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| Law of definite (constant) composition: |
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| elements in a given compound are always combined in the same proportion by mass. This law form the basis for the definition of a chemical compound |
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| for and system closed to all transfers of matter and energy the mass of the system must remain constant over time. *Mass can neither be created or destroyed* |
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| Carbon oxide is made up of 57.1% oxygen and 42.9% carbon. How many grams of carbon and oxygen are in 100 grams of the carbon oxide? |
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| 57.1 g of Oxygen and 42.9 g of Carbon |
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Dalton's atomic theory
1. All matter consists of _______.
2. Atoms of one element cannot be _______.
3. Atoms of one element are identical in ______ and _______. They are different from_____________.
4. Compounds result from the chemical combination of specific _______ of atoms of different elements. |
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1. Atoms
2. converted to atoms of another element
3. mass, properties, atoms of another element
4. ratio |
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| mass/charge ratio of the electron |
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| the nucleus contains most of the mass of the atom, rest is empty space. Used Rutherford gold leaf experiment |
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| different atoms of the same element with a different number of neutrons |
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| isotopes of an element have the _________ chemical properties |
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| isotopes of an element have the _________ physical properties |
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| isotopes of an element have the _________ nuclear properties. |
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| 1g is equal to ________ amu |
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| The process of determining masses and abundances of particles very precisesly |
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The sample is turned into a gas using an electrical heater
step one |
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sample is bombarded with electrons and given a positive charge
step 2 |
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Positive ions are electronically accelerated and all have same kinetic energy
step 3 |
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The positive ions paths are altered with a magnetic field. Lighter ions have less momentum and are deflected more than heavier ions. For a given field, only ions with a particular mass/charge ratio will make it to the detector.
step 4 |
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The magnetic field strength is slowly increased. This changes the mass charge ration of ions that can reach the detector. A mass spectrum is produced.
step 5 |
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| A substance with high electrical conductivity, luster, and malleability, which readily loses electrons to form positive ions (cations). Metals are otherwise defined according to their position on the Periodic Table, including groupings as alkali metals, alkaline earth metals, transition metals, and rare earth metals. |
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| an element with properties intermediate between those of a metal and nonmetal. Metalloids may also be defined according to their location on the Periodic Table. |
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| One of the elements which do not exhibit metallic properties, generally located in the upper righthand corner of the Periodic Table. |
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| compounds are composed of cations and anions. |
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| result of sharing electrons |
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| Filtration is a mechanical or physical process to separate solid particulates from fluids. |
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Definition: Distillation is the technique of heating a liquid to create vapor which is collected when cooled separate from the original liquid.
Examples:
Pure water can be separated from salt water through distillation. Salt water is boiled to create water steam, but the salt remains in the solution. The steam is collected and allowed to cool back into salt-free water. |
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| when an atom loses an electron. positive charge. |
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| when an atom gains and electron. negative charge. |
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The alkali metals and silver (all form 1+ cations)
(Memorize) The alkaline earths, zinc and cadmium (all form 2+ cations)
Aluminum and scandium (form 3+ cations)
For all other metals, the use of Roman numerals is required. |
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| Decimal Prefixes Used with SU units |
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• Mega M 106
• Kilo k 103
• Deci d 10-1
• Centi c 10-2
• Milli m 10-3
• Micro μ 10-6
• Nano n 10-9
• Pico p 10-12 |
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Rules for Significant Figures in Answers
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1. For multiplication and division. The number with the
least certainty limits the certainty of the result. therefore, the
answer contains the same number of significant figures as
there are in the measurement with the fewest significant
figures. Multiply the following numbers:
9 2 cm x 6 8 cm x 0 3744 cm = 23 4225 cm3 = 23 cm3 9.2 cm x 6.8 cm x 0.3744 cm = 23.4225 cm = 23 cm
2. For addition and subtraction. The answer has the same
number of decimal places as there are in the measurement
with the fewest decimal places. Example, adding two volumes
83.5 ml + 23.28 ml = 106.78 ml = 106.8 ml
Example subtracting two volumes:
865.9 ml - 2.8121393 ml = 863.0878607 ml = 863.1 ml |
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