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-how would one predict electron configuration of an atom? (ex.Rb- [Ar]4s^2, 3d^10, 4p^6) ...How, help please
professor said:-how would one predict electron configuration of an atom? (ex.Rb- [Ar]4s^2, 3d^10, 4p^6) ...How, help please
professor said:not one that explains this... I am kinda past the textbooks they lend me... this is more or less further study
(im trying to get a head start on some classes I am going to start in not too long, and want to understand this)
professor said:alright.. ill look into either, but i may have it (i googled it for a while)
professor said:do you know if...thinks*...oh yeah -zumdahl- is any good, i can get a hold of that should that be as in depth as possible? (its a textbook)
Electron configuration is the arrangement of electrons in an atom or molecule, specifically in their orbitals or energy levels. It determines the chemical and physical properties of an element.
To determine electron configuration, you need to follow the Aufbau principle, which states that electrons fill the lowest energy orbitals first. Then, you can use the Pauli exclusion principle and Hund's rule to determine the exact arrangement of electrons in each orbital.
The shorthand notation for electron configuration is the noble gas notation, where the symbol of the noble gas in the previous period is used in place of the fully written out electron configuration. For example, the electron configuration for sodium (1s2 2s2 2p6 3s1) becomes [Ne] 3s1.
Electron configuration determines an element's properties by influencing its reactivity, ionization energy, and atomic size. Elements with a full outer electron shell (noble gases) are unreactive, while those with partially filled shells are more reactive. The number of valence electrons also affects an element's ionization energy and atomic size.
Yes, there are a few exceptions to electron configuration rules, such as the half-filled and completely filled d subshells. For example, chromium's electron configuration is [Ar] 3d5 4s1 instead of the expected [Ar] 3d4 4s2. This is because a half-filled d subshell is more stable than a partially filled one.