atomic structure and electron configuration
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atomic number =
number of protons
number of protons=
number of electrons(in neutral atom)
Isotopes
atoms of the same element which contain different number of neutrons
of neutrons =
mass number - atomic number
in isotope notation state where the mass # is and the atomic number
mass number on the top atomic number below mass number
how are ions formed
when atoms gain or lose electrons when reacting chemically
in ionically charge atoms does # of protons equal # of electrons
no
how to find relative atomic mass?
divided percentages by 100 then multiply that number by the mass number that goes along with that percentage. there should be addition between each parenthesis
energy level shell: max # of electrons
1:2 2:8 3:18 4:32 energy level on left, max # of electrons on right
sub level: max # of electrons
S:2 P:6 D:10 F:14
which level gets removed before: level 4 electrons or 3d
level 4, because level is lower in energy due to less electron repulsion
electron configuration example
1s2,2s2,3p6 and so on
Chronium electron configuration(24e)
1s2,2s2,2p6,3s2,3p6,4s1,3d5 instead of having 4s2 ad 3d4 write 4s1 3d5 same goes with copper: write 4s1 3d9
Orbitals
think of them as the boxes can only contain a max of two electrons in each box
sub level: # of orbitals
S:1 P:3 D:5 F:7
drawing of orbitals( explain what the 4 different variations are
S= spherical Px= dumbbell across x axis Py= dumbbell across y axis Pz= diagonal dumbell
electron configuration of ions
if the charge is + then remove if the charge is negative then add