1. Chemistry – Unit 1, 2
07-PS1-2, 07-PS1-5

2. What is Matter? Journal Prompt 1. Write date in journal
2. Restate question by responding to the following question
What is Matter?

3. Sort Activity
1 – With your talk partner, sort cards by determining matter and non-matter.
2 – Discuss what properties matter has to have to make it matter.
3 – Discuss with your quad what makes matter matter.
4 – Create a graphic organizer with your talk partner and write a statement that describes the properties of matter.

4. Physical and chemical change song

5. 1. Have you written in your agenda yet?
2. Have you turned in your homework?
3. Read article, “Does it Matter?” following directions.
4. Turn to your “talk partner” discuss article.
5. Complete questions at the end of article.

6. Lab safety

7. Physical Properties Lab
1 – Read all directions carefully
2 – Remember Safety Rules
3 – Rotate clockwise through stations when directed to
4 – There are 6 stations
#1 – Density of an regular object
#2 – Density of an irregular object
#3 – States of matter
#4 - Solubility
5 – Record your findings in you journal

8. Vocabulary Relay race 1 – Wait for row # to be called
2 – Race to the back find the word or definition
3 – Hand it to the person at the back of the column
4 – Say the vocabulary word and the definition
5 – Pass the word or definition forward repeating the vocabulary word and definition until it makes it to the front
6 – The team that makes it to the front with the right word and definition scores points
7 – Team with most points win

9. Chemical Reaction

10. A process in which one or more substances change to make one or more new substances.

11. Precipitate

12. A solid that is produced when a chemical reaction occurs in a solution

13. Reactants

14. A substance or molecule that is part of the chemical reaction

15. Products

16. The substance that forms as a result of a chemical reaction.

17. Law of Conservation of Mass

18. A law that states that mass cannot be created or destroyed in ordinary chemical and physical changes.

19. Atom

20. The smallest unit of matter.

21. Molecule

22. The smallest unit of substance that keeps all of the physical and chemical properties of that substance.

23. Compound

24. A substance made up of two or more different atoms bonded chemically.

25. Pure Substance

26. A substance that contains only one kind of element or a single compound that has chemical and physical properties.

27. Chemical Bond

28. An interaction that holds atoms or ions together.

29. Atomic Mass

30. The mass of an atom when you add up its subatomic particles (protons, neutrons.)

31. Chemical Equation

32. A representation of a chemical reaction that uses symbols to show how the reactants and products combine together.

33. Describe the Law of Conservation of Matter
Journal
Describe the Law of Conservation of Matter

34. 1 - Draw a picture of an atom 2 - Label the parts of an atom
Journal
1 - Draw a picture of an atom
2 - Label the parts of an atom

35. Vocabulary Chemical reaction Molecule Precipitate Compound Reactants
Atomic mass
Products
Chemical bond
Law of Conservation of Mass
Pure substance
Atom
Chemical equation

36. Study Jams – Atoms, Protons, Neutrons, Electrons
Atoms are Amazing
Study Jams – Atoms, Protons, Neutrons, Electrons

37. Atomic Structure
The Atoms Family Song

39. Structure of an atom (page 256 in Sciencesaurus)
Nucleus – The core of an atom. Contains protons and neutrons.
Protons – Positively (+) charged particles found in the nucleus of an atom.
Neutrons – Neutrally charged particles found in the nucleus of an atom.
Electrons – Negatively (-) charged particles found outside the nucleus of an atom.

40. Describe the following:
Journal
Element, Compound, Mixture
Describe the following:
Element
Compound
Molecule
Mixture

42. A pure chemical substance consisting of a single type of atom
Element
A pure chemical substance consisting of a single type of atom
A mixture elements
A single element

43. http://chemistry. tutorvista. com/physical-chemistry/covalent-bonding
Molecule
A term used to describe any atoms that are connected by chemical bonds.

44. http://www. freedrinkingwater
Compounds
A molecule made of atoms from different elements. All compounds are molecules, but not all molecules are compounds

45. Which are Which? (identify in your Journal)

46. Mixtures
A substance made up of two or more different substances which are mixed but are not combined chemically.

47. Journal
Elements
Molecules
Compounds
Mixtures
Similar
Different

48. What does a chemical equation tell us?9 8 10 20 30 7 5 2 3 4
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49. Chemical equations tell us how many atoms or molecules react with each other and how much of a substance is needed to react properly with another.

50. Identify the reactants, products, subscripts, and coefficients in this chemical equation:
6 CO2 + 6 H2O + light → C6H12O6 + 6 O2 9 8 10 20 30 7 5 2 3 4
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51. COUNTING ATOMS

52. RULES FOR COUNTING ATOMS
SUBSCRIPTS only refer to the atom that they are BEHIND. For example…
H2S
There are TWO atoms of HYDROGEN and only ONE atom of SULFUR.

