CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313299
For the second period elements the correct increasing order of first ionisation enthalpy is:
1 Li < Be < B < C < N < O < F < Ne
2 Li < B < Be < C < O < N < F < Ne
3 Li < B < Be < C < N < O < F < Ne
4 Li < Be < B < C < O < N < F < Ne
Explanation:
‘Be’ and ‘N’ have comparatively more stable valence sub-shell than ‘B’ and ‘O’. \(\therefore \) Correct order of first ionisation enthalpy is: Li < B < Be < C < O < N < F < Ne
NEET - 2019
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313130
The diagonal relationship in Be and Al is due to
1 similar ionisation enthlapy
2 similar metallic character
3 similar ionic size and charge/radius ratio
4 similar electronegativity
Explanation:
The diagonal relationship in Be and Al is due to similar ionic size and charge/radius ratio. Generally, on moving from left to right across a period, the ionic charge increases to maximum and then decreases, while the ionic size decreases, causing an increase in its polarising power (Fajan’s rule). On the other hand, on moving down a group the ionic charge remains the same while ionic size increases. Therefore, polarising power decreases. On moving diagonally, these two effects partly balance each other and therefore, there is no marked change in their properties.
MHTCET - 2019
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313131
Statement A : Be and Al show some similar properties. Statement B : The metallic radius of Be is less than the metallic radius of Al.
1 Statement A is correct but statement B is incorrect
2 Statement A is incorrect but statement B is correct
3 Both statements are correct
4 Both statements are incorrect
Explanation:
Be and Al show diagonal relationship because Be resembles their properties with Al. So, the option (3) is correct.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313132
Among the following pairs of elements, the pair that is different from others is
1 Lithium and Magnesium
2 Nitrogen and Phosphorus
3 Beryllium and Aluminium
4 Boron and Silicon
Explanation:
Boron and Silicon belong to two different groups. Thus, they do not share common properties. But the pairs of elements given in the other options have similar properties as they either belong to the same group or are diagonally related. Nitrogen and Phosphorus belong to group 15. Li and Mg diagonally related. Similarly, Be and AI have diagonal relationship. So correct option is (4).
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313299
For the second period elements the correct increasing order of first ionisation enthalpy is:
1 Li < Be < B < C < N < O < F < Ne
2 Li < B < Be < C < O < N < F < Ne
3 Li < B < Be < C < N < O < F < Ne
4 Li < Be < B < C < O < N < F < Ne
Explanation:
‘Be’ and ‘N’ have comparatively more stable valence sub-shell than ‘B’ and ‘O’. \(\therefore \) Correct order of first ionisation enthalpy is: Li < B < Be < C < O < N < F < Ne
NEET - 2019
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313130
The diagonal relationship in Be and Al is due to
1 similar ionisation enthlapy
2 similar metallic character
3 similar ionic size and charge/radius ratio
4 similar electronegativity
Explanation:
The diagonal relationship in Be and Al is due to similar ionic size and charge/radius ratio. Generally, on moving from left to right across a period, the ionic charge increases to maximum and then decreases, while the ionic size decreases, causing an increase in its polarising power (Fajan’s rule). On the other hand, on moving down a group the ionic charge remains the same while ionic size increases. Therefore, polarising power decreases. On moving diagonally, these two effects partly balance each other and therefore, there is no marked change in their properties.
MHTCET - 2019
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313131
Statement A : Be and Al show some similar properties. Statement B : The metallic radius of Be is less than the metallic radius of Al.
1 Statement A is correct but statement B is incorrect
2 Statement A is incorrect but statement B is correct
3 Both statements are correct
4 Both statements are incorrect
Explanation:
Be and Al show diagonal relationship because Be resembles their properties with Al. So, the option (3) is correct.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313132
Among the following pairs of elements, the pair that is different from others is
1 Lithium and Magnesium
2 Nitrogen and Phosphorus
3 Beryllium and Aluminium
4 Boron and Silicon
Explanation:
Boron and Silicon belong to two different groups. Thus, they do not share common properties. But the pairs of elements given in the other options have similar properties as they either belong to the same group or are diagonally related. Nitrogen and Phosphorus belong to group 15. Li and Mg diagonally related. Similarly, Be and AI have diagonal relationship. So correct option is (4).
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313299
For the second period elements the correct increasing order of first ionisation enthalpy is:
1 Li < Be < B < C < N < O < F < Ne
2 Li < B < Be < C < O < N < F < Ne
3 Li < B < Be < C < N < O < F < Ne
4 Li < Be < B < C < O < N < F < Ne
Explanation:
‘Be’ and ‘N’ have comparatively more stable valence sub-shell than ‘B’ and ‘O’. \(\therefore \) Correct order of first ionisation enthalpy is: Li < B < Be < C < O < N < F < Ne
NEET - 2019
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313130
The diagonal relationship in Be and Al is due to
1 similar ionisation enthlapy
2 similar metallic character
3 similar ionic size and charge/radius ratio
4 similar electronegativity
Explanation:
The diagonal relationship in Be and Al is due to similar ionic size and charge/radius ratio. Generally, on moving from left to right across a period, the ionic charge increases to maximum and then decreases, while the ionic size decreases, causing an increase in its polarising power (Fajan’s rule). On the other hand, on moving down a group the ionic charge remains the same while ionic size increases. Therefore, polarising power decreases. On moving diagonally, these two effects partly balance each other and therefore, there is no marked change in their properties.
MHTCET - 2019
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313131
Statement A : Be and Al show some similar properties. Statement B : The metallic radius of Be is less than the metallic radius of Al.
1 Statement A is correct but statement B is incorrect
2 Statement A is incorrect but statement B is correct
3 Both statements are correct
4 Both statements are incorrect
Explanation:
Be and Al show diagonal relationship because Be resembles their properties with Al. So, the option (3) is correct.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313132
Among the following pairs of elements, the pair that is different from others is
1 Lithium and Magnesium
2 Nitrogen and Phosphorus
3 Beryllium and Aluminium
4 Boron and Silicon
Explanation:
Boron and Silicon belong to two different groups. Thus, they do not share common properties. But the pairs of elements given in the other options have similar properties as they either belong to the same group or are diagonally related. Nitrogen and Phosphorus belong to group 15. Li and Mg diagonally related. Similarly, Be and AI have diagonal relationship. So correct option is (4).
NEET Test Series from KOTA - 10 Papers In MS WORD
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CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313299
For the second period elements the correct increasing order of first ionisation enthalpy is:
1 Li < Be < B < C < N < O < F < Ne
2 Li < B < Be < C < O < N < F < Ne
3 Li < B < Be < C < N < O < F < Ne
4 Li < Be < B < C < O < N < F < Ne
Explanation:
‘Be’ and ‘N’ have comparatively more stable valence sub-shell than ‘B’ and ‘O’. \(\therefore \) Correct order of first ionisation enthalpy is: Li < B < Be < C < O < N < F < Ne
NEET - 2019
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313130
The diagonal relationship in Be and Al is due to
1 similar ionisation enthlapy
2 similar metallic character
3 similar ionic size and charge/radius ratio
4 similar electronegativity
Explanation:
The diagonal relationship in Be and Al is due to similar ionic size and charge/radius ratio. Generally, on moving from left to right across a period, the ionic charge increases to maximum and then decreases, while the ionic size decreases, causing an increase in its polarising power (Fajan’s rule). On the other hand, on moving down a group the ionic charge remains the same while ionic size increases. Therefore, polarising power decreases. On moving diagonally, these two effects partly balance each other and therefore, there is no marked change in their properties.
MHTCET - 2019
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313131
Statement A : Be and Al show some similar properties. Statement B : The metallic radius of Be is less than the metallic radius of Al.
1 Statement A is correct but statement B is incorrect
2 Statement A is incorrect but statement B is correct
3 Both statements are correct
4 Both statements are incorrect
Explanation:
Be and Al show diagonal relationship because Be resembles their properties with Al. So, the option (3) is correct.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313132
Among the following pairs of elements, the pair that is different from others is
1 Lithium and Magnesium
2 Nitrogen and Phosphorus
3 Beryllium and Aluminium
4 Boron and Silicon
Explanation:
Boron and Silicon belong to two different groups. Thus, they do not share common properties. But the pairs of elements given in the other options have similar properties as they either belong to the same group or are diagonally related. Nitrogen and Phosphorus belong to group 15. Li and Mg diagonally related. Similarly, Be and AI have diagonal relationship. So correct option is (4).
