The periodic table

Which part of the Periodic Table contains the least reactive non-metals?

Which Group 7 element is a red-brown liquid at room temperature?

A Fluorine

B Chlorine

C Bromine

D Iodine

This question is about elements in Group 1 and Group 7 of the Periodic Table.

Sodium is below lithium in Group 1.

Table 12.1 describes the observations when small pieces of lithium and sodium are placed in water.

Table 12.1

Describe how these observations show how the reactivity of the elements increases going down Group 1.

Potassium is below sodium in Group 1.

Describe one observation when a small piece of potassium is placed in water.

Use information from Table 12.1.

When sodium reacts with water, it forms sodium hydroxide and hydrogen.

Complete the word equation for the reaction of potassium with water.

The equation for sodium, Na, reacting with a Group 7 element, X, is:

Sodium is a solid at room temperature.

Complete the equation by writing in the missing state symbol for sodium.

State the name of element X.

A more reactive Group 7 element displaces a less reactive Group 7 element from a solution of one of its salts.

Chlorine reacts with potassium bromide as chlorine is more reactive than bromine.

Bromine reacts with potassium iodide as bromine is more reactive than iodine.

Iodine does not react with potassium chloride as iodine is less reactive than chlorine.

Table 12.2 shows the results of mixing three Group 7 elements and solutions of their salts.

Table 12.2

Key ✓ = reaction ✗ = no reaction

Complete Table 12.2 by putting a tick (✓) or cross (✗) in the three answer spaces.

Which statement about how Mendeleev arranged his version of the Periodic Table is incorrect

A He arranged elements in order of atomic number.

B He arranged elements with similar properties in groups.

C He left gaps for undiscovered elements.

D He swapped the order of pairs of some elements.

Chlorine is an element found in Group 7 of the Periodic Table.

What are the elements in Group 7 called?

Tick (✓) one box.

Why is chlorine found in Group 7 of the Periodic Table?

Use ideas about electron arrangement.

The diagram shows the reaction between a small piece of hot sodium and chlorine gas.

The sodium burns with a bright yellow flame and a white solid is produced.

What is the name of the white solid made in the reaction?

A student thinks that the experiment is unsafe.

How could the experiment be improved to make it safe?

The metal spoon is made from an alloy of copper.

Suggest a property of this alloy which makes it suitable to use in the experiment.

The Group 7 elements can be placed into an order of reactivity by using displacement reactions.

The table shows the results of mixing three Group 7 elements, X, Y and Z, and solutions of their salts.

Key ✓ = reaction ✗ = no reaction

Describe how the reactivity of the Group 7 elements changes going down the group.

Use the Periodic Table.

Which of the elements X, Y or Z is chlorine?

Which statements about the reactivity of the Group 7 elements are true, and which are false ?

Tick (✓) one box in each row.

This diagram shows how water is treated so it is safe to drink.

At which stage, 1–4, is chlorine added to water?

Why is chlorine added to water?

Elements in the Periodic Table are made from atoms.

Atoms are made from three particles called protons, neutrons and electrons.

The diagram shows an atom.

Label the names of the three particles on the diagram.

Complete the sentence about the atom.

The particle with the lowest relative mass is the proton / neutron / electron.

The first of these three particles to be discovered was by J.J. Thomson.

Complete the sentence about the particles.

The particle that was discovered first was the proton / neutron / electron.

Write the symbol of the element made from atoms with nine protons.

Use the Periodic Table on the Data Sheet.

The table shows part of Mendeleev’s Periodic Table published in 1871.

Which property did Mendeleev use to arrange the elements in his Periodic Table?

Tick (✓) one box.

Give one reason why Mendeleev left gaps in his Periodic Table.

Elements from which Group(s) are present in both Mendeleev’s Periodic Table and the modern Periodic Table?

Use the Periodic Table on the Data Sheet.

Tick (✓) one, two or three boxes.

A teacher investigates some reactions of chlorine.

Why is it important that the teacher does not breathe in chlorine?

A Chlorine is highly flammable.

B Chlorine is inert.

C Chlorine is strongly alkaline.

D Chlorine is toxic.

This question is about Groups 1, 7 and 0 in the Periodic Table.

What are the properties of the elements in Group 1, Group 7 and Group 0?

Tick (✓) one, two or three boxes in each row in Table 12.1.

Table 12.1

Table 12.4 shows the boiling points of some Group 0 elements.

Table 12.4

Describe what happens to the boiling points going from helium to xenon.

Estimate the boiling point of argon. Use the information in Table 12.4.

A teacher investigates some reactions of chlorine.

