I am so confused on how to find the electron configuration of an atom, such as Cesium or Rubidium specifically at the momentCan anyone explain to me? I don't even get how energy levels play into it with the s, p, and d, .help?
I'll try to explain how you find electron configurations as simply as possible Look at your periodic tableElements are divided into s, p, d and f blocksS blocks contain 2 elements, p blocks contain 6 elements, d elements contain 10 elements and f blocks contain 14 elements (you will understand this more when you further study energy levels and quantum numbers) The first two elements are the first s blockExample: We would say that helium has an electron configuration of 1s^2(1 for energy level, s for s block and 2 for 2 electrons in the s blockHydrogen would be 1s^1The next two elements are the second s blockExample: Lithium would have an electron configuration of (without spaces) 1s^2 2s^1(1s^2 for containing all blocks up till now, and 2s^1 for having one electron in the second s blockThe next six elements are the first p block, but the p block has an energy level of 2 so we say 2p rather than 1pExample: Nitrogen would have an electron configuration of (without spaces) 1s^2 2s^2 2p^3 for all of the blocks up until now, and 3 electrons in the first p block This pattern continuesExample: Aluminium is (without spaces) 1s^2 2s^2 2p^6 3s^2 3p^1When we reach the d block (transitional metals), same thing but begin with 3d, not 2d or 1dExample: Iron is (without spaces) 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^6Important tip: You can count up the exponents in each case and if it equals the atomic number of the element then you are doing it rightThese patterns continueI'm sorry if this wasn't the most helpful explanation but it should be able to get you started:)
