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Atomic Structure - Coggle Diagram
Atomic Structure
Isotopes
what are they?
atoms of the same element
with the same no of protons and electrons
with different no, of neutrons
examples
chlorine exists as 2 isotopes (chlorine-35 and chlorine-37)
properties
similar chemical properties
similar electronic configuration
different physical properties
different relative masses
Removing Electrons
rules
electrons are removed from orbitals with the highest n first
electronic configuration of the neutral atom must be determined first
electronic configuration of ions
cations --> loses elctrons
anions --> gain electrons
Isonisation Energy
what is it?
energy require to remove an electron
in its gaseos atom/tion
at ground sate
measures the ease of an atom/ion losing an electron
units: kJ/mol
chemical equation
2nd: X+ (g) --> X2+ (g) + e-
3rd: X2+ (g) --> X3+ (g) + e-
1st: X (g) --> X+ (g) + e-
Successive Ionisation energies
Successive IE increases
after the removal of 1st electron, a +ve ion is formed
greater amt of energy is needed to remove
electrons from cation vs neutral atom
Sharp Increase in IE
more energy is require to remove electron
as it is from the inner electron shell
electron more strongly attracted to nucleus
Atomic Orbitals and Quantum No.
Principal quantun number, n
takes on integral values (eg. 1, 2, 3)
as n increases, the orbital becomes larger
--> electron is further from nucleus
each principal quantum no. corresponds to an electron shell
n=1 is the closes to the nucleus and has the lowest energy
Second quantum number, l
integral values from 0 to n-1
defines the shape of theorbital
each sub-shell consists of a specific no. of orbitals
(each orbital can hold a max. of 2 electrons)
p - 3
d - 5
s - 1
f - 7
Electron Configurations
rules to achieve ground state
(energy is low as possible)
electrons occuoy the orbitals
of the lowest energy first
orbitals of a given subshell have the same amount of energy
(eg all the 2ps have the same energy level)
4s has a lower energy than 3d
Within a sublevel, electrons is places in
each orbital before paring them up
