Chemistry Final Study Guide

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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


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