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WorksheetsElectrons Quiz Review
Total questions: 60
Worksheet time: 56mins
Name
Class
Date
1.
Adding or subtracting neutrons (charge = 0, mass = 1) makes the element change into an...
a)
ion
b)
mixture
c)
isotope
d)
neutral atom
2.
The atomic number is equal to _.
a)
the number of protons and electrons
b)
the number of neutrons only
c)
the total number of protons and neutrons
d)
the number of protons neutrons and electrons
3.
What is the charge on a lithium atom that looses 1 electron?
a)
+1
b)
0
c)
-1
d)
-2
4.
Helium (He atomic number 2) has 2 protons, 2 neutrons, and 2 electrons) is the He element shown above an atom, an element, or an isotope?
a)
atom
b)
cation (+ ion)
c)
isotope
d)
anion (-)
5.
What is the net charge on the element shown above?
(Calcium - atomic number 20)
(Calcium - atomic number 20)
a)
cation +1 charge
b)
cation +2 charge
c)
anion -1 charge
d)
anion -2 charge
6.
How many protons does this isotope of titanium have? Hint titanium has an atomic number of 22.
a)
48
b)
22
c)
26
d)
70
7.
What is an ion?
a)
A Charged Atom
b)
A Large Atom
c)
A Small Atom
d)
A Cute Atom
8.
Barium atoms want to form...
a)
an anion
b)
a cation
c)
an onion
d)
a cuddly kitten friend
9.
Why are ions formed?
a)
To make our lives difficult
b)
Because atoms want 8 valence electrons
c)
Because atoms have the same number of protons and electrons
d)
Because atoms gained neutrons
10.
Cations are...
a)
Positive
b)
Negative
c)
Neutral
d)
Purring
11.
Anions are...
a)
Positive
b)
Negative
c)
Neutral
d)
Crying
12.
An atom becomes _________ when it gains electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
13.
An atom becomes _______ when it loses electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
14.
A Silicon atom wants...
a)
3 more electrons
b)
3 less electrons
c)
4 more or less electrons
d)
2 more electrons
15.
A Radium atom wants...
a)
One more electron
b)
One less electron
c)
Two more electrons
d)
Two less electrons
16.
What is a Rubidium ion's symbol?
a)
Rb-
b)
Rb+
c)
Rb-2
d)
Rb+2
17.
What is the ionic symbol for a phosphorus atom?
a)
P-3
b)
P+3
c)
P-2
d)
P+2
18.
What is the ionic symbol for a Gallium atom?
a)
Ga+3
b)
Ga-3
c)
Ga+2
d)
Ga-2
19.
What is the ionic symbol for Selenium?
a)
Se-2
b)
Se+2
c)
Se-3
d)
Se+3
20.
What is the ionic symbol for Krypton?
a)
Kr
b)
Kr+
c)
Kr-
d)
Kr-2
21.
What is the ionic symbol for a Caesium atom?
a)
Cs+
b)
Cs-
c)
Cs+2
d)
Cs-2
22.
What is the charge of a sodium ion?
a)
+2
b)
+1
c)
-1
d)
-2
23.
Group 17 always has ions with a charge of
a)
+1
b)
+2
c)
-1
d)
-2
24.
What charge will an Oxygen ion have?
a)
+1
b)
-1
c)
+2
d)
-2
25.
If an element has 3 valence electrons, what charge will likely form on its ion ?
a)
+3
b)
+5
c)
-3
d)
-5
26.
Which of the following has a -3 charge?
a)
Boron
b)
Fluorine
c)
Nitrogen
d)
Neon
27.
charge of lithium ion
a)
-2
b)
-1
c)
+1
d)
+2
28.
charge of beryllium ion
a)
-2
b)
-1
c)
+1
d)
+2
29.
Which of the following has a -1 charge?
a)
Aluminum
b)
Bromine
c)
Calcium
d)
Potassium
30.
Elements on the LEFT side of the periodic table will most likely form:
a)
Positive ions
b)
Negative ions
c)
Neutral Ions
d)
None of these
31.
Valence electrons are
a)
outer shell electrons
b)
electrons involved in reactions
c)
s and p orbital electrons
d)
all of these
32.
Which of the following atoms is an anion?
a)
Na
b)
Mg
c)
Al
d)
Si
33.
Nonmetals are
a)
usually cations
b)
likely to lose electrons
c)
usually negative ions
d)
all of these
34.
A +2 ion will
a)
likely be a nonmetal
b)
add 2 electrons
c)
gain electrons
d)
subtract 2 electrons
35.
If an atom has the configuration of 1s2 2s2 2p6 3s1 the atom will probably
a)
gain 1 electron
b)
lose 1 electron
c)
fill the 3p orbital
d)
lose the 2p orbital
36.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
37.
What atom matches this electron configuration?
1s22s22p63s2
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
38.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
39.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
40.
The electron configuration of an atom is 1s22s22p6. The number of electrons in the atom is
a)
3
b)
6
c)
8
d)
10
41.
What do you start electron configuration with?
a)
1s2
b)
1d10
c)
1f14
d)
1p6
42.
What is this element?
1s22s22p63s2
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
43.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
44.
There are 4 different types of subshells s,p,d,f
a)
true
b)
false
45.
Which electron configuration belongs to Copper (Cu)?
a)
1s2 2s2 2p6 3s2 3p6 4s2 3d8
b)
1s2 2s2 2p6 3s2 3p6 4s2 3d9
c)
1s2 2s2 2p6 3s2 3p6 4s2 3d10
46.
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
47.
What is the noble gas configuration for beryllium?
a)
[He]1s2
b)
[He]2s2
c)
[Li]2s1
d)
[Li]2s2
48.
What is the noble gas configuration for boron?
a)
[He]1s22s2
b)
[He]2s22p2
c)
[He]2s22p1
d)
[Li]2s22p1
49.
What is the noble gas configuration for Sulfur?
a)
[Ar] 3p4
b)
[He] 3s2 3p4
c)
[Ne] 3s2 3p4
d)
[Na] 3s2 3p4
50.
What is the noble gas configuration for phosphorus?
a)
[Ar] 3p5
b)
[He] 3s2 3p5
c)
[Ne] 3s2 3p3
d)
[Na] 3s2 3p5
51.
[He]2s22p4 is the noble gas configuration for which element?
a)
oxygen
b)
sulfur
c)
phosphorus
d)
fluorine
52.
This orbital diagram represents:
a)
C
b)
B
c)
N
d)
O
53.
This orbital diagram represents:
a)
C
b)
B
c)
N
d)
O
54.
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 there should only be 1 orbital in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
55.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
56.
How many electrons can the s sublevel hold?
a)
14
b)
10
c)
2
d)
6
57.
How many electrons can the p sublevel hold?
a)
14
b)
10
c)
2
d)
6
58.
[Ne]3s23p1 is the noble gas configuration for which element?
a)
scandium
b)
boron
c)
nitrogen
d)
aluminum
59.
An electron occupies the lowest energy orbital that can receive it.
a)
Hund’s rule
b)
Pauli exclusion principle
c)
Bohr model of the atom
d)
Aufbau principle
60.
This orbital diagram represents:
a)
C
b)
B
c)
N
d)
O
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