Introductory Chemistry: An Active Learning Approach
6th Edition
ISBN: 9781305079250
Author: Mark S. Cracolice, Ed Peters
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Question
Chapter 6, Problem 27E
Interpretation Introduction
Interpretation:
The names and formulas of the five -ic acids that must be memorized before learning the acid nomenclature system is to be stated.
Concept introduction:
The number of each kind of atom which makes up the particle generally called as the composition, is denoted by the chemical formula. Besides, at normal temperature seven elements are found as two atoms. Physical observation tells us the acid is a substance having sour taste. Chemically, acid is a substance which is having a proton (H+ ion) and it can be detached by a water molecule when the acid meets water.
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
ings
ools
Molecular compounds are usually composed solely
of nonmetals. A binary molecular compound is one
in which the compound contains only two elements
(regardless of how many atoms are present of
each). When naming binary molecular compounds,
prefixes are used to specify the number of atoms of
each element. Take a moment to review some of
the prefixes shown here.
Prefix Number
mono
di
nona
one
three
tetra
four
penta five
hexa six
hepta seven
octa eight
nine
deca
two
ten
For example, SF6 is named sulfur hexafluoride.
Note that the prefix mono is not used in naming the
first element. Also note that the second element in
the name should end with the suffix ide.
▼
Part A
Using the rules for naming molecular compounds described in the introduction, what is
the name for the compound PC15?
Spell out the full name of the compound.
►View Available Hint(s)
Submit
Part B
Using the rules for naming molecular compounds described in the introduction, what is
the name for the compound N₂ CL?…
What is the nomenclature (name) of this acid H P?
O Hydrophoshporic acid
O Phosphoric acid
O Phosphorous acid
O Hydrogen phosphorus
Naming binary acids
When naming acids, start by naming the anion. A monatomic anion, such as CI , is simple named by replacing the ending of the element name with ide. For example, CI is
named chloride and 02- is named oxide.
Once the anion is named, name the acid based on this anion. Start by adding the prefix hydro, and then change the ide suffox to ic. For example, HCl would require the anion
chloride to be changed to chloric. Adding the prefix hydro creates hydrochloric acid.
Part A
What is the name of the acid whose formula is HI?
Spell out the full name of the acid.
• View Available Hint(s)
Chapter 6 Solutions
Introductory Chemistry: An Active Learning Approach
Ch. 6 - Review of Selected Concepts Related to...Ch. 6 - Prob. 2ECh. 6 - Write the chemical formula of each of the...Ch. 6 - Write the chemical formula of each of the...Ch. 6 - Prob. 5ECh. 6 - Prob. 6ECh. 6 - Prob. 7ECh. 6 - Prob. 8ECh. 6 - Prob. 9ECh. 6 - Prob. 10E
Ch. 6 - Prob. 11ECh. 6 - Prob. 12ECh. 6 - Prob. 13ECh. 6 - CCl4, CBr4, NO, dinitrogen monoxide, sulfur...Ch. 6 - Prob. 15ECh. 6 - Write an equation that shows the formation of a...Ch. 6 - Prob. 17ECh. 6 - Prob. 18ECh. 6 - Prob. 19ECh. 6 - Prob. 20ECh. 6 - Prob. 21ECh. 6 - Prob. 22ECh. 6 - What are the names of AgBr, SnF2, Fe2O3, and...Ch. 6 - Prob. 24ECh. 6 - Prob. 25ECh. 6 - Prob. 26ECh. 6 - Prob. 27ECh. 6 - Prob. 28ECh. 6 - Prob. 29ECh. 6 - Fill in the blanks in the following table....Ch. 6 - Prob. 31ECh. 6 - Prob. 32ECh. 6 - What is the formula of sodium tellurate; what are...Ch. 6 - Prob. 34ECh. 6 - Explain how an anion can behave like an acid. Is...Ch. 6 - Prob. 36ECh. 6 - Prob. 37ECh. 6 - Prob. 38ECh. 6 - Prob. 39ECh. 6 - Prob. 40ECh. 6 - Among the following, identify all hydrates and...Ch. 6 - Prob. 42ECh. 6 - Prob. 43ECh. 6 - Prob. 44ECh. 6 - Prob. 45ECh. 6 - Prob. 46ECh. 6 - Prob. 47ECh. 6 - Prob. 48ECh. 6 - Prob. 49ECh. 6 - Prob. 50ECh. 6 - Prob. 51ECh. 6 - Prob. 52ECh. 6 - Prob. 53ECh. 6 - In each box, write the chemical formula of the...Ch. 6 - Prob. 55ECh. 6 - Prob. 56ECh. 6 - Prob. 57ECh. 6 - Prob. 58ECh. 6 - Prob. 59ECh. 6 - Prob. 60ECh. 6 - Prob. 61ECh. 6 - Prob. 62ECh. 6 - Prob. 63ECh. 6 - Prob. 64ECh. 6 - Prob. 65ECh. 6 - Prob. 66ECh. 6 - Prob. 67ECh. 6 - Prob. 68ECh. 6 - Prob. 69ECh. 6 - Prob. 70ECh. 6 - Prob. 71ECh. 6 - Prob. 72ECh. 6 - Prob. 73ECh. 6 - Prob. 74ECh. 6 - Prob. 75ECh. 6 - Prob. 76ECh. 6 - Prob. 77ECh. 6 - Prob. 78ECh. 6 - Prob. 79ECh. 6 - Prob. 80ECh. 6 - Prob. 81ECh. 6 - Prob. 82ECh. 6 - Prob. 83ECh. 6 - Prob. 84ECh. 6 - Prob. 85ECh. 6 - Prob. 86ECh. 6 - Prob. 1CLECh. 6 - Prob. 2CLECh. 6 - Prob. 3CLECh. 6 - Prob. 4CLECh. 6 - Prob. 1PECh. 6 - Prob. 2PECh. 6 - Prob. 3PECh. 6 - Prob. 4PECh. 6 - Prob. 5PECh. 6 - Prob. 6PECh. 6 - Prob. 7PECh. 6 - Prob. 8PECh. 6 - Prob. 9PECh. 6 - Prob. 10PECh. 6 - Prob. 11PECh. 6 - Prob. 12PECh. 6 - Prob. 13PECh. 6 - Prob. 14PECh. 6 - Prob. 15PECh. 6 - Prob. 16PECh. 6 - Prob. 17PE