53. COEFFICIENTS ATOMS OF HYDROGEN: ATOMS OF SULFUR: 4 2
COEFFICIENTS apply to the entire compound. You MULTIPLY the coefficients and SUBSCRIPTS.
2 H2S
ATOMS OF HYDROGEN:
ATOMS OF SULFUR: 4 2
IF THERE ISN’T A SUBSCRIPT BEHIND AN ELEMENT, ASSUME THERE IS ONLY ONE ATOM OF THAT ELEMENT!

54. PARENTHESES Ba(OH)2 ATOMS OF BARIUM: ATOMS OF OXYGEN:
3. If elements or compounds are inside of PARENTHESES, then the SUBSCRIPT behind the parentheses applies to everything inside.
Ba(OH)2
ATOMS OF BARIUM:
ATOMS OF OXYGEN:
ATOMS OF HYDROGEN: 1 2 2

55. LET’S PRACTICE! 1 2 Al2S3 Atoms of Aluminum: Atoms of Sulfur: 2 3
MgCl2
Atoms of Magnesium:
Atoms of Chlorine: 1 2
Al2S3
Atoms of Aluminum:
Atoms of Sulfur: 2 3

56. PRACTICE 2 1 4 CH3OH Atoms of Carbon: Atoms of Hydrogen: 1
H2SO4
Atoms of Hydrogen:
Atoms of Sulfur:
Atoms of Oxygen: 2 1 4
CH3OH
Atoms of Carbon:
Atoms of Hydrogen:
Atoms of Oxygen: 1 4 1

57. THIS COULD BE A LITTLE TRICKY…
Ca3(PO4)2
Atoms of Calcium:
Atoms of Phosphorus:
Atoms of Oxygen: 3 2 8
Al2(SO4)3
Atoms of Aluminum:
Atoms of Sulfur:
Atoms of Oxygen: 2 3 12

58. What about this BAD BOY??? Atoms of Calcium: Atoms of Phosphorus: 6
2Ca3(PO4)2
Atoms of Calcium:
Atoms of Phosphorus:
Atoms of Oxygen: 6 4 16

59. State the Law of Conservation of Mass
Journal
State the Law of Conservation of Mass
Conservation of Mass Video 8 7 9 20 6 10 4 2 3
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60. Law of Conservation of Matter
Matter cannot be created nor destroyed in an ordinary chemical reaction.

61. Law of Conservation of Mass
In a chemical reaction, in a closed system, the mass of the products will equal the mass of the products.

62. http://images. tutorcircle

63. Conservation of Mass
Doc Brown's Chemistry - GCSE/IGCSE/GCE (basic A level) O Level  Online Chemical Calculations

64. Conservation of Mass Lab

65. Conservation of Mass Lab procedure
1. Collect materials and tools.
2. Put 5 grams of baking soda into your balloon with a funnel. Measure 40 ml of vinegar and pour into coke bottle.
3. Measure the mass of your reactants (baking soda and vinegar) before mixing together. Record results.
4. Place balloon over the top of your coke bottle but do not allow baking soda to be released yet.
5. Mix reactants together. Observe the reaction and record results.
6. Measure the mass of your products (measure with the containers and products), record your results.
7. Draw conclusion about whether or not mass was conserved.

66. Journal
Identify the following as a compound, molecule, element or combination:
1. CaCl2
2. H
3. K
4. O2
Identify the following parts of a chemical equation:
1. reactants
2. products
3. # of reactants in the equation
4. # of Hydrogen atoms
2H2 + O H2O

67. Journal
Using what you have learned about atoms, compounds, and molecules, write a chemical formula for the 4 diagrams shown.

68. Journal
1. A variable is ……..
2. The three kinds of variable are……….

69. 2. Describe where the energy comes from and how we use this energy.
Journal
1. List 3 types of energy.
2. Describe where the energy comes from and how we use this energy.

70. Reviewing Matter
Three principal states of matter
Solid
Liquid
Gas

71. States of matter
Solid: molecules are tightly packed together; definite shape and volume
Liquid: molecules are able to move around, but are still bonded; no definite shape, but definite volume
Viscosity: the resistance of a liquid to flowing.
High viscosity flows slowly
Low viscosity flows quickly
Gas: molecules are spread apart, filling the space available; no definite shape or volume

72. Physical Properties of matter
Boiling point (vaporization): the temperature at which a liquid changes to a gas
Melting point: the temperature at which a solid changes to a liquid
Condensation point: the temperature at which a gas turns to a liquid (the same temperature as the boiling point)
Freezing point: the temperature at which a liquid changes to a solid (the same temperature as the melting point)

73. Changes in Matter
Physical change: alters the form of a substance, but not its identity
Examples: mixing salt and water, freezing water
Chemical change: substances combine or break apart to form new substances
Examples: burning wood, heating sugar to make caramel

75. Mixtures: two or more substances that are in the same place but are not chemically combined
Examples: Kool-aid, sea water
Pure substances: made of only one kind of matter and has definite properties.

76. Elements: a substance that cannot be broken down into other substances by chemical or physical means
Examples: iron, copper, aluminum
Compounds: a substance made of two or more elements that are chemically combined
Examples: sugar, salt