List the four orbital shapes.
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1 Review Question List the four orbital shapes. The orbital shapes are: s, p, d, and f. Summarize Aufbau s rule for filling orbitals. Electrons fill orbitals with the lowest energy level possible first.
2 THIS WEEK WE WILL... SC3 Students will use the modern atomic theory to explain the characteristics of atoms. b. Use the orbital configuration of neutral atoms to explain its effect on the atom s chemical properties.
3 ELECTRON LOCATION: ELECTRON ORBITALS 5.2
4 DESCRIBE SHAPE OF THE ELECTRON ORBITALS s p d f
5 THE ELECTRON ORBITALS s orbitals are spherical There is only one way to turn the s orbital along the xyz axis s orbitals hold 2 electrons
6 THE ELECTRON ORBITALS p orbitals are shaped like a set of dumbbells There are three ways to turn the p orbitals along the xyz axis. p orbitals hold a total of 6 electrons.
7 THE ELECTRON ORBITALS Most of the d orbitals are shaped like a double dumbbell. One d orbital is shaped like a dumbbell with a ring around it. There are 5 ways to turn the d orbitals along the xyz orbitals. d orbitals can hold a total of 10 electrons.
8 THE ELECTRON ORBITALS f orbitals have an intricate shape. There are 7 ways to orient the f orbitals along the xyz axis. f orbitals can hold a total of 14 electrons.
9 HOW ARE THE ORBITALS FILLED? Pauli Aufbau Hund
10 CONFIGURATION The system used to describe the best known location of electrons is called the electron configuration. Elements have electron configurations that are unique to their kind. It is the arrangement of electrons in the atoms of an element that give that element its characteristics and properties.
11 RULES FOR DETERMINING AN ELECTRON CONFIGURATION Aufbau principle explains that electrons will occupy the lowest energy orbital available. Pauli exclusion principle shows that no two electrons can have the exact same location (as described by the four quantum numbers) Hund s rule states that orbitals of equal energy are occupied by one electron before any orbital is occupied by a second electron. The Hund s rule also states that when orbitals of equal energy are occupied by one electron, those electrons have the same spin.
12 IN OTHER WORDS... Lazy Electrons are located in the orbital with lowest energy level possible. Unique No two electrons can share the same position and spin. Electrons that are on the same orbital have different spins, clockwise and counter clockwise. Share When orbitals have the same energy level, each orbital gets one electron before any orbital gets two electrons.
13 ENERGY LEVELS The first energy level is closest to the nucleus, and the seventh energy level is furthest from the nucleus. There are a total of 7 energy levels As the energy levels increase, there is overlap. This means that 4s sublevel is lower in energy than the 3d sublevel. (there are several other examples of this overlap)
14 AUFBAU FILLING ORDER OF ATOMIC ORBITALS 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f
15 HOW WAS INFORMATION ABOUT ELECTRON ORBITALS DISCOVERED? Quatum science
16 GPB VIDEO You will notice cloudlike shapes. Try to pick out the s, p, d, or f shapes.
17 REPRESENTING ELECTRON LOCATION 1. Orbital notation: N (7e - ): 2s 1s 2p 2p 2p
18 6 ELECTRONS 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f
19 11 ELECTRONS 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f
20 ZINC 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f
21 IODINE I 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f
22 GROUP WORK Divide your paper into 4 sections. Draw the orbital notation for each element given to your group. When you have successfully completed your group set, evaluate your answers. Make any necessary revisions to your orbital notations. Complete the individual/partner practice set.
23 REVIEW Agenda: Quick-Check Electron Basics Orbitals & Orbital Filling Notes Practice Problems List the four orbital shapes. The orbital shapes are: s, p, d, and f. Summarize Aufbau s rule for filling orbitals. Electrons are lazy. They fill the lowest energy level orbitals first.
24 REVIEW Agenda: Complete Orbital Notation Group Practice Electron Configuration Group Practice Electron Configuration Independent Practice Take a few minutes to review your notes about electrons. In a orbital diagram, what do the arrows represent? The arrows are used to represent electrons. Summarize Pauli s rule for filling orbitals.
25 REPRESENTING ELECTRON LOCATION 2. Electron Configuration:
26 6 ELECTRONS 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f
27 11 ELECTRONS 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f
28 IRON Fe 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f
29 IODINE I 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f
30 GROUP WORK Divide your paper into 4 sections. Draw the electron configuration for each element given to your group. When you have successfully completed your group set, evaluate your answers. Make any necessary revisions to your orbital notations. Complete the individual/partner practice set.
