Chemistry A level electronic configurations and bonding and shapes of molecules

Definition of an orbital

A region around the nucleus that can hold up to 2 electrons with opposite spins

What is the difference between shells, subshells and orbitals

Orbitals are a pair of electrons

Subshells are sections of a shall

Shells are the energy level

Covalent bond definition

A strong electrostatic force of attraction between a shared pair of electrons and the nuclei of bonded atoms

How do ionic bonds dissolve in water

Water has a positive and negative end, so ions attract and separate from the lattice structure and water surrounds the ions

Lone pair of electrons

Electrons not involved in bonding

Difference between a sigma bond and a pi bond

A sigma bond’s orbitals overlap end to end, and a pi bond has a side overlap

The 3 sigma bond diagrams

How many covalent bonds can phosphorus form

5

Can boron form covalent bonds

Yes (e.g. BF3)

Names of all the subshells

S P D F

How to calculate number of electrons in a given energy level

2n²

What is the aufbau principle?

Electrons fill the lowest energy subshells singly

Shape of an s orbital

Sphere

Shape of P orbital

Dumbell

Electron density

How likely you are to find an electron in a given position at a time

What is the heisenberg uncertainty principle

You cant know both the position of the electron and its momentum

Exceptions to the order of filling electrons

Copper and chromium, they both only have 1 electron is 4s

Angle of a tetrahedronal structure

109.5

Angle of linear structure

180

Angle of a pyramidal structure

107

Angle of non linear structre

104.5

Angle of a trigonal planar

120

Angle of tetrahedronal structure

109.5

Angles of an octohedronal shape

90

How much will a lone pair decrease the bond angle by

2.5

Symbol for molecule going into of page

dashed wedge

Symbol for molecule in line with page

line

Symbol for bond coming out of page

Solid wedge