1. Atomic Structure

2. Atomic Structure Atomic Number = Number of Protons or Electrons
Atomic Weight = Number of protons and the number of Neutrons
Example
Magnesium
Atomic Number = 12
Atomic Weight = AMU or grams/mole

3. Atomic Structure
Elemental
Name
Atomic
Number
Abbreviation
Weight

4. Atomic Model Concept Democritus (465 BC) Greek Philosopher
Matter is made up of discrete particles, can not be divided infinitely
First to use the term atomas (Atom)

5. Atomic Model Concept John Dalton (1766-1844) English school teacher
Developed the first Atomic Model
Differentiated atoms based on mass
Atoms can not be changed but can combine to form compounds

6. Thompson Model J.J. Thompson (1856-1940)
Experimented with Cathode rays and magnetism
Identified negatively charged particles in elements
Particles were called electrons

7. A02119MV CATHODE RAY TUBE

8. Rutherford Model Ernest Rutherford (1871-1931)
Alpha particles were deflected when passing through a gold foil.
The Positively charged proton was identified as the reason.
Determined that the Atom is mostly empty space.

9. Gold Foil Experiment

10. a02120mu

11. Chadwick Model James Chadwick (1891-1974)
Atoms were more massive than could be explained
Needed additional weight without effecting the charge.
Identified Neutrons as the additional component.

12. Quarks and Leptons
Two currently recognized groups of fundamental particles, which are subatomic and indivisible
Represent the smallest known units of matter
Six quarks and six leptons are the basic building blocks for everything in the universe.

13. Bohr’s Model Niels Bohr (1885-1962)
Utilized the science of spectroscopy
Determined that electrons could only exist in definite energy levels.

14. Devised the Solar System Model
Bohr’s Model
Devised the Solar System Model

15. Quantum Model Werner Heisenberg (1901-1976)
Bohr’s model only worked well for atoms with one electron.
The laws of motion did not account for the movements of all electrons
Determined a rationale to explain and describe their movements.

16. The Heisenberg Uncertainty Principle!
Quantum Model
The Heisenberg Uncertainty Principle!
It is impossible to know both the energy and exact position of an electron at the same time

17. Quantum Model
This replaced Bohr’s precise orbits with three dimensional regions of probable positions.
A orbital then became a map of where the electron is most likely to be at any given time
Electrons exist in energy levels

18. Quantum Model
For the first 112 elements there are only 7 possible energy levels that can be identified or determined.

19. Electron Cloud Model

20. Quantum Model
Subdivides all but the first principle energy level into sublevels
The sublevels contain other divisions called orbitals
The orbitals contain electrons

21. s p d f Quantum Model There are four sublevels
They are identified by the letters
s p d f

22. Energy level Sublevels
2 sp
3 spd
4 spdf
5 spdf
6 spd
7 sp

23. Different Sub-levels
F D P S

24. Quantum Model
The s sublevel is the simplest of all and only contains one orbital which can hold two electrons.
The s sublevel is found in all levels
An orbital can not contain more than two electrons

25. Sublevels Total Electron Capacity

26. Quantum Model
The p sub level contains only three orbitals which can hold two electrons each.
This sub level can contain a maximum of six electrons

27. Sub Electrons s p

28. Quantum Model
The d sublevel contains five orbitals which can hold two electrons each.
This sub level can contain a maximum of ten electrons

29. Sub Electrons s p d

30. Quantum Model
The f sublevel contains seven orbitals which can hold two electrons each.
This sub level can contain a maximum of fourteen electrons

31. Sub Electrons s p d f

32. 4th and 5th Energy Levels
F D P S

33. Quantum Model
The quantum model is only a mathematical picture of something we can not see.
It describes something in terms we can understand and help account for some of the properties of electrons.

34. Energy level Sublevels Electron Total
sp 8
spd 18
spdf 32
spdf 32
6 spd 18
7 sp 8

35. Quantum Model Sublevels can also be ranked according to energy
The further a sub level is away from the nucleus the more energy it has.
There is a filing order that can be used to understand energy levels

36. Quantum Model Some levels overlap
Because of this, part of a higher level may have a slightly lower energy capability than the one underneath it.

