Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > Chemistry- Structure and Bonding > Flashcards

Chemistry- Structure and 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

Electrons always occupy …. .

A

shells

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

The lowest energy levels (those closest to the nucleus) are always filled ….. .

A

first

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

1st Shell:
2nd Shell:
3rd Shell:

A

2,8,8

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

A substance which contains only one sort of atom is called an

A

element

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

The atomic particle with a positive charge is the ……. .

A

proton

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

The atomic particle with a negative charge is the ……. .

A

electron

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

The atomic particle with no charge is the …….. .

A

neutron

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

The part of an atom in which ……… are found is the nucleus.

A

protons

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

……… have no overall electrical charge.

A

Atoms

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

In a …………. ………, the number of electrons is equal to the number of protons.

A

neutral atom

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

Each ……… in an atom is at a particular energy level (in a particular shell).

A

electron

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

The atomic particle with a negligible mass is the ………. .

A

electron

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

The simplest atom is the ………… atom which contains one proton and one electron.

A

hydrogen

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

Neutrons are found in part of the atom called the ……. .

A

nucleus

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

All atoms of a particular element have the same number of …….. in their nuclei.

A

protons

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

The mass number of carbon is ….

A

12

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

The proton number of carbon is …..

A

6

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

The number of protons in one atom of fluorine is …..

A

9

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

The mass number of fluorine is ……

A

19

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

The number of protons in one atom of sodium is …..

A

11

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

Why do atoms react?

A

Most atoms ‘want’ to react. This is why so many compounds exist.

Atoms want to gain a full outer shell of electrons (this is the most stable arrangement of electrons).

Therefore all atoms (apart from the noble gases) want to react and achieve a full outer electron shell.

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

How do atoms react?

A

Only the outer shell electrons take part in reactions.

Atoms tend to react by transferring or sharing electrons in order to obtain a full outer shell.

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

Melting/ boiling points of ionic compounds:

The strong electrostatic attractions in the lattice mean that……….

A

ionic compounds have very high melting and boiling points.

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

How can ionic compounds conduct electricity?

A

As solids, ionic compounds cannot conduct electricity because their ions are bonded together in the lattice.

When molten (melted to a liquid), the ions break away from the lattice are free to move. The ions are chafed particles and can conduct electricity.

Many ionic compounds are soluble and form a solution.
When dissolved, the ions are free to move and can conduct electricity.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

When the compound is hit- the layer of ions are dislodged so they match and …… and therefore …….

A

repel

shatter

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

When non-metal atoms join together they form …… ……. .

A

covalent bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

In covalent bonding, the atoms are wanting to obtain .. ….. ….. … … …….

A

a full outer shell of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Two (or more) non-metal atoms can gain electrons by ………

A

sharing

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

If their outer shells overlap, they share some of each others …..

A

electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

metal + non- metal

A

ionic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

non-metal + non-metal

A

covalent

32
Q

Substances formed from covalent bonds can be classified into two groups. What are they?

A

Simple molecular structures (simple covalent)

Giant covalent Structures

33
Q

oxygen, water and carbon dioxide are ……

A

molecules

34
Q

They have a simple molecular structure because they only contain a few….

A

atoms

35
Q

Most molecular substances are … .. …….. at room temperature

A

gas or liquid

36
Q

They have low ………. …. …….. points.

A

melting and boiling

37
Q

A few are solids with fairly low melting points , give an example

A

iodine

38
Q

When water boils, it is the weak …….. ………… that break. The strong covalent bonds remain intact.

A

inter molecular

39
Q

Explain why methane is a gas at room temperature and water is a liquid.

A

Methane is a gas at room temperature because it has very weak inter molecular bonds; weaker than water.

40
Q

Why do they not conduct electricity?

A

Simple molecular structures have no free electrons (they are shared in covalent bonds and not free to move) and they have no ions.
No free electrons, no ions, therefore cannot conduct electricity.

41
Q

In some substances, millions of atoms join together by

A

covalent bonding.

42
Q

This produces giant covalent structures, not

A

molecules

43
Q

All the bonds are covalent, which means that giant covalent structures have a very high …… ….. ……… ……., and are usually hard.

A

melting and boiling point

44
Q

In the element carbon, atoms bond in different ways, creating different kinds of giant structures.
Three of these structures are diamond, graphite and buckminsterfullerene. They are called

A

allotropes of carbon.

45
Q

What are the properties of Diamond?

A

The hardest natural material known.
Very high melting point
Does not conduct electricity

46
Q

Structure of Diamond?

A

It is a giant covalent structure
It has very strong covalent bonds
In Diamond, each carbon atom is surrounded by 4 other carbon atoms
It requires a lot of energy to break the bonds.
It does not conduct electricity because all of the electrons are in covalent bonds. NO FREE ELECTRONS

47
Q

What are the properties of Graphite?

