1. Unit 2 Practice Review Ch. 3,4,5 no periodic trends

2. Do Now (5 min)
How much energy is given off by an electron emitting a wave with a frequency of 7.00 x 1014 Hz?
As the wavelength of light increases,
The frequency increases
The speed of light increases
The energy decreases
The intensity increases
Justify your answer with a diagram. 1st person with correct drawing can go to the board for 5 pts

3. Announcements Test 2 Thursday 11/29 Friday 11/30
Unit 2 atomic structure: Bohr and Quantum Theory
Test 2
Thursday 11/29 Friday 11/30

4. Review Questions
If you work efficiently, we may have time to play a jeopardy game at the end of class 

5. Electromagnetic Spectrum Questions (10 min)

6. Electromagnetic Spectrum
Write the equation relating the speed of light with frequency and wavelength. Write the equation relating energy and frequency. Label the variables in each.
The speed of light always equals ____________.
Answer questions #11-14 on p. 157.
Which has more energy, a radio wave or a gamma ray?
If a radio wave has a frequency of 106 Hz, what is its wavelength? How much energy does it carry?
If purple light has a wavelength of 4.00 x 10-7 m, how much energy does it have?

7. Bohr Model vs. Quantum Model Questions (10 min)

8. (5 min)
How many electrons are needed to fill the first, second, and third principal energy levels in the Bohr Model of the atom?
Draw the Bohr Models for Aluminum and Neon.
What is an “orbital” (in the Quantum Mechanical Model)? How is it different than an “orbit” (in the Bohr Model)?
How does the Bohr Model of the atom differ from the Quantum Mechanical Model? List at least three ways.

9. (5 min)
How many electrons can fit into the s, p, and d sublevels? How is this information shown on the periodic table?
How many orbitals do the s, p, d, and f sublevels have? What is the relationship between the number of orbitals a sublevel has and the number of electrons that sublevel can hold?
How is the amount of an energy an electron has related to the orbit(al) that electron is in (in both the Bohr Model and Quantum Mechanical Model of the atom)

10. Electron Configuration Questions (10 min)

11. (5 min)
Make a rough sketch of the periodic table and label the different sections: s, p, d, and f.
What do the 1, s, and 2 mean, respectively, in this electron configuration: 1s2?
Write electron configurations for the following elements: Lithium, Carbon, Neon, Silicon, Iron.

12. (5 min)
Write the Noble Gas Configuration (shortcut) configurations for Silicon and Iron.
Write electron configurations for elements with the following numbers of electrons: 4, 7, 16.
Where on the periodic table would you expect to find an element whose ground-state electron configuration ended in 4p5? 3s1?

13. Orbital Diagram Questions (10 min)

14. How many boxes do the s, p, and d sublevels get
How many boxes do the s, p, and d sublevels get? How do these numbers compare to the number of orbitals in those sublevels?
Identify the problem in each of the following orbital diagrams. Which rule(s) is(are) being violated? b. c.

15. Write the symbol for the elements with the following orbital diagrams:

16. How many unpaired electrons (single electrons in an orbital) do each of the following elements have: Na, Ca, O?

17. Groups, Families and Valence Electron Questions (10 min)

18. How is the Periodic Table organized?
Describe in 5 words or less where to find each of the following on the periodic table: Metals, Nonmetals, Metalloids (semi-metals).
List three common physical properties of metals. Do the same for nonmetals.
Match the following families (groups) to their columns on the periodic table:
Halogens
Noble Gases
Alkali Metals
Alkaline Earth Metals
Transition Metals (list the range of columns)

19. Are the elements in a group (column) or period (row) on the periodic table more similar to each other? Explain. Skip 1st question.
How does reactivity change as you go down the periodic table? Which element is more reactive than potassium, but less reactive than Cesium?
What family would elements with the following electron configuration belong to:
1s2 2s2
1s2 2s2 2p5
1s2 2s2 2p6
[Ne] 3s1
[Ne] 3s2 3p6
[Ar] 4s2 3d6

20. What is a valence electron
What is a valence electron? Where can you look on the periodic table to figure out how many valence electrons an element has?
How many valence electrons do the following elements have: Sodium, Calcium, Neon, Fluorine, Chlorine, Oxygen, Phosphorous?

