Fill in the following table: 8^15O^+ ? ? ? Mass number ? 27 ?

step 1 In this problem, we're asked to complete the table. We are given the following information. For

Fill in the following table: 8^15O^+ ? ? ? ...

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

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

Key Concepts

Electron Count

The electron count is determined by balancing the number of protons against the ion's charge. In neutral atoms, the electron count equals the atomic number; however, for ions, electrons are either gained or lost, resulting in a net positive or negative charge that influences chemical reactivity.

Isotopes

Isotopes are variants of a given element that have the same number of protons but a different number of neutrons. This difference in neutron number causes variations in the mass number, which can alter the stability and physical properties of the atom without changing its chemical identity.

Ion Charge

Ion charge results from an atom either losing or gaining electrons. This charge, denoted by a positive or negative sign, reflects the difference between the number of protons and electrons, fundamentally affecting the atom's behavior in chemical bonding and reactions.

Mass Number

The mass number is the sum of an atom's protons and neutrons, reflecting the overall mass of the nucleus. This critical value helps differentiate between isotopes of an element, as isotopic variations arise from differences in neutron count while the atomic number remains unchanged.

Atomic Number

The atomic number represents the number of protons in an atom's nucleus, defining the element’s identity and its position on the periodic table. It is pivotal in determining the arrangement of electrons, thus influencing the atom's chemical properties and interactions.

Neutron Number

The neutron number, found by subtracting the atomic number from the mass number, indicates the number of neutrons in the nucleus. Neutrons contribute to nuclear stability and play a vital role in whether an isotope is stable or radioactive, influencing nuclear reactions and decay processes.

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