IB Chemistry on Ionization energy and electron configuration
1. Periodic Table of elements – divided into s, p, d, f blocks
s block
• s orbitals partially fill
d block
• d orbitals partially filled
• transition elements
f block
• f orbital partially fill
p block
• p orbital partially fill
2. s block elements
• s orbitals partially fill
1
H
He
p block elements
• p orbital partially fill
5
1s2
n = 2 period 2
B
[He] 2s2 2p1
6
1s1
2
Periodic Table – s, p d, f blocks elements
C
[He] 2s2 2p2
7
N
[He] 2s2 2p3
3
Li
[He] 2s1
8
O
[He] 2s2 2p4
4
Be
[He] 2s2
9
F
[He] 2s2 2p5
11
Na
[Ne] 3s1
10
Ne
[He] 2s2 2p6
12
Mg
[Ne] 3s2
13
Al
[Ne] 3s2 3p1
14
20
K
Ca
[Ne] 3s2 3p2
[Ar]
15
P
[Ne] 3s2 3p3
[Ar]
4s2
16
S
[Ne] 3s2 3p4
17
19
Si
4s1
CI
[Ne] 3s2 3p5
18
Ar
[Ne] 3s2 3p6
d block elements
• d orbitals partially fill
• transition elements
21
Sc
[Ar] 4s2 3d1
22
Ti
[Ar] 4s2 3d2
23
V
[Ar] 4s2 3d13
24
Cr
[Ar] 4s1 3d5
25
Mn
[Ar] 4s2 3d5
26
Fe
[Ar] 4s2 3d6
27
Co
[Ar] 4s2 3d7
28
Ni
[Ar] 4s2 3d8
29
Cu
[Ar] 4s1 3d10
30
Zn
[Ar] 4s2 3d10
f block elements
• f orbitals partially fill
Video on electron configuration
Click here electron structure
Click here video on s,p,d,f notation
Click here video s,p,d,f blocks,
3. Periodic Table – s, p d, f blocks elements
Electron structure
Chromium d block (Period 4)
Electron structure
Germanium p block, Gp 4 (Period 4)
1s2 2s2 2p6 3s2 3p6 4s1 3d5
[Ar] 4s1 3d5
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2
[Ar] 4s2 3d10 4p2
d block – d partially filled
Electron structure
Iodine p block, Gp 7 (Period 5)
1s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10 5p5
[Kr] 5s2 4d10 5p5
Gp 4 -4 valence electron
Gp 7 - 7 valence electron
Ge
Cr
I
Cd
Hg
Electron structure
Cadmium d block (Period 5)
1s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10
[Kr] 5s2 4d10
d block – d partially filled
Pb
Electron structure
Mercury d block (Period 6)
1s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10 5p6 6s2 4f14 5d10
[Xe] 6s2 4f14 5d10
d block – d partially filled
Electron structure
Lead p block, Gp 4 (Period 6)
1s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10 5p6 6s2 4f14 5d106p2
[Xe] 6s2 4f14 5d10 6p2
Gp 4 -4 valence electron
4. Electron filled according to 3 Principles
1
Aufbau Principle
• electron occupy orbitals of lower energy first
