wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Moc exam- G11 ASP

Total questions: 130

Worksheet time: 3hrs 46mins

Name
Class
Date
1.

Order the elements S, Cl, and F in terms of increasing ionization energy.

a)

S, Cl, F

b)

Cl, F, S

c)

F, S, Cl

d)

F, Cl, S

e)

S, F, Cl

2.

Order the elements S, Cl, and F in terms of increasing atomic radii.

a)

S, Cl, F

b)

Cl, F, S

c)

F, S, Cl

d)

F, Cl, S

e)

S, F, Cl

3.

Which of the following atoms would have the largest second ionization energy?

a)

Mg

b)

Cl

c)

S

d)

Ca

e)

Na

4.

Choose the element with the highest ionization energy.

a)

Na

b)

Mg

c)

Al

d)

P

e)

S

5.

List the following atoms in order of increasing ionization energy: Li, Na, C, O, F.

a)

Li<Na<C<O<F

b)

Na<Li<C<O<F

c)

F<O<C<Li<Na

d)

Na<Li<F<O<C

e)

Na<Li<C<F<O

6.

Consider the ionization (IE) of the magnesium atom. Which of the following is true?

a)

The IE of Mg is lower than that of Na.

b)

The IE of Mg is lower than that of Ne.

c)

The IE of Mg is lower than that of Be.

d)

The IE of Mg is higher than that of Ca.

e)

The IE of Mg is lower than that of Mg+.

7.

Which of the following statements is true?

a)

The first ionization potential of H is greather than that of He.

b)

The ionic radius of Fe+ is larger than that of F3+.

c)

The ionization energy of S2- is greater than that of Cl-.

d)

The atomic radius of Li is larger than that of Cs.

e)

All are false.

8.

What is the frequency of light (s-1) that has a wavelength of 1.23 x 10-6 cm?

a)

2.44 x 1016

b)

1.04 x 10-13 C

c)

9.62 x 1012

d)

3.69

9.

The wavelength of a photon that has an energy of 5.25 x 10-19 J is __________ m

a)

4.21 x 10-24

b)

2.38 x 1023

c)

2.64 x 106

d)

3.79 x 10-7

10.

Of the following transitions in the Bohr hydrogen atom, the __________ transition results in the emission of the highest-energy photon.

a)

n = 6 ¬ n = 1

b)

n = 1 ¬ n = 6

c)

n = 3 ¬ n = 6

d)

n = 6 ¬ n = 3

11.

The lines in the emission spectrum of hydrogen result from __________.

a)

electrons given off by hydrogen as it cools

b)

decomposing hydrogen atoms

c)

electrons given off by hydrogen when it burns

d)

energy given off in the form of visible light when an electron moves from a higher energy state to a lower energy state

12.

Which one of the following represents an acceptable possible set of quantum numbers (in the order n, l, ml, ms) for an electron in an atom?

a)

2, 1, 0, 0

b)

2, 2, 0, 1/2

c)

2, 0, 2, +1/2

d)

2, 0, 1, -1/2

e)

2, 1, -1, 1/2

13.

Which of the following correctly represents the second ionization of calcium?

a)

Ca+ (g) -> Ca2+ (g) + e

b)

Ca (g) --> Ca+ (g) + e

c)

Ca- (g) + e- -> Ca2- (g)

d)

Ca+ (g) + e- -> Ca (g)

e)

Ca+ (g) + e- ->Ca2+ (g)

14.

Which ion in the isoelectronic series below has the smallest radius in a crystal?

a)

O2-

b)

N3-

c)

Na+

d)

Al3+

e)

F-

15.

Which element could #3 be based on ionization energy?

a)

Na

b)

Mg

c)

Al

d)

Si

16.

Which Lewis dot structure shows exactly two unshared pairs of valence electrons?

a)

H2S

b)

CO2

c)

NH3

d)

CBr4

17.

What is the formal charge of Cl?

a)

0

b)

+1

c)

-1

d)

-2

18.

Which of the following substances contains both ionic and

covalent bonds?

a)

NH3

b)

CH4

c)

NaOH

d)

C2H5OH

19.

Which bond is the most polar?

a)

F-O

b)

H-O

c)

Na -O

d)

Sn-O

20.

Why can a molecule with the structure of NBr5 not exist?

a)

Nitrogen only has two energy levels and is thus unable to expand its octet.

b)

Bromine is much larger than nitrogen and cannot be a terminal atom in this molecule

c)

It is impossible to complete the octets for all six atoms using only valence electrons.

d)

Nitrogen does not have a low enough electronegativity to be the central atom of this molecule.

21.

Which of the following compounds would have the highest lattice energy?

a)

LiF

b)

MgCl2

c)

CaBr2

d)

C2H6

22.

Which structure is more likely to correspond with the actual Lewis diagram for the sulfate ion?

a)

Structure A; single bonds are more stable than double bonds

b)

Structure A; it has the most unshared pairs of electrons

c)

Structure B; there are more possible resonance structures

d)

Structure B; fewer atoms have formal charges

23.

The Lewis structure of N2H2 shows __________.

a)

a nitrogen-nitrogen triple bond

b)

a nitrogen-nitrogen single bond

c)

each nitrogen has one lone pair

d)

each nitrogen has two lone pairs

e)

each hydrogen has one lone pair

24.

A valid Lewis structure of _______ cannot be drawn without violating the octet rule.

a)

NF3

b)

IF3

c)

PF3

d)

SbF3

e)

SO42-

25.

Which atom can accommodate an octet of electrons, but doesn't necessarily have to accommodate an octet?

a)

N

b)

C

c)

H

d)

O

e)

B

26.

As the number of covalent bonds between two atoms increases, the distance between the atoms ______ and the strength of the bond between them ______.

a)

increases, increases

b)

decreases, decreases

c)

increases, decreases

d)

decreases, increases

e)

is unpredictable

27.

The Lewis structure of the CO32- ion is

a)
b)
c)
d)
e)
28.

Which of these bonds takes the most energy to break?

a)

single

b)

double

c)

triple

d)

quadruple

29.

The ion NO- has _____ valence electrons.

a)

10

b)

12

c)

14

d)

15

e)

16

30.

The formal charge on carbon in the molecule shown is _______.

a)

0

b)

+1

c)

+2

d)

+3

e)

-1

31.
The electronegativity of C is 2.5, F is 4.0.  predict the character of a C-F bond.
a)
polar covalent
b)
nonpolar covalent
c)
ionic
d)
metallic
32.
The interaction energy of two hydrogen atoms is shown on the graph above. Which of the answer choices displayed on the graph best represents the bond length of the H2 molecule?
a)
A
b)
B
c)
C
d)
D
33.

When the atoms in a molecule can form two different structures (not resonance structures), formal charge can help determine the best one (where lower or zero FC is best). A and B both follow the octet rule: use formal charge to determine which structure is the better one for NH3O.

a)

A is the better structure for NH3O

b)

B is the better structure for NH3O

c)

Both structures are equally good.

d)

Both structures are incorrect.

34.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

35.
How are compounds with metallic bonds similar to ionic compounds? 
a)
Both tend to have double and triple bonds
b)
Both tend to have low boiling points 
c)
Both tend to have poor conductivity
d)
Both tend to have high melting points 
36.

How many peaks should oxygen have in it's PES diagram?

a)

1

b)

2

c)

3

d)

4

37.

Given the peaks of a PES diagram of oxygen, the peaks of fluorine would be

a)

shifted to the right (assuming binding energy goes from highest energy to lowest energy on the x axis)

b)

shifted to the left (assuming binding energy goes from highest energy to lowest energy on the x axis)

c)

be in the same position, just higher (assuming binding energy goes from highest energy to lowest energy on the x axis)

38.

The melting point of MgO is higher than that of NaF. Which of the following best explains this observation?

a)

O2- is more negatively charged than F-

b)

Mg2+ is more positively charged than Na+

c)

The O2- ion is smaller than the F- ion

d)

Mg2+ is more positively charged than Na+ and O2- is more negatively charged than F-

39.

The elements C and Se have the same electronegativity value, 2.55. Which of the following claims about the compound that forms from C and Se is most likely to be true?

a)

The carbon-to-selenium bond is unstable.

b)

The carbon-to-selenium bond is nonpolar covalent.

c)

The compound has the empirical formula CSe.

d)

A molecule of the compound will have a partial negative charge on the carbon atom.

40.

Which of the following correctly indicates whether the solid represented by the particulate model shown above conducts electricity and explains why or why not?

a)

It conducts electricity because it is made of positive and negative ions.

b)

It conducts electricity because it is made of particles of different sizes.

c)

It does not conduct electricity because its ions cannot move freely within the solid.

d)

It does not conduct electricity because there are small spaces between the particles.

41.

Identify the element that would produce this spectrum.

