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Chemistry Midterm Review

Learn the fundamentals of chemistry with topics such as fission, fusion, nuclear reactions, electron configurations, periodic table trends, and chemical bonding.

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Chemistry Midterm Review

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  1. Chemistry Midterm Review

  2. Explain the difference between fission and fusion • Fission is splitting of a big nucleus into 2 smaller ones • Fusion is combining 2 nuclei to make one bigger one

  3. Write a balanced decay equation for the decay of Pb-210 Beta decay forming Bi-210

  4. A sample of I-131 decays to 1 g in 40 days. What was the mass of the original sample? • 1g 2g 4g 8g 16g 32g • 40 32 24 16 8 time 0

  5. Write the symbol, mass and charge for the alpha, beta and gamma particles • Alpha mass = 4, charge = 2 • Beta mass = 0, charge = -1 • Gamma mass = 0 charge = 0

  6. Nuclear reactions release large amounts of energy. Why? • Mass is converted to energy

  7. Name the 5 types of reactions • Synthesis • Decomposition • Single replacement • Double replacement • combustion

  8. Complete and balance the following reaction: sodium chloride and barium • 2 NaCl + Ba 2 Na + BaCl2

  9. What 2 products always form in a combustion reaction? • Carbon dioxide • water

  10. Balance and Identify the type of reaction:Chromium and oxygen yields chromium (III) oxide • 4Cr + 3 O2 2 Cr2O3 • synthesis

  11. If it has mass and takes up space it is called…. • matter

  12. How many e- pairs in and F orbital? • 7

  13. Draw Lewis Dot structure of N and C

  14. What element is represented by [Ne] 3s2 3p4 S

  15. How many neutrons are in Se-79? 45

  16. What were 2 conclusions from Rutherford’s Gold Foil Experiment? • Atoms have small dense + charged nucleus • Atoms are mostly empty space

  17. Draw orbital notation for e- in oxygen atom • 1s2 2s2 2p4

  18. How many valence e- are in gold and what orbitals are they in? 6s1 or 6s2

  19. The first element to contain a pair of e- in a d orbital is: Ti

  20. Isotopes of B are B-11 (80.2%) and B-10 (19.8 %). Show set up for calculating ave atomic mass (11 x 80.2) + (10 x 19.8) ______________________ 100

  21. Which atom has the smallest radius: Cs, Fr, Ba, Ra, and explain why • Ba, because Ba has more protons than Cs, pulling e- closer and making it smaller • Ba also has less energy levels than Ra

  22. What is the definition of atomic radius? • One-half the distance between the nuclei of 2 adjacent atoms

  23. Name the 3 types of elements on the periodic table • Metals, non metals, and metalloids

  24. List 3 properties of metals • Malleable, • ductile, • Conductors • luster

  25. List 2 properties of non metals • Brittle • Poor conductors • No luster

  26. Which group contains elements in all 3 phases of matter at room temperature? 17

  27. The elements in the modern Periodic Table are arranged according to: Atomic number

  28. Describe the ionization energy of metals: low

  29. What happens to atomic radius from left to right across a period? Why? Radius gets smaller because more protons pull electron closer in

  30. Which element has an ionic radius that is larger than its atomic radius?K, Zn, Cl, Cr Cl

  31. Define electronegativity • An element’s ability to attract e- in a compound

  32. Which element has the largest atomic radius: Li, O, C, F, N? Why? Li, because the others have more protons pulling e- in closer

  33. What is the trend in ionization energy as you go across period 3? Why? • Increases, because more protons pulling on e-

  34. What is the trend in ionization energy as you go down group 16? Why? • Decreases, because of shielding, e- farther from nucleus and easier to remove

  35. What intermolecular force acts on molecules of hydrogen gas? Van Der Waals

  36. Which bond has the greatest ionic character: Al-F, C-O, K-Br, C-N? Al-F

  37. Use poetic language to describe the metallic bond • Positive ions immersed in a sea of mobile electrons

  38. Give an example of a polar covalent bond H-Cl

  39. Ionic bonds form between what two types of elements? • Metal and non metals

  40. What are the 7 diatomic elements H, O, N, F, Cl, Br, I

  41. When does hydrogen bonding occur? • H • + N, O or F

  42. Draw a Lewis Dot structure of calcium fluoride

  43. Draw a Lewis dot structure of the ammonium ion

  44. What kind of bond will form between H and N? Polar covalent

  45. Write formula for Cobalt (III) fluoride CoF3

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