1. TAMING THE TAKS TEST

2. OBJECTIVE FOUR Chemistry
Periodic Table (metals, nonmetals, noble gases)
Atoms and bonding atoms
Properties of Matter
Physical vs Chemical Changes
pH levels
Everything to know about WATER and SOLUTIONS

3. Color the Table like this picture
Red, Green, Blue are METALS
Yellow are NONMETALS
Orange are NOBLE GASES

4. What are Groups & Periods?
Groups/Families
Vertical Columns (Up & Down)
Elements share SIMILAR PROPERTIES because they have the same # of valence electrons (outer energy level)
Periods
Horizontal Rows (Side to Side)
Elements are very DIFFERENT from each other

5. 3 Which of the following groups contains members with similar chemical reactivity?
A Li, Be, C
B Be, Mg, Sr
C Sc, Y, Zr
D C, N, O

6. 4 Basic Types of Elements
Metals: found on the left and center of the Table of Elements
Non-metals: found on the right side of the Table of Elements
Metalloids: found along the stair-step line
Synthetic: made in the laboratory and not yet found in nature – many of the Actinide and Lanthanide series and very large # elements.

7. Where are the metal elements?
Left of the Stair-step line!

8. Properties of Elements - Metals
Metals are:
Conductors
Lustrous
Electron donors
Malleable
Ductile

9. Where are the nonmetals?
To the Right of the stair step line, and Hydrogen!

10. Properties of Nonmetals
Nonmetals are brittle, insulators, electron acceptors
Usually form negative ions (except H)
Many are gases at room temperature
Found to the right of the stair-step line

11. Where are Noble Gases?
Last column on the right! They are perfect!

12. Use the Table provided! What do the numbers mean?
This is the atomic number. It is the number of protons in a single atom of this element. By the way, its also # of electrons. 11 Na
The symbol for this element.
This is the atomic mass, it is the number of protons + neutrons, or the mass of the nucleus of an atom.
22.990
sodium
This is the name of the element.

13. Atoms are. . . The smallest part of a single element.
The basis of all matter.
Made of mostly empty space.
Have a positive core or nucleus.
Have electrons in orbit in clouds.

14. The BOHR Model of an Atom
This is the first model to have a nucleus with protons and neutrons.
The electrons are in various energy levels and circle the nucleus.
Model most people draw today.

15. What are Valence Electrons
Every circle is an energy shell or orbit number
Each shell holds a certain number of electrons
Shell # # of Electrons
1 2
2 8
3 18
MAGIC NUMBER TO REMEMBER IS 8
8 IS GREAT!

16. 23 According to the periodic table, which element most readily accepts electrons?
A Fluorine
B Nitrogen
This is a nonmetal, so it accepts electrons but it will also share them as in NO31-.
C Arsenic
This is a metalloid, so it only sometimes accepts electrons.
D Aluminum
This is a metal so it donates electrons.
Fluorine only needs 1 electron to complete its shell of 8, so it will accept it from any other element very very very easily. This periodic property increases as you move up and left in the table, except for the Noble Gases.

17. Vocabulary
Compound - a pure substance composed of two or more elements whose composition is constant
Mixture - an aggregate of two or more substances that are not chemically united and that exist in no fixed proportion to each other.
Solution - such a substance, as dissolved sugar or salt in solution
Alloy - a substance composed of two or more metals, or of a metal or metals with a nonmetal, intimately mixed, as by fusion or electrodeposition.

18. Law of Conservation of Mass
Mass cannot be created or destroyed…its always there.
Ionic bonding
Covalent bonding

19. Names of Compounds – Ionic
Ionic compounds consist of cations (positive ions) and anions (negative ions).
A Roman numeral in parentheses, preceded by the name of the element, is used for elements that can form more than one positive ion. This is usually seen with metals.
Fe2+ Iron (II) Cu+ Copper (I) Fe3+ Iron (III) Cu2+ Copper (II)

20. Ionic compounds – naming cont.
The -ide ending is added to the name of a single element when it becomes an ion of that element. Oxide, Nitride, Sulfide etc.
Some polyatomic anions have a names ending in -ite for the lower # of oxygens and –ate for more oxygens.
NO2 nitrite NO3 nitrate

