Brainscape's Knowledge GenomeTM

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


See full index

nat 5 chemistry > Bonding > Flashcards

Bonding Flashcards

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

What are the three main types of bonding ?

A

Covalent bonds
Metallic bonds
Ionic bonds

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

What is covalent bonds between?

A

Non-metals

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

What are metallic bonds between?

A

Metals

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

What are ionic bonds between ?

A

Compound containing metals and non-metals

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

What is the only group to exist as single atoms and do not bond ?

A

Noble gases

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

What do atom achieve when they bond ?

A

Full outer electron shell

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

What is a covalent bond?

A

The attraction between the two positive nuclei and a shared pair of electrons (negative)

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

What is a molecule?

A

A group of atoms held together by covalent bonds.

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

What are chemical bonds ?

A

Invisible forces of attraction between positive and negative charges that hold atoms together

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

What are the 2 types of covalent substances ?

A

Covalent molecular

Covalent network

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

What are covalent molecular structures like ?

A

Discrete and held together by weak intermolecular forces (called Van Der Waals force)

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

Why do covalent molecular substances have low melting and boiling points ?

A

Only weak Van Der Waals need to be broken

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

What do covalent network structures consist of ?

A

A giant lattice of atoms all covalently bonded to each other

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

Why do covalent network substances have high melting and boiling points?

A

Strong covalent bonds must be broken

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

Give 3 examples of covalent network?

A

Carbon diamond
Carbon graphite
Silicon dioxide

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

What is the difference between the melting point of a covalent network and a covalent molecular?

A

Covalent molecular : low mp/bp

Covalent network : high mp/bp

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

What is the difference in the type of bond broken to melt between a covalent network and a covalent molecular ?

A

Covalent molecular : intermolecular forces (weak Van Der Waals)
Covalent network : strong covalent bond

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

What condition can covalent molecules be at room temperature?

A

Solid
Liquid
Or gas

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

What condition are covalent networks at room temperature ?

A

Always solid

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

What are ionic bonds formed between?

A

Metals and nonmetals

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

How do ionic compounds form?

A

By transferring electron(s) from the metal to the nonmetal

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

When ionic compounds react, what happens to the metal atoms?

A

Loses electrons to become positively charged ions.

23
Q

When ionic compounds react, what happens to the nonmetal atoms?

A

Gain electrons to become negatively charged ions.

24
Q

What are the resulting ions considered as after an ionic compound has been formed?

A

The resulting ions are oppositely charged and attract each other

25
Q

What is the definition for ionic bonding ?

A

The force of attraction between positive and negative ions.

26
Q

Describe ionic bonds?

A

Very strong

27
Q

When an ionic bond forms what do both ions gain?

A

A full outer electron shell

28
Q

What structure do ionic compounds form?

A

A giant lattice of oppositely charged ions

29
Q

Why do ionic substances have high melting and boiling points?

A

Strong ionic bonds must be broken to separate them

30
Q

What condition are ionic substances in at room temperature?

A

Solid

31
Q

What is the only compound which would appear to be ionic but isn’t ?
State what it is, it’s condition at room temperature, what is its actual bonding, how we know this?

A

Titanium (IV) chloride
Liquid at room temp
Covalent molecular substance
Low melting/boiling point

32
Q

Describe the electrons on the outer shell of metal atoms ?

A

They are very loosely held and easily become delocalised.

33
Q

What are delocalised electrons attached to?

A

Their own nucleus and neighbouring nuclei.

34
Q

What is the definition for metallic bonding?

A

The force of attraction between positively charged ions and delocalised electrons.

35
Q

What does delocalised mean?

A

Able to move freely

36
Q

What is an electrical current?

A

A flow of charged particles (either electrons or ions)

37
Q

When will a substance conduct electricity ?

A

When charged particles are free to move through the material

38
Q

Describe the conductivity of covalent substances ?

A

Covalent substances (solid,liquid,solutions) do not conduct electricity since they are made up of molecules which are uncharged and there are no free charged particles

39
Q

What is the only covalent substance which conducts electricity and why?

A

Carbon (graphite) conducts electricity because it contains free electrons.

40
Q

Describe the conductivity of ionic substances and why?

A

Solid ionic substances do not conduct electricity because the ions are held tightly in an ionic lattice and are not free to move.

Ionic liquids(molten/in solution) will conduct electricity because ions are free to move

41
Q

What will melting or dissolving an ionic substance do?

A

Break down the lattice and allow ions to move freely.

42
Q

What is an electrolyte ?

A

An ionic liquid which conducts electricity.

43
Q

Describe the conductivity of metal elements and why ?

A

Metal elements (solid/liquid) are conductors of electricity because they contain delocalised electrons which are free to move.

44
Q

In terms of solubility in water, what do ionic compounds tend to be?

A

Soluble in water

45
Q

In terms of solubility in water, what do covalent substances tend to be ?

A

Insoluble in water

46
Q

What does electrolysis use electricity to do?

A

Break down ionic compounds

47
Q

What does ‘lysis’ mean ?

A

To break/breaking

48
Q

What ions move towards in terms of electrolysis?

A

The oppositely charged electrode

49
Q

Why is a DC power supply used?

A

So that electrodes stay the same charge throughout and the products could be identified at each electrode.

50
Q

What happens at the negative electrode during electrolysis ?

A

Positive ions (metals) gain electrons to become atoms.

51
Q

How can we show metal atoms gaining electrons or nonmetals losing electrons?

A

Write as an ion-electron equation

52
Q

Write the ion-electron equation for copper?

A

2+ -

Cu + 2e } Cu

53
Q

Give the ion-electron equation for chlorine?

A
  • -
    2Cl } Cl + 2e
    2
54
Q

What must ion-electron equations be for nonmetals ?

A

Reversed

nat 5 chemistry (13 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions