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Metallic and Covalent Bonding Cheat Sheet (DRAFT) by

common properties of metals in relation to lattice structure, common properties of ionic bonds in relation to crystal structure, naming and formulas of ions, polyatomic ions, precipitation reactions, balancing equations

This is a draft cheat sheet. It is a work in progress and is not finished yet.

properties of metals

malleable and ductile
electrons are able to reposition themselves to maintain electr­ostatic bonds when put under pressure, preventing the material from splitting
lustre
electrons are good reflectors of photons
high melting and boiling point
metals are held together by strong non-di­rec­tional electr­ostatic attrac­tion, meaning a large amount of heat energy is required to deform the structure of the crystal lattice
electrical conduc­tivity
free moving electrons can carry electr­icity across the material
heat conduc­tivity
electrons aren't held in place firmly so can vibrate enough to pass and hold heat

balancing chemical equations

1. the number of atoms of an element should be the same on both sides of the equation (may require multiples of compounds)
2. all compounds should have no net charge (swap and drop)
 

properties of cations

brittle, hard
low melting point
unable to conduct electr­icity solid
electrical conduc­tivity in aqueous and molten states

naming ionic compounds

cation
when writing the name of an ionic compound the cation keeps its original name
anion
whereas the anion is reduced to its root and the suffix '-ide' is added
transition metals
transition metals are able to gain and lose a variation of electrons as required, therefore when written the charge should be included in brackets in roman numerals

precip­itation reactions

1. reactants are two compound
2. being aqueous, the compounds are actually separated into ions
3. the reactants swap anions
4. solubility is determined by solubility table, one resulting compound must be a solid for it to qualify as a precip­itate reaction
 

polyatomic ions

ammonium
NH4+
hydroxide
OH-
nitrate
NO3-
bicarb­onate
HCO3-
carbonate
CO32-
sulfate
SO42-
phosphate
PO43-

always soluble compounds

soluble compounds
insoluble exceptions
Grp 1 ions
None
NO3- & CH3COO-
None
Cl-, Br- & I-
Ag+, Pb2+ & Hg+