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Nomenclature Chemical Formulas Reactions. Which is an example of a synthesis reaction?. A. HCl + KOH  KCl + H 2 O B. Pb(NO 3 ) 2 + 2HBr  PbBr 2 + 2HNO 3 C. C + O 2  CO 2 D. Mg + H 2 SO 4  MgSO 4 + H 2.

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Nomenclature Chemical Formulas Reactions


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    1. NomenclatureChemical FormulasReactions

    2. Which is an example of a synthesis reaction? A. HCl + KOH  KCl + H2O B. Pb(NO3)2 + 2HBr  PbBr2 + 2HNO3 C. C + O2 CO2 D. Mg + H2SO4 MgSO4 + H2

    3. The coefficients of the correctly balanced equation for the reaction illustrated are — A. 1, 1, 1 B. 1, 1, 2 C. 2, 1, 2 D. 2, 2, 1

    4. Which of the following equations is balanced?

    5. What would be the product(s) of this reaction? A. 2Mg3Al2O2 B. Mg3Al2 + 3O2 C. 6Mg + Al3O2 D. 3Mg + Al2O3

    6. Elements from which two groups in the periodic table would most likely combine with each other to form an ionic compound? A. 1 and 2 B. 16 and 17 C. 1 and 17 D. 17 and 18

    7. The diagram is a potential energy curve for a reaction. Which number represents the effect of a catalyst on the reaction? A. 1 B. 2 C. 3 D. 4

    8. Which is the correct formula for iron (III) sulfate? A. Fe3(SO4)2 B. FeSO4 C. Fe2(SO4)3 D. Fe2(SO3)3 Remember the Roman Numeral is the charge of the Iron *Fe’s oxidation number

    9. Which of these represents the empirical formula and the molecular formula, respectively, for a given organic compound? A. CH and C2H2 B. CH and CH4 C. CH2 and C2H2 D. CH3 and C3H12 Empirical formula is the simplest whole number ratio Molecular formula is a multiple of the Empirical formula

    10. The system that shows a decrease in entropy (disorder) is — • air escaping from a tire • snow melting • salt dissolving in water • water freezing

    11. In chemical compounds, covalent bonds form when — A. the electronegativity difference between two atoms is very large B. electrons are completely transferred between two metals C. pairs of electrons are shared between two nonmetal atoms D. two nonmetal ions are attracted to each other by opposite charges

    12. Each beaker shown above contains 2.2 grams of iron and 1 liter of 3M H2SO4 at STP. Which reaction will go to completion first and why? A. Beaker A because of increased surface area B. Beaker B because of increased surface area C. Beaker A because of a higher concentration level D. Beaker B because of a higher concentration level

    13. A catalyst is a substance used in chemical reactions to — A. provide a higher activation energy pathway B. decrease collisions between reactant molecules C. increase the rate of the reaction D. change the equilibrium to favor products

    14. Which reaction type best describes the reaction above? A. Combination B. Decomposition C. Single replacement D. Combustion

    15. ? AgNO3 + ?AlCl3 → ?AgCl + ?Al(NO3)3 Which of these sets of coefficients will balance this equation? A. 3, 3, 2, 1 B. 3, 1, 3, 1 C. 1, 6, 1, 9 D. 9, 3, 3, 3

    16. The formula for lithium nitride is — A. LiN B. Li3N C. Li3N3 D. NLi3

    17. This diagram of a chemical reaction shows that the reaction is — A. endothermic B. exothermic C. reversible D. at equilibrium

    18. Ni(C2H3O2)4How many atoms are represented in this formula? A. 5 B. 8 C. 28 D. 29

    19. The correct structural formula for C2H4 is

    20. What type of reaction does this illustration represent? A. Decomposition B. Synthesis C. Single-replacement D. Double-replacement

    21. Which of these reactions shows simple chemical decomposition?

    22. A compound has 50% sulfur and 50% oxygen. What is its empirical formula? • SO4 • S2O4 • SO3 • SO2

    23. A compound has 50% sulfur and 50% oxygen. What is its empirical formula?

    24. A compound has 50% sulfur and 50% oxygen. What is its empirical formula? • SO4 • S2O4 • SO3 • SO2

    25. The Lewis electron dot system represents electrons in the — A. outer energy level B. inner level C. middle level D. core level X

