Chapter 5, electron structure Flashcards
Quanta?
Quantity of energy that electrons possess and so can only exist in certain quantised energy levels
how are quantised energy levels labelled
with a principle quantum number, n: for example n=1
what happens to energy of the shells and the shell number increases?
It increases
What happens to the distance between energy levels as they increase
It decreases (they get closer together)
maximum number for electrons in first 4 energy levels?
2,8,18,32
How can electrons move between energy levels
by emitting or absorbing energy equal to the difference in energy between two energy levels: delta E
Atomic orbital definition?
Make up shells, a region of space around the nucleus that can hold up to two electrons with opposite spins
Different types of orbitals?
s,p,d,f they all have different shapes
Atomic orbital in regard to probability?
Region where there there is the highest probability of finding electrons with a certain quanta of energy
Shape of s orbitals
spherical
As the shell number (n) increases the radius of the s orbital
increases
what does an electron being further away from the nucleus mean
it has more energy
what shape are p orbitals
3 separate dumbell shaped orbitals at right angles to each other
As the shell number (n) increases the distance of the p orbital from the nucleus..
increases
subshells?
orbitals of the same shape grouped together
With which sub orbitals is there an abnormality
4s has less energy than 3d so should be filled before 3d is
electrons with opposite spins
Electrons have up spin or down spin. Electrons occupying the same orbital must have opposite spins
‘sitting on the bus’ when filling orbitals
when there are multiple of the same orbital, like 3 p orbitals, each orbital of the same energy should be occupied before spin pairing occurs in the first orbital
s/p/d/f block elements
Elements on the periodic table with their highest energy electrons in s/p/d/f subshell respectively
which elements can be included in shorthand notation
Only G8 bc they have full outer shells
Exceptions to electron configuration?
Chromium and copper
Electron configuration of chromium
1s^2 2s^2 2p^6 3s^2 3p^6 3d^5 4s^1/ [Ar]3d^5 4s^1
Electron configuration of copper
1s^2 2s^2 2p^6 3s^2 3p^6 3d^10 4s^1
from where do ions of block d elements lose electrons first
From 4s before 3d despite the order of filling
Ionic bonding definition
The electrostatic attraction between positive ions and negative ions
Ground level?
Minimum/ typical energy level of electrons
