Question
Group 2 elements have two valence electrons. Which kind of bond will they most likely form, and why?(1 point)
Responses
An ionic bond is likely because they are metals and will want to bond with nonmetals.
A covalent bond is likely because they want to share those two valence electrons in order to become stable.
An ionic bond is likely because they will want to give away two valence electrons in order to become stable.
A metallic bond is likely because they are metals and can bond with other metals.
An ionic bond is likely because they will want to give away two valence electrons in order to become stable.
Explanation: Group 2 elements (also known as the alkaline earth metals), such as beryllium, magnesium, calcium, strontium, barium, and radium, have two electrons in their outermost shell. These elements typically tend to lose these two electrons to achieve a noble gas configuration, which makes them more stable. When they lose the electrons, they become positively charged ions (cations with a 2+ charge). These cations can then form ionic bonds with nonmetals that need additional electrons to achieve a full outer shell. The nonmetals gain the electrons, becoming negatively charged ions (anions), and the electrostatic attraction between the oppositely charged ions results in the formation of an ionic compound.
what is the correct answer
The correct answer is:
An ionic bond is likely because they will want to give away two valence electrons in order to become stable.
To determine which kind of bond Group 2 elements are most likely to form, we need to understand their properties and their tendency to gain or lose electrons.
Group 2 elements, also known as alkaline earth metals, have two valence electrons in their outermost energy level. These elements include beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba), and radium (Ra).
Option 1 suggests that an ionic bond is likely because Group 2 elements are metals and will want to bond with nonmetals. This statement is incorrect because Group 2 elements generally do not form ionic bonds. They have a tendency to lose their two valence electrons, not gain additional electrons.
Option 2 states that a covalent bond is likely because Group 2 elements want to share those two valence electrons in order to become stable. This option is also incorrect because Group 2 elements typically lose their valence electrons rather than share them.
Option 3 proposes that an ionic bond is likely because Group 2 elements will want to give away two valence electrons in order to become stable. This option is correct. Group 2 elements have a strong tendency to lose their two valence electrons and form ionic bonds with nonmetals, which have a tendency to gain electrons.
Option 4 suggests that a metallic bond is likely because Group 2 elements are metals and can bond with other metals. This statement is partially correct. Group 2 elements can form metallic bonds when they are in a metallic crystal lattice, but this is not their most likely bonding behavior.
Therefore, the correct answer is: "An ionic bond is likely because they will want to give away two valence electrons in order to become stable."