Chemistry: Chapter 7 - Writing Equations

7.1 Chemical Equations
Word Equation: Everything in full English.

Chemical Equations: Symbols of elements.

7.2 Ionic Equations
Ionic Equations: Symbols of elements, charge of element and state of elements.

Spectator ions are not to be included in the ionic equations.
Spectator ions are ions still in solution at the end of the reaction.

Chemistry: Chapter 9 - Chemical Calculations

9.1 Calculations from Chemical Reactions
A balanced chemical equation shows the important facts about a reaction:

• The reactants
• The products
• The ration of the amounts (in moles) of the reactants and the products
• The state of the reactants and products indicated.

The relationship between the amounts of reactants and products involved in a chemical equation is know as the stoichiometry of the reaction.

9.2 The Volumes of Reacting Gases
Volume of a gas is proportional to the number of moles of the gas, and vice versa.

9.3 Limiting Reactants
The reactant that is completely used up in a reaction is known as the limiting reactant.
The reactants that are not used up are called the excess reactants.

9.4 The Concentration of a Solution
The concentration of a solution is given by the amount of a solute dissolved in a unit volume of a solution.
Concentration (g/dm³) = Mass of Solute in Grams / Volume of Solution in dm³

Molar Concentration
Concentration (mol/dm³) = number of moles of solute / volume of solution in dm³

Concentration (mol/dm³) = concentration (g/dm³) / Molecular mass of solute

9.5 Volumetric Analysis
Volumetric analysis is a technique used to determine the volumes of solutions that react together. In volumetric analysis, titration is performed to get the results.

Chemistry: Chapter 6 - Chemical Bonding

6.1 The Stable Noble Gas Structure
Atoms of noble gases are usually unreactive or stable.
An atom is stable if it has a duplet or octet configuration.

6.2 Forming Ions
An ion is a charged particle formed from an atom or a group of atoms by the loss or gain of electrons.

Metals form positively charged ions (cations) whereas non-metals form negatively charged ions (anions).

Metals give electrons and non-metals take electrons.

6.3 Ionic Bond : Transferring Electrons
When metals react with non-metals, an ionic compound is formed.

Positive ions and negative ions are attracted to one another by electrostatic attraction.

An ionic bond may also be known as an electrovalent bond.
Compounds that has ionic bonds are called ionic compounds.

Structure of Ionic Compounds
Ionic compounds are arranged in a giant lattice structure or crystal lattice.


Physical Properties of Ionic Compounds

1. Ionic compounds have high melting and high boiling points. (Non-volatile substances)
2. Ionic compounds are soluble in water but not in oil.
3. Ionic compounds do not conduct electricity in the solid state but in the molten state as there are free-moving ions that conduct electricity.

6.4 Covalent Bond: Sharing Electrons
When non-metals react with non-metals, an covalent bond is formed.

Structure of Covalent Bond Compounds



Physical Properties of Covalent Substances

1. Covalent compounds have low melting and low boiling points.
   
2. Covalent compounds are soluble in oil but now in water.
3. Covalent compounds do not conduct electricity in any state.

*Ionic compounds have electrostatic attraction. Covalent compounds have intermolecular forces.

Physics: Chapter 13 - Sound

13.2 Transmission of Sound
Sound waves need a medium in order to travel from one point to another.

13.3 Reflection of Sound
An echo is formed when a sound is reflected off hard, flat surfaces such as a large wall or a distant cliff.

Uses of echos
Use to detect the position of mines and submarines.

13.4 Pitch and Loudness
Pitch
Pitch is related to the frequency of a sound wave.
Sound with lower frequency has a lower pitch.
Sound with higher frequency has a higher pitch.

Loudness
Loudness is related to the amplitude of a sound.
The larger the amplitude, the louder the sound.
The shorter the amplitude, the softer the sound.

Physics: Chapter 12 - Electromagnetic Waves

12.1 Electromagnetic Waves
Ronald Mcdonald is very ugly X-cept Gary

Radio Waves - Longer wavelength Lower Frequency
Microwaves
Infrared
Visible light
Ultraviolet
X-rays

Gamma rays - Shorter wavelength High Frequency

Properties of electromagnetic waves

1. Electromagnetic waves are transverse waves.
2. They transfer energy from one place to another.
3. They can travel through vacuum. Do not require any medium to travel around.
4. They travel at a speed of 3.0 X 10⁸ ms^-1 in vacuum.
5. They obey the laws of reflection and refraction.
6. They carry no electric charge.
7. Their frequencies do not change when they travel from one medium to another. Only their speeds and wavelengths change from one medium to another.
   

