Hello i need help with these blanks Fill in the blanksCompositional NameHydrogen bromideDinitrogen perta oxicleElementsFormulaH,BrHBrin each rowN2O5There areSe;sBitHHiNNitHCcePiFI,0Xe FAS,OBi,0Selenium sulfideno typos!BH3H(N3)NH3AmmoniaCarbon tetrachloridePfsPhosphorus pentafluoride1,03XeF6As406Xennon hexa@tenorideBi,O3Bismuth f)oxide

We have to fill the blanks in each row as follows in step 2:

Compositional Name Hydrogen bromide Dinitrogen pentaoxidle Elements Formula Fill in the blanks HBr HBr in each row N,O5 There are Ses BitHt H,N NH C.ce PiF I,0 Xe,F AS,0 Bi,0 Selenium sulfide no typos! BH3 H(N3) NH3 Ammonia Carbon tetrachloride Pfs Phosphorus pentafluoride I,03 XeF6 As406 BizO3 Xenon hexadenoride Bismuth fJoxide

Compositional Name Hydrogen bromide Dinitrogen pentaoxidle Elements Formula Fill in the blanks HBr HBr in each row N,O5 There are Ses BitHt H,N NH C.ce PiF I,0 Xe,F AS,0 Bi,0 Selenium sulfide no typos! BH3 H(N3) NH3 Ammonia Carbon tetrachloride Pfs Phosphorus pentafluoride I,03 XeF6 As406 BizO3 Xenon hexadenoride Bismuth fJoxide

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter21: Chemistry Of The Nonmetals

Section: Chapter Questions

Problem 34QAP

See similar textbooks

Similar questions

Suppose we introduce the following pointdefects.(a) Mg2+ ions substitute for yttrium ionsin Y2O3; (b) Fe3+ ions substitute for magnesiumions in MgO;(c) Li1+ ions substitute for magnesiumions in MgO; and(d) Fe2+ ions replace sodium ions inNaCl.What other changes in each structuremight be necessary to maintain a chargebalance? Explain.
A major challenge in implementing the “hydrogen economy”is finding a safe, lightweight, and compact way of storinghydrogen for use as a fuel. The hydrides of light metalsare attractive for hydrogen storage because they can store ahigh weight percentage of hydrogen in a small volume. Forexample, NaAlH4 can release 5.6% of its mass as H2 upondecomposing to NaH1s2, Al1s2, and H21g2. NaAlH4 possessesboth covalent bonds, which hold polyatomic anionstogether, and ionic bonds. (a) Write a balanced equationfor the decomposition of NaAlH4. (b) Which element inNaAlH4 is the most electronegative? Which one is the leastelectronegative? (c) Based on electronegativity differences,predict the identity of the polyatomic anion. Draw a Lewisstructure for this ion. (d) What is the formal charge on hydrogenin the polyatomic ion?
The lead(IV) oxide used in car batteries is prepared by coat-ing the electrode plate with PbO and then oxidizing it to leaddioxide (PbO₂). Despite its name, PbO₂ has a nonstoichiometricratio of lead to oxygen of about 1/1.98. In fact, the holes in the PbO₂ crystal structure due to missing O atoms are responsiblefor the oxide’s conductivity. (a) What is the mole % of O miss-ing from the PbO₂ structure? (b) What is the molar mass of the nonstoichiometric compound?
The prefix eka- comes from the Sanskrit word for “one.”Mendeleev used this prefix to indicate that the unknownelement was one place away from the known element thatfollowed the prefix. For example, eka-silicon, which we nowcall germanium, is one element below silicon. Mendeleevalso predicted the existence of eka-manganese, which was notexperimentally confirmed until 1937 because this element isradioactive and does not occur in nature. Based on the periodictable shown in Figure 7.1, what do we now call the elementMendeleev called eka-manganese?
Thiosulfate ion (S2O32-) and dithionite anion (S2O42-) are teo sulfur containing reducing agents. What are the oxidation states of sulfur in the two ions? Please show or explain calculations
In many ways, arsenate (AsO4 3−) is very similar to phosphate (PO4 3-), yet it does not substitute for phosphate in biomolecules. After reviewing the essential atomic characteristics of the element arsenic, explain this phenomenon.
Does sodium sulphide and calcium permanganate and iron oxide and nitride oxide and carbon fluoride and nitrogen oxide contain a multivalent metal?
At 400 °C, the ΔG°rxn for the oxidation of a monoatomic liquid element Z in the presence of O2(g) forming ZO(s) is -25.0 kJ per mol O2. In the compound ZO(s), Z has a +2 formal charge. Which of the following statements is CORRECT? ZO cannot be reduced back to Z at any temperature because reduction of ZO to Z has +ΔG. Z cannot be oxidized to ZO because Z is more stable than 20 at 400 °C or any T above it The oxidation of Z with O2 is exothermic. The oxidation of Z with O2 is marked by an increase in entropy.
why cant D be cleaved by PERIODIC ACID
A major challenge in implementing the “hydrogen economy”is finding a safe, lightweight, and compact way of storinghydrogen for use as a fuel. The hydrides of light metalsare attractive for hydrogen storage because they can store ahigh weight percentage of hydrogen in a small volume. Forexample, NaAlH4 can release 5.6% of its mass as H2 upondecomposing to NaH(s), Al(s), and H2(g). NaAlH4 possessesboth covalent bonds, which hold polyatomic anionstogether, and ionic bonds. (a) Write a balanced equationfor the decomposition of NaAlH4. (b) Which element inNaAlH4 is the most electronegative? Which one is the leastelectronegative? (c) Based on electronegativity differences,predict the identity of the polyatomic anion. Draw a Lewisstructure for this ion. (d) What is the formal charge on hydrogenin the polyatomic ion?
Alkaline earth metals are involved in two key diagonal rela-tionships in the periodic table. (a) Give the two pairs of elementsin these diagonal relationships. (b) For each pair, cite two simi-larities that demonstrate the relationship. (c) Why are the mem-bers of each pair so similar in behavior?
Why alkali metals donot exist as free in nature?