• building up, construction from bottom up
4Be
High energy
- 1s2 2s2
5B
- 1s2 2s2 2p1
2p
2p
2s
2s
Click here to view simulation
1s
1s
lower energy
2
Hund’s Principle
• electron occupy orbitals singly first before pairing up
7N
High energy
- 1s2 2s2 2p3
8O
- 1s2 2s2 2p4
2p
2s
Click here to view simulation
1s
3
lower energy
Pauli Exclusion Principle
• each orbital occupy by 2 electron opposite spin
4Be
- 1s2 2s2
High energy
10Ne
- 1s2 2s2 2p6
Click here to view simulation
lower energy
5. Electron Notation
Atom
Positive/Negative Ion
s, p, d, f notation
Complete configuration
Noble gas notation
Condensed configuration
Noble gas notation
Complete configuration
10
Ne
1s2 2s2 2p6
10
Ne
[Ne]
10
Ne
1s2 2s2 2p6 /[Ne]
11
Na
1s2 2s2 2p6 3s1
11
Na
[Ne] 3s1
11
Na+
1s2 2s2 2p6 / [Ne]
12
Mg
1s2 2s2 2p6 3s2
12
Mg
[Ne] 3s2
12
Mg2+
1s2 2s2 2p6 / [Ne]
13
Al
1s2 2s2 2p6 3s2 3p1
13
Al
[Ne] 3s2 3p1
13
Al3+
1s2 2s2 2p6 / [Ne]
14
Si
1s2 2s2 2p6 3s2 3p2
14
Si
[Ne] 3s2 3p2
14
Si4+
1s2 2s2 2p6 / [Ne]
15
P
1s2 2s2 2p6 3s2 3p3
15
P
[Ne] 3s2 3p3
15
P3-
1s2 2s2 2p6 3s2 3p6 /[Ar]
16
S
1s2 2s2 2p6 3s2 3p4
16
S
[Ne] 3s2 3p4
16
S2-
1s2 2s2 2p6 3s2 3p6 /[Ar]
17
CI
1s2 2s2 2p6 3s2 3p5
17
CI
[Ne] 3s2 3p5
17
CI-
1s2 2s2 2p6 3s2 3p6/ [Ar]
18
Ar
1s2 2s2 2p6 3s2 3p6
18
Ar
[Ar]
19
[Ne]
18
Ar
[Ar]
K
[Ar]
4s1
19
K+
1s2 2s2 2p6 3s2 3p6 /[Ar]
20
Ca
[Ar] 4s2
20
Ca2+
1s2 2s2 2p6 3s2 3p6 / [Ar]
21
Sc
[Ar] 4s2 3d1
22
Ti
[Ar] 4s2 3d2
1s2 2s2 2p6 3s2 3p6 4s2 3d3
23
V
[Ar] 4s2 3d3
Cr
1s2 2s2 2p6 3s2 3p6 4s1 3d5
24
Cr
[Ar] 4s1 3d5
25
Mn
1s2 2s2 2p6 3s2 3p6 4s2 3d5
25
Mn
[Ar] 4s2 3d5
26
Fe
1s2 2s2 2p6 3s2 3p6 4s2 3d6
26
Fe
[Ar] 4s2 3d6
27
Co
1s2 2s2 2p6 3s2 3p6 4s2 3d7
27
Co
[Ar] 4s2 3d7
28
Ni
1s2 2s2 2p6 3s2 3p6 4s2 3d8
28
Ni
[Ar] 4s2 3d8
29
Cu
1s2 2s2 2p6 3s2 3p6 4s1 3d10
29
Cu
[Ar] 4s1 3d10
30
Zn
1s2 2s2 2p6 3s2 3p6 4s2 3d10
30
Zn
[Ar] 4s2 3d10
K
1s2
2s2
2p6
3s2
3p6 4s1
19
20
Ca
1s2 2s2 2p6 3s2 3p6 4s2
21
Sc
1s2 2s2 2p6 3s2 3p6 4s2 3d1
22
Ti
1s2 2s2 2p6 3s2 3p6 4s2 3d2
23
V
24
[Ar]
6. Electron configuration
5
B
1s2 2s2 2p1
6
C
1s2 2s2 2p2
7
N
1s2 2s2 2p3
8
O
1s2 2s2 2p4
9
F
1s2 2s2 2p5
10
Ne
1s2 2s2 2p6
11
Na
1s2 2s2 2p6 3s1
12
Mg
1s2 2s2 2p6 3s2
13
Al
1s2 2s2 2p6 3s2 3p1
14
Si
1s2
15
P
1s2 2s2 2p6 3s2 3p3
16
S
1s2 2s2 2p6 3s2 3p4
17
CI
1s2
18
Ar
1s2 2s2 2p6 3s2 3p6
19
K
1s2
20
Ca
1s2 2s2 2p6 3s2 3p6 4s2
21
Sc
1s2 2s2 2p6 3s2 3p6 4s2 3d1
22
Ti
