topic 4: inorganic chemistry and the periodic table Flashcards
down the group, what happens to the atomic radius of group 2 and why?
increases
because of the addition of electron shells
down the group, what happens to the ionisation energy of group 2 and why?
decreases
- extra shells aded means that there is more electron shielding so there is weaker nuclear attraction between the positive nucleus and negative outer electrons
- larger atomic radius so the outer electrons are also further from the nucleus which weakens nuclear attraction
- easier to remove the outer electron so less energy is needed
down the group, what happens to the reactivity of group 2 and why?
increases
increased electron shielding and atomic radius makes the outer electrons easier to lose therefore reactivity increases
what is formed when group 2 metals react with chlorine?
down the group why do the reactions become more vigorous?
- metal chlorides (white precipitates)
-> e.g Mg + Cl2 -> MgCl2 - the elements are more reactive (increased electron shielding and atomic radius makes the outer electrons easier to lose therefore reactivity increases)
what is formed when group 2 metals react with water?
down the group why do the reactions become more vigorous?
If Mg reacts slowly with water, how can the reaction be sped up?
- forms metal hydroxides (base) which form an alkaline solution
-> Mg + 2H2O -> Mg(OH)2 +H2 - the elements are more reactive (increased electron shielding and atomic radius makes the outer electrons easier to lose therefore reactivity increases)
- reaction of Mg and water is faster using steam as it provides the reaction with extra energy
what is formed when group 2 metals react with oxygen?
strontium and barium can react oxygen and heat energy to form?
- forms oxides
e.g 2Mg + O2 -> 2MgO - metal peroxides
M (metal)
M + O2 -> MO2
how are alkaline solutions formed when group 2 metals are added to water?
- oxides react readily with water to make hydoxides which dissociate to form OH- ions
- becomes more strongly alkaline as we go down the group as the hydroxides become more soluble
what happens when group 2 reacts with dilute acids?
metal compounds + hydrogen gas
what forms when group 2 hydroxides react with dilute acid?
- forms salt and water (neutralisation reaction)
HCl: chloride salt
sulfuric acid: sulfate salt
nitric acid: nitrate salts
down the group, why does the solubility of group 2 hydroxides increase?
the ionic size of the metal ions increases. Larger ions have weaker attractive forces and lower lattice energies. The decrease in lattice energy makes it easier for the larger hydroxide compounds to dissolve in water
Larger metal ions in Group 2 elements have a lower charge density, making them more easily surrounded by water molecules. This process of hydration releases energy, known as hydration energy. The increase in the number of water molecules surrounding larger ions leads to a more stable and soluble complex in solution.
down the group, why do group 2 sulphates decrease in solubility
the ionic size of the metal ions increases. Larger ions have weaker attractive forces between them and the water molecules in solution. This decrease in attraction makes it more difficult for the larger ions to be fully surrounded by water molecules and consequently reduces their solubility.
the lattice energy decreases because the larger ions have a lower charge density and weaker attraction, resulting in a less stable lattice. With a weaker lattice, the sulfates are less likely to dissolve readily in water
what is thermal decomposition?
the breakdown of a compound into simpler substancesvia heat
after undergoing thermal decomposition, group 2 carbonates produce
metal oxide + carbon dioxide
e.g XCO3 -> XO + CO2
after undergoing thermal decomposition, group 2 nitrates produce
powdered metal oxide + nitrogen dioxide (brown gas) + oxygen
2X(NO3)2 -> @XO + 4NO2 + O2
what happens for group 1 during thermal decomposition?
lithium acts in the same way as group 2 nitrates and carbonates
group 1 nitrates produce a metal nitrite and oxygen
group 1 carbonates will not decompose upon heating in a lab as extremely high temperatures are required
why does thermal stability increase down both nitrate and carbonate groups
down the group, the larger metal cations have weaker interaction with the other anion and have less polarising power, distorting the bond in the electron cloud less
what is the flame test procedure?
- dip a clean nichrome wire loop into fresh concentrated HCL to clean
- heat wire on the edge of a blue flame of a bunsen burner until no colour is produced
- dip wire into solid sample
- observe colour of flame
in a flame test, why does the wire have to be made of nichrome of platinum?
these materials are inert, stable, unreactive and produce no colour when heated in the flame
