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-Matter is composed of atoms that contain electrons
-Ex: blueberry cake
cake is positive(protons)
blueberries are negative(electrons) |
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| Matter is composed of indestructable, indivisable atoms which are identical for one element, but different for another |
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-An atom is composed of a very small nucleus, which contains positive charges and most of the mass of the atom. The rest of the atom is made up of mostly empty space with very small negative electrons occupying the surrounding area.
-Proved this with gold foil and gamma rays
-some rays went through, some deflected back at different angles. Therefore some sort of positive center or nuclues, and the rest of the atom is mostly empty space |
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| Rutherford and Associates |
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| -Proton has an equal and opposite charge to and electron and is 1836 times its mass. |
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| -Nucleus also contained neutrallly charged particles called neutrons. This explained isotopes |
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-Atoms with the same number or protons, but differnt number of neutrons
-Ex: C-12, C-14 |
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A: Mass Number
Z: Atomic Number
-Ex: C-12 126C |
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| -An isotope that emits radioactive particles as it decays |
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| Planck's Quantum Hypothesis |
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Definition
-Energy could be gained or transfered in whole-number quanties
-Light it emitted in bursts, packets or quantites of energy. IT IS NOT CONTINOUS
-Photon: unit of light energy |
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| -It is impossible to simultaneuosly know the exact position and spped of an electron. |
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| -The region around the nucleus where there is a high probibility of finding an electron |
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| -An electrons lowest, most stable energy level |
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1. Well defined circular path 1. Region of space
2. 2-D motion 2. 3-D motion
3. Max electron is 2n2 3. Max electron is 2
4. Circular shape 4. different shapes |
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| What the quantum number do |
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Definition
-They describe the quantu mechanical properties of orbitals
Principle (n)
Seconday (l)
Magnetic (ml)
Spin (ms) |
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| Principle Quantum Number (n) |
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| -The energy level the electron is located (shell) |
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| Secondary Quantum Number (l) |
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Definition
-Describes the shape of the orbital
0=s orbital (shpere)
1=p orbital (peanut)
2= d orbital (2 peanuts)
3=f
4=g
1=n-1
-Ex: 3n, 1=2,1,0(d,p,s) |
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Magnetic Quantum Number (ml)
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Definition
-Describes the orientation of the orbital in space relative to the other orbitals
-ml= -l to +l
-Ex: l=2 ml=-2,-1,0,1,2 (5 different orientations) |
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-+1/2 counterclockwise
- -1/2 colckwise
Two electrons in the same shell must be spinning oppositly of each other |
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| Pauli Exclusion Principle |
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| Every electron in an atom will have its own set of 4 quantum numbers |
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| In a set of orbitals with the same energy level, the lowest energy configuration for an atom is the one with the max number of unpaired electrons. This means that before any 2 electrons can occupy an orbital in a subshell, other orbitals in the sam esubshell must have one electron occupying it already. |
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| An atom is "bulit up" by the additon of electrons which fill orbiats starting at the lowest availibe energy orbital beofre filing higher energy levels |
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| Energy Level Diagrams-Anions |
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Definition
| -Just add extra electrons |
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| Energy Level Diagrams-Cations |
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| -Do full E.L.D, then substract amount of charge from the highest possible energy level |
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Electron Configuration
Na
Sn+1 |
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Definition
Na:1s2, 2s2, 2p6, 3s1
Sn+1: 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p6, 5s2, 4d10 |
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Cr:[Ar]4s1, 3d5
cu:[Ar]4s1, 3d10
-it is more stable to have half filled orbitals then orbitals with empty spaces |
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Definition
Ferromagnetism: Ni, Co, Fe
Paramagnetism: weak magnetic field |
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-Electronegatitives between 0.4 and 1.7
-If a symmetrical coumpond has polar bonds, the total compund is non polar, because each bond is beinnging pulled in equal and opposite directions |
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-Electronegativites between 0 and 0.4
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-Electronegativites 1.7+
-Usually between metals and non-metals |
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-Metal(anions) and non-metals(cations)
-ex: NaCl
-hard, britte, high melting/boiling points
-crystal
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-Metals
-ex: Zinc/Iron
-shiny, silvery, flexible and conduct electricity/heat
-nuclei are fixed and valance electrons are mobile (electron sea)
-Electrons act as glue to hold nuclei together
-strong bonding (+nuclei and -valance electrons) |
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-Non-metals
-ex: iodine, carbon dioxide
-low melting/boiling point, non conductors
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| Covalent Netwrok Crystals |
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Definition
-ex: diamond and graphite
-very hard and strong, high boiling/melting points
-some can conduct electricity (graphite)
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VSEPR Theory
A= central atom
X= bonding electrons
E= unbonded electron pairs |
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-Valance Shell Electron Pair Repulsion Theory
-helps you to predict the shape of molecules due to their bonding and non-bonding pairs of electrons
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