Which compound would you expect to have the highest melting point? Base your answer off of the bonding theory presented in this course.
BeO
MgO
CaO
SrO
caO
You can look them up on Google.
It is mgo because of its fajans factor
To determine which compound would have the highest melting point, we need to consider the bonding theory presented in this course. The melting point of a compound is mainly influenced by the strength of the bonds between its atoms.
In this case, all the compounds listed (BeO, MgO, CaO, SrO) are metal oxides, where the metal (Be, Mg, Ca, Sr) is bonded to oxygen (O). These metal oxides are known as ionic compounds because they are made up of positively charged metal cations and negatively charged oxide anions.
According to the bonding theory, the strength of an ionic bond is directly related to the charge of the ions and the distance between them. A higher charge or a shorter distance between the ions results in stronger electrostatic attractions, leading to a higher melting point.
In comparing the listed compounds, we can assume that the ionic charge of these metal cations increases from Be to Sr because they are all in the same group (Group 2) of the periodic table. This means that the positive charge on the cation increases, making the ionic bond stronger.
Additionally, as we move down the group, the atomic radius of the metal cations also increases. This results in a larger distance between the cations and the anions, which weakens the electrostatic attraction.
Based on these considerations, we can conclude that the compound with the highest melting point would be CaO. This is because calcium (Ca) has a larger ionic charge and a smaller atomic radius compared to the other elements in the list. Hence, CaO will have stronger ionic bonding and a higher melting point compared to BeO, MgO, and SrO.
Remember, when determining melting points of compounds, it is essential to consider the principles of bonding, specifically the ionic bond strength based on ion charges and distances.