Flame test practical

Purpose:
Conduct an experiment to find out which color is the flame of certain ionic compounds (liquid), by exposing them to a flame with a wire loop.

Materials:
• Acid
• Liquid PotassiumNitrate (KNO3)
• Liquid Calcium Chloride (CaCl2)
• Liquid Barium Chloride (BaCl2)
• Liquid Copper Sulfate (CuSO4)
• Liquid Lead Nitrate (Pb2)
• Liquid Sodium Chloride (NaCl)

Equipment:
• Bunsenburners
• Test tubes
• Wire loops
• Matches
• Goggles
• Lab coat

Safety/Method/ Instructions:
• Warning: Practical involves fire and ionic compounds that might give unwanted reactions to itshandler like a chemical burn, for instance the acid used. Stowe away all bags and keep the aisles bag free so no one will trip and tie hair back so nobody´s hair will get burn. Use the goggles and labcoats properly for extreme safety.
• Set up Bunsen burners by adjusting it´s red “hose” to the gas dispenser.
• Clean the wire loop with acid and then expose it to the flame so it’ll get rid of anypast chemicals.
• Dip wire loop into known samples and test in flame- record the color seen.
• Clean the wire loop again with the acid and burn until it doesn’t release a flame of a specific color.• Repeat with other known samples.
• Repeat with unknown samples.

Results Known Elements:
Known Samples KNO3 or
KCl CaCl2 or Ca(NO3)2 BaCl2 CuSO4 or Cu(NO3)2 Pb(NO3)2 NaCl
Color of FlameViolet/pink Red Light green Strong green Violet Orange

Results Unknown Elements:
Unkown Samples Color of Flame Ionic Compound
1 Light green BaCl2
2 violet/pink KNO3 or KCl
3 Red CaCl2 orCa(NO3)2
4 orange NaCl

Conclusion:
The main reason as to why the different ionic compounds produce different flames is because they have their electrons that get excited due to the heat energy, in thiscase, that they are exposed to, and when they go back to their ground state they release energy and produce a photon of light which varies from compound to compound due to their properties (flame...