1. Chemistry – Matter Unit
What is matter?
What is chemistry?
What is the organization of matter?
What is the nature of matter?

2. What is NOT Matter?
Energy !

4. Types of Energies
Mechanical
Chemical
Heat
Atomic
Light
Electrical

5. Is Air matter? What are the two criteria for matter?
Does it take up space?
Does it have mass?

6. What is chemistry?
“Chemistry is the study of the composition, structure, and the properties of matter and the changes it undergoes.”
All chemical reactions involve energy.

7. What is the composition of matter?
Pure Matter Substance
Impure Matter Mixture

8. What is a pure substance?
A pure substance has a definite composition (proportion).
The composition of a substance will have the same percent of elements no matter where the sample was obtained.
Water from Lake Okechobee and water from the Atlantic Ocean (once cleaned up) will have the same composition of hydrogen to oxygen.
Gold is the same as other gold (once cleaned up).

9. What is a pure substance?
A pure substance, by definition, is an element or a compound.
A container with an almost pure compound:

10. Pure Substance
Pure Substance
Compound
Element

11. What is an element? “a pure substance made of only one kind of atom”
A substance that cannot be decomposed any farther by simple chemical means
An element has a definite composition. Gold from South Africa is the same, when purified, as a sample from California.

12. Periodic Table of Elements
Most elements on the periodic chart are metals.
Elements through 114 but not 113 have been discovered or made.

13. Zinc, copper, lead, carbon, sulfur
Elemental Samples
Zinc, copper, lead, carbon, sulfur

14. What is a compound?
“A compound is a substance that is made from the atoms of two or more elements that are chemically bonded.”
The definition is actually more involved than this.

15. What is a compound?
A compound is a substance that cannot be decomposed any farther by simple physical means.
A compound has a definite composition by mass.
A compound is made up of two or more elements chemically combined.

16. What is a compound?
A compound no longer has the properties of its constituent elements.
Table salt, NaCl or sodium chloride, is a compound of the element sodium and the element chlorine.

17. Sodium

18. Sodium metal Soft, can be cut with a knife Shiny
Good conductor of electricity
Very reactive

19. Sodium in water

20. Chlorine gas

21. Chlorine gas
Greenish gas
Poisonous
Heavier than air

22. Sodium in chlorine gas

23. Sodium chloride, NaCl
Sodium chloride dissolves in water rather than reacts with water.
Sodium chloride is a white solid, not a poisonous green gas.
Sodium chloride is its own substance with its own properties, not those of either sodium or chlorine.

24. Samples of Other Compounds
Sucrose (table sugar), Sodium Chloride, Water, Copper(II) sulfate

25. Colored Compounds
Cobalt(II) chloride, Iron(II) sulfate, Potassium dichromate, Potassium chromate, Nickel(II) nitrate, copper(II) sulfate

26. What is the composition of matter?
Pure Substance
Impure Matter
Mixture

27. Impure Matter - Mixture
“A mixture is a blend of two or more kinds of matter, each of which retains its own identity and properties.”
A mixture is made up of two or more substances that are not chemically combined.

28. Mixtures Mixtures can be separated by simple physical means.
Two mixtures containing the same substances may not have the same proportions.
Example: Very salty water versus barely salty water. Very sweet sugar water versus slightly sweet sugar water.

29. Two mixtures of the same substances may have different proportions.
Water and Dye Mixture
Two mixtures of the same substances may have different proportions.

30. Mixtures
Mixtures
Homogeneous Mixture
Heterogeneous Mixture ?

31. Solutions
Mixtures
Mixture = a blend of two or more kinds of matter, each of which retains its own identity and properties
a) homogeneous mixture = a mixture that is uniform in composition throughout
Ex: Food coloring and water
b) heterogeneous mixture = a mixture that is NOT uniform in composition throughout
Ex: Oil and water

32. Heterogeneous Mixtures
Sand and water on the left and sand and gravel on the right.

33. Heterogeneous Mixture

34. Types of Mixtures: Ex: Sand and water
1) solution = a homogeneous mixture
2) suspension = a mixture in which the particles are so large that they settle out unless the mixture is constantly stirred or agitated
Heterogeneous mixture
Ex: Sand and water
3) colloid = a mixture consisting of particles that are
intermediate in size between those in solutions and those in suspensions
Heterogeneous mixture
Ex: Milk

