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CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313328 The $I_{1}$ values of Li, Be and C are 5.4 eV/atom, 9.32 eV/atom and 11.26 eV/atom. The $I_{1}$ value of Boron is

1 13.6 eV/atom

2 8.29 eV/atom

3 14.5 eV/atom

4 21.5 eV/atom

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313329 Calculate the energy needed to convert three moles of sodium atoms in the gaseous state to sodium ions. The ionization energy of sodium is $495 k J m o l^{- 1} .$

1 1485 kJ

2 495 kJ

3 148.5 kJ

4 None

Explanation:

Energy needed to convert 1 mole of sodium (g) to sodium ions = 495 kJ
$∴$ Energy needed to convert 3 mole of Na (g) to $N a^{+} i o n s = 495 \times 3 = 1485 k J$

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313330 Read the Assertion and Reason carefully and mark the correct option
Assertion :
The first ionization enthalpy of 3d series elements is more than that of group 2 metals.
Reason :
In 3d series of elements successive filling of d-orbitals takes place.

1 Both Assertion and Reason are true and Reason is the correct explanation of Assertion.

2 Assertion is true but Reason is false.

3 Assertion is false but Reason is true.

4 Both Assertion and Reason are true but Reason is not the correct explanation of Assertion.

Explanation:

I.E. of $3 d -$ series elements in $k J / m o l$
$\underset{631}{S c} \underset{656}{T i} \underset{650}{V} \underset{653}{C r} \underset{717}{M n} \underset{762}{F e} \underset{758}{C o} \underset{736}{N i} \underset{745}{C u} \underset{906}{Z n}$
I.E. values in $k J / mol o f 2^{n d}$ group elements is
$\underset{899}{B e} \underset{737}{M g} \underset{590}{C a} \underset{549}{S r} \underset{503}{B a} \underset{509}{R a}$
From Sc to Mn , I.E. values are less than that of $M g (B e$ , a non-metal need not to be considered).
So, Assertion is false. Reason is correct.

JEE - 2023

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313331 Which represents the correct order of first ionisation potential of third period elements?

1

Na > Mg > Al > Si

2

Na < Mg < Al < Si

3

Na < Si < Al < Mg

4

Na < Al < Mg < Si

Explanation:

Generally, ionisation potential increases, as we move from left to right in a period. However, the ionisation potential of II A group elements is higher than that of the III A group elements. This is because of the fully-filled $s$ -orbitals in II A group elements.
Hence, the correct order of ionisation potential is
$Na < Al < Mg < Si$

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313328 The $I_{1}$ values of Li, Be and C are 5.4 eV/atom, 9.32 eV/atom and 11.26 eV/atom. The $I_{1}$ value of Boron is

1 13.6 eV/atom

2 8.29 eV/atom

3 14.5 eV/atom

4 21.5 eV/atom

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313329 Calculate the energy needed to convert three moles of sodium atoms in the gaseous state to sodium ions. The ionization energy of sodium is $495 k J m o l^{- 1} .$

1 1485 kJ

2 495 kJ

3 148.5 kJ

4 None

Explanation:

Energy needed to convert 1 mole of sodium (g) to sodium ions = 495 kJ
$∴$ Energy needed to convert 3 mole of Na (g) to $N a^{+} i o n s = 495 \times 3 = 1485 k J$

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313330 Read the Assertion and Reason carefully and mark the correct option
Assertion :
The first ionization enthalpy of 3d series elements is more than that of group 2 metals.
Reason :
In 3d series of elements successive filling of d-orbitals takes place.

1 Both Assertion and Reason are true and Reason is the correct explanation of Assertion.

2 Assertion is true but Reason is false.

3 Assertion is false but Reason is true.

4 Both Assertion and Reason are true but Reason is not the correct explanation of Assertion.

Explanation:

I.E. of $3 d -$ series elements in $k J / m o l$
$\underset{631}{S c} \underset{656}{T i} \underset{650}{V} \underset{653}{C r} \underset{717}{M n} \underset{762}{F e} \underset{758}{C o} \underset{736}{N i} \underset{745}{C u} \underset{906}{Z n}$
I.E. values in $k J / mol o f 2^{n d}$ group elements is
$\underset{899}{B e} \underset{737}{M g} \underset{590}{C a} \underset{549}{S r} \underset{503}{B a} \underset{509}{R a}$
From Sc to Mn , I.E. values are less than that of $M g (B e$ , a non-metal need not to be considered).
So, Assertion is false. Reason is correct.

JEE - 2023

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313331 Which represents the correct order of first ionisation potential of third period elements?

