Chemistry Final Study Guide
What are the rules for naming acids?
-ide -> -ic acid -ite -> -ous acid -ate -> -ic acid
Decomposition Reaction
a chemical change in which a single compound is broken down into two or more simpler products
Combustion Reaction
a chemical change in which an element or a compound reacts with oxygen, often producing energy in the form of heat and light
Single Replacement Reaction
a chemical change in which one element replaces a second element in a compound; also called displacement reaction
Synthesis Reaction
a chemical change in which two or more substances react to form a single new substance; also called a combination reaction
Double Replacement Reaction
a chemical change that involves an exchange of positive ions between two compounds
Molecular Formula
a chemical formula of a molecular compound that shows the kinds and numbers of atoms present in a molecule of a compound
Electrolyte
a compound that conducts an electric current when it is in an aqueous solution or in the molten state; all ionic compounds are electrolytes, but most covalent compounds are not
Empirical Formula
a formula with the lowest whole-number ratio of elements in a compound; the empirical formula of hydrogen peroxide (H2O2) is HO
Solution
a homogenous mixture; consists of solutes dissolved in solvent
Bronsted-Lowry Base
a hydrogen ion acceptor
Bronsted-Lowry Acid
a hydrogen-ion donor
Endothermic Reactions
a process that absorbs heat from the surroundings
Exothermic Reactions
a process that releases heat to its surroundings
Precipitate
a solid that forms and settles out of a liquid mixture
Saturated Solution
a solution containing the maximum amount of solute for a given amount of solvent at a constant temperature and pressure; an equilibrium exists between undissolved solute and ions in a solution
Unsaturated Solution
a solution that contains less solute than a saturated solution at a given temperature and pressure
Supersaturated Solution
a solution that contains more solute than it an theoretically hold at a given temperature; excess solute precipitates if a seed crystal is added
62. Find the mass of each substance. a. 1.50 mol C5H12 b. 14.4 mol F2 c. 0.780 mol Ca(CN)2 d. 7.00 mol H2O2 e. 5.60 mol NaOH f. 3.21x10^-2 mol Ni
a. 1.50 mol C5H12 -> 108 g b. 14.4 mol F2 -> 547 g c. 0.780 mol Ca(CN)2 -> 72 g d. 7.00 mol H2O2 -> 238 g e. 5.60 mol NaOH -> 224 g f. 3.21x10^-2 mol Ni -> 1.89 g
37. Balance the following equations: a. PbO2(s) -> PbO(s) + O2(g) b. Fe(OH)3(s) -> Fe2O3(s) + H2O (s) c.(NH4)2CO3(s) -> NH3(g) + H2O(g) + CO2(g) d. CaCl2(aq) + H2SO4(aq) -> CaSO4(s) + HCl(aq)
a. 2PbO2(s) -> 2PbO(s) + O2(g) b. 2Fe(OH)3(s) -> Fe2O3(s) + 3H2O (s) c.(NH4)2CO3(s) -> 2NH3(g) + H2O(g) + CO2(g) d. CaCl2(aq) + H2SO4(aq) -> CaSO4(s) + 2HCl(aq)
43. Balance each equation and identify its type. a. Hf(s) + N2(g) -> Hf3N4(s) b. Mg(s) + H2SO4(aq) -> MgSO4(aq) + H2(g) c. C2H6(g) + O2(g) -> CO2(g) + H2O(g) d. Pb(NO3)2(aq) + NaI(aq) -> PbI2(s) + NaNO3(aq)
a. 3Hf(s) + 2N2(g) -> Hf3N4(s); synthesis b. Mg(s) + H2SO4(aq) -> MgSO4(aq) + H2(g); single replacement c. 2C2H6(g) + 7O2(g) -> 4CO2(g) + 6H2O(g); combustion d. Pb(NO3)2(aq) + 2NaI(aq) -> PbI2(s) + 2NaNO3(aq); double replacement
40. Use the activity series of metals to write a balanced chemical equation for each single-replacement reaction. a. Au(s) + KNO3(aq) -> b. Zn(s) + AgNO3(aq) -> c. Al(s) + H2SO4(aq) ->
a. Au(s) + KNO3(aq) -> no reaction b. Zn(s) + 2AgNO3(aq) -> Zn(NO3)2(aq) + 2Ag c. 2Al(s) + 3H2SO4(aq) -> Al2(SO4)3 + 3H2(g)
