Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > C3 Structure And Bonding > Flashcards

C3 Structure And 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

Do opposite charges attract or repel

A

Attract

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

Why are metals alloyed

A

To increase strentgh

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

Intermolecular force

A

The force that arise between the molecules of a substance

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

What boiling, melting point do molecules have

A

Low

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

Ionic lattice

A

lattice is formed as ions attract each other and form a pattern

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

Why ionic compounds have a high melting point

A

Large amounts of energy needed to break the many strong bonds

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

Double bond in diatomic molecule

A

Forms between a carbon atom and an oxygen atom

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

When do ionic compounds conduct electricity

A

When molten or dissolved in water

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

Examples of small molecules which contain covalent bonds

A

Nitogen

Water

Ammonia

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

How covalent bond forms

A

When pairs of electrons are shared by atoms

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

How size of molecule affect boiling melting points

A

Larger molecules have higher boiling and melting points

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

Substances that would have weak intermolecular forces

A

Gases, liquids or low melting point solids

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

How double and triple covalent bonds formed

A

When more than one pair of electrons are shared between the atoms for a full outer shell

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

How surface area to volume increases as particle size reduces

A

Decreasing the length of a cube by 100 increases its surface area by 100

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

Can nanoparticles be used in sun cream

A

Yes

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

Uses of nanoparticles

A

Drug delivery

Diagnostic

Tissue engineering

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

Advantages of using nanoparticles

A

Lower costs

Produce stronger and lighter wind turbines

Can save energy

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

Disadvantages of using nanoparticles

A

Lung inflammation

Heart problems

19
Q

Why nanotechnology research should continue

A

Can change dental medicine, healthcare and human life

20
Q

How to classify a particle as a coarse, fine or nanoparticles

1 x 10 and 2.5 x 10

A

-5 -6
Coarse - 10 10
-7 -6
Fine - 10 10

21
Q

Describe, with an example, how a Group 1 metal atom becomes a positive ion

A

+
Lithium loses 1 electron to become Li

22
Q

Factors that affect rate of evaporation

A

Temperature

Surface area

Wind speed

23
Q

Charges of ion group 1,2,6,7

A

Group 1 = +1

Group 2 - +2

Group 6 = -2

Group 7 = -1

24
Q

How unfamiliar elements become ions

A

Metal atoms lose electrons to form cations

Non-metal atoms tend to gain electrons and form anions

25
Q

How the position of an element on the periodic table relates to the charge on its most stable monatomic ion

A

Elements often form anions with negative charge

26
Q

Ratio of metal and non-metal ions in compounds

A

2:1

27
Q

Why substances have different melting and boiling points from each other

A

The stronger the forces between particles, the higher its melting and boiling points

28
Q

Properties of diamond

A

Hard in nature

Molecules closely packed

No prescence of free carbon atoms

29
Q

Properties of graphite

A

High melting and boiling points

Good electrical conductivity

Softness

30
Q

Physical properties of fullerenes

A

Behaviour depends on temperature

31
Q

Physical properties of metals

A

Malleable

Ductile

Good conductors of heat and electricity

32
Q

Structure of pure metal

A

Giant metallic structure

33
Q

Do giant covalent structure have high or low melting point

A

High

34
Q

Describe relationship between graphite and graphene

A

Graphene is one single layer of graphite

35
Q

Explain the structure of fullerenes

A

Hexagonal rings of carbon atoms joined by covalent bonds

36
Q

Use for graphite

A

Used in pencils, lamps, batteries

37
Q

Use for diamonds

A

Embedded into saw blades

Drill bits

Grinding wheels

38
Q

How metals form giant structures

A

The outer shell electrons become delocalised and surround the positive metal ions

39
Q

Why small molecules don’t conduct electricity

A

Small molecules have no overall electric charge

40
Q

Why ionic compounds conduct electricity in molten state

A

Ions break free to move and can conduct electricity

41
Q

Process of melting

A

Molecules of a solid speed up enough that the motion overcomes the attraction so molecules can move past each other as a liquid

42
Q

Process of boiling

A

A liquid turns into vapour when heated to its boiling point

43
Q

Process of condensing

A

Water vapour in the air is changed into liquid water

Chemistry (4 decks)

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