Bonding, structure and properties of substances GapFill

Substances can be in one of three states of matter, which are called solid, liquid and  gasparticleaquamixturesteamair. Substances are different states at different  chargestimeshumiditiesconcentrationsvoltagestemperatures. The states of matter can also be given symbols, which are  [s], [l], [m] and [aq](so), (li), (ga) and (aq)(s), (l), (g) and (aq)[sol], [liq], [gas] and [aqu](s), (l), (m) and (a)(so), (li), (pa) and (aq).

Ionic compounds have high  positivityconductivitymelting pointsentropyconcentrationsdensities due to strong electrostatic  layersproductschargesrepulsionsreactionsattractions between oppositely charged ions.

Small molecules have very weak  ionic interactionslatticesintermolecular forcesmolecular bondsdelocalised electronsmetallic attractions and so they melt and boil at very low temperatures.

Polymers are large molecules with  electricioniclayeredliquidmetalliccovalent bonds between atoms. Polymers have relatively strong intermolecular forces, so are mostly  whitechargedsolidfrozenlocalisedconductive at room temperature.

Large, regular structures of covalently bonded atoms are called  giga-covalent formationshuge covalent compoundsionic latticesgiant covalent structuresalloysmega-covalent lattices. Diamond and  waterozonecarbon dioxidesodium chloridesilicaammonia are examples.

In metals, atoms arrange into  cubestrianglessquareslayerslinesspheres which can slide over each other when the metal is bent. Mixtures of metals, called  isotopesbronzecrystalssteelalloyspolymers, have distorted layers, and so are  shinierdarkerpalersofterdullerharder than pure metals. Many metals are good  creatorsusersconserverstransducersinsulatorsconductors of electricity and heat due to their  ionic interactionssmall sizedelocalised electronsflexibilitystrong bondingpositive charges.