37. d sub level probability cloud

38. Filling Order Energy level (1-7)
3d __ p __
3p __ s__ n=4
3s __ n=3
2p __
2s __ Increasing energy
1s2s2p3s3p4s3d4p5s4d5p6s4f5d6p7s5f6d7p

39. 1s2s2p3s3p4s3d4p5s4d5p6s4f5d6p7s5f6d7p Filling Order
Energy level (1-7)
1s2s2p3s3p4s3d4p5s4d5p6s4f5d6p7s5f6d7p 2s 2p 3s 3p 4s 3d

40. Increasing energy
1s2s2p3s3p4s3d4p5s4d5p6s4f5d6p7s5f6d7p

41. Quantum Model Worksheet Room Filling order per Hotel Management
1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p
Guests
Per
Floor
Room 6d
Room 6s
Room 6p
Energy Level 6
Room 5d
Room 5f
Energy Level 5
Room 5s
Room 5p
Room 4d
Room 4f
Room 4s
Room 4p
Energy Level 4
Room 3d
Room 3s
Room 3p
Energy Level 3
Room 2s
Room 2p
Energy Level 2
Energy Level 1
Room 1s
Element: __________ Atomic Number: ____ Atomic Weight: ______ Number of Protons: ____ Number of Electrons: _____ Number of Neutrons: ____

42. Quantum Model Practice
How many electrons can a d sublevel hold? 10

43. Quantum Model Practice
How many electrons can a d orbital hold? 2

44. Quantum Model Practice
What type of sublevel is found in all principle energy levels? s

45. Quantum Model Practice
Which of the following orbitals is the highest in energy? ( 2s, 3d, 4s) 3d

46. Quantum Model Worksheet Room Filling order per Hotel Management
1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p
Guests
Per
Floor
Room 6d
Room 6s
Room 6p
Energy Level 6
Room 5d
Room 5f
Energy Level 5
Room 5s
Room 5p
Room 4d
Room 4f
Room 4s
Room 4p
Energy Level 4
Room 3d
Room 3s
Room 3p
Energy Level 3
Room 2s
Room 2p
Energy Level 2
Energy Level 1
Room 1s
Element: __________ Atomic Number: ____ Atomic Weight: ______ Number of Protons: ____ Number of Electrons: _____ Number of Neutrons: ____

47. Electron Configuration
Arrangement of electrons
Example – Li 1s22s1

48. Element: __________ Atomic Number: ____ Atomic Weight: ______
Electron Configuration
1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p
Element: __________ Atomic Number: ____ Atomic Weight: ______
Number of Protons: ____ Number of Electrons: _____ Number of Neutrons: ____

49. (start with the smallest and work up)
Aufbau Principle
The arrangements of electrons in an atom may be determined by the addition of electrons to a smaller atom.
(start with the smallest and work up)

50. Aufbau Principle
This means that each successive element has one additional proton and one additional electron.
As a rule electrons fill the least energetic orbital possible.

51. Orbital notation
Picture of the electron configuration 1s
H ___
H 1s1

52. Orbital notation He 1s2 Picture of the electron configuration He ___

53. Aufbau Principle
When two electrons have filled up a sub-level they move in opposite directions from each other.
This is known as “spin”
___

54. Hund’s Rule
States that when electrons fill a sublevel, all orbitals receive one electron before any receive two
Examples: Carbon, Oxygen

55. Carbon (6)
Electron configuration
1s 2s 2p

56. Carbon (6)
Orbital notation
1s 2s 2p
___ ____ ___ ___ ___

57. Oxygen (8)
Electron configuration
1s 2s 2p

58. Oxygen (8)
Orbital notation
1s 2s 2p
___ ____ ___ ___ ___

59. Titanium (22) ___ ___ ___ ___ ___ ___ ___ ___ ___
1s 2s 2p 3s 3p 4s 3d 4p
1s 2s 2p s 3p
___ ___ ___ ___ ___ ___ ___ ___ ___
4s 3d p
___ ___ ___ ___ ___ ___ ___ ___ ___

60. Arsenic (33) ___ ___ ___ ___ ___ ___ ___ ___ ___
1s 2s 2p 3s 3p 4s 3d 4p
1s 2s 2p s 3p
___ ___ ___ ___ ___ ___ ___ ___ ___
4s 3d p
___ ___ ___ ___ ___ ___ ___ ___ ___

