Chapter 5,6,24 -bonding and polymers

Question 1

What happens in ionic bonding?

Answer 1

Electrons are transferred from one atom to another

Question 2

What happens in covalent bonding?

Answer 2

When atoms share electrons

Question 3

Which type of bonding produces a charged atom?

Answer 3

Ionic bonding

Question 4

What type of atoms does covalent bonding occur between?

Answer 4

Two non metals

Question 5

What type of atoms do ionic bonds form between?

Answer 5

A metal and a non metal

Question 6

What is a positive ion called? What about a negative ion?

Answer 6

Positive is a cation, negative is an anion

Question 7

What are ionic lattices? What are they held together by?

Answer 7

Ionic lattices are made of tightly packed ions forming a 3D structure. They are held together by electrostatic forces

Question 8

What are electrostatic forces?

Answer 8

The force of attraction between positive and negative atoms

Question 9

Name the ion formula for Hydroxide, carbonate, sulfate, nitrate and phosphate?

Answer 9

OH-, CO3 2-, SO4-, NO3- and PO4-

Question 10

What is the name for an atom being stable and having a full outer shell? It has …

Answer 10

Noble has configuration

Question 11

What is the valency of an element?

Answer 11

The combining power of an element, related to the number of electrons on its outer shell, the bonds / electron transfers it has to make to become stable, 8 electrons on outer shell. So group 4 would be 4, 3 would be 3, 6 would be 2, etc

Question 12

Give some examples of simple covalent compounds

Answer 12

H2 O, CO2, N2, Cl2, NO(nitrogen oxide) NO2(nitrogen dioxide)

Question 13

In what state can ions only conduct?

Answer 13

Ions can only conduct in liquid as they are free to move

Question 14

Give some examples of properties of ionic bonding

Answer 14

They are brittle, conduct when free to move in a liquid, have high melting and boiling points, solid at room temperature

Question 15

What are intermolecular forces?

Answer 15

Forces between molecules

Question 16

Are intermolecular forces weak?

Answer 16

Yes. That’s why molecules separate easily and have a low melting point

Question 17

What are the bonds that hold covalently bonded atoms together? Are they strong or weak?

Answer 17

Strong covalent bonds hold the atoms together

Question 18

Why are simple covalent bonds liquid or gas at room temperature?

Answer 18

The intermolecular forces are weak so don’t require much energy to break and have a low melting point

Question 19

What are polymers?

Answer 19

Large molecules made of hundreds of monomers joined together in a chain

Question 20

What are plastics?

Answer 20

Synthetic polymers that can be shaped by heat or pressure

Question 21

What are monomers in a polymer joined together by?

Answer 21

Covalent bonds between atoms

Question 22

What are monomers?

Answer 22

Small molecules with double bonds so they can join to form polymers

Question 23

Name some properties of metals

Answer 23

Malleable, delocalised electrons/good conduction, high melting and boiling points, sonorous, tightly compact atoms, conduct heat

Question 24

What does sonorous mean?

Answer 24

It makes a deep or ringing sound

Question 25

What is a lattice?

Answer 25

A regular repeating pattern of atoms

Question 26

What side of the periodic table are metals on? What does this mean for the charge of the ion made in ionic bonding?

Answer 26

Metals are on the left hand side of the periodic table meaning they always loose electrons so always gain a positive charge

Question 27

What strong force holds delocalised electrons and positive nuclei in metals?

Answer 27

Strong electrostatic forces

Question 28

The more delocalised electrons a metal has the higher its...

Answer 28

Melting point is

Question 29

Name the 4 main types of diagrams and models of atoms and their bonding

Answer 29

Ball and stick diagram, ionic models, displayed formula, cross and dot diagrams

Question 30

What is the difference between simple covalent and giant covalent?

Answer 30

Giant covalent have many more covalent bonds that form a lattice structure, whereas in simple covalent atoms share electrons but are held together by weak intermolecular forces

Question 31

Give some examples of giant covalent structures

Answer 31

Graphite, diamond

Question 32

Which type of bonding conduct electricity?

Answer 32

Ionic, as a liquid, and metallic

Question 33

What are the 4 types of bonding?

Answer 33

Ionic, simple covalent, giant covalent and , metallic

Question 34

Give some examples of ionic compounds

Answer 34

Sodium chloride, NaCl Lithium Fluorine Copper sulfate, CuSO4

Question 35

Which is the only type of bonding which leaves its atoms not solid at room temperature?

Answer 35

Simple covalent bonding as it has a low melting point

Question 36

Name some properties of simple covalent bonding

Answer 36

``` Low melting/boiling point Doesn’t conduct No overall charge Small molecules Liquid/gas at room temperature ```

Question 37

How are metals malleable ?

Answer 37

They have no fixed directional bonds so they can be cut/moved into any form as they are not just in layers like lattices

Question 38

Why does an the loss of an electron always form a cation?

Answer 38

Loss of electron means there is more positive charge as there are more protons than electrons in the atom left over

Question 39

How are copper sulfate and copper sulfide different in terms of the elements they contain?

Answer 39

Copper sulfate contains oxygen atoms as well as copper and sulfide

Question 40

Describe a physical property test you could use to tell the difference between copper sulfide (fools gold)and metallic gold

Answer 40

Test it’s electrical conductivity, gold metal will conduct

Question 41

Suggest some reasons why graphite would be suitable in mobile touchscreens by referring to some of its properties

Answer 41

It’s strong as it’s held together by covalent bonds so it won’t smash easily Smooth and malleable so can be cut into layers Thin so it won’t add to weight of phone

Question 42

Fullerenes are made of carbon. Why do fullerenes have lower melting points than graphite or graphene ?

Answer 42

Because the intermolecular forces in fullerenes are weaker as there are less bonds

Question 43

Why does heating some molecules cause them to change state but not cause them to break apart?

Answer 43

They have weak intermolecular forces so molecules break apart but the bonds between atoms are strong so those don’t break apart

Question 44

What element are both graphite and diamond made from? They are allotropes of ...

Answer 44

Carbon | They are allotropes of carbon

Question 45

What is an allotrope?

Answer 45

Different forms/ structures of the same element with different structures of molecules of that element

Question 46

What are the similarities between graphite and diamond?

Answer 46

They are made of carbon, both solid, both giant covalent structures, strong covalent bonds

Question 47

What are the differences between graphite and diamond?

Answer 47

Graphite has bonds with 3 cartons (carbon surrounded by 3 others) therefore has one free electron as carbon is group 4. Diamond is carbon covalently bonded with 4 carbons, Graphite is softer Graphite conducts electricity

Question 48

Why does graphite conduct electricity? How?

Answer 48

Charge is able to flow through graphite as there is a free electron, as not all of the 4 electrons in some of the carbons are covalently bonded. This free electron becomes delocalised and can flow through the whole layer (the bonding layer) of the graphite

Question 49

Why is diamond extremely useful and strong?

Answer 49

It has very very strong covalent bonds as it is in a lattice structure and has all of the electrons and atoms covalently bonded, all 4 carbons covalently bonded to another carbon. This means it is strong and can be used on the edges of drills / tools

Question 50

Why is graphite soft and can be split into layers?

Answer 50

Graphite is soft as it is split into layers that can slide over each other, as they are only held weakly by intermolecular forces

Question 51

What is Graphene ?

Answer 51

A layer of graphite, one atom thick and able to conduct, not a simple molecule as it can keep extending

Question 52

What is graphenes lattice shape?

Answer 52

A one atom thick layer that keeps building / extending

Question 53

What are fullerenes?

Answer 53

Simple molecules ( which do have a limit to how far they extend), formed from carbon and are a spherical or tube shape.

Question 54

What are the properties of fullerenes ?

Answer 54

Low melting / boiling point, soft and slippery

Question 55

Name all the allotropes of carbon

Answer 55

Diamond, fullerenes, graphite and graphene (one layer of graphite)