iii. Vinyl chloride is the starting material for the production of poly(vinyl chloride), abbreviated PVC. Its recycling code is "V". The major use of PVC is for tubing in residential and commercial construction. H Cl C= H H Vinyl chloride (a) Complete the Lewis structure for vinyl chloride by showing all unshared pairs of electrons. (b) Predict the H-C-H, H–C-C and Cl–C–H, bond angles in this molecule. (c) Does vinyl chloride have polar bonds?
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.
![iii. Vinyl chloride is the starting material for the production of
poly(vinyl chloride), abbreviated PVC. Its recycling code is
"V". The major use of PVC is for tubing in residential and
commercial construction.
H
Cl
H
H
Vinyl chloride
(a) Complete the Lewis structure for vinyl chloride by showing
all unshared pairs of electrons.
(b) Predict the H-C-H, H-C-C and Cl–C–H, bond angles in this
molecule.
(c) Does vinyl chloride have polar bonds?
(d) Is it a polar molecule?
(e) Does it have a dipole?
iv. Diazene (N,H,) and hydrazine (NH,NH,) are reactive nitrogen
compounds. Use the hybrid orbitals theory to compare the
bonding in these two molecules, and describe the differences in
their molecular structures.
v. Which molecules in the following figure show an increase in
bond order when one electron is added to the molecule? (Hint:
Use the molecular orbitals theory.)
Liz
Be,
C2
N2
F2
Ne,
vi. Use the molecular orbitals theory to decide whether NF would
be stabilized or destabilized by adding one electron to make the
corresponding anion and by removing an electron to form the
corresponding cation. {Hint: Describe the bonding in all
species.}](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F59b158d1-80f7-4e88-9120-6cf56606431e%2Fd782808e-4214-4ce8-88f5-dd638cdcf6bc%2F05ok5kb_processed.jpeg&w=3840&q=75)
![Exercise 10
i. Based on the concept of formal charge, what is the central atom
in NOCI (Cl is always a terminal atom)?
ii. Answer true or false.
(a) A covalent bond is formed between two atoms whose
difference in electronegativity is less than 1.9.
(b) If the difference in electronegativity between two atoms is
zero (they have identical electronegativities), then the two
atoms will not form a covalent bond.
(e) A covalent bond formed by sharing two electrons is called a
double bond.
(d) In the hydrogen molecule (H,), the shared pair of electrons
completes the valence shell of each hydrogen.
(e) In the molecule CH4, each hydrogen has an electron
configuration like that of helium, and carbon has an electron
configuration like that of neon.
(1) In a polar covalent bond, the more electronegative atom has a
partial negative charge (8-) and the less electronegative atom
has a partial positive charge (&+).
(g) These bonds are arranged in order of increasing polarity C-H
<N-H<O-H.
(h) These bonds are arranged in order of increasing polarity H-F
<H-Cl < H-Br.
(1) A polar bond has a dipole with the negative end at the more
electronegative atom.
(1) In a single bond, two atoms share one pair of electrons; in a
double bond, they share two pairs of electrons; and in a triple
bond, they share three pairs of electrons.
(k) The Lewis structure for ethane, C,H6, must show eight
valence electrons.
(1) The Lewis structure for formaldehyde, CH,O, must show 12
valence electrons.
(m) The Lewis structure for the ammonium ion, , must show nine
valence electrons.
(n) Atoms of third-period elements can hold more than eight
electrons in their valence shells.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F59b158d1-80f7-4e88-9120-6cf56606431e%2Fd782808e-4214-4ce8-88f5-dd638cdcf6bc%2Fvjhs87m_processed.jpeg&w=3840&q=75)
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