Second term review
Upcoming SlideShare
Loading in...5
×
 

Like this? Share it with your network

Share

Second term review

on

  • 842 views

 

Statistics

Views

Total Views
842
Views on SlideShare
842
Embed Views
0

Actions

Likes
0
Downloads
51
Comments
0

0 Embeds 0

No embeds

Accessibility

Categories

Upload Details

Uploaded via as Microsoft Word

Usage Rights

© All Rights Reserved

Report content

Flagged as inappropriate Flag as inappropriate
Flag as inappropriate

Select your reason for flagging this presentation as inappropriate.

Cancel
  • Full Name Full Name Comment goes here.
    Are you sure you want to
    Your message goes here
    Processing…
Post Comment
Edit your comment

Second term review Document Transcript

  • 1. Second Term Review<br />Instructions: Answer the following questions, thoroughly, you may either type your answers or answer them by hand (make sure your writing is legible). DO ALL THE PROBLEMS!<br />Review is due on Thursday September 30th, 2011.<br />
    • Define the following words:
    • 2. Quantum Numbers
    • 3. Principle Quantum Number
    • 4. Angular Momentum Quantum Number
    • 5. Magnetic Quantum Number
    • 6. Spin Quantum Number
    • 7. Aufbau Principal
    • 8. Pauli Exclusion Principal
    • 9. Hund’s Rule
    • 10. Atomic Radius
    • 11. Ionization Energy
    • 12. Ionic Radius
    • 13. Electronegativity
    • 14. Oxidation number (oxidation state)
    • 15. Chemical bond
    • 16. Draw the Aufbau diagram up to the 6th energy level.
    • 17. How are elements arranged in the periodic table?
    • 18. What are the three types of elements found on the periodic table?
    • 19. Which elements are the most electronegative?
    • 20. What group of elements is also known as inert gases?
    • 21. Why don’t the transition elements always follow the rules for valence electrons?
    • 22. What are valence electrons? How many valence electrons does Francium have?
    • 23. Do the electron dot structure of the following:
    • 24. Carbon
    • 25. Iodine
    • 26. Calcium
    • 27. Gallium
    • 28. Write the element’s orbital notation and electron notation:
    • 29. Beryllium
    • 30. Nitrogen
    • 31. Aluminum
    • 32. Sodium
    • 33. Do the following noble-gas notation of the following elements:
    • 34. Rh
    • 35. P
    • 36. Zr
    • 37. Which electron notation describes an element in the excited state?
    • 38. [Ar]4s23d104p2
    • 39. [Ne]3s23p5
    • 40. [Kr]5s24d1
    • 41. [Ar]4s12d84p1
    • 42. Given any two elements within a group, is the element with the larger atomic number likely to have a larger o smaller atomic radius than the other?
    • 43. The metal used to make soda can has the electron configuration [Ne]3s23p1. Identify the metal and give its group, period, and block.
    • 44. Do the orbital notation of Sulfur and state how it becomes an ion. Tell whether its ion is an anion or a cation. What is sulfur’s oxidation number?
    • 45. With their orbital notation, show the reaction to form calcium fluoride.
    • 46. Give the names of the following ionic compounds
    • 47. MgO
    • 48. KI
    • 49. AgCl
    • 50. NaClO
    • 51. KNO3
    • 52. BaOH2
    • 53. Give the formula for the following ionic compounds
    • 54. Calcium iodide
    • 55. Copper(II) chloride
    • 56. Potassium periodate
    • 57. Silver (I) acetate
    TIPS FOR GOOD GRADES:<br />
    • Review the chapters and your notes
    • 58. Do the review
    • 59. Ask questions
    • 60. Help each other out (STUDY GROUPS)
    • 61. Don’t stress out!!!!