Chemistry: Electron Configurations and Lewis Structures
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Questions and Answers

Which type of elements typically have electron configurations ending with 5, 6, or 7 electrons?

  • Noble gases
  • Nonmetals (correct)
  • Metals
  • Transition metals

    • Noble gases have electron configurations ending with 7 electrons.

    False

    Name one metal found in the periodic table.

    Lithium

    The electron configuration of helium ends with _____ electrons.

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

    Match the following elements with their classification:

    <p>Lithium = Metal Chlorine = Nonmetal Neon = Noble gas Calcium = Metal</p> Signup and view all the answers

    What do elements in the same group have in common?

    <p>They have the same number of electrons in their outermost shell.</p> Signup and view all the answers

    All elements in the same period have the same number of valence electrons.

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

    What is the electron configuration of sulfur (S)?

    <p>1s² 2s² 2p⁶ 3s² 3p⁴</p> Signup and view all the answers

    The element _____ is in the same period as chlorine (Cl).

    <p>Aluminum (Al)</p> Signup and view all the answers

    Match the following elements with their number of valence electrons:

    <p>Oxygen (O) = 6 Sulfur (S) = 6 Sodium (Na) = 1 Chlorine (Cl) = 7</p> Signup and view all the answers

    How many unpaired electrons are present in the Lewis structure of sulfur?

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

    The valency of sulfur is represented as trivalent.

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

    What is the electron configuration of sulfur?

    <p>2, 8, 6</p> Signup and view all the answers

    The number of valence electrons for elements in group 5A equals _______.

    <p>8 - number of last energy level electrons</p> Signup and view all the answers

    Match the following elements to their corresponding valencies:

    <p>Li = Monovalent Be = Divalent C = Tetravalent F = Monovalent</p> Signup and view all the answers

    Which group does oxygen belong to based on its Lewis structure?

    <p>6A</p> Signup and view all the answers

    Noble gases have a valency of 2.

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

    What is the significance of pairing dots in the Lewis dot structure?

    <p>Pairing dots represents the presence of paired electrons until all valence electrons are distributed.</p> Signup and view all the answers

    What is the atomic number of element (X), which is located in period 2 and group 7A?

    <p>9</p> Signup and view all the answers

    The atomic number of element (Y) located in period 3 and group 0 is 18.

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

    If an element has an electron configuration of 2, 7, what is its group number?

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

    The total number of electrons in element (Y) is _____ across its energy levels.

    <p>18</p> Signup and view all the answers

    Match the following elements with their corresponding atomic numbers:

    <p>Element (X) = 9 Element (Y) = 18 Element (Z) = unknown Sulfur (S) = 16</p> Signup and view all the answers

    What is the group number of Magnesium (Mg) in the periodic table?

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

    Helium (He) has an electron configuration that ends with 8 electrons.

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

    What is the electron configuration of Neon (Ne)?

    <p>2, 8</p> Signup and view all the answers

    The group number of Argon (Ar) is _____.

    <p>0</p> Signup and view all the answers

    Match the following elements with their corresponding valency:

    <p>H = Monovalent Mg = Divalent O = Divalent Ne = 0</p> Signup and view all the answers

    How many occupied energy levels does Sodium (Na) have?

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

    The elements Lithium (Li), Sodium (Na), and Potassium (K) are all found in group 0.

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

    The Lewis structure of Oxygen (O) is represented as _____ .

    <p>:Ö:</p> Signup and view all the answers

    Which element is represented as a liquid at room temperature?

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

    The chemical activity of alkali metals decreases as the atomic number increases.

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

    What are the physical states of elements X and Y at room temperature if element X's melting point is lower and boiling point is higher than room temperature, and both properties of element Y are lower than room temperature?

    <p>Element X is a liquid; Element Y is a gas.</p> Signup and view all the answers

    Cesium is the most active metal, while ______ is the most active nonmetal.

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

    Match the following elements with their classification based on their chemical activity:

    <p>Lithium = Alkali Metal Barium = Alkaline Earth Metal Chlorine = Halogen Oxygen = Nonmetal</p> Signup and view all the answers

    Which of the following elements has an atomic number of 14?

    <p>Element Z</p> Signup and view all the answers

    The melting points of alkali metals increase as their atomic number increases.

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

    How many energy levels does Element Z have?

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

    Chlorine is a _____ at room temperature.

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

    Match the following elements with their melting point states at room temperature:

    <p>Lithium = Solid Bromine = Liquid Chlorine = Gas Iodine = Solid</p> Signup and view all the answers

    Which of the following statements regarding the atomic radii trend is correct?

    <p>Atomic radii increase down a group.</p> Signup and view all the answers

    Element X and Element Z both have 4 electrons in their outermost energy level.

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

    What is the physical state of potassium (K) at room temperature?

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

    Study Notes

    Electron Configuration and the Periodic Table

    • Metals: Typically have electron configurations ending with 1, 2, or 3 electrons in their outermost shell
    • Nonmetals: Typically have electron configurations ending with 5, 6, or 7 electrons in their outermost shell
    • Noble gases: Have electron configurations ending with 8 electrons in their outermost shell (except for Helium, which has 2)
    • Elements in the same group (vertical column) have the same number of electrons in their outermost energy level
    • Elements in the same period (horizontal row) have the same number of energy levels occupied by electrons

    Lewis Dot Structures

    • Lewis dot structures represent the number of valence electrons (electrons in the outermost energy level) around an element's symbol
    • Valence electrons are represented by dots distributed individually, then paired, on the four sides of the element's symbol
    • The number of unpaired electrons in a Lewis dot structure determines the valency (combining capacity) of an element

    Group A Elements in the Periodic Table

    • To determine the position of a Group A element based on atomic number:
      • Write the electron configuration
      • Determine the period number (number of occupied energy levels)
      • Determine the group number (number of electrons in the last energy level)

    Atomic Number and Properties

    • Atomic Radii: Increase as atomic number increases within a group (down a column)
    • Melting/Boiling Points (Alkali Metals): Decrease as atomic number increases within a group (down a column)
    • Melting/Boiling Points (Halogens): Increase as atomic number increases within a group (down a column)

    Physical State at Room Temperature

    • Solid: Melting point and boiling point are both higher than room temperature (25°C)
    • Liquid: Melting point is lower than room temperature, but boiling point is higher
    • Gas: Both melting point and boiling point are lower than room temperature

    Chemical Activity

    • Alkali and Alkaline Earth Metals: Chemical activity increases as atomic number increases (down the group)
    • Halogens: Chemical activity decreases as atomic number increases (down the group)

    Key Examples

    • Alkali Metals: Lithium (Li), Sodium (Na), Potassium (K)
    • Halogens: Chlorine (Cl), Bromine (Br), Iodine (I)
    • Noble Gases: Helium (He), Neon (Ne), Argon (Ar)

    Important Notes

    • Helium (He) is the only noble gas with an electron configuration ending with 2 electrons, not 8
    • Inert gases are found in Group 0 (also known as Group 8A) of the periodic table
    • Scientists cannot discover a new element between existing elements because atomic numbers are integers and increase by one

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    Description

    This quiz covers essential concepts of electron configurations in metals, nonmetals, and noble gases, as well as the use of Lewis dot structures for representing valence electrons. Understand how these concepts relate to the periodic table and the structure of atoms. Test your knowledge of the periodic trends and electron distribution.

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