Self and Group Evaluations Criteria Unacceptable 1 Marginal 2 Very good 3 Outstanding 4 Quality of work Work was not usable, or regularly needed major rework Work often had flaws and omissions that needed fixing Generally high quality of work, only occasional fixes needed Amazingly good output, well beyond expectations Quantity of work Did hardly any work. Contributed OK, somewhat less than their share. Worked hard, carried their share of the load. Considerable extra work, more than their share. Dependability and meeting commitments Could not be counted on at all. Usually met commitments. Needed some reminders or follow-up. Conscientious about commitments. Very dependable. Went out of the way to pick up slack for others who miss commitments. Interaction, supporting other team members, sharing information Was a major problem to interact and work with. Some interaction problems, unhelpfulness, or failure to communicate. Interacted well with others, helpful, flexible, pleasure to work with. Went out of the way to help teammates and enable them to contribute. Team meetings: participation, use of team time Little participation in discussions and activities, wasted the class team time. Participation spotty: not always participative, did not always use class team time effectively Participated fully in all team activities, used the class team time wisely Drew out others and ensured that everyone participated, used and encouraged the team to use the class meeting time efficiently Overall Contributions Rating Often failed to complete assigned work, was difficult to work with and made no real contributions to the team. Sometimes failed to complete assigned work, was often unprepared, but made some contributions Consistently good contributions, valuable member of the team, and usually prepared Did everything well and added some outstanding contributions

Today’s Do Now 9/9/2014 Number of protons in the nucleus 1. What is the definition of atomic number? 2. What is the definition of atomic mass? Number of protons in the nucleus Neutrons + Protons; mass of an atom

Today’s Catalyst 9/9/2014 D, E, Q 1 3

By the end of the class period today, I will be able to…. compare and contrast Mendeleev and Moseley’s periodic tables. explain the benefits and drawbacks of the Bohr model of the atom, and describe the currently accepted theory of the locations of electrons around an atom.

History of the Periodic Table By 1860, more than 60 elements had been discovered (How should we organize all of these elements!?)

History of the Periodic Table Mendeleev is credited with developing the periodic table (father of the PT!) Created his table in 1869

History of the Periodic Table Mendeleev arranged the elements in order of increasing atomic mass and noticed that certain similarities in element’s properties appeared at regular intervals

Mendeleev’s Table Arranged in order of increasing atomic mass Rows and columns switched

Henry Moseley In 1911, Henry Moseley created a periodic table that was arranged by increasing atomic number. How is the PT organized today?

Write-Pair-Share What is the main difference between Mendeleev and Moseley’s periodic table? What are some similarities between the two tables?

Rows (periods): elements are put in rows by increasing atomic number Columns (groups): elements are put into columns (groups) based on how they react (chemical properties)

Take out your Periodic Table!

Natural States of the Elements (solid/liquid/gas)

Next objective! explain the benefits and drawbacks of the Bohr model of the atom, and describe the currently accepted theory of the locations of electrons around an atom.

What’s wrong with this picture??

By the end of class today I will be able to… describe the organization of the electron cloud into energy levels and sublevels list the amount of electrons that can fill each energy level

Electrons must occupy specific energy levels. What Bohr Did Right… Electrons must occupy specific energy levels.

What Bohr Did Right… Electrons of increasing energy occupy orbits farther and farther from the nucleus Electrons exist in quantized orbits (specific energy levels). Electrons can’t exist between energy levels

Electrons Exist in Quantized Energy Levels

Electrons exist in Quantized Energy Levels… just like steps on a staircase Electrons can’t exist between energy levels, just like people can’t stand between stair steps

Group Practice With the partner who is sitting next to you, create an analogy about quantized energy

Partner Work Expectations Both partners need to contribute to the final product Conversation should be on task 2 minute time limit!!

Draw your analogy/something brilliant below: Electrons exist in Quantized Energy Levels… just like “something brilliant.” Draw your analogy/something brilliant below:

Electrons exist in Quantized Energy Levels… just like Draw your analogy/something brilliant below:

Where Bohr Went Wrong… Electrons do not travel in neat, planet-like orbits  

Atoms actually look something like this: This will blow your mind!

Bringing it all together: +

Energy levels contain orbitals Energy level= stair 1. 2. 3. 4. Stairs contain shapes Shapes contain orbitals

What is an orbital?? Orbital: a three-dimensional region around the nucleus Each orbital contains 2 electrons; where the electrons spend 90% of their time

Total number of electrons Guided Notes Orbital (Subshell) Shape Number of Orbitals Total number of electrons S Sphere 1 2 P D F

S orbital

Total number of electrons Guided Notes Orbital (Subshell) Shape Number of Orbitals Total number of electrons S Sphere 1 2 P Peanut 3 6 D F

P orbital

Total number of electrons Guided Notes Orbital (Subshell) Shape Number of Orbitals Total number of electrons S Sphere 1 2 P Peanut 3 6 D Clover 5 10 F

d orbital

Total number of electrons Guided Notes Orbital Shape Shape Number of Orbitals Total number of electrons S Sphere 1 2 P Peanut 3 6 D Clover 5 10 F Flower? 7 14

f orbital

Practice, practice, practice Whiteboard directions/expectations

Practice, practice, practice How many electrons can an orbital hold?

Practice, practice, practice How many electrons can an orbital hold? 2

Practice, practice, practice True or false? Each energy level contains shapes.

Practice, practice, practice True or false? Each energy level contains shapes. Answer: TRUE

Practice, practice, practice How many electrons can the S orbital shape hold?

Practice, practice, practice How many electrons can the S orbital shape hold? Answer: 2

Practice, practice, practice What is the shape of d orbitals? 

Practice, practice, practice What is the shape of d orbitals? Answer: Clover

Practice, practice, practice Name that orbital: This orbital shape can hold 6 electrons and is shaped like a peanut/dumbbell.

Practice, practice, practice Name that orbital: This orbital can hold 6 electrons and is shaped like a peanut/dumbbell. Answer: p orbital

Practice, practice, practice Put your notes away!

Practice, practice, practice How many orbitals does the f orbital shape contain?

Practice, practice, practice How many orbitals does the f orbital shape contain? Answer: 7

Practice, practice, practice How many electrons does the f orbital shape contain?

Practice, practice, practice How many electrons does the f orbital shape contain? Answer: 14

Practice, practice, practice What is the number of orbitals in the p-shape? What is the number of electrons total in the p-shape?

Practice, practice, practice What is the number of orbitals in the p-shape? What is the number of electrons total in the p-shape? Answer: 3 orbitals; 6 electrons

Practice, practice, practice Why was Bohr’s model wrong?

Practice, practice, practice Why was Bohr’s model wrong? Electrons do not orbit the nucleus on singular paths (like planets around the sun)

Practice, practice, practice Where do electrons have more energy? Closer or farther from the nucleus?

Practice, practice, practice Where do electrons have more energy? Closer or farther from the nucleus?

Which electron has more energy? #1 #2