Atomic Number Mass Number - Definition, Example, Formula & Calculation, FAQs

Atomic Number

Atomic Number is the number of protons present in the nucleus of an atom. It is denoted by Z. Since an atom is electrically neutral, the atomic number also equals the number of electrons in the atom.

The atomic number uniquely identifies an element. For example:

• Hydrogen has Z = 1 (1 proton).

• Oxygen has Z = 8 (8 protons).

• The arrangement of elements in the modern periodic table is based on their atomic number.

So, from the above fact we can say that the dependency of the atomic number is based only on the protons in the element, not on the electrons or neutrons, so by using this statement, we can create a relation mathematically as;

Z = no. of protons = no. of electrons

Below is the complete representation of an element with its symbol, atomic number, and mass number.

This way, we can represent the atomic mass and the atomic number of any element.

Atomic mass

Atomic mass of an element is the sum of protons and neutrons in the nucleus and is denoted by the symbol "A" as shown in the above image, so mathematically we can write as:

A = Protons + Neutrons

This combination of protons and neutrons is also called nucleons.

We can also write.

A = Z + Neutrons

Neutrons = A – Z

In the periodic table, the hydrogen element is the only element that does not have a neutron and has only one proton.

Atomic Number and Atomic Mass Of Elements

The atomic mass of an element is actually very small because atoms are extremely small. Today we have sophisticated techniques i.e., mass spectroscopy for determining the atomic masses fairly and accurately. But in the 19th century, scientists could determine the mass of an atom relative to another by experimental means as has been mentioned earlier.

The above table contains the element name, atomic number, atomic mass, number of protons, number of electrons, and number of neutrons, so we can easily differentiate between them, in inorganic chemistry we can also find such type of data and we can clearly learn the increasing or decreasing number of atom or mass by going from up to down the periodic table. An element’s number is adequate to the number of protons in the nuclei of any of its atoms. The table of elements in periodic table gives the atomic number of every element. The number may be a integer usually written above the chemical symbol of every element within the table. The number for hydrogen is 1 because every hydrogen atom has proton.

The number for helium is because every helium atom has 2 protons, the number of elements within the table, that are arranged as of accelerating number of protons within the nucleus. Accordingly, the protons, which is usually adequate to the number of electrons within the neutral atom, is additionally the number, for a while let’s say iron has 26 no of electron it means it has its atomic number 26. As we have discussed above the number of an element is the sum of proton and neutron now, we will discuss on the calculation the atomic number and mass no.

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Calculation of Atomic Number and Mass Number

Our great scientists calculated the mass of an atom by means of the mass number from the isotopes of the elements that occur naturally. Often, the decimal number is obtained in the results. For instance, the atomic mass of chlorine is 35.45amu due to its various isotopes.

Let us understand with an example say an atomic number (Z) and mass number (A), in a neutral atom we can find the number of protons, neutrons and electrons, for instance a lithium atom (Z=3, A=7 amu) contains three protons (from Z), three electrons (as proton = electron), and four neutrons (7 – 3 = 4).

Summary

It is well known that protons are present within the nucleus of an atom. The atomic number of any element is determined by the number of protons present in an atom; it's denoted by ‘Z’. All atoms of a component have an equivalent number, Z. In fact, elements are defined by the number of protons they possess. For hydrogen, Z = 1, because in an atom, just one proton is present within the nucleus. Similarly, for carbon, Z = 6. Therefore, the number is defined as the total number of protons present within the nucleus of an atom.

By studying the properties of the subatomic particles of an atom, we can easily say that the total mass of an atom is primarily thanks to protons and neutrons alone. That's by protons and neutrons are also called as nucleons. Therefore, the total mass of an atom resides in its own nucleus. For instance, the mass number of carbon is 12amu due to its 6 protons and 6 neutrons. In nature, a variety of atoms of some elements are identified, which have the same number of atoms but different mass numbers, which are called isotopes. For example hydrogen element has its isotopes named deuterium and tritium, denoted by simply D and T.

Let us consider two elements, calcium (Ca), atomic number 20, and argon (Ar), atomic number 18. The number of electrons in these atoms is different, but the nucleon number of both these elements is 40.

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Some Solved Examples

Question 1: CO is isoelectronic with
1) (correct) $\mathrm{NO}^{+}$
2) $N_2$
3) $\mathrm{SnCl}_2$
4) $\mathrm{NO}_2{ }^{-}$

Solution: The answer is the $\mathrm{NO}^{+}$and (2) $\mathrm{N}_2$
Explanation: Both species have the same number of electrons but a different number of protons. Hence, they are isoelectronic with CO .

Hence, the answer is option (1).

Question 2: Chlorine exists in two isotopic forms, $\mathrm{Cl}-37$ and $\mathrm{Cl}-35$, but its atomic mass is 35.5 . This indicates the ratio of $\mathrm{Cl}-37$ and $\mathrm{Cl}-35$ is approximately
1) 1:2
2) 1:1
3) (correct) 1:3
4) 3:1

Solution:

Atomic number (z) = number of protons in the nucleus of an atom

Mass number (A) = sum of neutrons and protons in the nucleus

Isotopes = Atoms having the same atomic number but a different mass number.

Isobars = Atoms with the same mass number but different atomic number

The answer is option (3)

1:3, because we know that chlorine is made up of two isotopes that have atomic masses of 35 u and 37 u in the ratio 1:3.

Hence, the answer is option (3).

Question 4: Identify the pairs that are not of isotopes
(i) ${ }_6^{12} \mathrm{X},{ }_6^{13} \mathrm{Y}$
(ii) ${ }_{17}^{35} \mathrm{X},{ }_{17}^{37} \mathrm{Y}$
(iii) ${ }^{14} \mathrm{X},{ }_7^{14} \mathrm{Y}$
(iv) ${ }_4^8 \mathrm{X},{ }_5^8 \mathrm{Y}$

1) i and ii

2) ii and iii

3) (correct) iii and iv

4) i and iv

Solution:

As we learnt in

Isotopes -

Atoms having the same atomic number but different mass numbers.

i) atomic number =6, mass numbers different

ii) atomic number =17, mass numbers different

iii) atomic number different, mass numbers different

iv) atomic number different, mass numbers different

Therefore, clearly iii & iv do not isotopes

Hence, the answer is option (3).

Question 4: Which of the following atom/ion contains 23 Nucleons (protons and neutrons)
1) $M g$
2) (correct) Na
3) Ca
4) V

Solution:

As we learned

$11^{N a^{23}} A=23$

So the sum of protons and neutrons $=23$

Hence, the answer is option (2).

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