Chapter 1 -bonding and polymers Flashcards Preview

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Flashcards in Chapter 1 -bonding and polymers Deck (55):
1

What happens in ionic bonding?

Electrons are transferred from one atom to another

2

What happens in covalent bonding?

When atoms share electrons

3

Which type of bonding produces a charged atom?

Ionic bonding

4

What type of atoms does covalent bonding occur between?

Two non metals

5

What type of atoms do ionic bonds form between?

A metal and a non metal

6

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

Positive is a cation, negative is an anion

7

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

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

8

What are electrostatic forces?

The force of attraction between positive and negative atoms

9

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

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

10

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

Noble has configuration

11

What is the valency of an element?

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

12

Give some examples of simple covalent compounds

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

13

In what state can ions only conduct?

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

14

Give some examples of properties of ionic bonding

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

15

What are intermolecular forces?

Forces between molecules

16

Are intermolecular forces weak?

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

17

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

Strong covalent bonds hold the atoms together

18

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

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

19

What are polymers?

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

20

What are plastics?

Synthetic polymers that can be shaped by heat or pressure

21

What are monomers in a polymer joined together by?

Covalent bonds between atoms

22

What are monomers?

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

23

Name some properties of metals

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

24

What does sonorous mean?

It makes a deep or ringing sound

25

What is a lattice?

A regular repeating pattern of atoms

26

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

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

27

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

Strong electrostatic forces

28

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

Melting point is

29

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

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

30

What is the difference between simple covalent and giant covalent?

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

31

Give some examples of giant covalent structures

Graphite, diamond

32

Which type of bonding conduct electricity?

Ionic, as a liquid, and metallic

33

What are the 4 types of bonding?

Ionic, simple covalent, giant covalent and , metallic

34

Give some examples of ionic compounds

Sodium chloride, NaCl
Lithium Fluorine
Copper sulfate, CuSO4

35

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

Simple covalent bonding as it has a low melting point

36

Name some properties of simple covalent bonding

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

37

How are metals malleable ?

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

38

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

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

39

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

Copper sulfate contains oxygen atoms as well as copper and sulfide

40

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

Test it’s electrical conductivity, gold metal will conduct

41

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

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

42

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

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

43

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

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

44

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

Carbon
They are allotropes of carbon

45

What is an allotrope?

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

46

What are the similarities between graphite and diamond?

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

47

What are the differences between graphite and diamond?

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

48

Why does graphite conduct electricity? How?

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

49

Why is diamond extremely useful and strong?

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

50

Why is graphite soft and can be split into layers?

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

51

What is Graphene ?

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

52

What is graphenes lattice shape?

A one atom thick layer that keeps building / extending

53

What are fullerenes?

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

54

What are the properties of fullerenes ?

Low melting / boiling point, soft and slippery

55

Name all the allotropes of carbon

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