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| John Dalton's Atomic Theory |
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1. Elements: are composed of extremely small particles called atoms. All atoms of a given element are identical, having the same size, mass, and chemical properties. The atoms of one element are different from the atoms of all other elements
2. Compounds: are composed of atoms of more than one element. In any compound, the ratio of the numbers of atoms of any two of the elements present is either an integer or a simple fraction. (incorporates laws of definite proportions and multiple proportions)
a. Law of definite proportions: different samples of the same compound always contain its constituent elements in the same proportions by mass.
b. Law of multiple proportions: If two elements can combine to form more than one compound, the masses of one element that combine with a fixed mass of the other element are in ratios of small whole numbers (use CO and CO2 as an example: 12 to 16 versus 12 to 32.)
c. Law of conservation of mass: matter can be neither created nor destroyed
3. A chemical reaction involves only the separation, combination, or rearrangement of atoms; it does not result in their creation or destruction. |
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| the basic unit of an element that can enter into chemical combinations |
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| Atoms composed of ____, _______, and _______. |
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| charge and mass of electrons |
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negatively charged
mass= 9.1096 x 10^-31 kg |
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| charge and mass of protons |
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positively charged
mass= 1.6727 x 10^-27 kg |
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| charge and mass of neutrons |
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neutral
mass= 1.6750 x 10^-27 kg |
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| 3 kinds of particles and/or radiation emitted by radioactive substances |
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alpha particles (helium nuclei)
beta (ß) particles (electrons)
gamma rays |
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Z
number of protons in nucleus= number of electrons in a neutral atom |
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A
sum of protons plus number of neutrons in nucleus |
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| a form of matter in which all of the atoms have the same atomic number |
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when two atoms have the same number of protons but a different number of neutrons
Therefore, two atoms of the same element can have different mass numbers |
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| an aggregated of at least two atoms in a definite arrangement held together by chemical forces (bonds) |
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H, N, O, F, Cl, Br, I
H2, N2, O2, F2, Cl2,Br2, I2 diatomic |
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| charged species formed from a neutral atom or molecule when electrons are gained or lost as a result of a chemical change |
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| express the composition of molecules and ionic compounds in terms of chemical symbols |
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shows the exact number of atoms of each element in the smallest unit of a substance
EX: Methane = CH4 |
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one of two or more forms of an element
Ex: oxygen, O2 and ozone, O3 |
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tells which atoms are present and the simplest whole number ratio of the atoms (determined by experiment)
glucose contains C, H, O in 1:2:1 ratio
therefore the empirical formula is CH2O |
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| discrete molecules are not present; ionic compounds are represented by their empirical formulas |
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1. ionic
2. molecular (covalent)
3. acids
4. bases, hydrates |
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| a substance that yields hydrogen ions (H+) when dissolved in water |
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| acids that contain hydrogen, oxygen, and another element |
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| a substance that gives hydroxide anions (OH-) when dissolved in water |
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compounds that have a specific number of water molecules attached
EX: BaCl2•2 H2O barium chloride dihydrate
Sr(NO3)2•4 H2O strontium nitrate tetrahydrate |
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hydrocarbons composed of what?
Alkanes |
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composed of carbon and hydrogen
CnH(2n+2)
CH4= methane
C2H6=ethane
C3H8=propane
C4H10=butane
C5H12=pentane
C6H14=hexane
C7H16=heptane
C8H18=octane
C9H20=nontane
C10H22=decane |
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| hydrogen carbonate or bicarbonate |
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