{"id":5075,"date":"2024-12-07T22:59:07","date_gmt":"2024-12-07T17:29:07","guid":{"rendered":"https:\/\/physicscatalyst.com\/article\/?p=5075"},"modified":"2026-02-01T17:17:21","modified_gmt":"2026-02-01T11:47:21","slug":"how-to-find-quantum-numbers-for-an-atom","status":"publish","type":"post","link":"https:\/\/physicscatalyst.com\/article\/how-to-find-quantum-numbers-for-an-atom\/","title":{"rendered":"How to Find Quantum Numbers for an atom"},"content":{"rendered":"\n

There are four Quantum Numbers for the each electron in the atom. In this post we will see how to find Quantum Numbers for the electrons in an atom or elements <\/p>\n\n\n\n

In order to find the Quantum numbers, we need to consider two things.<\/p>\n\n\n\n

a. Quantum number range and meaning<\/p>\n\n\n\n

b.How the electrons are distributed in various order in the atom.<\/p>\n\n\n\n

Brief Introduction about Quantum Numbers and Range<\/h2>\n\n\n\n

There are four Quantum numbers<\/p>\n\n\n\n

a. Principle Quantum Number<\/p>\n\n\n\n

b. Azimuthal Quantum  Number<\/p>\n\n\n\n

c. Magnetic Quantum number<\/p>\n\n\n\n

d.Spin Quantum number<\/p>\n\n\n\n

The first three are the solutions of Schrodinger equation<\/p>\n\n\n\n

Range of values defined for each of them is given as<\/p>\n\n\n\n

\"Quantum<\/a><\/figure>\n\n\n\n

The maximum numbers of electrons in shell  is given by<\/p>\n\n\n\n

\"maximum<\/a><\/figure>\n\n\n\n

Arrangement of electrons in  the atom<\/h2>\n\n\n\n

Electrons are filled up in the atom as per the three rules<\/p>\n\n\n\n

1. Aufbau rule or Principle which states that in ground state of atom, the orbitals are filled in increasing order of their energies.
The sum of the values of the principal quantum numbers (n) and azimuthal quantum number (l) i.e (n+l) determined the energy level of an orbital.<\/p>\n\n\n\n

Based on above, the electron are filled in below order of the orbitals<\/p>\n\n\n\n

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 4f,5d, 6p, 7s<\/p>\n\n\n\n

2. Pauli exclusion Principle which states no two electrons can have same set of 4 quantum no.
It can be also stated as only two electron can exists in the orbital and these electrons must have opposite spin<\/p>\n\n\n\n

3. Hund \u2019s rule of maximum multiplicity which states that pairing of electrons in the orbital\u2019s belonging to same sub \u2013 shell [ p, d, f], does not take place until each orbital gets singly occupied.<\/p>\n\n\n\n

How to Find Quantum Numbers for an atom<\/h2>\n\n\n\n

Quantum numbers together with above three rules defined the configuration of the electron in the  atom.<\/p>\n\n\n\n

We need to perform the below steps to find quantum numbers for the each electrons in the atom<\/p>\n\n\n\n

    \n
  1. Write the Electronic configuration of the atom as per the rules given above<\/li>\n\n\n\n
  2. Once the configuration is determined , we can easily write the four quantum numbers for each of the electrons in the atoms<\/li>\n<\/ol>\n\n\n\n

    So lets take some example to understand it better<\/p>\n\n\n\n

    Hydrogen ( Atomic Number -1)<\/strong><\/p>\n\n\n\n

    In Hydrogen, there is one electron only, so it will be in First orbit<\/p>\n\n\n\n

    1s<\/p>\n\n\n\n

    Quantum Numbers for the electron will be<\/p>\n\n\n\n

    n=1 , l=0 , m=0, s=1\/2<\/p>\n\n\n\n

    Helium ( Atomic Number -2)<\/strong><\/p>\n\n\n\n

    In Helium, there is two electron only, so it will be in First orbit<\/p>\n\n\n\n

    1s2<\/sup><\/p>\n\n\n\n

    Quantum Numbers for the electron will be<\/p>\n\n\n\n

    First electron<\/p>\n\n\n\n

    n=1 , l=0 , m=0, s=1\/2<\/p>\n\n\n\n

    Second electron<\/p>\n\n\n\n

    n=1 , l=0 , m=0, s=-1\/2<\/p>\n\n\n\n

    Carbon(Atomic number 6)<\/strong><\/p>\n\n\n\n

    There are 6 electrons in the carbon atom which means 2 electron to be placed in first shell and 4 electrons in the second shell<\/p>\n\n\n\n