31 REVIEW Agenda: Complete Orbital Notation Group Practice Electron Configurations In a orbital diagram, what do the arrows represent? The arrows are used to represent electrons. Summarize Pauli s rule for filling orbitals. Electrons are Unique. No two electrons can share the same position and spin.
32 REVIEW Agenda: Noble Gas Configuration In an orbital notation, why are the p orbitals written 3 times? P orbitals have 3 different rotations along the x y and z axes. Summarize Hund s rule for filling orbitals.
33 TOMORROW S QUIZ Use your notes to review Photoelectric Effect Atomic Theory Scientists Quantum Numbers Orbitals Orbital Filling Rules Orbital Notation Electron Configuration
34 ELECTRON BASICS QUIZ REVIEW
35 The Photoelectric Effect Electrons absorb energy from electromagnetic radiation and move from the low energy ground state to the high energy excited state. Excited electrons move back to the ground state by releasing photons of light.
36 DALTON S ATOM Many years later, Dalton again proposed the idea of that all matter is made of indivisible and indestructible atoms. Dalton s model of the atom was one solid sphere.
37 THOMSON S PLUMB PUDDING Thomson tried to show how electrons were situated in the atom. He proposed in a model in which the atom was a positively charged ball with negatively charged electrons stuck onto the surface. It was called the plum pudding model, since the electrons in the atom resembled the raisins in a plum pudding.
38 RUTHERFORD S SPINNING ELECTRONS Ernest Rutherford's experiments led him to describe the atom as having a relatively small but heavy nucleus with electrons in orbit around it.
39 BOHR S ENERGY LEVELS He suggested that electrons could only have certain motions: The electrons travel in orbits at specific distances from the small nucleus. These distances were called energy levels.
40 SCHRODINGER Viewed electrons as continuous clouds and introduced "wave mechanics" as a mathematical model of the atom. Used quantum math to show the probability of an electron being in a given area, and he called those areas electron clouds.
41 PRINCIPLE QUANTUM NUMBER The principle quantum number (n) indicates the main energy level occupied by the electron. n can only be a positive whole number 1-7. Small n values indicate close proximity to the nucleus. Large n values indicate that an electron is farther from the nucleus.
42 ANGULAR MOMENTUM QUANTUM NUMBER The angular momentum quantum number (l) indicates the shape of the orbital. For a given energy level, the number of angular momentum values allowed is equal to n The angular values allowed are 0 through n-1. The angular momentum quantum number defines s, p, d, and f orbital shapes.
43 MAGNETIC QUANTUM NUMBER The magnetic quantum number (m) indicates the orientation of an orbital around the nucleus. It describes how the orbital lies on an axis x, y, z. s orbitals only have 1 orientation in space. p orbitals can have 3 orientations in space. d orbitals can have 5 orientations in space. f orbitals can have 7 orientations in space.
44 SPIN QUANTUM NUMBER The spin quantum number (s) indicates the direction of an electron s spin. Electrons are thought of as having two spins. (clockwise & counter clockwise) There are only two possible values for the spin quantum number, +1/2 and -1/2.
45 ORBITAL SHAPE s -- sphere (1 orientation; 2 electrons) p -- dumbbell (1 orientation; 2 electrons) (3 orientations; 6 electrons) d --double dumbbell dumbbell & doughnut (5 orientation; 10 electrons) f -- very complex shape (7 orientation; 14 electrons)
46 RULES FOR DETERMINING AN ELECTRON CONFIGURATION Aufbau principle explains that electrons will occupy the lowest energy orbital available. Pauli exclusion principle shows that no two electrons can have the exact same location (as described by the four quantum numbers) Hund s rule states that orbitals of equal energy are occupied by one electron before any orbital is occupied by a second electron. The Hund s rule also states that when orbitals of equal energy are occupied by one electron, those electrons have the same spin.
47 IN OTHER WORDS... Lazy Electrons are located in the orbital with lowest energy level possible. Unique No two electrons can share the same position and spin. Electrons that are on the same orbital have different spins, clockwise and counter clockwise. Share When orbitals have the same energy level, each orbital gets one electron before any orbital gets two electrons.
48 REPRESENTING ELECTRON LOCATION 3. Noble Gas Configuration:
49 6 ELECTRONS 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f
50 11 ELECTRONS 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f
51 IRON Fe 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f
52 IODINE I 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f
53 REVIEW Agenda: Noble Gas Configuration In an orbital notation, why are the p orbitals written 3 times? P orbitals have 3 different rotations along the x y and z axes. Summarize Hund s rule for filling orbitals. Electrons Share. When filling similar orbitals, distribute one electron to each before giving a second electron. Quiz Tomorrow Photoelectric Effect Atomic Theory Scientists Quantum Numbers Orbitals Orbital Filling Rules Orbital Notation Electron Configuration
54 REVIEW Electron Quiz Dot Diagrams In an electron configuration, what do the exponents represent? The superscript numbers are not exponents. They represent the number of electrons in each orbital. Describe the difference between Bohr s model of the atom and the Orbital model. Use your notes to review for the Quiz: Photoelectric Effect Atomic Theory Scientists Quantum Numbers Orbitals Orbital Filling Rules Orbital Notation Electron Configuration
55 ESSENTIAL QUESTION
56 ESSENTIAL QUESTION
57 ESSENTIAL QUESTION
58 ELECTRON BASICS QUIZ
59 REPRESENTING ELECTRON LOCATION 4. Electron Dot Diagram Shows only the last energy level of the atom s electron configuration Each electron is represented as one dot Imagine a box around your element symbol. A pair of dots can be placed on each side around the element s symbol. There cannot be more than 8 dots in total.
60 6 ELECTRONS 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f
61 11 ELECTRONS 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f
62 IRON Fe 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f
63 IODINE I 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f
64 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f
65 REVIEW Agenda: Electron Quiz Dot Diagrams In an electron configuration, what do the exponents represent? The superscript numbers are not exponents. They represent the number of electrons in each orbital. Describe the difference between Bohr s model of the atom and the Orbital model. Use your notes to review for the Quiz: Photoelectric Effect Atomic Theory Scientists Quantum Numbers Orbitals Orbital Filling Rules Orbital Notation Electron Configuration
66 REVIEW Agenda: Acrostic Review Electrons Complete Noble Gas Configuration 1-36 Where are noble gases located on the periodic table? Noble gases are located on the far right in group 18. Which noble gas should you select when making a noble gas configuration for a given element?
67 ACROSTIC PROTON P R O T O N
68 CREATE AN ACROSTIC FOR ELECTRON E L E C T R O N
69 REVIEW Agenda: Acrostic Review Electrons Complete Noble Gas Configuration 1-36 You will need a periodic table to complete today s work. Where are noble gases located on the periodic table? Noble gases are located on the far right in group 18. Which noble gas should you select when making a noble gas configuration for a given element? Select the noble gas that is closest without going over in number of electrons to the given element.
70 REVIEW Agenda: Dot Diagrams Complete Dot Diagrams 1-36 Turn in all work Describe the process for creating a noble gas configuration. Select the noble gas that is closest to your element without going over and put it in brackets. Add any additional orbitals necessary to complete the configuration for your element. How do you determine the number of dots to use in a dot diagram?
71 REPRESENTING ELECTRON LOCATION-QUIZ 1. Orbital Notation 2. Electron Configuration 3. Noble Gas Configuration 4. Dot Diagram
72 REVIEW Agenda: Dot Diagrams Complete Dot Diagrams 1-36 Turn in all work Describe the process for creating a noble gas configuration. Select the noble gas that is closest to your element without going over and put it in brackets. Add any additional orbitals necessary to complete the configuration for your element. How do you determine the number of dots to use in a dot diagram? Count the number of electrons in the highest energy level-valence electrons.
73 REVIEW Agenda: Five Square Review Ion Configuration & Stability How is an ion created? Negative ions are created when electrons are gained. Positive ions are created when electrons are lost. What arrangement of electrons demonstrates stability? Full s and p orbitals in the outer energy level - s 2 p 6
74 IONS Cations - Positive ions have lost electrons Anions - Negative ions have gained electrons Why do neutral elements become ions? Full octet (s and p orbitals) Behave like a noble gas
75 STABILITY: atoms are most stable when they have full s and full p orbitals in their highest energy levels 8 valence electrons He is stable with just 2 valence electrons. Why?
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79 IONS: PREDICT THE CHARGES OF THE FOLLOWING ELEMENTS BASED ON THEIR ELECTRON CONFIGURATIONS THEN WRITE THE NEW CONFIGURATION Oxygen Magnesium Chlorine Potassium
80 IONS: PREDICT THE CHARGES OF THE FOLLOWING ELEMENTS BASED ON THEIR ELECTRON CONFIGURATIONS THEN WRITE THE NEW CONFIGURATION Neon Iron Nitrogen
81 REVIEW Agenda: Five Square Review Ion Configuration & Stability How is an ion created? Negative ions are created when electrons are gained. Positive ions are created when electrons are lost. What arrangement of electrons demonstrates stability? Full s and p orbitals in the outer energy level - s 2 p 6
82 REVIEW Agenda: Four Square Review Ion Configuration & Stability In terms of orbitals, what does it mean to have a full octet? In the highest energy level s 2 p 6. List four different ways to represent electron location.