12.3 Uses of Electromagnetic Waves
Application of elctromagnetic waves
Gamma Rays: Radiation therapy (Cancer treatment)
X-Rays: Medical and everyday application
Ultraviolet: Sunbeds and sterilisation of medical equipment
Visible light: Optical fibres
Infrared: Remote controllers and ear thermometers
Microwaves: Ovens and satellites
Radio waves: Radio and telecommunications

Effects of Electromagnetic Waves
Infrared heating - Skin absorbs infrared waves, making us feel warm.

Physics: Chapter 11 - Waves

11.1 Describing Waves
The source of a wave is vibration or oscillation.
Waves transfer energy from one point to another.
In waves, energy is transferred without the medium moving/ being transferred.

Transverse waves are waves that travel in a direction perpendicular to the direction of vibration of the particles.
Examples of transverse waves: Light waves

Longitudinal waves are waves that travel in a direction parallel to the direction of vibration of particles.

Examples of longitudinal waves: Sound waves.

11.2 Properties of Wave Motion


Crest and troughs: Highest and lowest points of a transverse waves.
Compression and rarefaction : Highest and lowest points of a longitudinal waves.

Phase: Points of a wave which move in the same direction, have the same speed and the same displacement from the original position.

Wavelength λ: Shortest distance between any two points in a wave that are in phase.
SI Unit: metre (m)

Amplitude A: Maximum distance from the rest position. It is the height of a crest or depth of a trough.
SI Unit: metre (m)


Period (T): Time taken for one point on the wave to complete one oscillation.
SI Unit: second (s)

Frequency (f): Number of complete waves produced per second.
SI Unit: Hertz (Hz)
f = 1/T

Wave speed (v): v = fλ
Wave speed = wavelength(period)
SI Unit: metre per second (m s^-1)

Wavefront: Imaginary line on a wave that joins all points that are in the same phase.

Physics: Chapter 9 - Thermal Properties of Matter

9.1 Temperature and Internal Energy
Internal energy is made up of kinetic energy and potential energy.

9.2 Melting and Solidification
Melting is the change of state from solid to liquid, without a change in temperature
During melting, the temperature remains constant at the melting point.
Thermal energy is absorbed by the substance.

Solidification is the change of state from liquid to solid, without a change in temperature.
During solidification, the temperature remains constant at the freezing point.
Thermal energy is released by the substance.

9.3 Boiling and Condensation
Boiling is the change of state from a liquid into vapour, occurring at a constant temperature called the boiling point.
During boiling, the temperature remains constant at its boiling point.
Thermal energy is being absorbed by the substance.

Condensation is the process whereby vapour changes into liquid at the same constant temperature. Heat is given out during condensation.
During condensation, the temperature remains constant at the condensation point. Thermal energy is released by the substance.

9.4 Evaporation
Factors affecting the rate of evaporation

1. Temperature
2. Humidity of the surrounding air
3. Surface area of the liquid
4. Movement of air
5. Pressure
6. Boiling point of the liquid

1. Temperature
Heating a liquid will increase the rate of evaporation because it means a greater number of molecules at the surface layer are energetic enough to escape.

2. Humidity of the surrounding air
Rate of evaporation decreases with increasing humidity (Water vapour present in the air).

3. Surface area of the liquid
Larger surface area = Increase in evaporation

4. Movement of air
Rate of evaporation increases when the surrounding air is moving.
Moving air removes the molecules of the liquid as soon as they escape from the surface of something.

5. Pressure
Reducing the atmospheric pressure increases the rate of evaporation.
Example: Things can dry faster on mountaintops than at sea level.

6. Boiling point of the liquid
Liquids with lower boiling point evaporates faster.

Physics: Chapter 8 - Transfer of Thermal Energy

8.1 Transfer of Thermal Energy
Thermal energy always flows from a region of higher temperature to a region of lower temperature.

8.2 Conduction
Conduction is the process of thermal energy transfer without the medium flowing.
Occurs mostly in solids, good conductor of heat.

Thermal energy is supplied to a material -> Particles at hot end vibrate vigorously -> Particles collide with neighbouring particles -> Kinetic energy is transferred to the neighbouring particles.
This happens because metals contain many free electrons which move randomly between the atoms or molecules.

8.3 Convection
Convection is the transfer of thermal energy by means of currents in a fluid or gases.

When water at the bottom of a container is heated, it expands -> Expanded water is less dense and start to ride -> Cooler regions of the water in the upper part on container became denser and sinks.

