Periodic Table Flashcards
Group no. indicates
No. of valence electrons
Period no. indicates
No. of electron shells
How does metal get a full valence shell?
Lose electrons
How does non-metal get a full valence shell?
Gain electrons
Physical properties of Group I metals
Low melting points
* soft - easily cut
* low densities
Chemical properties of Group I metals
Reacts with water to form metal hydroxide & H2
Example:
2Li + 2H2O → 2LiOH + H2
2Na + 2H2O → 2NaOH + H2
2K + 2H2O → 2KOH + H2
Trends of Group I metals
M.P. & B.P. decreases
* Density increases
Reactivity increases
* Fast rxn
* Very fast rxn, sparks
* Explosion
Group VII Metals
Halogens; 7 valence electrons; diatomic
Group I Metals
Alkali metals; 1 valence electron
Physical properties of Group VII Metals
- cannot conduct electricity
- relatively low m.p. & b.p., density
- coloured
Chemical properties of Group VII Metals
Displacement → a more reactive halogen will displace a less reactive halogen from an aqueous solution of its ions
- Example:
Cl2 + 2KI → 2KCl + I2 - Observation:
The colourless potassium iodide (KI) will form a
black precipitate in a brown solution as iodine (I2)
is formed.
Trends of Group VII
M.P. & B.P.
increases
* Color
darkens
* Density
increases
Reactivity increases
Group 0
Monoatomic; Noble Gases; unreactive as they have full valence shells; no need to form bonds with other atoms
How are the elements
arranged in the Periodic Table?
According to proton number.
Why are noble gases
unreactive?
They have full valence shell.