Concept explainers
Interpretation:
The Lewis structures of the given molecules and ions are to be represented.
Concept introduction:
A Lewis structure is the representation of bonding and non-bonding electron pairs present in the outermost shell of all atoms present in the molecule.
The number of bonds formed by an atom in the molecule is determined by the valance electron pairs.
Dots are placed above and below as well as to the left and right of symbol.
Number of dots is important in Lewis dot symbol but not the order in which the dots are placed around the symbol.
In writing symbol pairing is not done until absolutely necessary.
For metals, the number of dots represents the number of electrons that are lost when the atom forms a cation.
For second period non metals, the number of unpaired dots is the number of bonds the atom can form.
Atomic ions can also be represented by dot symbols, by simply adding (for anions) and subtracting (for cations) the appropriate number of dots from Lewis dot symbol.
The octet rule states that every atom reacts to form bonds till its octet of electrons gets completely filled.

Answer to Problem 49QP
Solution: The Lewis structures of the given molecules and ions are shown below.
a)
b)
c)
d)
e)
f)
Explanation of Solution
a)
The electronic configuration of carbon, oxygen, and bromine in
A carbon atom has the tendency to form four bonds because of the presence of four electrons in its outermost shell, bromine has the tendency to form one bond because of the presence of five electrons in its
b)
The electronic configuration of hydrogen and selenium in
A selenium atom contains four valance electrons in its
The Lewis structure of
c)
The electronic configuration of nitrogen, oxygen, and hydrogen in
A nitrogen atom has the tendency to form three bonds because of the presence of three electrons in its outermost shell, an oxygen atom has the tendency to form two bonds because of the presence of four electrons in its
d)
The electronic configuration of carbon, nitrogen, and hydrogen in
A carbon atom has the tendency to form four bonds because of the presence of four electrons in its outermost shell, hydrogen has the tendency to form one bond because of the presence of one electron in its outermost shell, and nitrogen has the tendency to form three bonds due to the presence of three valance electrons in its
e)
The electronic configuration of oxygen, carbon, chlorine, and hydrogen in
A carbon atom has the tendency to form four bonds because of the presence of four electrons in its outermost shell, hydrogen has the tendency to form one bond because of the presence of one electron in its outermost shell, and bromine has the tendency to form one bond because of the presence of five valance electrons in its
f)
The electronic configuration of nitrogen and chlorine in
A nitrogen atom contains three valance electrons in its
The Lewis structure of
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Chapter 8 Solutions
BURDGE CHEMISTRY VALUE ED (LL)
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