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.
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.
3 answers
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.
An ionic bond is likely because they will want to give away two valence electrons in order to become stable.
1 answer