1. Starter: Quick Review How many minutes are in 2 weeks?
Express the answer to 10.5m m in correct sig figs
Express 525K in degrees Celcius
The mass of a sample of salt is 20kg. The density of the salt is 4g/cm3. What is the volume of the sample of salt in mL?

2. As you come in, The Materials: Paper and pencil for notes
½ sheet of paper
History timeline
Pick up packet.
The Plan:
Discuss your Unit One tests (return ASAP)
Learn about basic atomic structure
Homework:
Complete the Atomic Structure Numbers Worksheet
NOTE: Models of the Atom, Isotopes, Atomic Mass &, Atomic Structure Numbers Quiz on Monday

3. Starter: Let’s Jog Your Memory
So…what is an atom?
Draw a diagram of an atom labeling the following parts: nucleus, electron cloud, proton, electron, neutron
Describe the 3 subatomic particles (Ex: location, charge, mass, etc)

4. Back to the Reading
Who theorized that all matter is composed of fire, air, water, and earth?
Name the famous Greek philosopher who agreed with the theory described above.
Name the scientist who established the Law of Conservation of Matter.
Name the famous Greek philosopher who disagreed with #1 and said that matter could be broken down into “atomos.”
Who said that “All atoms of a given element are identical.”?

5. Atomic Theory History of the Theory: Early ideas of the atom
Democritus
Aristotle
John Dalton (pg. 56)

6. Atomic Theory History of the Theory: Early ideas of the atom
Democritus - “atomos”; atoms exist
Aristotle - atoms do NOT exist
John Dalton (pg. 56) years later; atoms exist
Matter is made up of atoms.
Atoms are indivisible.
Atoms of same (different ) elements are same (different)
LAW OF CONSERVATION OF MATTER

7. More Recent Atomic Theory
JJ Thomson
Found Electrons through the cathode ray experiment
E. Rutherford
Nucleus in gold foil experiment
(Protons travel in different directions when they hit the nucleus)

8. Modern Atomic Theory Neils Bohr Schrodinger
First atomic model to show Energy levels
Schrodinger
Sublevels & orbitals

9. Subatomic Particles Proton Nucleus +1 1.673x10-24 1 Neutron None
Location
Charge
Actual Mass
Relative Mass
Proton
Nucleus +1
1.673x10-24 1
Neutron
None
1.675x10-24
Electron
Electron Cloud (in energy levels) -1
9.11x10-28
1840

10. Proton Significance Gives the atom its identity
Equivalent to the atomic number
Massive particle so adds to the atom’s mass
Gives the nucleus its positive charge
Balances the negative charge of the electrons

11. Neutron Significance Neutron glue that holds the nucleus together
Massive particle so adds to the atom’s mass (mass number= p + n)
Number can differ from one atom to another giving isotopes

12. Electron Significance
Responsible for chemical properties
Forms ions when gained or lost, which leads to a charge

13. Atomic Number The picture is NOT completely correct.
Atomic # IS the number of protons in the atom. It is NOT always the number of electrons.
Therefore, the atomic # gives the atom its identity...its name.

14. Atomic Number
In isotopic notation, the atomic number is shown in the lower left corner of the element symbol.
Example: 6C

15. Atomic Number- Quick Check
If an atom is found to have 28 protons, what is its identity?
What is the atomic number of phosphorus?
How many protons does barium have?
Show the following elements in “isotopic notation”:
Lithium, sodium, sulfur, lead

16. Atomic Number- Quick Check
If an atom is found to have 28 protons, what is its identity? Ni = Nickel
What is the atomic number of phosphorus? 15
How many protons does barium have? 56
Show the following elements in “isotopic notation”:
Lithium, sodium, sulfur, lead

17. Charge Charge = oxidation state
Oxidation state is just a fancier way to say it.
A charged atom results from an inequality between protons and electrons in an atom.
Which of those particles (protons or electrons) are more likely to be gained or lost from an atom? Why?

