Monday, 12 January 2015

1f) Ionic compounds + 1g) covalent compounds

Ionic bonding:

  • strong electrostatic attraction 
  • opposite charged ions 
  • throughout lattice 

Properties of ionic compounds:
  • high melting point 
  • strong electrostatic attraction 
  • giant ionic lattice 
  • soluble in water 
  • Ions attracted to polar water molecules 
  • conduct electricity 
  • ions can move and carry charge
A Lattice is a 3-D network of ions in fixed positions bonded together 


OIL RIG 

Oxidation- loses electrons                      Reduction- gains electrons 



Group 1 2 3 4 5 6 7 0/8
Charge 1+ 2+ 3+ X 3- 2- 1- X

Covalent bonding:
  • non metal with non metal 
  • outer shells overlap 
  • electron shared in pairs 
  • atoms achieve outer shells (full)
  • attracts both nuclei 


Properties of simple covalent molecules:
  • very strong bonds
  • low melting and boiling points 
  • insoluble in water 
  • no free electrons 
  • Don't conduct electricity 
  • soluble in organ solvents 
Intermolecular forces 
  • weak bonds
  • easily broken 
Giant covalent bonds 
  • strong bonds 
  • no free electrons 
  • rigid 
  • all atoms joined together 
  • covalent unreactive 
Diamonds 
  • rigid 
  • hard 
  • sparkly
  • four covalent bonds  
Graphite
  • layers three covalent bonds 
  • slide over each other 
  • free electrons 
  • good conductor of electricity 
  • lubricant 

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