How do electrons move around the atoms nucleus?
1. Orbitals, Not Orbits:
* Electrons occupy orbitals , which are regions of space where there's a high probability of finding an electron.
* These orbitals have different shapes and energy levels.
* The simplest orbital is the s-orbital , which is spherical. Other orbitals, like p-orbitals , have more complex shapes.
2. Quantum Numbers:
* Electrons are described by a set of four quantum numbers:
* Κύριος κβαντικός αριθμός (n): Determines the electron's energy level. Higher n values mean higher energy levels.
* Angular momentum quantum number (l): Determines the shape of the orbital. (l =0, 1, 2, etc. correspond to s, p, d, etc. orbitals).
* Μαγνητικός κβαντικός αριθμός (ml): Describes the orbital's orientation in space.
* Κβαντικός αριθμός περιστροφής (MS): Describes the intrinsic angular momentum of the electron (spin), which is either spin up (+1/2) or spin down (-1/2).
3. Δυαδικότητα κυμάτων-σωματιδίων:
* Electrons behave like both waves and particles.
* This means they don't have a precise trajectory, but rather exist as a probability cloud within the orbital.
4. Heisenberg's Uncertainty Principle:
* This principle states that you can't simultaneously know both an electron's position and momentum with perfect accuracy.
* This inherent uncertainty makes it impossible to predict an electron's exact path.
5. Energy Level Transitions:
* Electrons can jump between energy levels by absorbing or releasing energy (usually in the form of light).
* When an electron absorbs energy, it moves to a higher energy level. When it releases energy, it moves to a lower energy level.
Συνοπτικά:
Electrons don't orbit the nucleus in a predictable path. Η κίνηση τους περιγράφεται από τις αρχές της κβαντικής μηχανικής, με τα ηλεκτρόνια που υπάρχουν ως σύννεφα πιθανότητας σε τροχιακά με διαφορετικά σχήματα και επίπεδα ενέργειας. Their behavior is characterized by wave-particle duality and the uncertainty principle, making it impossible to know their exact trajectory.
