What are the relative masses of the subatomic particles? (3)
- Proton = 1 (1)
- Neutron = 1 (1)
- Electron = 1/2000 (1)
What is the top and bottom number of an element? (4)
- Top = mass number (1)
- Number of protons and neutrons in the nucleus (1)
- Bottom = Atomic number (1)
- Number of protons in the nucleus (1)
What is an isotope? (2)
- Different mass number but same atomic number (1)
- Different number of neutrons (1)
What is relative isotopic mass? (2)
- The mass of an atom of an isotope (1)
- Compared to 1/12 mass of an atom of carbon-12 (1)
How do you work out relative isotopic mass? (1)
RIM = (abundanceM/Z) + (abundance M/Z)
/100
What are the S and P orbital shapes? (3)
- S = Spherical (1)
- P = 3 Dumbbells make up P sub-shell (1)
- 2 electrons can move within these orbital shapes (1)
What is spin-pairing? (2)
- When 2 electrons occupy one orbital (1)
- Spin in opposite directions (1)
Whats the maximum electron configuration or every shell? (4)
- 1s2
- 2s2 2p6
- 3s2 3p6 3d10
- 4s2 4p6 4d10 4f14
What are the 2 rules when filling orbitals? (3)
- We fill from the lowest energy upwards (1)
- Hence why 4s is typically filled before 3d (1)
- Orbitals are filled singly before paired due to electron repulsion (1)
What elements behave differently in electron configuration and why? (2)
- Chromium and copper (1)
- 4s1 to have a more stable 3d sub-shell (1)
Where are the electron blocks located? (4)
- S-block is on the left side (1)
- D-block is located at the middle (1)
- P-block is located on the right side (1)
- F-block is located at the bottom (1)
How does the atomic emission spectra? (3)
- Element is heated and electrons absorbs energy becoming excited
(1) - Electron moves from ground state to a higher energy level (1)
- Eventually electrons move down and release energy in the form in
light (1)
What is ionisation energy? (2)
- The minimum energy required to remove 1 mole of electrons (1)
- From one mole of atoms in gaseous states (1)
Whats the trend of ionisation as you move down a group? (2)
- Energy decreases (1)
- Increase in shielding and atomic radius (1)
What is successive ionisation and what do the jumps in energy indicate? (3)
- More than one electron removed from the same atom (1)
- Small increase as it becomes a more positive ion (1)
- Large increase from a removal of a closer shell (1)
What is the 2nd ionisation energy of Magnesium? (1)
Mg+(g) → Mg2+(g) + e- (1)
What do the changes of ionisation in periods indicate? (3)
- General increase come from increase of protons and same
shielding (1) - Significant decrease (Elements located at Al) in row indicates outer
electron sitting in a sub-shell further from nucleus (1) - Slight decrease (Elements located at S) as 2 electrons in same orbital
cause repulsion (1)
What are the trends of melting points in period 3? (4)
- (Na, Mg, Al) have metallic bonding with increasing positive charge (1)
- Silicon has giant covalent structure and highest melting point (1)
- (P4, C8, Cl2) are simple molecular with different London forces (1)
- Ar exist as an individual atom with the lowest melting point (1)
Why do some elements have similar chemical reactions? (2)
- Same number of electrons in the outer shell (1)
- Electrons govern chemical reactions (1)
What is the reason for logarithm being used? (1)
- Makes it easier to plot large numbers (1)
What is periodicity? (1)
- A trend of repeating properties (1)