Why is it important that the teacher does not breathe in chlorine?

A Chlorine is highly flammable.

B Chlorine is inert.

C Chlorine is strongly alkaline.

D Chlorine is toxic.

The elements in Group 1 of the Periodic Table show trends in their properties.

The table shows the diameter of atoms and arrangement of electrons for the first three elements in Group 1.

Describe and explain the trend in the diameter of atoms of the elements in Group 1.

Rubidium is the element below potassium in Group 1.

Predict the diameter of atoms of rubidium.

Describe and explain how the diameter of the atoms affects the reactivity of the elements in Group 1.

Which part of the Periodic Table contains the most reactive metals?

Which particles do atoms in Group 7 gain when they react?

A Electrons

B Ions

C Neutrons

D Protons

The reversible reaction.

The reaction of a very reactive metal.

The reaction of a green gas.

The reaction where a more reactive metal displaces a less reactive metal.

The reaction where a metal is extracted using electrolysis.

Lithium, sodium and potassium are metals in Group 1 of the Periodic Table.

Table 13.1 shows the melting points of lithium, sodium and potassium.

Table 13.1

Complete the bar chart to show the melting point of sodium.

State and explain which of the metals lithium, sodium or potassium is the softest. Use information from Table 13.1.

Metal........

Reason........

Lithium, sodium and potassium can be cut with a knife as shown in the diagram.

At first the freshly cut surface looks shiny, but then begins to go dull.

Complete Table 13.2 by estimating the times for lithium and potassium surfaces to go dull.

Table 13.2

Lithium, sodium and potassium are stored in oil to prevent them reacting with gases in the air.

Which gases in the air react with lithium, sodium and potassium?

Tick (✓) two boxes.

Which row correctly describes the Group 0 elements?

A small piece of a Group 1 metal is added to a trough of water.

The metal floats, fizzes vigorously and melts to form a silvery ball.

Which Group 1 metal was added to the water?

A Lithium

B Potassium

C Rubidium

D Sodium

When a solution of bromine, Br₂(aq), is mixed with a solution of sodium chloride, NaCl (aq), there is no reaction.

Why is there no reaction?

A Bromine gains electrons more easily than chlorine.

B Bromine loses protons more easily than chlorine.

C Chlorine gains electrons more easily than bromine.

D Chlorine loses protons more easily than bromine.

14* Magnesium, calcium and strontium are metals in Group 2 of the Periodic Table.

Tables 14.1 and 14.2 show some information about these metals.

Table 14.1

Reactions of the metals with cold water

Table 14.2

Energy required to form a 2+ ion

Barium is below strontium in Group 2.

Describe and explain the reactivity of barium.

Include observations of the reaction of barium with water.

Use information from Tables 14.1 and 14.2.

Iodine is an element in Group 7 of the Periodic Table.

Seaweed has small amounts of compounds containing iodine. It is possible to extract iodine from seaweed.

The diagram shows the stages in the extraction of iodine.

In Stage 1 iodide ions are produced by reduction.

Explain reduction in terms of electrons.

In Stage 2 iodide ions are oxidised to iodine.

Complete the half-equation for the oxidation of iodide ions into iodine.

In Stage 3 if the solution is heated for too long, iodine vapour is formed.

What colour is iodine vapour?

0.13 g of iodine is produced from 5.0 g of seaweed.

Calculate the percentage mass of iodine in the seaweed.

What produced the gases present in the Earth’s early atmosphere?

Tick (✓) one box.

What is the percentage of oxygen in the Earth’s atmosphere today ?

The amounts of carbon dioxide and water vapour in the Earth’s early atmosphere decreased over time.

Draw lines to connect each gas with the correct description of how it decreased over time

The Earth’s atmosphere today contains gases from Group 0 in the Periodic Table.

The table shows the amounts of the gases from Group 0 in the Earth’s atmosphere

The total amount of the gases from Group 0 is 0.938%.

Complete the table by calculating the exact amount of krypton in the Earth’s atmosphere today.

Write your answer in the box in the table.

What is a property of the Group 0 gases?

Tick (✓) one box.

The student writes the word equation for the reaction.

Complete the word equation for the reaction.

Why does this reaction happen?

Use the reactivity series in Fig. 12.1.

Use the reactivity series in Fig. 12.1 to answer parts (b), (c) and (d).

Another student repeats the experiment but places a different metal in the solution of copper sulfate.

There is no chemical reaction.

Suggest a metal that this student used.

Name one metal that can be extracted by heating its oxide with carbon.

Name one metal that can be extracted from its oxide by electrolysis but not by heating its oxide with carbon.

Complete the sentence below to explain the difference in the reactivity of sodium and lithium.

Use one of the words.

electrons neutrons protons

Sodium atoms lose........ more easily than lithium atoms.

State the trend in reactivity of the Group 1 metals.

Name a Group 1 metal which is more reactive than sodium.

This question is about the Group 7 elements.

Table 16.1 shows some information about the Group 7 elements.

Table 16.1

Complete the table by predicting the appearance of astatine at room temperature.

Write your answer in the box in Table 16.1.

The sizes of the molecules are measured in picometres (pm).

What is the size of a fluorine molecule in metres (m)?

Tick (✓) one box.

Use Table 16.1 to complete the x axis and plot a line graph of the boiling points of fluorine, chlorine, iodine and astatine against the size of their molecules.

Draw a line of best fit.

Use your graph to predict the boiling point of bromine.

Table 16.1 is repeated below.

Table 16.1

A student thinks that fluorine molecules have the weakest intermolecular forces.

Give two reasons why they are correct.

Use data from Table 16.1.

Describe one similarity and one difference in the arrangement of electrons in atoms of fluorine and chlorine.

Similarity........

Difference........

This question is about the Group 7 elements.

Table 11.1 shows some information about the Group 7 elements.

Table 11.1

Complete the table by predicting the appearance of astatine at room temperature.

Write your answer in the box in Table 11.1.

The sizes of the molecules are measured in picometres (pm).

What is the size of a fluorine molecule in metres (m)?

Tick (✓) one box.

Which element has a molecule that is closest to twice the size of a molecule of fluorine?

Tick (✓) one box.

Use Table 11.1 to complete the x axis and plot a line graph of the boiling points of fluorine, chlorine, iodine and astatine against the size of their molecules.

Draw a line of best fit.

Use your graph to predict the boiling point of bromine.

Table 11.1 is repeated below.

Table 11.1

A student thinks that fluorine molecules have the weakest intermolecular forces.

Give two reasons why they are correct.

Use data from Table 11.1.

Describe one similarity and one difference in the arrangement of electrons in atoms of fluorine and chlorine.

For many years it was thought that the Group 0 elements were completely unreactive.

However, more recently, scientists have been able to react some of the Group 0 elements with fluorine.

The table shows information about some of the compounds Group 0 elements make with fluorine.

Give a reason why the Group 0 elements are usually described as unreactive.

Give a reason why scientists have used fluorine to make compounds of the Group 0 elements.

Xenon difluoride, XeF₂, is a solid at room temperature. It melts at 129 °C and boils at 155 °C. It does not conduct electricity in any state.

Suggest the structure of xenon difluoride, XeF₂.

Give two reasons for your answer in (c)(i).

Describe how the trend in reactivity of the Group 0 elements is linked to the size of the atoms.

The table shows information about four different elements.

Which element, A, B, C or D, is in Group 7 of the Periodic Table?

Which statement about the Group 0 elements is correct?

A They exist as simple molecules.

B They exist as single atoms.

C They react to form giant covalent molecules.

D They react to form ionic compounds.

In 2010, scientists discovered a new Group 7 element called tennessine. Its symbol is Ts.

The diagram shows where tennessine is placed in Group 7 of the Periodic Table.

Use your knowledge of the properties and trends of the Group 7 elements to predict the answer to the following questions.

How many outer shell electrons are there in an atom of tennessine?

1 7 17

What is the physical state of tennessine at room temperature?

gas liquid solid

This question is about the Group 1 metals.

A teacher adds a small piece of a Group 1 metal to a trough of water, as shown in Fig. 12.1

The metal burns with a lilac flame, sparks and explodes.

Which Group 1 metal did the teacher add to the water in Fig. 12.1 ?

lithium sodium potassium rubidium caesium

Sodium is a soft metal with a dull coating.

It is shiny when it is freshly cut.

After several seconds, the shiny surface goes dull.

Which gas in the air reacts with the sodium as it goes dull?

What is the name of the chemical compound made as the sodium goes dull?

How long would it take a piece of freshly cut lithium to go dull compared to sodium?

Give a reason for your answer.

Fig. 12.2 shows the trend in the density of the Group 1 metals from lithium to caesium.

Which Group 1 metal does not fit the general trend?

Give a reason for your answer using information from Fig. 12.2.

A teacher demonstrates the reactions of the Group 1 metals with water.

Table 13.1 shows information about how the first four elements in Group 1 react with water.

When potassium is added to cold water it melts and moves very quickly across the surface of the water.

Write down one other observation when potassium is added to cold water.

Complete Table 13.1 for rubidium.

