Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry Paper 1 > Topic 2 - Bonding > Flashcards

Topic 2 - Bonding Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

What is a cation?

A

Positive ions that are formed when when metal atoms lose electrons (in ionic bonding it would be a + charge)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is an anion?

A

Negative ions that are formed when non-metals gain electrons (in ionic bonding they’d have a - charge)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is an ionic bond?

A

An ionic bond is a strong electrostatic force of attraction between oppositely charged ions.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What are most ionic bonds formed between?

A

A metal and a non metal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What ion will form if a group1/group 2 element lose an electron?

A

Group 1 = +

Group 2 = 2+

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What ion will form if a group 6/group 7 element gain electrons?
.

A

Group 6 = 2-

Group 7 = -

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

How are ionic compounds formed?

A

By the losing or gaining of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What holds ionic compounds together?

A

Strong electrostatic forces of attraction between oppositely charged ions (ionic bonds)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

How is a lattice structure formed?

A

The strong ionic bonds allow loads (billions) of ions to be packed together in a regular repeating arrangement

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is the polyatomic ion for sulfate?

A

2-
SO
4

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What’s the polyatomic ion for nitrate?

A

-
NO
3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is the polyatomic ion for carbonate?

A

2-
CO
3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What’s the polyatomic ion for hydroxide?

A

-

OH

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What’s the polyatomic ion for ammonium?

A

+
NH
4

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Why do ionic compounds have high melting and boiling points?

A

Because they’re ionic bonds are held together by strong electrostatic forces of attraction between ions which need a lot of energy to overcome/break.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Why do some ionic compounds have a higher melting/boiling point?

A

Some ions have more than one charge so these highly charged ions will attract other ions more strongly and more energy is needed to overcome the strong electrostatic forces of attraction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What does a substance need to conduct electricity?

A

It must contain charged particles

These particles must be free to move

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

When can an ionic compound conduct electricity ?

A

When it is in an aqueous solution

19
Q

Why can’t ionic compounds conduct electricity in a solid state?

A

Because it is the charged ions that carry the current of electricity and in a solid state these ions are not free to move
However, in an aqueous solution, the ions are free to move and so they conduct electricity

20
Q

What are anions (negative ions) attracted to?

A

The positive electrode I.e. the anode

21
Q

What are cations (positive ions) attracted too?

A

The negative electrode I.e. the cathode

22
Q

What is a covalent bond?

A

A shared pair of electrons

23
Q

What are covalent bonds normally formed between ?

A

Non-metals

24
Q

When do atoms form double bonds?

A

When the atoms share two pairs of electrons

25
Q

Why do covalent bonds I.e. hydrogen have low melting and boiling points?

A

They have weak intermolecular forces which don’t need a lot of energy to overcome break
However the covalent bonds themselves are strong

26
Q

What is the valency?

A

The number of covalent bonds formed

I.e. oxygen has a double bond so it has two bonds so it has a valency of 2

27
Q

Why can’t covalently bonded molecules conduct electricity?

A

Because in a covalent bond, electrons are shared between two atoms.
The strong forces between the negatively charged electrons and the positively charged nucleus hold the electrons in place
Therefore, the electrons can’t move and the current can’t be carried/flow.

28
Q

Why do long polymers have higher melting/boiling points than smaller polymers?

A

Because they have more intermolecular forces

29
Q

What are the properties of fullerene?

A

It has weak intermolecular forces between the molecules so it has low melting points
The weak forces also make them soft and slippery
However, the molecules themselves are strong due to covalent bonds

30
Q

What are the properties of graphene?

A

It is very light as it’s only one atom thick
However, the covalent bonds make it strong
Electrons are free to move across its surface so it is a good electrical conductor

31
Q

What are graphite and diamond both examples of?

A

Giant covalent structures

32
Q

What are the properties of graphite?

A

It has 3 covalent bonds creating sheets of carbon atoms (the 3 strong covalent bonds are hard to overcome to so it has high melting point)
Electrons are free to move and are delocalised so graphite is a good electrical conductor (useful for making electrodes)
It doesn’t have covalent bonds between the layers - the layers are held together very weakly which causes the layers to slide past each other
This makes graphite soft and slippery
(So it’s ideal as a lubricating material)

33
Q

What are the properties of diamond?

A

Has 4 strong covalent bonds which take a lot of energy to break so it has a high melting point
The covalent bonds also hold the atoms in a rigid lattice which makes diamond hard
(This is why diamond is used to make tools/strengthen cutting tools)
It is an electrical insulator because it has no free delocalised electrons(no free charged particles)

34
Q

What are the properties of metals?

A 
High melting points (as solids)
Shiny (when polished)
Malleable
High density
Good conductors of electricity
35
Q

What are the properties of non metals?

A 
Low melting points
Not usually shiny (as solid)
Brittle (hard but breakers easily) - when a solid
Low density 
Poor conductors of electricity
36
Q

What is metallic bonding?

A

The electrostatic attraction between the positive metal ions and the negative delocalised electrons

37
Q

Why do metals have high melting and boiling points?

A

The electrostatic attraction is strong so it needs a lot of energy to break/overcome

38
Q

Why are metals malleable?

A

When you hit the metal, it doesn’t shatter because the layers of ions slide over each other
The sea of electrons holds the ions together so the metal changes shape instead of breaking

39
Q

Why can metals conduct electricity?

A

Because it has a sea of delocalised electrons which are free to move

40
Q

What happens when you apply a voltage/current to both sides of a metal?

A

The electrons will flow towards the positive side.

This flow of electrons transfers energy and forms an electrical current

41
Q

Why do some metals have a higher electrical conductivity?

A

They have a higher number of delocalised electrons
Sodium is a + ion and will contribute one electron to the sea of delocalised electrons
Magnesium is a 2+ ion and will contribute two electrons so it has a higher conductivity

42
Q

What substances are soluble/insoluble in water?

A

Most ionic compounds are soluble
A few simple covalent structures are soluble (not a lot)
Giant covalent are insoluble
Metals are insoluble

43
Q

What is a problem with dot and cross diagrams?

A

Doesn’t show the structure formed

44
Q

What are the problems with metallic models?

A

Doesn’t show that the ions will be vibrating all the time (but does show that metal ions are held in a lattice)

Chemistry Paper 1 (6 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions