Periodic table Flashcards
Aufbau principle
subshells are filled in order from lowest energy to highest energy and that lower subshell energy levels will be filled before higher energy subshells
Pauli exclusion principle
a max of 2 electrons in orbital with opposite spin
Core charge
num of protons -num of electrons in the inner shell
measure of net attractive force felt by the valence shell electrons towards the nucleus
Atomic radius down a group
Increases
- the number of occupied energy levels increases
- core charge remains constant
Atomic radius across a period
decreases
number of occupied energy levels remains constant
core charge increases=valence shell electrons pulled in more
Electronegativity
the strength with which atoms of an element attract electrons when they are chemically combined with another element
Electronegativity down a group
decreases
- num of occupied energy levels increases
- nuclear charge increases, however electron shielding also increases so core charge stays the same.
Electronegativity across a period
increases
- atomic radius decreases
- core charge increases
First Ionisation energy
the energy required to remove an electron from each of a mole of gaseous atoms
Ionisation energy down a group
decreases
- atomic radius increases
- core charge remains constant
- therefore less energy required to remove an electron
Ionisation across a period
increases
- atomic radius decreases
- core charge increases
- therefore more energy is required to remove an electron
Reactivity of metals across a period
decreases
- core charge increases
- general increases in energy required to remove an electron
reactivity of metals down a group
increases
core charge remains the same
-energy levels+ electron shielding increases
- decrease in energy required to remove an electron
Reactivity of non metals down a group
decrease
reactivity of no metals across a period
increases