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introductory chemistry atoms first

Introductory Chemistry Atoms First 5th Edition Steve Russo And Michael Silver - Solutions

When aqueous H2SO4 is added to an aqueous solution of Pb(NO3)2(aq), a precipitate forms.(a) What is the precipitate?(b) Write a net ionic equation for the precipitation reaction.(c) Did adding Pb(NO3)2(aq) to the sulfuric acid neutralize the acid? Explain.
Consider the covalent bond in H2. Why must energy be added to break this bond (in other words, what is the added energy used for)?
Consider the ionic bonds between Na+ ions and Cl– ions in NaCl(s). Why must energy be added to break these bonds (in other words, what is the added energy used for)?
Suppose you have an aqueous solution containing Cu2+ ions and Na+ ions. What could you add that would remove the Cu2+ ions from solution without adding any new type of cations to the solution?
Suppose you have an aqueous solution of Pb2+ and Ba2+ ions.(a) How could you remove just the Pb2+ ions from the solution?(b) How could you remove both the Pb2+ and the Ba2+ ions from the solution at the same time?
Nitric acid consists of NO3– and a proton, H+.(a) Draw a Lewis dot diagram for the nitrate ion.(b) Draw a Lewis dot diagram for nitric acid.(c) Which species, nitrate ion or nitric acid, is more likely to be found in aqueous solution? Explain.
Write the intact-molecule equation and the net ionic equation for the neutralization reaction between perchloric acid, HClO4(aq), and NaOH(aq). What salt is in solution once the reaction is run?
Balance the following equation and classify the reaction it represents as combination, decomposition, single-replacement, or double-replacement:Fe + CdCl2 → FeCl3 + Cd
Would you expect a reaction in which all reactants are in the gas phase to go faster, slower, or remain at the same rate if the temperature is increased while everything else is held constant? Explain your answer.
Draw dot diagrams for the reactants and products in each equation, and indicate which bonds are broken and which bonds are formed:(a) CH4 + I2 → CH3I + HI(b) C2H4 + F2 → FCH2CH2F
Hydrogen gas is produced when elemental tin reacts with HF to produce hydrogen and tin(II) fluoride. Write the balanced equation for this reaction.
Classify each compound as acid, base, or salt:(a) KCl(b) CH3COOH(c) Al(OH)3(d) H3BO3(e) LiC2H3O2
Write the balanced chemical equation for the reaction between pentane, C5H12, and oxygen gas that produces carbon dioxide and water.
Write the balanced equation, the complete ionic equation, and the net ionic equation for the neutralization reaction that occurs when nitric acid, HNO3, is mixed with calcium hydroxide, Ca(OH)2.
Write the formula of the precipitate formed when these solutions are mixed:(a) Aluminum nitrate and sodium hydroxide (b) Potassium phosphate and calcium chloride (c) Magnesium sulfate and sodium carbonate
Write the balanced equation for the preparation of iron(III) oxide from iron metal and oxygen gas.What type of reaction is this?
Balance this chemical equation and classify it as combination, decomposition, single-replacement, or double-replacement:K2SO3 + S8 → K2S2O3
Which equations represent chemical reactions:(a) CO2(s) → CO2(g)(b) 3O2(g) → 2O3(g)(c) NaCl(s) + H2O(l) → NaOH(aq) + HCl(aq)(d) H2O(g) + CH4(g) → CH4(g) + H2O(g)
Balance this chemical equation, and classify it as combination, decomposition, single-replacement, or double-replacement: H₂PO4 + Ca(OH)2 →Ca3(PO4)2 + H₂O
Ammonia, NH3, reacts with chlorine gas, Cl2, to form ammonium chloride, NH4Cl, and nitrogen trichloride, NCl3. Write a balanced equation for this reaction.
Classify each reaction as combination, decomposition, single-replacement, or double-replacement:(a) 2 NaCl → 2Na + Cl2(b) Ba3N2 → 3Ba + N2(c) Cl2 + 2 NaI → 2NaCl + I2(d) KNO3 + AgBr → AgNO3 + KBr
What is the number of molecules of NaOH required to neutralize one molecule of:(a) H2SO4(b) HI(c) H3PO4(d) HNO3(e) CH3COOH
Oxygen can be produced by the decomposition of potassium chlorate, KClO3. The products of the reaction are KCl and O2. Write a balanced equation for the reaction.
Balance each equation:(a) Zn + HCl → ZnCl2 + H2(b) Na2O + H2O → NaOH(c) CH4 + H2S → CS2 + H2(d) CO + H2 → CH3OH
Calcium hydroxide can be used as an antacid to neutralize HCl, the acid found in the stomach. Water and calcium chloride, CaCl2, are the products of the reaction. Write the balanced equation for the reaction.
