1. Chemistry in Motion: Unit 4
Hobbs

2. The oxidation number (charge) of an atom is show with a _______.
1. Bell Ringer: March 31, 2014
The oxidation number (charge) of an atom is show with a _______.
Negative number
Positive Number
Superscript
Subscript

3. 2. Bell Ringer: Tuesday,
What three items are needed for a Lewis structure? **If you missed the Unit 3 Test the last day to make it up is Thursday!!!! Study!

4. 3. Bell Ringer: Wednesday, 04.02.14
In a chemical formula, like H2O, the number of each type of atom in the compound is shown by numbers called ___________.
Superscripts
Chemical symbols
Oxidation numbers
Subscripts

5. 4. Bell Ringer:
What is the correct chemical formula for magnesium oxide? a. MgO b. MgO2 c. Mg2O2 d. Mg2O ***Naming Quiz TODAY!!!!*** TODAY is the last day to make up your UNIT 3 TEST!!!!

6. ___NH3 + ___ HCl  ___ NH4Cl
5. Bell Ringer: Friday,
Balance the following equation:
___NH3 + ___ HCl  ___ NH4Cl

7. 11. Bell Ringer: 04.14.14 __CaBr2 + __Na2CO3 __CaCO3 + __NaBr
Balance the following chemical equation:
__CaBr2 + __Na2CO3 __CaCO3 + __NaBr

8. 12. Bell Ringer:
What is the difference between the two mixtures below? Can you name each?

9. 13. Bell Ringer: Wednesday, 04.16.14
What is the difference between unsaturated, saturated, and supersaturated? (Think in terms of how much solute vs. solvent)

10. 14. Bell Ringer: Thursday,
Lenox made sweet tea for her family’s dinner that evening. She mixed the sugar in the tea, but not all of the sugar would dissolve. Has Lenox made an unsaturated, saturated, or supersaturated solution? Explain your answer.

11. 16. Bell Ringer: Monday,
The concentration of a solution that contains a large amount of solute in the solvent could be described as ___________.
Concentrated
Dilute
Polar
Unsaturated

12. 17. Bell Ringer: Tuesday,
A substance that produces hydroxide (OH-) ions in water is a(n)
Acid
Base
Hydrocarbon
Salt
Thursday is BLACK and WHITE DAY!
BRING MONEY THURSDAY for the RELAY RALLY 4th BLOCK!!!

13. 18. Bell Ringer: Wednesday, 04.23.14
In a ________________ reaction, an acid and a base produce a salt and water.
A. decomposition
B. dilute
C. neutralization
D. concentrated
Thursday is BLACK and WHITE DAY!
BRING MONEY THURSDAY for the RELAY RALLY 4th BLOCK!!!
DO NOT TOUCH ANYTHING, UNTIL I TELL YOU TO DO SO OTHERWISE, IT IS BOOKWORK for THE WHOLE BLOCK!

14. 19. Bell Ringer: Thursday,
Tomato juice has a pH of 4. What substance would be needed to neutralize tomato juice?
A. vinegar (pH 3)
B. pure water (pH 7)
C. soap (pH 10)
D. ammonia (pH 12)
BRING MONEY THURSDAY for the RELAY RALLY 4th BLOCK!!!

15. 20. Bell Ringer: Friday,
Which solutions are most likely acids?
A. 1 and 3
B. 2 and 5
C. 3 and 6
D. 4 and 7
Solution
Effect on Blue Litmus
Effect on Red Litmus 1
None
Turns blue 2 3 4
Turns red 5 6 7
Once you finish, turn in BELL RINGERS and STUDY for your TEST, don’t act like you didn’t know you had a test, it’s been on the board for weeks and I have also been telling you all week!

16. Unit 3 Review
Two elements with the same number of protons, but different number of neutrons?

17. What is the name of the elements along the stair step line?
Unit 3 Review
What is the name of the elements along the stair step line?

18. Halogens are located in which group?
Unit 3 Review
Halogens are located in which group?

19. Differences between alpha-beta-gamma?
Unit 3 Review
Differences between alpha-beta-gamma?

20. What are the general properties of metals?
Unit 3 Review
What are the general properties of metals?

21. Unit 3 Review
Boron has a mass number of 11 and an atomic number of 5. How many neutrons are in a boron atom?

22. How many electrons are in the outer energy level of Group 17 elements?
Unit 3 Review
How many electrons are in the outer energy level of Group 17 elements?

