if value of spin quantum number`(s)=-1//2,0,+1//2` then calculate number of groups in the new form of periodic table if all other rules of electronic configurations are remain same.

Answer

To solve the problem of determining the number of groups in the new form of the periodic table with the given spin quantum numbers, we will follow these steps:

### Step 1: Understand the Spin Quantum Number
The spin quantum number (s) indicates the orientation of the electron's spin. In the standard model, electrons can have a spin of -1/2 or +1/2. However, in this case, we have three possible values: -1/2, 0, and +1/2.

### Step 2: Determine the Electron Filling in Orbitals
In the new configuration, each orbital can accommodate three electrons due to the three possible spin states. This means that for each type of orbital (s, p, d), we will fill the electrons differently.

### Step 3: Analyze Each Block of the Periodic Table
1. **s-block**:
- Normally, the s-block can hold 2 electrons (one for each spin state). With the new configuration, it can hold 3 electrons.
- Number of groups in s-block = 1 (since it can only accommodate one group of s orbitals).

2. **p-block**:
- The p-block can normally hold 6 electrons (2 per orbital for 3 orbitals). With the new configuration, each p orbital can hold 3 electrons.
- Number of groups in p-block = 3 (since there are 3 p orbitals).

3. **d-block**:
- The d-block can normally hold 10 electrons (2 per orbital for 5 orbitals). With the new configuration, each d orbital can hold 3 electrons.
- Number of groups in d-block = 5 (since there are 5 d orbitals).

### Step 4: Calculate Total Number of Groups
Now, we can sum the number of groups from each block:
- s-block: 1 group
- p-block: 3 groups
- d-block: 5 groups

Total groups = 1 (s-block) + 3 (p-block) + 5 (d-block) = 9 groups.

### Conclusion
The total number of groups in the new form of the periodic table, considering the spin quantum number values of -1/2, 0, and +1/2, is **9 groups**.

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