Chapter 2 from Chem 1303 – Flashcards
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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 (?) particles (electrons) gamma rays |
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Atomic number |
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Z number of protons in nucleus= number of electrons in a neutral atom |
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mass number |
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A sum of protons plus number of neutrons in nucleus |
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Element |
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a form of matter in which all of the atoms have the same atomic number |
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isotopes |
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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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Special names 1A |
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alkali metal |
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Special names 2A |
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alkaline earth metals |
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special names 7A |
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halogens |
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special names 8A |
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noble gases |
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Molecule |
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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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7 diatomic elements |
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H, N, O, F, Cl, Br, I H2, N2, O2, F2, Cl2,Br2, I2 diatomic |
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Ion |
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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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cations |
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positive |
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anions |
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negative |
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Chemical Formulas |
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express the composition of molecules and ionic compounds in terms of chemical symbols |
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Molecular formula |
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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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Allotrope |
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one of two or more forms of an element Ex: oxygen, O2 and ozone, O3 |
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Empirical formula |
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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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ionic compounds |
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discrete molecules are not present; ionic compounds are represented by their empirical formulas |
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Four types of compounds |
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1. ionic 2. molecular (covalent) 3. acids 4. bases, hydrates |
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mono- |
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1 |
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di- |
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2 |
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tri- |
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3 |
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tetra- |
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4 |
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penta- |
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5 |
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hexa- |
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6 |
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hepta- |
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7 |
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octa- |
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8 |
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nona- |
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9 |
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deca- |
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10 |
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acid |
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a substance that yields hydrogen ions (H+) when dissolved in water |
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oxoacids |
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acids that contain hydrogen, oxygen, and another element |
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base |
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a substance that gives hydroxide anions (OH-) when dissolved in water |
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hydrates |
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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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NH4+ |
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ammonium |
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H3O+ |
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hydronium |
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Hg2 2+ |
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mercury I |
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CN- |
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cyanide |
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OCN- |
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cyanate |
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SCN- |
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thiocyanate |
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OH- |
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hydroxide |
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C2H3O2- |
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acetate |
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MnO4- |
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permanganate |
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NO3- |
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nitrate |
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NO2- |
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nitrite |
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H2PO4- |
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dihydrogen phosphate |
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HCO3- |
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hydrogen carbonate or bicarbonate |
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HSO4- |
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hydrogen sulfate |
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HSO3- |
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hydrogen sulfite |
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ClO4- |
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perchlorate |
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ClO3- |
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chlorate |
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ClO2- |
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chlorite |
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ClO- |
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hypochlorite |
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O2 2- |
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peroxide |
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C2O4 2- |
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oxalate |
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CrO4 2- |
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chromate |
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Cr2O7 2- |
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dichromate |
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HPO4 2- |
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hydrogen phosphate |
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CO3 2- |
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carbonate |
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SO4 2- |
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Sulfate |
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SO3 2- |
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sulfite |
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S2O3 2- |
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thiosulfate |
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PO4 3- |
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phosphate |
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AsO4 3- |
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aresenate |
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