(a)  

42.

Write the electron configuration for the element represented in this PES.

(a)  

43.

Sr2+ and Br- are isoelectronic. Which has a smaller radius and why?

a)

Sr2+ because it has a greater nuclear charge, which applies a greater force of attraction on the electrons, thereby pulling them closer to the nucleus.

b)

Sr2+ because it has fewer electron shells, therefor have a less distance from the valence electrons to the nucleus.

c)

Br- because it has a greater nuclear charge, which applies a greater force of attraction on the electrons, thereby pulling them closer to the nucleus.

d)

Br- because it has fewer electron shells, therefor have a less distance from the valence electrons to the nucleus.

44.

According to Coulomb's Law, which peak would experience the greatest force of attraction to the nucleus in this PES?

a)

A

b)

B

c)

C

d)

D

45.

Which element is the most electronegative?

a)

Potassium

b)

Fluorine

c)

Neon

d)

Selenium

46.

Which chemical formula would be expected for one formula unit of Aluminum Sulfide?

a)

AlS

b)

Al3S2

c)

Al2S

d)

Al2S3

47.

Use the data for germanium in the table above to identify the most probable values for the atomic radius and electronegativity of selenium from the choices below.

a)

Atomic Radius:155 pm, electronegativity: 2.55

b)

Atomic Radius:120 pm, electronegativity: 2.55

c)

Atomic Radius:155 pm, electronegativity: 1.85

d)

Atomic Radius:120 pm, electronegativity: 1.85

48.

Removing a single electron from which of the following neutral atoms in the gas phase would require the greatest amount of energy?

a)

K

b)

Rb

c)

Br

d)

I

49.

Which of the following lists K, Na, Cl, and Br in order of decreasing atomic radius?

a)

K > Na > Br > Cl

b)

Na > K > Cl > Br

c)

Cl > Br > Na > K

d)

Br > Cl > Na > K

50.

Identify the element

a)

Zr

b)

Tc

c)

In

d)

Mo

51.

The successive ionization energies for a certain element are outlined in the table. Predict the identity of the element from the information given.

a)

Na

b)

Mg

c)

Al

d)

Si

52.

Which orbital diagram represents an atom with six valence electrons?

a)

A

b)

B

c)

C

d)

D

53.

Which of the following answer choices provides a correct prediction and justification for relative differences in the first ionization energies of hydrogen and lithium?

a)

The first ionization energy for lithium is greater than that of hydorgen because lithium has more protons in its nucleus.

b)

The first ionization energy for lithium is greater than that of hydrogen because the radius of the 1s orbital in lithium is smaller than the 1s orbital in hydrogen.

c)

The first ionization energy for lithium is less that that of hydrogen because lithium has a smaller atomic radius.

d)

The first ionization energy for lithium is less than that of hydrogen because hydrogen has a smaller atomic radius.

54.

Which of the following ranks elements in order of increasing ability to attract electrons toward themselves in a chemical bond?

a)

Rb< Zr < Cd< Hg

b)

I < Sn < Cd < Zn

c)

B< Al < In < Ag

d)

Ga < Ge < As < N

55.

Which of the following ranks ions in order to increasing ionic radii?

a)

Na+ < Al+3 < S-2 < Cl-

b)

Ca2+ < K+ < Se2- < Br-

c)

Sr2+ < Rb+ < I- < Te2-

d)

F- < O2- < Be2+ < Li+

56.

The proper pair of the L value with the orbital shape.

a)

0; f

b)

3; p

c)

1; s

d)

2; d

57.

If n = 3, what are the allowed values of L? Tick all that apply:

a)

0

b)

1

c)

2

d)

3

58.

For L = 2, tick the possible values of m:

a)

-2

b)

-1

c)

0

d)

1

e)

2

59.

Which of the following sets of quantum numbers (n, l, ml, and ms) describes the valence electron of Na?

a)

2, 1, 0, -½

b)

2, 0, 0, -½

c)

3, 1, 1, +½

d)

3, 0, 0, +½

60.

Which of the following sets of quantum numbers (n, l, ml, and ms) describes the valence electron of 4s1?

a)

2, 0, 0, +1/2

b)

2, 1, 0, +1/2

c)

4, 0, 0, +1/2

d)

4, 1, 1, +1/2

61.

