Alkaline Earth Metals Quiz
9 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

What is the common characteristic that distinguishes alkaline earth metals from other elements?

  • They are highly reactive with water.
  • They are produced by mixing metals and oxides.
  • They are found in minerals called alkaline earths.
  • They have two valence electrons in their outermost shell. (correct)

    • Which of the following elements exhibits a diagonal relationship with beryllium?

  • Sodium (Na)
  • Magnesium (Mg)
  • Aluminium (Al) (correct)
  • Lithium (Li)

    • What is the primary reason for the oxides of alkaline earth metals being referred to as 'alkaline earths'?

  • They are found in abundance in the earth's crust.
  • They react with water to form alkaline solutions. (correct)
  • They are obtained from ores that are alkaline in nature.
  • They are the most stable oxides in the respective period.

    • In which group of the periodic table are alkaline earth metals located?

    <p>Group 2 (B)</p> Signup and view all the answers

    Which of the following statements is TRUE about radium?

    <p>It is a highly reactive element. (A), It is rarely found in nature. (B)</p> Signup and view all the answers

    Which of the following elements has an electronic configuration different from the other alkaline earth metals?

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

    What is the general electronic configuration of the alkaline earth metals in their valence shell?

    <p>ns² (B)</p> Signup and view all the answers

    Which of these elements has the electronic configuration [Kr]5s²?

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

    Why are elements like Beryllium, Magnesium, Calcium, Strontium, Barium, and Radium grouped together in the periodic table?

    <p>They have similar chemical properties due to the same valence electron configuration (A)</p> Signup and view all the answers

    Flashcards

    Group IIA Elements

    Elements with same electronic configuration, ns².

    Electronic Configuration of Group IIA

    The valence electron configuration is ns², where n is the period number.

    Beryllium's Properties

    Beryllium shows abnormal properties due to its unique configuration.

    S-block Elements

    Elements where the last electron enters the ns orbital.

    Signup and view all the flashcards

    Gradation of Properties

    Gradual change in properties as atomic number increases.

    Signup and view all the flashcards

    Alkaline Earth Metals

    Group IIA metals, including Be, Mg, Ca, Sr, Ba, Ra, known for their basic oxides.

    Signup and view all the flashcards

    Beryllium

    The first element of the alkaline earth metals, less active, resembling aluminum.

    Signup and view all the flashcards

    Radium

    The last alkaline earth metal, known for its radioactive properties.

    Signup and view all the flashcards

    Diagonal Relationship

    Beryllium's similarity in behavior with Aluminum due to their position in the periodic table.

    Signup and view all the flashcards

    Alkaline Earth Group

    The group of six elements in Group IIA that follow alkali metals in the periodic table.

    Signup and view all the flashcards

    Study Notes

    Alkaline Earth Metals and Their Compounds

    • Alkaline earth metals are in Group IIA or 2 of the periodic table
    • These include beryllium, magnesium, calcium, strontium, barium, and radium
    • They're called alkaline earth metals because their oxides are basic (alkaline) and were found in the earth's crust (earths)
    • Calcium, strontium, and barium oxides were known before the metals themselves
    • The metals, when discovered, were also referred to as alkaline earths
    • The elements are found in various minerals, with Be3Al2(SiO3)6 being an example for beryllium

    Position in Periodic Table

    • Group IIA elements are in the periodic table
    • Examples include beryllium, magnesium, calcium, strontium, barium, and radium

    Electronic Configuration

    • Valence electron configuration is ns² (period n)
    • Examples include Be (1s² 2s²), Mg (1s² 2s² 2p⁶ 3s²), Ca (1s² 2s² 2p⁶ 3s² 3p⁶ 4s²)
    • The valence shell is ns²
    • The penultimate shell has 8 electrons, except for beryllium (2 electrons in its outer shell)
    • Beryllium has an abnormal electronic configuration

    Physical Properties

    • All are silvery-white metals
    • They are soft, but harder than alkali metals due to stronger metallic bonding
    • Hardness decreases as atomic number increases
    • Atomic and ionic radii progressively increase down the group
    • Density increases gradually from Be to Ca, then increases slightly up to Ra due to differences in crystal structures
    • Melting and boiling points are higher than corresponding alkali metals
    • First and second ionization energies decrease down the group
    • Electropositive character increases progressively from Be to Ba
    • Electronegativity is low and decreases as the atomic number increases
    • Good conductors of heat and electricity due to presence of two loosely bound valence electrons
    • Flame coloration depends on the element. E.g., calcium gives brick-red coloration, strontium crimson, barium green
    • Reducing nature increases as the atomic number increases

    Studying That Suits You

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

    Quiz Team

    Related Documents

    Inorganic Chemistry II Past Lecture Notes PDF

    Description

    Test your knowledge on alkaline earth metals, their properties, and electronic configurations. This quiz covers elements in Group IIA including beryllium, magnesium, calcium, and more. Explore the significance and applications of these essential elements in chemistry.

    More Like This

    Use Quizgecko on...
    Browser
    Open
    Browser
    Browser