Identify the major type of attractive force between the particles of each of the following:
BrF
dipole dipole attraction
ionic bond
dispersion forces
hydrogen bond
dipole-dipole attraction
The major type of attractive force between the particles of each of the following substances is:
1. BrF: The major type of attractive force between BrF molecules is dipole-dipole attraction. This occurs because BrF is a polar molecule due to the difference in electronegativity between bromine (Br) and fluorine (F). The partial positive charge on the Br atom attracts the partial negative charge on the F atom in adjacent molecules.
2. Ionic Bond: Ionic bonds are the major type of attractive force in ionic compounds. This occurs when one or more electrons are transferred completely from one atom to another, resulting in the formation of positively charged cations and negatively charged anions. The attractive force between the oppositely charged ions keeps the compound together.
3. Dispersion Forces: Dispersion forces, also known as London dispersion forces, are the major type of attractive force in nonpolar molecules, such as noble gases or hydrocarbons. These forces arise due to temporary fluctuations in electron distribution, creating temporary dipoles in nearby molecules that induce attraction.
4. Hydrogen Bond: Hydrogen bonding occurs when a hydrogen atom is bonded to a highly electronegative atom (e.g., oxygen, nitrogen, or fluorine) and is attracted to another electronegative atom in a nearby molecule. This type of attraction is stronger than the dipole-dipole forces and is responsible for many unique properties of substances like water, ammonia, or DNA.
To identify the major type of attractive force between the particles of each of the following substances, we will need to analyze their molecular composition and consider the type of chemical bonding present. Let's break it down:
1. BrF:
BrF stands for Bromine Fluoride. It is composed of one bromine atom (Br) and one fluorine atom (F).
The molecular structure of BrF is linear, with the bromine atom bonded to the fluorine atom.
The electronegativity difference between bromine and fluorine is large enough to result in a highly polar covalent bond.
Therefore, the major type of attractive force between the particles in BrF is dipole-dipole attraction.
2. Ionic bond:
An ionic bond forms between a metal and a non-metal.
It involves the transfer of electrons from the metal to the non-metal, resulting in the formation of positively charged cations and negatively charged anions.
An example of a substance that has an ionic bond is sodium chloride (NaCl), where the electrons are transferred from sodium to chlorine.
Ionic bonds exhibit strong electrostatic attractions between the oppositely charged ions.
3. Dispersion forces:
Dispersion forces, also known as London dispersion forces, exist between all atoms and molecules.
These forces result from temporary fluctuations in electron density, leading to the formation of temporary dipoles.
Substances composed of non-polar molecules, such as noble gases or non-polar compounds, mainly experience dispersion forces.
Dispersion forces are the weakest of the intermolecular forces.
4. Hydrogen bond:
Hydrogen bonding occurs when a hydrogen atom is covalently bonded to an electronegative atom (such as nitrogen, oxygen, or fluorine) and interacts with another electronegative atom nearby.
This interaction creates strong attraction between hydrogen and the lone pair of electrons on the other atom.
Hydrogen bonding is stronger than dipole-dipole interactions and is responsible for many unique properties of substances, such as water (H2O).
In conclusion:
- For BrF, the major type of attractive force is dipole-dipole attraction.
- Ionic bonds occur between metals and non-metals.
- Dispersion forces are present in all atoms and molecules.
- Hydrogen bonding forms between hydrogen and electronegative atoms.