Periodic Trends and Reactivity Quiz
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Questions and Answers

What trend does electron gain enthalpy generally follow across a period?

  • It becomes less negative.
  • It becomes more positive.
  • It becomes more negative. (correct)
  • It stays constant.

    • Which element is expected to have the most negative electron gain enthalpy?

  • Oxygen
  • Fluorine
  • Phosphorus
  • Chlorine (correct)

    • How does electron gain enthalpy change within a group as atomic size increases?

  • It becomes more positive.
  • It becomes more negative.
  • It remains the same.
  • It becomes less negative. (correct)

    • Why is the electron gain enthalpy of oxygen and fluorine less negative than that of the succeeding elements?

    <p>Added electrons experience significant repulsion. (C)</p> Signup and view all the answers

    Which quantum level is more affected by electron-electron repulsion when adding an electron?

    <p>n = 2 (D)</p> Signup and view all the answers

    What is the IUPAC name for the element with atomic number 120?

    <p>Unbinilium (A)</p> Signup and view all the answers

    What does electronegativity refer to in a chemical compound?

    <p>The ability to attract shared electrons. (B)</p> Signup and view all the answers

    Which orbital begins to fill in the third period?

    <p>3s (C)</p> Signup and view all the answers

    Which of the following scales is used to measure electronegativity?

    <p>Pauling scale (B)</p> Signup and view all the answers

    How does the effective nuclear charge affect the ease of adding an electron?

    <p>It increases the nuclear attraction. (B)</p> Signup and view all the answers

    How many elements are there in the second period?

    <p>8 elements (B)</p> Signup and view all the answers

    What is the electronic configuration of beryllium?

    <p>1s2 2s2 (B)</p> Signup and view all the answers

    Which element's atomic number is represented by 'n = 2' in the second period?

    <p>Lithium (B)</p> Signup and view all the answers

    What do the roots 'un', 'bi', and 'nil' represent in naming elements?

    <p>One, two, and zero (A)</p> Signup and view all the answers

    When does the filling of the 4s orbital begin?

    <p>After 3p (A)</p> Signup and view all the answers

    How many elements are in the third period?

    <p>8 elements (B)</p> Signup and view all the answers

    What does the valence of an element represent?

    <p>The number of electrons in the outermost orbitals (D)</p> Signup and view all the answers

    What is the valence of aluminium when it forms compounds?

    <p>3 (B)</p> Signup and view all the answers

    What is the oxidation state often used to describe?

    <p>The charge of an element in a compound (C)</p> Signup and view all the answers

    In the compound Na2O, what is the valence of sodium?

    <p>1 (A)</p> Signup and view all the answers

    What is the formula for the oxide formed by aluminium?

    <p>Al2O3 (D)</p> Signup and view all the answers

    What periodic trend is associated with the valence of non-metals?

    <p>Decreasing valence across a period (D)</p> Signup and view all the answers

    What is the valence of sulphur in compounds?

    <p>2 (B)</p> Signup and view all the answers

    Which of the following compounds has a formula that reflects the valence of phosphorus?

    <p>PH3 (C)</p> Signup and view all the answers

    What is the oxidation state of aluminum in [AlCl(H2O)5]?

    <p>+3 (C)</p> Signup and view all the answers

    Which element is likely to form the most basic oxide?

    <p>Na (D)</p> Signup and view all the answers

    Which of the following oxides is considered acidic?

    <p>Cl2O7 (A)</p> Signup and view all the answers

    What is the covalency of aluminum in [AlCl(H2O)5] according to the content?

    <p>6 (D)</p> Signup and view all the answers

    How does non-metallic character change across a period?

    <p>Increases from left to right (A)</p> Signup and view all the answers

    Which of the following statements about p-block elements is accurate?

    <p>The first member is more likely to form pπ – pπ bonds than subsequent members. (C)</p> Signup and view all the answers

    What type of oxides do elements in the center of a period typically form?

    <p>Amphoteric or neutral (A)</p> Signup and view all the answers

    Which of the following reactions best illustrates the chemical reactivity of an element?

    <p>Reaction with oxygen (B)</p> Signup and view all the answers

    Which element is likely to be the least reactive based on its ionization enthalpy values?

    <p>Element III (A)</p> Signup and view all the answers

    Which element is likely the most reactive metal?

    <p>Element II (A)</p> Signup and view all the answers

    Which element is expected to be the most reactive non-metal based on its electron gain enthalpy?

    <p>Element III (A)</p> Signup and view all the answers

    Which of the following elements would likely be categorized as the least reactive non-metal?

    <p>Element I (A)</p> Signup and view all the answers

    Which element is likely to form a stable binary halide of the formula MX2 where X is a halogen?

    <p>Element IV (A)</p> Signup and view all the answers

    Which metal can predominantly form a stable covalent halide in the form of MX?

    <p>Element II (C)</p> Signup and view all the answers

    In the modern periodic table, what does the period number indicate?

    <p>The number of shells occupied by electrons (B)</p> Signup and view all the answers

    Which statement regarding the modern periodic table is incorrect?

    <p>p-block corresponds to the azimuthal quantum number of 1. (C)</p> Signup and view all the answers

    Study Notes

    • The periodic table is a systematic way to organize the elements based on their properties
    • Elements in the same group (column) share similar chemical properties
    • As you go down a group, atomic radius increases due to the addition of electron shells
    • As you move across a period (row), atomic radius decreases due to increasing nuclear charge

    Ionization Enthalpy

    • Ionization enthalpy is the energy required to remove an electron from a gaseous atom in its ground state
    • It increases as you move across a period due to increased nuclear charge and smaller atomic radius
    • It decreases as you move down a group due to increased atomic radius and less attraction between the nucleus and outermost electron

    Electron Gain Enthalpy

    • Electron gain enthalpy is the energy change when an electron is added to a gaseous atom in its ground state
    • It generally becomes more negative moving across a period due to increased effective nuclear charge
    • It generally becomes less negative moving down a group due to increased size of the atom and reduced attraction between the nucleus and incoming electron
    • There are exceptions: oxygen and fluorine have less negative electron gain enthalpy than the succeeding elements due to electron-electron repulsion

    Electronegativity

    • Electronegativity is the ability of an atom in a compound to attract shared electrons to itself
    • Electronegativity increases across a period due to increased nuclear charge and smaller atomic radius
    • Electronegativity decreases down a group due to larger atomic radius and weaker attraction between the nucleus and electrons
    • The valence of an element is the number of electrons used in bonding
    • Valence is usually related to the number of electrons in the outermost shells
    • The oxidation state is a more modern term for valence

    Variable Valence

    • Many elements exhibit variable valence depending on the nature of the compound they are in

    Metallic and Non-Metallic Character

    • Metallic character increases as you move down a group
    • Metallic character decreases as you move across a period
    • Non-metallic character increases as you move across a period
    • Non-metallic character decreases as you move down a group

    Reactivity of Elements with oxygen

    • Elements on the extremes of a period readily react with oxygen
    • Elements on the left side of the periodic table form basic oxides
    • Elements on the right side of the periodic table form acidic oxides
    • Elements in the middle tend to form amphoteric or neutral oxides

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    Description

    Test your understanding of periodic trends and chemical reactivity in this quiz. Explore concepts such as atomic radius, ionization enthalpy, and electron gain enthalpy. Challenge yourself to accurately answer questions based on the organization of elements in the periodic table.

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