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| All materials can be cut smaller and smaller until theres only one piece left. Called an Atomos of substance. Indivisible in Greek. Definition of atom- smallest part of mater that retains the property of that matter. |
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Second to edit Atomic Theory.
British. Colorblind. Proposes 6 postulates about atoms.
1) All elements are made up of atoms.
2) All atoms of the same element are identitcal (isotopes- NOT TRUE)
3) Atoms of one element are different from atoms of all other elements.
4) Atoms combine in whole number ratios to form compounds.
5) Atoms are indivisible and indestructable (FALSE- nuclear reactions)
[image]--> Extremely simple design. |
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Third to edit Atomic Theory
Comes up with the crooks tube. Used in tvs, computers. Metal plates in tube with little to no air. Makes green beam of light. |
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Fourth to edit Atomic Theory.
Crookes tube green beam of light deflected by magnet. Discovers green beam is able to spin pinwheel in tube. Beam attracted toward positive and away from negetive charges. Sub stomic particle- particles have negitive charges known as electrons.
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Fifth to edit atomic theory
Thompsons student. Gold foil experiment. Positive part of atom is consentrated in a very small part of the atom- center known as the nucleus. Most alpha particles go through but 1% get deflected. Lead box radio active materal. |
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Nobel peace proze in 1923- american!
Oil drop experiment!
Results: Mass and charge of one electron, electrons exist and proven. good support to electrons, turns out to be incorrect.
The experiment (dont need to know):
Takes oil and puts in metal can. Metals have mobile electrons moved along very easily. Good electricity conductors. Sprays oil threw atomizer, fine mist- fog of oil. Oil comes out throw atomizer and picks up mobile electrons. Negative charged. Fall throw hole and sitt between 2 plates. One positive charged and one negative. Positive attracts charges on plates so it suspends particles exactly in the center between the two plates. Redoes 100s of times to find mass of one drop.
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Why dont electrons get drawn into the nucleus? The fact that they are moving orbiting..
Uses a prisom and looks at hydrogen. Sees sharp lines. Bright line spectrum- visible part is small. Each line is a specific amount of energy. Theorizes- That electrons are orbiting the nucleus in spectific movements. Electrons can go up/down energy leverls but can never be inbetween (FALSE- not possible).
PROBLEMS- Doesnt work for anything over one electron, cant not be inbtween energy levels.
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Equation gives possible locations of electron. Makes graph of possible locations of electrons. Equation still used today. Volume in space enclosing 95% of Schrodingers electrons/ graph points for a particular electron. Electrons only have to move faster to gain energy, dont need to move back levels. Plotted points to see electrons POSSIBLE locations. Draws circle to enclose most electrons- called an orbital. 95% PROBABILITY that electron is in that circle. Most modern Theory.
PROVED BOHR WAS WRONG- IMPOSSIBLE TO KNOW EXACT ELECTRON LOCATION- only estimate. SHOWN BELOW
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| Democritus -- Dalton -- Thompson -- Rutherford -- Bhor -- Schrodinger |
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7p --- (3)
6d ----- (5)
5f ------- (7)
7s - (1)
6p --- (3)
5d ----- (5)
4f ------- (7)
6s - (1)
5p --- (3)
4d ----- (5)
5s - (1)
4p --- (3)
3d ----- (5)
4s - (1)
3p --- (3)
3s - (1)
2p --- (3)
2s - (1)
1s - (1) |
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Electrons, Protons, Charge, Mass #, Atomic #, Symbol, - ions |
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In a neutral atom the # of electrons = the # of protons
Charge is protons - electons
Mass number is protons + neutrons
Atomic # = # of protons
Symbol is atomic # or protons
- ion gained electons
Take from highest principal energy level first when moving electrons.
5s2, 4s2 Five is higher!!
Looses --> more positive- cation
Gains --> less positive- anion
METALS ARE LOSERS
NON METALS ARE GETTERS |
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Same number of electrons
Nb is isoelectronic with Kripton if it looses 5 electrons. becomes Nb +5. called an ion.
An element that gains or looses elctrons becomes an ion. |
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| Chemical Behavior Exceptions |
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Cr down
Cu down
(6 ELEMENTS ARE EXCEPTIONS)
Half full more stable then S orbital
Cr= [Ar] 4s2, 3d4
natually becomes= [Ar] 4s1, 3d5
s2, d9 = s1, d10 |
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| Excited/ Ground/ Impossible States |
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Ground is normal electron configuration (no levels skipped)
Excited is when electrons are zapped with energy and jump levels. Bumping up in energy level by placing over flame or electricity.
[Ar] 5s2, 4d3 = EXCITED
[Ar] 4s2, 3d3 = GROUND
p7, d12, s3 is an IMPOSSIBLE STATE because the s orbitals only hold 2 electrons, not three. |
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No 2 electrons can have the same set of 4 quantum numbers.
N= principle quantum bumber (principle energy level)
(Range is 1-7) Ex. 4s2
L= Azimuthal quantum number. (orbital type)
(S=0, P=1, d=2, f=3) Ex. 2s2 would be 0.
ML= Spatial orientation (Specific orbital) (-L...0...+L)
Ex. 3p1 _._ __ __
-1 0 1
Ms= Spin number ( +1/2 or -1/2)
First electron in orbital is always +1/2, second in -1/2.
These were the variables Schrodinger plugged into his equation.
N, L, Ml, Ms.
EXAMPLE:
P=[Ne] 3s2, 3p3
Quantum numbers are N= 3, L= 1, Ml = 1, Ms= +1/2
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