Brainscape's Knowledge GenomeTM

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


See full index

Chemistry 4th form > Bonding > Flashcards

Bonding Flashcards

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

What is an ion?

A

Charged particles

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

Give an example of a single atom.

A

Na plus (+)

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

Give an example of a group of atoms

A

NO - 3

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

What is a negative ion?

A

Anion

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

What is a positive ion?

A

Cations

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

How are negative ions formed?

A

When atoms gain electrons

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

How are positive ions formed?

A

When atoms lose electrons

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

Gaining electons means…

A

Having more electrons than protons

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

Loosing electrons means…

A

Having more protons than electrons

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

how does the number of electrons lost or gained compared to the charge on the ion?

A

The number of electrons lost or gained is the same as the charge on the ion.

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

What is the charge if 2 electrons are lost?

A

2+

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

What is the charge if 3 electrons are gained?

A

3-

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

Which groups on the periodic table are metals?

A

1, 2, 3

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

Do groups 1,2 and 3 lose or gain electrons?

A

They lose electrons to form positive ions.

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

Which groups on the periodic table are non-metals?

A

5, 6, 7

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

Do groups 5, 6 and 7 gain or lose electrons?

A

They gain electrons to form negative ions

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

How does the group of the ion relate to the electrons in the outer shell?

A

Elements in the same group have the same number of electrons in their outer shell.

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

What is the charge of hydrogen?

A
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What is the charge of Hydroxide?

A
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What is the charge of Ammonium?

A
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What is the charge of carbonate?

A
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What is the charge of nitrate?

A
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What is the charge of sulfate?

A
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What is an ionic compound?

A

A transfer of electrons

25
Q

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

A

The metal atom loses electrons to form positive ions. The non-metal gains these electrons to form a negative ion.

26
Q

By what are these oppositely charged ions attracted to each other?

A

Electrostatic attractions.

27
Q

What is the name of the attraction between oppositely charged ions?

A

Ionic bond

28
Q

Give an example of ionic bonding

A

The reaction of sodium and chlorine.

29
Q

What is the overall charge of any ionic compound?

A

Zero
All the negative charges in the compound must balance all the positive charges.

30
Q

What do you need to work out the formula for the ionic compound?

A

The charges on the individual ions present

31
Q

What kind of structure do ionic compounds have?

A

A lattice structure

32
Q

What kind of structure do compounds with ionic bonding have?

A

Giant ionic structures

33
Q

How are the irons held together in a giant ionic structure?

A

In a closely packed, 3D, lattice arrangement

34
Q

Name, two features of ionic compounds.

A

High, melting point.
High boiling point.

35
Q

In what state do ionic, compounds conduct electricity?

A

When melted or dissolved in water.

36
Q

What Is covalent bonding?

A

When atoms bond by sharing pairs of electrons

37
Q

What do convalent substances contain?

A

Shared pair of electrons

38
Q

What sort of attraction is there in covalent bonding?

A

There is a strong electrostatic attraction between the negatively charged shared electrons and the positively charged nuclei.

39
Q

Describe the forces of attraction between molecules?

A

Weak

40
Q

Why are the melting and boiling points of simple molecular substances low?

A

Because the molecules are easily separated as they have weak intermolecular forces.

41
Q

Describe The relationship between the size of a molecule and the strength of attraction.

A

Intermolecular forces are stronger between molecules with a high relative molecular mass between smaller molecules. This is because there are more points along the larger molecule for the forces that act so more energy is needed to break these forces.

42
Q

What state are most molecular substances at room temperature ?

A

Gases or liquids

43
Q

Name a difference between giant ionic structures and giant covalent structures

A

Giant covalent structures have no charged ions.

44
Q

Do you giant covalent structures, have strong or weak covalent bonds.

A

Strong bonds - meaning takes a lot of energy to break them.

45
Q

Do giant covalent structures have high or low, melting and boiling points?

A

High melting and boiling points - as a lot of energy is required to break the bonds.

46
Q

Name, two properties of giant covalent structures.

A

They don’t conduct, electricity, except graphite.
They are insoluble in water.

47
Q

What kind of atoms are diamond and graphite made up of?

A

Only carbon atoms.

48
Q

How many covalent bonds does diamonds have?

A

Four covalent bonds formed by carbon atoms.

49
Q

Does Diamond have high or low melting point?

A

High melting point as it has very strong covalent bonds.

50
Q

Why does diamond not conduct electricity?

A

Because it has no free electrons or ions.

51
Q

What makes diamonds hard?

A

To strong covalent bonds, hold the atoms in a very rigid, lattice structure.

52
Q

How many covalent bonds does graphite have?

A

Three. Covalent bonds, creating layers of carbon atoms.

53
Q

What are the carbon layers held together by in graphite?

A

Weak intermolecular forces.

54
Q

What makes graphite, soft and slippery?

A

The weak, intermolecular forces are free to slide over each other.

55
Q

Describe graphite, melting point.

A

The fight has a high melting point as the layers of carbon need loads of energy to break

56
Q

How is graphite able to conduct electricity?

A

Three out of carbon’s four outer electrons are used in bonds, so each carbon atom has one electron that delocalised and can move.

57
Q

describe C. 60 fullerene

A

A simple molecular substance made of 60 carbon atoms in which a hollow spheres. Made up of large covalent molecules. It’s not a giant covalent structure

58
Q

What makes the C 60 fullerene material, soft?

A

Molecules are only held together by intermolecular forces, so they can slide over each other.

59
Q

Then why C, 60 fullerene is a poor conductor of electricity

A

It has one delocalised electron however, the electrons can’t move between the molecules.

Chemistry 4th form (6 decks)

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