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WorksheetsElectrons and Atomic Structure
Total questions: 87
Worksheet time: 3hrs 31mins
Name
Class
Date
1.
What atom matches this electron configuration?
1s22s22p63s2
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
2.
The electron configuration of an atom is 1s22s22p6. The number of electrons in the atom is
a)
3
b)
6
c)
8
d)
10
3.
Identify the Electron Configuration for Aluminum (Al)
a)
1s2 2s2 2p6 3s2 3p1
b)
1s2 2s2 2p6 3s2 3p3
c)
1s2 2s2 2p6 3s2 4p1
4.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
5.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
6.
What is the shorthand electron configuration for Sulfur atom? (Unfamiliar Situation)
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
7.
What element in Period 4 has 5 valence electrons? (Unfamiliar Situation)
a)
Zr
b)
As
c)
V
d)
Sb
8.
As you move down the periodic table atoms get bigger. This is because ____________. (Unfamiliar Situation)
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more neutrons
9.
What are the maximum number of electrons that go on the first 3 energy levels?
a)
2,4,16
b)
2,8,18
c)
4,8,12
d)
3,4,6
10.
What are valence electrons?
a)
electrons on the first orbital always
b)
nucleus
c)
the outermost shell
d)
the number of electrons on the outermost orbital
11.
How many energy levels would an atom of Boron have?
a)
1
b)
2
c)
3
d)
4
12.
How many valence electrons would an atom of Oxygen have?
a)
3
b)
6
c)
8
d)
16
13.
Which elements have the most similar chemical properties?
a)
K and Na
b)
K and Ca
c)
K and Cl
d)
K and S
14.
How many electron shells/levels does this atom have?
a)
1
b)
2
c)
3
d)
4
15.
An element is a
a)
pure substance
b)
compound
c)
mixture
d)
molecule
16.
Which of the following is not a compound?
a)
HCl
b)
Cl
c)
NaCl
d)
CO2
17.
Type of bond in which electrons are shared
a)
Ionic
b)
Covalent
c)
Hydrogen
d)
Metallic
18.
Type of bond in which electrons are transferred
a)
Hydrogen
b)
Ionic
c)
Covalent
d)
Metallic
19.
This type of bond forms between a metal and nonmetal
a)
Covalent
b)
Ionic
c)
Hydrogen
d)
Metallic
20.
Occurs between two atoms of the same or different NONMETAL
a)
Ionic
b)
Covalent
c)
Hydrogen
d)
Metallic
21.
What does the number 37 represent in Chlorine-37?
a)
Atomic number
b)
Mass number
c)
Number of protons
d)
Number of neutrons
22.
What is the charge of a cation
a)
positive
b)
negative
c)
neutral
23.
____ tend to form anions
a)
Nonmetals
b)
Metals
c)
Isotopes
24.
If Aluminum loses 3 electrons, what will its charge be?
a)
Neutral
b)
-3
c)
+3
d)
+8
25.
Ag--110 and Ag--112 are two forms of silver with different mass # so they are
a)
compounds
b)
isotopes
c)
orbitals
d)
neutrons
26.
Lithium with atomic # 3 and mass number of 7 has how many neutrons?
a)
3
b)
4
c)
10
d)
7
27.
Isotopes are atoms of the same element that have different
a)
number of electrons
b)
charges
c)
atomic numbers
d)
masses
28.
An element has two naturally occurring isotopes. One is 10.013 amu and is 19.9% abundant. The other is 11.01 amu and is 80.1% abundant. What is the average atomic mass? What element is it?
a)
9.012, Beryllium
b)
12.011, Carbon
c)
6.941, Lithium
d)
10.812, Boron
29.
The electronic configuration of the 7N3- ion is
a)
1s2 2s2 2p3
b)
1s2 2s2 2p6
c)
1s2 2s2 2p3 2p6 3s2 3p2
d)
1s2 2s2 2p3 2p6 3s2 3p6
30.
