Categorize each molecule according to its hydrogen-bonding characteristics. a. CH3OCH3b. CH3CH2CH3c. CH3CH2NH2d. H2Oe. CH3OH

H2O > CH3OH > CH3CH2NH2 > CH3OCH3 > CH3CH2CH3

Explanation:

Hydrogen bonding exists in molecules in which hydrogen is bonded to a highly electronegative element such as fluorine, chlorine, oxygen, sulphur, nitrogen etc.

Water has the highest degree of hydrogen bonding among the listed substances hence its very high boiling point, stemming from intermolecular hydrogen bonding. CH3CH2NH2 has a lesser degree of hydrogen bonding because nitrogen is less electronegative than oxygen.

Alcohols show significant hydrogen bonding in solution, the same applied to amines. However, ethers do not form hydrogen bonds with each other but they can form hydrogen bonds with other molecules such as alcohols and amines. Alkanes do not form hydrogen bonds at all.

alkaline metals are lithium, sodium, rubidium, potassium, cesium and francium.

alkali metals have electronegativity from 0.7 to 1, lowest in periodic table of elements, which means that alkali metals (i group in periodic table) has positive oxidation number in compounds.

electronegativity is a chemical property that describes the tendency of an atom to attract a shared pair of electrons towards itself.

alkaline metals (far left in main group) have lowest ionizations energy and easy remove valence electrons,

for example, potassium is the alkali metal and has a single valence electron in the outer electron shell.

electron configuration of potassium is: ₁₉k 1s²2s²2p⁶3s²3p⁶4s¹.

they can not exist alone in nature, because they are very reactive.

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