Chemical Bonding.
The electrostatic attraction between positive and negative charged ions.
Positive and negative charges.
The presence of positive and negative ions.
The transfer of electrons between atoms.
Sodium (Na).
Chlorine (Cl).
Sodium ion (Na⁺).
Chloride ion (Cl⁻).
Fluorine (F), Oxygen (O), and Nitrogen (N).
Methane (CH₄).
Al2Cl6.
A covalent bond with a separation of charge between one end and the other.
O2
The molecule does not have a charge difference between one end and the other.
Molecules with hydrogen bonds have a higher boiling point than those with permanent dipoles.
Van der Waals forces.
A covalent bond.
They can move to one end, reversing the polarity of the molecule.
Electrons from one atom.
There is a separation of charge between one end and the other, creating a slightly positive 'top' and a slightly negative 'bottom'.
A covalent bond where both electrons come from the same atom.
Ethane has a lower boiling point than fluoromethane.
It is overall non-polar with a slightly negative 'top' and 'bottom'.
Dative covalent bond.
Attractions between one molecule and a neighboring molecule.
The Pauling scale.
A shared pair of electrons.
Three hydrogen atoms.
Metals generally have lower electronegativity than nonmetals.
H₂
The difference in electronegativity between atoms and the molecular shape.
A charge of +2.
A hydrogen atom bonded to a strongly electronegative atom and another electronegative atom with a lone pair of electrons.
4.0.
Molecules with a permanent separation of charge, leading to dipole-dipole interactions.
Caesium and francium.
H2 or Cl2.
Higher electronegativity differences lead to polar bonds, contributing to molecular polarity.
Electrons from the nitrogen atom.
Octahedral.
Polar molecules.
No, it does not exist; only Al2Cl6 does.
A measure of the tendency of an atom to attract a bonding pair of electrons.
To represent the transfer of electrons between atoms.
Non-polar.
Rapidly fluctuating temporary dipoles.
Electrons from the hydrogen atoms.
Trigonal bipyramidal.
Cl₂
HCl
To illustrate ionic bonding between magnesium and chlorine.
An intermolecular force that forms when a hydrogen atom bonded to a strongly electronegative atom interacts with another electronegative atom that has a lone pair of electrons.
The tendency of an atom to attract electrons in a chemical bond.
They have a partial positive charge on one end and a partial negative charge on the other.
They have an even distribution of electrical charge.
Two electrons.
Van der Waals forces.
V-shape.
CHCl3 is a polar molecule.
CO2
A bond where two pairs of electrons are shared between the atoms.
Hydrogen bond > Permanent dipole > Temporary dipole (Van der Waals forces).
Hydrogen bond.
The more electronegative atom attracts more electron density, becoming slightly negative, while the other atom becomes slightly positive, as in HCl.
By its asymmetrical shape and the presence of polar bonds.
Involves the sharing of electron pairs between atoms.
Greater Van der Waals forces.
Because xenon has a higher number of electrons, leading to stronger temporary dipole forces.
Polar molecules have higher boiling points.
Butane molecules are longer with bigger temporary dipoles and can lie closer together.
Two chloride ions (Cl-).
Molecules with permanent dipoles have higher boiling points than those with only van der Waals forces.
Due to the large permanent dipole on the molecule, as CH3F is polar.
NH3.
They have the same tendency to attract the bonding pair of electrons, as seen in H2 or Cl2 molecules.
A type of intermolecular attraction known as Van der Waals force.
Linear.
Dots represent magnesium's electrons, and crosses represent chlorine's electrons.
120 degrees.
The more electronegative atom (B).
Slightly positive.
Trigonal pyramidal.
CCl4 is a non-polar molecule.
Van der Waals forces or temporary dipole forces.
The polarities of the molecules.
It continues to fluctuate in synchronization.
H2 or Br2.
Electronegativity increases from left to right across a period.
Magnesium ions (Mg²⁺) and oxide ions (O²⁻).
Electronegativity decreases as you move down a group.
Two electrons.
It leads to electrical distortion and temporary dipoles.
Dots represent magnesium's electrons, and crosses represent oxygen's electrons.
To illustrate the ionic bonding between calcium and fluoride ions.
Due to the continuous fluctuation in their polarities.
Covalent bonding.
Temporary dipole (Van der Waals forces).
Polar.
Fluorine.
Electrons from another atom.
Trigonal pyramidal.
Calcium ions (Ca²⁺) and fluoride ions (F⁻).
A charge of -1.
Two fluoride ions.
A strong type of intermolecular attraction that occurs between molecules containing hydrogen bonded to highly electronegative atoms.
0.7.
Lone pair - lone pair.
Bond pair - bond pair.
Ionic bond.
