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All Textbook Solutions for Introductory Chemistry: A Foundation
True or false? Mixtures always result in a chemical reaction because they consist of two or more substances and thus combine to create a new product.Choose an element or compound with which you are familiar in everyday life. Give twophysicalproperties and twochemicalproperties of your choice of element or compound.56APGive an example of each of the following: a heterogeneous mixture a homogeneous mixture an element a compound a physical property or change a chemical property or change a solution58APSketch the apparatus commonly used for simple distillation in the laboratory, identifying each component.60APWhich of the following best describes the substanceXeF4 ? element compound heterogeneous mixture homogeneous mixture62CPWhich of the following describes a chemical property? The density of iron is 7.87 g/cm3. A platinum wire glows red when heated. An iron bar rusts. Aluminum is a silver-colored metal.64CP1CR2CRYou have learned the basic way in which scientists analyze problems, propose models to explain the systems under consideration, and then experiment to test their models. Suppose you have a sample of a liquid material. You are not sure whether the liquid is a purecompound(for example, water or alcohol) or asolution. How could you apply the scientific method to study the liquid and to determine which type of material the liquid is?Many college students would not choose to take a chemistry course if it were not required for their major. Do you have a better appreciation ofwhychemistry is a required course for your own particular major or career choice? Discuss.5CR6CR7CR8CR9CRWhat ismatter? What is matter composed of? What are some of the different types of matter? How do these types of matter differ, and how are they the same?11CR12CR13CR14CR15CR16CR17CRa. Given that 1100. mL of ethyl alcohol weighs 78.5 g, calculate the density of ethyl alcohol. b. What volume would 1.59 kg of ethyl alcohol occupy? c. What is the mass of 1.35 L of ethyl alcohol? d. Pure aluminum metal has a density of 2.70 g/cm3. Calculate the volume of 25.2 g of pure aluminum. e. What will a rectangular block of pure aluminum having dimensions of 12.0 cm × 2.5 cm × 2.5 cm weigh?Which of the following represent physical properties or changes, and which represent chemical properties or changes? You curl your hair with a curling iron. You curl your hair by getting a “permanent wave” at the hair salon. Ice on your sidewalk melts when you put salt on it. A glass of water evaporates overnight when it is left on the bedside table. Your steak chars if the skillet is too hot. Alcohol feels cool when it is spilled on the skin. Alcohol ignites when a flame is brought near it. Baking powder causes biscuits to rise.Exercise 4.1 Write the formula for each of the following compounds, listing the elements in the order given. A molecule contains 4 phosphorus atoms and lo oxygen atoms. A molecule contains one uranium atom and six fluorine atoms. A molecule contains one aluminum atom and three chlorine atoms.The average diameter of an atom ¡s1.31010 m. What if the average diameter of an atom were 1 cm? How tall would you be?You have learned about three different models of the atom: Dalton’s model, Thomson’s model, and Rutherford’s model. What if Dalton was correct? What would Rutherford have expected from his experiments with the metal foil? What if Thomson was correct? What would Rutherford have expected from his experiments with the metal foil?Exercise 4.2 Give the number of protons, neutrons, and electrons in the atom symbolized by3890Sr . Strontium-90 occurs in fallout from nuclear testing. It can accumulate in bone marrow and may cause leukemia and hone cancer.Exercise 4.3 Give the number of protons, neutrons, and electrons in the atom symbolized by80201HgExercise 4.4 Give the symbol for the phosphorus atom (Z = 15) that contains 17 neutrons.Exercise 4.5 Give the symbol and atomic number for each of the following elements. Also indicate whether each element is a metal or a nonmetal and whether it is a member of a named family. a. argon b. chlorine c. barium d. cesiumThomson and Rutherford helped to show that atoms consist of three types of subatomic particles, two of which are charged. What if subatomic particles had no charge? How would this affect what you have learned?4.6SCKnowing the number of protons in the atom of a neutral element enables you to determine which of the following? the number of neutrons in the atom