Identify the major type of attractive force between the particles of each of the following:
KCI
dipole dipole attraction
ionic bond
dispersion forces
hydrogen bond
KCI:
- Ionic bond (between the potassium cation (K+) and chloride anion (Cl-))
Dipole dipole attraction:
- molecules that have polar covalent bonds and interact through the attraction between their partial positive and partial negative charges
Dispersion forces:
- weak forces of attractions between atoms or molecules due to temporary fluctuations in the electron distribution
Hydrogen bond:
- a stronger type of dipole-dipole attraction that occurs when hydrogen is directly bonded to a highly electronegative atom (such as oxygen, nitrogen, or fluorine) and is attracted to another electronegative atom in a different molecule.
KCI:
The major type of attractive force between the particles in KCI is an ionic bond. Ionic bonding occurs between a metal cation (K+) and a non-metal anion (Cl-), resulting in the formation of a crystal lattice structure.
Dipole-dipole attraction:
Dipole-dipole attractions occur between polar molecules. They can be thought of as the electrostatic interaction between the positive end of one molecule and the negative end of another molecule. This type of attractive force exists among polar molecules due to the separation of positive and negative charges within the molecule.
Dispersion forces:
Dispersion forces, also known as London forces, are attractive forces that exist between all molecules, regardless of whether they are polar or non-polar. These forces arise from temporary fluctuations in electron distribution, resulting in a temporary partial charge on one molecule, which induces a partial charge in a neighboring molecule, causing them to attract each other.
Hydrogen bond:
Hydrogen bonding is a special type of dipole-dipole attraction that occurs when a hydrogen atom is bonded to a highly electronegative atom (such as N, O, or F) and experiences a strong attraction to another electronegative atom in a different molecule. Hydrogen bonding is responsible for many important properties of substances such as water and DNA.
To identify the major type of attractive force between the particles in each of the following substances, we need to understand the nature of the particles and the type of bonding involved:
1. KCI (potassium chloride): The attractive force between the particles in KCI is an ionic bond. KCI is made up of positively charged potassium ions (K+) and negatively charged chloride ions (Cl-). Ionic bonds form when one or more electrons are transferred from the metal atom (potassium) to the non-metal atom (chlorine), resulting in the formation of oppositely charged ions that are attracted to each other.
2. Dipole-dipole attraction: This type of attractive force occurs between polar molecules. Polar molecules have asymmetric charge distributions, meaning they have a partially positive end and a partially negative end. When dipole-dipole attractions occur, the positive end of one polar molecule is attracted to the negative end of another polar molecule. This force is weaker than ionic bonds and typically occurs in compounds with significant differences in electronegativity, such as hydrogen fluoride (HF) or chloroform (CHCl3).
3. Dispersion forces (also called London dispersion forces or van der Waals forces): These forces exist in all molecules, including atoms. Dispersion forces occur due to temporary fluctuations in electron distribution, creating temporary dipoles. These temporary dipoles induce dipoles in neighboring particles, leading to attractive forces. Dispersion forces are the weakest type of intermolecular force and are present in all substances, including nonpolar molecules like hydrocarbons.
4. Hydrogen bond: Hydrogen bonding occurs when a hydrogen atom, bonded to an electronegative atom such as nitrogen (N), oxygen (O), or fluorine (F), is attracted to another electronegative atom in a different molecule. Hydrogen bonds are stronger than dipole-dipole attractions and are responsible for many of the unique properties of substances such as water (H2O) and ammonia (NH3).