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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?

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?

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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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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.}
Transcribed Image Text: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.}
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.
Transcribed Image Text: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.
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