23. How many protons are in the nucleus of Kr-81?
Unit 3 Review
How many protons are in the nucleus of Kr-81?

24. A(n) ________________ is a horizontal row in the periodic table.
Unit 3 Review
A(n) ________________ is a horizontal row in the periodic table.

25. A vertical column of elements is also referred to as what?
Unit 3 Review
A vertical column of elements is also referred to as what?

26. Unit 3 Review
When an atom is chemically stable, how many electrons are in its outer energy level?
a. 0 b. 7 c. 4 d. 8

27. Make sure group numbers, oxidation numbers and valence electrons are CORRECT!!!!

28. Electron Dot Diagram/Lewis Structure
Electron dot diagram – a diagram or drawing where you use the element’s chemical symbol and valence electrons to show how atoms bond.

29. Electron Dot Diagram/Lewis Structure
Find your element on the periodic table.
Determine the number of valence electrons.
This is how many electrons you will draw.
Find out which group (column) your element is in.
This will tell you the number of valence electrons your element has.
You will only draw the valence electrons.

30. C Lewis Structures Write the element symbol.
Carbon is in the 4th group, so it has 4 valence electrons.
Starting at the right, draw 4 electrons, or dots, counter-clockwise around the element symbol. C

31. C Lewis Structures On your worksheet, try these elements on your own:P Ca Ar Cl Al C

32. Useful Vocabulary
Subscript - is number next to the symbol of an element. It represents how many atoms of a particular element is present in the chemical formula.
Superscript – is the number above the symbol of an element. It represents the oxidation number (charge) of an atom/molecule.
Binary compound – a compound composed of two elements.

33. Chemistry
Chemical bond – attraction between atoms that allows the formation of chemical substances with two or more atoms.

34. Bonding Metallic Bonds Metal and metal bonded Ionic Bonds
Metal and nonmetal bonded to form a compound
Metal is giving its valence electron to the nonmetal
Example: NaCl
Covalent Bonds
Nonmetal and nonmetal bonded to form a compound
The valence electrons will be shared
Example: N2O2

35. Compounds
A compound is a substance composed of two or more elements combined in a specific ratio and held together by chemical bonds.
Familiar examples of compounds are water and salt (sodium chloride).

36. Ionic Compounds
The resulting electrically neutral compound, sodium chloride, is represented with the chemical formula NaCl. The chemical formula, or simply formula, of an ionic compound denotes the constituent elements and the ratio in which they combine.

37. Naming Ions and Ionic Compounds

39. Balancing Equations
Law of Conservation of Mass - in a chemical reaction, the mass of the products equals the mass of the reactants.

40. Balancing Equations: Parts of an Equation
1. Reactants – come after the yield sign
2. Products – come before the yield sign
3. Coefficients – are used to multiply and occur in front of chemical formula

41. Balancing Equations

42. Types of Chemical Reactions
Synthesis: A synthesis reaction is when two or more simple compounds combine to form a more complicated one. These reactions come in the general form of:
A + B ---> AB
One example of a synthesis reaction is the combination of iron and sulfur to form iron (II) sulfide:
8 Fe + S8 ---> 8 FeS

43. Types of Chemical Reactions
Decomposition: A decomposition reaction is the opposite of a synthesis reaction - a complex molecule breaks down to make simpler ones. These reactions come in the general form:
AB ---> A + B
One example of a decomposition reaction is the electrolysis of water to make oxygen and hydrogen gas:
2 H2O ---> 2 H2 + O2

44. Types of Chemical Reactions
Single replacement: This is when one element trades places with another element in a compound. These reactions come in the general form of:
A + BC ---> AC + B
One example of a single displacement reaction is when magnesium replaces hydrogen in water to make magnesium hydroxide and hydrogen gas:
Mg + 2 H2O ---> Mg(OH)2 + H2

45. Types of Chemical Reactions
Double replacement: This is when the anions and cations of two different molecules switch places, forming two entirely different compounds. These reactions are in the general form:
AB + CD ---> AD + CB
One example of a double displacement reaction is the reaction of lead (II) nitrate with potassium iodide to form lead (II) iodide and potassium nitrate:
Pb(NO3)2 + 2 KI ---> PbI2 + 2 KNO3

