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Chemistry IGCSE > The Periodic Table, metals and non-metals > Flashcards

The Periodic Table, metals and non-metals Flashcards

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1
Q

In what order is the elements in the periodic table arranged?

A

by Proton number

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2
Q

What is it meant by periods and groups of the periodic table

A

The periods are rows and Groups are columns of the periodic table.

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3
Q

Where are transition elements located in the periodic table.

A

In the middle block.

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4
Q

What can be predicted using an elements position in the periodic table.

A

Its properties.

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5
Q

In a periodic table,what is the primary classification of the elemnts

A

metals and non-metals

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6
Q

Where are most metals in the periodic table located?

A

To the left of the bold zigzagged line.

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7
Q

What are the properties of metals? [7]

A
  1. Shiny appearance.
  2. Solids, except for Mercury.
  3. High melting points.
  4. High densities.
  5. Good conductors of electricity.
  6. Good conductors of heat.
  7. Malleable.
    [Many of the properties of Metals are due to metallic bonding]
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8
Q

What are the properties of Non-metals?

A
  1. Dull appearance.
  2. Half are solids and half are gases. Bromine is a liquid.
  3. Low melting points.
  4. Low densities.
  5. Poor conductors of electricity.
  6. Poor conductors of heat
  7. Brittle.
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9
Q

Why are metals malleable?

A

Because the layers of atoms can slide over each other

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10
Q

What is an alloy?

A

is a mixture of a metal and at least one other element.

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11
Q

Why are alloys harder than pure metal?

A

In alloys, the atoms of different structures disrupts the layered structure of metals, The layers cannot slide over each other and so it is harder.

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12
Q

Describe Brass, in terms of elements mixed together, its properties and its uses.

A
  • Stronger than copper, but still has very good electrical conductivity.
  • Used in electrical fittings.
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13
Q

Describe Duralumin, in terms of elements mixed together, its properties and its uses.

A
  • comprised of 96% aluminium, 4% copper and other metals.
  • Stronger than aluminium, yet still low density and lightweight.
  • used in aircraft manufacture.
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14
Q

Describe stainless steel, in terms of elements mixed together, its properties and its uses.

A
  • Iron with at least 11% chromium and other metals. e.g, nickel.
  • corrosion resistant and stronger than iron.
  • used in cutlery.
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15
Q

Describe the reaction between metals and and oxygen.

A
  • Metal oxides formed.
  • Ionic solids.
  • e.g Calcium + Oxygen - > Calcium oxide
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16
Q

Describe the reaction between a metal and an acid.

A
  • Basic salt is formed.
  • Hydrogen produced.
  • e.g Zinc + Nitric acid - > zinc Nitrate + Hydrogen.
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17
Q

Describe the electrons in outer shells, Ion charge and reactivity of all groups 1-8. Also, distinguish them between metallic and non-metallic.

A
  • Letts revision guide, page 93.
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18
Q

What are group 1 metals known as?

A

Alkali metals.

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19
Q

What are the physical properties of Group 1 elements?

A

-soft, compared to other metals.
-Shiny when cut, but dulls as they react with gases in the air
-Low densities; float on water. Densities increase, going down the group.
-Low melting points, compared to other metals (like iron)
e.g. [Fe: 1540 degrees Celsius]
Li : 180
Na : 98
K : 63

20
Q

Describe the chemical properties of group 1 elements. What is the trend of reactivity.

A

Very reactive.

Become more reactive, going down the group.

21
Q

Why are Group 1 elements generally stored under oil?

A

They react with water and air.

22
Q

Describe the general reaction of group 1 elements with water.

A

They float, fizz (effervescence) and move around. The fizzing is due to hydrogen gas being formed.

23
Q

Describe the reactions, with water of Lithium, sodium, and potassium.

A

The reactivity increases, going down the group:

  • Li : fizzes less vigorously tan sodium or potassium but does not melt.
  • Na: produces enough heat to melt and forms a molten ball as it moves around the surface of water.
  • K : So exothermic that potassium melts into a molten ball, the hydrogen catches fire and burns with a lilac flame.
24
Q

Using general trends in group 1, predict the properties of rubidium which is lower down the group in the periodic table.

A

-soft metal ball that reacts violently with water.

25
Q

Why,in terms of electrons, do all group 1 elements show similar characteristics when reacting.
Why do they get more reactive down the group?

A

All have 1 electron in outer shell.
They can easily lose this electron to leave a full outer shell.
As the number of shells increases, there is a greater distance between the positive neutron and electron, means it is further form attraction and the electrons can be easily lost.

26
Q

Describe transition elements.

A

a block of metals in the periodic tale between groups I and III, that have similar properties that behave like typical metals.

27
Q

In comparison with group I metals, describe the physical properties of transition elements.

A
  • Melting point: Transition elements have high and Group 1 has low.
  • Density: transition metals have higher than group 1.
28
Q

In comparison with group I metals, describe the chemical properties of transition elements.

A
  • color of compounds: transition metals have colored compounds while group 1 has white.
  • Reaction with water: Transition metals have slow or no reactions, while Group 1 has vigorous reactions.
  • Reaction with acids: usually slow of no reactions while group 1 has violent reactions.
29
Q

Describe two situations, where transition metals are used as catalysts.

A
  1. Iron in Haber process.

2. Vanadium oxide in contact processes of production of sulfuric acid.

30
Q

What is a recurring difference between transition elements.

A

Their oxidation states.

31
Q

What is group VII

A

The Halogens.

32
Q

Name 3 common halogens.

A

Chlorine, iodine and bromine.

33
Q

Describe the trends seen in halogens.

A
  • They become darker down the group.
  • The increase in density down the group.
  • Reactivity decreases down the group.
34
Q

Describe the colour and state of Chlorine, Bromine and Iodine.

A

Chlorine: a pale green gas
Bromine: Red-Brown liquid.
Iodine: Grey-black solid.

35
Q

What is are displacement reactions?

A

are reactions where a more reactive element will displace a less reactive one from its compound.

36
Q

Why are group VII elements so reactive.

A
  • 7 electrons in the outer shell.

- can easily gain one more.

37
Q

what is group VIII known as?

A

the noble gases.

38
Q

Why are they unreactive?

A
  • full outer shells.
  • do not lose, gain or share electrons.
  • Mono-atomic.
39
Q

When are noble gases used?

A

To provide inert atmospheres.

eg. helium in balloons and argon in light bulbs.

40
Q

What is the reactivity series?

A

is a list of metals in the order of reactivity, the most reactive, being at the top.

41
Q

The more reactive a metal is…

A
  • the easier it is to form compounds.

- the harder it is to break its compounds down.

42
Q

list the reactivity series.

A 
potassium
stop
calcium
magnesium
aluminium
[carbon]
zinc
Iron
[Hydrogen]
copper
43
Q

For potassium, sodium and calcium, describe its reaction with steam and HCl

A
  • steam: fizz in cold water, giving off hydrogen gas and forming an alkaline hydroxide solution.
  • HCl: Violent and explosive.
44
Q

For Magnesium, zinc and Iron,describe its reaction with steam and HCl.

A
  • Steam: produce hydrogen gas, and metal oxide.

- HCl: produce a salt, giving off hydrogen gas.

45
Q

For copper, describe its reaction with steam and HCl.

A

no reactions.

46
Q

Describe displacement in terms of position in the reactivity series.

A

Metals higher up, displace metals lower down.

47
Q

Describe Aluminium’s displacement of Iron from iron(III)oxide.

A

-Aluminum form ions more easily that iron. so will displace.
-Energy is released- so exothermic, iron melts.
-Oxidation of Al; oxidation sates increasing from 0 to +3
-

Chemistry IGCSE (10 decks)

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