Knowledge Booster
Similar questions
- What are the IUPAC names of the following compounds? manganese dioxide mercurous chloride ( Hg2Cl2) ferric nitrate [Fe( No 3)3] titanium tetrachioride cupric bromide (CuBr2)arrow_forwardWhen is it okay to use Greek prefixes for naming ionic substances? For example, I have seen TiO2 named titanium dioxide and Ti(IV) oxide. Which one is the correct name? I have seen Greek prefixes used with other ionic substances as well. It was my understanding that Greek prefixes were only used for molecular substances and not ionic. In ionic substances we use charges to name the substances and in molecular we do not. Thank you for your time.arrow_forwardMolecular compounds: Are there any prefixes needed.Ionic compounds: Which ones need Roman numerals and Why?Indicate which ones have polyatomic ion and if they are they cations or anions?Are there any acids or bases? Are the acids binary acids or oxyacid? Which have a strong acid or a strong base.Why do you think it is important to understand how to write formulas? How will this knowledge help you in your healthcare career? Name Ionic Molecular Prefix Required Polyatomic Cation Polyatomic Anion Acid/ Base Strong Acid/Base Binary/ oxyacid Roman Num Name CuSO4 HCl NaOH SnCl2 HNO3 H2SO4 PCl3arrow_forward
- Some of the names below are incorrect. Beside each name, write an “X” for an incorrect name and a “✔” for a correct name. For each incorrect name, explain what is wrong and why it is incorrect. I attatched the chart as well as my answers. I was unsure if the ending of the polyatomic names were changed to "ide" or not. I have also found that some periodic tables have more charges on elements than others, so I wasn't sure if Chlorine was a multivalent metal or not, as different periodic tables said different things. Thanks.arrow_forwardIn order to correctly name a compound, you must first be able to classify the type of compound. Identify the following compounds as one of the following within the list of 4 types. The abbreviations are shown in the parenthesis. Notice this on this assignment, binary and polyatomic binary are catagorized as a single category. lonic (1), molecular (M), binary acid (BA), oxyacid (OA) 1. CBr3 M 2. KCI 1 3. HCI [Select] 4. RbOH [Select] 5. Cu₂0 1 6. Si2S4 | Select] 7. Au2Br10 [Select] 8. H3PO4 (clue: acid) [Select]arrow_forwardBoth questions refer to each otherarrow_forward
- Now that we have a reference for many of the common polyatomic ions, let's look at how to write the chemical formulas for compounds that contain them. There are two main things to keep in mind: If a compound contains more than one polyatomic ion of the same type, we need to place parentheses around the ion's formula beforeusing a subscript to indicate how many ions of that type are in the compound. The overall charge for the ionic compound must be neutral, which means the sum of the charges from the cations and anions should add up to zero.We can use this rule to figure out the formula of an ionic compound when we know the charge on the anion and the cation. This rule can also be useful for deducing the charge of an ion when the chemical formula for the ionic compound is known. Example: Write the chemical formula for calcium hydroxide (calcium and hydroxide). Calcium is an alkaline earth metal in Group 2 on the periodic table, so it forms ions with a 2+ charge. From our table…arrow_forwardNow that we have a reference for many of the common polyatomic ions, let's look at how to write the chemical formulas for compounds that contain them. There are two main things to keep in mind: If a compound contains more