment

e) Rutherford and the gold foil experiment

1. Which ground-state atom has an electron configuration described by the following orbital diagram? (1B)
[Ar] ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑ ↑ ↑
4s 3d 4p
a) phosphorus
b) germanium
c) selenium
d) tellurium
e) arsenic

e) arsenic

2. The electron configuration of a ground-state Co atom is (1B)
a) [Ar]4s24d7
b) [Ar]4s13d5
c) 1s22s22p63s23d9
d) [Ar]4s23d7
e) [Ne]3s23d7

d) [Ar]4s23d7

3. Lithium forms compounds which are used in dry cells and storage batteries and in high-temperature
lubricants. It has two naturally occurring isotopes, 6Li (isotopic mass 6.015121 amu) and 7Li
(isotopic mass = 7.016003 amu). Lithium has an atomic mass of 6.9409 amu. What is the percent
abundance of lithium-7? (1B)
a) 92.50%
b) 86.66%
c) 46.16%
d) 7.503%
e) 6.080%

a) 92.50%

4. Which of the following atoms has the highest first ionization energy? (1B)
a) Li b) Na c) F d) O e) C

c) F

5. Consider the Bohr model of the hydrogen atom. When an electron moves from the n = 1 orbit to the
n = 6 orbit, which of the following statements is true?
(1B)
a) energy is absorbed
b) light is emitted
c) the electron can have a continuous range of energies in between those of the n=1 and 6 orbits
d) all of the above
e) none of the above

a) energy is absorbed

6. Line spectra from all regions of the electromagnetic spectrum, including the Paschen series of infrared lines for hydrogen, are used by astronomers to identify elements present in the
atmospheres of stars.

Calculate the wavelength of the photon emitted when the hydrogen atom undergoes a transition from n = 5 to n = 2 . (1B)

a) 205.1 nm
b) 434.2 nm
c) 683.8 nm
d) 1282 nm
e) 1500 nm

b) 434.2 nm

7. Which of the following atoms has the largest atomic radius? (1B)
a) Be
b) Sn
c) Sr
d) Ne
e) Xe

c) Sr

8. What is the electron configuration of Mn2+? (1B)
a) [Ar]3d5
b) [Ar]3d44s1
c) [Ar] 3d34s2
d) [Ar]3d54s2
e) [Ar]3d64s2

a) [Ar]3d5

9. Of the following atoms, which contain(s) five 3d electrons in the ground state (1B)
a) Cr
b) Tc
c) Mn
d) a and b are correct
e) a and c are correct

ALL ANSWERS COUNTED CORRECT

10. Which of the following combinations of quantum numbers would not be possible for an electron in
an atom? (1B)
n l ml ms
a) 1 0 1 -1/2
b) 3 2 -1 -1/2
c) 2 0 0 +1/2
d) 2 1 1 -1/2
e) 3 1 -1 +1/2

a) 1 0 1 -1/2

11. Which of the following diagrams represents the shape of a "p" orbital? (1B)
X O ∞ + or two answers are correct

12. Who is credited with discovering the atomic nucleus? (1B)
a) Dalton and his atomic theory
b) Millikan and the oil drop experiment
c) Thomson and cathode ray tubes
d) Chadwick using beryllium sheets
e) Rutherford and the gold foil experiment

e) Rutherford and the gold foil experiment

13. Atoms X, Y, Z, and R have the following nuclear compositions: Which two are isotopes? (1B)
a) X & Y
b) X & Z
c) Y & R
d) Z & R
e) X & R

b) X & Z

14. How many atoms are in 2.38 g of nickel, Ni? (1B)
a) 1.13 × 1024 atoms
b) 1.48 × 1025 atoms
c) 2.44 × 1022 atoms
d) 3.21 × 1023 atoms
e) 6.98 × 1021 atoms

c) 2.44 × 1022 atoms

15. What is defined as the number of waves that pass through a particular point in one second? (1B)
a) light
b) frequency
c) magnitude
d) wavelength
e) amplitude

b) frequency

16. The radii of the species, I, I+, and I- decrease in the following order: (1B)
a) I > I+ > I-
b) I+ > I > I-
c) I > I- > I+
d) I+ > I- > I
e) I- > I > I+

e) I- > I > I+

17. A sample of iron weighing 2.68 g contains how many moles of iron atoms? (1B)
a) 0.0480 moles
b) 0.0558 moles
c) 0.109 moles
d) 0.917 moles
e) 9.17 moles

a) 0.0480 moles

18. What is the frequency of light having a wavelength of 250 nm? (1B)
a) 8.3 × 10^14 s-1
b) 108 s-1
c) 1.2 × 10^-6 s-1
d) 1.2 × 10^15 s-1
e) 8.3 × 10^5 s-1

d) 1.2 × 10^15 s-1

19. Infrared radiation from the sun has a wavelength of 6200 nm. Calculate the energy of one photon
of that radiation. (1B)
a) 4.l × 10-30 J
b) 3.2 × 10-29 J
c) 4.l × 10-39 J
d) 3.2 × 10-20 J
e) 3.2 × 10-26 J

d) 3.2 × 10-20 J

20. The size of an atomic orbital is associated with (1B)
a) the principal quantum number (n).
b) the angular momentum quantum number (l).
c) the magnetic quantum number (ml).
d) the spin quantum number (ms).
e) the angular momentum and magnetic quantum numbers, together.

a) the principal quantum number (n)

21. Which of the following is a correct set of quantum numbers for an electron in a 4f orbital? (1B)
a) n = 5, l = 3, ml = +1
b) n = 4, l = 2, ml = +1
c) n = 5, l = 2, ml = +3
d) n = 5, l = 4, ml = 3
e) n = 4, l = 3, ml = 0

e) n = 4, l = 3, ml = 0

22. How many electrons in an atom can have the quantum numbers n = 4, l = 1?(1B)
a) 2
b) 5
c) 10
d) 18
e) 6

e) 6

23. How many valence electrons does a tellurium (Te) atom have? (1B)
a) 2
b) 4
c) 6
d) 36
e) 52

c) 6

24. Which one of these ions has the smallest radius? (1B)
a) Cl-
b) K+
c) S2-
d) Na+
e) O2-

d) Na+

26. A possible set of quantum numbers for the last electron added (based on the build-up or aufbau principle) to complete an atom of aluminum Al in its ground state is (1B)
n l ml ms
A 4 0 0 -1/2
B 3 0 0 -1/2
C 4 1 0 +1/2
D 3 1 1 +1/2
E 4 2 1 +1/2
a) A b) B c) C d) D e) E

d) D

27. What is the electron configuration for selenium? (1B)
a) 1s22s22p63s23p64d104s14p5
b) 1s22s22p63s23p63d104s24p3
c) 1s22s22p63s23p64d104s24p4
d) 1s22s22p63s23p63d104s24p4
e) 1s22s22p63s23p63d104s14p5

d) 1s22s22p63s23p63d104s24p4

28. Consider the element with the electron configuration [Kr] 5s24d105p6. This element is (1B)
a) a halogen
b) an actinide element
c) a transition metal
d) a noble gas
e) an alkali metal

d) a noble gas

29. Which of the following metric relationships is incorrect? (1B)
a) 1 liter = 1000 milliliters
b) 1 kilogram = 103 grams
c) 1 microgram = 10-6 grams
d) 1 centimeter = 10-2 meters
e) 1 nanometer = 109 meters

e) 1 nanometer = 109 meters

30. What is the elemental symbol for the isotope (1B)
15
31X?
a) Ga
b) Ar
c) Zr
d) P
e) Kr

d) P

31. Give the number of protons (p), electrons (e), and neutrons (n) in one atom of chlorine-37. (1B)
a) 37 p, 37 e, 17 n
b) 37 p, 17 e, 20 n
c) 17 p, 17 e, 37 n
d) 17 p, 37 e, 17 n
e) 17 p, 17 e, 20 n

e) 17 p, 17 e, 20 n

32. The alkali metal elements are found in _______ of the periodic table. (1B)
a) Group 3A b) Group 2A c) Group 1A d) Period 7 e) Period 1

