QBManager

Classification of Elements and Periodicity in Properties

89556 The ionisation potential of which element is highest?

1

H

2

He

3

Ar

4

F

Explanation:

The ionization potential of $He$ element is highest because ionization potential (Energy) decreases as move from down a group and increases as move from left to right across a period.
So, inert gas has highest ionization potential.

CG PET-22.05.2022

Classification of Elements and Periodicity in Properties

89560 The first ionization potential of $Na, Mg$ and $Si$ are respectively 496,737 and $786 kJ mol^{- 1}$ . The ionization potential of $Al$ will be closer to

1

760 kJ {mol}^{- 1}

2

575 kJ {mol}^{- 1}

3

801 kJ {mol}^{- 1}

4

419 kJ {mol}^{- 1}

Explanation:

The ionization energy of $Mg$ will be larger than that of $Na$ due to fully filled configuration. The ionization energy of $Al$ will be smaller than that of $Mg$ due to one electron extra than the stable configuration but smaller than Si due to increase in effective nuclear of Si. Hence, the ionization potential of $Al$ will be $760 kJ / mole$ .

AMU-2014

Classification of Elements and Periodicity in Properties

89561 The decreasing order of the ionization potential of the following elements is

1

Ne > Cl > P > S > Al > Mg

2

Ne > Cl > P > S > Mg > Al

3

Ne > Cl > S > P > Mg > Al

4

Ne > Cl > S > P > Al > Mg

Explanation:

On moving from left to right in a period ionization potential increases. On moving from top to bottom in a group ionization potential decreases. Rare gases are more ionization potential than full filled orbital than half-filled orbital. Hence, the order is $Ne >$ $Cl > P > S > Mg > Al$ .

CG PET -2005

Classification of Elements and Periodicity in Properties

89562 In which of the following arrangements, the order is NOT according to the property indicated against It

1

Li < Na < K < Rb

:
Increasing metallic radius

2 I

< Br < F < CI

:
Increasing electron gain enthalpy

3 B

< C < N < O

Increasing first ionization enthalpy

4

{Al}^{3 +} < {Mg}^{2 +} < {Na}^{+} < F^{-}

Increasing ionic size

Explanation:

When we move from $B$ to $O$ in periodic table first ionization enthalpy increases due to the attraction of nucleus towards the outer most of electron. Hence, the order is- $B < C < N < O$ : increasing first ionization enthalpy.

AIIMS-2015

Classification of Elements and Periodicity in Properties

89563 In the following, the element with the highest ionization energy is

1

[Ne] 3 s^{2} 3 p^{2}

2

[Ne] 3 s^{2} 3 p_{4}^{3}

3

[Ne] 3 s^{2} 3 p^{2}

4

[Ne] 3 s^{2} 3 p^{4}

Explanation:

The given electronic configuration [Ne] $3 s^{2}$ $3 p^{3}$ are half-filled electronic configuration on removing the one electron the amount of energy is required to high. So, it has highest ionisation energy.

JIPMER-2010

Classification of Elements and Periodicity in Properties

89556 The ionisation potential of which element is highest?

1

H

2

He

3

Ar

4

F

Explanation:

The ionization potential of $He$ element is highest because ionization potential (Energy) decreases as move from down a group and increases as move from left to right across a period.
So, inert gas has highest ionization potential.

CG PET-22.05.2022

Classification of Elements and Periodicity in Properties

89560 The first ionization potential of $Na, Mg$ and $Si$ are respectively 496,737 and $786 kJ mol^{- 1}$ . The ionization potential of $Al$ will be closer to

1

760 kJ {mol}^{- 1}

2

575 kJ {mol}^{- 1}

3

801 kJ {mol}^{- 1}

4

419 kJ {mol}^{- 1}

Explanation:

The ionization energy of $Mg$ will be larger than that of $Na$ due to fully filled configuration. The ionization energy of $Al$ will be smaller than that of $Mg$ due to one electron extra than the stable configuration but smaller than Si due to increase in effective nuclear of Si. Hence, the ionization potential of $Al$ will be $760 kJ / mole$ .

AMU-2014

Classification of Elements and Periodicity in Properties

89561 The decreasing order of the ionization potential of the following elements is

1

Ne > Cl > P > S > Al > Mg

2

Ne > Cl > P > S > Mg > Al

3

Ne > Cl > S > P > Mg > Al

4

Ne > Cl > S > P > Al > Mg

Explanation:

On moving from left to right in a period ionization potential increases. On moving from top to bottom in a group ionization potential decreases. Rare gases are more ionization potential than full filled orbital than half-filled orbital. Hence, the order is $Ne >$ $Cl > P > S > Mg > Al$ .

