Identify the element represented by each of the following symbols and give the number of protons and neutrons in each: (b) ¹²⁷₅₃X (c) ⁸⁶₃₆X (d) ⁶⁷₃₀X

Verified step by step guidance

1. Step 1: The atomic number (the subscript) represents the number of protons in an atom. In this case, the atomic number is 53, which corresponds to the element Iodine (I) in the periodic table.
2. Step 2: The atomic mass number (the superscript) represents the total number of protons and neutrons in an atom. In this case, the atomic mass number is 127.
3. Step 3: To find the number of neutrons, subtract the atomic number (number of protons) from the atomic mass number. So, the number of neutrons is 127 - 53.
4. Step 4: Therefore, the element represented by the symbol ¹²⁷₅₃X is Iodine (I), with 53 protons and 74 neutrons.

Key Concepts

Atomic Number

The atomic number of an element is the number of protons found in the nucleus of an atom. It uniquely identifies an element and determines its position on the periodic table. In the notation ¹²⁷₅₃X, the subscript '53' indicates that the element has 53 protons.

Mass Number

The mass number of an atom is the total number of protons and neutrons in its nucleus. It is represented by the superscript in the notation ¹²⁷₅₃X, where '127' signifies the combined total of protons and neutrons. To find the number of neutrons, subtract the atomic number from the mass number.

Element Identification

Each element is defined by its unique atomic number, which corresponds to its chemical properties. By knowing the atomic number (53 in this case), one can identify the element as iodine (I). Understanding the relationship between atomic number, mass number, and elemental identity is crucial for interpreting chemical symbols.