c) Group 1A

33. Which of these elements is chemically similar to nitrogen? (1B)
a) sulfur
b) calcium
c) phosphorus
d) nickel
e) sodium

c) phosphorus

34. The orbital diagram for a ground-state nitrogen atom is (1B)

1s 2s 2p
a) ↑↓ ↑↓ ↑ ↑ ↑
b) ↑↓ ↑↓ ↑↓ ↑
c) ↑↓ ↑ ↑ ↑ ↑
d) ↑↓ ↑↓ ↑↓ ↑ ↑
e) ↑↓ ↑↓ ↑↓ ↑↓ ↑

a) a b) b c) c d) d e) e

a) a

1. Which of the following statements is TRUE concerning d orbitals? (1A10)
A. Each one is spherical in shape.
B. All of the other answers are false.
C. They all have two lobes and are "dumbbell" shaped.
D. There are three of them for a given n value.
E. A 3d orbital is smaller than a 5d orbital

E. A 3d orbital is smaller than a 5d orbital

2. Identify the element of Period 2 which has the following successive ionization energies, in kJ/mol. (1A10)
A. None of these choices is correct.
B. Ne
C. O
D. B
E. Li

C. O

3. Which of these elements has the greatest electron affinity? (1A10)
A. S
B. Mg
C. P
D. Si
E. Al

A. S

4. The electron configuration of a cobalt(III) ion is (1A10)
A. [Ar]3d5.
B. [Ar]4s13d5.
C. [Ar]4s23d9.
D. [Ar]3d6.
E. [Ar]4s23d4.

D. [Ar]3d6.

5. In what group of the periodic table is the element with the electron configuration
[Ar]4s23d104p3? (1A10)
A. 3A
B. 1A
C. 5A
D. 2A
E. 4A

C. 5A

6. Calculate the wavelength of a neutron that has a velocity of 2.00 m s-1. (The mass of a neutron = 1.675 × 10^- 27 kg). (1A10)
A. 198 nm
B. 5.05 mm
C. 216 nm
D. 1.98 × 10^-9 m
E. 1.8 × 10^50 m

A. 198 nm

7. Consider the element with the electron configuration [Rn]7s25f7. This element is (1A10)
A. a representative element.
B. a noble gas.
C. a nonmetal.
D. a lanthanide element.
E. an actinide element .

E. an actinide element .

8. Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n= 4 to the n = 1 principal energy level. (1A10)
A. 8.22 × 10^14 s-1
B. 1.03 × 10^8 s-1
C. 1.35 × 10^-51 s-1
D. 3.08 × 10^15 s-1
E. 2.06 × 10^14 s-1

D. 3.08 × 1015 s-1

9. Select the correct set of quantum numbers (n, l, ml, ms) for the first electron removed from tin, Sn. (1A10)
A. 5, 1, 0, ½
B. 5, 2, 1, ½
C. 5, 2, -1, ½
D. 5, 2, 0, ½
E. 5, 1, 2, ½

A. 5, 1, 0, ½

10. When J. J. Thomson discovered the electron, what physical property of the electron did he measure? (1A10)
A. its temperature, T
B. its charge-to-mass ratio, e/m
C. its charge, e
D. its mass, m
E. its atomic number, Z

B. its charge-to-mass ratio, e/m

11. Which of the following is a correct set of quantum numbers for an electron in a 3p orbital? (1A10)
A. n = 3, l = 3, ml = +2
B. n = 3, l = 2, ml = -2
C. n = 3, l = 1, ml = +3
D. n = 3, l = 1, ml = -1
E. n = 3, l = 2, ml = 3

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

12. An atom of the isotope sulfur-31 consists of how many protons, neutrons, and electrons? (p = proton, n =neutron, e = electron) (1A10)
A. 16 p, 31 n, 16 e
B. 16 p, 15 n, 16 e
C. 16 p, 16 n, 15 e
D. 15 p, 16 n, 15 e
E. 32 p, 31 n, 32 e

B. 16 p, 15 n, 16 e

13. What is defined as the vertical distance from the midline of a wave to the top of the peak or the bottom ofthe trough? (1A10)
A. magnitude
B. frequency
C. wavelength
D. light
E. amplitude

