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GCSE Chemistry > C2.2 Bonding > Flashcards

C2.2 Bonding Flashcards

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1
Q

List the physical properties of metal elements.

A

They are shiny
Their melting and boiling point are usually high
They are in the solid state at room temperature
They are malleable
They are ductile so they can be pulled into wires
They are good conductors of thermal and electricity

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2
Q

Define a physical property

A

A physical property is a characteristic that can be observed or measured

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3
Q

What do non-metals produce when they react with each other?

A

Non-metals react with each other to produce compounds that consist of molecules.

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4
Q

How did Mendeleev arrange all the elements in his periodic table?

A

In the order of increasing atomic weight, and he grouped together the ones with similar chemical properties.

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5
Q

Metal and oxygen react to produce…

A

…metal oxides

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6
Q

Non-metals and oxygen form to produce…

A

…non-metal oxides

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7
Q

When metal oxides dissolve in water what do they produce?

A

They produce alkaline solutions

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8
Q

What direction do ionic bonds act in an ionic compound?

A

They act in all directions

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9
Q

Do metals react with each other? If not what do they form

A

Metals do not react with each other but instead they mix to form alloys.

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10
Q

When non-metal oxides dissolve in water, what do they produce?

A

They produce acidic solutions

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11
Q

Why are metals good conductors of heat and electricity?

A

This is because they contain a sea of delocalised electrons which move freely through the metal, carrying the electrical current.

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12
Q

What does the group the lemony is in tell you about the element’s electronic configuration?

A

It tells you the amount of electrons in the outer shells

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13
Q

What does the electronic structure of an element show?

A

The electronic structure of an element shows how the electrons are arranged in the atoms.

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14
Q

How bonds do each carbon form in a diamond?

A

Four covalent bonds

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15
Q

Define an ion

A

An ion is an electrically charged particle formed when an atom, or group of atoms, loses or gains electrons to obtain a full outer shell.

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16
Q

What is a chemical property?

A

A chemical property is a characteristic of a substance that can only be determined by studying its chemical reactions.

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17
Q

Do giant covalent lattices have a high melting and boiling point?

A

They have a very high melting and boiling points because the atoms are boned to each other by strong covalent bonds.

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18
Q

What does the period the element is in tell you about the electronic structure?

A

The period tells you how many shells are in the electronic configuration

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19
Q

Describe the structure of ionic compounds.

A

Ionic compounds have a giant ionic lattice structure.

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20
Q

What are the ions held in place by in an ionic compound?

A

They are held in place by ionic bonds

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21
Q

Describe ionic bonds

A

Ionic bonds are strong electrostatic forces of attraction between oppositely charged ions

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22
Q

Do the ions only bonds to the ions they gained or donated an electron from/to?

A

No

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23
Q

What type of bonds do group 4 elements form?

A

They form covalent bonds

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24
Q

List the physical properties of non-metal elements

A

They have a dull appearance
Their melting point boiling point are usually low
About half are in the solid state and half are in the gas state at room temperature
They are brittle so they shatter when hammered
They are non-ductile so they snap when pulled
They are poor conductors of heat and electricity

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25
Q

List the properties of graphite

A 
Lustrous
High melting point
Insoluble in water
Black and opaque 
Slippery
And electrical conductor
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26
Q

What are the disadvantages of display formulas?

A

Can’t show space between atoms
Does not show the 3D shape of the molecule
We don’t know the strength of the bonds
It doesn’t show electron movement

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27
Q

Do ionic compounds have high melting and boiling points? Why/why not?

A

They have high melting and boiling point due to their strong electrostatic forces of attraction as it takes a large amount of energy to overcome this attraction.

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28
Q

Do ionic compounds dissolve easily in water?

A

Yes

29
Q

What are the disadvantages of ball and stick models?

A

There aren’t enough colours to show all the elements
Don’t know the strength of bonds
We can’t show space between atoms
It doesn’t show electron movement
The size of atoms and the length of bonds are exaggerated

30
Q

What is a covalent bond?

A

A covalent bond is a shared pair of electrons

31
Q

Does diamond conduct electricity? Why/why not?

A

Diamonds don’t conduct electricity because they don’t have any free electrons or ions.

32
Q

From the first shell to the fourth shell what are the maximum number of electrons that can go in each one?

A

First-2
Second -8
Third-8
Fourth-18

33
Q

Between what type of elements do covalent bonds form?

A

Covalent bonds form between two non-metal atoms when the atoms get close enough to share electrons in their outer shells

34
Q

Explain the melting and boiling point of simple covalent compounds.

A

Simple covalent compounds have a low boiling and melting point because they have weak intermolecular forces so not much energy is needed to overcome a simple covalent compound

35
Q

Why were there spaces in Mendeleev’s periodic table?

A

He left space for the elements that he though existed but we’re not yet discovered, and predicted their properties from those of nearby elements.