    26. A(s) + B(s)  D(g) + heatThe reaction shown above is — A. an endothermic reaction B. an exothermic reaction C. a decomposition reaction D. a double-replacement reaction

    27. The correct name for MgI2 is — A. magnesium iodide B. magnesium iodite C. magnesium (II) iodide D. magnesium diiodide

    28. If the diagram were the correct representation for the Lewis structure of a molecule, then the X would be representative of the element — A. oxygen B. fluorine C. nitrogen D. sulfur

    29. Chlorine and bromine are in the same family in the periodic table. According to the information in the table, what would be the correct formula for sodium bromate? A. NaBrO B. Na2BrO C. Na3BrO3 D. NaBrO3

    30. Which of the groups below has the electron dot structure shown above? A . Noble gases B. Halogens C. Alkali metals D. Transition elements

    31. When naming a transition metal that has more than one oxidation number, the numeric value of the oxidation number is indicated by a — A. Roman numeral B. Greek prefix C. subscript D. suffix

    32. A compound is composed of 85.64% carbon and 14.36% hydrogen. The compound has a formula mass of 42.08 grams. What is the molecular formula? A. CH2 B. C3H6 C. C2H4 D. C2H18

    33. Which of the following is the correct molecular shape of CH4? A. Bent B. Linear C. Pyramidal D. Tetrahedral

    34. According to the table, which of these probably has the strongest bonds? A. Hydrogen gas B. Iron crystals C. Sodium chloride D. Water

    35. The empirical formula for ethyne (C2H2) is — A. CH B. C2H2 C. CH2 D. C2H

    36. The type of reaction represented by the above equation is — A. single-replacement B. double-replacement C. synthesis D. decomposition

    37. When this equation is correctly balanced, the coefficient of the AlCl3 will be — A. 1 B. 2 C. 4 D. 6

    38. A catalyst accelerates a chemical reaction because the — A. catalyst decreases the number of collisions in a reaction B. activation energy of the reaction is lowered in the presence of a catalyst C. catalyst decreases the concentration of the reactants D. temperature of the reaction increases due to the catalyst

    39. A compound is composed of 58.8% C, 9.8% H, and 31.4% O, and the molar mass is 102 g/mol. What is the molecular formula for this compound? A. C2H10O 3 B. C5H5O3 C. C5H10O2 D. CH3O3

    40. Which of these completes this reaction? A. Oxygen B. Hydrogen C. Metal oxide D. Air

    41. A balanced chemical equation has equal numbers of atoms of each type on both sides of the equation. This illustrates the principle of — A. conservation of energy B. conservation of mass C. action and reaction D. natural selection

    42. The type of bond found in magnesium chloride is — A. covalent B. nonpolar C. ionic D. metallic

    43. If the temperature of a reaction is increased, the reaction proceeds at a much quicker rate because the — A. activation energy increases B. energy of the products increases C. frequency of collisions between reactants increases D. energy of the activated complex increases

    44. In the above reaction, a cloudiness at completion due to colloidal suspension of sulfur appears. If the reaction is carried out at various temperatures, at which temperature would it proceed at the fastest rate? A. 20º C B. 30º C C. 40º C D. 50º C

    45. The formula H2SO4 is representative of which of the following? A. A catalyst B. A base C. An acid D. An organic compound

    46. A heated liquid placed in a closed container will vaporize until — A. the boundary between liquid and vapor disappears B. all the liquid molecules become vapor molecules C. the number of liquid molecules vaporizing equals the number of vapor molecules condensing D. the vapor pressure is greater than the atmospheric pressure

    47. Which compound contains both ionic and covalent bonds? A. NH4Cl B. MgBr2 C. CH4 D. NH3

    48. Which of the following containers of water best shows dynamic equilibrium between vapor and liquid?

    49. To indicate the number of atoms of each element present in a molecular compound, scientists use — A. Roman numerals B. superscripts C. prefixes D. subscripts

    50. Using the chart, which of these combinations will probably form a precipitate? A. Ammonium chloride B. Barium bromide C. Calcium chromate D. Copper (II) carbonate