Module 2.2 electronic structure
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What are the shells of an atom identified by, and what symbol represents this?
Their principal quantum number (n)
What happens as you move along the shells further away from the nucleus? (2)
Shells become larger Greater energy is stored by the electrons in the shell
How many electrons can fill the first shell?
2
How many electrons can fill the second shell?
8
How many electrons can fill the third shell?
18
How many electrons can fill the fourth shell?
32
What is an atomic orbital?
a region around the nucleus that can hold up to two electrons with opposite spins. It forms part of the subshell which forms part of the shell
what is a quantum number?
a set of numbers used to define the state of an electron
How many electrons can be in an atomic orbital?
2
What is important about the electrons in an atomic orbital?
they have opposite spin
What are the 4 types of orbital?
s orbital p orbital d orbital f orbital
What is the shape of s orbitals?
spherical
which shells contain s orbitals?
All of them
how many s orbitals are there per shell? Therefore how many electrons are held in the s orbital in each shell?
a) 1 b) 2
What shape are p-orbitals?
3 dimensional dumbbell shape
Which shells have p-orbitals?
from n=2 upwards
a) how many p-orbitals are there in each shell? b) how many electrons are there in p-orbitals in each shell?
a) 3 b) 6
What is a subshell?
all the orbitals of one type in a shell
Which shells have d-orbitals?
From n=3 upwards
How many d-orbitals are there in a subshell?
5
How many electrons can be held in d-orbitals in a shell?
10
How many electrons can be held in f-orbitals in a shell?
14
How many f-orbitals are there in a subshell?
7
Which shells have f-orbitals?
n=4 upwards