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CHEMISTRY HCS112
Elements : they can not split to anything simpler and they can be in any stage
...
Compounds can be
separated by a physical process
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4x10-4

Mass to moles:
Mass(g)/molar mass(g/mol-1) = no of moles(mol)

Moles to mass
Mass(g) = no of moles (mol) x molar mass

CONCENTRATION
Molarity (M) = C x Volume

C1xV1 = C2xV2

Quantum Numbers:
1
...

3
...


Energy shell
Shape of electron cloud
Orientation of orbitals
Electron environment

Quantum Number:
1) Principal number (n)
• For energy level
• 1= lowest energy
• Increasing n = electrons are further away from the nucleus
2) Azimuthal number (l)
• For angular momentum
• Related with the shape of the orbital
• l=0 s-spherical
• l=1 p-dump bell
• l=2 d-four lobe
• l=3 f-six lobe
3) Magnetic (m1)
• Orientation in space
4) Spin (ms)
• Defines the electron spin

Energy shell, Possible values of l, Subshell name, Possible values, Electron number
1, 0, 1s, 0, 2
2, 0, 2s, 0, 2
2, -1, 2p, -1/0/+1, 6

1) Pauli exclusion number: “ no 2 electrons in a single atom can have the same set of 4
quantum numbers”
•
•

No more than two electrons in any atomic orbital
If there are 2 electrons in an orbital they must have opposing spin

2) Aufbau principle: electrons occupy orbitals of the lowest energy first
( 1s<2s<2p<3s<3p<3d<…)

3) Hund’s rule of maximum multiplicity: each orbital of equal energy is filled singly with
electrons of the same spin before the pairing occurs

Prefix of alkanes (single bond -a-)
For alkenes: meth- prefix is not
available
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Triple bond -y-

Endings :
a)
b)
c)
d)
e)

Alcohols -ol
Aldehyde -al
Ketone -one
Carboxylic acid -oic
Ester -oate

Isomerism: Isomerism is defined as the existence of two or more compounds (isomers) having the
same molecular formula but different arrangement of atoms within the molecule
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