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10/12 Review: What is atomic radius?

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mrheffner

The document contains data from multiple quizzes and exams, showing the class's goal score of 80% and their actual scores just below the goal. It also contains information about an upcoming mid-term exam covering three units of material and notes the need to ask questions if anything is not understood to improve scores. The document discusses trends in atomic radius, explaining that radius decreases left to right across periods and increases top to bottom in groups on the periodic table. It includes examples comparing elements to determine which has a smaller or larger atomic radius.

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Launch: 10/12 1.  What is the main difference? Unit #2 Exam Data: 2.  What is the biggest reason for the difference? Quiz #4 Data: Our Goal: 80% Our Score: 79.29%
Launch: 10/12 1.  What is the main Unit #2 Exam Data: difference? 2.  What is the biggest reason for the difference? Quiz #4 Data: Our Goal: 80% Our Score: 79.29%
Launch: 10/12 1.  What is the main difference? Unit #2 Exam Data: 2.  What is the biggest reason for the difference? Quiz # 4 Data: Our Goal: 80% Our Score: 79.17%
Launch: 10/12 1.  What is the main difference? Unit #2 Exam Data: 2.  What is the biggest reason for the difference? Quiz # 4 Data: Our Goal: 80% Our Score: 79.00%
Mid-Term Exam Info   Cumulative exam   Unit #1: Atomic Structure   Unit #2: The Periodic Table   Unit #3: Nuclear Processes   Opportunity to change your grade   We don’t have much time!   If you don’t understand something, ask!   No copying
What is the trend in atomic radius? Mr. Heffner 10/12/09
Review: Period vs. Group   Period = row (left to right)   Group = column (top to bottom)
Atomic Radius   Atomic radius is…   the size of an atom. 0 0 0 0   big radius = big atom
Atomic Radius   The trend: 1.  Atomic radius decreases across a period (LR) 2.  Atomic radius increases down a group (Top  Bottom) Decreases Increases
Example Which has a smaller atomic radius, fluorine (F) or nitrogen (N)?   Step #1: Find the elements
Example Which has a smaller atomic radius, fluorine (F) or nitrogen (N)?   Step #2: Look at the keyword Which has a smaller atomic radius, fluorine (F) or nitrogen (N)?
Example Which has a smaller atomic radius, fluorine (F) or nitrogen (N)?   Step #3: Identify which is closest to He
Example Which has a larger atomic radius, sodium (Na) or potassium (K)?   Step #1: Find the elements
Example Which has a larger atomic radius, sodium (Na) or potassium (K)?   Step #2: Look at the keyword Which has a larger atomic radius, sodium (Na) or potassium (K)?
Example Which has a larger atomic radius, sodium (Na) or potassium (K)?   Step #3: Identify which is closest to Fr
Practice Questions   Review Worksheet #1   Use the 3-step method!
Atomic Radius   The trend: 1.  Atomic radius decreases across a period (LR) 2.  Atomic radius increases down a group (Top  Bottom) Decreases Increases
Homework   Review your notes   Finish Review Worksheet #1   Make a problem from scratch like question 6 or 7 on the worksheet. Solve it!

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10/12 Review: What is atomic radius?

  • 1. Launch: 10/12 1.  What is the main difference? Unit #2 Exam Data: 2.  What is the biggest reason for the difference? Quiz #4 Data: Our Goal: 80% Our Score: 79.29%
  • 2. Launch: 10/12 1.  What is the main Unit #2 Exam Data: difference? 2.  What is the biggest reason for the difference? Quiz #4 Data: Our Goal: 80% Our Score: 79.29%
  • 3. Launch: 10/12 1.  What is the main difference? Unit #2 Exam Data: 2.  What is the biggest reason for the difference? Quiz # 4 Data: Our Goal: 80% Our Score: 79.17%
  • 4. Launch: 10/12 1.  What is the main difference? Unit #2 Exam Data: 2.  What is the biggest reason for the difference? Quiz # 4 Data: Our Goal: 80% Our Score: 79.00%
  • 5. Mid-Term Exam Info   Cumulative exam   Unit #1: Atomic Structure   Unit #2: The Periodic Table   Unit #3: Nuclear Processes   Opportunity to change your grade   We don’t have much time!   If you don’t understand something, ask!   No copying
  • 6. What is the trend in atomic radius? Mr. Heffner 10/12/09
  • 7. Review: Period vs. Group   Period = row (left to right)   Group = column (top to bottom)
  • 8. Atomic Radius   Atomic radius is…   the size of an atom. 0 0 0 0   big radius = big atom
  • 9. Atomic Radius   The trend: 1.  Atomic radius decreases across a period (LR) 2.  Atomic radius increases down a group (Top  Bottom) Decreases Increases
  • 10. Example Which has a smaller atomic radius, fluorine (F) or nitrogen (N)?   Step #1: Find the elements
  • 11. Example Which has a smaller atomic radius, fluorine (F) or nitrogen (N)?   Step #2: Look at the keyword Which has a smaller atomic radius, fluorine (F) or nitrogen (N)?
  • 12. Example Which has a smaller atomic radius, fluorine (F) or nitrogen (N)?   Step #3: Identify which is closest to He
  • 13. Example Which has a larger atomic radius, sodium (Na) or potassium (K)?   Step #1: Find the elements
  • 14. Example Which has a larger atomic radius, sodium (Na) or potassium (K)?   Step #2: Look at the keyword Which has a larger atomic radius, sodium (Na) or potassium (K)?
  • 15. Example Which has a larger atomic radius, sodium (Na) or potassium (K)?   Step #3: Identify which is closest to Fr
  • 16. Practice Questions   Review Worksheet #1   Use the 3-step method!
  • 17. Atomic Radius   The trend: 1.  Atomic radius decreases across a period (LR) 2.  Atomic radius increases down a group (Top  Bottom) Decreases Increases
  • 18. Homework   Review your notes   Finish Review Worksheet #1   Make a problem from scratch like question 6 or 7 on the worksheet. Solve it!