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Chemistry The Central Science 12th edition Theodore Brown, Eugene LeMay, Bruce Bursten, Catherine Murphy, Patrick Woodward - Solutions

Gold is one of the few metals that can be obtained by panning, where a simple pan is used to separate gold from other deposits found in or near a stream bed. What two properties of gold make it possible to find gold, but not metals like copper, silver, lead, and aluminum, by panning?
The accompanying photo shows the reaction between a solution of Cd(NO3)2 and one of Na2S.What is the identity of the precipitate? What ions remain in solution? Write the net ionic equation for the reaction.
Suppose you have a solution that might contain any or all of the following cations: Ni2+, Ag+, Sr2+, and Mn2+. Addition of HCl solution causes a precipitate to form. After filtering off the precipitate, H2SO4 solution is added to the resulting solution and another precipitate forms. This is
You choose to investigate some of the solubility guidelines for two ions not listed in Table 4.1, the chromate ion (CrO42-) and the oxalate ion (C2O42-). You are given 0.01 M solutions (A, B, C, D) of four water-soluble salts: When these solutions are mixed, the following observations are
Antacids are often used to relieve pain and promote healing in the treatment of mild ulcers. Write balanced net ionic equations for the reactions between the HCl(aq) in the stomach and each of the following substances used in various antacids: (a) Al(OH)3(s) (b) Mg(OH)2(s) (c) MgCO3(s) (d)
The commercial production of nitric acid involves the following chemical reactions:(a) Which of these reactions are redox reactions?(b) In each redox reaction identify the element undergoing oxidation and the element undergoing reduction.
Consider the following reagents: zinc, copper, mercury (density 13.6 g/mL), silver nitrate solution, nitric acid solution. (a) Given a 500-mL Erlenmeyer flask and a balloon can you combine two or more of the foregoing reagents to initiate a chemical reaction that will inflate the balloon? Write a
Lanthanum metal forms cations with a charge of 3+. Consider the following observations about the chemistry of lanthanum: When lanthanum metal is exposed to air, a white solid (compound A) is formed that contains lanthanum and one other element. When lanthanum metal is added to water, gas bubbles
A 35.0-mL sample of 1.00 M KBr and a 60.0-mL sample of 0.600 M KBr are mixed. The solution is then heated to evaporate water until the total volume is 50.0 mL. What is the molarity of the KBr in the final solution?
We can draw an analogy between the attractions of an electron to a nucleus and seeing a light bulb-in essence, the more nuclear charge the electron "sees," the greater the attraction.(a) Within this analogy, discuss how the screening by core electrons is analogous to putting a frosted-glass
(a) Moseley's experiments on X-rays emitted from atoms led to the concept of atomic numbers. Where exactly do these X-rays come from? Draw an energy-level diagram to explain. (b) Why are chemical and physical properties of the elements more closely related to atomic number than they are to atomic
The elements of group 4A-carbon, silicon, germanium, tin, and lead-go from nonmetal through metalloid to metal as we go down the column. (a) Predict the order of melting temperature from highest to lowest in this group and justify your logic. (b) Using the CRC Hand book of Chemistry and Physics or
Zinc in its 2+ oxidation state is an essential metal ion for life.Zn2+ is found bound to many proteins that are involved in biological processes, but unfortunately Zn2+ is hard to detect by common chemical methods. Therefore, scientists who are interested in studying Zn2+-containing proteins will
A historian discovers a nineteenth-century notebook in which some observations, dated 1822, were recorded on a substance thought to be a new element. Here are some of the data recorded in the notebook: "Ductile, silver-white, metallic looking. Softer than lead. Unaffected by water, Stable in air
In April 2010, a research team reported that they had made Element 117. The report has yet to be confirmed. Write out Element 117's ground-state electron configuration, and estimate values for its first ionization energy, electron affinity, atomic size, and common oxidation state based on its
We will see in Chapter 12 that semiconductors are materials that conduct electricity better than nonmetals but not as well as metals. The only two elements in the periodic table that are technologically useful semiconductors are silicon and germanium. Integrated circuits in computer chips today are
Moseley established the concept of atomic number by studying X-rays emitted by the elements. The X-rays emitted by some of the elements have the following wavelengths: Element Wavelength (A) Ne .............................. 14.610 Ca ................................ 3.358 Zn
(a) Write the electron configuration for Li, and estimate the effective nuclear charge experienced by the valence electron.(b) The energy of an electron in a one-electron atom or ion equalsWhere Z is the nuclear charge and n is the principal quantum number of the electron. Estimate the first
One way to measure ionization energies is ultraviolet photoelectron spectroscopy (UPS, or just PES), a technique based on the photoelectric effect. In PES, monochromatic light is directed onto a sample, causing electrons to be emitted. The kinetic energy of the emitted electrons is measured. The
Mercury in the environment can exist in oxidation states 0, +1, and +2. One major question in environmental chemistry research is how to best measure the oxidation state of mercury in natural systems; this is made more complicated by the fact that mercury can be reduced or oxidized on surfaces
Consider the gas-phase transfer of an electron from a sodium atom to a chlorine atom: Na (g) + Cl (g) → Na+ (g) + Cl- (g) (a) Write this reaction as the sum of two reactions, one that relates to ionization energy and one that relates to an electron affinity. (b) Use the result from part (a), data
(a) What is meant by the term effective nuclear charge? (b) How does the effective nuclear charge experienced by the valence electrons of an atom vary going from left to right across a period of the periodic table?
