Ionic, Covalent And Metallic Bonding

Question 1

How are ions formed by electron loss or gain

Answer 1

Ions which are 3 or less away from having a full outer shell will gain electrons and ions which at 3 or less away from having an empty shell will lose electrons

Question 2

What is the charge of group 1

Answer 2

+1

Question 3

What is the charge of group 2

Answer 3

2+

Question 4

What is the charge of group 3

Answer 4

3+

Question 5

What is the charge of group 5

Answer 5

-3

Question 6

What is the charge of group 6

Answer 6

-2

Question 7

What is the charge of group 7

Answer 7

-1

Question 8

What is the symbol of the silver ion

Answer 8

Ag+

Question 9

What is the symbol of the copper ion

Answer 9

Cu2+

Question 10

What is the symbol of the iron (2) ion

Answer 10

Fe2+

Question 11

What is the symbol of the iron (3) ion

Answer 11

Fe3+

Question 12

What is the symbol of the lead ion

Answer 12

Pb2+

Question 13

What is the symbol of the zinc ion

Answer 13

Zn2+

Question 14

What is the symbol of the hydrogen ion

Answer 14

H+

Question 15

What is the symbol of the hydroxide compound formed by ions

Answer 15

OH-

Question 16

What is the symbol of the ammonium compound formed by ions

Answer 16

NH4+

Question 17

What is the symbol of the carbonate compound formed by ions

Answer 17

CO3 2-

Question 18

What is the symbol of the nitrate compound formed by ions

Answer 18

NO3-

Question 19

What is the symbol of the sulfate compound formed by ions

Answer 19

SO4 2-

Question 20

Define ionic bonding

Answer 20

The strong electrostatic attractions between positively charged ions (cations) and negatively charged ions (anions)

Question 21

Why do compounds with giant ionic lattices have high melting and boiling points

Answer 21

Giant ionic lattices have strong ionic bonds which need lots of energy to break therefore needing a higher melting and boiling point

Question 22

Do ionic compounds conduct electricity

Answer 22

They do not when solid but do conduct when molten and in a aqueous solution

Question 23

How do ionic compounds sometimes conduct electricity

Answer 23

They do because in a aqueous or molten solution the ions can move but in a solid the ions can’t move

Question 24

What type of materials is a ionic bond made from

Answer 24

Metals and non-metals

Question 25

What is a covalent bond

Answer 25

The strong electrostatic attractions between a shared pair of electrons and the positive nuclei of two atoms

Question 26

How are covalent bonds formed

Answer 26

By atoms sharing a pair of electrons

Question 27

Why do simple molecular structure have low boiling points or are made from gases or liquids

Answer 27

They have weak intermolecular forces which need little energy to overcome

Question 28

Why do giant covalent structures have high melting and boiling points

Answer 28

They have strong covalent bonds which need a lot of energy to break

Question 29

Describe the structure of diamond

Answer 29

High melting and boiling points-giant covalent structures, strong covalent bonds (4 per carbon atom), lots of energy required to break therefore needing bonds

Question 30

Can diamonds conduct electricity and why

Answer 30

They cannot due to having localised electrons that are not free to move

Question 31

What is the material of diamond

Answer 31

Hard material-strong covalent bonds which require lots of energy to break, they are also arranged in a tetrahedral arrangement

Question 32

What is the structure of graphite

Answer 32

High melting and boiling points-giant covalent structures, strong covalent bonds (3 per carbon atom), weak forces of attraction between the layers, lots of energy required to break the bonds

Question 33

Does graphite conduct electricity and why

Answer 33

Yes because it has delocalised electrons that are free to move

Question 34

What type of materials is graphite and why is it good for pencil lead

Answer 34

Soft material-layers can slide off easily onto paper due to the weak forces of attraction between layers, carbon atoms are arranged in hexagons

Question 35

What is the structure of C60 fullerene

Answer 35

Low melting and boiling points-simple molecular structure, strong covalent bonds (3 per carbon atom), weak intermolecular forces of attraction between bonds, little energy is required to break weak intermolecular forces

Question 36

Does C60 fullerene conduct electricity and why

Answer 36

It does not because despite having delocalised electrons moving within a molecule they cannot jump from molecule to molecule

Question 37

What material is C60 fullerene

Answer 37

Slippery/soft material-weak intermolecular forces of attraction

Question 38

Why do covalent compounds not conduct electricity

Answer 38

They have localised electrons which are not free to move around

Question 39

What is metallic bonding

Answer 39

The strong electrostatic attract is between positively charged ions and delocalised electrons

Question 40

What materials make up metallic bonding

Answer 40

Metals

Question 41

What are 5 general properties of metals

Answer 41

High melting and boiling points, malleable, conduct electricity, ductile, shiny

Question 42

Can metallic bonds conduct electricity

Answer 42

Yes because they have delocalised electrons which are free to move

Question 43

Why do the melting and boiling points of substances with a simpler molecular structure increase with increasing relative molecular mass

Answer 43

We have to put in more energy to break the intermolecular forces as the relative molecular mass increases. This is because the intermolecular forces of attraction become stronger as the relative molecular mass increases

Question 44

What type of elements are in groups 1, 2 and 3 of the periodic table

Answer 44

Metals

Question 45

What type of elements are in groups 5, 6 and 7 of the periodic table

Answer 45

Non-metals

Question 46

What are the diatomic molecules

Answer 46

Hydrogen, oxygen, nitrogen, fluorine, chlorine, bromine, iodine