18. Charge Example
Example: Bromine has 35 protons. It often gains electrons to other atoms. If Bromine gains an electron, the atom will have 36 electrons. What will the charge be?
Answer: -1 charge

19. Charge...Now , you try
Example: Calcium has 20 protons. It often loses electrons to other atoms. If calcium loses 2 electrons, the atom will have only 18 electrons. What will the charge be?
Answer: +2 charge

20. Charge
In symbolic notation, the charge is listed in the top right corner of the element symbol. If the charge is neutral, then the corner is left blank.
Question: What does Cl-1 means for the amount of protons and electrons for a chlorine atom?
Answer: protons = 17 (don’t change), electrons = 18 (gained one)

21. Charge Quick Check
What is the charge of sulfur when it gains 2 electrons to the neutral atom?
Write the symbolic notation to represent an atom of aluminum that has lost 3 electrons leaving 13 protons and 10 electrons.
How many protons and electrons are in the following atom? Cu 2+

22. Charge Quick Check
What is the charge of sulfur when it gains 2 electrons to the neutral atom? S-2
Write the symbolic notation to represent an atom of aluminum that has lost 3 electrons leaving 13 protons and 10 electrons. Al3+
How many protons and electrons are in the following atom? Cu P, 27E

23. Mass Number
Consider the subatomic particles. Which TWO particles have enough mass to matter?
Mass number is always a whole number...no decimals.
Mass number is calculated by adding the number of protons to the number of neutrons.

24. **Important Equations**
Mass Number
In symbolic notation, the mass number is shown in the upper left corner of the element symbol.
Example:
126C
**Important Equations**

25. Mass Number Quick Check
If a sodium atom has 11 protons and 12 neutrons, what is the atom’s mass number?
How many neutrons does a copper atom with a mass number of 64 have?
How many protons and neutrons are in the atom represented with this symbolic notation: 3216S

26. Isotopic Notation Summary
Shorthand way to record the element symbol, atomic number, charge, and mass number.
With this information, you can deduce the number of protons, neutrons, and electrons in the atom being represented. X
Mass #
Charge
Atomic #

27. Starter: Atomic Structure
How many protons, electrons and neutrons are in the following atom?
58 Cerium-140
Write the correct isotopic notation for the element that has 26 protons, 30 neutrons, and 23 electrons.
Isotopes of the same element have different numbers of _________ in their atom but the same number of _______.
________ do not affect the atom’s mass but determine the oxidation state.

28. Take 10…Finish Up Complete at least 4 stations in the gallery walk
Isotopic Notation must be complete (atomic #, atomic number)
The assignment will be turned in for a grade today
If you finish early, take out your Unit 2 review packet that you received yesterday and work on the Atomic Number WS
Please ask if you have any questions

29. Atomic Structure: Part II
Students will understand…
The difference between mass number and atomic mass
How to calculate average atomic mass and relative abundance

30. Blocks on the Table
PROTONS give an atom its identity. They are the ONLY subatomic particle that must be identical from one atom to another. Neutrons AND electrons can vary...
SO, how can we create ONE box on the periodic table to represent ALL atoms of an element? We must represent AVERAGE atoms. (That’s why the atomic mass has decimals.)

31. Atomic Mass
Atomic mass = the weighted average of all of the types of atoms (isotopes) of the element
Must know the % abundance (how much of it is found in nature relative to other isotopes) and the mass number
Check out the example!

32. Atomic Mass Example
Copper exists as a mixture of 2 types of atoms. The lighter copper has 29 protons and 34 neutrons, and it makes up 69.17% of all copper atoms. The heavier type has 29 protons and 36 neutrons. It makes up the remaining 30.83% of copper on earth. What is the atomic mass of copper?

33. Atomic Mass Example
Element Z exists in 3 isotopic forms. The isotopic mixture consists of 15% Z-16, 35% Z-17, and Z-18 makes up the remaining percent. What is the atomic mass of this element? 33

34. Relative Abundance Calculation
Element X has two naturally-occurring isotopes with isotopic weights of 10 and 12. You look on the periodic table to find that its average atomic mass = 10.5 What is th relative and percentage abundance of each isotopes?

35. Relative Abundance Calculation
Silver has two naturally-occurring isotopes with isotopic weights of and What is the relative and percentage abundance of each isotopes?