E. amplitude

14. Which of the following elements has the largest atomic size? (1A10)
A. Ba
B. S
C. Ca
D. Po
E. Rn

A. Ba

15. Which of these elements exhibits chemical behavior similar to that of calcium? (1A10)
A. chlorine
B. sulfur
C. magnesium
D. iron
E. sodium

C. magnesium

16. Consider the emission spectrum for a hydrogen atom and determine which of the following statements is
FALSE? (1A10)
A. Light is emitted in the visible, infrared and ultraviolet regions of the electromagnetic radiation spectrum
B. The dark regions in the spectrum correspond to allowed electron transitions
C. Atoms emit light
D. Emission lines correspond to electron transitions from distances farther from the nucleus to those closer to
the nucleus
E. An atom is quantized (i.e. has only certain energies available to it)

B. The dark regions in the spectrum correspond to allowed electron transitions

17. Which of the following elements has the largest first ionization energy? (1A10)
A. Te
B. Ca
C. Na
D. Cl
E. Br

D. Cl

18. Select the diamagnetic ion. (1A10)
A. Sc3+
B. Cr3+
C. Cr2+
D. Cu2+
E. Ni2+

A. Sc3+

19. Which element has the following ground-state electron configuration? (1A10)
[Kr]5s24d105p2
A. Ge
B. Te
C. Sn
D. Sb
E. Pb

C. Sn

20. Which two electron configurations represent elements that would have similar chemical properties? (1A10)
(1) 1s22s22p4
(2) 1s22s22p5
(3) [Ar]4s23d104p3
(4) [Ar]4s23d104p4
A. (2) and (4)
B. (1) and (2)
C. (2) and (3)
D. (1) and (4)
E. (1) and (3)

D. (1) and (4)

21. The orbital diagram for a ground-state nitrogen atom is (1A10)
1s 2s 2p
a) ↑↓ ↑↓ ↑ ↑ ↑
b) ↑↓ ↑↓ ↑↓ ↑
c) ↑↓ ↑ ↑ ↑ ↑
d) ↑↓ ↑↓ ↑↓ ↑ ↑
e) ↑↓ ↑↓ ↑↓ ↑↓ ↑
A. a
B. b
C. c
D. d
E. e

A. a

22. For which of these reactions is the energy change equal to the third ionization energy of vanadium? (1A10)
A. V(g) → V3+(g) + 3e-
B. V2-(g) + e- → V3-(g)
C. V3+(g) → V4+(g) + e-
D. V2+(g) → V3+(g) + e-
E. V3+(g) + e- → V2+(g)

D. V2+(g) → V3+(g) + e-

23. Atoms X, Y, Z, and R have the following nuclear compositions:
Which two are isotopes? (1A10)

192 192 194 193
78 X 77 Y 77 Z 75 R
A. Y & Z
B. Z & R
C. X & R
D. Y & R
E. X & Y

A. Y & Z

24. How many valence electrons are there in an atom of arsenic (As)? (1A10)
A. 3
B. 5
C. 2
D. 15
E. 10

B. 5

25. An aluminum ion, Al3+, has: (1A10)
A. 16 protons and 13 electrons
B. 13 protons and 13 electrons
C. 10 protons and 13 electrons
D. 13 protons and 10 electrons
E. 27 protons and 24 electrons

D. 13 protons and 10 electrons

26. Infrared radiation from the sun has a wavelength of 6200 nm. Calculate the energy of one photon of that radiation. (1A10)
A. 3.21 x 10^-20 J
B. 4.10 × 10^-30 J
C. 3.21 × 10^-29 J
D. 4.10 × 10^-39 J
E. 3.21 × 10^-26 J

A. 3.21 x 10-20 J

27. How many unpaired electrons does a ground-state atom of cobalt (Co) have? (1A10)
A. 1
B. 4
C. 3
D. 2
E. 0

C. 3

28. Which of these elements has the greatest metallic character? (1A10)
A. Br
B. Si
C. As
D. Ni
E. Se

D. Ni

29. Which of these choices is the general electron configuration for the outermost electrons of elements in the alkaline earth group? (1A10)
A. ns2
B. ns2np5
C. ns2np6(n -1)d6
D. ns2np4
E. ns1

