Scientists A AA B CBC Scientists B AA B CBC Scientists C A BA B CC Electron Configuration theory AA B CBC Radioactivity AA B CBC Ionization Energy AA.

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Presentation transcript:

Scientists A AA B CBC Scientists B AA B CBC Scientists C A BA B CC Electron Configuration theory AA B CBC Radioactivity AA B CBC Ionization Energy AA B CBC Reactivity AA B CBC Energy levels AA B CBC Quantum theory AA B CBC Writing electron configuration AA B CBC Radiation equations AA B CBC Bonding AA B CBC

John Dalton

Dmitri Mendeleev

Radioactivity, discovered 2 new elements and discovered x rays.

Discovered the nucleus of the atom in his gold foil experiment.

Rutherford

J.J. Thomson

Democritus- first mention of atom Dalton- Atomic theory Thomson- electron Curie- xrays, radiation Rutherford- proton and nucleus Bohr- electron orbits Schrodinger- quantum model Chadwick- neutron

It tells us the path the electrons are following with about 90% certainty

The mathematical equations that explained and supported the quantum theory.

Lowest, highest

S can hold 2 P can hold 6 D can hold 10 F can hold 14

1 st level- 2 2 nd level – 8 3 rd level – 18 4 th level th level th level- 18

2 protons and 2 neutrons, in other words a He nucleus.

An electron

Gamma, Beta, Alpha

The amount of energy required to remove an electron from an element’s outside shell. The higher the ionization energy the more difficult it is to remove the electron.

1 valence electron, there is a sharp increase in the ionization between E1 and E2 which shows that we have moved from the unfilled electron shell to a filled one.

Ionization energy increases across the period, this is because the attractive force of the nucleus increases and because the radius of the atom decreases slightly.

As you move down the group the reactivity in metals increases because the valence (reacting) electrons are held more loosely.

As you move down the group on the nonmetal side the reactivity decreases because nonmetals which to attract electrons and the valence electrons are moving farther from the nucleus.

Na, Ra, F

2 nd energy level

3 rd energy level

The innermost shell

1 st to 2 nd, as you move away from the nucleus each energy level has less and less energy difference.

When they are moving down and energy level energy is released. Energy is absorbed when they move up a level.

The d orbital is in between the 3 rd and 4 th energy level in regards to it’s energy. Therefore it nestles in between the two and is halfway between them. We represent this by having them on the 4 th period on the periodic table.

1s 2 2s 2 2p 6 3s 2 3p 4

4s 2 4p 2

F- Flourine

4 2 He

Am

Beta radiation

That elements will combine in small whole number ratios to produce new compounds.

+2

The group number indicates the number of valence electrons an atom has. The valence electrons determine what charge the ion will have, very few valence electrons will form + ions and larger numbers of valence electrons form – ions.