5) Complete the table based on VSEPR predictions for neutral...

5) Complete the table based on VSEPR predictions for neutral single-bonded atoms Molecule | CO2 | NH3 | IBr3 | ClF4- --- | --- | --- | --- | --- Lewis structure | | | | Electron geometry | | | | Molecular shape | | | | Bond angles | | | | 6) Draw the VSEPR structure for the following molecules. Determine the molecular geometry, electron domain geometry, formal charge on the central atom, and whether each structure is polar of nonpolar. If there are resonance structures, draw them. a) CO3 2- b) PCl5

Transcript

00:01 In the first part of the question we have to draw louis structure louis structure plain or give electron domain geometry so electron geometry molecular geometry molecular geometry and bond angles of the following given compounds in the question bond angles so the first compound here is co2 that is carbon dioxide the lowest dot structure of co2 is like this carbon forms double bond with both the oxygen and the structure is linear and oxygen contains two lone pairs here only two lone pairs will be present on geometry is linear and since electron geometry is linear so the bond angle will be 180 degree and molecular geometry is also linear second is ammonia that is nh3 so here nitrogen contains one lone pair and three bond pair and through bond pair hydrogen atom is attached so the lewis dot structure becomes like this here nitrogen contains one lone pair and here three bond pairs to which three hydrogen atoms are attached and here the electron geometry is tetrahedral but because of one lone pair on the nitrogen atom the molecular geometry becomes trigonal pyramidal triangle pyramidal pira middle not a tetrahedral and the bond angle between them is 107 degree third structure is ibr3 ibr3 so it is a enter halogen compound and here the structure of ibr3 is like this iodine contain two lone pairs and three bond pairs to which br atom is attached so louis dot structure will be will be like this here two lone pairs on iodine atom and here the br atoms are attached through single bonds and each br atom contain 3 -3 lone pairs electron geometry is trigonal bipyramidal it is t -shaped so it is also known as t -shaped structure trigonal bipyramidal molecular geometry is also trigonal bipyramidal by pyramidal bypiremiddle and bond angles between them is 90 degree last structure is clf4 minus.

02:45 So fourth is clf4 minus.

02:49 The structure of clf4 minus is like this.

02:52 Cl contains two loan pair and three bond pairs and each fluorine atoms are attached through a single bond and each fluorine atom contain three loan pairs over it and all the atoms are present at 90 degree to each other.

03:11 Molecular geometry and electron geometry is trigonal bipyramidal again diagonal by pyramidal and bond angle is nearly 90 degree this is the first part of the question in second part we have to draw the vasc br structure of carbonate ion carbonate ion is co3 -2 minus so the structure of carbonate ion is like this c double bond o here single bond o o and two oxygen atom contains minus 1 formal charge carbon here contains zero formal charge and the oxygen which is attached with double bond also contains zero formal charge here the polarity will be like this and the resultant dipole moment will be like this so it is dipole moment is equal to zero so it is a non polar compound non polar compound the geometry is diagonal panel molecular geometry and electron domain geometry both are same and and and it is trigonal planar since it is a trigonal planar structure so the bond angle is 120 degree and hybrid structures are like this c double bond o here o and o so here two negative charge now this negative charge will shift like this so here three resonating structure are possible there is circulation of these negative charges only so here like this like this okay so here three resonating structure are possible...

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