of the neutral element the number of electrons in the atom of the neutral element the name of the element two of the above none of the above Explain.The average mass of a carbon atom is 12.011. Assuming you could pick up one carbon atom, what is the chance that you would randomly get one with a mass of 12.011? a. 0% d. 12.011% b. 0.01 1% e. greater than 50% c. about 12% f. none of the above Explain.3ALQ4ALQThe vitamin niacin (nicotinic acid,C6H5NO2 ) can he isolated from a variety of natural sources, such as liver, yeast, milk, and whole grain. It also can be synthesized from commercially available materials. Which Source of nicotinic acid, from a nutritional view, is best for use in a multivitamin tablet? Why?One of the best indications of a useful theory is that it raises more questions for further experimentation than it originally answered. How does this apply to Dalton’s atomic theory? Give examples.7ALQHow does Dalton’s atomic theory account for the law of constant composition?9ALQThese questions concern the work of J. J. Thomson: From Thomson’s work, which particles do you think he would feel are most important in the formation of compounds (chemical changes) and why? Of the remaining two subatomic particles, which do you place second in importance for forming compounds and why? Come up with three models that explain Thomson’s findings and evaluate them. To be complete you should include Thomson’s findings.Heat is applied to an ice cube until only steam is present. Draw a sketch of this process, assuming you can see it at an extremely high level of magnification. What happens to the size of the molecules? What happens to the total mass of the sample?What makes a carbon atom different from a nitrogen atom? How are they alike?Hundreds of years ago, alchemists tried to turn lead into gold. Is this possible? If not, why not? If yes, how would you do it?Chlorine has two prominent isotopes,37Cl and35Cl . Which is more abundant? How do you know?15ALQ16ALQRutherford was surprised when some of theparticles bounced hack. He was surprised because he was thinking of Thomson’s model of the atom. What if Rutherford believed atoms were as Dalton envisioned them? What do you suppose Rutherford would have expected, and what would have surprised him?It is good practice to actively read the textbook and to try to verify claims that are made when you can. The following claim is made in your textbook: “. . . if the nucleus were the size of a grape, the electrons would be about 1 mile away on average.” Provide mathematical support for this statement.Why is the term “sodium chloride molecule” incorrect but the term “carbon dioxide molecule” is correct?Both atomic elements and molecular elements exist. Are there such entities as atomic compounds and molecular compounds? If so, provide an example and microscopic drawing. If not, explain why not.Now that you have gone through Chapter 4, go back to Section 4.3 and review Dalton’s Atomic Theory. Which of the premises are no longer accepted? Explain your answer.Write the formula for each of the following substances, listing the elements in the order given. List the phosphorus atom first. a molecule containing two boron atoms and six hydrogen atoms a compound containing one calcium atom for every two chlorine atoms List the carbon atom first. a compound containing two iron atoms for every three oxygen atoms a molecule containing three hydrogen atoms, one phosphorus atom, and four oxygen atoms23ALQWhat were the four fundamental substances postulated by the Greeks?2QAP3QAP4QAPWhat are the live most abundant elements (by mass) in the earth’s crust, oceans, and atmosphere?Read the “Chemistry in Focus” segment Trace Elements: Small but Crucial, and answer the following questions. What is meant by the termtrace element? Name two essential trace elements in the body and list their function(s).7QAPThe symbols for most elements are based on the first few letters of the respective element’s common English name. In some cases, however, the symbol seems to have nothing to do with the element’s common name. Give three examples of elements whose symbols are not directly derived from the element’s common English name.Find the symbol in Column 2 for each name in Column 1. Column 1 Column 2 a. helium 1. Si b. sodium 2. So c. silver 3. S d. sulfur 4. He e. bromine 5. C f. potassium 6. Co g. neon 7. Ba h. barium 8. Br I. cobalt 9. K j. carbon 10. Po 11. Na 12. Ag 13. Ne 14. Ca10QAPUse the periodic table shown in Fig. 4.9 to find the symbol or name for each of the following elements. Symbol