Bonding

Question 1

Metallic bonding

Answer 1

Electrostatic attraction between positive ions and delocalised electrons

Question 2

Structure in metallic bonding

Answer 2

Giant metallic lattice

Question 3

What attraction is broken when melting or boiling a substance with metallic bonding

Answer 3

Metallic bonds

Question 4

Properties of metals

Answer 4

-Conductive as delocalised electrons are free to move and carry a current
-Malleable and ductile as layers of ions can slide past each other

Question 5

Type of elements involved in ionic bonding

Answer 5

Mental and a non metal

Question 6

Ionic bonding

Answer 6

Electrostatic attraction between oppositely charged ions

Question 7

Structure in ionic bonding

Answer 7

Giant ionic bonds

Question 8

Properties of compounds with ionic bonding

Answer 8

When molten they are conductive as ions are free to move and carry a current

Question 9

Elements involved in covalent bonding

Answer 9

Two non metals

Question 10

Covalent bonding

Answer 10

Started pair of electrons

Question 11

2 types of Covalent structures

Answer 11

Marco and simple molecular

Question 12

What is broken when melting or boiling a Macro molecular structures

Answer 12

Covalent bonds

Question 13

What is broken when melting or boiling simple molecular elements

Answer 13

Intermolecular forces

Question 14

Are macro molecular structures conductive

Answer 14

No except graphite

Question 15

Are simple molecular compounds conductive

Answer 15

No as there is no electrons to carry The charge

Question 16

Factors determining strength of metallic bonding

Answer 16

-size of an ion=smaller ion means stronger bonding
-charge of a metal ion=greater charge means stronger bonding
- number of delocalised electrons=more delocalised electrons means stronger bonding

Question 17

Factors determining strength of ionic bonding

Answer 17

-charge of ions=greater charge means stronger bonding
-size of ions =smaller ion stronger bonding

Question 18

Compare convalent bonds and intermolecular attractions

Answer 18

Convalent bonds are stronger, in simple molecular structures imf breaks at much lower temperatures than convalent bonds

Question 19

Coordinate bond

Answer 19

Both electrons in them shared pair have come from the same atom.On a diagram they are represented by an arrow

Question 20

Effect of lone pairs

Answer 20

Repel more than bonding pairs ,reducing the bond angle by 2.5

Question 21

Electronegativity

Answer 21

Ability of an atom to attract electron density in a covalent bond

Question 22

Factors affecting electro negativity

Answer 22

Shielding= less shielding means stronger electronegativity
Atomic radius=smaller radius means greater electronegativity
Charge=greater charge means greater electronegativity

Question 23

Trends in electronegativity

Answer 23

Across a period it increases , down a group it decreases

Question 24

Describe how induced dipole-dipole attractions occur

Answer 24

Random movement of electrons in one molecule results in uneven distribution of electrons,creating a temporary dipole in one molecule.this induces a dipole in a neighbouring molecules.dipoles attract

Question 25

Factors affecting the strength of induced dipole dipole

Answer 25

-Number of electrons as more electrons means stronger attraction -shape of molecule as straight chain molecules have more surface contact than branched so stronger attraction

Question 26

Polar molecule

Answer 26

Not symmetrical, so individual dipoles don’t cancel out eg cf4

Question 27

Non polar

Answer 27

Symmetrical dipoles cancel out eg nh3 ch3F