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11CHEM > Metals and Non-Metals > Flashcards

Metals and Non-Metals Flashcards

1
Q

What state are most metals at room temperature?

A

Solids

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2
Q

What state are most non-metals at room temperature?

A

Gases, liquids or solids

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3
Q

In what state are metals good conductors of electricity?

A

Liquid or solid state

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4
Q

Which non-metal is the only one to be able to conduct electricity?

A

Carbon in the form of graphite

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5
Q

Do metals have lustre?

A

Yes, all do when polished

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6
Q

Metal melting and boiling points

A

Both high

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7
Q

Can metals conduct heat?

A

Yes due to the free valence electrons

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8
Q

Describe non-metals properties - brittle, ductile, lustre etc

A

Most are brittle, all are not ductile, and most solids are dull

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9
Q

Non-metal melting and boiling point

A

Both low due to weak intermolecular forces between molecules

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10
Q

Can non-metals conduct heat?

A

No, they are poor conductors and may be used as insulators

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11
Q

Malleable

A

Able to be beaten/hammered or pressed into a sheet

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12
Q

Ductile

A

Able to be drawn into a wire

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13
Q

Lustre

A

Shiny when polished. Able to reflect light from its surface

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14
Q

What is the structure of metals?

A

The metal atoms are packed together in a lattice structure. The valence electrons of each atom are able to move freely. The metallic bonding explains the metal’s physical properties.

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15
Q

Why can metals conduct electricity?

A

As electrons are free to move and carry charge with them

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16
Q

Why are metals malleable and ductile?

A

The metal atoms can easily slide alongside each other without breaking the metallic bonds.

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17
Q

What is the best way to determine if a substance is metal or non-metal?

A

Test if they can conduct electricity. Non-metals cannot conduct electricity with the exception of carbon in the form of graphite.

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18
Q

All metals have how many valance electrons?

A

1, 2, or 3

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19
Q

The more reactive a metal is, the more easily…

A

It loses it’s valence electrons to form a cation.

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20
Q

Activity series elements

A

Li K Na Ca Mg Al Zn Fe Sn Pb (H) Cu Ag Au Pt

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21
Q

Why is hydrogen in the activity series when it is a non-metal?

A

It represents the H in dilute acids

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22
Q

Metals react depending on what?

A

Their position in the activity series, any protective coatings and whether it is an alloy or not.

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23
Q

Aluminium is high in the activity series but unlikely to react. Why?

A

It forms a protective coating on the surface of the metal called aluminium oxide.

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24
Q

The ease of extraction of metals depends on their reactivity. Explain.

A

The least active metals will exist uncombined with other metals. All other metals occur in their ores and can be extracted. The very reactive metals require electrolysis to obtain metal from the ore.

25
Q

Metal and oxygen —>

A

Metal oxide

26
Q

Metals react with oxygen depending on what?

A

Their position in the activity series and whether or not they form a protective coating

27
Q

Metal + water –>

A

Metal hydroxide + hydrogen

28
Q

Four ways to prevent iron from rusting (by providing a surface layer to prevent the air or water from coming in contact with the iron)

A

Galvanising, painting, chrome plating and plastic coating

29
Q

Metal +acid –>

A

Salt + hydrogen

30
Q

Can metals below hydrogen in the activity series perform metal + acid reactions?

A

No, they won’t produce hydrogen

31
Q

Displacement reactions

A

A metal and ionic solution reacts spontaneously. The metal solid and metal ion swap (displace)

32
Q

What type of reaction is A + BC -> B + AC

A

Displacement

33
Q

Metals higher up in the activity series will displace metals above or below them?

A

Below them. If the metal solid is lower in the activity series than the metal ion, no reaction will occur.

34
Q

Spectator ion

A

A spectator ion is an ion which is present when a reaction occurs but does not take part in the reaction and remain unchanged.

35
Q

In a displacement reaction, when the metal solid and metal ion swap places, what happens to the charge?

A

The metal ion will be charged. When it displaces, it loses it’s charge and gives it to the metal solid.

36
Q

What conditions are necessary for a displacement reaction to occur?

A

Metal solid has to be higher in the activity series than the metal ion.

37
Q

What is an alloy?

A

An alloy is a mixture of two or more elements in a solid in which the major component is metal.

38
Q

How are alloys made?

A

By melting a metal and at least one other element together.

39
Q

Why are alloys used more than metals?

A

They are a mixture, so they have varied compositions that modify the properties of pure metals.

40
Q

Why are alloys harder than metals?

A

They have atoms of different sizes so the regular arrangement is distorted and it is harder for the layers to slide past each other.

41
Q

What do smart alloys like Nitonel do?

A

Return to their original shape.

42
Q

Where are non-metals found on the periodic table?

A

On the upper right side

43
Q

What is covalent bonding?

A

Two non-metal atoms share up to 3 electrons to achieve a full valence shell.

44
Q

What is the difference between intermolecular forces and covalent bonding?

A

Intermolecular forces are between the molecules and are weak, giving non-metals low melting and boiling points. Covalent bonds are between the atoms in the molecule and are very strong.

45
Q

What is an allotrope?

A

In some elements, the atoms can be arranged in lots of different ways and each of these forms will have very different properties. Each of the different forms is called an allotrope.

46
Q

What are the allotropes of carbon?

A

Diamond, graphite, graphene and buckminsterfullerene

47
Q

Structure of the diamond allotrope of carbon

A

Each carbon is covalently bonded to four other carbons, giving a rigid 3-D structure with a high melting point. No free electrons so is an insulator

48
Q

Structure of the graphite allotrope of carbon

A

Graphite has layers where each carbon atom forms covalent bonds to three other carbon atoms. In each layer, there are rings fo six carbon atoms. Between the layers are weak intermolecular attractions so the layers can pass over each other, so is soft. One valance electron is free to move between the layers and can carry charge so it can conduct electricity.

49
Q

Structure of buckminsterfullerene allotrope

A

Spherical structure of 60 carbon atoms covalently bonded together.

50
Q

What is graphene?

A

An allotrope of carbon

51
Q

What are the three impure forms of carbon?

A

Charcoal, coke, lamp soot.

52
Q

What are the four main uses of nitrogen?

A

The inert atmosphere in welding to prevent chemical reactions, in food packaging to keep foods fresh, to make ammonia gas, liquid nitrogen is used as a refrigerant or to burn off warts

53
Q

What does nitrous oxide do?

A

It is laughing gas

54
Q

What are the four main uses of oxygen?

A
  • As an aid to breathing in hospitals, deep sea diving and mountaineering
  • In steelmaking to remove impurities from steel
  • In oxy-acetylene torches for cutting up and welding steel
  • As rocket fuels for space travel
55
Q

What are oxygen’s two allotropes?

A

Oxygen (O2) and ozone (O3)

56
Q

What is the ozone layer?

A

A layer of oxygen that is converted into ozone by the sun. Prevents radiation from entering the earth. The amount of chlorofluorocarbons present in the atmosphere has reduced the amount of ozone.

57
Q

How is the S8 molecule formed (sulfur)?

A

The rhombic sulfur (at room temp) is heated between 96-119 to create a monoclinic sulfur. It is cooled very quickly to make plastic sulfur.

58
Q

What are the three main uses of sulfur?

A
  • To make sulfuric acid by the contact process
  • Added to rubber to make it harder and more elastic
  • Used in production for matches, fireworks, fungicides and medicines

11CHEM (7 decks)

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