Question

Consider an atom of \({ }^{58} \mathrm{Ni}\). (a) How many protons, neutrons, and electrons does this atom contain? (b) What is the symbol of the ion obtained by removing two electrons from \({ }^{58} \mathrm{Ni}\) ? (c) What is the symbol for the isotope of \({ }^{58} \mathrm{Ni}\) that possesses 33 neutrons?

Short answer

(a) 28 protons, 30 neutrons, 28 electrons. (b) \( ^{58} \text{Ni}^{2+} \). (c) \( ^{61} \text{Ni} \).

Step-by-step solution

Determine the Number of Protons

The atomic number of Nickel (Ni) is 28, which means each Ni atom contains 28 protons.

Determine the Number of Neutrons

The mass number of \( ^{58} \text{Ni} \) is 58. The number of neutrons is calculated by subtracting the number of protons from the mass number: \( 58 - 28 = 30 \) neutrons.

Determine the Number of Electrons

In a neutral atom, the number of electrons is equal to the number of protons. Therefore, \( ^{58} \text{Ni} \) has 28 electrons.

Determine the Symbol of the Ion

Removing two electrons from Nickel creates a positive ion with two fewer electrons than protons. The symbol for this ion is \( ^{58} \text{Ni}^{2+} \).

Identify the Isotope with 33 Neutrons

An isotope of \( ^{58} \text{Ni} \) with 33 neutrons has an altered mass number. The new mass number is calculated as: 33 (neutrons) + 28 (protons) = 61. The symbol is \( ^{61} \text{Ni} \).

Key concepts

Atomic Structure

At the very core of understanding chemistry is comprehending atomic structure. Atoms are the basic units of matter, which are composed of three main sub-atomic particles: protons, neutrons, and electrons.

• Protons carry a positive charge and are located in the atom's nucleus. The number of protons determines the atomic number of the element. In this exercise, Nickel (Ni) has 28 protons, represented by its atomic number 28.
• Neutrons are neutral; they have no electric charge and are also found in the nucleus. Neutrons, together with protons, account for most of the atom's mass.
• Electrons are negatively charged and orbit around the nucleus in electron shells. In a neutral atom, the number of electrons equals the number of protons.

This balanced configuration of charges ensures that the atom is neutral. Thus, for Nickel, there would also be 28 electrons in its neutral state, perfectly balancing the 28 positive charges of the protons.

Chemical Ions

Understanding chemical ions involves recognizing how atoms gain or lose electrons. When an atom does not have the same number of protons and electrons, it becomes a charged particle known as an ion.

• If electrons are removed from an atom, it results in a positive charge, forming a cation. For Nickel ( ^{58} ext{Ni} ), removing two electrons results in a ^{58} ext{Ni}^{2+} ion, meaning the ion has two fewer electrons than protons.
• Conversely, if an atom gains electrons, it becomes negatively charged and is known as an anion.

These changes in charge have profound effects on the chemical properties of the element, influencing how they interact and bond with other elements in various compounds. Chemical ions are critical for countless biological and chemical processes.

Mass Number

The concept of mass number is vital for understanding isotopes and for calculating neutrons in an atom. Mass number, often denoted by the letter A, is the total count of protons and neutrons in an atom's nucleus. For Nickel ( ^{58} ext{Ni} ), its mass number is 58, indicating that its nucleus contains a total of 58 protons and neutrons combined. The mass number is an integer that helps identify specific isotopes of an element. Isotopes are variants of a chemical element that differ only in neutron count, not in proton count. Thus, when you think about mass number: - It is specific to each isotope and affects the atomic mass. - It helps differentiate between different isotopes without affecting the overall charge of the atom, as protons determine the chemical identity and charge.

Neutron Calculation

Calculating neutrons in an atom involves using its atomic and mass numbers. It’s quite simple:1. Take the mass number of the isotope; for ^{58} ext{Ni}, this is 58.2. Subtract the atomic number (number of protons) from the mass number. Nickel has an atomic number of 28, so:\[ ext{Neutrons} = 58 - 28 = 30 \]This calculation is useful in identifying isotopes and understanding elemental structures. For example, if a Nickel isotope has 33 neutrons, then the new mass number would be:\[ ext{Mass Number} = 28 + 33 = 61 \]This results in the isotope ^{61} ext{Ni}, showing how alterations in the neutron count affect the isotope identity without altering its chemical properties.