Exam Cards - Unit 1: The Periodic Table Flashcards
What do all the elements in a period have in common?
They have the same number of electron shells.
What do all the elements in a group have in common?
They have the same number of electrins in their outer shell.
Does the atomic radius increase or decrease across a period and why?
Decreases because as the number of protons increases, the positive charge of the nucleus increases, drawing electrons closer to the nucleus.
Does ionisation energy increase or decrease across a period and why?
Increases because the increased number of electrons causes increased nuclear attraction, meaning that it’s harder to remove electrons.
Does ionisation energy increase or decrease down a group and why?
Decreases because of the increased number of electron shells, which means outer-shell electrons are further from the nucleus and experience less nuclear attraction. Also, the inner shells create electron shielding.
Does reactivity increase or decrease down Group 2?
Increases.
What do Group 2 metals react with water to produce?
Metal hydroxides and hydrogen.
What do Group 2 metals react with oxygen to produce?
Metal oxides.
What do Group 2 carbonates decompose to form?
Metal oxides and carbon dioxide.
Does the thermal stability of Group 2 carbonates increase or decrease down the group?
Increases.
Why do the boiling and melting points of halogens increase the group?
Increased strength of van der Waals forces.
Why do halogens become less reactive down the group?
Since halogens react by gaining an electron, it’s harder for halogens down the group to attract electrons with nuclear attraction because of the increased number of shells.
