1. ATOMIC STRUCTURE
1. Relate the number of protons, neutrons and electrons in an atom (including
isotopes) or a monatomic ion, to the atomic number, mass number and charge.
2. State the electron arrangement of atoms and/or ions of the first 20 elements in
the Periodic Table.
3. Relate the charge on monatomic ions to the position of the element on the Periodic
Table.
4. State the electron arrangement of atoms and/or ions of the first 20 elements in
the Periodic Table.
5. Relate the charge on monatomic ions to the position of the element in the Periodic
Table
6. Draw Lewis diagrams of :
• atoms selected from the first 20 elements
• molecules including those with single bonds, e.g. H2O, CH4, H2, Cl2 & PCl3 and
those with multiple bonds
Thursday, 22 April 2010
5. Term Definition GLOSSARY 1
crystal
lattice
melting
boiling
Thursday, 22 April 2010
6. Term Definition GLOSSARY 1
atom
element
proton
electron
neutron
neutral
atomic number
mass number
group
row
valence
relative
isotope
octet rule
duet rule
valence
molecule
Thursday, 22 April 2010
7. Term Definition GLOSSARY 1 - MATCH UP
A. geology 1. natural substances with a definite composition and structure
B. rock 2. formation of crystals from molten rock or solution
C. minerals 3. describes solids which do not have a crystalline structure
D. elements 4. solid substances showing definite geometrical shapes
5. mass of an object compared to the mass of the same volume
E. compounds
of water
F. crystals 6. substances made of identical atoms
G. solidify 7. the degree of shine on the surface of a solid
H. crystallise 8. light does not pass through
I. amorphous 9. changing from a molten to as solid state
J. lustre 10. study of the Earth’s structure and its rocks
K. relative 11. used to describe an object which will affect a nearby
density compass needle
L. magnetic 12. made out of crystals
M. crystalline 13. light passes through but not clearly
N. transparent 14. substances made of non-identical atoms bonded together
O. translucent 15. light passes through clearly
P. opaque 16. solid, non-living material that forms the earth’s crust
Thursday, 22 April 2010
8. Term Definition GLOSSARY 2
Lewis structure
lone pair
single bond
double bond
triple bond
anion
cation
group
period
reactivity
solubility
electric current
Thursday, 22 April 2010
11. Elements THE BASICS Complete:
Elements are like the letters of the alphabet. There are 26
letters and these can be joined together in different ways to make up to 750 000
different words. Letters cannot be split into anything simpler.
• Elements are substances that contain particles called .
• An element consists of only one type of atom only.
• Atoms cannot be easily into anything .
• There are 90 different elements and these can be .
to make all the other in the world
Atoms
Part of Where Electrical
atom found Charge
Proton
+
+ Neutron
Proton Electron
Word list: substances, atoms,
simpler, split, joined, proton,
electron, empty space, negative,
positive, neutral, neutron, in the
“History of the atom” nucleus, outside the nucleus.
Thursday, 22 April 2010
12. Element names
H Na
He Mg
Li Al
Be Si
B P
C S
N Cl
O Ar
F K
Ne Ca
An easy way to remember the first 20 elements Flashcards
(in exercises)
Harry He Likes Beer By Cupfuls Not Over Flowing
Never Natter Magic Although Science Possesses Some Clues
Arthur Kicks Cats “Element
Bingo” (in starters)
Thursday, 22 April 2010
14. THE PERIODIC TABLE
Hydrogen - not a metal
but here because of its
electron arrangement
1 2 3 4 5 6 7 8
Non-metals
Less reactive
More reactive metals Inert gases
metals
Thursday, 22 April 2010
15. ORGANISATION OF THE PERIODIC TABLE
Atomic number
Atomic numbers are the smaller of the two numbers associated with
each element. Atomic numbers increase by one from left to right of
the table
Rows
The atoms get larger in size from left to right across a row as their
mass increases
Columns
The atoms get larger in size and increase in mass from top to bottom
of a column. Elements in a column have similar properties. Columns
are often called groups.
Groups start at 1 (at the left) and finish with group 8 (at the right of
the table)
Thursday, 22 April 2010
17. MASS NUMBERS & ATOMIC NUMBERS
An element in the periodic table is described like this:
The mass number is 19.
19 The number of protons plus neutrons =19
9 F
Fluorine The atomic number is 9.
There are 9 protons in the nucleus and 9 electrons around it
In this example:
The 19 particles in the nucleus are protons or neutrons I’m lost!
9 of these particles are protons
therefore there are 10 neutrons in the nucleus
Summary
For an atom:
• The atomic number gives the number of protons
• The atomic number is also gives the number of electrons
• The mass number is the number of protons plus neutrons
• neutron number = mass number - atomic number
Thursday, 22 April 2010
18. An exercise done as a class:
4
He This shows how Helium appears in the periodic table
2
Helium
This means: The atomic number is ___.
so there are: 2 protons in the nucleus
and 2 electrons surrounding it
The mass number is ____.
so the number of protons plus neutrons =4
Therefore the number of neutrons must be ___ ( = __ - __)
number of
Symbol of element number of protons number of neutrons
electrons
11 B
5
16 O
8
28 Si 14
35 Cl 20
31 P 15
Thursday, 22 April 2010
19. Individual Exercise TRY THIS!
number of
Symbol of element number of protons number of neutrons
electrons
9 Be
4
21 Ne
10
27 Al 13
39 K 20
15P 16
42 Ca
20
12 C 6
7 Li
3
23 Na
11
24 Mg 12
14 N
7
16S 16
Thursday, 22 April 2010
20. ELECTRON ARRANGEMENTS
Electrons in the electron cloud are not arranged randomly around the nucleus.
• Those close to the nucleus have low energy
• Those far away from the nucleus have high
energy
Electrons are arranged in energy levels
For the 1st 20 elements there are 4 energy levels:
Level 1 can hold a maximum of 2 electrons
Level 2 “ “ “ “ “ 8 electrons
Level 3 “ “ “ “ “ 8 electrons
Level 4 “ “ “ “ “ 2 electrons
Example 1
20 protons in the nucleus
20
(the atomic number)
Ca => 20 electrons around the
40
nucleus
2.8.8.2
Electron arrangement: “ 2 in the 1st shell, 8 in the 2nd shell, .......
