?Explain the difference between a molecular formula and an empirical formula

Do the properties of an element change when it combines with another element to form a compound? Explain.

How might the world be different if elements did not combine to form compounds?

What is the law of constant composition? Who discovered it?

What is a chemical formula? List some examples.

In a chemical formula, which element is listed first?

In a chemical formula, how do you calculate the number of atoms of an element within parentheses? Provide an example.

Explain the difference between a molecular formula and an empirical formula.

What is a structural formula? What is the difference between a structural formula and a molecular model?

What is the difference between a molecular element and an atomic element? List the elements that occur as diatomic molecules.

What is the difference between an ionic compound and a molecular compound?

What is the difference between a common name for a compound and a systematic name?

List the metals that form only one type of ion (that is, metals whose charge is invariant from one compound to another). What are the group numbers of these metals?

Identify the block in the periodic table of metals that tend to form more than one type of ion.

What is the basic form for the names of ionic compounds containing a metal that forms only one type of ion?

What is the basic form for the names of ionic compounds containing a metal that forms more than one type of ion?

Why are roman numerals needed in the names of ionic compounds containing a metal that forms more than one type of ion?

How are compounds containing a polyatomic ion named?

Which polyatomic ions have a 2- charge? Which polyatomic ions have a 3- charge?

What is the basic form for the names of molecular compounds?

How many atoms does each prefix specify? mono-, di-, tri-, tetra-, penta-, hexa-.

What is the basic form for the names of binary acids?

What is the basic form for the name of oxyacids whose oxyanions end with -ate?

What is the basic form for the name of oxyacids whose oxyanions end with -ite?

What is the formula mass of a compound?

Two samples of sodium chloride are decomposed into their constituent elements. One sample produces 4.65 g of sodium and 7.16 g of chlorine, and the other sample produces 7.45 g of sodium and 11.5 g of chlorine. Are these results consistent with the law of constant composition? Explain your answer.

Two samples of carbon tetrachloride are decomposed into their constituent elements. One sample produces 32.4 g of carbon and 373 g of chlorine, and the other sample produces 12.3 g of carbon and 112 g of chlorine. Are these results consistent with the law of constant composition? Explain your answer.

Upon decomposition, one sample of magnesium fluoride produced 1.65 kg of magnesium and 2.57 kg of fluorine. A second sample produced 1.32 kg of magnesium. How much fluorine (in grams) did the second sample produce? Remember that, according to the law of constant composition, the ratio of the masses of the two elements must be the same in both samples.

The mass ratio of sodium to fluorine in sodium fluoride is 1.21:1. A sample of sodium fluoride produces 34.5 g of sodium upon decomposition. How much fluorine (in grams) forms? Hint: the \(\text { ratio } \frac{\text { mass sodium }}{\text { mass fluorine }}=1.21\). Text Transcription: ratio\mass sodium\mass fluorine=1.21

Use the law of constant composition to complete the table summarizing the amounts of nitrogen and oxygen produced upon the decomposition of several samples of dinitrogen monoxide. Remember that, according to the law of constant composition, the ratio of the masses of the two \(\text { elements }\left(\frac{\text { mass nitrogen }}{\text { mass oxygen }}\right)\) must be the same in all samples. Text Transcription: elements\mass nitrogen\mass oxygen

Use the law of constant composition to complete the table summarizing the amounts of iron and chlorine produced upon the decomposition of several samples of iron(III) chloride. Remember that, according to the law of constant composition, the ratio of the masses of the two elements \(\left(\frac{\text { mass chlorine }}{\text { mass iron }}\right)\) must be the same in all samples. Text Transcription: mass chlorine/mass iron

Write a chemical formula for the compound containing one nitrogen atom for every three iodine atoms.

Write a chemical formula for the compound containing one carbon atom for every four bromine atoms.

Write chemical formulas for compounds containing: (a) three iron atoms for every four oxygen atoms (b) one phosphorus atom for every three chlorine atoms (c) one phosphorus atom for every five chlorine atoms (d) two silver atoms for every oxygen atom

Write chemical formulas for compounds containing: (a) one calcium atom for every two iodine atoms (b) two nitrogen atoms for every four oxygen atoms (c) one silicon atom for every two oxygen atoms (d) one zinc atom for every two chlorine atoms

How many oxygen atoms are in each chemical formula? (a) \(\mathrm{H}_{3} \mathrm{PO}_{4}\) (b) \(\mathrm{Na}_{2} \mathrm{HPO}_{4}\) (c) \(\mathrm{Ca}\left(\mathrm{HCO}_{3}\right)_{2}\) (d) \(\mathrm{Ba}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}\) Text Transcription: H_3PO_4 Na_2HPO_4 CaHCO_32 BaC_2H_3O_2_2

How many hydrogen atoms are in each of the formulas in Question 35?

