bonding and structure

metals want to _____ electrons

non-metals want to ____ electrons

metals want to lose electrons to get pos charge

non-metals want to gain electrons to get neg charge

Ionic bond

the electrostatic attraction between oppositely charged ions

poly atomic ions

hydroxide

nitrate

carbonate

sulphate

ammonium

ionic compound structure

giant ionic lattice of negative and positive ions held together by electrostatic force of attraction

ionic compounds

1. MP and BP

2. Solubility

3. Electrical conductivity

1. high - electrostatic attraction is very strong , at room temp there is insufficient energy to overcome the attraction so ionic compounds are mostly solid at room temperatures - higher charge = higher attraction

2. ions must separate and force of attraction must be overcome - many dissolve in polar solvents (like water) - water molecules surround the lattice, if attraction between water molecules and ions is greater than between ions - substance will dissolve - higher charge = decr. solubility

3. to conduct electricity - charged particles that are free to move - ionic compound has charged particles but they are not free→ needs to be melted or dissolved

covalent bonding

covalent bonding is the string electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

carbon standard form

graphite

number of covalent bonds

energy is released everytime a covalent bond is formed

energy lost = more stable

an atom wants to make as many covalent bonds as possible

boron bonds

3 covalent bonds

6 outer electrons

pg 27 chap 5 booklet

read it

single covalent bond]

double covalent bond

triple covalent bond

one shared pair of electrons

two shared pairs of electrons

three shared pairs of electrons

dative/coordinate covalent bond

covalent bond in which both electrons in the shared pair have been provided by the same atom

shared electron pair was originally a lone pair

shown by a bond with an arrow head