Chemistry Unit 9: The Periodic Table

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As reference, here is a Periodic Table; you can refer to this as you go along the syllabus statements. If you didn't know already, you will be provided with a Periodic Table when you take you exams!

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1. Describe the way the Periodic Table classifies elements in order of proton number.

Elements are ordered in numerical order according to the number of protons it contains. Hydrogen has one proton so it is first, followed by helium, lithium, etc.

2. Use the Periodic Table to predict properties of elements by means of groups and periods.

On the Periodic Table there are groups. The important ones that the syllabus covers are alkali metals (group 1), transition metals (group 3), halogens (group 7) and noble gases (group 0/8).




Unit 9.1 Periodic Trends

1. Describe the change from metallic to non-metallic character across a period.

As you run across the Periodic Table horizontally, the character of the element goes from metallic to non-metallic.

2. Describe the relationship between Group number, number of outer-shell (valency) electrons and metallic /non-metallic character.

The valency of the outer shell depends on what group the element is in. Here's a little advice: once you get your Periodic Table in the exam, start from Group 1 and label +1, +2, +3, +4, -3, -2, -1, full, ending on Group 8. This determines the valency of the element, helping you to balance equations.




Unit 9.2 Group Properties

1. Describe lithium, sodium and potassium in Group I as a collection of relatively soft metals showing a trend in melting point and reaction with water.

Metal	Hardness	Reactivity	Melting point	Reaction with water
Lithium	Soft	Reactive	180.5°c	Fizzes on water, releases hydrogen
Sodium	Softer	More reactive	97.7°c	Fizzes on water, burns with a yellow flame, release hydrogen
Potassium	Softest	Most reactive	63.4°c	Fizzes on water, burns with a lilac flame, release hydrogen

From my experience, exam boards like to throw in a question worth 6-9 marks about lithium, sodium and potassium comparisons, so it's worth remembering these points.

2. Predict the properties of other elements in Group I, given data where appropriate.

Properties of alkali metals
• relatively soft metals
• low boiling and melting points --> decrease as you go down the group
• reacts with water to form metal hydroxide + hydrogen
• reacts with oxygen to form metal oxide
• reactivity increases as you go down the group
• densities increase as you go down the group

3. Describe the trends in properties of chlorine, bromine and iodine in Group VII including colour, physical state and reactions with other halide ions.

Halogen	State at room temperature	Colour	Reaction with halide ions
Chlorine	Gas	Yellow-green	Oxidises bromine and below
Bromine	Liquid	Red-brown	Oxidises iodine and below
Iodine	Solid	Purple	Oxidises astatate and below

4. Predict the properties of other elements in Group VII, given data where appropriate.

Properties of halogens

• melting and boiling points increase as you go down the group

• reactivity decreases as you go down the group

• kills bacteria

• react with metals to form metal halides

Unit 9.3 Transition Elements

1. Describe the transition elements as a collection of metals having high densities, high melting points and forming coloured compounds, and which, as elements and compounds, often act as catalysts.

Properties of transition metals

• high densities

• high melting points

• forms coloured compounds

• can act as catalysts

Unit 9.4 Noble Gases

1. Describe the noble gases as being unreactive.

Noble gases are unreactive because their outer shells are full. This means that they are stable without having to gain or lose electrons. They are also described as inert. 

2. Describe the uses of the noble gases in providing an inert atmosphere, i.e. argon in lamps, helium for filling balloons.

Under normal conditions, noble gases are odourless, colourless and nonflammable. 

• argon is used in lightbulbs

• helium is used to inflate tires and balloons

• neon is used in neon lights because it glows when electricity is passed through it

• xenon is used in photocopying 

Physics Unit 4: Simple Kinetic Molecular Model of Matter

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Unit 4.1 States of Matter

1. State the distinguishing properties of solids, liquids and gases.

Solid	Liquid	Gas
Particles are tightly packed in a regular pattern	Particles are loosely bonded with gaps between them	Particles are completely seperated
Particles vibrate together, keeping its shape and position	Particles vibrate and slide past one another	Particles are free to move
Retains a fixed volume and shape	Takes shape of its container	Takes shape of its container
Does not flow easily	Flows easily	Flows easily

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Unit 4.2 Molecular Model

1. Describe qualitatively the molecular structure of solids, liquids and gases. 

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As mentioned above, particles in solids are in fixed positions, while particles in liquids and gases are more free.

2. Relate the properties of solids, liquids and gases to the forces and distances between molecules and to the motion of the molecules.

In solids, the particles are close together because they are bonded in fixed positions. In liquids, the particles are attached together but are not as rigorously held together as particles in a solid. In gases, the molecules are completely unattached so the space between particles can be far and wide. 

3. Interpret the temperature of a gas in terms of the motion of its molecules.

When a gas is hot, its particles move quickly and collide often. This is because heat energy is given to the particles, giving them the kinetic energy to move. The hotter the gas, the faster the particles will move. 

4. Describe qualitatively the pressure of a gas in terms of the motion of its molecules.

Imagine you've got a sealed container containing gas. When the gas particles move, they hit the sides of the container; this creates pressure on the container. The pressure of the gas depends on how often and how hard the molecules are colliding with the inside of the container. 

5. Describe qualitatively the effect of a change of temperature on the pressure of a gas at constant volume.

You know that a high temperature = faster motion and faster motion = more pressure. Therefore, the higher the temperature of gas, the more pressure of the gas at constant volume. 

Unit 4.3 Evaporation

1. Describe evaporation in terms of the escape of more energetic molecules from the surface of a liquid.

Evaporation occurs when there are particles in a liquid that move faster, so fast that if they are near the surface they have enough energy to escape and become a gas. 

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2. Demonstrate understanding of how temperature, surface area and air flow over a surface influence evaporation.

Temperature: a higher temperatures means that the particles have more energy to escape, resulting in  a faster rate of evaporation.

Surface area: with a bigger surface area, more of the molecules are at the surface, allowing them to escape.

Air flow: air flow picks up molecules at the surface before they can become liquid again. The higher rate of air flow, the faster the evaporation. 

3. Relate evaporation to the consequent cooling.

When water evaporates, it takes some thermal energy from whatever is has been on, resulting in that thing being cooler. Faster particles escape first, so slower particles are left behind; this means the temperature is lower than before. 

Unit 4.4 Pressure Changes

1. Relate the change in volume of a gas to change in pressure applied to the gas at constant temperature and use the equation pV = constant at constant temperature.

Boyle's law states that pressure and volume are inversely proportionate when the gas is at a constant temperature. Lowering the volume will increase in a higher pressure, and vice versa. This is because if a gas has a smaller volume, there is less space for the particles to move; they hit the sides of the container more frequently, resulting in higher pressure. 

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