3.1.1 Periodicity Flashcards
How are elements arranged in the periodic table?
They are arranged in order of increasing atomic numbers
What is a period on the periodic table?
The horizontal rows on the table
What is ment by periodicity?
The repeating trends in chemical and physical properties
What change happened across each period?
Elements change from metals to non-metals
How can an electronic configuration be written in short?
The Nobel gas before the element is used to abbreviate eg. [He]2s1
Define the first ionisation energy
The energy required to remove one mol of electrons from 1 mol of gaseous atoms to form one mol of gaseous 1+ ions
What are the factors affecting ionisation energy?
Atomic radius, nuclear charge and electron shielding or screening
Explain the trend on the ionisation energy graph as you go across a period
Increase nuclear charge decreased atomic radius, same electron shielding
This means more energy is required to remove the first electron
Why does the first ionisation energy decrease between group 2 to 3?
Decrease between 2 to 3 because in group 3 the Altemus electrons are in P orbitals whereas in group 2 they are in S orbitals so the electrons are easier to remove
Why does the first ionisation energy decrease between group 5 to 6?
The decrease between 5 to 6 is due to the group 5 electrons in the orbital or single electrons and in group 6 the outermost electrons are spin paired with some repulsion therefore the electrons are slightly easier to remove
Does the first ionisation increase or decrease between the end of one period and the start of thet? Why?
decreases
There is an increase in atomic radius
Increase in electron shielding
Does the first ionisation increase or decrease between the end of one period and the start of thet? Why?
decreases
There is an increase in atomic radius
Increase in electron shielding
Does the first ionisation increase or decrease down a group? Why?
Decrease
Shielding increases -weaker attraction
Atomic radius increases so distance between outer electron and nucleus increases - weaker attraction
Increase in number of protons is out weighed by increase in distance and shielding
What are properties of giant metallic latices?
High melting and boiling point
Good electrical conductors
Malleability
Ductility
What is a ductile metal?
The metal can be made stretched, e.g. can be made into wires
