Starter # (1) Why was Rutherford s model not good enough and need to be modified by scientists?
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1 1. (1) Why was Rutherford s model not good enough and need to be modified by scientists? It could not explain or predict any chemical behavior of any elements 2. (1) What is one of the only things that can behave as both a particle and a wave and was the thing used to advance our understanding of atoms past Rutherford s Model? Light 3. (3) What are each of the following things called? a) (1) What is the number of waves that pass a given point per second Frequency b) (1) Shortest distance between equivalent points on a wave Wavelength c) (1) Height of a crest or depth of trough from origin Amplitude 4. (1) What is energy that exhibits wavelike behavior called? Electromagnetic Radiation 5. (1) What is the minimum amount of energy that can be gained/lost by an atom called? Quantum 6. (2) What is the value and unit for Plank s Constant? x J s 7. (1) What is a photon? Starter # Particle of electromagnetic radiation with no mass and has quantum of energy
2 1. (4) If a wave has a wavelength of 1.5x10-5 m, what is the frequency? Show work and use correct S.F. and unit. c = λv v = = v = Hz 2. (4) If a photon has a frequency of the answer to #1, what is the energy of that photon? Show work and use correct S.F. and unit. E = hv E = E = J 3. (2) Convert the wavelength from #1 into nanometers. Show your work m nm 1 m Quiz # = nm or nm
3 Starter # (1) Whose model began to describe and predict the movement of electrons within an atom? Niels Bohr 2. (1) What is the lowest allowable energy state of an atom? Ground State 3. (1) What is the any higher energy state of an atom called? Excited State 4. (1) What is the formula for calculating the change in energy of an electron? E = E high E orbit E low E orbit 5. (1) Who added to the model of the atom using the wave-particle nature of light and was able to explain the whole-number of waves observed? Louis DeBroglie 6. (1) What is the equation for calculating the wavelength of any particle moving at any speed? λ = h mv 7. (1) Who stated that it is impossible to know both the speed and location of an electron at the same time? Werner Heisenberg 8. (1) Who is the one who created the math formula for the model of the atom we use today? Erwin Schrodinger 9. (1) What is the current model of the atom called? Quantum Mechanical Model 10. (1) What is the region where you are 90% likely to find an electron orbiting an nucleus called? Atomic Orbital
4 1. (2) An electron jumps from an energy level with 35 joules of energy to one with 30 joules of energy. a. (1) Calculate the quantum of energy for this electron Quantum = Δenergy = 30 J 35 J = 5 J b. (1) Did the electron gain or lose energy? Lost energy because it went down in energy (negative #) 2. (1) Each energy level (n) contains how many sublevels? n sublevels each energy level has the same number of sublevels as its principal quantum number 3. (4) How many orbitals are in each sublevel? s = 1, p = 3, d = 5, f = 7 4. (1) Each energy level (n) contains how many orbitals? n 2 5. (1) How many electrons can each orbital hold? Maximum of 2 Quiz # (1) Each energy level (n) can hold how many electrons? 2n 2
5 1. (6) What are the 3 rules for determining the electron configuration of an atom called, and what do they state? Aufbau Principle = Electrons occupy lowest energy orbitals available Pauli Exclusion Principle = Each orbital can hold up to 2 electrons with opposite spins Hund s Rule = Single electrons with same spin occupy equal-energy orbitals before electrons will pair up with opposite spins at that energy level 2. (1) What are the diagrams of electron configurations called? Orbital Diagrams 3. (1) Which two elements are exceptions to the rules for electron configurations? Chromium(Cr) and Copper (Cu) 4. (1) What is the name of the electrons that occupy the outer-most orbitals? Valence Electrons 5. (1) What are the diagrams that contain the symbol of the element surrounded by the outer-most electrons called? Electron-Dot Structures Starter #11 5.3
6 Quiz # (5) Draw the Bohr Model for Magnesium-23 (1) Magnesium is #12 so it has 12p + & 12 (1) = 11 n 0 (1) 2 go on the first energy level (1) 8 go on the second energy level (1) Last 2 go on the third energy level 12 p+ 11 n 0 2. (1) What is the full electron configuration for Chlorine? Cl = 1s 2 2s 2 2p 6 3s 2 3p 5 3. (1) What is the noble gas electron configuration for Chlorine? Cl = [Ne]3s 2 3p 5 4. (1) What is the full electron configuration for Iron? Fe = 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 6 5. (1) What is the noble gas electron configuration for Iron? Fe = [Ar]4s 2 3d 6 6. (1) What is the full electron configuration for Copper? Cu = 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 1
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