35. Colloidal Suspension
Fog

36. Tyndall Effect

37. THE NATURE OF SOLUTIONS:
Solvent = the substance that does the dissolving in a solution
a) Typically present in the greatest amount
b) Typically a liquid
c) Water is the most common or “universal” solvent
2) Solute = substance being dissolved in a solution
a) Typically present in the least amount
b) Typically a solid

38. 9 Possible Solution Combinations:

39. Factors Affecting the Rate of Dissolving (Increase Solution Rate):
1) Grinding: increases surface area
2) Stirring: allows solvent continual contact with solute
3) Heating: increases kinetic energy; increases mixing

41. SOLUBILITY:
1) Solubility = quantity of solute that will dissolve in specific amount of solvent at a certain temperature.
(pressure must also be specified for gases).
Ex: 204 g of sugar will dissolve in 100 g of water at 20°C
soluble and insoluble are relative terms
solubility should NOT be confused with the rate at which a substance dissolves
2) saturated solution = a stable solution in which the maximum amount of solute has been dissolved.

42. 3) solution equilibrium = state where the solute is dissolving at the same rate that the solute is coming out of solution (crystallizing). a) Opposing processes of the dissolving and crystallizing of a solute occur at equal rates. b) solute + solvent solution

43. 4) unsaturated solution = a solution that contains less solute than a saturated solution under existing conditions 5) supersaturated solution = a solution that temporarily contains more than the saturation amount of solute than the solvent can hold (unstable)

44. 3 FACTORS EFFECTING SOLUBILITY:
The extent to which a given solute dissolves in a solvent depends on the identity of the solute and solvent and also on the existing conditions of pressure & temperature
1) Nature of solute and solvent
“Like dissolves like” = rule of thumb for predicting whether or not one substance dissolves in another
• “Alikeness” depends on:
o Intermolecular forces
o Type of bonding
o Polarity or nonpolarity of molecules:
ionic solutes tend to dissolve in polar
solvents but not in nonpolar solvents

45. Solvent-Solute Combinations:

46. 2) Pressure:
a)Pressure has little effect on the solubility of liquids or solids in liquid solvents.
b)The solubility of a gas in a liquid solvent
INCREASES when pressure increases. It is a direct relationship.

47. 3) Temperature:
a)The solubility of a gas in a liquid solvent DECREASES with an increase in temperature.
b)The solubility of a solid in a liquid solvent MOST OFTEN increases with an increase in temperature. However, solubility changes vary widely with temperature changes
sometimes decreasing with temperature increases.

48. Mixtures vs. Compounds Rocks are mixtures.
Minerals are pure substances
Granite rock

49. Mixtures vs Compounds
Minerals are pure substances although many have impuities that must be cleaned up first.

50. Minerals
Amethyst
Halite
Diamond

51. What is the nature of matter?
An atom is the smallest unit of an element that maintains the properties of that element
An atom is made up of electrons, protons, and neutrons as well as other particles.
Protons and neutrons are made up of quarks.

52. What is the nature of matter?
A molecule is a unit that consists of more than one atom bonded together.
A molecule can have atoms of the same element such as oxygen. These are called diatomic elements.

53. Blue – diatomic elements
Diatomic elements – blue
Tetraatomic element – red
Octatomic element - yellow
Blue – diatomic elements

54. What is the nature of mature?
A molecule can have atoms of more than one type of element.
Water
Sugar (sucrose)

55. Atoms and Molecules Three particles: One particle: 2 atoms of hydrogen
1 atom of oxygen
One particle:
1 molecule of water

56. Nuclear Reaction Atoms
How can an atom of an element be broken up into atoms of other elements or into other smaller particles and energy?
Nuclear Reaction

57. Compound Use a chemical separation method.
How is a compound broken up into its elements or other simpler compounds?
Use a chemical separation method.
What are some examples of chemical separation methods?