Name Co rubidium Rn radium12QAP13QAP14QAPA given compound always contains the same proportion (by mass) of the elements. This principle became known as .Correct each of the following misstatements from Dalton’s atomic theory. Elements are made of tiny particles called molecules. All atoms of a given element are very similar. The atoms of a given element may be the same as those of another element. A given compound may vary in the relative number and types of atoms depending on the source of the compound. A chemical reaction may involve the gain or loss of atoms as it takes place.17QAPA given compound always contains the same relative masses of its constituent elements. How is this related to the relative numbers of each kind of atom present?Based on the following word descriptions, write the formula for each of the indicated substances. a compound whose molecules each contain six carbon atoms and six hydrogen atoms an aluminum compound in which there are three chlorine atoms for each aluminum atom a compound in which there are two sodium atoms for every sulfur atom a compound whose molecules each contain two nitrogen atoms and tour oxygen atoms a compound in which there is an equal number of sodium, hydrogen, and carbon atoms, but there are three times as many oxygen atoms as atoms of the other three elements a compound that has equal numbers of potassium and iodide atomsBased on the following word descriptions, write the formula for each of the indicated substances. a compound whose molecules contain twice as many oxygen atoms as carbon atoms a compound whose molecules contain an equal number of carbon and oxygen atoms a compound in which there is an equal number of calcium and carbon atoms, but there are three times as many atoms of oxygen as of the other Iwo elements a compound whose molecules contain twice as many hydrogen atoms as sulfur atoms and four times as many oxygen atoms as sulfur atoms a compound in which there are twice as many chlorine atoms as barium atoms a compound in which there are three sulfur atoms for every two aluminum atomsScientists J. J. Thomson and William Thomson (Lord Kelvin) made numerous contributions to our understanding of the atom’s structure. Which subatomic particle did J. J. Thomson discover, and what did this lead him to postulate about the nature of the atom? William Thomson postulated what became known as the “plum pudding” model of the atom’s structure. What did this model suggest?True or false? Rutherford’s bombardment experiments with metal foil suggested that the particles were being deflected by coming near a large, positively charged atomic nucleus.Where are neutrons found in an atom? Are neutrons positively charged, negatively charged, or electrically uncharged?What are the positively charged particles found in the nuclei of atoms called?Do the proton and the neutron have exactly the same mass? How do the masses of the proton and the neutron compare to the mass of the electron? Which particles make the greatest contribution W the mass of an atom? Which particles make the greatest contribution to the chemical properties of an atom?The proton and the (electron/neutron) have almost equal masses. The proton and the (electron/neutron) have charges that are equal in magnitude but opposite in nature.An average atomic nucleus has a diameter of about m.28QAP29QAPTrue or false? The mass number of a nucleus represents the number of protons in the nucleus.For an isolated atom, why do we expect the number of electrons present in the atom to be thesameas the number of protons in the nucleus of the atom?Why do we not necessarily expect the number of neutrons in the nucleus of an atom to be the same as the number of protons?Dalton’s original atomic theory proposed that all atoms of a given element areidentical. Did this turn out to be true after further experimentation was carried out? Explain.34QAPFor each of the following elements, use the periodic table shown in Fig. 4.9 to write the element’s atomic number, symbol, or name. Atomic Number Symbol Name 8 Cu 78 phosphorus 17 Sn zinc36QAPWrite the atomic symbol(ZAX) for each of the isotopes described below. the isotope of carbon with 7 neutrons the isotope of carbon with 6 neutrons Z= 6, number of neutrons 8 atomic number 5, mass number 11 number of protons = 5, number of neurons = 5 the isotope of boron with mass number 10Write the atomic symbol(ZAX) for each of the isotopes described below. Z=26,A=54 the isotope of iron with 30 neutrons number of protons = 26, number of neutrons = 31 the isotope of nitrogen