Convection currents occur only in fluids such as liquids and gas but not in solids.
Because convection involves the bulk movement of the fluids which carry thermal energy with them.

8.4 Radiation
Radiation is the continual emission of infrared waves from the surface of all bodies, transmitted without the aid of a medium.
The process in which energy is emitted as particles or waves.

Radiation can take place in a vacuum.

Factors affecting rate if infrared radiation

1. Colour and texture of the surface
2. Surface temperature
3. Surface area

Absorption = take in
Emission = give out

Best absorption and emission: dull black surface

Physics: Chapter 7 - Kinetic Model of Matter

Matter are tiny particles which are always in continuous, random motion.

Solid

• Closely packed atoms or molecules
• Strong intermolecular bonds
• Atoms or molecules vibrate about fixed positions.

Liquid

• Atoms or molecules occur in clusters
• Slightly further apart compared to solids
• Free to move about between clusters

Gas

• Atoms or molecules are very far apart
• Negligible attractive forces between atoms or molecules
• High speed, independent motion in random manner

Brownian motion
Gas particles move faster at higher temperature due to a increase of thermal energy which is converted to kinetic energy of the air molecules.

Physics: Chapter 6 - Energy, Work and Power

6.1 Energy
Energy is the capacity to do work.
SI Unit: joule (J)

Types of energy:

1. Kinetic Energy
   
2. Potential Energy (Chemical potential, elastic potential and gravitational potential)

1. Kinetic Energy
Moving objects have kinetic energy.

2a. Potential Energy - Chemical Potential Energy
Can be found in food, fossil fuels.

2b. Potential Energy - Elastic Potential Energy
A spring or rubber band possesses elastic potential energy when compressed or stretched.
When released, it is converted into kinetic energy.

2c. Potential Energy - Gravitational Potential Energy
The higher the object that leaves the ground, the greater the gravitational potential energy.

Principle of Conservation of Energy

Energy can neither be created nor destroyed in any process. It can be converted from one form to another or transferred from one body to another, but the total amount remains constant.

Conversion of energy
Efficiency = useful energy output divide energy input times 100%

6.2 Work

Work done by a constant force on an object is given by the product of the force and the distance moved by the object in the direction of the force.

W=F(s)
Work done by a constant force = constant force(distance moved by the object in the direction of the force)

One joule is defined as the work done by a force of one newton which moves an object through a distance of one metre in the direction of the force.

No work is done when:

1. The direction of the applied force and the direction in which the object moves are perpendicular to each other, and
2. The force is applied on the object but the object does not move.

Mechanical Energy

1. Kinetic energy and work done
2. Gravitational potential energy and work done

1. Kinetic energy and work done
Kinetic energy = 1/2(mass of body)(speed of body)²

2. Gravitational potential energy and work done
Ep = mgh
Potential energy = mass(gravitational field strength)(height)

6.3 Power
P= W/t = E/t
Power = work done over time = energy converted over time
SI Unit: watt (W)

One watt is defined as the rate of working or energy conversion of one joule per second

Physics: Chapter 5 - Turning Effect of Forces

5.1 Moments
The moment of a force is the product of the force and the perpendicular distance from the pivot to the line of action of the force.

Moment of a force = Fxd
Force(perpendicular distance from pivot) = Moments

Moment = turning effect of force

5.2 Principle of Moments
When a body is in equilibrium, the sum of clockwise moments about a pivot is equal to the sum of anticlockwise moments about the same pivot.

An object is said to satisfy the Principle of Moments when the force acting in clockwise motion is the same as force acting in anticlockwise motion on the same pivot.

Conditions for equilibrium:

1. All forces acting on it are balanced (Resultant force is 0)
2. The resultant moment about the pivot is 0 (Principle of Moments must apply)
   

5.3 Centre of Gravity

The centre of gravity of an object is defined as the point through which its whole weight appears to act for any orientation of the object.

The centre of gravity of a body is a single point through which its entire weight acts.

5.4 Stability
Stability refers to the ability of an object to return to its original position after it has been tilted slightly.

Three cases of equilibrium:

1. Stable equilibrium
2. Unstable equilibrium
3. Neutral equilibrium

To increase stability of an object:

1. The centre of gravity should be as low as possible
2. The area of a base should be as wide as possible

Physics: Chapter 4 - Mass, Weight and Density

4.1 Mass and Weight
Mass is a measure of the amount of matter or substance in a body.
SI Unit: kilogram (kg)

Weight is a force and has direction.
SI Unit: newton (N)
Also know as gravity.

