Lewis Shape Polarity 1

Drawing Lewis structures, determining VSEPR shape, and polarity (i.e., is there a dipole?)

Category:

Science & Technology

Tags:

• vsepr
• dipole

[sapphiremusic1993]

is this level of chemistry for highschool or UNI students?

[EnderlePhD]

@sapphiremusic1993 This class is a university first year general chemistry class for non-majors.

[Crowz]

Wait, What are residence structures? Does it have to do with simplifying the formal charge of the atoms?

[EnderlePhD]

@Crowz A resonance structure is when one takes the same Lewis structure and moves the electrons around to a different location.

[Scallop10v3]

I've got a question. Apparently from what i've learnt and the lewis diagram. I thought iodine chloride doesn't have lone pair. how come you added 4 more electrons? please help T_T im confused now.

[EnderlePhD]

@Scallop10v3 Do you mean why does the I atom have 4 lone pair electrons? If so, it must because all the valence electrons must be used and the I atom can hold more than an octet. Also, the lone pair electrons keep the formal charge on the I atom at -1.

I start putting electrons on internal atoms of the Lewis structure whenever there are too many electrons to account for. If you watch some of the other videos you'll get the idea.

[sapphiremusic1993]

@EnderlePhD Thanks :)

[Scallop10v3]

@EnderlePhD oh sweet.. i didnt know Iodine can hold more than 8 electrons... thanks :)

[djgiohappy]

Thank you EnderlePhD!

[EnderlePhD]

@djgiohappy These are only rules of thumb and may not help you in some examples.

1) If the central atom has no lone pair electrons, it is nonpolar.

2) Exception: Square planar and linear molecules are nonpolar.

3) Exception to the above 2 rules: An apparently nonpolar molecule is actually polar if the terminal atoms are different.