stud
bud
Sign up
Log in
Home
Library
Explore
SAT
More
Ionisation Energy in the Periodic Table Flashcards | StudBud
Explore
/
Ionisation Energy in the Periodic Table
Ionisation Energy in the Periodic Table
10 terms
·
StudBud Administration
·
60 plays
A quick test of your general knowledge
Flashcards
10 cards
F
Practice quiz
P
Host live
L
Questions
10
Answers
1
Which of the following best explains why ionisation energy decreases down a group?
None of the above
Electrons are further away and require less energy to remove
Electrons are closer and require more energy to remove
Because electrons are closer to the nucleus.
2
What is the definition of ionisation energy?
The energy required to add an electron
The energy required to remove an electron
The amount of energy to attract or bond an electron
None of the above are correct
3
Which has the set of elements has the element with the highest ionisation energy?
N, Xe, Rn, Fr
Al, Si, Ge, F, N, K
N, O, C, H, S
Mg, Ca, Be, B, N
4
Mg, Be, Ca, Sr are all in the same __________.
Period
Group
5
Ionisation increases down a group because the number of protons increases?
False
True
6
Which of the following elements has the lowest ionisation energy?
Sodium (Na)
Lithium (Li)
Rubidium (Rb)
Cesium (Cs)
7
Which of the following elements is in period 6 and group 4?
Hf
Zr
Ge
C
8
Order the elements in decreasing ionisation energy. Na, S, Al, F, K, O
Al, O, K, F, S, Na
Na, S, F, K, O, Al
K, Na, Al, S, O, F
F, O, S, Al, Na, K
9
True or false. There are 18 periods and 7 groups.
False
True
10
Which of the following has the largest ionisation energy?
Al
P
Si
N