W = mg
Weight = mass(gravitational field strength)
Earth = 10kg^-1

4.2 Inertia
Inertia of an object refers to the reluctance of the object to change its state of rest or motion.

4.3 Density
The density of a substance is defined as its mass per unit volume.
p = m/v
Density = mass/ volume
SI Unit: kilogram per cubic metre (kg m^-3)

Physics: Chapter 3 - Forces and Pressure

3.1 Forces

A force is a push or a pull that one object exerts on another.
It produces or tends to produce motion, and stops or tends to stop motion.

SI Unit: newton (N)

3.2 Scalars and Vectors
Scalar quantities are physical quantities that have magnitude only
Vector quantities, however, are physical quantities that possess both magnitude and direction.

3.3 Forces and Motion
A force can cause:

1. A stationary object to start moving
2. A moving object to increase speed
3. A moving object to decrease speed
4. A moving object to change its direction of motion

Forces and Zero acceleration

For an object with zero acceleration, the different forces acting on it are balanced or add up to zero.

Balanced forces and Newton's First Law

Every object will continue in its state of rest or uniform motion in a straight line unless a resultant force acts on it to change its state.

Unbalanced forces and Newton's Second Law

When a resultant force acts on an object of constant mass, the object will accelerate and move in the direction of the resultant force.
The product of the mass and acceleration of the object is equal to the resultant force.

F = ma
Force = mass(acceleration)

SI Unit: Newton (N)

Weight is a force
W = mg

Newton's Third Law

For every action, there is an equal and opposite reaction, and these forces act on mutually opposite bodies.

3.4 Friction and its Effects
Friction always opposes motion between two surface in contact.

3.5 Pressure
Pressure = force / area
P = F/ A
SI Unit: newton per square metre (N m^-2)

Physics: Chapter 2 - Kinematics

2.1 Distance, Time and Speed
Speed = Distance moved / time taken
v = d/t

Average speed = total distance travelled / total time taken

2.2 Speed, Velocity and Acceleration
Acceleration = change in velocity / time taken

2.3 Speed- Time graphs
Area under the speed time graph gives the distance moved.

2.4 Acceleration of free fall
Acceleration due to free fall (acceleration due to gravity) does not depend on the material, size or shape.

Physics: Chapter 1 - Measurement

1.3 Measurement of Length
SI Unit: metre (m)
Instrument: Metre rule, tape measure, calipers, vernier calipers and micrometer screw gauge

1.3 Measurement of Time
SI Unit: seconds (s)
Instrument: Watch, stopwatch

Physics: Chapter 17 - Practical Electricity

17.1 Uses of Electricity
Electricity is used for:

1. Heating (Kettle, iron, hotplate)
2. Lighting (Filament lamps, fluorescent lamps)
   
3. Electric Motors (Hair dryer, food mixer)

Filament Lamps
Advantages: Gives a cosy and relaxed atmosphere.
Disadvantages: Only a small % are converted to light energy while the rest are converted to heat energy.

Fluorescent lamps
Advantages: It is energy efficient.
Disadvantages: Costly. Mercury vapour in the lamp is toxic.

17.2 Measuring Electrical Energy
Electric Power P
P= VI
P= I²R
P= V²/R
SI Unit: watt (W)

Electric energy E
E= V²/R (t)
SI Unit: joule (J)

17.3 Dangers of Electricity
Faulty appliances or circuits can cause shock or fire.

1. Damaged insulation (shock)
   
2. Overheating of cables (fire)
   
3. Damp Conditions (shock)

1) Damaged insulation
Insulator can crack and break which exposed the conducting wires inside.
Exposed live wires can cause electric shock.

2) Overheating of cables
The higher resistance of thinner wires will produce more thermal heat that will damage the insulation and may cause a fire.

3) Damp conditions
Water provide a conducting path for a large current to flow. If can therefore shock a person to death.

17.4 Safe Use of Electricity at Home

1. Circuit breakers
2. Fuse
3. Correct placement of switch in the circuit
4. The three-pin plug
5. Earth wire
6. Double insulation of certain appliances

1) Circuit breakers are safety devices that can switch off the electrical supply in a circuit when there is an overflow of current.
a) Miniature circuit breaker MCB
b) Earth leakage circuit breaker ELCB

a) MCB prevents excessive current flow through in the circuit by tripping or breaking it.
It can be reset by switching it on again.

b) ELCB monitors the amount of current flowing from the live wire. Current in neutral wire should be the same as live wire. ELCB detects these small current leakages from the live wire to the earth wire.

