Unit 3: Atomic Structure
Practice Packet Unit 3: Atomic StructurePre-AP ChemistryUnit 3:Atomic StructureName:Class Period:1
Practice Packet Unit 3: Atomic StructurePre-AP ChemistryVocabularyFor each word, provide a short but specific definition from YOUR OWN BRAIN! Don’t give a textbook oran internet definition. Write something that will help YOU remember the word.Anion:Atom:Atomic Mass:Atomic Number:Bohr Model:Bright Line Spectra:Cation:Electron Configuration:Electron:Excited State:Ground State:Ion:Isotope:Mass Number:Neutron:Nuclear Charge:Nucleus:Orbital:Proton:Quantum Mechanical Model:Sublevel:Valence Electrons:2
Practice Packet Unit 3: Atomic StructurePre-AP ChemistryBuilding an Atom Inquiry Activity: Google “Build an Atom Phet” Run this simulation on “Atom”3
Practice Packet Unit 3: Atomic StructurePre-AP Chemistry4
Practice Packet Unit 3: Atomic StructurePre-AP Chemistry5
Practice Packet Unit 3: Atomic StructurePre-AP ChemistryLesson 1: Atomic Structure6
Practice Packet Unit 3: Atomic StructurePre-AP Chemistry7
Practice Packet Unit 3: Atomic StructurePre-AP ChemistryAdditional Practice: Lesson 18
Practice Packet Unit 3: Atomic StructurePre-AP ChemistryHistory of the Atomic Structure ModelsJohn Dalton (1766 – 1844):John Dalton was an English chemist. His ideas form the atomic theory of matter. Here are his ideas. All elements are composed (made up) of atoms. It is impossible todivide or destroy an atom.All atoms of the same elements are alike. (One atom of oxygen is likeanother atom of oxygen.)Atoms of different elements are different. (An atom of oxygen isdifferent from an atom of hydrogen.)Atoms of different elements combine to form a compound. Theseatoms have to be in definite whole number ratios. For example, wateris a compound made up of 2 atoms of hydrogen and 1 atom ofoxygen (a ratio of 2:1). Three atoms of hydrogen and 2 atoms ofoxygen cannot combine to make water.1. What is the name of John Dalton’s theory?2. What are elements made of?3. An atom of hydrogen and an atom of carbon are .4. What are compounds made of?5. The ratio of atoms in HCl is:a) 1:3b) 2:1c) 1:1J. J. Thompson (Late 1800s):J. J. Thompson was an English scientist. He discovered the electron whenhe was experimenting with gas discharge tubes. He noticed a movement ina tube. He called the movement cathode rays. The rays moved from thenegative end of the tube to the positive end. He realized that the rays weremade of negatively charged particles – electrons.1. What did J.J. Thompson discover?2. What is the charge of an electron?3. What are cathode rays made of?4. Why do electrons move from the negative end of the tube to the positive end?5. What was Thompson working with when he discovered the cathode rays?9
Practice Packet Unit 3: Atomic StructurePre-AP ChemistryLord Ernest Rutherford (1871 – 1937): Ernest Rutherford conducted afamous experiment called the gold foil experiment. He used a thin sheet ofgold foil. He also used special equipment to shoot alpha particles (positivelycharged particles) at the gold foil. Most particles passed straight through thefoil like the foil was not there. Some particles went straight back or weredeflected (went in another direction) as if they had hit something. Theexperiment shows: Atoms are made of a small positive nucleus; positive nucleusrepels (pushes away) positive alpha particlesAtoms are mostly empty space1. What is the charge of an alpha particle?2. Why is Rutherford’s experiment called the gold foil experiment?3. How did he know that an atom was mostly empty space?4. What happened to the alpha particles as they hit the gold foil?5. How did he know that the nucleus was positively charged?Niels Bohr (Early 1900s):Niels Bohr was a Danish physicist. He proposed a model of theatom that is similar to the model of the solar system. The electronsgo around the nucleus like planets orbit around the sun. Allelectrons have their energy levels – a certain distance from thenucleus. Each energy level can hold a certain number of electrons.Level 1 can hold 2 electrons, Level 2 - 8 electrons, Level 3 - 18electrons, and level 4 – 32 electrons. The energy of electrons goesup from level 1 to other levels. When electrons release (lose)energy they go down a level. When electrons absorb (gain) energy,they go to a higher level.1. Why could Bohr’s model be called a planetary model of the atom?2. How do electrons in the same atom differ?3. How many electrons can the fourth energy level hold?4. Would an electron have to absorb or release energy to jump from the second energy level to the third energy level?10
