Cards (83)

    • Where are alkaline earth metals located in the periodic table?
      Group 2
    • Alkaline earth metals are generally less reactive than alkali metals but more reactive than most other metals
    • Alkaline earth metals form stable cations with a +2 oxidation state.
    • What is the general electronic configuration of alkaline earth metals?
      [noble gas] ns^2
    • The electronic configuration of Magnesium (Mg) is [Ne] 3s^2
    • The electronic configuration of Calcium (Ca) is [Ar] 4s^2.
    • Match the alkaline earth metal with its electronic configuration:
      Magnesium ↔️ [Ne] 3s^2
      Calcium ↔️ [Ar] 4s^2
      Strontium ↔️ [Kr] 5s^2
      Barium ↔️ [Xe] 6s^2
    • What oxidation state do alkaline earth metals achieve when they lose two electrons?
      +2
    • Alkaline earth metals achieve a stable noble gas configuration by losing two electrons
    • Alkaline earth metals lose two electrons to achieve a stable noble gas configuration, resulting in a +2
    • What is the general electronic configuration of alkaline earth metals in Group 2?
      [Noble gas] ns^2
    • Match the alkaline earth metal with its electronic configuration:
      Magnesium (Mg) ↔️ [Ne] 3s^2
      Calcium (Ca) ↔️ [Ar] 4s^2
      Strontium (Sr) ↔️ [Kr] 5s^2
      Barium (Ba) ↔️ [Xe] 6s^2
    • The atomic radius of alkaline earth metals increases down the group due to greater electron shielding
    • Ionization energy of alkaline earth metals decreases as one descends Group 2.
    • Order the following alkaline earth metals based on increasing atomic radius:
      1️⃣ Magnesium (Mg)
      2️⃣ Calcium (Ca)
      3️⃣ Strontium (Sr)
      4️⃣ Barium (Ba)
    • Why does the melting point of alkaline earth metals decrease down the group?
      Weakening metallic bonding
    • The density of alkaline earth metals increases down the group because mass increases faster than volume
    • The melting points and boiling points of alkaline earth metals decrease down the group due to larger atomic radii and lower effective nuclear charges.
    • Where are alkaline earth metals located in the periodic table?
      Group 2
    • When alkaline earth metals form ions, they become +2 ions, which are smaller than their neutral atoms.
    • What is the atomic radius of calcium (Ca) in picometers?
      197 pm
    • Ionization energy decreases down Group 2 due to increasing atomic radius
    • Increased electron shielding makes it easier to remove outer electrons from alkaline earth metals as one descends the group.
    • What is the oxidation state of alkaline earth metals in their compounds?
      +2
    • For alkaline earth metals, the atomic radii increase down the group due to the addition of electron shells
    • Atomic radii increase down Group 2 due to increased electron shielding against the nuclear charge.
    • When alkaline earth metals form ions, they become +2
    • The ionic radii of alkaline earth metals are smaller than their atomic radii.
    • Match the element with its atomic radius:
      Magnesium (Mg) ↔️ 160 pm
      Calcium (Ca) ↔️ 197 pm
      Strontium (Sr) ↔️ 215 pm
      Barium (Ba) ↔️ 222 pm
    • Order the alkaline earth metals from smallest to largest atomic radius:
      1️⃣ Magnesium (Mg)
      2️⃣ Calcium (Ca)
      3️⃣ Strontium (Sr)
      4️⃣ Barium (Ba)
    • The first ionization energy of alkaline earth metals decreases as you move down the group
    • Ionization energy is the energy required to remove an electron from an atom in the gaseous phase.
    • Why does the ionization energy decrease down Group 2?
      Increasing atomic radius
    • Increased electron shielding reduces the nuclear attraction, making it easier to remove electrons.
    • Match the element with its first ionization energy:
      Beryllium (Be) ↔️ 899 kJ/mol
      Magnesium (Mg) ↔️ 738 kJ/mol
      Calcium (Ca) ↔️ 590 kJ/mol
      Strontium (Sr) ↔️ 549 kJ/mol
    • Order the alkaline earth metals from highest to lowest first ionization energy:
      1️⃣ Beryllium (Be)
      2️⃣ Magnesium (Mg)
      3️⃣ Calcium (Ca)
      4️⃣ Strontium (Sr)
      5️⃣ Barium (Ba)
    • The density of alkaline earth metals increases down Group 2.
    • Why does density increase down Group 2?
      Atomic mass increases more
    • The electrical conductivity of alkaline earth metals decreases down the group due to increasing atomic radius
    • The strength of metallic bonding in alkaline earth metals decreases down Group 2.
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