Chemistry Chapter 6: The Periodic Table
52 Questions
0 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 statement about ionization energy is true?

  • Ionization energy decreases as you move down a group. (correct)
  • Ionization energy increases as you move down a group.
  • Ionization energy is constant across a period.
  • Ionization energy is the energy required to add an electron.

    • The second ionization energy of an element is always lower than the first ionization energy.

    False

    What is the term used to describe the energy required to remove an electron from a gaseous atom?

    Ionization energy

    As nuclear charge increases, the ionization energy tends to __________.

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

    Which of the following elements has the highest first ionization energy?

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

    Ionization energy generally decreases from left to right across a period.

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

    What happens to ionization energy as more electrons are removed from an atom?

    <p>It increases.</p> Signup and view all the answers

    Who arranged elements according to increasing atomic mass in the mid-1800s?

    <p>Dmitri Mendeleev</p> Signup and view all the answers

    The modern periodic table is arranged according to increasing atomic mass.

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

    What is the Periodic Law?

    <p>When elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties.</p> Signup and view all the answers

    Elements on the periodic table are organized into horizontal rows called ______.

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

    What significant flaw did Mendeleev's periodic table have?

    <p>It had pairs of elements that were incorrectly placed.</p> Signup and view all the answers

    Match the following scientists with their contributions to the periodic table:

    <p>Dmitri Mendeleev = First periodic table based on atomic mass Henry Moseley = Periodic table based on atomic number J.W. Dobereiner = Triads of elements based on similar properties John Dalton = Early theories of atomic structure</p> Signup and view all the answers

    There are ______ periods in the periodic table.

    <p>7</p> Signup and view all the answers

    What are the three broad classes of elements mentioned?

    <p>Metals, nonmetals, and metalloids.</p> Signup and view all the answers

    Which of the following are classes of elements found in the periodic table?

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

    Nonmetals are generally good conductors of electricity.

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

    What is the main characteristic of noble gases in terms of their reactivity?

    <p>They are very stable and rarely react.</p> Signup and view all the answers

    The element _______ is a fuming dark red liquid nonmetal.

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

    Match the following classes of elements with their characteristics:

    <p>Metals = Good electrical conductors Nonmetals = Brittle and poor conductors Metalloids = Intermediate properties Noble Gases = Inert with full electron configurations</p> Signup and view all the answers

    Which groups are classified as representative elements?

    <p>1A to 2A and 3A to 8A</p> Signup and view all the answers

    Metals are typically ductile and malleable.

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

    What is the electron configuration of noble gases?

    <p>The outer s and p sublevels are completely full.</p> Signup and view all the answers

    Which of the following statements about noble gases is true?

    <p>Noble gases have 8 valence electrons.</p> Signup and view all the answers

    Alkali metals have 2 valence electrons.

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

    What is the electron configuration for Argon?

    <p>1s2 2s2 2p6 3s2 3p6</p> Signup and view all the answers

    Atoms form ions to achieve __________ gas configuration.

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

    Match the following blocks with their respective characteristics:

    <p>s-block = Includes alkali and alkaline earth metals p-block = Contains halogens and noble gases d-block = Transition metals that fill d orbitals f-block = Inner transition elements</p> Signup and view all the answers

    Which of the following elements is an alkaline earth metal?

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

    The first d orbital, 3d, fills up in period 3.

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

    Which statement accurately describes alkali metals?

    <p>They lose 1 electron to form positive ions.</p> Signup and view all the answers

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

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

    What are valence electrons?

    <p>Electrons in the outermost energy level.</p> Signup and view all the answers

    What phenomenon occurs when outermost electrons are blocked from the nucleus by inner electron layers?

    <p>Shielding effect</p> Signup and view all the answers

    The atomic radius generally _____ from left to right across a period.

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

    Match the following groups of elements with their tendency regarding electron loss or gain:

    <p>Alkali Metals = Lose 1 electron Alkaline-Earth Metals = Lose 2 electrons Halogens = Gain 1 electron Noble Gases = Do not gain or lose electrons</p> Signup and view all the answers

    Which factor primarily influences periodic trends in atomic radius?

    <p>All of the above</p> Signup and view all the answers

    As you go down a group in the periodic table, atoms generally become smaller.

