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Chemistry Final Exam Review
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Chemistry Final Exam Review Presentation Transcript

  • 1. The Moment of Truth Chemistry Style!
  • 2. The electron configuration of iron is [Ar]4s 2 3d 6 . What is the electron configuration for Fe 2+ ?
    • [Ar]3d 6
      • Valence electrons are in the highest energy level!
  • 3. Which Alkali Metal has the largest radius?
    • Francium
      • Atomic Radius increases down a group!
  • 4. What is the abbreviated electron configuration of the sulfide ion?
    • [Ar]
    • Sulfide is S 2-
    • When forming ions, main group elements obtain noble gas configurations!
  • 5. Where are the most electronegative elements found on the periodic table?
    • Top Right Corner
    • These are the smallest atoms and are the most reactive nonmetals!
  • 6. What is the ground state electron configuration of the element with atomic number 41?
    • 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 3
    • Atomic number 41 means 41 protons.
    • In a neutral atom the number of protons and electrons are equal!
  • 7. In a group, how does mass effect the number of core electrons? How does it effect the number of valence electrons?
    • As mass increases in a group so does the number of core electrons.
    • All elements in a group have the same number of valence electrons no matter what the mass is!
  • 8. Which element has the highest electronegativity? Cl, Ca, Sn, or Po
    • Cl! It is the smallest atom!
    • Since electronegativity and ionization energy follow the same pattern, Cl also has the highest first ionization energy!
  • 9. What is the symbol for an element with 12 protons, 13 neutrons, and 10 electrons?
    • Mg 2+
    • Protons ALWAYS determine the identity of a atom or ion!
    • The difference between the number of protons and electrons determines the charge!
    • Neutrons can vary and only effect the mass number.
  • 10. Give an example of a compound with ionic and covalent bonding.
    • Na 2 SO 4
    • Polyatomic ions always contain covalent bonding because they are made of nonmetals.
    • The cation and the polyatomic ion bond together ionically.
  • 11. How can you determine if a compound has ionic bonding or covalent bonding?
    • A compound with ionic bonding consists of a metal and nonmetal.
    • A compound with covalent bonding consists of nonmetals only!
  • 12. Give the shape of each of the following. H 2 Se, CH 4 , AsI 3 , CS 2 , BH 3
    • Bent, Tetrahedral, Trigonal Pyramidal, Linear, Trigonal Planar
    • Not sure about the Se, As, and S? Replace them with the first element in the group to help you out.
      • For example Se and O are in the same group, so they bond with H in the same way and you know that H 2 O is bent, so H 2 Se is also!
  • 13. Which of the following are soluble in a nonpolar solvent? H 2 O, CH 4 , CO 2 , NH 3 , NaCl
    • CH 4 and CO 2
    • Both are nonpolar and like dissolves like!
  • 14. Put the following intermolecular forces in order from weakest to strongest: Dipole, Hydrogen, London
    • London, Dipole Hydrogen
  • 15. Identify the element with the following electron configuration: 1s 2 2s 2 2p 6 3s 2 3p 5
    • Chlorine, Cl
    • NOT Cl - , the problem is asking for an element, not an ION!
  • 16. Fill in the blanks with letters:
    • A: pH 14-5.05 = 8.95
    • B: [OH - ] = 10^ -5.05 = 8.91 x 10 -6 M
    • C: [OH - ]=1.01 x 10 -6 M
    • [H + ][OH - ] = 1.0 x 10 -14
    C B A
  • 17. Which values in the diagram will change with the addition of a catalyst?
    • Only activation energy, E a
    • H reactants, H products, and ∆H are unchanged.
  • 18. Na 2 CO 3 + HCl  NaCl + H 2 O + CO 2 1. 0.455g sodium carbonate are titrate to the endpoint with 14.00mL of HCl, what is the concentration of the HCl
    • 0.613M HCl
  • 19. 2. What mass of KCl is need to prepare 250.mL of 0.300M solution?
    • 5.55g KCl
  • 20. 3. What volume of 0.500M NaOH is needed to prepare 250.mL of 0.200M solution?
    • 100. mL
  • 21. 4. For the reaction I 2 + Br 2 ↔ 2IBr, K eq = 66.8 If the concentration of I 2 and Br 2 are each 0.199M, what is the concentration of IBr?
    • 1.63M IBr
  • 22. Balance the following redox reaction: ClO 3 - + Fe  Cl - + Fe 2+
    • 6e - + 6H + + ClO3-  Cl - + 3H 2 O
    • (Fe  Fe 2+ + 2e - ) x3
    • 6H + + ClO 3 - + 3Fe  Cl - + 3H 2 O + 3Fe 2+