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GCSE Chemistry LTS > Chapter 1 Atomic Structure > Flashcards

Chapter 1 Atomic Structure Flashcards

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1
Q

What are all substances made from?

A

All substances are made from atoms.

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2
Q

What do elements contain only 1 type of?

A

Elements contain only one type of atom.

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3
Q

What is the name of the diagram used to list all elements in order?

A

Elements are listed in the periodic table.

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4
Q

What is on the periodic table to distinguish between different elements?

A

Each element has a name and a symbol.

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5
Q

What is the correct way to write the symbol for an element?

A

The symbol for an element always starts with a capital letter but may have lower case letter too.
Example: Sodium = Na
Nitrogen = N

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6
Q

Copy and complete the table to give the symbols for the first 20 elements.

Name of Element
Symbol
Hydrogen

Helium

Lithium

Beryllium

Boron

Carbon

Nitrogen

Oxygen

Fluorine

Neon

Sodium

Magnesium

Aluminium

Silicon

Phosphorus

Sulfur

Chlorine

Argon

Potassium

Calcium

A

The names and symbols for the first 20 elements are:

Hydrogen
H
Helium
He
Lithium
Li
Beryllium
Be
Boron
B
Carbon
C
Nitrogen
N
Oxygen
O
Fluorine
F
Neon
Ne
Sodium
Na
Magnesium
Mg
Aluminium
Al
Silicon
Si
Phosphorus
P
Sulfur
S
Chlorine
Cl
Argon
Ar
Potassium
K
Calcium
Ca

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7
Q

How is the periodic table arranged?

A

The periodic table is an arrangement of elements in groups and periods.

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8
Q

What are groups in the periodic table and how many are there?

A

Groups are the columns in the periodic table. There are 8 groups.

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9
Q

How are elements in the same group similar?

A

Elements in the same group will have similar chemical properties.

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10
Q

There is a ‘step’ in the periodic table. What type of elements are on the left of the step and what type are on the right?

A

The periodic table has a ‘step’ that separates metals from nonmetals. Metals are on the left of the step and nonmetals are on the right.

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11
Q

What are the ‘periods’ in the periodic table?

A

Periods are rows in the periodic table.

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12
Q

Give the definition for a compound and give an example of a compound.

A

Compounds contain more than one type of atom. This means they have more than one element.
Example: Carbon dioxide is a compound CO2

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13
Q

What do the letters and numbers in a chemical formula represent?

A

The letters in a chemical formula represent the element present. The numbers tell up how many atoms of each element there are.
Example: CO2 has 1 carbon atom and 2 oxygen atoms

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14
Q

How can compounds be separated into elements?

A

Compounds can only be separated into elements by chemical reactions.

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15
Q

What name do we give to the chemicals that react together in a chemical reaction?

A

Chemicals that react together are called reactants.

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16
Q

What name do we give to the chemicals that are produced in a chemical reaction?

A

Chemicals that are produced in a chemical reaction are called products.

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17
Q

When writing a chemical equation what symbol do we use to separate the reactants and the products?

A

The reactants and products are separated by an arrow in a chemical equation.
reactants → products

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18
Q

Why does the number of atoms of one element in the reactants need to be the same as the number of atoms of that element found in the products?

A

The number of atoms of one element in the reactants is the same as the number of atoms of that element in the products. This is because in a chemical reaction atoms cannot be created or destroyed. They are only rearranged.

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19
Q

State the law of conservation of mass.

A

The law of conservation of mass states that “The total mass of the products formed in a reaction is equal to the total mass of the reactants.”

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20
Q

What can we do to a chemical equation to make sure the number of atoms in the reactants is the same as the number of atoms of each element in the products?

A

Equations must be balanced to make sure the number of atoms of each element in the reactants is the same as the number of atoms of each element in the products.

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21
Q

Where do we add numbers to a chemical equation to balance it?

A

To balance an equation a number can be added to the front of the symbol for a reactant or product. The chemical formula for a compound or molecule cannot be changed.
Example:
Unbalanced: H2 + O2 → H2O
Balanced: H2 + 2O2 → 2H2O

The formula for water cannot be changed from water: H2O to peroxide: H2O2.

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22
Q

What do chemical reactions always result in?

A

Chemical reactions always result in the formation of one or more new substances.

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23
Q

What are the 4 states identified in chemical equations using state symbols?

A

State symbols are used to show whether a chemical is a solid, liquid, gas or aqueous.

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24
Q

What does aqueous mean?

A

Aqueous means dissolved in water.

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25
Q

Complete the table to show the state symbols:

State
Symbol
solid

liquid

gas

aqueous

A

The state symbols are:

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26
Q

What is a mixture?

A

A mixture is made up of 2 or more substances that are not chemically combined together.

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27
Q

What is a pure substance?

A

A pure substance is made up of only one type of element or compound.

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28
Q

What is an impure substance?

A

An impure substance is a mixture of elements or compounds.

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29
Q

How can compounds in mixtures be separated from each other?

A

The compounds in mixtures can be physically separated from each other.

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30
Q

Give 3 methods of separating mixtures.

A

Methods of separating mixtures include: filtration, crystallisation and simple distillation.

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31
Q

What is filtration used to separate?

A

Filtration can be used to separate insoluble substances from a solvent.

32
Q

Draw and label a diagram to show the process of filtration.

A

A filter funnel and filter paper is used during filtration.

33
Q

What is crystallisation used to separate? Draw a diagram to show the process of crystallisation.

A

Crystallisation can remove a soluble salt from a salt solution. To do this the solution needs to be heated to evaporate the water. The salt will then form crystals.

34
Q

What is simple distillation used to separate?

A

Simple distillation is used to separate a solvent from a mixture.

35
Q

Draw and label a diagram to show the process of simple distillation.

A

Simple distillation requires special equipment.

36
Q

Detail the stages in the distillation of salt water to obtain pure water.

A

The stages in the distillation of salt water to obtain pure water are:
The salt solution is heated in a flask.

Water from the solution evaporates and rises as steam.

The steam enters the condenser.

The stream is cooled by the condenser and turns into a liquid.

The liquid water is collected in a beaker.

Salt remains in the flask.

37
Q

What is fractional distillation used to separate?

A

Fractional distillation can be used to separate 2 liquids that have different boiling points.

38
Q

Give an example of 2 liquids that can be separated by fractional distillation and state what property allows them to be separated this way.

A

Examples of 2 liquids that can be separated by simple distillation are water and ethanol. Water has a boiling point of 100°C and ethanol has a boiling point of 78°C.

39
Q

Draw and label the equipment used for fractional distillation.

A

Fractional Distillation required special equipment. It is similar to the equipment for simple distillation but includes a fractionating column.

40
Q

Describe the fractionating column and what happens there.

A

Fractionating columns contain glass beads and allow the vapours of the liquid with the highest boiling point to condense and return to the flask.

41
Q

Give a way that mixtures in solution can be separated.

A

Mixtures in solution can be separated using a technique called paper chromatography.

42
Q

Detail the stages in the process of paper chromatography.

A

Stages in paper chromatography:
Draw a line in pencil 1 cm from the bottom of a sheet of chromatography paper.

Use a capillary tube to place a spot of the mixture on the line.

Place the bottom of the paper in a solvent taking care not to let the solvent cover the spot.

Wait for the solvent to travel up the paper carrying the mixture with it.

When the solvent front nearly reaches the top, remove from the solvent and observe.

43
Q

Draw a diagram to show what paper chromatography looks like when it is set up.

A

Paper chromatography looks like this when it is set up.

44
Q

How is paper chromatography able to separate mixtures?

A

Paper chromatography is able to separate mixtures because different substances have different solubilities in the solvent.

45
Q

What idea about the nature of atoms did John Dalton propose?

A

Ideas about the nature of atoms have changed over time. An early idea was proposed by John Dalton that the atoms were tiny hard spheres that could not be divided.

46
Q

When was the electron discovered and who discovered electrons?

A

The electron was discovered in 1897 by J. J. Thomson.

47
Q

Draw and describe the model of the atom JJ Thomson used.

A

Thomson proposed a ‘plum pudding’ model of the atom with negatively charged electrons embedded in a cloud of positive charge.

48
Q

Which scientists disproved JJ Thomson’s model and how did they do it?

A

The scientists Geiger and Marsden carried out an experiment called the alpha particle scattering experiment which disproved Thomson’s model.

49
Q

What is an alpha ( ɑ) particle?

A

An alpha ( ɑ) particle is a positively charged particle.

50
Q

What happens to alpha (ɑ) particles when they are fired at gold foil?

