Chemistry Periodic Table Development
13 Questions
6 Views

Choose a study mode

Play Quiz
Study Flashcards
Spaced Repetition
Chat to Lesson

Podcast

Play an AI-generated podcast conversation about this lesson

Questions and Answers

Which of the following correctly describes the trend of atomic radius across a period?

  • The atomic radius generally increases due to decreasing nuclear charge.
  • The atomic radius fluctuates without a clear pattern due to variations in electron configuration.
  • The atomic radius generally decreases due to an increase in nuclear charge. (correct)
  • The atomic radius remains constant because of consistent electron shielding.

    • What is the primary factor that causes the increase in atomic radius as you move down a group?

  • Decrease in the effective nuclear charge, allowing the atoms to expand
  • Addition of new electron shells, significantly increasing the volume (correct)
  • Increased nuclear charge pulling electrons outwards
  • Gain of protons in the nucleus causing expansion

    • How does ionization energy generally change across a period, and what is the main cause for this change?

  • It fluctuates unpredictably because of electron interactions.
  • It increases because of the increased nuclear charge, making it more difficult to remove electrons. (correct)
  • It remains constant as electron shielding balances nuclear charge.
  • It decreases due to smaller nuclear charge attracting electrons more weakly.

    • Which statement accurately describes how electronegativity changes as you move down a group?

    <p>Electronegativity decreases as electrons are further from the nucleus. (A)</p> Signup and view all the answers

    What is the main principle underlying the octet rule and what is an exception to this rule?

    <p>Atoms gain, lose, or share electrons to achieve 8 valence electrons, with first period elements being an exception. (B)</p> Signup and view all the answers

    Who arranged the elements in order of increasing atomic mass and also predicted the existence of undiscovered elements?

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

    According to the periodic law, which of the following determines the periodic repetition of chemical and physical properties of elements?

    <p>Increasing atomic number (B)</p> Signup and view all the answers

    Which term describes the vertical columns in the periodic table?

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

    Which of the following groups of elements are known for being highly reactive?

    <p>Alkaline metals and halogens (D)</p> Signup and view all the answers

    Which category of elements typically have properties of both metals and nonmetals?

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

    Which of the following is a characteristic of nonmetals?

    <p>Generally gases or brittle solids (C)</p> Signup and view all the answers

    Which group of elements is known for being extremely unreactive?

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

    Which block of elements contains only partially or completely filled s orbitals?

    <p>s block elements (A)</p> Signup and view all the answers

    Flashcards

    Periodic Law

    The periodic repetition of chemical and physical properties of elements when arranged by increasing atomic number.

    Antoine Lavoisier

    Compiled a list of the first known elements.

    John Newlands

    Arranged elements by increasing atomic mass and created the law of octaves.

    Dimitri Mendeleev

    Arranged elements by atomic mass and predicted undiscovered elements' properties.

    Signup and view all the flashcards

    Henry Moseley

    Discovered atomic number, arranging elements by it for periodic patterns.

    Signup and view all the flashcards

    Metalloids

    Elements with properties of both metals and nonmetals.

    Signup and view all the flashcards

    Alkaline Metals

    Group 1 elements, highly reactive except hydrogen.

    Signup and view all the flashcards

    Noble Gases

    Group 18 elements, extremely unreactive and useful in applications.

    Signup and view all the flashcards

    p block elements

    Elements in the periodic table with partially or completely filled p orbitals.

    Signup and view all the flashcards

    Ionic radius trend

    Ionic radius decreases across a period for cations and anions; increases down a group.

    Signup and view all the flashcards

    Ionization energy trend

    Ionization energy increases across a period and decreases down a group.

    Signup and view all the flashcards

    Electronegativity trend

    Electronegativity increases across a period and decreases down a group.

    Signup and view all the flashcards

    Octet rule

    Atoms gain, lose or share electrons to achieve a full set of 8 valence electrons, except first-period elements.