36. Starter: AM Review
Element M exists in 3 isotopic forms. The isotopic mixture consists of 20% M-10, 50% M-15, and M-20 makes up the remaining percent. What is the atomic mass of this element?
Chlorine has two isotopes. Chlorine-35 has an exact weight amu, and it has a 75.77% abundance. The other isotope has amu. What is the atomic mass? 36

37. Isotope/Atomic Mass Lab
You and your partner will analyze a sample of the element Candium.
Gather the data, and calculate the atomic mass of candium.
You can eat your sample at the end! 8-)
Work on the new atomic mass calculations ws at your desk when you are done.

38. Isotope/Atomic Mass Lab
Important Information:
You can write on the sheet provided
Be sure to keep correct sig figs after measuring the mass
Keep your candy on a paper towel if you plan to eat them
Straighten up your lab area when you are finished
Be sure to stay on task…the assignment is graded!

39. Starter
Hydrogen has two naturally-occurring isotopes with isotopic weights of and What is the relative and percentage abundance of each isotope?
True or False:
Isotopes of an atom have different numbers of protons.
Although atoms are mostly empty space, they still have mass.

40. Energetic Electron
Electrons are energetic, and they exist on energy levels.
Quantum: specific amount of energy needed to move from one energy level to the next; energy levels are given principal quantum numbers as a result
When electrons change energy levels, energy is absorbed and released.
Light is sometimes visible when the energy is released (Emission of Light)

41. Quantum Illustration Quantum = distance between two energy levels
Principal Quantum Number (n) = begin counting closest to the nucleus

42. Quantum Illustration Principal Quantum number (n):
Refers to the principal energy level, which tells you the amount of energy the electron has
The CLOSER the electron is to the NUCLEUS the LESS energy it has

43. Quantum Leap Illustration
An electron from n=2 (ground state) can absorb a quantum of energy and jump to n=3 (excited state).
Excited state is temporary.
The electron will soon release the quantum and fall back from the higher level to ground state.
EMISSION OF LIGHT can occur and the released energy will travel as a wave.

44. Electromagnetic Spectrum (All energy waves fall into one of these categories.)

45. Electromagnetic Spectrum Let’s see if you get it…wavelength vs frequency

46. Calculating the Emission of Energy
Two Equations to calculate the energy:
Speed of light = wavelength x frequency
c = λν
c = 3.0 x108 m/s (speed of light is constant)
2. Energy = Planck’s constant x frequency
E = hν
h=6.626x10-34 Jsec (Planck’s constant)

47. F
Multiple Choice
iRespond Question
Finding a Connection
Look at the two equations. What variable do they have in common?
A.) Speed of light (c)
B.) Wavelength (lambda)
C.) Frequency (nu)
D.) Energy (E)
E.)

48. Electromagnetic Wave Calculations
So, if I know the _______ of a wave, then I can calculate its wavelength AND its energy.

49. Energy Practice Problem:
If the wavelength is meters, then what is the frequency of the wave?
iRespond Question F
Multiple Choice
A.) 300,000 Hz
B.) 3.0x1011 Hz
C.) 3.33x10-12 Hz
D.) 6.626x10-37 Hz
E.)

50. Energy Practice Problem:
If the wavelength is meters, then what is the energy of the wave?
iRespond Question F
Multiple Choice
A.) 1.99x10-22 J
B.) 2.21x10-45 J
C.) 1.99x1046 J
D.) 6.626x10-37 J
E.)

51. Energy Practice Problem:F
Multiple Choice
iRespond Question
Energy Practice Problem:
If the frequency is 7.0x1013 Hz, what is the wavelength of the wave? What is the energy of the wave?
A.) 4.29x106 m; 4.63x1020 J
B.) 2.33x105 m; 1.55x10-28 J
C.) 4.29x10-6 m; 4.63x10-20 J
D.) None of these
E.)

52. Starter: When do electrons emit light?
If an electron moves farther from the nucleus what happens to its energy?
If the frequency is 4.0x1012 Hz, what is the wavelength of the wave? What is the energy of the wave?

