Electron Structure
- Created by: Florence A
- Created on: 28-04-19 13:59
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- Electron Structure
- Atomic Orbitals
- S-orbital
- Spherical shape
- From energy shell 1 upwards, each level contains one s orbital within an s sub-shell
- P-orbital
- Have a 3D dumb bell shape
- From energy shell 2 upwards, each level contains 3 p orbitals within a p sub-shell
- Each orbital holds 2 electrons
- Total of 6 p electrons in a full p sub-shell
- D-orbitals
- 5 d-orbitals within a d sub-shell
- Total of 10 electrons in a full d sub-shell
- More complex shape than p-orbitals
- An orbital is a space around the nucleus that can hold up to 2 electrons in opposite spin
- S-orbital
- 3rd and 4th Main Electron Shells Overlap
- The 4th shell starts to fill before the 3rd level is full
- Electrons go into 4s before 3d
- 4s also empties before 3d
- The 4th shell starts to fill before the 3rd level is full
- Periodic Trend in Electron Configuration
- Across a Period
- Each period starts with an electron in the new highest energy shell
- The s and p sub-shell are filled in the same way
- Down a Group
- Elements within the same group have the same number of electrons in the outer shell and in each sub-shell
- Across a Period
- Electron Configuration of Ions
- Positive Ions
- Electrons are removed from the highest energy level first
- Negative Ions
- Electrons will go into the lowest unoccupied energy level
- Positive Ions
- Trends in Atomic Radii
- Factors Affecting atomic radii (size of atom)
- Strength of attraction between nucleus and electrons
- Shielding: strength of repulsion between outer shell electrons and the other electrons in the inner shells
- With Increasing Atomic Number
- Atomic radius decreases across a Period
- Same shielding but increasing attraction
- Atomic radius increases down a group
- More full inner shells increases shielding so there is decreasing attraction
- Atomic radius decreases across a Period
- Factors Affecting atomic radii (size of atom)
- Ionisation Energy
- First IE is the energy required to remove one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions
- Trends in First IE
- Group Trend
- Decreases going down any group as the electron is removed from a shell further from the nucleus so is more shielded from the pull of the nucleus
- Period Trend
- Increases across any period as there is the same shielding but has an increasing number of protons creating a stronger nuclear attraction
- Group Trend
- Successive Ionisation Energies
- Each successive IE is larger than the one before because:
- As an electron is removed, the shell will be drawn closer to the nucleus
- As distance decreases, nuclear attraction increases
- Each successive IE is larger than the one before because:
- Atomic Orbitals
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