Chapter 5 - Periodic Table

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Chapter 5 - Periodic Table - Quiz

The periodic table can be used to predict properties of elements, even those that are yet to be discovered. By studying it you get to understand some trends in a group of elements and how chemical reactions may occur. Below is a quiz to test you on Chapter 5 which covered the organization, properties, and discovery of the periodic table.


Questions and Answers
  • 1. 

    The shorthand electron configuration [Ar] 4s2 4d1 is that of the element scandium.

    • A.

      True

    • B.

      False

    Correct Answer
    B. False
    Explanation
    It should be [Ar] 4s2 3d1 because when you move from the s to d sublevel you drop one main energy level.

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  • 2. 

    A division of the periodic table is labeled with the number 14. This section can be called a family.

    • A.

      True

    • B.

      False

    Correct Answer
    A. True
    Explanation
    The division of the periodic table labeled with the number 14 refers to the group 14 elements, which include carbon, silicon, germanium, tin, and lead. These elements have similar chemical properties and are often referred to as a family or group. Therefore, the statement that this section can be called a family is true.

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  • 3. 

    The lanthanides and actinides are in group 3 of the periodic table.

    • A.

      True

    • B.

      False

    Correct Answer
    B. False
    Explanation
    The statement is false because the lanthanides and actinides are not in group 3 of the periodic table. They are actually located in the f-block, which is below the main body of the periodic table. The f-block consists of two series of elements, the lanthanide series and the actinide series, which are placed separately at the bottom of the periodic table.

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  • 4. 

    The noble gases are located in the d block of elements.

    • A.

      True

    • B.

      False

    Correct Answer
    B. False
    Explanation
    The noble gases are actually located in the p block of elements, specifically in group 18 of the periodic table. The d block of elements is known as the transition metals. Therefore, the statement that the noble gases are located in the d block of elements is incorrect.

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  • 5. 

    Newlands left spaces in his periodic table and predicted the properties of the elements that belonged there.

    • A.

      True

    • B.

      False

    Correct Answer
    B. False
    Explanation
    Newlands did not leave spaces in his periodic table and predict the properties of the elements that belonged there. This statement is false.

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  • 6. 

    Doberiner's quartets stated that elements 2 and 3 have properties halfway between elements 1 and 4.

    • A.

      True

    • B.

      False

    Correct Answer
    B. False
    Explanation
    Doberiner's quartets did not state that elements 2 and 3 have properties halfway between elements 1 and 4. Instead, it proposed that elements 1 and 4 have similar properties, while elements 2 and 3 have properties that are different from both 1 and 4. This concept was later refined and expanded upon by Mendeleev in the development of the periodic table.

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  • 7. 

    Germanium has a higher metallic character then sodium.

    • A.

      True

    • B.

      False

    Correct Answer
    B. False
    Explanation
    Germanium does not have a higher metallic character than sodium. Metallic character refers to the ability of an element to exhibit metallic properties such as being malleable, ductile, and having a high electrical conductivity. Sodium is a highly reactive metal with a low melting point and is commonly found in its metallic form. Germanium, on the other hand, is a metalloid that exhibits both metallic and non-metallic properties. While it can conduct electricity, it is brittle and has a higher melting point compared to sodium. Therefore, the statement is false.

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  • 8. 

    The most common ion for the element Aluminum (Al) has a larger ionic radii than the most common ion for the element bromide.

    • A.

      True

    • B.

      False

    Correct Answer
    B. False
    Explanation
    The statement is false because the most common ion for aluminum (Al) has a smaller ionic radii than the most common ion for bromide. Aluminum typically forms a +3 ion (Al3+), which has a smaller ionic radius compared to the bromide ion (Br-).

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  • 9. 

    Atomic radii is measured in the unit am.

    • A.

      True

    • B.

      False

    Correct Answer
    B. False
    Explanation
    Atomic radii is not measured in the unit "am". The correct unit for measuring atomic radii is picometers (pm). The term "am" is not a recognized unit for measuring atomic radii.

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  • 10. 

    Period 6 elements have a lower ionization energy than period 2 elements.

    • A.

      True

    • B.

      False

    Correct Answer
    A. True
    Explanation
    Period 6 elements have a lower ionization energy than period 2 elements because as you move down a periodic table, the atomic radius increases. This means that the outermost electrons in period 6 elements are further away from the nucleus and experience less attraction, making it easier to remove them. In contrast, period 2 elements have smaller atomic radii, resulting in stronger attraction between the nucleus and outermost electrons, requiring more energy to remove them. Therefore, period 6 elements have lower ionization energies compared to period 2 elements.

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  • 11. 

    What is another name for a period?

    • A.

      Series

    • B.

      Series

    • C.