61. Quantum Numbers
Quantum numbers describe the location and energy levels of electrons.
They are a zip code for the location of electrons based on four different aspects of the electron position

62. Quantum Number First Position
The energy level from 1-7 in which the electron is located
N = main energy level
Example: N2 (energy level 2)

63. Quantum Number Second Position
The sub-level in which the electron is located (s-f)
L = sub-level
s = p = d = f = 3
Example: (N2,L1)

64. Quantum Number Third Position
The position within the sub-level based on the available positions peculiar to each.
M = Orbital value ( 0 or +/-)
p ____ ____ ____ =
Example: (N2,L1,M-1)

65. Quantum Number Fourth Position The Spin of the electron
S = Spin ( +1/2 or - 1/2)
p ____ ____ ____ = + 1/2
Example: N2,L1,M-1,S+1/ or (2,1,-1,+1/2)

66. Quantum Number Practice
What is the quantum number for this electrons position?
Second energy level, p sub-level, middle orbit, positive spin.
(2,1,0,+1/2)

67. Quantum Number Practice
What is the quantum number for this electrons position?
Third energy level, d sub-level, first orbit, negative spin.
(3,2,-2,-1/2)

68. Quantum Number Practice
What is the quantum number for this electrons position?
Fifth energy level, f sub-level, sixth orbit, negative spin.
(5,3,2,-1/2)

69. Quantum Number Practice
1s 2s 2p 3s 3p 4s 3d 4p
1s 2s 2p s 3p
___ ___ ___ ___ ___ ___ ___ ___ ___
4s 3d p
___ ___ ___ ___ ___ ___ ___ ___ ___

70. Quiz A Quiz B Element 1 – Lithium Element 2 - Sulfur
Element 1 – Sodium
Element 2 -Oxygen

71. Shorthand Notation
Ne 1s2 2s2 2p6
Mg 1s2 2s2 2p6 3s2
Mg [Ne] 3s2

72. Shorthand Notation Ti [Ar] Ar 1s2 2s2 2p6 3s23p6
Ti 1s2 2s2 2p6 3s23p6 4s23d2
Ti [Ar]

73. Where does the Filling Order come from?
1s2s2p3s3p4s3d4p5s4d5p6s4f5d6p7s5f6d7p

74. 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p
D block = N - 1
F block = N - 2

75. Atomic Particles

76. Atomic Mass
Atomic mass is the average mass of all naturally occurring forms of that element.
Atomic Mass is measured in “Atomic Mass Units” or AMU
AMU Unit = (1/12 of carbon atom)
AMU of Arsenic (As) = 74.92

77. (Atomic Number = protons /electrons)
Atomic Mass
Atomic Mass Number is the number of particles in the atom (protons + neutrons)
Atomic Number is their specific ID based on number of protons or electrons
(Atomic Number = protons /electrons)

78. Atomic Mass Element AMU Mass # Atomic # H 1.008 1 1 C 12.01 12 6Na

79. Isotopes
Atoms of the same element always have the same number of protons
Some atoms of the same element can have different number of neutrons, these are called isotopes.
Isotopes have a different mass number. (AMU=protons + neutrons)

80. Isotopic Notation Describes the exact composition of an atom. Example:
Boron Boron
AMU = AMU=12 B B

81. Isotopic Notation Boron Boron Isotope 11 12 5 5 AMU = 11 AMU=12
AMU = AMU=12
Protons = Protons = 5
Neutrons = Neutrons = 7 B B

82. Isotopic Notation Practice
Bromine Bromine
AMU = AMU=
Protons = Protons =
Neutrons = Neutrons = Br Br

83. Isotopic Notation Practice
Bromine Bromine
AMU = AMU=86
Protons = Protons = 35
Neutrons = Neutrons = 51 Br Br

84. Isotopic Notation Practice
Barium Barium
AMU = AMU=
Protons = Protons =
Neutrons = Neutrons = Ba Ba

85. Isotopic Notation Practice
Barium Barium
AMU = AMU=145
Protons = Protons = 56
Neutrons = Neutrons = 89 Ba Ba

86. Isotopic Notation Practice
Nickel Nickel
AMU = AMU=
Protons = Protons =
Neutrons = Neutrons = Ni Ni

87. Isotopic Notation Practice
Nickel Nickel Isotope
AMU = AMU=145
Protons = Protons = 28
Neutrons = Neutrons = 117 Ni Ni

88. Valence Electrons
The electrons in the outermost energy level are the ones most likely to be involved in chemical bonding.
They are what give elements their physical properties.
These electrons are known as the valence electrons.

