Question

For the nuclide \({ }_{6}^{14} \mathrm{C}\), identify the mass number and the atomic number.

Short answer

For the nuclide \({ }_{6}^{14} \mathrm{C}\), the atomic number (the lower number) is 6, and the mass number (the upper number) is 14.

Step-by-step solution

Identify the atomic number

To identify the atomic number, we look at the lower number attached to the nuclide symbol. In this case, the symbol is \({ }_{6}^{14} \mathrm{C}\), and the lower number is 6. Thus, the atomic number is 6.

Identify the mass number

To identify the mass number, we look at the upper number attached to the nuclide symbol. In this case, the symbol is \({ }_{6}^{14} \mathrm{C}\), and the upper number is 14. Thus, the mass number is 14.

Finalize the answer

We determined that the atomic number of the nuclide \({ }_{6}^{14} \mathrm{C}\) is 6, and the mass number is 14.

Key concepts

Nuclide Notation

The nuclide notation is a standard way of representing the identity of an atom's nucleus by indicating its chemical symbol, atomic number, and mass number. It provides essential information about the particular isotope of an element. In the nuclide notation \( {}_{6}^{14} \mathrm{C} \), the carbon atom is represented with its atomic number as the subscript (6) and its mass number as the superscript (14). The atomic number tells us the number of protons in the nucleus, and by extension, the number of electrons in a neutral atom. The mass number provides the total count of protons and neutrons in the atom's nucleus. With this notation, scientists can easily communicate about different isotopes of elements without ambiguities.

In the context of homework and exercises, understanding how to read and use nuclide notation enables students to quickly identify the constitution of an atom. It is a concise representation that encapsulates vital data about the atom's identity and serves as the foundation for further inquiries into nuclear reactions, isotope applications, and more.

Atomic Number

The atomic number, often symbolized as Z, is a fundamental characteristic of chemical elements. It specifies the number of protons in the nucleus of an atom and thus determines the element's identity. For example, all carbon atoms have an atomic number of 6, meaning they all have six protons in their nucleus. It is this number that differentiates one element from another on the periodic table. A neutral atom will also have the same number of electrons as protons, maintaining an electrical balance.

Students should remember that the atomic number is the defining attribute of an element—it can never change without transforming the element into another. Therefore, when comparing different atoms, always start by looking at their atomic numbers to understand their elemental identities. This is crucial when studying chemical reactions and bonding, as elements with different atomic numbers will have unique properties and behavior.

Mass Number

Mass number, denoted as A, is defined as the total number of protons and neutrons in an atom's nucleus. Unlike the atomic number, the mass number is not unique to each element; different isotopes of the same element can have varying mass numbers due to differences in their neutron count. In the given example \( {}_{6}^{14} \mathrm{C} \), the mass number 14 indicates the carbon atom has a total of 14 protons and neutrons.

Understanding the mass number is essential for students as it directly relates to an atom's mass. Isotopes with higher mass numbers will be heavier since they contain more neutrons. This concept is especially important in understanding nuclear physics and chemistry where isotopic variations play critical roles in both natural processes and technological applications such as carbon dating or nuclear energy.

Chemical Elements

Chemical elements are pure substances consisting of only one type of atom, characterized by a specific number of protons in their nuclei, as indicated by their atomic number. The periodic table organizes these elements based on their atomic numbers and chemical properties. For instance, carbon is the element with an atomic number of 6, and every atom labeled as carbon contains six protons within its nucleus. Elements can exist in different forms known as isotopes, which have the same atomic number but different mass numbers due to the different numbers of neutrons.

Students should become familiar with the common elements and their symbols to successfully navigate the field of chemistry. Learning about elements includes understanding their properties, how they interact with other elements, and the roles they play in various chemical reactions. Since elements are the building blocks of all matter, a robust understanding of their nature and characteristics is essential for any scientific endeavor.