Atomic orbitals Flashcards
What particles can be found in the nucleus?
In the middle protons with neutrons and outsude electrons.
Give the charge and mass for proton, electron and neutron?
Proton (positive) 1
Neutron (neutral or no charge) 1
Electron (negative) very small or 0
How many electrons can 5 shells hold?
1=2
2=8
3=18
4=32
5=50
Why orbitals are formed?
Electrons within each shell will not have the same amount og energy so it’s broken down into subshells called orbitals.
How orbitals are called?
S, P, D and F
How many electrons can orbital hold?
2 electrons maximum
How many electrons can each orbital hold?
S orbital= 2 electrons
P orbital= 6 electrons
D orbital= 10 electrons
F orbital= 14 electrons
State the definition for principal of quantum number?
The number given to an ebergy level that denotes its ebergy value.
Explain the Aufbau principle for electronic configuration?
Electrons fill the orbital with the lowest aviable energy before filling the orbitals with higher energy states. This will give stable electronic configuration.
State the definition for spins?
Electrons have 2 possible states “spin up or down”. In orbital, each electron will be in a different spin state.
Why I need to draw half arrows when filling the orbitals?
Half arrows represents each electron in orbital. Arrows drawn like this because each elecron have different spin.
Explain Hunds rule?
Maximum multiplicity.
If 2 or more orbitals of equal energy are aviable, electrons will occupy them singly before filling them in pairs.
Explain Bohr model of an atom?
Bohr stated that:
1. Small positively charged nucleus at the centre.
2. Number of electrons in the ouer orbital determines the property of an element.
3. Electrons closer to the nucleus have less ebergy, while those further away have more energy.
