This includes the entire chapter of 3.1 chemistry (OCR, A level from 2015 onwards) that I personally use for revision. Best coupled with past paper questions (you can find online for free). The information has been taken from lectures and has been rewritten in certain areas by my professors. Incred...
CHEMISTRY
MODULE 3 – PERIODIC TABLE AND ENERGY
3.1 – THE PERIODIC TABLE
Periodicity
Describe the arrangement of the periodic table.
o Ordered in increasing atomic (proton) number
o Periods show repeating trends in physical and chemical properties
o Grouped into elements with similar physical and chemical properties
Why is argon before potassium in the periodic table despite having a larger
atomic mass?
o Argon has a lower atomic number so it is before potassium
o Argon has the same chemical properties as other elements in group 8
o Potassium has the same chemical properties as other elements in group
1.
Describe periodicity.
o A repeating pattern across different periods
Why do elements in the same group exhibit similar properties?
o Similar outer shell electron configurations. This results in similar
properties.
o Outer electrons are what give suibstances their chemical properties.
o This is why isotopes of the same element have the same chemical
properties despite having different masses.
What can the periodic table tell you about electron configurations?
o The period an element is in tells you the number of energy levels that
element has
o The group an element is in tells you the number of electrons an electron
has in its outer shell
o The block an element is in tells you the sub shell that the last electron is
in
Ionisation energies
Define the first ionisation energy
o The amount of energy required to remove an electron from each atom in
a mole of gaseous atoms to form a mole of gaseous 1+ ions.
Define successive ionisation energy
o A measure of the energy required to remove each electron in turn from
each atom or ion in a mole of gaseous atoms or ions.
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