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CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313353 The electronic configuration with the highest ionisation enthalpy is:

1

[N e] 3 s^{2} 3 p^{1}

2

[N e] 3 s^{2} 3 p^{2}

3

[N e] 3 s^{2} 3 p^{3}

4

[A r] 3 d^{10} 4 s^{2} 4 p^{3}

JEE - 2017

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313354 The ionisation energy of nitrogen is larger than that of oxygen because of

1 greater attraction of electrons by the nucleus

2 the size of the nitrogen atom being smaller

3 the half-filled p-orbitals possess extra stability

4 greater penetration effect.

Explanation:

Electronic configuration of $N = 1 s^{2} 2 s^{2} 2 p^{3}$
Electronic configuration of $O = 1 s^{2} 2 s^{2} 2 p^{4}$
Since, half - filled p-orbital is more stable thus, it is very difficult to remove an electron from it hence, N has greater ionisation energy than O .

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313355 The ionisation energy of sodium is $495 k J m o l^{- 1} .$ How much energy is needed to convert atoms present in 2.3 mg of sodium into sodium ions

1 4.95 J

2 49.5 J

3 495 J

4 0.495 J

Explanation:

Ionization energy of sodium = 495 kJ/mol
Number of moles of sodium convert to sodium ions $= \frac{2 .3 \times 1 0^{- 3}}{23} = 1 0^{- 4} m o l e s$
1 moles require energy is 495 kJ/mol
$1 0^{- 4}$ moles require energy is $495 \times 1 0^{3} \times 1 0^{- 4} J = 49 .5 J$

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313356 Among the following, the third ionisation energy is highest for

1 magnesium

2 boron

3 beryllium

4 aluminium

Explanation:

The electronic configuration of the given elements is as follows:
$_{12} M g = [N e] 3 s^{2}_{5} B = [H e] 2 s^{2}, 2 p^{1}$
$_{4} B e = [H e] 2 s^{2}_{13} A l = [N e] 3 s^{2}, 3 p^{1}$
From the electronic configuration, it is clear that third ionisation energy of $Mg$ and $Be$ is higher than that of $Al$ and $B$ In them, the third electron has to be removed from the stable inert gas configuration.
Between $Mg$ and, Be third IE of Be is high because of its smaller size than Mg as both lie in the same group.

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313357 Which of the following represents the correct order of increasing first ionisation enthalpy for Ca, Ba, S, Se and Ar?

1 Ca < S < Ba < Se < Ar

2 S < Se < Ca < Ba < Ar

3 Ba < Ca < Se < S < Ar

4 Ca < Ba < S < Se < Ar

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313353 The electronic configuration with the highest ionisation enthalpy is:

1

[N e] 3 s^{2} 3 p^{1}

2

[N e] 3 s^{2} 3 p^{2}

3

[N e] 3 s^{2} 3 p^{3}

4

[A r] 3 d^{10} 4 s^{2} 4 p^{3}

JEE - 2017

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313354 The ionisation energy of nitrogen is larger than that of oxygen because of

1 greater attraction of electrons by the nucleus

2 the size of the nitrogen atom being smaller

3 the half-filled p-orbitals possess extra stability

4 greater penetration effect.

Explanation:

Electronic configuration of $N = 1 s^{2} 2 s^{2} 2 p^{3}$
Electronic configuration of $O = 1 s^{2} 2 s^{2} 2 p^{4}$
Since, half - filled p-orbital is more stable thus, it is very difficult to remove an electron from it hence, N has greater ionisation energy than O .

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313355 The ionisation energy of sodium is $495 k J m o l^{- 1} .$ How much energy is needed to convert atoms present in 2.3 mg of sodium into sodium ions

1 4.95 J

2 49.5 J

3 495 J

4 0.495 J

Explanation:

Ionization energy of sodium = 495 kJ/mol
Number of moles of sodium convert to sodium ions $= \frac{2 .3 \times 1 0^{- 3}}{23} = 1 0^{- 4} m o l e s$
1 moles require energy is 495 kJ/mol
$1 0^{- 4}$ moles require energy is $495 \times 1 0^{3} \times 1 0^{- 4} J = 49 .5 J$

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313356 Among the following, the third ionisation energy is highest for

1 magnesium

2 boron

3 beryllium

4 aluminium

Explanation:

The electronic configuration of the given elements is as follows:
$_{12} M g = [N e] 3 s^{2}_{5} B = [H e] 2 s^{2}, 2 p^{1}$
$_{4} B e = [H e] 2 s^{2}_{13} A l = [N e] 3 s^{2}, 3 p^{1}$
From the electronic configuration, it is clear that third ionisation energy of $Mg$ and $Be$ is higher than that of $Al$ and $B$ In them, the third electron has to be removed from the stable inert gas configuration.
Between $Mg$ and, Be third IE of Be is high because of its smaller size than Mg as both lie in the same group.