2) Fuse
A fuse is a safety device included in an electrical circuit to prevent excessive current flow.
A fuse consists of a short thin piece of wire which becomes hot and melts when the current flowing through it is greater than its rated value.

Fuses should have a current rating just slightly higher than the current an electrical appliance will use under normal conditions.

3) Switches
Switches must be fitted onto the live wire so that switching off disconnects the high voltage from an appliance.

4) Plugs and sockets
Live wire : Brown
Earth wire: Green & Yellow
Neutral wire : Blue

5) Earthing
The earth wire is a low-resistance wire.
It is usually connected to the metal casing of the appliance.

6) Double insulation
Appliance that use a two-pin plug requires double insulation.

Physics: Chapter 16 - D.C. Circuits

Physics: Chapter 15 - Current Electricity

15.1 Electric Current
Electric current is formed by moving electrons.

Conventional current and electron flow
Electron flow: Electrons moving from a negatively charged end to a positively charged end

Conventional current flow: Positive charges flowing from a positively charged end to a negatively charged end.

Measurement of electric current

An electric current I is a measure of the rate of flow of electric charge Q through a given cross section of a conductor.

I = Q/t
Current = Charge / time

SI unit: ampere
Symbol: A
Instrument to measure: Ammeter
Ammeter must be connected in series in an electric circuit. Flow from + to - terminal.



Electric Circuit symbols


15.2 Electromotive Force and Potential Difference

The electric force (e.m.f.) of an electrical energy source is defined as the work done by the source in driving a unit charge round a complete circuit.

E = W/Q
E.M.F. of the power supply = work done/ charge

SI unit: joules per coulomb (J C^-1) or Volt (V)
Instrument to measure: Voltmeter



Potential Difference

The potential difference (p.d.) between two points in an electric circuit is defined as the amount of electrical energy converted to other forms of energy when one coulomb of positive charge passes between the two points.

V = W/Q
Potential difference = Work done/Charge

SI unit: volt (V)

E.M.F. is provided by a source of electric energy.
P.D. refers to the electrical energy converted to other forms by a circuit component.

15.3 Resistance
Resistance is a measure of how difficult it is for an electric current to pass through a material.

The resistance R of a component is defined as the ratio of the potential difference V across it to the current I flowing through it.

R = V/I
Resistance = Potential difference/current

SI unit: ohm (Ω)
Instruments: Fixed resistors or rheostats


Ohm's Law

The current passing through a metallic conductor is directly proportional to the potential difference across its ends, provided the physical conditions (such as temperature) are constant.

15.4 Resistivity
Resistance of a conductor depends on

1. its length
2. its cross-sectional are or thickness of the wire
3. the type of material

p = RA/l
resistivity = resistance(cross-sectional area)/length

Physics: Chapter 14 - Static Electricity

14.1 Electrostatics
It is the study of static electric charges.

Electrostatic charging by friction
Some objects acquire electric charges by rubbing them together to transfer electrons from one object to another.

There are two types of charges: positive and negative.
Like charges repel, unlike charges attract.

Measurement of electric charge
Electric charge is measured in coulombs, C.

14.2 Electric Field
An electric field is a region where an electric charge experiences an electric force.

The direction of the field is defines as the direction of the force on a small positive charge.

The strength of an electric field is indicated by how close the field lines are to each other.

Chemistry: Chapter 15 - Energy Changes

15.1 Exothermic and Endothermic Changes
Energy cannot be created or destroyed.
However, it can be changed from one form to another.

a) Exothermic Reactions
Reactions that give out heat energy to the surroundings are called exothermic reactions.

Characteristics of exothermic reactions

1. Heat is liberated and is transferred from the chemicals to the surroundings, and
2. the temperature of the reaction mixture rises. 

Examples of exothermic reactions include:

• combustion of fuels
• rusting of iron
• corrosion of metals
• reaction between acid and alkali (neutralisation)
• respiration

b) Endothermic Reactions
Reaction that absorb heat from the surroundings are called endothermic reactions.

Characteristics of endothermic reaction:

1. Heat energy is absorbed and is transferred from the surroundings to the reactants, and
2. the temperature of the reaction mixture falls.

Examples of endothermic reactions include

• Photosynthesis
• Action of light on silver bromide in photographic film
• thermal decomposition

Heat Changes in a Reaction
The amount of energy involved in a reaction is known as the heat change or enthaly change of the reaction.

