Podcast
Questions and Answers
Hydrogen bonding occurs between molecules with Hydrogen atoms bonded to Nitrogen, Oxygen, or Fluorine.
Hydrogen bonding occurs between molecules with Hydrogen atoms bonded to Nitrogen, Oxygen, or Fluorine.
True (A)
Hydrogen bonding is considered the weakest form of intermolecular force.
Hydrogen bonding is considered the weakest form of intermolecular force.
False (B)
Water's high boiling point is due to the weak hydrogen forces that easily break when heated.
Water's high boiling point is due to the weak hydrogen forces that easily break when heated.
False (B)
A molecule of nitrogen has 1 sigma bond and 2 pi bonds resulting from the sharing of valence electrons.
A molecule of nitrogen has 1 sigma bond and 2 pi bonds resulting from the sharing of valence electrons.
Electronegativity is defined as the relative attraction of an atom for a shared pair of protons in a covalent bond.
Electronegativity is defined as the relative attraction of an atom for a shared pair of protons in a covalent bond.
Ammonia (NH3) and silane (SiH4) both have the same bond angle of 107.3°.
Ammonia (NH3) and silane (SiH4) both have the same bond angle of 107.3°.
The lone pair of electrons has less repelling power compared to a bond pair of electrons.
The lone pair of electrons has less repelling power compared to a bond pair of electrons.
Hydrogen bonding involves attractions between Hydrogen atoms bonded to Sulfur, Carbon, or Phosphorus.
Hydrogen bonding involves attractions between Hydrogen atoms bonded to Sulfur, Carbon, or Phosphorus.
Strong hydrogen forces contribute to a low boiling point in substances like water.
Strong hydrogen forces contribute to a low boiling point in substances like water.
Electronegativity represents the ability of an atom to attract electrons when forming a chemical bond.
Electronegativity represents the ability of an atom to attract electrons when forming a chemical bond.
Silane (SiH4) has a lower bond angle than ammonia (NH3).
Silane (SiH4) has a lower bond angle than ammonia (NH3).
A lone pair of electrons contributes to differences in bond angles between different molecules.
A lone pair of electrons contributes to differences in bond angles between different molecules.
