metallic bonding

Question 1

define metallic bonding

Answer 1

electrostatic force of attraction between delocalise electrons and positive metal ions in a lattice

Question 2

define isoelectronic

Answer 2

species with the same number of electrons but differ in nuclear charge

Question 3

describe the structure of metals

Answer 3

regularly arranged and closely packed

Question 4

if you have 6 Mg2+ ions, how many delocalised electrons do you have

Answer 4

12 delocalised electrons
(4 delocalised electrons in each row of 3 mg2+)

Question 5

Why does Al have stronger metallic bonds than Na and Mg

Answer 5

Al has stronger metallic bonds than Na and Mg so has a higher boiling point. This is due to having stronger electrostatic forces and the charge on Al being greater therefore there are more delocalized electrons

Question 6

what 2 factors impact the strenth of a metallic bond and how

Answer 6

charge on an ion
(the greater the charge on an ion, the greater the number of delocalised electrons and the stronger the elctrostatic attraction between sportive ions and electrons)

size of an ion
(the smaller the ion, the closer the electrons are to the positives nucleus and the stronger the bond)

Question 7

Describe the structure and bonding in magnesium

Answer 7

giant metallic lattice​

Mg2+ ions in a sea of delocalised electrons​

strong electrostatic forces between Mg2+ ions and sea of delocalised electrons

Question 8

Explain why copper is a good conductor of electricity ​

Answer 8

copper has Cu2+ ions in a sea of delocalised electrons​

delocalised electrons are able to move and flow through the metal lattice and carry charge