1s2 2s2 2p6 3s2 3p6 4s2 3d2
23
V
1s2 2s2 2p6 3s2 3p6 4s2 3d3
24
Cr
1s2 2s2 2p6 3s2 3p6 4s1 3d5
25
Mn
1s2 2s2 2p6 3s2 3p6 4s2 3d5
26
Fe
1s2 2s2 2p6 3s2 3p6 4s2 3d6
27
Co
1s2 2s2 2p6 3s2 3p6 4s2 3d7
28
Ni
1s2 2s2 2p6 3s2 3p6 4s2 3d8
29
Cu
1s2 2s2 2p6 3s2 3p6 4s1 3d10
30
Zn
Electron occupy 4s first then 3d
Energy level and sublevels
1s2 2s2 2p6 3s2 3p6 4s2 3d10
2s2
2s2
2s2
2p6
2p6
2p6
4s energy level lower than 3d
3s2
3s2
3s2
4s
3d
3p
3p2
3s
18Ar
– 1s2 2s2 2p6 3s2 3p6
2p
2s
3p5
3p6 4s1
Electrons fill 4s first
3d
4s
1s
3p
19K
– 1s2 2s2 2p6 3s2 3p6 4s1
3s
4s then 3d is fill
2p
3d
2s
4s
1s
21Sc
3p
3s
– 1s2 2s2 2p6 3s2 3p6 4s2 3d1
2p
2s
1s
7. d block
Exception to d block elements
4s energy level lower than 3d
3d
4s
3p
Electron configuration d block
3s
21
Sc
1s2 2s2 2p6 3s2 3p6 4s2 3d1
22
Ti
V
1s2 2s2 2p6 3s2 3p6 4s2 3d3
24
Cr
1s2
25
Mn
1s2 2s2 2p6 3s2 3p6 4s2 3d5
26
Fe
1s2 2s2 2p6 3s2 3p6 4s2 3d6
27
Co
Ni
1s2 2s2 2p6 3s2 3p6 4s2 3d8
29
Cu
1s2 2s2 2p6 3s2 3p6 4s1 3d10
30
Zn
1s2 2s2 2p6 3s2 3p6 4s2 3d10
2s2
2p6
3s2
3p6 4s1
3d5
4s energy level lower than 3d
2p
1s2 2s2 2p6 3s2 3p6 4s2 3d7
28
– 1s2 2s2 2p6 3s2 3p6 4s2 3d1
1s2 2s2 2p6 3s2 3p6 4s2 3d2
23
21Sc
2s
1s
24Cr
– 1s2 2s2 2p6 3s2 3p6 4s13d5
24Cr
– 1s2 2s2 2p6 3s2 3p6 4s2 3d4
3d
✔
4s
3p
3s
✗
Half fill energetically more stable
2p
2s
1s
29Cu
29Cu
–1s2 2s2 2p6 3s2 3p6 4s1 3d10
–1s2 2s2 2p6 3s2 3p6 4s2 3d9
✔
✗
4s
3p
3s
Half fill energetically more stable
2p
2s
1s
3d
8. d block
Exception to d block elements
4s energy level lower than 3d
Noble gas notation
Condensed configuration
Electron configuration d block
Positive Ions
21
Sc
1s2 2s2 2p6 3s2 3p6 4s2 3d1
21
Sc
[Ar] 3d1 4s2
21
Sc3+
[Ar]
22
Ti
1s2 2s2 2p6 3s2 3p6 4s2 3d2
22
Ti
[Ar] 3d2 4s2
22
Ti4+
[Ar]
23
V
1s2 2s2 2p6 3s2 3p6 4s2 3d3
23
V
[Ar] 3d3 4s2
23
V3+
[Ar] 3d2
24
Cr
1s2 2s2 2p6 3s2 3p6 4s1 3d5
24
Cr
[Ar] 3d5 4s1
24
Cr3+
[Ar] 3d3
25
Mn
1s2 2s2 2p6 3s2 3p6 4s2 3d5
25
Mn
[Ar] 3d5 4s2
25
Mn2+
[Ar] 3d5
26
Fe
1s2 2s2 2p6 3s2 3p6 4s2 3d6
26
Fe
[Ar] 3d6 4s2
26
Fe2+
[Ar] 3d6
27
Co
1s2 2s2 2p6 3s2 3p6 4s2 3d7
27
Co
[Ar] 3d7 4s2
27
Co2+
[Ar] 3d7
28
Ni
1s2 2s2 2p6 3s2 3p6 4s2 3d8
28
Ni
[Ar] 3d8 4s2
28
Ni2+
[Ar] 3d8
29
Cu
1s2 2s2 2p6 3s2 3p6 4s1 3d10
29
Cu
[Ar] 3d10 4s1
29
Cu2+
[Ar] 3d9
30
Zn
1s2 2s2 2p6 3s2 3p6 4s2 3d10
30
Zn
[Ar] 3d10 4s2
30
Zn2+
[Ar] 3d10
Why electron fill 4s first?
