(C) The jump between $IE_3$ and $IE_4$ is very large ($2750$ to $11580 \ kJ \cdot mol^{-1}$),indicating that the fourth electron is removed from a sta

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(C) The jump between $IE_3$ and $IE_4$ is very large ($2750$ to $11580 \ kJ \cdot mol^{-1}$),indicating that the fourth electron is removed from a stable inner shell (noble gas configuration).This means the element has $3$ valence electrons.Among the given options,Aluminum $(Al)$ has $3$ valence electrons $([Ne] 3s^2 3p^1)$.

Class 11 Chemistry Classification of Elements and Periodicity in Properties Ionisation energy

Medium

For one of the elements,various successive ionization enthalpies (in $kJ \cdot mol^{-1}$) are given below:

$I.E.$ $1^{st}$ $2^{nd}$ $3^{rd}$ $4^{th}$ $5^{th}$

Value $577.5$ $1810$ $2750$ $11580$ $14820$

The element is:

KCET 2015 All KCET

A
$Si$
B
$P$
C
$Al$
D
$Mg$

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Class 11

Chemistry Questions

Chapter

Classification of Elements and Periodicity in Properties

Subtopic

Ionisation energy

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The $CORRECT$ order of first ionisation enthalpy is:

MediumJEE MAIN 2021

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The energy required to remove an electron of a gaseous atom from its ground state is called

Easy

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How would you explain the fact that the first ionization enthalpy of sodium is lower than that of magnesium but its second ionization enthalpy is higher than that of magnesium?

Difficult

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The order of first ionization potentials of elements $Li, Be, B, Na$ is:

Medium

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$X_{(g)} \to X^{+}_{(g)} + e^-$,$\Delta H = +720 \ kJ \ mol^{-1}$
Calculate the amount of energy required to convert $110 \ mg$ of $X$ atom in gaseous state into $X^{+}$ ion .................... $kJ$ (Atomic weight for $X = 7 \ g \ mol^{-1}$)

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$I.E.$	$1^{st}$	$2^{nd}$	$3^{rd}$	$4^{th}$	$5^{th}$
Value	$577.5$	$1810$	$2750$	$11580$	$14820$

For one of the elements,various successive ionization enthalpies (in $kJ \cdot mol^{-1}$) are given below: $I.E.$ $1^{st}$ $2^{nd}$ $3^{rd}$ $4^{th}$ $5^{th}$ Value $577.5$ $1810$ $2750$ $11580$ $14820$ The element is:

Similar Questions

The $CORRECT$ order of first ionisation enthalpy is:

The energy required to remove an electron of a gaseous atom from its ground state is called

How would you explain the fact that the first ionization enthalpy of sodium is lower than that of magnesium but its second ionization enthalpy is higher than that of magnesium?

The order of first ionization potentials of elements $Li, Be, B, Na$ is:

$X_{(g)} \to X^{+}_{(g)} + e^-$,$\Delta H = +720 \ kJ \ mol^{-1}$Calculate the amount of energy required to convert $110 \ mg$ of $X$ atom in gaseous state into $X^{+}$ ion .................... $kJ$ (Atomic weight for $X = 7 \ g \ mol^{-1}$)

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For one of the elements,various successive ionization enthalpies (in $kJ \cdot mol^{-1}$) are given below:

$I.E.$ $1^{st}$ $2^{nd}$ $3^{rd}$ $4^{th}$ $5^{th}$

Value $577.5$ $1810$ $2750$ $11580$ $14820$

The element is:

$X_{(g)} \to X^{+}_{(g)} + e^-$,$\Delta H = +720 \ kJ \ mol^{-1}$
Calculate the amount of energy required to convert $110 \ mg$ of $X$ atom in gaseous state into $X^{+}$ ion .................... $kJ$ (Atomic weight for $X = 7 \ g \ mol^{-1}$)