21. Unit 2 Review
Created by Educational Technology Network

22. Electron Configuration Periodic Table/Trends Electromagnetic Spectrum
POWERPOINT JEOPARDY
Atom Models
Electron Configuration
Orbital Diagram
Periodic Table/Trends
Electromagnetic Spectrum 10 10 10 10 10 20 20 20 20 20 30 30 30 30 30 40 40 40 40 40 50 50 50 50 50

23. Name the 4 orbitals and describe the shapes – 10 Points

24. Sodium (Na) has how many electrons in the third energy level
Sodium (Na) has how many electrons in the third energy level? – 20 Points

25. Copper has how many electrons in the 3d sublevel? – 30 Points

26. Draw the Bohr model for Argon (Ar)– 40 Points

27. Draw the quantum model for Neon– 50 Points

28. What is the electron configuration for Neon (Ne) – 10 Points

29. Write the electron configuration for an element that would have 14 protons – 20 Points

30. Silicon has an electron configuration of 1s22s22p63s23p2
Silicon has an electron configuration of 1s22s22p63s23p2. How many electrons does silicon have in its highest sublevel? – 30 Points

31. Write the electron configuration for Bromine (Br) – 40 Points

32. Which element would have the following shortcut electron configuration: [Ar]4s23d104p4– 50 Points

33. Which rule is being violated in the orbital diagram below? – 10 Points
    _  _
1s s p s

34. Which element is represented by the following orbital diagram – 20 Points
        
1s s p s p

35. Which rule is being violated in the orbital diagram below? – 30 Points
        
1s s p s p

36. Which rule is being violated in the orbital diagram below?– 40 Points
        ___
1s s p s p

37. Draw the orbital diagram for Silicon – 50 Points

38. What are the rows and columns called in the periodic table – 10 Points

39. Which has the greater Ionization Energy. Electronegativity
Which has the greater Ionization Energy? Electronegativity? Atomic radius? Fluorine or Oxygen?– 20 Points

40. If I am an element that is shiny, hard, and a good conductor of heat and electricity, what kind of element am I? – 30 Points

41. If I react vigorously with water, what family am I in and where can you find me on the periodic table and how many valence electrons do I have? – 40 Points

42. What family does the following element belong to and how many valence electrons does it have: 1s22s22p63s23s5– 50 Points

43. What is the wavelength for a wave with a frequency of 2 x 103 Hz– 10 Points

44. What is the frequency for a wave with a wavelength of 100 m – 20 Points

45. What is the energy if the frequency is 4 x 1010 Hz? – 30 Points

46. What is the frequency if the energy is 2 x 10-19?– 40 Points

47. What is my energy if my wavelength is 300 m– 50 Points

48. Periodic Trends Questions (10 min)
Answer the questions from the sheet on a separate sheet of paper that you will turn in at the end of class.

49. Periodic Trends Questions
Define electronegativity, atomic radius, and ionization energy.
How does electronegativity vary from left to right on the periodic table?
How does atomic radius vary across a period and down a group in the table?
Which two atomic properties have similar trends? Offer a possible explanation for this similarity.
Why do noble gases have the highest ionization energy?
Which is more reactive? Lithium or Potassium? Oxygen or Fluorine?

50. Electromagnetic Spectrum Questions (10 min)
Answer the questions from the sheet on a separate sheet of paper that you will turn in at the end of class.

51. Electromagnetic Spectrum
Write the equation relating the speed of light with frequency and wavelength. Write the equation relating energy and frequency. Label the variables in each.
The speed of light always equals ____________.
Answer questions #11-14 on p. 157.
Which has more energy, a radio wave or a gamma ray?
If a radio wave has a frequency of 106 Hz, what is its wavelength? How much energy does it carry?
If purple light has a wavelength of 4.00 x 10-7 m, how much energy does it have?