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chemistry a molecular approach

Chemistry A Molecular Approach 5th Edition Nivaldo Tro - Solutions

Write an equation for the precipitation reaction that occurs (if any) when solutions of potassium carbonate and nickel(II) chloride are mixed.
Why do the names of some ionic compounds include the charge of the metal ion while others do not?
Explain how to name binary acids and oxyacids.
Calculate the formula mass of glucose, C6H12O6.
How many helium atoms are there in a helium blimp containing 536 kg of helium?
Scientists at the National Institute for Standards and Technology (NIST) wrote the initials of their agency with 70 individual cobalt atoms (as shown below). Calculate the total mass of these letters in grams.
Calculate the average mass, in grams, of one platinum atom.
A 7.83 g sample of HCN contains 0.290 g of H and 4.06 g of N.Find the mass of carbon in a sample of HCN with a mass of 3.37 g.
The ratio of sulfur to oxygen by mass in SO2 is 1.0:1.0.a. Find the ratio of sulfur to oxygen by mass in SO3.b. Find the ratio of sulfur to oxygen by mass in S2O.
The ratio of oxygen to carbon by mass in carbon monoxide is 1.33:1.00. Find the formula of an oxide of carbon in which the ratio by mass of oxygen to carbon is 2.00:1.00.
The ratio of the mass of a nitrogen atom to the mass of an atom of 12C is 7:6, and the ratio of the mass of nitrogen to oxygen in N2O is 7:4. Find the mass of 1 mol of oxygen atoms.
An a particle, 4He2+, has a mass of 4.00151 amu. Find the value of its charge-to-mass ratio in C/kg.
Use the mass spectrum of lead to estimate the atomic mass of lead. Estimate the mass and percent intensity values from the graph to three significant figures. Intensity % 100%- 50%- 204 206 207 208 Mass (amu)
Naturally occurring iodine has an atomic mass of 126.9045 amu. A 12.3849 g sample of iodine is accidentally contaminated with an additional 1.00070 g of 129I, a synthetic radioisotope of iodine used in the treatment of certain diseases of the thyroid gland. The mass of 129I is 128.9050 amu. Find
Use the mass spectrum of mercury to estimate the atomic mass of mercury. Estimate the masses and percent intensity values from the graph to three significant figures. Intensity % 100% 50%- 196 198 199 200 201 202 204 Mass (amu)
Fill in the blanks to complete the table. Symbol Z A Si 14 S²- 2+ Cu²+ 15 32 Number Number Number of p of e of n 14 14 15 34 16 Charge 2- 2+
Nuclei with the same number of neutrons but different mass numbers are called isotones. Write the symbols of four isotones of 236Th.
Fill in the blanks to complete the table. Symbol Z 8 20 Ca²+ Mg2+ N³- A 25 14 Number of p Number Number of e of n 8 20 13 10 Charge 2- 2+
Neutron stars are composed of solid nuclear matter, primarily neutrons. Assume the radius of a neutron is approximately 1.0 * 10-13 cm. Calculate the density of a neutron. [For a sphere V = (4/3)πr3.] Assuming that a neutron star has the same density as a neutron, calculate the mass (in kg) of a
Carbon-12 contains six protons and six neutrons. The radius of the nucleus is approximately 2.7 fm (femtometers), and the radius of the atom is approximately 70 pm (picometers). Calculate the volume of the nucleus and the volume of the atom.What percentage of the carbon atom’s volume is occupied
A penny has a thickness of approximately 1.0 mm. If you stacked Avogadro’s number of pennies one on top of the other on Earth’s surface, how far would the stack extend (in km)? [For comparison, the sun is about 150 million km from Earth, and the nearest star (Proxima Centauri) is about 40
Consider the stack of pennies in the previous problem. How much money (in dollars) would this represent? If this money were equally distributed among the world’s population of 7.0 billion, how much would each person receive? Would each person be a millionaire? A billionaire? A trillionaire?
The mass of an average blueberry is 0.75 g, and the mass of an automobile is 2.0 * 103 kg. Find the number of automobiles whose total mass is the same as 1.0 mol of blueberries.
Suppose that atomic masses were based on the assignment of a mass of 12.000 g to 1 mol of carbon, rather than 1 mol of 12C.What would the atomic mass of oxygen be? (The atomic masses of carbon and oxygen based on the assignment of 12.000 g to 1 mol of 12C are 12.011 amu and 15.9994 amu,
A pure titanium cube has an edge length of 2.78 in. How many titanium atoms does it contain? Titanium has a density of 4.50 g/cm3.
