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CS: Chemistry (Atomic structure (Isotopes (Relative Atomic Mass (Average…
CS: Chemistry
Atomic structure
Atomic Models
John Dalton, 1803 first suggested all matter was made up of atoms and that these atoms cannot be split.
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JJ Thompson, 1897, Plum Pudding Model was the discovery of electrons.
Plum Pudding Model, Dough= ball of positive charge and negative electrons= currents.mixed in with said "dough"
Ernest Rutherford, 1909, discovered alpha particles could bounce back off atoms.
He concluded that the atom's mass was concentrated on the atom's center. The nucleus. This contains positive charged particles called protons.
Modern Model, Neils Bohr/ James Chadwick
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In 1932 James Chadwick discovered some particles in the nucleus don't have a charge at all he called these neutrons.
Isotopes
Atoms, same element= same no.0 of protons
But different no. of neutrons, known as isotopes.
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Protium, 1 proton and no neutrons, 99% are protiums
Deuterium, 1 proton 1 neutron, 0.02% are deuterium used for nuclear fusion.
Tritium, 1 proton and 2 neutrons, very rare, used in thermonuclear fusion weapons.
Relative Atomic Mass
Average mass of all isotopes of an element, how often each isotope is found, aka the isotope abundance.
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For example Chlorine, Ar is 35.5 because its an average mass of an isotope of chlorine.
Nuclides are a type of isotope that refers to a specific nucleus that contains a certain number of protons and neutrons.
A carbon nuclide with 6 protons and 6 neutrons compared to a carbon nuclide with 6 protons and 7 neutrons are both isotopes of carbon but very different.
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