Iron has a proton number of 26. What is the electronic configuration of Fe2+?
a)
[Ar] 4s2 3d6
b)
[Ar] 3d6
c)
[Ar] 4s2 3d4
d)
[Ar] 4s2 3d5
31.
Electrons in the outermost orbital.
a)
Protons
b)
Neutrons
c)
Valence Electrons
d)
Isotopes
32.
Group on the periodic table that is naturally stable and does not react with other elements.
a)
Noble Gases
b)
Alkali Metals
c)
Alkaline Earth Metals
d)
Halogens
33.
The atoms along the staircase are called
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
34.
Elements on the right side of the of the zigzag line are normally?
a)
non metals
b)
metals
c)
metalloids
d)
rare earth metals
35.
What period and group is Silver (Ag)?
a)
Period 2, Group 1
b)
Period 3, Group 16
c)
Period 5, Group 11
d)
Period 2, 14
36.
The charge on an ion is
a)
always positive.
b)
always negative.
c)
either positive or negative.
d)
zero.
37.
How many protons are present in phosphorus-31
a)
15
b)
16
c)
31
d)
46
38.
The number 27 in the symbol pictured is the element's
a)
mass
b)
atomic number
c)
charge
d)
name
39.
In a correctly written symbol what would be located in the "A" position?
a)
number of neutrons
b)
atomic number
c)
number of electrons
d)
mass number
40.
Changing the number of electrons in an atom changes its...
a)
element type.
b)
charge.
c)
isotope type.
d)
atom type.
41.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
42.
Who came up with this model of an atom?
a)
J.J. Thompson
b)
Ernest Rutherford
c)
Neils Bohr
d)
James Chadwick
43.
Which orbital has the least amount of energy?
a)
p orbital
b)
d orbital
c)
s orbital
d)
What is an orbital?
44.
How many total electrons can the f orbitals in a sublevel hold?
a)
2
b)
14
c)
6
d)
10
45.
What is the maximum number of electrons that an orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
46.
What is the maximum number of electrons that can be on the p sublevel?
a)
6
b)
3
c)
2
d)
4
47.
There are 4 different types of sublevels: s,p,d,f
a)
true
b)
false
48.
Gaining or losing electrons in an atom changes its...
a)
element type.
b)
charge.
c)
isotope type.
d)
atom type.
49.
This is the correct dot diagram for sodium (Na)
a)
true
b)
false
50.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
51.
This is the correct dot diagram for nitrogen (N)
a)
true
b)
false
52.
This is a correct dot diagram for neon (Ne)
a)
true
b)
false
53.
What element is this?
a)
Helium
b)
Hydrogen
c)
Argon
d)
Silver
54.
What element is represented in this Bohr Model?
a)
Carbon
b)
Hydrogen
c)
Aluminum
d)
Lithium
55.
How many valence electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
56.
Horizontal rows on the periodic table are called?
a)
Columns
b)
Periods
c)
Families
57.
The yellow atoms are called
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
58.
The period for Bromine is ___________.
a)
3
b)
2
c)
4
59.
Beryllium is in group number______.
a)
Group 2
b)
Group 3
c)
Group 4
d)
Group 7
60.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
61.
How many unpaired electrons would lithium have?
a)
1
b)
2
c)
3
d)
0
62.
How many half-filled orbitals would silicon contain?
a)
0
b)
2
c)
1
d)
3
63.
Which element would have zero half-filled orbitals?
a)
potassium
b)
copper
c)
magnesium
d)
oxygen
64.
Which element would have 5 half-filled orbitals?
a)
sodium
b)
manganese
c)
sulfur
d)
uranium
65.
What is the correct configuration for uranium?
a)
[Xe] 6s2 4d 3
b)
[Rn] 7s2 5f3
c)
[Rn] 7s2 6d1 5f3
d)
[Rn] 7s2 6d1 6f3
66.
