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IONIZATION ENERGY TRENDS
Test Description: Practice ionization energy trends
Instructions: Answer all questions to get your test result.
1) Ionization energy increases down a group because the number of protons increases and it's more difficult to lose electrons because they are being pulled closer.
A
True
B
False
2) Which of the following has the largest ionization energy?
A
Si
B
Al
C
N
D
P
3) Which of the following elements has the lowest ionization energy?
A
Cesium (Cs)
B
Lithium (Li)
C
Sodium (Na)
D
Rubidium (Rb)
4) Order the elements in decreasing ionization energy. Na, S, Al, F, K, O
A
Al, O, K, F, S, Na
B
F, O, S, Al, Na, K
C
Na, S, F, K, O, Al
D
K, Na, Al, S, O, F
5) What is the definition of ionization energy?
A
The energy required to add an electron
B
None of the above are correct
C
The energy required to remove an electron
D
The amount of energy to attract or bond an electron
6) Which of the following best explains why ionization energy decreases down a group?
A
Ionization energy decreases because electrons are further away and require less energy to remove.
B
Ionization energy decreases because electrons are closer and require more energy to remove.
C
None of the above.
D
Ionization energy increases, because electrons are closer to the nucleus.
7) Which has the set of elements has the element with the highest ionization energy?
A
Mg, Ca, Be, B, N
B
Al, Si, Ge, F, N, K
C
N, Xe, Rn, Fr
D
N, O, C, H, S
8) Mg, Be, Ca, Sr are all in the same __________.
A
Group
B
Period
9) True or false. There are 18 periods and 7 groups.
A
True
B
False
10) Which of the following elements is in period 6 and group 4?
A
Hf
B
C
C
Ge
D
Zr
*select an answer for all questions
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