Master this deck with 43 terms through effective study methods.
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Bright red
Bright yellow
Lilac
Alkaline earth metals
Have a smaller ionic radius and have2 delocalised electrons per ion and the 2+ ions are more strongly attracted to the electrons
Increase as there are more sub shells
It decreases because the outer s electrons get further from the nucleus as there are more sub shells and there is more shielding so the attraction between the nucleus and the electrons is weaker
Group 2 ions have a higher positive charge of +2 instead of +1 and they are acting on 1 less electron. Therefore the effective nuclear charge is stronger between the nucleus and outer electrons so the attraction is stronger
Reducing agents
They burn in oxygen to form a white ionic oxide with M2+ ion sand 02-
Strontium and Barium can burn in excess air and excess temperature to form the peroxides Ba02 and St02
Increases because the outer electrons are lost more easily because the atomic radius increases and there is more shielding which outweighs the stronger nuclear charge
As group 1 metals only have to remove on electron and their fist ionisation energy is less then the sum of the first and second ionisation energy on the group 2 metals. The atomic radius on the group 2 atoms is also smaller so it takes more energy
Increases because the atoms lose electrons easier because the atomic radius is larger and there shielding is increased
solubility increases
Forms magnesium hydroxide which is not very soluble and hydrogen
Burns with a white flame and forms magnesium oxide (white powder) and hydrogen
Initially the calcium hydroxide dissolved but then becomes saturated and a white precipitate appears
Barium reacts even faster and it's hydroxide is even more soluble
All the metals form white chlorides which are all soluble
They are white solids and are bases
It's slightly soluble in water forming an alkaline solution called limewater. This reacts with carbon dioxide to form calcium carbonate which is insoluble and white
the oxide and carbon dioxide
They get more thermally stable down the group. The metal ions get less polarising so the bond between the carbonate/nitrate and the cation is stronger
it is small, so is charge dense enough
Form nitrogen dioxide an oxide and oxygen E.G. 2Mg(N03)2 -> 4N02 +2MgO + 02
Form a metal nitrite + oxygen E.g. 2Mg(N03)2 -> 2MgN02 + 02
no colour
no colour
brick red
red
pale green
green
they get less soluble
they get less soluble
brown gas
its covalent
As the hydroxides are alkaline, this is a neutralisation reaction and forms a salt + water
because it forms a layer of beryllium oxide on the surface which stops any further oxygen from reacting
react to form metal hydroxides and hydrogen. The metal hydroxide solution is alkaline which is why they are called alklali metals
Take a nichrome wire and dip it in concentrated hydrochloric acid and then put it into a blue bunson burner flame. Repeat this cleaning until there is no coloured flames. Dip the wire into the metal and place into bunson burner
Electron exist in orbitals and when energy is supplied and absorbed by the metal, the electrons become excited and are promoted to a higher energy level. The electrons will drop back down to their original orbital they were in and this process releases energy, some in the form of light.
The colour depends on the wavelength of light. When some electrons drop down to their original orbitals, the energy emitted might not have a wavelength in the visible part of the electro-magnetic spectrum.