Question

Write the full symbols for the isotopes of oxygen having 8,9, and 11 neutrons.

Short answer

The full symbols for the oxygen isotopes with 8, 9, and 11 neutrons are: \(^{16}_8\)O, \(^{17}_8\)O, and \(^{19}_8\)O.

Step-by-step solution

Identify the atomic number and symbol for oxygen

Oxygen has an atomic number (Z) of 8, which signifies it has 8 protons in its nucleus. The symbol for oxygen is O.

Determine the mass number for each isotope

To find the mass number (A) of an isotope, we add the number of protons and neutrons in the nucleus. We know that oxygen has 8 protons, and we are given the number of neutrons for each isotope. Using this information, we can calculate the mass number for each isotope: - For 8 neutrons: A = 8 (protons) + 8 (neutrons) = 16 - For 9 neutrons: A = 8 (protons) + 9 (neutrons) = 17 - For 11 neutrons: A = 8 (protons) + 11 (neutrons) = 19

Write the full symbol for each isotope

Now that we have the atomic number (Z) and mass number (A) for each isotope, we can write the full symbols for each isotope using the following format: ^A_Z X, where X is the element symbol. - For the oxygen isotope with 8 neutrons: \(^{16}_8\)O - For the oxygen isotope with 9 neutrons: \(^{17}_8\)O - For the oxygen isotope with 11 neutrons: \(^{19}_8\)O

Key concepts

Atomic Number

The atomic number, typically represented by the letter 'Z', is a key concept in understanding elements and their isotopes. It indicates the number of protons in the nucleus of an atom which, for any given element, is always constant. In our discussion about oxygen, the atomic number is 8, meaning every atom of oxygen contains 8 protons.

The uniqueness of the atomic number is what defines the identity of an element. For example, hydrogen has an atomic number of 1, while carbon has an atomic number of 6. Therefore, no matter how many neutrons an atom of oxygen might have, it will always be oxygen if the number of protons remains 8. This is crucial in identifying elements as we explore their isotopes and their respective places in the periodic table.

Mass Number

When we speak of the mass number, represented by 'A', we're considering the total count of protons and neutrons in an atom's nucleus. It's useful to differentiate between isotopes of an element, which can have varying numbers of neutrons but the same number of protons.

For instance, with oxygen, the mass number changes when we alter the number of neutrons. If we have an isotope of oxygen with 8 neutrons, its mass number becomes 16 (since 8 protons + 8 neutrons = 16). If it has 9 neutrons, the mass number rises to 17, and with 11 neutrons, it increases to 19. Different mass numbers in isotopes of the same element lead to variations in their physical properties and are essential in fields such as nuclear chemistry and radioactive dating.

Nuclear Chemistry

Nuclear chemistry is the field that deals with the reactions and properties of atomic nuclei. The understanding of isotopes is a cornerstone of nuclear chemistry. Isotopes are atoms of the same element that have different mass numbers due to variations in the number of neutrons.

This has profound implications, including the stability of nuclei and the type of nuclear reactions they may undergo. For example, certain isotopes are unstable and emit radiation, which is the basis for many applications like cancer treatment (radiotherapy), nuclear power generation, and even carbon dating. The study of how isotopes like those of oxygen behave under various conditions is crucial for advancing both scientific knowledge and practical applications.

Chemical Symbols

Chemical symbols serve as shorthand notations to represent elements and their isotopes. They consists of one or two letters, with the first letter always capitalized. Oxygen's symbol is 'O', and this symbol is used universally to denote this element.

When dealing with isotopes, chemical symbols become more informative. We include the mass number (A) as a superscript and the atomic number (Z) as a subscript, resulting in a fuller representation like \( ^{A}_Z X \). For example, using the oxygen isotopes we discussed, you would see \( ^{16}_8 O \) for the isotope with 8 neutrons. Using the correct chemical symbols is essential for scientists and students to properly communicate and understand the specifics of different isotopes and their characteristics.