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Unit 2 Note Companion Atomic Structure Subatomic Particle in the Atom Particle Location Charge Mass Proton Neutron Electron Atomic Symbol Draw and Label the atomic symbol for Gold Examples • Write the atomic Symbol for Silver • Write the atomic symbol for carbon • Write the atomic symbol for Carbon-12 Atomic number and mass Atomic number = Atomic mass= What is an isotope? What is an ion? Examples Element Protons Neutrons Electrons Carbon-13 Ca 2+ F131 53 I 131 54 Xe Summary Average Atomic Mass What is average atomic mass? • _______________ average of all isotopes (like your grades) • on the Periodic Table • round to 2 decimal places Average atomic mass= • Calculate the avg. atomic mass of oxygen if its abundance in nature is 99.76% 16O, 0.04% 17O, and 0.20% 18O. Summary History of the Atom-Part 1 Democritus • The first ___________________________ • Matter is made of empty space through which _________________________ • Atoms are ___________________________________________ • _______________atoms have _______________sizes and shapes • Changes in matter are due to changes in _____________________________________________ What is the law of conservation of matter? Matter cannot be Law of Definite Composition A compound will have the ___________________________________________________ Will always have the same ratio Dalton’s Atomic Theory • All matter is made of small, _____________________________________called atoms • Atoms of the__________ element have ________________________________ • Atoms of __________________ elements have ____________________________ • Atoms obey the _________________________________________ Atoms obey the _________________________________________ Law of Multiple Proportions If two elements can make Summary History of the atom- Part 2 Briefly Explain the Cathode ray Experiment that Thomson performed Plum Pudding Model • When Thomson ________________________________________, he came up with a model for the structure of the atom • Atoms are ____________________________________ _____________________________________________ • No “anode rays”, so it was thought that the _______________________________________ were seen as ___________________________________ from one place to another Briefly Explain the Gold Foil Experiment that Rutherford performed Explanations to Rutherford’s Observations Positively charged alpha particles would pass through most of the time without being deflected Some particles were deflected Nuclear model The positive charge is all concentrated in the Summary The Bohr Model Bohr Model e- (electrons) only exist in orbits Therefore Bohr Model • Concluded the electrons _____________________________________________ • The orbitals ________________to the nucleus have the _______________ amount of energy and the orbitals gain energy the _______________ they get from the nucleus How the Bohr model relates to light • When an atom is at rest, each electron lies in its _____________________________________________ • Energy is __________________to an atom, the electrons ____________ it and jump to _________________________ orbitals (_______________________) • • • The electrons fall back to the _________________________, giving off the energy as ______________ Because there are so many orbitals, there are only ___________________________ of light that can be given off by an atom No two atomic spectra will ever be the same (the light given off by the atom) What is spectroscopy? Problems with Bohr model Even though It only worked for Summary The Modern Atom Light is a Wave Light is characterized by Draw and label the diagram of the wave Wavelength (λ)= Frequency (v)= How are wavelength and frequency related? Frequency and wavelength are inversely proportional, which means_____________________________________ Equation for the speed of light • • • c: : : speed of light (3.00 108 m/s) wavelength (m, nm, etc.) frequency (Hz) Find the frequency of a light particle with a wavelength of 434 nm. How Are Frequency and Energy Related? The energy of a wave is proportional to its frequency, which means __________________________________________ Equation for energy E: h: : energy (J, joules) Planck’s constant (6.6262 10-34 J·s) frequency (Hz) Find the energy of a red photon with a frequency of 4.57 1014 Hz. The Electromagnetic Spectrum __low_Wavelength ________Frequency ____high__Energy ___________Wavelength ____low_frequency __________energy Gamma Rays, Xrays, UV, Visible, Infrared, Microwaves, Radiowaves Light is quantized When something is quantized, it means Planck concluded Light is a particle Einstein concluded Einstein observed a certain frequency Defined a light particle as a _______________ Summary The Quantum Model- Standard Modifications of the Bohr Model • In the Bohr Model there was only one variable on where the electrons were (___________________________________________________________________________) • Schrodinger proved there were 4 variables on where the electrons were • 4 quantum numbers This idea is similar to the idea of an address • 1st Quantum number or the Principle Quantum number • This number determine the main _________________________________ • Also indicates the ______________ of the orbital • • 2nd Quantum Number or the Angular Momentum Quantum Number Determined the _________________________ of the electron (_________________ of the orbital) • • • • 3rd Quantum Number or the Magnetic Quantum Number Determines the ___________________________ of the orbitals Can be oriented in three ______________________ This number tells you what _______________ the electron is in • • The 4th quantum number or the Spin Quantum Number This number indicates which electron we are talking about in the orbital (each orbital can hold two electrons) • An orbital can hold _________electrons that spin ___________________________ directions. • Pauli Exclusion Principle • No two electrons in an atom can have the same 4 quantum numbers. • Each e- has a unique “address”: Principal #Ang Mom #Magnetic #Spin #Summary