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Unit 2 - Atomic Theory UNIT 2 - ATOMIC THEORY VOCABULARY: Allotrope Electron Configuration Nuclear Charge Anion Element Nucleons Atom Excited state Nucleus Atomic Mass Ground state Orbital Atomic Mass unit (a.m.u.) Ion Proton Atomic number Isotope Quantum Theory Bohr model Kernel electron(s) Valence electron(s) Cation Lewis Dot Diagram Wave-mechanical model Compound Mass number Electron Neutron OBJECTIVES: Upon completion of the unit you will be able to do the following: • Understand that the modern model of the atom has evolved over a long period of time through the work of many scientists • Discuss the evolution of the atomic model • Relate experimental evidence to models of the atom • Identify the subatomic particles of an atom (electron, proton, and neutron) • Know the properties (mass, location, and charge) of subatomic particles • Determine the number of protons, electrons, and neutrons in a neutral atom and an ion • Calculate the mass number and average atomic weight of an atom • Differentiate between an anion and a cation • Identify what element the amu unit is derived from • Define the term orbital • Distinguish between ground and excited state • Identify and define isotopes • Write electron configurations • Generate Bohr diagrams • Differentiate between kernel and valence electrons • Draw Lewis Dot Diagrams for an element or an ion 1 THE EVOLUTION OF THE ATOMIC MODEL Atom = Democritus = Dalton (1803) o Known as the ______________ of the atomic theory o Dalton invented the word ___________ as the basic unit of matter which were considered to be ____________________ o Dalton also claimed that all atoms of a given element are ____________________ o He also discovered that atoms of different elements have different __________________________________ o Found that combining atoms of different elements formed ____________________ o Theory referred to as the _________________ theory (it looked like a simple sphere) *What does this name tell you about Dalton’s atom? J.J. Thomson (1897) o While using a ______________________ he discovered that the ray was deflected (due to a magnetic/electrical field) o From this discovery he concluded that atoms contain small negatively charges particles called ________________ o Theory famously referred to as the ____________________ model because he visualized the ______________ being _____________ within the structure of the atom (just like raisin bread) o The _________ of the rest of the atom (besides the electrons) was thought to be ____________________ and _____________________ 2 * Rutherford (1909) * o Experiment called the ___________________ where he ______________ a thin piece of ___________ with a _________________________________ o Often referred to as the __________ model o Most alpha particles went _________________ & some were ____________ o Two conclusions were therefore made: 1) most of the atom is _____________________ 2) atoms have a _____________ , ____________________ called the _________________ * Neils Bohr (1913) * o Proposed that the atom consists of a dense nucleus with _______________ found in _____________________________________ o He therefore stated that each electron orbiting the nucleus must possess a ______________________________ to keep it in place within its orbital o Known as the _____________ model (looks much like our solar system) Wave-Mechanical/Cloud Model (Modern Present day model) o Developed after the famous discovery that energy is made up of BOTH _________ & _________________ o Still the same dense positively charged ______________ o Electrons now have distinct amounts of energy and move in areas called ____________ or __________________________________________ _________________________________________________________ _________________________________________________________ o ___________________________ have contributed to this theory o Different from the Bohr diagram—now the location of the electron is based on _____________________ within the orbital *3-dimensional model 3 Atomic Model Conclusion(s) Date: Scientist: Name of Model: Date: Scientist: Name of Model: Date: Scientist: Name of Model: 4 Atomic Model Conclusion(s) Date: Scientist: Name of Model: Date: Scientist: Name of Model: 5 VOCABULARY (of the Periodic Table) SUBATOMIC PARTICLES Subatomic Charge Relative Mass Location Symbol How to Calculate Particle Proton Neutron Electron 6 Let’s Practice Calculating Subatomic Particles in Different Atoms: Symbol # # # Atomic Mass Nuclear Protons Neutrons Electrons Number Number Symbol 35 Cl 17 15 16 C-14 8 Mass number = Nuclear Charge = Nucleons = 7 ATOMS (neutral) VS. IONS (charged) Vocabulary Term Definition Example/Diagram Neutral Atom Ion Anion Cation 8 ISOTOPE = Example: Isotopes of Carbon (C-12, C-13, & C-14) 12 13 14 C C C 6 6 6 U-238 