Subatomic particles

Atoms of neon are made up of subatomic particles.

Figure 9 shows some information about the subatomic particles in neon atoms.

Complete Figure 9 with the missing information.

All atoms of neon have an atomic number of 10.

Describe what information about the number of subatomic particles can be obtained from the atomic number of neon.

Explain why atoms of neon are electrically neutral.

*(b) The structure of the periodic table and the position of the elements in the periodic table are linked to the electronic configuration of the elements.

Figure 10 shows the structure of the periodic table and the first 12 elements with their atomic numbers.

group

Use the first 12 elements shown in Figure 10 to explain

• how the structure of the periodic table is linked to the electronic configuration of the atoms of the elements

• how the arrangement of the elements is linked to their electronic configuration.

Atoms of neon are made up of subatomic particles.

Figure 1 shows some information about the subatomic particles in neon atoms.

Complete Figure 1 with the missing information.

All atoms of neon have an atomic number of 10.

Describe what information about the number of subatomic particles can be obtained from the atomic number of neon.

Explain why atoms of neon are electrically neutral.

A sample of neon contains three isotopes

90.48% of neon-20

0.27% of neon-21

9.25% of neon-22

Using this information, calculate the relative atomic mass of this sample of neon.

relative atomic mass =_........

This question is about molecules containing two atoms.

In an experiment, hydrochloric acid is reacted with zinc.

The volume of gas produced is measured by collecting the gas in an upturned measuring cylinder over water.

Give a method of collecting and measuring the gas that would give a more accurate volume of gas.

Iodine has an atomic number of 53 and a mass number of 127.

How many electrons are there in an iodine molecule, I₂?

Iodine reacts with hydrogen to form hydrogen iodide, H I.

Explain whether or not a solution of hydrogen iodide in water conducts electricity.

Chlorine gas is bubbled through a colourless solution of potassium bromide, KBr. The mixture turns orange.

Give the name of the substance that causes the orange colour.

Write the balanced equation for this reaction.

Hydrogen iodide reacts with oxygen to form water and iodine.

The equation for this reaction is

Calculate the energy change for this reaction using the bond energies in Figure 7.

Include a sign and unit in your answer.

energy change =_........

Chlorine reacts with silicon to form silicon chloride.

A sample of silicon chloride contains 1.4 g of silicon atoms and 7.1 g of chlorine atoms.

Calculate the empirical formula of this sample of silicon chloride.

(relative atomic masses: Si = 28, C l = 35.5)

empirical formula =_........

The modern periodic table is organised into groups and periods.

State in which group and in which period of the periodic table silicon is found.

You should use the periodic table to help you answer this question.

group =_........

period =_........

Describe two differences between Mendeleev’s periodic table and the modern periodic table.

Figure 1 shows the structure of a molecule of each of four compounds, A, B, C and D.

The formula of a molecule of compound A is H₂O.

Give the formula of a molecule of compound D.

The names of two of the compounds in Figure 1 are shown below.

Draw one straight line from each name to the structure of a molecule of that compound.

Figure 2 shows information about the number of electrons in the outer shell of each of the different atoms in a molecule of compound C.

Use the information in Figure 2 to complete the dot and cross diagram for a molecule of compound C.

The atomic number of phosphorus, P, is 15.

One atom of phosphorus has a relative atomic mass of 31.

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

number of protons =_........

number of neutrons =_........

number of electrons =_........

An atom of aluminium has an atomic mass of 27.

Aluminium has an atomic number of 13.

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

number of electrons =_........

number of neutrons =_........

number of protons =_........

Aluminium reacts with bromine to form aluminium bromide. A sample of aluminium bromide contains 1.35 g of aluminium atoms and 12.00 g of bromine atoms.

Calculate the empirical formula of this sample of aluminium bromide.

(relative atomic masses: A l = 27.0, Br = 80.0)

empirical formula =_........

Gallium is in the same group in the periodic table as aluminium and in the same period in the periodic table as bromine.

State in which group and period of the periodic table gallium can be found.

You may want to refer to the periodic table.

group =_........

period =_........

Gallium had not been discovered when Mendeleev created his first periodic table.

Figure 5 shows some properties of gallium that Mendeleev predicted and some of the actual properties of gallium.

Describe how Mendeleev predicted these properties of gallium.

Chlorine has an atomic number of 17.

Figure 3 shows the arrangement of electrons in an atom of chlorine.

What is the electronic configuration of this atom?

Explain, using Figure 3, why chlorine belongs to group 7 of the periodic table.

The nucleus of an atom is made up of protons and neutrons. Atoms of chlorine contain 17 protons.

Figure 4 shows some information about a proton, a neutron and an electron.

Explain, using the information in Figure 3 and Figure 4, why atoms of chlorine have no overall charge.

Atoms of chlorine-37 have a mass number of 37.

Calculate the number of neutrons in atoms of chlorine-37.

number of neutrons =_........

There are two isotopes of chlorine, chlorine-35 and chlorine-37.

Explain the meaning of the term isotopes.

Calcium has an atomic number of 20. A calcium atom has a mass number of 40.

Which row of the table shows the number of protons and number of neutrons in this atom of calcium?

Figure 6 shows the arrangement of electrons in an atom of calcium.

Explain, using the information in Figure 6, in which period of the periodic table calcium can be found.

Calcium and potassium react with water in similar ways.

One similarity in the reactions is that hydrogen gas is produced.

State one other similarity in the products of the reactions of calcium and potassium with water.

Potassium is higher in the reactivity series than calcium and reacts more vigorously with water than calcium reacts with water.

State why potassium is higher in the reactivity series and reacts more vigorously with water than calcium.

*(c) Calcium chloride can be prepared by the reaction of calcium with chlorine gas.

Figure 7 shows some properties of calcium, chlorine and calcium chloride.

Explain, in terms of bonding and structure, why the properties of the product, calcium chloride, are different from the properties of the reactants, calcium and chlorine.

In Figure 5, 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.

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

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

give the letters of two elements in period 2

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

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

All atoms of element E in this sample contain

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.

In Figure 1, 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.

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

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

give the letters of two elements in period 2

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

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

All atoms of element E in this sample contain

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 =_........

Plants release oxygen into the atmosphere.

What is the name of the process that releases oxygen into the atmosphere?

The atmosphere contains 21% of oxygen.

Figure 1 shows an incomplete bar chart of the main gases in the atmosphere.

Complete the bar chart by showing the percentage of oxygen in the atmosphere.

Calculate the volume of oxygen present in 300 cm³ of air.

(volumes are measured under the same conditions of temperature and pressure)

volume of oxygen =_........ cm³

An atom of an element has an atomic number and a mass number.

Draw one straight line from each of these to the numbers of subatomic particles it shows to be present in an atom.

number of subatomic particles in an atom

Which test shows a gas is oxygen?

(a) Atoms contain electrons, neutrons and protons.

Draw one line to link each particle to its correct relative charge.

Which of the following is the relative mass of a proton?

Argon is in group 0 of the periodic table.

Identify, using the periodic table on the back cover of this paper, which of these elements is in the same period as argon.

Figure 1 shows the atomic number and mass number of two isotopes of argon.

Describe the structure of an atom of argon-38 and of an atom of argon-40.

(a) A chlorine atom contains 17 electrons, 18 neutrons and 17 protons.

State the mass number of this chlorine atom.

Give the electronic configuration of this chlorine atom.

Describe what you would see if damp, blue litmus paper is placed into chlorine gas.

Chlorine exists as diatomic molecules.

In a molecule, two chlorine atoms are joined by a covalent bond.

Describe what is meant by a covalent bond.

Explain why chlorine is a gas, rather than a liquid, at room temperature.

When the gas hydrogen chloride, HC l, is dissolved in water, a solution forms. Blue litmus paper dipped in this solution turns red.

State why the litmus paper turns red.

Figure 7 lists the halogens in the order in which they appear in group 7 of the periodic table.

The melting points of four of the halogens are given.

Estimate the melting point of iodine.

_........ °C

Bromine reacts with heated iron.

Give the name of one halogen that would react with iron more vigorously than bromine.

(a) A chlorine atom contains 17 electrons, 18 neutrons and 17 protons.

State the mass number of this chlorine atom.

Give the electronic configuration of this chlorine atom.

Describe what you would see if damp, blue litmus paper is placed into chlorine gas.

Chlorine exists as diatomic molecules.

In a molecule, two chlorine atoms are joined by a covalent bond.

Describe what is meant by a covalent bond.

Explain why chlorine is a gas, rather than a liquid, at room temperature.

When the gas hydrogen chloride, HC l, is dissolved in water, a solution forms. Blue litmus paper dipped in this solution turns red.

State why the litmus paper turns red.