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Chapter 3: Problem 141

Atom A has 35 protons and 44 neutrons in its nucleus. Atom \(\mathrm{B}\) has 35 protons and 46 neutrons in its nucleus. Should we expect similar or different chemical properties for these atoms? Explain.

Short Answer

Expert verified
Atom A and Atom B have similar chemical properties because they are both isotopes of bromine with the same atomic number (35 protons), leading to similar electron configurations and chemical reactivity.

Step by step solution

01

Identify the atomic number for both atoms

As both Atom A and Atom B have 35 protons, their atomic number is 35.
02

Determine the mass number for both atoms

The mass number of an atom is the sum of its protons and neutrons. For Atom A, the mass number is 35 (protons) + 44 (neutrons) = 79. For Atom B, the mass number is 35 (protons) + 46 (neutrons) = 81.
03

Identify the elements

Using the periodic table, we can find the element that has an atomic number of 35. Both Atom A and Atom B have 35 protons, which means they are both the element bromine (Br).
04

Determine if the atoms are isotopes

Since Atom A and Atom B are both bromine atoms but have different mass numbers (79 and 81, respectively), they are isotopes of bromine. This means that they are the same element but with a different number of neutrons in their respective nuclei.
05

Compare the chemical properties of isotopes

Isotopes of the same element have the same chemical properties due to their identical atomic numbers, which determine the arrangement of electrons in their electron shells and their chemical reactivity.
06

Conclusion

Atom A and Atom B have similar chemical properties because they are both isotopes of bromine, which have the same atomic number (35 protons) and hence similar electron configurations.

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Most popular questions from this chapter

Explain the difference between mass number and atomic mass.

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

Arrange \(\mathrm{Na}, \mathrm{Cs}, \mathrm{S}, \mathrm{Cl}\) in order of increasing first ionization energy.

For each pair, indicate which atom loses an electron more easily: (a) \(\mathrm{Na}\) or \(\mathrm{K}\) (b) Na or Al (c) \(\mathrm{Rb}\) or \(\mathrm{Ca}\) (d) \(\mathrm{S}\) or \(\mathrm{Cl}\) (e) Br or Kr

Fill in the following table: $$ \begin{array}{lcccc} & { }_{8}^{15} \mathrm{O}^{+} & ? & ? & ? \\ \hline \text { Mass number } & ? & 27 & ? & 58 \\ \text { Atomic number } & ? & ? & 15 & ? \\ \text { Number of protons } & ? & 13 & ? & ? \\ \text { Number of neutrons } & ? & ? & 16 & 30 \\ \text { Number of electrons } & ? & ? & ? & 27 \\ \text { Charge on ion } & ? & +3 & -3 & +1 \\ \hline \end{array} $$
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