Chemistry (atomic structure) Flashcards
What are the 3 subatomic particles?
Proton, electron, neutron
Relative charge=
Proton= +1 (positive) Electron= -1 (negative) Neutron= 0 (no charge)
Relative mass=
Proton= 1 Electron= 1/1835 (negligible) Neutron= 1
The nucleus-
- It’s I. The middle of the atom
- It contains protons and neutrons
- It has a positive charge.
- almost the whole mass of the atom is concentrated in the nucleus.
- Compared to the overall size of the atom, the nucleus is tiny.
The electrons-
- Electrons move around the nucleus in the electron shells.
- They’re negatively charged.
- They’re tiny, but their shells cover a lot of space.
- The size of their shells determines the size of the atom. Atoms have a radius (known as the atomic radius) of about 10(to the power of -10)
5 Electrons have a tiny mass.
23
Na
11
Top number= mass number
Bottom number= atomic number
Mass number= protons and neutrons
Atomic number= protons only
Isotopes-
Are different forms of the same element, which have the same number of protons but a different number of neutrons.
They have the same atomic number but different mass numbers.
Relative atomic mass-
The relative atomic mass of an element is the average mass of one atom of the element, compared to 1/12 of the mass of one atom of carbon-12
Isotopic abundance-
Overall proportions
How to work out the relative atomic mass of an element…
Multiply each relative isotopic mass by its isotopic abundance, and add up the results.
Divide by the sum of the abundances.
Electron shell rules:
1st shell= 2 electrons
2nd shell= 8 electrons
3rd shell= 8 electrons.