2.2.1 Electron structure
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what is the principal quantum number n also known as
• the shell number or energy level number
what increases as the shell number increases
• energy • further the shell is from nucleus
what are shells made up of
• atomic orbitals
what is an atomic orbital
• a region around the nucleus that can hold up to 2 electrons with opposite spins > its a region in space where there is a high probability of finding an electron
what are the different types of orbitals
s- p- d- f-
in an s subshell how many s orbitals are there
• 1 x s orbital
in a p subshell how many p orbitals are there
• 3 x p orbitals
in a d subshell how many d orbitals are there
• 5 x d orbitals
in an f subshell how many f orbitals are there
• 7 x f orbitals
what does the first shell n=1 contain
• 1s orbital • 2 electrons • 1 orbital overall
what does the second shell n=2 contain
• 2s orbital + 3 (2p) orbitals • 8 electrons • 4 orbitals overall
what does the third shell n=3 contain
• 3s orbital + 3 (3p) orbitals + 5 (3d) orbitals • 18 electrons • 9 orbitals overall
what does the fourth shell n=4 contain
• 4s orbital + 3 (4p) orbitals + 5 (4d) orbitals + 7(4f) orbitals • 32 electrons • 16 orbitals
what shape is an s-orbital
• spherical shape
how many electrons can an orbital hold
• up to 2e-
name the 3 rules for filling atomic orbitals
• Rule 1: orbitals fill in order of increasing energy • Rule 2: electrons pair with opposite spins • Rule 3: orbitals with the same energy are occupied slightly first
why do electrons pair with opposite spins
• electrons repel each other • electrons have a property called spin - either up or down • 2 electrons in an orbital must have opposite spins to minimise the repulsion between them
why do orbitals with same energy occupied singly first
• this prevents repulsion between paired electrons until there is no further orbitals available at the same energy level