Grade 12 Chemistry
Which of the following chemicals is not likely to exhibit dipole-dipole forces and
hydrogen bonding?
Question 22 options:
a) H2O
b) CH3OH
c) H2
d) NH3
e) HF
c) H2
To determine which chemical is not likely to exhibit dipole-dipole forces and hydrogen bonding, we need to consider the molecular structure and its ability to form hydrogen bonds.
Dipole-dipole forces occur when there is a significant difference in electronegativity between the atoms in a molecule, causing a partial positive charge on one atom and a partial negative charge on another atom. Hydrogen bonding is a specific type of dipole-dipole force that occurs when hydrogen is directly bonded to a highly electronegative atom like oxygen, nitrogen, or fluorine.
Let's analyze each option:
a) H2O (water) - Water molecules are polar due to the electronegativity difference between hydrogen and oxygen. Water exhibits both dipole-dipole forces and hydrogen bonding.
b) CH3OH (methanol) - Methanol is also polar because of the electronegativity difference between carbon, hydrogen, and oxygen. It can exhibit dipole-dipole forces, but hydrogen bonding is less likely because hydrogen is not directly bonded to strongly electronegative elements like nitrogen or oxygen.
c) H2 (hydrogen gas) - Hydrogen gas consists of diatomic molecules held together by a single covalent bond. Since both hydrogen atoms have the same electronegativity, there is no significant electronegativity difference, and therefore, no dipole-dipole forces or hydrogen bonding.
d) NH3 (ammonia) - Ammonia is a polar molecule due to the electronegativity difference between nitrogen and hydrogen. It can exhibit both dipole-dipole forces and hydrogen bonding.
e) HF (hydrogen fluoride) - Hydrogen fluoride is a polar molecule with a strong electronegativity difference between hydrogen and fluorine. It can exhibit dipole-dipole forces and hydrogen bonding.
From the options given, the chemical that is not likely to exhibit dipole-dipole forces and hydrogen bonding is:
c) H2 (hydrogen gas)
To determine which of the following chemicals is not likely to exhibit dipole-dipole forces and hydrogen bonding, we need to consider the molecular structure of each compound.
a) H2O (water): Water exhibits both dipole-dipole forces and hydrogen bonding. It forms hydrogen bonds due to the presence of a hydrogen atom bonded to an oxygen atom.
b) CH3OH (methanol): Methanol also exhibits both dipole-dipole forces and hydrogen bonding. It contains an oxygen atom bonded to a hydrogen atom, allowing it to form hydrogen bonds.
c) H2 (hydrogen gas): Hydrogen gas does not exhibit dipole-dipole forces or hydrogen bonding. It consists of two hydrogen atoms that share electrons equally, resulting in a nonpolar molecule.
d) NH3 (ammonia): Ammonia exhibits both dipole-dipole forces and hydrogen bonding. It contains a nitrogen atom bonded to three hydrogen atoms, enabling it to form hydrogen bonds.
e) HF (hydrogen fluoride): Hydrogen fluoride exhibits both dipole-dipole forces and hydrogen bonding. It contains a hydrogen atom bonded to a fluorine atom, which enables it to form hydrogen bonds.
Based on the options provided, the chemical that is not likely to exhibit dipole-dipole forces and hydrogen bonding is option c) H2 (hydrogen gas).