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(a)
Interpretation:
The Lewis structure of strongest oxoacid of bromine should be drawn.
Concept introduction:
Lewis structures are the diagrams that show the bonding between the atoms of the molecules and existing lone pairs of electrons.
(b)
Interpretation:
The Lewis structure of a hydrogen compound of nitrogen in which there is an −N-N- bond should be drawn.
Concept introduction: : Lewis structures are the diagrams that show the bonding between the atoms of the molecules and existing lone pairs of electrons.
(c)
Interpretation:
The Lewis structure of an acid added to cola drinks should be drawn.
Concept introduction:
Lewis structures are the diagrams that show the bonding between the atoms of the molecules and existing lone pairs of electrons.
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Chapter 21 Solutions
CHEMISTRY:PRIN.+REACTIONS-OWLV2 ACCESS
- The elements sodium, aluminum, and chlorine are in the same period. (a) Which has the greatest electronegativity? (b) Which of the atoms is smallest? (c) Which is the largest possible oxidation state for each of these elements? (d) Will the oxide of each element in the highest oxidation state (write its formula) be acidic, basic, or amphoteric?arrow_forwardCompounds such as NaBH4, Al(BH4)3, and LiAlH4 are complexhydrides used as reducing agents in many syntheses.(a) Give the oxidation state of each element in these compounds.(b) Write a Lewis structure for the polyatomic anion in NaBH4, and predict its shape.arrow_forward(b) (i) Draw the Lewis structure of methanol, CH3OH(ℓ). (ii) Show with a simple diagram how methanol dissolves in water. Explain.arrow_forward
- Draw a Lewis structure for(a) The cyclic silicate ion Si₄O₁₂⁸⁻(b) A cyclic hydrocarbon with formula C₄H₈arrow_forward(a) Which poisonous gas is evolved when white phosphorus is heated with Cone. NaOH solution? Write the chemical equation. (b) Write the formula of first noble gas compound prepared by N. Bartlett. What inspired N. Bartlett to prepare this compound? (c) Fluorine is a stronger oxidising agent than chlorine. Why? (d)Write one use of chlorine gas.arrow_forwardChlorine dioxide gas (ClO2) is used as a commercial bleachingagent. It bleaches materials by oxidizing them. In thecourse of these reactions, the ClO2 is itself reduced. (a)What is the Lewis structure for ClO2? (b) Why do you thinkthat ClO2 is reduced so readily? (c) When a ClO2 moleculegains an electron, the chlorite ion, ClO2-, forms. Draw theLewis structure for ClO2-. (d) Predict the O—Cl—O bondangle in the ClO2- ion. (e) One method of preparing ClO2is by the reaction of chlorine and sodium chlorite:Cl2(g) + 2 NaClO2(s)------>2 ClO2(g) + 2 NaCl(s)If you allow 15.0 g of NaClO2 to react with 2.00 L of chlorinegas at a pressure of 1.50 atm at 21 °C, how many gramsof ClO2 can be prepared?arrow_forward
- Ammonium chloride, NH4Cl, is a very soluble salt in water.(a) Draw the Lewis structures of the ammonium and chlorideions. (b) Is there an N—Cl bond in solid ammonium chloride?(c) If you dissolve 14 g of ammonium chloride in 500.0 mLof water, what is the molar concentration of the solution?(d) How many grams of silver nitrate do you need to add tothe solution in part (c) to precipitate all of the chloride as silverchloride?arrow_forwardWrite a Lewis structure for each of the following molecules and ions:(a) (CH3)3SiH(b) SiO44−(c) Si2H6(d) Si(OH)4(e) SiF62−arrow_forwardComplete and balance the following acid-base equations:(a) A solution of HClO4 is added to a solution of LiOH.(b) Aqueous H2SO4 reacts with NaOH.(c) Ba(OH)2 reacts with HF gas.arrow_forward
- Each of the chemically active Period 2 elements forms stable compounds in which it has bonds to fluorine. (a) What are the names and formulas of these compounds? (b) Does ∆EN increase or decrease left to right across the period? (c) Does percent ionic character increase or decrease left to right? (d) Draw Lewis structures for these compoundsarrow_forwardPhosphoric acid, one of the acids used in some cola drinks, is produced by the reaction of phosphorus(V) oxide, an acidic oxide, with water. Phosphorus(V) oxide is prepared by the combustion of phosphorus.(a) Write the empirical formula of phosphorus(V) oxide.(b) What is the molecular formula of phosphorus(V) oxide if the molar mass is about 280.(c) Write balanced equations for the production of phosphorus(V) oxide and phosphoric acid.(d) Determine the mass of phosphorus required to make 1.00 × 104 kg of phosphoric acid, assuming a yield of 98.85%.arrow_forwardWrite the Lewis structure for each of the following. You may wish to review the chapter on chemical bonding and molecular geometry.(a) PH3(b) PH4+(c) P2H4(d) PO43−(e) PF5arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
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