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Linear combination of two hybridised orb...

Linear combination of two hybridised orbitals belonging to the two atoms , each having one electron leads to a

A

(a) sigma bond

B

(b) double bond

C

(c) coordinate bond

D

(d) pi-bond

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To solve the question regarding the linear combination of two hybridized orbitals from two atoms, each having one electron, we can follow these steps: ### Step-by-Step Solution: 1. **Understanding Hybridization**: - Hybridization involves the mixing of atomic orbitals to form new hybrid orbitals that can participate in bonding. Each hybrid orbital can hold a maximum of two electrons. 2. **Identifying the Orbitals**: - In this case, we are considering two hybridized orbitals from two different atoms, each containing one unpaired electron. 3. **Linear Combination of Orbitals**: - The linear combination of two orbitals refers to the mathematical addition of their wave functions. When two orbitals combine, they can overlap in two ways: end-to-end (sigma bond) or side-to-side (pi bond). 4. **Formation of Sigma Bond**: - The end-to-end overlapping of the two hybridized orbitals leads to the formation of a sigma bond. This type of bond is characterized by the electron density being concentrated along the axis connecting the two nuclei. 5. **Examples**: - For instance, if we take two hydrogen atoms, each with one electron in their 1s orbital, the linear combination of these orbitals results in a sigma bond (σ). Similarly, if we consider two 2pz orbitals from different atoms, their linear combination also results in a sigma bond (σ). 6. **Excluding Other Options**: - A double bond involves both a sigma bond and a pi bond, which is not formed through linear combination of hybridized orbitals. A coordinate bond is formed when one atom donates both electrons to the bond, which is not the case here. A pi bond is formed through side-to-side overlap, which again does not apply to this scenario. 7. **Conclusion**: - Therefore, the linear combination of two hybridized orbitals from two atoms, each containing one electron, leads to the formation of a sigma bond. ### Final Answer: The answer is **Option A: Sigma bond**.
To solve the question regarding the linear combination of two hybridized orbitals from two atoms, each having one electron, we can follow these steps: ### Step-by-Step Solution: 1. **Understanding Hybridization**: - Hybridization involves the mixing of atomic orbitals to form new hybrid orbitals that can participate in bonding. Each hybrid orbital can hold a maximum of two electrons. 2. **Identifying the Orbitals**: ...
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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 beloging to sasme atom but in different sub-shells so as to intermix and redistibute energies to from equivalent orbitals called hybrid orbitals.Depending upon toh enumber 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. The d-orbital involved in dsp^(2) hybridisation is:

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