Thursday, 22 April 2010
21. CONFIGURE THIS!
Use your knowledge of electron
arrangement to complete the
table below. The electron 1
arrangements are shown below H
1
the element names Hydrogen
1
4
2 He
Helium
2
7 9 11 12 14 16 19 20
3 Li 4 Be 5 B 6 C 7 N 8 O 9 F 10 Ne
Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon
2.1 2.2 2.3 2.4
23 24 27 28 31 32 37 40
11 Na 12 Mg 13 Al 14 Si P S Cl Ar
Sodium Magnesium Aluminium Silicon Phosphorus Sulphur Chlorine Argon
2.8.1
39 40
K Ca
Potassium Calcium
Thursday, 22 April 2010
22. SHELL DIAGRAMS
Electrons fill up an atoms shell in order, first they fill up the
inner shell (first electron shell) then the next shell and so on
An exercise done as a class:
Process:
40 x 1. Use your periodic table to find the atomic
Ca x x
x x
x
x
number.
x x
Calcium x
x x 2. The atomic number will tell you how
x x
x many electrons there are
x x
x x
x Ca 3. Fill the electrons according to the rule:
Level 1 can hold a maximum of 2 electrons
Example 2 - Silicon Level 2 “ “ “ “ “ 8 electrons
Level 3 “ “ “ “ “ 8 electrons
14
28
Level 4 “ “ “ “ “ 2 electrons
Si
28 4. Start filling the levels from level 1.
2.8.4
5. When level 1 is full start filling level 2. When
Si
level 2 is full start filling level 3 and so on.
6. Stop filling the levels when you have used all
the electrons that the atom has.
Thursday, 22 April 2010
23. Individual Exercise A DIFFERENT WAY OF SHOWING IT! Key: p = proton
n = neutron
Example: Fluorine, 9
19F has 9p, 10n, 9e e = electron
e
e For each of the following atoms draw the
electron shell diagram. Show the nucleus as
a solid circle.
n p e e
e n p p
n p n n p A second example
n p p p n
n n
e n p 1. 13
27Al x 2. 11
23Na
x
e x x x
x x x x
e
x x x
e x
3. 14
28Si 4. 15
31P 5. 16
32S
Homework (in science books):
(i) Be (ii) F (iii) Ne (iv) Ar
Thursday, 22 April 2010
28. ATOMS TO IONS
An ion is an atom that has lost or gained electrons
“Ions are more stable than atoms. IONS HAVE AN OUTER SHELL THAT IS FULL...
Using this knowledge it is possible to work out the arrangement of electrons in
ions.”
Sodium atom --> Sodium ion
1 electron
E x x
x x x
lost
x
X
x
x x x
x
x x x
A x x x x
x
x x 1+ charge
M Na Na+
P Chlorine atom --> Chloride ion
1 electron
L
x x
x
x x x x x
x gained
x x x x x
E
x
x x
x x x x
x x x x
S x
x
x
x
x x
x
x
x
x
Cl Cl- 1- charge
Thursday, 22 April 2010
29. IRONING OUT THE IONS
“Metal atoms lose electrons. Non-metal atoms gain electrons.
No more than 3 electrons can be lost or gained”
Copy & complete the following table showing the electron arrangements of the atoms
and their ions:
Metal atom Metal ion Non-metal atom Non-metal ion
C: 2, 4 no ion formed Cl: 2, 8, 7 Cl-: 2, 8, 8
Mg: 2, 8, 2 Mg2+: 2, 8 N: 2, 5 N3-: 2, 8
Li: 2, 1 Li+: 2 Ar: 2, 8, 8 No ion formed
Be O
Ca S
Al F
Na P
Draw small Beryllium Sulphide Aluminium
shell diagrams
for the
following ions
Thursday, 22 April 2010
30. FORMULAE FOR SIMPLE IONS
Background
A chemical formula shows how atoms or ions are joined to make compounds. (A
compound consists of two or more different atoms that are joined chemically).
An ionic compound is formed when positive and negative ions are attracted to each
other. Some ions comprise groups of atoms that have gained or lost electrons. These
groups are the “-ides” or “-ates”.
A table of common ions is shown below:
+1 +2 +3 _,,
-1
H* Mg2* Al3+ c1- gz-
hydrogen magnesium aluminium chloride oxide
Li* Ca2* Fe3* oH- COr'-
lithium calcium iron(III) hydroxide carbonate
Na+ Fe2* No,* Soo'-
sodium iron(II) nitrate sulfate
K+ Cu2* HCO3- PO43-
potasslum copper(II) hydrogen carbonate Phosphate
Zn2*
zinc
Pb2+
lead
Thursday, 22 April 2010
31. GETTING TO KNOW THE “-IDES” AND “-ATES”
“-ates” end in O4 and O3
An exercise done as a class: the rest are “-ides”
+ ion - ion Formula + ion - ron Formula
Znzr N3- ZneNz Ca2* NOs- Ca(NOs)z
Pb2* Br PbBrz Fe3* SO+2- Fe2(S04)3
I Ag* s2- Li* COs2- LizCOs
) Fe3* cl- 6 Ag* PO+3-
3 Na* 02- 7 NH+* SO+2-
K+ t- KI 8 Pbz* COs2-
Cu2* SO+2- CuSOa 9 Al3* oH-
4 Mgz+ COs2- 10 Cu2* s2-
5 Zn2* 02- 11 (+ HCOg-
On the table (above):
1. Circle the “-ates” using a red pen
2. Circle the “-ides” using a blue pen
3. and name them Exercises: “-ide or -ate”
Thursday, 22 April 2010
32. ION FORMATION AND THE PERIODIC TABLE
1 2 Groups of the periodic table 3 4 5 6 7 8
1+ 2+ Charge on ions formed by atoms in each group 3+ 3- 2- 1-
Do not form ions
Thursday, 22 April 2010
51. PROPERTIES OF SOLIDS, LIQUIDS AND GASES BOB: Unscramble
Appearance & Particles Energy Compressibility Melting &
behaviour in a arrangement boiling
container points
A D. Particles are G. The very high J. high M. Moderate
disordered energy of the
and widely particles
SOLID
spaced causes random
& rapid
E. Particles H. The low K. very little N. High
closely energy of the
spaced & particles
arranged in causes them
LIQUID B a lattice. to vibrate
This explains about fixed
the positions
crystalline
appearance
F. Particles are I. The moderate L. virtually O. Low
disordered energy of the none
and closely particles
GAS C
spaced causes them
to move
randomly
Answers: SOLID __ __ __ __ __ LIQUID __ __ __ __ __ GAS __ __ __ __ __
Thursday, 22 April 2010
52. http://
PROPERTIES OF SOLIDS, LIQUIDS AND GASES www.harcourtschool.com/
activity/states_of_matter/
Appearance & Particles Energy Compressibility Melting &
behaviour in a arrangement boiling
container points
Particles are The low energy virtually none High
closely of the particles
spaced and causes them to
arranged in a vibrate about
SOLID fixed positions
lattice. This
explains the
crystalline
appearance
Particles are The moderate very little Moderate
disordered energy of the
LIQUID and closely particles causes
spaced them to move
randomly
Particles are The very high high Low
disordered energy of the
GAS and widely particles causes
spaced random & rapid
movement
Thursday, 22 April 2010
54. ATOMS, ELEMENTS, COMPOUNDS & MIXTURES
P
U
R
E
Element Element Compound
N
O
T
P
U
R
E
Mixture Mixture
of elements of element with compound
Thursday, 22 April 2010
55. Interactive Complete the mind map
All substances
X
.............. Not pure
...................
