(a)
Interpretation: The balanced chemical equation should be written for the reaction of hydrogen gas with oxygen.
Concept introduction: The reaction of elements with hydrogen produces either ionic metal hydrides or molecular compounds. The reaction of hydrogen with metals produces ionic metal hydrides. The electronegativity of hydrogen is more than metals and hence, metals bear positive charge and hydrogen has a negative charge. Thus, the oxidation number of hydrogen in ionic metal hydrides is
The oxidation number of metals in ionic hydrides and non-metals in molecular compounds are according to the group number and valence electron configuration of these elements.
So, hydrogen reacts with both metals and non-metals to produce hydrides of corresponding elements. However, the elements belonging to the noble gas family have very low chemical reactivity and therefore do not combine with hydrogen.
(b)
Interpretation: The balanced chemical equation should be written for the reaction of hydrogen gas with chlorine.
Concept introduction: The reaction of elements with hydrogen produces either ionic metal hydrides or molecular compounds. The reaction of hydrogen with metals produces ionic metal hydrides. The electronegativity of hydrogen is more than metals and hence, metals bear positive charge and hydrogen has a negative charge. Thus, the oxidation number of hydrogen in ionic metal hydrides is
The oxidation number of metals in ionic hydrides and non-metals in molecular compounds are according to the group number and valence electron configuration of these elements.
So, hydrogen reacts with both metals and non-metals to produce hydrides of corresponding elements. However, the elements belonging to the noble gas family have very low chemical reactivity and therefore do not combine with hydrogen.
(c)
Interpretation: The balanced chemical equation should be written for the reaction of hydrogen gas with nitrogen.
Concept introduction: The reaction of elements with hydrogen produces either ionic metal hydrides or molecular compounds. The reaction of hydrogen with metals produces ionic metal hydrides. The electronegativity of hydrogen is more than metals and hence, metals bear positive charge and hydrogen has a negative charge. Thus, the oxidation number of hydrogen in ionic metal hydrides is
The oxidation number of metals in ionic hydrides and non-metals in molecular compounds are according to the group number and valence electron configuration of these elements.
So, hydrogen reacts with both metals and non-metals to produce hydrides of corresponding elements. However, the elements belonging to the noble gas family have very low chemical reactivity and therefore do not combine with hydrogen.
Want to see the full answer?
Check out a sample textbook solutionChapter 21 Solutions
Chemistry & Chemical Reactivity
- The reaction of elemental phosphorus and excess oxygen produces P4O10. Name the compound. (a) phosphorus oxide (b) phosphoric acid (c) phosphorus decaoxide (d) tetraphosphorus decaoxidearrow_forwardPhosphorous acid, H3PO3, is oxidized to phosphoric acid, H3PO4, by nitric acid, which is reduced to nitrogen monoxide, NO. Write the balanced equation for this reaction.arrow_forward4.48 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_forward
- Write balanced equations for the reaction of scandium metal to produce the scandium(III) salt with the following nonmetals: (a) sulfur (c) nitrogen (b) chlorine (d) oxygen (forming the oxide)arrow_forwardComplete and balance the equations of the following reactions, each of which could be used to remove hydrogen sulfide from natural gas: (a) Ca(OH)2(s)+H2S(g) (b) Na2CO3(aq)+H2S(g)arrow_forwardWrite balanced chemical equations for the following reactions: (a) cadmium burned in air. (b) elemental cadmium added to a solution of hydrochloric acid. (c) cadmium hydroxide added to a solution of acetic acid, CH3CO2Harrow_forward
- Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co
- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning