Test: Hybridisation (NCERT) - NEET MCQ

The hybridised orbitals have different energies for each orbital

The number of hybrid orbitals is equal to the number of atomic orbitals that are hybridised

Hybrid orbitals form multiple bonds

The orbitals with different energies undergo hybridisation

CH₄

CO₂

BF₃

BeF₂

sp²- hybridised

sp³d - hybridised

Sp - hybridised

sp³ - hybridised

sp², sp² sp

sp², sp, sp

sp, sp², sp³

sp³, sp², sp

Four orbitals with tetrahedral orientation

Three orbitals with trigonal orientation

Two orbitals with linear orientation

Two orbitals with perpendicular orientation

dsp³

dsp²

sp³d

sp³d²

SF₆

BeF₅

PCl₅

[Ni(CN)₄]^2-

SO^2-₄ and BF^-₄

NH₃ and NH⁺₄

CO₃^2- and CO₂

CH₄ and BF₃

sp², sp³d, sp³d²

sp³d, sp³d², sp³d³

sp³d², sp³d, sp³d³

sp², sp³, sp³d

sp²,sp,sp³

sp, sp², sp³

sp³,sp²,sp

sp², sp³, sp

dsp²−90^∘

sp³d²−90^∘

sp³d−90^∘

sp³−109.5^∘

sp³ < sp² < sp 

sp < sp² < sp³ 

sp² < sp < sp³ 

sp² < sp³ < sp 

(A)→(i),(B)→(iii),(C)→(ii),(D)→(iv) 

(A)→(iii),(B)→(i),(C)→(iv),(D)→(ii)

(A)→(ii),(B)→(iii),(C)→(i),(D)→(iv)

(A)→(iv),(B)→(i),(C)→(iii),(D)→(ii)

sp² hybridised orbitals form sigma bond while the unhybridised (p_x or p_y) overlaps sidewiseto form π-bond

sp² hybridised orbitals form π-bond while the unhybridised (p_z) overlaps to form σ-bond

sp² hybridised orbitals overlap with s-orbitals of H atoms while unhybridised orbitals form C—C bond

sp² hybridised orbitals form sigma bonds with H atoms while unhybridised orbitals form π-bonds between C atoms

Due to octahedral shape ofSatoms

Due to presence of vacant 3d-orbitals which provide 6 unpaired electrons in excited state

Due to sp³ hybridisation of S atom which provides 6 electrons to 6 F atoms

Due to presence of 3 sigma and 3 pi bonds between S and F