Carbon dioxide gas and calcium oxide are produced when calcium carbonate, CaCO3, is heated strongly. Write the balanced equation for this process.
Name the acid and base that combine to form:(a) KNO3(b) Ca3(PO4)2(c) Li2SO4(d) NaI
Mineral compounds containing sulfur are converted to oxygen-containing compounds by a process known as roasting, which involves heating the mineral in the presence of oxygen. In addition to the mineral oxide, sulfur dioxide is also produced. Write the balanced chemical equation for the roasting of
To calculate an oxidation state for an atom in a molecule you need to know:(a) How many electrons on the atom are core electrons.(b) The number of valence electrons in a free atom of the element.(c) The number of protons the atom owns.(d) The total number of valence electrons in the molecule.
Balance the following chemical equations.CH4 + O2S → CO2 + H2O
Chemical reactions occur when new substances are produced as a result of bonds being ________ in the reactants and bonds being _________ in the products.
Balance this equation and classify it as combination, decomposition, single-replacement, or double-replacement: K₂CrO4 + Al(NO3)3 → Al2(CrO4)3 + KNO3
When propane gas, C3H8, reacts with oxygen gas, carbon dioxide gas and water are produced. Write the balanced equation for the reaction.
The reaction of carbon monoxide gas with water vapor produces carbon dioxide gas and hydrogen gas. Write the balanced equation for the reaction.
When an aqueous acid is combined with an aqueous base, the products are a ________ and _________.
Which anions form compounds that are generally soluble in water: CO2, NO3, Br, SO2, OH, PO³-?
Balance this equation and classify it as combination, decomposition, single-replacement, or double-replacement:Mn + S → MnS2
Sulfur dioxide and water are formed when hydrogen sulfide, H2S, reacts with oxygen gas. Write the balanced equation for the reaction.
Write the balanced equation for the decomposition of magnesium oxide, MgO, into Mg and O2.
A solution containing which anion can be added to separate:(a) Na+(aq) from Ag+ (aq)(b) Na+(aq) from Ca2+ (aq)
Balance this equation and classify it as combination, decomposition, single-replacement, or double-replacement:H2O2 → H2O + O2
Write the net ionic equation for the reaction between solutions of:(a) Aluminum nitrate and sodium hydroxide(b) Potassium phosphate and calcium chloride(c) Magnesium sulfate and sodium carbonate
Heating magnesium carbonate results in the production of carbon dioxide and magnesium oxide. Write the balanced equation for this process, and indicate the type of reaction.
Is the reaction LiOH + HCN → H2O + LiCN a combination, decomposition, single-replacement, or double-replacement?
Indicate whether a precipitate forms when these solutions are mixed, and write the formula of the precipitate if one forms:(a) Silver nitrate and potassium iodide (b) Lithium sulfate and silver acetate (c) Sodium chloride and ammonium sulfate
What does it mean when the label (aq) is attached to the formula for an ionic compound?
The ______________ ionic equation for a reaction is obtained by canceling the spectator ions in the ____________ ionic equation.
Write the balanced equation, the complete ionic equation, and the net ionic equation for the reaction between aqueous potassium chloride and lead(II) nitrate that produces lead chloride and potassium nitrate.
Acids produce _____ ions when dissolved in water, and bases produce ______ ions when dissolved in water.
The reaction between an acid and a base is called an acid–base ________________ reaction.
Write the balanced equation for the reaction that occurs when an aqueous solution of carbonic acid, H2CO3, is mixed with an aqueous solution of lithium hydroxide, LiOH.
Of the types of reactions discussed in the chapter, list three ways the reaction Ca(OH)2 + H2SO4 → CaSO4 + 2 H2O can be classified.
If either statement is false, explain why.(a) True or false? It is possible for a reaction to be simultaneously a single-replacement reaction and a combination reaction.(b) True or false? It is possible for a reaction to be simultaneously a double-replacement reaction and a neutralization reaction.
Would you expect a reaction in which all reactants are in the gas phase to go faster, slower, or remain at the same rate if the size of the container is increased while everything else is held constant? Explain.
Nitrous oxide, N2O, is produced when ammonium nitrate, NH4NO3, is heated gently. Water is also produced in the reaction. Write the balanced equation for the reaction.
