Element A, B, C, D and E have the following electronic configurations
A: ` 1s ^(2) 2s ^(2) 2p ^(1) `
`B: 1s ^(2) 2s ^(2) 2p ^(6) 3s ^(2) 3p ^(1)`
`C:1s ^(2) 2s ^(2) 2p ^(6)3s ^(2) 3p ^(3)`
`D: 1s ^(2) 2s ^(2) 2p ^(6) 3s ^(2) 3p^(5)`
`E : 1s ^(2) 2s ^(2) 2p ^(6) 3s ^(2) 3p ^(6) 4s ^(2)`
Which among these will belong to the same group in the periodic table ?

Explanation

To determine which elements A, B, C, D, and E belong to the same group in the periodic table based on their electronic configurations, we will follow these steps:

### Step 1: Identify the Valence Shell
The valence shell is the outermost shell of an atom that contains electrons. The group of an element in the periodic table is determined by the number of valence electrons in this shell.

### Step 2: Write Down the Electronic Configurations
The electronic configurations provided are:
- A: `1s² 2s² 2p¹`
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