with 7 neutrons Z=7,A=15 atomic number 7, number of neutrons = 8How many protons and neutrons are contained in the nucleus of each of the following atoms? Assuming each atom is uncharged, how many electrons are present? a.56130Ba c .2246Ti e.36Li b.56136Ba d.2248Ti f.37LiRead the Chemistry in Focus” segment “Whair”Do You Live? How can isotopes he used to identify the general region of a person’s place of residence?Read the “Chemistry in Focus” segmentIsotope Tales. Define the termisotope, and explain how isotopes can he used to answer scientific and historical questions.Complete the following table. Name Symbol Atomic Number Mass Number Number of Neutrons 817O 8 9 iron 10 20 80244Pu 56 80202Hg cobalt 59 56 919F 28 chromium 26True or false? The elements are arranged in the periodic table in order of increasing mass.44QAPList the characteristic physical properties that distinguish the metallic elements from the nonmetallic elements.Where are the metallic elements found on the periodic table? Are there more metallic elements or nonmetallic elements?47QAPList five nonmetallic elements that exist as gaseous substances under ordinary conditions. Do any metallic elements ordinarily occur as gases?Under ordinary conditions, only a few pure elements occur as liquids. Give an example of a metallic and a nonmetallic element that ordinarily occur as liquids.The elements that lie close to the “stair-step” line as shown below in blue are called .51QAPWithout looking at your textbook or the periodic table, name three elements in each of the following groups (families). halogens alkali metals alkaline earth metals noble/inert gases53QAP54QAPMost substances are composed of _________ rather than elemental substances.56QAP57QAP58QAPMolecules of nitrogen gas and oxygen gas are said to be , which means they consist of pairs of atoms.Give three examples of gaseous elements that exist as diatomic molecules. Give three examples of gaseous elements that exist as monatomic species.61QAPIf sodium chloride (table salt) is melted and then subjected to an electric current, elemental gas is produced, along with sodium metal.63QAPThe two most common elemental forms of carbon are diamond and ________ .An isolated atom has a net charge of ________ .66QAPA simple ion with a 3+ charge (for example, A13+) results when an atom (gains/loses) electrons.An ion that has two more electrons outside the nucleus than there are protons in the nucleus will have a charge of_________.69QAP70QAP71QAPTrue or false?N3 andP3 contain a different number of protons but the same number of electrons. Justify your answer.How many electrons are present in each of the following ions? a.Ba2+ c.Mn2+ e.Cs+ b.P3 d.Mg2+ f.Pb2+74QAPFor the following processes that show the formation of ions, use the periodic table to indicate the number of electrons and protons present in both theionand theneutral atomfrom which the ion is made. a.CaCa2++2e b.P+3eP3 c.Br+eBr d.FeEe3++3e e.AlAl3++3e f.N+3eN3For the following ions, indicate whether electrons must begainedorlostfrom the parent neutral atom, andhow manyelectrons must be gained or lost. a.O2 c.Cr3+ e.Rb+ b.P3 d.Sn2+ f.Pb2+For each of the following atomic numbers, use the periodic (able to write the formula (including the charge) for the simple ion that the element is most likely to form. a. 53 c. 55 e. 9 b. 38 d. 88 f. 1.13On the basis of the element’s location in the periodic table, indicate what simple ion each of the following elements is most likely to form. a. P c. At e. Cs b. Ra d. Rn f. SeList some properties of a substance that would lead you to believe it consists of ions. How do these properties differ from those of nonionic compounds?80QAP81QAP82QAPFor each of the following positive ions, use the concept that a chemical compound must have a net charge of zero to predict the formula of the simple compounds that the positive ions would form with theCl ,S2 , andN3 ions. a.K+ c.Al3+ e.Li+ b.Mg2+ d.Ca2+For each of the following negative ions, use the concept that a chemical compound must have a net charge of zero to predict the formula of the simple compounds that the negative ions would form with theCs+ ,Ba2+ , andAl3+ ions. a.I c.P3 e.H b.O2 d.Se285AP86AP87APWhich of the following is/are true regarding the number of neutrons in an atom? Identifies the element. Gives the number of protons in a neutral atom. Gives the number of electrons in a neutral atom. Contributes to the mass number.89APWhich subatomic particles contribute most to the atom’s mass? Which subatomic particles determine the atom’s chemical