Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry > C4 The Periodic Table > Flashcards

C4 The Periodic Table Flashcards

1
Q

An atom is surrounded by electrons

A

-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

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

A

-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

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

A

-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Atomic number is the number of protons in an atom

A

-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

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

A

-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

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

A

-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Who discovered electrons?

A

J.J Thompson

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

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

A

Ernest Rutherford

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Who discovered that electrons orbit the nucleus?

A

Neil Bohr

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is the nucleus made up of?

A

Protons and Neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Describe isotopes

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Define ion

A

Ion is a charged atom or group of atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Compare the melting points of sodium chloride and magnesium oxide

A

MgO has a greater melting point

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

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

A

-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Sodium chloride conducts electricity

A

-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

MgO and NaCl conduct electricity when molten

A

-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Describe the structure of MgO and NaCl

A
  • Giant ionic lattice in which positive ions are strongly attracted to the negative ions
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Name the two types of bonding

A
  • Covalent bonding (between metals)

- Ionic bonding (between metals and non-metals)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Describe a period of elements

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

- Same number of electronic shells

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions