CH 101 1st Edition Lecture 6 Outline of Last Lecture I. Light wavesA. How to Calculate the Wavelength and the FrequencyII. The Bohr ModelA. Absorbing energyB. Emitting energyIII. Recap of Important EquationsOutline of Current Lecture I. The Schrodinger Model of the Atom A. NodesII. Introduction to Quantum NumbersIII. The Pattern Within Energy LevelsIV. What Orbitals Look Like B. Electron ConfigurationV. Quantum Numbers on the Periodic TableCurrent LectureI. The Schrodinger Model of the Atom - When it was discovered that electrons don’t always act as particles but can act as waves, the Bohr model of the atom had to be revised. The revised model is called the Schrodinger model, it shows the electrons in an atom moving in wave patterns. The wavelength of a wave can be determined if you know the energy level of the electron, the equation is λ = 2L / n where L is the length in centimeters. A. Nodes – Nodes are the points of the wave that seem to stay in place. If you are just given the energy level (n), The amount of nodes in that energy level can be determined by n – 1 = amount of nodes. Therefore, the first energy level has zero nodes, the second energy level as one node, and so on. II. Introduction to Quantum Numbers – Schrodinger came up with quantum numbers to representwhere the electron is within the atom.These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.Principal Quantum Number ( n ) – Tells you the energy level or shell the electron is on. This is similar to the Bohr model because the larger the n value is, the farther away from the electron is from the nucleus. Orbital Quantum Number ( l ) – Is a sublevel of the energy levels and determines the amount of nodes, the value of l can never be the same or more than the value of n. The values of l are represented with letters, 0 = s, 1 = p, 2 = d, 3 = f, 4 = g, and 5 = h. For example within the n = 2 energy level there are two sub levels 2s and 2p, the third energy level has three sublevels, 3s, 3p, and 3d.Magnetic Orbital Quantum Number ( ml ) – This number determines the orientation of the sublevel because it is the amount of orbitals a sublevel can have. The value of ml Is determined by taking the amount for l and subtracting it from 0 . Then you count the number of orbitals within the range l of and -l . For example the sublevel p equals 1 node, to determine the you write out -1, 0, 1 and determine that the sublevel p has ml = 3.Spin Quantum Number ( ms ) – The spin quantum number can only equal ½ or -½. This tells youthe direction of the electrons spin around the nucleus. III. The Pattern Within Energy Levels- Just because the n is larger, doesn’t mean the electron has more energy. The ranking of energy is determined by n + l and if two answers come out the same, the electron with the larger n is higher in energy. This means that an electron at 3d has more energy than an electron at 4s.Ex) An electron at which orbital would have the most energy, 4d or 5s?Start by determining what n and l equal. n equals the coefficient and equals the letter which corresponds toa number 0 = s, 1 = p, 2 = d, 3 = f, 4 = g, and 5 = h. Then plug it into the equation n + l 4d -> n = 4 l = 2, 4 + 2 = 6 <- This is the higher number, therefore 4d has more energy than 5s.5s -> n = 5 l = 0, 5 + 0 = 5IV. What Orbitals Look Like - The shape of the orbital is determined by the n, the l, and the ml. The l determines the shape, the ml determines how many orbitals there are (an orbitals means the path the electron travels within the subshell), and the n determines how big the orbital is (the larger the n the larger the orbital). The exact orientation of each orbital is not as important as knowing the general shape of it. Here is a simple chartto help you understand how the amount of nodes and orbitals affect the shape. The l = the amount of nodes The ml = The amount of orbitals General shape of the orbitals = 0 nodes 0 -> only 1 orbitalp = 1 node -1, 0, 1 -> 3 orbitalsd = 2 nodes -2, -1, 0, 1, 2 -> 5 orbitalsf = 3 nodes -3, -2, -1, 0, 1, 2, 3 -> 7 orbitals A. Electron Configuration- Electron configurations are created out of quantum numbers. The l letters (s, p, d, f, etc) tell you the maximum amount of electrons that can be in that orbital by multiplying the number of orbitals (ml) bytwo because the orbital is formed when two electron are attracted to each other. The amount of electrons in an atom are represented by an electron configuration. - Here is what an electron configuration chart looks like, each blank square can hold two electron facing opposite directions (one electron must always be pointing up and the other pointing down). If there arenot enough electrons to fill a row of boxes, distribute the electrons so that every box in that row gets an electron, there cannot be a box with two electrons in it in the same row as a blank box, the electron would need to be dispersed to fill the blank box. - Neon’s electron configuration is 1s2 2s2 2p6 showing that neon has 10 electrons. When you draw out the electron configuration of neon it looks like this.- Oxygen’s electron configuration is 1s2 2s2 2p4 because oxygen only has 8 electrons. Its electron configuration chart would look like this.Excited State- An electron is in an excited state when there electron configuration has an odd number or if a level isn’t filled and an electron is on the next level. Here are examples of excited states Grounded State- A ground state is when an electron configuration has no unpaired electrons and if it does has unpaired electron they fill up the whole orbital level. These are examples of ground states. V. Quantum Numbers on the Periodic Table- Quantum numbers are easy to find on the periodic table because they are grouped together. The only thing you have to remember is that helium moves to the s block. Using the periodic table to find the electron configuration of an element is tedious but with practice you will start to understand how the table works. - First locate the element and see what row it is in. - Next start with the s block and see how many rows you have to go through till you get to the element ifyou start at hydrogen in the top left corner and move from left to …