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FNI 1E Chemistry 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 MatterSolid Keeps shape Keeps
volumeSalt, gold, copper
Liquid Takes shape of container
Keeps volume
Water, alcohol, oil
Gas Takes shape of container
Takes volume of container
Air, argon, helium, methane
Plasma – like a gas of charged particles.
Takes shape of container
Takes volume of container
Stars, nebula, lightning, plasma reactors
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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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Grain Structure in Steel
FNI 1E Chemistry 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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The Periodic Table1H
2He
3Li
4Be
5B
6 C
7N
8O
9F
10Ne
11Na
12 Mg
13 Al
14 Si
15P
16 S
17 Cl
18 Ar
19K
20 Ca
21Sc
22Ti
23V
24Cr
25Mn
26Fe
27Co
28Ni
29Cu
30Zn
31Ga
32Ge
33As
34Se
35Br
36Kr
37Rb
38Sr
39Y
40Zr
41Nb
42Mo
43Tc
44Ru
45Rh
46Pd
47Ag
48Cd
49In
50Sn
51Sb
52Te
53I
54Xe
55Cs
56Ba
57La
72Hf
73Ta
74W
75Re
76Os
77Ir
78Pt
79Au
80Hg
81Tl
82Pb
83Bi
84Po
85At
86Rn
87Fr
88Ra
89Ac
104Rf
105Db
106Sg
107Bh
108Hs
109Mt
110Ds
111 112 113 114 115 116 117 118
58Ce
59Pr
60Nd
61Pm
62Sm
63Eu
64Gd
65Tb
66Dy
67Ho
68Er
69Tm
70Yb
71Lu
90Th
91Pa
92U
93Np
94Pu
95Am
96Cm
97Bk
98Cf
99Es
100Fm
101Md
102No
103Lr
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Subatomic ParticlesMost 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 0 1839 Nucleus
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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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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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The Atom Game
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Electron Orbitals
http://www.shef.ac.uk/chemistry/orbitron/1s
2s 2p
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Chemical Bonding
Covalent bonds Ionic bonds Metal bonding
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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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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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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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Covalent and Ionic BondingAtom # of Covalent Bonds Typical charge for an
Ion
H 1 +1
C 4
O 2 -2
N 3
F, Cl, Br, I 1 -1
S 2 -2
Si 4
Li, Na, K +1
Be, Mg, Ca, Sr, Ba +2
FNI 1E Chemistry 18
Electronegativity and Polar Molecules Electronegativity
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. http://www.nyu.edu/pages/mathmol/library/
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Intermolecular BondingBonding between moleculesvan 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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Hydrogen Bonding
+
--+
H
OH
FNI 1E Chemistry 21
Hydrogen Bonding
OH
H
OH
H
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Dipole Interaction
http://www.chemguide.co.uk/atoms/bonding/vdw.html
The partial positive and negative ends of the molecules hold the molecules together.
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London Forces
Two hexane molecules approach.
The hexane molecules bump into each other.
The electron clouds rearrange to form a temporary dipole.
+ + +- - -
+ + +
- - -
London forces are induced dipoles caused by temporary rearrangement of the electron cloud.
FNI 1E Chemistry 24
Polymers
Polymers are large chainlike molecules that are built from smaller molecules called monomers.
For example polyethylene is formed from ethylene:
Proteins are natural polymers. http://www.pslc.ws/macrog.htm
C C
H H
H H
)(n
nCH2=CH2
FNI 1E Chemistry 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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Structure of Materials
Grains Crystals Crystal
Unit CellElectron orbitalsAtom
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Biological Organization
Tissue Cells Organelles
Proteins Nucleic AcidsMembranes
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Mind Map
FNI 1E Chemistry 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
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