Explain, in terms of electron loss or gain, the difference between lithium and sodium when they react with cold water.

Table 13.2 shows the density of the Group 1 metals from lithium to caesium.

Which Group 1 metal does not fit the general trend?

Explain your answer using information from Table 13.2.

The table shows the boiling points of the first five Group 0 elements.

Which statement describes the trend in the boiling points?

A The boiling points decrease as the molecules get larger.

B The boiling points decrease as the molecules get smaller.

C The boiling points increase as the atoms get larger.

D The boiling points increase as the atoms get smaller.

Table 14.1 shows the melting points of some of the Group 1 metals.

Plot the data in Table 14.1 on the grid in Fig. 14.1.

Draw a line of best fit.

Describe the relationship between the atomic number of the Group 1 metals and their melting points shown in Fig. 14.1.

Describe the metallic bonding in sodium.

Use information from Fig. 14.2 in your answer.

Look at the melting points of sodium and lithium in Table 14.1.

Suggest a reason for the difference in their melting points.

The diagram shows what happens when a small amount of potassium bromide solution, KBr, is added to a solution of chlorine, Cl₂.

Write the balanced symbol equation for the reaction between potassium bromide, KBr, and chlorine, Cl₂.

Write down the name of the chemical which makes the solution orange.

In this reaction is chlorine oxidised or reduced?

Explain your answer.

Explain why chlorine is more reactive than bromine.

The elements neon and argon in Group 0 are unreactive.

Which statement explains why?

A These elements have 8 electrons in the nucleus.

B These elements have 8 electrons in the outer shell.

C These elements have 8 protons in the nucleus.

D These elements have 8 protons in the outer shell.

This question is about Group 1 and Group 7 elements.

A Group 1 element D reacts with water.

This is the equation:

Name element D.

A teacher shows this reaction to his class.

Describe one safety precaution he should use.

E is a colourless gas.

How can you show if the gas is hydrogen or oxygen?

Describe the tests for hydrogen and oxygen, and the results you would expect with gas E.

test for hydrogen........

result with gas E........

result with gas E........

Group 1 elements are very reactive.

Write down the reason why.

Table 11.1 shows the densities of the first four Group 1 elements at room temperature_.

Calculate how many times larger the density of rubidium is than the density of lithium

Give your answer to 1 significant figure.

1 g of sodium and 1 g of potassium are mixed to form an alloy.

Calculate the density of the alloy.

Density =........ g / cm³

The element caesium (Cs) is also in Group 1. Caesium is found below rubidium in the Periodic Table.

Use the information in Table 11.1 and your knowledge of trends in properties for Group 1 elements to estimate the density of caesium.

Density of caesium =........ g / cm³

A student reacts a solution of KBr with chlorine, Cl₂.

Balance the equation for this reaction.

What is the name of the chemical KBr?

Tick (✓) one box.

What does the reaction tell you about the reactivity of Br₂ and Cl₂?

Explain your answer.

How are atoms arranged in the modern Periodic Table?

A In order of atomic number

B In order of relative atomic mass

C In order of the number of neutrons

D In order of reactivity

Look at the table.

Which row in the table has the correct information about chlorine?

The Group 0 elements are unreactive.

Why are they unreactive?

A They all exist as single atoms.

B They are all gases.

C They have a full outer electron shell.

D They need one electron to gain a full outer electron shell.

Look at the boiling points of some Group 7 elements.

What is the most likely boiling point of iodine?

A −20 °C

B 50 °C

C 184 °C

D 350 °C

Fluorine is the most reactive element in Group 7 (Group 17).

Why?

A Fluorine atoms gain an electron more readily than the other Group 7 elements.

B Fluorine is a gas.

C Fluorine exists as diatomic molecules.

D Fluorine atoms lose electrons more readily than the other Group 7 elements.

Which of these solutions will react with each other?

A Sodium bromide and iodine

B Sodium chloride and bromine

C Sodium chloride and iodine

D Sodium iodide and bromine

Which statement about the halogens (Group 7 elements) is correct?

A Astatine is the most reactive halogen.

B Chlorine has the electronic structure 2.8.7.

C Fluorine is the element with the darkest colour.

D The halogens have the molecular formula X₃.

Look at the information about three elements X, Y and Z in the Periodic Table.

* Student A thinks that elements X, Y and Z are in the same Group of the Periodic Table.

Student B thinks they are in different Groups of the Periodic Table.

Analyse and explain the information in the table that supports both Student A’s and Student B’s conclusions.

Who do you think is correct?

Write a balanced symbol equation for the reaction of element Y with water.

Use ‘ Y ’ to represent element Y.