In: Chemistry
In each pair complete the following 3 parts;
i) identify ALL the intermolecular forces present in each (ion-dipole; H-bonding; diploe-dipole; dispersion)
ii) circle the substance in each pair with the higher boiling point
iii) explain your choice for “ii”
in aqueous solution
a) CH3Bror CH3F b) CH3CH2CH2OH or CH3CH2OCH3 c) MgCl2 or SrCl2
i: i: i:
iii: iii: iii:
FOR 1ST we have
1.ch3br and ch3f
type of bond :-ch3br(Dipole-dipole interactions and dispersion forces).
ch3f(dipole dipole becauseCH3F is a polar molecule, it has a permanent dipole. In this case hydrogen bonding does NOT occur, since the F atom is bonded to the central C atom (F must be bonded to H in order for hydrogen bonding to occur).
2. for boiling point we have ch3br having higher than ch3f.
3. reason :-
CH3Br is quite much more heavy molecule compared to CH3F. As CH3F does not form hydrogen bonds and a slight increase in polarity does not really have that large effect in the intermolecular forces. So the weight is the main factor.
Dipole-dipole is not as strong as you think, Br has a lot more electrons than F making the dispersion forces a LOT stronger..
FOR 2ND
CH3CH2CH2OH AND CH3CH2OCH3
1.CH3CH2CH2OH(h bonding) AND CH3CH2OCH3(dipole-dipole interactions,)
2.boiling point is higher in case of ch3ch2oh than ch3ch2och3 beacuse 1st having h bonding is quite higher than ether group having dipole dipole ineraction.
FOR 3RD
we have mgcl2 and srcl2 (both are ionic bond)
mgcl2 boiling point 1412` C AND Boiling point of srcl2 1250`c
beacuse mgcl2 having less electronic crowding than crcl2.