Determine the number of each type of atom in each formula. (a) \( \mathrm{MgCl}_{2}\) (b) \(\mathrm{NaNO}_{3}\) (c) \(\mathrm{Ca}\left(\mathrm{NO}_{2}\right)_{2}\) (d) \(\mathrm{Sr}(\mathrm{OH})_{2}\) Text Transcription: MgCl_2 NaNO_3 CaNO_2_2 SrOH_2

Determine the number of each type of atom in each formula. (a) \(\mathrm{NH}_{4} \mathrm{Cl}\) (b) \(\mathrm{Mg}_{3}\left(\mathrm{PO}_{4}\right)_{2}\) (c) \(\mathrm{NaCN}\) (d) \(\mathrm{Ba}\left(\mathrm{HCO}_{3}\right)_{2}\) Text Transcription: NH_4Cl Mg_3PO_4_2 NaCN BaHCO_3_2

Complete the table.

Complete the table.

Give the empirical formula that corresponds to each molecular formula. (a) \(\mathrm{C}_{2} \mathrm{H}_{6}\) (b) \(\mathrm{N}_{2} \mathrm{O}_{4}\) (c) \(\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{2}\) (d) \(\mathrm{NH}_{3}\) Text Transcription: C_2H_6 N_2O_4 C_4H_6O_2 NH_3

Give the empirical formula that corresponds to each molecular formula. (a) \(\mathrm{C}_{2} \mathrm{H}_{2}\) (b) \(\mathrm{CO}_{2}\) (c) \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\) (d) \(\mathrm{B}_{2} \mathrm{H}_{6}\) Text Transcription: C_2H_2 CO_2 C_6H_12O_6 B_2H_6

Classify each element as atomic or molecular. (a) chlorine (b) argon (c) cobalt (d) hydrogen

Which elements have molecules as their basic units? (a) helium (b) oxygen (c) iron (d) bromine

Classify each compound as ionic or molecular. (a) \(\mathrm{CS}_{2}\) (b) CuO (c) KI (d) \(\mathrm{PCl}_{3}\) Text Transcription: CS_2 PCl_3

Classify each compound as ionic or molecular. (a) \(\mathrm{PtO}_{2}\) (b) \(\mathrm{CF}_{2} \mathrm{Cl}_{2}\) (c) CO (d) \(\mathrm{SO}_{3}\) Text Transcription: PtO_2 CF_2Cl_2 SO_3

Match the substances on the left with the basic units that compose them on the right. Remember that atomic elements are composed of atoms, molecular elements are composed of diatomic molecules, molecular compounds are composed of molecules, and ionic compounds are composed of formula units. helium molecules \(\mathrm{CCl}_{4}\) formula units \(\mathrm{K}_{2} \mathrm{SO}_{4}\) diatomic molecules bromine single atoms Text Transcription: CCl_4 K_2SO_4

Match the substances on the left with the basic units that compose them on the right. Remember that atomic elements are composed of atoms, molecular elements are composed of diatomic molecules, molecular compounds are composed of molecules, and ionic compounds are composed of formula units. \(\mathrm{NI}_{3}\) molecules copper metal single atoms \(\mathrm{SrCl}_{2}\) diatomic molecules nitrogen formula units Text Transcription: NI_3 SrCl_2

What are the basic units—single atoms, molecules, or formula units—that compose each substance? (a) \(\mathrm{BaBr}_{2}\) (b) Ne (c) \(\mathrm{I}_{2}\) (d) CO Text Transcription: BaBr_2 I_2

What are the basic units—single atoms, molecules, or formula units—that compose each substance? (a) \(\mathrm{Rb}_{2} \mathrm{O}\) (b) \(\mathrm{N}_{2}\) (c) \(\operatorname{Fe}\left(\mathrm{NO}_{3}\right)_{2}\) (d) \(\mathrm{N}_{2} \mathrm{~F}_{4}\) Text Transcription: Rb_2O N_2 FeNO_3_2 N_2F_4

