2. (6 poists) Describe Water (HO) Bensene (C.lt CO, (solid 3. (a points) Describ
ID: 591786 • Letter: 2
Question
2. (6 poists) Describe Water (HO) Bensene (C.lt CO, (solid 3. (a points) Describe predominant intermolecular interacti together ons between the following compounds mised For example: NaCI dissolved in Water: lon-dipole a. NaCI dissolved in Benzene b. CH OH dissolved in Water e. Co, dissolved in Benzene d. KBr dissolved in Water 4 redict crystal types (ionic, molecular, covalent, or metallic) and describe predominant 1. (10 points) P intermolecular forces in each substance. Cirele the substance in each pair that should have the higher boiling point? Predominant intermolecular forces Crystal type MgClh Cl2 Please circle the substance with the higher boiling point Predominant intermolecular forces Crystal type CO2 CS2 Please circle the substance with the higher boiling pointExplanation / Answer
2.a)The primary intermolecular force in Water is Hydrogen bonding which occurs due to the two lone pair of electrons on Oxygen atoms which can form Hydrogen bonds with Hydrogen atoms of other molecule.Also Oxygen being more electronegative than Hydrogen it will pull more electrons towards itself thus it will have a partial negative charge while hydrogen will have partial positive charge because the electrons have been pulled away from it.Because of this strong dipole dipole attraction, Hydrogen bonding happens.
b)The primary intermolecular force in Benzene is London dispersion forces. Though it is the weakest kind of forces but Benzene being a non polar compound Hydrogen bonding and dipole interactions are not possible. Dispersion forces occur when one side of the molecule becomes more positive or negative. Benzene being non polar and a bigger molecule, these forces are predominant in it.
c) Though Carbon dioxide has polar C-O bonds but it is a non polar molecule because of its linear symmetry the dipoles cancel each other. Hence permanent dipole dipole interaction is not possible. The predominant force here is London dispersion forces or Van der Waal forces where O being more electronegative than C. London dispersion forces are the temporary attractive forces that results when electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles. Hydrogen bonding cannot happen because there is no H in CO2.
d)The predominant intermolecular force in KF is ionic bonding. F being very much electronegative than K, electrons are accepted by F nd given by K thus forming ionic bonds.
e)The strongest intermolecular force in Methanol is Hydrogen bonding because of the presence of O-H bond and Oxygen having two lone pair of electrons.
f)The predominant force in Nitrogen is London dispersion forces because Nitrogen is a non polar molecule and Hydrogen bonding and dipole dipole interactions are not possible.
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