The Periodic Table Flashcards
What happens to atomic radius down Group 2 & why ?
- Increases
- Greater atomic number = more electrons = more shielding
What is the difference in atomic radius between Group 1 & 2 ?
- Group 2 atoms are smaller
- Extra proton holds electrons closer to the nucleus
What happens to ionic radius down Group 2 & why ?
- Increases
- Ions are smaller than atoms
- Remaining electrons are now in fewer shells
What happens to melting point down Group 2 & why ?
- Decrease
- Each atom contributes 2 electrons to delocalised cloud
- Metallic bonding gets weaker due to increased size of ion
What happens to first ionisation energy down Group 2 & why ?
- Decreases
- Extra shielding/ increasing atomic radius
- less energy required to lose electrons
Which metal oxide has covalent character ?
BeO
What happens to solubility down Group 2 ?
- Increases
What happens when a metal oxide reacts with water ?
- Hydroxide is formed
E.g:
CaO + H20 = Ca(OH)2
What colour is floruine, chlorine, bromine and iodine ?
F - yellow
Cl - green
Br - red/brown
I - grey
What happens to the boiling point down the halogens ?
- Increases
- Larger size = Increased dipole-dipole interactions
- More energy is require to sepearate the molecules
What happens to atomic radius down the halogens ?
- Increases
- Greater atomic number = more electrons in shells = increasingly futher from the nucleus
What happens to ionic radius down the halogens ?
- Increases
- Ions larger than atoms = added electron repels the others = radius is larger
What happens to electronegativity down the halogens ?
- Decreases
- Allthough has increasinng nuclear charge due to greater number of protons.
- There is increase in shells = more shielding = less pull
- Increasing atomic radius = attraction drops as distance increases
What happens to oxidising power down the group ?
- Decreases
- Oxidising power (ability to gain electron - reduce)