Topic 4: Inorganic Chemistry And The Periodic Table Flashcards
What is a common name given to group 2 metals?
Alkaline earth metals
What is the most reactive metal of Group 2?
Barium
List 3 physical properties of group 2 metals?
- High melting and boiling points
- Low density metals
- Form white compounds
The highest energy electrons of Group 2 metals are in which subshell?
S subshell
What is the trend in reactivity down group 2? Why is it this way?
- It increases down the roup
- Electrons are lost more easily due to larger atomic radius and increased shielding
What is the trend in ionisation energy down group 2? Why is it this way?
- it decreases
- increased number of shells, so more shielding
- increased atomic radius, so weaker forces of attraction to nucleus
- so less energy is needed to remove electron
What type of reaction is the reaction between group 2 elements and oxygen?
- redox reaction
What are the products when group 2 elements react with water?
- hydroxide (OH-)
- hydrogen gas (H2)
Which group 2 element does not react with water?
Beryllium
Which group 2 element reacts very slowly with water?
Magnesium
What type of reaction is the reaction between group 2 metals and water?
Redox reaction
What are the products when a group 2 oxide reacts with a dilute acid?
- salt
- water
What is formed when group 2 oxides react with water?
- metal hydroxide
Which group 2 metal oxide is insoluble in water?
Beryllium oxide
What is the trend in hydroxide solubility down group 2?
- increases down the group
- Mg(OH)2 is slightly soluble
- Ba(OH)2 creates a strong alkaline solution
What is the trend is sulfate solubility down group 2?
- they become less soluble down the group
What is the reasoning behind the trend in thermal stability for Group 1 carbonates and nitrates?
- they do not decompose except for lithium
- they dont have big enough charge densities to polarise the carbonate ion as they only form 1+ ions
- lithium ion is just small enough to have the polarising effect so it can decompose
What is the reasoning behind the trend in thermal stability for Group 2 carbonates and nitrates?
- more thermally stable as you go down the group
- cations get bigger so have less of a polarising effect (distort the carbonate/nitrate ion less)
- C-O/N-O bond not weakened as much and therefore it is harder to break down
List the flame colours for the group 1 elements?
- Lithium = red
- Sodium = orange/yellow
- Potassium = lilac
- Rubidium = red
- Caesium = blue
List the flame colours for Group 2 elements?
- Magnesium = no colour
- Calcium = brick red
- Strontium = crimson red
- Barium = pale green