Download Orbitals and Electrons

 Name _____________________________ Class Period 1 2 3 4 5 6 Date _________ Notebook Page_______ Orbitals and Electrons https://goo.gl/y5u2QU Energy Levels 1. Complete the chart. # of Orbitals Total Electrons Nucleus 1st Energy Level 2nd Energy Level 3rd Energy Level 2. Which energy level is closest to the nucleus? Orbitals 1. What is an orbital? 2. In what ways does the author compare orbitals to a loveseat? 3. Complete the chart Shape Energy Level s orbital p orbital 4. What is Hund’s Rule? 5. How many orbitals are in the d orbital? 6. How many orbitals are in the f orbital? Notation Styles 1. The author gives the example of boron. How many electrons does Boron have? How does that relate to the atomic number? 2​ 2​ 1​
2. The author says the electron placement notation for boron is 1s​
2s​
2p​
. If you add the superscript (numbers in small font, at an elevated level) numbers together what does this represent? Where else have you seen that number? 3. Review the second style of orbital notation. How is it similar and different from the first? Reflection 1. What shape is the s orbital? 2. What shape is the p orbital? 3. Why is it that the p orbital has an x, y, and z? 4. How does the x, y, and z axis apply to what you know about math? 5. Revisit the interactive periodic table that shows the orbital configuration (​
https://goo.gl/SccILb​
) a. Look at the element Ca (Calcium). What’s it’s atomic number? How does that relate to the number of electrons it has? b. Place your cursor over H (upper left hand corner) and move down from row 1 to toward Fr in row 7 while watching the electron configuration. What do you notice? c. Does this same idea with the rows (across) carry through the rest of the table? d. When you examine the Orbital configuration area it starts with number 1 at the bottom and moves up to seven. i. Why is there only one box next to the one? Why does that same single box carry up? What level is this? How do you know? ii.
Just above the single box next to the number two there’s a string of three boxes. What level is this? How do you know? iii.
What orbital is represented by the string of five boxes? iv.
What orbital is represented by the string of seven boxes? TEACHER COPY­Do Not Duplicate 1. Complete the chart. # of Orbitals Total Electrons N/A N/A 1st Energy Level 1 2 2nd Energy Level 4 8 3rd Energy Level 9 18 Nucleus 2. Which energy level is closest to the nucleus? The first energy level. Orbitals 1. What is an orbital? It’s an area of probability where an electron can be found. 2. In what ways does the author compare orbitals to a loveseat? Loveseats can only seat two people, in the same way electron orbitals can only hold two electrons. 3. Complete the chart Shape Energy Level s orbital round 1st p orbital propeller blade 2nd 4. What is Hund’s Rule? Why do they refer to it as the “good mother” rule? P orbitals must receive one electron in each orbital before getting a second. In the same way that everyone should get a first helping before they get a second according to your mother. 5. How many orbitals are in the d orbital? Five 6. How many orbitals are in the f orbital? Seven. Notation Styles 1. The author gives the example of boron. How many electrons does Boron have? How does that relate to the atomic number? Boron has 5 electrons and it’s atomic number is 5. 2​ 2​ 1​
2. The author says the electron placement notation for boron is 1s​
2s​
2p​
. If you add the superscript (numbers in small font, at an elevated level) numbers together what does this represent? Where else have you seen that number? The numbers sum is 5, 5 is also the atomic number of Boron. 3. Review the second style of orbital notation. How is it similar and different from the first? Both styles show the same information. The second style uses arrows to show the number of electrons in each orbital. The second style also visually shows there are three p orbitals (x, y, z axis). Reflection 1. What shape is the s orbital? Round. 2. What shape is the p orbital? Propeller or dumbbell. 3. Why is it that the p orbital has an x, y, and z? The p orbital has three orbitals, and they are on the horizontal (x axis), vertical (y axis) and diagonal (z axis). 4. How does the x, y, and z axis apply to what you know about math? In a typical graph you would have a x and y axis. You could graph an ordered pair (x,y) in a two dimensional system. A z axis adds a third dimension. 5. Revisit the interactive periodic table that shows the orbital configuration (​
https://goo.gl/SccILb​
) a. Look at the element Ca (Calcium). What’s it’s atomic number? How does that relate to the number of electrons it has? Both are 20. b. Place your cursor over H (upper left hand corner) and move down from row 1 to toward Fr in row 7 while watching the electron configuration. What do you notice? The row number corresponds to whether or not there’s electrons in the s orbital. c. Does this same idea with the rows (across) carry through the rest of the table? Yes. d. When you examine the Orbital configuration area it starts with number 1 at the bottom and moves up to seven. i. Why is there only one box next to the one? Why does that same single box carry up? What level is this? How do you know? It’s the s orbital because it’s the lowest energy level and it only has a maximum of two electrons. ii.
Just above the single box next to the number two there’s a string of three boxes. What level is this? How do you know? The p level has three orbitals (x, y, z). In order to fill the p orbital the 1s and 2s orbitals must be filled first. iii.
What orbital is represented by the string of five boxes? d orbital iv. What orbital is represented by the string of seven boxes? f orbital