1. Physical properties
- A property that can be observed without changing the sample - color, density, and odor
2. Physical changes
- Material remains the same but its form appears to have changed
3. Chemical change
- An interaction of matter that results in the formation of one or more new substances
4. Chemical properties
- Properties only observed by changing the chemical identity of a sample
5. Burning
- Combustion
6. Metals
- A material with properties like luster, ductility, conductivity, and malleability
7. Nonmetals
- A material with properties such as brittleness, lack of luster, non conductivity/insulators
8. Metalloids
- A material with properties between those of metals and nonmetals
9. Malleability
- The property of a material that permits it to be flattened without breaking
10. Al - Aluminum
11. Sb - Antimony
12. Ar - Argon
13. Ba - Barium
14. Be - Beryllium
15. Bi - Bismuth
16. B - Boron
17. Br - Bromine
18. Cd - Cadmium
19. Ca - Calcium
20. C - Carbon
21. Cs - Cesium
22. Cl - Chlorine
23. Cr - Chromium
24. Co - Cobalt
25. Cu - Copper
26. F - Fluorine
27. Au - Gold
28. He - Helium
29. H - Hydrogen
30. I - Iodine
31. Fe - Iron
32. Kr - Krypton
33. Pb - Lead
34. Li - Lithium
35. Mg - Magnesium
36. Mn - Manganese
37. Hg - Mercury
38. N - Nitrogen
39. Ne - Neon
40. Ni - Nickel
41. O - Oxygen
42. P - Phosphorus
43. Pt - Platinum
44. K - Potassium
45. Rn - Radon
46. Si - Silicon
47. Ag - Silver
48. Na - Sodium
49. S - Sulfur
50. Sn - Tin
51. W - Tungsten
52. U - Uranium
53. Zn - Zinc
54. Why didn't the government make money fully out of copper or zinc?
Copper was too expensive and zinc was too chemically reactive
55. Moles
- represents a number of atoms, molecules, or formula units large enough to be weighed or measured (a chemist's counting unit)
56. Avogadro's number
- 6.02 x 10²³
57. Molar mass
- the mass of one mole in a substance
58. Percent composition
- percent by mass of each component in a material/the percent by mass of each element within a compound
59. How do you find the molar mass of an element?
- Take the number of atoms in an element and multiply it by it's atomic weight to find the molar mass of that element. Then add all the molar masses of all the elements together to get the molar mass of the substance.
60. Chemical change
- Combustion, rusting of iron, and mixing substances
61. Physical change
- Electricity, states of matter, melting, freezing, vaporization, condensation
62. What is the difference between chemical and physical changes?
- A chemical change makes a new substance (light, heat, color change, gas production, odor, or sound). Physical changes are the same material, even though they look different.
63. What are the 3 layers of Earth?
- Atmosphere, hydrosphere, lithosphere (crust, mantle, core)
64. Atmosphere
- Gaseous envelope surrounding Earth containing nitrogen, oxygen, neon, and argon
65. Hydrosphere
- All parts of Earth where water is found
66. Lithosphere
- Solid outer layer of Earth that contains a variety of chemical resources
67. Ore
- A rock/mineral that contains metals and other useful substances in them
68. Mineral
- A solid substance removed from ores to get a particular element
69. Ductility
- The ease of being drawn into thin wires
70. Properties of copper
- Conducts electricity, low cost, resists corrosion, ductile
71. Life of copper
- Copper is mined out, then reduced from the ore and built into something else. It is then recycled and melting into another object.
72. Describe metals
- Luster, malleable, conduct electricity, react with acids, black colored elements
73. Who created the periodic table?
- Dimitri Mendeleev
74. How is the periodic table organized?
- Atomic weight and combining capacity
75. How was the first periodic table organized?
- Elements with similar chemical properties were put in the same vertical column. Elements with increasing atomic weights were put in horizontal rows.
76. What type of elements are in the leftmost columns? Rightmost?
- Reactive metals, unreactive (noble) gases
77. Atomic number
- The number of protons in an atom
78. Isotopes
- Atoms with the same number of protons but different numbers of neutrons, making them have different mass numbers
