11: Reactivity of Metals Flashcards
List 4 parameters to compare the reactivity of metals.
- formation rate of products
- consumption rate of reactants
- reacting temperature
- amount of energy change during the reaction
List 3 metals that react with cold water in decreasing order of reactivity.
potassium, sodium, calcium
List 5 metals that react with steam but not with cold water in decreasing order of reactivity.
magnesium, aluminium, zinc, iron, tin
List a metal that reacts with dilute acid but not with steam.
lead
List 2 metals that react with oxygen in air but not with dilute acid in decreasing reactivity.
copper, mercury
What is the word equation for metals’ reaction with oxygen?
metal + oxygen -> metal oxide
What is the word equation for metals’ reaction with liquid water?
metal + water -> metal hydroxide + hydrogen gas
What is the word equation for metals’ reaction with steam?
metal + water(g) -> metal oxide + hydrogen gas
What is the word equation for metals’ reaction with dilute acid?
metal + dilute acid -> metal salt + hydrogen gas
What is the balanced chemical equation for sodium’s reaction with oxygen?
4Na + O2 -> 2Na2O
What is the balanced chemical equation for postassium’s reaction with oxygen?
4K + O2 -> 2K2O
What is the balanced chemical equation for alkali metals’ reactions with oxygen?
4M + O2 -> 2M2O
What is the balanced chemical equation for calcium’s reaction with oxygen?
2Ca + O2 -> 2CaO
What is the balanced chemical equation for magnesium’s reaction with oxygen?
2Mg + O2 -> 2MgO
What is the balanced chemical equation for alkaline earth metals’ reactions with oxygen?
2M + O2 -> 2MO
What is the balanced chemical equation for aluminium’s reaction with oxygen?
4Al + 3O2 -> 2Al2O3
What is the balanced chemical equation for zinc’s reaction with oxygen?
2Zn + O2 -> 2ZnO
What is the balanced chemical equation for iron’s reaction with oxygen?
3Fe + 2O2 -> FeO * Fe2O3
What is the word equation for iron’s reaction with oxygen?
iron + oxygen -> iron(II, III) oxide
What is the balanced chemical equation for lead’s reaction with oxygen?
2Pb + O2 -> 2PbO
What is the balanced chemical equation for copper’s reaction with oxygen?
2Cu + O2 -> 2CuO
Do aluminium compounds have a flame colour?
No, they have no particular colour. The reason they burn with a bright white light is becasue the reaction between aluminium and oxygen gives out a lot of energy.
Do magnesium compounds have a flame colour?
No, they have no particular colour. The reason they burn with a bright white light is becasue the reaction between magnesium and oxygen gives out a lot of energy.
What is the balanced chemical equation for sodium’s reaction with liquid water?
2Na + 2H2O -> 2NaOH + H2
What is the balanced chemical equation for potassium’s reaction with liquid water?
2K + 2H2O -> 2KOH + H2
What is the balanced chemical equation for alkali metals’ reactions with liquid water?
2M + 2H2O -> 2MOH + H2
What is the balanced chemical equation for calcium’s reaction with liquid water?
Ca + 2H2O -> Ca(OH)2 + 2H2
What is the balanced chemical equation for calcium’s reaction with steam?
Ca + H2O -> CaO + 2H2
What is the balanced chemical equation for magnesium’s reaction with steam?
Mg + H2O -> MgO + H2
What is the balanced chemical equation for aluminium’s reaction with steam?
2Al + 3H2O -> AL2O3 + 3H2
Why do metals form oxides when reacted with steam and hydroxides when reacted with water?
In steam, the water molecules are packed less closely together. One metal atom is less likely to react with two water molecules to form metal hydroxides than to form metal oxides.
List 5 metals that react with steam but not cold water in decreasing order of reactivity.
magnesium, aluminium, zinc, iron, tin
List 6 metals that react with do not react with water nor steam in decreasing order of reactivity.
lead, copper, mercury, silver, platinum, gold
What is the balanced chemical equation for alkali metals’ reactions with dilute hydrochloric acid?
2M + 2HCl -> 2MCl + H2
What is the balanced chemical equation for alkali metals’ reactions with dilute sulphuric acid?
2M + H2SO4 -> M2SO4 + H2
What is the balanced chemical equation for alkali metals’ reactions with dilute nitric acid?
2M + 2HNO3 -> 2MNO3 + H2
What is the balanced chemical equation for alkaline earth metals’ reactions with dilute hydrochloric acid?
M + 2HCl -> MCl2 + H2
What is the balanced chemical equation for alkaline earth metals’ reactions with dilute sulphuric acid?
M + H2SO4 -> MSO4 + H2
What is the balanced chemical equation for alkaline earth metals’ reactions with dilute nitric acid?
M + 2HNO3 -> M(NO3)2 + H2
What is the balanced chemical equation for lead’s reaction with dilute nitric acid?
Pb + 2HNO3 -> Pb(NO3)2 + H2
What is the balanced chemical equation for iron’s reaction with dilute sulphuric acid?
Fe + H2SO4 -> FeSO4 + H2
What is the word equation for iron’s reaction with dilute sulphuric acid?
iron + dilute sulphuric acid -> iron(II) sulphate + hydrogen
List 2 metals that react with dilute hydrochloric acid explosively in decreasing order of reactivity.
potassium, sodium
List 5 metals that do not react with dilute hydrochloric acid in decreasing order of reactivity.
copper, mercury, silver, platinum, gold
What is the meaning of a double arrow in chemical equations?
The reaction is reversible.
What is the definition of reactivity of metals?
The most reactive metal is the one that has the highest tendency to lose the outermost shell electron(s) to form a positive ion.
Why are alkali metals more reactive than alkaline earth metals in the same period?
Alkali metals lose one electron to form ions, while alkaline earth metals lose 2. Losing one electron is easier than losing 2 electrons. This is because once an electron is removed from an atom, a positive ion is created and it attracts a negatively charged ion more strongly than a neutral atom. Therefore, more energy is required to remove the second electron and so on.
Why are metals from lower periods more reactive than those from upper periods from the same group?
shielding effect: as the number of protons increases, the attraction force between nucleus and electrons increases. However, the inner shell electrons exert more repulsion to the outermost electrons. The increase in shielding effect outweighs the increase in nuclear charge, so it is overall easier for metals to lose electrons down the group. Therefore, metals are more reactive down the group.
What is a displacement reaction?
In a displacement reaction, a more reactive metal displaces a less reactive metal from its compound in a solution.
List 2 observations when a piece of copper is added to silver nitrate solution.
- A grey solid is deposited on the copper.
- The solution turns from colourless to blue.
What is the definition of spectator ions?
Spectator ions are ions that do not change their physical state nor chemical nature in a chemical reaction.
What is the ionic equation of silver nitrate’s reaction with sodium chloride?
- balanced chemical equation with physical states: AgNO3(aq) + NaCl(aq) -> AgCl(s) + NaNO3(aq)
- rewriting aqueous compounds as ions: Ag+(aq) + NO3-(aq) + Na+(aq) + Cl-(aq) -> AgCl(s) + Na+(aq) + NO3-(aq)
- deleting spectator ions: the ionic equation is Ag+(aq) + Cl-(aq) -> AgCl(s)
What is the ionic equation of sodium hydroxide’s reaction with hydrochloric acid?
- balanced chemical equation with physical states: NaOH(aq) + HCl(aq) -> NaCl(aq) + H2O(l)
- rewriting aqueous compounds as ions: Na+(aq) + OH-(aq) + H+(aq) + Cl-(aq) -> Na+(aq) + Cl-(aq) + H2O(l)
- deleting spectator ions: the ionic equation is H+(aq) + OH-(aq) -> H2O(l)
What is the relationship between the reactivity and the ease of extraction of a metal?
The more reactive a metal is, the more difficult it is the be extracted from its ore.
What is the relationship between the reactivity of a metal and the stability of its compounds?
The more reactive a metal is, the more stable its compounds are likely to be. (example: the less reactive a metal is, the more readily its oxide decomposes when heated.)
What is the definition of thermit reaction?
Thermit reactions are exothermic reactions between a metal powder and a metal oxide.
