Important question related to ionisation energy:
Question 1
Ionisation energy of gases is higher. why?
ans. because of higher stable of ns^2 np^6 configuration.
or
noble gases have completely filled valence shell whuchbis more stable. so removal of electron is very difficult. hence I. E of noble gases is high.
Question 2
which have more ionisation energy Oxygen & nitrogen?
ans
O
(8) 1s^2 2s^2 2p^4
N
(7) 1s^2 2s^2 2p^3
Nitrogen has exactly half filled p subshell .whuch is more stable as a result removal electron becomes difficult. hence I. E of nitrogen is more than oxygen.
hence peaks show half filled & completely filled subshell of atom .which required more energy for removal of electron .hence I. E is more
Question 3
First I. E of aluminum is less than magnesium. why?
ans
Al
(13) 1s^2 2s^2 2p^6 3s^2 3p^1
Mg
(12) 1s^2 2s^2 2p^6 3s^2
in aluminum we have to remove electron from 3p orbital which required comparatively less energy .hence first I. E of aluminum is less than magnesium.
Question 4
First I. E of magnesium is higher than that of aluminum .while 2nd I. E of sodium is higher than Magnesium.
ans
Mg
(12) 1s^2 2s^2 2p^6 3s^2
Al
(13) 1s^2 2s^2 2p^6 3s^2 3p^1
in Mg when first electron remove its remove from the s subshell which highly stable. so we required large amount of energy to remove electron from Mg as compare to Al. so I. E(1) is more than Aluminum of magnesium
Mg^+
(12) 1s^2 2s^2 2p^6 3s^1
Al ^+
(13) 1s^2 2s^2 2p^6 3s^2
when I. E(2) is removed than aluminum taken more energy as compare to magnesium. so we can say that I. E(2) of Aluminium is more than magnesium
Question 1
Ionisation energy of gases is higher. why?
ans. because of higher stable of ns^2 np^6 configuration.
or
noble gases have completely filled valence shell whuchbis more stable. so removal of electron is very difficult. hence I. E of noble gases is high.
Question 2
which have more ionisation energy Oxygen & nitrogen?
ans
O
(8) 1s^2 2s^2 2p^4
N
(7) 1s^2 2s^2 2p^3
Nitrogen has exactly half filled p subshell .whuch is more stable as a result removal electron becomes difficult. hence I. E of nitrogen is more than oxygen.
Question 3
First I. E of aluminum is less than magnesium. why?
ans
Al
(13) 1s^2 2s^2 2p^6 3s^2 3p^1
Mg
(12) 1s^2 2s^2 2p^6 3s^2
in aluminum we have to remove electron from 3p orbital which required comparatively less energy .hence first I. E of aluminum is less than magnesium.
Question 4
First I. E of magnesium is higher than that of aluminum .while 2nd I. E of sodium is higher than Magnesium.
ans
Mg
(12) 1s^2 2s^2 2p^6 3s^2
Al
(13) 1s^2 2s^2 2p^6 3s^2 3p^1
in Mg when first electron remove its remove from the s subshell which highly stable. so we required large amount of energy to remove electron from Mg as compare to Al. so I. E(1) is more than Aluminum of magnesium
Mg^+
(12) 1s^2 2s^2 2p^6 3s^1
Al ^+
(13) 1s^2 2s^2 2p^6 3s^2
when I. E(2) is removed than aluminum taken more energy as compare to magnesium. so we can say that I. E(2) of Aluminium is more than magnesium
similarly
Question 5
I. E(1) of magnesium is higher than that of Na while I. E(2) of Na is higher than Mg.
Question 6
First ionisation energy of alkaline earth metal is low and second is higher but show deviated state (+2) ?
ans
because hydration energy of group 2 element is large. so at The I. E(2) when electron remove is attain more energy. so I. E (2) is more due to hydration energy.
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