1. ChemI Block : 2.23.14 Due: Atomic Structure Ranking Task Worksheet
Objectives:
I can illustrate the composition and size of an atom. (Ranking Task Wksht. /Basketball Lab)
I can predict properties of an atom based on its atomic structure. (Ranking Task Wksht.)
I can distinguish between isotopes of the same element. (Atomic Structure Wkshts.)

2. Atomic Ranking Task Worksheet
Answer qts. using:
Background Knowledge

3. Atomic Ranking Task Worksheet
Answer qts. using:
Background Knowledge
Resources(textbook)-marker

4. Atomic Structure: Ranking Task
Mass # ?
Atom I.D. ?
Istopes ?

5. Atomic Number The number of protons within an atom’s nucleus.
Its an atom’s I.D.
Atoms of the same element always have the same number of protons.
Do you notice any patterns with atomic numbers on the periodic table?

6. Subatomic Particles in an Atom
symbol
charge
location
Mass (g)
mass # (amu)
proton
1.674 x 1
electron
9.11 x 10-28
neutron
1.675 x 6

7. Mass Number Mass number : The mass of a single atom.
Sum of the p+ and n0 within an atom.
Common unit: atomic mass unit (amu)
*The mass number is NOT the same as atomic mass located on your periodic table.

8. Atomic Structure: Ranking Task Worksheet
Answered Qts. using….
Background Knowledge
*Peer Collaboration*
3. Resources (text/internet)

9. Atomic Number ?

10. Atomic Structure: Ranking Task
Mass # ?
Atom I.D. ?
Istopes ?
1. # of p+ in an atom.
2. # of (p+) and (n0) in an atom.
3. # of p+, n0, and e- in an atom. 4.
atomic mass- protons.

11. Atomic Number The number of protons within an atom’s nucleus.
Its an atom’s I.D.
Atoms of the same element always have the same number of protons.
Do you notice any patterns with atomic numbers on the periodic table?

12. Element’s Atomic Numbers

13. Mass Number?

14. Atomic Number The number of protons within an atom’s nucleus.
Its an atom’s I.D.
Atoms of the same element always have the same number of protons.
Do you notice any patterns with atomic numbers on the periodic table?

15. Mass Number Mass number : The mass of a single atom.
Sum of the p+ and n0 within an atom.
Common unit: atomic mass unit (amu)
*The mass number is NOT the same as atomic mass located on your periodic table.

16. Subatomic Particles in an Atom
symbol
charge
location
Mass (g)
mass # (amu)
proton
1.674 x 1
electron
9.11 x 10-28
neutron
1.675 x 16

17. Subatomic Particles in an Atom
symbol
charge
location
Mass (g)
mass # (amu)
proton
1.674 x 1
electron
9.11 x 10-28
neutron
1.675 x 17

18. Isotopes?

19. ChemI Block : 2.24.14 Due: Atomic Structure Ranking Task Worksheet
Objectives:
I can illustrate the composition and size of an atom. (Ranking Task Wksht. /Basketball Lab)
I can predict properties of an atom based on its atomic structure. (Ranking Task Wksht.)
I can distinguish between isotopes of the same element. (Atomic Structure Wkshts.)

20. Subatomic Particles in an Atom
symbol
charge
location
Mass (g)
mass # (amu)
proton
1.674 x 1
electron
9.11 x 10-28
neutron
1.675 x 20

21. Atomic Structure
Atomic Number?
Mass Number?
Isotopes?

22. Atomic Number The number of protons within an atom’s nucleus.
Its an atom’s I.D.
Atoms of the same element always have the same number of protons.
Do you notice any patterns with atomic numbers on the periodic table?

23. Mass Number Mass number : The mass of a single atom.
Sum of the p+ and n0 within an atom.
Common unit: atomic mass unit (amu)
*The mass number is NOT the same as atomic mass located on your periodic table.

24. Subatomic Particles in an Atom
symbol
charge
location
Mass (g)
mass # (amu)
proton
1.674 x 1
electron
9.11 x 10-28
neutron
1.675 x 24

25. Isotopes
What are isotopes?

26. Bell Ringer: Atom’s Subatomic Particles
1. : A cesium (Cs) atom has a mass of 133 amu and an atomic number of 55.
How many p+, e-, and n0 are there?
Illustrate where the subatomic particles are located within the cesium atom.
2.: An iron(Fe) atom has an atomic number of 26 and consists of 30 neutrons.
How many p+ and e- are there?
What is iron’s mass number (amu)?