A

When alpha particles ( ɑ particles) were aimed at gold foil the particles emerge at different angles.

51
Q

Why do alpha (ɑ) particles behave as they do when fired at gold foil?

A

Opposite charges repel so the alpha particles were deflected by the positive charges in the atom.

52
Q

What did Ernest Rutherford conclude?

A

Ernest Rutherford took these findings and concluded that negative electrons were orbiting around a positively charged nucleus.

53
Q

What additional modification did Niels Bohr make to the model in 1914?

A

In 1914 Niels Bohr modified the model by showing that electrons orbit the nucleus at set distances.

54
Q

Draw and label the GCSE model of the atom that we use.

A

The GCSE model of the atom has a nucleus containing protons and neutrons. Negatively charged electrons orbit the nucleus in shells.

55
Q

What name do we give to the 3 types of particles that make up atoms?

A

The atom is made up of protons, neutrons and electrons. These are known as subatomic particles.

56
Q

What mass do protons and neutrons have? What units do we use for the mass of subatomic particles?

A

Protons and neutrons have a mass of 1 atomic mass unit (amu).

57
Q

What is the mass of an electron?

A

Electrons have a mass of 1/2000 of an amu.This is virtually zero.

58
Q

What is the charge on a proton? What is the charge on a neutron?

A

Protons have a charge of +1. Neutrons have no charge and electrons have a charge of -1.

59
Q

Complete the table to show a summary of charges and masses of subatomic particles:

Subatomic Particle
Relative Charge
Relative Mass (amu)
proton

1

0

electron

1/2000

A

Summary of charges and masses of subatomic particles:

60
Q

Why do atoms have an overall charge of 0?

A

Atoms contain the same number of electrons as protons. This results in atoms having an overall charge of 0.

61
Q

What is the atomic number?

A

The atomic number is the number of protons in an atom.

62
Q

Which subatomic particle determines what element an atom is?

A

Elements in the periodic table are arranged in order of atomic number. The number of protons (atomic number) determines which element it is.
Example: An atom with 6 protons is always carbon. An atom with 12 protons is always magnesium.

63
Q

How can the atomic mass be calculated?

A

The mass of an atom is equal to the number of protons added to the number of neutrons. This is because only protons and neutrons have mass. The mass of electrons is negligible.

64
Q

Use your periodic table to write the nuclide notation for carbon.

A

Nuclide notation is used to show the number of protons in an element as well as the mass and charge (more on charges later).
Example:

65
Q

Describe how to calculate the number of neutrons in an atom.

A

The number of neutrons in an atom can be worked out by subtracting the atomic number from the mass number.

Protons = 17
Mass = 35
Neutrons = 35 - 17 = 18

66
Q

What is the relative atomic mass?

A

The relative atomic mass is the average mass of an atom taking into account the abundance of each isotope of an atom.

67
Q

What happens to the charge on an atom when it gains an electron?

A

If an atom gains electrons it becomes negatively charged. This is because electrons are negatively charged. Charged atoms are called ions.

68
Q

Chlorine gains one electron. Write the nuclide notation for chlorine and include the charge in the correct location.

A

The nuclide notation for a chloride ion looks like this.

69
Q

What is the charge on an atom that loses an electron? What type of atoms lose electrons?

A

Metals lose electrons to make positive ions.

70
Q

What are isotopes?

A

Isotopes are atoms of the same element but with a different number of neutrons.
Example:

71
Q

How are isotopes of an element the same and how are they different?

A

Isotopes have the same chemical properties but their density is different.

72
Q

Which electron shell is the lowest energy level?

A

Electrons are arranged in energy levels (sometimes called shells). The shell closest to the nucleus has the lowest energy level.

73
Q

How many electrons can the first energy level hold? How many can the second energy level hold?

A

The first energy level can hold up to 2 electrons. The 2nd level can hold up to 8 electrons. When the first energy level needs to fill up before the 2nd one starts to fill up.

74
Q

What feature of an atom determines how the atom will react?

A

The number of electrons in the outer shells determines the way that an element reacts.

75
Q

What does ‘electronic configuration’ mean?

A

The way electrons are organised in shells around the nucleus is called the electronic configuration. The number of electrons in each shell is given
Example: The electronic configuration for an atom of sodium would be 2,8,1.

GCSE Chemistry LTS (15 decks)

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