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Question 1
An atom of nitrogen can form a nitride ion with an electronic configuration of 1s22s22p6. |
a) | State the formula of the nitride ion.
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b) | An element forms an ion, W, with a single negative charge that has the same electron configuration as the nitride ion. State the formula of W.
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c) | An element forms an ion, R, with a single positive charge that has a full 3p sub-shell as its highest energy level. State the formula of R.
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Question 2
a) | Define the term isotope.
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b) | Define the term relative atomic mass.
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c) | Calculate the relative atomic mass of silicon using information in the table below. Give your answer to two decimal places.
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Question 3
In the late 1800s physist JJ Thomson discovered the electron. He proposed the 'plum pudding' model of the atom whereby negatively-charged electrons were distributed evenly throughout a sphere of positive charge. The figure below shows an atom of element Q using the ‘plum pudding’ model. An atom of Q contains eight electrons. |
a) | State two differences between the ‘plum pudding’ model and the model of atomic structure used today.
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b) | Deduce the full electron configuration of an atom of element Q.
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c) | Complete the missing values in the table to show the numbers of sub-atomic particles in an atom and an ion of magnesium.
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d) | Explain why different isotopes of magnesium have similar chemical properties.
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Question 4
a) | Give the full electronic configuration of an atom of sulfur.
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b) | Give the full electronic configuration of a copper(II) ion.
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c) | Time of flight mass spectrometry is used to analyse a sample of tin. The sample is ionised by electron impact to form 1+ ions. The mass spectrum of this sample of tin has four peaks. Data from the spectrum is shown in the table below. |
Calculate the relative atomic mass of tin in this sample. Give your answer to one decimal place.
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Question 5
This question is about atomic structure. |
a) | Define the mass number of an atom.
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b) | The table below gives some isotopic information about an atom and an ion of nickel. Identify the missing values A-D.
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c) | A sample of nickel contains three isotopes, 58Ni, 60Ni and 62Ni. This sample has a relative atomic mass of 58.7 In this sample the ratio of abundance of isotopes 60Ni and 62Ni is 7:1 |
Calculate the percentage abundance of 58Ni in this sample. Give your answer to one decimal place.
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d) | The figure below is a model proposed by Rutherford to show the structure of an atom. |
State two features of the current model that are not shown in the Rutherford model.
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Question 6
a) | State the number of electrons that can fill the first 4 energy levels. First energy level = electrons Second energy level = electrons Third energy level = electrons Fourth energy level = electrons two eight eighteen thirty two
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b) | A sample of iron, which consists of three isotopes, has a relative atomic mass of 55.909. The isotopic information for two of the isotopes is shown in the table below. The data for one of the isotopes, mFe, is missing. |
Use this data to calculate m, the mass number of mFe.
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Question 7
This question is about isotopes. Most elements contain atoms of different isotopes. |
a) | State one similarity and one difference between the atomic structures of isotopes of the same element.
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b) | Mass spectrometry can be used to identify the isotopes of chlorine. Part of the mass spectrum of chlorine is shown below. |
c) | Calculate the relative atomic mass of chlorine. Give your answer to two decimal places.
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c) | Three molecular ion peaks, M+, are found in the mass spectrum of chlorine, Cl2. The three M+ peaks have m/z values of 70, 72 and 74 respectively. Suggest why each M+ peak is observed.
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Question 8
Elements are arranged into blocks in the Periodic Table based on their electron configuration. We now know that electrons are in shells; shells have sub-shells and sub-shells have orbitals. |
a) | Define the term orbital.
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b) | State the maximum number of electrons which can fill each region of an atom: The 2s orbital: electrons The 2p orbital: electrons The 3d sub-shell: electrons The third energy level: electrons 2 6 10 18
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c) | Write the full electronic configuration of an atom of copper.
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d) | An atom has 2 more protons and 5 more neutrons than an atom of 65Zn. Write the symbol, including the mass number, for this atom:
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e) | Draw the shape of an s orbital and the shape of a p orbital.
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Question 9
This question is about the isotopes of krypton. A sample of krypton containing the isotopes 82Kr, 83Kr, 84Kr and 86Kr has a relative atomic mass of 83.8. The sample contains 11.6% each of the 82Kr and 83Kr isotopes. |
a) | Calculate the percentage abundance of each of the other two isotopes. Give your answers to one decimal place.
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Question 10
The mass spectrum of a sample of selenium is shown below. |
a) | Use this spectrum to calculate the relative atomic mass of this sample of selenium. Give your answer to one decimal place.
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b) | Explain why the Ar value of selenium you have calculated differs slightly from the relative atomic mass given in the Periodic Table.
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