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313357 Which of the following represents the correct order of increasing first ionisation enthalpy for Ca, Ba, S, Se and Ar?

1 Ca < S < Ba < Se < Ar

2 S < Se < Ca < Ba < Ar

3 Ba < Ca < Se < S < Ar

4 Ca < Ba < S < Se < Ar

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313353 The electronic configuration with the highest ionisation enthalpy is:

1

[N e] 3 s^{2} 3 p^{1}

2

[N e] 3 s^{2} 3 p^{2}

3

[N e] 3 s^{2} 3 p^{3}

4

[A r] 3 d^{10} 4 s^{2} 4 p^{3}

JEE - 2017

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313354 The ionisation energy of nitrogen is larger than that of oxygen because of

1 greater attraction of electrons by the nucleus

2 the size of the nitrogen atom being smaller

3 the half-filled p-orbitals possess extra stability

4 greater penetration effect.

Explanation:

Electronic configuration of $N = 1 s^{2} 2 s^{2} 2 p^{3}$
Electronic configuration of $O = 1 s^{2} 2 s^{2} 2 p^{4}$
Since, half - filled p-orbital is more stable thus, it is very difficult to remove an electron from it hence, N has greater ionisation energy than O .

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313355 The ionisation energy of sodium is $495 k J m o l^{- 1} .$ How much energy is needed to convert atoms present in 2.3 mg of sodium into sodium ions

1 4.95 J

2 49.5 J

3 495 J

4 0.495 J

Explanation:

Ionization energy of sodium = 495 kJ/mol
Number of moles of sodium convert to sodium ions $= \frac{2 .3 \times 1 0^{- 3}}{23} = 1 0^{- 4} m o l e s$
1 moles require energy is 495 kJ/mol
$1 0^{- 4}$ moles require energy is $495 \times 1 0^{3} \times 1 0^{- 4} J = 49 .5 J$

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313356 Among the following, the third ionisation energy is highest for

1 magnesium

2 boron

3 beryllium

4 aluminium

Explanation:

The electronic configuration of the given elements is as follows:
$_{12} M g = [N e] 3 s^{2}_{5} B = [H e] 2 s^{2}, 2 p^{1}$
$_{4} B e = [H e] 2 s^{2}_{13} A l = [N e] 3 s^{2}, 3 p^{1}$
From the electronic configuration, it is clear that third ionisation energy of $Mg$ and $Be$ is higher than that of $Al$ and $B$ In them, the third electron has to be removed from the stable inert gas configuration.
Between $Mg$ and, Be third IE of Be is high because of its smaller size than Mg as both lie in the same group.

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313357 Which of the following represents the correct order of increasing first ionisation enthalpy for Ca, Ba, S, Se and Ar?

1 Ca < S < Ba < Se < Ar

2 S < Se < Ca < Ba < Ar

3 Ba < Ca < Se < S < Ar

4 Ca < Ba < S < Se < Ar

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313353 The electronic configuration with the highest ionisation enthalpy is:

1

[N e] 3 s^{2} 3 p^{1}

2

[N e] 3 s^{2} 3 p^{2}

3

[N e] 3 s^{2} 3 p^{3}

4

[A r] 3 d^{10} 4 s^{2} 4 p^{3}

JEE - 2017

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313354 The ionisation energy of nitrogen is larger than that of oxygen because of

1 greater attraction of electrons by the nucleus

2 the size of the nitrogen atom being smaller

3 the half-filled p-orbitals possess extra stability

4 greater penetration effect.

Explanation:

Electronic configuration of $N = 1 s^{2} 2 s^{2} 2 p^{3}$
Electronic configuration of $O = 1 s^{2} 2 s^{2} 2 p^{4}$
Since, half - filled p-orbital is more stable thus, it is very difficult to remove an electron from it hence, N has greater ionisation energy than O .