1
Why electrons lost from 4s first
4s fill first – 4s2
4s – greater penetration/closer to nucleus
4s – lower in energy
3d
2
3d – filled
3d – higher energy
3
4
4s – higher in energy
4s – e lost first
4s
4s
4s
– [Ar] 4s2 3d0
4S – FIRST IN – FIRST OUT
3d once filled
3d e attracted by increasing nuclear charge
3d orbitals lower in energy - shield 4s e
3d
20Ca
Electrons lost from
4s then 3d
21Sc
– [Ar] 4s2 3d1
3d
3d
21Sc
– [Ar] 3d2 4s2
lose 2 electron
21Sc2+ –
[Ar] 3d2 4s0
9. d block
d block elements and ions
4s energy level lower than 3d
Electron configuration d block
Electron lost from 4s then 3d
21
Sc
22
Ti
[Ar] 3d2 4s2
23
V
Cr
25
Mn
[Ar] 3d5 4s2
26
Fe
[Ar] 3d6 4s2
27
Co
28
Ni
[Ar] 3d8 4s2
29
Cu
[Ar] 3d10 4s1
30
Zn
[Ar] 3d10 4s2
3d
3d
4s
4s
lose 2 e
3d
3d
V3+
[Ar] 3d2
24
Cr3+
[Ar] 3d3
Mn2+
[Ar] 3d5
Fe2+
[Ar] 3d6
Co2+
[Ar] 3d7
28
Ni2+
[Ar] 3d8
29
Cu2+
[Ar] 3d9
30
[Ar] 3d7 4s2
lose 3 e
[Ar]
26
4s
Ti4+
25
4s
[Ar]
27
[Ar] 3d5 4s1
3d
Sc3+
23
3d
21
22
lose 3 e
[Ar] 3d3 4s2
24
4s
4s
[Ar] 3d1 4s2
Positive Ions
Zn2+
[Ar] 3d10
Video on Ionization energy
Click here to view IE
Click here to view IE
Click here to view IE
10. Why IE increases across the period?
Why IE decreases down a group ?
Ionization energy (IE)
1st Ionization energy
Min energy to remove 1 mole e from
1 mole of element in gaseous state
M(g) M+ (g) + e
2nd Ionization energy
Min energy to remove 1 mole e from
1 mole of +1 ion to form +2 ion
M+(g) M2+ (g) + e
Ionization energy
Factors affecting ionization energy
1
2
Distance from nucleus
3
Nuclear charge
electron
+3
+4
+5
+6
Effective Nuclear Charge (ENC)/(Zeff)
• Screening effect/shielding
• Effective nuclear charge (ENC)/(Zeff)
(Zeff) = Nuclear charge (Z) – shielding effect
• Net positive charge felt by valence electrons.
Nuclear charge increase
Distance near to nucleus – IE High
Distance far away nucleus – IE Low
Nuclear charge high (more proton) – IE High
Nuclear charge low (less proton) – IE Low
+6
Inner electron – shield valence e from positive charge
Distance near
Nuclear charge
Higher electron/electron repulsion
Strong electrostatic forces
attraction bet nucleus and e
Strong electrostatic forces
attraction bet nucleus and e
Easier valence e to leave
IE – High
IE – High
IE – Low
11. IE drop from Be to B and N to O
Ionization Energy- Period 2
Why IE increases across the period 2?
