Question

Naturally occurring sulfur consists primarily \((94.9 \%)\) of the isotope with mass number 32 , but small amounts of the isotopes with mass numbers \(33,34,\) and 36 also are present. Write the nuclear symbol for each of the isotopes of sulfur. How many neutrons are

Short answer

The nuclear symbols for the isotopes of sulfur are: \[{}^{32}S\], \[{}^{33}S\], \[{}^{34}S\], and \[{}^{36}S\]. The number of neutrons in each isotope is: 16 neutrons for Sulfur-32, 17 neutrons for Sulfur-33, 18 neutrons for Sulfur-34, and 20 neutrons for Sulfur-36.

Step-by-step solution

Find the atomic number of sulfur

The atomic number of sulfur (S) is 16. This number represents the number of protons in the nucleus of an atom. Since the number of protons is the same for all isotopes of an element, each isotope of sulfur has 16 protons.

Write the nuclear symbols

Using the atomic number (Z) and the mass numbers (A) provided for each isotope, we can write the nuclear symbols as follows: Isotope 1 (Sulfur-32): \[{}^{32}S\] Isotope 2 (Sulfur-33): \[{}^{33}S\] Isotope 3 (Sulfur-34): \[{}^{34}S\] Isotope 4 (Sulfur-36): \[{}^{36}S\]

Determine the number of neutrons

To find the number of neutrons in each isotope, subtract the atomic number (the number of protons) from the mass number (total number of protons and neutrons) for each isotope. Isotope 1 (Sulfur-32): Number of neutrons \(= 32 - 16 = 16\) Isotope 2 (Sulfur-33): Number of neutrons \(= 33 - 16 = 17\) Isotope 3 (Sulfur-34): Number of neutrons \(= 34 - 16 = 18\) Isotope 4 (Sulfur-36): Number of neutrons \(= 36 - 16 = 20\) Therefore, the number of neutrons in each isotope of sulfur is as follows: Sulfur-32: 16 neutrons Sulfur-33: 17 neutrons Sulfur-34: 18 neutrons Sulfur-36: 20 neutrons

Key concepts

Atomic Number

Understanding atomic number is fundamental in the study of chemistry and physics. It is denoted by the symbol 'Z' and represents the number of protons in the nucleus of an atom. Since protons are positively charged, the atomic number also indicates the total positive charge of the nucleus.

For example, sulfur has an atomic number of 16, which means every sulfur atom has 16 protons in its nucleus, regardless of the isotope. This atomic number is unique to sulfur, and it's what distinguishes it from other elements on the periodic table. Knowing the atomic number allows chemists to predict the element's chemical properties and its place in the periodic system.

Mass Number

The mass number, symbolized by 'A', is another crucial concept, representing the total number of protons and neutrons in an atom's nucleus. Unlike the atomic number, the mass number can vary even among atoms of the same element, leading to different isotopes.

For sulfur isotopes, the mass numbers are 32, 33, 34, and 36, corresponding to each isotope. To determine the mass number of an isotope, one simply adds together the count of protons and neutrons within the atom's nucleus. It is important to note that while electrons are also part of an atom, their mass is negligible compared to protons and neutrons and therefore not included in the mass number.

Nuclear Symbol

A nuclear symbol provides a concise way to convey important information about a particular isotope of an element. It includes the element's symbol on the periodic table, the mass number on the upper left, and the atomic number on the lower left.

For example, the nuclear symbol for the most common isotope of sulfur would be written as \[{}^{32}_{16}S\]. The upper number, 32, indicates the mass number, and the lower number, 16, represents the atomic number. Using such symbols allows scientists to quickly identify and differentiate between isotopes of the same element, as each isotope will have a unique mass number.

Neutrons in Isotopes

The number of neutrons in isotopes can vary and is one of the defining features of an isotope. Neutrons are neutrally charged particles within an atom's nucleus. While their presence doesn't affect the chemical properties of the element, it does influence the atomic mass and the stability of the atom.

For sulfur isotopes, the neutron counts are obtained by subtracting the atomic number from the mass number. This gives us neutron counts of 16, 17, 18, and 20 for isotopes Sulfur-32, Sulfur-33, Sulfur-34, and Sulfur-36, respectively. By comparing neutron numbers among various isotopes, one can infer the relative stability and natural abundance of each isotope.