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CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313370 Among the following processes, the one that requires largest amount of energy is

1

A l (g) \to A l^{+} (g) + e^{-}

2

A l^{+} (g) \to A l^{2 +} (g) + e^{-}

3

A l^{2 +} (g) \to A l^{3 +} (g) + e^{-}

4 All the above processes require same amount of energy

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313371 Sodium forms $N a^{+}$ ion but it does not form $N a^{+ 2}$ because

1 Very low value of

I E_{1} a n d I E_{2}

2 Very high value of

I E_{1} a n d I E_{2}

3 Low value of

I E_{1} a n d

and low value of

I E_{2}

4 Low value of

I E_{1} a n d

high value of

I E_{2}

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313372 A large difference between the fourth and fifth ionization energies indicates the presence of

1 4 valence electrons in an atom

2 5 valence electrons in an atom

3 3 valence electrons in an atom

4 8 valence electrons in an atom

Explanation:

After four electrons, ion gets stability so it has great ${IP}_{5}$ . It means it has 4 valence electrons.

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313373 The ionisation energy of B and Al as compared to Be and Mg are

1 Lower

2 Higher

3 Equal

4 None of these

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313374 Arrange the following elements in increasing order of first ionization enthalpy:
$Li, Be, B, C, N$
Choose the correct answer from the options given below:

1

Li < Be < B < C < N

2

Li < B < Be < C < N

3

Li < Be < C < B < N

4

Li < Be < N < B < C

Explanation:

The penetration of a 2 s -electron to the nucleus is more than that of a 2 p -electron; hence the $2 p$ electron of boron is more shielded from the nucleus by the inner core of electrons than the 2 s electrons of beryllium. Therefore, it is easier to remove the $2 p$ -electron from boron compared to the removal of a 2 s - electron from beryllium. Thus, boron has a smaller first ionization enthalpy than beryllium. From left to right,i.e, increases. Hence ,the order is $Li < B < Be < C < N$ .

NEET - 2024

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313370 Among the following processes, the one that requires largest amount of energy is

1

A l (g) \to A l^{+} (g) + e^{-}

2

A l^{+} (g) \to A l^{2 +} (g) + e^{-}

3

A l^{2 +} (g) \to A l^{3 +} (g) + e^{-}

4 All the above processes require same amount of energy

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313371 Sodium forms $N a^{+}$ ion but it does not form $N a^{+ 2}$ because

1 Very low value of

I E_{1} a n d I E_{2}

2 Very high value of

I E_{1} a n d I E_{2}

3 Low value of

I E_{1} a n d

and low value of

I E_{2}

4 Low value of

I E_{1} a n d

high value of

I E_{2}

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313372 A large difference between the fourth and fifth ionization energies indicates the presence of

1 4 valence electrons in an atom

2 5 valence electrons in an atom

3 3 valence electrons in an atom

4 8 valence electrons in an atom

Explanation:

After four electrons, ion gets stability so it has great ${IP}_{5}$ . It means it has 4 valence electrons.

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313373 The ionisation energy of B and Al as compared to Be and Mg are

1 Lower

2 Higher

3 Equal

4 None of these

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313374 Arrange the following elements in increasing order of first ionization enthalpy:
$Li, Be, B, C, N$
Choose the correct answer from the options given below:

1

Li < Be < B < C < N

2

Li < B < Be < C < N

3

Li < Be < C < B < N

4

Li < Be < N < B < C

Explanation:

The penetration of a 2 s -electron to the nucleus is more than that of a 2 p -electron; hence the $2 p$ electron of boron is more shielded from the nucleus by the inner core of electrons than the 2 s electrons of beryllium. Therefore, it is easier to remove the $2 p$ -electron from boron compared to the removal of a 2 s - electron from beryllium. Thus, boron has a smaller first ionization enthalpy than beryllium. From left to right,i.e, increases. Hence ,the order is $Li < B < Be < C < N$ .

NEET - 2024

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313370 Among the following processes, the one that requires largest amount of energy is

1

A l (g) \to A l^{+} (g) + e^{-}

2

A l^{+} (g) \to A l^{2 +} (g) + e^{-}

3

A l^{2 +} (g) \to A l^{3 +} (g) + e^{-}

4 All the above processes require same amount of energy

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313371 Sodium forms $N a^{+}$ ion but it does not form $N a^{+ 2}$ because

1 Very low value of

I E_{1} a n d I E_{2}

2 Very high value of

I E_{1} a n d I E_{2}

3 Low value of

I E_{1} a n d

and low value of

I E_{2}

4 Low value of

I E_{1} a n d

high value of

I E_{2}

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313372 A large difference between the fourth and fifth ionization energies indicates the presence of

1 4 valence electrons in an atom

2 5 valence electrons in an atom

3 3 valence electrons in an atom

4 8 valence electrons in an atom

Explanation:

After four electrons, ion gets stability so it has great ${IP}_{5}$ . It means it has 4 valence electrons.