1

Na > Mg > Al > Si

2

Na < Mg < Al < Si

3

Na < Si < Al < Mg

4

Na < Al < Mg < Si

Explanation:

Generally, ionisation potential increases, as we move from left to right in a period. However, the ionisation potential of II A group elements is higher than that of the III A group elements. This is because of the fully-filled $s$ -orbitals in II A group elements.
Hence, the correct order of ionisation potential is
$Na < Al < Mg < Si$

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313328 The $I_{1}$ values of Li, Be and C are 5.4 eV/atom, 9.32 eV/atom and 11.26 eV/atom. The $I_{1}$ value of Boron is

1 13.6 eV/atom

2 8.29 eV/atom

3 14.5 eV/atom

4 21.5 eV/atom

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313329 Calculate the energy needed to convert three moles of sodium atoms in the gaseous state to sodium ions. The ionization energy of sodium is $495 k J m o l^{- 1} .$

1 1485 kJ

2 495 kJ

3 148.5 kJ

4 None

Explanation:

Energy needed to convert 1 mole of sodium (g) to sodium ions = 495 kJ
$∴$ Energy needed to convert 3 mole of Na (g) to $N a^{+} i o n s = 495 \times 3 = 1485 k J$

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313330 Read the Assertion and Reason carefully and mark the correct option
Assertion :
The first ionization enthalpy of 3d series elements is more than that of group 2 metals.
Reason :
In 3d series of elements successive filling of d-orbitals takes place.

1 Both Assertion and Reason are true and Reason is the correct explanation of Assertion.

2 Assertion is true but Reason is false.

3 Assertion is false but Reason is true.

4 Both Assertion and Reason are true but Reason is not the correct explanation of Assertion.

Explanation:

I.E. of $3 d -$ series elements in $k J / m o l$
$\underset{631}{S c} \underset{656}{T i} \underset{650}{V} \underset{653}{C r} \underset{717}{M n} \underset{762}{F e} \underset{758}{C o} \underset{736}{N i} \underset{745}{C u} \underset{906}{Z n}$
I.E. values in $k J / mol o f 2^{n d}$ group elements is
$\underset{899}{B e} \underset{737}{M g} \underset{590}{C a} \underset{549}{S r} \underset{503}{B a} \underset{509}{R a}$
From Sc to Mn , I.E. values are less than that of $M g (B e$ , a non-metal need not to be considered).
So, Assertion is false. Reason is correct.

JEE - 2023

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313331 Which represents the correct order of first ionisation potential of third period elements?

1

Na > Mg > Al > Si

2

Na < Mg < Al < Si

3

Na < Si < Al < Mg

4

Na < Al < Mg < Si

Explanation:

Generally, ionisation potential increases, as we move from left to right in a period. However, the ionisation potential of II A group elements is higher than that of the III A group elements. This is because of the fully-filled $s$ -orbitals in II A group elements.
Hence, the correct order of ionisation potential is
$Na < Al < Mg < Si$

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313328 The $I_{1}$ values of Li, Be and C are 5.4 eV/atom, 9.32 eV/atom and 11.26 eV/atom. The $I_{1}$ value of Boron is

1 13.6 eV/atom

2 8.29 eV/atom

3 14.5 eV/atom

4 21.5 eV/atom

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313329 Calculate the energy needed to convert three moles of sodium atoms in the gaseous state to sodium ions. The ionization energy of sodium is $495 k J m o l^{- 1} .$

1 1485 kJ

2 495 kJ

3 148.5 kJ

4 None

Explanation:

Energy needed to convert 1 mole of sodium (g) to sodium ions = 495 kJ
$∴$ Energy needed to convert 3 mole of Na (g) to $N a^{+} i o n s = 495 \times 3 = 1485 k J$

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313330 Read the Assertion and Reason carefully and mark the correct option
Assertion :
The first ionization enthalpy of 3d series elements is more than that of group 2 metals.
Reason :
In 3d series of elements successive filling of d-orbitals takes place.

1 Both Assertion and Reason are true and Reason is the correct explanation of Assertion.

2 Assertion is true but Reason is false.

3 Assertion is false but Reason is true.

4 Both Assertion and Reason are true but Reason is not the correct explanation of Assertion.

Explanation:

I.E. of $3 d -$ series elements in $k J / m o l$
$\underset{631}{S c} \underset{656}{T i} \underset{650}{V} \underset{653}{C r} \underset{717}{M n} \underset{762}{F e} \underset{758}{C o} \underset{736}{N i} \underset{745}{C u} \underset{906}{Z n}$
I.E. values in $k J / mol o f 2^{n d}$ group elements is
$\underset{899}{B e} \underset{737}{M g} \underset{590}{C a} \underset{549}{S r} \underset{503}{B a} \underset{509}{R a}$
From Sc to Mn , I.E. values are less than that of $M g (B e$ , a non-metal need not to be considered).
So, Assertion is false. Reason is correct.

JEE - 2023

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313331 Which represents the correct order of first ionisation potential of third period elements?

1

Na > Mg > Al > Si

2

Na < Mg < Al < Si

3

Na < Si < Al < Mg

4

Na < Al < Mg < Si

Explanation:

Generally, ionisation potential increases, as we move from left to right in a period. However, the ionisation potential of II A group elements is higher than that of the III A group elements. This is because of the fully-filled $s$ -orbitals in II A group elements.
Hence, the correct order of ionisation potential is
$Na < Al < Mg < Si$

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