When magnesium metal is burned in air (Figure 3.6), two products are produced. One is magnesium oxide, MgO. The other is the product of the reaction of Mg with molecular nitrogen, magnesium nitride. When water is added to magnesium nitride, it reacts to form magnesium oxide and ammonia gas.(a)
(a) The measured Bi - Br bond length in bismuth tribromide, BiBr3, is 2.63 Å. Based on this value and the data in Figure 7.7, predict the atomic radius of Bi.
(a) How is the concept of effective nuclear charge used to simplify the numerous electron-electron repulsions in a many electron atom? (b) Which experiences a greater effective nuclear charge in a Be atom, the 1s electrons or the 2s electrons? Explain.
Detailed calculations show that the value of Zeff for the outermost electrons in Na and K atoms is 2.51+ and 3.49+, respectively. (a) What value do you estimate for Zeff experienced by the outermost electron in both Na and K by assuming core electrons contribute 1.00 and valence electrons
Detailed calculations show that the value of Zeff for the outermost electrons in Si and Cl atoms is 4.29+ and 6.12+, respectively. (a) What value do you estimate for Zeff experienced by the outermost electron in both Si and Cl by assuming core electrons contribute 1.00 and valence electrons
Which will experience the greater effective nuclear charge, the electrons in the n = 3 shell in Ar or n = 3 the shell in Kr? Which will be closer to the nucleus? Explain.
Arrange the following atoms in order of increasing effective nuclear charge experienced by the electrons in the n = 3 electron shell: K, Mg, P, Rh, and Ti. Explain the basis for your order.
(a) Because an exact outer boundary cannot be measured or even calculated for an atom, how are atomic radii determined? (b) What is the difference between a bonding radius and a nonbonding radius? (c) For a given element, which one is larger? (d) If a free atom reacts to become part of a
(a) Why does the quantum mechanical description of many electron atoms make it difficult to define a precise atomic radius? (b) When non-bonded atoms come up against one another, what determines how closely the nuclear centers can approach?
Tungsten has the highest melting point of any metal in the periodic table: 3422 °C. The distance between W atoms in tungsten metal is 2.74 Å. (a) What is the atomic radius of a tungsten atom in this environment? (This radius is called the metallic radius.) (b) If you put tungsten metal under
If you look up the radius of the sulfur atom in this book, you will find just one number: 1.02 Ã…. However, if you look deeper into the chemical literature, you can find another number for the radius of a sulfur atom: the nonbonding radius of 1.80 Ã…. This is a very large
Based on the radii presented in Figure 7.6, predict the distance between Si atoms in solid silicon. How does this compare to the distance between the C atoms in diamond, which has the same structure as solid silicon?
How do the sizes of atoms change as we move? (a) From left to right across a row in the periodic table, (b) From top to bottom in a group in the periodic table (c) Arrange the following atoms in order of increasing atomic radius: O, Si, I, Ge.
(a) Among the nonmetallic elements, the change in atomic radius in moving one place left or right in a row is smaller than the change in moving one row up or down. Explain these observations. (b) Arrange the following atoms in order of increasing atomic radius: Si, Al, Ge, Ga.