A pure copper sphere has a radius of 0.935 in. How many copper atoms does it contain? [The volume of a sphere is (4/3)πr3, and the density of copper is 8.96 g/cm3.]
What is the radius (in cm) of a pure copper sphere that contains 1.14 * 1024 copper atoms? [The volume of a sphere is (4/3)πr3, and the density of copper is 8.96 g/cm3.]
What is the edge length (in cm) of a titanium cube that contains 2.55 * 1024 titanium atoms? The density of titanium is 4.50 g/cm3.
Boron has only two naturally occurring isotopes. The mass of boron-10 is 10.01294 amu, and the mass of boron-11 is 11.00931 amu. Calculate the relative abundances of the two isotopes.
Lithium has only two naturally occurring isotopes. The mass of lithium-6 is 6.01512 amu, and the mass of lithium-7 is 7.01601 amu. Calculate the relative abundances of the two isotopes.
Common brass is a copper and zinc alloy containing 37.0% zinc by mass and having a density of 8.48 g/cm3. A fitting composed of common brass has a total volume of 112.5 cm3. How many atoms (copper and zinc) does the fitting contain?
A 67.2 g sample of a gold and palladium alloy contains 2.49 * 1023 atoms. What is the composition (by mass) of the alloy?
Naturally occurring chlorine is composed of two isotopes: 75.76% Cl-35 (mass 34.9688 amu) and 24.24% Cl-37 (mass 36.9659 amu). Naturally occurring oxygen is composed of three isotopes:99.757% O-16 (mass 15.9949 amu), 0.038% O-17 (mass 16.9991 amu), and 0.205% O-18 (mass 17.9991 amu). The compound
Silver is composed of two naturally occurring isotopes: Ag-107 (51.839%) and Ag-109. The ratio of the masses of the two isotopes is 1.0187. What is the mass of Ag-107?
The U.S. Environmental Protection Agency (EPA) sets limits on healthful levels of air pollutants. The maximum level that the EPA considers safe for lead air pollution is 1.5 mg/m3. If your lungs were filled with air containing this level of lead, how many lead atoms would be in your lungs? (Assume
Pure gold is usually too soft for jewelry, so it is often alloyed with other metals. How many gold atoms are in an 0.255-ounce, 18 K gold bracelet? (18 K gold is 75% gold by mass.)
It was stated that 1 mol of sand grains would cover the state of Texas to several feet. Estimate how many feet by assuming that the sand grains are roughly cube-shaped, each one with an edge length of 0.10 mm. Texas has a land area of 268,601 square miles.
Below is a representation of 50 atoms of a fictitious element called pearsonium (Ps). The red spheres represent Ps-296, the blue spheres Ps-297, and the green spheres Ps-298.a. Assuming that the sample is statistically representative of a naturally occurring sample, calculate the percent natural
Use the concepts in this chapter to obtain an estimate for the number of atoms in the universe. Make the following assumptions:(a) All of the atoms in the universe are hydrogen atoms in stars. (This is not a ridiculous assumption because over threefourths of the atoms in the universe are in fact
The ratio of oxygen to nitrogen by mass in NO2 is 2.29. The ratio of fluorine to nitrogen by mass in NF3 is 4.07. Find the ratio of oxygen to fluorine by mass in OF2.
Naturally occurring cobalt consists of only one isotope, 59Co, whose relative atomic mass is 58.9332. A synthetic radioactive isotope of cobalt, 60Co, has a relative atomic mass of 59.9338 and is used in radiation therapy for cancer. A 1.5886 g sample of cobalt has an apparent “atomic mass” of
A 7.36 g sample of copper is contaminated with an additional 0.51 g of zinc. Suppose an atomic mass measurement was performed on this sample. What would be the measured atomic mass?
The ratio of the mass of O to the mass of N in N2O3 is 12:7.Another binary compound of nitrogen has a ratio of O to N of 16:7. What is its formula? What is the ratio of O to N in the next member of this series of compounds?
