Chemistry Essay
5.)
a.)
b.) Ethyne (C₂H₂) has the shortest C-to-C bond because there is a triple bond between the two C’s. The shorter the bond, the smaller the distance between the two bonded atoms, a single bond has the largest distance between two bonded atoms.
c.)
i.) trigonal planar ii.) pyramidal
d.) This is not true because the bonds described are intramolecular forces, C-H, C-O, O-H, which are not affected by boiling. When boiling occurs, added energy overpowers intermolecular forces, not intramolecular forces.
e.) Ethyne is nonpolar because of the structure of the compound, linear. The linear shape causes all the bond dipole moments to cancel making Ethyne nonpolar.
f.) Ethanol is completely soluble in water rather than Ethanethiol which is partially soluble because Ethanol has a hydrogen bond (OH) which attracts to water (H₂O). Ethanthiol has London-dispersion forces which does not attract to water because there is no Oxygen to bond to water.
6.)
a.) i.) ii.)
b.) In Box X, Compound 2 is represented because of the stronger intermolecular forces present (Hydrogen-bonding intermolecular forces), therefore creating a higher boiling point (78ᵒ).
c.) Dichloromethane has greater solubility in water than Carbon tetrachloride because Dichloromethane is polar while Carbon tetrachloride is nonpolar. Since Dichloromethane is polar, it interacts with water by dipole-dipole forces, while Carbon tetrachloride only interacts with water by London-dispersion, which is weaker.
d.) Dichloromethane has a higher vapor pressure than Carbon tetrachloride because of Dichloromethane’s intermolecular forces, London-dispersion and dipole-dipole, while Carbon tetrachloride has London-dispersion forces. Dichloromethane has weaker intermolecular forces therefore increasing the vapor pressure.
e.)
7.)
a.)
i.) has London-dispersion and Hydrogen-bonding forces, while has London-dispersion and dipole-dipole forces. ii.) The boiling point of has a
a.)
b.) Ethyne (C₂H₂) has the shortest C-to-C bond because there is a triple bond between the two C’s. The shorter the bond, the smaller the distance between the two bonded atoms, a single bond has the largest distance between two bonded atoms.
c.)
i.) trigonal planar ii.) pyramidal
d.) This is not true because the bonds described are intramolecular forces, C-H, C-O, O-H, which are not affected by boiling. When boiling occurs, added energy overpowers intermolecular forces, not intramolecular forces.
e.) Ethyne is nonpolar because of the structure of the compound, linear. The linear shape causes all the bond dipole moments to cancel making Ethyne nonpolar.
f.) Ethanol is completely soluble in water rather than Ethanethiol which is partially soluble because Ethanol has a hydrogen bond (OH) which attracts to water (H₂O). Ethanthiol has London-dispersion forces which does not attract to water because there is no Oxygen to bond to water.
6.)
a.) i.) ii.)
b.) In Box X, Compound 2 is represented because of the stronger intermolecular forces present (Hydrogen-bonding intermolecular forces), therefore creating a higher boiling point (78ᵒ).
c.) Dichloromethane has greater solubility in water than Carbon tetrachloride because Dichloromethane is polar while Carbon tetrachloride is nonpolar. Since Dichloromethane is polar, it interacts with water by dipole-dipole forces, while Carbon tetrachloride only interacts with water by London-dispersion, which is weaker.
d.) Dichloromethane has a higher vapor pressure than Carbon tetrachloride because of Dichloromethane’s intermolecular forces, London-dispersion and dipole-dipole, while Carbon tetrachloride has London-dispersion forces. Dichloromethane has weaker intermolecular forces therefore increasing the vapor pressure.
e.)
7.)
a.)
i.) has London-dispersion and Hydrogen-bonding forces, while has London-dispersion and dipole-dipole forces. ii.) The boiling point of has a