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introductory chemistry atoms first

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

If marriage is truly supposed to be “till death do us part,” what metal does the EMF series indicate should be used for wedding rings? Explain your answer.
The corrosion of metals:(a) Is more likely the more active a metal is.(b) Involves a redox reaction in which the metal is oxidized.(c) Involves an electron transfer reaction in which the metal is oxidized.(d) All of the above statements are correct.
Use the shortcut rules to assign oxidation states to all atoms.Cu2+
Indicate whether each reaction is a redox reaction. If it is, which atom gets oxidized and which atom gets reduced? Consult the shortcut rules.P4 + 6Br2 → 4PBr3
Indicate whether each reaction is a redox reaction. If it is, which atom gets oxidized and which atom gets reduced? Consult the shortcut rules.4Fe + 3O2 → 2Fe2O3
Indicate whether each reaction is a redox reaction. If it is, which atom gets oxidized and which atom gets reduced? Consult the shortcut rules.Ca + 2H+ → Ca2+ +H2
Indicate whether each reaction is a redox reaction. If it is, which atom gets oxidized and which atom gets reduced? Consult the shortcut rules.2NaBr + MgO → MgBr2 + Na2O
For each redox reaction, indicate which substance is the oxidizing agent and which is the reducing agent.P4 + 6 Br2 → 4 PBr3
For each redox reaction, indicate which substance is the oxidizing agent and which is the reducing agent.4Fe + 3O2 → 2Fe2O3
Construct a battery in which the redox reaction is:To answer, draw a battery similar to the one you drew for WorkPatch 10.7, label which way the electrons flow, and label cathode, +, and anode, –.Data from WorkPatch 10.7Design and label a battery based on the redox reaction between magnesium
For each redox reaction, indicate which substance is the oxidizing agent and which is the reducing agent.Ca + 2H+ → Ca2+ +H2
For the nickel–lead battery of Practice Problem 10.18,(a) What is the oxidizing agent?(b) What is the reducing agent?(c) Which electrode gets larger over time?(d) Which electrode is eaten away over time?Data from Problem 10.18Construct a battery in which the redox reaction is:To answer, draw a
A battery is constructed from iron, Fe, and silver, Ag, by dipping a strip of each metal into a solution of its ions (Fe3 + and Ag+, respectively). As the battery operates, the Fe3+ concentration increases while the Ag+ concentration decreases.(a) What is getting oxidized?(b) What is getting
What will happen if a piece of Zn metal is placed in a solution of Al3+ ions?
Which of the following reactions is spontaneous? 2+ 3 Zn²+ + 2 Al-3 Zn + 2 A1³+ (a) (b) 3 Zn + 2 2+ Al³+3 Zn²+ + 2 Al
Using a diagram, show how you would construct a zinc–aluminum battery. Label the cathode, the anode, the + electrode, and the – electrode. Indicate the direction of electron flow, and identify the beaker in which oxidation occurs and the beaker in which reduction occurs.
Consider a battery made from lead, Pb, and copper, Cu, along with Pb2+ ions and Cu2+ ions. In such a battery, what is the oxidizing agent, and what is the reducing agent?
How is electricity similar to water flowing in a hose?
How is electricity mechanically produced in a power plant?
What is an electron-transfer reaction?
Why did chemists find it necessary to invent oxidation states?
What do we mean by electron bookkeeping?
Which method of assigning shared electrons is correct—the double-counting method of the octet rule or the oxidation-state method?
When assigning an oxidation state to an atom, why do we need to know how many valence electrons are present on a free atom of that element?
According to the oxidation-state method of electron bookkeeping, which atom is assigned the shared electrons in a bond between two atoms?
Draw a Lewis dot diagram for NF2H, and use the oxidation-state method of electron bookkeeping to determine how many electrons each atom should be assigned.
Draw a Lewis dot diagram for H2O2 (hydrogen peroxide), and use the oxidation-state method of electron bookkeeping to determine how many electrons each atom should be assigned.
Draw a Lewis dot diagram for NO3–, and use the oxidation-state method of electron bookkeeping to determine how many electrons each atom should be assigned.
Assign an oxidation state to every atom in the molecules in Problems 10.33–10.35.Data from Problem 10.33Draw a Lewis dot diagram for NF2H, and use the oxidation-state method of electron bookkeeping to determine how many electrons each atom should be assigned.Data from Problem 10.34Draw a Lewis
Consider the following molecules. Without using the shortcut rules, determine the oxidation state for each atom in the molecules and show how you calculated it.(a) H2 (b) O2 (c) Cl2 (d) IF
What does the answer to Problem 10.37 teach you?Data from Problem 10.37Consider the following molecules. Without using the shortcut rules, determine the oxidation state for each atom in the molecules and show how you calculated it.H2 O2 Cl2 IF
What must always be true when you add up all the oxidation states for the atoms in a molecule?
