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CHM 2120 Lecture Notes - Lecture 15: Chemical Polarity, Covalent Bond, Formal Charge

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whitespider72
13 Nov 2016
School
University of Ottawa
Department
Chemistry
Course
CHM 2120
Professor
Julian Chan

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Document Summary

Formal charge= number of valence electrons no of bonds no. of lone electrons. Example, in the structure of ozone, there are three oxygen atoms, two connected by a ouble bond to each other, and one connected by a single bond to the middle oxygen. So total no of valence electrons = 6 x 3 electrons because oxygen has a atomic number of 6 and there are 3 oxygens. A double bond and a single bond means 3 sticks and the no of lone electrons left is 15 so 18-15-3= 0 so formal charge is zero. Another easy way of finding the formal charge is by looking at each atom individually and see if they have octets and find formal charge of each atom and add them up to get the overall charge. The power of an atom to attract electrons to itself. We can look at electronegativity values in the periodic table.

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Related Questions

Draw a Lewis Structure for SO2 in which all atoms obey the octet rule. Show formal charges. Do not consider ringed structures.

Submit your answer to the following in complete sentences, providing your choice, your evidence, and your reasoning as indicated below.

Which two of the elements listed have the most similar Lewis structures?

A) S and Se

B) Si and P

C) Al and Ge

D) Rb and Ca

Which of the following correctly describes the Lewis structure of the compound formed between Mg and Cl?

A) The one Mg will have a negative charge and eight dots around its symbol, whereas the two Cl symbols will have a positive charge and no dots around the symbol.

B) The one Mg will have a positive two charge and no dots around its symbol, whereas the two Cl symbols will have a negative charge and eight dots around the symbol.

C) The one Mg will have a positive charge and no dots around its symbol, whereas the one Cl will have a negative charge and eight dots around its symbol.

D) The one Mg will have a negative charge and no dots around its symbol, whereas the two Cl symbols will have a positive charge and eight dots around the symbol.

In the Lewis structure for a molecule, one of the nitrogen atoms shares six electrons with a carbon atom and has two electrons that it does not share with any other atom. Which of the following correctly describes this nitrogen atom?

A)three single bonds and one lone pair

B)three single bonds and two lone pairs

C)triple bond and two lone pairs

D) triple bond and one lone pair

Under which of the following circumstances would the molecular geometry be the same as the electron geometry?

A) identical terminal atoms

B) no lone pairs on the central atom

C) presence of multiple bonds on the central atom

D) presence of lone pairs on the central atom

(2 points) Referring to the reading, "The Lewis Structure of Ozone," describe why the two Lewis structures shown are incorrect.