A. ns2

30. What is the maximum number of electrons in an atom that can have the following set of quantum numbers? (1A10)
n = 4 l = 3 ms = +1/2
A. 14
B. 7
C. 1
D. 0
E. 2

B. 7

31. Which one of the following groups does not contain any metals? (1A10)
A. Cu, P, Se, Kr
B. Cl, Al, Si, Ar
C. N, Ne, Nd, Np
D. C, S, As, H
E. Xe, Hg, Ge, O

D. C, S, As, H

32. The shape of an atomic orbital is associated with (1A10)
A. the magnetic quantum number (ml).
B. the spin quantum number (ms).
C. the principal quantum number (n).
D. the magnetic and spin quantum numbers, together.
E. the angular momentum quantum number (l).

E. the angular momentum quantum number (l)

33. What element is represented by the electron configuration 1s22s22p63s23p64s13d5? (1A10)
A. V
B. K
C. Mn
D. Cr
E. Ca

D. Cr

34. Considering the fact that the visible region of the electromagnetic spectrum spans from 290 nm to 850 nm, what is true concerning the transition of an electron from the n = 1 orbit to the n = 6 orbit. (1A10)
A. light is absorbed that cannot be seen by the human eye
B. visible light is absorbed
C. light is emitted that cannot be seen by the human eye
D. visible light is emitted

A. light is absorbed that cannot be seen by the human eye

35. Select the correct electron configuration for indium (In) (Z = 49). (1A10)
A. [Kr]5s24d105p1
B. [Kr]5s24f105p1
C. [Kr]5s24d104p1
D. [Kr]5s25d105p1
E. [Kr]5s25p64d8

A. [Kr]5s24d105p1

36. What is the wavelength of light having a frequency of 4.80 x 1014 s-1? (1A10)
A. 1.60 x 10-3 nm
B. 6.30 x 10-7 nm
C. 1.60 x 103 nm
D. 1.60 x 103 m
E. 6.30 x 102 nm

E. 6.30 x 102 nm

37. A possible set of quantum numbers for the last electron added to complete an atom of nickel in its ground state is (1A10)
n l ml ms
a 4 2 0 +1/2
b 3 0 +1 -1/2
c 4 1 -1 +1/2
d 3 2 +1 -1/2
e 4 2 +2 -1/2
A. a
B. b
C. c
D. d
E. e

D. d

What is the mass number of an iron atom that has 29 NEUTRONS? (PQ1)

55

How many sig figs

60104

5

sig figs

5.6792 + 0.6 + 4.33

10.6

Can you do percent abundance

yes

I think it's time to take a 5 minute break

good job, keep going

Which of the following is always the same for atoms of the same element

Mass Number
Atomic Number
Mass of an atom
Neutron number

Atomic Number

Iodine-124 has how many protons and neutrons?

53 protons
71 neutrons

silver and nickel samples have the same mass

who contains more atoms?

nickel

in waves, energy and frequency and wavelength are related how?

E increases, frequency increases, wavelength decreases

What are the energy, wavelength, and frequency equations

E(energy) = hv
c= frequency x wavelength

Can you name the electromagnetic spectrum?

low e/low v/long wavelength
radio
microwave
infrared
visible
ultraviolet
x-ray
gamma rat
high e/high v/short wavelength

lower energy -> high energy orbit
electrons (absorb/emit) energy?

absorb energy

what is the wavelength of a photon emitted by a hydrogen atom when the electron drops from n=4 to n=1

97.2 m

which results in emission of the higher-energy photon?

n = 4 to n = 3
n = 3 to n=2

n = 3 to n=2

How many upaired e- does Mn have?

5

1. Predict the ideal bond angles in GeCl4 (2A10)
A. 120°
B. 90°
C. < 90°
D. 109.5°
E. 180°

D. 109.5°

2. The formula for magnesium sulfite is: (2A10)
A. MgSO3
B. MnS
C. MgS
D. MgSO4
E. MnSO3

A. MgSO3

3. Valence bond theory predicts that iodine will use _____ hybrid orbitals in ICl2- (2A10)
A. sp3d2
B. None of these choices is correct.
C. sp3d
D. sp2
E. sp3

C. sp3d

4. What is the molecular geometry (shape) of NOCl ? (2A10)
A. trigonal planar
B. trigonal pyramidal
C. linear
D. tetrahedral
E. bent

E. bent

5. In which of these pairs of atoms would the bond be the most polar? (2A10)
A. C-C
B. N-C
C. C-Cl
D. C-H
E. O-C

E. O-C

6. Which of these atoms is the most electronegative? (2A10)
A. As
B. Cs
C. Li
D. Ge
E. P

E. P

7. Which of the following molecules has a net dipole moment (i.e. is polar)? (2A10)
A. KrF2
B. CCl4
C. CO2
D. BeCl2
E. SF2

E. SF2

8. Predict the actual bond angles in SF3+ . (2A10)
A. exactly 120°
B. between 109.5° and 120°
C. less than 90°
D. between 90° and 109.5°
E. more than 120°

D. between 90° and 109.5°

9. Predict the electron domain geometry around the central atom in BCl3 (2A10)
A. trigonal bipyramidal
B. trigonal planar
C. trigonal pyramidal
D. octahedral
E. tetrahedral

B. trigonal planar

10. Complete this sentence: The PCl5 molecule has (2A10)
A. nonpolar bonds, and is a nonpolar molecule.
B. nonpolar bonds, but is a polar molecule.
C. polar bonds, but is a nonpolar molecule.
D. polar bonds, and is a polar molecule.

C. polar bonds, but is a nonpolar molecule.

11. The number of resonance structures for the best Lewis structure of sulfur dioxide is: (2A10)
A. 4
B. there is only one structure (i.e. no resonance)
C. 3
D. 2

B. there is only one structure (i.e. no resonance)

12. Which response includes all the molecules below that do not follow the octet rule for the central atom? (2A10)
(1) H2S (2) BCl3 (3) PH3 (4) SF4
A. PH3 and SF4
B. BCl3 and PH3
C. BCl3 and SF4
D. All four Lewis structures obey the octet rule for the central atom
E. H2S and BCl3

C. BCl3 and SF4

13. Which is the correct formula for copper(II) phosphate? (2A10)
A. Cu(PO3)2
B. Cu(PO4)2
C. Cu2PO3
D. Cu3(PO4)2
E. Cu2PO4

D. Cu3(PO4)2

14. Predict the electron domain geometry around iodine, the central atom in the ion ICl2¯ : (2A10)
A. trigonal bipyramidal
B. octahedral
C. bent
D. tetrahedral
E. trigonal planar

A. trigonal bipyramidal

15. Indicate the type of hybrid orbitals used by the central atom in SF6. (2A10)
A. sp3d2
B. sp2
C. sp3
D. sp3d
E. sp

A. sp3d2

16. What is the name of PCl3? (2A10)
A. trichlorophosphide
B. phosphorus trichlorate
C. phosphorus trichloride
D. phosphorus chloride
E. phosphoric chloride

C. phosphorus trichloride

17. DRAW the best Lewis structure for NOCl, a reactive material used as an ionizing solvent. (2A10)

. . . . . .
O == N -- Cl :
. . . .

18. What is the molecular geometry (shape) of ClF2¯ ? (2A10)
A. T-shaped
B. tetrahedral
C. bent
D. see-saw
E. linear

E. linear

19. What is the name of HClO4 ? (2A10)
A. hydrochlorate acid
B. chlorous acid
C. chloric acid
D. hydrochloric acid
E. perchloric acid

E. perchloric acid

20. Select the compound with the smallest magnitude lattice energy. (2A10)
A. NaCl(s)
B. SrO(s)
C. CsBr(s)
D. KBr(s)
E. CaO(s)

