Atomic and Electron Structure, Periodic Table and Ionisation Energy (2.1, 2.2, 5.1, 7.1, 7.2) Flashcards
What are isotopes?
Atoms of the same element with different numbers of neutrons and different masses but the same number of protons
Describe the atomic structure
Consists of a nucleus made up of two subatomic particles: protons and neutrons
Third subatomic particle: electron arranged around the nucleus in shells
What is the relative isotopic mass?
The mass of an isotope relative to 1/12th of the mass of an atom of carbon-12
What is the relative atomic mass?
The weighted mean mass of an atom relative to 1/12th of the mass of an atom of carbon-12
What is the relative molecular mass?
The average mass of a molecule or formula unit, compared to 1/12th of the mass of an atom of carbon-12
What are the numbers of shells (energy levels) called?
Principal quantum numbers
How does energy change in the shells?
Shells further from the nucleus have a higher energy than shells closer to the nucleus
What are the names of the different sub-shells?
s, p, d, f
What does each sub-shell have?
A different number of orbitals
How many electrons can one orbital hold?
2
How many orbitals does an s sub-shell have?
1
How many electrons can an s sub-shell hold?
2
How many orbitals does a p sub-shell have?
3
How many electrons can a p sub-shell hold?
6
How many orbitals does a d sub-shell have?
5
How many electrons can a d sub-shell hold?
10
What is an atomic orbital?
A region around the nucleus that can hold up to two electrons, with opposite spins
What are the sub-shells in the 1st shell?
1s
How many electrons can the 1st shell hold?
2
What are the sub-shells in the 2nd shell?
2s, 2p
How many electrons can the 2nd shell hold?
8
What are the sub-shells in the 3rd shell?
3s, 3p, 3d
How many electrons can the 3rd shell hold?
18
What are the sub-shells in the 4th shell?
4s, 4p, 4d, 4f