1 salt crystals 6 helium (in a balloon) 2 feso 4.7h 2 o(s) 7 steel 3 aluminium foil 8 ice 4 hno 3...
TRANSCRIPT
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1 salt crystals 6 helium (in a balloon)
2 FeSO4.7H2O(s) 7 steel
3 aluminium foil 8 ice
4 HNO3(aq) 9 CH3COOH(l)
5 sodium carbonate solution 10 Br2(l)
Mixtures Mixtures – two or more substances that are not – two or more substances that are not chemically combined with each other and can be chemically combined with each other and can be separated by physical means. separated by physical means. ElementsElements – simplest form of pure substance. They – simplest form of pure substance. They cannot be broken into anything else by physical or cannot be broken into anything else by physical or chemical means.chemical means.CompoundsCompounds – pure substances that are the unions of – pure substances that are the unions of two or more elements. They can be broken into simpler two or more elements. They can be broken into simpler substances by chemical meanssubstances by chemical means..Decide whether each of these substances is an element, a compound or a mixture.
Compound
Compound
Compound
Compound
Mixture
Mixture
Mixture
Element
Element
Element
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RevisionRevision
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HISTORY OF THE ATOMHISTORY OF THE ATOM
460 BC Democritus develops the idea of atoms
he pounded up materials in his pestle and
mortar until he had reduced them to
smaller and smaller particles which he
called
ATOMAATOMA
(greek for indivisible)
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HISTORY OF THE ATOMHISTORY OF THE ATOM
1808 John Dalton
suggested that all matter was made up of
tiny spheres that were able to bounce
around with perfect elasticity and called
them
ATOMSATOMS
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HISTORY OF THE ATOMHISTORY OF THE ATOM
1898 Joseph John Thompson
found that atoms could sometimes eject a
far smaller negative particle which he
called an
ELECTRONELECTRON
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HISTORY OF THE ATOMHISTORY OF THE ATOM
Thompson develops the idea that an atom was made up of
electrons scattered unevenly within an elastic sphere
surrounded by a soup of positive charge to balance the
electron's charge
1904
like plums surrounded by pudding.
PLUM PUDDING
MODEL
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HISTORY OF THE ATOMHISTORY OF THE ATOM
1910 Ernest Rutherford
oversaw Geiger and Marsden carrying out
his famous experiment.
they fired Helium nuclei at a piece of gold
foil which was only a few atoms thick.
they found that although most of them
passed through. About 1 in 10,000 hit
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HISTORY OF THE ATOMHISTORY OF THE ATOM
gold foil
helium nuclei
They found that while most of the helium nuclei passed
through the foil, a small number were deflected and, to
their surprise, some helium nuclei bounced straight back.
helium nuclei
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HISTORY OF THE ATOMHISTORY OF THE ATOM
Rutherford’s new evidence allowed him to propose a
more detailed model with a central nucleus.
He suggested that the positive charge was all in a
central nucleus. With this holding the electrons in place
by electrical attraction
However, this was not the end of the story.
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HISTORY OF THE ATOMHISTORY OF THE ATOM
1913 Niels Bohr
studied under Rutherford at the Victoria
University in Manchester.
Bohr refined Rutherford's idea by
adding that the electrons were in
orbits. Rather like planets orbiting the
sun. With each orbit only able to
contain a set number of electrons.
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Bohr’s Atom
electrons in orbits
nucleus
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HELIUM ATOM
+N
N
+-
-
proton
electron
neutron
Shell
What do these particles consist of?
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ATOMIC STRUCTUREATOMIC STRUCTURE
Particle
proton
neutron
electron
Charge
+ ve charge
-ve charge
No charge
1
1
nil
Mass
Nucleus
NucleusAround
outside
Location
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ATOMIC STRUCTUREATOMIC STRUCTURE
the number of protons in an atom
the number of protons and neutrons in an atom
HeHe22
44 Atomic mass
Atomic number
number of electrons = number of protons
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ATOMIC STRUCTUREATOMIC STRUCTURE
Electrons are arranged in Energy Levels
or Shells around the nucleus of an atom.
• first shell a maximum of 2 electrons
• second shell a maximum of 8
electrons
• third shell a maximum of 8
electrons
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ATOMIC STRUCTUREATOMIC STRUCTURE
There are two ways to represent the atomic
structure of an element or compound;
1. Electronic Configuration
2. Dot & Cross Diagrams
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ELECTRONIC CONFIGURATIONELECTRONIC CONFIGURATION
With electronic configuration elements are
represented numerically by the number of
electrons in their shells and number of shells. For
example;
N
Nitrogen
7
14
2 in 1st shell
5 in 2nd shell
configuration = 2 , 5
2 + 5 = 7
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ELECTRONIC CONFIGURATIONELECTRONIC CONFIGURATION
Write the electronic configuration for the following elements;
Ca O
Cl Si
Na20
40
11
23
8
17
16
35
14
28B
11
5
a) b) c)
d) e) f)
2,8,8,2 2,8,1
2,8,7 2,8,4 2,3
2,6
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DOT & CROSS DIAGRAMSDOT & CROSS DIAGRAMS
With Dot & Cross diagrams elements and
compounds are represented by Dots or Crosses to
show electrons, and circles to show the shells. For
example;
Nitrogen N XX X
X
XX
X
N7
14
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DOT & CROSS DIAGRAMSDOT & CROSS DIAGRAMS
Draw the Dot & Cross diagrams for the following elements;
O Cl8 17
16 35a) b)
O
X
XX
X
X
X
X
X
Cl
X
X
X
X X
X
XX
X
X
X
X
X
XX
X
X
X
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SUMMARYSUMMARY
1. The Atomic Number of an atom = number of
protons in the nucleus.
2. The Atomic Mass of an atom = number of
Protons + Neutrons in the nucleus.
3. The number of Protons = Number of Electrons.
4. Electrons orbit the nucleus in shells.
5. Each shell can only carry a set number of electrons.
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1. An atom’s electron arrangement is also known as its electron ___.2. A __ is composed of two or more atoms, joined together by covalent
bonds.3. Almost all the volume occupied by an atom is ___ space.4. The total number of protons and neutrons in an atom is known as its
___ number.5. At the centre of an atom is a very ___, very dense, positively-charged
nucleus.6. The particle with no charge inside atoms is called the ___.7. The positively-charged particles inside atoms are called ___.8. Ions with a positive charge have ___ electrons.9. Positively-charged ___ particles were used to discover the structure
of the atom.10. To calculate the number of neutrons, ___ atomic number from mass
number.
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1 configuration 6 neutron2 molecule 7 protons3 empty 8 lost4 mass 9 alpha
5 small 10 subtract