The discussion revolves around the complete equation for the formation of a metal oxide, represented as MO. Participants explore the nature of metals in reactions, particularly whether they react as atoms or molecules, and how to balance the chemical equation involving oxygen.
Participants express varying views on the nature of metals in reactions, with some asserting that metals do not form diatomic molecules while others acknowledge the existence of diatomic molecules under certain conditions. The discussion remains unresolved regarding the specifics of how metals react and how to balance the equations accurately.
Participants mention the importance of understanding the periodic table and the properties of different groups of elements, as well as the concept of bonding, which may influence the formation of metal oxides.
That's the problem. As I know 2 atoms of 'O' make a molecule of O2 But how to calculate the atoms of M that makes a molecule?CWatters said:Find out how many atoms of each element make a molecule of that element. Then you can write the left hand side of the equation.
The right hand side contains MO.
Then make adjustments to ensure the equation balances.
The periodic table breaks down into groups that in general behave similarly. You will have to read up on the different groups, their properties and the way bonding works.Indranil said:That's the problem. As I know 2 atoms of 'O' make a molecule of O2 But how to calculate the atoms of M that makes a molecule?
Note the idea of "formula units" instead of "molecules".CWatters said:The periodic table breaks down into groups that in general behave similarly. You will have to read up on the different groups, their properties and the way bonding works.
Most metals don't form molecules due to the way they share electrons.
Hammad Shahid said:diatomic bonds