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Chemistry > TOPIC C2 > Flashcards

TOPIC C2 Flashcards

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1
Q

Which groups are most likely to form Ions

A

Groups 1,2 and 6, 7

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2
Q

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

A

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

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3
Q

What is the attraction between the two electrostatic force

A

This is called ionic bond

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4
Q

What does the dot and cross diagrams show

A

It shows the arrangement of elements on an atom or ion

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5
Q

What is the Ionic compounds structure called

A

A giant ionic lattice

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6
Q

What are the properties of ionic bonding

A

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

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7
Q

How are covalent bonds formed

A

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

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8
Q

What does a covalent bond provide

A

It provides an extra shared electrons for each of them

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9
Q

Where does covalent bonding happen

A

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

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10
Q

What are the properties of simple molecular substances

A

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

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11
Q

How are the structure of the giant covalent all bonded together

A

By a strong covalent bond

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12
Q

Giant covalent have

A

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

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13
Q

What are the main examples of a giant covalent bond

A

Diamonds and graphite

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14
Q

What are the attraction that hold atoms together

A

In a regular structure and it’s called metallic bonding

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15
Q

Describe the structure of a diamond molecule

A

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

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16
Q

Describe the structure of a Graphite molecules

A

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

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17
Q

Explain the structure of the silicon dioxide

A

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

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18
Q

Is diamond hard

A

Yes very hard

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19
Q

What is diamond made out of

A

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

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20
Q

What are Ions

A

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

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21
Q

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

A

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

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22
Q

Why so atoms need to have a full outer shell

A

Because if they have an outer shell they age her stable

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23
Q

What happens when metals form ions

A

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

24
Q

What happens to non-metals when they for ions

A

They gain electrons into their outer shell to form negative ions

25
Q

Why do ionic compounds have a high melting and boiling point

A

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

26
Q

When the ions are solid do they conduct electricity

A

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

27
Q

What happens what the compounds melt

A

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

28
Q

What happens then the ionic compounds dissolve in water

A

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

29
Q

Covalent Bonds

A

Sharing Electrons

30
Q

What happens when non-metals atoms bond together

A

They share pairs of electrons to make covalent bonds

31
Q

When do atoms share electrons

A

In their outer shell

32
Q

When does covalent bonding happen

A

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

33
Q

What do substances containing covalent bonds usually have

A

Simple molecular structures

34
Q

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

A

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

35
Q

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

A

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

36
Q

What are most molecular substances at a room temperature

A

Gases and liquid at a room temperature

37
Q

What increases the intermolecular forces increases

A

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

38
Q

Do molecular compounds conduct electricity

A

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

39
Q

What is the structure of the giant covalent

A

Macromolecules

40
Q

How are the atom bonded to together in giant covalent structure

A

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

41
Q

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

A

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

42
Q

If particles don’t contain charged particles

A

It means they don’t conduct electricity

43
Q

What is metallic bonding

A

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

44
Q

Is metallic bonding strong true or false

A

True

45
Q

What to substances are held together by metallic bonding

A

Metallic elements and metallic alloys

46
Q

What are compounds metallic compounds like

A

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

47
Q

What does it mean if most metals are melleable

A

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
Q

Why is alloys more useful than metals

A

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
Q

Why are alloys harder then pure metals

A

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
Q

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

A

It’s solid

51
Q

If it’s a above the boiling point its

A

It’s a gas

52
Q

If it’s between the two points it’s

A

Liquid

53
Q

What are the three states of matter

A

Solid
Liquid
Gas

54
Q

Graphite is very soft

A

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

55
Q

Diamond if very hard

A

It is made up of four covalent bonds

56
Q

Why does graphite conduct electricity

A

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

Chemistry (5 decks)

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