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Difficulty: MediumAtomic Structure and Periodic Table

Elements in the periodic table are organized into families based on recurring valence electron configurations and characteristic chemical properties. Match each periodic table group on the left with its defining valence configuration and reactivity property on the right.

  • Alkali metals (Group 1)Contain 11 valence electron, act as highly reactive metals, and readily lose 11 electron to form +1+1 cations.
  • Alkaline earth metals (Group 2)Contain 22 valence electrons, act as reactive metals, and readily lose 22 electrons to form +2+2 cations.
  • Halogens (Group 17)Contain 77 valence electrons, act as highly reactive nonmetals, and readily gain 11 electron to form −1-1 anions.
  • Noble gases (Group 18)Contain a complete outer electron shell, exhibit high stability, and are chemically inert under normal conditions.

Answer

Alkali metals (Group 1) match with having 11 valence electron and forming +1+1 cations; Alkaline earth metals (Group 2) match with having 22 valence electrons and forming +2+2 cations; Halogens (Group 17) match with having 77 valence electrons and forming −1-1 anions; Noble gases (Group 18) match with having a complete outer electron shell and being chemically inert.
Each chemical family's behavior is dictated by its valence electron configuration: Group 1 has 11 valence electron forming +1+1 ions; Group 2 has 22 valence electrons forming +2+2 ions; Group 17 has 77 valence electrons gaining 11 electron to form −1-1 ions; Group 18 has complete outer shells resulting in chemical inertness.

Step-by-Step Solution

1
Identify the valence electron count and typical ion formation for Group 1 (Alkali metals).
Group 1 elements have 11 valence electron and lose it easily to form +1+1 cations.
Losing 11 electron gives alkali metals the stable electron configuration of the preceding noble gas.
2
Identify the valence electron count and typical ion formation for Group 2 (Alkaline earth metals).
Group 2 elements have 22 valence electrons and lose them to form +2+2 cations.
Losing both valence electrons achieves a stable outer octet.
3
Identify the valence electron count and typical ion formation for Group 17 (Halogens).
Group 17 elements have 77 valence electrons and gain 11 electron to form −1-1 anions.
Nonmetals with 77 valence electrons require only 11 additional electron to reach a full octet.
4
Identify the outer shell characteristics and reactivity of Group 18 (Noble gases).
Group 18 elements have completely filled valence shells and are non-reactive (inert).
A filled outer shell provides maximum thermodynamic stability without sharing, gaining, or losing electrons.

Key Concept

Periodic table groups reflect valence electron numbers that determine characteristic chemical properties and predictable ion formation.
Estimated Time:1m 0s
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Topics

Atomic Structure and Periodic Table

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