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Chapter 3: Problem 39

Uranium exists mainly as two isotopes in nature, possessing mass numbers 235 and 238 . Write the full atomic symbols for both isotopes.

Short Answer

Expert verified
The full atomic symbols for uranium-235 and uranium-238 are \(_{92}^{235}U\) and \(_{92}^{238}U\), respectively.

Step by step solution

01

Find the atomic number of uranium

Since uranium is present in the periodic table, look up the atomic number of uranium. The atomic number of uranium is 92, which is denoted by \(Z\).
02

Write the full atomic symbol for uranium-235

Using the atomic number (92) and the mass number (235), we can write the full atomic symbol for uranium-235 as \(_{92}^{235}U\).
03

Write the full atomic symbol for uranium-238

Similarly, using the atomic number (92) and the mass number (238), we can write the full atomic symbol for uranium-238 as \(_{92}^{238}U\). Thus, the full atomic symbols for uranium-235 and uranium-238 are \(_{92}^{235}U\) and \(_{92}^{238}U\), respectively.

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Most popular questions from this chapter

Suppose we wanted to use one of the more massive atoms, like \({ }_{92}^{235} \mathrm{U}\), as the standard reference for the atomic mass scale. (a) What would be the universally agreed-upon atomic mass of the \({ }^{235} \mathrm{U}\) isotope? (b) Why don't we use \({ }_{92}^{235} \mathrm{U}\) instead of \({ }_{6}^{12} \mathrm{C}\) ?

If one considers just the representative elements, how many groups would the periodic table have?

A student claims that isotopes of the same element have the same number of neutrons but different numbers of protons. Is he correct? Justify your answer.

Use Dalton's hook atomic models to sketch a molecule of \(\mathrm{H}_{2} \mathrm{~S}\).

How many protons, electrons, and neutrons are there in: (a) \(^{79} \underline{\mathrm{Br}}\) (b) \(^{81} \mathrm{Br}^{-}\) (c) \({ }^{23} \mathrm{Na}^{+}\) (d) \({ }^{3} \mathrm{H}^{+}\)
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