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Chemistry > Chemistry- Structure and Bonding > Flashcards

Chemistry- Structure and Bonding Flashcards

(75 cards)

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1
Q

Electrons always occupy …. .

A

shells

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2
Q

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

A

first

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3
Q

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

A

2,8,8

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4
Q

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

A

element

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5
Q

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

A

proton

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6
Q

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

A

electron

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7
Q

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

A

neutron

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8
Q

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

A

protons

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9
Q

……… have no overall electrical charge.

A

Atoms

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10
Q

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

A

neutral atom

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11
Q

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

A

electron

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12
Q

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

A

electron

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13
Q

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

A

hydrogen

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14
Q

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

A

nucleus

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15
Q

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

A

protons

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16
Q

The mass number of carbon is ….

A

12

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17
Q

The proton number of carbon is …..

A

6

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18
Q

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

A

9

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19
Q

The mass number of fluorine is ……

A

19

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20
Q

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

A

11

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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.

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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.

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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.

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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.

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25
When the compound is hit- the layer of ions are dislodged so they match and ...... and therefore .......
repel | shatter
26
When non-metal atoms join together they form ...... ....... .
covalent bonds
27
In covalent bonding, the atoms are wanting to obtain .. ..... ..... ... ... .......
a full outer shell of electrons
28
Two (or more) non-metal atoms can gain electrons by .........
sharing
29
If their outer shells overlap, they share some of each others .....
electrons
30
metal + non- metal
ionic
31
non-metal + non-metal
covalent
32
Substances formed from covalent bonds can be classified into two groups. What are they?
Simple molecular structures (simple covalent) | Giant covalent Structures
33
oxygen, water and carbon dioxide are ......
molecules
34
They have a simple molecular structure because they only contain a few....
atoms
35
Most molecular substances are ... .. ........ at room temperature
gas or liquid
36
They have low .......... .... ........ points.
melting and boiling
37
A few are solids with fairly low melting points , give an example
iodine
38
When water boils, it is the weak ........ ............ that break. The strong covalent bonds remain intact.
inter molecular
39
Explain why methane is a gas at room temperature and water is a liquid.
Methane is a gas at room temperature because it has very weak inter molecular bonds; weaker than water.
40
Why do they not conduct electricity?
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
In some substances, millions of atoms join together by
covalent bonding.
42
This produces giant covalent structures, not
molecules
43
All the bonds are covalent, which means that giant covalent structures have a very high ...... ..... ......... ......., and are usually hard.
melting and boiling point
44
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
allotropes of carbon.
45
What are the properties of Diamond?
The hardest natural material known. Very high melting point Does not conduct electricity
46
Structure of Diamond?
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
What are the properties of Graphite?
Soft and slippery conducts electricity high melting point
48
Structure of Graphite?
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
Info on Buckyball (3 points)
It is also called C60 It is ‘just’ considered giant It is used as a lubricant and can deliver drugs into the body.
50
Other allotropes of carbon
Graphene, Carbon nanotubes
51
Info on sand (3 points)
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
Explain why it is possible to bend a piece of metal-
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
An alloy is...
a mixture of a metal with at least one other element.
54
Steels are alloys of iron with...
carbon and/or other elements.
55
Why is steel stronger than iron?
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
What’s so clever about smart alloys?
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
Metals are found in the...
Earth’s crust
58
We find most metals combined chemically with other chemical elements, often with...
oxygen or sulphur
59
This means that the metal must be ..... ...... from its compounds before it can be used.
chemically separated
60
What is metal ore?
Metal Ore: enough metal (or compound) in a rock to make it worth extracting the metal. Ores are mined from the ground.
61
Gold and silver are so un reactive that they are found in Earth as ....
the metals (elements) themselves.
62
The way that we extract a metal depends on...
its place in the reactivity series.
63
A more reactive metal will displace a..
less reactive metal.
64
``` What is the reactivity series? P S C M A C Z I T L C S G P ```
``` 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
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....
to extract the metals from their oxides.
66
The removal of oxygen fro a compound is called ...
chemical reduction.
67
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.
moderately Blast Furnace commonly
68
What happens (in order) in the Blast Furnace?
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
carbon burns with oxygen to form
carbon dioxide
70
carbon dioxide reacts with more carbon to form
carbon monoxide
71
carbon monoxide reduces the iron oxide to form
iron
72
Calcium Carbonate decomposes to form
calcium oxide
73
Calcium oxide reacts with silicon dioxide to form
calcium silicate (slag)
74
What type of reaction produces iron?
Reduction
75
Explain why recycling iron is necessary for sustainable development.
decreasing waste materials reserves materials/ ore decreases - global warming - carbon dioxide

Chemistry (3 decks)

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