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Transcript
Atomic structure review - H People Thompson – discovered electrons Rutherford – discovered the nucleus – small dense positive nucleus, volume empty space Bohr – electrons have quantized (specific) energy, shell model Heisenberg – due to wave nature of electrons you can’t know the position and momentum of an electron at the same time Pauli – no more than two electrons can occupy 1 orbital, that’s why a set of 4 quantum numbers belongs to only 1 electron, when two electrons are in they differ in spin (the ms quantum number) Hund – each orbital in a sublevel partially fills before pairing up - wavelength and frequency are inversely proportional energy and frequency are directly proportional hi energy light has high frequency and short wavelength Isolelectronic means that species have the same number of electrons Isotopes are species with the same number of protons and different numbers of neutrons Mass number = protons + neutrons in a single atom Atomic mass is a weighted average of all naturally occurring isotopes of an element, this is the mass on the periodic table Negative ions are atoms that have gained electrons negative ions Positive ions are atoms that have lost electrons positive ions Atoms are neutral 5 or more valence electrons become 3 or fewer valence electrons become protons = electrons Number of neutrons = mass number – atomic number Valence electrons are all the electrons in the highest energy level 1s2 2s2 2p3 this is nitrogen in the ground state, it has 5 valence electrons Dot structures show valence electrons only – all members of a group have the same dot structure Quantum numbers The first number is the shell number The second number is the sublevel s is 0 l is 1 d is 2 The second number must be less than the first !!!!!!! f is 3 Each value of n (shell number) has that number of sublevels 1st energy level only has the s sublevel 2nd energy level has s and p sublevels 3rd energy level has s, p, d sublevels 4th energy level has s, p, d, f sublevels S sublevel has 1 orbital (box) P sublevel has 3 orbitals D sublevel has 5 orbitals F sublevel has 7 orbitals After the 3 p orbitals are filled electrons go to 4s (K and Ca) then after 4s they go to 3d For an element like Scandium which is 3d1 the 4s2 electrons are the valence electrons 1s22s22p63s23p63d14s2 Atomic number is the number of protons Electrons are negative and massless Electrons become excited by absorbing energy, they release that energy in the form of light when the electrons return to lower energy levels (spectral lines)