Chemistry
Assertion (A): Noble gases Ne, Ar have electron affinity zero.
Reason (R): Greater the value of electron affinity, the more electronegative is the element.
- Both A & R are true and R is the correct explanation of A.
- Both A & R are true but R is not the correct explanation of A.
- A is true but R is false
- A is false but R is true.
Periodic Table
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Answer
Both A & R are true but R is not the correct explanation of A.
Reason — Noble gas elements have completely filled outer-shell. Such electronic configurations are highly stable and as such noble gases find it difficult to accept electrons. Thus electron affinity of noble gas elements is zero. Hence, the assertion (A) is true.
Elements with high electron affinity tend to strongly attract electrons, and are therefore usually more electronegative. So, greater the value of electron affinity, the more electronegative is the element. Hence, the reason (R) is true but it doesn't explain why nobel gases have zero electron affinity.
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Related Questions
Identify the following:
(a) An element in period 1 which can be placed in both group 1 and group 17 of the Periodic Table.
(b) The element having electronic configuration 2, 8, 6.
(c) The most electronegative element of period 3.
The following table shows the electronic configuration of the atoms A, B, C and D.
Element A B C D Electronic configuration 2, 8, 8, 2 2, 6 2, 8, 7 2, 4 (a) Write the formula of the compound formed between:
- A and B
- D and C
(b) Which of the above elements will exhibit catenation?
Assertion (A): Elements with high electronegativity are usually non-metals.
Reason (R): Non-metallic atoms have high ionisation potential & tend to gain electrons.
- Both A & R are true and R is the correct explanation of A.
- Both A & R are true but R is not the correct explanation of A.
- A is true but R is false
- A is false but R is true.
The oxide of the metallic element with three valence electrons, in its third shell is:
- Basic
- Weakly acidic
- Amphoteric
- Strongly basic