Elements ...................
Element
................ with Different
elements compound .................
Questions
1. Explain the difference between Co and CO
__________________________________________________________________
__________________________________________________________________
2. Explain the difference between O2 and 2O
__________________________________________________________________
__________________________________________________________________
Thursday, 22 April 2010
56. Copy ATOMS, ELEMENTS, COMPOUNDS & MIXTURES
• An atom is a particle that cannot be made smaller by simple chemical methods.
• An element is a substance that contains only one type of atom.
• A compound is a substance that contains two or more types of atom chemically
joined together in a constant ration by mass.
• A mixture contains two or more different types of particle.
• A solution is a special mixture where the solid particles are spread evenly
throughout a liquid medium
All substances
Pure Not pure
Mixture
Elements Compounds
Element
Different with Different
elements compound compounds
Ex 3A: 1 to 4 - Answers only
Thursday, 22 April 2010
58. SOLUTIONS PRE - TEST (out of 8)
Use the diagram, word list and prior knowledge to complete the cloze
exercise:
1. Salt added to water will form a ______________.
2. Salt is an example of an _________ solid
3. The ions present in salt are ___________ and _____________ .
4. Theses ions arrange themselves into a _____________.
5. Solids with __________ structures have a _____________ appearance. This
means the visible particles have __________ edges and __________ faces.
Cl- Na+ Cl-
Na+ Cl- Na+
Cl- Na+ Cl-
Word list
lattice sodium ionic flat chloride sharp solution crystalline
Thursday, 22 April 2010
59. SOLUTIONS PRE - TEST (out of 8)
Use the diagram, word list and prior knowledge to complete the cloze
exercise:
solution
1. Salt added to water will form a ______________.
2. Salt is an example of an _________ solid
3. The ions present in salt are ___________ and _____________ .
4. Theses ions arrange themselves into a _____________.
5. Solids with __________ structures have a _____________ appearance. This
means the visible particles have __________ edges and __________ faces.
Cl- Na+ Cl-
Na+ Cl- Na+
Cl- Na+ Cl-
Word list
lattice sodium ionic flat chloride sharp crystalline
Thursday, 22 April 2010
60. SOLUTIONS PRE - TEST (out of 8)
Use the diagram, word list and prior knowledge to complete the cloze
exercise:
solution
1. Salt added to water will form a ______________.
ionic
2. Salt is an example of an _________ solid
3. The ions present in salt are ___________ and _____________ .
4. Theses ions arrange themselves into a _____________.
5. Solids with __________ structures have a _____________ appearance. This
means the visible particles have __________ edges and __________ faces.
Cl- Na+ Cl-
Na+ Cl- Na+
Cl- Na+ Cl-
Word list
lattice sodium flat chloride sharp crystalline
Thursday, 22 April 2010
61. SOLUTIONS PRE - TEST (out of 8)
Use the diagram, word list and prior knowledge to complete the cloze
exercise:
solution
1. Salt added to water will form a ______________.
ionic
2. Salt is an example of an _________ solid
sodium
3. The ions present in salt are ___________ and _____________ .
4. Theses ions arrange themselves into a _____________.
5. Solids with __________ structures have a _____________ appearance. This
means the visible particles have __________ edges and __________ faces.
Cl- Na+ Cl-
Na+ Cl- Na+
Cl- Na+ Cl-
Word list
lattice flat chloride sharp crystalline
Thursday, 22 April 2010
62. SOLUTIONS PRE - TEST (out of 8)
Use the diagram, word list and prior knowledge to complete the cloze
exercise:
solution
1. Salt added to water will form a ______________.
ionic
2. Salt is an example of an _________ solid
sodium chloride
3. The ions present in salt are ___________ and _____________ .
4. Theses ions arrange themselves into a _____________.
5. Solids with __________ structures have a _____________ appearance. This
means the visible particles have __________ edges and __________ faces.
Cl- Na+ Cl-
Na+ Cl- Na+
Cl- Na+ Cl-
Word list
lattice flat sharp crystalline
Thursday, 22 April 2010
63. SOLUTIONS PRE - TEST (out of 8)
Use the diagram, word list and prior knowledge to complete the cloze
exercise:
solution
1. Salt added to water will form a ______________.
ionic
2. Salt is an example of an _________ solid
sodium chloride
3. The ions present in salt are ___________ and _____________ .
lattice
4. Theses ions arrange themselves into a _____________.
5. Solids with __________ structures have a _____________ appearance. This
means the visible particles have __________ edges and __________ faces.
Cl- Na+ Cl-
Na+ Cl- Na+
Cl- Na+ Cl-
Word list
flat sharp crystalline
Thursday, 22 April 2010
64. SOLUTIONS PRE - TEST (out of 8)
Use the diagram, word list and prior knowledge to complete the cloze
exercise:
solution
1. Salt added to water will form a ______________.
ionic
2. Salt is an example of an _________ solid
sodium chloride
3. The ions present in salt are ___________ and _____________ .
4. Theses ions arrange themselves into a _____________.
lattice
5. Solids with __________ structures have a _____________ appearance. This
means the visible particles have __________ edges and __________ faces.
