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Ionization Enthalpy

The successiv...

Question

The successive ionization energies for element X is given below
$I E_{1}$ : $250 k J m o l^{- 1}$
$I E_{2}$ : $820 k J m o l^{- 1}$
$I E_{3}$ : $1100 k J m o l^{- 1}$
$I E_{4}$ : $1400 k J m o l^{- 1}$
Find out the number of valence electrons for the element X.

3

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4

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2

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1

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Solution

The correct option is B $1$
There are in all four ionisation energies given. That means after losing the fourth electron, noble gas configuration comes. So the number of valence electrons is 1.

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Similar questions

X

I E_{1} = 250 {kJ mol}^{- 1}

I E_{2} = 820 {kJ mol}^{- 1}

I E_{3} = 1100 {kJ mol}^{- 1}

I E_{4} = 1400 {kJ mol}^{- 1}

X

Successive ionization enthalpies of an element 'X' are given below

IE1. IE2. IE3. IE4

165. 195. 556. 595

Electronic configuration of the element'X' is?

X

I E_{1} = 250 {kJ mol}^{- 1}

I E_{2} = 820 {kJ mol}^{- 1}

I E_{3} = 1100 {kJ mol}^{- 1}

I E_{4} = 1400 {kJ mol}^{- 1}

X

k J / m o l

I E_{1} = 580, I E_{2} = 1815, I E_{3} = 2740, I E_{4} = 11, 600

I E_{5} = 14, 842

{I E}_{1}

{I E}_{2}

{I E}_{3}

{I E}_{4}

N i

P t

{N i}^{2 +}

{P t}^{2 +}

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