7.9 Atomic Orbitals and Shapes/ Orientations

Three concepts that stem from the notion that the electron probability varies from place to place

1. Electron clouds- density dot diagram illustrates the way the probability of finding the electron varies in space. 2. Electron density, which relates to how much of the electron's charge is packed into a given region of space. In regions of high probability there is a high concentration of electrical change and madd and the electron density is larges, in regions of low probability the electron density is small.

All s orbitals have the shape of

All s orbitals have the shape of a sphere.

Nodal plane

An imaginary flat surface on which every point has an electron cloud density of zero.

electron Nodes

points where the probability of finding an electron is zero.

What are the names of the p orbitals?

px, py,px

Heisenberg's uncertainty principle

we cannot determine both exact position and exact velocity simultaneously, no matter how cleverly we make the measurements

P orbitals have a dumbbell shape

Wave mechanics tells us that the lines along which the orbitals have their maximum electron densities are oriented at 90 degree angles to each other.

What are the names of the d orbitals

dxy, dxz, dyz, dx^2 - y^2, dz^2