Elements in the periodic table are organized into families based on their shared subatomic… — Armed Services Vocational Aptitude Battery (ASVAB)

Elements in the periodic table are organized into families based on their shared subatomic properties, valence electron arrangements, and chemical reactivity. Match each chemical family on the left with its defining valence electron configuration and ionization behavior on the right.

Alkali Metals (Group 1)Possess a single valence electron ( $ns^1$ ) that is readily lost to achieve a stable noble-gas core, forming $+1$ cations.
Alkaline Earth Metals (Group 2)Possess two valence electrons ( $ns^2$ ) in their outermost energy level that are lost in chemical reactions to form $+2$ cations.
Halogens (Group 17)Contain seven valence electrons ( $ns^2 np^5$ ) with high electron affinity, readily gaining one electron to form $-1$ anions.
Noble Gases (Group 18)Have a stable, completely filled valence shell octet ( $ns^2 np^6$ ) with exceptionally high ionization energy and negligible chemical reactivity.

Answer

Alkali Metals pair with the single valence electron (

ns^1

) forming

+1

cations; Alkaline Earth Metals pair with two valence electrons (

ns^2

) forming

+2

cations; Halogens pair with seven valence electrons (

ns^2 np^5

) forming

-1

anions; Noble Gases pair with the filled valence octet (

ns^2 np^6

) displaying high ionization energy and chemical inertness.

Each periodic family possesses a distinct valence electron configuration that dictates its chemical reactivity and ionic charges. Group 1 alkali metals possess one outer

s

electron which they lose to form

+1

cations. Group 2 alkaline earth metals possess two outer

s

electrons and form

+2

cations. Group 17 halogens possess seven valence electrons and gain one electron to form

-1

anions. Group 18 noble gases have full outer electron shells, rendering them inert with exceptionally high ionization energies.

Step-by-Step Solution

Analyze the valence configuration and ion formation of Group 1 (Alkali Metals).

Group 1 elements have

1

valence electron in the outermost

s

-orbital (

ns^1

), leading to low first ionization energy and

+1

cation formation.

Matching requires identifying the subatomic electron configuration unique to Group 1.

Analyze the valence configuration and ion formation of Group 2 (Alkaline Earth Metals).

Group 2 elements have

2

valence electrons in the outermost

s

-orbital (

ns^2

), forming

+2

cations.

Differentiating Group 2 from Group 1 based on the number of valence electrons lost.

Analyze the valence configuration and ion formation of Group 17 (Halogens).

Group 17 nonmetals have

7

valence electrons (

ns^2 np^5

), requiring one electron to complete an octet and forming

-1

anions.

Halogens seek to achieve a noble gas configuration by gaining one electron.

Analyze the valence configuration and chemical properties of Group 18 (Noble Gases).

Group 18 elements possess complete valence shells (

ns^2 np^6

), making them chemically unreactive with very high ionization energies.

Filled valence shells confer maximal stability and chemical inertness.

Key Concept

Periodic table family trends, valence electron configurations, and resulting ionic behavior.

Estimated Time:1m 30s

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