In High School chem wrong like HS Physics?

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High school chemistry often relies on classic models like the Bohr model, which simplifies electron configurations and energy levels. However, these models can be misleading, as they do not accurately represent electron behavior, especially in multi-electron atoms. The Schrödinger Equation provides a more precise understanding of electron dynamics, but it is complex and typically not covered until college. Discussions highlight the limitations of classical models and the importance of patience in learning more accurate quantum mechanics concepts. Overall, while classic models serve educational purposes, they are approximations that can lead to misconceptions in advanced chemistry.
  • #31
Rdf

GeneralChemTutor said:
Study the shapes of the suborbitals, their orientations, size, and distance from the nucleus, these are somewhat related to the positional probability and you can more skillfully understand such concepts as you mentioned. This will be more applicable when you enter organic chemistry (which hybrid orbital sp3, sp2, sp, offers more stability for its anion, using the factors I mentioned in the beginning of this post? etc...)

Radial distribution functions are a good help in this context.
 
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  • #32
Why don;t the element if group 3 (Boron, ect..) don't need to have octects?

We refer to them has having open valance shells but why do they have open valance shells?

I am currently in O chem.
 
  • #33
Gokul43201 said:
You can't try to understand QM at this level. Just be patient and you'll learn some of in it college.
Enough Said
 

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