Write the complete ionic equation and the net ionic equation for the reaction that occurs between aqueous solutions of:(a) Silver nitrate and potassium iodide (b) Lithium sulfate and silver acetate
Write a balanced chemical equation for each reaction:(a) Calcium metal reacts with solid phosphorus, P4, to form calcium phosphide.(b) Sodium metal reacts with water to produce aqueous sodium hydroxide and hydrogen gas.(c) Ammonium nitrate powder explodes to form nitrogen gas, oxygen gas, and water
Ammonia gas reacts with fluorine gas to form ammonium fluoride and nitrogen gas.(a) Write a balanced chemical equation for this reaction.(b) Draw a picture representing the molecular view of the reactant mixture.(c) Draw a picture representing the molecular view of the product mixture.
One of the following diagrams shows a situation that is incorrect. Which is it and why is it incorrect? (a) CH₂Cl₂ CI- CH₂2+ Cl- (b) MgCl CI- 2+ Mg²+ Cl-
Write the complete ionic equation and net ionic equation for the neutralization reaction between aqueous hydrobromic acid and barium hydroxide.
A student draws the diagram below and includes some reactions to represent the diagram. NaNO3 J + KCI 00 CI- Na+ KNO3(s) NaNO3 (aq) + KCl(aq) → KNO3(s) + NaCl(aq) K+ (aq) + NO3 (aq) →KNO3(s) (a) Which reaction is the net ionic reaction? (b) Something is wrong with what the student wrote or
Using molecular formulas, write a balanced equation for the following gas-phase reaction. Then translate the balanced reaction into an English sentence. H" H H + Cl-Cl H H H Cl +H-Cl Cl
How would you classify the molecule in the left beaker? HC OH н+ || HC 0
In the chapter, we saw the combustion reaction for methane. This was actually a complete combustion reaction because carbon ended up as carbon dioxide. If the same reaction is carried out where the oxygen supply is limited, incomplete combustion takes place, yielding toxic carbon monoxide, CO,
Pb(NO3)2 (lead (II) nitrate), upon sufficient heating, turns into PbO (lead (II) oxide), oxygen gas, and nitrogen dioxide gas. Write a balanced equation for this reaction, and classify the reaction type.
Simple soaps, like sodium laurate, NaC12H22O2, are ionic compounds with small cations and large covalent anions. These soaps are somewhat soluble in water but form a soap scum if the water is “hard,” which means it contains calcium ions Ca2+ or magnesium ions, Mg2+ . Write a net ionic equation
Ammonia, NH3, is a gas, but it is very soluble in water, so when you bubble ammonia gas into water you produce an aqueous solution of ammonia. Interestingly, this solution is basic (hydroxide ions are formed). Postulate a reaction that occurs between ammonia and water to make the solution basic,
When you strike a match, trace amounts of white phosphorus (P4) are converted into an oxide of phosphorus, P4O10. This conversion releases sufficient heat to ignite the match head. Write a balanced reaction for this conversion, and classify the reaction type(s).
Barium ions are extremely toxic to most living things, especially humans. And yet, despite its toxicity, barium sulfate cocktails are often given to patients undergoing a CAT scan because barium readily absorbs X-rays and can therefore serve as a contrast medium which helps in the imaging of
Starting from 1,3-butadiene, how would you prepare 2,3-dibromobutane?
Bromine (Br2) can be made to add across a C = C double bond. Knowing this, postulate an alternative synthesis to the one you proposed in problem 8.144 for the preparation of 2,3-dibromobutane.Data from Problem 8.144Starting from 1,3-butadiene, how would you prepare 2,3-dibromobutane?
For the reaction CH4 + O2 → CO2 + H2O,(a) A2 is needed in front of H2O.(b) A 2 is needed in front of O2.(c) A 2 in needed in front of CH4 and CO2.(d) A 2 is needed in front of O2 and H2O.
We can define movie agents by the action they perform. A movie agent is someone who gets you a job starring in a movie. Discuss how you would define an oxidizing agent and a reducing agent in terms of an action they perform. Then suppose you wanted to rob an electron bank. Would you hire a reducing
Using the oxidation-state method of electron bookkeeping, determine how many electrons each atom owns in NH2F.
Voltage is:(a) The same as electricity.(b) The force or “push” behind the electrons flowing through a wire.(c) The flow of electrons in a wire.(d) The amount of electrons that flow through a wire per unit time.
Consider the NH2F molecule from WorkPatch 10.1. Assign an oxidation state to each atom in the molecule.Data from WorkPatch 10.1Using the oxidation-state method of electron bookkeeping, determine how many electrons each atom owns in NH2F.
