Identify the major type of attractive force between the particles of each of the following:
Which one is
NF3
dipole dipole attraction
ionic bond
dispersion forces
hydrogen bond
NF3 has a dipole-dipole attraction.
The major type of attractive force between the particles of each of the following compounds is as follows:
1. NF3 (Nitrogen Trifluoride):
- Dipole-dipole attraction: In NF3, there is a significant electronegativity difference between nitrogen and fluorine atoms, resulting in a polar molecule. The partial positive charge on nitrogen interacts with the partial negative charges on fluorine atoms, leading to dipole-dipole attraction.
2. Ionic bond:
- Ionic bond: Ionic bonds occur when there is a transfer of electrons from one atom to another, resulting in the formation of ions. Positive and negative ions attract each other through electrostatic forces. This type of bond is typically formed between metals and nonmetals.
3. Dispersion forces (also referred to as London dispersion forces):
- Dispersion forces: Dispersion forces are the weakest intermolecular forces and occur between all molecules, regardless of their polarity. These forces arise from temporary shifts in electron density, resulting in instantaneous dipoles. In the case of NF3, there are dispersion forces present in addition to dipole-dipole attractions.
4. Hydrogen bond:
- Hydrogen bond: Hydrogen bonds occur when a hydrogen atom is bonded to a highly electronegative atom (such as nitrogen, oxygen, or fluorine) and forms an attraction with a neighboring electronegative atom. In NF3, hydrogen bonding is not present. Hydrogen bonds are typically stronger than the other intermolecular forces mentioned.
To identify the major type of attractive force between the particles in a substance, we need to consider the nature of the particles involved.
1. NF3 (Nitrogen Trifluoride):
- The NF3 molecule contains nitrogen (N) and fluorine (F) atoms.
- The nitrogen atom is more electronegative than the fluorine atoms, resulting in a polar covalent bond.
- The major type of attractive force between NF3 molecules is dipole-dipole attraction.
- Dipole-dipole attractions occur due to the electrostatic interactions between the positive end of one polar molecule and the negative end of another polar molecule.
2. Ionic Bond:
- Ionic bonds occur when there is a complete transfer of electrons from one atom to another, resulting in the formation of positive and negative ions.
- Ionic bonds usually exist between metals and nonmetals.
- In ionic compounds, such as NaCl (sodium chloride), the major type of attractive force is the electrostatic attraction between positive and negative ions.
3. Dispersion Forces:
- Dispersion forces, also known as London Forces, are the weakest type of intermolecular forces.
- They exist between all types of molecules, whether polar or nonpolar.
- Dispersion forces arise from temporary fluctuations in electron distribution within molecules, resulting in temporary dipoles.
- These temporary dipoles induce corresponding dipoles in neighboring molecules, leading to attractions between the molecules.
- The strength of dispersion forces increases with increasing molecular size and shape.
4. Hydrogen Bond:
- Hydrogen bonding occurs when a hydrogen atom is bonded directly to an electronegative atom (such as nitrogen, oxygen, or fluorine), and the hydrogen atom interacts with a lone pair of electrons on another electronegative atom in a neighboring molecule.
- Hydrogen bonding is a stronger type of dipole-dipole attraction.
- Substances such as water (H2O) exhibit hydrogen bonding, which contributes to unique properties like high boiling point, high surface tension, and strong cohesion.
In summary, for NF3, the major type of attractive force between its particles is dipole-dipole attraction. For ionic compounds, the major type of attractive force is the ionic bond. Dispersion forces exist between all molecules, while hydrogen bonding occurs between molecules with hydrogen atoms bonded to highly electronegative atoms.