The most abundant isotope of nickel is 28^58 Ni. (4.4) a. How many protons, neutrons, and elect

step 1 Okay, so let's find the number of protons, neutrons, and electrons on this element right here. T

The most abundant isotope of nickel is 28^58 Ni. (4.4) a....

The most abundant isotope of nickel is ${ }_{28}^{58} \mathrm{Ni}$. (4.4) a. How many protons, neutrons, and electrons are in $\frac{58}{28} \mathrm{Ni}$ ? b. What is the atomic symbol of another isotope of nickel with 35 neutrons? c. What is the name and symbol of an atom with the same mass number as in part $\mathbf{b}$ and 34 neutrons?

The most abundant isotope of nickel is ${ }_{28}^{58} \mathrm{Ni}$. (4.4)
a. How many protons, neutrons, and electrons are in $\frac{58}{28} \mathrm{Ni}$ ?
b. What is the atomic symbol of another isotope of nickel with 35 neutrons?
c. What is the name and symbol of an atom with the same mass number as in part $\mathbf{b}$ and 34 neutrons?

Key Concepts

Isotopes

Isotopes are variations of the same element that have the same atomic number but different numbers of neutrons, resulting in different mass numbers. While isotopes exhibit nearly identical chemical behavior because they have the same number of protons and electrons, their physical properties and nuclear stability can differ significantly due to the variation in neutron count.

Atomic Number

The atomic number of an element represents the number of protons in the nucleus of an atom. It defines the identity of an element and determines its position on the periodic table. In a neutral atom, the atomic number is also equal to the number of electrons, which play a key role in chemical bonding and reactivity.

Mass Number

The mass number is the sum of the protons and neutrons in an atom's nucleus. It provides an approximation of the atom's atomic mass and is vital when distinguishing between different isotopes of the same element. Changes in the number of neutrons will alter the mass number without affecting the atomic number.

Atomic Symbol Notation

Atomic symbol notation, often written with the mass number as a superscript and the atomic number as a subscript preceding the element’s symbol, provides a concise way to represent isotopes. This notation encodes important information about the number of protons, neutrons, and overall mass of the nucleus, helping to distinguish between various isotopes and elements.

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