78. Which pair of molecules has the same empirical formula? a. C2H4O2, C6H12O6 b. NaCrO4, Na2Cr2O7
a. C2H4O2, C6H12O6
79. What is the molecular formula for each compound? Each compound's empirical formula and molar mass are given. a. CH2O, 90 g/mol b. HgCl, 472.2 g/mol
a. CH2O, 90 g/mol -> C3H6O3 b. HgCl, 472.2 g/mol -> HgCl2
57. Give the expected charges on the ions of elements of these groups of the periodic table. a. Group 6A b. Group 1A c. Group 7A d. Group 3A
a. Group 6A -> -2 b. Group 1A -> +1 c. Group 7A -> -1 d. Group 3A -> +3
73. Give the name or the formula for these acids. a. HCl b. HNO3 c. sulfuric acid d. acetic acid
a. HCl -> hydrochloric acid b. HNO3 -> nitric acid c. sulfuric acid -> H2SO4 d. acetic acid -> HC2H3O2
83. Name each substance. a. LiClO4 b. Cl2O c. HgF2 d. CaO e. Ba3(PO4)2 f. I2 g. SrSO4 h. CuC2H3O2 i. SiCl4
a. LiClO4 -> lithium perchlorate b. Cl2O -> dichlorine monoxide c. HgF2 -> mercury(II) fluoride d. CaO -> calcium oxide e. Ba3(PO4)2 -> barium phosphate f. I2 -> iodine g. SrSO4 -> strontium sulfate h. CuC2H3O2 -> copper(I) acetate i. SiCl4 -> silicon tetrachloride
84. Name each compound a. Mg(MnO4)2 b. Be(NO3)2 c. K2CO3 d. N2H4 e. LiOH f. BaF2 g. PI3 h. ZnO i. H3PO3
a. Mg(MnO4)2 -> magnesium permanganate b. Be(NO3)2 -> beryllium nitrate c. K2CO3 -> potassium carbonate d. N2H4 -> dinitrogen tetrahydride e. LiOH -> lithium hydroxide f. BaF2 -> barium fluoride g. PI3 -> phosphorous triiodide h. ZnO -> zinc oxide i. H3PO3 -> phosphorous acid
82. Name these compounds. a. NaClO3 b. Hg2Br2 c. K2CrO4 d. HClO4 e. SnO2 f. Fe(C2H3O2)3 g. KHSO4 h. Ca(OH)2 i. BaS
a. NaClO3 -> sodium chlorate b. Hg2Br2 -> mercury (I) bromide c. K2CrO4 -> potassium chromate d. HClO4 -> perchloric acid e. SnO2 -> tin (IV) oxide f. Fe(C2H3O2)3 -> iron(III) acetate g. KHSO4 -> potassium hydrogen sulfate h. Ca(OH)2 -> calcium hydroxide i. BaS -> barium sulfide
72. Write the formula or name for the following compounds: a. P2O5 b. CCl4 c. boron trichloride d. dinitrogen tetrahydride
a. P2O5 -> diphosphourours pentoxide b. CCl4 -> carbon tetrachloride c. boron trichloride -> BCl3 d. dinitrogen tetrahydride -> N2H4
76. Write the names or formulas for these compounds. a. Pb(OH)2 b. Co(OH)2 c. copper(II) hydroxide d. iron(III0 hydroxide
a. Pb(OH)2 -> lead(II) hydroxide b. Co(OH)2 -> cobalt(II) hydroxide c. copper(II) hydroxide -> Cu(OH)2 d. iron(III) hydroxide -> Fe(OH)2
85. Write formulas for these compounds. a. calcium bromide b. silver chloride c. aluminum carbide d. nitrogen dioxide e. tin(IV) cyanide f. lithium hydride g. strontium acetate h. sodium silicate
a. calcium bromide -> CaBr2 b. silver chloride -> AgCl c. aluminum carbide -> Al4C3 d. nitrogen dioxide -> NO2 e. tin(IV) cyanide -> Sn(CN)4 f. lithium hydride -> LiH g. strontium acetate -> Sr(C2H3O2)2 h. sodium silicate -> Na2SiO3
75. Write the formulas of these compounds. a. nitrous acid b. aluminum hydroxide c. hydroselenic acid d. strontium hydroxide e. phosphoric acid
a. nitrous acid -> HNO2 b. aluminum hydroxide -> Al(OH)3 c. hydroselenic acid -> H2Se d. strontium hydroxide -> Sr(OH)2 e. phosphoric acid -> H3PO4
61. Calculate the mass of 1.00 mol of each of these substances. a. silicon dioxide (SiO2) b. diatomic nitrogen (N2) c. iron(III) hydroxide (Fe(OH)3) d. copper (Cu)
a. silicon dioxide (SiO2) -> 60g/mol b. diatomic nitrogen (N2) -> 28g/mol c. iron(III) hydroxide (Fe(OH)3) -> 107g/mol d. copper (Cu) -> 64g/mol
What are the pH values for acids/bases?
