Term
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Definition
| A method of conversion using the relation between units of measurement |
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Term
| Dimensional Analysis Problem: Convert 6.2 grams to ounces |
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Definition
1 g=0.035274oz
6.2g(0.035274oz/1g)=0.2186988oz
0.22 oz in 6.2 g |
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Term
Dimension Analysis Problem: meters/second to miles/hour
Convert 18 m/s to mi/hr |
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Definition
.001 km=1m
1 km=0.621371 mi
1 min=60 s
60 min=1 hr
18m(.001km/1m)(0.621371mi/1km)=0.01118468 mi/s
0.01118468 mi/s (60s/1min)(60mins/1hr)=40.264848 mi/hr
4.0 x 10^1 mi/hr |
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Term
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Definition
| A physical property; mass divided by volume (D=M/V) |
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Term
Density Problem:
What is the volume of a piece of aluminum with a mass of 0.002 g?
(Density of aluminum is 2.7 g/cc) |
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Definition
D=M/V
2.7 g/cc=0.002g/V
V=0.002g/2.7g/cc
V=0.0007407
V=7 x 10^-4 |
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Term
Dimensional Analysis Problem:
Convert 6 square inches to square centimeters |
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Definition
1 in=2.54 cm
6 in^2 (2.54cm/1 in)^2=51.8616 cm^2
50 cm^2 |
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Term
Density Problem:
Find the mass of a piece of steel with a volume of 6.8 cc
(Density of steel is 7.85g/cc) |
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Definition
D=M/V
7.85g/cc=M/6.8cc
M=53.38g
M=53g |
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Term
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Definition
| A substance that is homogenous and cannot be separated by physical means; compounds, elements |
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Term
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Definition
| A substance containing only one type of atom; hydrogen, oxygen |
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Term
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Definition
| A substance containing two or more elements that can be separated by chemical, but not physical, change; water, carbon dioxide |
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Term
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Definition
| A combination of substances that can be separated through physical means; salt water, a salad |
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Term
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Definition
| A mixture in which the different properties of the substances are visible; salad |
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Term
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Definition
| A mixture in which the different properties of the substances are not visible; salt water |
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Term
| Characteristic Properties of Pure Substances |
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Definition
| Density, boiling point, melting point, solubility, color, etc |
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Term
| Chemical Property vs Physical Property |
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Definition
| A chemical property can only be observed through a chemical change or reaction, whereas a physical property can be observed without changing the matter's composition |
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Term
| Chemical Change vs Physical Change |
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Definition
| A chemical change involves the rearrangement of atoms to form one or more new substances with different properties, whereas a physical change affects the form of a substance rather than its composition |
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Term
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Definition
| Matter is always conserved. The matter before a reaction is equal to the matter after a reaction. |
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Term
Application of the Law of Conservation:
Two substances react. There are 6.3 grams of substance A, and the reaction of substances A and B results in 9.7 grams of substance C. How many grams of substance B were involved in the reaction?
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Definition
6.3 g+ x g=9.7 g
x=3.4g
3.4 g of substance B |
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Term
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Definition
1. All matter is composed of small, indivisible particles called atoms.
2. All atoms of a given element are identical in mass and properties.
3. Compounds are formed by a combination of two or more atoms in definite arrangements in the ratio of small whole numbers.
4. Atoms are not created, destroyed or converted into other kinds of atoms during chemical reactions. They are simply rearranged into new compounds.
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Term
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Definition
| Positively charged subatomic particle inside of the nucleus |
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Term
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Definition
| Subatomic particle inside of the nucleus with no charge |
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Term
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Definition
| Negatively charged subatomic particle orbiting nucleus in the electron cloud |
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Term
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Definition
An atom has no charge, so number p+=number e-
An ion is charged either positively or negatively. An ion of an element has more (neg ion) or less (pos ion) electrons than an atom of that element (the number of protons does not change, because the number of protons identifies the element) |
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Term
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Definition
| A unit of mass used to express atomic weights. It is equal to the weight of 1/12 of a carbon-12 atom |
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Term
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Definition
| The abundance of an isotope in nature as compared to other isotopes of that element |
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Term
Isotopic Abundance Problem:
In element X, there are two different isotopes. X-13 has an isotopic abundance of 93.456% and X-12 has an isotopic abundance of 6.544%. What is the atomic mass of this element? |
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Definition
13x.93456+12x.006544=12.227808
Atomic Mass of 12.227808 amu |
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Term
| How to determine whether isotopes are of the same element |
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Definition
| Number of protons (or, if a neutral atom, electrons) |
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Term
Use Area of Aluminum Foil Lab:
Determine the area of a piece of aluminum foil with a mass of 1.78 g
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Definition
D=2.7g/cc
2.7g/cc=1.78g/V
V=1.78g/2.7/cc
V=0.6592593 cc
V=0.66cc |
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Term
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Definition
| Variants of an element wherein the number of neutrons (and mass number) are different but the number of protons remains the same |
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Term
| Forms of Electromagnetic Radiation (from Left to Right) |
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Definition
| Radio, Microwave, Infrared, Visible (ROYGBIV), Ultraviolet, X-Ray, Gamma Ray |
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Term
| From High to Low Energy on the Electromagnetic Spectrum |
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Definition
-Frequency Decreases
-Wavelength Increases |
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Term
| Law of Multiple Proportions |
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Definition
| When two elements can combine to form more than one compound the amounts of one of them that combines with a fixed amount of the other will exhibit a simple multiple relation. |
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Term
| Rutherford's Experiment (Gold Foil) |
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Definition
| Rutherford aimed alpha particles at a piece of gold foil, expecting them all to pass through. He was surprised to find that some of them were deflected back. This was because they hit the dense, positive nucleus; this discovery changed the model of the atom. |
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Term
| Thomson's Model of the Atom |
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Definition
| Thomson created the plum pudding model of the atom: a positively charged mass with negatively charged particles dispersed throughout |
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Term
| Electron Excitation in Relation to Absorption and Emission |
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Definition
| When an atom absorbs energy in the form of photons (light), an electron can gain enough energy to get excited and move to another energy level. When an electron drops to a lower energy level, this corresponds with the emission of light. |
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Term
How to Use the Formula C=wf
(And an example problem: What is the frequency of a photon of light with the wavelength of 600 nm? |
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Definition
speed of light=(wavelength)(frequency)
speed of light=3.00x10^8 m/s
w is in nm (1x10^-9m) and f in hertz (1/seconds)
3.00x10^8m/s=600nm(1x10^-9nm/1nm)(f)
5x10^16s=f
f=2x10^-17 hertz |
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Term
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Definition
| Hardwater, soft water, supermarket salt, drugstore hydrogen peroxide |
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