Chemistry: Ionic and Covalent Bonding

A chemical bond formed between two non-metals by the sharing of electrons.

A type of covalent bond where both electrons in the shared pair come from the same atom.

A chemical bond formed between a metal and a non-metal by the transfer of electrons.

A charged particle formed when an atom gains or loses electrons.

A large, repeating three-dimensional structure held together by electrostatic forces between oppositely charged ions.

A diagram that shows the arrangement of electrons in an atom or molecule.

The number of covalent bonds an atom forms, which depends on the number of electrons it needs to share to achieve a full outer shell.

A chemical compound with a distinct formula that consists of a single type of ion and another polyatomic ion.

A model of metallic bonding where positively charged ions are arranged in a lattice and surrounded by a sea of delocalized electrons.

The strength of the electrostatic attraction between the positive ions and the delocalised electrons in a metallic lattice. This force is determined by the charge on the ions and their size.

Metals are good conductors of electricity due to the movement of delocalised electrons, which carry charge.

Metals are malleable because the layers of positive ions can slide over each other without breaking the metallic bond. Delocalised electrons allow for this movement.

Metals have high melting points due to the strong electrostatic forces of attraction between the positive ions and delocalised electrons.

A type of crystal structure characterized by a lattice of positively charged ions surrounded by a sea of delocalised electrons.

Physical properties of a substance are characteristics that can be observed without changing the substance's chemical composition. Examples include melting point, boiling point, and conductivity.

Different types of bonding, such as ionic, metallic, covalent, and van der Waals, create different crystal structures, leading to varying physical properties.

A type of intermolecular force that acts between molecules, holding them together in a structure. They are much weaker than covalent bonds.

Substances with a simple molecular structure consist of molecules held together by weak van der Waals forces. These substances have low melting and boiling points and are poor conductors of electricity.

Substances with a macromolecular structure are covalently bonded into a giant lattice structure. Each atom has multiple strong covalent bonds, resulting in high melting points and rigidity.

A giant lattice structure made up of carbon atoms, each bonded to four other carbon atoms. Its strong covalent bonds make it one of the hardest and strongest materials known.

Another macromolecular structure made up of carbon atoms, but with a layered structure. Each carbon atom is bonded to three others in flat sheets, with free electrons moving between these layers, allowing it to conduct electricity.

The shape of a molecule is determined by the number of electron pairs around the central atom. Electron pairs repel each other, resulting in the largest possible bond angles between covalent bonds.

Lone pairs of electrons around the central atom create additional repulsive forces, which changes the bond angles between covalent bonds.

Mercury is the only metal that is liquid at room temperature.

The tendency of an atom to attract electrons towards itself when forming a covalent bond.

The reduction in the angle between covalent bonds caused by the presence of lone pairs.

A molecule with two bonded atoms having different electronegativities, resulting in an uneven distribution of charge.

A covalent bond where the electrons are not shared equally, creating a separation of charge due to differences in electronegativity.

A molecule with a permanent separation of charge due to a difference in electronegativity between the bonded atoms.

The arrangement of atoms and lone pairs in a molecule, determining its shape and properties.

A decrease in electronegativity as you move down a group in the periodic table.

An increase in electronegativity as you move across a period in the periodic table.

Interaction between molecules with permanent dipoles, where the positive and negative ends of one molecule attract opposite ends of another molecule, creating a lattice structure.

The strongest type of intermolecular force. It arises from a special dipole-dipole interaction between a hydrogen atom bonded to a highly electronegative atom (N, O or F) and a lone pair of electrons on an adjacent molecule.

A temporary dipole induced in a molecule due to the presence of an external charged particle or a nearby permanent dipole. This induces a temporary uneven charge distribution within the molecule.

The forces acting between molecules, holding them together in a substance. They are weaker than intramolecular forces (like covalent bonds) within a molecule.

Higher melting and boiling points for substances with hydrogen bonding compared to non-hydrogen bonded molecules. This is because stronger intermolecular forces require more energy to break.