Subatomic particles

Which row describes the nucleus of an atom?

Atoms are made up of protons, neutrons and electrons.

The table shows the relative mass and relative charge for a proton and electron.

Complete the table to show the relative mass and relative charge of a neutron.

Use numbers from the list.

The mass of a proton is 1.67 × 10^–27 kg. (b)

An electron is 0.0005 times lighter than a proton.

Calculate the mass of an electron in kg.

Give your answer in standard form.

The symbol for an atom of nitrogen is:

The table shows the number of protons in this atom of nitrogen.

Complete the table by writing in the number of neutrons and number of electrons.

Nitrogen reacts with hydrogen to form ammonia, NH₃.

This is the equation for the reaction.

What is the missing number that balances the equation?

Tick (✓) one box.

Calculate the relative formula mass, M_r, of ammonia, NH₃.

Relative atomic masses (A_r): H = 1 N = 14

A student thinks that the empirical formula of ammonia is NH₃.

Explain why the student is correct.

Tick (✓) one box.

Fig. 14.1 shows the ball and stick model for a molecule of ammonia.

Fig. 14.1

Which statements about a ball and stick model are true, and which are false ?

Tick (✓) one box in each row.

Fig. 14.2 shows the structure of a molecule of ammonia.

Fig. 14.2

Complete the dot and cross diagram for a molecule of ammonia.

Only show the outer shell electrons.

Which row describes the nucleus of an atom?

Atoms are made from the sub-atomic particles protons, neutrons and electrons.

Table 12.1 shows the relative mass and relative charge of the three sub-atomic particles.

Complete Table 12.1 by writing the name of a sub-atomic particle in each space.

Table 12.1

An atom of phosphorus has an atomic number of 15 and a mass number of 31.

Calculate the number of protons, neutrons and electrons in this atom of phosphorus.

Phosphorus reacts with oxygen to form an oxide called phosphorus trioxide.

Phosphorus trioxide has the molecular formula P₄O₆.

What is the empirical formula of phosphorus trioxide?

Tick (✓) one box.

Complete the balanced symbol equation for the reaction of phosphorus trioxide with water.

Table 12.2 shows the melting point and boiling point of phosphorus trioxide.

Table 12.2

In the box draw the particle arrangement for phosphorus trioxide at 100 °C.

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.

This question is about diamond and graphite.

The diagram shows the structure of diamond.

Which element is diamond made from?

What is the maximum number of covalent bonds that each atom in diamond can form?

The atoms in diamond have a diameter of 0.000000000154 m.

What is the diameter of the atoms in standard form?

Tick (✓) one box.

The properties of diamond can be explained in terms of its structure and bonding.

Draw lines to connect each property with its correct explanation.

Lithium reacts with oxygen to form lithium oxide.

The symbols for lithium and oxygen on the Periodic Table are:

Explain how the positions of lithium and oxygen in the Periodic Table are used to decide that lithium is a metal and oxygen is a non-metal.

Use the Periodic Table on the Data Sheet.

Lithium reacts with oxygen to make lithium oxide.

Complete the balanced symbol equation for the reaction.

Write the electron arrangement for an atom of lithium.

A student thinks that sodium reacts in a similar way to lithium.

Explain why they are correct.

Use the Periodic Table on the Data Sheet.

Lithium can exist as two isotopes.

Explain what isotope means.

Lithium can be added to aluminium to make an alloy. One alloy contains 2% lithium.

A student draws a diagram of the alloy.

Calculate the percentage of lithium atoms in the alloy drawn by the student.

Suggest a reason why the student’s diagram is incorrect.

Lithium reacts with oxygen to form lithium oxide.

The symbols for lithium and oxygen on the Periodic Table are:

Explain how the positions of lithium and oxygen in the Periodic Table are used to decide that lithium is a metal and oxygen is a non-metal.

Use the Periodic Table on the Data Sheet.

Lithium reacts with oxygen to make lithium oxide.

Complete the balanced symbol equation for the reaction.

Write the electron arrangement for an atom of lithium.

When an atom of lithium reacts with oxygen it forms a lithium ion, Li +. (d)

Describe how an atom of lithium forms a lithium ion.

A student thinks that sodium reacts in a similar way to lithium.

Explain why they are correct.

Use the Periodic Table on the Data Sheet.

Lithium can exist as two isotopes.

Explain what isotope means.

Lithium can be added to aluminium to make an alloy. One alloy contains 2% lithium.

A student draws a diagram of the alloy.

Calculate the percentage of lithium atoms in the alloy drawn by the student.

Suggest a reason why the student’s diagram is incorrect.

The diagram shows the model of the atom developed by Rutherford.

The model developed by Rutherford was based on the results of an experiment performed whilst working with Geiger and Marsden.

They fired positively charged alpha particles at very thin gold foil.

State two observations made in the experiment and the conclusion Rutherford reached.

Describe how Bohr improved Rutherford’s model of the atom.

What is the typical atomic radius size of an atom in metres?

Give your answer in standard form.

What is the part of the atom labelled X called?

C Nucleus

D Shell

Atoms of the same element can have different structures.

Fig. 15.1 shows the structure of two different atoms, Y and Z, of the same element.

Fig. 15.1

What name is given to different atoms of the same element such as Y and Z ?

Write the number of protons, neutrons and electrons in an atom of Z.

Write the mass number of an atom of Z.

Write the name of the element that contains atoms of Y and Z.

Use the Periodic Table.

Complete Fig. 15.2 to show the arrangement of electrons in the ions.

What is the formula of the ionic compound formed when atoms of sodium react with atoms of Y ?

Tick (✓) one box.

Why does sodium react with Y and Z in a similar way?

Tick (✓) one box.

The ionic compound formed in Fig. 15.2 has a high melting point.

Explain why. Use ideas about structure and bonding.

Atoms of the same element can have different structures.

Fig. 11.1 shows the structure of two different atoms, Y and Z, of the same element.

Fig. 11.1

What name is given to different atoms of the same element such as Y and Z ?

Write the number of protons, neutrons and electrons in an atom of Z.

Write the mass number of an atom of Z.

Write the name of the element that contains atoms of Y and Z.

Use the Periodic Table.

Complete Fig. 11.2 to show the arrangement of electrons in the ions.

What is the formula of the ionic compound formed when atoms of sodium react with atoms of Y ?

Tick (✓) one box.

Why does sodium react with Y and Z in a similar way?

Tick (✓) one box.

The ionic compound formed in Fig. 11.2 has a high melting point.

Explain why. Use ideas about structure and bonding.

Atoms are made from protons, neutrons and electrons.

The table shows the relative mass and relative charge of a proton, neutron and electron.

Complete the table.

Write your answers in the three boxes in the table.

An atom of helium contains:

• 2 protons

• 2 neutrons

• 2 electrons.

Draw a labelled diagram to show the arrangement of protons, neutrons and electrons in an atom of helium.

Which two elements are in Group 1 of the Periodic Table?

Which element is in Period 4 of the Periodic Table?

Which element has a mass number of 12?

Which two elements are isotopes?

Which element forms an ion with a 2+ charge?

Aluminium forms an Al³⁺ ion and chlorine forms a Cl^– ion. (e)

Three students write down the formula of aluminium chloride.

Student A: A l C l

Student B: Al Cl₃

Student C: Al₃Cl

Which student is correct?

Explain your answer.

Fullerenes are allotropes of carbon that have many uses.

Fig. 15.1 shows a molecule of a fullerene.

Fig. 15.1

Which group of allotropes contain this fullerene?

Tick one (✓) box.

The carbon atoms in fullerenes are joined by covalent bonds.

Explain how two atoms of carbon form a covalent bond.

How many covalent bonds does one atom of carbon form in a molecule of fullerene, as shown in Fig. 15.1 ?

The model used to show the molecule of fullerene in Fig. 15.1 has limitations.

The table shows some statements about the model.

Which statements about this model are true, and which are false ?

Tick (✓) one box in each row.

Fullerenes can be used as lubricants. Lubricants reduce the friction between moving parts.

Fig. 15.2 shows a lubricant being sprayed onto the chain of a motorbike.

Fig. 15.2

Explain why fullerenes can be used as lubricants.

Use ideas about the structure and bonding of the fullerene shown in Fig. 15.1 in your answer.

A lubricant may need to be used at high temperatures.

Explain why fullerenes can be used at high temperatures.

Use ideas about the structure and bonding of the fullerene shown in Fig. 15.1 in your answer.

Which statement describes the isotopes of an element?

A Atoms that have different numbers of protons but the same number of electrons.

B Atoms that have different numbers of protons but the same number of neutrons.

C Atoms that have the same number of protons but different numbers of electrons.

D Atoms that have the same number of protons but different numbers of neutrons.

Fullerenes are allotropes of carbon that have many uses.

Fig. 11.1 shows a molecule of a fullerene.

Fig. 11.1

Which group of allotropes contain this fullerene?

Tick one (✓) box.

The carbon atoms in fullerenes are joined by covalent bonds.

Explain how two atoms of carbon form a covalent bond.

How many covalent bonds does one atom of carbon form in a molecule of fullerene, as shown in Fig. 11.1 ?

The model used to show the molecule of fullerene in Fig. 11.1 has limitations.

The table shows some statements about the model.

Which statements about this model are true, and which are false ?

Tick one (✓) box in each row.

Fullerenes can be used as lubricants. Lubricants reduce the friction between moving parts.

Fig. 11.2 shows a lubricant being sprayed onto the chain of a motorbike.

Fig. 11.2

Explain why fullerenes can be used as lubricants.

Use ideas about the structure and bonding of the fullerene shown in Fig. 11.1 in your answer.

A lubricant may need to be used at high temperatures.

Explain why fullerenes can be used at high temperatures.

Use ideas about the structure and bonding of the fullerene shown in Fig. 11.1 in your answer.

16* Helium and neon are the first two elements in Group 0 of the Periodic Table.

Look at the symbols for helium and neon.

Describe the similarities and differences in the atomic structures of helium and neon.

Look at the symbol for boron.

Which is the symbol for the element with an atom that contains 1 more proton and 2 more neutrons than an atom of boron?

Which statement best describes an atom?

A The nucleus is small compared to the atom and contains little of the atom’s mass.

B The nucleus is large compared to the atom and contains little of the atom’s mass.

C The nucleus is small compared to the atom and contains most of the atom’s mass.

D The nucleus is large compared to the atom and contains most of the atom’s mass.

Atoms are made of particles called protons, neutrons and electrons.

Complete the table to show the relative charges of protons, neutrons and electrons.

Sodium is a metal in the Periodic Table.

Sodium is an example of an atom that can form an ion.

Describe what happens to a sodium atom when it becomes an ion.

Look at this statement about the Periodic Table.

‘Atoms are placed in groups according to the total number of electrons they have.’

Explain why this statement is incorrect.

A new element has been discovered and has these properties:

• a high melting point

• reacts with oxygen to form oxides

• conducts electricity

• solid at room temperature.

Suggest what type of bonding the new element has.

Explain your answer.

Which statement best describes an atom?

A The nucleus is small compared to the atom and contains little of the atom’s mass.

B The nucleus is large compared to the atom and contains little of the atom’s mass.

C The nucleus is small compared to the atom and contains most of the atom’s mass.

D The nucleus is large compared to the atom and contains most of the atom’s mass.

The following table contains information about protons, neutrons and electrons.

One piece of information in the table is incorrect.

Which correction needs to be made?

A Electron charge should be 0.

B Electron mass should be 1.

C Neutron charge should be 0.

D Proton charge should be 0.

Aluminium, phosphorus and magnesium are all in Period 3 of the Periodic Table.

Aluminium has an atomic number of 13 and mass number of 27.

Describe the nucleus of an aluminium atom in terms of sub-atomic particles.

What is the overall charge on the nucleus of an atom of aluminium?

Which sub-atomic particles surround the nucleus?

Phosphorus has a higher atomic number and a higher mass number than aluminium.

A student says that phosphorus must be an isotope of aluminium because it has a different number of neutrons.

Is the student correct?

Tick (✓) one box.

Explain your answer.

Phosphorus can react with oxygen to form oxides. One oxide of phosphorus is called phosphorus pentoxide.

Phosphorus pentoxide has the molecular formula P₄O₁₀.

What is the empirical formula of phosphorus pentoxide?

Aluminium oxide and phosphorus pentoxide have different types of bonding.

The boiling point of aluminium oxide is 2977 °C.

The boiling point of phosphorus pentoxide is 360 °C.

What conclusion can you make about the type of bonding in each oxide?

Explain your answers.

The student is given a sample of the metal magnesium and a solution of an unknown nitrate of metal M, MNO₃(aq).

The student does an experiment to identify metal M.

The student weighs the magnesium. Then the student adds the magnesium to the solution of the metal nitrate.

A displacement reaction takes place forming metal M:

The student separates the metal M and then weighs metal M.

Look at the student’s results: Mass of magnesium = 0.729 g Mass of metal M = 6.476 g

Calculate the moles of magnesium used in the experiment.

Calculate the relative atomic mass of metal M.

Give your answer to 3 significant figures.

Use your answer from (d)(ii) and the Periodic Table to identify the metal M.