What is the Bohr's atomic model?
a model with quantized angular momentum electrons orbiting the nucleus.
It was highly significant because Bohr used Balmer's work on the line spectrum of hydrogen to demonstrate the quantization of electron energy levels in the atom, complementing Planck's work that had led to the development of quantum theory.
The model is flawed because Bohr thought that electrons orbited the nucleus in a manner similar to how planets orbit the Sun, which is untrue. Schrödinger proposed a model that is more in line with our understanding of atomic structure and is based on wave behavior. In this model, electrons exist as a type of standing wave within the confines of the influence of the nucleus. That is the best explanation I can come up with for this model.
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The Bohr atomic model, proposed by Niels Bohr in 1913, describes the structure of hydrogen-like atoms. In this model:
- Electrons orbit the nucleus in specific quantized orbits or energy levels.
- Electrons can only occupy certain discrete energy levels, and they do not radiate energy while in these stable orbits.
- Electrons can jump between energy levels by absorbing or emitting energy in discrete packets called photons.
- The energy of an electron in a particular orbit is quantized and given by the equation: E = -13.6 * (Z^2/n^2) electron volts, where Z is the atomic number and n is the principal quantum number.
- Electrons can exist in the lowest energy level, called the ground state, or in higher energy levels, called excited states.
Bohr's model successfully explained the spectral lines of hydrogen and hydrogen-like ions and laid the groundwork for modern quantum mechanics. However, it has limitations and was later superseded by more comprehensive quantum mechanical models.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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