CHE 110 Fall 2018 Exam 1

Your Name: Your ID:

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Question #: 1

Which quantum number determines the direction of the spin of an electron?

A. s

B. ms

C. ml

D. l

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Question #: 2

Consider the orbital diagram of an atom below.

What are the subshells labeled xx and yy? xx = 1 yy = 2

1.

2.

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Question #: 3

Coulomb's Law in conjunction with the difference in penetration between the electrons in a 2s orbital verses a 2p orbitals results in

A. the 2p subshell having higher energy than the 2s subshell.

B. the 2p subshell having lower energy than the 2s subshell.

C. a greater effective nuclear charge of electrons in the 2p versus the 2s subshell.

D. a greater effective nuclear charge of electrons in the 2s versus the 2s subshell.

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Question #: 4

Consider the orbital diagram of an atom below.

What element has this orbital diagram? 1 Provide name or symbol.

1.

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Question #: 5

Which statement is true concerning the orbital diagram above?

A. The atom is diamagnetic because there are orbitals with only 1 electron in them.

B. The diagram represents the ground state electronic structure of an atom.

C. If the two electrons in the subshell labeled yy (in red) should be in the same box with

opposite spins.

D. This orbital diagram does not exist for any atom in its ground state or its excited state.

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Question #: 6

Which quantum number must be different for the two arrows indicated by the blue box?

A. n

B. l

C. ml

D. ms

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Question #: 7

What principle or rule is violated by the following orbital diagram?

A. Pauli exclusion principle

B. Aufbau principle

C. Hund's rule

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Question #: 8

How many electrons in an atom could have these sets of quantum numbers? n = 3 1 n = 3, ml= 1 2 n = 3, l = 1, ml= 0 3

1.

2.

3.

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Question #: 9

How many valence electrons are in the atom indicated by the orbital diagram below? 1

1.

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Question #: 10

Write the shorthand ground state electron configuration of calcium. 1 Provide spaces between subshells and do not format the superscripts. For example [He] 2s2 2p2 for [He] 2s2 2p2

1.

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Question #: 11

What element has the shorthand ground state electron configuration of [Ar] 4s1 3d5? Enter either the element name or symbol. 1

1.

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Question #: 12

Which orbitals are degenerate in the following orbital diagram?

A. Only the two, completely filled, 2p orbitals.

B. All three 2p orbitals.

C. The 1s with the 2s.

D. The one 2p orbital with a single electron.

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Question #: 13

Provide the symbol for the element (M) with a 2+ charge (M2+) that has the electron configuration [Kr] 4d1. M = 1

1.

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Question #: 14

Provide the symbol for the element (E) 3– charge (E3–) that has the electron configuration 1s2 2s2 2p6. E = 1

1.

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Question #: 15

Select the statement that provides the element with the smaller radius between P and Cl and provides the correct chemical reason for the difference.

A. P is smaller because it lies farther to the left on the periodic table.

B. Cl is smaller because it lies farther to the right on the periodic table.

C. P is smaller because its nuclear charge is smaller.

D. Cl is smaller because its effective nuclear charge is greater.

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Question #: 16

Which answer provides the atoms in order of increasing atomic radii (smallest to largest)?

A. Mg Ca O S

B. O S Mg Ca

C. Mg Ca S O

D. S O Ca Mg

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Question #: 17

What is the nuclear charge (z) of S? 1 What is the shielding constant (σ) of S? 2 What is the effective nuclear charge of S? 3

1.

2.

3.

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Question #: 18

Description of the above image. The blue spheres represent a diatomic molecule. The black dots are the atom's nuclei. Line segment A reaches from outside edge of one atom to the outside edge of the other atom. Line segment B reaches from nucleus to nucleus. How is atomic radius defined?

A. Length of line A.

B. ½ the length of line A.

C. Length of line B.

D. ½ the length of line B.

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Question #: 19

Examine each pair of atoms and/or ions. Select the two that list the smaller atomic or ionic radius first.

A. Li, Li+

B. O, O2–

C. O2–, Na+

D. Na+, Li+

E. Ne, F–

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Question #: 20

Select the two pairs of atoms or ions that are isoelectronic.

A. Li, Li+

B. O, O2–

C. O2–, Na+

D. Ne, F–

E. Na+, Li+

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Question #: 21

Select the true statement.

