Electron Configuration Flashcards
Excited state
When an electron absorbs energy/ increase to a higher subshell or energy level
Grounded state/relaps
Lowest possible subshell, and energy level an electron can occupy. Observed when a photon on electromagnetic radiation is released in wavelength of light
Nucleus of atom
Small dense protons and neutrons
Electrin cloud
Region of space where there is probability of electron being found.
Electron shell
An energy level within an atom that may be occupied by a number of fixed electrons
Subshells
Subdivision of electron shells containing fixed number of orbital at the same energy level
Orbital
A region of space containing up to 2 electrons
Subshell names, and Max electrons
S= 2 in every shell- sphere P= 6 oriented in 3 dif positions D= 10 F= 14
Subshell notation
1,S,2 2,S,2 2,P,6 3,S,2
1 shell, s sub shell, 2 electrons
Abrivated notation
Use lightest noble gas, then use normal notation
(Ar) 4,S,2
Pauli exclusion principle
Maximum 2 electrons in orbital
If 2 full, opposite spin
Aufbau principle
Subshells fill from lowest energy to highest
This means overlap, 4S Filled before 3D
Hunds rule
Every orbital must be filled half in each subshell before fully filled
Exceptions to hunds rule
Copper 4,S,1 3,D,10
Chromium 4,S,1 3,D,5
Ions forming
Outermost shell electrons are lost because occupy highest energy
4,s electron lost before 3,d
Trends in electronegativty
High when atomic radius is low/ increase room in valence shell for shared electrons
Core charge is high because nuclear charge high electron shielding low
Move down column-
Core charge no change increase electron shielding
Electronegativty
Strength which atom of an element attract electron when they combined with another electron
In covalent bonds electrons more likely to be closer to atom with greater electroneg
Core charge
Effective nuclear charge is a measure of net attractive force felt by valence shell electrons towards nuclei
Down column constant core energy
Across group core energy increase
Atomic radius across a period
Decrease
N/o of occupied energy levels remain contst
Core energy increase resulting in valence electron being more strongly attracted to nucleus
Atomic radius down a group
Increase
N/o of energy levels occupied by electrons increases
Core energy remains constant
Atomic radius
Half the distance between 2 nuclei of a molecule
Assuming a singular covalent bind exists between 2 identical atoms
Ionisation
Energy required to remove an electron from each mole of gaseous atom
Produces gaseous ion charge of 1 plus
Na=Na+ + e-
Trends in ionisation energy
Greater pull between electrons and nucleus are harder to pull electrons away Need greater amounts of ionisation energy
Repulsion of electrons= easier to pull away
Core charge= if higher require more ionisation energy
Atomic radius= if greater needs less ionisation energy because further from nucleus
Ionisation energy across a period
Increase- atomic radius decreases/ core charge increase
Ionisation energy down a group
Decreased- atomic radius increase/ core energy stays the same
Successive ionisation
Cation becomes more positive, but becomes more difficult to pull electrons away- requires more energy
2nd ionisation energy always greater then 1st
Relative atomic mass
Average mass of all the isotope of an element weighted for their relative abundance
