Introduction to Chemistry
4th Edition
ISBN: 9781259288722
Author: BAUER
Publisher: MCG
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 2, Problem 111QP
A 100-g sample of zinc sul�de contains 67.1 g zinc and 32.9 g sulfur. if a 1.34-g sample of zinc is heated with excess sulfur, 2.00 g of zinc sul�de form. Show how these data are in agreement with the law of de�nite proportions.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Chapter 2 Solutions
Introduction to Chemistry
Ch. 2 - What evidence suggests that matter is composed of...Ch. 2 - How can the composition of atom differ?Ch. 2 - How do ions differ from the atoms of elements?Ch. 2 - How can we describe the mass of the atoms of the...Ch. 2 - How does the periodic table relate to the...Ch. 2 - For the atom represented in the following diagram,...Ch. 2 - A rare isotope of carbon has a mass number of 14....Ch. 2 - Write two representations for the following...Ch. 2 - Determine the number of neutrons in each of the...Ch. 2 - How many protons and electrons compose the...
Ch. 2 - Write the isotope symbols for ions that have the...Ch. 2 - The copper mined from Earth’s crust consists of...Ch. 2 - The element lithium is composed of two isotopes,...Ch. 2 - Identify the element that is described. (a) the...Ch. 2 - Prob. 10PPCh. 2 - Match the key terms with the descriptions...Ch. 2 - Match the key terms with the descriptions...Ch. 2 - Prob. 3QPCh. 2 - What modern technique allows us to “see� the...Ch. 2 - How does Dalton‘s atomic theory describe atoms...Ch. 2 - How does Dalton’s atomic the theory the law of...Ch. 2 - How does Dalton‘s atomic theory explain the law...Ch. 2 - How does Dalton's atomic theory explain the...Ch. 2 - Does the following diagram represent a chemical...Ch. 2 - Does the following diagram represent a chemical...Ch. 2 - Which experiment showed that all atoms contain...Ch. 2 - What information about the structure of the atom...Ch. 2 - Which subatomic particles are negatively charged?Ch. 2 - Which subatomic particles are positively charged?Ch. 2 - Helium is used in balloons and blimps because of...Ch. 2 - Hydrogcn-3 (tritium) is used as a tracer in...Ch. 2 - Which subatomic particle has approximately the...Ch. 2 - Which of the following best describes about how...Ch. 2 - Explain why the mass of a carbon atom is about...Ch. 2 - Which subatomic particle was discovered last? Why...Ch. 2 - Prob. 21QPCh. 2 - How many protons are in each atom of each of the...Ch. 2 - The number of which subatomic particle determines...Ch. 2 - How do isotopes of an element differ?Ch. 2 - What information do you need to determine the...Ch. 2 - What information do you need to determine the mass...Ch. 2 - Which of the following are always the same for...Ch. 2 - Which of the following are different for isotopes...Ch. 2 - Given the composition of the nuclei, what are the...Ch. 2 - Identify the element from the atom shown. What are...Ch. 2 - What are the atomic number, neutron number, and...Ch. 2 - Identify the element from the atom shown. What are...Ch. 2 - Prob. 33QPCh. 2 - How many protons, neutrons, and electrons are in...Ch. 2 - What is the isotope symbol for atoms that contain...Ch. 2 - What is the isotope symbol for atoms that contain...Ch. 2 - How many protons and neutrons are in an atom...Ch. 2 - How many protons and neutrons are in an atom...Ch. 2 - A study of blood flow in heart muscle uses...Ch. 2 - Phosphorus-32 can be used to treat eye tumors. How...Ch. 2 - Complete the following table for the designated...Ch. 2 - Complete the following table for the designated...Ch. 2 - How do an atom and an ion of the same element...Ch. 2 - What changes when an ion forms from an atom, or...Ch. 2 - Prob. 45QPCh. 2 - What forms when an ion with a 1+ charge undergoes...Ch. 2 - Prob. 47QPCh. 2 - Write the symbol for the ion that is formed after...Ch. 2 - How many protons and electrons are found in each...Ch. 2 - How many protons and electrons are found in each...Ch. 2 - Prob. 51QPCh. 2 - Prob. 52QPCh. 2 - What element has 18 electrons when it forms a...Ch. 2 - What element has 18 electrons when it forms an...Ch. 2 - What element has 27 electrons when it forms a...Ch. 2 - What element has 46 electrons when it forms a...Ch. 2 - How do 7Li+6Li each differ from a neutral...Ch. 2 - How do B3579r and B3581r Br differ in their...Ch. 2 - Potassium citrate is a compound found in some...Ch. 2 - Calcium citrate is a compound found in some...Ch. 2 - What is the basis for the atomic mass unit (amu)...Ch. 2 - What is the mass of a carbon-12 atom on the amu...Ch. 2 - What is