For each representation of a nucleus A through E, write the atomic symbol and identify which are isotopes. (4.4, 4.5) Proton (red) Neutron (white)a.

Verified step by step guidance

1. Count the number of protons (red) and neutrons (white) in each nucleus representation A through E.
2. Determine the atomic number (Z) for each nucleus, which is equal to the number of protons.
3. Determine the mass number (A) for each nucleus, which is the sum of protons and neutrons.
4. Write the atomic symbol for each nucleus using the format: \( ^A_Z \text{X} \), where X is the element symbol corresponding to the atomic number.
5. Identify isotopes by comparing the atomic numbers and mass numbers; isotopes have the same atomic number but different mass numbers.

Key Concepts

Atomic Structure

The atomic structure consists of protons, neutrons, and electrons. Protons (red) and neutrons (white) are found in the nucleus, while electrons orbit around the nucleus. The number of protons defines the element, while the total number of protons and neutrons gives the atomic mass. Understanding this structure is essential for identifying isotopes.

Isotopes

Isotopes are variants of a particular chemical element that have the same number of protons but different numbers of neutrons. This difference in neutron count results in different atomic masses. For example, carbon-12 and carbon-14 are isotopes of carbon, with 6 and 8 neutrons, respectively. Identifying isotopes involves comparing the neutron counts in the given representations.

Atomic Symbol

The atomic symbol is a notation that represents an element and its isotopes, typically consisting of one or two letters derived from its name, along with a superscript indicating the atomic mass. For instance, the atomic symbol for carbon is 'C', and for its isotopes, it can be written as '¹²C' for carbon-12 and '¹⁴C' for carbon-14. This notation is crucial for accurately identifying and differentiating isotopes in the question.