Practice Packet Unit 3: Atomic StructurePre-AP ChemistryLesson 2: Electron ConfigurationPART A – ORBITAL DIAGRAMS & LONGHAND ELECTRON CONFIGURATIONUse the patterns within the periodic table to draw orbital diagrams and write longhand electron configurations forthe following atoms.Symbol1.# e-Orbital Diagram andLonghand Electron ConfigurationMg2.P3.V4.Ge5.Kr6.O11
Practice Packet Unit 3: Atomic StructurePre-AP ChemistryPART B – SHORTHAND ELECTRON CONFIGURATIONUse the patterns within the periodic table to write the shorthand electron configurations for the following elements.Symbol7.Ca8.Pb9.F10.U# e-Shorthand Electron ConfigurationPART C – RULES OF ELECTRON CONFIGURATIONSWhich of the following “rules” is being violated in each electron configuration below? Explain your answer foreach. Hund’s Rule, Pauli Exclusion Principle, Aufbau Principle11.12.13.14. 1s2s2p 1s2s2p3s 1s2s2p2s2p3p 3s 1s 3p 3s3p3d12
Practice Packet Unit 3: Atomic StructurePre-AP ChemistryLesson 3: Ions13
Practice Packet Unit 3: Atomic StructurePre-AP Chemistry14
Practice Packet Unit 3: Atomic StructurePre-AP ChemistryAdditional Practice: Lesson 315
Practice Packet Unit 3: Atomic StructurePre-AP ChemistryLesson 4: Isotopes and Average Atomic Mass16
Practice Packet Unit 3: Atomic StructurePre-AP ChemistryAdditional Practice: Lesson 417
Practice Packet Unit 3: Atomic StructurePre-AP Chemistry18
Practice Packet Unit 3: Atomic StructurePre-AP Chemistry19
Practice Packet Unit 3: Atomic StructurePre-AP ChemistryLesson 5: Ground vs. Excited State20
Practice Packet Unit 3: Atomic StructurePre-AP ChemistryEmission SpectraBase your answers for questions 4-5 on the diagram below, which shows the bright-line spectra of selectedelements.4.5.21
Practice Packet Unit 3: Atomic StructurePre-AP ChemistryLesson 6: Lewis Dot Diagrams22
Practice Packet Unit 3: Atomic StructurePre-AP ChemistryAdditional Practice: Lesson 623
Lesson 2: Electron Configuration PART A – ORBITAL DIAGRAMS & LONGHAND ELECTRON CONFIGURATION Use the patterns within the periodic table to draw orbital diagrams and write longhand electron configurations for the following atoms. Symbol # e-Orbital Diagram and Longhand Electro
Physical & Chemical Properties Chemical & Physical Changes Matter Obj. 2.1.2 Atomic Structure Isotopes Matter Obj. 2.1.2 Rate Atomic Structure Obj. 2.1.4 Matter Obj. 2.1.2 Phase Change Test Matter Matter Atomic Structure Obj. 2.1.4 Atomic Structure Obj. 2.1.4 Atomic Structure Structure Atomic Structure Obj.
53.Gram atomic mass of oxygen 16g. 54.Gram atomic mass of sodium 23g. 55.Atomic mass is expressed in atomic mass unit (amu). 56.One atomic mass unit is defined as 1/12th part of the mass of one atom of carbon. 57.The relative molecular mass of an element o
Atomic Structure Worksheet **Assume all are neutral atoms! Fill in the blanks in the following worksheet. Please keep in mind that the isotope represented by each space may NOT be the most common isotope or the one closest in atomic mass to the value on the periodic table. Atomic symbol Atomic number Protons Neutrons Electrons Mass number
The Atomic Theory of Matter Dalton’s Atomic Theory Postulates 10 2. All atoms of a given element are identical, having the same size, mass and chemical properties. The atoms of different elements are different. Different elements have different atomic properties such as atomic mass.
Unit 2 – Atomic Structure and Nuclear Chemistry Unit Goals: As you work through this unit, you should be able to: 1. describe Dalton’s atomic theory and compare to our modern understanding of the atom (4.1) 2. distinguish among protons, electrons, and neutrons in terms of mass and char
Page 1 of 3 1.4 w-1 Atomic Structure Worksheet.docx Atomic Structure Worksheet Fill in the blanks in the following table. Note: The mass may not match the mass on your periodic table. Assume all atoms are neutral Atomic symbol Atomic number Protons Neutrons Electrons Mass number C 8 12 24 31 40 40 89 30 35 42 98
1. describe previous atomic theories and compare to our modern understanding of the atom (4.1) 2. distinguish among protons, electrons, and neutrons in terms of mass and charge. (4.2) 3. describe the structure of the atom. (4.2) 4. explain why isotopes differ and why atomic masses are not whole numbers. (4.3) 5. understand how atomic mass is .
Trigonometry Unit 4 Unit 4 WB Unit 4 Unit 4 5 Free Particle Interactions: Weight and Friction Unit 5 Unit 5 ZA-Chapter 3 pp. 39-57 pp. 103-106 WB Unit 5 Unit 5 6 Constant Force Particle: Acceleration Unit 6 Unit 6 and ZA-Chapter 3 pp. 57-72 WB Unit 6 Parts C&B 6 Constant Force Particle: Acceleration Unit 6 Unit 6 and WB Unit 6 Unit 6