properties?Is it possible for the same Iwo elements to form more than one compound? Is this consistent with Dalton’s atomic theory? Give an example.Carbohydrates, a class of compounds containing the elements carbon, hydrogen, and oxygen, were originally thought to contain one water molecule(H2O) for each carbon atom present. The carbohydrate glucose contains six carbon atoms. Write a general formula showing the relative numbers of each type of atom present in glucose.93APHow many protons and neutrons are contained in the nucleus of each of the following atoms? For an atom of the element, how many electrons are present? a.2963Cu b.3580Br c.1224MgThough the common isotope of aluminum has a mass number of 27, isotopes of aluminum have been isolated (or prepared in nuclear reactors) with mass numbers of 24, 25, 26, 28, 29, and 30. How many neutrons are present in each of these isotopes? Why are they all considered aluminum atoms, even though they differ greatly in mass? Write the atomic symbol for each isotope.96AP97APWhat is the symbol for an ion with a 1 — charge. 36 electrons, and 46 neutrons?99AP100AP101APA metal ion with a 2+ charge contains 34 neutrons and 27 electrons. Identify the metal ion and determine its mass number.103APWrite the simplest formula for each of the following substances, listing the elements in the order given. a molecule containing one carbon atom and two oxygen atoms a compound containing one aluminum atom for every three chlorine atoms per chloric acid, which contains one hydrogen atom, one chlorine atom, and four oxygen atoms a molecule containing one sulfur atom and six chlorine atoms105APWrite the atomic symbol(ZAX) for each of the isotopes described below. Z= 6. number of neutrons = 7 the isotope of carbon with a mass number of 13 Z=6,A= 13 Z=19,A=44 the isotope of calcium with a mass number of 41 the isotope with 19 protons and 16 neutronsHow many protons and neutrons are contained in the nucleus of each of the following atoms? In an atom of each element, how many electrons are present? a.2241Ti d.3686Kr b.3064Zn e.3375As c.3276Ge f.1941K108AP109AP110AP111CP112CPComplete the following table. Number of Protons Number of Neutrons Symbol 34 45 19 20 53 74 4 5 24 32114CPUsing the periodic table, complete the following table. Atoms Number of Protons Number of Neutrons 2555Mn 818O 2859Ni 92238U 80201Hg116CPWhich of the following is(are) correct? a.40Ca2+ contains 20 protons and 18 electrons. b. Rutherford created the cathode-ray tube and was the founder of the charge-to-mass ratio of an electron. c. An electron is heavier than a proton. d. The nucleus contains protons, neutrons, and electrons.Exercise 5.1 Name the following compounds. a.Rb2Ob.SrI2c.K2S1CTExercise 5.2 Give the names of the following compounds. a. PbBr2 and PbBr4 b. FeS and Fe2S3 c. AlBr3 d. Na2S e. CoCl3Exercise 5.3 Name the following compounds. a.CCl4b.NO2e.IF5Exercise 5.4 Name the following compounds. a.SiO2b.O2F2c.XeF6Exercise 5.5 Name the following binary compounds. a.CIF3d.MnO2 b.VF5e.MgO c.CuClf.H2OExercise 5.6 Name each of the following compounds. a.Ca(OH)2d.(NH4)2Cr2O7g.Cu(NO2)2 b.Na3PO4e.Co(ClO4)2 c.KMnO4f.KClO3Exercise 5.7 Name the following compounds. NaHCO3c.CsClO4e.NaBrg.Zn3(PO4)2 BaSO4d.BrF5f.KOCl1CT5.8SCIn some cases the Roman numeral in a name is the same as a subscript in the formula, and in some cases it is not. Provide an example (formula and name) for each of these cases. Explain why the Roman numeral is not necessarily the same as the subscript.2ALQThe formulas MgO and CO look very similar. What is the name for each compound? Why do we name them differently?Explain how to use the periodic table to determine that there are two chloride ions for every magnesium ion in magnesium chloride and one chloride ion for every sodium ion in sodium chloride. Then write the formulas for calcium oxide and potassium oxide and explain how you got them.5ALQ6ALQName each of the following compounds. SO5 P2S5Why do we callBa(NO3)2 barium nitrate hut callFe(NO3)2 iron(II) nitrate?What is the difference between sulfuric acid and hydrosulfuric acid?The “Chemistry in Focus” segment Sugar of Lead discusses Pb(C2H3O2)2 , which originally was known as sugar of lead. Why was it called sugar of lead? What is the systematic name for Pb(C2H3O2)2? Why is it necessary to have a system for the naming of chemical compounds?2QAP3QAP4QAP5QAP6QAP7QAPWe indicate the charge of a metallic element that forms more than one cation by adding a(n) after the name of the cation.9QAP10QAP11QAP12QAP13QAP14QAP15QAP16QAPWrite the name