Periodic Trends and Bonding Concepts
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Questions and Answers

What type of bond typically forms between a metal and a nonmetal?

  • Ionic bond (correct)
  • Nonpolar covalent bond
  • Covalent bond
  • Polar covalent bond

    • Which describes a nonpolar covalent bond?

  • ΔEN is greater than 1.7
  • ΔEN is less than or equal to 0.5 (correct)
  • Formed between metals and nonmetals
  • Electrons are shared unequally

    • How is the name of an ionic compound typically structured?

  • Anion first, then cation
  • Cation with a suffix, anion without
  • Cation and anion both with -ide suffix
  • Cation first followed by an anion with an -ide suffix (correct)

    • What determines the geometry of a molecule according to VSEPR theory?

    <p>The number of electron pairs around the central atom (A)</p> Signup and view all the answers

    In which scenario would a polar covalent bond likely form?

    <p>Moderate difference in electronegativity between 0.5 and 1.7 (B)</p> Signup and view all the answers

    What is the typical bond angle in a linear molecular geometry?

    <p>180° (A)</p> Signup and view all the answers

    How do you determine the oxidation state in naming transition metals in ionic compounds?

    <p>Specify the oxidation state using Roman numerals (C)</p> Signup and view all the answers

    What kind of elements compose covalent compounds?

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

    Which statement accurately describes electronegativity trends in the periodic table?

    <p>Electronegativity increases across a period. (A)</p> Signup and view all the answers

    What charge balance is required for an ionic compound to be neutral?

    <p>Total positive charge must be equal to the total negative charge. (B)</p> Signup and view all the answers

    Which type of bond is likely to form if the difference in electronegativity between two atoms is 0.3?

    <p>Nonpolar covalent bond (B)</p> Signup and view all the answers

    When naming a covalent compound, which prefix would be used for two atoms of the same element?

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

    In VSEPR theory, what is the bond angle in a bent molecular geometry with two bonding pairs and one lone pair?

    <p>Less than 120° (C)</p> Signup and view all the answers

    What is the expected bond character when the difference in electronegativity between two atoms is greater than 1.7?

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

    Which step is NOT part of determining molecular geometry using VSEPR theory?

    <p>Identify the atomic number of the central atom. (D)</p> Signup and view all the answers

    Which of the following correctly describes how to name the compound FeCl₂?

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

    What happens to electronegativity as you move from left to right across a period in the periodic table?

    <p>It increases due to increased nuclear charge. (A)</p> Signup and view all the answers

    Which type of bond typically forms when the difference in electronegativity is between 0.5 and 1.7?

    <p>Polar covalent bond (C)</p> Signup and view all the answers

    In the naming of ionic compounds, which suffix is used for the anion?

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

    How are covalent compounds named when there are two atoms of the same element present?

    <p>Omit the prefix for the first element only. (A)</p> Signup and view all the answers

    What is the bond angle in a linear molecular geometry according to VSEPR theory?

    <p>180° (C)</p> Signup and view all the answers

    Which of the following terms refers to the ability of an atom to attract electrons in a bond?

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

    When determining molecular geometry, what is the first step in the VSEPR theory process?

    <p>Draw the Lewis structure. (A)</p> Signup and view all the answers

    What is the relationship between the number of lone pairs and the geometry of a molecule?

    <p>Lone pairs can alter the bond angles and molecular shape. (C)</p> Signup and view all the answers

    Flashcards

    Electronegativity

    An atom's ability to attract electrons in a bond.

    Ionic Bond

    Bond formed between atoms with a large electronegativity difference.

    Covalent Bond

    Bond formed between atoms with a smaller electronegativity difference.

    VSEPR Theory

    Electron pairs repel to maximize distance, influencing molecular shape.

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    Ionic Compound Naming

    Name cation (metal) first, then anion (nonmetal) with -ide; transition metals use Roman numerals.

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    Covalent Compound Naming

    Use prefixes (mono-, di-, tri-) to show number of atoms; omit mono- for first element.

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    Polar Covalent Bond

    Unequal sharing of electrons in a covalent bond.

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    Nonpolar Covalent Bond

    Equal sharing of electrons in a covalent bond.

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    Electronegativity Trend Across a Period

    Electronegativity increases as you move from left to right across a period in the periodic table.

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    Electronegativity Trend Down a Group

    Electronegativity decreases as you move down a group in the periodic table.

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    Ionic Bond Formation

    Forms between atoms with a large electronegativity difference (ΔEN > 1.7), typically between metals and nonmetals.

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    Covalent Bond Formation

    Forms between atoms with a smaller electronegativity difference (ΔEN ≤ 1.7), typically between nonmetals.

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    What determines bond type?

    The difference in electronegativity (ΔEN) between two atoms predicts the type of bond they form. A large ΔEN (>1.7) indicates an ionic bond, while a smaller ΔEN (≤1.7) suggests a covalent bond.

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    VSEPR Theory: What affects molecular shape?

    The VSEPR Theory states that electron pairs around a central atom will arrange themselves as far apart as possible to minimize repulsion. This arrangement determines the molecule's geometry.

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    Linear Geometry

    A molecular shape with two electron regions, resulting in a 180° bond angle.

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    Bent Geometry

    A molecular shape with two bonding pairs and 1-2 lone pairs, resulting in a bond angle less than 180°.

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    Study Notes

    • Electronegativity increases across periods and decreases down groups.
    • Electronegativity is an atom's ability to attract electrons in a bond.
    • Higher nuclear charge leads to higher electronegativity across periods.
    • Added electron shells cause lower electronegativity down groups.
    • Ionic bonds form when the difference in electronegativity (ΔEN) is greater than 1.7, typically between metals and nonmetals.
    • Covalent bonds form when ΔEN is less than or equal to 1.7, typically between nonmetals.
    • Polar covalent bonds occur with moderate ΔEN (0.5 < ΔEN ≤ 1.7) where electrons are shared unequally.
    • Nonpolar covalent bonds occur with small ΔEN (ΔEN ≤ 0.5) where electrons are shared equally.

    Naming and Writing Formulas for Ionic and Covalent Compounds

    • Ionic compounds consist of a metal cation and a nonmetal anion.
    • Name the cation followed by the anion (e.g., NaCl = sodium chloride).
    • Transition metal ions require specification of their oxidation state using Roman numerals (e.g., FeCl₂ = iron(II) chloride).
    • Balance ionic charges to create a neutral compound (e.g., Al³⁺ and Cl⁻ → AlCl₃).
    • Covalent compounds consist of two or more nonmetals.
    • Use prefixes to denote the number of each atom: mono-, di-, tri-, etc. Omit "mono-" for the first element. (e.g., CO₂ = carbon dioxide, N₂O₄ = dinitrogen tetroxide).
    • Formulas for covalent compounds are determined according to the prefixes.

    VSEPR Theory and Molecular Geometry

    • VSEPR (Valence Shell Electron Pair Repulsion) theory explains molecular shapes.
    • Electron pairs (bonding & lone pairs) repel each other to maximize distance.
    • VSEPR shapes are used to classify molecular geometry.
    • Linear geometry has 2 regions of electron density and a 180° bond angle (e.g., CO₂).
    • Bent geometry has two bonding pairs and 1-2 lone pairs with bond angles determined accordingly by the number of lone pairs.

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    Description

    Explore the fascinating world of periodic trends and how they influence bond prediction. This quiz covers the concepts of electronegativity, types of chemical bonds, and the naming and writing of formulas for ionic and covalent compounds. Test your understanding of these essential chemistry topics!

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