27. Bell Ringer: Atom’s Subatomic Particles
1. : A cesium (Cs) atom has a mass of 133 amu and an atomic number of 55.
How many p+, e-, and n0 are there?
Illustrate where the subatomic particles are located within the cesium atom.
2.: An iron(Fe) atom has an atomic number of 26 and consists of 30 neutrons.
How many p+ and e- are there?
What is iron’s mass number (amu)?

28. Chem I: Homework
1. Calculate subatomic particles in each set of isotopes and illustrate each isotope with correct location and number of subatomic particles. a. Li-6 and Li-7 b. H-1 and H-2 c. O-16 and O-17 d. B-10 and B Research and state the difference between the following atomic terms: mass number and atomic mass. *Record answers on separate sheet.

29. Chem I: Homework
1. Calculate subatomic particles in each set of isotopes and illustrate each isotope with correct location and number of subatomic particles. a. Li-6 and Li-7 b. H-1 and H-2 c. O-16 and O-17 d. B-10 and B Research and state the difference between the following atomic terms: mass number and atomic mass. *Record answers on separate sheet.

30. Mapping Atomic Structure Lab
Purpose:
Model the size difference between the nucleus and the electron cloud.
Data Section:
Need to include units with measurements.
Show work with calculations for credit.
Draw radius of atom on map.
Conclusion:
What does your data section inform you about the size difference between the electron cloud and nucleus of an atom?

31. Chem I Block : 9.25.14 Objectives:
I can illustrate the composition and size of an atom. (Ranking Task Wksht. /Basketball Lab)
I can predict properties of an atom based on its atomic structure.
I can distinguish between isotopes of the same element.

32. Isotope Applications
Calculate the number of protons, neutrons, and electrons in each neutral isotope below.
Na and Na-23
2. For each isotope, illustrate the location and quantity of each subatomic particle in the atom.
3. Does Na-18 and Na-23 isotopes have similar chemical properties? Explain.

33. What distinguishes each element below from one another?

34. Distinguishing Atoms
education.jlab.org
What distinguishes one element’s atom from another element’s atom?

35. Atom’s Subatomic Particles
Problem A: A cesium (Cs) atom has a mass of 133 amu and an atomic number of 55.
How many p+, e-, and n0 are there?
Illustrate a Cs atom, identifying where the subatomic particles would be located.
Problem B: An iron atom has an atomic number of 26 and consists of 30 neutrons.
How many p+ and e- are there?
What is iron’s mass number (amu)?

36. Isotopes
Annotate resource and complete practice problems on front.

37. Chem I: Homework
1. Calculate subatomic particles in each set of isotopes and illustrate each isotope with correct location and number of subatomic particles. a. Li-6 and Li-7 b. H-1 and H-2 c. O-16 and O-17 d. B-10 and B Research and state the difference between the following atomic terms: mass number and atomic mass. *Record answers on separate sheet.

38. Atomic Structure
education.jlab.org
What do you predict the size difference is between an atom’s nucleus and its electron cloud?

39. ICP: 9/29 Due: Isotope Worksheet Objectives:
I can distinguish between isotopes of the same element.
I can illustrate the composition and size of an atom. (Ranking Task Wksht. /Basketball Lab)
I can predict properties of an atom based on its atomic structure.

40. Mapping Atomic Structure Lab
Data Section:
Need to include units with measurements.
Show work with calculations for credit.
Draw radius of atom on map.
Conclusion:
What does your data section inform you about the size difference between the electron cloud and nucleus of an atom?

41. What is the mass number for an atom?
Subatomic
Particle
symbol
charge
location
Mass (g)
mass # (amu)
proton p+ +1
nucleus
1.674 x 1
electron e-
- 1
cloud
9.11 x 10-28
neutron n0
1.675 x 41

42. What is the mass number for an atom?
Subatomic
Particle
symbol
charge
location
Mass (g)
mass # (amu)
proton p+ +1
nucleus
1.674 x 1
electron e-
- 1
cloud
9.11 x 10-28
neutron n0
1.675 x 42

43. An Atom’s Mass Mass number : The mass of a single atom.
Sum of the p+ and n0 within an atom.
Common unit: atomic mass unit (amu)
*The mass number is NOT the same as atomic mass located on your periodic table.

