Effective Nuclear Charge & Periodic Trends
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Elements Y and X are compared. Element Y has a larger radius than Element X. Based on this, you could say:

  • Element Y is further to the left side of the periodic table.
  • Elements Y and X are probably in the same group.
  • A and B are correct. (correct)
  • Element X is closer to the top of the periodic table.

    • Atomic radius generally increases as elements move:

  • down a group and from left to right across a period
  • down a group and from right to left across a period (correct)
  • up a group and from right to left across a period
  • up a group and from left to right across a period

    • The atomic radius of main-group elements generally increases down a group because the:

  • effective nuclear charge decreases down a group
  • effective nuclear charge increases down a group
  • effective nuclear charge zigzags down a group
  • the principal quantum number of the valence orbitals increases (correct)

    • Which one of the following atoms has the largest radius?

    <p>S</p> Signup and view all the answers

    Which one of the following atoms has the largest radius?

    <p>Rb</p> Signup and view all the answers

    Which one of the following atoms has the smallest radius?

    <p>Cl</p> Signup and view all the answers

    Which one of the following atoms has the largest radius?

    <p>Ba</p> Signup and view all the answers

    Which one of the following elements has the largest atomic radius?

    <p>Se</p> Signup and view all the answers

    Which one of the following elements has the largest atomic radius?

    <p>Al</p> Signup and view all the answers

    In which of the following atoms is the 2s orbital closest to the nucleus?

    <p>Cl</p> Signup and view all the answers

    Which of the following correctly lists the five atoms in order of increasing size (smallest to largest)?

    <p>F &lt; K &lt; Ge &lt; Br &lt; Rb</p> Signup and view all the answers

    In which of the following atoms is the 3s orbital closest to the nucleus?

    <p>Cl</p> Signup and view all the answers

    Which of the following correctly lists the five atoms in order of increasing size (smallest to largest)?

    <p>O &lt; F &lt; S &lt; Mg &lt; Ba</p> Signup and view all the answers

    The ability of an atom in a molecule to attract electrons is best quantified by the atom's:

    <p>electronegativity</p> Signup and view all the answers

    Electronegativity ______ from left to right within a period and ______ from top to bottom within a group.

    <p>increases, decreases</p> Signup and view all the answers

    Of the atoms below, ______ is the most electronegative.

    <p>F</p> Signup and view all the answers

    Of the atoms below, ______ is the most electronegative.

    <p>Cl</p> Signup and view all the answers

    Of the atoms below, ______ is the least electronegative.

    <p>Rb</p> Signup and view all the answers

    Which of the elements below has the largest electronegativity?

    <p>S</p> Signup and view all the answers

    In general, as you go across a period in the periodic table from left to right: the atomic radius ______; the electronegativity ______; and the first ionization energy ______.

    <p>decreases, increases, increases</p> Signup and view all the answers

    The first ionization energies of the elements ______ as you go from left to right across a period of the periodic table, and ______ as you go from the bottom to the top of a group in the table.

    <p>increase, decrease</p> Signup and view all the answers

    Of the choices below, which gives the order for first ionization energies?

    <p>Cl &gt; S &gt; Al &gt; Si &gt; Ar</p> Signup and view all the answers

    Of the following atoms, which has the largest first ionization energy?

    <p>O</p> Signup and view all the answers

    Of the following elements, which has the largest first ionization energy?

    <p>Cl</p> Signup and view all the answers

    Of the following elements, which has the largest first ionization energy?

    <p>Ca</p> Signup and view all the answers

    Of the following elements, which has the largest first ionization energy?

    <p>Se</p> Signup and view all the answers

    Of the following elements, which has the largest first ionization energy?

    <p>N</p> Signup and view all the answers

    Of the elements below, ______ has the largest first ionization energy.

    <p>H</p> Signup and view all the answers

    ______ have the lowest first ionization energies of the groups listed.

    <p>Alkali metals</p> Signup and view all the answers

    Which equation correctly represents the first ionization of aluminum?

    <p>Al(g) → Al+(g) + e-</p> Signup and view all the answers

    Which of the following correctly represents the second ionization of aluminum?

    <p>Al+(g) → Al^2+(g) + e-</p> Signup and view all the answers

    Which equation correctly represents the first ionization of phosphorus?

    <p>P(g) → P+(g) + e¯</p> Signup and view all the answers

    Which of the following correctly represents the second ionization of phosphorus?

    <p>P+(g) + e¯ → P^2+(g)</p> Signup and view all the answers

    Which equation correctly represents the first ionization of barium?

    <p>Ba(g) → Ba+(g) + e¯</p> Signup and view all the answers

    Which of the following correctly represents the second ionization of calcium?

    <p>Ca⁺(g) → Ca^2+(g) + e-</p> Signup and view all the answers

    Of the elements below, ______ is the most metallic.

    <p>K</p> Signup and view all the answers

    The list that correctly indicates the order of metallic character is ______.

    <p>P &gt; S &gt; Se</p> Signup and view all the answers

    Between which two elements is the difference in metallic character the greatest?

    <p>Rb and O</p> Signup and view all the answers

    What is the effective nuclear charge on a valence electron in Se?

    <p>16</p> Signup and view all the answers

    What is the effective nuclear charge on a valence electron in Cs?

    <p>1</p> Signup and view all the answers

    What is the effective nuclear charge on a valence electron in B?

    <p>3</p> Signup and view all the answers

    What is the effective nuclear charge on a valence electron in Pb?

    <p>28</p> Signup and view all the answers

    A valence electron in which of the following elements has the highest effective nuclear charge?

    <p>F</p> Signup and view all the answers

    A valence electron in which of the following elements has the highest effective nuclear charge?

    <p>Cl</p> Signup and view all the answers

    Study Notes

    Effective Nuclear Charge & Periodic Trends

    • Element Radius & Periodic Table Position: If element Y has a larger radius than element X, Y is likely further left on the periodic table and X closer to the top. Elements Y and X might be in the same group.

    • Atomic Radius Trends: Atomic radius generally increases going down a group and from right to left across a period.

    • Main-Group Atomic Radius Increase: The atomic radius of main-group elements increases down a group because the principal quantum number of the valence orbitals increases.

    • Multiple Choice Questions (Examples): Elements with larger atomic radii are found further left and/or toward the bottom of the periodic table. The 2s orbital is found closer to the nucleus in lighter elements.

    • Electronegativity Trends: Electronegativity increases from left to right across a period and from bottom to top of a group.

    • Electronegativity Examples: Fluorine (F) is the most electronegative element. Rubidium (Rb) is a less electronegative element than Chlorine (Cl).

    • Ionization Energy Trends: Ionization energy generally increases from left to right across a period and from bottom to top of a group.

    • Ionization Energy Examples: Elements with higher ionization energies are more difficult to remove electrons from. Elements further right in a period, have higher ionization energies.

    • Factors Affecting Effective Nuclear Charge: Effective nuclear charge increases going across a period from left to right, while it is fairly constant down within a group.

    • Effective Nuclear Charge Examples: The effective nuclear charge of an element is the positive charge of the nucleus that an electron feels. Specific examples of effective nuclear charges are stated with the elements in other questions. For example, an element like Lead (Pb) has a higher effective nuclear charge from left to right in the periodic table.

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    Effective Nuclear Charge & Periodic Trends PDF

    Description

    Explore the concepts of effective nuclear charge and periodic trends in this quiz. Assess your understanding of atomic radius variations, electronegativity, and their influences on elemental properties across the periodic table.

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