58. Chemical Separation Methods
Heat the compound.

59. Chemical Separation Methods
Use Electrolysis which is using an electric current to decompose the compound.
An electrolyte has been added to the water since water does not conduct.

60. Mixtures How can mixtures be separated?
Use Physical Separation Methods.
What are examples of physical separation methods?

61. Physical Separation Methods
Distillation is the separation of mixtures by using the difference in boiling points of liquids.
A water cooled condenser is used.

62. Physical Separation Methods
Filtration uses the difference in particle size to separate mixtures.
Filter papers have different size pores.

63. Physical Separation Methods
Chromatography uses the difference in solubility in various solvents.
Gas, liquid, thin layer, and paper chromatography are widely used.

64. Three states of matter:
Liquid, solid, gas

65. Physical Changes
During physical changes matter changes in appearance without forming new substances.
What some examples of physical changes?

66. Physical Change Examples
Breaking or tearing

67. Physical Change Examples
Boiling or condensing

68. Physical Change Examples
Freezing or melting

69. Physical Change Examples
Sublimation

70. Physical Change Examples
Sublimation:
“The change of state directly to a gas is known as sublimation.”
“The reverse process is called deposition, the change of state from a gas directly to a solid.”

71. Chemical Changes
During chemical changes new substances are formed with different properties than the original substances.
What is an example of a chemical change?

72. Chemical Change Example
Heating baking soda, sodium hydrogen carbonate, forms sodium carbonate, carbon dioxide, and water. The formation of carbon dioxide is what causes cakes to rise.

73. Mixture or Pure Substance
These bottles contain sodium chloride, sucrose, and a mixture of the two. Which is which and how can they be identified?

74. Physical and Chemical Properties
What are some physical properties of this pen?

75. Physical Properties Examples: Color Hardness Texture Volume Length
Mass

76. Physical Properties More Examples: Density (mass/volume ratio) Odor
Sound
Boiling point
Melting point
Magnetism

77. Melting Point and freezing point temperatures are the same.
Physical Properties
Melting Point and freezing point temperatures are the same.

78. Chemical Properties A chemical property is how something reacts.
Does the pen float is physical.
Does the pen dissolve is physical.
Does the pen react with water is chemical.

79. Chemical Properties Does the pen burn is a chemical property.
Whether and how something reacts is chemical.

80. Extensive vs Intensive
Extensive Properties depend upon the amount of matter that is present.
Intensive Properties do not depend on the amount of matter present. These properties are the same for a given substance regardless of how much of the substance is present.

81. Extensive vs Intensive
Which of the properties listed earlier are extensive and which are intensive?
Comparisons of several properties are used together to identify an unknown.

82. Matter Unit
Now it is time to try “Chemistry Vocabulary Worksheet: Application of Matter”. .

83. Chemistry Vocabulary H C O Fe Cl Ag Cu Ba Cf
A Symbol is a representation of an element.
One or two letters may be used.
The first letter is upper case while the second is lower case.
H C O
Fe Cl Ag
Cu Ba Cf

84. Chemistry Vocabulary
A formula is a representation of a molecule of an element or a molecule of a compound.

85. Chemistry Vocabulary
The subscript represents the number of atoms of a particular element in the molecule.
12 atoms of carbon
22 atoms of hydrogen
11 atoms of oxygen

86. Chemistry Vocabulary
If no subscript is shown. An understood one is indicated.
2 atoms of hydrogen
1 atom of sulfur
4 atoms of oxygen

87. Chemistry Vocabulary
A coefficient is a number in front of a formula and represents the number of molecules.
If no coefficient is shown, one molecule is indicated.
2 molecules of sucrose
24 atoms of carbon
44 atoms of hydrogen
22 atoms of oxygen

88. Chemistry Vocabulary
An equation is a sentence showing what is happening in a chemical reaction.

89. Chemistry Vocabulary
The reactants are the substances (elements or compounds) that will react. They are on the left or starting side.

90. Chemistry Vocabulary
The products on the right side of the equation are what are formed or are produced during the reaction.

91. Chemistry Vocabulary
An atom is the smallest unit of an element that maintains the properties of that element
An atom is made up of electrons, protons, and neutrons as well as other particles.
Protons and neutrons are made up of quarks.