A

Soft and slippery
conducts electricity
high melting point

48
Q

Structure of Graphite?

A

Has a layered structure
Bonds in the layers are strong covalent bonds
Each carbon atom is surrounded/ bonded by 3 carbon atoms
There is a weka inter-molecular bond between the layers. This means they can slide.
It can conduct electricity because there is a free electron between the layers.

49
Q

Info on Buckyball (3 points)

A

It is also called C60
It is ‘just’ considered giant
It is used as a lubricant and can deliver drugs into the body.

50
Q

Other allotropes of carbon

A

Graphene, Carbon nanotubes

51
Q

Info on sand (3 points)

A

Sand is an impure form of silicon dioxide (quartz). It has a giant covalent structure with certain similarities to diamond.
Each silicon is bonded covalently to 4 oxygen atoms.
Sand has a very high melting point.

52
Q

Explain why it is possible to bend a piece of metal-

A

The layers off atoms can move easily allowing the piece of metal to bend.
There are delocalised/ free electrons
Move/slide
Attraction when bend metal

53
Q

An alloy is…

A

a mixture of a metal with at least one other element.

54
Q

Steels are alloys of iron with…

A

carbon and/or other elements.

55
Q

Why is steel stronger than iron?

A

The atoms in pure iron are arranged in densely packed layers. these layers ca slide over each other. This makes pure iron a very soft material. The atoms of other elements are different sizes. When other elements are added to iron, their atoms distort the regular structure of the iron atoms.
It is more difficult for the layers of iron atoms in steel to slide over each other and so this alloy is stronger than pure iron.

56
Q

What’s so clever about smart alloys?

A

Shape memory alloys or smart alloys are metals that return to their original shape after being deformed. Shape memory alloys can be used in medicine and dentistry. For example, nitnol, made from nickel and titanium, is used in dental braces.

57
Q

Metals are found in the…

A

Earth’s crust

58
Q

We find most metals combined chemically with other chemical elements, often with…

A

oxygen or sulphur

59
Q

This means that the metal must be ….. …… from its compounds before it can be used.

A

chemically separated

60
Q

What is metal ore?

A

Metal Ore: enough metal (or compound) in a rock to make it worth extracting the metal. Ores are mined from the ground.

61
Q

Gold and silver are so un reactive that they are found in Earth as ….

A

the metals (elements) themselves.

62
Q

The way that we extract a metal depends on…

A

its place in the reactivity series.

63
Q

A more reactive metal will displace a..

A

less reactive metal.

64
Q 
What is the reactivity series?
P
S
C
M
A
C
Z
I
T
L
C
S
G
P
A 
Potassium  (extracting using electrolysis)
Sodium
Calcium
Magnesium
Aluminium

Carbon

Zinc (extracted using carbon in a blast furnace)
Iron
Tin
Lead
Copper

Silver (found native, no extraction required)
Gold
Platinum

65
Q

We can find many metals, such as copper, lead, iron and zinc, combined with oxygen as metal oxides. Because carbon is more reactive than each of these metals, we can use carbon….

A

to extract the metals from their oxides.

66
Q

The removal of oxygen fro a compound is called …

A

chemical reduction.

67
Q

Iron is a ………. reactive metal.
Iron ore is plentiful and relatively easy to reduce to iron metal.
Iron ore is reduced by heating with carbon in a ………. ………… .
It is cheap, strong and malleable.
Iron is the most ………. used metal.

A

moderately
Blast Furnace
commonly

68
Q

What happens (in order) in the Blast Furnace?

A

Raw materials are added to the furnace.
Carbon Dioxide reacts with coke to form carbon monoxide.
Hot air added.
Carbon rich coke is burnt in oxygen.
Carbon Dioxide is formed.
Iron oxide in the iron ore is reduced by the carbon monoxide to form iron.
Molten iron produced collects in furnace.
Limestone reacts with impurities to form slag which is drained.
Carbon Dioxide and Nitrogen are released as waste gases.

69
Q

carbon burns with oxygen to form

A

carbon dioxide

70
Q

carbon dioxide reacts with more carbon to form

A

carbon monoxide

71
Q

carbon monoxide reduces the iron oxide to form

A

iron

72
Q

Calcium Carbonate decomposes to form

A

calcium oxide

73
Q

Calcium oxide reacts with silicon dioxide to form

A

calcium silicate (slag)

74
Q

What type of reaction produces iron?

A

Reduction

75
Q

Explain why recycling iron is necessary for sustainable development.

A

decreasing waste materials
reserves materials/ ore
decreases - global warming
- carbon dioxide

Chemistry (3 decks)

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