      SERIES

    Correct Answer(s)
    A. Series
    B. Series
    C. SERIES
    Explanation
    The correct answer for the question is "series" or "Series" or "SERIES". The question is asking for another name for a period, which refers to a sequence or set of events or actions that occur in a particular order. Therefore, "series" is an appropriate term to describe a period.

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  • 12. 

    How many groups make up the s block of elements?

    • A.

      2

    • B.

      Two

    • C.

      Two

    • D.

      TWO

    Correct Answer(s)
    A. 2
    B. Two
    C. Two
    D. TWO
    Explanation
    The s block of elements consists of two groups.

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  • 13. 

    What is the main thing Mendeleev knowingly based the order of his periodic table on, causing him to order it like no one else had done before?

    • A.

      Atomic number

    • B.

      Chemical properties

    • C.

      Physical properties

    • D.

      Atomic mass

    Correct Answer
    B. Chemical properties
    Explanation
    Mendeleev knowingly based the order of his periodic table on chemical properties. He arranged the elements according to their similar chemical properties, which allowed him to group elements with similar behaviors together. This arrangement was unique and different from any previous attempts at organizing the elements. Mendeleev's periodic table became the foundation for the modern periodic table we use today.

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  • 14. 

    What did Mosley use to determine the atomic number of the elements?

    • A.

      An electron microscope

    • B.

      An electron balance

    • C.

      A compilation of data from other scientists

    • D.

      X-Rays

    Correct Answer
    D. X-Rays
    Explanation
    Mosley used X-Rays to determine the atomic number of the elements. X-rays have the ability to penetrate materials and interact with the electrons in an atom. By studying the X-ray spectra produced by different elements, Mosley was able to identify patterns and correlations between the spectra and the atomic number. This led to the discovery of the relationship between the atomic number and the number of protons in the nucleus, which is now known as the basis of the modern periodic table.

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  • 15. 

    Which scientist discovered the group 18 elements, the noble gases?

    • A.

      Ramsey

    • B.

      Mayer

    • C.

      Mendeleev

    • D.

      Newlands

    Correct Answer
    A. Ramsey
    Explanation
    Ramsey is the correct answer because he was the scientist who discovered the group 18 elements, also known as the noble gases.

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  • 16. 

    The element with the configuration [Ar] 4s2 3d10 4p1 is located in which period and group?

    • A.

      Period 6 No Group

    • B.

      Period 4 Group 13

    • C.

      Period 2 Group 2

    • D.

      No period Group 14

    Correct Answer
    B. Period 4 Group 13
    Explanation
    The element with the electron configuration [Ar] 4s2 3d10 4p1 belongs to period 4 because the highest energy level (valence shell) is the fourth energy level. It belongs to group 13 because it has one valence electron in the p orbital, which corresponds to group 13 on the periodic table.

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  • 17. 

    What can be defined as "The energy change that occurs when an atom gains an electron to form an ion?"

    • A.

      Ionization energy

    • B.

      Ionic radii

    • C.

      Electron affinity

    • D.

      Metallic character

    Correct Answer
    C. Electron affinity
    Explanation
    Electron affinity refers to the energy change that occurs when an atom gains an electron to form an ion. It quantifies the attraction between an atom and an additional electron. When an atom gains an electron, energy is released, resulting in a negative electron affinity value. This process is important in understanding the reactivity and chemical behavior of elements, as it helps determine the likelihood of an atom gaining an electron to form an ion.

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  • 18. 

    Which of the following is true about atomic radii?

    • A.

      It increase from left to right across a period

    • B.

      It increases as you go down a group

    • C.

      It is one-fourth the distance between the nuclei of identical bonded atoms

    • D.

      It decrease from left to right across a period

    Correct Answer
    B. It increases as you go down a group
    Explanation
    The atomic radii refers to the size of an atom. As you move down a group in the periodic table, the number of energy levels or shells increases. This results in an increase in atomic size because there are more electrons and a greater distance between the nucleus and the outermost energy level. Therefore, the statement "It increases as you go down a group" is true.

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  • 19. 

    The elements in which block(s) are known as the main group elements?

    • A.

      D and f

    • B.

      S and d

    • C.

      P and s

    • D.

      D only

    Correct Answer
    C. P and s
    Explanation
    The main group elements in the periodic table are located in the s and p blocks. These blocks consist of the elements in the first two columns (Group 1 and 2) and the last six columns (Group 13 to 18). The s block contains elements with their outermost electron in the s orbital, while the p block contains elements with their outermost electron in the p orbital. Therefore, the correct answer is p and s.

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  • Current Version
  • Mar 21, 2022
    Quiz Edited by
    ProProfs Editorial Team
  • Feb 12, 2008
    Quiz Created by
    Gagedy
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