Metal + oxygen = ?
Metal oxide
Oxidation reaction
gaining oxygen loss electron
Reduction reaction
losing oxygen gain electron
What happens when group 1 reacts with water
Reacts vigorously and produces alkaline solution
Displacement reaction
A more reactive element can displace a less reactive element from its compound
Oxidation is the gain/loss of electrons
Reduction is the gain/loss of electrons
LOSS
GAIN
2e+ has this lost or gain electrons
lost
Acid produce hydrogen ions (??) in aqueous solutions
H+
Bases
chemicals which can neutralise acid and produce salt n water
Bases soluble in water also called ???
alkalis
Alkalis produce hydroxide ions (???) in aqueous solutions
OH-
Is 0 on the pH scale acid or alkali
Acid
Acid + Metal = ???
Salt + Hydrogen
Neutralisation
acid and a base react to form water and a salt
3 common salts
Chloride
Sulfate
Nitrate
Acid + Carbonate =
Salt + Water + Carbon Dioxide
Making soluble salts
Start with a fixed amount of hydlochoric acid
Gently heat until almost boiling
Add copper oxide and stir - keep repeating until it doesn't the oxide doesn't disappear after stirring anymore
Use filtration to remove unreacted copper oxide
Place Copper sulfate in evaporating dish and heat until half remains
Leave it for 24h for crystals to form
Scrape onto paper towel and pat it dry
Strong acids partially/fully ionise in aqueous solutions
Weak acids partially/fully ionise in aqueous solutions
Fully
partially
Positive Electrode
Anode - lack of electrons
Negative Electrode
Cathode - covered with electrons
Positive ions attracted to Anode or Cathode
Cathode
Anode is oxidation (loss) / reductions (gain)
Oxidation
Metals more reactive than carbon extracted with ?
Metals less reactive than carbon extracted with ?
Electrolysis
Displacement with carbon
Hydrogen produced at cathode if metal more reactive then ??
Hydrogen (only copper silver less reactive than hydrogen btw)
Oxygen is always produced at anode unless what?
Unless there a halogen ion and in that case that halogen is produced
Electrolysis practical
use a measuring cylinder to add 40 ml of copper chloride solution into a beaker
place two graphite rods into the copper sulfate solution - attaching one electrode to the negative terminal of a dc supply, and the other electrode to the positive terminal
place two small test tubes over each electrode to collect any gases produced
turn on the power supply and observe what happens at each electrode
test any gas produced by holding a piece of blue litmus next to the electrode, or by holding a lit splint next to it
record your observations and the results of your tests
repeat steps 1‒6 using sodium chloride solution