Chemical Bonding - Grade 10 MCQ

2,6        

2,8            

2,10        

2,9

SF₄        

OF₂            

OF₄        

O₂F₂

I,III        

I,II,V            

I,III,V        

I,II,IV

square planar    

trigonal bipyramidal    

tetrahedral    

trigonal pyramidal

sp,sp²,sp³    

sp³,sp²,sp        

sp²,sp³,sp    

sp²,sp,sp³

It contains a lone pair only on carbon        

It contains a lone pair only on oxygen                

In carbonyl, oxygen end is attached to the metal    

None of these atoms    

Methane molecule is tetrahedral in shape        

P₂O₅ is like two pyramids joined at their apices    

Nickel tetrachloride is square planar in shape  

Acetylene is linear

(SnCI₆)^2-        

(GeCI₆)^2-            

(CCI₆)^2-        

none of these exist

same as that of CI-Be-CI in BeCI₂            

greater than H-N-H bond angle in NH₃    

greater than H-Se-H and less than H-O-H        

same as CI-Sn-CI in SnCI₂

CF₄,SF₄        

PCI₃,BF₃            

XeF₂,CO₂    

PF₅,IF₅

Lone pair of electrons present on central atom can give rise to dipole moment    

Dipole moment is vector quantity    

CO₂ molecule has dipole moment    

Difference in electronegativities of combining atoms can lead to dipole moment

bonding molecular orbitals possess less energy than combining atomic orbitals    

bonding molecular orbitals have low electron density between the two nuclei.    

every electron in bonding molecular orbitals contributes to attraction between atoms    

they are formed when the lobes of the combining atomic orbitals have same sign.

BF₃ < NF₃ < PF₃ < CIF₃                

CIF₃ < PF₃ < NF₃ < BF₃    

BF₃ = NF₃ < PF₃ < 3CIF₃                

ClF₃ < NF₃ < PF₃ > BF₃

BeF^-₃

OH⁺₃        

NH⁺₄                

NF₃    

SO^2-₃

NO^-₃

NH₃

C(C₆H₅)^-₃

1        

2        

3/2            

1/2

CCI₄        

CH₄        

NH⁺₄

H₂O

BeF₂

H₂O

NH₃

CH₄

low bond energy                    

absence of bond polarity     

unsymmertical electron distribution        

 presence of more number of electrons in bonding orbitals.

H₂O molecule as linear while BeF₂ is bent        

BeF₂ molecule is linear while H₂O is bent    

fluorine is more electronegative than oxygen    

Be is more electronegative than oxygen

π-bond is formed when a sigma bond already formed    

π-bond is formed from hybrid orbitals    

π-bond may be formed by the overlapping of p-orbitals    

π-bond results from lateral overlap of atomic orbitals

PO^3-₄

NH⁺₄

SCl₄

SO^2-₄

Every AB₅ molecule does in fact have square pyramid structure.    

Multiple bonds are always shorter than corresponding single bonds.    

The electron-deficient molecules can act as Lewis acids    

The canonical structures have no real existence.

RbF        

CsF        

NaF        

KF

CIO₂        

SO₂        

CO₂        

SiO₂

Dissimilar in hybridization for the central atom with different structure    

Isostructural with same hybridization for the central atom.    

Isostruectural with different hybridization for the central atom.    

Similar is hybridization for the central atom with different structure

8

12

16

4

T F T F    

T T F F        

F T T T        

F T F T

Paramagnetic behaviour decreases when it undergoes in dimerization    

It is coloured in its dimeric form.    

The colour is due to the presence of unpaired electron.    

It is an odd elecetron molecules.