Honors Unit 3: The Electron and Periodic Table
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Questions and Answers

Which of the following properties is not characteristic of metals?

  • Luster (shiny)
  • Good conductors of heat and electricity
  • Brittle and shatter when hit (correct)
  • Malleable and ductile

    • What type of elements can both gain and lose electrons to form ions?

  • Metals (correct)
  • Metalloids
  • Nonmetals
  • All of the above

    • Which sample is most likely to be a nonmetal based on its conductivity?

  • Sample B - Light bulb does not light (correct)
  • Sample B - Malleable
  • Sample A - Light bulb lights
  • Sample C - Light bulb lights

    • In terms of physical properties, which statement is true about metalloids?

    <p>Exhibit properties of both metals and nonmetals</p> Signup and view all the answers

    What procedure would you use to test for malleability of a sample?

    <p>Touch the sample to see if it bends</p> Signup and view all the answers

    What is a unique property of nonmetals compared to metals?

    <p>They usually exist as gases</p> Signup and view all the answers

    Which of the following statements describes metals in terms of electron behavior?

    <p>They lose electrons to form cations</p> Signup and view all the answers

    Which statement most accurately describes the appearance of metals?

    <p>They have high luster and are generally shiny</p> Signup and view all the answers

    What is the noble gas that comes before Aluminum (Al)?

    <p>Neon (Ne)</p> Signup and view all the answers

    What is the correct shorthand electron configuration for Strontium (Sr)?

    <p>[Kr] 5s2</p> Signup and view all the answers

    Determine the correct noble gas configuration for tellurium (Te).

    <p>[Kr] 5s2 4d10 5p4</p> Signup and view all the answers

    What should the sum of the superscripts equal to for an element with atomic number 20?

    <p>20</p> Signup and view all the answers

    Which atom among the following has the greatest shielding effect?

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

    What is the electron configuration for Zinc (Zn)?

    <p>[Ar] 4s2 3d10</p> Signup and view all the answers

    What is the effective nuclear charge (Z_eff) for Al?

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

    If the size of an atom increases, which statement is true about its ionization energy?

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

    Which noble gas is used in the configuration of Arsenic (As)?

    <p>Argon (Ar)</p> Signup and view all the answers

    Which atom will have a stronger hold on its electrons?

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

    Identify the electron orbital notation for Gallium (Ga).

    <p>[Ar] 4s23d104p1</p> Signup and view all the answers

    What is the noble gas configuration for Mercury (Hg)?

    <p>[Xe] 6s2 4f14 5d10</p> Signup and view all the answers

    In the alkali metal group, which of the following statements is true regarding atomic radius?

    <p>Atomic radius increases down the group.</p> Signup and view all the answers

    Which of the following correctly describes electronegativity trends across a period?

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

    If an atom has greater electron affinity, what can be inferred about its behavior?

    <p>It adds electrons easily.</p> Signup and view all the answers

    What would be expected if the atomic radius decreases?

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

    What is the electron configuration for Sodium?

    <p>1s22s22p63s1</p> Signup and view all the answers

    Which rule states that no two electrons will have the same spin?

    <p>Pauli’s Exclusion Principle</p> Signup and view all the answers

    What is the valence shell for Bromine?

    <p>4</p> Signup and view all the answers

    Which group of elements in the periodic table is characterized as reactive nonmetals?

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

    What is the noble gas configuration for Oxygen?

    <p>[He] 2s22p4</p> Signup and view all the answers

    What does the Aufbau Principle state regarding electron configurations?

    <p>Electrons should always fill the lowest energy orbitals first.</p> Signup and view all the answers

    Which of the following best describes alkali metals?

    <p>Reactive, soft metallic solids that are lustrous</p> Signup and view all the answers

    Why does strontium have a larger atomic radius compared to magnesium?

    <p>More electron shells</p> Signup and view all the answers

    How many valence electrons does Calcium (atomic # 20) have?

    <p>2</p> Signup and view all the answers

    Which of the following describes the characteristics of nonmetals?

    <p>Solids, liquids, and gases that are brittle</p> Signup and view all the answers

    Which rule explains that no two electrons in the same orbital can have the same spin?

    <p>Pauli Exclusion Principle</p> Signup and view all the answers

    What is the correct electron configuration for Arsenic (atomic # 33)?