U-240 So why does Carbon have a mass of 12.011 on the Reference Table? This is carbon’s ATOMIC MASS which is the average weighted mass of all naturally occurring isotopes of carbon (there exist three different isotopes of carbon in the atmosphere – as seen just above) 9 Calculating Atomic Mass (for any element): Atomic Mass = the weighted average of an element’s naturally occurring isotopes (abundance in decimal form) (mass of isotope 1) (abundance in decimal form) (mass of isotope 2) + (abundance in decimal form) (mass of isotope 3) Example 1 12 C = 98.89% of carbon in the atmosphere 13 C = 1.11% of carbon in the atmosphere Step 1: Multiply the mass of each separate isotope by its percent abundance (in decimal form!!!!!!!) Step 2: Add up the products of all the calculated isotopes from step 1. Example 2: The element Boron occurs in nature as two isotopes. Isotope mass percent abundance Boron 10.0130 amu 19.9% Boron 11.0093 80.1% 10 Example 3: Isotope of Hydrogen Percent Abundance 1 H Protium 99.0% 1 2 H Deuterium 0.6% 1 3 H Tritium 0.4% 1 ATOMIC MASS VS. MASS NUMBER 11 ELECTRON CONFIGURATIONS = a dashed chain of numbers found in the _________________________ of an element box (see below); tells us the number of __________________ as well as the number of ___________ in each level (tells us how the electrons are arranged around the nucleus) **All electron configurations on the Periodic Table are NEUTRAL (p=e) Substance Electron Configuration Magnesium Mg +2 Bromine Br -1 Barium *Lead * shortcut allows you to cut out the first two orbitals to shorten the “address” Valence Electrons: electrons found in the ________________ shell or orbital; the __________ number in the electron configuration Kernel Electrons: _______________ electrons (all non-valence electrons) Sulfur # valence e- ____ Nitrogen # valence e- ____ # kernel e- ____ # kernel e- ____ 12 Principle Energy Level (n) = electron energy levels that contain a certain number of ______________________ ; each sublevel contains one a set number of _____________ Maximum # of electrons in an energy level = ___ where n = ____________ # (or period #) Principle Energy Level (n) Maximum number of electrons ( ) 1 2 3 4 Sample Question: What is the maximum number of electrons that can occupy the 3 rd principal energy level in any atom? ___________ BOHR DIAGRAMS (one method for expressing electron location in an atom or ion); _______________________ MUST be drawn ________________ 1. Look up electron configuration of element at hand on Periodic Table (if you are working with an ion, add/subtract the proper amount of electrons from outer shell(s) of configuration) Example: Carbon is __________ 2. Draw nucleus (with a circle) and notate correct amount of protons and neutrons inside 3. Using rings or shells (these are your orbitals), place the proper amount of electrons in their appropriate orbital(s) – there should be as many rings/shells as dashed number in electron configuration 13 Carbon Fluorine Beryllium Al Li I Na + S-2 LEWIS (ELECTRON) DOT DIAGRAMS - a shorter way of expressing electron location; an _________________________________ • Only illustrates ______________________________________! 1. Write the element’s symbol 2. Retrieve electron configuration from Periodic Table. The last number in the configuration is the _________________________. 3. Arrange the valence electrons (DOTS) around the symbol using the following rules: • Only two electrons maximum per side of the symbol (therefore no more than 8 total surrounding symbol – 8 is great!) • Always “pair” the first two • If you have more than 2 valence electrons, deal them one at a time to the other three sides until you run out 1 2 X 4 7 4. If you are working with an ion you must adjust the valence electrons (add or subtract electrons) in the configuration before constructing your Dot Diagram – be sure to draw your final diagram with the initial charge on the ion 14 Draw LEWIS ELECTRON-DOT DIAGRAMS for the following: Argon Phosphorus Carbon Beryllium Oxygen Aluminum Sodium Bromine Na +1 O-2 15 Ground State vs. Excited State *Notice that one electron from the 2nd orbital has moved to the 3rd orbital Ground State = electrons in _____________________________ possible (configuration found on ___________________); electrons _____________________________ as physically possible ground state electron configuration for Li is _____ Excited State = electrons are ___________________________ _________________ (____ configuration ____ found on PT) excited state electron configuration for Li could be ______ Distinguish between ground state and excited state electron configurations below: Bohr Electron Configuration Ground (G) or Excited (E) state? 2-1 2-0-1 1-1-1 2-7-3 2-8-2 2-8-8-2 2-8-17-6 2-8-18-8 2-6-18-1 2-5-18-32 16 The greater
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