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Study Resources (Chemistry)

10.2   Bimodal Questions 1) The diatomic molecule N2 is held together by a ________ covalent bond. A) double B) single C) ionized D) triple E) polar 2) The diatomic molecule Cl2 is held together by a ________ covalent bond. A) single B) double C) ionized D) polar E) triple 3) The shape of a molecule of methane, CH4, is ________. A).
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9.2   Bimodal Questions 1) Magnesium sulfate reacts with barium chloride according to the following balanced equation. How many moles of barium sulfate are formed from 0.0831 mol of magnesium sulfate? MgSO4(aq) + BaCl2(aq) → BaSO4(s) + MgCl2(aq) A) 1.00 mol B) 0.500 mol C) 0.200 mol D) 0.0831 mol E) 0.166 mol Barium chloride and sodium sulfate.
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12.2   Bimodal Questions 1) Acetic acid can be classified as a(n) ________. A) gas B) solid C) weak electrolyte D) strong electrolyte E) ionic compound 2) The molarity of a solution of 5.00 g of KCl in 150. mL of solution is ________. A) 0.0382 M B) 0.0667 M C) 0.447 M D) 0.132 M E) 33.3 M 3) How many.
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11) The most electronegative element is fluorine. 12) The oxygen-hydrogen bond is a polar covalent bond. 13) Water molecules are attracted to each other by hydrogen bonds. 14) The strongest forces between CH4 molecules are hydrogen bonds. 15) Fats are the building blocks of proteins. 16) The shape of a.
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8.3   True/False Questions 1) A chemical reaction has the reactants on the left and products on the right separated by a reaction arrow. 2) When methane, CH4, reacts with oxygen, one product is nitrogen gas. 3) When C2H4 reacts with oxygen, one product is water. 4) When nitrogen reacts with hydrogen.
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11) Hydrogenation is used to convert alkenes and alkynes to alkanes. 12) The functional group of amines is ?OH. 13) An alkyne has a carbon-carbon double bond. 14) Carbohydrates contain hydroxyl and aldehyde or ketone functional groups. 15) Lipids are soluble in water. 16) Proteins are biologically active polymers of.
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31) The difference in electronegativity between hydrogen and sulfur is 0.4. What type of bond is found in the molecule H2S? A) polyatomic B) ionic C) nonpolar covalent D) polar covalent E) double covalent 32) The difference in electronegativity between potassium and oxygen is 2.7. What type of bond is expected in the compound K2O?.
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11.3   Matching Questions Indicate the effect of each change upon the pressure of a gas. A) decreases B) no change C) increases 1) decrease in volume (n, T constant) 2) The temperature is doubled. 3) The volume and the Kelvin temperature are reduced by one-half. 4) A leak occurs and gas escapes. 5) increase in volume, increase in temperature 6).
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10.1   Multiple Choice Questions 1) Double and triple bonds form because A) the atoms involved have high electronegativities. B) single covalent bonds do not give all of the atoms in the molecule eight valence electrons. C) one of the atoms in the molecule has more than 8 valence electrons. D) the ions involved have.
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10.3   Matching Questions Indicate the type of bonding you would expect between the following elements. A) polar covalent B) ionic C) none D) nonpolar covalent 1) Na and F 2) N and F 3) F and F 4) He and F 5) H and F Match the molecule to its shape. A) trigonal planar B) linear C) sulfur oxide D) tetrahedral E) bent F) trigonal pyramidal 6).
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11) In the reaction of nitrogen and hydrogen to give ammonia, all the reactants and products are ________.  A) gases B) liquids C) solids D) boiling E) frozen 12) A chemical reaction has reached equilibrium when A) the concentrations of reactants and products are equal. B) all reactants have been converted to products. C) all products have.
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Identify each of the following molecules as polar or nonpolar. 8) carbon tetrachloride 9) water 10) carbon dioxide 11) hydrogen sulfide 12) hydrogen fluoride 13) A bond in which the electrons are shared between atoms is a ________ bond. 14) The strongest attractive forces between N2 molecules are ________. 15) The strongest attractive forces between.
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13.1   Multiple Choice Questions 1) A catalyst is A) a reactant in a chemical reaction. B) a product in a chemical reaction. C) a substance that speeds up a reaction without being consumed in the reaction. D) a substance that increases the energy of the products. E) a substance that decreases the energy of the.
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12.1   Multiple Choice Questions 1) The O-H bond in water is polar because A) it is an ionic bond. B) oxygen is much more electronegative than hydrogen. C) oxygen occupies more space than hydrogen. D) hydrogen is much more electronegative than oxygen. E) it is a hydrogen bond. 2) A hydrogen bond is A) an attraction.
