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Transcript
KEY Atomic Structure & Electron Arrangement Test Review Practice Questions: 1. The atomic number is equal to the number of protons. 2. The mass number is equal to the protons+ neutrons. 3. Electrons in the outermost energy level are known as valence electrons and are available to be lost, gained or shared when molecules are formed. 4. What causes an atom to be neutrally charged? An equal number of protons and electrons 5. Describe how an atom would become negatively charged. To be negatively charged, an atom must have gained more electrons. Identify the major contribution of each of the following to current atomic theory (be sure to include any model that they proposed and the experiment that they did): 6. Aristotle – everything was made from earth, wind, fire, water, and ether; alchemist 7. Democritus – first to propose the idea of an atom (indivisible particle)! 8. Dalton – developed the basis for the modern atomic theory 9. Thomson - used the cathode ray tube to discover the first subatomic particle the electron; developed the Plum Pudding Model 10. Rutherford - Gold foil experiment- expected all of the radiation to pass through and was very surprised when some of the particles were deflected led to the discovery of the NUCLEUS (centrally located positive charge) and the concept that the atom is mostly empty space. Also discovered the proton and neutron. 11. Bohr - His atomic model (planetary model) had atoms built up of successive orbital shells of electrons. Electrons move between shells based on specific amounts of energy being lost or gained. 12. Electron Cloud Model - This model is based on quantum mechanics which states that you cannot know the speed and location of a particle. So this model shows the most probable location of the electrons. 13. List the four/five points of Dalton’s Atomic Theory and indicate which ones are known to be incorrect today. • All matter is composed of tiny particles called atoms. TRUE • Atoms of an element are identical in size, mass and other properties. FALSE (isotopes) • Atoms cannot be created, destroyed or subdivided. FALSE (subatomic particles) • Atoms of different elements can combine in simple whole number ratios to form compounds. TRUE • In chemical reactions, atoms are combined, separated or rearranged. TRUE Compare the subatomic particles according to the following criteria: LOCATION IN THE ATOM, CHARGE AND MASS. 14. Proton – in the nucleus, positive charge, mass = 1 amu 15. Neutron - in the nucleus, neutral, mass = 1 amu 16. Electron – in the electron cloud around the nucleus, negative charge, mass = 0 amu Complete the following chart: Isotope Name Carbon-13 Nitrogen - 17 Boron - 11 Francium - 223 Nuclear Atomic Mass # of # of # of Symbol Number Number Protons Neutrons Electrons C 6 13 6 7 6 N 7 17 7 10 7 B 5 11 5 6 5 Fr 87 223 87 136 87 13 6 17 7 11 223 5 87 17. There are three common isotopes of hydrogen: protium – 1H, deuterium – 2H, and tritium – 3H. Based on the average atomic mass given on the periodic table, predict which isotope is most common and explain your answer. Since the average atomic mass is closest to 1 amu, protium must be the most common because the weighted average will be closest to the most abundant isotope. 18. An element consists of three naturally occurring isotopes with the following mass numbers: 24, 25 and 26. The relative abundances of these three isotopes are 78.70, 10.13 and 11.17 percent respectively. Calculate the average atomic mass and identify the element. Show your work! (24 x .7870) + (25 x .1013) + (26 x .1117) = 24.3247 amu - Magnesium Use this graph of mass spec data to answer questions #17 – 20. 19. What masses of isotopes are observed? 35 amu and 37 amu 20. What percentage of each isotope is observed? 35 Cl – 75% 37Cl – 25% 21. What is the average atomic mass of the element? SHOW ALL WORK! (35 x .75) + (37 x .25) = 35.5 amu 22. Atoms of what element is presented in the graph? Chlorine 23. Write T for true or F for false. If a statement is false, replace the underlined word with one that will make the statement true, and write your correction in the blank provided. a. If two electrons occupy the same orbital, they must have opposite spins. TRUE b. Electrons occupy the highest energy level possible. FALSE - lowest c. Single electrons in an orbital of equal energy spin in opposite directions. FALSE – the same 24. Complete the following table Energy level Number of Name of Number of Max number sublevels sublevels orbitals Of electron 1 1 s 1 2 2 2 s,p 4 8 3 3 s,p,d 9 18 4 4 s,p,d,f 16 32 25. Answer the following short answer questions a. What is the shape of an “s” orbital? Sphere b. What is the shape of a “p” orbital? dumbbell 26. Draw orbital diagrams for a. Beryllium b. Carbon c. Aluminum 27. Write electron configurations (full and Noble gas) for a. Lithium a. 1s22s1 b. [He] 2s1 b. Arsenic a. 1s22s22p63s23p64s23d104p3 b. [Ar] 4s23d104p3 c. Silver a. 1s22s22p63s23p64s23d104p65s24d9 b. [Kr] 5s24d9 d. Uranium a. 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s25f4 b. [Rn] 7s25f4 28. Draw the electron dot diagrams for the following a. Lithium b. Arsenic c. Argon d. Calcium