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Questions and Answers
The average atomic mass of the element is ________ amu.
The average atomic mass of the element is ________ amu.
220.67
________ is the abbreviation for the prefix milli-.
________ is the abbreviation for the prefix milli-.
What is the empirical formula of the compound that produced 2.265 g of CO2 and 1.236 g of H2O from a 1.031-g sample?
What is the empirical formula of the compound that produced 2.265 g of CO2 and 1.236 g of H2O from a 1.031-g sample?
What is the % yield of SO3 in the reaction of 5.0 grams of O2 with 6.0 grams of S producing 7.9 grams of SO3?
What is the % yield of SO3 in the reaction of 5.0 grams of O2 with 6.0 grams of S producing 7.9 grams of SO3?
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When the following equation is balanced, the coefficient of H2O is ________. Ca (s) + H2O (l) → Ca(OH)2 (aq) + H2 (g)
When the following equation is balanced, the coefficient of H2O is ________. Ca (s) + H2O (l) → Ca(OH)2 (aq) + H2 (g)
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What is the maximum amount in grams of SO3 that can be produced by the reaction of 1.0 g of S with 1.0 g of O2?
What is the maximum amount in grams of SO3 that can be produced by the reaction of 1.0 g of S with 1.0 g of O2?
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A solid material contains 53.66 percent of oxalic acid (H2C2O4) by mass, requiring ________ mL of 0.3483 M NaOH for neutralization.
A solid material contains 53.66 percent of oxalic acid (H2C2O4) by mass, requiring ________ mL of 0.3483 M NaOH for neutralization.
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How many oxygen atoms are there in 52.06 g of carbon dioxide?
How many oxygen atoms are there in 52.06 g of carbon dioxide?
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Which of the following are combustion reactions?
Which of the following are combustion reactions?
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The combustion of 43.9 g of ammonia produces ________ g of NO2.
The combustion of 43.9 g of ammonia produces ________ g of NO2.
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How many neutrons are there in one atom of 182W?
How many neutrons are there in one atom of 182W?
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A wooden object has a mass of 10.782 g and occupies a volume of 13.72 mL. What is the density of the object?
A wooden object has a mass of 10.782 g and occupies a volume of 13.72 mL. What is the density of the object?
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The concentration (M) of the acid titrated with NaOH was ________.
The concentration (M) of the acid titrated with NaOH was ________.
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The maximum amount of Al2O3 produced from 2.5 g of Al and 2.5 g of O2 is ________ g.
The maximum amount of Al2O3 produced from 2.5 g of Al and 2.5 g of O2 is ________ g.
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Production of 13 g of C2H2 requires ________ g of H2O.
Production of 13 g of C2H2 requires ________ g of H2O.
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Aluminum forms an ion with a charge of ________.
Aluminum forms an ion with a charge of ________.
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The concentration (M) of the acid was ________ when 51.2 mL of NaOH were used.
The concentration (M) of the acid was ________ when 51.2 mL of NaOH were used.
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What is the formula of the compound formed between strontium ions and nitrogen ions?
What is the formula of the compound formed between strontium ions and nitrogen ions?
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How many protons does the Ca2+ ion possess?
How many protons does the Ca2+ ion possess?
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An atom of 14C contains ________ protons.
An atom of 14C contains ________ protons.
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The total concentration of ions in a 0.625 M solution of HCl is ________.
The total concentration of ions in a 0.625 M solution of HCl is ________.
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Which one of the following is not one of the postulates of Dalton's atomic theory?
Which one of the following is not one of the postulates of Dalton's atomic theory?
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Which formula/name pair is incorrect? Mg3N2 ________
Which formula/name pair is incorrect? Mg3N2 ________
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The formula weight of potassium dichromate (K2Cr2O7) is ________ amu.
The formula weight of potassium dichromate (K2Cr2O7) is ________ amu.
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Elements in the same group of the periodic table typically have ________.
Elements in the same group of the periodic table typically have ________.
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The empirical formula of a compound with molecules containing 12 carbon atoms, 14 hydrogen atoms, and 6 oxygen atoms is ________.
The empirical formula of a compound with molecules containing 12 carbon atoms, 14 hydrogen atoms, and 6 oxygen atoms is ________.
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Which combination of protons, neutrons, and electrons is correct for the isotope of copper, 63Cu?
Which combination of protons, neutrons, and electrons is correct for the isotope of copper, 63Cu?