Using only the periodic table, arrange each set of atoms in order from largest to smallest: (a) K, Li, Cs; (b) Pb, Sn, Si; (c) F, O, N
Using only the periodic table, arrange each set of atoms in order of increasing radius: (a) Ba, Ca,Na; (b) Sn, Sb, As; (c) Al, Be, Si.
(a) Cations are larger than their corresponding neutral atoms. (b) Li+ is smaller than Li. (c) Cl- is bigger than I-. True or False:
Explain the following variations in atomic or ionic radii: a. I- > I > I+ b. Ca2+ > Mg2+ > Be2+ c. Fe > Fe2+ > Fe3+
In the reactionWhich sphere represents a metal and which represents a nonmetal? Explain your answer.
Consider the A2X4 molecule depicted here, where A and X are elements. The A-A bond length in this molecule is d1, and the four bond lengths are each d2.(a) In terms of d1 and d2, how could you define the bonding atomic radii of atoms A and X?(b) In terms of d1 and d2, what would you predict for the
Some ions do not have a corresponding neutral atom that has the same electron configuration. For each of the following ions, identify the neutral atom that has the same number of electrons and determine if this atom has the same electron configuration. If such an atom does not exist, explain
Consider the iso-electronic ions F- and Na+. (a) Which ion is smaller? (b) Using Equation 7.1 and assuming that core electrons contribute 1.00 and valence electrons contribute 0.00 to the screening constant, S, calculate Zeff for the 2p electrons in both ions. (c) Repeat this calculation using
Consider the iso-electronic ions Cl- and K+. (a) Which ion is smaller? (b) Using Equation 7.1 and assuming that core electrons contribute 1.00 and valence electrons contribute nothing to the screening constant, S, calculate Zeff for these two ions. (c) Repeat this calculation using Slater's rules
Consider S, Cl, and K and their most common ions. (a) List the atoms in order of increasing size. (b) List the ions in order of increasing size. (c) Explain any differences in the orders of the atomic and ionic sizes.
For each of the following sets of atoms and ions, arrange the members in order of increasing size: (a). Se2-, Te2-, Se (b). Co3+, F2+, Fe3+ (c). Ca, Ti4+, Sc3+ (d). Be2+, Na+, Ne
In the ionic compounds LiF, NaCl, KBr, and RbI, the measured cation-anion distances are 2.01 Ã… (Li-F), 2.82 Ã… (Na-Cl), 3.30 Ã… (K-Br), and 3.67 Ã… (Rb-I), respectively.(a) Predict the cation-anion distance using the values of ionic radii given in
Write equations that show the processes that describe the first, second, and third ionization energies of an aluminum atom. Which process would require the least amount of energy?
Make a simple sketch of the shape of the main part of the periodic table, as shown.(a) Ignoring H and He, write a single straight arrow from the element with the smallest bonding atomic radius to the element with the largest.(b) Ignoring H and He, write a single straight arrow from the element with
(a)Why does Li have larger first ionization energy than Na? (b) The difference between the third and fourth ionization energies of scandium is much larger than the difference between the third and fourth ionization energies of titanium. Why? (c) Why does Li have much larger second ionization
(a) What is the general relationship between the size of an atom and its first ionization energy? (b) Which element in the periodic table has the largest ionization energy? Which has the smallest?
(a) What is the trend in first ionization energies as one proceeds down the group 7A elements? Explain how this trend relates to the variation in atomic radii. (b) What is the trend in first ionization energies as one move across the fourth period from K to Kr? How does this trend compare with the
For each of the following pairs, indicate which element has the smaller first ionization energy: (a) Ti, Ba; (b) Ag, Cu; (c) Ge, Cl; (d) Pb, Sb. (In each case use electron configuration and effective nuclear charge to explain your answer)
Write the electron configurations for the following ions: (a) Fe2+, (b) Hg2+, (c) Mn2+, (d) Pt2+, (e) P3-.
Write electron configurations for the following ions, and determine which have noble-gas configurations: (a). Cr3+ (b). N3- (c). Sc3+ (d). Cu2+ (e). Tl+ (f). Au+
Find three examples of ions in the periodic table that have an electron configuration of nd8 (n = 3, 4, 5...).
