Choose one element from Group 2 (alkaline earth metals) and one from Group 16 (Halogens) on the Periodic Table, Describe how the atomic structure of each element including the number of protons,electrons and valence electrons, determines its specific position within its group and period. Explain how these structural features influence the elements chemical properties, such as reactivity and bonding tendencies. Create a visual diagram or a chart to illustrate your explanation, showing the atomic structure and how it relates to the elements position on the Periodic Table

Question

Cuterua for Evaluation
Correct identification of the selected elements and their respective groups.
Clear and accurate explanation of how atomic structure (protons electrons valence electrons) influence Periodic Table positioning
Through description of how the atomic structure affects the chemical properties and reactivity of each element
Effective use visual aids to enhance the clarity and understanding of explanation

Answer 1

Let's select Magnesium (Mg) from Group 2 (alkaline earth metals) and Chlorine (Cl) from Group 17 (halogens) for our discussion.

Atomic Structure

Magnesium (Mg)

• Position on the Periodic Table: Group 2, Period 3
• Atomic Number: 12
• Protons: 12
• Electrons: 12 (in a neutral atom)
• Valence Electrons: 2 (in the outermost shell, which is the third shell in the case of Magnesium: 1s² 2s² 2p⁶ 3s²)

Chlorine (Cl)

• Position on the Periodic Table: Group 17, Period 3
• Atomic Number: 17
• Protons: 17
• Electrons: 17 (in a neutral atom)
• Valence Electrons: 7 (in the outermost shell: 1s² 2s² 2p⁶ 3s² 3p⁵)

Atomic Structure Influence on Positioning

The position of an element in the Periodic Table is determined by its atomic number (number of protons), which indirectly reveals its electron arrangement and therefore its group and period:

• Groups relate to the number of valence electrons. In Magnesium (Group 2), the presence of 2 valence electrons indicates that it can lose these electrons easily, allowing it to participate in chemical bonding and ionic reactions. In Chlorine (Group 17), having 7 valence electrons means it tends to gain one more electron to achieve a stable octet, characteristic of halogens.

• Periods indicate the number of electron shells surrounding the nucleus. Both Magnesium and Chlorine are in Period 3, which means they have three electron shells.

Chemical Properties Influenced by Atomic Structure

• Reactivity:

  • Magnesium (Mg): Magnesium is reactive, but not as much as Group 1 alkali metals, due to its two valence electrons that it readily loses to form +2 ions (Mg²⁺). This reactivity allows it to bond with nonmetals, giving rise to compounds like MgO (magnesium oxide) and MgCl₂ (magnesium chloride).
  • Chlorine (Cl): Chlorine is highly reactive, significantly more than Mg, as it only needs to gain one electron to complete its octet. It readily forms -1 ions (Cl⁻) and participates in ionic bonding (e.g., NaCl) and covalent bonding (e.g., Cl₂).

• Bonding Tendencies:

  • Magnesium typically forms ionic bonds by losing its two valence electrons.
  • Chlorine typically forms ionic bonds by gaining an electron, or covalent bonds by sharing electrons.

Visual Diagram/Chart

Below is a textual representation of a visual diagram that can be drawn to illustrate the atomic structures of Magnesium and Chlorine:

                            PERIODIC TABLE
                          --------------------------
                          |  Group 2 | Group 17    |
                          |  Mg    | Cl          |
                          --------------------------
                           Atomic Structure
          +------------------+           +---------------------+
          |   Magnesium (Mg) |           |    Chlorine (Cl)    |
          |------------------|           |---------------------|
          | Protons: 12      |           | Protons: 17         |
          | Electrons: 12    |           | Electrons: 17       |
          | Valence Electrons:|          | Valence Electrons:  |
          | 2                |           | 7                   |
          |                  |           |                     |
          | Reactivity:         |         | Reactivity:            |
          | Moderate (ionic bonds)|       | High (ionic / covalent bonds) |
          +------------------+           +---------------------+

Conclusion

By understanding the atomic structure of Magnesium and Chlorine, we see how their configurations of protons, electrons, and valence electrons dictate their positions on the Periodic Table, influencing their chemical properties, such as reactivity and bonding tendencies. Magnesium — a metallic element — is characterized by its ability to lose electrons easily, while Chlorine — a nonmetal — is known for its high reactivity due to its tendency to gain electrons. This fundamental understanding of atomic structure is key to grasping the broader concepts of periodicity in chemical behavior.