For exothermic reaction, energy change is negative because it lose energy to the surroundings.
For endothermic reaction, energy change is positice because it gain energy to the surroundings.

15.2 Combustion of Fuels
Fuels give out energy when burnt.

Imcomplete combustion occurs when there is a limited supply of air is used.
The combustion of fuels is an exothermic reaction.

***

Hot, Exothermic

Cold, Endothermic

Chemistry: Chapter 5 - Atomic Structure

5.1 Inside Atons
Atoms are made up of protons, neutrons and electrons.

 Electrons:

• Carries one negative electric charge -1
• Has a relative mass of 1/1840

Protons:

• Carries one positive electric charge +1
• Has a relative mass of 1

Neutrons:

• Carries no electric charge
• Has a relative mass of 1

5.2 The Proton Number and Nucleon Number
Proton number + Nucleon number = Nucleon number

5.3 Isotopes
Isotops are atoms of the same element with the same number of protons but different number of neutrons.

5.4 Arranging Electrons in Atoms
First shell

• Hold a maximum number of 2 electrons.
• Is always filled first.

Second, third and sebsequent shells

• Can hold up to 8 electrons each.
• Are filled in order. Second shell must be filled before going to third, fourth shell.

The way the electrons are arranged in an atom is called electronic structure or electronic configuration.
The shell that is furthest from the nucleus is called the outer shell or the valence shell.
The electrons in this shell are called valence electrons.

Chemistry: Chapter 2 - Measurement and Experimental Techniques

2.1 Measuring Time
S.I. unit: second (s)
Other units: minute (min), hour (h)
Apparatus used: stopwatch 

2.2 Measuring Temperature
S.I. unit: Kelvin (K)
Other units: degree Celsius (°C)
Apparatus used: Mercury thermomenter, data logger

2.3 Measuring Mass
S.I. unit: kilogram (kg)
Other units: gram (g)
Apparatus used: Electronic balance, beam balance

2.4 Measuring Volume
S.I. unit: cubic metre (m³)
Other units: cubic centimetre (cm³), litre (ℓ), millilitre (ml)
Apparatus used: beaker, measuring cylinder, burette, pipette
Accuracy:

1. beaker -  used to estimate the volume of a liquid e.g. approximately 100cm³
2. measuring cylinder - more accurate than a beaker; measures up to the nearest cm³
   
3. burette - accurately measures out the volume of a liquid to the nearest ± 0.1cm³
   
4. pipette - accurately measures out fixed bolumes of liquids e.g. 20.0cm³

2.5 Collecting Gases and Measuring Volumes of Gases

To collect a gas, we have to take note of the

• Solubility - how soluble the gas is in water
• Density - how dense the gas is compared to air

Methods to collect gas:

• Displacement of water - suitable for gas which are insoluble or slightly soluble in water
• Downward delivery - suitable for gas that are soluble in water and denser than air
• Upward delivery - suitable for gas that are soluble in water but less dense that air

Measuring of gas

Using a gas syringe can measure the volume of a gas.

2.6 Determining if a Substance is Pure
A pure substance is made up of only one substances.

a) Solids
A pure solid will melt completely at one temperature.
Impurities affect the melting point of a substance in two ways.

• The > the amount of inpurities, the lower the melting point.
• They cause melting to take place over a range of temperatures.

b) Liquids
A pure liquid has an exact and constant boiling point.
Impurities affect the boiling point.

• Boiling point will increase and will boil over a range of temperatures.

Pressure will affect the boiling point.

• If pressure ↑, boiling point is raised. 
• If pressure ↓, boiling point is lowered. 

***

Common gases arranged in terms of Solubility:

Ammonia (Extremely soluble) -> Hydrogen Chloride, Sulphur Dioxide (Very soluble) -> Oxygen (Very slightly soluble) -> Chlorine (Soluble) -> Carbon Dioxide (Slightly soluble) -> Hydrogen (Not soluble)

Common gases arranged in terms of Density

Sulphur Dioxide, Hydrogen Chloride, Chlorine, Carbon Dioxide (Denser) -> Oxygen (Slightly denser) -> Ammonia, Hydrogen (Less dense)

Social Studies: Book 3 Chapter 5 - Bonding Singapore

1 & 2 Introduction + Singapore; Who are we?
Singapore is a multi-ethnic country with people from many different racial, cultural and religious background.
It is important to maintain peace and harmony in Singapore.

