The Periodic Table (Edexcel GCSE Chemistry): Exam Questions

The diagram shows the electron structures of some elements. 

Which two elements have similar chemical properties? 

In Figure 8, the letters A, E, G, J, X and Z show the positions of six elements in the periodic table.

These letters are not the symbols of the atoms of these elements.  

Figure 8

Using the letters A, E, G, J, X and Z

i) give the letters of the two elements that are non-metals

(1)

ii) give the letters of two elements in period 2 

(1)

iii) give the letter of an element that normally forms an ion with a charge of +1.

(1)

Element E has an atomic number of 5. In a sample of E there are two isotopes. One isotope has a mass number of 10 and the other isotope has a mass number of 11.

i) Explain, in terms of subatomic particles, what is meant by the term isotopes. 

(2)

ii) All atoms of element E in this sample contain

(1)

Element X has an atomic number of 18.

State the electronic configuration of an atom of element X. 

In an experiment, 3.5 g of element A reacted with 4.0 g of element G to form a compound.

Calculate the empirical formula of this compound. (relative atomic masses: A = 7, G = 16)

You must show your working. 

empirical formula of this compound=...........................

An oxygen atom has six electrons in its outer shell.

A hydrogen atom has one electron in its outer shell.

Complete the dot and cross diagram of a molecule of water, H₂O.

Show outer shell electrons only.

An element has the configuration 2.8.3. 

Which group and period is this element in? 

Mendeleev arranged the elements in order of atomic mass. 

He then reversed the order of some pairs of elements. 

Why did he do this?

Figure 1 below shows the periodic table Mendeleev produced in 1869.

His periodic table was more widely accepted than previous versions

Figure 1 

The atomic weight of iodine (I) is 127 and that of tellurium (Te) is 128.

Why did Mendeleev reverse the order of these two elements?

Why did Mendeleev leave gaps for undiscovered elements?

Name the particle that allowed the elements to be arranged in order of their atomic number in the modern Periodic Table.

Mendeleev's periodic table shows lithium, sodium and potassium all in the same column. 

These elements are in the same column, Group 1, of the modern periodic table. 

Explain the reactivity of these elements going down Group 1. 

The modern periodic table is arranged in order of: 

The positions of four elements are shown on the Periodic Table. 

The letters are not the atomic symbols of these elements. 

Which element will react with oxygen to form an acidic oxide? 

Figure 1 shows part of the Periodic Table, with elements represented by the letters L, M, Q, R and T.

The letters in the diagram represent elements but are not their chemical symbols.

Figure 1

Give the letter from the diagram that represents a noble gas.

Elements L and M are in the same group.

State why they have similar chemical reactions.

An atom of element Q has 31 protons.

Use this information to explain how you can determine the number of protons in an atom of element R.

Compare the electronic structures of atoms M and R. 

This question is about the Periodic Table. 

What did Mendeleev arrange his elements in order of?

Once Mendeleev had arranged his Periodic Table, he swapped the positions of some elements around. 

Explain why he did this. 

The elements in Mendeleev's Periodic Table didn't always end up in order of increasing relative atomic mass because the existence of isotopes was unknown.

Explain, in terms of subatomic particles, what is meant by an isotope. 

Higher Only 

Some information about the mass number and percentage abundance for the isotopes of gallium is shown in Figure 1. 

Figure 1

Calculate the relative atomic mass of gallium. 

The electronic structures of atoms from three different elements are shown.

    2.8.1                         2.8.8                        2.8.8.1
element W               element Y                  element Z

Name the elements W, Y and Z.

Explain why element Z is more reactive than element W.

Explain why element Y is unreactive.

Give the formula of the ion formed by element W.

Three elements - X, Y and Z, have different physical properties.

At room temperature:

Element X is a shiny grey solid.

Element Y is a colourless gas.

Element Z is a dull yellow solid.

Predict which two elements are in the same group in the Periodic Table.

Give a reason for your answer.

Two of the elements are in the same period.

Explain why you cannot predict which these are, based on this information in part (a).

State what information you would need in order to say which of the elements are in the same period.

Neon and argon are both in Group 0 of the Periodic Table.

Predict one property that they both share.

Figure 1 shows the melting points of the Group 1 elements.

Figure 1

Describe the trend in melting point as you go down Group 1 in the Periodic Table.

Estimate the melting point of potassium (K).

The atoms in a metal are held together by metallic bonds.

Describe how the strength of the metallic bonds in the elements changes as you go down Group 1.

Use your knowledge of how metallic bonds form to suggest a reason for the trend in the melting points of the Group 1 elements.

The compound sodium chloride, NaCl, is made when two elements in Period 3 of the Periodic Table react.

For each of the elements in sodium chloride:

i) State whether it is a metal or a non-metal.

[1]

ii) Explain the difference in their position in the Periodic Table in terms of their electronic configuration.

[2]

Complete the table using the Periodic Table.

Sodium chloride is made up of ions.

Explain how these ions form.

Give the electronic configuration of:

i) A sodium ion.

[1]

ii) A chloride ion.

[1]

Mendeleev devised a Periodic Table in 1869.

It is shown in Figure 1.

Figure 1

Mendeleev ordered the elements in terms of their atomic mass.

i) How are the elements in the modern Periodic Table ordered?

[1]

ii) Not including this difference, compare Mendeleev’s Periodic Table to the modern version.

[4]

Mendeleev reversed the order of some of the elements.

For example, he put tellurium, which has an atomic mass of 128 before iodine, which has an atomic mass of 127.

i) Explain why he did this.

[1]

ii) Mendeleev did not know about isotopes.

Explain why this meant that his order was not always correct.

[1]

Mendeleev left some gaps, shown by the shaded areas.

Explain why he did this.

At the time, many other scientists did not accept Mendeleev’s Periodic Table.

Suggest two reasons why.

Figure 1 shows one group from Mendeleev’s Periodic Table from 1869.

  Figure 1

Eka-aluminium is the name that Mendeleev gave to an undiscovered element. This element is now known as gallium.

Gallium has the atomic number 31.

State two things that this number tells you about gallium atoms.

Mendeleev was able to make some predictions for the properties of gallium.

These are shown in Figure 2.

Figure 2

Explain why he was able to make these predictions.

Estimate the relative atomic mass of gallium.

Gallium was discovered in 1875.

Suggest why the discovery of gallium convinced other scientists that Mendeleev’s Periodic Table was correct.

Mendeleev classified the known elements into a table by arranging them in order of what he believed to be their relative atomic mass. 

His Periodic Table was published in 1869 and it showed the elements that had been discovered at that time.

Part of his Periodic Table is shown in Table 1.

Use the information in Table 1 and your Periodic Table to answer the questions.

Table 1

Hydrogen is an element from Mendeleev's table that is not in the same group as the modern Periodic Table.

Give two reasons why it should not be in Group 1.

Give two reasons why hydrogen could be placed in Group 1.

Give two reasons why hydrogen could be placed in Group 7.

The modern periodic table arranges the elements in order of atomic number.

What scientific discoveries allowed elements to be placed in their correct period and group?

How did this knowledge allow elements to be correctly placed?

Explain why Mendeleev had not actually arranged his elements in order of relative atomic mass.

Figure 1 shows properties of the elements found in Group 1 of the Periodic Table.

Figure 1

Use data from Figure 1 to explain why the elements in the table all float on water.

When the elements in Figure 1 are cut, a shiny surface is exposed which turns dull over time. Predict how the time taken for this to happen changes as you go down the group.

Give a reason for your answer.

Rubidium is found below potassium in Group 1 of the Periodic Table.

Suggest what you would observe when rubidium is added to water.

Give a reason for your answer.

Give the formula of the compound formed when:

i) Lithium reacts with chlorine

[1]

ii) Potassium reacts with oxygen

[1]

Figure 1 shows the electronic configuration (E.C.) of the elements in Period 3 of the Periodic Table.

Figure 1

i) Write the electronic configuration for magnesium and silicon.

[1]

ii) Describe the two links between electronic configuration and position in the Periodic Table.

[2]

Figure 2 shows a trend in a property of the elements as you go across Period 3.

Figure 2

The label for the x-axis is missing. State what it should be.

Describe how electrical conductivity changes across Period 3

You should refer to Figure 2.

Explain this trend in electrical conductivity across Period 3

Figure 1 shows Mendeleev’s Periodic Table from 1869.

The modern Periodic Table is based on Mendeleev’s ideas.

Figure 1

Mendeleev placed six elements in group VIII.

State what evidence Mendeleev used to put the six elements into the same group.

Name the group that these elements are found in the modern Periodic Table.

Group VIII in the modern Periodic Table contains the noble gases.

Explain why the noble gases are unreactive.

Suggest why Mendeleev did not include the noble gases in his table.

Figure 1 shows the boiling points of the halogens.

Figure 1

The halogens are all placed in Group 7 of the Periodic Table.

Explain why, in terms of their electronic configuration.

Determine the state of chlorine and bromine at room temperature (20°C).

Give a reason for your answer.

Describe the trend in boiling point as you go down Group 7.

Explain the trend in boiling point down Group 7.