Which of the following compound has a maximum "C$—$C" single bond length?

1. CH₂CHCCH        
2. HCCCCH  
3. CH₃CHCH₂        
4. CH₂CHCHCH₂

$BeC{l}_2$ is not isostructural with :

(1)$IC{l_2}^{-}$

(2) $C_2{H}_2$

(3) $Xe{F}_2$

(4) $GeC{l}_2$

Which statement is true about the most stable Lewis structure for $C{S}_2$ ?

(1) There are no lone pairs in molecule 

(2) All bonds are double bonds 

(3) The central atom does not have an octet of electrons 

(4) A sulfur atom must be the central atom for the stucture to be stable 

Minimum $\mathrm{F}—\mathrm{S}—\mathrm{F}$ bond angle present in:

1. ${\mathrm{SSF}}_{2<mspace\; width="1em"></mspace>}$                                                     

2. ${\mathrm{SF}}_6$

3. ${\mathrm{SF}}_2$                                                       

4. ${\mathrm{F}}_3\mathrm{SSF}$

$Sb{F}_5$ reacts with $Xe{F}_4$ and $Xe{F}_6$ to form ionic compounds $\left[Xe{F_3}^{+}\right]$ $\left[Sb{F_6}^{-}\right]$ and $\left[Xe{F_5}^{+}\right]$ $\left[Sb{F_6}^{-}\right]$ then molecular shape of $\left[Xe{F_3}^{+}\right]$ ion and $\left[Xe{F_5}^{+}\right]$ ion respectively :

(1) Square pyramidal, T-shaped 

(2) Bent T-shape, Square pyramidal

(3) See- saw , square pyramidal 

(4) Square pyramidal , See-saw

In which of the following species maximum atom can lie in same plane? 

1. XeF₂O₂

2. $PC{l}_5$

$\mathrm{3.\; A}s{H_4}^{+}$

4. $Xe{F}_4$

The geometry of ammonia molecule can be best described as:

The molecular geometry that is least likely to result from a trigonal bipyramidal electron geometry is:

Which of the following orbital can not form $\mathrm{\pi }$ as well as $\delta$-bond?

(1) $d_{xy}$                    (2) $d_{z^2}$

(3) $d_{x^2-y^2}$               (4) $d_{yz}$

Give the correct order of initials T and F for following statements. use T if statement is true and F if it is false :

(a) The order of repulsion betweeen different pair of electrons is $l_p-l_p>l_p-b_p>b_p-b_p$ 

(b) In general , as the number of lone pair of electrons on central atom increases, value of bond angle from normal bond angle also increases

(c) The number of lone pair on O in $H_{2}O$ is 2 while on N in $N{H}_3$ is 1 

(d) The structure of xeon fluorides and xenon oxyfluorides could not be explained on the basis of VSEPR 

(1) TTTF 

(2) TFTF

(3) TFTT 

(4) TFFF