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IB Chemistry SL - 2024 - Questionbank

Topic 3 All - Periodicity

All Questions for Topic 3 (Periodicity). Periodic Table, Periodic Trends

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Question 1

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An outline of the periodic table is shown below:

3.1-547

Which of the following are the correct names for the groups labelled X, Y and Z?


XYZ
\hspace{1em} A.\hspace{1em}Transition metalsHalogensNoble gases
\hspace{1em} B.\hspace{1em}Transition metalsNoble gasesHalogens
\hspace{1em} C.\hspace{1em}Alkali metalsHalogensNoble gases
\hspace{1em} D.\hspace{1em}Alkali metalsNoble gasesHalogens

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Question 2

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Chromium appears to the right of vanadium in the periodic table, as shown below:

3.1-556

Which of the following statements is true?

  • A.\hspace{1em}Cr atoms always have a higher atomic number and atomic mass than V atoms

  • B.\hspace{1em}Cr atoms have a higher atomic mass than V atoms but the atomic number may be lower

  • C.\hspace{1em}Cr atoms have a higher atomic number than V atoms but the atomic mass may be lower

  • D.\hspace{1em}Cr atoms may have a lower atomic number or atomic mass than V atoms

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Question 3

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Which chemical equation represents the definition of first ionization energy?

  • A.\hspace{1em}X(s)_{(s)}+ e^- → X(s)^-_{(s)}

  • B.\hspace{1em}X(s)_{(s)}→ X(s)+^+_{(s)} + e^-

  • C.\hspace{1em}X(g)_{(g)} → X(g)+^+_{(g)} + e^-

  • D.\hspace{1em}X(g)_{(g)}+ e^- → X(g)^-_{(g)}

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Question 4

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Which element would have the least attraction for a shared pair of electrons in a covalent bond?

  • A.\hspace{1em}Carbon

  • B.\hspace{1em}Nitrogen

  • C.\hspace{1em}Oxygen

  • D.\hspace{1em}Fluorine

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Question 5

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A group 2 metal oxide dissolved in water would produce a solution that is:

  • A.\hspace{1em}Acidic

  • B.\hspace{1em}Basic

  • C.\hspace{1em}Neutral

  • D.\hspace{1em}Possibly either acidic or basic

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Question 6

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Metalloid elements play important roles in electronic components, such as solar cells and computer chips. Which of the following is the correct definition of a metalloid?

  • A.\hspace{1em}Elements with a mixture of metallic and non-metallic physical properties

  • B.\hspace{1em}Elements that convert from metals to non-metals with changing temperature

  • C.\hspace{1em}Metals found in the p block of the periodic table

  • D.\hspace{1em}Metals with incomplete d subshells

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Question 7

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The electron affinity of carbon is -122 kJ mol1 kJ\ mol^{-1}, whereas the electron affinity of boron is -27 kJ mol1 kJ\ mol^{-1}. Which statement below best explains this difference?

  • A.\hspace{1em}Carbon has more protons resulting in an increased attraction for its valence electrons

  • B.\hspace{1em}The electrons in boron are located in a lower energy level than carbon

  • C.\hspace{1em}Boron has fewer electrons than carbon

  • D.\hspace{1em}The trend decreases from left to right across the periodic table

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Question 8

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For elements in the same row X or column Y of the periodic table, some features of the outer electron shell remain constant.

3.1-552

Which of the following is correct?


Name of XName of YNumber of electron shellsNumber of outer shell electrons
\hspace{1em} A.\hspace{1em}PeriodGroupConstant across XConstant down Y
\hspace{1em} B.\hspace{1em}PeriodGroupConstant down YConstant across X
\hspace{1em} C.\hspace{1em}GroupPeriodConstant across XConstant down Y
\hspace{1em} D.\hspace{1em}GroupPeriodConstant down YConstant across X

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Question 9

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[Maximum mark: 3]

The reaction shown below will not occur under standard conditions:

Br2(l)_{2{(l)}} + 2 NaF(aq)_{(aq)} → F2(g)_{2{(g)}} + 2 NaBr(aq)_{(aq)}

  1. State a balanced chemical equation for a reaction that will occur, producing sodium bromide. [2]

  2. Describe an observation that allows the progress of the monitoring of the reaction written in part (a). [1]

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Question 10

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The atomic numbers in two periods of the d block of the periodic table are shown below:

3.1-553

Why does the atomic number increase by a larger amount across period 6 of the d block than across period 5?

  • A.\hspace{1em} In the period 6 lanthanoids, electrons are added to 7 f orbitals rather than the d subshell.

  • B.\hspace{1em} In the period 6 lanthanoids, electrons are added to 14 f orbitals rather than the d subshell.

  • C.\hspace{1em} In the period 6 actinoids, electrons are added to 7 f orbitals rather than the d subshell.

  • D.\hspace{1em} In the period 6 actinoids, electrons are added to 14 f orbitals rather than the d subshell.

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Question 11

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Atom X is an isotope of an alkali metal. Which of the following is a possible symbol for atom X?

  • A.\hspace{1em}3.1-551a

  • B.\hspace{1em} 3.1-551b

  • C.\hspace{1em}3.1-551c

  • D.\hspace{1em}3.1-551d

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Question 12

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[Maximum mark: 8]

An atomic nucleus of element X is surrounded by electron shells, as shown below:

CH0558

  1. The diagram does not fully describe the electron configuration of the atom or ion or the identity of element X.

    1. State why it is not possible to determine the position of element X in the periodic table from the electron configuration alone. [1]

    2. An alternative method for describing the electron configuration of an atom or ion is to draw the orbitals as boxes and the electrons as arrows. The box-and-arrow diagram for a helium atom is shown below:

      CH0558 Draw a similar diagram for the atom or ion of element X, including labels for the occupied subshells. [3]

    3. Suggest the block of the periodic table in which element X is likely to be found, giving a reason for your answer. [2]

  2. Element X could be found in group 1 of the periodic table.

    1. State the name given to elements in group 1 of the periodic table. [1]
    2. State the most likely period number of element X, assuming that the electron configuration in the diagram is as close as possible to that of the neutral atom. [1]

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Question 13

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The complete electron configuration of a neutral atom is shown below:

3.1-554

In which group and period of the periodic table would this element be found?


Groupperiod
\hspace{1em}A.\hspace{1em}142
\hspace{1em}B.\hspace{1em}143
\hspace{1em}C.\hspace{1em}162
\hspace{1em}D.\hspace{1em}163

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Question 14

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The condensed electron configuration of an element is[Ar] 3d104sX24pX5\ce{[Ar] {3d^{10}}{4s}^2{4p}^5}.

Which statement is correct about this element?


  • A. \hspace{1em} It belongs to group 4

  • B. \hspace{1em} It belongs to group 15

  • C. \hspace{1em} It belongs to period 3

  • D. \hspace{1em} It belongs to period 4

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Question 15

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Which of the following statements regarding the periodic table are correct?

  • I. Anions have larger ionic radii than the atomic radius of their parent atom
    II. Elements in the periodic table are arranged according to their number of protons
    III. Elements within the same period will have similar physical properties
  • A.\hspace{1em}I, II, and III

  • B.\hspace{1em}I and II only

  • C.\hspace{1em}I and III only

  • D.\hspace{1em}II and III only

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Question 16

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[Maxium mark: 9]

The table below contains data for the elements nitrogen, fluorine, sulfur and chlorine in no particular order:

ElementAtomic Radius (1012^{-12} mm)First Ionization Energy (kJ mol1kJ\ mol^{-1})
1711402
21041000
31001251
4601681


  1. Identify element 2 and justify your answer using the atomic radius and the first ionization energy data shown. [3]

    1. Identify the number of valence electrons for element 1 and justify your answer using
      the atomic radius and first ionization energy data shown. [2]

    2. State the electron configuration for the common ion formed from element 1. [1]

    3. Using section 9 (Section 10- 2025 Syllabus) in the data booklet, compare the size of the ionic radius of the common ion formed from element 1 to its atomic radius. Explain this change in size.[2]

  2. An electron affinity for element 1 is not published and the electron affinity for element 4 is -328kJ mol1kJ\ mol^{-1}. In terms of atomic structure, explain why element 1 does not have a value for electron affinity. [1]

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Question 17

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Which of the following does NOT have two valence electrons?


  • A.\hspace{1em}Al+^+

  • B.\hspace{1em}Zn

  • C.\hspace{1em}Ca

  • D.\hspace{1em}Sc3+^{3+}

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Question 18

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How many fully occupied pp orbitals are there in selenium, Se, atom?


  • A. \hspace{1em} 2

  • B. \hspace{1em} 3

  • C. \hspace{1em} 7

  • D. \hspace{1em} 9

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Question 19

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Which gives the correct observation when gaseous chlorine is bubbled through a sodium iodide solution?

  • A. \hspace{1em} Formation of a clear, colorless solution

  • B. \hspace{1em} Formation of a pale green solution

  • C. \hspace{1em} Deposits of a black solid

  • D. \hspace{1em} Formation of a dark red/brown solution

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Question 20

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Which of the following statements regarding the melting points of elements are correct?

  • I.\hspace{1em} Group 17 melting points increase down the group due to increased covalent bond strength
    II.\hspace{0.9em} Lithium has a higher melting point than potassium
    III.\hspace{0.8em} Bromine has a higher melting point than chlorine


  • A.\hspace{1em}I, II, and III

  • B.\hspace{1em}I and II only

  • C.\hspace{1em}II and III only

  • D.\hspace{1em}II only

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Question 21

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[Maximum mark: 8]

  1. Bromine has a relative atomic mass of 79.90 and two common isotopes 79^{79}Br and 81^{81}Br. Calculate the percentage abundance of the 81^{81}Br isotope. [2]

  2. State the equation for the first electron affinity of iodine. [1]

  3. Describe and explain the trend in the magnitude of electron affinity from fluorine to iodine. [3]

  4. Fluorine reacts with sodium iodide. State the net ionic equation for this reaction and name the type of reaction. [2]

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Question 22

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[Maximum mark: 8]

The period 3 elements magnesium, silicon and sulfur are found in the second, fourteenth and sixteenth columns of the periodic table.

  1. State the name given to a column of elements in the periodic table. [1]

  2. State how the numbers of electron shells and outer shell electrons vary across period 3. [2]

  3. Selected physical properties of magnesium, silicon and sulfur are given in the table below:

ElementAppearanceMechanical properties
MagnesiumShiny, greyDuctile
SiliconShiny, greyBrittle
SulfurDull, yellowBrittle

Explain how the positions of the elements across period 3 help to explain their similarities and differences. [3]

  1. Period 3 contains more elements than period 1 but is equal in size to period 2. Suggest why the number of elements increases between periods 1 and 2 but not between periods 2 and 3. [2]

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Question 23

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[Maximum marks: 10]

Magnesium is an element in group 2 of the periodic table.

  1. State the full electron configuration for magnesium and the block it can be found in the periodic table. [2]

  2. Explain how successive ionization energies can prove that magnesium is in group 2 and period 3 of the periodic table. [3]

  3. State the equation for the second ionization energy of magnesium. [1]

  4. State an equation for the reaction between magnesium oxide and water, and comment on the pH of the resultant solution. [2]

  5. By referring to their relative ionization energies, compare the metallic behavior of magnesium to calcium and beryllium (values from the data booklet are not required). [2]

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Question 24

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[Maximum mark: 7]

Phosphorus is an element in group 15 of the periodic table.

  1. State the total number of occupied p orbitals at all levels in an atom of phosphorus. [1]

  2. Phosphorus, PX4\ce{P4}, reacts with oxygen to form phosphorus oxide, PX4OX10\ce{P4O10}, by the following equation, PX4+5OX2PX4OX10\ce{P4 + 5O2 → P4O10}.

    1. Calculate the minimum volume of oxygen gas required to fully react with 16.7gg phosphorus at 273 KK and 100 kPakPa. [2]

    2. 20.4gg of phosphorus oxide was formed during this reaction. Calculate the percentage yield. [2]

  3. Describe the acid-base nature of phosphorus oxide and use an equation to demonstrate this behaviour. [2]

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Question 25

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Which of the following single replacement reactions will NOT occur?

  • A.\hspace{1em}F2(g)_2{_{(g)}}+ 2NaBr(aq){_{(aq)}} → Br2(l)_2{_{(l)}}+ 2NaF(aq){_{(aq)}}

  • B.\hspace{1em}K(s){_{(s)}}+ NaI(aq){_{(aq)}} → Na(s){_{(s)}}+ KI(aq){_{(aq)}}

  • C.\hspace{1em}Rb(s){_{(s)}}+ LiCl(aq){_{(aq)}} → Li(s){_{(s)}}+ RbCl(aq){_{(aq)}}

  • D.\hspace{1em}I2(s)_2{_{(s)}}+ CaBr2(aq)_2{_{(aq)}} → Br2(l)_2{_{(l)}}+ 2CaI2(aq)_2{_{(aq)}}

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Question 26

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Which statement regarding the periodic table is true?

  • A.\hspace{1em}Atomic radius increases across a period

  • B.\hspace{1em}Selenium (Se) has a higher ionization energy than sulfur (S)

  • C.\hspace{1em}Nonmetal oxides produce acidic solutions when dissolved in water

  • D.\hspace{1em}Copper (Cu) is considered to be more metallic than cesium (Cs)

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Question 27

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[Maximum mark: 10]

Lithium metal is known to react vigorously with water.

  1. Write a balanced equation for the reaction that occurs. [1]

  2. State the block of the periodic table where lithium is found. [1]

  3. If the resulting pH of the solution is 13.70, calculate the concentration of the lithium product formed in the reaction in (a). [2]

  4. If the volume of the solution is equal to 1.5 dm31.5\ dm^{3}, calculate the mass of solid Li required to reach a pH of 13.70. [2]

  5. If an equivalent mass of lithium oxide was added to the same volume of water, calculate the new pH of the solution and whether this results in more or less HX+\ce{H+} concentration in solution compared to pH 13.70 for Li in water. [2]

  6. Describe the bonding structure that exists in solid lithium. [1]

  7. Describe the bonding structure that exists in solid lithium oxide. [1]

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Question 28

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[Maximum mark: 10]

Iodine and astatine are both elements in group 17 of the periodic table.

  1. State the name given to the elements in this group. [1]

  2. Explain why the elements in group 17 are described as being in a different block of the periodic table than the elements in group 1, based on the electron configurations of their neutral atoms. [2]

  3. The electron configuration of a neutral iodine atom is indicated by its location in the periodic table.

    1. The electron configuration of a neutral sodium atom can be written in condensed notation as [Ne] 3s1^1. State the electron configuration, in condensed notation, of a neutral iodine atom. [3]
    2. Explain how the electron configuration of the neutral iodine atom is related to the period number and group number for this element. [2]
  4. The following outline of the periodic table shows how elements in groups 13 to 18 can be placed in three categories, x, y and z, based on their physical properties.

3.1-559

\hspace{1em} Suggest why the thermal conductivity of astatine is much greater than that of iodine, based on the locations of these elements in the periodic table. [2]

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Question 29

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Which is in the correct order from smallest to largest radius?

  • A.\hspace{1em}Ca2+^{2+}, Na+^+, Ne, O2^{2-}

  • B.\hspace{1em}O2^{2-}, Ne, Ca2+^{2+}, Na+^+

  • C.\hspace{1em}Ne, Na+^+, O2^{2-}, Ca2+^{2+}

  • D.\hspace{1em}Na+^+, Ne, O2^{2-}, Ca2+^{2+}

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Question 30

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[Maximum mark:6]

The oxides of two period 3 elements, X and Y, react in water according to the equations below.

  • I.\hspace{1em} XO2(s)_2{_{(s)}} + H2_2O(l){_{(l)}} → H2_2XO3(aq)_{3{(aq)}}
  • II.\hspace{1em} YO(s)_{(s)} + H2_2O(l){_{(l)}} → Y(OH)2(aq)_{2{(aq)}}
  1. Identify elements X and Y. Justify your response. [4]

  2. Predict whether element X or Y would have a higher melting point. Justify your prediction. [2]

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Question 31

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Which of the following is the electron configuration of a neutral atom in group 12 and period 6 of the periodic table?

  • A.\hspace{1em} [Xe] 4f14^{14} 6s2^2

  • B.\hspace{1em} [Xe] 4f14^{14} 5d10^{10} 6s2^2

  • C.\hspace{1em} [Rn] 5f14^{14} 7s2^2

  • D.\hspace{1em} [Rn] 5f14^{14} 6d10^{10} 7s2^2

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Question 32

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[Maximum mark: 5]

The successive ionization energies for element X is shown in the table below:

Successive Ionization Energies (kJ mol1kJ\ mol^{-1}):

1st IE2nd IE3rd IE4th IE5th IE6th IE7th IE8th IE
1000225233634556700484962710831724
  1. Write the equation that represents the 2nd ionization energy of element X. [1]

  2. Predict the number of valence electrons for element X and justify your response. [2]

  3. Another element, Y, is found below and in the same group as element X in the periodic table. The electronegativity value of element Y is 2.6. Predict a reasonable value for the electronegativity value of element X. Explain your reasoning.[2]

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Question 33

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[Maximum mark: 10]

The positions of selected elements in the s and d blocks are shown in the periodic table below:

3.1-560

  1. State the electron configuration of a neutral atom of Fe, including orbitals in both the inner and outer shells. [3]

  2. Atoms of Cu and K both contain one electron in the 4s subshell.

    Explain why copper is described as a d block element, whereas potassium is found in the s block. [2]

  3. The elements Ac and Rf are separated by 14 elements in the f block of the periodic table.

    1. State the name given to the elements between Ac and Rf. [1]
    2. Explain why there are 14 elements between Ac and Rf. [2]
  4. Fe and Cu both form atoms or ions with partially filled d subshells.

    1. State the name given to elements of this type. [1]
    2. Suggest why the name stated in (i) can also be applied to some of the 14 elements between Ac and Rf. [1]

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Question 34

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Which statement(s) about the reaction of PX4OX10\ce{P4O10} with water is(are) correct?

  • I. \hspace{1em} The pH of the resulting solution is below 7.00 at 25°25\degree C
  • II. \hspace{.7em} The product formed is HX3POX4\ce{H3PO4}
  • III. \hspace{.4em} PX4OX10\ce{P4O10} is classified as an amphoteric oxide


  • A. \hspace{1em} I only

  • B. \hspace{1em} II only

  • C. \hspace{1em} III only

  • D. \hspace{1em} I and II only

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