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Chemistry > C4 The Periodic Table > Flashcards

C4 The Periodic Table Flashcards

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1
Q

An atom is surrounded by electrons

A

-

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2
Q

The nucleus is positively charged, an electron is negatively charged and an atom is neutral

A

-

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3
Q

Mass number is the total number of protons and neutrons in an atom

A

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4
Q

Atomic number is the number of protons in an atom

A

-

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5
Q

An element is a substance that cannot be broken down chemically and it contains only one type of atom

A

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6
Q

A compound is a substance that can be broken down chemically and it contains 2 or more types of elements

A

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7
Q

What was Dalton’s atomic theory?

A
  • atoms can’t be created or destroyed
  • all matter is made from atoms
  • all atoms of an element are identical
  • different elements contain different types of atoms
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8
Q

Who discovered electrons?

A

J.J Thompson

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9
Q

Who discovered that an atom is mostly empty space, with electrons arranged around the central object called the nucleus?

A

Ernest Rutherford

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10
Q

Who discovered that electrons orbit the nucleus?

A

Neil Bohr

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11
Q

What is the nucleus made up of?

A

Protons and Neutrons

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12
Q

Explain why an atom is neutral in terms of its subatomic particles

A

The number of electrons is equal to the number of protons, which have the charge of -1 and +1 respectively

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13
Q

Describe isotopes

A

Isotopes are varieties of an element that have the same atomic number but different mass number

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14
Q

Describe how the work of scientists contributed to the development of the theory of atomic structure

A
  • the theory changed as new evidence was found

- science explanations are provisional but more convincing when predictions are later confirmed

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15
Q

Define ion

A

Ion is a charged atom or group of atoms

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16
Q

Compare the electrical conductivity of sodium chloride in solid, molten liquid and solution

A

The ionic compound can conduct electricity when a molten liquid or solution as the ions are free to move from place to place, which isn’t possible in a solid

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17
Q

Compare the melting points of sodium chloride and magnesium oxide

A

MgO has a greater melting point

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18
Q

Atoms with a full outer shell of 8 electrons have a stable electronic structure

A

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19
Q

Describe ionic bonding

A

A metal and non-metal combine by transferring electrons to form positive ions and negative ions that attract to one another

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20
Q

Sodium chloride conducts electricity

A

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21
Q

MgO and NaCl conduct electricity when molten

A

-

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22
Q

Describe the structure of MgO and NaCl

A
  • Giant ionic lattice in which positive ions are strongly attracted to the negative ions
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23
Q

Explain in terms of structure and bonding, some of the physical properties of NaCl

A
  • High melting points

- Electrical conductivity of molten liquid and solution

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24
Q

Explain in terms of structure and bonding, why the melting point of NaCl is lower than that of MgO

A

The attraction of positive and negative ions in MgO is stronger than the attraction of the ions in NaCl

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25
Q

Name the two types of bonding

A
  • Covalent bonding (between metals)

- Ionic bonding (between metals and non-metals)

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26
Q

Why do carbon dioxide and water not conduct electricity?

A

Carbon dioxide and water molecules have no overall electrical charge. Their electrons are not free to move from place to place, so these compounds do not conduct electricity

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27
Q

Describe a group of elements

A
  • Element all in the same vertical column of the periodic table
  • Similar chemical properties, such as: same number of electrons in the outer shell
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28
Q

Describe a period of elements

A
  • Elements in the same horizontal row of the periodic table

- Same number of electronic shells

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29
Q

Describe the main stages in the development of the periodic table

A
  • Dobereiner: noticed that certain elements with similar properties could be placed into groups of three. The relative atomic mass of the middle element was roughly the mean of the other 2 elements. He could not explain his observations
  • Newlands: he found patterns in the properties of elements when arranged in order of relative atomic mass, but this only worked to calcium
  • Mendeleev: similar to Newlands but swapped elements around if it worked better. Left gaps for undiscovered elements; closest to modern periodic table
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30
Q

Explain in terms of structure and bonding the physical properties of water and carbon dioxide

A

Low melting points

Doesn’t conduct electricity

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31
Q

Group 1 elements are known as the Alkali metals, why is this so?

A

Because they all react with water in a vigour manner and produce alkaline solutions

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32
Q

Why are Group 1 elements stored under oil?

A

Because they are so reactive with water and air, by storing under water, it prevents air and water reaching the metal when stored

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33
Q

Describe the reaction of K, Li, Na with water

A
  • Hydrogen is formed
  • An alkali is formed which is the hydroxide of the metal
  • The reactivity increases as we go down group 1
  • Potassium gives a lilac colour, changes shape as it melts and disappears slowly, ignites explosively
  • Lithium keeps it shape, changes shape as it melts and disappears very quickly, doesn’t ignite
  • Sodium changes shape as it melts, and disappears quickly, doesn’t ignite
34
Q

Reaction of group 1 element

A

Metal + Water —-> Metal Hydroxide + Hydrogen

35
Q

Flame tests

A

Lithium - Red
Sodium - Orange
Potassium - Lilac

36
Q

Predict properties of other Group 1 elements such as Rubidium and Caesium when reacted with water

A

They will be a lot more reactive as it easier to lose the electrons as you go down the Group as there are more electronic shells reducing the strength of the intermolecular forces

37
Q

Symbol equation for reaction between Sodium and a Water

A

2Na + 2H2O —-> 2NaOH + H2

38
Q

Explain why Group 1 elements have similar properties

A

They all have 1 electron in their outer shell, they all lose one electron to form a positive ion with a stable electronic structure

39
Q

Construct a balanced symbol equation to show formation of an ion of a Group 1 element from its atom

A

M—-> M+ + e-

40
Q

Explain why the process of water reacting with a Group 1 element is always oxidation

A

Electrons are always lost

41
Q

Describe how a flame test is conducted

A
  • Use of moistened flame test wire ( hydrochloric acid and nichrome alloy wire is used)
  • Flame test wire dipped into solid sample
  • Flame Test wire put into Bunsen flame
  • Colour of the flame is to be noted
42
Q

What are Group 7 elements known as?

A

Halogens

43
Q

Describe uses of chlorine and iodine

A

Chlorine :

  • To sterilise water
  • To make pesticides and plastic

Iodine :
- To sterilise wounds

44
Q

How do Group 7 elements react with group 1 elements?

Give a word and symbol equation

A

They react vigorously.
Sodium + Bromine —-> Sodium Bromide
2Na + Br2. —-> 2NaBr

45
Q

How does the reactivity change as you go down Group 7 elements?

A

It decreases

46
Q

Word equation of a reaction between a metal halide and Group 7 element

A

Bromine + sodium astatine —-> Astatine + Sodium bromide

47
Q

Recall the colours and state of group 7 elements at room temperature

A

Chlorine is a green gas
Bromine is an orange liquid
Iodine is a grey solid

48
Q

General ionic equation for reaction of group 7 elements

A

X2 + 2MY —> Y2 + 2MX

49
Q

Where are transition elements found?

A

Between group 2 and 3

50
Q

Typical properties of transitional elements are metallic properties

A

-

51
Q

Describe thermal decomposition

A

A reaction where a substance is broken down to at least 2 other substances by heat

52
Q

General word equation for thermal decomposition

A

Metal carbonate —-> metal oxide + carbon dioxide

53
Q

What is the test for carbon dioxide?

A

Turns limewater milky

54
Q

Describe a precipitation reaction

A

A reaction between solutions that make an insoluble solid

55
Q

Compounds of transition elements and their colours

A

Copper compounds are often blue
Iron (II) compounds are often light green
Iron (III) compounds are often orange/brown

56
Q

Where are iron and nickel used?

A

Iron is used as a catalyst for the Haber process

Nickel is used as a catalyst for margarine production

57
Q

Cu2+ gives a blue solid
Fe2+ gives a green/grey solid
Fe3+ gives a orange/brown solid
Sodium hydroxide is used to identify the presence of transition metal ions

A

Solids are called precipitate.

58
Q

Why is iron used to make cars and bridge

A

Strong, high tensile strength and hard

59
Q

Why is copper used to make electrical wires?

A

Good conductors of electricity

60
Q

List physical properties of metal

A 
Lustrous
Shiny 
Good conductors of heat and electricity 
High melting and boiling points 
High tensile strength
61
Q

What are particles in a metal held by?

A

Metallic Bonds

62
Q

When can some metals be superconductors?

A

At low temperature

63
Q

Why do metals have high boiling and melting points?

A

Strong metallic bonds

64
Q

Describe metallic bonding

A

A strong attraction between a sea of delocalised electrons and closely packed positive metal ions

65
Q

Explain in terms of structure why metals are able to conduct electricity efficiently

A

Because they have a sea of delocalised electrons which are easily able to move across the structure of the metal.

66
Q

Describe the term superconductors

A

Materials which have very little resistance to the flow of electricity, some have no resistance

67
Q

Describe some benefits of using superconductors

A
  • Loss free power transmission
  • Super-fast electronics circuits
  • Powerful electromagnets
  • Maglev trains
68
Q

Explain some drawbacks of superconductors

A

Work at extremely low temperatures: -272C

69
Q

List different types of water resources

A
  • lakes
  • rivers
  • aquifers
  • reservoirs
70
Q

What can water be used as in industrial processes

A
  • a solvent to dissolves other substances
  • a cheap raw material
  • a coolant to stop overheating happening
71
Q

Pollutant which can be found in domestic water supplies

A

Nitrate residues
Lead compounds
Pesticide residues

72
Q

List the type of substances present in water before it is purified

A

Dissolved salts and minerals
Microbes
Pollutants
Insoluble materials

73
Q

What process kills microbes in water

A

Chlorination

74
Q

Barium chloride solution is used to test for Sulfate ions, how are they detected

A

A white precipitate is formed

75
Q

Silver nitrate solution is used to test for halide ions

A

Chloride ion gives a white
Bromide ion gives a cream colour
Iodide ions give a yellow colour

76
Q

Explain why it is important to conserve water

A

Fresh water is very scarce approximately 97% is salt water

77
Q

Explain why water may contain:

  • Nitrate
  • Lead compounds
  • Pesticides
A
  • Fertilisers that run off the fields
  • From old lead pipes
  • from spraying crops in fields near the water resource
78
Q

Describe the 3 main stages in water purification

A

Sedimentation: removes large suspended particles
Filtration: removes small suspended particles
Chlorination: kills microbes in the water

79
Q

Explain why some soluble substances are not removed during water purification

A

These may be poisonous, so strict limits are placed on how much of these can be in the wate

80
Q

Explain the disadvantages of using distillation of sea

Water to make large quantities of freshwater

A

A lot of energy is needed

It is too expensive to make large amounts of fresh water in this way

Chemistry (4 decks)

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