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8/3/2019 Practise Ch2 Matter
http://slidepdf.com/reader/full/practise-ch2-matter 1/8
Chapter 2 : The Structure of the Atom
A Matter
1. Matter is anything that occupies space and has mass. Matter exists in three states – solid, liquid
and gas.
2. Matter is made up of tiny and discrete particles.
3. An atom is the smallest particle of an element that can participate in a chemical reaction.
4. An ion is a positively-charged or negatively-charged particle.
5. Particles in matter are in motion.
6. Diffusion occurs when particles of a substance move in between the particles of another subtance.
7. Diffusion of matter occurs most rapidly in gases, slower in liquids and slowest in solids, due to thedifferent arrangement and movement of particles in the three states of matter.
The kinetic theory of matter.
(diagram)
i) The change in heat changes the state of matter.
ii) When a substance is heated, the particles gain kinetic energy and move faster.iii) When a substance is cooled, the particles loss their kinetic energy and move slower.
State of Matter
Characteristic
Solid liquid gas
Arrangement of particles are packed closelytogether in an orderly
manner
are packed closelytogether but not in
orderly manner
Very far apart and in arandom motion
Forces of attraction Strong forces Strong forces but
weaker than the forces
in a solid
Weak forces
Movement of particles Particles vibrate and
rotate about their
fixed positon
Particles vibrate,
rotate and move
throughout the liquid.
They collide against
each other
Particles vibrate,
rotate and move
freely. The rate of
collision is greater
than in liquid
Shape / volume - has a fixed volume
and shape
- has a fixed volume
and follows the shape
of the container
Does not have a fixed
shape of volume
compressibility Cannot be compressed Cannot be compressed
easily
Can be compressed
easily
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Do it yourself 2.1
1.Figure 1 below shows the heating curve of a pure substance at room temperature and pressure.
Temperature/oC U
S T
119 Q R
P
Time / minute
Figure 1
(a)Describe the movement of the particles of the pure substance at stage PQ of the curve ?
(b)Draw a diagram to show the arrangement of particles of the substance at stage QR in the box below.
(c)Explain why the pure substance is not water ?
(d)Samples of the pure substance at stage RS and TU are taken. Compare the movement of the particles
of the substance at these two stages.
(e)After heating at 500oC, the substance is cooled. Draw and label the cooling curve.
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2. P Q
U T S R
(a)Name the process in
P: Q :
R: S :
T: U :
(b)What will occur if matter undergoes a change of state ?.
(c)Compare the intermolecular distance and the packing of particles in the solid state and the liquid state.
Ice water Salt solution
water steam salt water
Applyheat Apply
heat
Saturate it thencool the solution
Boil it, then coolthe vapour
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B The Atomic Structure
The historical development of atomic models.
Scientist Atomic Models
1. John Dalton
- imagined the atom as a small indivisible ball similar to a very tiny ball
2.J.J. Thomson
- described the atom as a sphere of positive charge which contains a few
negatively-charged particles called electrons.
3. Ernest Rutherford
discovered proton
the positive charge and most of the mass of the atom are concentrated in a
small, central region called the nuclues
electrons move in a space that is larger than the space occupied by the nucleus
4.Neils Bohr
proposed that the electrons in an atom move in shells around the nucleus
5.James Chadwick
proved the existence of neutrons, the neutral particles in the nucleus. Neutronscontribute approximately to half the mass of an atom.
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Protons, neutrons and electrons are subatomic particles of an atom.
i) At
om
s
are
electrically neutral.
ii) The number of protons is equal to the number of electrons.
iii) The proton number of an element is the number of protons in its atom.
iv) The nucleon number of an element is the total number of protons and neutrons in its atom.
Therefore,
v) Each element has its own proton number.
vi) Each element is given a name and a symbol
Proton
number
Element symbol Proton
number
Element symbol
1 Hydrogen H 11 Sodium Na
2 Helium He 12 Magnesium Mg
3 Lithium Li 13 Aluminium Al
4 Beryllium Be 14 Silicon Si
5 Boron B 15 Phosphorus P
6 Carbon C 16 Sulphur S
7 Nitrogen N 17 Chlorine Cl
8 Oxygen O 18 Argon Ar
9 Flourine F 19 Potassium K
10 Neon Ne 20 Calcium Ca
An atom of an element can be written as A
X
Z
Where A is the nucleon number,
X is the symbol of an element,Z is the proton number.
Subatomic
particle
Symbol Relative
mass
Charge Location
Proton p 1 +1 In the nucleus
Electron e 1/1840 -1In orbits around
the nucleus
Neutron n 1 0 In the nucleus
Nucleon number = proton number + number of neutrons
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Do it yourself 2.2
Complete the table below.
Complete the table below
Element
(symbol)
number of protons Number of neutrons Symbol of atoms
Lithium
(Li)
Neon
(Ne)
Zinc
(Zn)
Symbol of atom
27
Al
13
19
F
7
23
Na
11Proton number
Nucleon number
Number of protons
Number of electrons
Number of neutrons
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2.3 Isotopes and Their Importance
1. The isotopes of an element are the atoms of that element which contain a same
number of protons, but a different number of neutrons.
2. Isotopes of some element
Element Isotopes
Hydrogen H1
1
1 proton0 neutron
H2
1
1 proton1 neutron
H3
1
1 proton2 neutrons
Carbon C12
6
6 protons6 neutrons
C13
6
6 protons7 neutrons
C14
6
6 protons8 neutrons
Oxygen O16
8
8 protons8 neutrons
O17
8
8 protons9 neutrons
O18
8
8 protons10 neutrons
Sulphur S32
16
16 protons16 neutrons
S34
16
16 protons18 neutrons
-
Bromine r B79
35
35 protons44neutrons
r B81
35
35 protons46 neutrons
-
3. The uses of isotopes in daily life
Field Isotopes applications
Medical • Gamma rays from cobalt- 60 are used to killcancer cell without surgery in patient. Thistreatment is known as radiotherapy.
• Medical instrument are sterilized using gammarays.
• Radioactive materials such as iodide-131 areinjected into patients to detect malfunction of thyroid glands.
Archeology • Radioisotope carbon -14 is used to study theage of ancient artifacts.
Agricultural
• Carbon -14 is used to study the passage of
carbon in photosynthesis of green plants.
Industrial • Isotope sodium-24 is used to detect leakage of underground pipes.
SPM
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4. The electron arrangement of elements with proton number 1 to 20.
( must know how to memorize)
2.4 Electron Arrangements / Electron Structures
Element Number of neutrons
Number of protons
Number of electrons
Number of nucleon
Electronarrangement
Number of valence
electrons
Hydrogen
Helium
Lithium
Beryllium
Boron
Carbon
NitrogenOxygen
Fluorine
Neon
Sodium
Magnesium
Aluminum
Silicon
Phosphorus
Sulphur
Chlorine
Argon
Potassium
Calcium
First shell: 2 electrons
Second shell: 8 electrons
Third shell: 8 electrons
Nucleus ( contains protons and nucleus)
Last electron/s in the last outermost shell, we
called as valence electron.