A hydrogen bond is a type of chemical interaction, which is specific to the presence of Lewis bases. The molecule that contains the lone pair and another molecule that has an electron-deficient atom are considered to be capable of forming hydrogen bonds. These interactions can occur with molecules such as water (H2O) or alcohol (CH3OH). While these two examples show nontoxic substances, there are other types including ammonia (NH3) and formaldehyde (HCHO).
Which of these molecules can exhibit hydrogen bonding as a pure liquid: NH3, H2O, CH4?
The molecule that contains the lone pair and another molecule that has an electron-deficient atom are considered to be capable of forming hydrogen bonds. These interactions can occur with molecules such as water (H20) or alcohol (CH30). While these two examples show nontoxic substances, there are other types including ammonia (NH30) and form aldehyde (HCHO).
As water is a molecule that contains the lone pair, it can exhibit hydrogen bonding as a pure liquid. Ammonia and formaldehyde are not capable of exhibiting this feature because they do not have an electron-deficient atom needed for hydrogen bond formation.
The following molecules can exhibit hydrogen bonding as a pure liquid:
Water (H20)
Alcohol (CH30)
Ammonia (NH30)
Formaldehyde (HCHO).
Note that hydrogen-bonded water is a pure liquid because it has the lone pair and electron-deficient atom needed for this type of bonding. Ammonia and formaldehyde are not capable of exhibiting this feature because they do not have the lone pair and electron-deficient atom needed for hydrogen bond formation.
Hydrogen bonding is an attractive force between two atoms or groups of atoms that occurs when there is a dissociation between electrons on one atom (don’t worry if you don’t remember all the technical terms). The electron-deficient atom will form a bond with an electron-rich atom by giving its own electron away to fill the other’s electron shell.
It is a strong force, but temporary and only between the two bonded atoms or molecules involved in the process. The bond will be broken when there are enough external forces to disturb it-this can happen with changes of temperature (although this doesn’t always work), pressure or even light since hydrogen bonding involves electrons that aren’t fully shielded from the effects of photons.
Hydrogen bonding is most prevalent in molecules with high electronegativity values, which are atoms that have an easy time stealing electrons (like oxygen and nitrogen). When these atoms steal electron density, they can form bonds to other neutral hydrogens or even polar covalent partners like water. Hydrogen bonding will naturally happen when there’s a lack of additional forces available to break it-this means things like hydrogen ions don’t usually exhibit this type of bond because their molecular weight isn’t as low and so aren’t exposed to enough external forces for long periods.
Molecules showing strong evidence of hydrogen bonding include ammonia (NH,) methanol ((CH), chloroform CHCl) and water (HOH).
The molecule with the strongest hydrogen bond is water. When there’s a lack of additional forces available to break it-this means things like hydrogen ions don’t usually exhibit this type of bond because their molecular weight isn’t as low and so aren’t exposed to enough external forces for long periods, water will naturally take on an H-bonded form that gives rise to molecules joined by two or three other polar covalent bonds in which each partner has donated one electron pair per shared side.
Water exhibits the strong force of hydrogen bonding more than any other compound because its electronegativity values are higher than average–it also has more protons: oxygen atoms balance out electrons rather than steal them, and the water molecule has a flexible structure.
The other molecules listed can exhibit hydrogen bonding as a pure liquid, but not in its strongest form because their electronegativity values are lower and so they’re more likely to steal electrons from oxygen atoms instead of donating them.
Examples: methane (CH), ethylene oxide (C(O)CH=CHO), propane (COC).
“Water exhibits the strong force of hydrogen bonding more than any other compound because its electronegativity values are higher than average–it also has more protons: oxygen atoms balance out electrons rather than steal them, and the water molecule has a flexible structure.”
“Water exhibits the strong force of hydrogen bonding more than any other compound because its electronegativity values are higher than average–it also has more protons: oxygen atoms balance out electrons rather than steal them, and the water molecule has a flexible structure.”
“The other molecules listed can exhibit hydrogen bonding as a pure liquid, but not in its strongest form because their electronegativity values are lower and so they’re more likely to steal electrons from oxygen atoms instead of donating them.”
The following compounds or polymers can exhibit hydrogen bonding as a pure ject:
Polyvinyl acetate, a type of plastic used for industrial purposes and in adhesives. It is also found as the major component in lacquer paints commercially sold under various trade names including “lacquer” or “enamel”.
Celluloid was one of the first plastics to be created; it was invented by John Wesley Hyatt and patented on June 29, 1869. Celluloid can exhibit hydrogen bonding as a pure liquid but not in its strongest form because celluloids electronegativity values are lower than average-so they’re more likely to steal electrons from oxygen atoms instead of donating them.
Nylon fibers were discovered accidentally while trying to synthesize other substances.