89. Valence Electrons 1s2 2s2 2p6 3s23p6 Example : Argon (Ar)
Electron Structure by energy (2,8,8)
Electron configuration
Valence Electrons = 8
1s2 2s2 2p6 3s23p6

90. Valence Electrons 1s2 2s2 2p6 3s23p3 Example : Phosphorus(P)
Electron Structure by energy (2,8,5)
Electron configuration
Valence Electrons = 5
1s2 2s2 2p6 3s23p3

91. Electron Dot Symbols Valence electrons determine how atoms bond
Electron Dot symbol is a short hand way of representing atoms.

92. Electron Dot Symbols

93. Na Electron Dot Symbols Sodium (Na)
Electron Structure by Energy = (2,8,1)
Valence Electrons = 1 Na

94. Al Electron Dot Symbols Aluminum (Al)
Electron Structure by Energy = (2,8,3)
Valence Electrons = 3 Al

95. Cl Electron Dot Symbols Chlorine (Cl)
Electron Structure by Energy = (2,8,7)
Valence Electrons = 7 Cl

96. O Electron Dot Symbols Oxygen (O) Electron Structure by Energy = (2,6)
Valence Electrons = 6 O

97. O Electron Dot Symbols Orbital notation ___ ____ ___ ___ ___ . . . . .
1s 2s 2p
___ ____ ___ ___ ___ O . . . . . .

98. Ionic Charges
Electrons can be lost, gained or shared during chemical bonding.
This process can cause the charge of an atom to become unbalanced either positively or negatively.
The atom does not lose its identity because the number of protons is the same.

99. Ionic Charges An atom in its normal state is neutral in charge.
Atoms that lose an electron become positively charge ( + or cation )
Atoms that gain an electron become negatively charged. (- or anion)

100. Na - 1 electron = Na Na 1+ Ionic Charge Sodium (Na)
Electron Structure by Energy = (2,8,1)
Valence Electrons = 1
Na electron = Na Na 1+
Positive Ion (cation) .

101. Electron Dot Symbols Fluorine (F) Electron Structure by Energy = (2,7)
Valence Electrons = 7
F electron = F F -1
Negative Ion (anion) . . . . . . . . . . . . . . .

103. Flame test
A flame test is a procedure used in chemistry to detect the presence of certain elements, primarily metal ions, based on each elements characteristic emission spectrum.
The test involves introducing a sample of the element or compound to a hot, non-luminous flame, and observing the color that results.

104. Flame Color
An atom consists of a nucleus with electrons orbiting around it. The electrons location is based on the filling order (Quantum theory).
Each orbit or shell has an occupancy limit and no more than that number can be there.
1s2 2s2 2p6 3s23p3

105. Flame Color
Electrons have a tendency to be as close to the nucleus as they can, because that is a lower energy state.
The farther from the nucleus, the more energy the electron must have.

106. Flame Color
If an atom is "zapped" by some kind of energy ( e.g. heat, electric discharge, electromagnetic radiation),
One or more electrons may pick up enough energy to be knocked into a more distant, and more energetic, shell.

107. Flame Color
After a short interval the electron drops back into a lower shell. When it returns to a lower shell it now has too much energy.

109. Flame Color
This surplus is emitted in the form of a photon - a tiny particle of light

110. Properties of Light
Visible light is a form of electromagnetic radiation.
This radiation exhibits wave like behavior as it travels through space.
The speed of light is 3.00 x 108 meters/second

111. Properties of Light

113. Flame Color
The color of the light (i.e. its wavelength) is determined by the difference in energy levels of the two shells between which the electron fell.
Because electrons can be knocked out of more than one shell, and they can be bumped up by more than just one level 4s

114. Flame Color
They also can return to their original level in one big transition, or in several stages. 4s

115. Flame Color
The end result is that an element which is excited produces light of a number of colors. The exact mix of colors is characteristic of that element and serves to identify it.
The mix is called the spectrum of that element.

