1. Nanochemistry
FNI 1E Chemistry

2. Review of Chemistry States of Matter Atoms, Molecules and Ions
Subatomic particles
Periodic Table
Covalent and ionic bonding
Chemical reactions
Inter-molecular forces
FNI 1E Chemistry

3. States of Matter Solid Keeps shape Keeps volume Salt, gold, copper
Liquid
Takes shape of container
Water, alcohol, oil
Gas
Takes volume of container
Air, argon, helium, methane
Plasma – like a gas of charged particles.
Stars, nebula, lightning, plasma reactors
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4. Matter
Solution: A uniform mixture of two substances such that molecules are separate from each other and move around randomly. Usually these are liquids. Solutions are usually transparent.
Colloids: A mixture of much larger particles ranging from 20 nm to 100 μm. Milk and paint are colloids.
Grains: Some materials are made up of many small crystals called grains. A grain is an individual crystal of such a solid. Different grains may have the crystal lattice oriented in different directions.
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5. Grain Structure in Steel
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6. Elements, Atoms and Molecules
Atoms: All matter is made up of tiny particles called atoms.
Molecules: Sometimes two or more atoms are found bound together to form molecules.
The atoms can be categorized into about 115 different types based on the charge of the nucleus.
Elements are made up of only one type of atom.
The element carbon takes the form of graphite, diamond and buckminsterfullerene as well as others.
It is only possible to change one type of atom into another through nuclear processes such as take place in a nuclear power plant, the sun, atomic bombs or particle accelerators.
The elements do not change in ordinary chemical reactions.
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7. The Periodic Table 1 H 2 He 3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10 Ne 11 Na
12 Mg
13 Al
14 Si 15 P
16 S
17 Cl
18 Ar 19 K
20 Ca 21 Sc 22 Ti 23 V 24 Cr 25 Mn 26 Fe 27 Co 28 Ni 29 Cu 30 Zn 31 Ga 32 Ge 33 As 34 Se 35 Br 36 Kr 37 Rb 38 Sr 39 Y 40 Zr 41 Nb 42 Mo 43 Tc 44 Ru 45 Rh 46 Pd 47 Ag 48 Cd 49 In 50 Sn 51 Sb 52 Te 53 I 54 Xe 55 Cs 56 Ba 57 La 72 Hf 73 Ta 74 W 75 Re 76 Os 77 Ir 78 Pt 79 Au 80 Hg 81 Tl 82 Pb 83 Bi 84 Po 85 At 86 Rn 87 Fr 88 Ra 89 Ac
104 Rf
105 Db
106 Sg
107 Bh
108 Hs
109 Mt
110 Ds
111
112
113
114
115
116
117
118 58 Ce 59 Pr 60 Nd 61 Pm 62 Sm 63 Eu 64 Gd 65 Tb 66 Dy 67 Ho 68 Er 69 Tm 70 Yb 71 Lu 90 Th 91 Pa 92 U 93 Np 94 Pu 95 Am 96 Cm 97 Bk 98 Cf 99 Es
100 Fm
101 Md
102 No
103 Lr
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8. Subatomic Particles
Most of matter is made of three subatomic particles:
Particle
Symbol
Relative Charge
Relative Mass
Location
Electron e- -1 1
Electron Cloud
Proton p+ +1
1836
Nucleus
Neutron n0
1839
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9. Ions
Usually atoms have the same number of electrons as protons so the charges cancel each other out.
Sometimes an atom can have more or fewer electrons than protons resulting in a net positive or negative charge. When this happens it is called an ion.
Example: Na loses an electron to form Na+
Chlorine can gain an electron to from Cl-
We can tell what type of charge an ion is expected to have by looking at where it is in the periodic table.
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10. Isotopes
Atoms with the same number of protons but different numbers of neutrons
Deuterium, tritium, Carbon 12, U235
Some isotopes are radioactive while others are stable
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11. The Atom Game
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12. Electron Orbitals http://www.shef.ac.uk/chemistry/orbitron/ 1s 2s 2p
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13. Chemical Bonding Covalent bonds Ionic bonds Metal bonding
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14. Covalent bonds
Covalent bonding is when electrons are shared between to atoms or more.
The number of covalent bonds an atom is likely to form is determined by its place in the periodic table and the number of valence electrons it has.
An atom will share electrons with another atom so that it results in them both having a full valence shell. Usually this will be 8 electrons.
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15. Ionic bonds
When a metal and a non-metal form bonds they are typically ionic bonds where electrons are transferred from the metal to the non-metal.
Some metals will lose enough electrons to achieve a complete valence shell.
Non-metals will usually gain enough electrons to achieve a complete valence shell.
Many metals are able to form ions with more than one charge.
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16. Metal bonding
In metals the atoms are held together by metal bonding. Electrons can easily transfer from one atom to the next. This suggests a model of positive ions in a sea of electrons. Metals can conduct electricity because electrons flow easily in any direction.
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17. Covalent and Ionic Bonding
Atom
# of Covalent Bonds
Typical charge for an Ion H 1 +1 C 4 O 2 -2 N 3
F, Cl, Br, I -1 S Si
Li, Na, K
Be, Mg, Ca, Sr, Ba +2
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18. Electronegativity and Polar Molecules
This is the tendency for a type of atom to attract electron density.
Polar Molecules
If the electron density is not distributed evenly around a molecule then they are polar.
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19. Intermolecular Bonding Bonding between molecules van der Waals forces
Hydrogen bonding
This relatively strong type of inter-molecular bonding which typically occurs between a hydrogen atom of one molecule and an electron pair or electronegative atom of another molecule.
Multiple hydrogen bonds hold the DNA double helix together.
Dipole interaction
London forces
These are induced forces caused by a temporary rearrangement of the electron clouds when molecules bump together.
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20. Hydrogen Bonding + + - - O H H
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21. Hydrogen Bonding O H O H
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22. Dipole Interaction
The partial positive and negative ends of the molecules hold the molecules together.
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23. London Forces
London forces are induced dipoles caused by temporary rearrangement of the electron cloud.
Two hexane molecules approach.
The hexane molecules bump into each other.
The electron clouds rearrange to form a temporary dipole. - - - + + + - - - + + +
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24. ( ) Polymers http://www.pslc.ws/macrog.htm nCH2=CH2
Polymers are large chainlike molecules that are built from smaller molecules called monomers.
For example polyethylene is formed from ethylene:
Proteins are natural polymers. C H ) ( n
nCH2=CH2
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25. Chemical Reactions Involve the making or breaking of chemical bonds.
Chemical reactions result in making a new substance with different properties from the original substance.
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26. Structure of Materials
Grains
Crystals
Crystal
Unit Cell
Electron orbitals
Atom
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27. Biological Organization
Tissue
Cells
Organelles
Membranes
Proteins
Nucleic Acids
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28. Mind Map
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29. Review of Chemistry States of Matter Atoms, Molecules and Ions
Subatomic particles
Periodic Table
Covalent and ionic bonding
Chemical reactions
Intra-molecular forces
Polymers
FNI 1E Chemistry