Cl- Na+ Cl-
Na+ Cl- Na+
Cl- Na+ Cl-
Word list
flat sharp crystalline
Thursday, 22 April 2010
65. SOLUTIONS PRE - TEST (out of 8)
Use the diagram, word list and prior knowledge to complete the cloze
exercise:
solution
1. Salt added to water will form a ______________.
ionic
2. Salt is an example of an _________ solid
sodium chloride
3. The ions present in salt are ___________ and _____________ .
4. Theses ions arrange themselves into a _____________.
lattice crystalline
5. Solids with __________ structures have a _____________ appearance. This
means the visible particles have __________ edges and __________ faces.
Cl- Na+ Cl-
Na+ Cl- Na+
Cl- Na+ Cl-
Word list
flat sharp
Thursday, 22 April 2010
66. SOLUTIONS PRE - TEST (out of 8)
Use the diagram, word list and prior knowledge to complete the cloze
exercise:
solution
1. Salt added to water will form a ______________.
ionic
2. Salt is an example of an _________ solid
sodium chloride
3. The ions present in salt are ___________ and _____________ .
4. Theses ions arrange themselves into a _____________.
lattice crystalline
5. Solids with __________ structures have a _____________ appearance. This
sharp
means the visible particles have __________ edges and __________ faces.
Cl- Na+ Cl-
Na+ Cl- Na+
Cl- Na+ Cl-
Word list
flat
Thursday, 22 April 2010
67. SOLUTIONS PRE - TEST (out of 8)
Use the diagram, word list and prior knowledge to complete the cloze
exercise:
solution
1. Salt added to water will form a ______________.
ionic
2. Salt is an example of an _________ solid
sodium chloride
3. The ions present in salt are ___________ and _____________ .
4. Theses ions arrange themselves into a _____________.
lattice crystalline
5. Solids with __________ structures have a _____________ appearance. This
sharp flat
means the visible particles have __________ edges and __________ faces.
Cl- Na+ Cl-
Na+ Cl- Na+
Cl- Na+ Cl-
Word list
Thursday, 22 April 2010
69. Solutions SEPARATING MIXTURES
http://phet.colorado.edu/new/simulations/sims.php?sim=Salts_and_Solubility
An animation showing how substances dissolve:
Solvent
Solute
Solution
Reading with exercises ->
Thursday, 22 April 2010
70. SEPARATING MIXTURES
• Separation techniques based on the differences in the physical properties of the
substances making up the mixture.
Separation Why it can be separated using this
Type of mixture
technique technique
Decanting The particles in the mixture are different
Suspension (Liquid & sizes. Small liquid and solid particles
insoluble solid) pass through whilst larger solid particles
Filtration
do not
The solvent has a lower boiling point and
evaporates away. In the case of two
Solution (containing a Evaporation liquids that are mixed, the liquid with the
solvent & a solute or lower boiling point will evaporate away
two liquids that are
mixed) Based on evaporation but allows the
Distillation solvent or high boiling point liquid to be
kept
Different solvents have different
Solutions that contain solubility in the solvent used so they
Chromatography travel at different speeds alont the
many solutes
chromatography paper
Thursday, 22 April 2010
72. ATOMIC THEORY
History
1803 - Dalton’s model: “Atoms are indestructible spheres”
1911 - Rutherford: An atom is mainly empty space. It has a central dense,
positively charged nucleus. The nucleus is tiny compared
to the overall size of the atom.
1932 - Chadwick shows that neutrons exist
Atoms
Electron
+ Neutron
+
Proton
Part of Where Relative Electrical
atom found mass Charge
Proton nucleus 1 positive
Neutron nucleus 1 neutral
outside
Electron 0.0005 negative
nucleus
p31 & 32 - ESA -> Ex. 4A: Q.1 to 4 - answers only
Thursday, 22 April 2010
73. ISOTOPES
16 17 18
O O O
8 8 8
Thursday, 22 April 2010
74. ISOTOPES
Atoms with the same atomic number but different mass numbers.
Example
Below are the symbols of the common isotopes of Oxygen.
Notice that the mass numbers are different
16 17 18
O O O
8 8 8
Each isotope has 8 protons
8 neutrons 9 neutrons 10 neutrons
Each different isotope has
different numbers of neutrons
Thursday, 22 April 2010
75. ATOMIC MASS
An isotope has a mass number.
An element that consists of different isotopes will have an atomic mass.
Ex 4B Q.1 to 3 - answers only
Thursday, 22 April 2010
76. ATOMIC MASS
An isotope has a mass number.
An element that consists of different isotopes will have an atomic mass.
The atomic mass of an element is the weighted average of the mass numbers of all
the isotopes in that element.
Ex 4B Q.1 to 3 - answers only
Thursday, 22 April 2010
77. ATOMIC MASS
An isotope has a mass number.
An element that consists of different isotopes will have an atomic mass.
The atomic mass of an element is the weighted average of the mass numbers of all
the isotopes in that element.
Example
A naturally occurring sample of Copper has 3 atoms of 63
Cu to each one atom of
65
Cu:
63
Cu 63
Cu 63
Cu 65
Cu
Ex 4B Q.1 to 3 - answers only
Thursday, 22 April 2010
78. ATOMIC MASS
An isotope has a mass number.
An element that consists of different isotopes will have an atomic mass.
The atomic mass of an element is the weighted average of the mass numbers of all
the isotopes in that element.
Example
A naturally occurring sample of Copper has 3 atoms of 63
Cu to each one atom of
65
Cu:
Atomic mass = 63 + 63 + 63 + 65
63
Cu 63
Cu 63
Cu 65
Cu 4
= 63.5
(or “3 x 63 + 65”)
Ex 4B Q.1 to 3 - answers only
Thursday, 22 April 2010
79. ATOMIC MASS
An isotope has a mass number.
An element that consists of different isotopes will have an atomic mass.
The atomic mass of an element is the weighted average of the mass numbers of all
the isotopes in that element.
Example
A naturally occurring sample of Copper has 3 atoms of 63
Cu to each one atom of
65
Cu:
Atomic mass = 63 + 63 + 63 + 65
63
Cu 63
Cu 63
Cu 65
Cu 4
= 63.5
(or “3 x 63 + 65”)
Chlorine is another element which consists of different isotopes. It has an atomic
mass of 35.5
Ex 4B Q.1 to 3 - answers only
Thursday, 22 April 2010
80. ATOMIC MASS
An isotope has a mass number.
An element that consists of different isotopes will have an atomic mass.
The atomic mass of an element is the weighted average of the mass numbers of all
the isotopes in that element.