In the chemical process called electron transfer, an electron is transferred from one atom or molecule to another. (We will talk about electron transfer extensively in Chapter 20.) A simple electron transfer reaction is A(g) + A(g) → A+(g) + A-(g) In terms of the ionization energy and electron
Find three atoms in the periodic table whose ions have an electron configuration of nd6 (n = 3, 4, 5...).
The first ionization energy and electron affinity of Ar are both positive values. (a) What is the significance of the positive value in each case? (b) What are the units of electron affinity?
If the electron affinity for an element is a negative number, does it mean that the anion of the element is more stable than the neutral atom? Explain.
Although the electron affinity of bromine is a negative quantity, it is positive for Kr. Use the electron configurations of the two elements to explain the difference.
What is the relationship between the ionization energy of an anion with a 1-charge such as F- and the electron affinity of the neutral atom, F?
Consider the first ionization energy of neon and the electron affinity of fluorine. (a) Write equations, including electron configurations, for each process. (b) These two quantities will have opposite signs. Which will be positive, and which will be negative? (c) Would you expect the magnitudes
Write an equation for the process that corresponds to the electron affinity of the ion. Also write the electron configurations of the species involved. What is the magnitude of the energy change in the process?
It is possible to define metallic character as we do in this book and base it on the reactivity of the element and the ease with which it loses electrons. Alternatively, one could measure how well electricity is conducted by each of the elements to determine how "metallic" the elements are. On the
Discussing this chapter, a classmate says, "An element that commonly forms a cation is a metal." Do you agree or disagree? Explain your answer.
An element X reacts with F2 (g) to form the molecular product shown here(a) Write a balanced equation for this reaction (do not worry about the phases for X and the product).(b) Do you think that X is a metal or nonmetal? Explain.
Predict whether each of the following oxides is ionic or molecular: SnO2, Al2O3, CO2, Li2O, Fe2O3, H2O Explain the reasons for your choices.
Some metal oxides, such as Sc2O3, do not react with pure water, but they do react when the solution becomes either acidic or basic. Do you expect Sc2O3 to react when the solution becomes acidic or when it becomes basic? Write a balanced chemical equation to support your answer.
(a) What is meant by the terms acidic oxide and basic oxide? (b) How can we predict whether an oxide will be acidic or basic based on its composition?
Chlorine reacts with oxygen to form Cl2O7. (a) What is the name of this product (see Table 2.6)? (b) Write a balanced equation for the formation of Cl2O7 (l) from the elements. (c) Under usual conditions, Cl2O7 is a colorless liquid with a boiling point of 81oC. Is this boiling point expected or
An element X reacts with oxygen to form XO2 and with chlorine to form XCl4. XO2 is a white solid that melts at high temperatures (above 1000oC). Under usual conditions, XCl4 is a colorless liquid with a boiling point of 58oC. (a) XCl4 reacts with water to form XO2 and another product. What is the
Write balanced equations for the following reactions: (a) Barium oxide with water, (b) Iron (II) oxide with perchloric acid, (c) Sulfur trioxide with water, (d) Carbon dioxide with aqueous sodium hydroxide.
Write balanced equations for the following reactions: (a) Potassium oxide with water, (b) Diphosphorus trioxide with water, (c) Chromium (III) oxide with dilute hydrochloric acid, (d) Selenium dioxide with aqueous potassium hydroxide.
Does the reactivity of a metal correlate with its first ionization energy? Explain.
Explain the structure of the periodic table-two columns on the left, a block of ten for the transition metals, a block of six on the right, and a pair of 14-member rows below, with reference to the orbital's we discussed in Chapter 6.
Silver and rubidium both form +1 ions, but silver is far less reactive. Suggest an explanation, taking into account the ground-state electron configurations of these elements and atomic radii.
(a) Why is calcium generally more reactive than magnesium? (b) Why is calcium generally less reactive than potassium?
(a) One of the alkali metals reacts with oxygen to form a solid white substance. When this substance is dissolved in water, the solution gives a positive test for hydrogen peroxide, H2O2. When the solution is tested in a burner flame, a lilac-purple flame is produced. What is the likely identity of
Write a balanced equation for the reaction that occurs in each of the following cases: (a) Potassium metal burns in an atmosphere of chlorine gas. (b) Strontium oxide is added to water. (c) A fresh surface of lithium metal is exposed to oxygen gas. (d) Sodium metal is reacted with molten sulfur.
Write a balanced equation for the reaction that occurs in each of the following cases: (a) Cesium is added to water. (b) Strontium is added to water. (c) Sodium reacts with oxygen. (d) Calcium reacts with iodine.
(a) As described in Section 7.7, the alkali metals react with hydrogen to form hydrides and react with halogens-for example, fluorine-to form halides. Compare the roles of hydrogen and the halogen in these reactions. How are the forms of hydrogen and halogen in the products alike? (b) Write
The interior of the planets Jupiter and Saturn are believed to contain metallic hydrogen: hydrogen that is put under such tremendous pressure that it no longer exists as H2 molecules, but instead exists as an extended metallic solid. Predict what properties metallic hydrogen might have compared to
Compare the elements bromine and chlorine with respect to the following properties: (a) Electron configuration, (b) Most common ionic charge, (c) First ionization energy, (d) Reactivity toward water, (e) Electron affinity, (f) Atomic radius. Account for the differences between the two elements.
Little is known about the properties of astatine, At, because of its rarity and high radioactivity. Nevertheless, it is possible for us to make many predictions about its properties.(a) Do you expect the element to be a gas, liquid, or solid at room temperature? Explain. (b) Would you expect At to
Until the early 1960s the group 8A elements were called the inert gases; before that they were called the rare gases. The term rare gases were dropped after it was discovered that argon accounts for roughly 1% of Earth's atmosphere. (a) Why was the term inert gases dropped? (b) What discovery
(a) Why does xenon react with fluorine, whereas neon does not? (b) Using reference sources such as the CRC Handbook of Chemistry and Physics or online sources look up the bond lengths of Xe - F bonds in several molecules. How do these numbers compare to the radii of the elements?
Write a balanced equation for the reaction that occurs in each of the following cases: (a) Ozone decomposes to di oxygen. (b) Xenon reacts with fluorine. (Write three different equations.) (c) Sulfur reacts with hydrogen gas. (d) Fluorine reacts with water.
Write a balanced equation for the reaction that occurs in each of the following cases: (a) Chlorine reacts with water. (b) Barium metal is heated in an atmosphere of hydrogen gas. (c) Lithium reacts with sulfur. (d) Fluorine reacts with magnesium metal.
Consider the stable elements through lead (Z = 82). In how many instances are the atomic weights of the elements in the reverse order relative to the atomic numbers of the elements? What is the explanation for these cases?
We saw in Chapter 6 that the probability of finding an electron in three-dimensional space depends on what orbital it is in. Look back at Figures 6.19 and 6.22, which show the radial probability distribution functions for the s orbitals and contour plots of the 2p orbitals, respectively.(a) Which
(a) If the core electrons were totally effective at screening the valence electrons and the valence electrons provided no screening for each other, what would be the effective nuclear charge acting on the 3s and 3p valence electrons in P? (b) Repeat these calculations using Slater's rules. (c)
The size of an atomic nucleus is on the order of 10-15 m. If two protons were able to make a bond, what would you predict the bond length to be?
As we move across a period of the periodic table, why do the sizes of the transition elements change more gradually than those of the representative elements?
In the series of group 5A hydrides, of general formula MH3, the measured bond distances are P - H, 1.419 Ã…; As - H, 1.519 Ã…; , 1.707 Ã….(a) Compare these values with those estimated by use of the atomic radii in Figure 7.6.(b) Explain the steady increase in M -
Elements in group 7A in the periodic table are the halogens; elements in group 6A are called the chalcogens. (a) What is the most common oxidation state of the chalcogens compared to the halogens? Can you suggest an explanation for the difference? (b) For each of the following periodic properties,
You might have expected that the elements would have been discovered in order of their relative abundance in the Earth's crust (Figure 1.6), but this is not the case. Suggest a general reason.
Note from the following table that the increase in atomic radius in moving from Zr to Hf is smaller than in moving from Y to La. Suggest an explanation for this effect.
(a) Which ion is smaller, Co3+ or Co4+? (b) In a lithium ion battery that is discharging to power a device, for every Li+ that inserts into the lithium cobalt oxide electrode, a Co4+ ion must be reduced to a Co3+ ion in order to balance charge. Using the CRC Handbook of Chemistry and Physics or

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