What is the correct configuration for lead?
a)
[Rn] 6s2 5d10 4f14 6p2
b)
[Xe] 6s2 6d10 6p2
c)
[Xe] 6s2 5d10 6p2
d)
[Xe] 6s2 5d10 4f14 6p2
67.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There is nothing incorrect with this diagram
c)
In the 2p box there should only be 1 electron in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
68.
This orbital diagram represents:
a)
C
b)
B
c)
N
d)
O
69.
What do you start an electron configuration with?
a)
1s2
b)
1d10
c)
1f14
d)
1p6
70.
Identify the Noble Gas Shorthand notation for Barium (Ba)
a)
[Xe] 5s1
b)
[Xe] 6s2
c)
[Rn] 6s-10
71.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
72.
What noble gas should be used to write the shorthand configuration for Te?
a)
Ar
b)
Kr
c)
Xe
d)
Sb
73.
Electron arrangement that uses arrows
a)
Electron configuration
b)
Shorthand configuration
c)
Lewis dot structure
d)
Orbital diagram
74.
The electron configuration of an atom is 1s22s22p6. The number of electrons in the atom is
a)
3
b)
6
c)
8
d)
10
75.
What is the electron configuration for this atom?
a)
1s22s22p6
b)
1s22s22p5
c)
1s22s22p3
d)
2s22p3
76.
What is this element?
[Ne] 3s23p64s2
[Ne] 3s23p64s2
a)
Calcium
b)
Sodium
c)
Scandium
d)
Titanium
77.
An element has two naturally occurring isotopes. One is 10.013 amu and is 19.9% abundant. The other is 11.01 amu and is 80.1% abundant. What is the average atomic mass? What element is it?
a)
9.012, Beryllium
b)
12.011, Carbon
c)
6.941, Lithium
d)
10.812, Boron
78.
Nitrogen has three occurring isotopes: Nitrogen-13, Nitrogen-14, Nitrogen-15. Which isotope is the most abundant?
a)
Nitrogen-13
b)
Nitrogen-14
c)
Nitrogen-15
d)
Based on the information given, it cannot be determined
79.
Do the following atoms belong to the same element? Explain
Aluminum-27
An atom with 14 protons and 13 neutrons
Aluminum-27
An atom with 14 protons and 13 neutrons
a)
Yes because they have the same number of protons
b)
Yes because they have the same mass
c)
No because they have different number of protons
d)
No because they have different number of neutrons
80.
Calculate the average atomic mass of silver.
a)
106.38649amu
b)
111.91896amu
c)
107.8677amu
d)
121
81.
Calculate the average atomic mass of silver.
a)
106.38649amu
b)
111.91896amu
c)
107.8677amu
d)
121
82.
Complete the missing label on the diagram.
a)
Neutron
b)
Centre
c)
Nucleus
d)
Sub atomic particle
83.
What is the average atomic mass of this element?
Mass Abundance
49.946050 4.345%
51.940512 83.789%
52.940654 9.501%
53.938885 2.365%
Mass Abundance
49.946050 4.345%
51.940512 83.789%
52.940654 9.501%
53.938885 2.365%
a)
51.9961376
b)
71.5275405
c)
52.0176462
d)
51.9959724
84.
What is the average atomic mass of this element?
Mass Abundance
62.929601 69.17%
64.927794 30.83%
Mass Abundance
62.929601 69.17%
64.927794 30.83%
a)
63.5456439
b)
63.9286975
c)
64.8482257
d)
62.0215955
85.
What is the average atomic mass of this element?
Mass Abundance
62.929601 69.17%
64.927794 30.83%
Mass Abundance
62.929601 69.17%
64.927794 30.83%
a)
63.5456439
b)
63.9286975
c)
64.8482257
d)
62.0215955
86.
What is the average atomic mass of this element?
Mass Abundance
68.925581 60.108%
70.924705 39.892%
Mass Abundance
68.925581 60.108%
70.924705 39.892%
a)
69.7230715
b)
69.925143
c)
70.005438
d)
68.8897
87.
How many neutrons does the isotope below have? 89 36Kr
a)
53
b)
36
c)
89
d)
125
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