Naturally occurring magnesium has an atomic mass of 24.312 and consists of three isotopes. The major isotope is 24Mg, natural abundance 78.99%, relative atomic mass 23.98504. The next most abundant isotope is 26Mg, relative atomic mass 25.98259.The third most abundant isotope is 25Mg, whose natural
Which answer is an example of the law of multiple proportions? Explain.a. Two different samples of water are found to have the same ratio of hydrogen to oxygen.b. When hydrogen and oxygen react, the mass of water formed is exactly equal to the mass of hydrogen and oxygen that reacted.c. The mass
Lithium has two naturally occurring isotopes: Li-6 (natural abundance 7.5%) and Li-7 (natural abundance 92.5%). Using circles to represent protons and squares to represent neutrons, draw the nucleus of each isotope. How many Li-6 atoms are present, on average, in a 1000-atom sample of lithium?
As we saw in the previous problem, lithium has two naturally occurring isotopes: Li-6 (natural abundance 7.5%; mass 6.0151 amu) and Li-7 (natural abundance 92.5%; mass 7.0160 amu).Without doing any calculations, determine which mass is closest to the atomic mass of Li.a. 6.00 amu b. 6.50 amu c.
The table shown here includes data similar to those used by Mendeleev when he created the periodic table. On a small card, write the symbol, atomic mass, and a stable compound formed by each element. Without consulting a periodic table, arrange the cards so that atomic mass increases from left to
The mole is defined as the amount of a substance containing the same number of particles as exactly 12 g of C-12. The amu is defined as 1/12 of the mass of an atom of C-12. Why is it important that both of these definitions reference the same isotope?What would be the result, for example, of
Without doing any calculations, determine which of the samples contains the greatest amount of the element in moles. Which contains the greatest mass of the element?a. 55.0 g Cr b. 45.0 g Ti c. 60.0 g Zn
The atomic radii of the isotopes of an element are identical to one another. However, the atomic radii of the ions of an element are significantly different from the atomic radii of the neutral atom of the element. Explain.
The U.S. Environmental Protection Agency (U.S. EPA) monitors air quality in the United States. Lead is among the pollutants regularly monitored and regulated. Lead is released into the atmosphere primarily by the processing of metal ores containing lead and by leadbased battery manufacturing. The
In a naturally occurring sample, 19.8% of boron atoms have five neutrons and 80.2% have six neutrons. What is the mass number of each boron isotope? Sketch a sample of 10 atoms that is nearly representative of a natural sample. What is the average mass of the atoms in your drawing? What is the
In complete sentences, describe the similarities and differences between:a. Different isotopes of an element b. A neutral atom and an ion of the same element
Calculate the mass in grams of one mole of each of the following (the mass of a single item is given in parentheses): electrons (9.10938 * 10-28 g), protons (1.67262 * 10-24 g), neutrons (1.67493 * 10-24 g), atoms of carbon-12 (1.992646 * 10-23 g), and doughnuts (74 g). Compare the mass of one mole
Write empirical formulas for the compounds represented by the molecular formulas.(a) C4H8 (b) B2H6 (c) CCl4
What type of bond—ionic or covalent—forms between nitrogen and oxygen?(a) Ionic (b) Covalent
What is the empirical formula of a compound with the molecular formula C10H8?a) C5H3b) C2H4c) C5H4d) CH
How do the properties of compounds compare to the properties of the elements from which the compounds are composed?
Classify each of the substances as an atomic element, molecular element, molecular compound, or ionic compound.(a) Xenon (b) NiCl2 (c) Bromine (d) NO2(e) NaNO3
Select the structural formula for water.(a) H—O (b) H—H(c) H—O—H (d) H2O
Based on what you learned in Chapter 2 about atoms, what part of the atom do you think the spheres in the molecular space-filling models shown in Table 3.1 represent? If you were to superimpose a nucleus on one of these spheres, how big would you draw it?(a) Each sphere represents the hard outer
Write the formula for the ionic compound that forms between aluminum and oxygen. 3+ A1³+ 0²-
Which substance is an ionic compound?a) SrI2b) N2O4c) Hed) CCl4
What is a chemical bond? Explain the difference between an ionic bond and a covalent bond.
What is the correct formula for the compound formed between calcium and sulfur?a) CaSb) Ca2Sc) CaS2d) CaS3
Write the formula for the ionic compound that forms between calcium and oxygen. Ca²+ 0²-
Explain the different ways to represent compounds. Why are there so many?
Classify the substance represented by the molecular view shown here.(a) Atomic element(b) Molecular element(c) Molecular compound(d) Ionic compound
Name the compound SrI2.a) Strontium iodideb) Strontium diiodidec) Strontium(II) iodided) Strontium(II) diiodide
What is the difference between an empirical formula and a molecular formula?
Name the compound CaBr2.
Which statement best summarizes the difference between ionic and molecular compounds?(a) Molecular compounds contain highly directional covalent bonds, which result in the formation of molecules. Ionic compounds contain nondirectional ionic bonds, which result (in the solid state) in the formation
What is the formula for manganese(IV) oxide?a) Mn4Ob) MnO4c) Mn2Od) MnO2
Define and provide an example for each of the following: atomic element, molecular element, ionic compound, molecular compound.
Name the compound PbCl4.
Which metal has the same charge in all of its compounds?(a) Fe (b) Mo(c) Pb (d) Sr
Name the compound Pb(C2H3O2)2.a) Lead(II) carbonateb) Lead(II) acetatec) Lead bicarbonated) Lead diacetate
Explain how to write a formula for an ionic compound given the names of the metal and nonmetal (or polyatomic ion) in the compound.
Identify the polyatomic ion and its charge in each compound: KNO2, CaSO4, Mg(NO3)2. (a) NO₂, SO42, and NO3 (c) K+, Ca2+, Mg2+, NO₂, SO42, and NO3 (b) K+, Ca²+, and Mg²+ (d) NO₂2, SO4, and NO3²-
Name the compound Li2Cr2O7.
The compound NCl3 is nitrogen trichloride, but AlCl3 is simply aluminum chloride. Why?(a) The name forms differ because NCl3 is an ionic compound and AlCl3 is a molecular compound. Prefixes such as mono-, di-, and tri- are used for ionic compounds but not for molecular compounds.(b) The name forms
Name the compound HNO2(aq).a) Hydrogen nitrogen dioxideb) Hydrogen nitratec) Nitric acidd) Nitrous acid
Name the acid HI(aq).
Throughout this book, you will find space-filling molecular models to represent molecules. Which number is the best estimate for the scaling factor used in these models? In other words, by approximately what number would you have to multiply the radius of an actual oxygen atom to get the radius of
Determine the number of CH2Cl2 molecules in 25.0 g CH2Cl2.a) 0.294 moleculesb) 1.77 * 1023 moleculesc) 1.28 * 1027 moleculesd) 1.51 * 1025 molecules
Explain how to name molecular inorganic compounds.
Name the acid HC2H3O2(aq).
Use the flowchart in Figure 3.11 to name each compound.(a) SO2 (b) HClO4(aq)(c) CoF2 Inorganic Nomenclature Flowchart Metal forms one type of ion only. name of cation (metal) IONIC Metal and nonmetal name of cation (metal) Example: Cal₂ calcium iodide Metal forms more than one type of ion. base
Without doing any calculations, list the elements in C6H6O in order of decreasing mass percent composition.(a) C > O > H (b) O > C > H (c) H > O > C (d) C > H > O
List the elements in the compound CF2Cl2 in order of decreasing mass percent composition.a) C > F > Clb) F > Cl > Cc) Cl > C > Fd) Cl > F > C
How many atoms are specified by each of these prefixes: mono-, di-, tri-, tetra-, penta-, hexa-?
The molecular formula for water is H2O. Which ratio can be correctly derived from this formula? Explain.(a) 2 g H : 1 g H2O (b) 2 mL H : 1 mL H2O (c) 2 mol H : 1 mol H2O
Determine the mass of potassium in 35.5 g of KBr.a) 17.4 gb) 0.298 gc) 11.7 gd) 32.9 g
Which elements are normally present in organic compounds?
Upon combustion, a compound containing only carbon and hydrogen produces 1.83 g CO2 and 0.901 g H2O. Find the empirical formula of the compound. GIVEN: 1.83 g CO₂, 0.901 g H₂O FIND: empirical formula
What is the difference between an alkane, an alkene, and an alkyne?
Upon combustion, a 0.8233-g sample of a compound containing only carbon, hydrogen, and oxygen produces 2.445 g CO2 and 0.6003 g H2O. Find the empirical formula of the compound. GIVEN: 0.8233-g sample, 2.445 g CO2, 0.6003 g H₂O FIND: empirical formula
What are functionalized hydrocarbons? Cite an example of a functionalized hydrocarbon.
Write a generic formula for each of the families of organic compounds.a. Alcohols b. Ethersc. Aldehydes d. Ketonese. Carboxylic acids f. Estersg. Amines

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