Chemistry - Key Concepts - (2) Bonding and Structure

A substance with a giant lattice structure where positive and negative ions are strongly held together by electrostatic forces.

Metals have a giant metallic lattice where metal atoms lose outer electrons, forming a 'sea' of delocalized electrons that surround positively charged ions.

A bond formed by the sharing of electrons between two atoms, usually resulting in a molecular structure.

A three-dimensional network of carbon atoms, each covalently bonded to four others. Known for its extreme hardness and high melting point.

Another allotrope of carbon, where each atom is covalently bonded to three others, forming layers stacked together. Soft, good conductor of electricity.

The strong electrostatic forces between positively and negatively charged ions in a lattice structure.

The strong attraction between positive metal ions and delocalized electrons in a giant metallic lattice.

The sharing of a pair of electrons between two atoms, creating a strong bond.

They have low melting and boiling points because the weak intermolecular forces between molecules are easily broken.

Because they lack free-moving electrons to carry charge.

A pure element that exists in multiple forms with different structures and properties.

Diamond is hard because each carbon atom is bonded to four other carbons, creating a strong, rigid structure.

Diamond does not conduct electricity because all the electrons are tightly bound in covalent bonds, preventing electron flow.

Graphite's layers are held together weakly, allowing them to slide over each other, resulting in its softness.

Graphite conducts electricity because its structure allows delocalized electrons to move freely within the layers.

A model showing the 3D structure of molecules using spheres for atoms and sticks for bonds.

Different forms of the same element with distinct structures and properties.

When a substance can be split into simpler substances because it contains two or more elements joined together.

A substance formed by the covalent bonding of two or more atoms.

A long chain molecule formed by joining many smaller molecules (monomers) together.

Substances with low melting and boiling points have weak intermolecular forces.

Longer polymers have more intermolecular forces, requiring more energy to break the bonds, thus increasing their boiling and melting points.

A three-dimensional network of many carbon atoms, each covalently bonded to four other carbon atoms. This structure is responsible for diamond’s hardness.

In graphite, each carbon atom is covalently bonded to three other carbon atoms, forming layers that are held together by weak forces. These layers can slide over one another, making graphite soft.

Covalent compounds have low melting and boiling points because the weak intermolecular forces between molecules are easily broken.

Substances with large molecules have higher melting and boiling points because they experience stronger intermolecular forces, which require more energy to break.

Covalent compounds don’t conduct electricity because they lack free-moving electrons. Their electrons are fixed within the covalent bonds.