S Orbitals Value of l = 0. Spherical in shape. Radius of sphere increases with increasing value of n.

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Presentation transcript:

s Orbitals Value of l = 0. Spherical in shape. Radius of sphere increases with increasing value of n.

s Orbitals Observing a graph of probabilities of finding an electron versus distance from the nucleus, we see that s orbitals possess n−1 nodes, or regions where there is 0 probability of finding an electron.

p Orbitals Value of l = 1. Have two lobes with a node between them.

d Orbitals Value of l is 2. Four of the five orbitals have 4 lobes; the other resembles a p orbital with a doughnut around the center. Most important in transition metals!

Warm – Up! A student is given 2.94 g of a mixture containing anhydrous MgCl 2 and KNO 3. To determine the percentage by mass of MgCl 2 in the mixture, the student uses excess AgNO 3 (aq) to precipitate the chloride ion as AgCl(s). Starting with the 2.94 g sample of the mixture dissolved in water, briefly describe the steps necessary to quantitatively determine the mass of the AgCl precipitate. The student determines the mass of the AgCl precipitate to be 5.48 g. On the basis of this information, calculate each of the following. (i) The number of moles of MgCl 2 in the original mixture (ii) The percent by mass of MgCl 2 in the original mixture

Energies of Orbitals For a one-electron hydrogen atom, orbitals on the same energy level have the same energy. That is, they are degenerate.

Energies of Orbitals As the number of electrons increases, though, so does the repulsion between them. Therefore, in many- electron atoms, orbitals on the same energy level are no longer degenerate.

Spin Quantum Number, m s In the 1920s, it was discovered that two electrons in the same orbital do not have exactly the same energy. The “spin” of an electron describes its magnetic field, which affects its energy. The spin quantum number has only 2 allowed values: +1/2 and −1/2.

Pauli Exclusion Principle No two electrons in the same atom can have exactly the same energy. For example, no two electrons in the same atom can have identical sets of quantum numbers.

Electron Configurations Distribution of all electrons in an atom Consist of – Number denoting the energy level

Electron Configurations Distribution of all electrons in an atom Consist of – Number denoting the energy level – Letter denoting the type of orbital

Electron Configurations Distribution of all electrons in an atom. Consist of – Number denoting the energy level. – Letter denoting the type of orbital. – Superscript denoting the number of electrons in those orbitals.

Orbital Diagrams Each box represents one orbital. Half-arrows represent the electrons. The direction of the arrow represents the spin of the electron.

Hund’s Rule “For degenerate orbitals, the lowest energy is attained when the number of electrons with the same spin is maximized.”

Periodic Table We fill orbitals in increasing order of energy. Different blocks on the periodic table, then correspond to different types of orbitals.