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This is one of our many quizzes on Molecular geometry. Click on this to access more such competitive quizzes on Physical Chemistry.

Molecular geometry Quiz 2

chemistry

 What is the geometry of the molecules having: $ \\ $ $(1)$ Bonding electron pair $= 4$ $ \\ $ Lone pair $= 2$ $ \\ $ Bond angle = ${{90}^{\circ }},{{180}^{\circ }}$   $ \\ $ $(2)$ Bonding electron pair $= 5$ $ \\ $ Lone pair $= 0$ $ \\ $ Bond angle $= {{120}^{\circ }},{{90}^{\circ }},{{180}^{\circ }}$  

 $(1)$ The geometry having Bonding electron pair=4; Lone pair=2 and Bond angle = ${{90}^{\circ }},{{180}^{\circ }}$ is square planar. $ \\ $ $(2)$ The geometry having Bonding electron pair=5 ;Lone pair=0 and Bond angle = ${{120}^{\circ }},{{90}^{\circ }},{{180}^{\circ }}$ is Trigonal bipyramidal. 

From the geometries of the molecules , we can say that option 1 has square planar geometry and option 2 has trigonal bipyramidal geometry. $ \\ $ Their geometries are: $ \\ $ <img  src="https://cmds-vedantu.s3.ap-southeast-1.amazonaws.com/prod/question-sets/c66e3d8d-f333-419a-a0a6-c776dc62f18e2189993089950762632.png"/> <img  src="https://cmds-vedantu.s3.ap-southeast-1.amazonaws.com/prod/question-sets/b230eb38-39eb-4c44-a0c0-78ef39e2ec7f1351274822263727751.png"/>

 Match the Hybridization in column A with their coordination number in Column B and shapes in column C. $ \\ $ <img  src="https://cmds-vedantu.s3.ap-southeast-1.amazonaws.com/prod/question-sets/b8e53f41-72f9-4be8-aaa0-6ef298d1ba638312357861194471120.png"/>

 In octahedral geometry, C.N. is 6 and it has two d-orbitals, three p-orbitals and one s-orbital, square pyramidal has 1 d-orbital, 3 p-orbitals and one s-orbital and trigonal bipyramidal geometry has the same C.N. as that of the square pyramidal i.e. 5.

 Match the molecules in column A with their lone pairs and bond angles in Column B and C respectively; $ \\ $ <img  src="https://cmds-vedantu.s3.ap-southeast-1.amazonaws.com/prod/question-sets/94fe318a-46d0-4730-a30c-dea12a1323ee168454739340639297.png"/>

  $Xe{{F}_{4}}$ has the same bond angle as that of the $Br{{F}_{5}}$ i.e. ${{90}^{\circ }}$ whereas the bond angle in $Xe{{F}_{2}}$ is ${{180}^{\circ }}$ and $S{{F}_{4}}$ has the number of lone pair as that in $Br{{F}_{5}}$ i.e. 1.  

 The lithium oxide should have bent shaped geometry but its geometry is linear in shape. It is so because; 

 Sharing of electrons results in the linear geometry of lithium oxide.

 The lithium oxide has linear shaped geometry because the bond between lithium and oxygen is covalent in nature.

 Depict the shapes and the bond angles of the following given geometries: $ \\ $ $(i)$ <img  src="https://cmds-vedantu.s3.ap-southeast-1.amazonaws.com/prod/question-sets/d1deb33a-db7e-4e49-9d0d-e4cafdfc2ca59112902162993023376.png"/> $ \\ $ $(ii)$ <img  src="https://cmds-vedantu.s3.ap-southeast-1.amazonaws.com/prod/question-sets/9e150498-4df0-49e4-bb82-377778df19b61007632696861726750.png"/> $ \\ $ $(iii)$ <img  src="https://cmds-vedantu.s3.ap-southeast-1.amazonaws.com/prod/question-sets/f885126b-2bcd-4208-9cae-5b283e799559821679702957720662.png"/>

  In seesaw geometry , there is one lone pair of electron and four bond pairs with bond angle of ${{90}^{\circ }},{{120}^{\circ }}$ whereas in  angular geometry, there are two bond pairs and two lone pair of electrons with the angle of ${{109.5}^{\circ }}$.

 $(i)$ <img  src="https://cmds-vedantu.s3.ap-southeast-1.amazonaws.com/prod/question-sets/f52c8ef0-10de-428a-b602-c44b178304e04928097125527734351.png"/>             $ \\ $ Geometry= Seesaw ; Bond angle = ${{90}^{\circ }},{{120}^{\circ }}$  $ \\ $ $(ii)$  <img  src="https://cmds-vedantu.s3.ap-southeast-1.amazonaws.com/prod/question-sets/908f605f-9702-44e5-a3b6-0c2943aa20124686912962397978060.png"/> $ \\ $ Geometry= angular ; Bond angle = ${{109.5}^{\circ }}$  $ \\ $ $(iii)$ <img  src="https://cmds-vedantu.s3.ap-southeast-1.amazonaws.com/prod/question-sets/0bbd2c73-5483-4169-8345-fc67d2daac906869335780514832737.png"/>$ \\ $ Geometry= Pentagonal bipyramidal ; bond angle = ${{90}^{\circ }},{{72}^{\circ }}$ 