1. Matter and Change/Atomic Structure
Objectives:
1. I can classify matter into substances and mixtures.
2. I can identify and distinguish between physical and chemical properties.
3. I can identify and distinguish between the two types of forces that affect the nature of molecules.
4. I can understand and distinguish between physical and chemical changes.
5. I can identify techniques used to separate mixtures.
6. I can identify an atom and its properties based on it atomic structure.
7. I can distinguish between isotopes of the same element.
8. I can calculate the atomic mass for an element.

2. Chemistry I:
Due:
Signed Syllabus and Lab Contract-place in tray
Learning Style Survey
Classifying Matter Vocabulary
Objectives:
Evaluate how you learn best.
I can classify matter into substances and mixtures

3. Learning Style Survey
Hypothesis: How do you think you learn best? Experiment: Complete Test Analysis of Data: Create a Table and Graph illustrating your results.

4. What is Chemistry the study of?

5. Classification of Matter
What is matter?
Using background knowledge define and illustrate the
following terms.
Substance
Mixture
Element
Homogenous Mixture
Compound
Heterogenous Mixture

6. Classification of Matter-2nd

7. Chemistry I: 1.10.17 Infinite Campus: Lab Safety Exam-35 pts.
Lab Safety Worksheet-10 pts.
Learning Style Survey-15 pts.
Due:
Classifying Matter Worksheet and Vocabulary
Objectives:
I can classify matter into substances and mixtures.
I can identify and distinguish between physcial and chemical properties/changes.

8. Learning Style Inventory Assessment
*Answer with complete sentences.
*Correct grammar/punctuation.
*Label tables and graphs properly.
nwlink.com

9. Learning Style Inventory Assessment
Visual Learners:
Diagrams/Graphs/Charts
Highlight notes
Note Cards with pics
Organize resources in binder and color code
Auditory:
Teacher Instruction(lecture)
Online tutorials/ video clips
Jingles
Read notes out loud
Kinesthetic:
Labs/Projects
Collaboration with peers
Fieldtrips/educational clips
nwlink.com

10. Classification of Matter10

11. Classification of Matter
What is matter?
Using background knowledge define and illustrate the
following terms.
Substance
Mixture
Element
Homogenous Mixture
Compound
Heterogenous Mixture

12. What is Matter?
One or more atoms that take up space and has mass.

13. Classification of Matter Lab13

14. Classification of Matter Lab14

15. Elements Simplest class of matter that maintains its properties
Purest class: composed of only one kind of atom.
Each kind of atom is called an element.
A symbol is used to represent each element. 15

16. A compound’s fixed ratio is called a chemical formula.
Chemical combination of elements in a fixed amount or ratio.
A compound’s fixed ratio is called a chemical formula.
Ex. Sodium chloride = NaCl
When elements chemically combine the compound produced has new properties.
Sodium (Na) Chlorine (Cl) = Salt (NaCl) 16

17. Mixture
Substances (elements or compounds) are physically mixed together to produce a mixture.
The composition of substances in a mixture varies from one sample to another.
The physical properties of each substance in a mixture is preserved.

18. Heterogenous Mixures Observe multiple phases (parts) because the substances do NOT mix well.18

19. Homogenous Mixtures Also called solutions
Substances mix so well they look like one phase.

20. Substances in Matter The symbol/formula for matter identifies
Kind and number of substances in matter
Identifies class of matter
Salt: NaCl
Compound
Salt Water: NaCl + H2O
mixture: homo mix
Sodium: Na
Element 20

21. Classifying Matter: Substances vs. Mixtures
Definite chemical make-up
Elements or compounds
Ex. Silicon chip or H2O
Mixtures
Varied chemical make-up
2 or more substances physically combined
Homo or Hetero Mixtures
Pizza and salt water

22. Classifying Matter: Substances vs. Mixtures
Element
Pure and simplest substance
One type of atom
Periodic table
Symbol, (He= Helium)
Homogenous Mixture
2 or more substances physically combined.
Substances are very soluble in one another-mix well – one phase
Substances in mix properties are preserved
Separated by physical processes.
Also called a solution
Ex. salt water, kool-aid
Compound
2 or more substances chemically
combined
Definite composition
Break-down only thru chemical processes
Substances making up cmpd gain new properties.
Chemical Formula, H2O
Ex. iron rust
Heterogenous Mixture
Substances are not soluble in one another-do not mix well-multiple phases
Substances in mixture properties are preserved.
Separated by physical processes
Ex. Oil and water, pizza, soil

23. Chemistry:
Due:
Classification of Matter worksheet and Venn Diagram
Objectives:
I can classify matter into substances and mixtures. (Quiz tomorrow over classifying)
I can identify and distinguish between physical and chemical properties/changes.

24. Classifying Matter: Micro Level24

25. Classification of Substances
Compounds
Elements
Substances

26. Classification of Mixtures
Homo Mixtures
Hetero Mixtures
Mixtures

27. Classification of Matter
The symbol/formula for matter identifies
Kind and number of substances in matter
Identifies class of matter
Salt: NaCl
Salt Water: NaCl + H2O
Sodium: Na 27

28. Classifying Matter: Micro Level
Substances?
Mixtures?

29. Classifying Matter: Micro Level

30. Classifying Matter Worksheet

31. Classifying Matter Lab
Purpose: Classify matter as a type of substance or a type of mixture using background knowledge/resources.