Which of the following sets of quantum numbers (n, l, ml, and ms) describes the electron 3p6?

a)

3, 1, 0, - 1/2

b)

3, 1, -1, -1/2

c)

1, 2, -1, -1/2

d)

1, 3, -1, -1/2

62.

n = 2

l = 2

m = 0

s = +1/2


Which is the correct notation

a)

2p1

b)

2p2

c)

2s2

d)

No correct answer

63.

What is the maximum number of electrons that can be found in the n3 energy level

max number= 2n²

a)

3

b)

6

c)

8

d)

9

e)

18

64.

Which of the following sub levels correspond to n=3 l=2

l = 0–>n-1

a)

2p

b)

3s

c)

3p

d)

3d

e)

3f

65.

n=4, l=3?

a)

4f

b)

4d

c)

3s

d)

3p

66.

How many unpaired electrons does an atom of chromium contain?

this can be tricky...

a)

2

b)

3

c)

4

d)

5

e)

6

67.

Which of the following elements is Paramagnetic?

look at the atomic numbers.

a)

Mg

b)

Ne

c)

P

d)

Ca

e)

Kr

68.

What is the maximum number of electrons numbers n=4 and ms= 1/2

Think 2n²

a)

8

b)

16

c)

24

d)

32

e)

64

69.

Which of the following values does NOT represent a valid electron?

a)

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

b)

n=(4), l=(2), ml=(-1), ms=(-1/2)

c)

n=(2), l=(0), ml=(0), m=(-1/2)

d)

n=(4), l=(2), ml=(-3), ms=(+1/2)

70.

De Broglie equation

a)

relates the momentum of a mass to its wavelength

b)

relates the energy of a mass to its wavelength

c)

relates the frequency of a mass to its wavelength

d)

relates the work function of a mass to its wavelength

71.

The wavelength associated with an electron accelerated through a potential difference of 100V is of the order

a)

1000 Ao

b)

10.5 Ao

c)

100 Ao

d)

1.2 Ao

72.

Multiple answers can be correct: Energy of light is proportional to:

a)

Directly proportional to frequency

b)

Inversely proportional to wavelength.

c)

Directly proportional to speed of light.

d)

Independant of speed and wavelength

73.

An unknown particle released from a Cepheid type II star is found to have a mass of 1.66 x 10-28kg and a velocity near the speed of light. What is the wavelength of the particle?

a)

7.56 x 10-14 m

b)

1.33 x 10-14 m

c)

2.55 x 10-12 m

d)

5.00 x 10-18 m

74.

The de Broglie wavelength of an electron is 1.21 x 10-2 nm. It is traveling at what percent of the speed of light?

a)

10

b)

20

c)

30

d)

40

75.

What is the de Broglie wavelength for a proton (m= 1.67* 10-27kg) moving at a speed of 6.0 *106

m/s?

a)

2.0*10-13 m

b)

0.33*10-13 m

c)

1.3*10-13 m

d)

0.66*10-13m

76.

The de Broglie wavelength of a 0.060 kg golf ball is 4.28 * 10-34m. What is its speed?

a)

15 m/s

b)

26 m/s

c)

31 m/s

d)

48 m/s

77.

The energy of photoelectrons emitted from a metal surface can be increased by

a)

using light of higher frequency.

b)

using light of longer wavelength.

c)

using light of higher intensity.

d)

using monochromatic, polarized light.

78.

A metal with a work function of 3.5 eV is exposed to photons with an energy of 3.7 eV. What is the maximum kinetic energy of the emitted photoelectrons?

a)

0.2 eV

b)

0.9 eV

c)

1.1 eV

d)

7.7 eV

79.

What is the energy of a photon with a frequency of 5x1014 Hz? (you need to do calculation. You have enough time) h=6.6x10-34 J/Hz

a)

2.5x10-19 J

b)

3.0x10-19 J

c)

3.3x10-19 J

d)

4.5x10-19 J

80.

A photon with frequency of 1.5 x 10^15 Hz is incident on a piece of metal in the standard photoelectric experimental setup. What is the wavelength of this photon?

a)

20 nm

b)

150nm

c)

200nm

d)

500nm

81.

How much energy is carried by this electron?

a)

1.33 eV

b)

6.21 eV

c)

9.7 x 10^-19 J

d)

1.33 x 10^-19 J

82.

An electron inside the metal has a binding energy of 7.3eV.

a)

This electron cannot be reached by the UV light.

b)

This electron can be reached by the UV light, but will not absorb it.

c)

This electron can be reached by the UV light, will absorb it, but will not escape the metal.

d)

The electron can be reached by the UV light, will absorb it, and will escape the metal.

