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AS Skills 4 Ionisation energies Flashcards | StudBud
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AS Skills 4 Ionisation energies
AS Skills 4 Ionisation energies
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1
Why is the second ionisation energy of an atom always greater than the first? *click two that apply*
the second ionisation energy removes electrons from the 2+ ion
Fewer electrons, so less electron repulsion
the second ionisation energy removes electrons from the 1+ ion
Fewer electrons, so more electron repulsion
2
*Find the Falsie*
Why is the second ionisation energy of sodium much greater than the first?
The 2nd IE goes into a new shell
1st electron removed is 2p6 second electron removed is 3s1
The 2nd IE takes an electron from an increasingly positive ion
1st electron removed is 3s1 second electron removed is 2p6
3
What is the mostly likely formula of the oxide that forms when
X
burns in oxygen (if Oxygen forms a O
2-
Oxide ion)?
XO2 (X is in group 4)
X2O3 (X is in group 3)
X2O (X is in group 1)
XO (X is in group 2)
4
*Find the Falsie*
Why are anions always smaller than the corresponding atoms?
because they have more repulsion
because they have fewer protons
because they have more electrons
5
*Find the Falsie*
Why are cations always smaller than the corresponding atoms?
because they have a smaller atomic radius
because they have less repulsion
because they have more protons
because they have fewer electrons
6
*Find the Falsie*
Why do all successive ionisation energies increase?
the atomic radius is getting smaller
less repulsion is being experienced between electrons
electrons are being removed from increasingly positive ions
electrons are being removed from increasingly negative ions
7
What is the trend shown in all successive ionisation energies?
They generally decrease
They always decrease
They always increase
They generally increase
8
Why does helium have the highest first ionisation energy of all the elements?
Increased shielding, but its electrons are held by a lot of protons
No shielding, so its electrons are closely held by two protons
Decreased shielding, and its electrons are held by a lot of protons
Increased shielding, but its electrons are closely held by two protons
9
What group is J in?
Group 4
Group 3
Group 2
Group 1
10
Which element has the highest First ionisation energy of all the elements?
Cesium
Neon
Hydrogen
Helium
11
If J formed a compound with chlorine, what would its formula be? (use your GCSE chemistry)
JCl4
JCl3
JCl2
JCl
12
Why is the first ionisation energy of Boron (800 KJ mol
-1
) less than that of Beryllium(900 KJ mol
-1
)?
B's 1st electron is the 2p subshell, which is higher energy than 2s subshel
Boron has more protons in its nucleus
Beryllium has more protons in its nucleus
Be's 1st electron is the 2s subshell, which is higher energy than 2p subshe
13
Why do first ionisation energies decrease down a group?
No. protons increases, No. shells increases, Shielding/Repulsion decrease
No. protons increases, No. shells increases, Shielding/Repulsion increase
No. protons decreases, No. shells increases, Shielding/Repulsion increase
Number of protons increases, shielding stays the same
14
Why is the first ionisation energy of Oxygen (1314 KJ mol
-1
) less than that of Nitrogen (1402 KJ mol
-1
)?
There is more repulsion in the 2px orbital in O
Oxygen has more protons in its nucleus
N's 5th electron is the 2p subshell
Nitrogen has more protons in its nucleus
15
Why does the first ionisation energy of atoms generally increase across a period?
Number of protons increases, shielding stays the same
Number of protons decreases, stays the same
Number of protons decreases, shielding decreases
Number of protons increases, shielding increases
16
Which pair of elements has
the second element having a bigger 1st ionisation energy
than the first element?
A Al>Mg
D Na>K
B O>N
C Ne>Na
