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Chem Topic 1 - Coggle Diagram
Chem Topic 1
Rules of orbital occupancy
1.Electrons will always fill orbital with lowest energy level
2.Each orbital can only be filled with electrons
of opposite spins
3.Orbitals must be
filled singly
before creating a pair
4s comes before 3d as
it has a lower energy level
, so electrons will occupy 4s subshell first
Identify unpaired electrons
Atomic structure
Subatomic particles
p
Charge: +1
Mass in amu: 1.0073
n
Charge: 0
Mass in amu:1.0087
e
Charge: -1
Mass in amu: 1/1837
Number of electrons in atom= Number of protons in atom
Atomic number=number of protons in atom= identity of element
Ions
Number of protons do not equal number of electrons
Isotopes: atoms with the same number of protons but different number of neutrons
Different mass numbers
Temperature scale conversion
From F to C:
C=[F-32]/1.8
From C to K:
C+273.15
Dimensional analysis
Conversion factor: ratio that links final unit to starting unit
SI units
SI prefixes-must remember!
Must check sf of final answer consistent to sf of question
Electronic structure of an atom
Electron shells
Outermost shell> valence shell
outermost electrons> valence electrons
subshell: s, p, d, f etc.
orbital: 3-dimensional spaces where mostly likely to find electrons
Max number of electrons per shell: 2n2
Type of subshells found in each shell
n=2>s, p
n=3>s, p, d(5 d orbitals)
n=1>s
n=4> s, p, d, f
Also known as principal quantum number, n
