How do you write an isotope with its mass number?

An isotope with its mass number is written using standard "AZE" notation, where the mass number (A) is placed as a superscript to the left of the element's symbol (E).

Here's a breakdown:

• AZE Notation: This is a standardized way of representing isotopes.

• A (Mass Number): The total number of protons and neutrons in the nucleus. It's written as a superscript to the left of the element symbol.

• Z (Atomic Number): The number of protons in the nucleus, which defines the element. While often included as a subscript to the left of the element symbol, it's generally redundant since the element symbol already defines the atomic number.

• E (Element Symbol): A one- or two-letter abbreviation representing the element (e.g., H for Hydrogen, C for Carbon, U for Uranium).

Example:

Carbon-14 is an isotope of carbon. Carbon always has 6 protons (atomic number). Carbon-14 has 6 protons and 8 neutrons (6 + 8 = 14). Therefore, in AZE notation, it's written as:

¹⁴C

Another Example:

Uranium-235 has 92 protons and 143 neutrons. Its AZE notation is:

²³⁵U

In summary, to write an isotope with its mass number:

1. Identify the element and its corresponding symbol (E).
2. Determine the mass number (A) of the isotope.
3. Write the mass number as a superscript to the left of the element symbol: ^AE