the approximate mass, in atomic mass...Ch. 2 - Estimate the combined mass (in atomic mass units)...Ch. 2 - Approximately how much greater in mass is a D2...Ch. 2 - Approximately how much greater in mass is a D2O...Ch. 2 - Approximately how much greater in mass is a...Ch. 2 - Approximately how much greater in mass is a...Ch. 2 - Why do we use the amu mass scale instead of the...Ch. 2 - What is the relationship between grams and atomic...Ch. 2 - What is the difference between the mass of an atom...Ch. 2 - Which isotope has exactly the same mass (in atomic...Ch. 2 - How is the mass of an individual atom determined?...Ch. 2 - Which of the following is most likely the mass of...Ch. 2 - Naturally occurring calcium is composed of two...Ch. 2 - Naturally occurring silicon is composed mostly of...Ch. 2 - An unknown element (X) discovered on a planet in...Ch. 2 - Suppose that the isotope abundance of magnesium on...Ch. 2 - The mass spectrum of nickel is shown. (a) What is...Ch. 2 - The mass spectrum of magnesium is shown. (a) What...Ch. 2 - What is the mass in amu of 1000 boron atoms?Ch. 2 - What is the mass in amu of 1000 mercury atoms?Ch. 2 - Which contains more atoms, 2500 amu of boron atoms...Ch. 2 - A sample of pure silver and a simple of pure gold...Ch. 2 - Identify which of the elements Br, K, Mg, Al, Mn,...Ch. 2 - Identify which of the elements He, Zn, Pb, L Ca,...Ch. 2 - Prob. 87QPCh. 2 - Name the element that is an alkaline earth metal...Ch. 2 - What element is in group IVB (4) and in period 4?Ch. 2 - What element is in group IVA (14) and in period 2?Ch. 2 - Identify each of the following elements as a...Ch. 2 - Identify each of the following elements as a...Ch. 2 - Identify the following elements as a main-group...Ch. 2 - Identify the following elements as a main-group...Ch. 2 - Prob. 95QPCh. 2 - Prob. 96QPCh. 2 - Prob. 97QPCh. 2 - Prob. 98QPCh. 2 - Prob. 99QPCh. 2 - The noble gases are sometimes called “inert...Ch. 2 - The ions of many of the main-group elements have...Ch. 2 - Prob. 102QPCh. 2 - Identify the groups of the periodic table in which...Ch. 2 - For each group listed. identify the charge on the...Ch. 2 - Prob. 105QPCh. 2 - Prob. 106QPCh. 2 - Prob. 107QPCh. 2 - Chlorine gas reacts with potassium to form a...Ch. 2 - When iron rusts. a compound forms with the formula...Ch. 2 - Is the law of conservation of mass obeyed in the...Ch. 2 - A 100-g sample of zinc sul�de contains 67.1 g...Ch. 2 - A 100-g sample of HgO contains 92.6 g mercury and...Ch. 2 - What properties of electrons contributed to why...Ch. 2 - What experimental evidence led to each of the...Ch. 2 - Which isotope has a mass number of 60 and an...Ch. 2 - Why is it impossible for an element to have a mass...Ch. 2 - How many protons and neutrons are in a...Ch. 2 - What number of each type of subatomic particle is...Ch. 2 - Explain why the relative atomic mass of cobalt is...Ch. 2 - Which element has an isotope that has a mass...Ch. 2 - Some tables list relative atomic mass to as many...Ch. 2 - How many atoms are in each of the following...Ch. 2 - Naturally occurring iodine is composed of only one...Ch. 2 - Prob. 124QPCh. 2 - A sample of pure carbon and a sample of pure...Ch. 2 - Two equal-volume balloons contain the same number...Ch. 2 - Naturally occurring boron comprises two isotopes,...Ch. 2 - Prob. 128QPCh. 2 - Prob. 129QPCh. 2 - Nitrogen and oxygen are the main components of the...Ch. 2 - Prob. 131QPCh. 2 - Which element is the only nonmetal in group IVA...Ch. 2 - Prob. 133QPCh. 2 - Prob. 134QPCh. 2 - Complete the following table for the designated...Ch. 2 - Atoms of the element shown in this photo contain...Ch. 2 - Positron emission tomography (PET) is used in...Ch. 2 - When silver tarnishes, a chemical reaction occurs...Ch. 2 - The iron found in the human body is in the form of...Ch. 2 - Which has the greater density, an ice cube...Ch. 2 - Prob. 141QPCh. 2 - After he conducted cathode ray tube experiments...Ch. 2 - Analysis of carbon-14 content is used to date...Ch. 2 - A naturally occurring isotope of potassium has a...Ch. 2 - Prob. 145QPCh. 2 - A monatomic ion with a 4+ charge has the same...Ch. 2 - Which of the following has the greatest number of...Ch. 2 - Prob. 148QPCh. 2 - Atoms that are isotopes of the same element differ...Ch. 2 - Which of the following statements about atoms and...Ch. 2 - Elements in which group always form monatomic ions...Ch. 2 - Identify the number of protons and neutrons in an...Ch. 2 - Naturally occurring gallium (Ga) is made of two...Ch. 2 - Which of the following elements is classi�ed as...
