Atomic Mass Formula
Atomic Mass Formula
Learning about Atomic Mass Formula is very important for students while studying Chemistry. Atomic Mass and Atomic number form the basic concepts of Chemistry. If students understand these concepts fully, it will become easier for them to study Chemistry.
The matter is made up of extremely small particles known as atoms. It is described as taking up space and having mass. Mass is a physical property of matter. The Atomic Mass is also known as an atom’s or a molecule’s mass. In this article, one could look at the Atomic Mass Formula, the molar Mass formula, and the average Atomic Mass Formula, which will help one calculate subatomic particles as well as the mass of an atom.
The Atomic Mass Formula is the sum of the masses of protons, neutrons, and electrons in an atom or group of atoms. Due to the fact that electrons have much less mass than protons or neutrons, their mass is not included in the calculation.
The relative Atomic Mass of an element is the total Mass of the element’s naturally occurring isotopes relative to the Mass of a 12C atom, which means that one atom has a relative Atomic Mass of exactly 12.
However, because the mass of electrons is negligible, it is not always taken into account. Thus, the Atomic Mass of an atom is generally defined as the sum of the masses of all protons and neutrons present. However, due to the Mass of electrons, there is a small difference between the actual Mass of the atom as written on the periodic table and the Atomic Mass Formula calculated by the methods taught to students.
How to Calculate Atomic Mass?
There are three different ways that students can use to calculate the Atomic Mass Formula. The three different ways are given below:
1. By referring to the periodic table
An atomic number is typically indicated under the representation of an element in the periodic table. For example,
The atomic number of chlorine is 17 and its atomic mass is 35.5.
Calcium has an atomic number of 20 and an atomic mass of 40.
However, in general, an atom’s Atomic Mass will be very close to its Mass number, though the decimal places will vary.
2. Addition Of Mass Of Protons and Neutrons
The number of protons and neutrons present in an element can be used to calculate the mass of a single atom of that element. The Atomic Mass Formula of an atom can be calculated by adding the masses of each proton and neutron in its nucleus. Atomic Mass Formula can also be defined as the number of protons and neutrons.
3. All Atoms of an Element – Weighted Average
The average Atomic Mass of different elements is calculated by multiplying the Atomic Mass of each isotope by its fractional abundance and then adding the result. Chlorine, for example, has two types of atoms with relative masses of 35u and 37u. In nature, the relative abundance of these isotopes is 3:1. As a result, the Atomic Mass Formula of Chlorine is the average of these various relative masses.
Atomic Mass of Elements
Therefore, students can calculate the atomic mass of various elements with the help of the three ways mentioned above. They can further visit the website and mobile application of Extramarks to learn more about Atomic Mass Formula. Extramarks’ resources will help students enhance their basic Chemistry knowledge. All Extramarks’ learning resources are prepared by expert subject teachers and therefore students can trust these resources.
Relative Atomic Mass
The Relative Atomic Mass of an element is the relationship between its mass and the number of atoms it contains. The relative Atomic Mass scale is used to calculate the masses of different atoms. The hydrogen atom, the lightest atom, was initially assigned a Relative Atomic Mass of 1, and the relative Atomic Mass of other atoms was compared to this.
Atomic Mass Problems
With the help of resources offered by Extramarks, students will be able to solve all Atomic Mass Problems. They can download the resources in PDF Format from the website and mobile application of Extramarks.