ATOMIC STRUCTURE AND PERIODIC TABLE QUESTIONS1.(a) (i) Complete the electronic configuration of the magnesium atom. (1)1s2 (ii) Complete the electronic configuration of the chlorine atom. (1)1s2 (b) (i) Write the equation, including state symbols, for the reaction of magnesium with chlorine. (2)(ii) Name the type of bonding present in magnesium chloride. (1)(iii) Draw a diagram (using dots or crosses) to show the bonding in magnesium chloride. Include ALL the electrons in each species and the charges present. (3) (c) State the type of bonding that exists in solid magnesium. (1)* (d) Explain fully why the melting temperature of magnesium is higher than that of sodium. (3)

2. (a) A gaseous sample of an element can be analysed using a mass spectrometer.(i) Describe briefly how positive ions are formed from gaseous atoms in a mass spectrometer. (2) (ii) What is used to accelerate the positive ions in a mass spectrometer? (1) (iii) What is used to deflect the positive ions in a mass spectrometer? (1) (b) The following data were obtained from the mass spectrum of a sample of chromium.Mass/charge ratio% abundance

50.04.3

52.083.8

53.09.5

54.02.4

Calculate the relative atomic mass of chromium in this sample. Give your answer to three significant figures.(2) (c) Explain why the four isotopes of chromium behave identically in chemical reactions. (1) (d) In which block of the Periodic Table is chromium found? (1)

3. (a) Define the term first ionization energy. (3) (b) Write an equation, with state symbols, to illustrate the process occurring when the second ionization energy of sodium is measured. (2)(c) The graph below shows the variation in the first ionization energies of some of the elements in Period 3.

(i) On the graph, use crosses to show the approximate values of the first ionization energies for the elements Na, P and S. Join the crosses to complete your graph. (1)* (ii) Explain why the first ionization energies generally increase across the period sodium to argon (Na to Ar).(3)* (iii) Explain why the first ionization energy of aluminium is less than that of magnesium. (2) (d) Place the following species in order of increasing first ionization energy, starting with the lowest S+ S S (1)4. The diagram below shows a mass spectrometer, which can be used to determine the percentage abundances of isotopes in an element.

(a) Explain, in terms of sub-atomic particles, what is meant by the term isotopes. (2) (b) Describe the role of the following parts of the mass spectrometer.(i) Electric field (1) (ii) Magnetic field (1) (c) A sample of the element barium is made up of four isotopes. The data below were taken from a mass spectrum of this sample.Mass/charge ratio% abundance

1359.01

13610.81

13712.32

13867.86

Calculate the relative atomic mass of the sample, giving your answer to one decimal place. (2)(d) The element bromine has two stable isotopes, 79Br and 81Br. How many peaks corresponding to Br2+ ions would be seen in the mass spectrum of bromine? Justify your answer. (2) (e) Suggest another application of mass spectrometry, other than to determine the relative atomic mass of an element. (1)

5. The relative atomic mass of an element is determined using a mass spectrometer.(a) Define the term relative atomic mass. (2) (b) The mass spectrum of rubidium is shown below.

(i) Explain why there are two peaks in the spectrum. (1) (ii) Use the spectrum to calculate the relative atomic mass of rubidium. (2)

6. The first ionization energy of each of the elements from neon to argon is shown on the graph below. The first ionization energy of potassium has been omitted.

(a) Define the term first ionization energy. (3)(b) Explain why, in moving from Na to Ar, the general trend is for the first ionization energy to increase.(3) (c) Explain why the first ionization energy decreases from P to S. (2) (d) Estimate the value of the first ionization energy of potassium, K, and write your answer below. (1)................................................... kJ mol1

7. (a) State how the following processes are achieved in a mass spectrometer.(i) Ionization of the sample. (1) (ii) Acceleration of the ions. (1) (iii) Deflection of the ions. (1) (b) State how you could find the molecular mass of a substance from its mass spectrum.(1) (c) Living things take up the radioactive isotope carbon-14 from the atmosphere. In recent years a particular linen cloth was shown, using mass spectrometry, to have been made from flax grown in the early 14th century. Suggest how mass spectrometry can be used to estimate the age of the cloth. (2)

*8. The melting temperatures of the elements of Period 3 are given in the table below. Use these values to answer the questions that follow.

(a) Explain why the melting temperature of sodium is very much less than that of magnesium. (3) (b) Explain why the melting temperature of silicon is very much greater than that of white phosphorus. (3) (c) Explain why the melting temperature of argon is the lowest of all the elements of Period 3. (1) (d) Explain why magnesium is a good conductor of electricity whereas sulfur is a non-conductor. (2)

9. (a) Define the term relative isotopic mass. (2) (b) Naturally occurring chlorine contains 75.53% of 35Cl and 24.47% of 37Cl.(i) Calculate the relative atomic mass of chlorine to four significant figures. (2)(ii) Two of the peaks in the mass spectrum of chlorine, Cl2, are at m/e 70 and 74. Identify the species giving rise to these peaks. (2)70 74 (iii) What is the m/e value of the other peak that you would expect to see in this region of the mass spectrum and the identity of the species giving rise to it? (2)Value Species

10. (a) Define the term first ionization energy. (2)*(b) Explain why the first ionization energy of the elements down Group 1 decreases even though the atomic number increases. (2) (c) The eleven successive ionization energies for sodium are given below. (i) Explain why the successive ionization energies increase.(1)*(ii) Explain how these ionization energies give evidence for the electronic structure of sodium. You may use a sketch graph if you wish. (2) (d) The first ionization energy of aluminium (element 13) is lower than that of magnesium (element 12).(i) Give the electronic structures of magnesium and of aluminium in s, p and d notation. (1)Magnesium Aluminium *(ii) Explain the difference in the first ionization energies of the two metals. (1)

11.Hydrogen has three isotopes, 1H, known as protium, 2H, deuterium, and 3H, tritium.(a) In terms of sub-atomic particles, give the similarities and differences between atoms of these three isotopes of hydrogen. (3) (b) When a nitrogen atom collides with a high energy neutron, one atom of tritium and one atom of another element are formed. Complete the equation below. (1) (c) Tritium-deuterium gas, consisting of molecules each containing one deuterium atom and one tritium atom, is used in some nuclear warheads. Typically, each warhead has about 4.0 g of the gas added.(i) Calculate the number of moles of tritium-deuterium in 4.0 g. (2)(ii) Calculate the volume, in cm3, of 4.0 g of tritium-deuterium gas. [Molar volume of a gas under these conditions = 24 000 cm3 mol1] (1) (d) Tritium is not usually included in calculations of the relative atomic mass of hydrogen, because it is radioactive and has a relatively short half-life. Calculate the relative atomic mass of hydrogen with the following isotopic composition. Give your answer to four decimal places. (2)(e) The electronic energy levels in hydrogen are shown below.

(i) Mark on the energy level diagram, with an arrow, the transition that represents the ionization energy of hydrogen. (1)(ii) In some versions of the Periodic Table, hydrogen is placed in the same group as sodium. Give the electronic configurations for both a hydrogen atom and a sodium atom, using the s and p notation.Use these electronic configurations to suggest why this is a reasonable grouping.(2)H Na *(f ) Which element in the Periodic Table has the highest first ionization energy? Justify your answer. (3)

12. This question is about the elements arsenic to rubidium which have atomic numbers 33 to 37. The first ionization energies, Em1, of these elements are given in the table.(a) Write the equation, with state symbols, which represents the first ionization energy of arsenic. (2)(b) Suggest the formulae of the hydrides of arsenic and selenium. (2)(c) (i) Complete the electronic configuration for an arsenic and a selenium atom using the electrons-in-boxes notation. (2)

*(ii) Explain why the first ionization energy of selenium is lower than that of arsenic. (2)*(d) Explain why the first ionization energy of krypton is higher than that of selenium.(2)*(e) Explain why the first ionization energy of rubidium is lower than that of krypton. (2) (f ) Which of the elements, arsenic to rubidium, is likely to have atoms with the smallest atomic radius? (1)

13 This question is about some of the elements in Period 3 of the Periodic Table.(a) (i) An atom of silicon has mass number 29. Complete the table below showing the numbers of sub-atomic particles in this atom of silicon. Use the Periodic Table as a source of data. (1)Sub-atomic particles present inone atom of 29SiNumber

protons

electrons

neutrons

(ii) Complete the electronic configuration of silicon. (1)1s2*(b) Explain the following, referring to differences in structure and bonding.(i) Silicon has a higher melting temperature than phosphorus. (3) (ii) Magnesium has a higher melting temperature than sodium. (2)(c) Suggest why the atomic radius decreases going across the Periodic Table from sodium to silicon. (2) (d) At room temperature, silicon tetrachloride, SiCl4, is a liquid that does not conductelectricity.Draw a dot and cross diagram illustrating the bonding in silicon chloride. Show only the outer electron shells of the atoms. Use crosses to represent the electrons from silicon and dots to represent the electrons from chlorine. (2)(e) The diagram below shows the values of the first ionization energies of sodium and magnesium.

(i) On the diagram, add crosses to mark the approximate positions for the values of the first ionization energies of the elements Al and Si. (1)*(ii) Justify your suggested values in terms of the atomic structure and electronic configuration of the elements.(2)Aluminium Silicon

14. In atoms, electrons fill up the sub-shells in order of increasing energy.(a) Fill in the last two boxes in the table below to show the order in which the next two sub-shells are filled.

(b) Electrons in atoms occupy orbitals. (i) Explain the term orbital. (1) (ii) Draw diagrams below to show the shape of an s-orbital and of a p -orbital. (2)s-orbital p-orbital(c) State the total number of electrons occupying all the p-orbitals in one atom of chlorine. (1) (d) State the number of electrons present in an ion of calcium, Ca2+. (1)*(e) Define the term first ionization energy. (3) (f ) The ionization energies of sodium, Na, are shown in the table below. Show with a tick (_), in the third row of the table below, all the ionization numbers that involve the removal of an electron from an s-orbital.(2)

Ionization energy KJ mol-14964563691395441335216611201152549128934141367159071

Ionization number1st2nd3rd4th5th6th7th8th9th10th11th

15 (a) In a mass spectrometer being used to determine relative atomic masses, gaseous atoms are ionized. The ions are then accelerated and deflected before being detected.(i) Explain how atoms are ionized in a mass spectrometer. (1) (ii) How are the ions accelerated in a mass spectrometer? (1) (iii) How are the ions deflected in a mass spectrometer? (1)(b) The following data were obtained from the mass spectrum of a sample of platinum.Peak at m/e%

19432.8

19530.6

19625.4

19811.2

Calculate the relative atomic mass of platinum in this sample. Give your answer to one decimal place. (2)(c) In which block of the Periodic Table is platinum found? (1)(d) Most solids exist as lattice structures.(i) Complete the table, using a tick if the substance conducts electricity or a cross if the substance does not conduct electricity.(2)SubstanceConducts electricity in theSOLID state? Conducts electricity in theLIQUID state?

Sodium, Na

Sodium oxide, Na2O

*(ii) Explain the electrical conductivities of sodium and of sodium oxide in the solid and liquid states. (3)

16 This question concerns the Periodic Table.(a) An atom of argon has mass number 40. Complete the table below showing the numbers of sub-atomic particles in this atom of argon. Use the Periodic Table as a source of data.(1)Sub-atomic particles present inone atom of 40ArNumber

Protons

electrons

neutrons

(b) An atom of potassium has mass number 39. Explain why argon is placed before potassium in the modern Periodic Table. (1) (c) In the context of the Periodic Table, explain what is meant by the term periodicity.(2)(d) The graph shows the variation in melting temperatures of the elements across Period 3 (Na to Ar) of the Periodic Table.(i) Name one of the elements above that is composed of simple molecules at room temperature and pressure. (1) (ii) Silicon has a giant atomic structure. Explain how this structure results in the high melting temperature shown on the graph. (2)(iii) Explain why the melting temperature of magnesium is higher than that of sodium. (3)

17 Naturally occurring samples of potassium contain three isotopes, 39K, 40K and 41K.(a) The isotopes can be separated in a mass spectrometer.(i) In the diagram below, particles are ionized at A and detected at D. Name the processes occurring in the mass spectrometer at B and C. (2)B C (ii) A sample of potassium has the following composition.Isotope39K 40K 41K

% abundance93.220.126.66

Calculate the relative atomic mass of this sample of potassium, giving your answer to two decimal places. (2)(iii) Complete the table below to show the numbers of sub-atomic particles in an atom of each of the isotopes 39K and 41K. (1)IsotopeElectronsprotonsNeutrons

39K

41K

(iv) Complete the electronic configuration for an atom of 39K. (1)1s2 (v) Why is potassium placed after argon in the Periodic Table, even though it has a smaller relative atomic mass? (1)*(vi) Explain why a potassium ion is smaller than a potassium atom. (2) (b) The type of bonding in potassium is metallic. Draw a labelled diagram to illustrate the metallic bonding in potassium. (2) (c) The graph shows the variation of first ionization energy with atomic number for six successive elements in the Periodic Table, including potassium. The letters used to label the elements are not their symbols. (i) Define the term first ionization energy. (3) (ii) Identify, with a reason, which element is potassium. (1)

18 This question is about atomic structure.(a) Draw diagrams to show the shape of an s-orbital and of a p-orbital. (2)s-orbital p-orbital

(b) Complete the table to show the number of electrons that completely fill the following regions. (3)RegionNumber of electrons presentwhen completely filled

a d-orbital

a p sub-shell

the third shell (n = 3)

(c) The energy diagram below is for the eight electrons present in an oxygen atom. Complete the diagram for an oxygen atom by adding labels to identify the other occupied sub-shells arrows to show how the remaining six electrons are arranged in the orbitals. (2)

(d) Successive ionization energies provide evidence for the arrangement of electrons in atoms. The eight successive ionization energies of oxygen are shown in the table below. Ionizationnumber1st 2nd 3rd 4th 5th 6th 7th 8th

Ionization energy/ kJ mol1

1314 3388 5301 7469 10989 13327 71337 84080

(i) Define the term first ionization energy. (3)(ii) Write an equation, with state symbols, to show the third ionization energy of oxygen.(2)*(iii) Explain how the data in the table provide evidence that there are two occupied electron shells in an oxygen atom. (2)

Section A questions.1. When an Al4+ ion is formed from an Al atom, the fourth electron is lost from theA 1s sub-shell.B 2s sub-shell.C 2p sub-shell.D 3s sub-shell.2. Which pair of ions is isoelectronic?A Ca2+ and O2B Na+ and O2C Li+ and ClD Mg2+ and Cl3. Bromine has two isotopes with relative isotopic masses 79 and 81. Which of the following values for mass/charge ratio could correspond to a peak in the mass spectrum of bromine, Br2? You should assume the ions detected have a single positive charge.A 79.9B 80C 159D 1604 The first five ionization energies of an element, X, are shown in the table.

What is the mostly likely formula of the oxide that forms when X burns in oxygen?A X2OB XOC X2O3D XO25 Which of the following has the largest ionic radius?A S2B ClC K+D Ca2+6 In which of the following series does the melting temperature of the element increase from left to right?A Li, Na, KB Al, Si, PC Si, P, SD Na, Mg, Al7 Which of the following represents the electronic structure of a nitrogen atom?

8 The electronic structures of four elements are given below. Which of these elements has the highest first ionization energy?

9 Which of the graphs shows (from left to right) the trend in the ionic radius of the isoelectronic ions N3, O2, F, Na+, Mg2+, Al3+?

10 The first eight ionization energies for an element in kJ/mol are: 789, 1577, 3232, 4356, 16091, 19785, 23787, 29253. The element is inA Group 1B Group 2C Group 3D Group 411 Which of the following graphs shows the variation in the ionic radius of the Group 2 elements?

12 The first five ionization energies of an element, Z, are: 790, 1600, 3200, 4400, 16100 kJ mol1In which group of the Periodic Table is Z found?A 2B 3C 4D 513 The electronic configurations of the atoms of four different elements are given below. For which element would you expect the value of the first ionization energy to be the largest?A 1s1B 1s2C 1s2 2s1D 1s2 2s214 Which of the following has the smallest ionic radius?A FB Na+C Mg2+D O215 Which pair of atomic numbers represents elements which are both in the p-block of thePeriodic Table?A 4, 8B 6, 12C 8, 16D 10, 2014 The electronic structure of an atom of an element in Group 6 of the Periodic Table could beA 1s2 2s2 2p2B 1s2 2s2 2p4C 1s2 2s2 2p6 3s2 3p6 3d6 4s2D 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p616 Which of the following formulae for compounds of germanium, Ge, is unlikely to be correct, given the position of germanium in the Periodic Table?A GeF3B GeS2C GeO2D GeH417 The first five successive ionization energies of an element, X, are shown in the table below.Ionization energy first second third fourth fifthValue/ kJ mol1 590 1100 4900 6500 8100Which ion is X most likely to form when it reacts with chlorine?A X+B X2+C X3+D X4+18 The nucleus of a atom containsA 11 protons and 12 neutrons.B 11 protons and 12 electrons.C 23 protons and 11 neutrons.D 23 protons and 11 electrons.19 The mass spectrum for a sample of a metal is shown below.The relative atomic mass of the metal isA 63.2B 63.4C 63.6D 64.020 Going across the Periodic Table from sodium to aluminium,A the melting temperature increases.B the radius of the atom increases.C the radius of the metal ion increases.D the bonding in the element changes from metallic to covalent.21 Going down Group 1 from lithium to rubidiumA the radius of the atom decreases.B the radius of the ion decreases.C the first ionization energy decreases.D the polarizing power of the ion increases.22 The graph below shows the second ionization energy of a series of elements with consecutive atomic numbers. Which element could be lithium?ABCD