21. Covalent Compounds – Names are the Formulas
These are nonmetal to nonmetal compounds.
The name tells you the formula.
Carbon dioxide
1 C and 2 O
CO2

22. Special Names of Compounds Acids and Bases
Acids that are two elements are named Hydro-nonmetal –ic Acid such as
HCl hydrochloric acid
Group -ate becomes –ic and -ite becomes –ous.
H2SO3 sulfurous acid
H2SO4 sulfuric acid
Bases end in the hydroxide anion OH-
They are named with the metal and hydroxide.
NaOH is sodium hydroxide

23. 15 An advertisement claims that patients can be cured of the common cold in 48 hours by vitamin C tablets with secret mineral supplements. In a scientific experiment to test these claims, which data can be considered irrelevant?
A The amount of vitamin C in each tablet
B The severity of the patients’ cold symptoms
C The chemical formula for vitamin C
D The amount of time before symptoms improve

24. What doesn’t matter to the test?
A The amount of vitamin C in each tablet
This should be a controlled variable!
B The severity of the patients’ cold symptoms
This would be very hard to control, but a large experimental group should allow for differences
C The chemical formula for vitamin C
Compound formulas NEVER change so this is our answer it is irrelevant!!!
D The amount of time before symptoms improve
This is what we are testing, it is most relevant.

25. Matter
Anything that has mass and takes up space.
Energy is NOT matter

26. Matter is divided into 3 types:
Elements
Compounds
Mixtures

27. The 3 types can be further separated in two categories:
Mixtures are not pure substances and we will deal with them in a few minutes.
Pure Substances
Elements are the simplest pure substances
Compounds which are formed when two or more elements share electrons or become ions that attract other elements.

28. The 3 types can be further separated in two categories:
Mixtures are not pure substances. Each part of a mixture keeps its own properties, and can be separated out by a physical change.
Pure Substances
Elements are the simplest pure substances
Compounds which are formed when two or more elements share electrons or become ions that attract other elements.

29. P r o p e r t i e s o f M i x t u r e s :
E a c h s u b s t a n c e r e t a i n s i t s o w n p r o p e r t i e s .
S u b s t a n c e s c a n b e p r e s e n t i n a n y a m o u n t .
S u b s t a n c e s c a n b e s e p a r a t e d b y s i m p l e p h y s i c a l m e a n s.

30. There are two types of mixtures:
Heterogeneous- mixture is not the same from place to place.
Chocolate chip cookie, gravel, soil.
Homogeneous- same composition throughout.
Kool-aid, air, brass.

31. Decide if the substance is Element, Compound , or Mixture?
1. Water
1. Compound
2. Compound
2. Table Salt
3. Element
3. Oxygen
4. Mixture
4. Dirt
5. Mixture/Solution
5. Air
Click Mouse button to see answers!

32. Let’s try a few more! 6. Copper 6. Element 7. Solution/Mixture 7. Soda
8. Steel
9. Mixture
9. Rain
10. Mixture
10. Ice-cream
Click Mouse button to see answers!

33. Other Properties of Matter
Density – the amount of matter in a given volume (diet coke vs coke)
Viscosity – resistance of fluid to flow (blood is thicker than water)
Buoyancy – tendency of a less dense substance to float in a more dense liquid (diet coke vs coke)

34. Density
If you’ve ever carried bags of groceries, you know that some bags have greater mass than others, even though the volumes of the bags are the same. Mass and volume are general properties of all matter. Density is the ratio of mass to volume. The density of a specific kind of matter helps to identify it and to distinguish it from other kinds of matter. The unit for density of a liquids is grams per milliliter (g/mL).

35. The density of a piece of matter is a combination of how compressed the material is and how much its atoms or molecules mass per unit volume. Water has a greater density than steam because the atoms in a liquid are closer together than those in a gas. But iron is denser than ice, because the iron atoms are heavier than the water molecules, even though they both are solids.

36. Density is defined as the mass of a substance divided by its volume
Density is defined as the mass of a substance divided by its volume. The equation that is used for determining the density, D, of a substance is D = m/V, where m is the mass of the object, and V is its volume. More dense liquids will sink in the presence of less dense liquids.