3 What are the challenges of a multi-ethnic society?

1. Managing perceptions of different racial groups
2. Managing perceptions of different religious groups
3. Threats from external forces

3.1 + 3.2 Managing perceptios of different racial or religious groups.
Lack of understanding among the racial or religious groups can create suspicion and unhappiness among the people.
Riots and fight may occur between racial or religious groups and this make Singapore unsafe.
Investments from other countries will decrease and economy will be in a bad state.
In whole, Singapore may not be prosperous if people in Singapore behave insensitively.

Examples for racial riot:
1964 riot
PAP wants Malaysia to be a country where everybody would be given equal rights and privilleges -> United Malays National Organisation (UMNO) felt threatened -> Anti-PAP campaign organised by some UMNO leaders spread incorrect information about PAP treating the Malays in Singapore unfairly -> Caused dissatisfaction among Singapore Malays towards PAP

July 1964, Prophet Muhammad's birthday celebration -> Clash between a Chinese policeman and a group of Malay participants during the celebration -> Full-blown race race riots occured over the next few days -> Properties destroyed, people injured -> Broke peace and harmony in Singapore because of irresponsible media reports

Examples for religious riot:
Maria Hertogh riot
In 1940s, a Dutch couple was imprisoned by the Japanese -> They placed their daughter Maria Hertogh under the care of a Malay lady, Aminah -> Maria was raised as a Muslim and got married to a Malay teacher at the age of 13 -> The Dutch couple demanded that Maria be returned to them

A court trial followed and it had much media coverage which provoked much unhappiness among the Muslim community -> Court decided to give custody to the Hertoghs -> The Muslims felt that British legal system was unfair -> Outbreak of riots happened between the Muslims and Christians

3.3 Threats from external forces
Threats from other countries are unpredictable, unexpected and cannot be control.
People in Singapore can be influenced by incorrect ideology through exposure from

1. teachings, 
2. internet, 
3. media, 
4. travelling to other countries or 
5. communicating with people from other countries.

They (people) might bring back those ideology and influence other people.
They may attempt to commit acts of terrorism / attempt to brain-wash people into believing their extreme beliefs.
Example would be Jemaah Islamiyah (JI).
They planned to bomb Yishun MRT and when their plots were exposed, other races / religious groups began to get suspicious of the Muslims.
Singapore became unstable. Religious leaders had to come out to clarify their stand.
If not handled properly, Singapore would be unstable and investments would decrease.

4 Can ethnic diversity be managed?

1. Building a national identity
2. Safeguarding the interest of the minority groups
3. Deceloping common space

4.1 Building a national identity

• a) Multi- racialism
• b) Common practices
• c) Bilingualism

a) Multi- racialism
This policy promotes equality among the races, with no special rights granted to any particular racial or religious group. Favouring a certain group of people because of their race or religion is prohibited.

b) Common practices
Actions that Singaporeans carry out together like singing the national anthem, taking the pledge and attending the flag raising ceremony help foster national identity by inculcating loyalty and national pride to Singapore. This gets Singaporeans to see themselves as one people.

National Pledge

We, the citizens of Singapore
pledge ourselves as one united people,
regardless of race, language or religion,
to build a democratic society,
based on justice and equality,
so as to achieve happiness, prosperity and
progress for our nation.

c) Bilingualism
Students were expected to learn English and their own Mother Tongue. With bilingualism, English is used as the language linking the different ethnic groups. Mother Tongue language is used to impart moral values and cultural traditions of each race.

4.2 Safeguarding the interests of the minority groups

• a) Minority representation
• b) Self-help groups

a) Minority representation
The policy of minority representation gives minority groups a say in governance.
The Presidential Council of Minority Rights (PCMR) and the Group Representation Constituency (GRC) are two examples of how representation of the minority groups is achieved.

PCMR consists of members from the minority racial and religious groups. It ensures that no racial or religious group is disadvantaged as a result of a law that is passed in Parliment.