CG PET -2005

Classification of Elements and Periodicity in Properties

89562 In which of the following arrangements, the order is NOT according to the property indicated against It

1

Li < Na < K < Rb

:
Increasing metallic radius

2 I

< Br < F < CI

:
Increasing electron gain enthalpy

3 B

< C < N < O

Increasing first ionization enthalpy

4

{Al}^{3 +} < {Mg}^{2 +} < {Na}^{+} < F^{-}

Increasing ionic size

Explanation:

When we move from $B$ to $O$ in periodic table first ionization enthalpy increases due to the attraction of nucleus towards the outer most of electron. Hence, the order is- $B < C < N < O$ : increasing first ionization enthalpy.

AIIMS-2015

Classification of Elements and Periodicity in Properties

89563 In the following, the element with the highest ionization energy is

1

[Ne] 3 s^{2} 3 p^{2}

2

[Ne] 3 s^{2} 3 p_{4}^{3}

3

[Ne] 3 s^{2} 3 p^{2}

4

[Ne] 3 s^{2} 3 p^{4}

Explanation:

The given electronic configuration [Ne] $3 s^{2}$ $3 p^{3}$ are half-filled electronic configuration on removing the one electron the amount of energy is required to high. So, it has highest ionisation energy.

JIPMER-2010

Classification of Elements and Periodicity in Properties

89556 The ionisation potential of which element is highest?

1

H

2

He

3

Ar

4

F

Explanation:

The ionization potential of $He$ element is highest because ionization potential (Energy) decreases as move from down a group and increases as move from left to right across a period.
So, inert gas has highest ionization potential.

CG PET-22.05.2022

Classification of Elements and Periodicity in Properties

89560 The first ionization potential of $Na, Mg$ and $Si$ are respectively 496,737 and $786 kJ mol^{- 1}$ . The ionization potential of $Al$ will be closer to

1

760 kJ {mol}^{- 1}

2

575 kJ {mol}^{- 1}

3

801 kJ {mol}^{- 1}

4

419 kJ {mol}^{- 1}

Explanation:

The ionization energy of $Mg$ will be larger than that of $Na$ due to fully filled configuration. The ionization energy of $Al$ will be smaller than that of $Mg$ due to one electron extra than the stable configuration but smaller than Si due to increase in effective nuclear of Si. Hence, the ionization potential of $Al$ will be $760 kJ / mole$ .

AMU-2014

Classification of Elements and Periodicity in Properties

89561 The decreasing order of the ionization potential of the following elements is

1

Ne > Cl > P > S > Al > Mg

2

Ne > Cl > P > S > Mg > Al

3

Ne > Cl > S > P > Mg > Al

4

Ne > Cl > S > P > Al > Mg

Explanation:

On moving from left to right in a period ionization potential increases. On moving from top to bottom in a group ionization potential decreases. Rare gases are more ionization potential than full filled orbital than half-filled orbital. Hence, the order is $Ne >$ $Cl > P > S > Mg > Al$ .

CG PET -2005

Classification of Elements and Periodicity in Properties

89562 In which of the following arrangements, the order is NOT according to the property indicated against It

1

Li < Na < K < Rb

:
Increasing metallic radius

2 I

< Br < F < CI

:
Increasing electron gain enthalpy

3 B

< C < N < O

Increasing first ionization enthalpy

4

{Al}^{3 +} < {Mg}^{2 +} < {Na}^{+} < F^{-}

Increasing ionic size

Explanation:

When we move from $B$ to $O$ in periodic table first ionization enthalpy increases due to the attraction of nucleus towards the outer most of electron. Hence, the order is- $B < C < N < O$ : increasing first ionization enthalpy.

AIIMS-2015

Classification of Elements and Periodicity in Properties

89563 In the following, the element with the highest ionization energy is

1

[Ne] 3 s^{2} 3 p^{2}

2

[Ne] 3 s^{2} 3 p_{4}^{3}

3

[Ne] 3 s^{2} 3 p^{2}

4

[Ne] 3 s^{2} 3 p^{4}

Explanation:

The given electronic configuration [Ne] $3 s^{2}$ $3 p^{3}$ are half-filled electronic configuration on removing the one electron the amount of energy is required to high. So, it has highest ionisation energy.

JIPMER-2010

Classification of Elements and Periodicity in Properties

89556 The ionisation potential of which element is highest?

1

H

2

He

3

Ar

4

F

Explanation:

The ionization potential of $He$ element is highest because ionization potential (Energy) decreases as move from down a group and increases as move from left to right across a period.
So, inert gas has highest ionization potential.

CG PET-22.05.2022

Classification of Elements and Periodicity in Properties

89560 The first ionization potential of $Na, Mg$ and $Si$ are respectively 496,737 and $786 kJ mol^{- 1}$ . The ionization potential of $Al$ will be closer to

1

760 kJ {mol}^{- 1}

2

575 kJ {mol}^{- 1}

3

801 kJ {mol}^{- 1}

4

419 kJ {mol}^{- 1}

Explanation:

The ionization energy of $Mg$ will be larger than that of $Na$ due to fully filled configuration. The ionization energy of $Al$ will be smaller than that of $Mg$ due to one electron extra than the stable configuration but smaller than Si due to increase in effective nuclear of Si. Hence, the ionization potential of $Al$ will be $760 kJ / mole$ .

