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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
Name the two types of bonding
- Covalent bonding (between metals) | - Ionic bonding (between metals and non-metals)
26
Why do carbon dioxide and water not conduct electricity?
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
27
Describe a group of elements
- Element all in the same vertical column of the periodic table - Similar chemical properties, such as: same number of electrons in the outer shell
28
Describe a period of elements
- Elements in the same horizontal row of the periodic table | - Same number of electronic shells
29
Describe the main stages in the development of the periodic table
- 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
30
Explain in terms of structure and bonding the physical properties of water and carbon dioxide
Low melting points | Doesn't conduct electricity
31
Group 1 elements are known as the Alkali metals, why is this so?
Because they all react with water in a vigour manner and produce alkaline solutions
32
Why are Group 1 elements stored under oil?
Because they are so reactive with water and air, by storing under water, it prevents air and water reaching the metal when stored
33
Describe the reaction of K, Li, Na with water
- 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
Reaction of group 1 element
Metal + Water ----> Metal Hydroxide + Hydrogen
35
Flame tests
Lithium - Red Sodium - Orange Potassium - Lilac
36
Predict properties of other Group 1 elements such as Rubidium and Caesium when reacted with water
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
Symbol equation for reaction between Sodium and a Water
2Na + 2H2O ----> 2NaOH + H2
38
Explain why Group 1 elements have similar properties
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
Construct a balanced symbol equation to show formation of an ion of a Group 1 element from its atom
M----> M+ + e-
40
Explain why the process of water reacting with a Group 1 element is always oxidation
Electrons are always lost
41
Describe how a flame test is conducted
- 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
What are Group 7 elements known as?
Halogens
43
Describe uses of chlorine and iodine
Chlorine : - To sterilise water - To make pesticides and plastic Iodine : - To sterilise wounds
44
How do Group 7 elements react with group 1 elements? | Give a word and symbol equation
They react vigorously. Sodium + Bromine ----> Sodium Bromide 2Na + Br2. ----> 2NaBr
45
How does the reactivity change as you go down Group 7 elements?
It decreases
46
Word equation of a reaction between a metal halide and Group 7 element
Bromine + sodium astatine ----> Astatine + Sodium bromide
47
Recall the colours and state of group 7 elements at room temperature
Chlorine is a green gas Bromine is an orange liquid Iodine is a grey solid
48
General ionic equation for reaction of group 7 elements
X2 + 2MY ---> Y2 + 2MX
49
Where are transition elements found?
Between group 2 and 3
50
Typical properties of transitional elements are metallic properties
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51
Describe thermal decomposition
A reaction where a substance is broken down to at least 2 other substances by heat
52
General word equation for thermal decomposition
Metal carbonate ----> metal oxide + carbon dioxide
53
What is the test for carbon dioxide?
Turns limewater milky
54
Describe a precipitation reaction
A reaction between solutions that make an insoluble solid
55
Compounds of transition elements and their colours
Copper compounds are often blue Iron (II) compounds are often light green Iron (III) compounds are often orange/brown
56
Where are iron and nickel used?
Iron is used as a catalyst for the Haber process | Nickel is used as a catalyst for margarine production
57
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
Solids are called precipitate.
58
Why is iron used to make cars and bridge
Strong, high tensile strength and hard
59
Why is copper used to make electrical wires?
Good conductors of electricity
60
List physical properties of metal
``` Lustrous Shiny Good conductors of heat and electricity High melting and boiling points High tensile strength ```
61
What are particles in a metal held by?
Metallic Bonds
62
When can some metals be superconductors?
At low temperature
63
Why do metals have high boiling and melting points?
Strong metallic bonds
64
Describe metallic bonding
A strong attraction between a sea of delocalised electrons and closely packed positive metal ions
65
Explain in terms of structure why metals are able to conduct electricity efficiently
Because they have a sea of delocalised electrons which are easily able to move across the structure of the metal.
66
Describe the term superconductors
Materials which have very little resistance to the flow of electricity, some have no resistance
67
Describe some benefits of using superconductors
- Loss free power transmission - Super-fast electronics circuits - Powerful electromagnets - Maglev trains
68
Explain some drawbacks of superconductors
Work at extremely low temperatures: -272C
69
List different types of water resources
- lakes - rivers - aquifers - reservoirs
70
What can water be used as in industrial processes
- a solvent to dissolves other substances - a cheap raw material - a coolant to stop overheating happening
71
Pollutant which can be found in domestic water supplies
Nitrate residues Lead compounds Pesticide residues
72
List the type of substances present in water before it is purified
Dissolved salts and minerals Microbes Pollutants Insoluble materials
73
What process kills microbes in water
Chlorination
74
Barium chloride solution is used to test for Sulfate ions, how are they detected
A white precipitate is formed
75
Silver nitrate solution is used to test for halide ions
Chloride ion gives a white Bromide ion gives a cream colour Iodide ions give a yellow colour
76
Explain why it is important to conserve water
Fresh water is very scarce approximately 97% is salt water
77
Explain why water may contain: - Nitrate - Lead compounds - Pesticides
- Fertilisers that run off the fields - From old lead pipes - from spraying crops in fields near the water resource
78
Describe the 3 main stages in water purification
Sedimentation: removes large suspended particles Filtration: removes small suspended particles Chlorination: kills microbes in the water
79
Explain why some soluble substances are not removed during water purification
These may be poisonous, so strict limits are placed on how much of these can be in the wate
80
Explain the disadvantages of using distillation of sea | Water to make large quantities of freshwater
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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