Classify each compound as ionic or molecular. If it is ionic, determine whether the metal forms only one type of ion or more than one type of ion. (a) KCl (b) \(\mathrm{CBr}_{4}\) (c) \(\mathrm{NO}_{2}\) (d) \(\mathrm{Sn}\left(\mathrm{SO}_{4}\right)_{2}\) Text Transcription: CBr_4 NO_2 SnSO_4_2

Classify each compound as ionic or molecular. If it is ionic, determine whether the metal forms only one type of ion or more than one type of ion. (a) \(\mathrm{CoCl}_{2}\) (b) \(\mathrm{CF}_{4}\) (c) \(\mathrm{BaSO}_{4}\) (d) NO Text Transcription: CoCl_2 CF_4 BaSO_4

Write a formula for the ionic compound that forms from each pair of elements. (a) sodium and sulfur (b) strontium and oxygen (c) aluminum and sulfur (d) magnesium and chlorine

Write a formula for the ionic compound that forms from each pair of elements. (a) aluminum and oxygen (b) beryllium and iodine (c) calcium and sulfur (d) calcium and iodine

Write a formula for the compound that forms from potassium and (a) acetate (b) chromate (c) phosphate (d) cyanide

Write a formula for the compound that forms from calcium and (a) hydroxide (b) carbonate (c) phosphate (d) hydrogen phosphate

Write formulas for the compounds formed from the element on the left and each of the elements on the right. (a) Li N, O, F (b) Ba N, O, F (c) Al N, O, F

Write formulas for the compounds formed from the element on the left and each polyatomic ion on the right. (a) \(\mathrm{Rb} \quad \mathrm{NO}_{3}^{-}, \mathrm{SO}_{4}^{2-}, \mathrm{PO}_{4}^{3}\) (b) \(\mathrm{Sr} \quad \mathrm{NO}_{3}^{-}, \mathrm{SO}_{4}^{2-}, \mathrm{PO}_{4}^{3}\) c) \(\mathrm{In} \quad \mathrm{NO}_{3}^{-}, \mathrm{SO}_{4}^{2-}, \mathrm{PO}_{4}^{3}\) (Assume In charge is 3+.) Text Transcription: Rb Sr In NO_3^- SO_4^2- PO4^3

Name each ionic compound. In each of these compounds, the metal forms only one type of ion. (a) CsCl (b) \(\mathrm{SrBr}_{2}\) (c) \(\mathrm{K}_{2} \mathrm{O}\) (d) LiF Text Transcription: SrBr_2 K_2O

Name each ionic compound. In each of these compounds, the metal forms only one type of ion. (a) LiI (b) MgS (c) \(\mathrm{BaF}_{2}\) (d) NaF Text Transcription: BaF_2

Name each ionic compound. In each of these compounds, the metal forms more than one type of ion. (a) \(\mathrm{CrCl}_{2}\) (b) \(\mathrm{CrCl}_{3}\) (c) \(\mathrm{SnO}_{2}\) (d) \(\mathrm{PbI}_{2}\) Text Transcription: CrCl_2 CrCl_3 SnO_2 PbI_2

Name each ionic compound. In each of these compounds, the metal forms more than one type of ion. (a) \(\mathrm{HgBr}_{2}\) (b) \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) (c) \(\mathrm{CuI}_{2}\) (d) \(\mathrm{SnCl}_{4}\) Text Transcription: HgBr_2 Fe_2O_3 CuI_2 SnCl_4

Determine whether the metal in each ionic compound forms only one type of ion or more than one type of ion and name the compound accordingly. (a) \(\mathrm{Cr}_{2} \mathrm{O}_{3}\) (b) NaI (c) \(\mathrm{CaBr}_{2}\) (d) SnO Text Transcription: Cr_2O_3 CaBr_2

Determine whether the metal in each ionic compound forms only one type of ion or more than one type of ion and name the compound accordingly. (a) \(\mathrm{FeI}_{3}\) (b) \(\mathrm{PbCl}_{4}\) (c) \(\mathrm{SrI}_{2}\) (d) BaO Text Transcription: FeI_3 PbCl_4 SrI_2

Name each ionic compound containing a polyatomic ion. (a) \(\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}\) (b) \(\mathrm{Pb}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}\) (c) \(\mathrm{NH}_{4} \mathrm{I}\) (d) \(\mathrm{KClO}_{3}\) (e) \(\mathrm{CoSO}_{4}\) (f) \(\mathrm{NaClO}_{4}\) Text Transcription: BaNO_3_2 PbC_2H_3O_2_2 NH_4I KClO_3 CoSO_4 NaClO_4

