Trends in the Properties of Elements in Period 3 Flashcards
(11 cards)
Which elements in Groups 1,2 and 3 are metals and what structures do they form?
Sodium,magnesium and aluminium are metals with giant structures
How do metals in Groups 1,2 and 3 form compounds?
They lose their outer electrons to form ionic compounds
What type of bonding does silicon in Group 4 exhibit?
Silicon forms four covalent bonds using its four outer shell electrons
What do non - metals in Groups 5, 6 and 7 do to form compounds?
They either accept electrons to form ionic compounds or share electrons to form covalent compounds
What is special about argon in Group 0?
Argon is a noble gas with a full outer shell, making it unreactive
Why is there a clear break in melting and boiling points between elements in the middle of the Periodic Table?
Because elements on the left have giant structures (with high melting + boiling points) and elements on the right have molecular or atomic structures (low melting and boiling points)
What type of structures have high melting and boiling points?
What type of structures have low melting and boiling points?
Giant structures
Molecular or atomic structures
Why do the melting points of metals increase from sodium to aluminium?
Due to the increased strength of metallic bonding
How does metallic bonding strengthen from sodium to aluminium?
The charge of the ion increases and more electrons joint he delocalised ‘sea’ of electrons, strengthening the metallic lattice
What factors determine the melting points of non - metals with molecular structrues?
The size of van der Waals forces between molecules, which depend on the number of electrons and how closely molecules pack together
Why does silicon have a higher melting point compared to other non - metals?
This is because silicon has a giant covalent structure