44. Isotope Worksheet Homework: Annotate the passage on isotopes.
Complete the worksheet (front and back)

45. Isotope Worksheet Homework: Due Wed., Feb. 26th
Annotate the passage on isotopes.
Complete the worksheet (front and back)

46. Chem I: 9/26 Due: Mapping Atomic Structure Lab Atomic Mass Worksheet
Objectives:
I can illustrate the composition and size of an atom. (Ranking Task Wksht. /Basketball Lab)
I can predict properties of an atom based on its atomic structure.
I can distinguish between isotopes of the same element.
I can distinguish between mass number and atomic mass.

47. Atomic Properties
If most of the atom is empty space, why doesn’t matter pass through one another?
spiff.rit.edu

48. Atomic Forces Electrostatic Forces : Forces between charged particles.
Types of electrostatic forces:
Attractive: (p+ and e-)
Repulsion: (p+ and p+
e- and e-)
Nuclear Forces:
Forces that holds p+ and n0
together in nucleus.

49. Chem I: 9/29 Due: Isotope Worksheet Kandium Lab
Evolution of the Atom (qts. 1)
Objectives:
I can illustrate the difference between isotopes of the same element.
I can distinguish between mass number and atomic mass.
I can calculate atomic mass for an element.
I can investigate the evolution of the atom.
Homework:

50. Isotope Applications
3. Calculate the number of protons, neutrons, and electrons in each neutral isotope below.
Na and Na-23
4. For each isotope, illustrate the location and quantity of each subatomic particle in the atom.
5. Does Na-18 and Na-23 isotopes have similar chemical properties? Explain.
6. What did you learn is the difference between mass number and atomic mass?

51. Mass Number vs. Atomic Mass

52. Calculating Atomic Mass of an Element
It is an average mass calculated from all the isotopes of a particular element.
It is a weighted average mass due to their being a possible unequal distribution of isotopes in matter.
Located on the periodic table.
How do you calculate atomic mass?
1. For each isotope, multiply its mass (mass #) by its natural abundance (decimal form) to get the weighted mass for each isotope.
2. Add up the isotopes weighted masses to get the atomic mass (average mass) for the element. 52

53. Calculating Atomic Mass
Gold’s Isotopes
Natural Abundance (%)

54. Homework: Review for Matter and Energy Make-up Exam
Complete Atomic Mass Worksheet

55. Chem I: 2/28 Due: Atomic Mass Worksheet (front side) Objectives:
Chemistry Make-up Exam
I can locate and calculate subatomic particles in an atom.
I can illustrate the difference between isotopes of the same element.
I can distinguish between mass number and atomic mass.
I can apply atomic mass with Kandium Lab.

56. Chemistry I Block: 9.30.14 Due: Kandium Lab
Evolution of the Atom packet
Objectives:
I can identify, illustrate, and calculate subatomic particles in an atom.
I can assess isotopes of the same element.
I can distinguish between mass number and atomic mass.
I can investigate the evolution of the atom.

57. Atomic Structure Review: Bell Ringer
1. Identify the number of protons, neutrons, and electrons for each isotope of Rb.
Does Rb-86 and Rb-87 isotopes have similar chemical properties? Explain how you know this.
a.Calculate the atomic mass of Rubidium.
b. What is the difference between mass
number and atomic mass?
a. Distinguish between the two types of forces within an atom.
b. Which force is stronger? Explain how you know this.
Rubidium’s Isotopes
Natural Abundance (%)
Rb-86
72.2
Rb-87
27.8

58. Evolution of the Atom Predict the developmental order of the atom.
Rank them 1(earliest) to 5(current). Include your reasoning for credit.
Discuss ranking with a peer. Report similarities and differences. Were you persuaded to make modifications to your initial ranking, explain?

59. Chem I: 10/01.14 Due: Evolution of the Atom (qts. 1) Objectives:
I can illustrate the difference between isotopes of the same element.
I can distinguish between mass number and atomic mass.
I can calculate atomic mass for an element.
I can investigate the evolution of the atom.
Homework:
Atomic Structure Study Guide

60. Evolution of the Atom

61. Chem I: 10/02.14 Due: Subatomic Particles Wksht. Objectives:
I can illustrate the difference between isotopes of the same element.
I can distinguish between mass number and atomic mass.
I can calculate atomic mass for an element.
I can investigate the evolution of the atom.
Homework:
Review for Atomic Structure Test

63. History of the Atom

64. Democritus(400b.c.) Greek Philosopher

65. Democritus(400b.c.) Greek Philosopher
1) Observed matter to be made up of atoms.
2) Atoms are the smallest form of matter.
3. Atoms cannot be broken down.
4) The types of atoms in matter determine its properties.

