Ba2+

Definition

Ba2+ is a barium ion that has lost two electrons, resulting in a +2 charge. This positively charged ion is formed when barium, an alkaline earth metal, reacts with other elements and compounds. Understanding Ba2+ is essential in studying ionic bonding, as it highlights the behavior of metals in forming ionic compounds and their interactions with nonmetals.

5 Must Know Facts For Your Next Test

1. Barium has an atomic number of 56 and is located in Group 2 of the periodic table, making it an alkaline earth metal.
2. When barium loses two electrons to become Ba2+, it achieves a stable electron configuration similar to that of noble gases.
3. Ba2+ readily forms ionic bonds with nonmetals, such as chlorine or sulfur, to create compounds like barium chloride (BaCl2) or barium sulfide (BaS).
4. In aqueous solutions, Ba2+ can influence the solubility of certain compounds and is often used in medical imaging procedures due to its opacity to X-rays.
5. The formation of Ba2+ illustrates the principle of charge balance in ionic compounds, where the total positive charge must equal the total negative charge for electrical neutrality.

Review Questions

• How does the formation of Ba2+ demonstrate the principles of ionic bonding?
  • The formation of Ba2+ exemplifies ionic bonding as barium, an alkaline earth metal, loses two electrons to achieve a stable electron configuration. This loss creates a positively charged ion that can interact with negatively charged ions from nonmetals. When Ba2+ bonds with anions like Cl-, it leads to the formation of ionic compounds, showcasing how metals tend to lose electrons while nonmetals gain them during bonding.
• Discuss the role of electronegativity in the interaction between Ba2+ and nonmetal ions.
  • Electronegativity plays a crucial role in the interaction between Ba2+ and nonmetal ions. While barium has a low electronegativity, indicating it readily loses electrons to form Ba2+, nonmetals typically have higher electronegativities. This difference drives the transfer of electrons from Ba to nonmetals like chlorine, leading to strong ionic bonds where Ba2+ attracts Cl- ions due to their opposite charges. Understanding this relationship helps explain why barium readily forms stable ionic compounds.
• Evaluate the significance of Ba2+ in practical applications, particularly in medical imaging and environmental chemistry.
  • Ba2+ has significant implications in both medical imaging and environmental chemistry. In medical imaging, barium sulfate (BaSO4) is used as a contrast agent for X-ray imaging of the gastrointestinal tract because it absorbs X-rays effectively. This practical application highlights the importance of understanding ionic compounds containing Ba2+. In environmental chemistry, knowing how Ba2+ interacts with other ions can help assess its impact on ecosystems, as excessive barium can be toxic to aquatic life. Analyzing these applications reveals how understanding Ba2+ is crucial for both health and environmental safety.

Related terms

Ionic Bonding: The electrostatic attraction between positively and negatively charged ions, resulting in the formation of ionic compounds.

Electronegativity: The ability of an atom to attract electrons in a chemical bond, influencing how ions form during bonding.

Alkaline Earth Metals: The group of elements in Group 2 of the periodic table, which includes barium and is characterized by their tendency to form +2 cations.