2. Electronic Structure
Shells
They are regarded as energy levels
Energy increases as shell number increases
Shell number is the principal quantum number (n)
Electrons in shells
Electrons have properties of waves and particles
Maximum number of electrons in shell = 2n 2
4. Electronic Structure
Orbitals
A region around a nucleus that can hold up to two electrons with opposite spins
or a high probability of finding an electron
Each orbital (s , p , f , d) is a different shape
S orbital
Spherical
Each shell contains one
The greater the shell number (n) the greater its radius
5. Electronic Structure
P orbital
Dumbbell shape
Each shel from n=2 contain a three (at right angles from eachother)
Greater the shell number (n) the further it is from the nucleus
D and F orbitals
Double dumbbell shape
Each shell from n=3 has five d orbitals
Each shell from n=4 has seven f orbitals
6. Electronic structure
Sub shells
Each new shell gains a new type of orbital
Number of orbitals increases with each orbital
Number of electrons in each sub shell also increases
Orbitals fill in order of increasing size
Each new type of sub shell has a higher energy
However 4S fills before 3D
7. Electronic Structure
Electrons pair with opposite spins
Electrons have a negative charge so repel one another, and hence have a
property called spin (shown by either an upwards or downwards arrow) to
counteract the repulsion
Orbitals with same energy are occupied singularly first
One electron occupies each orbital before pairing starts, this prevents repulsion
until there is no other choice
8. Electronic Structure
Eectronic Configuration
E.g. Lithium 1S 2 , 2S 1
Can be written in shorthand using the previous noble gas’ chemical symbol and
the remaining electron sub shells
Ions
Positive ions are cations they’re formed when atoms lose electrons
Negative ions are anions they’re formed when atoms gain electrons
9. Electronic Structure
Blocks on the periodic table
S block (highest energy electrons in s sub shell) left block of two groups
P block (highest energy electrons in p sub shell) right block of six groups
D block (highest energy electrons in d sub shell) centre block of ten groups
Ions of S and P block elements
Highest energy sub shells lose of gain electrons
Ions of D block elements
4S sub levels fills and emptied before 3D (as 4S has lower enegy)
10. Ionic Bonding and Structure
Ionic bonding
It is the electrostatic attraction between positively and negatively charged ions.
Popular cations: metals and ammonium
Popular anions: non-metals and polyatomic ions
Ionic compounds
Outer shell electrons from a non metal atom are transferred to the outer shell of a non
metal atom
Cations and anions are formed
Ions have same configuration as noble gases (full outer shell)
11. Ionic Bonding and Structure
Structure of ionic compounds
Each ion attracts oppositely charged ions in all directions
This results in a giant ionic lattice structure containing lots of ions
Properties of ionic compounds
Melting and boiling points: Almost all ionic compounds are solid at room
temperature. There are very strong electrostatic forces of attraction between ions
so bonds need a lot of energy to be overcome (giving the compounds high
melting and boiling points). The greater the ionic charge the larger the strength
of the bonds and hence higher the melting point
12. Ionic Bonding and Structure
Solubility: Many ionic compounds dissolve in polar solvents (e.g water) as the
positive and negative charges of the molecule attract the ions. The greater the
ionic charge thr stronger the bonds between the ions so compounds become less
soluble
Electrical conductivity: ionic compounds conduct electricity when molten or
dissolved as the ionic lattic breaks down allowing ions to be mobile and carry a
charge
13. Ionic Bonding and Structure
Teeth
The enamel on your teeth is made of the ionic compound calcium
hydroxyapatite which can be removed in acidic conditions (resulting in tooth
decay). Saliva helps neutralise the acid but it’s not always enough, so toothpaste
contains fluoride in the form of calcium fluoride which replaces lost ions by
forming fluoropatite which is stronger and more resistant than hydroxypatite
14. Covalent Bonding
Covalent compounds and molecules
Covalent bonding is the strong electrostatic attraction between a shared pair of
electrons and the nuclei of the bonded atoms.
It occurs between atoms in: non metals, compounds of nom metals and
polyatomic ions
The atoms are bonded together into a single unit: a small molecule (H2), a giant
covalent structure (SiO2) or a charged polyatomic ion (NH4
+)
15. Covalent Bonding
Orbital Overlap
A covalent bond is the overlap of atomic O rbitals, each containing one electron,
to give a shared pair of electrons
The shared pair of electrons are attracted to the nuclei of both bonding atoms
Bonded atoms often have the same electronic structure as a noble gas (full outer
shell)
16. Covalent Bonding
Localised
The attraction is localised (directional) and hence acts solely between the
involved atoms. This can result in a small unit (a molecule).
A molecule is the smallest part of a covalent compound that can exist whilst
retaining the chemical properties of a compound
Lone pairs
Paired electrons that are not shared
17. Covalent Bonding
Multiple covalent bonds
Two atoms share more than one pair of electrons (e.g double and triple)
Examples include carbon dioxide (double bond) and nitrogen (triple bond)
Dative covalent bond
A active (co-ordinate) bond is one in which the shared pair of electrons come from one atom (originally
the lone pair).
Usually bonds to a H+ ion
Shown in display formula as arrow from the donating atom
Average bond enthalpy
A measurement of covalent bond strength (larger = stronger )