Two people have a joint savings account together. To simplify their bookkeeping, one person will be in charge and get to spend the money while the other watches. Are they abiding by the oxidation-state formalism or octet-rule formalism? How would they spend their money if they used the other
Assign oxidation states for all the oxygen atoms in ozone, O3, using this rule: When two atoms of the same element (and therefore of identical electronegativity) share electrons, the oxidation-state method of electron bookkeeping divides the electrons equally between the atoms. To do the
Oxidation states are useful for:(a) Determining the charges of atoms in a molecule.(b) Confirming whether the octet rule is obeyed.(c) Deciding if electron transfer is occurring during a chemical reaction.(d) All of the above are correct.
In carbon dioxide, CO2, (a) Assign an oxidation state to each atom in the molecule.(b) How many electrons does the C atom own by oxidation-state electron bookkeeping?(c) How many more or fewer valence electrons are assigned to the C atom here than are present in a free C atom?(d) Is it correct or
Suppose a chlorine atom in a compound has an oxidation state of –1.(a) Is the number of valence electrons assigned to this atom by oxidation state bookkeeping more or fewer than the number of valence electrons in a free chlorine atom?(b) How many more or fewer?(c) In order for a chlorine atom in
When electron bookkeeping by the oxidation-state method, it is true that:(a) The most electronegative element in a bond “owns” the shared electrons.(b) Each atom “owns” half of the shared electrons in a bond between identical elements.(c) Lone pairs are completely owned by the atom they are
In methane, CH4,(a) Assign an oxidation state to each atom in the molecule.(b) How many electrons does the C atom own by oxidation-state electron bookkeeping?(c) How many more or fewer valence electrons are assigned to the C atom here than are present in a free C atom?
Consider the chlorate ion, ClO3–, in which all three oxygen atoms are bound to a central chlorine atom. The oxidation state of the Cl atom in this ion is not –1.(a) Why doesn’t the halide rule apply for the chlorate ion?(b) What is the oxidation state of the Cl atom in chlorate?
Using this dot diagram for acetic acid, assign each atom an oxidation number. Η I-O-I H=C=C Η :O: :0 Η
In chloroform, CHCl3, (a) Assign an oxidation state to each atom in the molecule.(b) How many electrons does the C atom own by oxidation-state electron bookkeeping?(c) How many more or fewer valence electrons are assigned to the C atom here than are present in a free C atom?(d) Is it correct or
According to the shortcut rules for assigning oxidation states:(a) Halide atoms usually have a zero oxidation state.(b) Oxygen atoms usually have a +2 oxidation state.(c) The sum of all the oxidation states must be zero for molecules and ions.(d) The sum of all the oxidation states must equal the
Use the shortcut rules to assign oxidation states to all atoms.COCl2 (oxygen and chlorine bonded to the central carbon)
Step 1. Use Rules 1–7 to assign oxidation states to the atoms and ions in the reactionZn + Cu2+ → Zn2+ + CuStep 2. Now answer the following questions:(a) Is this a redox reaction? How can you tell?(b) If so, what was oxidized?(c) If so, what was reduced?(d) If so, what was the oxidizing
The way to recognize an electron transfer reaction from a balanced chemical equation is:(a) To draw a dot diagram of every reactant and product and see that the octet rule is not obeyed for some atoms.(b) To assign oxidation states to every atom and see if they always add to give the charge of the
Design and label a battery based on the redox reaction between magnesium metal and silver ions:Does your battery show electrons flowing from the Mg electrode to the Ag electrode? It should! Mg + 2 Agt → Mg²+ + 2 Ag
Use the shortcut rules to assign oxidation states to all atoms.MgBr2
Which of the following is true?(a) Oxidation is the gain of electrons.(b) The reducing agent loses electrons and is itself oxidized.(c) Reduction is the loss of electrons.(d) The oxidizing agent loses electrons and is itself reduced.(e) All the statements are true.
Return to the drawing of the battery you made in WorkPatch 10.7 and add the labels, cathode, +, and anode, –.Data from WorkPatch 10.7Design and label a battery based on the redox reaction between magnesium metal and silver ions:Does your battery show electrons flowing from the Mg electrode to the
Use the shortcut rules to assign oxidation states to all atoms.Fe2O3
In a battery:(a) Oxidation occurs at the anode.(b) Reduction occurs at the anode.(c) Oxidation occurs at the cathode.(d) Electrons flow from what gets reduced to what gets oxidized.
Use the shortcut rules to assign oxidation states to all atoms.HClO (Cl and O bonded to each other)
Multiple choice: In general, which way do electrons flow in a battery?(a) From what gets oxidized to what gets reduced.(b) From what gets reduced to what gets oxidized.Explain how you made your choice.
The EMF series is useful for:(a) Determining oxidation states.(b) Determining which way the electrons will flow in a battery.(c) Balancing electron transfer reactions.(d) Determining if a salt bridge is required.
Use the shortcut rules to assign oxidation states to all atoms.CO32–

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