To find the difference between the sizes of a hydrogen atom and an oxygen atom, we'll first clarify the sizes given.
You noted that the size of a hydrogen atom is given as "about m." Let's assume that it is a placeholder, so I'll use an approximate value for a hydrogen atom, which is about \(1.1 \times 10^{-10}\) m.
The size of the oxygen atom is \(0.000000000152\) m, which can be expressed in scientific notation as: \[ 1.52 \times 10^{-10} \text{ m} \]
Now, we will calculate the difference between the sizes of the hydrogen atom and the oxygen atom:
\[ \text{Size of Hydrogen (H)} - \text{Size of Oxygen (O)} = (1.1 \times 10^{-10}) - (1.52 \times 10^{-10}) \]
To perform this subtraction, we can express both numbers clearly for subtraction:
\[ (1.1 - 1.52) \times 10^{-10} = -0.42 \times 10^{-10} \]
Since we would typically want the result in a positive format, we can express it as:
\[ 0.42 \times 10^{-10} = 4.2 \times 10^{-11} \text{ m} \]
However, it seems none of the options directly match this result. Let's evaluate the differences in context of the given options.
- Specifically, we are usually interested in absolute differences: \[ |1.1 \times 10^{-10} - 1.52 \times 10^{-10}| = 0.42 \times 10^{-10} \]
Now, rounding the \(0.42\) value to one decimal digit will lose precision. In case the hydrogen atom size input needs to be changed or reaffirmed based on your study material, reconfirm it as \(1 \times 10^{-10}\) is a common reference.
When estimating:
- If we use \( 0.1 \times 10^{-9} \) (or effectively \(1 \times 10^{-10}\)) reduces ambiguity.
To conclude, based on available choices, the closest valid representation appears to correctly adjust around \(3.2 \times 10^{-10}\) within applied context. In a robust academic forum, rechecking the fundamental sizes often leads back to atomic radius references, which might align further.
If you hold specific values for hydrogen, submit corrected entries for precision now acknowledging the likely resulting differences in the available options.