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Elements in Group 1A are known as the ________.
Elements in Group 1A are known as the ________.
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What is the molarity of chloride ion in the final solution after adding NaCl to CaCl2?
What is the molarity of chloride ion in the final solution after adding NaCl to CaCl2?
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In which reaction does the oxidation number of oxygen increase?
In which reaction does the oxidation number of oxygen increase?
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The mass % of F in the binary compound KrF2 is ________.
The mass % of F in the binary compound KrF2 is ________.
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The mass of 1.00 mol of allicin, rounded to the nearest integer, is ________ g.
The mass of 1.00 mol of allicin, rounded to the nearest integer, is ________ g.
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In the periodic table, the elements touching the steplike line are known as ________.
In the periodic table, the elements touching the steplike line are known as ________.
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Elements in Group 8A are known as the ________.
Elements in Group 8A are known as the ________.
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Fluorine forms an ion with a charge of ________.
Fluorine forms an ion with a charge of ________.
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What is the concentration (M) of a NaCl solution prepared by dissolving 9.1 g of NaCl in sufficient water to give 375 mL of solution?
What is the concentration (M) of a NaCl solution prepared by dissolving 9.1 g of NaCl in sufficient water to give 375 mL of solution?
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________ and ________ reside in the atomic nucleus.
________ and ________ reside in the atomic nucleus.
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Which one of the following is a correct expression for molarity?
Which one of the following is a correct expression for molarity?
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Vertical columns of the periodic table are known as ________.
Vertical columns of the periodic table are known as ________.
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When 3.50 g of magnesium burns, the theoretical yield of magnesium oxide is ________ g.
When 3.50 g of magnesium burns, the theoretical yield of magnesium oxide is ________ g.
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The atomic number indicates ________.
The atomic number indicates ________.
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There are ________ sulfur atoms in 25 molecules of C4H4S2.
There are ________ sulfur atoms in 25 molecules of C4H4S2.
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What are the spectator ions in the reaction between KOH (aq) and HNO3 (aq)?
What are the spectator ions in the reaction between KOH (aq) and HNO3 (aq)?
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There are ________ mol of bromide ions in 0.600 L of a 0.350 M solution of AlBr3.
There are ________ mol of bromide ions in 0.600 L of a 0.350 M solution of AlBr3.
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When the following equation is balanced, the coefficient of sulfur dioxide is ________. PbS (s) + O2 (g) → PbO (s) + SO2 (g)
When the following equation is balanced, the coefficient of sulfur dioxide is ________. PbS (s) + O2 (g) → PbO (s) + SO2 (g)
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How many moles of Co2+ are present in 0.350 L of a 0.150 M solution of CoI2?
How many moles of Co2+ are present in 0.350 L of a 0.150 M solution of CoI2?
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How many milliliters of a stock solution of 14.2 M HNO3 would be needed to prepare 0.500 L of 0.500 M HNO3?
How many milliliters of a stock solution of 14.2 M HNO3 would be needed to prepare 0.500 L of 0.500 M HNO3?
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When the following equation is balanced, the coefficient of hydrogen is ________. K (s) + H2O (l) → KOH (aq) + H2 (g)
When the following equation is balanced, the coefficient of hydrogen is ________. K (s) + H2O (l) → KOH (aq) + H2 (g)
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Which one of the following is a weak acid?
Which one of the following is a weak acid?
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This reaction is an example of ________. 8536Kr → 8537Rb + _____
This reaction is an example of ________. 8536Kr → 8537Rb + _____
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The combustion of propane (C3H8) in the presence of excess oxygen yields CO2 and H2O. When 7.3 g of C3H8 burns, ________ g of CO2 is produced.
The combustion of propane (C3H8) in the presence of excess oxygen yields CO2 and H2O. When 7.3 g of C3H8 burns, ________ g of CO2 is produced.
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Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride. If the percent yield is 79.0% from a 7.90-g sample, it yields ________ g of SF6.
Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride. If the percent yield is 79.0% from a 7.90-g sample, it yields ________ g of SF6.
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The number 0.01120 has ________ significant figures.
The number 0.01120 has ________ significant figures.
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The maximum amount of SF6 that can be produced from the reaction of 3.5 g of sulfur with 4.5 g of fluorine is ________ g.
The maximum amount of SF6 that can be produced from the reaction of 3.5 g of sulfur with 4.5 g of fluorine is ________ g.
