Group 2 elements have two valence electrons. Which kind of bond will they most likely form, and why? (1 point)
o A covalent bond is likely because they want to share those two valence
electrons in order to become stable.
o An ionic bond is likely because they are metals and will want to bond with
nonmetals.
• A metallic bond is likely because they are metals and can bond with other
metals.
o An ionic bond is likely because they will want to give away two valence
electrons in order to become stable.
o An ionic bond is likely because they will want to give away two valence electrons in order to become stable.
The correct answer is: An ionic bond is likely because they will want to give away two valence electrons in order to become stable.
Group 2 elements, also known as alkaline earth metals, have two valence electrons. These elements have a tendency to lose these valence electrons in order to achieve a stable electron configuration. As a result, they form positive ions with a charge of +2.
To achieve stability, these positive ions then bond with negatively charged particles, usually nonmetals, which have a tendency to gain electrons. This electrostatic attraction between the positive and negative ions forms an ionic bond.
Therefore, an ionic bond is most likely to be formed by Group 2 elements because they will want to give away their two valence electrons to become stable.
The correct answer is: A metallic bond is likely because they are metals and can bond with other metals.
To explain why this is the most likely bond, we need to understand the properties of Group 2 elements. Group 2 elements, also known as alkaline earth metals, include elements such as beryllium, magnesium, calcium, and so on. These elements have two valence electrons in their outermost energy level.
Group 2 elements have a strong tendency to lose these two valence electrons in order to achieve a stable electron configuration. By losing these electrons, they can achieve a filled outermost energy level, which is the more stable state for atoms.
In the case of metallic bonding, the valence electrons are not transferred or shared between atoms, like in ionic or covalent bonds. Instead, the valence electrons are delocalized and move freely among the positively charged metal ions.
This delocalization of electrons allows the metal atoms to form a lattice structure with positive metal ions surrounded by a "sea" of delocalized electrons. This leads to the characteristic properties of metals such as high electrical and thermal conductivity, malleability, and ductility.
Therefore, based on the properties of Group 2 elements and their tendency to lose valence electrons, it is most likely that they will form metallic bonds with other metals.