Name each ionic compound containing a polyatomic ion. (a) \(\mathrm{Ba}(\mathrm{OH})_{2}\) (b) \(\mathrm{Fe}(\mathrm{OH})_{3}\) (c) \(\mathrm{Cu}\left(\mathrm{NO}_{2}\right)_{2}\) (d) \(\mathrm{PbSO}_{4}\) (e) KClO (f) \(\mathrm{Mg}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}\) Text Transcription: BaOH_2 FeOH_3 CuNO_2_2 PbSO_4 MgC_2H_3O_2_2

Name each polyatomic ion. (a) \(\mathrm{BrO}^{-}\) (b) \(\mathrm{BrO}_{2}^{-}\) (c) \(\mathrm{BrO}_{3}^{-}\) (d) \(\mathrm{BrO}_{4}^{-}\) Text Transcription: BrO^- BrO_2^- BrO_3^- BrO_4^-

Name each polyatomic ion. (a) \(\mathrm{IO}^{-}\) (b) \(\mathrm{IO}_{2}^{-}\) (c) \(\mathrm{IO}_{3}^{-}\) (d) \(\mathrm{IO}_{4}^{-}\) Text Transcription: IO^- IO_2^- IO_3^- IO_4^-

Write a formula for each ionic compound. (a) copper(II) bromide (b) silver nitrate (c) potassium hydroxide (d) sodium sulfate (e) potassium hydrogen sulfate (f) sodium hydrogen carbonate

Write a formula for each ionic compound. (a) copper(I) chlorate (b) potassium permanganate (c) lead(II) chromate (d) calcium fluoride (e) iron(II) phosphate (f) lithium hydrogen sulfite

Name each molecular compound. (a) \(\mathrm{SO}_{2}\) (b) \(\mathrm{NI}_{3}\) © \(\mathrm{BrF}_{5}\) (d) NO (e) \(\mathrm{N}_{4} \mathrm{Se}_{4}\) Text Transcription: SO_2 NI_3 BrF_5 N_4Se_4

Name each molecular compound. (a) \(\mathrm{XeF}_{4}\) (b) \(\mathrm{PI}_{3}\) (c) \(\mathrm{SO}_{3}\) (d) \(\mathrm{SiCl}_{4}\) (e) \(\mathrm{I}_{2} \mathrm{O}_{5}\) Text Transcription: XeF_4 PI_3 SO_3 SiCl_4 I_2O_5

Write a formula for each molecular compound. (a) carbon monoxide (b) disulfur tetrafluoride (c) dichlorine monoxide (d) phosphorus pentafluoride (e) boron tribromide (f) diphosphorus pentasulfide

Write a formula for each molecular compound. (a) chlorine monoxide (b) xenon tetroxide (c) xenon hexafluoride (d) carbon tetrabromide (e) diboron tetrachloride (f) tetraphosphorus triselenide

Determine whether the name shown for each molecular compound is correct. If not, provide the compound’s correct name. (a) \(\mathrm{PBr}_{5}\) \quad phosphorus(V) pentabromide (b) \(\mathrm{P}_{2} \mathrm{O}_{3}\) \quad phosphorus trioxide (c) \(\mathrm{SF}_{4}\) \quad monosulfur hexafluoride (d) \(\mathrm{NF}_{3}\) nitrogen trifluoride Text Transcription: PBr_5 P_2O_3 SF_4 NF_3

Determine whether the name shown for each molecular compound is correct. If not, provide the compound’s correct name. (a) \(\mathrm{NCl}_{3}\) \quad nitrogen chloride (b) \(\mathrm{CI}_{4}\) \quad carbon(IV) iodide (c) CO \quad carbon oxide (d) \(\mathrm{SCl}_{4}\) \quad sulfur tetrachloride Text Transcription: NCl_3 CI_4 SCl_4

Determine whether each acid is a binary acid or an oxyacid and name each acid. If the acid is an oxyacid, provide the name of the oxyanion. (a) \(\mathrm{HNO}_{2}(a q)\) (b) HI(aq) (c) \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)\) (d) \(\mathrm{HNO}_{3}(a q)\) Text Transcription: HNO_2aq H_2SO4aq HNO_3aq