79. Nucleus
- A positively charged region (due to protons) in the center of an atom
80. Mass number
- The total number of protons and neutrons
81. Periods
- Horizontal rows with increasing atomic numbers with similar properties
82. Group/family
- Vertical columns with similar properties in elements
83. Alkali metal family
- 6 elements (starting with lithium) in the first column on the left side
84. Noble gas family
- Elements on rightmost side that are unreactive
85. Halogen family
- Group of elements directly to the left of the noble gas family
86. How do you find the density of an element?
- Average the two elements above and below it
21. Cs - Cesium
22. Cl - Chlorine
23. Cr - Chromium
24. Co - Cobalt
25. Cu - Copper
26. F - Fluorine
27. Au - Gold
28. He - Helium
29. H - Hydrogen
30. I - Iodine
31. Fe - Iron
32. Kr - Krypton
33. Pb - Lead
34. Li - Lithium
35. Mg - Magnesium
36. Mn - Manganese
37. Hg - Mercury
38. N - Nitrogen
39. Ne - Neon
40. Ni - Nickel
41. O - Oxygen
42. P - Phosphorus
43. Pt - Platinum
44. K - Potassium
45. Rn - Radon
46. Si - Silicon
47. Ag - Silver
48. Na - Sodium
49. S - Sulfur
50. Sn - Tin
51. W - Tungsten
52. U - Uranium
53. Zn - Zinc
54. Why didn't the government make money fully out of copper or zinc?
Copper was too expensive and zinc was too chemically reactive
55. Moles
- represents a number of atoms, molecules, or formula units large enough to be weighed or measured (a chemist's counting unit)
56. Avogadro's number
- 6.02 x 10²³
57. Molar mass
- the mass of one mole in a substance
58. Percent composition
- percent by mass of each component in a material/the percent by mass of each element within a compound
59. How do you find the molar mass of an element?
- Take the number of atoms in an element and multiply it by it's atomic weight to find the molar mass of that element. Then add all the molar masses of all the elements together to get the molar mass of the substance.
60. Chemical change
- Combustion, rusting of iron, and mixing substances
61. Physical change
- Electricity, states of matter, melting, freezing, vaporization, condensation
62. What is the difference between chemical and physical changes?
- A chemical change makes a new substance (light, heat, color change, gas production, odor, or sound). Physical changes are the same material, even though they look different.
63. What are the 3 layers of Earth?
- Atmosphere, hydrosphere, lithosphere (crust, mantle, core)
64. Atmosphere
- Gaseous envelope surrounding Earth containing nitrogen, oxygen, neon, and argon
65. Hydrosphere
- All parts of Earth where water is found
66. Lithosphere
- Solid outer layer of Earth that contains a variety of chemical resources
67. Ore
- A rock/mineral that contains metals and other useful substances in them
68. Mineral
- A solid substance removed from ores to get a particular element
69. Ductility
- The ease of being drawn into thin wires
70. Properties of copper
- Conducts electricity, low cost, resists corrosion, ductile
71. Life of copper
- Copper is mined out, then reduced from the ore and built into something else. It is then recycled and melting into another object.
72. Describe metals
- Luster, malleable, conduct electricity, react with acids, black colored elements
73. Who created the periodic table?
- Dimitri Mendeleev
74. How is the periodic table organized?
- Atomic weight and combining capacity
75. How was the first periodic table organized?
- Elements with similar chemical properties were put in the same vertical column. Elements with increasing atomic weights were put in horizontal rows.
76. What type of elements are in the leftmost columns? Rightmost?
- Reactive metals, unreactive (noble) gases
77. Atomic number
- The number of protons in an atom
78. Isotopes
- Atoms with the same number of protons but different numbers of neutrons, making them have different mass numbers
79. Nucleus
- A positively charged region (due to protons) in the center of an atom
80. Mass number
- The total number of protons and neutrons
81. Periods
- Horizontal rows with increasing atomic numbers with similar properties
82. Group/family
- Vertical columns with similar properties in elements
83. Alkali metal family
- 6 elements (starting with lithium) in the first column on the left side
84. Noble gas family
- Elements on rightmost side that are unreactive
85. Halogen family
- Group of elements directly to the left of the noble gas family
86. How do you find the density of an element?
- Average the two elements above and below it
Study Guide for Test 2
1. What is pH? Give examples of substances on the pH scale.
- The pH scale is an acidic graph. On the graph, 1 is vinegar, 7 is water, 9 is ammonia, and 14 is the highest number. Numbers 1-7 on the graph are acids, 7-14 on the graph are basics.
2. Convert 100 km/hr to m/s.
- 360, 000, 000
3. Convert 905 mg to kg.
- 0.000905
4. What are the charges and weights of electrons, protons, and neutrons?
- Electrons: negative with the lowest weight
- Protons: positive with the same weight as neutrons
- Neutrons: neutral with the same weight as protons
- Protons and neutrons have higher weights than electrons
5. How are cations formed?
- Cations are formed when an atom loses any amount of electrons
6. How many electrons are gained or lost in the first column on the periodic table and what are the charges of those ions?
- They lose 1 electron giving them a charge of 1+
7. How many electrons are gained or lost in the second column on the periodic table and what are the charges of those ions?
- They lose 2 electrons giving them a charge of 2+
8. How many electrons are gained or lost in the sixth column on the periodic table and what are the charges of those ions?
- They gain 2 electrons giving them a charge of 2-
9. How many electrons are gained or lost in the seventh column on the periodic table and what are the charges of those ions?
- They gain 1 electron giving the a charge of 1-
10. How many electrons are gained or lost in the eighth column on the periodic table and what are the charges of those ions? What are these ions called?
- The don't gain or lose any electrons. They are called noble gases.
11. Give examples of cations and anions.
- Anion: Bromine
- Cation: Sodium
12. What is an atoms composed of?
- Nucleus, protons, neutrons, and electrons
13. Why can't water be 100% sure? What is in even the purest water?
- To make water 100% sure would be too expensive but even then there would still be atmospheric gases in the water.
