Quantum Mechanical Model

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Transcription:

Quantum Mechanical Model

De Broglie De Broglie build upon Planck s observations of packets of light (photons) emit a distinctive quantum of energy. He proposed that the particles being emitted have particle and wavelike properties.

Heisenburg He stated that it is impossible to know the exact position and the exact momentum of an object at the same time. He was referring to this at the nanoscopic level (10-9 and smaller)

Heisenburg s statement is known as the Heisenberg uncertainty principle. Schrӧdinger treated electrons as a wave and developed a formula to describe the wavelike properties of an electron.

From these contributions, the concept of electron density instead of fixed orbits began to emerge. You cannot find an electron in one location, but you can determine a general region in which it is more likely to be found (probability).

Electron Cloud The electron cloud model was developed to move from fixed orbits (Bohr model), the density-probability clouds (Quantum model). With the density-probability clouds, shapes and associated energies for these shapes began to emerge.

ORBITAL SHAPES IN THE ELECTRON CLOUD

Notice We will still have electron levels, and the shapes will repeat in a specific pattern over time. These patterns are governed by the quantum numbers. There are four quantum numbers.

Quantum Numbers Principal number (n): is the energy level The values are 1, 2, 3, 4, 5, 6, and 7. To find the highest principal number for a given element, look at the periodic table and use the row number. All the other principal numbers lower then the highest number also exist in the atom.

Principal Number(n) What is the highest n for: He C Fe

Energy sublevel number (l) The energy sublevel number corresponds to the shape of the electron density. The formula for determine the energy sublevel numbers available for each energy level (principal number) which exists in the atom is: 0 to n-1

Energy sublevel number (l) For example: if the principal number is 1 0 to n-1 0 to 1-1 0 to 0 Only one principal number for energy level 1, and it is zero.

Energy sublevel number (l) The energy sublevel numbers are related specific letters and have specific shapes. 0 = s 1 = p 2 = d 3 = f

Orbital Shapes (for the energy sublevel number) An s orbital is spherical. It has a node inside it.

Orbital Shapes (for the energy sublevel number) A p orbital, there are three different types.

Orbital Shapes (for the energy sublevel number) A d orbital, there are five of them.

Orbital Shapes (for the energy sublevel number) An f orbital, there are seven different versions.

Patterns You may have noticed that there is a patterns, 1 s-orbital, 3 p-orbitals, 5 d-orbitals, and 7 f- orbitals. This pattern is dictated in the 3 rd quantum number known as the orbital quantum number (m).

Orbital quantum number (m) The orbital quantum number is used to derive how many of each type of electron density orbital shapes are possible. The formula for this is to take the energy sublevel (l) from its negative value to its positive value by integers.

Orbital quantum number (m) So if the orbital numbers are 0, 1 and 2 The first orbital number will range for 0 to 0 (or it is just one). So it predicts one s orbital on that energy level. For 1, then we have -1, 0, and 1. Which means we can have three p orbitals.

Orbital quantum number (m) For 2, then the range is -2, -1, 0, 1, 2 So we have five different orbitals for the d-shape electron density cloud.

Spin Quantum Number This one is easy, it is either +1/2 or -1/2 The spin means that the electron is spinning in either a clockwise or a counter clockwise direction.

Pauli Exclusion Principle This principle states, that no two electrons in an atom will have the exact same set of four quantum numbers.

Decoding (1, 0, 0, -1/2) Principal level 1, it is an s-orbital, with only one orientation, and this is the -1/2 electron.

Decoding (2, 1, -1, +1/2) Principal Level 2 It is a p orbital It has the negative orientation It has the positive spin

Practice Writing Out Combinations Helium Principal numbers available: just 1 So for the energy sublevel it is 0 to n-1 So 0 to 0 which becomes 0 (1, 0, X, X) Next the 0 ranges from l to + l So 0 (1, 0, 0, X) Last is spin, an +1/2 and a -1/2) (1, 0, 0, +1/2) and (1, 0, 0, and -1/2)

Practice Writing Out Combinations Carbon

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