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Unit 1B Electronic Structure

Total questions: 24

Worksheet time: 14mins

Name
Class
Date
1.
How many protons, electrons, and neutrons, respectively, does this species have?
a)
15, 15, 16
b)
15, 12, 16
c)
15, 18, 16
d)
15, 12, 27
2.
Representative elements (elements in the tall columns of the periodic table) tend to:
a)
have high ionization energies
b)
have high metallic character
c)
gain or lose electrons to remain neutral
d)
gain or lose electrons to become isoelectronic with a noble gas
3.
Which of the following would represent an atom containing 26 protons, 24 electrons and 30 neutrons?
a)
56Fe2+
b)
56Cr2+
c)
56Fe2-
d)
30Fe2+
4.
How many dots would you place on a lewis dot structure for Phosphorus?
a)
15
b)
3
c)
5
d)
31
5.
Which color of visible light has the highest frequency? (of those provided)
a)
Orange
b)
Red
c)
Blue
d)
Green
6.
When an electron absorbs a packet of energy called a __________, it moves to the ___________
a)
proton, ground state
b)
photon, excited state
c)
photon, ground state
d)
photon, emission spectrum
7.
The electron configuration for an atom of potassium is:
a)
1s22s22p63s23p3
b)
1s22s22p63s23p6
c)
1s22s22p63s23p64s1
d)
1s22s22p63s23p64s2
8.
Halogens have how many valence electrons?
a)
1
b)
7
c)
8
d)
17
9.
What element has the electron configuration:  [Xe]6s24f145d10
a)
Iron
b)
Cadmium
c)
Mercury
d)
Lead
10.
Where would an electron with the following quantum numbers be located in an atom?
n = 2, l = 1, ml=0, ms= +1/2
a)
2s
b)
2p
c)
2d
d)
This is an impossible set of quantum numbers.
11.
Where would an electron with the following quantum numbers be located in an atom?
n = 3, l = 3, ml=1, ms= +1/2
a)
3s
b)
3p
c)
3d
d)
This is an impossible set of quantum numbers.
12.
How many electrons in the same atom could have the following quantum numbers:
n = 2
a)
2
b)
6
c)
8
d)
none
13.
How many electrons in the same atom could have the following quantum numbers:
n = 4, l = 3, ml = 3, ms = +1/2
a)
1
b)
2
c)
10
d)
14
14.
How many electrons in the same atom could have the following quantum numbers:
n = 3, l = 1
a)
2
b)
6
c)
10
d)
18
15.
Which is the best conductor of heat and electricity
a)
Ag
b)
Cd
c)
Au
d)
Hg
16.
Which answer has the species in the correct order of increasing ionic/atomic radius?
a)
S < S-2 < S+2
b)
S+2 < S < S-2 
c)
S-2 < S+2 < S
d)
S-2 < S < S+2
17.
What is the most electronegative element of those listed?
a)
Al
b)
P
c)
Ag
d)
In
18.
Which has the elements listed in decreasing atomic radius
a)
Sr>Y>Sc>Ti
b)
Ti>Y>Sc>Sr
c)
Ti>Sc>Y>Sr
d)
Sr>Sc>Y>Ti
19.
24.1% of all the isotopes of a an element have a mass of 75.23 amu, 48.7% have a mass of 74.61 amu, and 27.2% have a mass of 75.20 amu.
What is the average mass of this element?
a)
74.92 amu
b)
24.97 amu
c)
75.01 amu
d)
74.51 amu
20.

According to Coulomb's law, what happens to the force between two charged particles if the distance between them is doubled?

a)

The force between the two charged particles will decrease by a factor of two.

b)

The force between the two charged particles will decrease by a factor of four.

c)

The force between the two charged particles will increase by a factor of four.

d)

The force between the two charged particles will remain the same.

21.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
22.
 Which of the following generally applies to the noble gases? 
a)
high ionization energy, low electronegativity, high reactivity
b)
high ionization energy, high electronegativity, high reactivity
c)
low ionization energy, low electronegativity, low reactivity
d)
high ionization energy, low electronegativity, low reactivity 
23.

What is ionization energy?

a)

energy required to capture an electron.

b)

energy required to remove one electron,

c)

energy required to move an electron.

d)

energy required to relax an electron.

24.

As you move across the periodic table, atoms tend to get smaller because, ______________.

a)

the atoms have more mass.

b)

the atoms have less mass.

c)

the atoms have more protons.

d)

the atoms have fewer electrons.

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