14. How can we dissolve more solute in water?
- Make the temperature higher by putting pressure on it
15. Name the ionic compounds for the following: K+ and I-, Ba2+ and OH-, Al3+ and O2-
- KI
- Ba(OH)2
- Al2O3
16. What is the atomic symbol for mercury? What is the atomic number and weight? How many protons, neutrons, and electrons are in mercury?
- Hg
- 80, 200.59
- 80 protons, 120 neutrons, and 80 electrons
17. What is an unsaturated solution? What is a saturated solution?
- A solution with a lower amount of solute than a saturated solution
- A solution where the solvent has as much dissolved solute that it can hold at a specific temperature
18. Explain how to make a supersaturated solution?
- Boil the solution until the solution has lost about a tenth of its volume. Let it cool slowly and drop a crystal of the solute into the solution. When the crystals settle to the bottom, the solution is supersaturated.
19. a. Polarity: Opposites attract - the positive and negative ends in atoms
b. Ionic bonds vs. Covalent bonds: Ionic bonds are not as strong as covalent bonds
c. Reactants vs. Products:
- Reactants are the starting substances in a chemical reaction
- Products are the answer of the chemical reaction
d. Solute vs. Solvent vs. Solubility vs. Solution:
- Solute is the substance that is being dissolved
- The solvent is the dissolving agent
- Solubility is an amount of a solute that dissolves in a solvent to form saturated solution
- Solutions are homogeneous mixture of two or more substances
e. Saturated vs. Unsaturated vs. Supersaturated:
- Saturated solution is a solution where the solvent has dissolved as much solute as it can
- Unsaturated solution is a solution with a lower amount of solute than a saturated solution
- Supersaturated solution has higher amounts of solute than a saturated solution once the solvent
has been heated and cooled.
f. Mean vs. Median:
- Mean is the average
- Median is all the data put together and finding the number exactly in the middle
g. Chlorine vs. Chloride:
- Chlorine is an element
- Chloride in an ion
h. Subscript vs. Superscript
- Subscripts are written below the writing line indicating the number of atoms in an element
- Superscripts are written above indicating the charge of an ion
i. Suspension vs. Solution
- Suspension is a mixture with dispersed solid particles that settle or can be separated by filtration
- Solutions are homogeneous mixture of two or more substances
j. Tyndall Effect
- The scattering of light due to the reflection of particles
k. Catalyst
- Catalysts speed up the process of a chemical reaction
l. Conservation of Matter
- No matter is destroyed or created
Unit 1B (1-4) Vocab
Matter:
Any thing that occupies space and has mass
- Solids
- Liquids
- Gas
Physical Properties:
Properties that can be observed and measured without changing the chemical makeup of the substance
- Density
- Freezing, melting, and boiling points
Density:
Mass of material within a given volume
Freezing Point:
The temperature where a liquid turns into a solid
Aqueous Solution:
A water-based solution or a solution where water dissolves a substance
Mixture:
The result of when 2 or more substances are combined but they keep their individual properties
Heterogeneous Mixture:
A mixture that doesn't have the same concentration throughout
Suspension:
A mixture containing dispersed solid particles that settle or can be separated by filtration
Tyndall Effect:
The scattering of light due to the reflection of particles
Colloid:
A mixture containing small particles that don't settle
Homogeneous Mixture:
A mixture that has the same concentration throughout
Solution:
A homogeneous mixture of 2 or more substances
Solute:
The dissolved substance in a mixture
Solvent:
The dissolving agent in a mixture
Particulate Level:
The area of interest of unseen atoms, molecules, and ions in contrast to observable macroscopic entities
Atoms:
The smallest particle possessing the properties of an element
Element:
The fundamental chemical substances from which all other substances are made
Compound:
A substance that is composed of the atoms of 2 or more elements linked together chemically
Chemical Formulas:
An expression representing the elements in a substance with subscripts that indicate the number of atoms in each element
Substance:
An element or a compound or a material with a uniform, a definite composition, and distinct properties
Molecule:
The smallest particle of a substance keeping all the properties of that substance
Chemical Bond:
The force that holds atoms and ions together
Unit 1A Vocab
Filtration:
Solid particles are separated from a liquid by passing the mixture through a material that retains the solid particles and allows the liquid to pass through
Filtrate:
The liquid collected after it has been filtered
Adsorbs:
Attracts and holds on it's surface
Percent Recovery:
The proportion of sought material recovered in a process
Histogram:
A graph indicating the frequency or number of instances of particular values(or value ranges) within a set of related data
Range:
The difference between the largest and smallest values in a data set
Average:
Adding all the values together and dividing the sum by the total number of values
Mean:
Average
Median:
The middle value
Electrical Conductivity:
The ability to transmit an electric current
Direct Water Use:
Water consumed by an end user and can be directly measured
Indirect Water Use:
Water consumed in the preparation, production, or delivery of goods and services
Gaseous State:
Water vapor in the air
Liquid State:
In lakes, rivers, oceans and clouds
Solid State:
Ice
Surface Water:
Water found on Earth’s surface, such as oceans, rivers, and lakes
Ground Water:
Water from an aquifer or other underground source
Aquifer:
A structure of rock, sand, or gravel that holds water beneath Earth’s surface
No comments:
Post a Comment