Lesson 1.2: Intermolecular Forces of Attraction Flashcards
The force of attraction between oppositely charged particles (i.e., ions) present in ionic compounds gives rise to __________.
ionic bonds
Because these particles have distinct charges, the force of attraction that holds the formula units (particles of ionic compounds) together is described as __________ in nature and is strong enough to keep the compound solid at room temperature.
coulombic
It refers to the particles of ionic compounds.
formula units
It refers to the particles of covalent compounds.
neighboring molecules
They are with relatively weaker intermolecular forces that may only exist as liquids.
covalent compounds
Example of a covalent compound.
water
Substances with no appreciable intermolecular forces have their molecules freely moving around and less contained by the attraction of other surrounding molecules.
gases
What are dipole-dipole and London dispersion forces collectively known as?
van der Waals forces
A type of bond that is formed when 1 atom transfers electrons to another atom, resulting in the formation of oppositely charged ions.
ionic bond
It is composed of a cation and an anion.
ion
A type of bond in which electrons are transferred from a metal to a nonmetal.
ionic bond
A type of bond that increases the melting and boiling point.
ionic bond
The electronegativity difference of ionic bond.
> _2.0 (large)
A type of bond wherein the electrons are shared between two nonmetal atoms.
covalent bond
The electronegativity difference of covalent bonds.
<2.0 (small)
A type of bond wherein its bond strength is strong due to electrostatic forces.
ionic bond
A type of bond wherein its bond strength is generally weaker than ionic bond.
covalent bond
Examples of covalent bonds.
- Water (H20)
- Carbon Dioxide (CO2)
- Methane (CH4)
It refers to the tendency of an atom to attract shared electrons in a bond.
electronegativity
The EN of a nonpolar covalent.
<0.4 (0-0.4)
The EN of a polar covalent.
<2.00 (0.5-2.0)
The EN of an ionic bond.
> _2.0 (2.1-above)
The EN of a nonpolar bond.
0
The EN of a polar bond.
0.9
It refers to a molecule or a part of a molecule with 2 opposite charges (a + end and a - end), resulting from an unequal distribution of electrons between two atoms involved in a chemical bond.
dipole
It refers to the term that means evenly distributed and equal number of protons and electrons.
neutral
An intermolecular force that exist between polar molecules.
dipole-dipole forces
Example of dipole-dipole forces.
Hydrogen Chloride (HCI)
An intermolecular force that possess a permanent dipole moment attributed to the difference in electronegativities of their component atoms and how these atoms are arranged in space.
dipole-dipole forces
An intermolecular force that is a special type of dipole-dipole interaction that exists only in molecules that contain a hydrogen atom bonded to a small, highly electronegative atom.
hydrogen bond
Example of a hydrogen bond.
N, O, or F.
An intermolecular force that the more electronegative atom pulls the electron toward itself and gains a relatively large partial negative charge.
hydrogen bond
Unlike covalent bonding, where electrons are involved and shared between atoms, __________ is not a real chemical bond participated in by electrons.
hydrogen bond
It is a type of intramolecular force of attraction.
covalent bond
It is intermolecular in nature.
hydrogen bonds
An intermolecular force that is stronger than regular dipole-dipole forces.
hydrogen bonds
An intermolecular force that acts between an ion and a polar molecule.
ion-dipole forces
It refers to the positively charged ions.
cations
They interact more strongly with dipoles than anions.
cations
They are negatively charged ions.
anions
An intermolecular force that is common in solutions of ionic compounds dissolved in polar solutions.
ion-dipole forces
An intermolecular force that have these kinds of examples:
- Na+ ions interacting with water molecules in a saltwater solution
- Sodium ion in Methanol
- Chloride ion in Ammonia
ion-dipole forces
An intermolecular force that are simply dispersion forces.
London dispersion forces
An intermolecular force that exist between all atoms and molecules.
London dispersion forces
An intermolecular force that are the only forces acting in nonpolar molecules.
London dispersion forces
An intermolecular force that arise from the continuous movement of electrons in particles.
London dispersion forces
They have zero dipole moment because their electron density is uniform and symmetrical.
nonpolar molecules
It refers to a temporary dipole.
instantaneous dipole
This dipole can then induce dipoles in neighboring molecules.
instantaneous dipole
An intermolecular force that are attractions between an instantaneous dipole and an induced dipole, as in the two helium atoms.
London dispersion forces
It can affect the London dispersion force between two molecules.
the size of a molecule
An intermolecular force that have the weakest IMF.
London dispersion forces
An intermolecular force that attract between noble gases.
London dispersion forces
An intermolecular force that uses Have No Fear of Iced Cold Beer.
London dispersion forces
An intermolecular force that are stronger than London dispersion forces.
dipole-dipole forces
