Identify the predominant intermolecular force in each of these substances.

1. Hydrogen 2. Dipole-Dipole 3. London
A)H20
B)NH3
C)CH3 C=O OCH3
D)CH4
E)CH OH-C-OH CH3

what I have so far is A) 1 B) 1 C) 2 D) 3 E) I'm not sure about E, I think it might be dispersion?

NEVER MIND. it was hydrogen bonding, I didn't see the OH group

Everything is correct, except "E" is Hydrogen Bonding because there is a Hydrogen directly bonded with the Oxygen.

a)1 b)1 C)2

The answer to E is 1

To determine the predominant intermolecular force in each substance, you need to consider the molecular structure and the types of atoms present in each substance.

1. H20 (water): In water, the dominant intermolecular force is hydrogen bonding (1). Due to the electronegativity difference between oxygen and hydrogen, water molecules form hydrogen bonds with each other.

2. NH3 (ammonia): In ammonia, the main intermolecular force is also hydrogen bonding (1). Nitrogen in ammonia is more electronegative than hydrogen, creating a polarity that allows for hydrogen bonding.

3. CH3-C=O-OCH3 (dimethyl ether): This compound contains a polar carbonyl group (C=O) bonded to a nonpolar methyl group (CH3). The dominant intermolecular force is dipole-dipole interactions (2). The positive end of the carbonyl group is attracted to the negative end of neighboring molecules.

4. CH4 (methane): Methane consists of nonpolar carbon and hydrogen bonds, so the main intermolecular force is London dispersion forces (3). These forces result from temporary fluctuations in electron distribution, creating temporary dipoles that interact with other molecules.

5. CH OH-C-OH CH3 (1,2-ethanediol): This compound contains two hydroxyl groups (OH) that can form hydrogen bonds with neighboring molecules. Therefore, the predominant intermolecular force is hydrogen bonding (1).

In summary:
A) H20: Hydrogen bonding (1)
B) NH3: Hydrogen bonding (1)
C) CH3-C=O-OCH3: Dipole-dipole interactions (2)
D) CH4: London dispersion forces (3)
E) CH OH-C-OH CH3: Hydrogen bonding (1)