3.1.2 Group properties

• What are group properties in the periodic table?

  Trends and similarities
• What happens to the atomic radius as you move down a group in the periodic table?

  Increases
• Ionization energy decreases as you move down a group in the periodic table.
• The addition of more electron shells causes electronegativity to decrease down a group.


  True
• Why does the atomic radius increase down a group in the periodic table?

  Addition of electron shells
• Trends in group properties as you move down a group in the periodic table:

  1️⃣ Atomic radius increases

  2️⃣ Electronegativity decreases

  3️⃣ Ionization energy decreases

  4️⃣ Reactivity increases
• As you move down a group, the electronegativity decreases
• As you move down a group, the valence electrons become easier to lose
• The alkali metals (Group 1) exhibit consistent trends in their properties as you move down the group.


  True
• Alkali metals are more reactive than the corresponding Group 2 elements.
• Alkali metals have weaker metallic bonding, resulting in lower melting and boiling points compared to Group 2 metals.

  True
• Halogens exist as diatomic molecules with strong covalent bonds.
• Group properties are observed in the chemical and physical properties of elements within the same vertical column of the periodic table.

  True
• Group properties refer to the trends and similarities observed in the chemical and physical properties of elements within the same group
• Electronegativity increases as you move down a group in the periodic table.

  False
• What happens to the reactivity of elements as you move down a group in the periodic table?

  Increases
• The increase in reactivity down a group is due to the easier loss of valence electrons.
• Why are alkaline earth metals less reactive than alkali metals?

  Two valence electrons
• The atomic radius increases as you move down a group due to the addition of more electron shells.


  True
• The key group properties include atomic radius, electronegativity, ionization energy, and reactivity.


  True
• The atomic radius of alkali metals is larger than the corresponding Group 2 elements.

  True
• Trends in melting and boiling points of alkali metals as you move down the group:

  1️⃣ Melting points decrease

  2️⃣ Boiling points decrease
• The alkaline earth metals are less reactive than the alkali metals due to having two valence electrons.


  True
• Trends in halogen properties as you move down the group:

  1️⃣ Atomic radius increases

  2️⃣ Electronegativity decreases

  3️⃣ Ionization energy decreases

  4️⃣ Reactivity decreases
• Noble gases have a full valence shell, making them extremely stable and unreactive.

  True
• As you move across a period, the atomic radius decreases due to a stronger nuclear charge.


  True
• Trends in group properties across periods:

  1️⃣ Atomic radius decreases

  2️⃣ Electronegativity increases

  3️⃣ Ionization energy increases

  4️⃣ Reactivity decreases
• Halogens become less reactive down the group due to increasing atomic size and weaker nuclear attraction.


  True
• The reactivity of noble gases decreases down the group.
• Across a period, the ionization energy increases due to a stronger nuclear charge.
• Match the group comparison with the correct property:

  Group 1 vs. Group 2 ↔️ Group 1 has lower ionization energy

  Group 7 vs. Group 0 ↔️ Group 7 requires one electron