Using a suitable reference such as the CRC Handbook of Chemistry and Physics or http://www.webelements.com, look up the following information for nickel: (b) the atomic masses (in u), (c) the natural abundances of the five most abundant isotopes.

Verified step by step guidance

1. Step 1: Understand that isotopes are atoms of the same element with different numbers of neutrons, resulting in different atomic masses.
2. Step 2: Recognize that the atomic mass of an element is a weighted average of the masses of its isotopes, based on their natural abundances.
3. Step 3: Use a reliable reference source such as the CRC Handbook of Chemistry and Physics or WebElements to find the atomic masses of nickel's isotopes.
4. Step 4: Look up the natural abundances of the five most abundant isotopes of nickel in the same reference source.
5. Step 5: Compile the information gathered: list the isotopes, their atomic masses, and their natural abundances.

Key Concepts

Atomic Mass

Atomic mass is the weighted average mass of an element's isotopes, measured in atomic mass units (u). It reflects both the mass and the relative abundance of each isotope in nature. For nickel, the atomic mass is influenced by its isotopes, which vary in their number of neutrons.

Isotopes

Isotopes are variants of a chemical element that have the same number of protons but different numbers of neutrons, resulting in different atomic masses. For nickel, there are several isotopes, and their natural abundances can vary, affecting the overall atomic mass of the element.

Natural Abundance

Natural abundance refers to the relative proportions of different isotopes of an element found in nature. It is usually expressed as a percentage and is crucial for calculating the average atomic mass of an element. For nickel, knowing the natural abundances of its isotopes helps in understanding its chemical properties and behavior.