AMU-2014

Classification of Elements and Periodicity in Properties

89561 The decreasing order of the ionization potential of the following elements is

1

Ne > Cl > P > S > Al > Mg

2

Ne > Cl > P > S > Mg > Al

3

Ne > Cl > S > P > Mg > Al

4

Ne > Cl > S > P > Al > Mg

Explanation:

On moving from left to right in a period ionization potential increases. On moving from top to bottom in a group ionization potential decreases. Rare gases are more ionization potential than full filled orbital than half-filled orbital. Hence, the order is $Ne >$ $Cl > P > S > Mg > Al$ .

CG PET -2005

Classification of Elements and Periodicity in Properties

89562 In which of the following arrangements, the order is NOT according to the property indicated against It

1

Li < Na < K < Rb

:
Increasing metallic radius

2 I

< Br < F < CI

:
Increasing electron gain enthalpy

3 B

< C < N < O

Increasing first ionization enthalpy

4

{Al}^{3 +} < {Mg}^{2 +} < {Na}^{+} < F^{-}

Increasing ionic size

Explanation:

When we move from $B$ to $O$ in periodic table first ionization enthalpy increases due to the attraction of nucleus towards the outer most of electron. Hence, the order is- $B < C < N < O$ : increasing first ionization enthalpy.

AIIMS-2015

Classification of Elements and Periodicity in Properties

89563 In the following, the element with the highest ionization energy is

1

[Ne] 3 s^{2} 3 p^{2}

2

[Ne] 3 s^{2} 3 p_{4}^{3}

3

[Ne] 3 s^{2} 3 p^{2}

4

[Ne] 3 s^{2} 3 p^{4}

Explanation:

The given electronic configuration [Ne] $3 s^{2}$ $3 p^{3}$ are half-filled electronic configuration on removing the one electron the amount of energy is required to high. So, it has highest ionisation energy.

JIPMER-2010

Classification of Elements and Periodicity in Properties

89556 The ionisation potential of which element is highest?

1

H

2

He

3

Ar

4

F

Explanation:

The ionization potential of $He$ element is highest because ionization potential (Energy) decreases as move from down a group and increases as move from left to right across a period.
So, inert gas has highest ionization potential.

CG PET-22.05.2022

Classification of Elements and Periodicity in Properties

89560 The first ionization potential of $Na, Mg$ and $Si$ are respectively 496,737 and $786 kJ mol^{- 1}$ . The ionization potential of $Al$ will be closer to

1

760 kJ {mol}^{- 1}

2

575 kJ {mol}^{- 1}

3

801 kJ {mol}^{- 1}

4

419 kJ {mol}^{- 1}

Explanation:

The ionization energy of $Mg$ will be larger than that of $Na$ due to fully filled configuration. The ionization energy of $Al$ will be smaller than that of $Mg$ due to one electron extra than the stable configuration but smaller than Si due to increase in effective nuclear of Si. Hence, the ionization potential of $Al$ will be $760 kJ / mole$ .

AMU-2014

Classification of Elements and Periodicity in Properties

89561 The decreasing order of the ionization potential of the following elements is

1

Ne > Cl > P > S > Al > Mg

2

Ne > Cl > P > S > Mg > Al

3

Ne > Cl > S > P > Mg > Al

4

Ne > Cl > S > P > Al > Mg

Explanation:

On moving from left to right in a period ionization potential increases. On moving from top to bottom in a group ionization potential decreases. Rare gases are more ionization potential than full filled orbital than half-filled orbital. Hence, the order is $Ne >$ $Cl > P > S > Mg > Al$ .

CG PET -2005

Classification of Elements and Periodicity in Properties

89562 In which of the following arrangements, the order is NOT according to the property indicated against It

1

Li < Na < K < Rb

:
Increasing metallic radius

2 I

< Br < F < CI

:
Increasing electron gain enthalpy

3 B

< C < N < O

Increasing first ionization enthalpy

4

{Al}^{3 +} < {Mg}^{2 +} < {Na}^{+} < F^{-}

Increasing ionic size

Explanation:

When we move from $B$ to $O$ in periodic table first ionization enthalpy increases due to the attraction of nucleus towards the outer most of electron. Hence, the order is- $B < C < N < O$ : increasing first ionization enthalpy.

AIIMS-2015

Classification of Elements and Periodicity in Properties

89563 In the following, the element with the highest ionization energy is

1

[Ne] 3 s^{2} 3 p^{2}

2

[Ne] 3 s^{2} 3 p_{4}^{3}

3

[Ne] 3 s^{2} 3 p^{2}

4

[Ne] 3 s^{2} 3 p^{4}

Explanation:

The given electronic configuration [Ne] $3 s^{2}$ $3 p^{3}$ are half-filled electronic configuration on removing the one electron the amount of energy is required to high. So, it has highest ionisation energy.

JIPMER-2010