A. All atoms and ions that have the same number of electrons must have isoelectronic

ground state electron configurations.

B. Ti2+ is isoelectronic with Ca.

C. Mn2+ is isoelectronic with Fe3+.

D. All of the above are true.

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Question #: 22

Which equation is the reaction associated with the first ionization of Li?

A. Li(g) →Li+(g) + e–

B. Li(g) + e– →Li+(g)

C. Li(g) →Li–(g) + e–

D. Li(g) + e–→ Li–(g)

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Question #: 23

Ionization energy is

A. endothermic and always negative in value.

B. exothermic and always negative in value.

C. exothermic and always positive in value.

D. endothermic and always positive in value.

E. sometimes endothermic and sometimes exothermic.

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Question #: 24

Select the element that has the highest first ionization energy.

A. Li

B. Be

C. K

D. Ca

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Question #: 25

The successive ionization energies of one of the elements below is provided. Select the element.

A. K

B. Ca

C. Sc

D. Ga

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Question #: 26

Elements with high electrons affinities (that is, they are very exothermic)

A. tend to form cations easily.

B. tend to form anions easily.

C. are highly reactive metals.

D. are unreactive nonmetals.

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Question #: 27

Electron affinity is the energy 1 [required, released, change] when an electron is 2 [added to, removed from] a gaseous atom.

1.

2.

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Question #: 28

Provide the group name (not group number) of the elements with the greatest electron affinity (most exothermic). Group name is 1 .

1.

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Question #: 29

Which properties can be typically paired together?

A. High metallic character with low ionization energy.

B. High metallic character with high ionization energy.

C. High metallic character with high electron affinity (very exothermic).

D. High metallic character with greater number of valence electrons.

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Question #: 30

Bonus Question: The speed of light is 3.00 ×108 m/s. How long (in milliseconds) will it take light to travel the distance across the diameter of a human hair that is 175 micrometers. 1 ms Report your answer with three significant figures. Do NOT include units in your answer. Use the format 2.2E2 or 2.2E-2 if you use scientific notation.

1.

DRAFTDo Not Use Until Posted.

CHE 110 Fall 2018 Exam 1 - Confidential

Your Name: Your ID:

Question #: 1

Which quantum number determines the direction of the spin of an electron?

A. s

✓B. ms C. ml D. l

Question #: 2

Consider the orbital diagram of an atom below.

What are the subshells labeled xx and yy?

xx =     1    

yy =     2    

 

1. 3s

2. 3p

Question #: 3

Coulomb's Law in conjunction with the difference in penetration between the electrons in a 2s

orbital verses a 2p orbitals results in

✓A. the 2p subshell having higher energy than the 2s subshell.

B. the 2p subshell having lower energy than the 2s subshell. C. a greater effective nuclear charge of electrons in the 2p versus the 2s subshell. D. a greater effective nuclear charge of electrons in the 2s versus the 2s subshell.

Question #: 4

Consider the orbital diagram of an atom below.

What element has this orbital diagram?     1    

Provide name or symbol.

1. S|sulfur|

Question #: 5

Which statement is true concerning the orbital diagram above?

A. The atom is diamagnetic because there are orbitals with only 1 electron in them.

✓B. The diagram represents the ground state electronic structure of an atom. C. If the two electrons in the subshell labeled yy (in red) should be in the same box with

opposite spins. D. This orbital diagram does not exist for any atom in its ground state or its excited state.

Question #: 6

Which quantum number must be different for the two arrows indicated by the blue box?

A. n B. l

✓C. ml D. ms

Question #: 7

What principle or rule is violated by the following orbital diagram?

A. Pauli exclusion principle B. Aufbau principle

✓C. Hund's rule

Question #: 8

How many electrons in an atom could have these sets of quantum numbers?

n = 3      1      

n = 3, ml= 1     2      

n = 3, l = 1, ml= 0       3    

1. 18

2. 4

3. 2

Question #: 9

How many valence electrons are in the atom indicated by the orbital diagram below?     1    

1. 7

Question #: 10

Write the shorthand ground state electron configuration of calcium.

    1    

Provide spaces between subshells and do not format the superscripts. For example [He] 2s2 2p2

for [He] 2s2 2p2

 

1. [Ar] 4s2

Question #: 11

What element has the shorthand ground state electron configuration of [Ar] 4s1 3d5?