GRC ensures that at least one of the candidates in the team contesting in the General Election is from the minority racial communities such as Malay, Indian or Eurasian. GRC system ensures that the minority racial groups are represented in the Parliment. Needs of the minority groups are made known to the government.

b) Self- help groups
Self- help groups play an important role in helping members of their community who are less fortunate. They also give moral support to their members of their own community.
Self help groups in Singapore

• Chinese Development Assistance Council (CDAC)
• Singapore Indian Development Association (SINDA)
• Mendaki
• Eurasian Association

4.3 Developing common space
Common space refers to the time and place that people come together. This provide opportunities for Singaporeans to interact.
Ways to make Singaporeans interact:

• a) Events and programmes organised by grassroots organisation
• b) Opportunities offered by educational institutions
• c) Common living space provided by public housing
• d) Activities conducted by Inter-Racial Confidence Circles (IRCCs) and Harmony Circles (HCs)
• e) Shared experience through National Service

a) Events and programmes organised by grassroots organisation
Organisations such as People's Association (PA) create common space through their wide range of programmes and activities developed to cater to the needs and interests of every Singaporean.

b) Opportunities offered by educational institutions
Daily interaction that take place among students during lessons and school activities provides an opportunity for friendships to be cultivated and strengthened.

Co- Curricular Activities (CCAs) in schools helps to promote closer bonds among youths from all races.

c) Common living space provided by public housing
Ethnic integration policy was introduced to ensure that there is an even distribution of the different races in all the housing estates.

d) Activities conducted by Inter-Racial Confidence Circles (IRCCs) and Harmony Circles (HCs)
IRCCs and HCs were introduced to provide common space to foster greater inter-racial understanding.

e) Shared experience through National Service
NS was introduced in 1967 requires all able-bodied men to serve in the defense of the country. The shared experiences help to strengthen the bond among the men.

5 Why is it important to manage ethnic diversity?
For:

• Security and peace
• Economic progress

6 Conclusion
People in Singapore need to be sensitive to one another's needs.
Failure to understand and respect one another's way of life will affect the country.
Managing racial and religious sensitivities will promote tolerance and harmony.
Building a national identity will instill a sense of belonging.
Staying vigilant and active in identifying threats and strengthening social bonds are responsibilities of the Singapore government and its people.

Chemistry: Chapter 1 - Kinetic Particle Theory

1.1 States of Matter
a) Matter is a substance that has mass and occupies space.
b) 3 forms of matter:

1. Solid
2. Liquid
3. Gas
   

1.2 Kinetic Particle Theory
a) Solid state:

1. Orderly, closely packed arrangement.
2. Very strong attractive force between particles.
3. Very low kinetic energy of particles.
4. Particles vibrate and rotate about a fixed position.
   

b) Liquid state:

1. Disorderly, less closely packed than in a solid arrangement.
2. Strong attractive force between particles.
3. Low kinetic energy of particles.
4. Particles slide over each other.

c) Gaseous state:

1. Disorderly, very far apart arrangement.
2. Very weak attractive force between particles.
3. High kinetic energy of particles.
4. Particles move about at a great speed.

1.3 Changes of State and the Kinetic Particle Theory

1. Melting
2. Freezing
3. Boiling
4. Evaporation
5. Condensation
6. Sublimation

1. Melting (Solid to Liquid)
a)Solid --------------------------------b)--------------------------------c)Liquid
a) Heat energy that is absorbed is converted to kinetic energy which cause the praticles to vibrate faster about their fixed positions.
b) Particles begin to break away from their fixed positions as they gain enough vibration to overcome the attractive forces between them. (Temperature remains constant throughout that period)
c) Particles are no longer in their fixed positions. They slide over one another. Substance is now a liquid.

2. Freezing (Liquid to Solid)
a)Liquid --------------------------------b)--------------------------------c)Solid
a) Particles give out energy which decreases their kinetic energy and they began to move slowly.
b) Particles no longer have energy to move about which cause them to settle into fixed positions. (Temperature remains the same throughout the period)
c) Particles settle into fixed position and can only vibrate about in their fixed positions. Substance is now a solid.

3. Boiling (Liquid to Gas)
a)Liquid ------------------------------------------------------------------b)Gas
a) Through heating, energy is absorbed and kinetic energy increases causes the particles in a liquid to move faster.
b) Eventually, the particles have enough energy to overcome the forces that is holding them together. Particles can now spread far apart in all directions. Substance is now a gas.
*Temperature remains constant during the boiling process.*

4. Evaporation (Liquid to Gas at a lower boiling point)
a) Evaporation occurs because some particles have enough energy to escape as a gas from the surface of the liquid.

5. Condensation (Gas to Liquid)
a) Condensation occurs because gas particles that evaporate loses energy and move more slowly. Movement of parrticles becomes slow enough for the gas to change into a liquid.

6. Sublimation (Solid to Gas)
a)Sublimation occurs because particles at the surface of the solid have enough energy to break away from the solid and escape as a gas. Example: Dry ice

*Heat absorbed causes particles to move faster. OR Heat given out causes particles to move slower.