00:01
Okay, so here we have to determine the dominant force of attraction in the given molecule, okay? the dominant intermolecular force.
00:11
We have ammonia, nh3.
00:15
So here, this nitrogen is bonded to three hydrogen atoms.
00:22
Okay.
00:22
When there is a direct interaction of hydrogen and a electronegative atom like nitrogen, oxygen or chlorine, then that is hydrogen.
00:33
Hydrogen bonding.
00:34
Hydrogen bonding is the dominant kind of force of attraction here.
00:39
Okay.
00:40
Of course in this molecule, diapole moment can be possible.
00:44
So diapole forces are there.
00:46
In this molecule, we have vanderbord force that is a universal force present in each and every molecule.
00:53
So that is there.
00:54
But i am discussing about the dominant force of attraction and that is hydrogen bonding.
01:00
Okay.
01:01
So do you? to interaction between electronegative, let me write it again, nitrogen and hydrogen, okay.
01:37
Then we have second part and that is k2s, okay? so here we have potassium and sulfur.
01:49
Okay, so that belongs to group first okay and that is a strong metal while sulfur is a non -metal okay that belongs to oxygen family so here we have ionic bond and why so because there is bond between metal and non -metal okay so metal are those elements which have tendency to lose electron and non -metal are those elements which have tendency to gain electron.
02:36
Then third part we have hcl.
02:44
So now the dominant force of attraction possible here that is dipole dipole forces.
02:57
So here it is to be noted that there is interaction between hydrogen and chlorine group.
03:02
Chlorine is electronegative in nature but we have the dominant force of attraction present here is dipole dipole forces not hydrogen bond okay there is the dominant force of attraction is not hydrogen bonding but dipole dipole forces and why so because chlorine has less electronegativity okay so hydrogen bonding is only possible when there is interaction of hydrogen with the most electron negative atom like nitrogen oxygen and fluorine when we have chlorine or bromine and iodine so what happens then down the group the electronegativity decreases okay so as the electrone negativity decreases so the hydrogen bonding is that becomes less and less prominent okay so although there is hydrogen bonding but that is not dominant kind of force of here okay the dominant force of attraction possible here is dipole dipole forces okay because there is polarity in bond again this polarity in bond is due to unsymmetrical distribution of charge because there is electro -nitivity difference okay greater the electro -nitivity difference greater will be the polarity greater will be the dipole -dipole forces okay so here you can see hydrogen is from group first, okay? and chlorine is from group 17.
04:42
So you can see they are present on both extreme poles in the periodic table, right? so there is very much electronity difference and that's why there is higher polarity and that's why there is higher dipole movement and dipole dipole diphth.
04:59
So now fourth one, we have f2.
05:07
Now here you have two fluorine atoms bonded together.
05:11
Okay so when the two same atoms are bonded together in this means that there is no electronegativity difference at all or you can say there is very poor electro -negativity difference because we have both same kind of atoms right so when there is no polarity difference okay so this means that the molecule is non -polar right and for non -polar molecules the general force we have the only possibility we have that is weak london forces or you can say vendor wall forces okay so here we have weak london forces that is the dominant kind of force of attraction okay and so for weak london forces this is because we have a non -polar molecule and and fifth part, we have pcl3, okay? so pcl3 can be drawn like this.
06:31
So phosphorus is here, chlorine, chlorine, and we have.
06:42
So phosphorus is from group 15, fibrill and electrons are there, right? let me draw the structure again.
06:57
So this will be phosphorus bonded to three chlorine atom and we have a pair of unbounded electron.
07:07
So there is unsymmetrical charge distribution because there is polarity between phosphorus and chlorine.
07:17
This is the direction of dipole moment and there is diaboloment due to this lone pair of electron too.
07:24
Okay.
07:25
So here mu is not equal to zero.
07:28
Okay.
07:29
So this is a polar molecule.
07:33
And for polar molecule, the dominant force of attraction possible here is dipole dipole forces okay because there is unsymmetrical let me write it again or i should say unequal distribution of charge okay so then we have sixth part n acl okay so here we have a sodium that is a metal chlorine non -metal so the force of attraction dominant here is ionic bond or electrostatic forces and that is due to bond between metal and non let me write it again metal then we have seventh part that is a so2 so how to draw this structure we have sulfur which is from oxygen family six valence electrons are there four of the electrons involved in bonding and rest is unbounded okay so now there is unequal distribution of charge again okay so this is a polar molecule molecule and for polar molecule there is dipole dipole force is since mu is not equal to zero that is net dipole moment is unequal okay due to unequal distribution of charge eighth part we have co2 so this can be drawn as carbon bonded to oxygen two oxygen atoms by double bonds it is a linear molecule and if you see here the dipole moment is present due to the this is the direction of diabol moment for carbon oxygen bond but here we have mu is equal to zero that is there is no dipole net dipole at all okay and this net dipole moment is not present because the overall dipolement cancelled out being equal and opposed okay so that's why it is a non polar molecule and for non polar molecule you know we have the only kind of force of attraction dominant is weak london forces because dipole moment cancels out okay i should say net dipole moment cancels out being equal and opposite okay so then we have ninth part ninth part says h2 here again two same hydrogen atoms are bonded together okay and there is no electronegivity difference so that's why there is weak vendor wall force or you can say london force okay and why so why so because let me write it again so there is non -polar molecule okay least electron activity difference because the two atoms are same then tenth part we have ch4 let me write it again and let me draw the structure for same so this will be or carbon, let me draw it again, carbon bonded to four hydrogen atoms like this.
13:40
This ch4 is a symmetrical molecule, okay? and in a symmetrical molecule, we have net dipole moment zero.
13:51
So here, mu is equal to zero.
13:59
Okay and that is the dominant force of attraction here is weak london forces or vanderwall forces okay because ch4 being symmetrical just like co2 okay nullifies net dipole moment then 11 part so we have chcl 3 so the structure is just similar to ch4 tetrahedral okay but this time so the direction of dipole moment is like this okay and there is unequal distribution of charge so that's why mu is not equal to zero that's why there is slight polarity so we have dipole dipole forces the dominant force okay then we have 12th part co let me draw the structure so carbon with the help of three bonds bonded to oxygen atom okay now here this carbon forms a sort of coordinate bond with this oxygen actually to complete the octet both sides okay so now here the overall dipole moment that is from carbon to oxygen so there is polarity okay so that's why mu is not equal to zero and that's why this is a polar molecule so that is there is dipole dipole forces then we have 13th part so we have n2 nitrogen...