117. 1. Copper acetate
2. Copper
3. Potassium iodide
4. Magnesium
5. Iron
6. Lithium carbonate
7. Strontium nitrate
8. Sodium chloride
Green flame Blue-green flame
Violet flame
White sparks Yellow sparks
Blue flame Red flame
Yellow flame

118. Is this a physical or chemical change?
Flame Color
Is this a physical or chemical change? 1s 1s 1s 2s 1s 2s 2s
Protons = 3
Electrons = 3
Protons = 3
Electrons = 3
Protons = 3
Electrons = 3

120. Quiz Quiz A Quiz B Mg (12) Ca (20) P (15)) N (7) As (33) Se (34)
Ar (18)
P (15)
K (19)
Quiz B
Ca (20)
P (15))
Se (34)
Cl (17)
O (8)
Sr (38)

121. Quantum Number Practice
Third energy level, d sub-level, first orbit, negative spin.
Fifth energy level, f sub-level, sixth orbit, negative spin.
Fourth energy level, p sublevel, central orbit, positive spin.

122. Quantum Number Practice
Third energy level, d sub-level, first orbit, negative spin. (3,2,-2,-1/2)
Fifth energy level, f sub-level, sixth orbit, negative spin. (5,3,2,-1/2)
Fourth energy level, p sublevel, central orbit, positive spin (4, 1,0,+1/2)

123. You conduct an experiment twice to confirm the density of an object
You conduct an experiment twice to confirm the density of an object. The mass of the object is 3.00 x 103 grams. The volume of displacement of the object you weighed is listed below for each experiment. Determine the observed density from both your experiments as well as the percent error if the actual density is suppose to be 1.58 x 102 grams/liter.
A B
1.01 x 101 liters x 101 liters x 101 liters x 101 liters

124. Perform the following operation using bridge unit Analysis and Scientific notation.
What is the average acceleration of an object that travels x 103 meters in x 105 seconds. Provide the answer in Kilometers. speed = dist / time Acc = speed / time B
What is the average acceleration of an object that travels x 102 meters in 2.31 x 106 seconds. Provide the answer in Kilometers. speed = dist / time Acc = speed / time

125. Assignment Atomic Number, Atomic weight, protons, neutrons, electrons.
Isoptic Notation
Electron Configuration
Orbital Notation
Valence number
Dot structure

126. Quiz A
Element 1= Sodium (11)
Element 2 = Oxygen (8)
Quiz B
Element 1 = Beryllium (4)
Element 2 = Sulfur (16)

127. Filtration Lab Problem: How do you separate salt from sand?
Hypothesis: If I dissolve the salt in water then I can filter it and separate it from the sand.
Design:
Mix salt and sand
Dissolve salt with water
Filter the water
Evaporate the water
Measure the salt and compare results

128. Filtration Lab
Data:
Started with one gram of salt
Retrieved 0.75 grams of salt
25% error in experiment
Conclusion: The process of separating the salt from sand using water to dissolve it was successful. Additional water was most likely needed needed to dissolve the salt in this experiment and improve the amount retrieved.
Reference: Chapter _____ page ____ of the Prentice Hall Chemistry text book.

129. Module 4 Test Uncertainty Principle Hunds Rule, Aufbau Principle
Electron Configuration
Orbital notation
Isoptic Notation
Electron Dot Structure
Scientists (know primary contribution)
Rutherford, Dalton, Chadwick, Heisenberg, Bohr, Thompson, Democritus
Honors – Quantum Number, shorthand notation

130. Physical or Chemical Change Lab
Problem: Determine if a physical or chemical change occurs.
Hypothesis: If the color changes and heat is given off or taken in, the weight changes and/or the pH changes than a chemical change has occurred.
Design:
Check the pH of the acid
Check the color of the acid with reagent
Combine with Sodium Bicarbonate
Evaluate the color, pH, weight and temperature

131. Physical or Chemical Change Lab
Data:
Conclusion:
Reference: Chapter _____ page ____ of the Prentice Hall Chemistry text book.