Tutorial 1.3 - structure, bonding and properties of elements, periodicity Flashcards
1
Q
Possible periodic properties of the gaseous atoms of elements in a particular period [4]
A
- First ionisation energy [1]
- Formulae of ions formed [1]
- Formulae of compounds [1]
- Electronic configuration in outer shell [1]
(FICE)
2
Q
Explain why silicon has the highest melting point of the group 3 elements. [4]
A
- giant structure
- Covalent bonding
- Bonds are very strong
- Lots of energy required to break the bond
3
Q
State and explain the trend in electrical conductivity of the elements Na to Al. [3]
A
- conductivity increases
- because metallic bonding
- so more delocalised electrons
4
Q
Si forms a what ion
A
4+
5
Q
Explain why atomic radii of period 3 elements are significantly larger than those of period 2 elements. [3]
A
- they have an extra FULL shell of electrons
- electrons repel each other
- occupying space
6
Q
State and explain why no data is available on the ionic radius of argon ions. [2]
A
- argon cannot form on ions
- because too much energy is required