46. How do we classify matter?
Solute
Atoms
Molecules
Matter
Substances
Elements
Compounds
Mixtures
Homogeneous
Heterogeneous
Solvent

47. Matter Matter is anything made of atoms and molecules.
It is anything that has mass and takes up space.

48. How do we classify matter?
Atoms – is the simplest form of matter
Molecules - a group of atoms bonded together, representing the smallest fundamental unit of a chemical compound

49. Substance
A pure substance is a sample of matter with both definite and constant composition with distinct chemical properties (ex: fluorine)

50. How do we classify matter?
Elements – substance that cannot be broken into two or more simpler substances (ex: mercury)
Compounds - is a substance formed when two or more chemical elements are chemically bonded together. (ex: NO2)

51. Mixture
a mixture is when two or more substances are mixed together but not combined chemically.

52. How do we classify matter?
Mixtures
Homogeneous - is simply any mixture that is uniform in composition throughout, therefore the different parts cannot be seen. (examples: koolaid, lemonade, sweet tea)
Heterogeneous - is made of different substances that remain physically separate, so the different parts are seen.
(ex: trail mix, salads, cereal)

53. Mixtures
Solute – is the smaller portion of the mixture and the part that is being dissolved.
Solvent – the bigger portion of the mixture and the part doing the dissolving.

61. Mixtures
Mixtures
Homogeneous - is simply any mixture that is uniform in composition throughout, therefore the different parts cannot be seen. (examples: koolaid, lemonade, sweet tea)
Heterogeneous - is made of different substances that remain physically separate, so the different parts are seen.
(ex: trail mix, salads, cereal)

62. Mixtures
Solute – is the smaller portion of the mixture and the part that is being dissolved.
Solvent – the bigger portion of the mixture and the part doing the dissolving.

63. Solutions Reading Essentials Book Page 378-382 On your own paper
Respond to questions in the margins, except DO NOT DO THE FOLDABLE!

64. Solutions
A solution is a mixture of two or more substances, aka homogeneous mixture.

65. Solubility
Saturated: describes a solution that has dissolved the maximum amount of solute
Unsaturated: describes a solution that has less than the maximum amount of solute dissolved
Supersaturated: describes a solution that has dissolved more than the maximum amount of solute

66. Solutions
Dilute - make (a liquid) thinner or weaker by adding water or another solvent to it.
Precipitate – a substance is deposited in solid form from a solution.

67. Solutions Scientist use the axiom “LIKE DISSOLVES LIKE”
Nonpolar solute dissolves in a nonpolar solvent
Polar solute dissolves in a polar solute
Electronegativity affects solubility of solutions. If you have nonpolar and polar, your solute will not dissolve.
As you go from left to right across the periodic table electronegativity increases.

68. Can a solution conduct electricity?
Electrolytes are substances that conduct electricity when dissolved in water.
Nonelectrolytes are substances that don’t conduct electricity when in these states.
Examples: NaCl and Sucrose

69. What affects solubility rate of solute?
A. Temperature – heat vs. room temperature or cold
B. Surface Area – compare small area to large area
C. Agitation – stirring, shaking

70. Solubility Curve

73. Solubility Curve
What temperature would a solution need to be to dissolve 110kg of solute?

74. Solubility Curve
If a solution had 100kg of solute dissolved in 80°C, is it a saturated solution?

75. Solubility Curve Which solute is most soluble at 10°C?
How much NaCl can be dissolved in 90°C solvent?

76. Solubility Curve: Gases
Affected by:
Temperature
Pressure
Inverse relationship
Ex: O2 and lake

77. Create a foldable: Acids and Bases
Need 2 pieces of paper
Fold one into the other, create four flaps, then staple the top two corners
1. How Litmus paper/pH paper works
2. List of household Acids and Bases and pH
3. pH scale with numbers and labels (weak acid, weak base, neutral, strong acid, strong base)
4. Acids and Bases Facts
Acids and Bases starts on page 694
Once you finish, start on page

78. Litmus paper Changes colors in the presence of acids and bases
Litmus paper can be either blue or red
ABR – acids turn BLUE litmus paper RED
BRB – bases turn RED litmus paper BLUE

79. pH paper
pH paper is blotting paper that has been treated with a mixture of different indicators. Each indicator changes color over a different pH range.