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9.4   Short Answer Questions 1) Acetylene gas, C2H2, reacts with oxygen according to the following equation. If 5.00 mol of acetylene react completely with sufficient oxygen, how many mol of carbon dioxide are produced? 2 C2H2(g) + 5 O2 (g) → 4CO2(g) + 2H2O(g) acetylene 2) Acetylene gas, C2H2, reacts with oxygen according.
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21) Which of the following elements has the lowest electronegativity? A) Li B) C C) N D) O E) F 22) Which of the following compounds contains a polar covalent bond? A) NaF B) HCl C) Br2 D) MgO E) O2 23) Which of the following compounds contains an ionic bond? A) NH3 B) H2O C) CaO D) H2 E) CH4 24) If the electronegativity.
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10.4   True/False Questions 1) Oxygen, O2, is held together by a triple ionic bond. 2) N2 is held together by a multiple covalent bond. 3) The total number of valence electrons in the fluorine molecule, F2, is 14. 4) The carbon dioxide molecule contains a triple covalent bond. 5) Carbon dioxide.
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11.4   True/False Questions 1) The kinetic energy of a gas sample is directly proportional to the Kelvin temperature of the gas. 2) The air we breathe is about 21% oxygen. 3) Gas law calculations normally require the use of the Kelvin temperature scale. 4) Carbon dioxide and water vapor together account.
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11.2   Bimodal Questions 1) A barometer is a device for measuring ________. A) atmospheric pressure B) blood pressure C) gas pressure in a container D) gas pressure in the lung E) vapor pressure 2) A kiloPascal is a unit of ________. A) pressure B) temperature C) energy D) mass E) volume 3) A container of variable volume contains oxygen gas at.
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11.5   Short Answer Questions 1) Nitrogen makes up about ________ percent of the atmosphere. 2) A barometer is usually filled with ________. 3) One atmosphere is the same as ________ mmHg. 4) The pressure unit 1 mmHg is the same as the pressure unit ________. 5) At 125 °C, the pressure.
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11) Which of the following statements is NOT true about water? A) Water molecules are attracted to each other by hydrogen bonds. B) Gasoline is insoluble in water. C) Water molecules are covalently bonded. D) Water dissolves polar substances well. E) The water molecule is linear. 12) A solution containing a large concentration of dissolved.
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12.4   True/False Questions 1) A dental amalgam is an example of a solid solution. 2) Carbon tetrachloride, CCl4, is soluble in water. 3) Sodium acetate is a weak electrolyte. 4) Hydrochloric acid is a strong electrolyte. 5) Glucose is a nonelectrolyte. 6) A solution of a nonelectrolyte contains only ions. 7).
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11.1   Multiple Choice Questions 1) Which of the following is NOT part of the kinetic molecular theory of gases? A) A gas is composed of very small particles. B) There is very little empty space in a gas. C) Gas particles move rapidly. D) Gas particles do not attract or repel one another. E) Gas.
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41) The building blocks of proteins are  A) fatty acids. B) carbohydrates. C) amino acids. D) steroids. E) not known. 42) Proteins are A) chains of amino acids. B) important biological molecules. C) transport molecules in the body. D) part of the structural components in the body. E) all of the above 43) When a solid is converted directly to.
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12.3   Matching Questions Identify the term defined in each description. A) ionic equation B) hydrogen bonding C) nonelectrolyte D) net ionic equation E) dissociation F) solute G) solution H) solvent I) unsaturated J) saturated K) weak electrolyte L) strong electrolyte 1) a solution that contains the highest amount of solute that dissolves at a given temperature 2) the major attraction between water molecules 3).
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9.1   Multiple Choice Questions 1) Which of the following correctly illustrates the conservation of mass for the reaction below? 4Na(s) + O2(g) → 2Na2O(s) A) 23.0 g Na, 16.0 g O2, 39.0 g Na2O B) 92.0 g Na, 16.0 g O2, 108 g Na2O C) 92.0 g Na, 32.0 g O2, 124 g Na2O D).
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11) Magnesium sulfate reacts with barium chloride according to the following balanced equation. If 1.20 g of magnesium sulfate is allowed to react with 10.0 g of barium chloride in a water solution, what is the theoretical yield of barium sulfate? MgSO4(aq) + BaCl2(aq) → BaSO4(s) + MgCl2(aq) A) 1.20 g B).
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8.4   Short Answer Questions 1) Write the balanced equation for the reaction of copper(II) chloride with sodium hydroxide to produce copper(II) hydroxide and sodium chloride. 2) Write the balanced equation for the reaction of sodium hydroxide with sulfuric acid to give water and sodium sulfate. 3) Write the balanced equation for.
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