36
Q

Why are diamonds hard?

A

Diamonds are hard because each carbon atoms forms four covalent bonds in a very rigid giant covalent structure.

37
Q

Describe the appearance of graphite.

A

Black and opaque

38
Q

What are the advantages of ball and stick models?

A

There are different colours for different molecules.

Shows 3D shape

39
Q

What is the difference between a giant ionic lattice and a giant covalent lattice?

A

Giant covalent lattices don’t contain charged particles whereas giant ionic lattices do.

40
Q

What does lattice mean?

A

Regular arrangement

41
Q

Can ionic compounds conduct electricity?

A

Solid ionic compounds don’t conduct electricity because the ions are fixed in their place and can’t move.
But molten ionic compounds can conduct electricity because the ions are free to move around and will carry an electric current.

42
Q

What are the advantages of displayed formulas?

A

We have a symbol for each element so we can show each element

43
Q

What is the maximum number of covalent bonds carbon can form?

A

Carbon atoms can form up to four covalent bonds.

44
Q

Does diamond have a high melting point? Why/why not?

A

They have a very high melting and boiling point because it takes a lot of energy to break all the covalent bonds as it has many.

45
Q

List the properties of diamond

A 
Lustrous
Transparent and colourless
Hard
High melting point
Insoluble in water
Insulator
46
Q

List the properties of graphene

A 
Strongest material ever tested 
Very light
Better electricity conductor than graphite
Flexible 
Very High melting and boiling points
47
Q

What did Henry Moseley discover?

A

He discovered that an atom’s atomic number was actually the number of protons in its nucleus. This also explained how Mendeleev was right to swap tellurium and iodine around.

48
Q

Describe the bonds between the layers in graphite.

A

The layers in graphite are held together weekly so they are slippery and can be rubbed off onto paper to leave a black mark .

49
Q

Do giant covalent lattices conduct electricity? Why /why not?

A

They don’t conduct electricity at all (not even when they are molten)

50
Q

What are the patterns of chemical properties in the periodic table?

A
  • Elements are arranged in order of increasing atomic number
  • The atomic number is the number of protons in an atom
  • The number of electrons in an atom is equal to the number of protons
  • Electronic structure is determined by the number of electrons
  • The electronic structure of an element determines its chemical properties
51
Q

What is polymerisation?

A

It is a reaction when monomers join together to form polymers.
It requires high pressure and a catalyst.

52
Q

Melting and boiling point of graphite?

A

Graphite’s got a high melting point because the covalent bonds need loads of energy to break

53
Q

Describe a giant covalent structure.

A

A giant covalent structure consists of many non-metal atoms joined by covalent bonds and arranged in a repeating regular pattern called a giant lattice.

54
Q

How can graphite conduct electricity?

A

Since only three out of each carbon’s four outer electrons are used in bonds, there are lots of delocalised electrons that can move so graphite can conduct electricity.

55
Q

Define allotropes

A

Allotropes are different forms of an element in the same but with different atomic arrangements.

56
Q

How many covalent bonds do each carbon atom form in graphite?

A

Each carbon atom atom forms three covalent bonds.

57
Q

Thermosoftening polymer

A

Their chains are held by weak intermolecular forces so the chains are free to slide over each other. This means that the plastic can be stretched easily and will have a low boiling point

58
Q

How are the carbon atoms arranged in fullerenes?

A

The carbon atoms are arranged in rings

59
Q

List the properties of fullerenes

A

Soft and slippery
Brittle
Electrical conductors because they have delocalised electrons
High melting and boiling point but not as high as diamond, graphite and graphene

61
Q

Thermosetting polymer

A

Chains joined together by strong covalent bonds, called cross linking.
These plastics have higher melting points, are rigid and can’t be stretched as the cross-links hold the chains firmly together.

62
Q

What didn’t Mendeleev know when he developed his periodic table?

A

He didn’t know about atomic structure

63
Q

What are metallics bonds?

A

Metallic bonds are strong electrostatic forces of attraction between the delocalised electrons and the closely packed positively charged metal ions.

64
Q

Why did Mendeleev swap the positions of tellurium and iodine?

A

Because he felt that this matched their chemical properties better

65
Q

Who discovered argon?

A

Lord Rayleigh and William Ramsay in 1894

66
Q

Describe what monomers are.

A

Monomers are simple molecules so they consist of a few non-metal atoms joined together by covalent bonds.

67
Q

What is graphene?

A

Graphene is a single sheet of graphite

68
Q

Describe the appearance of diamond.

A

Pure diamonds are lustrous and colourless

69
Q

Are covalent bonds strong? Why/why not?

A

Covalent bonds are strong because there’s a strong electrostatic force of attraction between the nuclei and the shared electrons but the intermolecular forces between the molecules are weak.

69
Q

How are polymers formed?

A

They are formed when lots of small molecules called monomers join together.

GCSE Chemistry (9 decks)

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