Can the subscripts in a chemical formula be fractions? Explain. Can the coefficients in a balanced chemical equation be fractions? Explain. Changing the subscripts of chemicals can balance the equations mathematically. Why is this unacceptable?

In a chemical formula, subscripts represent the number of atoms of each element present in the compound. Since atoms are discrete units and cannot be broken down into fractions, it is not possible for subscripts in a chemical formula to be fractions. Each subscript must be a whole number because it represents whole atoms.

In a balanced chemical equation, coefficients indicate the number of molecules or moles of each compound needed for the reaction to proceed. While it is more common to express coefficients as whole numbers for simplicity, fractions can sometimes be used when balancing equations as long as the coefficients represent a ratio. For example, consider the following unbalanced equation: \[H_2 + O_2 \rightarrow H_2O\] To balance this equation, we can use a fractional coefficient for \(O_2\): \[2H_2 + \frac{1}{2} O_2 \rightarrow 2H_2O\] In this case, the fractional coefficient represents a ratio. However, we often prefer to work with whole numbers and eventually multiply all coefficients by the lowest common multiple to eliminate the fraction: \[2(2H_2 + \frac{1}{2} O_2) \rightarrow 2(2H_2O)\] So, the balanced equation with whole-number coefficients would be: \[4H_2 + 2O_2 \rightarrow 4H_2O\]

Changing the subscripts in a chemical formula to balance the reaction would mean changing the identity of the compounds involved. Since a chemical formula represents a specific compound with a definite composition, altering the subscript would create a new compound with different properties. Balancing a chemical equation is about preserving the law of conservation of mass, so we do not change the actual composition or identity of the compounds in the reaction. That's why we can only adjust the coefficients to balance a chemical equation, as changing the subscripts would violate the basic principles of chemical reactions.