Example
A naturally occurring sample of Copper has 3 atoms of 63
Cu to each one atom of
65
Cu:
Atomic mass = 63 + 63 + 63 + 65
63
Cu 63
Cu 63
Cu 65
Cu 4
= 63.5
(or “3 x 63 + 65”)
Chlorine is another element which consists of different isotopes. It has an atomic
mass of 35.5
Most elements consist mainly of one isotope and therefore their atomic mass is
close to a whole number.
Ex 4B Q.1 to 3 - answers only
Thursday, 22 April 2010
81. ESA p41 Boron is unshaded because it does not covalently bond with itself??
LEWIS
STRUCTURES
Thursday, 22 April 2010
82. ELECTRON CONFIGURATION
• Electrons around the nucleus of the atom have different levels of energy:
• High energy electrons move in regions which are further away from the nucleus
than low energy electrons.
Level 1 can hold a maximum of 2 electrons
Level 2 “ “ “ “ “ 8 electrons
Level 3 “ “ “ “ “ 8 electrons
Level 4 “ “ “ “ “ 2 electrons
• Greater stability is achieved when the outer energy level is fully occupied by
electrons (usually 8) - this is the octet rule.
Ion formation occurs according to this rule
Example Sodium atom GREATER
Sodium ion
STABILITY
Na Na+
1 electron is lost
Note: Inert gases are stable because the outer level is fully occupied by electrons
Thursday, 22 April 2010
83. ATOM MODELS
Models are used to explain things that we can’t see and/or understand.
Showing only the outer electrons (valence electrons) is a useful model.
Examples - “electron dot diagrams”
Electron configuration is 2.5 but only the 5 valence electrons
N are shown
(the 7 protons and 7 neutrons are not shown in this model)
Electrons are displayed as dots and shown in pairs as they are
thought to occupy the same region in an energy level.
Cl
Thursday, 22 April 2010
84. “CAN YOU SEE THE PATTERN?”
Metal
Key
Borderline but more non - metal
Non - metal
“Which atoms will bond covalently to form molecules?”
Thursday, 22 April 2010
85. COVALENT BONDING
Covalent bonds are formed between non-metal atoms. The bond is
based on the mutual attraction of 2 different positively charged nuclei to the
same pair of negatively charged electrons.
Molecules are formed.
Example: Chlorine, Cl2
Chlorine does not normally exist as individual atoms. Two chlorine atoms pair up to
make a molecule. A pair of electrons is shared between the two atoms:
Each chlorine atom
7 valence
Cl + Cl Cl Cl now has 8 valence
electrons
electrons
A lone pair of electrons A shared pair
“The octet rule is nearly always obeyed except where Hydrogen is involved
in a covalent bond. The outer energy level of hydrogen is fully occupied
when it contains 2 electrons. Hydrogen obeys the duet rule”
Thursday, 22 April 2010
86. LEWIS STRUCTURES
The chlorine molecule drawn (above) is an example of a Lewis structure
Other Lewis structures
Water H2O
O H
H
Hydrogen chloride HCl H Cl
Note
Both the octet and duet rules are both obeyed in the examples (above)
The attraction between atoms is called a bond
A bond can be drawn as a line:
H
H - Cl
O O
Thursday, 22 April 2010
87. DOUBLE BONDS
Sometimes, in order to obey the octet rule, two atoms will need to share
two pairs of electrons.
This TWO shared pair of electrons forms the basis of a double bond.
Examples
Silicon dioxide, SiO2 contains 2 double bonds
O Si O O Si O
TWO pairs are shared The octet rule is
satisfied for each atom
Carbon tetrachloride CCl4 contains only in the molecule
single bonds
Cl Cl
Cl C Cl Cl C Cl
Cl Cl
Thursday, 22 April 2010
88. TRIPLE BONDS
When three pairs of electrons are shared, a triple bond is formed.
Example
Propyne, C3H4
H
H C C C H
H
THREE pairs are shared
Note
• Two atoms joined by a double bond are closer together than two atoms joined by a
single bond. The double bond is shorter and stronger but allows the molecule to be
more reactive because there are more electrons concentrated there.
• The same applies for a triple bond compared to a double bond.
Thursday, 22 April 2010
91. IONIC BONDING
Ionic bonds are formed between metal and non-metal ions.
The bond is based on the attraction between positively and
negatively charged ions. Ionic compounds are formed.
Cl- Na+ Cl- “Negative ions are
called anions”
Na+ Cl- Na+
“Positive ions are
Cl- Na+ Cl- called cations”
Note
• Because they are oppositely charged, Sodium and Chloride ions are attracted to
each other.
• This attraction extends in 3 dimensions and results in a huge cubic arrangement
of ions. This arrangement is called a lattice.
Thursday, 22 April 2010
100. THE PERIODIC TABLE
(numbers given to columns)
3 4
(numbers given to rows) Key: show relative atomic size.
Size increases across a row &
decreases down a column.
Note
• There are columns of less reactive metals (transition elements)
between groups 2 and 13
• The dotted line separates metals from non-metals
Thursday, 22 April 2010
101. REACTIVITY OF METALS
The reactivity of a metal is a measure of the metal’s ability to participate in a
chemical reaction.
Metals react when their atoms lose their valence electrons. The easier the electrons
are lost, the more reactive they will be.
Decreasing reactivity
As we move down As we move across a
the group the Li Be period (left to
valence electrons get Lithium Beryllium right),the positive
Increasing reactivity
further from the 2.1 2.2 nucleus increases in
nucleus so they charge so the
become easier to attractive force on
remove.
Na Mg Al the valence electrons
Sodium Magnesium Aluminium increases. Valence
2.8.1 2.8.2 2.8.3 electrons become
Highly more difficult to
reactive
Ca remove.
K
Potassium Calcium
2.8.8.1 2.8.8.2
Thursday, 22 April 2010
102. REACTIVITY OF NON-METALS
The reactivity trends of non-metals can be explained by the ease with which
they can gain electrons to form ions.
As we move across a period (left to right),the
size of the atom decreases so the attractive
force on valence electrons increases.
Electrons are gained more easily.
He
Increasing reactivity Helium
2
Highly
B C N O Ne
Decreasing reactivity
reactive
Boron Carbon Nitrogen Oxygen
F Neon
Fluorine
2.3 2.4 2.5 2.6 2.7 2.8
Si P S Cl Ar
Silicon Phosphorus Sulphur Chlorine Argon
2.8.4 2.8.5 2.8.6 2.8.7 2.8.8
As we move down the group the atoms increase
in size as the number of energy levels increases.
