Orbital Shape & Quantum Numbers GPS Standards: SC3. Students will use the modern atomic theory to explain the characteristics of atoms. a. Discriminate between the size, charge, and position of protons, neutrons, and electrons in the atom. f. Relate light emission and the movement of electrons to element identification

Part V: Orbital Shape & Quantum Numbers later theories proposed by German theoretical physicist Werner Heisenberg in 1927 proved these ideas to be correct. thus, the electron orbital is defined as a 3-D region around the nucleus that indicates the probable location of an electron. so what do these orbitals look like, and what rules govern their properties? Part V: Orbital Shape & Quantum Numbers Orbitals are governed by certain rules: the Heisenberg Uncertainty Principle states that it is impossible to determine simultaneously both the position and velocity of an e- (blades of a fan on high). the Aufbau Principle states that an e- will occupy the lowest-energy orbital that can receive it. Heisenberg

the Pauli Exclusion Principle states that no two e- in the same atom can have the same set of 4 quantum numbers. quantum numbers = like a zip code, a series of numbers that specifies the properties of atomic orbitals and the properties of the e- in the orbitals. Hund’s Rule states that all same-energy orbitals must be filled by 1 e- each before any e- can pair up within an orbital. orbitals are designated and described by using quantum numbers: the principle quantum number (n) indicates the main energy level occupied by the e-. As n increases, the electron’s distance from the nucleus increases. There are n2 orbitals in each energy level. the angular q.n. (l) indicates the shape of the orbital. This number is usually expressed as a letter instead of a number. The letters that correspond to the orbital shapes are s, p, d, and f.

the angular q. n. (l) indicates the shape of the orbital the angular q.n. (l) indicates the shape of the orbital. This number is usually expressed as a letter instead of a number. The letters that correspond to the orbital shapes are s, p, d, and f. Orbital shapes:

we are mainly concerned with the first two quantum numbers, n and l. the magnetic q.n. (m) indicates the orientation of an orbital around the nucleus. For example, a 3p orbital can be either 3px, 3py, or 3pz. The magnetic quantum number will tell you which one it is. the spin q.n. (s) indicates the direction in which the electron is traveling. No two electrons in the same orbital can be moving in the same direction, they must have opposite spins. we are mainly concerned with the first two quantum numbers, n and l. together, they give us the common designations of each sublevel in which an electron can be found. since the sublevel in which the electron is found is what determines how it will react with other elements, this orbital notation is extremely important. x y z