37. As temperature is increased (or decreased) there is no change in the mass of an object. However, since substances generally expand as they are heated, the volume will increase with an increase in temperature. This increase in temperature will cause the density to decrease.

38. Density same on the Moon
Since density is related to the mass of an object, the density of a given volume of lead would be the same on both the Earth and the Moon, although the lead would weigh less on the Moon because of the lower gravity there.

39. Typically, when you freeze a liquid, its atoms or molecules get closer together, such that the solid is more dense than the liquid. An exception to this is when you freeze water. When ice is formed, it actually expands, thus making it less dense than water. After the temperature drops below -3 degrees C, the ice contracts and becomes more dense.

40. Viscosity
Viscosity is a property that is often called on when liquids need to be classified. Each liquid has a different viscosity, or resistance to flow. Peanut butter has a much higher resistance to flow than milk, and thus it has a much higher viscosity than milk. We like ketchup that has a high viscosity. Likewise, motor oil is more viscous than gasoline.

41. The viscosity of motor oil is what allows the motor oil to stick to the metal parts of the engine. The weights given on motors oils ,S.A.E. values, correspond to "real" viscosity, taken at specific temperatures. Oils that fall into a certain range are designated 5, 10, 20, 30, 40, 50 by the S.A.E. The W means the oil is suitable for Winter use.

42. Viscosity is a measure of the ease with which molecules move past one another.
Viscosity depends on the attractive force between the molecules.
Viscosity decreases with increasing temperature - the increasing kinetic energy overcomes the attractive forces and molecules can more easily move past each other.

43. Viscosity also affects the shapes of lava flows and the mountains they erupt from. The more viscous the magma, the fatter the lava flow. Also, the more viscous the magma erupted, the steeper the volcano.

44. The viscosity of a given liquid is due to:
the shapes of the molecules
the attractive forces present between the molecules.
Substances with a high viscosity typically have both of these characteristics. The polar ends of the molecules attract each other, while the long structures of the molecules "get tangled" with other molecules. A viscous liquid is somewhat like a tank of snakes with each snake biting another snake’s tail, and each snake’s body wrapped around another snake’s body.

45. You may have heard that 90% of an iceberg lies below the water
You may have heard that 90% of an iceberg lies below the water. Why is that? What determines whether something sinks or floats, and, if it floats, how much of it remains above the surface?

46. Buoyancy!
Buoyancy is the tendency of an object
to float in a fluid. It is controlled by differences in density between the object and the fluid. Buoyancy is summed up by Archimedes Principle: Any object, wholly or partly immersed in a fluid, is buoyed up by a force equal to the weight of the fluid displaced by the object.

47. People or objects that float are positively buoyant
People or objects that float are positively buoyant. Things that are too heavy and sink, they are negatively buoyant. Neutral buoyancy occurs when the force of gravity is balanced by the buoyant force. Divers want neutral buoyancy, a scuba diver does not want to float to the surface or sink to the bottom.

48. Two important forces are in play when Surfing: Buoyancy and Gravity: The water exerts its force on every part of the board that it touches. The weight of the surfer and board give a downward force due to gravity.

49. Three cubes of equal size are put in a fish tank
Three cubes of equal size are put in a fish tank. The left cube is made of stone, the middle cube is made of a plastic with equal density as water, the right cube is made of wood
Positively buoyant
Buoyant force
Neutrally buoyant
Negatively buoyant
Force of Gravity

50. Whether an object floats or sinks, is based on
not only its weight, but also the amount of
water it displaces. That is why a very heavy
ocean liner can float. It displaces a large
amount of water.

51. When an object displaces a fluid it is basically pushing the fluid out of the way. Objects with a large volume displace more fluids that those with small volumes. The more fluid an object displaces the more buoyant that object will be.

52. A block of wood made of oak, for example, sits deeper in the water (and therefore displaces more of the water) than does a block of pine. The reason is that it's heavier for its size, or denser -- in this case, the molecules that make it up are more closely packed together than the molecules that make up the pine.