C. CsBr(s)

21. The number of sigma bonds in the molecule below is: (2A10)
A. 16
B. 10
C. 19
D. 14
E. 12

A. 16

22. What is the name for Al(NO3)3•2H2O ? (2A10)
A. aluminum(III) trinitrate dihydrate
B. aluminum trinitrate dihydrate
C. aluminum nitrate dihydrate
D. aluminum nitrate hydrate
E. aluminum nitrate

C. aluminum nitrate dihydrate

23. Phosphoryl iodide is used in the preparation of organophosphorus derivatives and phosphate esters. DRAWthe Lewis structure for POI3 which minimizes formal charges. (2A10)

I (single bond, two on 3 sides)
O (2 on top, 2 on bottom) ==== P ---- I (two on 3 sides)
I (single bond, two on 3 sides)

24. What is the formula for the binary compound formed by calcium and selenium? (2A10)
A. CaSe3
B. CaSe2
C. Ca3Se
D. CaSe
E. Ca2Se

D. CaSe

25. In the best Lewis structure of the iodate ion, IO3-, the formal charge on the central iodine atom is: (2A10)
A. 0
B. -2
C. +2
D. -1
E. +1

A. 0

26. Which of these compounds is most likely to be ionic? (2A10)
A. GaAs
B. NO2
C. H2O
D. SrBr2
E. CBr4

D. SrBr2

27. The average Te-O bond order in TeO4 (2A10)
2- is:
A. 1.0
B. 1.5
C. 1.33
D. 1.66
E. 2.0

B. 1.5

28. The compound, NaH2PO4, is present in many baking powders. What is its name? (2A10)
A. sodium hydrophosphate
B. sodium dihydride phosphate
C. sodium hydrogen phosphate
D. sodium biphosphate
E. sodium dihydrogen phosphate

E. sodium dihydrogen phosphate

29. What is the name of the compound formed when H2S gas is dissolved in water? (2A10)
A. hydrosulfuric acid
B. sulfuric acid
C. hydrosulfurous acid
D. sulfidic acid
E. sulfurous acid

A. hydrosulfuric acid

31. Lithium forms compounds which are used in dry cells and storage batteries and in high-temperature lubricants. It has two naturally occurring isotopes, 6Li (atomic mass = 6.015121 amu) and 7Li (atomic mass =7.016003 amu). Lithium has an average atomic mass of 6.9409 amu. What is the percent abundance of lithium-6? (2A10)
A. 7.503%
B. 46.16%
C. 6.080%
D. 92.50%
E. 86.66%

A. 7.503%

32. DRAW the best Lewis structure for ozone, O3? (2A10)

O (2 on 3 sides) ---- O (2 on 1 side) ==== O (2 on 2 sides)

33. DRAW the best Lewis structure for nitrogen trifluoride, NF3. (2A10)

F (2 on 3 sides) ---- N (2 on 1 side) ---- F (2 on 3 sides)
F (single bond, 2 on 3 sides)

34. The ideal value for the bond angle indicated by "a" in the illustration below is: (2A10)
A. 180°
B. 109.5°
C. 120°
D. 90°
E. 270°

B. 109.5°

35. The F S F bond angles in SF6 are: (2A10)
A. 180°
B. 120°
C. 90° and 180°
D. 90° and 120°
E. 109.5°

C. 90° and 180°

36. Which of the following is the empirical formula for C4H10O2 ? (2A10)
A. C8H20O4
B. C2H5O
C. CH2.5O0.5
D. C2H5
E. C4H10O2

B. C2H5O

37. DRAW the Lewis structure for XeO2F2 which correctly minimizes formal charges. (2A10)

O (double bond, 2 on 2 sides)
F (2 on 3 sides) ---- Xe ==== O (2 on 2 sides)
F (single bond, 2 on 3 sides)

38. Diiodine pentaoxide is used as an oxidizing agent that converts carbon monoxide to carbon dioxide. What is its chemical formula? (2A10)
A. I2O5
B. 2IO5
C. (IO5)2
D. I5O2
E. IO5

A. I2O5

39. What is the molecular geometry (shape) of BrF4¯ ? (2A10)
A. square pyramidal
B. octahedral
C. tetrahedral
D. see-saw
E. square planar

E. square planar

you should take a 5 minute break

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