Bonding

Question 1

Define Metallic Bonding

Answer 1

The strong electrostatic attraction between positive metal ions and delocalised electrons

Question 2

Draw this bonding ( metallic )- refer to notes for answer

Answer 2

Hint!
When drawing metallic bonding diagrams:
Always draw at least 6 ions (2 rows of 3)
Work out the charge of the ion (i.e. how many electrons are lost from the atom?)
Draw the correct number of delocalised electrons. (i.e. the sum of all the charges)

Question 3

The bonding in magnesium is stronger than sodium because …

Answer 3

-Mg has a greater charge of 2+
-Mg has twice as many electrons
-Mg ions are smaller, meaning there is a greater charge density
-The attraction between the Mg2+ ions and the delocalised electrons is stronger

Question 4

Property of metal: Conductivity

Answer 4

-Good electrical and thermal conductors
-Delocalised electrons are free to carry charge/current

Question 5

Property of metal:Strength

Answer 5

Strong due to strong electrostatic attraction between + ions and delocalised electrons

Question 6

Property of metal: malleable and ductile

Answer 6

• Ions can slide over each other in layers

Question 7

Covalent bond definition

Answer 7

Shared pair of electrons between two atoms

Question 8

What are the three macromolecules

Answer 8

Carbon, silicon oxide and silicon

Question 9

Explain the structure of diamond

Answer 9

-Each carbon forms 4 covalent bonds
-Tetrahedral arrangement
- Hard material with high melting point
Doesn’t conduct electricity as no delocalised electrons

Question 10

Explain the structure of graphite

Answer 10

• layers of carbon atoms, forms 3 covalent bonds
  -Delocalised electron to carry charge
  -Layers held together by van deer walks
  -high melting point due to lots of covalent bonds

Question 11

Ionic bond definition

Answer 11

Electrostatic attraction between oppositely charged ions

Question 12

Define coordinate bond

Answer 12

Shared pair of electrons which have both been donated by the same atom

Question 13

Explain repulsion between BP and no LP

Answer 13

Electron pairs repel as far apart as possible

Question 14

Define electronegativity

Answer 14

The ability of an atom to attract the pair of electrons in a covalent bond

Question 15

What factors affect electronegativity

Answer 15

-number of protons
-shielding
-distance from the nucleus
-shared electrons

Question 16

Define the term dipole- what does it create

Answer 16

Uneven distribution of electron density across a bond- creates a polar bond

Question 17

Polarity in cl2

Answer 17

Equal distribution of electron charge- same electronegativity, no dipole. No polarity

Question 18

Polarity in HCL

Answer 18

The Cl atom is more electronegative than H. Uneven distribution of electron charge, creating a dipole and a polar bond

Question 19

Hydrogen Bonding:How it arises

Answer 19

Very large difference in electronegativity between the two atoms. This creates a strong dipole. There is a strong attraction between the lone pair on the oxygen and the delta + on another molecule

Question 20

Permanent dipole dipole forces: how it arises

Answer 20

Difference in electronegativity between the atoms. This creates a polar bond, the dipoles don’t cancel out as it is asymmetrical. Attraction between delta - and delta + on another molecule

Question 21

Induced dipole dipoles: How it arises

Answer 21

Random movement of electrons in a molecule creates a temporary dipole (uneven distribution of electron density). this induces a dipole in another molecule. the delta + on one molecule attracts the delta - on another