53. Density = Mass / Volume THIS IS FROM THE FORMULA PAGE
25 A block of maple wood with a volume of
405 cubic centimeters and a density of
0.67 g/cm3 is sawed in half. The density
of the two smaller blocks is now —
A one-fourth the original density
B one-half the original density
C two times the original density
D the same as the original density
If the block is cut in half, you cut the mass in half AND you cut the volume in half, so Mass/ or Volume/2
Mass x (which is really 1) so
Volume 2

54. Use the formula page, D = M/V
20 A sample of an element has a volume of 78.0 mL and a density of 1.85 g/mL. What is the mass in grams of the sample? Record and bubble in your answer to the nearest tenth on the answer document.
Use the formula page, D = M/V
1.85 g/mL =
Multiply both sides by 78.0 mL and you get:
144.3 g Grid it in!

55. Changes in Matter – Physical, Chemical or Nuclear?
Physical changes do not change the substance.
Everything with water (ice is still water)
Cutting a piece of wood does not change the wood, it is simply smaller.
Chemical changes are also called chemical reactions.
When a different substance is produced than what was present at the start, a chemical change has occurred.
Fire, listen, smell

56. Nuclear Changes: Fission and Fusion
Fusion occurs when the nucleus of one atom is joined by the nucleus of another.
This is the reaction that occurs on the sun and stars.
It produces extreme energy release.
Fission occurs when the nucleus of an atom ejects particles and energy when hit by a subatomic particle such as a neutron.
This also causes a release of extreme energy and is the basis of atomic energy plants and bombs.

57. Separating Mixtures – Physical Changes
Separation of mixtures could be:
Magnetic removal (if there is Fe, Ni, Co)
Filtration (if there are large particles)
Hand sorting particles
Decanting (pouring off the less dense liquid)

58. Is this Physical or Chemical

59. Is this Physical or Chemical?
Saliva breaks down the food turning it into chyme and works its way through the digestive system

60. Another technique for separating mixtures:
Evaporation: changing from a liquid to vapor state– leaves behind the other component.

61. Distillation: Process used to remove vapor from liquid by heating
Great for separating two or more liquids which have different boiling points.

62. WATER! WATER! WATER! H2O = 2 hydrogens and 1 oxygen
Water is POLAR due to uneven sharing of electrons
The polarity makes water an effective solvent!
Covalent bonding O H H

63. pH Scale
pH scale ranges from 0 to 14 and measures the amount of H+ (hydrogen ions) and OH- (hydroxyl groups)
Each number represents a factor of 10

64. pH is a measure of the Strength of Acids & Bases
Acids have pH
Bases have pH
Remember because A begins the alphabet and zero begins numbers
Litmus turns red in acids and blue in bases
Phenothalein turns pink in a base and stays clear in acids.

65. Higher pH levels means? 33 Two clear solutions are placed in separate
beakers. The first solution has a pH of 4, and the pH of the second solution is unknown. If
the two solutions are mixed and the resulting
pH is 5, the second solution must have —
A fewer suspended solids
B a lower temperature
C more dissolved salt (NaCl) particles
D a higher concentration of OH– ions
Solutions are homogeneous and have no suspended solids.
Nothing is mentioned about temperature so B is invalid.
NaCl solutions are neutral so have no effect on pH.

66. Solutions
S o l v e n t the substance doing the dissolving in a solution
S o l u t e the substance that is being dissolved in a solution
Ex – Kool-aid
Water is the solvent
Sugar and powder is the solute

67. Solubility
Greatest amount of solute that a solvent will dissolve before the solution becomes saturated
Don’t understand …Then lets make some!

68. Factors that Influence Solubility
Temperature
Most solids increase solubility with increase in temperature
Gas solubility decreases with increasing temperatures
Pressure
Gas solubility always increases as pressure increases
Scuba divers = water pressure increases as you descend
Surface Area
Increase surface area to increase rate of dissolving
ex – granular sugar dissolves quicker than sugar cubes

69. The three methods to increase the rate of solution for a solid are?
Heat it!
Crush it!
Stir it!

70. Solubility Factors – What will dissolve?
Solubility Rules
1. All sodium, potassium, and ammonium salts are soluble.
2. All silver, lead, and mercury salts are insoluble.
3. All carbonates, sulfides, and hydroxides are insoluble.
4. All nitrates and sulfates are soluble except calcium sulfate and barium sulfate.