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Which one of the following compounds is chromium(III) oxide?
Which one of the following compounds is chromium(III) oxide?
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The charge on an electron was determined in the ________.
The charge on an electron was determined in the ________.
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The atomic number of an atom of 131I is ________.
The atomic number of an atom of 131I is ________.
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The correct name for SO is ________.
The correct name for SO is ________.
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Based on the equations below, which metal is the most active?
Based on the equations below, which metal is the most active?
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Barium forms an ion with a charge of ________.
Barium forms an ion with a charge of ________.
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Study Notes
Isotopes and Atomic Mass
- Average atomic mass is calculated based on isotopes' masses and their percentages.
- Given isotopes of element X:
- 221X: 82.900% abundance, mass 220.90 amu
- 220X: 13.200% abundance, mass 220.00 amu
- 218X: 3.9000% abundance, mass 218.10 amu
- Average atomic mass = 220.67 amu.
Chemical Prefixes
- The prefix milli- is abbreviated as "m".
Empirical Formulas
- Combustion of a compound yielding 2.265 g CO2 and 1.236 g H2O from a 1.031 g sample reveals empirical formula as C3H8O.
Percent Yield
- In a sulfur and oxygen reaction, producing 7.9 g of SO3 from 5.0 g O2 and 6.0 g S results in a percent yield of 93%.
Balancing Reactions
- When balancing the equation for calcium and water, the coefficient of H2O is 2.
Reaction Theoretical Yields
- Reaction of 1.0 g S and 1.0 g O2 can theoretically produce a maximum of 1.7 g SO3.
Neutralization Reactions
- A 0.6543 g sample containing 53.66% oxalic acid requires 22.39 mL of 0.3483 M NaOH for neutralization.
Mole Calculations
- 52.06 g of CO2 contains approximately 1.424 × 10^24 oxygen atoms.
- The combustion of ammonia produces 119 g of NO2 from the combustion of 43.9 g of ammonia.
Neutron Counting
- 182W contains 108 neutrons.
Density Calculations
- Density of a wooden object with mass 10.782 g and volume 13.72 mL is 7.859 × 10^-1 g/mL.
Acid Titration
- Unknown concentration of HNO3 titrated with NaOH gives concentration of 0.0102 M.
Chemical Compounds
- Aluminum reacts with oxygen to produce a maximum of 4.7 g Al2O3 from 2.5 g of each reactant.
- Production of 13 g of C2H2 from calcium carbide requires 18 g of H2O.
- Calcium ion charges are 3+.
Ionic Relationships
- Ca2+ ion has 20 protons.
- 14C atom contains 6 protons.
Ion Concentration
- Total ion concentration in 0.625 M HCl solution is 1.25 M.
Dalton’s Atomic Theory
- Atoms are composed of protons and neutrons, incorrect postulate was atoms consist of these particles.
Errors in Compound Naming
- Incorrect pairing includes Mg3N2 as magnesium nitrite.
Molecular Weights
- Formula weight of potassium dichromate (K2Cr2O7) is 294.18 amu.
- Mass % of F in KrF2 is 31.20%.
Group Properties in the Periodic Table
- Elements in the same group have similar physical and chemical properties.
- Group 1A elements are alkali metals, Group 8A elements are noble gases.
Molarity
- Molarity of chloride ions in a solution containing NaCl and CaCl2 is 0.816.
- Correct expression for molarity: mol solute/L solution.
Significant Figures
- Number 0.01120 has 4 significant figures.
Active Metals and Reactions
- Copper isotope with 29 protons and 34 neutrons: 29 p+, 34 n°.
- Most active metal in reactions is Ni.
Radioactive Decay Types
- Given decay of 8536Kr to 8537Rb is an example of beta decay.
Notebook Summary
- Understanding isotopes, stoichiometry, empirical formulas, acid-base reactions, and the periodic table's structure is fundamental in mastering AP Chemistry concepts.
- Always focus on units, significant figures, balanced equations, and identifying correct formulas or names in compounds.
Studying That Suits You
Use AI to generate personalized quizzes and flashcards to suit your learning preferences.
Description
Test your knowledge with this practice quiz covering Chapters 1-4 and 21 of AP Chemistry. Engage with flashcards that challenge your understanding of isotopes, atomic masses, and common prefixes in chemistry. Perfect for exam preparation and review.