    <p>1s22s22p63s23p64s23d104p3</p> Signup and view all the answers

    What is the significance of having 8 valence electrons in an atom?

    <p>It signifies a stable electron configuration.</p> Signup and view all the answers

    According to Hund's Rule, what must occur within a set of orbitals?

    <p>Each orbital must contain one electron before pairing begins.</p> Signup and view all the answers

    How many total electrons does Magnesium (Mg) have based on its configuration 1s22s22p63s2?

    <p>12</p> Signup and view all the answers

    In noble gas notation, which noble gas is used as the starting point for Argon (atomic # 18)?

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

    What is the valence shell for Boron (atomic # 5)?

    <p>2</p> Signup and view all the answers

    Why does calcium have a larger atomic radius than bromine?

    <p>Bromine's nuclear attraction pulls electrons in closer, making it smaller.</p> Signup and view all the answers

    What explains the larger size of the sulfide anion compared to the sulfur atom?

    <p>The sulfide anion has gained electrons, leading to increased electron-electron repulsions.</p> Signup and view all the answers

    Why is the potassium cation smaller than the potassium atom?

    <p>Potassium cation has lost an electron and one energy level.</p> Signup and view all the answers

    What trend does ionization energy follow in the periodic table?

    <p>Ionization energy generally increases across a period from left to right.</p> Signup and view all the answers

    Why does strontium have a smaller ionization energy compared to magnesium?

    <p>Strontium has more energy levels, making it easier to remove an electron.</p> Signup and view all the answers

    What contributes to bromine having a larger ionization energy than calcium?

    <p>Bromine has a stronger nuclear charge and is smaller.</p> Signup and view all the answers

    Which element in Group IIIA (3A) has the largest atomic radius?

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

    Which scientist is credited with arranging elements by atomic number?

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

    Study Notes

    Honors Unit 3: The Electron and Periodic Table

    • The periodic table displays elements arranged by atomic number.
    • Elements with similar properties are grouped together.
    • Rows on the table are called periods.
    • Columns on the table are called families or groups.
    • Atomic Models evolved over time with discoveries like the electron and nucleus.
    • Dalton's model, Thomson's model, Rutherford's model, Bohr Model, and the Quantum Mechanical model each expanded on previous understanding.
    • Atoms contain a nucleus with protons and neutrons, and electrons orbit the nucleus.
    • Electrons can gain or lose energy levels.
    • Light has wave properties, including amplitude and frequency, and wavelength.
    • Frequency and wavelength are inversely proportional. A shorter wavelength implies a higher frequency.
    • Elements emit light of specific wavelengths when heated. This is due to electrons switching energy levels.
    • The atomic emission spectrum is unique to each element.
    • Atomic orbitals are regions of space where electrons are likely found.
    • Orbitals have different shapes and orientations (s, p, d, f). Different orbitals hold various numbers of electrons.
    • Electron configuration describes the arrangement of electrons in orbitals within an atom.
    • Electron configuration follows the Aufbau Principle (filling lowest energy orbitals first), Hund's Rule (one electron in each orbital before doubling up), and Pauli Exclusion Principle (no two electrons have the same four quantum numbers).
    • Each electron can be represented by a coefficient (energy level), letter (orbital), and superscript (number of electrons).
    • Noble Gas notation is a shorthand representation of electron configuration.
    • Periods represent energy levels and groups represent valence electron similarities.
    • Periodic trends relate to properties like atomic radius, ionization energy, electronegativity, and electron affinity across the periodic table and within groups. These trends can be explained by changes in nuclear charge and shielding. An increase in nuclear charge results in a stronger attraction between the nucleus and electrons in an atom. Effective nuclear charge also affects the size of atoms.
    • Cations are positively charged ions (loss of electrons) while anions are negatively charged ions (gaining of electrons).
    • The size of ions differs from the size of parent atoms, depending on the gain or loss of electrons.

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    Honors Unit 3: The Electron and Periodic Table Packet PDF

    Description

    This quiz covers the fundamental concepts of the electron, atomic models, and the organization of the periodic table. Explore how atomic theory evolved through various models, the arrangement of elements by atomic number, and the properties of light associated with atomic emission. Test your understanding of these key principles in chemistry.

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