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- An element X bas five major isotopes, which are listed below along with their abundances. What is the element? Isotope Percent Natural Abundance Mass (u) 46x 8.00% 45.95232 47x 7.30% 46.951764 48x 73.80% 47.947947 49x 5.50% 48.947841 50x 5.40% 49.944792arrow_forward3.116 The simplest approximate chemical formula for the human body could be written as C728H4850O1970N104Ca24P16K4S4Na3Cl2Mg. Based on this formula, describe how you would rank by mass the ten most abundant elements in the human body.arrow_forwardThe density of a mixture of gases may be calculated by summing the products of the density of each gas and the fractional volume of space occupied by that gas. (Note the similarity to the calculation of the molar mass of an element from the isotopic masses and fractional abundances.) Assume dry air with CO2 removed is 20.96% (by volume) oxygen. 78.11% nitrogen, and 0.930% argon. Determine the density of argon.arrow_forward
- The element europium exists in nature as two isotopes: 151Eu has a mass of 150.9196 u and 153Eu has a mass of 152.9209 u. The average atomic mass of europium is 151.96 u. Calculate the relative abundance of the two europium isotopes.arrow_forwardThese questions concern the work of J. J. Thomson: From Thomson’s work, which particles do you think he would feel are most important in the formation of compounds (chemical changes) and why? Of the remaining two subatomic particles, which do you place second in importance for forming compounds and why? Come up with three models that explain Thomson’s findings and evaluate them. To be complete you should include Thomson’s findings.arrow_forwardEarly tables of atomic weights (masses) were generated by measuring the mass of a substance that reacts with 1.00 g of oxygen. Given the following data and taking the atomic mass of hydrogen as 1.00, generate a table of relative atomic masses for oxygen, sodium, and magnesium. Element Mass That Combines with 1.00g Oxygen Assumed Formula Hydrogen 0.126 g HO Sodium 2.875 g NaO Magnesium 1.500 g MgO How do your values compare with those in the periodic table? How do you account for any differences?arrow_forward
- The age of the universe is unknown, but some conclude from measuring Hubbles constant that the age is about 18 billion years old, which is about four times the age of Earth. If so, calculate the age of the universe in seconds. If you had a sample of carbon with the same number of carbon atoms as there have been seconds since the universe began, determine whether you could measure this sample on a laboratory balance that can detect masses as small as 0.1 mg.arrow_forwardThe action of bacteria on meat and fish produces a compound called cadaverine. As its name and origin imply, it stinks! (It is also present in bad breath and adds to the odor of urine.) It is 58.77% C, 13.81% H, and 27.40% N. Its molar mass is 102.2 g/mol. Determine the molecular formula of cadaverine.arrow_forwardIn Groups 4A-6A, there are several elements whose symbols begin with S. Name these elements, and for each one give its symbol, atomic number, group number, and period. Describe each as a metal, metalloid, or nonmetal.arrow_forward
- Reference Section 5-2 to find the atomic masses of 12C and 13C, the relative abundance of 12C and 13C in natural carbon, and the average mass (in u) of a carbon atom. If you had a sample of natural carbon containing exactly 10,000 atoms, determine the number of 12C and 13C atoms present. What would be the average mass (in u) and the total mass (in u) of the carbon atoms in this 10,000-atom sample? If you had a sample of natural carbon containing 6.0221 1023 atoms, determine the number of 12C and 13C atoms present What would be the average mass (in u) and the total mass (in u) of this 6.0221 1023 atom sample? Given that 1 g = 6.0221 1023 u, what is the total mass of I mole of natural carbon in units of grams?arrow_forwardThe element bromine is Br2, so the mass of a Br2 molecule is the sum of the mass of its two atoms. Bromine has two isotopes. The mass spectrum of Br2 produces three peaks with relative masses of 157.836, 159.834, and 161.832, and relative heights of 6.337, 12.499. and 6.164, respectively. (a) What isotopes of bromine are present in each of the three peaks? (b) What is the mass of each bromine isotope? (c) What is the average atomic mass of bromine? (d) What is the abundance of each of the two bromine isotopes?arrow_forwardNeon has three stable isotopes, one with a small abundance. What are the abundances of the other two isotopes? 20Ne, mass = 19.992435 u; percent abundance = ? 21Ne mass = 20.993843 u; percent abundance = 027% 22Ne mass = 21.991383 u: percent abundance = ?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Introductory Chemistry: A FoundationChemistryISBN:9781285199030Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781285199030
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Atomic Number, Atomic Mass, and the Atomic Structure | How to Pass ChemistryThe Nucleus: Crash Course Chemistry #1; Author: Crash Course;https://www.youtube.com/watch?v=FSyAehMdpyI;License: Standard YouTube License, CC-BY