80. pH scale pH is a measure of how acidic or basic a solution is.
The pH scale ranges from 0 to 14.
Acidic solutions have pH values below 7
A solution with a pH of 0 is very acidic.
A solution with a pH of 7 is neutral.
Pure water has a pH of 7.
Basic solutions have pH values above 7.

81. pH scale
A change of 1 pH unit represents a tenfold change in the acidity of the solution.
For example, if one solution has a pH of 1 and a second solution has a pH of 2, the first solution is not twice as acidic as the second—it is ten times more acidic.

82. Household Acids
Acids 0 - Hydrochloric Acid (HCl) Battery Acid (H2SO4 sulfuric acid) Lemon Juice Vinegar Apples Tomatoes Milk

83. Household Bases
Bases Human Blood Baking Soda (Sodium Bicarbonate) Milk of Magnesia Ammonia Lime (Calcium Hydroxide) Lye Sodium Hydroxide (NaOH)

84. Acid & Base Facts: What is an acid?
An acid is a solution that has an excess of H+ ions. It comes from the Latin word acidus that means "sharp" or "sour".
The more H + ions, the more acidic the solution.

85. Acid & Base Facts: Properties of an acid…
Tastes Sour
Conduct Electricity
Corrosive, which means they break down certain substances. Many acids can corrode fabric, skin, and paper
Some acids react strongly with metals
Turns blue litmus paper red

86. Acid & Base Facts: Uses of Acids
Acetic Acid = Vinegar
Citric Acid = lemons, limes, & oranges. It is in many sour candies such as lemonhead & sour patch.
Ascorbic acid = Vitamin C which your body needs to function.
Sulfuric acid is used in the production of fertilizers, steel, paints, and plastics.
Car batteries

87. Acid & Base Facts: What is a base?
A base is a solution that has an excess of OH- ions.
Another word for base is alkali.
Bases are substances that can accept hydrogen ions

88. Acid & Base Facts: Properties of a base
Feel Slippery
Taste Bitter
Corrosive
Can conduct electricity. (Think alkaline batteries.)
Do not react with metals.
Turns red litmus paper blue.

89. Acid & Base Facts: Uses of Bases
Bases give soaps, ammonia, and many other cleaning products some of their useful properties.
The OH- ions interact strongly with certain substances, such as dirt and grease.
Chalk and oven cleaner are examples of familiar products that contain bases.
Your blood is a basic solution.

90. Acid & Base Facts: Acid-Base Reactions
A reaction between an acid and a base is called neutralization. An acid-base mixture is not as acidic or basic as the individual starting solutions.
Acid + Base  salt + water

91. Acid & Base Facts: Acid-Base Reactions
Each salt listed in this table can be formed by the reaction between an acid and a base.

92. Acids vs. Bases Lab You will be in groups of 2-3 people
Each group will have ONE answer sheet
Each group will have one set of unknowns (one well plate)
Each group will have one set of test papers (red litmus paper, blue litmus paper, and pH paper)
Each UNKNOWN is to be tested with EACH PAPER!!!! (so test it once with the red litmus paper, once with the blue litmus paper, and once with pH paper and RECORD your FINDINGS AFTER EACH on your answer sheet)
Each group will need a paper towel, number the paper towel so you can place each unknown’s test strips in their respective place.

93. AFTER the LAB CLEAN UP YOUR MESS, I AM NOT YOUR MAID!
Complete page , will be graded for accuracy and completion
Complete page , will be graded for accuracy and completion

94. Unknowns 1. lemon juice 2. coffee creamer 3. coke 4. green tea
5. dish soap
6. coconut milk
7. ammonia
8. windex
9. lysol cleaner
10. coffee

95. TODAY:
Complete page , will be graded for accuracy and completion
Complete page , will be graded for accuracy and completion
REVIEW for TEST

96. : TEST DAY
Once finishing YOUR TEST, turn in your test to the lab table (stack for scantrons (A/B), stack for tests (A/B))
Turn in your textbook to Chapter 7 (page ), read the section and answer questions 1-5, bonus points if you answer question 6
NO TALKING UNTIL ALL TESTS and WORK IS TURNED IN!