83 FIVE SQUARE REVIEW Noble Gas Configuration Number of Protons, Neutrons, electrons Dot Diagram Electron Configuration Element Orbital Notation
84 REPRESENTING ELECTRON LOCATION QUIZ 1. Orbital Notation 2. Electron Configuration 3. Noble Gas Configuration 4. Dot Diagram Good Luck! After the quiz, begin outlines for your Electron Unit Activities.
85 REVIEW Agenda: Four Square Review Ion Configuration & Stability In terms of orbitals, what does it mean to have a full octet? In the highest energy level s 2 p 6. List four different ways to represent electron location. 1. Orbital notation 2. Electron configuration 3. Noble gas configuration 4. Dot diagram
86 Agenda: Four Square Review Ion Configuration & Stability Which two projects did you select as review activities? Element double bubble Atomic Theory double bubble Orbital tree map Orbital Filling Rules tree map Electron Unit taboo Electron Unit acrostic List two new things you learned about electrons during the electron unit lessons.
87 COMPLETE ELECTRON REVIEW PROJECTS
88 REVIEW Agenda: Four Square Review Ion Configuration & Stability Which two projects did you select as review activities? Element double bubble Atomic Theory double bubble Orbital tree map Orbital Filling Rules tree map Electron Unit taboo Electron Unit acrostic List two new things you learned about electrons during the electron unit lessons.
89 REVIEW Agenda: Electron Unit Projects Electron Unit Study Guide Br: Which two projects did you select as review activities? Element double bubble Atomic Theory double bubble Orbital tree map Orbital Filling Rules tree map Electron Unit taboo Electron Unit acrostic EQ: Name this element 1s 2 2s 2 2p 5 Fluorine
90 COMPLETE ELECTRON REVIEW PROJECTS
91 ELECTRON UNIT STUDY GUIDES
92 REVIEW Agenda: Electron Unit Projects Electron Unit Study Guide Which two projects did you select as review activities? Element double bubble Atomic Theory double bubble Orbital tree map Orbital Filling Rules tree map Electron Unit taboo Electron Unit acrostic Name this element 1s 2 2s 2 2p 5 Fluorine
93 REVIEW Agenda: Electron Unit Scavenger Hunt Review Electron Unit Study Guide Questions How is an emission spectrum created? A photon of light is released from an energized electron as it moves from the excited state back to the ground state. Name this element 1s 2 2s 1 Lithium
94 ELECTRON TEST REVIEW Electron Facts Scavenger Hunt Begin at any question #1-20 Write your answer the question in the appropriate space Look around the room to find the paper that matches your answer Read the next question
95 REVIEW Agenda: Electron Unit Scavenger Hunt Review Electron Unit Study Guide Questions How is an emission spectrum created? A photon of light is released from an energized electron as it moves from the excited state back to the ground state. Name this element 1s 2 2s 1 lithium
96 ELECTRON TEST TODAY Review your notes and study guide until the test begins. Take your time. Check your work. Eliminate careless mistakes.
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99 Orbital Notation Electron Configuration Noble Gas Configuration Dot Diagram
100 EXCEPTIONS Chromium Copper
101 & Double Bubble Map Meets Minimum Requirements ~ 90% Visually Attractive Orbital notation Electron configuration Noble gas configuration Dot diagram Group on periodic table Number of valence e - Exceeds Requirements ~ 100% All Minimum Requirements Visually Attractive Additional Information
102 After the Test... ORBITAL TREE MAP Shape Orientations in space Total number of electrons Energy levels ORBITAL FILLING RULES TREE MAP Definition Summarize in your words Incorrect example Correct example Topic Category Category Category Category detail detail detail detail detail detail detail detail detail detail detail detail detail detail detail detail detail detail detail detail
103 DISCOVERING PATTERNS Lightly Color: Orange-Any element with the last orbital of s Blue-Any element with the last orbital of p Green-Any element with the last orbital of d The periodic table is divided into s, p, d, and f blocks. Determine the location of the: s block-outline in orange marker p block-outline in blue marker d block-outline in green marker Look across each period and determine which energy level is being filled. Groups 1 and 2: write the dot diagram and the last orbital Groups 3-18: write the dot diagram and the last 2 orbitals Predictions Last orbital of: Ra Ag Pt Pb I Xe Where would the f block be located? Color and outline it in purple. Which elements will end in: 5s 2 4d 2 6s 1 6s 2 6p 3 5f 3 How many electrons would be gained/lost from elements for Groups 1,2, and 13-18? What charge would you expect for Groups1,2 and 13-18?
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