Concept explainers
(a)
Interpretation:
Name of the
Concept Introduction:
Ionic compounds:
Naming of ionic compounds that contain monoatomic ions are given by using the name of the cation (mostly metal), which is followed by the name of anion. The anion (mostly nonmetal) is named by adding the suffix “-ide”. When an ionic compound is made up of only two elements, it is known as binary compounds.
In case of binary compounds, the numerical prefixes are not shown in the name because the number of ions is inferred from the empirical formula.
Molecular compounds:
Two or more nonmetals combine to form molecular compounds. The naming of molecular compound is given by following two rules.
- Element that is present in far left of the periodic table appears in the name first.
- Element that is closer to bottom within any of the group appears in the name first.
Numerical prefixes are used in case of molecular compounds to mention how many times the atom of same elements occurs in the formula. Prefix mono is not used for the first element while for the second element it is used.
(b)
Interpretation:
Name of the
Concept Introduction:
Refer part (a).
(c)
Interpretation:
Name of the
Concept Introduction:
Refer part (a).
(d)
Interpretation:
Name of the
Concept Introduction:
Refer part (a).
Want to see the full answer?
Check out a sample textbook solutionChapter 2 Solutions
Chemistry: Principles and Practice
- write a balanced chemical equation for each (A) Iron (III) chloride reacts with sodium hydroxide to produce iron (III) hydroxide and sodium chloride. (B) Magnesium nitrite reacts with perchloric acid to produce magnesium perchlorate and nitrous acid. (C) Copper(II) hydroxide reacts with hydrosulfuric acid to produce copper (II) sulfide and water.arrow_forwardThe reaction of pentane, C5H12, with oxygen, O2, gives carbon dioxide and water. (a) Write a balanced equation for this reaction.arrow_forwardHydrazine 1N2H42 and dinitrogen tetroxide 1N2O42 form a self-igniting mixture that has been used as a rocket propellant. The reaction products are N2 and H2O. (a) Write a balanced chemical equation for this reaction.arrow_forward
- Ammonium dihydrogen phosphate, formed from the reaction of phosphoric acid with ammonia, is used as a crop fertilizer as well as a component of some fire extinguishers. (a) What are the mass percentages of N and P in the compound? (b) How much ammonia is incorporated into 100. g of the compound?arrow_forward(A) CsBr (B) MgCl2arrow_forward(a) List four physical characteristics of a solid metal. (b) List two chemical characteristics of a metallic element.arrow_forward
- Chrom ium metal reacts with oxygen to give chromiu m(III) oxide, Cr2O3. (a) Write a balanced equation for the reaction. (b) What mass (in grams) of Cr2O3 is produced if 0.175 g of chromium metal is converted completely to the oxide? (c) What mass of O2 (in grams) is required for the reaction?arrow_forwardWrite the empirical formula of the compound formed by (a) Al3+ and Cl - ions, (b) Al 3+ and O2 - ions, (c) Mg2+ and NO3 ions.arrow_forwardMost abundant metal on the surface of the earth:(a) Iron(b) Aluminium(c) Calcium(d) Sodiumarrow_forward
- Which statement about the properties of barium chloric and mercury(II) chloride is correct? (A) BaCl₂ has a higher melting point than HgCl₂. (B) BaCl₂ has a higher solubility in nonpolar solvents than HgCl₂. (C) BaCl₂ has a higher vapor pressure than HgCl₂. (D) Molten BaCl₂ has a lower electrical conductivity than molten HgCl2.arrow_forwardFor many years the recovery of gold—that is, the separation of gold from other materials—involved the use of potassium cyanide: Au + KCN + O2 + H2O à KAu(CN)2 + KOH (a) Balance the above chemical equation. (b) What is the minimum amount of potassium cyanide in grams needed to extract 29.0 g (about an ounce) of gold?arrow_forwardThe first step in the manufacture of nitric acid by the Ostwald process is the reaction of ammonia gas with oxygen, producing nitrogen oxide and steam. The reaction mixture contains 7.60 g of ammonia and 10.00 g of oxygen. After the reaction is complete, 6.22 g of nitrogen oxide are obtained.(a) Write a balanced equation for the reaction.(b) How many grams of nitrogen oxide can be theoretically obtained?(c) How many grams of excess reactant are theoretically unused?(d) What is the percent yield of the reaction?arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY