Group 2 Flashcards
What do the electron structures end in?
S2
How many valence electrons do they have?
2
What are the reactions?
Lose 2 electrons from the s orbital to from a dispositive (2+) ion
Normally oxidised so therefore they are good reducing agents
What is atomisation energy?
Energy needed to break the bonds holding the atoms together in the metallic lattice
What are 1st and 2nd ionisation energies needed for?
Needed to convert metal atoms into ions with a 2+ charge
Atomic radius down the group…
Increases
Number of electron shells…
Increases so therefore electrons are further from the nucleus
What happens to 1st ionisation energy and why?
Decreases because the atomic radius increases and there are more electron shells, therefore the electrons are further from the nucleus
Melting point down the group…
Decreases
Ionic radius…
Increases
Ions all have a 2+ charge- their is a decreases charge density and weaker attraction between ions and delocalised electrons
What compounds do group 2 form?
Colourless/white compounds
Are group 2 good or bad conductors of electricity?
Goood
High or low melting point?
High
What do group 2 carbonates decompose to form?
An oxide and carbon dioxide
What are the oxidation states of group 2 elements?
0
What are the oxidation states of group 2 compounds?
+2
How does magnesium burn and what does it form?
Burns with a bright white flame to produce magnesium oxide
How do group 2 metals react with HCL?
Form hydrogen gas and a colourless solution
Do group 2 hydroxides become more or less soluble down the group?
More soluble
Do group 2 sulphates become more or less soluble down the group?
Less soluble
What happens to reactivity down the group?
Increases
Do reactions get more or less vigorous down the group?
More
How are hydroxides formed?
By group 2 dissolving in water
How does Mg react with water?
Slowly with cold water
A few bubbles when reacted with steam
