Which of the following elements is most likely to form an oxide with the formula \(\mathrm{MO}_{3}: \mathrm{Zr}, \mathrm{Nb},\) or \(\mathrm{Mo} ?\)

Understanding the periodic table is crucial for predicting how elements will interact and what compounds they will form.
As you move across the periodic table from left to right, elements tend to have higher oxidation states due to an increase in the number of valence electrons they want to share, lose, or gain to achieve stability.

For example, if you look at elements in Group 4, such as zirconium (Zr), these typically have a +4 oxidation state. This is because they have four valence electrons, which they can either share or lose to reach a stable configuration.

Similarly, niobium (Nb) in Group 5 has a +5 oxidation state, since it tends to lose or share five valence electrons. Molybdenum (Mo), on the other hand, is in Group 6 and commonly exhibits a +6 oxidation state correlating with its six valence electrons.

By understanding these trends, predicting the formation of certain compounds becomes more intuitive. In our case, knowing that oxygen is a Group 16 element with a common -2 oxidation state allows us to determine the likely oxidation state needed from another element to form a stable oxide compound.

Chemical formulas represent the makeup of chemical compounds, showing the types and numbers of atoms involved. They're like recipes for creating molecules from atomic ingredients.

The symbol for each element is taken from the periodic table. For instance, 'O' stands for oxygen. The small numbers, known as subscripts, tell us how many atoms of an element are present. For instance, in \( \mathrm{H}_2O \), there are two hydrogen atoms and one oxygen atom in a water molecule.

In our exercise, the formula \( \mathrm{MO}_3 \) suggests that we're dealing with a molecule composed of one metal (M) and three oxygen atoms. The key to understanding this formula is to ascertain the correct metal (M) that forms an oxide compound with a 3:1 oxygen to metal ratio. By combining knowledge of oxidation states with this formula, we can determine that such an oxide would require the metal to have a +6 oxidation state to balance the overall charge of the three -2 charged oxygen atoms.

Oxide compounds contain at least one oxygen atom and one other element. They're widespread in the earth's crust and are commonly formed when oxygen combines with a metal or a nonmetal.

In metal oxides, like the one we're exploring in this exercise, the metal typically donates electrons to oxygen, which is a potent electron acceptor due to its high electronegativity. Therefore, the metal's oxidation state indicates how many electrons it donates.

For the oxide with the formula \( \mathrm{MO}_3 \), our search for the metal that could adopt a +6 oxidation state is necessary to balance the three -2 charges from the oxygen atoms, resulting in a neutral compound. This specific combination is key to understanding the chemical nature of oxide compounds and their formation, emphasizing the relationship between oxidation states and chemical formulas.