acids < 7 bases > 7
What conditions increase the rate for dissolving a solute in a solvent?
agitation, increased temperature, or decreased particle size
76. What is an empirical formula? Which of the following molecular formulas are also empirical formulas? a. ribose (C5H10O5) b. ethyl butyrate (C6H12O2) c. chlorophyll (C55H72MgN4O5) d. DEET (C12H17ON)
an empirical formula is a formula with the lowest whole-number ratio of elements in a compound. c. chlorophyll (C55H72MgN4O5) d. DEET (C12H17ON)
Limiting Reactant
any reactant that is used up first in a chemical reaction; it determines the amount of product that can be formed in the reaction
Henry's Law
at a given temperature the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid
Dalton's Law of Partial Pressures
at constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases
75. Which of the following compounds has the highest percent of iron by mass? a. FeCl2 b. Fe(C2H3O2)3 c. Fe(OH)2 d. FeO
d. FeO with 78%
Immiscible
describes liquids that are insoluble in one another; water and oil are immiscible
Miscible
describes liquids that dissolve in one another in all proportions
Solute
dissolved particles in a solution
What is the difference between a strong and weak electrolyte?
electrolytes which ionize almost completely in solutions are know as strong electrolytes while electrolytes which ionize only to a small extent in solutions are known as weak electrolytes
Boyle's Law
for a given mass of gas at constant temperature, the volume of the gas varies inversely with pressure
Under what conditions are gases most soluble?
high pressure and low temperature
What increases the pressure of a gas?
increased temperature, decreased volume, or increased amount of particles
What are the rules for naming ionic compounds?
it follows the same naming rules as the simple binary compounds but with an extra rule added in, so you still name the cation first, followed by the anion with the suffix -ide added to the end of it
Like Dissolves Like Rule
polar molecules with dissolve with other polar molecules while non-polar molecules will dissolve with other non-polar molecules
What are the properties of bases?
taste bitter, pH greater than 7, turn red litmus blue, neutralize bases producing a salt and water, proton acceptors, electrolytes, slippery
What are the properties of acids?
taste sour, pH less than 7, turn blue litmus red, neutralize bases producing a salt and water, proton donors, electrolytes,
Solubility
the amount of a substance that dissolves in a given quantity of solvent at specified conditions of temperature and pressure to produce a saturated solution
Molar Heat of Vaporization
the amount of heat absorbed by one mole of a liquid as it vaporizes at a constant temperature
Molar Heat of Fusion
the amount of heat absorbed by one mole of a solid substance as it melts to a liquid at constant temperature
Theoretical Yield
the amount of product that could form during a reaction calculated from a balanced chemical equation; it represents the maximum amount of product that can be formed from a given amount of reactant
Actual Yield
the amount of product that forms when a reaction is carried out in the laboratory
Pressure
the amount of times that particles collide with the edges of a container
Molarity
the concentration of solute in a solution expressed as the number of moles of solute dissolved in one liter of solution
Solvent
the dissolving medium in a solution
Combined Gas Law
the law that describes the relationship among the pressure, temperature, and volume of an enclosed gas
What are the rules for naming covalent compounds?
the prefixes used are mono-, di-, tri-, tetra-, penta-, hexa-, and so forth
Gay-Lussac's Law
the pressure of a gas is directly proportional to the Kelvin temperature if its volume in constant
Percent Yield
the ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction
Ideal Gas Law
the relationship PV=nRT, which describes the behavior of an ideal gas
Boiling Point
the temperature at which the vapor pressure of a liquid is just equal to the external pressure on the liquid
Charles' Law
the volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant
What are the properties of gases?
they are easy to compress, they expand to fill their containers, and they occupy far more space than the liquids or solids from which they form
68. When must parenthesis be used in a formula for a compound?
to identify if there are multiple polyatomic ions
Arrhenius Acid
when a hydrogen ion is lost during a chemical reaction
Arrhenius Base
when a hydroxide ion is lost during a chemical reaction
Polarity
when one end of a molecule is slightly positive and one end is slightly negative