It becomes more difficult to gain electrons.
Thursday, 22 April 2010
104. Ionic vs covalent FORMULAE Comparing & contrasting
Examples: Sodium Chloride, NaCl and Carbon dioxide, CO2
O C O
Cl- Na+ Cl-
• a molecule - a small particle
Na+ Cl- Na+ • a group of atoms joined.
2 atoms of oxygen joined to 1
atom of carbon
Cl- Na+ Cl-
O C O
• a lattice (a huge group of
positive and negative ions joined
to each other in an organised
The formula for an ionic compound
way)
has quite a different meaning to the
• Sodium and chloride ions are formula for a covalently bonded
present in a 1:1 ratio compound.
Thursday, 22 April 2010
105. Ionic vs covalent PHYSICAL PROPERTIES Comparing & contrasting
Properties Sodium Chloride Carbon dioxide
White solid at room
State Colourless gas
temperature
Melting point high low
Solubility in water High low
None when solid but
conducts well when in
Electrical conductivity None
the molten state or
when in solution
Thursday, 22 April 2010
107. Ionic vs covalent PHYSICAL PROPERTIES AND STRUCTURE Comparing &
contrasting
Ionic compounds are formed by the strong attraction between positive and
negative ions. This makes it difficult to separate the ions by heating the compound
so most ionic compounds are solid at room temperature.
Covalently bonded compounds usually have very weak forces of attraction
between molecules since each molecule is neutral. Separating the particles
(molecules) is easy. Most of them are already separated at room temperature
(making them solids or liquids).
Note - it is possible to have molecules that are ions - dealt with later
Solubility requires water molecules to surround each particle of a compound. Water
molecules have a positive end and a negative end. The water molecule’s negative end
will be attracted to a positive ion and its positive end to a negative ion. Because
molecules are uncharged this attraction to water molecules does not take place.
An electric current is the flow of charged particles. Ionic solids contain charges that
can be free to move and so can conduct electricity. Covalently bonded compounds can
not because they consist of molecules that are neutral.
Thursday, 22 April 2010
145. 5. IDENTIFY COMPOUNDS
Term Definition Example
Elements have only one kind of atom.
have two or more types of
Compounds atom that are chemically
joined
have elements and/or “Remember
Mixtures compounds that are not this!!!”
chemically joined
Elements can exist as molecules. Molecules are groups of atoms that are joined
Examples
Oxygen, O2 Hydrogen, H2 Helium, He Chlorine, Cl2 Carbon, C
Elements
Water, H2O Hydrogen Chloride, HCl Carbon Dioxide, CO2
Compounds
Thursday, 22 April 2010
146. The following table is not correct UN-MIXING THE TABLE
Copy the following table but match the term with its correct diagram
A. mixture of 1.
(i) Hydrogen and
different
elements Oxygen
B. mixture of 2.
(ii) Water and
different
compounds Hydrogen Chloride
3.
C. mixture of an (iii) Oxygen and
element with
a compound water
The following word equations describe
Answers _____ ______ ______
chemical reactions. CIRCLE THE
_____ ______ ______ COMPOUNDS
_____ ______ ______ A chemical reaction is a non-reversible change
in which new substances are formed.
(a) Aluminium + Iodine ----> Aluminium Iodide
(b) Sulfur + Oxygen ------> Sulfur Dioxide
Thursday, 22 April 2010
147. Demo MAKING A COMPOUND
Iron heated with sulphur
test-tube
mixture of powdered
sulphur and iron
Bunsen burner (blue flame)
Appearance of the elements before heating:
Iron _______________________________________________________
Sulphur _______________________________________________________
Appearance of the compound formed after heating:
______________________________________________________________
Name of compound formed: _______________
Thursday, 22 April 2010
148. MAGNETIC PROPERTIES
1 2
Magnet
Sulphur
Iron filings
3
Observations:
___________________________________
___________________________________
___________________________________
Iron Sulphide
(the product) ___________________________________
___________________________________
___________________________________
___________________________________
Thursday, 22 April 2010
149. Drawing A CLOSER LOOK
P
U
R
E
Element Element Compound
N
O
T
P
U
R
E
Mixture Mixture
of elements of element with compound
Thursday, 22 April 2010
150. MIND MAP
All substances
.............. Not pure
...................
Elements ...................
Element
................ with Different
elements compound .................
Questions
1. Explain the difference between Co and CO
__________________________________________________________________
__________________________________________________________________
2. Explain the difference between O2 and 2O
__________________________________________________________________
__________________________________________________________________
Thursday, 22 April 2010
151. 6. EXPLAIN HOW MANY ATOMS ARE PRESENT IN THE
FORMULA OF A COMPOUND
Study the pictures below and copy and complete the sentences below:
Oxygen, O2
Oxygen is an element, it consists of two oxygen atoms
that are chemically joined.
Hydrogen Chloride, HCl Hydrogen Chloride is a compound. It exists as
molecules. The molecules are not joined to each other
and move around randomly. Each molecule consists of
one atom of hydrogen and one atom of Chlorine.
Water, H2O Water is a compound. It exists as molecules. The
molecules are not joined to each other and move
around randomly. Each molecule consists of one atom
of oxygen and two atoms of Hydrogen. Each molecule
is shaped like a “V”.
This information can be summarised in a table. Complete the table (below):