Enter either the element name or symbol.     1    

1. Cr|Chromium|

Question #: 12

Which orbitals are degenerate in the following orbital diagram?

A. Only the two, completely filled, 2p orbitals.

✓B. All three 2p orbitals. C. The 1s with the 2s. D. The one 2p orbital with a single electron.

 

Question #: 13

Provide the symbol for the element (M) with a 2+ charge (M2+) that has the electron

configuration [Kr] 4d1.

M =     1    

1. Y

Question #: 14

Provide the symbol for the element (E)  3– charge (E3–) that has the electron configuration 1s2

2s2 2p6.

E =     1    

1. N

Question #: 15

Select the statement that provides the element with the smaller radius between P and Cl and

provides the correct chemical reason for the difference.

A. P is smaller because it lies farther to the left on the periodic table.

B. Cl is smaller because it lies farther to the right on the periodic table. C. P is smaller because its nuclear charge is smaller.

✓D. Cl is smaller because its effective nuclear charge is greater.

Question #: 16

Which answer provides the atoms in order of increasing atomic radii (smallest to largest)?

A. Mg Ca O S

✓B. O S Mg Ca C. Mg Ca S O D. S O Ca Mg

Question #: 17

What is the nuclear charge (z) of S?     1    

What is the shielding constant (σ) of S?     2    

What is the effective nuclear charge of S?     3    

1. 16|+16|

2. 10

3. 6|+6|

Question #: 18

Description of the above image. The blue spheres represent a diatomic molecule. The black dots

are the atom's nuclei. Line segment A reaches from outside edge of one atom to the outside edge

of the other atom. Line segment B reaches from nucleus to nucleus.

How is atomic radius defined?

A. Length of line A. B. ½ the length of line A. C. Length of line B.

✓D. ½ the length of line B.

Question #: 19

Examine each pair of atoms and/or ions. Select the two that list the smaller atomic or ionic

radius first.

A. Li, Li+

✓B. O, O2–

C. O2–, Na+

D. Na+, Li+ ✓E. Ne, F–

Question #: 20

Select the two pairs of atoms or ions that are isoelectronic.

A. Li, Li+ B. O, O2–

✓C. O2–, Na+

✓D. Ne, F–

E. Na+, Li+

Question #: 21

Select the true statement.

A. All atoms and ions that have the same number of electrons must have isoelectronic

ground state electron configurations.

B. Ti2+ is isoelectronic with Ca. ✓C. Mn2+ is isoelectronic with Fe3+.

D. All of the above are true.

Question #: 22

Which equation is the reaction associated with the first ionization of Li?

✓A. Li(g) →Li+(g) + e–

B. Li(g) + e– →Li+(g) C. Li(g) →Li–(g) + e–

D. Li(g) + e–→ Li–(g)

Question #: 23

Ionization energy is

A. endothermic and always negative in value. B. exothermic and always negative in value. C. exothermic and always positive in value.

✓D. endothermic and always positive in value. E. sometimes endothermic and sometimes exothermic. 

Question #: 24

Select the element that has the highest first ionization energy.

A. Li

✓B. Be C. K D. Ca

Question #: 25

The successive ionization energies of one of the elements below is provided. Select the element.

 

A. K

✓B. Ca C. Sc D. Ga

Question #: 26

Elements with high electrons affinities (that is, they are very exothermic)

A. tend to form cations easily.

✓B. tend to form anions easily. C. are highly reactive metals. D. are unreactive nonmetals.

Question #: 27

Electron affinity is the energy     1     [required, released, change] when an electron is     2    

[added to, removed from] a gaseous atom.

1. change

2. added to

Question #: 28

Provide the group name (not group number) of the elements with the greatest electron affinity

(most exothermic).

 

Group name is     1    .

1. halogens|halogen|

Question #: 29

Which properties can be typically paired together?

✓A. High metallic character with low ionization energy.

B. High metallic character with high ionization energy. C. High metallic character with high electron affinity (very exothermic). D. High metallic character with greater number of valence electrons.

Question #: 30

Bonus Question:

The speed of light is 3.00 ×108 m/s. How long (in milliseconds) will it take light to travel the

distance across the diameter of a human hair that is 175 micrometers.

    1     ms

Report your answer with three significant figures. Do NOT include units in your answer. Use

the format 2.2E2 or 2.2E-2 if you use scientific notation.

 

1. 5.83E-10