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10.
1.13 Describe how Dmitri Mendeleev arranged the elements, known at that time, in a table by using the of these elements and their compounds.
Describe how Dmitri Mendeleev used his table to predict the existence and of some elements not then discovered.
Explain that Dmitri Mendeleev thought he had arranged elements in order of increasing relative but this was not always true because of the relative abundance of elements in the periodic table.
Describe that in the periodic table:
a. Elements are arranged in order of increasing atomic number, in rows called s.
b. Elements with similar properties are placed in the same vertical columns called
s.
Explain the meaning of atomic number of an element in terms of position in the periodic table and number of protons in the nucleus.
Number of electrons in outer shell = number
Number of shells with elections = number
So sodium with a configuration of 2,8,1
is in period(There are 3 numbers)
Is in group (the last number is a 1)
Identify elements as metals or non-metals according to their position in the periodic table, explaining this division in terms of the atomic structures of the elements.
Metals occur on the hand side.
Non-metals occur on the hand side.
Predict the electronic configurations of the first 20 elements in the periodic table as diagrams and in the shorthand form, for example 2.8.1 for sodium.
He =
O =
Cl =
Explain how the electronic configuration of an element is related to its position in the periodic table.
e.g. 2.3
group =
period =
e.g. 2.8.8.2
Group =
Period =
6.1 Explain why some elements can be classified as metals (group 1), (group 7) or gases (group 0), based on their position in the periodic table
6.2 Recall that alkali metals:
a are relatively
b have relatively melting points
6.3 Describe the reactions of lithium, sodium and potassium with water
+ water → sodium + hydrogen.
2Na + 2H₂O → 2NaOH + H₂
6.4 Describe the pattern in reactivity of the alkali metals, lithium, sodium and potassium, with water; and use this pattern to predict the reactivity of other alkali metals.
From lithium to potassium the reactivity
Therefore will be reactive than potassium.
The reaction with water would be more .
6.5 Explain this pattern in reactivity in terms of electronic configurations
As group 1 is descended there are more of electrons.
The outermost electron is from the nucleus.
The outermost electron is attracted strongly to the nucleus.
The outermost electron can be lost easily
The reactivity down the group
6.4 Describe the pattern in reactivity of the alkali metals, lithium, sodium and potassium, with water; and use this pattern to predict the reactivity of other alkali metals.
From lithium to potassium the reactivity
Caesium will be
6.5 Explain this pattern in reactivity in terms of electronic configurations
As group 1 is descended there are more
The outermost electron is
The outermost electron is attracted
The outermost electron can be lost
The reactivity
Word bank (words can be reused)
further
increases
less
more
shells
sodium
