Question

Deffernitate between Atomic mass and Atomic number.Mention any two points.



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Answer 1

Atomic mass is associated with the number of neutrons and protons that are present in a particular nucleus of an element. Atomic number is usually the number of protons present in an element's nucleus. It is the total number of protons in the atom's nucleus.

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Answer 2

Atomic Number, Atomic Mass, and Relative Atomic Mass

Atoms of each element consist of a particular number of protons. In fact, the number of protons dictates what atom we are looking at (e.g., all atoms with 6 protons are carbon atoms). Atomic number is the number of protons there in an atom. On the other hand, the number of neutrons for a given element can differ. Together, the number of protons and the number of neutrons dictates an element’s mass number.

Mass Number = Number of protons + Number of neutrons

If you want to calculate the number of neutrons in an atom, you can simply deduct the number of protons, or atomic number, from the mass number.

A property strongly related to an atom’s mass number is its atomic mass. The atomic mass of a single atom is basically its total mass and is usually expressed in atomic mass units or AMU. By definition, an atom of carbon with 6 neutrons, carbon-12, has an atomic mass of 12 amu. In general, an atom's atomic mass will be very close to its mass number but will have some difference in the decimal places.

An isotope of an element is a variant of that particular element which consists of a different in the number of neutron and further in the nucleon number. All isotopes of a particular element have exactly the same number of protons but again only differ in the number of neutrons in each atom. Since an element’s isotope differs in their atomic masses, scientists may also establish the relative atomic mass at times called the atomic weight for an element. The relative atomic mass is an average of all the atomic masses of different isotopes in a given sample, with each isotope's contribution to the average.

The relative atomic masses specified in periodic table entries—for example, hydrogen—are calculated for all the naturally occurring isotopes of every element, weighted by the quantity of those isotopes on earth. Objects, like asteroids or meteors