83.
Which drawing represents the process by which an emission line is formed?
a)
A
b)
B
c)
C
d)
D
84.
Which drawing represents the process by which an absorption line is formed?
a)
A
b)
B
c)
C
d)
D
85.

What is the electron configuration for this PES graph?

a)

1s22s22p63s23p2

b)

1s22s22p63s23p1

c)

1s22s22p63s23p3

d)

1s22s22p63s2

86.

Which element is represented by this PES graph?

a)

argon

b)

potassium

c)

calcium

d)

scandium

87.

The complete photoelectron spectrum for an element is shown above. Which of the following observations would provide evidence that the spectrum is consistent with the atomic model of the element?

a)

A neutral atom of the element contains exactly two electrons.

b)

The element does not react with other elements to form compounds.

c)

In its compounds, the element tends to form ions with a charge of +1.

d)

In its compounds, the element tends to form ions with a charge of +3.

88.
What is the frequency of UV light that has an energy of 2.39 × 10 -18 J? 
a)
2.32 x 109 Hz
b)
3.60 x 1015 Hz
c)
1.58 x 10-51 Hz
d)
3 x 108  m/s
89.

The line with the shortest wavelength is produced in the hydrogen spectrum when electron moves

a)

from n=2 to n=1

b)

rom n=4 to n=1

c)

from n=3 to n=1

d)

from n=4 to n=3

90.
There are seven arrows shown. Which would correspond to the longest wavelength?
a)
the left Lyman arrow
b)
the right Lyman arrow
c)
the left Balmer arrow
d)
the Paschen arrow
91.

What evidence did you observe that proves that elements give off their own unique color spectrum?

a)

All of the gas tubes produced a full spectrum. (A rainbow.)

b)

When we looked at white light through a prism, we saw the rainbow.

c)

Each gas tube gave off its own unique color and color spectrum when we looked at the light through the spectroscope. None of them were the exact same.

d)

Each gas tube gave off the same color and color spectrum when we looked at the light through a spectroscope.

92.

Regardless of how hot the flame is, when a metal ion is placed in a flame, it always give off the same color light. Why?

a)

The number of protons is still the same, so the same number of electrons get excited and fall back to the ground state the same way and give off the same color every time.

b)

The number of electrons is still the same, so the same number of electrons get excited and fall back to the ground state the same way and give off the same color every time.

c)

The number of neutrons is still the same, so the same number of electrons get excited and fall back to the ground state the same way and give off the same color every time.

d)

The number of ions is still the same, so the same number of electrons get excited and fall back to the ground state the same way and give off the same color every time.

93.
What gases are in the unknown mixture?
a)
Gas B & Gas D
b)
Gas C & Gas B
c)
Gas A & Gas D
d)
Gas D & Gas C
94.
Which elements are in the unknown sample?
a)
A and B
b)
B and C
c)
A and D
d)
B and D
95.

Which electron transition releases a photon with the greatest energy?

a)

orbital 6 to orbital 3

b)

orbital 5 to orbital 3

c)

orbital 4 to orbital 3

d)

orbital 7 to orbital 3

96.

Line emission spectra is produced from atoms when

a)

electrons release energy as they move to their excited state.

b)

electrons absorb energy as they move to their excited state.

c)

electrons release energy as they return to the ground state.

d)

electrons absorb energy as they return to the ground state.

97.
Which molecule contains bonds with a GREATER polarity?
a)
HCl
b)
CCl4
98.
A diatomic molecule like O2 is always_______ because electrons are shared ________.
a)
nonpolar; equally
b)
polar; equally
c)
nonpolar; unequally
d)
nonpolar; unequally
99.
If Boron bonds with Hydrogen, a ____________ bond forms.
a)
polar covalent
b)
nonpolar covalent
c)
metallic
d)
ionic
100.

Which diagram shows the correct bonding and correct bond polarity in a molecule of oxygen difluoride?

a)
b)
c)
d)
101.

Which of these atoms has the highest electronegativity?

a)

Na

b)

Mg

c)

Cl

d)

Ar

102.

Which of the following gives the correct order of electronegativities of elements?

a)

F > Cl > O > H

b)

Cl > O > N > S

c)

O > S > H > Si

d)

Cl > N > O > F

103.

Which of the following pairs of atoms can form a polar covalent bond?

(1) N and O

(2) C and C

(3) C and N

a)

(1) and (2) only

b)

(1) and (3) only

c)

(2) and (3) only

d)

(1), (2) and (3)

104.

