Question

questions:

1. define the term elemental groups of families:

1. give four examples of elemental groups:
2. group 4: transition metals 2. noble gases
3. actinides 4. lanthanides
4. how does the group number of an elemental family compare with the number of valence electrons for the same group?

4a. list similar properties of the alkali metals.

4b. what similarities in electron arrangement do the alkali metals show?

5a. list similar properties of the halogens.

5b. what similarities in electron arrangement do the halogens show?

6a. list similar properties of the noble gases.

6b. what similarities in electron arrangement do the nobles gases show?

Explanation:

1. Elemental groups or families: In the periodic table, elements with similar chemical properties are grouped together. These groups or families share common characteristics due to their similar electron configurations.
2. Examples of elemental groups:

• Alkali metals (Group 1)
• Alkaline - earth metals (Group 2)
• Halogens (Group 17)
• Noble gases (Group 18)

1. Group number and valence electrons:

• For main - group elements (Groups 1, 2, 13 - 18), the group number (using the 1 - 18 numbering system) is related to the number of valence electrons.
• Groups 1 and 2: The group number is equal to the number of valence electrons. For example, Group 1 elements (alkali metals) have 1 valence electron.
• Groups 13 - 18: The number of valence electrons is equal to the group number minus 10. For example, Group 17 (halogens) has \(17 - 10=7\) valence electrons.

4a. Properties of alkali metals:

• They are soft metals.
• Highly reactive, especially with water.
• Have low melting and boiling points compared to many other metals.
• Good conductors of heat and electricity.

4b. Electron - arrangement similarity of alkali metals:

• They all have one electron in their outermost shell (valence electron configuration \(ns^{1}\), where \(n\) is the principal quantum number of the outermost shell).

5a. Properties of halogens:

• They are non - metals.
• Highly reactive (especially fluorine).
• Exist as diatomic molecules (\(F_{2}\), \(Cl_{2}\), \(Br_{2}\), \(I_{2}\)).
• Form salts when they react with metals.

5b. Electron - arrangement similarity of halogens:

• They all have seven electrons in their outermost shell (valence electron configuration \(ns^{2}np^{5}\)).

6a. Properties of noble gases:

• They are colorless, odorless gases.
• Have very low reactivity (inert under normal conditions).
• Exist as monatomic gases.

6b. Electron - arrangement similarity of noble gases:

• They have a full outer electron shell. For helium, it has a \(1s^{2}\) configuration, and for other noble gases (neon, argon, etc.), they have a \(ns^{2}np^{6}\) configuration.

Answer:

1. In the periodic table, elements with similar chemical properties are grouped together. These groups or families share common characteristics due to their similar electron configurations.
2. Alkali metals (Group 1), Alkaline - earth metals (Group 2), Halogens (Group 17), Noble gases (Group 18)
3. For main - group elements (Groups 1, 2, 13 - 18), Groups 1 and 2: The group number is equal to the number of valence electrons. Groups 13 - 18: The number of valence electrons is equal to the group number minus 10.

4a. Soft metals; highly reactive with water; low melting and boiling points; good conductors of heat and electricity.
4b. They all have one electron in their outermost shell (valence electron configuration \(ns^{1}\)).
5a. Non - metals; highly reactive (especially fluorine); exist as diatomic molecules; form salts with metals.
5b. They all have seven electrons in their outermost shell (valence electron configuration \(ns^{2}np^{5}\)).
6a. Colorless, odorless gases; very low reactivity; monatomic gases.
6b. Helium has a \(1s^{2}\) configuration, and other noble gases have a \(ns^{2}np^{6}\) configuration (full outer electron shell).