Chemistry In Context
9th Edition
ISBN: 9781259638145
Author: Fahlman, Bradley D., Purvis-roberts, Kathleen, Kirk, John S., Bentley, Anne K., Daubenmire, Patrick L., ELLIS, Jamie P., Mury, Michael T., American Chemical Society
Publisher: Mcgraw-hill Education,
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 1.6, Problem 1.10YT
In addition to aluminum, other metals such as scandium and yttrium, known as rare earth metals, are also found in cell phones and most electronic devices. What are the natural sources of these metals, and in which parts of the world are these minerals found?
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
The elements of Group 1-B (Cu, Ag, and Au) are sometimes referred to as the “coinage metals.” Why? What properties do they have that make them particularly useful for this purpose?
Magnesium is a valuable, lightweight metal. It is used as a structural metal and in alloys, in batteries, and in chemical synthesis. Although
magnesium is plentiful in Earth's crust, it is cheaper to "mine" the metal from seawater. Magnesium forms the second most abundant cation in
the sea (after sodium); there are about 1.30 g of magnesium in 1.00 kg of seawater. The method of obtaining magnesium from seawater
employs all three types of reactions discussed in this chapter precipitation, acid-base, and redox reactions. In the first stage in the recovery of
magnesium, limestone (CaCO3) is heated at high temperatures to produce quicklime, or calcium oxide (CaO):
CaCO3(s)
-----> CaO(s) + CO2a)
When calcium oxide is treated with seawater, it forms calcium hydroxide [Ca(OH)], which is slightly soluble and ionizes to give Ca2* and OH
ions:
CaO(s) + H2Om-> Ca (aq)
+2 OH (aq)
The surplus hydroxide ions cause the much less soluble magnesium hydroxide to precipitate:
Mg (aq)
+ 2 OH (aq)…
Identify the compound of calcium which is yellowish white powder and is used for disinfecting drinking water. Write its chemical name and formula. How is it manufactured? Write the chemical equation for the reaction involved. Also list two other uses of the compound.
Chapter 1 Solutions
Chemistry In Context
Ch. 1.1 - Prob. 1.2YTCh. 1.1 - Prob. 1.3YTCh. 1.2 - a. List some examples of macroscopic objects in...Ch. 1.3 - Prob. 1.5YTCh. 1.3 - For each of the following compounds, calculate...Ch. 1.3 - Prob. 1.7YTCh. 1.4 - Determine the number of protons and electrons in...Ch. 1.5 - Prob. 1.9YTCh. 1.6 - In addition to aluminum, other metals such as...Ch. 1.6 - For each of the values below, determine the number...
Ch. 1.6 - Prob. 1.12YTCh. 1.7 - Prob. 1.13YTCh. 1.7 - Prob. 1.14YTCh. 1.8 - Prob. 1.15YTCh. 1.8 - a. Express the current U.S. national debt and...Ch. 1.9 - Using a laser pointer, predict and then determine...Ch. 1.9 - a. An unknown metal was found to have a mass of...Ch. 1.10 - Prob. 1.19YTCh. 1.10 - Prob. 1.20YTCh. 1.11 - Prob. 1.21YTCh. 1 - The smallest building blocks inside your cell...Ch. 1 - In these diagrams, two different types of atoms...Ch. 1 - From the solids, liquids, or gases that are...Ch. 1 - Express each of these numbers in scientific...Ch. 1 - Prob. 5QCh. 1 - Prob. 6QCh. 1 - Consider the following blank periodic table. a....Ch. 1 - Classify each of these substances as an element, a...Ch. 1 - Prob. 9QCh. 1 - Provide the number of protons, neutrons, and...Ch. 1 - Classify each of the following compounds as...Ch. 1 - Calculate the atomic percentages for each of the...Ch. 1 - For the following molecules, list the number and...Ch. 1 - Prob. 14QCh. 1 - What are the oxidation states of the metals in the...Ch. 1 - Prob. 16QCh. 1 - The processor chips in portable and desktop...Ch. 1 - Prob. 18QCh. 1 - Prob. 19QCh. 1 - Prob. 20QCh. 1 - Prob. 21QCh. 1 - Prob. 22QCh. 1 - Prob. 23QCh. 1 - Prob. 24QCh. 1 - Prob. 25QCh. 1 - List some waste products generated from the...Ch. 1 - Prob. 27QCh. 1 - Prob. 29QCh. 1 - Prob. 30QCh. 1 - Prob. 31QCh. 1 - Prob. 32QCh. 1 - Prob. 33QCh. 1 - Prob. 34QCh. 1 - Prob. 35QCh. 1 - Prob. 36QCh. 1 - Prob. 37QCh. 1 - Using Internet resources, perform a life-cycle...Ch. 1 - Prob. 39QCh. 1 - Prob. 40QCh. 1 - Prob. 41Q
Additional Science Textbook Solutions
Find more solutions based on key concepts
Give the IUPAC name for each compound.
Organic Chemistry
Describe the evolution of mammals, tracing their synapsid lineage from early amniote ancestors to true mammals....
Loose Leaf For Integrated Principles Of Zoology
45. Calculate the mass of nitrogen dissolved at room temperature in an 80.0-L home aquarium. Assume a total pre...
Chemistry: Structure and Properties (2nd Edition)
How could you separate a mixture of the following compounds? The reagents available to you are water, either, 1...