Suppose an atom has an oxidation state of +3.(a) Would more or fewer electrons be assigned to this atom by oxidation-state bookkeeping than are present on a free atom of that element?(b) How many more or fewer?
Suppose an atom has an oxidation state of –2.(a) Would more or fewer electrons be assigned to this atom by oxidation-state bookkeeping than are present on a free atom of that element?(b) How many more or fewer?
Suppose the shortcut rules can determine the oxidation state of every atom in a compound except one. How can you find the oxidation state of the remaining atom?
Suppose the exothermic reactionhas come to equilibrium. Which of the following are true?(a) Adding O2(g) will shift the reaction to the left.(b) Cooling the reaction will shift it to the right.(c) Cooling the reaction will shift it to the left.(d) All of the above are true. (8) 10) = (8)' 10 2 OF
Write full nuclear reactions for Practice Problems 16.10 and 16.11.Data from Practice Problems 16.10The magnesium isotope 2512Mg is the daughter isotope created when a radioactive parent isotope undergoes electron capture. What is the full symbol for the parent isotope?Data from Practice Problems
What can we say about the n/p ratios of nuclei that lie in the light brown band of stability below the dark brown center region?
In principle, which of Problems 16.56, 16.59, and 16.62 could occur along with gamma-ray emission?Data from Problem 16.56The tantalum isotope 18673Ta is radioactive and decays by converting a neutron to a proton.Where is this atom likely to lie in the band of stability?Write a nuclear reaction for
What do we mean by the binding energy of an atom, and how does it compare to the energy that binds atoms to one another in a covalent bond?
Of all of the elements and all of their isotopes, which would take the most energy to convert its nucleus into isolated nucleons? Explain why.
What in Einstein’s energy equation ensures that a tiny mass defect results in a tremendous amount of energy? Explain.
Use the shortcut rules to assign an oxidation state to each atom in:(a) PCl3(b) H2S(c) MnO4–(d) HNO3(e) HCOOH(f) S2O32–
Use the shortcut rules to assign an oxidation state to each atom in:(a) CO(b) CH2Cl2(c) HCOO–(d) PtCl62–
Use the shortcut rules to assign an oxidation state to each atom in:(a) O2–(b) Li3N(c) MgSO4(d) MnO2
In the upper atmosphere, sunlight can convert oxygen to ozone:Is this a redox reaction? Completely justify your answer. 202-03 +0 Ozone
In the above figure, the water molecules are drawn so that an oxygen atom faces the Na+ ion and a hydrogen atom faces the Cl– ion. Explain why.
Δ(Any quantity) is always defined as (final value of quantity) – (initial value of quantity). Now consider the quantity ΔErxn.(a) For the forward reaction R → P, is ΔErxn = EReactants – EProducts? Explain your answer.(b) According to your answer to (a), what does it mean when ΔErxn for a
Consider the reaction: 2 NO(g) + 2H2(g) → N2(g) + 2 H2O(g) Initial concentrations and rates for this reaction are given in the table below.(a) From the data given, determine the order for each of the reactants, NO and H2, show your reasoning, and write the overall rate law for the reaction.(b)
The reaction of Problem 13.40 is run in the reverse direction (P → R).(a) Is it exothermic or endothermic?(b) Calculate ΔErxn.(c) Is what you just said and calculated for (a) and (b) consistent with the definition of Δ(any quantity) given in Problem 13.41? Explain.Data from Problem 13.40A
What do we mean by an energy-uphill reaction?What do we mean by an energy-downhill reaction? Include reaction-energy profiles with your explanations.
Consider the reactionKinetics studies reveal a first-order rate dependence on the concentration of the (CH3)3C—Br and a zero-order dependence on the concentration of H2O.(a) What happens to the reaction rate as the (CH3)3C—Br concentration is changed? What happens to the reaction rate as the
The equilibrium constant for the reaction N2O2(g) → N2(g) + O2(g) is 0.456 at 322 k. Suppose we put 1.00 mole of N2O2 into a 1.00-L container and heat it to 322 k. At time zero, the concentration of N2O2 would be 1.00 M, and the concentration of products N2 and O2 would both be zero. By the time
Given a reaction vessel with the initial conditions shown on the next page, which set of rate meters best describes the time-zero and equilibrium conditions? Explain why your choice is correct and why the other choices are incorrect. 다 Forward rate D 2 SO₂ + O₂ 2 50₂ Time zero At time
Starting only with reactants, a reaction can be said to have reached equilibrium when:(a) The concentration of reactants no longer decreases.(b) The concentration of products no longer increases.(c) The forward reaction rate equals the reverse reaction rate.(d) All of the above are true when a
Why can we ignore equilibrium for reactions that go to completion?
An equilibrium that lies far to the left means that at equilibrium:(a) There will be mostly products present.(b) The reaction goes to completion.(c) The forward and reverse reaction rates will not be equal.(d) There will be mostly reactants present.
Rearrange the equation kf[A] = kr[B] algebraically to solve for the ratio kf/kr.
A reaction starting with just reactants will eventually reach equilibrium because:(a) The rates of the forward and reverse reactions will remain constant as the reaction proceeds.(b) The forward reaction will slow and the reverse reaction will speed until their rates are equal.(c) The forward
Calculate the value of Keq for the NO reaction, given the following data: Start Reactants N₂(g) + O₂(g) 2 NO(g) -1.000 mol N₂ -1.000 mol O₂ Product Box volume 1.0 L 2027 °C At equilibrium -0.980 mol N₂ -0.980 mol O₂ 0.040 mol NO- Reactants Product
Consider the nuclear process shown below.(a) Identify the atoms on the left (the reactant atoms).(b) Is this fission, fusion or β decay? Explain.(c) Would this process take a little or a lot of energy to occur? Explain why.(d) Would this overall process be exothermic or endothermic? Explain
(a) What does the plot say about the stability of the nucleus of the iron isotope 5626Fe?(b) What is the total binding energy for the 5626Fe nucleus in kilojoules per mole of atoms?
The radioactive isotope of iodine 12353I is used to treat thyroid disease. Suppose a patient is given a 30 mg dose. How much will be left in the patient after 39.3 h? (See Table 16.1.) Table 16.1 Some Radioactive Isotopes Radioactive isotope Element Iodine Phosphorus Carbon Uranium 1331 P ¹4
The nuclear process which constantly produces 14C in the Earth’s atmosphere is illustrated below, along with the mechanism of its incorporation into the food chain. What is the major assumption upon which carbon dating is based. Discuss what could have happened in the past to make this assumption
All atoms have a mass defect because:(a) We can’t weigh single atoms accurately.(b) An atom weighs more than the sum of its parts.(c) An atom weighs less than the sum of its parts.(d) Of the Heisenberg Uncertainty Principle.
The nuclear binding energy between protons and neutrons in a nucleus is:(a) A repulsive force that can cause nuclear explosions.(b) A weak attractive force.(c) Comparable to the attractive force between atoms in a covalent bond.(d) Many millions of times stronger that the attractive forces between
Consider 20782Pb, which has a mass number of 207.(a) How many nucleons are in the 20782Pb nucleus?(b) Reading the plot of binding energy per mole of nucleon as best you can, calculate how many kilojoules it would take to remove 3 moles of protons from the atoms in 1 mole of lead-207.
What do we call atoms in which the nuclei undergo spontaneous change?
Three isotopes of carbon have mass numbers 12, 13, and 14.(a) Write the full atomic symbols for these three isotopes, including mass number and atomic number.(b) For each isotope, indicate the number of neutrons and protons in the nucleus.(c) For each isotope, determine the total number of nucleons
To be radioactive, an atom must possess a nucleus that:(a) Undergoes spontaneous change.(b) Emits radio waves.(c) Has an unequal number of protons and neutrons.(d) Has at least one electron in its nucleus.
Calculate the binding energy per mole (in kilojoules) for 42He.
The neutron-to-proton ratio for stable nuclei:(a) Can only be equal to 1.(b) Increases with increasing number of protons.(c) Decreases with increasing number of protons.(d) Means there can only be one stable isotope per element.
In an n/p plot, the band of stability curves up above the n/p = 1 line. Explain why.
Demonstrate that you understand the full symbols for the neutron and proton by answering the following questions.(a) Why do neutrons and protons have the same mass number?(b) Why is the atomic number for the neutron 0?(c) Why is the atomic number for the proton 1?
When a nucleus emits an alpha particle:(a) The atomic number decreases by 2.(b) The mass number decreases by 4.(c) The atom changes elemental identity equal to two steps to the left in the periodic table.(d) All of the above statements are true.
What would the answer to WorkPatch 16.6 be if there were another beta emission?WorkPatch 16.6Balance this nuclear reaction and predict the product: 2Pb→? + -e 214 82 B particle
Each of the following symbols has one mistake in it. Identify the mistake, explain why it is a mistake, and fix it: on op le
When a nucleus emits a beta particle:(a) The atomic number increases by 1.(b) The atomic number decreases by 1.(c) The atom changes elemental identity equal to one step to the left in the periodic table.(d) It ejects a particle equal to a +2 helium atom.
Balance this nuclear reaction and predict the product: 21Pb→? + je 0 82- B particle.
Suppose 3514Si undergoes beta emission. Write a nuclear reaction for this spontaneous change.
When a nucleus emits a positron:(a) The atomic number increases by 1.(b) The atomic number decreases by 1.(c) The nucleus ejects an electron.(d) The entire atom transforms into antimatter.
Balance this nuclear reaction and predict the product: 20 Po→? + He 209p 84 a particle
Suppose 4020Ca is the product of a beta-emission nuclear reaction. What was theparent isotope?
Electron capture is a process whereby an atom:(a) Ejects a particle of antimatter.(b) Increases its atomic number by 1.(c) Decreases its atomic number by 1.(d) Absorbs a gamma ray.
Replace each question mark with the correct number and sign: Alpha emission (a) Beta emission (B) Positron emission (3¹) Electron capture (-je) Particle He je tie -je Change in atomic number -2 ? ? ? Change in mass number ? ? ? Change in number of neutrons -2 ? ? ?
The fluorine isotope 179F undergoes positron emission.(a) Write a nuclear reaction for this emission.(b) Where on the band of stability would you expect to find 179F?
In the nuclear fusion that occurs in the Sun:(a) Heavy atoms are split into lighter atoms.(b) Energy is produced due to the conversion of mass into energy.(c) Helium atoms are fused to yield hydrogen atoms.(d) Hydrogen atoms are burned.
The argon isotope 3718Ar undergoes electron capture.(a) Write a nuclear reaction for this process.(b) Where on the band of stability would you expect to find 3718Ar?(c) What is the daughter nucleus produced?
What would be wrong with using 146C to determine the age of fossils that are 1 million years old?
The following can be said about gamma rays:(a) They can be emitted along with many different types of radioactive decay.(b) They are very energetic and therefore dangerous forms of electromagnetic radiation.(c) By themselves they cause no change in an atom’s atomic number or mass number upon
The magnesium isotope 2512Mg is the daughter isotope created when a radioactive parent isotope undergoes electron capture. What is the full symbol for the parent isotope?
The third generation of fission of 23592U produces 27 neutrons. How many neutrons would the tenth generation of fission produce?
The magnesium isotope 2512Mg is the daughter isotope created when a radioactive parent isotope undergoes positron emission. What is the full symbol for the parent isotope?
Positron emission moves us one step to the left in the periodic table, and alpha emission moves us two steps to the left. Does this mean that, for a given parent isotope, the daughter isotope resulting from two successive positron emissions is the same as the daughter isotope resulting from one
Starting from 23892U, demonstrate by writing balanced nuclear reactions that the answer to Practice Problem 16.13 is correct.Data from Problem 16.13Positron emission moves us one step to the left in the periodic table, and alpha emission moves us two steps to the left. Does this mean that, for a
If a radioactive element undergoes a single decay process and transforms into an element two spaces away on the periodic table, which decay process must have taken place? Explain why it could not be any other decay process.
If a radioactive element undergoes a single decay process and transforms into an element one step to the right in the periodic table, did a proton turn into a neutron or did a neutron turn into a proton? What do we call this type of decay?
A rock from an asteroid contains 2.57 g of 23892U and 3.83 g of 20682Pb. The molar mass of 20682Pb is 205.974 46 g/mol, the molar mass of 23892U is 238.029 g/mol, and the halflife of 23892U is 4.46 × 109 years. Assume that all the 20682Pb came from the radioactive decay of the 23892U.(a) How many
In part (b) of Practice Problem 16.17, why is the number of 23892U atoms initially present in the rock equal to the sum of the number of 23892U atoms and 20682Pb atoms present in the rock today?Data from Problem 16.17A rock from an asteroid contains 2.57 g of 23892U and 3.83 g of 20682Pb. The molar
Complete this nuclear reaction, and state whether it is fission or fusion. 23 Pu + nSr + ? + 3 n

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