Which of the following covalent bonds is the most polar?

a)

H---Cl

b)

S---F

c)

Si---O

d)

P--Br

105.

When the Lewis structure for HCOOCH3 is drawn, how many bond pairs and how many lone pairs of electrons are present?

a)

Bond pairs 8

Lone pairs 4

b)

Bond pairs 7

Lone pairs 5

c)

Bond pairs 7

Lone pairs 4

d)

Bond pairs 5

Lone pairs 5

106.

How do bond length and bond strength change as the number of bonds between two atoms increases?

a)

Bond length: increases

Bond strength: increases

b)

Bond length: increases

Bond strength: decreases

c)

Bond length: decreases

Bond strength: increases

d)

Bond length: decreases

Bond strength: decreases

107.

Which of the following will have the highest bond energy?

a)

H-F

b)

H-Cl

c)

H-Br

d)

H-I

108.

Which of the following will have the lowest bond energy?

a)

N-N

b)

N-O

c)

N-F

109.

Which TWO factors are most important in determining bond strength and bond length?

a)

polarity

b)

The bond order

c)

The number of valence electrons

d)

The atomic radius

110.

Based on electronegativity values, which bond is the most polar?

a)

B-C

b)

C-O

c)

N-O

d)

O-F

111.

Which substance has the lowest electrical conductivity?

a)

Cu(s)

b)

Hg(l)

c)

H2(g)

d)

LiOH(aq)

112.

Which fluoride is the most ionic?

a)

NaF

b)

CsF

c)

MgF2

d)

BaF2

113.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
114.

Factors affecting the value of lattice energy

a)

the size of the ion

b)

the charge of the ion

c)

the size of the ion and the charge of the ion

115.

Which are the particles in a metallic lattice?

a)

cations and anions

b)

delocalised electrons and anions

c)

cations and delocalised anions

d)

cations and delocalised electrons

116.

Which of the following compounds has the lowest lattice energy?

a)

LiF

b)

NaCl

c)

KBr

d)

RbI

117.

Which of the following would have the highest lattice energy?

a)

NaNO3

b)

MgSO4

c)

AlPO4

d)

Na2SO4

118.

Which set of elements is most likely to form an ionic compound?

a)

Na and O

b)

C and O

c)

Na and K

119.
Which of the following is NOT an ionic compound:
a)
CaO
b)
NaOH
c)
BaCl2
d)
Br2
120.

Lowest lattice enthalpy (∆LEH)?

a)

NaBr

b)

LiCl

c)

KI

121.

Greatest lattice enthalpy (∆LEH)?

a)

NaBr

b)

LiCl

c)

KI

122.

Carbonate (CO32-) has how many double bonds?

a)

0

b)

1

c)

2

d)

3

123.

In HCN (Carbon is usually the central atom) what kind of bond is between the C and N

a)

Single

b)

Double

c)

Triple

124.

Which of the following subshells has the lowest energy?

a)

4d

b)

5s

c)

5p

d)

5f

125.

Which type of bond is characterized by unequal "sharing" of electrons between two non-metals?

a)

non-polar covalent

b)

polar covalent

c)

coordinate

d)

hydrogen

e)

ionic

126.

How many binding energies (peaks) would you observe on the photoelectron spectrograph for sulfur?

a)

2

b)

3

c)

4

d)

5

127.

This photoelectron spectrograph shows data for which element?

a)

boron (B)

b)

phosphorous (P)

c)

arsenic (As)

d)

strontium (Sr)

128.

These PES spectra shows the binding energy of the 1s electron in nitrogen and oxygen. Why is the 1s binding energy less for nitrogen than for oxygen?

a)

In nitrogen atoms, there are more electron-electron repulsions.

b)

Nitrogen atoms are smaller than oxygen atoms.

c)

Nitrogen atoms have a smaller nuclear charge than oxygen atoms.

d)

There are fewer electrons in nitrogen atoms.

129.
The bond energy of a carbon-carbon double bond, when compared to the energy of a carbon-carbon single bond, is
a)
twice the bond energy of a single bond
b)
greater in bond energy than a single bond but less than twice the bond energy
c)
less than the bond energy of a single bond
d)
equal in bond energy to a single bond
130.

Molecule that has more than 8 electrons surrounding the central atom is classified as

a)

odd number electron

b)

expanded octet

c)

incomplete octet

d)

even number electron