Bonding key terms

ionic bond

The electrostatic attraction between oppositely charged ions. In Ionic bonding, ionic bond is used to explain describe ionic bonding as electrostatic attraction between oppositely charged ions with A-Level Chemistry precision.

electrostatic attraction

The force that draws together positively and negatively charged ions in an ionic bond.

ionic lattice

A three-dimensional structure formed by the electrostatic attraction between oppositely charged ions.

electrostatic attraction

The force that draws together positively and negatively charged ions in an ionic compound.

ionic lattice strength

The strength of an ionic lattice is determined by the charge of the ions and their ionic radii.

ionic radius

The ionic radius is the measure of an ion's size, which affects the distance between ions in an ionic lattice.

ionic bond

The electrostatic attraction between oppositely charged ions in an ionic compound. In Ionic bonding, ionic bond is used to explain explain the physical properties of ionic compounds using lattice structure with A-Level Chemistry precision.

lattice structure

A regular arrangement of ions in an ionic compound that determines its physical properties.

covalent bond

A covalent bond is formed when two atoms share pairs of electrons. In Covalent bonding and molecular shape, covalent bond is used to explain describe covalent bonding as shared pairs of electrons with A-Level Chemistry precision.

shared pairs of electrons

Shared pairs of electrons are pairs of electrons that are shared between two atoms, forming a covalent bond.

electron-pair repulsion

The principle that electron pairs around a central atom will arrange themselves as far apart as possible to minimize repulsion.

molecular shape

The three-dimensional arrangement of atoms in a molecule, determined by the number of bonding and lone pairs of electrons around the central atom.

lone pair

A pair of valence electrons that are not shared with another atom, influencing molecular geometry.

bond angle

The angle formed between two bonds that originate from the same atom, which can be affected by the presence of lone pairs.

molecular shape

The three-dimensional arrangement of atoms within a molecule, determined by the bonding and lone pairs of electrons.

bond angle

The angle formed between two bonds that originate from the same atom, influenced by electron pair repulsion.

metallic bonding

Attraction between positive metal ions and delocalised electrons. In Metallic bonding, metallic bonding is used to explain describe metallic bonding as attraction between positive ions and delocalised electrons with A-Level Chemistry precision.

delocalised electrons

Electrons that are free to move throughout a metallic structure, contributing to conductivity.

metallic bonding

Attraction between positive metal ions and delocalised electrons, allowing for electrical conductivity.

electrical conductivity

The ability of a material to conduct electricity, which in metals is due to the presence of delocalised electrons.

metallic bonding

Attraction between positive metal ions and delocalised electrons that allows metals to conduct electricity and be malleable.

malleability

The ability of a material to be shaped or deformed without breaking, due to the flexibility of metallic bonds.

metallic bond

The attraction between positive metal ions and delocalised electrons that holds the metal structure together.

melting point

The temperature at which a solid turns into a liquid, indicating the energy needed to overcome the forces holding the particles in a solid structure.

electronegativity

The ability of an atom to attract bonding electrons. In Electronegativity and bond polarity, electronegativity is used to explain define electronegativity as the ability of an atom to attract bonding electrons with A-Level Chemistry precision.

bond polarity

The distribution of electrical charge over the atoms joined by the bond. In Electronegativity and bond polarity, bond polarity is used to explain define electronegativity as the ability of an atom to attract bonding electrons with A-Level Chemistry precision.

electronegativity

The ability of an atom to attract bonding electrons in a covalent bond. In Electronegativity and bond polarity, electronegativity is used to explain use electronegativity differences to explain polar bonds with A-Level Chemistry precision.

polar bond

A covalent bond between two atoms with different electronegativities, resulting in a dipole moment.

polar bond

A polar bond is a type of covalent bond where the electrons are shared unequally between two atoms, resulting in a dipole moment.

polar molecule

A polar molecule is a molecule that has a net dipole moment due to the arrangement of polar bonds, leading to an overall charge separation.

bond dipole

A measure of the polarity of a bond, indicating the separation of positive and negative charges due to differences in electronegativity between bonded atoms.

molecular shape

The three-dimensional arrangement of atoms in a molecule, which influences the distribution of bond dipoles and overall molecular polarity.

London dispersion forces

Weak intermolecular forces arising from temporary dipoles in molecules. In Intermolecular forces, London dispersion forces is used to explain describe London dispersion forces between molecules with A-Level Chemistry precision.

molecular size

The size of a molecule, which affects the strength of London dispersion forces. In Intermolecular forces, molecular size is used to explain describe London dispersion forces between molecules with A-Level Chemistry precision.

London dispersion forces

Weak intermolecular forces arising from temporary dipoles in molecules due to fluctuations in electron distribution.

molecular size

The size of a molecule, which influences the strength of London dispersion forces based on surface area and contact.

permanent dipole-dipole forces

Attractive forces between the positive end of one polar molecule and the negative end of another polar molecule.

polar molecule

A molecule that has a net dipole moment due to the presence of polar bonds and an asymmetrical shape.

hydrogen bond

A strong type of intermolecular force that occurs between molecules containing hydrogen bonded to highly electronegative atoms such as nitrogen, oxygen, or fluorine.

conditions for hydrogen bonding

The presence of a hydrogen atom covalently bonded to a highly electronegative atom, which creates a dipole and allows for attraction to other electronegative atoms.

boiling point

The temperature at which a liquid's vapor pressure equals the external pressure, causing it to change into a gas.

volatility

The tendency of a substance to vaporize; higher volatility indicates a lower boiling point and weaker intermolecular forces.