Atoms 2 (Brett) Flashcards
Are all metals as reactive as others?
No
Effects of a metal being more reactive
Higher tendency to become another compound with another substance
Metal + Acid –>
Salt + Hydrogen
Proof tests for hydrogen
Squeaky pop test (light a match in hydrogen to make it combust, and hence you hear a squeaky pop
Salt combination
Metal + Non-Metal
Reactivity Series (names)
1.Potassium
2.Sodium
3.Calcium
4.Magnesium
5.Aluminum
6.Carbon
7.Zinc
8.Iron
9.Tin
10.Lead
11.Hydrogen
12.Copper
13.Silver
14.Gold
15.Platinum
Reactivity series (symbols)
1.K
2.Na
3.Ca
4.Mg
5.Al
6.C
7.Zn
8.Fe
9.Sn
10.Pb
11.H
12.Cu
13.Ag
14.Au
15.Pt
relationship with electron shielding and electrons
The more shielding, the more reactive and easier it is to lose electrons since they have less traction with the nucleus
Displacement Reactions
Occurs when one element replaces the other in a compound, the more reactive substance replaces the less reactive one
What do chemicals need to react together
Kinetic energy
Methods of increasing likelihood of reactions
1.Increase concentration
2.Increase temperature
3.Increase surface area
4.catalyst
How increasing concentration helps
More particles to react and collide together
How increasing temperature helps
Particles become more energized and move faster, hence meaning more collisions
How increasing surface area helps
More of the substance is exposed with the other substance, hence more particles and more collisions
How catalysts help
They lower the activation energy needed for a reaction to happen
RoR
Rate of Reaction
How to analyze a rate of reaction graph
The steeper the line, the faster the rate of reaction
Endothermic reaction
when the energy of products is more than the energy of reactants, so energy is absorbed hence making it cold
Exothermic reaction
When the energy of the products is less than the energy of the reactants, so energy is released making it hot
Activation energy
The amount of energy needed for the reaction to begin
Energy absorbed
The amount of energy the reactants absorb when forming new products
Energy released
The amount of energy the reactants release when forming new products
iron extraction method
1.Rocks of iron ore are found
2.These contain iron oxide
3.These are placed in a fire and heated up
4.Wood of charcoal is added so that carbon is present
5.Carbon displaces iron from iron oxide
6.Carbon dioxide and iron are formed
7.The pure iron can now be used
Electrolysis
a process that extracts metals in their pure state by melting them down to a liquid state and the running electricity through them
Elements that are extracted using electrolysis
Potassium (K), Sodium (Na), Calcium (Ca), Magnesium (Mg), Aluminum (Al)
Elements that are extracted from their ores with a displacement reaction
Zinc (Zn), Iron (Fe), Lead (Pb), Platinum (Pt)
Bauxite
aluminum oxide
Hematite
Iron oxide
Malachite
Copper carbonate
Copper & Carbon method
1.Put 1 spatula of copper oxide powder in the crucible. Add one spatula of charcoal powder and mix the two together
2.Sprinkle 1 spatula of charcoal powder over the mixture. Put the lid on the crucible
3.Put the crucible, a pipe - clay triangle on a tripod. Put the Bunsen burner under the crucible
4.Heat the crucible strongly for 5 minutes
5.Turn off the Bunsen and wait. don’t remove the lid until the crucible has cooled down