    Signup and view all the flashcards

    Study Notes

    Scientists and Periodic Table Development

    • Antoine Lavoisier: Compiled a list of early known elements.
    • John Newlands: Arranged elements by increasing atomic mass, noticing a pattern every eighth element (law of octaves).
    • Dimitri Mendeleev: Showed a link between atomic mass and element properties, arranged elements by increasing atomic mass, and predicted undiscovered elements.
    • Henry Moseley: Discovered atomic number (unique number of protons), arranged elements by increasing atomic number creating a periodic pattern of properties.
    • Periodic Law: States that elements' chemical and physical properties repeat periodically when arranged by increasing atomic number.

    Modern Periodic Table Structure

    • Groups: Vertical columns in the periodic table.
    • Periods: Horizontal rows in the periodic table.
    • Representative Elements: Groups 1, 2, and 13-18.
    • Transition Elements: Groups 3-12.
    • Metal Classification:
      • Metals: Shiny, solid at room temperature, good conductors of heat and electricity.
      • Alkaline Metals (Group 1): Most reactive elements (excluding hydrogen).
      • Alkaline Earth Metals (Group 2): Highly reactive.
      • Transition Metals (Groups 3-12): Wide range of properties.
      • Inner Transition Metals: Divided into Lanthanides and Actinides.
        • Lanthanides: F block elements following Lanthanum.
        • Actinides: F block elements following Actinium.
      • Metalloids: Exhibit properties of metals and nonmetals.
    • Nonmetals: Generally gases or brittle solids, poor conductors of heat and electricity. Bromine is the only liquid nonmetal.
    • Halogens (Group 17): Highly reactive elements often in compounds.
    • Noble Gases (Group 18): Unreactive, used in applications requiring inertness such as lasers, light bulbs, and neon signs.

    Valence Electrons and Electron Configurations

    • Valence Electrons: Electrons in the outermost energy level (determine chemical properties).
    • Period: Horizontal rows in the periodic table.
    • Representative Elements: Groups 1, 2, and 13-18 (s and p block elements).
    • s Block Elements: Groups 1, 2, and Helium (partially or completely filled s orbitals).
    • p Block Elements: Groups 13-18 (partially or completely filled p orbitals).
    • d Block Elements: Groups 3-12 (partially filled d orbitals).
    • f Block Elements: Inner transition elements (partially filled 4f or 5f orbitals).
    • Atomic Radius:
      • Period Trend: Decreases across a period due to increasing nuclear charge.
      • Group Trend: Increases down a group due to added electron shells.
    • Ionic Radius:
      • Period Trend: Decreases across a period for cations, also for anions.
      • Group Trend: Increases down a group due to added electron shells.
    • Ionization Energy:
      • Period Trend: Increases across a period due to increasing nuclear charge.
      • Group Trend: Decreases down a group due to increasing distance from the nucleus.
    • Electronegativity:
      • Period Trend: Increases across a period due to increasing nuclear charge.
      • Group Trend: Decreases down a group due to increasing distance from the nucleus.
    • Octet Rule: Atoms tend to gain, lose, or share electrons to achieve 8 valence electrons (except for the first period with a duet).

    Studying That Suits You

    Use AI to generate personalized quizzes and flashcards to suit your learning preferences.

    Quiz Team

    Description

    Test your knowledge on the historical development of the periodic table and the significant contributions made by key scientists. Explore how the arrangement of elements has evolved from Antoine Lavoisier to Henry Moseley. Understand the structure of the modern periodic table including groups and periods.

    More Like This

    Periodic Classification of Elements
    8 questions

    Periodic Classification of Elements

    ThrillingEquation avatar
    ThrillingEquation
    Periodic Table and Element Classification
    16 questions

    Periodic Table and Element Classification

    InfallibleStar avatar
    InfallibleStar
    Periodic Table Flashcards
    46 questions

    Periodic Table Flashcards

    GlisteningRadon avatar
    GlisteningRadon
    Chemistry Chapter 4 Flashcards
    10 questions

    Chemistry Chapter 4 Flashcards

    DetachableHydra avatar
    DetachableHydra
    Use Quizgecko on...
    Browser
    Open
    Browser
    Browser