of each of the following binary compounds of nonmetallic elements. KrF2d.XeO4 Se2S6e.BrF3 AsH3f.P2S5Write the name for each of the following binary compounds of nonmetallic elements. GeH4 d. CO2 N2Br4 e. nh5 P2O5 f. SiO2Name each of the following binary compounds, using the periodic table to determine whether the compound is likely to be ionic (containing a metal and a nonmetal) or nonionic (containing only nonmetals). Fe3P2d.PbCl4 CaBr2e.S2F10 N2O5f.Cu2OThe formulasNa2O andN2O look very similar. What is the name for each compound? Why do we use a different naming convention between the two compounds?Name each of the following binary compounds, using the periodic table to determine whether the compound is likely to be ionic (containing a metal and a nonmetal) or nonionic (containing only nonmetals), MgSd.ClBr AlCl3e.Li2O PH3f.P4O10Name each of the following binary compounds, using the periodic table to determine whether the compound is likely to be ionic (containing a metal or a nonmetal) or nonionic (containing only nonmetals). RaCl2d.Na3P SeCl2e.MnF2 PCl3f.ZnOWhat is apolyatomicion? Give examples of five common polyatomic ions.24QAP25QAP26QAP27QAP28QAP29QAP30QAP31QAP32QAPGive the name of each of the following polyatomic ions. a.HCO3d.OH b.C2H3O2e.NO2 c.CNf.HPO4234QAP35QAP36QAPGive a simple definition of anacid.38QAP39QAP40QAP41QAP42QAP43QAP44QAP45QAP46QAP47QAP48QAP49QAP50QAP51AP52AP53AP54AP55AP56APName the following compounds. Ca(C2H3O2)2 PCl3 Cu(MnO4)2 Fe2(CO3)3 LiHCO3 Cr2S3 Ca(CN)258AP59AP60APMost metallic elements formoxides, and often the oxide is the most common compound of the element that is found in the earth’s crust. Write the formulas for the oxides of the following metallic elements. potassium e. zinc(II) magnesium f. lead(II) iron(Il) g. aluminum iron(III)Consider a hypothetical simple ionDetermine the formula of the compound this ion would form with each of the following anions. acetate d. hydrogen phosphate permanganate e. hydroxide oxide f. nitrite63APA metal ion with a 2+ charge has 23 electrons and forms a compound with a halogen ion that contains 17 protons. What is the identity of the metal ion? What is the identity of the halogen ¡on and how many electrons does it contain? Determine the compound that it forms and name it.65AP66APThe noble metals gold, silver, and platinum are often used in fashioning jewelry because they are relatively .68APThe elements of Group 7 (fluorine, chlorine, bromine, and iodine) consist of molecules containing atom(s).70AP71APAn ion with one less electron than it has protons has a _________ charge.An atom that has lost three electrons will have a charge of .An ion with two more electrons than it has protons has a charge.For each of the negative ions listed in column 1, use the periodic table to find in column 2 the total number of electrons the ioncontains. A given answer may be used more than once. Column 1 Column 2 [ 1] Se2 [a] 18 [ 21 S2 [b] 35 [ 31 P3 [c] 52 [ 4] O2 [d] 34 [ 5] N3 [e]36 [6] I [f] 54 [7] F [g] 10 [8] Cl [h]9 [9] Br [i] 53 [101 At [j] 86For each of the following processes that show the format ion of ions, complete the process by indicating the number of electrons that must be gained or lost to form the ion. Indicate the total number of electrons in the ion, and in the atom from which it was made. AlAl3+d.FF SS2e.ZnZn2+ CuCu+f.PP3For each of the following atomic numbers, use the periodic table to write the formula (including the charge) for the simpleionthat the element is most likely to form. a. 36 d. 81 b. 31 e. 35 c. 52 f. 87For the following pairs of ions, use the principle of electrical neutrality to predict the formula of the binary compound that the ions are most likely to form. Na+andS2e.Cu2+andBr K+andClf.Al3+andI Ba2+andO2g.Al3+andO2 Mg2+andSe2h.Ca2+andN379AP80AP81AP82AP83APName each of the following compounds. Fe(C2H3O2)3d.SiBr4 BrFe.Cu(MnO4)2 K2O2f.CaCrO485AP86APWrite the foḿu1a for each of the following chromium-containing ions, including the overall charge of the ion. a. chromous c. chromic b. chromate d. dichromateGive the name of each of the following polyatomic anions. a.CO32d.PO43 b.ClO32e.ClO4 c.SO42f.MnO489AP90AP91AP92AP93APComplete the following table to predict whether the given atom will gain or lose electrons in forming the ion most likely to form when in ionic compounds. Atom Gain (G) or Lose (L) Electrons Ion Formed K Cs Br S Se95CP96CP97CP98CP1CR2CR3CRWithout consulting your textbook or notes, state as many points as you can of Dalton’s atomic theory. Explain in your own words each point of the theory.