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Flashcards in TOPIC C2 Deck (56):
1

Which groups are most likely to form Ions

Groups 1,2 and 6, 7

2

What happens when a non-metal and a metal react together

The metal atoms loses electrons to form a positively charged ion and the non-metal gains these electrons to form a negatively charged ions

3

What is the attraction between the two electrostatic force

This is called ionic bond

4

What does the dot and cross diagrams show

It shows the arrangement of elements on an atom or ion

5

What is the Ionic compounds structure called

A giant ionic lattice

6

What are the properties of ionic bonding

They all have a high boiling and melting point(because of the strong bonds)
They compounds can’t conduct heat when they’re a solid
When the ionic compounds melt the ions are free to move they’ll carry electric current

7

How are covalent bonds formed

When non-metal atoms bond together, they share pairs of electrons to make covalent bonds

8

What does a covalent bond provide

It provides an extra shared electrons for each of them

9

Where does covalent bonding happen

In compounds is non-metals and in non-metal elements

10

What are the properties of simple molecular substances

Melting and boiling point are very low
Gas or liquid at a room temperature
They don’t conduct heat

11

How are the structure of the giant covalent all bonded together

By a strong covalent bond

12

Giant covalent have

A very highly melting and boiling point as lots of energy if needed to beak the covalent bonds between the atoms

13

What are the main examples of a giant covalent bond

Diamonds and graphite

14

What are the attraction that hold atoms together

In a regular structure and it’s called metallic bonding

15

Describe the structure of a diamond molecule

Each carbon atom forms four covalent bonds in a very rigid giant covalent structure

16

Describe the structure of a Graphite molecules

Each carbon atom forms three covalent bonds to create layers of hexagons. Each carbon atom also has one delocalised electron

17

Explain the structure of the silicon dioxide

Sometimes called silica this is what sand is made out of. Each grain of sand is one haunt structure of silicon and oxygen

18

Is diamond hard

Yes very hard

19

What is diamond made out of

A giant covalent structure,made up of carbon atoms that each form four covalent bond

20

What are Ions

They are charged particles- they can be single atoms or groups of atoms

21

What is the point of atoms trying to gain or lose electrons

to form ions, they are trying to do it to get a full putt shell like the nobles (stable electric structure)

22

Why so atoms need to have a full outer shell

Because if they have an outer shell they age her stable

23

What happens when metals form ions

They lose electrons from their outer shell to form their positive ions

24

What happens to non-metals when they for ions

They gain electrons into their outer shell to form negative ions

25

Why do ionic compounds have a high melting and boiling point

Because the many strong bonds between ions so therefore it takes a lot of energy to break the attraction

26

When the ions are solid do they conduct electricity

Because they are solid and held in place they done conduct electricity

27

What happens what the compounds melt

They ions are free to move and they’ll carry electric current

28

What happens then the ionic compounds dissolve in water

The ions separate and are all free to move in the solution, so they’ll carry electric current

29

Covalent Bonds

Sharing Electrons

30

What happens when non-metals atoms bond together

They share pairs of electrons to make covalent bonds

31

When do atoms share electrons

In their outer shell

32

When does covalent bonding happen

It happens in the compounds of non-metals and in non-metal elements

33

What do substances containing covalent bonds usually have

Simple molecular structures

34

What are the molecules held together by in a simple molecular substance

Very strong covalent bonds so the forces between them is vey weak

35

Why do you need to break the feeble intermolecular force but not the covalent bonds in simple molecular

It’s to melt or boil a simple molecular compound so the melting and boiling point are easily parted from each other

36

What are most molecular substances at a room temperature

Gases and liquid at a room temperature

37

What increases the intermolecular forces increases

As the molecular get bigger so does the energy needed to break then down and the melting and boiling point increases too

38

Do molecular compounds conduct electricity

Simple because they aren’t charged so there are No free electrons or ions

39

What is the structure of the giant covalent

Macromolecules

40

How are the atom bonded to together in giant covalent structure

All the atoms are bonded to each other by strong covalent bonds

41

Why do giant covalent bond have a high melting and boiling point

Because a lot of energy is needed to break the covalent bonds between the atoms

42

If particles don’t contain charged particles

It means they don’t conduct electricity

43

What is metallic bonding

The strong forces of electrostatic attention between the positive metal ions and the shared negative electrons

44

Is metallic bonding strong true or false

True

45

What to substances are held together by metallic bonding

Metallic elements and metallic alloys

46

What are compounds metallic compounds like

They have a high boiling and melting point so they are solid at room temperature

47

What does it mean if most metals are melleable

The layers of atoms in a metal can slide over each other
This means that they can be bent or hammered or rolled into flat sheets

48

Why is alloys more useful than metals

Because it is a mixture of two or more metals or a metal and another element. Alloys are Hardee’s and so more useful then pure metals

49

Why are alloys harder then pure metals

Different elements have different sized atoms, so when another element is mixed with a pure metal, the new metal atoms will distort the layers of metal atoms

50

It’s a temperatures below the melting point of a substance it’s

It’s solid

51

If it’s a above the boiling point its

It’s a gas

52

If it’s between the two points it’s

Liquid

53

What are the three states of matter

Solid
Liquid
Gas

54

Graphite is very soft

Because there aren’t much bonds between the layers the hold together weekly

55

Diamond if very hard

It is made up of four covalent bonds

56

Why does graphite conduct electricity

Because each carbon atom has one electron that’s delocalised and can move