Bonding And Structure

Question 1

Define electronegativity

Answer 1

The power of an atom to attract electron density/ a shared pair of electrons to itself in a covalent bond

Question 2

What does electronegativity depend on ?

Answer 2

1.Nuclear charge
2.The distance between the nucleus and the outer most electron shell / orbital
3.The shielding of nuclear charge by inner shells of electrons , meaning the smaller the atom the closer the shared pair of electrons to the nucleus meaning the electronegativity is greater

Question 3

Patterns of electronegativity

Answer 3

Increasing electronegativity up the group
Increasing electronegativity along the period

Question 4

Describe a metallic crystal

Answer 4

A lattice if positively charged metal ions and a sea of delocalised electrons , which are held together by electrostatic forces of attraction

Question 5

Properties of a metallic crystal

Answer 5

High melting and boiling point , because of the strong electrostatic forces of attraction.
Good conductors of heat and electricity, this is due to the free delocalised electrons which are free to move and carry charge through the structure.
Malleable and ductile , because the ions can move within the lattice whilst still being attracted to the sea of delocalised electrons
strength of the metal - this is dependant of the charge on the ion ( the larger the charge the larger the force of attraction the greater the strength) . it is also dependant on size of the ion ( because the smaller the ion the closer the electrons are packed together towards the nucleus therefore the bonds are stronger)

Question 6

Give an example of a metallic crystal

Answer 6

Magnesium
Giant structure
Good conductor of heat and electricity
Malleable and ductile
High melting and boiling point