Chemistry: Structure and Properties
1st Edition
ISBN: 9780321834683
Author: Nivaldo J. Tro
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Question
Chapter 1, Problem 53E
Interpretation Introduction
To determine:
The mass of oxygen per gram of sulfur for each sample and show that these results are consistent with law of multiple proportions.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Indicate exactly (% and T)
where the eutectic point is
located
Temperature (°C)
2200
2000
Liquid
1800
1600
Cristobalite
+
Liquid
40
60
80
18
4000
3800
Liquid
3600
+
Alumina
3400
1890 ± 10°C
Mullite (ss)
Mullite
(ss)
+
Liquid
Alumina
Mullite (ss)
1587 ± 10°C
Mullite (ss)
+
Cristobalite
1400
0
20
40
(SiO2)
L
3200
3000
2800
2600
60
80
100
(Al2O3)
Composition (wt% Al2O3)
Temperature (°F)
18. Explain with the help of partial molecular orbitals the difference between an acceptor
and a donor ligand.
19. Construct molecular orbital diagram consistent with [Ni(NH))6]²
20. Draw the molecular orbital diagrams of
(a)
(b)
[FeCle]
[Fe(CN)6]³
Determine whether the complexes are high spin or low spin
What is the total number of molecular orbitals of each complex ion
Calculate the ligand field stabilization energy and the spin only magnetic moment of each
complex ion.
Calculate the value of the ionic packing factor of CsI, which has a CsCl structure, knowing that the radius of Cs+ is 0.165 nm and that of I– is 0.220 nm.
Chapter 1 Solutions
Chemistry: Structure and Properties
Ch. 1 - Which statement is true about matter? a) Matter is...Ch. 1 - A chemist mixes sodium with water and witnesses a...Ch. 1 - Two samples of a compound containing elements A...Ch. 1 - A compound containing only carbon and hydrogen has...Ch. 1 - Which concept was demostrated by Rutherford’s gold...Ch. 1 - A student re-creates Millikan’s oil drop...Ch. 1 - Prob. 7SAQCh. 1 - An isotope of an element contains 82 protons and...Ch. 1 - How many electrons are in the Cr3+ ion? 24...Ch. 1 - A naturally occurring sample of an element...
Ch. 1 - Copper has an atomic mass of 63.55 amu and two...Ch. 1 - Which sample contains the greatest number of...Ch. 1 - Explain this statement in your own words and give...Ch. 1 - Explain the main goal of chemistry.Ch. 1 - What are two different ways to classify matter?Ch. 1 - How do solids, liquids, and gases differ?Ch. 1 - Explain the difference between a pure substance...Ch. 1 - Explain the difference between an element and a...Ch. 1 - Explain the difference between a homogeneous and a...Ch. 1 - Describe the scientific approach to knowledge. How...Ch. 1 - Prob. 9ECh. 1 - What observations did Antoine Lavoisier make? What...Ch. 1 - What theory did John Dalton formulate?Ch. 1 - What is wrong with the expression, “That is just a...Ch. 1 - Summarize the history of the atomic idea. How was...Ch. 1 - Prob. 14ECh. 1 - State and explain the law of definite proportions.Ch. 1 - State and explain the law of multiple proportions....Ch. 1 - What are the main ideas in Dalton’s atomic theory?...Ch. 1 - How and by whom was the electron discovered? What...Ch. 1 - Explain Millikan’s oil drop experiment and how it...Ch. 1 - Prob. 20ECh. 1 - Describe Rutherford’s gold foil experiment. How...Ch. 1 - Describe Rutherford’s nuclear model of the atom....Ch. 1 - If matter is mostly empty space, as suggested by...Ch. 1 - List the three subatomic particles that compose...Ch. 1 - What defines an element?Ch. 1 - Explain the difference between Z (the atomic...Ch. 1 - Where do elements get their names?Ch. 1 - What are isotopes? What is percent natural...Ch. 1 - Describe the two different notations used to...Ch. 1 - Prob. 30ECh. 1 - Prob. 31ECh. 1 - Explain how