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. ${\mathrm{SSF}}_{2 }$                                                     

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:

(1) Nitrogen at one vertex of a regular tetrahedron, the other three vertices being occupied by three hydrogens 

(2) Nitrogen at the centre of the tetrahedron, three vertics being occupied by three hydrogens

(3) Nitrogen at the centre of an equilateral triangle, three corners being occupied by three hydrogens 

(4) Nitrogen at the junction of a T, three open ends being occupied by three hydrogens  

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

Which species is planar?

(a)$C{O_3}^{2-}$

(b) $S{O_3}^{2-}$

(c) $Cl{O_3}^{-}$

(d) $B{F_4}^{-}$

On the left are given decreasing orders of elements for a certain property and on right side is given the property. The incorrect order for the given properties is:

1. ${\mathrm{AlF}}_3>\mathrm{MgO}>{\mathrm{MgF}}_2$    : Lattice energy

2. $\mathrm{Li}>\mathrm{Na}>\mathrm{Al}>\mathrm{Mg}$       : Electron affinity

3. ${\mathrm{PF}}_5>$ ${\mathrm{SF}}_6$ $>$ ${\mathrm{SiF}}_4$    : Lewis acidic character

4. ${\mathrm{SiCl}}_4>{\mathrm{SiBr}}_4$ $>{\mathrm{SiI}}_4$   : Decreasing ionic character