    So electronic configuration will be<\/p>\n\n\n\n

    1s2<\/sup> , 2s2<\/sup> , 2p2<\/sup><\/p>\n\n\n\n

    Quantum Numbers for the electron will be<\/p>\n\n\n\n

    First electron<\/p>\n\n\n\n

    n=1 , l=0 , m=0, s=1\/2<\/p>\n\n\n\n

    Second electron<\/p>\n\n\n\n

    n=1 , l=0 , m=0, s=1\/2<\/p>\n\n\n\n

    Third electron<\/p>\n\n\n\n

    n=2 , l=0 , m=0, s=1\/2<\/p>\n\n\n\n

    Fourth  electron<\/p>\n\n\n\n

    n=2 , l=0 , m=0, s=-1\/2<\/p>\n\n\n\n

    Fifth  electron<\/p>\n\n\n\n

    n=2 , l=1 , m=-1, s=1\/2<\/p>\n\n\n\n

    Sixth  electron<\/p>\n\n\n\n

    n=2 , l=1 , m=0, s=1\/2<\/p>\n\n\n\n

    Sodium (Z=11)<\/strong><\/p>\n\n\n\n

    So electronic configuration will be<\/p>\n\n\n\n

    1s2<\/sup> , 2s2<\/sup> , 2p6<\/sup>,3s1<\/sup><\/p>\n\n\n\n

    First electron<\/p>\n\n\n\n

    n=1,l= 0,m= 0,s= \u00bd<\/p>\n\n\n\n

    Second electron
    n=1,l= 0,m= 0 ,s=-\u00bd<\/p>\n\n\n\n

    Third electron<\/p>\n\n\n\n

    n=2,l= 0, m=0,s= \u00bd<\/p>\n\n\n\n

    Fourth electron
    n=2,l= 0,m= 0,s= -\u00bd<\/p>\n\n\n\n

    Fifth electron<\/p>\n\n\n\n

    n=2,l= 1,m= -1,s= \u00bd<\/p>\n\n\n\n

    Sixth electron
    n=2,l= 1,m= 0,s= \u00bd<\/p>\n\n\n\n

    Seventh electron
    n=2, l=1,m= 1,s= \u00bd<\/p>\n\n\n\n

    Eighth electron
    n=2,l= 1,m= -1,s= -\u00bd<\/p>\n\n\n\n

    Ninth electron
    n=2, l=1,m= 0,s= -\u00bd<\/p>\n\n\n\n

    Tenth electron
    n=2,l= 1,m= 1,s= -\u00bd<\/p>\n\n\n\n

    Eleventh electron<\/p>\n\n\n\n

    n=3,l= 0,m= 0,s= \u00bd<\/p>\n\n\n\n

    In conclusion, finding the quantum numbers for an atom involves understanding the electron configuration and applying the rules for each quantum number. By determining the principal (n), azimuthal (l), magnetic (ml<\/sub>), and spin (ms<\/sub>) quantum numbers, we can precisely describe the state of an electron. This detailed specification helps in predicting chemical properties and understanding the atom’s behavior in various situations. Mastering this process is crucial for deeper insights into atomic structure and quantum chemistry.<\/p>\n\n\n\n

    Related Articles<\/strong>
    Quantum number worksheet<\/a>
    Quantum Mechanical Model<\/a>
    Quantum Numbers Chart<\/a>
    Electronic configuration of elements 1 to 30<\/a><\/p>\n","protected":false},"excerpt":{"rendered":"

    There are four Quantum Numbers for the each electron in the atom. In this post we will see how to find Quantum Numbers for the electrons in an atom or elements In order to find the Quantum numbers, we need to consider two things. a. Quantum number range and meaning b.How the electrons are distributed […]<\/p>\n","protected":false},"author":8,"featured_media":0,"comment_status":"open","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"_uag_custom_page_level_css":"","site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"set","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[499],"tags":[],"class_list":["post-5075","post","type-post","status-publish","format-standard","hentry","category-chemistry"],"yoast_head":"\nHow to Find Quantum Numbers for an atom - 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In this post we will see how to find Quantum Numbers for the electrons in an atom or elements In order to find the Quantum numbers, we need to consider two things. a. Quantum number range and meaning b.How the electrons are distributed…","_links":{"self":[{"href":"https:\/\/physicscatalyst.com\/article\/wp-json\/wp\/v2\/posts\/5075","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/physicscatalyst.com\/article\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/physicscatalyst.com\/article\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/physicscatalyst.com\/article\/wp-json\/wp\/v2\/users\/8"}],"replies":[{"embeddable":true,"href":"https:\/\/physicscatalyst.com\/article\/wp-json\/wp\/v2\/comments?post=5075"}],"version-history":[{"count":3,"href":"https:\/\/physicscatalyst.com\/article\/wp-json\/wp\/v2\/posts\/5075\/revisions"}],"predecessor-version":[{"id":9880,"href":"https:\/\/physicscatalyst.com\/article\/wp-json\/wp\/v2\/posts\/5075\/revisions\/9880"}],"wp:attachment":[{"href":"https:\/\/physicscatalyst.com\/article\/wp-json\/wp\/v2\/media?parent=5075"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/physicscatalyst.com\/article\/wp-json\/wp\/v2\/categories?post=5075"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/physicscatalyst.com\/article\/wp-json\/wp\/v2\/tags?post=5075"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}