IE increases across period 2
Nuclear charge increase
Strong electrostatic forces
attraction bet nucleus and e
IE – High
Li
Be
B
C
N
O
F
Ne
2p
2s
1s
1s2 2s1
1s2 2s2
1s2 2s2 2p1
1s2 2s2 2p2
1s2 2s2 2p3
1s2 2s2 2p4
IE drop from Be to B
IE drop from N to O
Electron in p sublevel of B
– further away from nucleus
2 electrons in same p orbital
- Greater e/e repulsion
Weak electrostatic force attraction
between nucleus and electron
Easier to remove e
IE - Low
IE - Low
period 2
1s2 2s2 2p5
1s2 2s2 2p6
12. IE drop from Mg to AI and P to S
Ionization Energy- Period 3
Why IE increases across the period 3?
IE increases across period 3
Nuclear charge increase
Strong electrostatic forces
attraction bet nucleus and e
IE – High
Na
Mg
AI
Si
P
S
CI
Ar
3p
3s
[Ne] 3s1
[Ne] 3s2
[Ne] 3s2 3p1
[Ne] 3s2 3p2
IE drop from Mg to AI
[Ne] 3s2 3p3
[Ne] 3s2 3p4
IE drop from P to S
Electron in p sublevel of AI
– further away from nucleus
2 electrons in same p orbital
- Greater e/e repulsion
Weak electrostatic force attraction
between nucleus and electron
Easier to remove e
IE - Low
IE - Low
Period 3
[Ne] 3s2 3p5
[Ne] 3s2 3p6
13. IE for Period 2 and 3
Ionization Energy- Period 2 and 3
Why IE period 3 lower than 2?
Period 3 – 3 shells/energy level
period 2
Period 3
Valence e further from nucleus
High shielding effect – more inner e
Weaker electrostatic forces
attraction bet nucleus and e
IE – Lower
period 2
Li
Be
B
C
N
O
F
Ne
2p
2s
1s
1s2 2s1
1s2 2s2
1s2 2s2 2p1
1s2 2s2 2p2
1s2 2s2 2p3
1s2 2s2 2p4
1s2 2s2 2p5
1s2 2s2 2p6
Period 3
Na
Mg
AI
Si
P
S
[Ne] 3s2 3p1
[Ne] 3s2 3p2
[Ne] 3s2 3p3
[Ne] 3s2 3p4
CI
Ar
3p
3s
2p
2s
1s
[Ne] 3s1
[Ne] 3s2
[Ne] 3s2 3p5
[Ne] 3s2 3p6
14. IE for Ne and Ar
Ionization Energy- Period 2 and 3
Why Ne and Ar have HIGH IE ?
Full electron configuration, 2.8/2.8.8
neon
argon
Most energetically stable structure
Difficult to lose electron
IE – High
period 2
Li
Be
B
C
N
O
F
Ne
2p
2s
1s
1s2 2s1
1s2 2s2
1s2 2s2 2p1
1s2 2s2 2p2
1s2 2s2 2p3
1s2 2s2 2p4
1s2 2s2 2p5
1s2 2s2 2p6
Period 3
Na
Mg
AI
Si
P
S
[Ne] 3s2 3p1
[Ne] 3s2 3p2
[Ne] 3s2 3p3
[Ne] 3s2 3p4
CI
Ar
3p
3s
2p
2s
1s
[Ne] 3s1
[Ne] 3s2
[Ne] 3s2 3p5
[Ne] 3s2 3p6
15. Successive Ionization Energy (IE) for Mg ( 2.8.2)
Successive Ionization Energy (IE) for magnesium
1st Ionization energy
Min energy to remove 1 mole e from
1 mole of element in gaseous state
M(g) M+(g) + e
2nd Ionization energy
Min energy to remove 1 mole e from
1 mole of +1 ion to form +2 ion
M+(g) M2+(g) + e
Mg
3rd energy
level
1st + 2nd electron
3s
2p
2nd energy
level
3rd to 8th electron
9th to 10th electron
2s
1st energy
level
11th to 12th electron
1s
1s2 2s2 2p6 3s2
1
Successive (IE) Mg (2.8.2) show
• IE increase when e removed
2
Successive (IE) Mg (2.8.2) show
• High jump in 2nd to 3rd IE
• High jump in 10th to 11th IE
3