71. 17 All of these can affect the rate at which a solid dissolves in water except —
A decreasing air pressure
B stirring the water
C increasing the temperature of the water
D using larger crystals of the solid

72. The three methods to increase the rate of solution for a solid are?
Heat it! C
Crush it! D slows it
Stir it! B
So this eliminates choices B, C & D
Which will NOT change it? A
Answer choices were:
A decreasing air pressure
B stirring the water
C increasing the temperature of the water
D using larger crystals of the solid

73. What are the 3 ways to increase the rate at which a solid dissolves?
10 A 0.2 g crystal of gypsum dissolves very slowly in 100 mL of water while the water is stirred. Which of these would cause the gypsum to dissolve faster?
What are the 3 ways to increase the rate at which a solid dissolves?
Heat it!
Crush it!
Stir it!
ANSWER? J
F Decreasing the water temperature
G Stopping the stirring
H Lowering the air pressure
J Crushing the crystal

74. How much solute will dissolve?
A solubility curve shows the amount of each solute that will dissolve in 100g H20 at each temperature.
Saturated is on the line.
Unsaturated is below the line.
Supersaturated is above the line.
Grams solute/100 g H2O

75. 51 At which temperature do KBr and KNO3 have the same solubility
51 At which temperature do KBr and KNO3 have the same solubility? A 27°C B 48°C C 65°C D 80°C

76. Try this one! 49 According to the graph, about how much
hemoglobin would be saturated at an O2
pressure of 7.3 kPa?
A 32%
B 67%
C 89%
D 92%

77. Concentrated or Dilute?
A concentrated solution has as little solvent as possible.
A dilute solution has added solvent.
After adding more solvent, there is still the same mass of solute that you started with.

78. Law of Conservation of Matter
Matter can not be created or destroyed.
The total mass of the substances before they are mixed is equal to the total mass as a mixture.

79. Chemical Reactions
Since matter can not be created or destroyed, chemical reactions must be balanced in terms of mass.
The amount of mass you start with must be equal to the mass of the products.
Reactants  Products
100g total = 100g total

80. 39 According to the law of conservation of mass, how much zinc was present in the zinc carbonate?
Since matter can not be created or destroyed in chemical reactions, the mass on both sides of the arrow must be equal. So 64g + 192g = 256g and 152 g + Zinc = 256g
There must be 104g of Zinc. Answer C.
A 40 g B 88 g C 104 g D 256 g

81. Chemical Equations
Whole numbers written in front of formulas are called coefficients. For example, 4 C6H12O6 indicates that there are 4 molecules of glucose sugar.
To determine how many total atoms of each element are present, multiply the coefficients by the subscripts for each element.
4 C6H12O6 would contain 24 atoms of carbon
(4 x 6), 48 atoms of hydrogen (4 x 12), and 24 atoms of oxygen (4 x 6).

82. To balance equations:
The number of atoms of each type of element on the reactant side (left of the arrow) must be equal those on the product side (right side of the arrow).
2 H2 + O H2O
There are 4 hydrogen atoms on the left (2 H2) and 4 hydrogen atoms on the right (2 H2O)
There are 2 atoms of oxygen (O2) on the left and 2 atoms of oxygen on the right (2 H2O). When a subscript is missing, it is understood to be 1.

83. K H2O  KOH + H2 2 2 2
H OH
19 What is the coefficient for H2O when the above equation is balanced?
A 1
B 2
C 3
D 4
To balance this equation, make water HOH, then you will see that you need 2 H and get 2 OH groups.
That means the KOH gets a coefficient of 2, the K gets a coefficient of 2 and
The water must also get a coefficient of 2.

84. Balance the equation below, the boxes should get the coefficients.2 2
Which element does not have the same number of atoms on both sides? Oxygen. It has 2 on the reactant side and 3 on the product side. If we put a coefficient of 2 in front of PbO, we will now have 4 O and 2 Pb on the right. By placing a coefficient of 2 in front of the reactant, we have 2 Pb and 2 x 2 O. That means it is balanced! Answer? C

85. WE REALLY NEED TO DO SOME TAKS QUESTIONS BECAUSE THE EXIT LEVEL TEST HAS MORE CHEMISTRY AND PHYSICS ON IT!