C2 - The Periodic Table
Independent Learning
Introduction
In this topic we will build on your understanding of how the atom has developed over time, to look at the historical development of the periodic table. The atom and the periodic table provide good examples of how scientific ideas and explanations develop as new evidence emerges. It provides chemists with a structured organisation of the known chemical elements from which they can make sense of their physical and chemical properties. The arrangement of elements in the modern periodic table can be explained in terms of atomic structure which provides evidence for the model of a nuclear atom with electrons in energy levels. This will help provide the fundamental ideas on which the whole of chemistry is based.
Specification links:
Task 1: Know
Task 1a: Use look, cover, write check and quizlet to learn the answers to the core questions and the keywords for this topic.
Learn
Task 2: Development of the Periodic Table
Task 2b: Make notes that:
Identify the significant groups of the periodic table.
Name the first 3 elements in group 0, 1 and 7.
Define group and period.
Describe how the elements are arranged in early versions of the periodic table.
Describe how the elements are arranged in the modern periodic table
Task 2c: Copy and complete the diagram
Task 2d: Answer this exam question
Task 2e: Check your answer to task 2d - click the arrow ->
a) (difference)
sodium has 1 electron and chlorine has 7 electrons in outer level / shell
or
number of electrons
(similarity)
both have three / same number of shells / levels
or
have electrons in third level/shell
or
both have incomplete outer levels / shells
Task 3: Metals, non-metals and the noble gases
Task 3b: Make notes that:
Compare the properties for metals and non-metals.
Describe how the electronic structure of metals and non-metals are different.
Explain why the noble gases are unreactive and the trend in their boiling points.
Complete table on slide 18.
Name the elements that are the noble gases.
Task 3c: Complete and self mark the exam questions
Key point check:
How is the modern periodic table arranged?
The elements are put in atomic number (number of protons) order and are arranged in:
groups - where the elements in the same group have the same number of electrons in the highest energy level/shell.
periods - where all the elements in a period have the same number of energy levels/shells.
Task 4: The alkali metals
Task 4b: Make notes that:
Name the first three elements in Group 1.
Write general word equations for the reactions of The Alkali Metals with water, oxygen and chlorine.
Explain why Group1 metals are called the alkali metals
Describe how you can show that hydrogen and metal hydroxides are made when Group 1 metals react with water.
Describe the trends in hardness, density and reactivity as you go down Group 1.
Explain the trend in reactivity as you go down Group 1.
Task 4c: Complete and mark the exam questions
Task 4d: Complete the progress quiz
Task 5: The halogens
Task 5b: Make notes that:
Name the first four elements in Group 7.
Describe the properties of halogens.
Explain why the elements in Group 7 react similarly.
Explain what a displacement reaction is.
Explain the trend in reactivity as you go down group 7.
Task 5c: Copy and complete:
Hint (not all of the reactions will work - see if you can explain why)
Sodium chloride + fluorine →
Sodium chloride + bromine →
Sodium iodide + chlorine →
Sodium iodide + bromine →
Sodium bromide + iodine →
Extension - can you write any as symbol equations?
Key point check:
Explain why the reactivity of the alkali metals increases as you go down the group.
The number of energy levels increases as you go down the group so:
The distance between the positively charged nucleus and the negatively charged electron in the highest energy level / shell gets larger.
There are also more electrons between the outermost electron and the nucleus which shield the nucleus so:
The electrostatic force of attraction between the positive nucleus and the outermost electron are smaller so:
Less energy is required to remove the electron and make the larger atoms react so:
As you go down the group the elements become more reactive.
Task 6: The transition metals - Set 1 only
Task 6b: Make notes that:
List the typical properties of transition metals and their compounds.
Describe how the properties of Group 1 metals compare with transition metals.
Justify the use of a the following uses of transition metals in terms of their properties:
Copper in electrical wires
Steel beams in bridges
Gold in jewelry
Task 6c: Complete exam question
Task 7: Summary
Task 7a: Watch the video
Task 7b: Complete the seneca learning unit for your set.
Task 7c: Make your own version of the revision summary on the slide and put it in your revision folder. Use the specification to help you:
Specification links:
Task 8: Check
Extend
Great documentary on this topic
Your next party trick?
'Harry Potter' can do it can you?