Bonding, structure and properties of substances GapFill

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

Ionic compounds have high  concentrationspositivityentropymelting pointsdensitiesconductivity due to strong electrostatic  chargeslayersproductsreactionsattractionsrepulsions between oppositely charged ions.

Small molecules have very weak  metallic attractionslatticesintermolecular forcesmolecular bondsdelocalised electronsionic interactions and so they melt and boil at very low temperatures.

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

Large, regular structures of covalently bonded atoms are called  mega-covalent latticesgiga-covalent formationsgiant covalent structuresionic latticeshuge covalent compoundsalloys. Diamond and  ammoniaozonecarbon dioxidewatersilicasodium chloride are examples.

In metals, atoms arrange into  linescubessquareslayersspherestriangles which can slide over each other when the metal is bent. Mixtures of metals, called  isotopescrystalsbronzepolymerssteelalloys, have distorted layers, and so are  harderdullershiniersofterdarkerpaler than pure metals. Many metals are good  transducersconductorsuserscreatorsconserversinsulators of electricity and heat due to their  small sizedelocalised electronsflexibilitypositive chargesstrong bondingionic interactions.