Complete the following table.
| Subatomic particle | Relative Charge | Relative Mass |
| Proton | 1 | |
| Neutron | ||
|
Electron |
 |
3 marksComplete the following table.
| Species | Number of protons | Number of neutrons | Number of electrons |
| 31P | |||
| 24Na+ | |||
| 37Cl– |
State the definition for relative atomic mass.
Explain why the chemical properties of 35Cl and 37Cl are the similar.
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2 marksSilicon exists as three isotopes, 28Si, 29Si and 30Si. In terms of the subatomic particles, state the difference between these isotopes of silicon.
1 markNaturally occurring isotopes of Europium are shown in Table 1. Calculate the relative atomic mass of Europium. Give your answer to 1 d.p.
| m/z value | 151 | 153 |
| Abundance / % | 47.8 % | 52.2 % |
1 markFigure 1 represents the mass spectrum of potassium. Use the information in the image to calculate the relative atomic mass of potassium.
Potassium reacts with water in a violent reaction to form potassium hydroxide solution and hydrogen. Write a balanced symbol equation, including state symbols, for this reaction.
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3 marksState the formula of the following compounds
State the names of the following compounds.
Write a balanced symbol equation for the reaction of magnesium oxide and hydrochloric acid to form magnesium chloride and water.
Ethanol, C2H5OH, burns in oxygen to form carbon dioxide and water. Write the balanced symbol equation for this reaction.
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State the definition for relative isotopic mass.
1 markDetermine the number of neutrons in atom of element X with mass number 58 and 26 protons.
3 marksA sample of Antinomy was analysed in the mass spectrometer and two main isotopes were found, 121Sb and 123Sb. Use your periodic table to help you give the number of protons and neutrons in both 121Sb and 123Sb of Antimony.
1 markFigure 1 represents the mass spectrum of antimony. Use the information in the image to calculate the relative atomic mass of antimony.
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Silicon exists as three isotopes, 28Si, 29Si and 30Si. In terms of the subatomic particles, state the difference between these isotopes of silicon.
A student stated that the isotopes of silicon will have different chemical properties due to the different mass numbers. Is the student correct? Justify your answer.
2 marksBeryl is a mineral composed of beryllium aluminium silicate with the formula Be3Al2Si6O18. Calculate the relative formula mass.
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In this part, you need to refer to the Periodic Table of the Elements in the Data Sheet.
From the first 18 elements only, choose an element which fits the following descriptions:
| 577 | 1820 | 2740 | 11600 |
2 marksA sample of element G was extracted from a meteorite. Table 1 shows the relative abundance of each isotope in a mass spectrum of this sample of G. Calculate the relative atomic mass of G and suggest an identity of G. Give your answer to 1 d.p.
Table 1
| Relative isotopic mass | 64 | 66 | 67 | 68 |
| % abundance | 38.9 | 27.8 | 14.7 | 18.6 |
Sometimes in the mass spectrum on G a very small peak with an m/z value of 32 is present. Explain the occurrence of this peak.
3 marksElement G can be alloyed with tin and lead to make solder. Lead exists as four isotopes shown in Table 2 and has an Ar value of 207.241.
Calculate the relative isotopic mass of W. Give your answer to 3 significant figures.
| Relative isotopic mass | W | 206 | 207 | 208 |
| % abundance | 1.4 | 24.1 | 22.1 | 52.4 |
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Oxyacids of chlorine include, HClO, HClO2, HClO3 and HClO4.
An acid base reaction occurs between a solution of HClO4 is added to a solution of strontium hydroxide.
Write a balanced symbol equation for this reaction including state symbols.
3 marksChlorine has two naturally occurring isotopes. 35Cl with a mass of 34.969 and 37Cl with a mass of 36.966.
The relative atomic mass of Cl is 35.5. Calculate the abundance of each isotope to 2 d.p.
Predict the size of the atomic radius of 35Cl relative to the atomic radius of 37Cl would be the largest. Explain your answer.
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Borax is one of the most important compounds of boron. The formula of anhydrous borax is Na2B4O7.
Anhydrous borax produces a sodium hydroxide and orthoboric acid, H3BO3, when dissolved in water.
Write an equation for this reaction.
5 marksA naturally occurring sample of the element boron, B, has two isotopes 10B and 11B and a relative atomic mass of 10.8.
3 marksHydrated borax powder has the formula Na2B4O7.xH2O when 2.01 g of hydrate is heated in a crucible until a constant mass is reached. The mass of the anhydrous Na2B4O7 salt is 1.01 g.
Calculate the value of x and therefore deduce the name of hydrated borax powder.
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Sulfur, S8, is a yellow solid that can react with nitric acid to form sulfuric acid, a brown gas, and water.
Write a balanced symbol equation for this reaction.
3 marksSulfur exists as four isotopes and has a relative atom mass of 32.0928.
Figure 1 shows the relative intensities of three of these isotopes. The total relative abundance is 94.99.
Calculate the relative isotopic mass of the fourth isotope of sulfur.
Predict and explain whether or not the isotopes of sulfur would have the same chemical properties.
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3 marksCopper is an easily moulded base metal that is often added to precious metals to improve their elasticity, flexibility, hardness, colour, and resistance to corrosion.
Table 1 shows the number of protons, neutrons and electrons of different isotopes and ions of copper.
| Species | Protons | Neutrons | Electrons |
| 34 | 27 | ||
| 65Cu+ | 29 |
3 marksCalculate the percentage abundance of 63Cu with a mass of 62.9296 and 65Cu with a mass of 64.9278, when the average mass of the Cu isotope is 63.546.
Give your answer to an appropriate number of significant figures.
Copper can form a salt with chlorine to form copper(II) chloride. This reacts with sodium phosphate to form two different salts only.
Write a balanced equation for this reaction.
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2 marksAtoms are made up of three subatomic particles; protons, neutrons and electrons.
| Particle | Proton | Neutron | Electron |
| Mass / kg | 1.673 x 10–27 | 1.675 x 10–27 | 9.000 x 10–31 |
Using the data and the Periodic Table, calculate the mass of one atom of carbon in kg.
1 mark12C, 13C and 14C are all isotopes of carbon.
State the difference between these three isotopes in terms of subatomic particles.
2 marksA student claims that the different isotopes of carbon will have different chemical properties.
Is the student correct? Explain your answer.
4 marksData on the relative isotopic abundance of a chemical element, E, is shown.
| Relative m/z | 46 | 47 | 48 | 49 | 50 |
| % abundance | 8.02 | 7.31 | 73.81 | X | 5.32 |
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3 marksThe Bohr model of an atom represents a central nucleus, consisting of protons and neutrons, with electrons surrounding it moving in circular orbits.
This model was proposed by Niels Bohr in 1913 and after some further research, energy levels and sublevels were recognised, and the model was refined.
Using your knowledge of atomic structure, complete the table for the particles found in an atom.
| Particle | Relative charge | Relative mass |
| Proton | ||
| Neutron | ||
| Electron |
2 marksState the block in the Periodic Table in which silicon is placed and explain your answer.
2 marksThe graph shows the mass spectrum of a sample of silicon.
Calculate the relative atomic mass, Ar, of this sample of silicon to 1 decimal place.
1 markSuggest why the relative atomic mass on the Periodic Table might be different to the relative atomic mass of a sample analysed using a mass spectrometer.
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1 markGeraniol is a colourless oil containing two carbon-carbon double bonds and one other functional group. It is the main component of citronella oil with low water solubility, but it is soluble in common organic solvents.
State the other functional group present in geraniol.
1 markThe mass spectrum of geraniol is shown below.
Deduce the relative molecular mass of geraniol.
2 marksA molecular formula of C7H54O is proposed for geraniol.
3 marksUsing your previous answers, suggest a molecular formula for geraniol.
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1 markSilicon is a hard, brittle, blue-grey crystalline semiconductor. It is also described as a tetravalent metalloid.
State the formulae of two common silicon ions.
1 markThe silicate ion is analogous to the carbonate ion.
Suggest the formula of the silicate ion.
2 marksWrite a balanced ionic equation to show the formation of aluminium silicate.
2 marksCalcium silicate can be used to store or trap carbon dioxide.
Write a balanced symbol equation for this reaction showing the formation of two solid products.
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3 marksA and B are different chemical elements, from different groups in the Periodic Table.
State why mA and nA have identical chemical properties, but mA and pB have different chemical properties.
3 marksAn atom has twice as many protons, and twice as many neutrons, as an atom of 19F.
Determine the chemical symbol for this atom, including the mass number, and deduce the number of electrons.
1 markName an instrument which would be used to measure the relative abundances of isotopes of an element
5 marksExplain the graph which would be produced when measuring the relative abundances of isotopes in an element.
Describe how the graph and data obtained can be used to calculate the relative atomic mass of the element in question.
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