which of the following molecules will exhibit hydrogen bonding?
a. CH3OCH3
b. HF
c. CH4
d. LiH
Technically, H bonding occurs between H and O, N, F atoms. Look at H bonding of HF.
I cannot found answer
Hydrogen bonding occurs when a hydrogen atom is bonded to an electronegative atom (such as nitrogen, oxygen, or fluorine) and interacts with another electronegative atom. Based on this definition, the molecule that will exhibit hydrogen bonding from the options you provided is:
b. HF
In HF, the hydrogen atom is bonded to fluorine (an electronegative atom), creating a hydrogen bonding interaction.
To determine which of the molecules will exhibit hydrogen bonding, we need to look at the characteristics of hydrogen bonding.
Hydrogen bonding occurs when hydrogen is directly bonded to oxygen, nitrogen, or fluorine. These elements are highly electronegative, meaning they attract electrons strongly. As a result, hydrogen atoms in molecules bonded to these electronegative atoms often have a partial positive charge.
Now let's analyze each option:
a. CH3OCH3 (dimethyl ether) - This molecule has two oxygen atoms, but it does not have a direct hydrogen bond to an electronegative atom. Therefore, it does not exhibit hydrogen bonding.
b. HF (hydrogen fluoride) - This molecule has a direct hydrogen bond between hydrogen and fluorine, which are both highly electronegative elements. Therefore, HF will exhibit hydrogen bonding.
c. CH4 (methane) - This molecule does not have an electronegative atom directly bonded to hydrogen. It consists of hydrogen and carbon atoms only, so it does not exhibit hydrogen bonding.
d. LiH (lithium hydride) - This molecule has a direct bond between hydrogen and lithium, but lithium is not an electronegative element. As a result, LiH does not exhibit hydrogen bonding.
So, the molecule that exhibits hydrogen bonding from the options given is:
b. HF