Name of the molecule Is it a compound Number of atoms
Thursday, 22 April 2010
152. Process for counting up atoms
1. Start inside the bracket.
2. Add up the numbers behind each symbol. No number counts as one atom.
3. Multiply this number by the number behind the bracket.
4. Add this to any other atoms in the formula.
5. Then multiply this total by the number in front of the formula.
1 EXAMPLE
2 Cu(OH)3
2
3
1 O and 1 H 4
x3 = 6
= 2 Atoms
= 7 5
1 Cu = 14
x2
OTHER EXAMPLES
How many atoms of each element are there in each of the following compounds:
KCl _____ KNO3 _____ Ca(OH)2 _____ AlPO4 _____
CuCO3 _____ CuSO4 _____ 2 Al2(SO4)3 _____ FeCl3 _____
Zn(NO3)2 _____ PbI2 _____ 3HNO3 _____ Na2CO3 _____
Thursday, 22 April 2010
153. COUNTING ATOMS Count the atoms in the
following formulae:
INSERT ANOTHER EXERCISE/PUZZLE
Thursday, 22 April 2010
154. EX
O ER
R CI
HW S
K ES
Thursday, 22 April 2010
156. PUT THOSE ELECTRONS IN THEIR PLACES
1. COMPLETE THE TABLE (BELOW) 2. Draw shell diagrams for the following atoms:
(i) Be (ii) F (iii) Ne (iv) Ar Use the
Metal atom Non-metal atom Use the spaces
spaces providedprovided
C: 2, 4 Cl: 2, 8, 7 (i) Be (ii)F
Mg: 2, 8, 2 N: 2, 5
Li: 2, 1 Ar: 2, 8, 8
Be: O:
Ca: S:
Al: F:
Na: P:
Si: B:
(iii) Ne (iv) Ar
Thursday, 22 April 2010
157. COMPOUND FRACTURE
For each of the following descriptions , write the word “mixture” or “compound” to
describe which category it fits into:
• Properties depend on the amount of each particle present ________________
• Consist of one type of particle only ________________
• Have a variable collection of elements ________________
• Have a fixed ratio of different elements ________________
• Consist of several different types of particle ________________
• Properties are always the same ________________
Each of the following is a compound made up of two elements combined. Starting at
sodium chloride, connect it to another compound that contains one of its elements.
Do the same for the second compound until you connect to lead sulfate.
Sodium Calcium Magnesium Aluminium
Chloride Sulfide Oxide Bromide
Magnesium Sodium Potassium
Iodide Fluoride Oxide
Calcium Potassium Aluminium Lead Sulfide
Bromide fluoride Iodide
Thursday, 22 April 2010
158. Complete the table:
Chemical formula Total number of atoms in each formula
Thursday, 22 April 2010
159. ELEMENT CUBES Each side of the cube:
1. Name & symbol of
Each student allocated a different element. Put into
letter box. Reallocate. element
Research -> element cube (book computers, 2. Uses of the element
finish for Hwk) 3. Classification (metal/non-metal)
4. Physical properties
(colour, s/l/g)
5. History - discovery
6. Extraction
138
Thursday, 22 April 2010
160. Name these scientists:
1. The Greek philosopher who first thought of the idea of atoms _________________
2. The English clergyman who thought atoms were like tiny billiard balls of different
sizes. ______________________________________
3. The English physicist who discovered the electron. ___________________
4. The New Zealander who discovered that the atoms have a nucleus surrounded by
electrons. ______________________________________
5. The English physicist who found that the atomic number is the same as the number
of protons _____________________________________
6. The English physicist the proof of existence of neutrons ______________________
Thursday, 22 April 2010
173. EXERCISES SEPARATION OF MIXTURES
Thursday, 22 April 2010
174. SEPARATING MIXTURES
A solution is made by mixing a solid and a liquid.
Initially:
Particles in the solid are ___________ around fixed positions with the liquid
particles moving about _____________ .
After a while:
_____________ forces between liquid particles and solid particles allow the
liquid particles to pull the solid particles away from their fixed positions
to __________ amongst the liquid ones. The solid particles in a solution are
very s _ _ _ _ .
A solution is a mixture of a solid in a liquid where the solid
particles are very small and are evenly spread amongst the
liquid particles.
Thursday, 22 April 2010
175. SEPARATING MIXTURES
A suspension is __________ from a solution because the solid particles in the
suspension are ________ and _________ to the bottom. Because the solid particles
are ________ it is not possible to _______ through a suspension.
Word List: settle, different, bigger, see
Examples of suspensions
in everyday life
Animation: (Filtration) http://www.bbc.co.uk/schools/ks3bitesize/science/chemistry/
elements_com_mix_8.shtml
Thursday, 22 April 2010
176. SEPARATING MIXTURES
Term Definition
A. solution 1. the substance that does the dissolving
B. solute 2. the substance that dissolves
3. a mixture of a solid with a liquid where the solid particles
do not spread evenly through the liquid but instead sink to
C. solvent
the
bottom.
4. a special mixture that looks and behaves like a single
D. suspension
substance
A _____ B _____ C _____ D _____
Thursday, 22 April 2010
177. SEPARATING MIXTURES
Word Meaning
Dilute
Concentrated
Solubility
Saturated
1. When sugar is mixed with water it ____________ . This shows the sugar is
____________ in water.
2. Sand is ______________ in water.
3. Salty water is a _____________, bud muddy water is not.
4. In salt water, the salt is the ____________, and the water is the ____________ .
5. The solute in a solution does not settle out, but the solid in a _______________
does.
6. A solution that can dissolve no more solute is ____________ .
7. Most solids are more ___________ in hot water than in __________ water.
Thursday, 22 April 2010
178. SEPARATING MIXTURES Lab 8
Filtration and decanting are used to make
milk glue
Decanting into a small beaker. Try not Filtering out the curds. The clear
to lose any of the curds. The small liquid (or filtrate) goes down the
beaker will ____________any that get sink. The __________ remains in
past the stirring rod. the filter paper.
Word list
Funnel Curds Beaker Filter paper catch residue Sink Stirring rod
Thursday, 22 April 2010
179. SEPARATING MIXTURES
• Evaporation occurs when a ______ changes into a ____. Word List
• Evaporation is a good way of separating a solution because cool
_____________________________________________________
gas
_____________________________________________________
• If you separate a solution but also want to keep the liquid then
condensation
you have to _____ it. This process is called ____________. liquid
• Condensation occurs when a _____ changes into a _______.
Example
Write a short paragraph to explain what is happening in the above example
_____________________________________________________________________
_____________________________________________________________________
_____________________________________________________________________
Thursday, 22 April 2010
180. SEPARATING MIXTURES
Word List
Solution _____________ distillate
(Ethanol vapour
and water)
condenser
boils
_____________ thermometer
liquid
_____________ round bottom flask
water
cooled
_____________
We were able to separate the ethanol from the water because the ethanol
_____________ at a lower temperature than the ________. The ethanol
_________ passes into the ____________ where it is ___________ to
become a __________ .
http://www.bbc.co.uk/schools/ks3bitesize/science/chemistry/elements_com_mix_8.shtml
Thursday, 22 April 2010
181. SEPARATING MIXTURES
Mixture Method of separation
Add _________. The soluble substance ____________ . The
____________ substance does not dissolve. Filtering the
Salt and sand mixture will collect the _____________ substance in the
filter paper. This is called the ____________ .
hold a magnet to the mixture. The _____________
Iron filings and
substance collects on the magnet. The other substance is left
sulphur
behind.
Add water. The sawdust __________. The sand _________.
