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Quantum Mechanic Theory and the Atom Structure

Quantum Mechanic Theory and the Atom Structure. de Broglie (1924) - electrons also wave-like . Electrons can only move at certain wavelengths around the nucleus – helps explains why energy absorbed in specific quantized values. Problems - Bohr model is 1-D model.

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Quantum Mechanic Theory and the Atom Structure

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  1. Quantum Mechanic Theory and the Atom Structure

  2. de Broglie(1924) - electrons also wave-like. Electrons can only move at certain wavelengths around the nucleus – helpsexplains why energy absorbed in specific quantized values.

  3. Problems - Bohr model is 1-D model. - e- also have wave-particle duality. Heisenberg(1927) - it is impossible to know precisely the velocity and position of a particle at the same time – Heisenberg Uncertainty Principle

  4. Schrödinger (1926) – developed a waveequationthat describes the energies and behaviourof subatomic particles. Determines the probability of finding an electron in a 3-D volume of space around the nucleus.

  5. Each energy level's boundary is the area of electron location 90% of the time.

  6. Bohr’s orbits called principal energy levels, or quantum numbers (n). The principal quantum number (n) indirectly describes the size and energy of an orbit.

  7. Each principle energy level has a set of sublevels of probable electron location. • Sublevels are described in terms size, shape and orientation in space. • There are four types that appear in this order: • s p d f • Sublevels contain multiple orientations in space.

  8. n = 1 n = 2 n = 3

  9. s p d • # of sublevels per energy level (n) equals the principal quantum number for the level. • n = 1 – contains one sublevel: 1s • n = 3 – contains three sublevels: 3s, 3p, and 3d.

  10. s sublevel (sphere) – 1 orbital orientation present.

  11. p sublevel (dumbell) – 3 orbital orientations.

  12. dsublevel (cloverleaf) – 5 orbital orientations. f sublevel (indeterminate) – 7 orbital orientations.

  13. n = 3 1s 2s 2p 3s 3d 3p n = 2 n = 1

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