1. Write Lewis symbols for the following atoms. (1pt each) (а) Kr (b) Ge (c) N (d) Ga (e) As (f) Rb 2. Write plausible Lewis structures for the following molecules that contain only single covalent bonds. (2 pts each) (a) FCI (b) I2 (c) SF2 (d) NF3 (е) Н-Те 3. By means of Lewis structures, represent bonding between the following pairs of elements (Your structures should show whether the bonding is essentially ionic or covalent): (2 pts each) (a) Cs and Br (b) H and Sb (c) B and Cl (d) Cs and Cl (e) Li and O (f) Cl and I 4. Assign formal charges to each of the atoms in the following structures. (3 pts each) (a) [H-C=C:]¯ (c) [CH3-CH-CH3I* (b) 2- :ö: :0: :0 5. What is the formal charge of the indicated atom in each of the following structures? (2 pts each) (a) the central O atom in 03 (b) Al in AIH4- (c) Cl in ClO3 (d) Si in SiF6²- (e) Cl in CIF3 6. Arrange the following elements in the order of decreasing electronegativity: fluorine, bromine, lithium, francium, silicon. (1 pt each per correctly ranked element)
Formal Charges
Formal charges have an important role in organic chemistry since this concept helps us to know whether an atom in a molecule is neutral/bears a positive or negative charge. Even if some molecules are neutral, the atoms within that molecule need not be neutral atoms.
Polarity Of Water
In simple chemical terms, polarity refers to the separation of charges in a chemical species leading into formation of two polar ends which are positively charged end and negatively charged end. Polarity in any molecule occurs due to the differences in the electronegativities of the bonded atoms. Water, as we all know has two hydrogen atoms bonded to an oxygen atom. As oxygen is more electronegative than hydrogen thus, there exists polarity in the bonds which is why water is known as a polar solvent.
Valence Bond Theory Vbt
Valence bond theory (VBT) in simple terms explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. It gives a quantum mechanical approach to the formation of covalent bonds with the help of wavefunctions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.
![1. Write Lewis symbols for the following atoms. (1pt each)
(a) Kr
(b) Ge
(c) N
(d) Ga
(e) As
(f) Rb
2. Write plausible Lewis structures for the following molecules that contain only single
covalent bonds. (2 pts each)
(а) FCI
(b) I2
(c) SF2
(d) NF3
(е) Н-Те
3. By means of Lewis structures, represent bonding between the following pairs of
elements (Your structures should show whether the bonding is essentially ionic or
covalent): (2 pts each)
(a) Cs and Br
(b) H and Sb
(c) B and Cl
(d) Cs and Cl
(e) Li and O
(f) Cl and I
4. Assign formal charges to each of the atoms in the following structures. (3 pts each)
(a)
[H–C=C:]¯
(c)
[CH3–CH-CH3]*
(b)
|2–
:0:
:0:
5. What is the formal charge of the indicated atom in each of the following structures?
(2 pts each)
(a) the central O atom in 03
(b) Al in AIH4-
(c) Cl in Cl03
(d) Si in SiF62-
(e) Cl in CIF3
6. Arrange the following elements in the order of decreasing electronegativity: fluorine,
bromine, lithium, francium, silicon. (1 pt each per correctly ranked element)
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