Polarity of Molecules?
Which one of the following is polar? Explain.
a. CCl4
b. BCl3
c. NCl3
d. BeCl2
I don't know why I'm having so much trouble figuring this one out. I've done the electron dot diagrams and tried to assign formal changers, but I don't think I'm doing it right because I always come up with 0 for each atom. :(
Answer:
CCl4 is not polar
BCl3 is not polar
NCl3 is polar
BeCl2 is not polar
Check link it will help you http://www.ausetute.com.au/molpolar.html...
C
Well CCl4 is tetrahedral and all the Cl atoms pull equally. For BCl3, B is electron deficient, so again each of the Cl pulls on it equally. For NCl3, the nitrogen has a lone pair of electrons which causes the molecule to become polar. BeCl2 is an ionic compound.
by ruling out, the only reasonable answer left is BeCl2.
CCl4 is non polar, it i totally symmetrical (sp3 hybrid, all bonds are the same), BCl3, slightly polar bonds, but it out to be a sp2 hybrid (B has only 3 electrons in the valence shell, so no other options here), so it is planar with 120 deg angles, i.e. also symmetrical. NCl3 is a known non-polar, cause of the non polar bonds.
so, having in mind that Be is in IIA group, it is a relatively strong metal, so the bond in BeCl2 should be mostly ionic, making the molecule polar.
CCl4 is non polar as though there is charge formation the net charge on the carbon is 0 as the charges cancel each other out.
The same thing happens with BCl3
With NCl3 there is a lone pair of electrons on the nitrogen which will contribute to it having a net charge>0,hence it will be polar.
BeCl2 is an ionic compound.
Have to disagree with chem-freak on this one. NCl3 is polar because the bonds are slightly polar and the three-dimensional vectors associated with each of the three N-Cl bonds, when added, do not give a zero resultant.
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a. CCl4
b. BCl3
c. NCl3
d. BeCl2
I don't know why I'm having so much trouble figuring this one out. I've done the electron dot diagrams and tried to assign formal changers, but I don't think I'm doing it right because I always come up with 0 for each atom. :(
Answer:
CCl4 is not polar
BCl3 is not polar
NCl3 is polar
BeCl2 is not polar
Check link it will help you http://www.ausetute.com.au/molpolar.html...
C
Well CCl4 is tetrahedral and all the Cl atoms pull equally. For BCl3, B is electron deficient, so again each of the Cl pulls on it equally. For NCl3, the nitrogen has a lone pair of electrons which causes the molecule to become polar. BeCl2 is an ionic compound.
by ruling out, the only reasonable answer left is BeCl2.
CCl4 is non polar, it i totally symmetrical (sp3 hybrid, all bonds are the same), BCl3, slightly polar bonds, but it out to be a sp2 hybrid (B has only 3 electrons in the valence shell, so no other options here), so it is planar with 120 deg angles, i.e. also symmetrical. NCl3 is a known non-polar, cause of the non polar bonds.
so, having in mind that Be is in IIA group, it is a relatively strong metal, so the bond in BeCl2 should be mostly ionic, making the molecule polar.
CCl4 is non polar as though there is charge formation the net charge on the carbon is 0 as the charges cancel each other out.
The same thing happens with BCl3
With NCl3 there is a lone pair of electrons on the nitrogen which will contribute to it having a net charge>0,hence it will be polar.
BeCl2 is an ionic compound.
Have to disagree with chem-freak on this one. NCl3 is polar because the bonds are slightly polar and the three-dimensional vectors associated with each of the three N-Cl bonds, when added, do not give a zero resultant.
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