You can scoop the sawdust off the top.
Sawdust and sand
Swirling the mixture in a shallow pan. The ___________
mud and sand fly out of the pan. The ______________ gold
Gold, mud and sand
gets left behind.
Word List: sinks heavier water dissolves insoluble lighter residue
magnetic floats
Thursday, 22 April 2010
182. CHEMICAL BINGO
From your periodic table of elements, choose any 14 symbols from the first 20 and fit them
into the unshaded squares. When the name of the element is called out cross it out using a
pen. When all the symbols have been crossed off, call “bingo”.
CHEMICAL BINGO
From your periodic table of elements, choose any 14 symbols from the first 20 and fit them
into the unshaded squares. When the name of the element is called out cross it out using a
pen. When all the symbols have been crossed off, call “bingo”.
Thursday, 22 April 2010
183. QUICK QUESTIONS
1. What is the name of the particle that cannot easily be made smaller?
2. Name 2 objects in the room that contain carbon.
3. Air is made up mainly of which element?
4. Explain the difference between an element and a compound.
5. Name one particle that can be found inside the nucleus of the atom. (Challenge!)
Thursday, 22 April 2010
184. THE TE PUKE KID
The Te Puke kid mounted his trusty steed, old (Au) ________. He strapped
his shooting (Fe) __________ to his side and headed out from the bright
(Ne) _________ lights. He was determined to rob the stage of its precious (U)
_________ load. He inhaled a deep breath of (O) ___________ and coughed on the
(S) ____________ from the nearby factories. It really was hot, the (Hg)
___________ was rising. He took a drink of (H2O) __________ and spat as he tasted
the (Cl) ___________ .
He rode north, his bones aching from (Ca) __________ deposits built up from years
of riding the (Zn) trail. Overhead he saw the stage coach. It was guarded by an old
sheriff with a (Sn) ___________ badge. “Stop”, the kid yelled, “or I’ll fill you full of
(Pb) _________.” The sheriff went for his gun but was too slow. Kid’s gun blazed like
flaming (Mg) ________________ and the (Cu) ____________ fell to the ground.
Anyone who drew on the kid should have known that his life was not worth a plugged
(Ni) ____________ . A pretty (Pt) ________________ blonde on the stage screamed
as the Kid pulled out some (N) _____________ compounds to blow the strongbox.
Suddenly a shout rang out. “Hi Ho (Ag) ____________” . A masked man on a white
horse raced across the (Si) _______________ sands like (Na) ___________
skittering on water. There’s a (Rn) __________, “ he cried. The Kid was captured and
was put behind (Co) ______________ steel bars.
Don’t let you life be a (C) ______________ of the Kid’s. Learn your Chemistry!!
Thursday, 22 April 2010
185. QUICK TEST - 1 Name _________________
1. What is the name of the particle that cannot easily be made smaller?
_____________________
2. Name 2 objects in the room that contain carbon. ________ , __________
3. Air is made up mainly of which element? _________
4. Explain the difference between an element and a compound.
________________________________________________
________________________________________________
5. Write the symbols for the following elements:
(a) Lithium ____ (b) Boron ____ (c) Fluorine ____ (d) Argon (e) Silicon ____
(f) Phosphorus _____ (g) Chlorine ____
(h) Sodium _____ (i) Potassium ____
6. Name the following elements:
(a) H __________(b) He __________ (c) Be __________
(d) C __________ (e) N __________ (f) O __________
(g) Ne __________ (h) Mg __________ (i) Al __________
(j) S __________(k) Ca __________
Thursday, 22 April 2010
186. QUICK QUESTIONS
Test yourself by copying and answering the FIRST FIVE QUESTIONS into the back
of your book
1. Explain why elements are like the letters of the alphabet.
2. Elements are made up of only ......... ............. .... ........... .
3. A compound (like an element) is a ............ substance but a compound will
contain ...(several words)....... which are
............... .
4. What is the main difference between a compound and a
mixture.
5. Explain why air is a mixture of elements and compounds.
Explain the following statement: “The nucleus is like
a flea in the Yankee Stadium”
Thursday, 22 April 2010
187. THE LANGUAGE OF THE PERIODIC TABLE
The atomic number
The atomic number of an atom is the number of ..................
in the ..................... of that atom.
An atom of the same element will always have the same
................. number.
The number of electrons
Because protons are positively charged and electrons are
negatively charged and an atom is electrically neutral then
the number of electrons surrounding an atom is always be ............. ..... the
number of protons in the nucleus.
The mass number
The mass number is equal to the number of .................. plus
the number of ..................... .
Thursday, 22 April 2010
188. TE
M AC
AT H
ER ER
IA
L
Thursday, 22 April 2010
189. Material World (level 5)
• Properties of Materials MW props: Investigate the physical and chemical properties of different groups of substances.
For example acids and bases, fuels and metals. Distinguish between pure substances and mixtures and between
elements and compounds.
• Structure of matter MW struct: Describe the structure of the atoms of different elements. Distinguish between an
element and a compound, a pure substance and a mixture at particle level.
• Chemistry and society MW soc: Link the properties of different groups of substances to the way they are used in
society or occur in nature.
SCHEME
Thursday, 22 April 2010
190. BC HISTORY OF THE ATOM As you watch the video (22 min) complete the
following timeline with the exact year, name of the
person with the idea and the explanation of the theory
Name Explanation
400 Ancient babylon - Gold from other elements (Zinc & Copper = Bronze ...)
Ancient Greece - (5th Cent BC) Alchemy - All matter = “Fire, water, air & earth”
384-322 Aristotle - “Atomless view”
Empedocles & Leucippus - believed in atoms
342
300 Epicurus - also believed in atoms, “ God is the prime mover”
270
200
100
95 Leucretius - “Romans didn’t care” about science (Alchemy) = The Dark Age of Alchemy
0
Thursday, 22 April 2010
191. 0
AD
500
1000
1500
1641 Pierre Gassandi - “Atoms exist but they are God’s building blocks
1661 Boyle & Newton - Gases are particles that move --> Pressure
1774 Joseph Priestly - “When things burn they lose mass”
Lavoisier - Discovered air. Metals take up Oxygen when burnt -> an increase in mass (Mercury)
1803 Dalton - Elements exist as atoms. Different atoms => different atomic weights. Combinations in
different ratios. In 1808 “Atomic theory” was published by Dalton. No alchemy & no
2000 atomic conversions
Thursday, 22 April 2010