chemistry 2 lesson 3.1 mass number aqa additional science
TRANSCRIPT
Aims
Class work 6 September 2007
Mass NumberLO’s• What is the mass number?• What’s an isotope?
Write it down!! Page 50© C Meyer
Chemistry Unit 2 Sections
Structures Structures and bonding and properties How
much? 3 of 7
© C Meyer
All• Know the relative masses of sub
atomic particles• Know what an isotope isMost• Work out the mass number of an
atomSome• Explain how isotopes are different
Aims
T/F Quiz – Back• Atoms are charged particles• Electrons are found in energy levels• Electrons are found in shells• Electrons have a negative charge• Protons are in the nucleus of the atom• Neutrons are found in shells around the
nucleus• The atomic number is the number of
protons
What have I learnt?
• What does the structure of the atom look like?What have I learnt?
• There are two properties of sub-atomic particles that are especially important:– Electrical charge (looked at before)– Mass (Need to look at now)
• Mass of proton = mass of neutron (relative mass = 1)• Ignore mass of electron
m5
ParticleParticle ChargeCharge Relative MassRelative Mass
Protons +1 1
Neutrons 0 1
Electrons -1 0.0005
ChargeChargeParticleParticle
-1Electrons
0Neutrons
+1Protons
Overall neutral
Atomic/Proton Number• The atom of any particular element
alwaysalways contains the same number of protons. E.g.– Hydrogen atoms always contain 1 proton– Carbon atoms always contain 6 protons– Magnesium atoms always contain 12 protons
• The number of protons in an atom is known as its atomic/proton number.
• It is the smaller of two numbers shown in most periodic tables
12
C6
What have I learnt?
How Many Protons?
• Here is some data about elements taken from the Periodic Table.
• What is the atomic number of the elements?
23
Na11
56
Fe26
119
Sn50
19
F9
27
Al13
11 26 50 9 13
Activity
How Many Protons?
• NoteNote elements have a definite and elements have a definite and fixed number of protons.fixed number of protons.
• Changing number of protons in atom changes that atom into a different element.
What have I learnt?
Mass Number – What is it?
• The mass of each atom comes almost entirely from the number of protons and neutrons that are present. (Remember that electrons have a relatively tiny mass).
Atom Protons Neutrons Mass NumberHydrogen 1 0 1
Lithium 3 4 7
Aluminium 13 14 27
MASS NUMBER = Number of protons + number of neutrons
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What is the mass number?
• In back - Calculate the mass number of the atoms shown.
Atom Protons Neutrons Mass Number
Helium 2 2
Copper 29 35
Cobalt 27 32
Iodine 53 74
Germanium 32 41
4
64
59
127
73
MASS NUMBER = Number of protons + number of neutrons
Activity
What is the mass number?
• Atomic/proton number = protons.• It is the smaller of two numbers
shown in periodic table
12
C6
What is the mass number?
• Mass number = protons + neutrons• It is the bigger of two numbers shown
in periodic table
m1
• In back - Calculate the number of neutrons in these atoms.
Atom Mass Number
Atomic Number
Number of Neutrons
Helium 4 2
Fluorine 19 9
Strontium 88 38
Zirconium 91 40
Uranium 238 92
Number of Neutrons = mass number - atomic number
2
10
50
51
146
Activity
What is the mass number?
• In Front - Copy and fill in the blank columns
Atom Protons Neutrons Electrons Atomic number
Mass Number
Boron 5 6
Potassium 19 20
Chromium 24 28
Mercury 80 121
Argon 18 22
5 5 11
19 19 39
24 24 52
80 80 201
18 18 40
Note – atomic number is defined as the number of protons rather than electrons because atoms can lose (or gain)
electrons but do not normally lose protons
Activity What have I learnt?
• Natural samples of elements are often a mixture of isotopes. About 1% of natural carbon is carbon-13.
ProtonsElectronsNeutrons
C12
699% C
13
61%
6
6
6
6
6
7
What’s an isotope?
What’s the difference?
m1
ATOMS are just like the Ford Fiesta
ISOTOPEISOTOPE
What is relative mass?
m2
Version1
Version 2
There are different versions of the FIESTA
Version 3
SPEEDYSPEEDY
m3
We also have different versions of the same
element’s atoms
WE CALL THEM
ISOTOPESISOTOPESm1
The only difference between the atoms in an
isotope is that they contain
different numbers of
NEUTRONNEUTRONSS
• It is not strictly true to say that elements consist of one type of atom.
Remember: The number of protons defines
the element
What’s an isotope?
•Atoms in an element always have the same
number of protons but may have different
numbers of neutrons.
•Atoms like this are called isotopes.isotopes.
Isotopes: Hydrogen• Hydrogen exists as 3 isotopes although
Hydrogen-1 makes up the vast majority of the naturally occurring element.
H1
1 H2
1 H31
ProtonsElectronsNeutrons
Hydrogen
ProtonsElectronsNeutrons
(Deuterium)
ProtonsElectronsNeutrons
(Tritium)
All can make water
m4
Isotopes: Chlorine• About 75% of natural chlorine is 35Cl the rest is 37Cl.
Cl35
1775%
17ProtonsElectronsNeutrons
17
18ProtonsElectronsNeutrons
171720
Cl37
1725%
How manyneutrons?
Isotopes of Oxygen
• Almost all of natural oxygen is 16O but about 0.2% is 18O.
• Produce a Table showing the particles in each isotope.
Protons
Electrons
Neutrons
16
O8
Oxygen-18Oxygen-16
8
8
8
Protons
Electrons
Neutrons
8
8
10
Activity
• Isotopes are virtually identical in their chemical reactions as have same number of protons and electrons.
• The uncharged neutrons only affect physical properties such as melting point and density.
What’s an isotope?
• Draw the electronic structure of carbon 12 and carbon 14
• Say how many protons, neutron• Draw up a table of similar
properties and differences
What have I learnt?
Same Different
What have I learnt?
C126
99% C13
61%
ProtonsElectronsNeutrons
6
6
7
6
6
6
Same Different
Same number electrons Different number neutrons
Same number protons Different mass number
Same chemical properties Different physical props
Same proton number
• Section 2 test
Homework
What have I learnt?
The End