NEW
Font size
S
M
L
XL
WorksheetsElectron Configuration and Ionic Bonding Review
Total questions: 50
Worksheet time: 50mins
Name
Class
Date
1.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
2.
Which of the following statements is true about the 3s and the 4s sublevels?
a)
These sublevels have the same energy
b)
These sublevels are the same distance from the nucleus
c)
These sublevels hold different amounts of electrons
d)
These sublevels have the same shape
3.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
4.
Hund’s rule states…
a)
Atomic orbitals have opposite spins and 2 electrons each
b)
Electrons occupy orbitals of highest energy first and energy level changes as you go up
c)
Electrons occupy orbitals of lowest energy first, starting with 1s
d)
Electrons occupy orbitals of equal energy, one electron enters EACH orbital ONE AT A TIME until orbitals of the entire energy level have one electron with the SAME SPIN.
5.
What is the Pauli Exclusion Principle?
a)
An atomic orbital can only hold a maximum of 2 electrons, each with opposite spins
b)
An atomic orbital can hold a minimum of 6 electrons, each with opposite spins
c)
An atomic orbital can hold a maximum of 6 electrons, each with the same spin
d)
An atomic orbital can hold a minimum of 2 electrons, each with opposite spins
6.
How many electrons can a d sublevel hold?
a)
14
b)
10
c)
2
d)
6
7.
The maximum number of electrons that can fit into the 2nd energy level is
a)
2
b)
8
c)
18
d)
32
8.
Region of high probability of finding an electron
a)
atomic orbital
b)
ground state
c)
Heisenberg uncertainty principle
d)
electron configuration
9.
The electrons that are on the outer most region of the atom
a)
Shell Electrons
b)
Violent Electrons
c)
Valence Electrons
10.
The different energy levels of electrons as they orbit the nucleus
a)
Electron Cloud
b)
Orbitals (Energy Levels)
c)
2, 8, 18, 32
11.
Alkali metals are located where on the periodic table?
a)
Group 1
b)
Group 8 and Period 4
c)
Period 7
12.
Alkaline Earth Metals...
a)
are semiconductors
b)
are the most reactive type of elements
c)
have two valence electrons
13.
What atom matches this electron configuration?
1s22s22p63s2
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
14.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
15.
The electron configuration of an atom is 1s22s22p6. The number of electrons in the atom is
a)
3
b)
6
c)
8
d)
10
16.
What do you start electron configuration with?
a)
1s2
b)
1d10
c)
1f14
d)
1p6
17.
There are 4 different types of subshells s,p,d,f
a)
true
b)
false
18.
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
19.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
20.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
21.
How many p orbitals are there in a sublevel?
a)
2
b)
1
c)
4
d)
3
22.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
23.
Electron arrangement that uses arrows
a)
Electron configuration
b)
Shorthand configuration
c)
Lewis dot structure
d)
Orbital diagram
24.
This orbital diagram represents:
a)
C
b)
B
c)
N
d)
O
25.
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.
26.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
27.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
28.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
29.
Which orbital shows a violation of the Aufbau Principle?
a)
A
b)
B
c)
C
d)
D
30.
As you move down the periodic table atoms get bigger. This is because ____________.
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
31.
Electronegativity is...
a)
the ability of an atom to attract/ accept 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.
32.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
33.
Metals tend to
a)
gain electrons
b)
lose electrons
34.
Nonmetals tend to
a)
gain electrons
b)
lose electrons
35.
If I gain electrons I become
a)
Positive because I've added to my atom
b)
negative because I've added electrons
c)
same because i'm balanced
d)
equal because now I have electrons
36.
When metals bond with non-metals they form what type of bonds
a)
covalent
b)
ionic
c)
cooperative
d)
lewis
37.
How do the following two elements bond together?
Cr3+ O2-
Cr3+ O2-
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
38.
AgF
a)
silver fluoride
b)
silver fluorine
c)
monosilver monofluoride
d)
silver monofluorine
39.
When a nonmetal gains electrons, it becomes this type of ion.
a)
Anion
b)
Cation
40.
When a metal loses electrons, it becomes this type of ion.
a)
anion
b)
cation
41.
Which of the following combinations would need roman numerals in the name?
a)
potassium + fluorine
b)
beryllium + oxygen
c)
boron + iodine
d)
silver + oxygen
42.
Name the following ionic compound: Cr(NO2)3
a)
chromium nitrite
b)
chromium nitride
c)
chromium III nitride
d)
chromium III nitrite
43.
Which of the following is NOT an ionic compound:
a)
CaO
b)
NaOH
c)
BaCl2
d)
Br2
44.
How many valence electrons does a bromine atom have?
a)
1
b)
2
c)
6
d)
7
45.
What is the correct formula for the compound, lithium oxide?
a)
LiO
b)
Li2O
c)
LiO2
d)
Li2O2
46.
LiBr is called
a)
lithium bromine
b)
lithium (I) bromine
c)
lithium bromide
d)
lithuim (I) bromide
47.
When naming ionic compounds you always write the name of the positive element _______ .
a)
first
b)
second
c)
with "ide"
d)
with a prefix
48.
In most cases, when naming you change the ending of the second element to ________.
a)
-ate.
b)
-ite.
c)
-ide.
d)
-ine.
49.
If my charge becomes 2+ what does that say about me?
a)
I am stealing 2 electrons
b)
I am losing 2 electrons
c)
I am in period 2
d)
I have an atomic # of 2
50.
What is the charge of copper in the compound: CuBr2
a)
+1
b)
+2
c)
-1
d)
-2
Reset