Organic Chemistry (8th Edition)
56. Global Positioning System. Learn more about the global positioning system and its uses. Write a short repo...
The Cosmic Perspective (8th Edition)
Label each statement about the polynucleotide ATGGCG as true or false. The polynucleotide has six nucleotides. ...
General, Organic, and Biological Chemistry - 4th edition
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
- 4.48 Elemental phosphorous is used in the semiconductor industry. It can be obtained from an ore called fluoroapatite via reaction with SiO2 and C: 4Ca5( PO4)3F+18SiO2+30C3P4+30CO+18CaSiO3+2CaF2 Suppose a particular semiconductor production plant requires 1500 kg of P4. If the recovery of P4 from this reaction is 73% efficient, what mass of fluoroapatite is needed?arrow_forwardPhosphorus occurs naturally in the form of fluorapatite, CaF2 3Ca3(PO4)2. The dot indicates 1 part CaF2 to 3 parts Ca3(PO4)2. This mineral is reacted with an aqueous solution of H2SO4 in the preparation of a fertilizer. The products are phosphoric acid, hydrogen fluoride, and gypsum, CaSO4 2H2O. Write the balanced equation describing this process.arrow_forwardFind out which sample of iron ore contains the highest iron content by calculating the mass percentage of iron in hematite (Fe2O3), magnetite (Fe304), and siderite (FeCO3)arrow_forward
- How to write a chemical equation for transition metal ions found in a solution? The ions found were Cobalt and Copper. Co2+ (aq) + Cu2+ (aq) was mixed with NaOH (aq). It formed Co(OH)2 (s) + Cu(OH)2 (s) + Na^+ (aq). The sample was decanted and Na+ was removed. NH3(aq) was added to Co(OH)2 (s) + Cu(OH)2 (s) and became Co(OH)2 + Cu(NH3)4 ^2+ and NH3. The sample was centrifuged and decanted the ions were now in their own tubes. One tube had Co(OH)2 and the other had Cu(NH3)4 ^2+ and NH3. The tube with Co(OH)2 was then mixed with HNO3 and became Co^2+. The tube with Cu(NH3)4 ^2+ and NH3 was mixed with HNO3 and became Cu^ 2+ and NH4^+.arrow_forwardThe legal limit for chromium in drinking water is 0.10 ppm. What is the maximum permissible mass of chromium (in \mu gμg) in exactly 1.0 cup (8.0 fl. oz.) of drinking water? Assume the density of drinking water is 1.00 g/mL. (1 fl. oz. = 29.57 mL)(Express your answer with two significant digits.)arrow_forwardPhosphorus may be determined analytically by precipitating it as MgNH4PO4 followed by ignition to Mg2P2O7. What mass of Mg2P2O7 will be obtained from a 9.346 g sample of phosphate rock which contains 71.24% Ca3(PO4)2?arrow_forward
- The most common minerals found in soils are combinations of which four elements, which are also the most common elements. A K, Zn, Cu, I B Si, AI, O, Fe с) S, H, О, N D) с, Н, О, Narrow_forwardA prospector wants to know how much gold is in the ore that he has been mining. A sample weighing 11.2456 grams is dissolved in Aqua Regia (a mixture of HCl and HNO3). That sample is then transferred to a 200.00 mL volumetric flask and diluted to the mark with water. This is called solution 1. A volumetric pipet is used to transfer 10.00 mL of solution 1 to a second 500.00 mL volumetric flask. The second flask is filled to the mark resulting in solution 2. 5.00 mL of solution 2 is analyzed and found to contain 13.45 ppm Au. Answer each of the questions below. 1. What is the concentration of Au in solution 1. The units should be ppm 2. How many micrograms of Au are in the 5.00 mL sample that was measured? 3. How many micrograms of gold were in the 500.00 mL flask containing solution 2. 4. How many grams Au were in the flask containing solution 1 5. What is the %Au in the original sample?arrow_forwardd) Which of the following substances can be considered chemically pure? ● ● Air ● Apple juice Brass Seawater ● A bar of 24-karat goldarrow_forward
- Ariana plans to react a sample of magnesium carbonate (MgCO3) with hydrochloric acid (HCl) to generate magnesium chloride (MgCl2), carbon dioxide gas (CO2), and liquid water (H2O). Write the balanced chemical equation for this reaction.arrow_forwardMg(OH)2(s)+2HNO3(aq)→ the balanced chemical formula?arrow_forwardElemental phosphorus is used in the semiconductor industry. It can be obtained from an ore called fluoroapatite via reaction with SiO2 and C: 4 Cas (PO4)3F + 18 SiO2 + 30 C → 3 P4 + 30 CO + 18 CaSiO3 + 2 CaF2 Suppose a particular semiconductor production plant requires 2100 kg of P4. If the recovery of P, from this reaction is 79% efficient, what mass of fluoroapatite is needed? Mass = kg Submit Answer Try Another Version 10 item attempts remainingarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
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: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher: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: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Bonding (Ionic, Covalent & Metallic) - GCSE Chemistry; Author: Science Shorts;https://www.youtube.com/watch?v=p9MA6Od-zBA;License: Standard YouTube License, CC-BY
Stoichiometry - Chemistry for Massive Creatures: Crash Course Chemistry #6; Author: Crash Course;https://www.youtube.com/watch?v=UL1jmJaUkaQ;License: Standard YouTube License, CC-BY