92. Chemistry Vocabulary
A atom is made up of a nucleus and particles outside the nucleus called electrons.
Electrons are negatively charged particles.
The mass of an electron is about 1800 times smaller than that of the proton and neutron.

93. Chemistry Vocabulary
The nucleus is the tiny positive core of the atom.
Two of the particles in the nucleus are the proton and the neutron.
The proton is a positively charged particle.

94. Chemistry Vocabulary What is wrong with this commonly used picture?
The nucleus is 1/10000 times smaller than the atom.
The atom is mostly empty space.

95. Chemistry Vocabulary Proton: A proton is made up of three quarks.
The charge on a proton is equal in magnitude but opposite in sign to the charge on an electron.
A proton is made up of three quarks.
Two quarks have a +2/3 charge.
One quark has a -1/3 charge.

96. Chemistry Vocabulary
The mass of a proton is approximately 1800 times heavier than an electron.
***The number of protons present is what determines the type of atom.***
If the number of protons change, an atom of a different element is formed.

97. Chemistry Vocabulary
The number of protons found in the nucleus is known as the atomic number.
Hydrogen with an atomic number of 1 has only one proton. If it had 2, it would be helium.
Uranium with an atomic number of 92 has 92 protons.

98. Chemistry Vocabulary
A neutron is an uncharged particle found in the nucleus.
The mass of a neutron is almost the same as the mass of a proton.
A neutron is made of three quarks.
One quark has a +2/3 charge.
Two quarks have a -1/3 charge.

99. Chemistry Vocabulary
Two atoms of the same element can have differing numbers of neutrons. These are called isotopes.
Hydrogen has three isotopes:
Hydrogen with 1 proton and 0 neutrons
Deuterium with 1 proton and 1 neutron
Tritium with 1 proton and 2 neutrons

100. Chemistry Vocabulary
The different masses of these isotopes give them different properties such as melting and boiling points and reactivities and stabilities.
Regular uranium is not radioactive enough for a nuclear fuel. Only certain isotopes of uranium will work.

101. Chemistry Vocabulary
The mass number is the total number of protons and neutrons in the nucleus of the atom.
The mass number is not found on the periodic table.
The masses on the table are the weighted averages of the isotopes.

102. Chemistry Vocabulary Particle Symbol Charge Mass Number Electron 1-
Proton 1+ 1
Neutron

103. Chemistry Vocabulary Nuclear Symbol: Mass Number Atomic number
Number of protons and neutrons
Atomic number
Number of protons
Found on Periodic Table

104. Chemistry Vocabulary Number of protons = 17 Number of neutrons = 18
Number of electrons=
The number of protons = number of electrons

105. Chemistry Vocabulary Number of protons = 12 Number of neutrons = 13
Number of electrons=

106. Chemistry Vocabulary
In a neutral atom the number of protons is equal to the number of electrons.
The number of protons can never vary in an atom.
The electrons are the particles that can be gained or lost in a reaction.

107. Chemistry Vocabulary
The sum of the positive protons and the negative electrons give the overall charge of the atom.
The term charge was once called valence.
The charge is shown as a superscript to the upper right.

108. Chemistry Vocabulary Number of protons = 17 Number of neutrons = 19
Number of electrons= 18
(17+) + (?-) = 1-
So ? = 18-

109. Chemistry Vocabulary Number of protons = 12 Number of neutrons =
Number of electrons= 10
(12+) + (?-) = 2+
?- = 10

110. Chemistry Vocabulary An ion is a charged atom or group of atoms.
A cation is a positively charged ion.
An anion is a negatively charged ion. The prefix an- can mean not or negative.

111. Chemistry Vocabulary
Free state – The atom or molecule is not combined with atoms of other elements.
Gold can be found in the free state.
Because of its reactivity, sodium cannot.
Combined state – The atom is part of a compound.

112. Matter Unit
Now it is time to try “Chemistry Vocabulary Worksheet: Application of Matter”.
The exam will cover the material in this unit, the lab safety material, and the lab drawer equipment.
Know the examples and how the ideas go together. Know all parts of the definitions.