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Topic 4: Inorganic Chemistry and the Periodic Table
4.1 Group 2: The Alkaline Earth Metals
4.1.1 Physical Properties
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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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