Chem 105; Ch. 5 – Flashcards
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What is the naming of compounds called?
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Binomial Nomenclature
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When do we use the Greek Prefix system to name compounds?
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1. Compound must be binary (can contain only 2 elements) 2. Elements must be nonmetals
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What are the first 10 prefixes of the Greek prefix system?
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1.mono 2. di 3. tri 4. tetra 5. penta 6. hexa 7. hepta 8. octa 9. nana 10. deca
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When must a prefix always be used?
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for the second element
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What must the sum of the oxidation of the elements equal?
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zero
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What comes first in an acid?
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Hydrogen
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What do all bases have at least one of?
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OH group
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The last word in the naming of all bases is _____.
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hydroxide
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Classify each compound as ionic or molecular. A. CO2 B. NiCl2 C. NaI D. PCl3
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A. molecular B. ionic C. ionic D. molecular
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Determine the emperical formula for the compound represented my each molecular formula A. N2O4 B. C5H12 C. C4H10
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A. NO2 B. C5H12 C. C2H5
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Determine the number of each type of atom in each formula. A. Mg3(PO4)2 B. BaCl2 C. Fe(NO2)2 D. Ca(OH)2
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A. 3 Mg; 2 P; 8 O B. 1 Ba; 2 Cl C. 1 Fe; 2 N; 4 O D. 1 Ca; 2 O; 2 H
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Name each ionic compound. A. Mg3N2 B. KF C. Na2O D. Li2S E. CsF F. KI
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A. Magnesium Nitride B. Potassium Fluoride C. Sodium Oxide D. Lithium Sulfide E. Cesium Fluoride F. Potassium Iodide
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Name each ionic compound. A. SnO B. Cr2S3 C. RbI D. BaBr2
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A. Tin (II) Oxide B. Chromium (III) sulfide C. Rubidium Iodide D. Barium Bromide
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Name each ionic compound containing a polyatomic ion. A. cuno2 B. Mg(C2H3O2)2 C. Ba(NO3)2 D. Pb(C2H3O2)2
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A. Copper (I) Nitrite B. Magnesium Acetate C. Barium Nitrate D. Lead (II) Acetate
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Write the formula for each ionic compound. A. sodium hydrogen sulfite B. lithium permanganate C. silver nitrate D. potassium sulfate E. rubidium hydrogen sulfate F. potassium hydrogen carbonate
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A. NaHSO3 B. limno4 C. AgNO3 D. K2SO4 E. RbHSO4 F. KHCO3
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Write the name from the formula or the formula from the name for each hydrated ionic compound. A. CoSO4 * 7H2O B. Iridium (III) bromide tetrahydrate C. Mg(BrO3)2 * 6H2O D. Potassium carbonate dihydrate
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A. Cobalt (II) Sulfate Heptahydrate B. IrBr3 * 4H2O C. Magnesium Bromate Hexahydrate D. K2CO3 * 2H2O
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Name each molecular compound. A. CO B. NI3 C. SiCl4 D. N4Se4
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A. Carbon monoxide B. Nitrogen triiodide C. Silicon tetrachloride D. Tetranitrogen tetraselenide
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Write a formula for each molecular compound. A. phosphorus trichloride B. chlorine monoxide C. disulfur tetrafluoride D. phosphorus pentafluoride
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A. PCl3 B. Cl2O C. S2F4 D. PF5
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Name each compound. A. SrCl2 B. SnO2 C. P2S5
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A. Strontium Chloride B. Tin (IV) Oxide C. Diphosphorus pentasulfide
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Name each compound. A. KClO3 B. I2O5 C. PbSO4
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A. Potassium Chlorate B. Diiodine pentaoxide C. Lead (II) Sulfate
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Calculate the formula mass for each compound. A. NO2 B. C4H10 C. c6h12o6 D. Cr(NO3)3
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A. 46.01 amu B. 58.12 amu C. 180.16 amu D. 238.03 amu
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Calculate the mass (in g) of each sample. A. 5.94E20 SO3 B. 2.8E22 H2O C. C6H12O6
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A. .o790 g B. .84 g C. 2.992E-22 g
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Calculate the mass percent composition of carbon in each carbon-containing compound. A. CH4 B. C2H6 C. C2H2 D. C2H5Cl
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A. 74.9% C B. 79.9% C C. 92.3% C D. 37.2% C
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Determine the number of moles of hydrogen atoms contained in each sample. A. 0.0885 mol C4H10 B. 1.3 mol CH4 C. 2.4 mol C6H12 D. 1.87 mol C8H18
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A. 0.885 mol H B. 5.2 mol H C. 28.8 mol H D. 33.7 mol H
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A chemist decomposes samples of several compounds; the masses of their constituent elements are shown below. Calculate the empirical formula for each compound. A. 1.651g Ag, .1224g O B. .672g Co, .569g As, .486g O C. 1.443g Se, 5.841g Br
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A. Ag2O B. Co3As2O8 C. SeBr4
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The elemental mass percent composition of ibuprofen is 75.69% C, 8.80% H, and 15.51% O. Determine the imperical formula for ibuprofen.
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C13H18O2
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The empirical formula and molar mass of several compounds are listed below. Find the molecular formula of each compound. A. c6h7N, 186.24 g/mol B. C2HCl, 181.44 g/mol C. C5H10NS2, 296.54 g/mol
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A. C12H14N2 B. C6H3Cl3 C. C10H20N2S4
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Classify each compound as organic or inorganic. A. CaCO3 B.C4H8 C. c4h6o6 D. LiF
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A. inorganic B. organic C. organic D. inorganic
