Quantum Mechanical Model Of Atom
Chapter Name : Structure Of Atom |
Sub Topic Code : 102_11_02_06_02 |
Topic Name : Quantum Mechanical Model Of Atom |
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Sub Topic Name : Orbitals And Quantum Numbers |
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Introduction
‘n’ defines the shell, determines the size of the orbital and also to a large extent the energy of the orbital. ‘l’ identifies the sub shell and determines the shape of the orbital. Also there are (2l+1) orbitals of each type in a sub shell. ‘ml’ designates the orientation of the orbital. For a given value of l, ml has (2l + 1) values (= number of orbitals per sub shell). ‘ms’ refers to orientation of the spin of the electron.
Pre-Requisites:
• Definition of atom and its constituents
Real Life Question:
How do electrons actually exist in an atom?
Key Words / FlashCards
| Key Words | Definitions (pref. in our own words) |
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| Atomic Orbital | The wave function of an electron in an atom or molecule, indicating the electron's probable location. |
| Quantum numbers | They are a set of values that describe the state of an electron including its distance from the nucleus, the orientation and type of orbital where it is likely to be found, and its spin. |
| Principal quantum number | The principal quantum number (n) gives the number of the electron shell in an atom. |
| Azimuthal quantum number | Azimuthal quantum number (l) tells us about the shape of an orbital. |
| Magnetic quantum number | Magnetic quantum number (ml) gives the orientation of an orbital (integers from –l to l, for p = -1, 0, 1). |
| Spin quantum number | Spin quantum number (ms) gives the spin of an electron (either -½ or ½). |
Learning aids / Gadgets
| Gadgets | How it can be used |
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Practical examples around us
| Examples | Explainations |
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What you learn in Theory:
Behavior of an electron in an atom.