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

    What happens to the size of atoms as you increase atomic number down a group?

    <p>Atoms get bigger.</p> Signup and view all the answers

    Which element has a greater nuclear charge compared to hydrogen?

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

    Oxygen has a higher first ionization energy than nitrogen.

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

    What is the electronegativity of fluorine?

    <p>4.0</p> Signup and view all the answers

    The first ionization energy of lithium is lower than that of _____.

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

    Match the elements with their corresponding first ionization energy trend:

    <p>Helium = Highest Hydrogen = Lower than He Lithium = Lower than H Beryllium = Higher than Li</p> Signup and view all the answers

    Which element has a lower first ionization energy than beryllium?

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

    Neon has a higher first ionization energy than helium.

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

    What trend occurs in electronegativity on the periodic table?

    <p>Increases from left to right and decreases from top to bottom.</p> Signup and view all the answers

    The measure of how strongly an atom attracts electrons when in a compound is called _____.

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

    Which factor primarily contributes to the increase in ionization energy from lithium to beryllium?

    <p>Greater nuclear charge</p> Signup and view all the answers

    Li has the same shielding effect as Be.

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

    What significantly affects the first ionization energy of sodium compared to lithium?

    <p>Increased shielding and distance from nucleus.</p> Signup and view all the answers

    Fluorine is the most ______________ element.

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

    Study Notes

    Chapter 6: "The Periodic Table"

    • The periodic table organizes elements based on their properties.
    • Initially, only about 13 elements were identified by 1700.
    • Chemists sought a systematic way to organize increasing numbers of discovered elements.
    • Early attempts like Dobereiner's triads grouped elements with similar properties.
    • In the mid-1800s, Dmitri Mendeleev's table organized elements by increasing atomic mass.
    • Mendeleev left spaces for undiscovered elements and predicted their properties accurately.
    • Henry Moseley, in 1913, arranged elements by increasing atomic number, which is the foundation of the modern periodic table.
    • The modern periodic table includes elements' symbols, atomic numbers, and atomic masses.

    Section 6.1: Organizing the Elements

    • Objectives included explaining how elements are organized in a periodic table, comparing early and modern periodic tables, and identifying three broad classes of elements.
    • Chemists used the properties of elements to group them.
    • Elements like gold and copper have been known for thousands of years, while most others were discovered later.

    Section 6.2: Classifying the Elements

    • Objectives included describing information in a periodic table, classifying elements based on electron configuration, distinguishing representative and transition metals.
    • The periodic table organizes elements according to their electron configurations.
    • Objectives included describing trends in atomic size, explaining how ions form, and describing periodic trends for first ionization energy, ionic size, and electronegativity.
    • Atomic size trends are affected by energy levels, nuclear charge, and shielding.
    • Ionization energy is the energy to remove an electron from a gaseous atom.
    • Trends in ionization energy are influenced by nuclear charge, shielding, and distance from the nucleus.
    • Electronegativity is the measure of how strongly an atom attracts electrons in a compound.
    • Electronegativity generally increases across a period from left to right but is lower for metals, who donate electrons, in comparison to nonmetals who prefer to accept electrons and in metals.

    Studying That Suits You

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

    Quiz Team

    Related Documents

    Hon Ch 6 Periodic Table 2020 PDF

    Description

    Explore the fascinating history and organization of the periodic table in this quiz. Learn how early chemists like Mendeleev and Moseley laid the groundwork for the modern classification of elements. Test your understanding of the principles behind the periodic table and the properties of elements.

    More Like This

    Chemical Elements Organization Quiz
    3 questions

    Chemical Elements Organization Quiz

    Periodic Table Organization
    10 questions

    Periodic Table Organization

    MagnificentWildflowerMeadow avatar
    MagnificentWildflowerMeadow
    Chemistry Chapter 5: The Periodic Table
    29 questions

    Chemistry Chapter 5: The Periodic Table

    WellBacklitJasmine avatar
    WellBacklitJasmine
    Periodic Table Overview and History
    37 questions

    Periodic Table Overview and History

    CelebratedAlpenhorn avatar
    CelebratedAlpenhorn
    Use Quizgecko on...
    Browser
    Open
    Browser
    Browser