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313355 The ionisation energy of sodium is $495 k J m o l^{- 1} .$ How much energy is needed to convert atoms present in 2.3 mg of sodium into sodium ions

1 4.95 J

2 49.5 J

3 495 J

4 0.495 J

Explanation:

Ionization energy of sodium = 495 kJ/mol
Number of moles of sodium convert to sodium ions $= \frac{2 .3 \times 1 0^{- 3}}{23} = 1 0^{- 4} m o l e s$
1 moles require energy is 495 kJ/mol
$1 0^{- 4}$ moles require energy is $495 \times 1 0^{3} \times 1 0^{- 4} J = 49 .5 J$

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313356 Among the following, the third ionisation energy is highest for

1 magnesium

2 boron

3 beryllium

4 aluminium

Explanation:

The electronic configuration of the given elements is as follows:
$_{12} M g = [N e] 3 s^{2}_{5} B = [H e] 2 s^{2}, 2 p^{1}$
$_{4} B e = [H e] 2 s^{2}_{13} A l = [N e] 3 s^{2}, 3 p^{1}$
From the electronic configuration, it is clear that third ionisation energy of $Mg$ and $Be$ is higher than that of $Al$ and $B$ In them, the third electron has to be removed from the stable inert gas configuration.
Between $Mg$ and, Be third IE of Be is high because of its smaller size than Mg as both lie in the same group.

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313357 Which of the following represents the correct order of increasing first ionisation enthalpy for Ca, Ba, S, Se and Ar?

1 Ca < S < Ba < Se < Ar

2 S < Se < Ca < Ba < Ar

3 Ba < Ca < Se < S < Ar

4 Ca < Ba < S < Se < Ar

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313353 The electronic configuration with the highest ionisation enthalpy is:

1

[N e] 3 s^{2} 3 p^{1}

2

[N e] 3 s^{2} 3 p^{2}

3

[N e] 3 s^{2} 3 p^{3}

4

[A r] 3 d^{10} 4 s^{2} 4 p^{3}

JEE - 2017

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313354 The ionisation energy of nitrogen is larger than that of oxygen because of

1 greater attraction of electrons by the nucleus

2 the size of the nitrogen atom being smaller

3 the half-filled p-orbitals possess extra stability

4 greater penetration effect.

Explanation:

Electronic configuration of $N = 1 s^{2} 2 s^{2} 2 p^{3}$
Electronic configuration of $O = 1 s^{2} 2 s^{2} 2 p^{4}$
Since, half - filled p-orbital is more stable thus, it is very difficult to remove an electron from it hence, N has greater ionisation energy than O .

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313355 The ionisation energy of sodium is $495 k J m o l^{- 1} .$ How much energy is needed to convert atoms present in 2.3 mg of sodium into sodium ions

1 4.95 J

2 49.5 J

3 495 J

4 0.495 J

Explanation:

Ionization energy of sodium = 495 kJ/mol
Number of moles of sodium convert to sodium ions $= \frac{2 .3 \times 1 0^{- 3}}{23} = 1 0^{- 4} m o l e s$
1 moles require energy is 495 kJ/mol
$1 0^{- 4}$ moles require energy is $495 \times 1 0^{3} \times 1 0^{- 4} J = 49 .5 J$

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313356 Among the following, the third ionisation energy is highest for

1 magnesium

2 boron

3 beryllium

4 aluminium

Explanation:

The electronic configuration of the given elements is as follows:
$_{12} M g = [N e] 3 s^{2}_{5} B = [H e] 2 s^{2}, 2 p^{1}$
$_{4} B e = [H e] 2 s^{2}_{13} A l = [N e] 3 s^{2}, 3 p^{1}$
From the electronic configuration, it is clear that third ionisation energy of $Mg$ and $Be$ is higher than that of $Al$ and $B$ In them, the third electron has to be removed from the stable inert gas configuration.
Between $Mg$ and, Be third IE of Be is high because of its smaller size than Mg as both lie in the same group.

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313357 Which of the following represents the correct order of increasing first ionisation enthalpy for Ca, Ba, S, Se and Ar?

1 Ca < S < Ba < Se < Ar

2 S < Se < Ca < Ba < Ar

3 Ba < Ca < Se < S < Ar

4 Ca < Ba < S < Se < Ar