a mass spectrometer works. What kind...Ch. 1 - Each shape represents a type of particle (such as...Ch. 1 - Using triangles to represent one type of atom and...Ch. 1 - Classify each substance as a pure substance or a...Ch. 1 - Classify each substance as a pure substance or a...Ch. 1 - Prob. 37ECh. 1 - Complete the table. Substance Pure or mixture Type...Ch. 1 - Determine whether each molecular diagram...Ch. 1 - Determine whether each molecular diagram...Ch. 1 - Classify each statement as an observation, a law,...Ch. 1 - Classify each statement as an observation, a law,...Ch. 1 - A chemist decomposes several samples of carbon...Ch. 1 - When astronomers observe distant galaxies, they...Ch. 1 - Prob. 45ECh. 1 - An automobile gasoline tank holds 21 kg of...Ch. 1 - Two samples of carbon tetrachloride are decomposed...Ch. 1 - Two samples of sodium chloride are decomposed into...Ch. 1 - The mass ratio of sodium to fluorine in sodium...Ch. 1 - Upon decomposition, one sample of magnesium...Ch. 1 - Two different compounds containing osmium and...Ch. 1 - Palladium forms three different compounds with...Ch. 1 - Prob. 53ECh. 1 - Sulfur and fluorine form several different...Ch. 1 - Which statements are consistent with Dalton’s...Ch. 1 - Which statements are inconsistent with Dalton’s...Ch. 1 - Which statements are consistent with Rutherford’s...Ch. 1 - Which statements are inconsistent with...Ch. 1 - A chemist in an imaginary universe, where...Ch. 1 - Imagine a unit of charge called the zorg. A...Ch. 1 - Which statements about subatomic particles are...Ch. 1 - Which statements about subatomic particles are...Ch. 1 - Write isotopic symbols in the form XA (e g., C-13)...Ch. 1 - Write isotopic symbols in the form ZAX for each...Ch. 1 - Determine the number of protons and the number of...Ch. 1 - Determine the number of protons and the number of...Ch. 1 - The amount of carbon-14 in ancient artifacts and...Ch. 1 - Uranium-235 is used in nuclear fission. Determine...Ch. 1 - Determine the number of protons and the number of...Ch. 1 - Determine the number of protons and the number of...Ch. 1 - Gallium has two naturally occurring isotopes with...Ch. 1 - Magnesium has three naturally occurring isotopes...Ch. 1 - The atomic mass of fluorine is 18.998 amu, and its...Ch. 1 - The atomic mass of copper is 63.546 amu. Do any...Ch. 1 - An element has two naturally occurring isotopes....Ch. 1 - An element has four naturally occuring isotopes...Ch. 1 - Bromine has two naturally occurring isotopes...Ch. 1 - Silicon has three naturally occurring isotopes...Ch. 1 - Use the mass spectrum of europium shown here to...Ch. 1 - Use the mass spectrum of rubidium shown here to...Ch. 1 - A 7.83-g sample of HCN contains 0.290 g of H and...Ch. 1 - The ratio of sulfur to oxygen by mass in SO2 is...Ch. 1 - Use the mass spectrum of lead shown here to...Ch. 1 - Use the mass spectrum of mercury shown here to...Ch. 1 - Nuclei with the same number of neutrons but...Ch. 1 - Fill in the blanks to complete the table. Symbol z...Ch. 1 - Silver is composed of two naturally occurring...Ch. 1 - To the right is a representation of 50 atoms of a...Ch. 1 - The ratio of oxygen to nitrogen by mass in NO2 is...Ch. 1 - Naturally occurring cobalt consists of only one...Ch. 1 - A 7.36-g sample of copper is contaminated with an...Ch. 1 - The ratio of the mass of O to the mass of N in...Ch. 1 - Naturally occurring magnesium has an atomic mass...Ch. 1 - A volatile liquid (one that readily evaporates) is...Ch. 1 - The diagram to the right represents solid carbon...Ch. 1 - Use triangles to represent atoms of element A and...Ch. 1 - Identify each statement as being most like an...
