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8/12/2019 Theory of particle matter & changes in state of matter
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BASICCHEMISTRY
CHAPTER 1:
THEORY OF
PARTICLES &
MATTER
CHAPTER 2:
CHANGES IN
STATE OF
PARTICLES
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MatterMade up of tiny &discrete particles
AtomThe smallest particleof an element thatcan participate in achemical reaction.
MoleculeA group of 2/> atomswhich are chemically
bonded together.
ElementA substance made
only of identicalatoms.
CompoundA substance made up of
2/> different atoms /ions.
IonA +ly charged / -ly
charged particles.
Matter:Anything thatoccupies space &has mass.
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1. 2.
3.
4.
5.
6.
7.
8.
9.
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Has a fixed volume.
Does not have a fixed shape but takes the shape of the
container.
Cannot be compressed easily.
Particles are packed closely together but not in an
orderly manner.
Particles are held together by strong forces butweaker than the forces in a solid.
Particles can vibrate, rotate & move throughout the
liquid. They collide against each other.
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Does not have a fixed shape or volume.
Can be compressed easily.
Particles are very far apart from each other and ina random motion.
Weak forces between the particles.
Particles can vibrate, rotate & move freely. The
rate of collision in gas is greater than liquid.
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4. Solid Liquid: Heat energy is absorbed.
5. Liquid Gas: Heat energy is absorbed.
6. Solid Gas: Heat energy is absorbed.
7. Gas Solid: Heat energy is given out.
8. Gas Liquid: Heat energy is given out.
9. Liquid Solid: Heat energy is given out.
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Temperature (C)
Time (min)
1
2 3
4 5
6Gas particlesabsorbs more
energy & movefaster
Liquid boiling: heatenergy is absorbed
Liquid particlesmove faster
Solid melting:particles absorb
heat energy
Solid particles absorbenergy & vibrate faster,kinetic energy increases.
m.p
b.p
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Exists in solid state.
Temperature below its melting point.
The particles are very closely packed togetherand can only vibrate.
1.
1. 2.
Particles absorb more energy and vibrate faster.
Temperature & kinetic energy increases.
2.
Exists in solid state.Heat energy absorbed by the particles is enough to
overcome the forces of attraction between them.
Solid begins to melt & changes into liquid.
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Exists in both solid and liquid state.
Temperature remain unchanged; the constant
temperature is the melting point. Energy absorbed is used to overcome the forces of
attraction between the particles.
2.
3.
Exists in liquid state.
The melting process ends.
3.
Exists in liquid state.
Temperature & kinetic energy increases.
The particles move faster.
3.
4.
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Exists in liquid state.
Heat energy absorbed by the particles is enough
to overcome the forces of attraction between them.Liquid begins to change into gas.
4.
4. 5.
Exists in both liquid and gaseous state.
Temperature remains unchanged; the constanttemperature is the boiling point.
Energy absorbed is used to overcome the forcesof attraction between the particles.
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Exists in gaseous state.
5.
5. 6.
The gas particles continue to absorb more energy
& move faster.Temperature increases as heating continues.
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Temperature (C)
Time (min)
1
2 3
4 5
6
Solid cooling
Liquid cooling:
particles losingkinetic energy
Gas condensing:Particles movingcloser
Gas cooling:particles losingkinetic energy
Liquid freezing: particlesmoving closer
m.p
b.p
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Exists in gaseous state.
The particles have very high energy and move
randomly The forces of attraction between the particles are very
weak
1.
1. 2.
Exists in gaseous state.
Particles lose kinetics energy.
Temperature decrease.
2.
Exists in gaseous state.
Stronger forces of attraction formed.
Gas begins to condense and changes into liquid.
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Exists in both gaseous and liquid state.
Temperature remain unchanged; the constant
temperature is the boiling point.Energy produced during the formation of forces
of attraction is equal to the heat energy releasedto the surroundings during cooling.
2.
3.
Exists in liquid state.
All the gas particles have condensed into liquid.
3.
Exists in liquid state.
Temperature decreases.
The particles lose more kinetic energy and move
slower.
3.
4.
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Exists in liquid state.
The particles have very little energy and begin to
move closer towards one another.Liquid begins to freeze into solid.
4.
4. 5.
Exists in both liquid and solid state.
Temperature remains unchanged; the constanttemperature is the freezing point.
Stronger forces of attraction formed duringfreezing releases energy. The energy released isthe same as the energy lost to the surroundingd.
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All the liquid freezes into solid.
The particles are closely packed in an orderly
manner.
5.
5. 6.
Exists as a solid.Temperature decreases as cooling continues.
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HISTORY
1. JohnDalton
2. J.JThomson
3. ErnestRutherford
4. NeilsBohr
5. JamesChadwick
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Atom is imagined as a small, indivisiblesimilar to a very tiny ball.
1. JohnDalton
Atom is described as a sphere of + chargewhich contains a few -ly charged particlescalled electrons.
2. J.JThomson
+ charge (proton) & most of the mass of theatom are concentrated in a small, centralregion called nucleus. Electrons moves inspherical space outside the nucleus.
3. ErnestRutherford
Electrons in an atom move in shells aroundthe nucleus.4. NeilsBohr
Neutrons contributes approximately to half
the mass of an atom.
5. James
Chadwick
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Nucleus
Proton
- symbol: p
- Relative charge: +1
- Relative mass: 1
Neutron
- symbol: n
- Relative charge: 0
- Relative mass: 1
Electron- symbol: e
- Relative charge: -1- Relative mass: approximately 0.0005
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Atoms of same element with same number of proton butdifferent number of neutrons.
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USES
Cobalt-60
Treatment ofcancer.
-Cobalt-60
Destroybacteria infood.
Carbon-14
Estimate theage of fossil &
artefacts
Phosphorus-32
In fertilizer tostudy the
metabolism ofP in plants
Sodium-24
Detect leaks inpipes carryinggas.
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Nucleus
1stshell = 2 electrons
2ndshell = 8 electrons
3rd shell = 8 electrons
Electron
Valence Electron
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