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313373 The ionisation energy of B and Al as compared to Be and Mg are

1 Lower

2 Higher

3 Equal

4 None of these

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313374 Arrange the following elements in increasing order of first ionization enthalpy:
$Li, Be, B, C, N$
Choose the correct answer from the options given below:

1

Li < Be < B < C < N

2

Li < B < Be < C < N

3

Li < Be < C < B < N

4

Li < Be < N < B < C

Explanation:

The penetration of a 2 s -electron to the nucleus is more than that of a 2 p -electron; hence the $2 p$ electron of boron is more shielded from the nucleus by the inner core of electrons than the 2 s electrons of beryllium. Therefore, it is easier to remove the $2 p$ -electron from boron compared to the removal of a 2 s - electron from beryllium. Thus, boron has a smaller first ionization enthalpy than beryllium. From left to right,i.e, increases. Hence ,the order is $Li < B < Be < C < N$ .

NEET - 2024

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313370 Among the following processes, the one that requires largest amount of energy is

1

A l (g) \to A l^{+} (g) + e^{-}

2

A l^{+} (g) \to A l^{2 +} (g) + e^{-}

3

A l^{2 +} (g) \to A l^{3 +} (g) + e^{-}

4 All the above processes require same amount of energy

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313371 Sodium forms $N a^{+}$ ion but it does not form $N a^{+ 2}$ because

1 Very low value of

I E_{1} a n d I E_{2}

2 Very high value of

I E_{1} a n d I E_{2}

3 Low value of

I E_{1} a n d

and low value of

I E_{2}

4 Low value of

I E_{1} a n d

high value of

I E_{2}

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313372 A large difference between the fourth and fifth ionization energies indicates the presence of

1 4 valence electrons in an atom

2 5 valence electrons in an atom

3 3 valence electrons in an atom

4 8 valence electrons in an atom

Explanation:

After four electrons, ion gets stability so it has great ${IP}_{5}$ . It means it has 4 valence electrons.

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313373 The ionisation energy of B and Al as compared to Be and Mg are

1 Lower

2 Higher

3 Equal

4 None of these

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313374 Arrange the following elements in increasing order of first ionization enthalpy:
$Li, Be, B, C, N$
Choose the correct answer from the options given below:

1

Li < Be < B < C < N

2

Li < B < Be < C < N

3

Li < Be < C < B < N

4

Li < Be < N < B < C

Explanation:

The penetration of a 2 s -electron to the nucleus is more than that of a 2 p -electron; hence the $2 p$ electron of boron is more shielded from the nucleus by the inner core of electrons than the 2 s electrons of beryllium. Therefore, it is easier to remove the $2 p$ -electron from boron compared to the removal of a 2 s - electron from beryllium. Thus, boron has a smaller first ionization enthalpy than beryllium. From left to right,i.e, increases. Hence ,the order is $Li < B < Be < C < N$ .

NEET - 2024

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313370 Among the following processes, the one that requires largest amount of energy is

1

A l (g) \to A l^{+} (g) + e^{-}

2

A l^{+} (g) \to A l^{2 +} (g) + e^{-}

3

A l^{2 +} (g) \to A l^{3 +} (g) + e^{-}

4 All the above processes require same amount of energy

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313371 Sodium forms $N a^{+}$ ion but it does not form $N a^{+ 2}$ because

1 Very low value of

I E_{1} a n d I E_{2}

2 Very high value of

I E_{1} a n d I E_{2}

3 Low value of

I E_{1} a n d

and low value of

I E_{2}

4 Low value of

I E_{1} a n d

high value of

I E_{2}

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313372 A large difference between the fourth and fifth ionization energies indicates the presence of

1 4 valence electrons in an atom

2 5 valence electrons in an atom

3 3 valence electrons in an atom

4 8 valence electrons in an atom

Explanation:

After four electrons, ion gets stability so it has great ${IP}_{5}$ . It means it has 4 valence electrons.

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313373 The ionisation energy of B and Al as compared to Be and Mg are

1 Lower

2 Higher

3 Equal

4 None of these

CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

313374 Arrange the following elements in increasing order of first ionization enthalpy:
$Li, Be, B, C, N$
Choose the correct answer from the options given below:

1

Li < Be < B < C < N

2

Li < B < Be < C < N

3

Li < Be < C < B < N

4

Li < Be < N < B < C

Explanation:

The penetration of a 2 s -electron to the nucleus is more than that of a 2 p -electron; hence the $2 p$ electron of boron is more shielded from the nucleus by the inner core of electrons than the 2 s electrons of beryllium. Therefore, it is easier to remove the $2 p$ -electron from boron compared to the removal of a 2 s - electron from beryllium. Thus, boron has a smaller first ionization enthalpy than beryllium. From left to right,i.e, increases. Hence ,the order is $Li < B < Be < C < N$ .

NEET - 2024