Determine whether each acid is a binary acid or an oxyacid and name each acid. If the acid is an oxyacid, provide the name of the oxyanion. (a) \(\mathrm{H}_{2} \mathrm{CO}_{3}(a q)\) (b) \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)\) (c) \(\mathrm{H}_{3} \mathrm{PO}_{4}(a q)\) (d) HCl(aq) Text Transcription: H_2CO_3aq HC_2H_3O_2aq H_3PO_4aq

Name each acid. (a) HClO (b) \(\mathrm{HClO}_{2}\) (c) \(\mathrm{HClO}_{3}\) (d) \(\mathrm{HClO}_{4}\) Text Transcription: HCIO_2 HCIO_3 HCIO_4

Name each acid. (Hint: The names of the oxyanions are analogous to the names of the oxyanions of chlorine.) (a) \(\mathrm{HBrO}_{3}\) (b) \(\mathrm{HlO}_{3}\) Text Transcription: HBrO_3 HIO_3

Write a formula for each acid. (a) phosphoric acid (b) hydrobromic acid (c) sulfurous acid

Write a formula for each acid. (a) hydrofluoric acid (b) hydrocyanic acid (c) chlorous acid

Calculate the formula mass for each compound. (a) \(\mathrm{HNO}_{3}\) (b) \(\mathrm{CaBr}_{2}\) (c) \(\mathrm{CCl}_{4}\) (d) \(\mathrm{Sr}\left(\mathrm{NO}_{3}\right)_{2}\) Text Transcription: HNO_3 CaBr_2 CCI_4 SrNO_3_2

Calculate the formula mass for each compound. (a) \(\mathrm{CS}_{2}\) (b) \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\) (c) \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}\) (d) \(\mathrm{C}_{7} \mathrm{H}_{16}\) Text Transcription: CS_2 C_6H_12O_6 FeNO_3_3 C_7H_16

Arrange the compounds in order of decreasing formula mass. \(\mathrm{Ag}_{2} \mathrm{O}\), \(\mathrm{PtO}_{2},\), \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\), \(\mathrm{PBr}_{3}\) Text Transcription: Ag_2O PtO_2 AINO_3_3 PBr_3

Arrange the compounds in order of decreasing formula mass. \(\mathrm{WO}_{2}\), \(\mathrm{Rb}_{2} \mathrm{SO}_{4}\), \(\mathrm{Pb}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}\), RbI Text Transcription: WO_2 Rb_2SO_4 PbC_2 H_3O_2_2

Write a molecular formula for each molecular model. (White = hydrogen; red = oxygen; black = carbon; blue = nitrogen; yellow = sulfur)

Write a molecular formula for each molecular model. (White = hydrogen; red = oxygen; black = carbon; blue = nitrogen; yellow = sulfur)

How many chlorine atoms are in each set? (a) three carbon tetrachloride molecules (b) two calcium chloride formula units (c) four phosphorus trichloride molecules (d) seven sodium chloride formula units

How many oxygen atoms are in each set? (a) four dinitrogen monoxide molecules (b) two calcium carbonate formula units (c) three sulfur dioxide molecules (d) five perchlorate ions

Specify the number of hydrogen atoms (white) represented in each set of molecular models:

Specify the number of oxygen atoms (red) represented in each set of molecular models:

Complete the table:

Complete the table:

Is each name correct for the given formula? If not, provide the correct name. (a) \(\mathrm{Ca}\left(\mathrm{NO}_{2}\right)_{2}\) calcium nitrate (b) \(\mathrm{K}_{2} \mathrm{O}\) dipotassium monoxide (c) \(\mathrm{PCl}_{3}\) phosphorus chloride (d) \(\mathrm{PbCO}_{3}\) lead(II) carbonate (e) \(\mathrm{KIO}_{2}\) potassium hypoiodite Text Transcription: CaNO_2_2 K_2O PCI_3 PbCO_3 KIO_2

Is each name correct for the given formula? If not, provide the correct name. (a) \(\mathrm{HNO}_{3}(a q)\) hydrogen nitrate (b) NaClO sodium hypochlorite (c) \(\mathrm{CaI}_{2}\) calcium diiodide (d) \(\mathrm{SnCrO}_{4}\) tin chromate (e) \(\mathrm{NaBrO}_{3}\) sodium bromite Text Transcription: HNO_3aq Cal_2 SnCrO_4 NaBrO_3

