Survey
* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
Name:____________________________________ Date:_____________ Answers for Chemistry 1 Atomic Theory Quiz Review 1. Name Each Scientist from the Democritus philosophers to Bohr. Describe their models, draw a picture, and state the theory Use the chart below Name Model Picture Properties being Measured Greek Earth, Wind, Fire, None, Only Limited Philosopher Water Observations Matter could be endlessly divided Democritus the smallest particles of matter that could not be further divided That different types of atoms existed for every type of matter. Atomos: “uncuttable Dalton • • • Thomson All matter is made up of atoms. Atoms are indestructible and cannot be divided into smaller particles. (Not currently true) All atoms of one element are exactly alike, but they are different from atoms of other elements. (Not currently true) Atoms were not just neutral spheres, but are composed of electrically charged particles. Atoms were composed of a positive sphere (the pudding) and had negatively charged particles called electrons (plums) embedded into the pudding. Rutherford Rutherford’s Model: An atom is made of a small, positively -charged , dense nucleus and negative “empty space” called the electron cloud. Only Limited Observations The size of Objects Observed the works of other scientists such as Law of Conservation of Matter and the Law of Multiple Proportions. The Cathode Ray Tube Experiment shows negative charges (electrons) moving towards a positive charge Some Dense, Positive Alpha Particles were deflected from the dense positive nucleus. Most alpha particles passed through the atom. Bohr Bohr’s Model: Electrons move around the atom within energy levels and only a certain amount of electrons can exist on one energy level at a time. His experiments looked at the emission spectrum of atoms, particularly hydrogen. Bohr observed that electrons absorbed energy, and then released the energy in the form of light. 2. A balanced equation follows what Law? Give an example of a balanced equation, and explain why it must be balanced Balancing demonstrates the Law of Conservation of Matter: Matter cannot be created or destroyed during a chemical reaction. Matter can only be rearranged. 2AgCl + Na2SO4 Ag2SO4 + 2NaCl 3. What are Dalton’s three points for his atomic theory. Are they all currently true? Explain. • All matter is made up of atoms. This point is currently true • Atoms are indestructible and cannot be divided into smaller particles. (Not currently true) Atoms can be divided into protons, neutrons, and electrons • All atoms of one element are exactly alike, but they are different from atoms of other elements. (Not currently true) Atoms of the same element are different because of isotopes. They differ in the amount of neutrons or mass. 4. What are the three classic subatomic particles? What are their charge, location, and mass? Particle Charge Location Proton +1 Neutron 0 Electron -1 5. Nucleus Nucleus Outside Nucleus Mass (Relative) 1 amu 1 amu 0 amu What is an element’s atomic number? Mass number? What does the atomic mass tell you? • • • Atomic Number = The amount of Protons in an atom. This number is also the amount of electrons in a neutrally charged atom. Mass Number = The mass of one atom. Protons + Neutrons Atomic Mass is the Weighted Average Mass of an elements isotopes. 6. What is an isotope? How is an element’s mass number different from its atomic mass? • An isotope is an atom of an element that differs in mass (the amount of neutrons). Isotopes are chemically identical, but physically different. 7. Explain why an atom’s atomic mass can be different from each isotope: • The Atomic Mass is a weighted average of the relative abundance of all the isotopes that comprise an element. • The Calculation for atomic mass demonstrates this idea 8. What is the atomic mass of Copper that has 69.2% Cu-63 and 30.8% Cu-65? Show work/units • (0.692 x 63amu) + (0.308 x 65amu) = 63.6 amu 9. What is the relationship between frequency, wavelength, energy and speed? • Both Waves move at the same speed 10. List the order of electromagnetic waves from lowest to highest wavelengths, Include Energy and Frequency. 11. Which color of light has the highest frequency? Lowest frequency? • Violet has the highest frequency • Red has the lowest frequency 12. What evidence told scientists that electrons were located on specific energy levels, rather than being scattered randomly around the nucleus? • The emission spectrum. Specific Frequencies of light are observed. The light is emitted from electrons when they return to the ground state energy level. • If all colors of light were of light were observed (as with a rainbow) then Bohr would have concluded that there were no energy levels 13. An atom emits 3 colors of light, Red, Blue and Violet when excited by an E.M. wave. Draw the Bohr Model of an atom that shows these colors of light being emitted • See the “Electron: How does it behave” Notes. This packet covers EM Waves and the Bohr Model. 14. Draw a Bohr Model & Lewis Dot model of Phosphorous, Potassium, Neon, Calcium. • See Lewis and Bohr Worksheet. You should have a stamp on this! 15. Now Draw a Bohr model for P-31 and Cl-37 including: • Labeled subatomic particles in correct amounts • Labeled regions P-31 Cl-37 16. What is a valence electron? • The outermost energy level electrons of a Bohr Model. These are the electrons that are shown in a Lewis Dot Model. A valence electron in an electron found on the highest or outermost energy level. An atom can have a maximum of 8 valence electrons. 17. What is the valence electron pattern that is observed as you move vertically on the periodic table? Horizontally? • There are the same amount of valence electrons within a vertical column\ • Valence electrons increase moving left to right. Fill in the chart. Symbol Atomic Number Mass Number Protons Neutrons Electrons Ne 10 20 10 10 10 Al 13 27 13 14 13 Na 11 21 11 10 11 Draw and label a diagram of each atomic model. . ~ . A I~CI ~i~.J.\..u i'4lMt ,,~~~ t.oI\-N-lbv f.tJ\,\ Sc.i~t-rs+a"~ ~ E"J{pui~~+. . 4. plum pudding model i I ) ('J~l4~ iVf Q, Le.- ....t r ~ 1'1 j • I u ..s I 5. nuclear atomic model ! 1 ~ lvt 1>~"'<t.e / ~vt~-.)s. ,. , i I Calculate the atomic mass of each element described below. Then use the periodic table to identify each element. 32. Mass (amu) Isotope 63X . 62.930 69.17 6SX 64.928 30.83 (~ '2 • q ::, 0 + _~ (" 4 _' 9 '2. '6 ",oM 33. Percent Abundance Isotope ,I 0" ~ C1 'l) '-1 " V c.IM-U o. Mass (amu) Percent Abundance 35X 34.969 75.77 37X 36.966 24.23 'S Cc.'6S) - , (3Y ~ >4- ( - 100 L, t"1 ~ (p , C( ~ (D Ct!M..U ~iML1 1 "- J O.lc.;7l ) O ~ ' ~ l S) ". .3 5. Y Sq'MV, = Chemistry: Matter and Change· Cha pter 4 F == - - Study Guide