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

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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

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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

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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

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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.

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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

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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

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Review of Chemistry

States of Matter Atoms, Molecules and Ions Subatomic particles Periodic Table Covalent and ionic bonding Chemical reactions Intra-molecular forces Polymers