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
- Calculate the atomic packing factor of quartz, knowing that the number of Si atoms per cm3 is 2.66x1022 and that the atomic radii of Si and O are 0.038 and 0.117 nm.arrow_forwardChoose one or more: Draw the Lewis structure. Consider and draw alternate resonance structures. Calculate the molar mass of the compound. Leave out the lone pairs of electrons. Complete the octets of each atom (dublet for H). Determine the central atom, if possible. Determine the number of covalent bonds in the structure. Check the structure with electron bookkeeping Question: Determine which of the following procedures are steps in drawing the resonance structures of pyridine and pyrazine. Check all that apply.arrow_forward1. Draw the shapes of the various d orbitals and explain why they are split into two groups; 12g and eg in an octahedral field Draw a diagram to show how the d orbitals are split into groups with different energy in an octahedral field. Some electronic configurations may exist in both high spin and low spin arrangements in an octahedral field. Draw all of these cases, and suggest which metal ions and which ligands might give rise to each. Draw an energy level diagram to show the lifting of degeneracy of the 3d orbitals in a tetrahedral ligand field . Give the number of unpaired electrons in a strong and weak octahedral field for (a) Cr² (b) Co and (c) Fe. Calculate the CFSE and magnetic moment in each casearrow_forward
- 9. Describe and explain the Jahn teller effect in octahedral complexes of Cu² and Cr Define paramagnetism and diamagnetism. What is the difference between an inner orbital complex and an outer orbital complex? The complex [NiCN)4] is diamagnetic, but [NiCla] is paramagnetic and has two unpaired electrons, explain these observations and deduce the structures of the two complexes The complex ion [Co (NH3)6] is octahedral and diamagnetic, the complexion [CoF6] is also octahedral but paramagnetic. How does valence bond theory account for this observation? How does crystal field explain color of complexes?arrow_forward5. Show how the d orbital splitting changes as an octahedral complex undergoes tetragonal distortion and eventually becomes a square planar complex. What is the spectrochemical series and what is its importance Using crystal field theory, (a) Draw the d-orbital electronic configuration of [Cr(CN)6]³ (b) How many unpaired electrons are present? (c) Calculate the CFSE and magnetic moment of the complex ion (c) If six Br groups were substituted for the six CN groups to give [CrBr.]³ would you expect Ao to increase or decrease? Why? Describe how Ao changes as the charge on the metal changes from M² to M and how it changes between a first row, second row or third row transition element.arrow_forward15. Describe clearly how crystal field theory explains satisfactorily the magnetic moment of transition metal complexes. Which complex has the larger crystal field splitting? Give reasons for your answer. (i) [Co(CN)6] or (ii) [Co(H2O)²+ or (iii) [Co(NH)6] or [Co(NH3)6] [Co(H_O)] [Rh(NH3)]* What relationship exist between A (the crystal field splitting) and the pairing energy (P) in determining whether a given complex will be high spin or low spin.arrow_forward
- Part 1 See Periodic Table Draw the major resonance contributor for the skeletal arrangement CNNO 2 (arrangement a). Include all nonbonding electrons and all nonzero formal charges. The skeleton has been given to you. Н Ν HCNO SE F ·N—N; ☑ P Cl Br Iarrow_forward5. Show how the d orbital splitting changes as an octahedral complex undergoes tetragonal distortion and eventually becomes a square planar complex. What is the spectrochemical series and what is its importance Using crystal field theory, (a) Draw the d-orbital electronic configuration of [Cr(CN)6]³ (b) How many unpaired electrons are present? (c) Calculate the CFSE and magnetic moment of the complex ion (c) If six Br groups were substituted for the six CN groups to give [CrBr.]³ would you expect Ao to increase or decrease? Why? Describe how Ao changes as the charge on the metal changes from M² to M and how it changes between a first row, second row or third row transition element.arrow_forwardPart 1 See Periodic Table One resonance structure of CNO¯ is shown. In the first box, add two curved arrows to show the movement of electrons that result in the resonance form with a -1 formal charge on the oxygen atom. In the second box, draw this resonance form with the -1 formal charge on the oxygen atom by adding bonds, lone pairs, and non-zero formal charges. =0% → [N=C=O 1 N-C-0arrow_forward
- Draw any major resonance contributor for S2O3, assuming that the S atoms are bonded to each other, and the O atoms are bonded to S atoms. Include all nonbonding electrons and all nonzero formal charges.arrow_forwardDetermine which of the following procedures are steps in drawing the resonance structures of pyridine and pyrazine. Check all that apply. Draw the Lewis structure.Consider and draw alternate resonance structures. Calculate the molar mass of the compound. Leave out the lone pairs of electrons. Determine the central atom, if possible. Complete the octets of each atom (dublet for H). Determine the number of covalent bonds in the structure. Check the structure with electron bookkeeping.arrow_forwardDetermine which of the following procedures are steps in drawing the resonance structures of pyridine and pyrazine. Check all that apply. Draw the Lewis structure.Consider and draw alternate resonance structures.Calculate the molar mass of the compound.Leave out the lone pairs of electrons.Determine the central atom, if possible.Complete the octets of each atom (dublet for H).Determine the number of covalent bonds in the structure.Check the structure with electron bookkeeping.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
The Bohr Model of the atom and Atomic Emission Spectra: Atomic Structure tutorial | Crash Chemistry; Author: Crash Chemistry Academy;https://www.youtube.com/watch?v=apuWi_Fbtys;License: Standard YouTube License, CC-BY