Midterm Review Questions Name:________________ Matter and its Properties 1. Define matter, element, compound, mixture to compare the four terms. 2. Name the phase changes and indicate what physical states of matter are changing. 3. What is the difference between chemical change and physical change? Elements 4. On the table below, diagram metals, nonmetals, and metalloids. 5. Indicate with arrows the directions of groups and periods. 6. Name groups 1, 2, 17, 18. Scientific Measurements 7. How many significant figures are in the number 13500L ? _________ How did you know? How many significant figures are in the number 0.100L ? _________ How did you know? 8. Write this number in Scientific Notation: How did you know? Write this number in Scientific Notation: How did you know? 0.000432 12001 Structure of the Atom 9. What is the mass, charge, and location of an electron? 10. What is the mass, charge, and location of a proton? 11. What is the mass, charge, and location of an neutron? 12. Draw a Bohr Diagram of chlorine- label protons, nucleus, electrons, electron cloud Counting Atoms 13. Label then define: Atomic Mass, and Atomic Number 21 Sc 44.956 14. What are isotopes, give an example. How many neutrons are in Uranium-238 ? (Show your work) Nuclear Chemistry 15. Why do unstable nuclides undergo nuclear reactions? Explain P& N Ratio 16. What is the product of this radioactive decay? What type is it? _________ Quantum Numbers 17. How many electrons fit in the 1st energy level of an atom?____ How many electrons fit in the 2nd energy level of an atom?____ How many electrons fit in the 3rd energy level of an atom?____ Circle the answer with the highest amount of energy. 18. Outline then label the blocks of each orbital on the table below. Draw the shape of each atomic orbital below: Electron Configuration 19. Write the Long hand electron configuration of Bromine 20. Write the short hand electron configuration of Lead Periodic Properties 21. Explain the group and periodic trend of atomic radii in relation to the periodic table. 22. Explain the group and periodic trend of ionization energy in relation to the p. table. 23. What is electronegativity, what does it have to do with chemical bonding? Intro to Chemical Bonding 24. Describe and compare the 3 types of chemical bonding: 25. Compare Polar vs. Non-Polar covalent bonds 26. Is HCl a polar or non-polar molecule? Show your work (electronegativities) 27. What kind of structure is formed by covalent bonds?_________________ Covalent Bonding 28. What is the octet rule? 29. Draw the Lewis Structure for: SiF4 SO2 N2 30. Name the following molecules CO2 H 2O CF4 C2O2 Water 31. Draw a molecule of water and label its polarity. What are properties of water due to this polarity?