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Mind Map by awesome.lois, updated more than 1 year ago
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Created by awesome.lois
almost 10 years ago
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AS Chemistry Unit 1 Periodic Trends
- Nuclear Charge
- Increases across a period as there are more
electrons being added to the outer shells.
- The nuclear charge of a group is the same
because in a group they all have the same
number of electrons on their outer shells.
- Increases across a period as there are more
electrons being added to the outer shells.
- Atomic Radius
- Increases down a group because more
shells are being added to the atom
making the radius bigger.
- Decreases across a
period because the
electron attraction is
increasing, pulling the
electrons closer
together.
- Increases down a group because more
shells are being added to the atom
making the radius bigger.
- Electron Shielding
- Stays the same across a period as the
electrons are being put in the same
shell.
- Increases down a group
as more shells are added.
- Stays the same across a period as the
electrons are being put in the same
shell.
- Nuclear Attraction
- Increases across a period because the
atomic radius gets smaller and the
nuclear charge increases.
- Decreases down a group due to
the increased atomic radius, so
there is more shielding.
- Increases across a period because the
atomic radius gets smaller and the
nuclear charge increases.
- Ionisation Energy
- Decreases down a group
because the atomic radius
increases therefore the electron
shielding increases so the nuclear
attraction decreases.
- Increases across a period because
the atomic radius decreases
therefore the nuclear attraction is
increasing, this makes it harder to
remove an electron.
- Decreases down a group
because the atomic radius
increases therefore the electron
shielding increases so the nuclear
attraction decreases.
- Melting and Boiling Points
- Giant Metallic Lattice
- High Boiling and Melting Point that increases
with charge (1+ to 3+)
- High Boiling and Melting Point that increases
with charge (1+ to 3+)
- Giant Covalent Lattice
- High Boiling and Melting Point
- High Boiling and Melting Point
- Simple Molecular Structures
- Low Boiling and Melting Point that increases
with the amount of molecules it attracts (e.g
Oxygen being diatomic (O2)).
- Low Boiling and Melting Point that increases
with the amount of molecules it attracts (e.g
Oxygen being diatomic (O2)).
- Period 3 Example
- Giant Metallic Lattice
- Periodic Table
- Arranged in order of the
number of protons
(atomic number)
- 7 Periods
- 8 Groups
- Arranged in order of the
number of protons
(atomic number)
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