66. Aristotle: Greek Philosopher (300b.c.)
Aristotle observed matter to be made from four things:
earth, water, air, and fire

67. John Dalton’s Atomic Model

68. John Dalton’s Atomic Model
English school teacher
Proved Democritus atoms hypothesis using the scientific method.
His conclusions produced:
Dalton’s Atomic Theory

69. Dalton’s Atomic Theory
Atoms are the building blocks of all matter.
2. Atoms cannot be subdivided.
3. Each element has the same kind of atoms.
4. A compound is composed of two or more atoms chemically combined in a fixed amount. Ex. NaCl
5. Atoms cannot be created or destroyed just rearranged during chemical reactions.

70. Thomson’s Plum Pudding Model

71. Thomson’s Cathode Tube Experiment
l-esperimento-piu-bello-della-fisica.bo.imm.c...

72. Subatomic Particle: Electron
J.J. Thomson (pg. 105)
1897 discovered electrons in gas atoms using a cathode ray tube.
Determined electrons have a negative charge.
Electrons have the same charge in all atoms.
Robert Millikan: Determined the mass of the electron to be very tiny.

73. J. J Thomson’s Plum Pudding Model
If atoms are made of electrons how come most matter does not shock us?
Atoms must have positive particles, too.
He proposed the Plum Pudding Atomic Model
An atom is equally made up of positive and negative particles.

74. Goldstein’s Cathode Tube Experiment
chemed.chem.purdue.edu
reich-chemistry.wikispaces.com
He discovered protons using a cathode ray tube.
Observe particles moving in the opposite direction.

75. Subatomic Particles: Protons
1886 Eugen Goldstein observed particles traveling in the opposite direction of the cathode rays(electrons).
He knew these particles must be (+) charged. They were called protons.
Protons charge is the same for all atoms
Protons have a significant mass compared to the electron.

76. Rutherford’s Model of the Atom
green-planet-solar-energy.com

77. Rutherford’s Gold Foil Experiment
If positively charged light particles traveled through a sample of matter composed of atoms with protons and electrons evenly distributed throughout the atom, what would happen to the trajectory (path) of the + charged light particles as it passes through these atoms?

78. Rutherford’s Gold Foil Experiment

79. Rutherford’s Conclusion
Most of the atom is empty space.
Small dense region composed of
(+) charged particles.
(Nucleus)

80. Rutherford’s Nuclear Atomic Model

81. Subatomic Particle: Neutron
What keeps the protons within the nucleus ?
(Like particles repel each other)
James Chadwick discovers that the nucleus also has neutral particles present. He called them neutrons.

82. Chadwick’s Experiments: Neutron
nobelprize.org

83. Bohr’s Model of the Atom

84. Bohr’s Model of the Atom

85. Bohr’s Model of the Atom
Electrons travel in fixed, circular paths
around the nucleus.
Each path has a specific energy requirement.
These circular paths are called energy levels.
Limited number of electrons on each energy level. (2n2 Rule)

86. Current Atomic Model
Erwin Schrodinger

87. Current Atomic Model Erwin Schrodinger blogs.stsci.edu
science.howstuffworks.com

88. Current Atomic Model Electrons do not travel in fixed paths around
the nucleus
Electrons constantly move to different
energy levels in the electron cloud.
Direction of movement is dependent
upon how much energy an electron has.
Observed several different paths electrons
can take around the nucleus.

89. Types of electron paths around nucleus

90. Chem I: 10/02.14 Due: Evolution of the Atom Packet Objectives:
I can illustrate the difference between isotopes of the same element.
I can distinguish between mass number and atomic mass.
I can calculate atomic mass for an element.
I can investigate the evolution of the atom.
Homework:
Atomic Structure Study Guide-Test Friday

91. Atomic Models Dalton’s Model Thomson’s Model Rutherford’s Model
Illustration
Description
Dalton’s Model
Thomson’s Model
Rutherford’s Model
Bohr’s Model
Schrodinger’s Model

92. Atomic Models Rutherford’s Dalton’s Atomic Model
Nuclear Model
Dalton’s Atomic Model
Thomson’s Plum Pudding Model
Bohr’s Planetary Model
Schrodinger’s Atomic Model
(current model)