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The concept of hybridisation has been in...

The concept of hybridisation has been introduced to explain the shapes of molecules. It involves the intermixing of two or more atomic orbitals belonging to same atom but in or more atomic orbitals belonging to same atom but in different sub-shells so as to intermix and redistribute energies to from equivalent orbitals called hybrid orbitals. Depending upon total number and nature of the orbitals involved, the hybridisation may be divided into sp (linear), `sp^(2)` (trigonal), `sp^(3)` (tetrahedral), `sp^(3)d` (trigonal bipyramidal), `sp^(3)d^(3)` (octahedral) and `sp^(3)d^(3)` (pentagonal bipyramidal) types. it may be noted that the orbitals of isolated atoms never hybridise and they do so at the time of bond formation.
Which carbon is maximum electronegative ?

A

`sp^(3)`-hybridise carbon

B

sp-hybridised carbon

C

`sp^(2)`-hybridised carbon

D

the electron attracting power of carbon is always the same irrespective of its hybrid state.

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To determine which carbon is the most electronegative based on hybridization, we can follow these steps: ### Step 1: Understand Hybridization and Electronegativity Hybridization involves the mixing of atomic orbitals to form new hybrid orbitals. The type of hybridization affects the percentage of s character in the hybrid orbitals, which in turn influences electronegativity. The more s character an orbital has, the more electronegative the atom tends to be. ### Step 2: Identify the Hybridization Types The common types of hybridization for carbon are: - **sp**: Linear (2 orbitals, steric number = 2) - **sp²**: Trigonal planar (3 orbitals, steric number = 3) - **sp³**: Tetrahedral (4 orbitals, steric number = 4) ### Step 3: Calculate the Percentage of s Character The percentage of s character for each type of hybridization can be calculated using the formula: \[ \text{Percentage of s character} = \left( \frac{\text{Number of s orbitals}}{\text{Total number of orbitals}} \right) \times 100 \] - For **sp** hybridization: - Number of s orbitals = 1 - Total orbitals = 2 - Percentage of s character = \( \frac{1}{2} \times 100 = 50\% \) - For **sp²** hybridization: - Number of s orbitals = 1 - Total orbitals = 3 - Percentage of s character = \( \frac{1}{3} \times 100 \approx 33.33\% \) - For **sp³** hybridization: - Number of s orbitals = 1 - Total orbitals = 4 - Percentage of s character = \( \frac{1}{4} \times 100 = 25\% \) ### Step 4: Compare the Percentages Now we compare the percentages of s character: - **sp**: 50% - **sp²**: 33.33% - **sp³**: 25% ### Step 5: Determine Maximum Electronegativity Since the percentage of s character is directly proportional to electronegativity, the carbon with **sp** hybridization (50% s character) is the most electronegative. ### Conclusion The carbon that is maximum electronegative is the one that is **sp hybridized**. ---
To determine which carbon is the most electronegative based on hybridization, we can follow these steps: ### Step 1: Understand Hybridization and Electronegativity Hybridization involves the mixing of atomic orbitals to form new hybrid orbitals. The type of hybridization affects the percentage of s character in the hybrid orbitals, which in turn influences electronegativity. The more s character an orbital has, the more electronegative the atom tends to be. ### Step 2: Identify the Hybridization Types The common types of hybridization for carbon are: - **sp**: Linear (2 orbitals, steric number = 2) ...
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