Identify the major type of attractive force between the particles of each of the following:
NF3
dipole dipole attraction
ionic bond
dispersion forces
hydrogen bond
NF3: dipole-dipole attraction, dispersion forces
The major type of attractive force between the particles of each of the given substances is as follows:
NF3:
- Dipole-dipole attraction: The NF3 molecule is polar, meaning it has a slight positive charge on the nitrogen atom and a slight negative charge on the fluorine atoms. This leads to an attraction between the positive and negative ends of neighboring NF3 molecules.
Dipole-dipole attraction:
- This is an attractive force between two polar molecules. It occurs when the positive end of one molecule is attracted to the negative end of another molecule.
Ionic bond:
- This is a type of chemical bond formed between atoms that have gained or lost electrons, resulting in positively charged ions (cations) and negatively charged ions (anions). The attraction between these oppositely charged ions leads to the formation of ionic compounds.
Dispersion forces:
- Also known as London dispersion forces or van der Waals forces, these are weak forces that exist between all atoms and molecules, regardless of their polarity. They arise due to temporary fluctuations in electron distribution, creating temporary dipoles in the particles and inducing similar dipoles in neighboring particles.
Hydrogen bond:
- This is a type of intermolecular force that occurs when a hydrogen atom is bonded to a highly electronegative atom (such as nitrogen, oxygen, or fluorine) and is attracted to a lone pair of electrons on a nearby molecule. Hydrogen bonds are stronger and more specific than dipole-dipole interactions.
To identify the major type of attractive force between the particles of each substance, we need to analyze the chemical composition of each one:
1. NF3 (Nitrogen Trifluoride):
The NF3 molecule consists of one nitrogen atom (N) and three fluorine atoms (F). In this case, the major type of attractive force between the particles is a dipole-dipole attraction.
Dipole-dipole attractions occur between polar molecules, which have an uneven distribution of electron density. In NF3, the fluorine atoms are more electronegative than the nitrogen atom, resulting in a polar covalent bond between nitrogen and fluorine. This leads to the formation of partial positive and negative charges, creating a dipole. These dipoles attract each other, resulting in dipole-dipole interactions between NF3 molecules.
2. Ionic Bond:
Ionic bonds occur between ions of opposite charges. They form when one or more electrons are transferred from one atom to another. This exchange of electrons creates positive and negative ions that attract each other due to their opposite charges.
3. Dispersion Forces:
Dispersion forces, also known as London dispersion forces, are the weakest type of intermolecular force. They occur between nonpolar molecules or atoms due to temporary fluctuations in electron distribution.
4. Hydrogen Bond:
A hydrogen bond is a special type of dipole-dipole interaction. It occurs when hydrogen is bonded to an electronegative atom (such as nitrogen, oxygen, or fluorine) and forms another polar bond with a nearby electronegative atom.
In summary:
- NF3 experiences dipole-dipole attractions.
- Ionic bonds occur between ions of opposite charges.
- Dispersion forces occur between nonpolar molecules or atoms.
- Hydrogen bonds occur between molecules containing hydrogen bonded to electronegative atoms.