Successive (IE) Mg (2.8.2) show
• Presence of 3 energy level
•
•
Ion become increasingly more positive as more e are removed
Electron-electron repulsion decrease as more e removed
High jump in IE – presence of new inner shell
1st + 2nd e – outmost shell
(3rd level)
High electrostatic
forces attraction
Electron nearer to nucleus –
High electrostatic forces attraction
3rd to 10th e – 2nd shell
(2nd level)
IE – High
IE – High
11th to 12th e – innermost shell
(1st level)
16. Successive Ionization Energy (IE) for Mg ( 2.8.2)
Successive Ionization Energy (IE) for magnesium
1st Ionization energy
Min energy to remove 1 mole e from
1 mole of element in gaseous state
M(g) M+(g) + e
2nd Ionization energy
Min energy to remove 1 mole e from
1 mole of +1 ion to form +2 ion
M+(g) M2+(g) + e
Mg
3rd energy
level
1st + 2nd electron
3s
2p
2nd energy
level
3rd to 8th electron
9th to 10th electron
2s
1st energy
level
11th to 12th electron
1s
1s2 2s2 2p6 3s2
•
Slow gradual increase in IE from 3rd to 10th e
4
Successive (IE) Mg (2.8.2) show
• Presence of sublevel, 2s + 2p
5
Successive (IE) Mg (2.8.2) show
• Succesive IE increasing
Species form increase in proton/e ratio by losing e
6
Successive (IE) Mg (2.8.2) show
• More difficult to lose e
M(g) M+(g) + e
M+ M2++ e
3rd to 8th e in 2p orbital
9th to 10th e inner 2s orbital
Species becomes more positively charged
M2+ M3++ e
More energy need to lose e
IE – High
IE – High
17. IB Questions on IE
s block elements
• s orbitals partially fill
1
H
He
5
1s2
n = 2 period 2
B
[He] 2s2 2p1
6
1s1
2
p block elements
• p orbital partially fill
C
[He] 2s2 2p2
7
N
[He] 2s2 2p3
3
Li
[He] 2s1
8
O
[He] 2s2 2p4
4
Be
[He] 2s2
9
F
[He] 2s2 2p5
11
Na
[Ne] 3s1
10
Ne
[He] 2s2 2p6
12
Mg
[Ne] 3s2
13
Al
[Ne] 3s2 3p1
14
Si
[Ne] 3s2 3p2
15
P
[Ne] 3s2 3p3
16
S
[Ne] 3s2 3p4
17
CI
[Ne] 3s2 3p5
18
Ar
[Ne] 3s2 3p6
19
K
20
1
Ca
[Ar]
[Ar]
1s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10 5p6 6s2 4f14 5d106p2
[Xe] 6s2 4f14 5d10 6p2
4s1
4s2
Identify position elements P, Q, R, S and T
Electron configuration :
P – 3s2 3p6
Q – 4s2 4p5
R – 3s2 3p6 4s2
S – 1s2 2s2 2p6 3s2 3p6 3d3 4s2
T – 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6
Answer
2
Write electron configuration for X, Y and Z
Element
Group
Period
X
2
3
Y
15
2
Z
18
3
Answer
Element
Group
Period
Classification
P
8/18
3
Noble gas
Q
7/17
4
p block
R
2
4
s block
S
5
4
d block
T
8/18
4
Noble gas
X – 1s2 2s2 2p6 3s2
Y – 1s2 2s2 2p3
Z – 1s2 2s2 2p6 3s2 3p6
3
Write electron structure for ions:
•
•
•
•
•
•
O - 1s2 2s2 2p4
O2- V - 1s2 2s2 2p6 3s2 3p6 4s2 3d3
V3+ Cu - 1s2 2s2 2p6 3s2 3p6 4s2 3d9
Cu2+ -
Answer
Write electron structure for ions:
•
•
•
•
•
•
O - 1s2 2s2 2p4
O2- -1s2 2s2 2p6
V - 1s2 2s2 2p6 3s2 3p6 4s2 3d3
V 3+ - 1s2 2s2 2p6 3s2 3p6 4s0 3d2
Cu - 1s2 2s2 2p6 3s2 3p6 4s2 3d9