For each compound, list the correct formula and calculate the formula mass. (a) tin(IV) sulfate (b) nitrous acid (c) sodium bicarbonate (d) phosphorus pentafluoride

For each compound, list the correct formula and calculate the formula mass. (a) barium bromide (b) dinitrogen trioxide (c) copper(I) sulfate (d) hydrobromic acid

Name each compound and calculate its formula mass. (a) \(\mathrm{PtO}_{2}\) (b) \(\mathrm{N}_{2} \mathrm{O}_{5}\) (c) \(\mathrm{Al}\left(\mathrm{ClO}_{3}\right)_{3}\) (d) \(\mathrm{PBr}_{5}\) Text Transcription: PtO_2 N_2O_5 AlCIO_3_3 PBr_5

Name each compound and calculate its formula mass. (a) \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}\) (b) \(\mathrm{P}_{2} \mathrm{O}_{3}\) (c) HClO(aq) (d) \(\mathrm{Cr}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{3}\) Text Transcription: AI_2SO_4_3 P_2O_3 CrC_2H_3O_2_3

A compound contains only carbon and hydrogen and has a formula mass of 28.06 amu. What is its molecular formula?

A compound contains only nitrogen and oxygen and has a formula mass of 44.02 amu. What is its molecular formula?

Carbon has two naturally occurring isotopes: carbon-12 (mass = 12.00 amu) and carbon-13 (mass = 13.00 amu). Chlorine also has two naturally occurring isotopes: chlorine-35 (mass = 34.97 amu) and chlorine-37 (mass = 36.97 amu). How many CCl4 molecules of different masses can exist? Determine the mass (in amu) of each of them.

Nitrogen has two naturally occurring isotopes: nitrogen-14 (mass = 14.00 amu) and nitrogen-15 (mass = 15.00 amu). Bromine also has two naturally occurring isotopes: bromine-79 (mass = 78.92 amu) and bromine-81 (mass = 80.92 amu). How many types of \(\mathrm{NBr}_{3}\) molecules of different masses can exist? Determine the mass (in amu) of each of them. Text Transcription: NBr_3

Examine each substance and the corresponding molecular view and classify it as an atomic element, a molecular element, a molecular compound, or an ionic compound.

Molecules can be as small as two atoms or as large as thousands of atoms. In 1962, Max F. Perutz and John C. Kendrew were awarded the Nobel Prize for their discovery of the structure of hemoglobin, a very large molecule that transports oxygen from the lungs to cells through the bloodstream. The chemical formula of hemoglobin is \(\mathrm{C}_{2952} \mathrm{H}_{4664} \mathrm{O}_{832} \mathrm{~N}_{812} \mathrm{~S}_{8} \mathrm{Fe}_{4}\). Calculate the formula mass of hemoglobin. Text Transcription: C_2952H_4664O_832N_312S_8Fe_4

Examine each consumer product label. Write chemical formulas for as many of the compounds as possible based on what you have learned in this chapter.

Write the correct formula for each species: carbon monoxide, carbon dioxide, the carbonate ion. List as many similarities and differences between these three species as you can. Try to get at least one contribution from each group member.

What questions do you need to ask about a substance in order to determine whether it is (1) an atomic element, (2) a molecular element, (3) a molecular compound, or (4) an ionic compound? Write a detailed set of instructions describing how to determine the classification of a substance based on the answers to your questions.

Name each compound: \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\), \(\mathrm{N}_{2} \mathrm{O}\), NaS, \(\mathrm{CrCl}_{3}\). For each compound, include a detailed step-by-step description of the process you used to determine the name. (Tip: Each group member could name one compound and present it to the whole group.) Text Transcription: CaNO_3_2 N_2O CrCI_3

Calculate the formula mass for each compound in Group Work Question 110.

Climate scientists have become increasingly concerned that rising levels of carbon dioxide in the atmosphere (produced by the burning of fossil fuels) will affect the global climate in harmful ways such as increased temperatures, rising sea levels, and coastal flooding. The graph at right shows the concentration of carbon dioxide in the atmosphere from the mid-1800s to the present time. Study the graph and answer the questions that follow. (a) What were the carbon dioxide concentrations in 1950 and 2000? How much did the carbon dioxide concentration increase during these 50 years? (b) What was the average yearly increase between 1950 and 2000? (c) Beginning from the carbon dioxide concentration in 2010 (390 ppm), and assuming the average yearly increase you calculated in part b, what will the carbon dioxide concentration be in 2050?