Central atom may exhibit `sp^(3)` hybridisation in how many of the following species:
(a)`CO_(2)` , (b)Graphite , ( c)Diamond , (d)`CO`
(e)`H_(3)BO_(3) (aq)` , (f)Zeolites `(Si`-central) , (g)Silicones `(Si)`
(h)Chlorosilane `(Si)`
(i)Borax (Boron) , (j) `Al_(2)Cl_(6)` , (k)`B_(2)H_(6)` , (l)`SiO_(2)`
(m)`H_(2)CO_(3)` , (n)`COCl_(2)` , (o)`CH_(4)` , (p)`C Cl_(4)`

Explanation

To determine how many of the given species exhibit `sp^(3)` hybridization, we will analyze each species one by one.

1. **CO₂ (Carbon Dioxide)**:
- Structure: O=C=O
- Hybridization: Carbon is bonded to two oxygen atoms with double bonds, hence it is `sp` hybridized.

2. **Graphite**:
- Structure: Layers of carbon atoms bonded in a planar structure.
- Hybridization: Each carbon atom is bonded to three other carbon atoms in a planar arrangement, hence it is `sp²` hybridized.

3. **Diamond**:
- Structure: Each carbon atom is tetrahedrally bonded to four other carbon atoms.
- Hybridization: Therefore, carbon in diamond is `sp³` hybridized.

4. **CO (Carbon Monoxide)**:
- Structure: C≡O
- Hybridization: Carbon is bonded to one oxygen atom with a triple bond and has one lone pair, making it `sp` hybridized.

5. **H₃BO₃ (Boric Acid)**:
- Structure: B(OH)₃
- Hybridization: Boron is bonded to three hydroxyl groups, hence it is `sp²` hybridized.

6. **Zeolites (Si-central)**:
- Structure: SiO₄ tetrahedra connected by oxygen atoms.
- Hybridization: Silicon is bonded to four oxygen atoms, hence it is `sp³` hybridized.

7. **Silicones (Si)**:
- Structure: Si-O-Si chains with organic groups.
- Hybridization: Each silicon atom is bonded to four groups (either R groups or oxygen), hence it is `sp³` hybridized.

8. **Chlorosilane (Si)**:
- Structure: SiCl₄ or similar.
- Hybridization: Silicon is bonded to four groups (two Cl and two R groups), hence it is `sp³` hybridized.

9. **Borax (Boron)**:
- Structure: Na₂B₄O₇·10H₂O
- Hybridization: One boron atom is `sp³` hybridized while the others are `sp²` hybridized.

10. **Al₂Cl₆ (Aluminum Chloride)**:
- Structure: Dimeric form where each aluminum is bonded to four chlorines.
- Hybridization: In the dimerized form, aluminum exhibits `sp³` hybridization.

11. **B₂H₆ (Diborane)**:
- Structure: B-H bonds with a unique bridging structure.
- Hybridization: Each boron atom is bonded to four hydrogen atoms, hence it is `sp³` hybridized.

12. **SiO₂ (Silicon Dioxide)**:
- Structure: Network solid with tetrahedral SiO₄ units.
- Hybridization: Silicon is bonded to four oxygen atoms, hence it is `sp³` hybridized.

13. **H₂CO₃ (Carbonic Acid)**:
- Structure: H₂C(=O)(OH)₂
- Hybridization: Carbon is bonded to three groups (two OH and one C=O), hence it is `sp²` hybridized.

14. **COCl₂ (Phosgene)**:
- Structure: C(=O)(Cl)₂
- Hybridization: Carbon is bonded to two chlorine atoms and one carbonyl oxygen, hence it is `sp²` hybridized.

15. **CH₄ (Methane)**:
- Structure: Tetrahedral with four hydrogen atoms.
- Hybridization: Carbon is bonded to four hydrogen atoms, hence it is `sp³` hybridized.

16. **CCl₄ (Carbon Tetrachloride)**:
- Structure: Tetrahedral with four chlorine atoms.
- Hybridization: Carbon is bonded to four chlorine atoms, hence it is `sp³` hybridized.

### Summary of Hybridization:
- **sp³ Hybridized**: Diamond, Zeolites, Silicones, Chlorosilane, one Boron in Borax, Al₂Cl₆, B₂H₆, SiO₂, CH₄, CCl₄
- **Total Count of sp³ Hybridized Species**: 10

### Final Answer:
The central atom may exhibit `sp^(3)` hybridization in **10** of the given species.