53. Electron Configuration
Electrons are arranged into different levels within the electron cloud based on their energy
In order to arrange the electrons, you must first know how many there are

54. Hoya Hotel…The analogy
Hotel = electron cloud
Floors = principal energy levels
1-7 COEFFICIENTS
Rooms = sublevels (consist of orbitals)
s = sphere, p = dumbbell, d & f
Guests = electrons
Up and down = direction of spin

55. Hoya Hotel Rooms (Sublevels) available:
S: Single room, has only one bed (sleeps 2)
P: Prestige room, has three beds (sleeps 6)
D: Deluxe room, has five beds (sleeps 10)
F: Fabulous room, has 7 beds (sleeps 14)

56. So…how can I remember these levels
The DIAGONAL RULE will help you to determine the order for placing the electrons into their sublevels
Lets practice…Write the electron configuration for the following
1. Oxygen Bromine

57. Noble Gas Notation
Noble Gas Notation is a shorter way to write out electron configurations
Start the configuration at the noble gas just before the atom and complete the normal electron configuration
Lets look at oxygen and bromine again…

58. Periodic Table Labeling
S block: blue d block: red
P block: yellow f block: green

59. Periodic Table Labeling
S block: blue d block: red
P block: yellow f block: green

60. What does this all mean? Let’s analyze the configuration of magnesium.
Energy levels
Sublevels
Electrons
Valence level and electrons
What can I NOT find represented in the electron configuration?
Orbitals
Pairing

61. Hoya Hotel Terms of Occupation:
Aufbau Principle: Each room/bed on the lower floors must be occupied before moving to a higher floor.
Pauli Exclusion: A maximum of two guests may occupy a bed. Guests must sleep head to foot.
Hund’s Rule: Single guests must occupy separate beds in a room. No pairing occurs unless no empty beds exist.

62. Orbital Diagrams Visual representation of electron cloud
Shows everything that electron configuration shows PLUS orbitals & pairing
How to Draw an Orbital Diagram
Write the electron configuration first.
Draw the “beds” (orbitals) under each room.
Put the electrons in the “beds.”

63. Let’s practice... Write the electron configuration for:
Fluorine
Magnesium
Palladium
Write the noble gas notation and orbital diagrams for the elements above.

64. Starter:
Write the correct electron configuration, noble gas notation, and orbital diagram for Barium
Which of the rules for filling orbitals does the picture to the right of the board violate?

65. Flame Test Lab Instructions
You will rotate between the stations from 1 to 6
Dip the wire into the solution and place in the fire. Observe the color.
In your data table, write a detailed description of each color you see
These descriptions will help you to determine your unknown

66. Analyzing Orbital Diagrams & Stability of Atoms
Electrons are responsible for the chemical properties (personalities) of atoms.
STABLE = All orbitals (beds) are full.
PRETTY STABLE = All orbitals (beds) are full OR half-full.
UNSTABLE = Empty orbitals (beds) exist.
NOTE: If an atom has to have an empty orbital, it is best for the empty orbital to be on the valence energy level so that it might be filled by electrons from a nearby atom.

67. F
Multiple Choice
iRespond Question
Analyzing Stability
Draw the orbital diagram of sodium. Is sodium stable, pretty stable, or unstable?
A.) Stable
B.) Pretty Stable
D.)
C.) Unstable
E.)

68. Draw the orbital diagram of chromium
Draw the orbital diagram of chromium. Is Cr stable, pretty stable, or unstable?
iRespond Question
Multiple Choice F
Analyzing Stability
A.) Stable
B.) Pretty Stable
C.) Unstable
D.)
E.)

69. Practice Analyzing Stability
1. Draw the orbital diagram of sodium. Is sodium stable, pretty stable, or unstable?
Answer: UNSTABLE; Sodium has one half-full orbital, but it’s third energy level has three empty p orbitals.
Draw the orbital diagram of chromium. Is Cr stable, pretty stable, or unstable?
Answer: UNSTABLE; chromium has one empty orbital.

70. Exceptions to the Rules
Exceptions to Aufbau principle:
Chromium and Copper columns ONLY
Stability of filled and half-filled sublevels
Arrangement’s impact on bonding

71. Atomic Emission Spectra
Unique to each element
“Fingerprint”
Used to identify unknowns
Shows all wavelengths of visible light given off by an atom
Flame Test Lab

73. Starter:
Write the correct electron configuration, noble gas notation, and orbital diagram for the following atoms:
Calcium Silver
True or False: Emission of light occurs when an electron absorbs energy and jumps from the ground state to a higher level.