than one polyatomic ion of the same type, we need to place parentheses around the ion's formula beforeusing a subscript to indicate how many ions of that type are in the compound. The overall charge for the ionic compound must be neutral, which means the sum of the charges from the cations and anions should add up to zero.We can use this rule to figure out the formula of an ionic compound when we know the charge on the anion and the cation. This rule can also be useful for deducing the charge of an ion when the chemical formula for the ionic compound is known. Example: Write the chemical formula for calcium hydroxide (calcium and hydroxide). Calcium is an alkaline earth metal in Group 2 on the periodic table, so it forms ions with a 2+ charge. From our table…arrow_forwardUsing the table below showing the names of common polyatomic anions, type out each compound's full name in the space provided. Note: Exact spelling using the table below is required for a correct answer. Also, for your answer to be counted as correct, the first word (the cation) should be capitalized, but the second word (the polyatomic anion) in the naming may or may not be to be counted correct in this problem. Names of common polyatomic anions Nonmetal Carbon Nitrogen Oxygen Phosphorus Sulfur b. Ca(OH)2: Formula CO3²- HCO3- CH3CO₂ CN- NO3- NO₂ OH- a. Na₂CO3: Sodium carbonate PO 3- HPO 2- H₂PO4 SO ₂²- HSO SO3²- HSO3- e. Mg3(PO4)2: Calcium hydroxide c. Mg(NO3)2: Magnesium nitrate d. Mn(CH3CO2)2 : Manganese (II) acet. Name Carbonate Hydrogen carbonate or bicarbonate Acetate Cyanide Nitrate Nitrite Hydroxide Phosphate Hydrogen phosphate Dihydrogen phosphate Sulfate Hydrogen sulfate or bisulfate Sulfite Hydrogen sulfite or bisulfitearrow_forward
- NOMENCLATURE Please write the name or the formula, as appropriate, for each of the following compounds or elements. Use pencil. Neatness counts! If I can't read it, it must be wrong. FeBr2 calcium oxalate AGHSO4 hydrogen peroxide NH,IO4 periodic acid Pd;N2 lithium hydrogen phosphate LİHCO3 vanadium(V) chromate Mn(MnO4)4 gold(III) hydroxide Fe2(SO3); barium cyanide N20 (g) tin(IV) sulfate HBr (g) diphosphorus tetrabromide HBr (aq) phosphorus pentafluoride НВГО (аq). calcium dichromate SeF6 ammonium hypobromite H2SO; (aq) aluminum nitride H;P(g) hydroselenic acid HIO2 (aq) manganese(IV) carbonate Ni3N2 nitrous acid KSCN palladium(II) acetate Mg3(PO4)2 nickel B2O3 iodine trichloride AIPO4:7H2O disulfur dioxidearrow_forwardComplete the table with the positive ion, negative ion, and the name for the compounds. Use the subscript (X2) and superscript (X2) buttons as needed. Normal BIIIU X2| X| - fxl ID e Formula Positive ion Negative ion Name CazSO4 Ca2+ so,2- Calcium sulfate Fe(OH)3 Sr3(PO4)2 Nacio Al(NO2)3 K2SO3arrow_forwardRead: An Ion is a charged atom, # protons ≠ # electrons. On page three, paragraph one states, “The prefix poly- means many and atomic refers to atoms, so a polyatomic ion is an ion that contains more than one atom. This differentiates polyatomic ions from monatomic ions, which contain only one atom.” Ions that contain only one atom are called monoatomic ions. Ions that contain more than one atom are called polyatomic ions. A monatomic ion is a single charged atom, with the number of protons not equal to the number of electrons. A polyatomic ion is a group of covalently-bonded atoms, with the total number of protons not equal to the total number of electrons. Using the image attached how could you further elaborate this answer? Cite evidence from the image.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Introductory Chemistry: An Active Learning Approa...ChemistryISBN:9781305079250Author:Mark S. Cracolice, Ed PetersPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningGeneral 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 by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Introductory Chemistry: An Active Learning Approa...
Chemistry
ISBN:9781305079250
Author:Mark S. Cracolice, Ed Peters
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
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 by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
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:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning