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- The element with atomic number 35 belongs to which group:Option: 1 13th groupOption: 2 17th
- #Joint Entrance Examination Main
- #Engineering
- #Chemistry
- #Classification of Elements and Periodic table
- #National Eligilibility Cum Entrance Test
The element with atomic number 35 belongs to which group:
13th group
17th group
16th group
2nd group
Answers (1)
How to find Group, Periods and Blocks of any element -
Period
The period of any element is determined by the last shell in which the last electrons enters. For example, Fe atomic number is 26. The electronic configuration can be written as:
1s22s22p63s23p64s23d6
Now, the last electron enters into the d-subshell and shell is 3. Therefore, Fe belongs to third period.
Block
The block of any element is determined by the last subshell in which the last electron enters. For example, Na has atomic number 11, thus its electronic configuration can be written as:
1s22s22p63s1
Now, its last electron enters into the s-subshell, therefore, Na belongs to the s-block.
Group
The group of any element is determined in different ways.
For p-block
If the last electron of any element enters into the p-subshell, then the group number is equal to (12 + the number of electrons in the last p-subshell).
For example, Ge has atomic number 32, thus its electronic configuration can be written as:
1s22s22p63s23p64s23d104p2
Now, it has 2 electrons in the last p-subshell, therefore its group number is:
12 + 2 = 14
Thus, Ge belongs to Group 14
-
The electronic configuration of the element with atomic number 35 is:
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5
Now, the group of the element is determined by the following formulae:
(i) For s-block: ns1 and ns2
(ii) For p-block: 12 + number of electrons in P-subshell of last shell.
=12 + 5 =17th group
(iii) For d-block: 2 + number of electrons in (n-1)d subshell.
Therefore, Option(2) is correct.
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