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Electron orbitals

Uni of Notts, fundamentals of inorganic & organic chemistry, first year

TermDefinition
Atomic orbital Wavefunction (mathematical expression) describing the region with the highest probability of an electron being found, this probability is highest closer to the nucleus
Basic properties of electron orbitals Each can fit up to 2 electrons with different spin. The higher the nuclear charge & the lower the shielding, the lower the energy of the electrons. The size, shape, & directional properties of the atom are determined by the orbitals
Electron nodes Region of an atom where there is a probability of 0 that an electron will be found
How s orbitals are drawn For 1s the e- density plot is represented as a circle around the nucleus with no nodes. With each increase in energy level, another circular node is added
How p orbitals are drawn 2 orbitals expanding out from the nucleus with a nodal plane between them. Pear shaped rather than spherical with 1 shaded in and the other left blank in the middle. Since they can stretch across any spatial axis the 3 orbitals are labelled Px, Py, & Pz
Nodal plane 2D section on either side of the nucleus where no electrons can be found
Degenerate orbitals 2 or more orbitals that have the same energy level
Hund’s rule Degenerate orbitals must fill evenly with 1 electron before higher energy electrons are filled, this follows the Aufbau principle
Aufbau principle Lower energy levels must be filled before higher energy levels
Molecular orbitals (MOs) When 2 orbitals from 2 different atoms combine, usually forming some kind of chemical bond. If their wavefunctions overlap they combine in phase, if they don’t overlap then they combine out of phase
In phase combination Additive combination causing constructive interaction & the sharing of electrons (e.g., in a covalent bond) to form a MO with a σ bond
Out of phase combination Subtractive combination causing destructive interaction & destabilisation of the molecules also known as an antibonding MO* which forms a nodal plane between orbitals forming a σ* bond
σ (sigma) bond & how it’s represented in p orbitals The orbital is in a symmetrical rotation around the internuclear axis This can be represented in phase as the orbitals with the same shading facing each other with the opposite being true for out of phase MO*
Bonding MO Antibonding MO* AOs (Atomic orbitals) combining in a way that the e- density is distributed between the nuclei of the 2 bonding atoms AOs combining in a way that the the e- density is distributed away from the nuclei of the 2 bonding atoms causing the nuclei to repel
Bond order The difference between the number of electrons in bonding orbitals & those in antibonding orbitals divided by 2. The lower the bond order the weaker the bond order & increasing the chance of bond dissociation & vice versa
End-on overlap Orbitals approach each other from the side forming a σ-bond, they’re symmetrical around the internuclear axis which causes better overlapping along the internuclear axis & allows the electrons to have lower energy
Edge-on overlap Orbitals approach parallel to each other causing them to form a π-bond asymmetrically around the internuclear axis which makes poorer overlapping above & below the internuclear axis & the electrons must be of a higher energy
Internuclear axis Imaginary straight line linking the nuclei of 2 bonding atoms together to serve as representation of the orientation & interaction of AOs in molecular bonding
Explain how AOs form MOs: AOs need to be similar energy If AO energy levels are too different, it will cause transfer of electrons & form an ionic compound rather than a chemical bond
Explain how AOs form MOs: AOs need to be similar size So that they can overlap properly & have a better interaction
Explain how AOs form MOs: AOs need to be fairly symmetrical They cannot combine without appropriate symmetry for their type of overlap (e.g., edge-on overlap can’t involve s orbitals since they’re always symmetrical due to being perfect circles & π-bonds must be asymmetrical)
Created by: Beech47
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