Cu 2+ - 1s2 2s2 2p6 3s23p6 4s0 3d9
18. IB Questions on IE
s block elements
• s orbitals partially fill
1
H
He
5
1s2
n = 2 period 2
B
[He] 2s2 2p1
6
1s1
2
p block elements
• p orbital partially fill
C
[He] 2s2 2p2
7
N
[He] 2s2 2p3
3
Li
[He] 2s1
8
O
[He] 2s2 2p4
4
Be
[He] 2s2
9
F
[He] 2s2 2p5
11
Na
[Ne] 3s1
10
Ne
[He] 2s2 2p6
12
Mg
[Ne] 3s2
13
Al
[Ne] 3s2 3p1
14
Si
[Ne] 3s2 3p2
15
P
[Ne] 3s2 3p3
16
S
[Ne] 3s2 3p4
17
CI
[Ne] 3s2 3p5
18
Ar
[Ne] 3s2 3p6
19
20
4
K
Ca
[Ar]
[Ar]
1s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10 5p6 6s2 4f14 5d106p2
[Xe] 6s2 4f14 5d10 6p2
4s1
4s2
Successive IE of X is shown below
Predict the group and arrange in order of increasing proton number
Element
1st IE
2nd IE
3rd IE
4th IE
P
746
1423
7689
10456
Q
920
1768
14578
21343
R
587
1134
4890
6453
S
542
1045
4121
5412
Answer
All in Gp 2 – 2 valence electron
Order increasing proton number Q, P, R, S
ReasonGp 2, cause 1st and 2nd IE low
Q – Highest IE (less shell/energy level)
S – Lowest IE (more shell/energy level)
5
Successive IE of X is shown below
Determine electron structure of X
Successive IE
(kJ/mol)
1314
3302
5436
Answer:
X = 6 outermost electron, Gp 6, 2.6
Reason - 1st IE to 6th IE are low.
7436
10647
13768
71564
84736
19. IB Questions on IE
6
Successive IE of sodium is shown below:
State full electron structure and explain how the successive IE
are related to Its electron configuration.
Answer:
1s2 2s2 2p6 3s1
Reason:
• 1st electron easiest to remove, or 1st e in outmost shell/n= 3 energy level
• Large increase in IE bet 1st and 2nd as 2nd electron located in inner level, n=2
• Next 8 electrons more difficult to remove as the ion now is positively charged
• Large increase in IE between 9th and 10th , two innermost electron 10th/11th
in n=1 (close to nucleus)
8
Successive IE for 4 element shown below
a) Which element form charge +1
b) Predict C in periodic table
c) Which element requires least amt energy to
charge a gaseous ion which carry charge +3
d) Which element belong to same group?
Element
1st IE
2nd IE
3rd IE
4th IE
A
423
3021
4657
5867
B
754
1431
7741
10432
C
557
1814
2735
11843
D
597
1104
4942
6342
7
Successive IE of magnesium is shown below:
Explain the large increase in 10th and 11th IE and the general trend of
Increasing successive IE for Mg.
Answer:
Reason:
• 10th electron comes from 2nd energy level, (n=2) and 11th electron from n=1
• Electron in 1st energy level (n=1) closer to nucleus/ not shielded by inner electrons
• Successive IE high as it is more difficult to remove e from a positively charged ion.
Answer:
A – Gp 1, B - Gp 2, C – Gp 3, D – Gp 2
a) A- Gp 1 – lose 1 electron foming +1
b) C – Gp 3
c) Total IE = 1st IE + 2nd IE + 3rd IE
A = 8101
B= 9926
C = 5106
D = 6643
C requires least – Gp 3 – lose 3 e easily
d) B and D