32. Chemistry: 1.12.17 Infinite Campus: Classifying Matter Lab Objectives:
I can classify matter into substances and mixtures. (Quiz)
I can identify and distinguish between physical and chemical properties/changes.

33. Classifying Matter 33

34. Classifying Matter: Micro Level
Substances?
Mixtures?

35. Bell Ringer: Classifying Matter
1. What is the difference between:
a substance and a mixture? Give an example of each.
b. a compound and a mixture? Give an example of each.

36. Matter: Physical vs. Chemical Properties
Physical Properties
Chemical Properties

37. Matter: Physical vs. Chemical Properties
Physical Properties
Does not change the chemical make-up of the matter.
Color, shape, mass, length, odor, states of matter, solubility
Chemical Properties
Does change the chemical make-up of matter.
flammable, neutralization, rusting,decomposing

38. Insoluble Soluble Solubility
How good one substance dissolves (physically mixes) with another substance.
Salt added to water
Insoluble
Soluble 38

39. Soluble Solutions Solutions are composed of: what is dissolved in the
Solute:
what is dissolved in the
solution.
substance you have less of
Solvent:
what dissolves the solute
substance you have more of
water is a common solvent .

40. Neutralization
Change in pH of a solution by the addition of an acid (H+ ions) or a base (OH- ion).

41. Flammability and Combustion
Matter that can catch on fire and produce a lot of energy.

42. Phase Changes physical properties of matter

43. Sublimation solid directly to a gas.
en.wikipedia.org
chemistryjournal104dianegan8.blogspot.com

44. Deposition gas directly to a solid.
www2.volstate.edu
n.wikipedia.org/wiki/Hail

45. Chem I: 1.17.17 Due: Physical vs. Chemical Properties/Change Worksheet
Atomic Structure Ranking Task Worksheet
Objectives:
I can classify changes with matter as physical or chemical. (Physical vs. Chemical Change Lab)
I can apply intermolecular and intramolecular forces with changes that matter undergoes.

46. Chemical vs. Physical Change
Chemical Change:
Physical Change:

47. Chemical vs. Physical Change
Chemical Change:
Matter’s chemical make-up changes.
New matter is produced with new properties.
Ex. Iron Rust (FeO)
Physical Change:
Physical properties change, but chemical properties are preserved.
Matter’s chemical make-up stays the same.
Ex. cutting paper

48. Matter and Forces
Intramolecular Forces Intermolecular Forces

49. Intramolecular Forces
Forces within a compound that hold the atoms
together. (chemical bonds)
Affected/altered during a chemical change.
H2O compound

50. Intermolecular Forces
Forces between compounds in a sample of matter. (group forces)
Affected/altered during a physical change.

51. Matter and Changes
Explain the difference between a matter’s physical property vs. a chemical property. Give an example of each.
Explain the difference between matter undergoing a physical change vs. a chemical change. Give an example of each.

52. Physical vs. Chemical Properties/Change Lab
Goggles must be worn at all times or you will be dismissed from the lab-NO exceptions!
Remember to record all observations.
(needs to be legible and descriptive)
Caution: Working with HCl acid, so be careful.
Disposal of Materials: Most can be discarded down drains except metal waste (Mg).

53. Physical vs. Chemical Properties/Change Lab
Conclusion:
Give an example from the lab where a physical change occurred. What evidence do you have to prove this was a physical change?
Give an example from the lab where a chemical change occurred. What evidence do you have to prove this was a chemical change?

54. Mixtures
Substances in a mixture can be separated from one another through physical processes.
Some common methods to separate mixtures are:
*Filtration
*Extraction
*Distillation
*Chromatography
Explain which methods you applied during the physical vs. chemical change lab?

55. Physical Separation Techniques
Physical property used for separation
For homo or hetero mixtures
Filtration
Extraction
Distillation
Chromatography

56. Filtration
Separating a solid from a liquid in a heterogenous mixture by their size difference. 56

57. Extraction Sand and Iron Filings
1. Extraction- separating substances in a heterogenous mixture from one another based on their unique physical properties.
Sand and Iron Filings 57

58. Physical Separation of Mixtures Distillation
Separation of liquids in a mixture by their differences in boiling points. Ex. Ethanol (78 0C) and Water (1000C)

59. Chromatography Stationary phase
Separates substances present within a homogenous mixture.
Stationary phase
Usually in solid state: ex.chromotography paper
Mobile Phase
Liquid or gas solvent
The two phases help separate
substances in a homogenous mixture based on solubility.

60. Conservation of Matter
Matter can go through physical and chemical changes, but the atoms are always conserved. 60

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

62. 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?

63. Element’s Atomic Numbers

64. 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.

65. 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 65

67. Ions

68. Isotopes

69. Chem I:Isotopes
1. Calculate the protons, neutrons, and electrons 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-11

70. Chem I:Isotopes
1. Calculate the protons, neutrons, and electrons 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-11

71. Mass Number vs. Atomic Mass

72. Mass number: An Atom’s Mass
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.

73. 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. 73

74. Calculating Atomic Mass
Isotope
Natural Abundance (%)

75. Kandium Lab
Purpose: To investigate an new element’s isotopes to calculate what its atomic mass is.