1. ChemI Block-1st: 3.4.15 Infinite Campus:
Matter and Energy Exam-32 pts.
Mapping Atomic Structure Lab-10pts.
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.)

3. Atomic Ranking Task Worksheet
What question(s) were you able to answer correctly using your background knowledge?
What question(s) did you have trouble with using your background knowledge? What did you learn from your research last night? Include the sources you used.

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

5. Atomic Structure: Ranking Task
Atomic Number
Mass Number
Isotopes
Atomic Mass

6. ChemI Block-1st:
Due:
Define the following vocabulary words: atomic number, mass number, and isotopes.
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.)

7. Atomic Structure: Bell Ringer
What is the atomic number for an atom?
2. Rank the following atoms from smallest to largest based on atomic number?
N b. H c. F d. O
3 . What is an atom’s mass number?

8. 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?

9. 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 9

10. 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 10

11. Atomic Structure Lab
education.jlab.org

12. Mass Number?

13. 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.

14. 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 14

15. Element’s Atomic Numbers

16. ChemI Block-1st: 3.10.15 Due: Elements Subatomic Differences 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.)

17. Elements: Subatomic Differences

18. 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)?

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

21. ChemI Block-1st: 3.11.15 Due: Isotope 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.)
I can calculate atomic mass for an element.

22. Elements :Isotopes

23. Isotopes
What is an isotope?

25. ChemI Block : 2.25.15 Due: Mapping Atomic Structure Lab-Post Lab Qts.
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.)
I can distinguish between mass number and atomic mass.

26. Isotopic Symbols

27. Isotope Applications
Calculate the number of protons, neutrons, and electrons in each neutral isotope below.
Na and Na-23

28. ChemI Block-1st: 3.12.15 Due: Kandium Lab 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.)
I can calculate atomic mass for an element.
I can investigate the evolution of the atom.

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.
Li-6 and Li-7
H-1 and H-2
c. O-16 and O-17
d. B-10 and B-11

30. Chem I: Homework
1. Calculate subatomic particles in each set of isotopes and illustrate each isotope with correct location and number of subatomic particles.
O-16 and O-17
b. B-10 and B-11

31. 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.

32. Kandium Lab
Purpose: To investigate an new element’s isotopes and to calculate its atomic mass

33. Mass Number vs. Atomic Mass

34. 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.

35. Calculating Atomic Mass of an Element
It is an average mass calculated from all the isotopes of a particular element.
The average mass is weighted because there is NOT an equal amount of each isotope in a sample.
How do you calculate a weighted average 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. 35

36. Calculating Atomic Mass
Isotope
Natural Abundance (%)

37. 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

39. ChemI Block : 3.13.15 Due: Kandium Lab
Isotopes and Atomic Mass Worksheet
Objectives:
Atomic Structure Quiz
I can identify forces within an atom.
I can investigate the evolution of the atom.
Homework:
Atomic Structure Study Guide-Test Tuesday

40. Element’s Isotopes and Atomic Mass
Questions?

41. Atomic Structure Quiz
Quiz includes the ranking task worksheet.

42. ChemI Block : 3.16.15 Due: Ranking Task Worksheet
Atomic Structure Study Guide-reviewed
Objectives:
I can identify forces within an atom.
I can investigate the evolution of the atom.
Atomic Structure Test-Wednesday!

43. Bell Ringer: Atomic Structure
If most of the atom is empty space, why is it matter (made of atoms) does not pass through one another?
2. What keeps the protons from leaving the nucleus and hooking up with the electrons?

44. Atomic Properties
If most of the atom is empty space, why doesn’t matter pass through one another?
“The Space Between Atoms” video clip.
spiff.rit.edu

45. 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.

46. Evolution of the Atom
Rank the models of the atom from earliest to most recent. (only use your background; context clues).

47. Evolution of the Atom
Rank the models of the atom from earliest to most recent. (only use your background; context clues).

48. 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.

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

50. John Dalton’s Atomic Model

51. 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.

52. Thomson’s Plum Pudding Model

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

54. 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.

55. 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.

56. 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.

57. 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.

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

59. 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?

60. Rutherford’s Gold Foil Experiment

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

62. Rutherford’s Nuclear Atomic Model

63. 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.

64. Chadwick’s Experiments: Neutron
nobelprize.org

65. Bohr’s Model of the Atom

66. Bohr’s Model of the Atom

67. 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)

68. Current Atomic Model
Erwin Schrodinger

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

70. 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.

71. Types of electron paths around nucleus

72. 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

73. 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)