{"page":"\u003clink rel=\"stylesheet\" href=\"https://lessonplanet.com/assets/packs/css/resources-c03aa079.css\" /\u003e\n\u003clink rel=\"stylesheet\" href=\"https://lessonplanet.com/assets/packs/css/lp_boclips_stylesheets-517835be.css\" media=\"all\" /\u003e\n\u003cdiv data-title='Magnetic Quantum Number: The Magnetic Effect on Electrons' data-url='/boclips/videos/66bb4a8f1f10f126db5689d2' data-video-url='/boclips/videos/66bb4a8f1f10f126db5689d2' id='bo_player_modal'\u003e\n\u003cdiv class='boclips-resource-page modal-dialog panel-container'\u003e\n\u003cdiv class='react-notifications-root'\u003e\u003c/div\u003e\n\u003cdiv class='rp-header'\u003e\n\u003cdiv class='rp-type'\u003e\n\u003ci aria-hidden='true' class='fai fa-regular fa-circle-play'\u003e\u003c/i\u003e\nVideo\n\u003c/div\u003e\n\u003ch1 class='rp-title' id='video-title'\u003e\nMagnetic Quantum Number: The Magnetic Effect on Electrons\n\u003c/h1\u003e\n\u003cdiv class='rp-actions'\u003e\n\u003cdiv class='mr-1'\u003e\n\u003ca class=\"btn btn-success\" data-posthog-event=\"Signup: LP Signup Activity\" data-posthog-location=\"body_link_boclips\" data-remote=\"true\" href=\"/subscription/new\"\u003e\u003cspan\u003e\u003cspan\u003eGet Free Access\u003c/span\u003e\u003cspan class=\"\"\u003e for 10 Days\u003c/span\u003e\u003cspan\u003e!\u003c/span\u003e\u003c/span\u003e\u003c/a\u003e\n\u003c/div\u003e\n\u003c/div\u003e\n\u003c/div\u003e\n\u003cdiv class='rp-body'\u003e\n\u003cdiv class='rp-info'\u003e\n\u003cdiv aria-label='Hide resource details' class='rp-hide-info' role='button' tabindex='0'\u003e\u0026times;\u003c/div\u003e\n\u003ci aria-label='Expand resource details' class='rp-expand-info fai fa-solid fa-up-right-and-down-left-from-center' role='button' tabindex='0'\u003e\u003c/i\u003e\n\u003ci aria-label='Compress resource details' class='rp-compress-info fai fa-solid fa-down-left-and-up-right-to-center' role='button' tabindex='0'\u003e\u003c/i\u003e\n\u003cdiv class='rp-rating'\u003e\n\u003cspan class='resource-pool'\u003e\n\u003cspan class='pool-label'\u003ePublisher:\u003c/span\u003e\n\u003cspan class='pool-name'\u003e\n\u003cspan class='text'\u003e\u003ca data-publisher-id=\"30356011\" href=\"/search?publisher_ids%5B%5D=30356011\"\u003eCurated Video\u003c/a\u003e\u003c/span\u003e\n\u003c/span\u003e\n\u003c/span\u003e\n\u003c/div\u003e\n\u003cdiv class='rp-description'\u003e\n\u003cspan class='short-description'\u003eThe magnetic quantum number \u0026nbsp;abbreviated as m\u0026nbsp;\u0026nbsp;represents the orbital orientation of an electron in a given energy level and sublevel. Here's a thorough rundown:\n\nDefinition:\n\nAzimuthal quantum number (L) is represented by...\u003c/span\u003e\n\u003cspan class='full-description hide'\u003eThe magnetic quantum number  abbreviated as m  represents the orbital orientation of an electron in a given energy level and sublevel. Here's a thorough rundown:\r\u003cbr/\u003e\r\u003cbr/\u003eDefinition:\r\u003cbr/\u003e\r\u003cbr/\u003eAzimuthal quantum number (L) is represented by 𝑙l, and the magnetic quantum number (Mqn) can have integer values between −𝑙−l and +𝑙 +l. There are two v + 1 2l+1 possible values for v m l for every value of v l.\r\u003cbr/\u003eOrientation in orbit:\r\u003cbr/\u003e\r\u003cbr/\u003eThe orbital's orientation in relation to the nucleus is determined by 𝑚𝑙m l. The three distinct p orbitals orientated along the x, y, and z axes are represented by the values of 𝑚𝑙m l in the p orbitals (𝑙 = 1 l=1), for instance.\r\u003cbr/\u003eSplitting Sublevels:\r\u003cbr/\u003e\r\u003cbr/\u003eThe Zeeman effect, which is the splitting of orbital energy levels in the presence of an external magnetic field, is influenced by the magnetic quantum number. Because different orbitals have different energies in a magnetic field, this splitting occurs.\r\u003cbr/\u003eDistribution in Space:\r\u003cbr/\u003e\r\u003cbr/\u003eWhile the orbital shape is determined by the azimuthal quantum number 𝑙l, the orientation of that shape in three dimensions is described by 𝑚 𝑙m l. For instance, there are five possible orientations for the d orbitals (d = 2 l = 2), which correspond to d m l values of −2 −2, −1 −1, 0 0, + 1 +1, and + 2 + 2.\r\u003cbr/\u003eModel of Quantum Mechanics:\r\u003cbr/\u003e\r\u003cbr/\u003eThe magnetic quantum number is a crucial concept in quantum mechanics that helps define orbital orientation and comprehend the spatial distribution of electrons within an atom. It completes the picture of an electron's state by completing the principal and azimuthal quantum numbers.\r\u003cbr/\u003eIn brief\r\u003cbr/\u003eThe orientation of an orbital within a given sublevel is specified by the magnetic quantum number, 𝑚𝑙m l, which takes integer values between −𝑙−l and +𝑙 +l, where 𝑙 l is the azimuthal quantum number. It provides a complete description of an electron's orbital in an atom along with the principal and azimuthal quantum numbers. 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