1. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Table of Contents Chapter 5 Ions and Ionic Compounds Section 1 Simple Ions Section 2 Ionic Bonding and Salts Section 3 Names and Formulas of Ionic Compounds

2. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Bellringer Review the properties and atomic structures of the noble gas (Group 18) elements. What do the electron configurations of these elements have in common? Section 1 Simple Ions Chapter 5

3. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Objectives Relate the electron configuration of an atom to its chemical reactivity. Determine an atom’s number of valence electrons, and use the octet rule to predict what stable ions the atom is likely to form. Explain why the properties of ions differ from those of their parent atoms. Section 1 Simple Ions Chapter 5

4. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chemical Reactivity How much an element reacts depends on the electron configuration of its atoms. For example, oxygen will react with magnesium. In the electron configuration for oxygen, the 2p orbitals, which can hold six electrons, have only four: [O] = __________ Neon has no reactivity. Its 2p orbitals are full: [Ne] = __________ Section 1 Simple Ions Chapter 5

5. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chemical Reactivity, continued Noble Gases Are the Least Reactive Elements Neon is a _______________. The noble gases, which are found in Group ___ of the periodic table, show almost no chemical __________. The noble gases have filled _________ energy levels. This electron configuration can be written as ns 2 np 6 where n represents the __________ energy level. Section 1 Simple Ions Chapter 5

6. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chemical Reactivity, continued Noble Gases Are the Least Reactive Elements, continued The eight electrons in the outer energy level fill the s and p orbitals, making these noble gases stable. In most chemical reactions, atoms tend to match the s and p electron configurations of the noble gases. This tendency to have either empty outer energy levels or full outer energy levels of eight electrons is called the octet rule. Section 1 Simple Ions Chapter 5

7. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chemical Reactivity, continued Alkali Metals and Halogens Are the Most Reactive Elements An atom whose outer s and p orbitals do not match the electron configurations of a noble gas will react to ______ or _____ electrons so the outer orbitals will be __________. When added to water, an atom of potassium (an alkali metal) gives up ___ electron in its _____ energy level. Then, it has the s and p configuration of a _________. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 1s 2 2s 2 2p 6 3s 2 3p 6 Section 1 Simple Ions Chapter 5

8. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chemical Reactivity, continued Alkali Metals and Halogens Are the Most Reactive Elements, continued Chlorine, a __________, is also very reactive. An atom of chlorine has _______ electrons in its outer energy level. By gaining just ___ electron, it will have the s and p configuration of a __________. 1s 2 2s 2 2p 6 3s 2 3p 5 1s 2 2s 2 2p 6 3s 2 3p 6 Section 1 Simple Ions Chapter 5

9. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Valence Electrons Potassium after it loses ____ electron has the same electron configuration as chlorine after it gains one. Both are the same as that of the noble gas argon. [Ar] = 1s 2 2s 2 2p 6 3s 2 3p 6 The atoms of many elements become ________ by achieving the electron configuration of a noble gas. The electrons in the outer energy level are known as ___________ electrons. Section 1 Simple Ions Chapter 5

10. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Valence Electrons, continued Periodic Table Reveals an Atom’s Number of Valence Electrons To find out how many valence electrons an atom has, check the ____________________. For example, the element magnesium, Mg, has the following electron configuration: [Mg] = [Ne]3s 2 This configuration shows that a magnesium atom has two valence electrons in the ____s orbital. Section 1 Simple Ions Chapter 5

11. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Valence Electrons, continued Atoms Gain Or Lose Electrons to Form Stable Ions All atoms are __________ because they have equal numbers of __________ and ___________. For example, a potassium atom has ___ protons and ___ electrons. After giving up one electron, potassium still has ___ protons but only ___ electrons. Because the numbers are _______ the same, there is a net __________ charge. Section 1 Simple Ions Chapter 5

12. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Valence Electrons, continued Atoms Gain Or Lose Electrons to Form Stable Ions, continued An ______ is an atom, radical, or molecule that has _________ or _________ one or more electrons and has a _________ or _________ charge. The following equation shows how a potassium atom forms an ion with a 1+ charge. K → K + + e − An ion with a positive charge is called a _________. Section 1 Simple Ions Chapter 5

13. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Valence Electrons, continued Atoms Gain Or Lose Electrons to Form Stable Ions, continued In the case of chlorine, far less energy is required for an atom to gain _______ electron rather than give up its ______ valence electrons to be more stable. The following equation shows how a chlorine atom forms an ion with a 1− charge. Cl + e − → Cl − An ion with a negative charge is called an _________. Section 1 Simple Ions Chapter 5

14. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Valence Electrons, continued Characteristics of Stable Ions Both an _______ and its _______ have the same number of _______ and _______, so the nuclei are the same. The chemical properties of an atom depend on the number and configuration of its _____________. Therefore, an atom and its ion have different ___________ properties. Section 1 Simple Ions Chapter 5

15. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Valence Electrons, continued Many Stable Ions Have Noble-Gas Configurations Many atoms can form stable ions with a full octet. For example, Ca, forms a stable ion. The electron configuration of a calcium atom is: [Ca] = _______________ By giving up its two valence electrons in the 4s orbital, it forms a stable cation with a 2+ charge: [Ca 2+ ] = _______________ This electron configuration is like that of argon. Section 1 Simple Ions Chapter 5

16. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Valence Electrons, continued Some Stable Ions Do Not Have Noble-Gas Configurations Not all stable ions have an electron configuration like those of noble gases. Transition _______ often form ions without complete ________. With the lone exception of rhenium, Re, the stable transition metal ions are all _________. Also, some elements, mostly _________ metals, form stable ions with more than _____ charge. Section 1 Simple Ions Chapter 5

17. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Atoms and Ions Both sodium and chlorine are very reactive. When they are mixed, a violent reaction takes place, producing a white solid—table salt (sodium chloride). It is made from sodium _______ and chloride _______. Ions and Their Parent Atoms Have Different Properties Having __________ electron configurations does not mean that a sodium cation is a neon atom. They still have different numbers of _______ and _______. Section 1 Simple Ions Chapter 5

18. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Atoms and Ions, continued Atoms of Metals and Nonmetal Elements Form Ions Differently Nearly all metals form ________. For example, magnesium metal, Mg, has the electron configuration: [Mg] = _______________ To have a noble-gas configuration, the atom must either gain ____ electrons or lose ____. Losing two electrons requires ______ energy than gaining six. Section 1 Simple Ions Chapter 5

19. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Atoms and Ions, continued Atoms of Metals and Nonmetal Elements Form Ions Differently, continued The atoms of all nonmetal elements form ______. For example, oxygen, O, has the electron configuration: [O] = _______________ To have a noble-gas configuration, an oxygen atom must either gain ____ electrons or lose ____. Acquiring two electrons requires _______ energy than losing six. Section 1 Simple Ions Chapter 5

20. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Bellringer Review the concepts of ionization energy, electron affinity, anion formation, cation formation, and vaporization. Write down whether each of these processes involves the gain or loss of energy. Section 2 Ionic Bonding and Salts Chapter 5

21. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Objectives Describe the process of forming an ionic bond. Explain how the properties of ionic compounds depend on the nature of ionic bonds. Describe the structure of salt crystals. Section 2 Ionic Bonding and Salts Chapter 5

22. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Ionic Bonding Pyrite is a mineral that is shiny like gold, but it is made of iron __________ and sulfur __________. Because _______ charges attract, cations and anions _______ one another and an ______ bond is formed. The iron cations and sulfur anions of pyrite attract one another to form an ionic _______________. Section 2 Ionic Bonding and Salts Chapter 5

23. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Ionic Bonding, continued Ionic Bonds Form Between Ions of Opposite Charge When sodium and chlorine react to form sodium chloride, sodium forms a stable ____ + cation and chlorine forms a stable ____ − anion. The force of _________ between the 1+ charge on the sodium cation and the 1− charge on the chloride anion creates the ________ bond in sodium chloride. Sodium chloride is a _________, the scientific name given to many different ionic compounds. Section 2 Ionic Bonding and Salts Chapter 5

24. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Ionic Bonding, continued Ionic Bonds Form Between Ions of Opposite Charge, continued All salts are electrically ________ ionic compounds that are made up of cations and anions held together by ionic bonds in a simple, whole-number ratio. However, the _________ between the ions in a salt do not stop with a single cation and a single anion. One cation attracts _________ anions, and one anion attracts _________ cations. They are all pulled together into a tightly packed __________ structure. Section 2 Ionic Bonding and Salts Chapter 5

25. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Ionic Bonding, continued Transferring Electrons Involves Energy Changes Ionization energy is the energy that it takes to _________ the outermost electron from an atom. The equation below shows this process for sodium. Na + __________ → Na + + e − With some elements, such as chlorine, energy is __________ when an electron is added. Cl + e − → Cl − + ____________ Section 2 Ionic Bonding and Salts Chapter 5

26. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Ionic Bonding, continued Transferring Electrons Involves Energy Changes, continued The energy __________ when chlorine accepts and electron is less than the energy required to remove an electron from a sodium atom. __________ and __________ electrons is only part of forming an ionic bond. The rest of the process of forming a salt supplies enough energy to make up the difference so that the overall process ____________ energy. Section 2 Ionic Bonding and Salts Chapter 5

27. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Ionic Bonding, continued Salt Formation Involves Endothermic Steps The process of forming the salt sodium chloride can be broken down into five steps. Energy is needed to make solid sodium a gas. Na(solid) + ____________ → Na(gas) Energy is also required to remove an electron from a gaseous sodium atom. Na(gas) + ____________ → Na + (gas) + e − Section 2 Ionic Bonding and Salts Chapter 5

28. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Ionic Bonding, continued Salt Formation Involves Endothermic Steps, continued 3.Chlorine exists as a molecule containing two chlorine atoms. Energy must be supplied to separate the chlorine atoms so that they can react with sodium. Cl–Cl(gas) + ___________ → Cl(gas) + Cl(gas) To this point, the first three steps have all been endothermic. These steps have produced sodium cations and chlorine atoms. Section 2 Ionic Bonding and Salts Chapter 5

29. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Ionic Bonding, continued Salt Formation Also Involves Exothermic Steps 4.An electron is added to a chlorine atom to form an anion. This step __________ energy. Cl(gas) + e − → Cl − (gas) + ___________ When a cation and anion form an ionic bond, it is an __________ process. Energy is released. Na + (gas) + Cl − (gas) → NaCl(solid) + ___________ The last step is the driving force for salt formation. Section 2 Ionic Bonding and Salts Chapter 5

30. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Ionic Bonding, continued Salt Formation Also Involves Exothermic Steps, continued The energy released when ionic bonds are formed is called the __________ energy. This energy is released when the __________ structure of a salt is formed as the separated ions bond. Without this energy, there would not be enough energy to make the overall process ______________. Section 2 Ionic Bonding and Salts Chapter 5

31. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Ionic Bonding, continued Salt Formation Also Involves Exothermic Steps, continued If energy is released when ionic bonds are formed, then energy must be ________ to break these bonds. As sodium chloride dissolves in water, ___________ supplies energy for the Na + and Cl − ions to separate. Because of its much higher lattice ____________, magnesium oxide does not dissolve well in water. There is not enough energy to separate the Mg 2+ and O 2− ions from one another. Section 2 Ionic Bonding and Salts Chapter 5

32. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Ionic Compounds Do Not Consist of Molecules The ratio of cations to anions is always such that an ionic compound has no ___________ charge. Ionic Compounds Water is a __________ compound, so individual water molecules are each made of two hydrogen atoms and one oxygen atom. Sodium chloride is an ionic compound, so it is made up of many Na + and Cl − ions all bonded together to form a crystal. There are ______ NaCl molecules. Section 2 Ionic Bonding and Salts Chapter 5

33. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Ionic Compounds, continued Ionic Compounds Do Not Consist of Molecules, continued Metals and nonmetals tend to form __________ compounds and not __________ compounds. The formula CaO likely indicates an ___________ compound because Ca is a metal and O is a nonmetal. In contrast, the formula ICl likely indicates a _________ compound because both I and Cl are nonmetals. Lab tests are used to confirm such indications. Section 2 Ionic Bonding and Salts Chapter 5

34. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Ionic Compounds, continued Ionic Bonds Are Strong Repulsive forces in a salt crystal include those between __________-charged ions. Each Na + ion __________ the other Na + ions. Each Cl − ion __________ the other Cl − ions. Another repulsive force exists between the electrons of ions that are close together. Attractive forces include those between the positive __________ of one ion and _________ of other ions. Section 2 Ionic Bonding and Salts Chapter 5

35. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Ionic Compounds, continued Ionic Bonds Are Strong, continued __________ forces exist between oppositely charged ions and involve more than a single cation and anion. Six Na + ions surround each Cl − ion and vice versa. As a result, the __________ force between oppositely charged ions is significantly greater in a crystal than it would be if the ions existed only in pairs. Overall, the attractive forces are much stronger than the repulsive ones, so ionic bonds are _______. Section 2 Ionic Bonding and Salts Chapter 5

36. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Ionic Compounds, continued Ionic Compounds Have Distinctive Properties Most ionic compounds have high melting and boiling points because of the ______ attraction between ions. To melt, ions cannot be in fixed locations. Because the bonds between ions are strong, a lot of ______________ is needed to free them. Still more energy is needed to move ions out of the liquid state and cause boiling, so ionic compounds are ____________ gaseous at room temperature. Section 2 Ionic Bonding and Salts Chapter 5

37. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Ionic Compounds, continued Liquid and Dissolved Salts Conduct Electric Current To conduct an electric current, a substance must satisfy two conditions: it must contain _______________ particles those particles must be free to _______________ Ionic solids, such as salts, generally are not conductors because the ions cannot _______________. When a salt melts or dissolves, the ions can move about and are excellent _______________ conductors. Section 2 Ionic Bonding and Salts Chapter 5

38. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Ionic Compounds, continued Salts Are Hard and Brittle Like NaCl, most ionic compounds are hard and brittle. __________ means that the crystal is able to resist a large force applied to it. __________ means that when the applied force becomes too strong to resist, the crystal develops a widespread fracture rather than a small dent. Both properties are due to the patterns in which the cations and anions are _________ in all salt crystals. Section 2 Ionic Bonding and Salts Chapter 5

39. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Ionic Compounds, continued Salts Are Hard and Brittle, continued The ions in a crystal are arranged in a repeating _______________, forming layers. Each layer is positioned so that a cation is next to an anion in the next layer. The attractive forces between opposite charges _______________ motion. As a result, the ionic compound will be ___________. Also, it will take a lot of ____________ to break all the bonds between layers of ions. Section 2 Ionic Bonding and Salts Chapter 5

40. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Ionic Compounds, continued Salts Are Hard and Brittle, continued If a force causes one layer to move, ions of the same charge will be positioned next to each other. The cations in one layer are now lined up with other cations in a nearby layer. The anions are also. Because ______ charges are next to each other, they will _______ each other and the layers will split apart. This is why all salts shatter along a line extending through the crystal known as a ____________ plane. Section 2 Ionic Bonding and Salts Chapter 5

41. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Ionic Compounds, continued How to Identify a Compound as Ionic All ionic compounds are ______ at room temperature. Tap the substance. Ionic compounds do not break apart easily and they fracture into tiny crystals. Heat the substance. Ionic compounds generally have high melting and boiling points. Use a conductivity device to find if the dissolved or melted substance conducts _______________. Dissolved and molten ionic compounds conduct electricity. Section 2 Ionic Bonding and Salts Chapter 5

42. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Salt Crystals Despite their differences, the crystals of all salts are made of simple repeating units. These repeating units are arranged in a salt to form a crystal _____________, the regular pattern in which a crystal is arranged. These repeating patterns within a salt are the reason for the crystal shape that can be seen in most salts. Section 2 Ionic Bonding and Salts Chapter 5

43. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Salt Crystals, continued Crystal Structure Depends on the Sizes and Ratios of Ions Formulas indicate ratios of ions. For example, the formula for NaCl indicates there is a 1:1 ratio of sodium cations and chlorine anions. Within a NaCl crystal, each Na + ion is surrounded by six Cl − ions, and each Cl − ion by six Na + ions. Because the __________ of the crystal do not have this arrangement, they are locations of __________ points. Section 2 Ionic Bonding and Salts Chapter 5

44. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Salt Crystals, continued Crystal Structure Depends on the Sizes and Ratios of Ions, continued The arrangement of cations and anions to form a crystal lattice depends on the ________ of the ions and the ratio of cations to anions. For example, the salt calcium fluoride has one Ca 2+ ion for every two F − ions. The cations and anions in calcium fluoride also have a greater difference in _________ than those in NaCl. Section 2 Ionic Bonding and Salts Chapter 5

45. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Salt Crystals, continued Crystal Structure Depends on the Sizes and Ratios of Ions, continued Because of the _____ differences of its ions and their ratio in the salt, the crystal lattice structure of calcium fluoride is different from that of sodium chloride. Each calcium ion is surrounded by eight fluoride ions. At the same time, each fluoride ion is surrounded by four calcium ions. Section 2 Ionic Bonding and Salts Chapter 5

46. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Salt Crystals, continued Salts Have Ordered Packing Arrangements All salts are made of repeating units. The smallest repeating unit in a crystal lattice is called a ________. The ways in which a salt’s unit cells are arranged are determined by X-ray diffraction _________________. X-rays that strike ions in a crystal are deflected, while X-rays that pass through the crystal form a ________. By analyzing this pattern, scientists can calculate the positions that the ions in the salt must have. Section 2 Ionic Bonding and Salts Chapter 5

47. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Bellringer Put the following names in the correct order: Einstein Albert Marie Madame Curie Carver Washington George Cations and anions can be thought of as the _______ and _______ names, respectively, of ionic compounds. Section 3 Names and Formulas of Ionic Compounds Chapter 5

48. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Objectives Name cations, anions, and ionic compounds. Write chemical formulas for ionic compounds such that an overall neutral charge is maintained. Explain how polyatomic ions and their salts are named and how their formulas relate to their names. Section 3 Names and Formulas of Ionic Compounds Chapter 5

49. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Naming Ionic Compounds Salts that are made of a simple cation and a simple anion are known as binary ionic compounds. The adjective ___________ indicates that the compound is made up of just _____ elements. Rules for Naming Simple Ions Simple cations borrow their names from the names of the elements. For example, K + is known as the potassium ion. Section 3 Names and Formulas of Ionic Compounds Chapter 5

50. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Naming Ionic Compounds, continued Rules for Naming Simple Ions When an element forms two or more ions, the ion names include _________ numerals to indicate charge. For example, the names of the two copper ions are: Cu + copper(I) ionCu 2+ copper(II) ion The name of a simple anion is also formed from the name of the element, but it ends in -_____. For example, Cl − is the chloride ion. Section 3 Names and Formulas of Ionic Compounds Chapter 5

51. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Naming Ionic Compounds, continued The Names of Ions Are Used to Name an Ionic Compound The name of a _________ ionic compound is made up of just two words: the name of the _____________ followed by the name of the ______________. NaCl sodium chlorideCuCl 2 copper(II) ______________ ZnS zinc _____________Mg 3 N 2 magnesium ____________ K 2 O potassium ________Al 2 S 3 aluminum ______________ Section 3 Names and Formulas of Ionic Compounds Chapter 5

52. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Writing Ionic Formulas Ionic compounds have a ____________ of positive and negative charges. Both ions in sodium chloride carry a ________ charge, so there are _______ numbers of the ions Na + and Cl −. The formula for sodium chloride is written as ________ to show this one-to-one ratio. The cation in zinc sulfide has a 2+ charge and the anion has a 2− charge. Thus, the formula ___________ shows a one-to-one ratio of ions. Section 3 Names and Formulas of Ionic Compounds Chapter 5

53. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Writing Ionic Formulas, continued Compounds Must Have No Overall Charge In some ionic compounds, the charges of the cation and anion __________. For example, in magnesium nitride, the Mg 2+ ion, has two positive charges, and the N 3− ion, has three negative charges. The cations and anions must be combined in such a way that there are the _______________ number of negative charges and positive charges. Section 3 Names and Formulas of Ionic Compounds Chapter 5

54. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Writing Ionic Formulas, continued Compounds Must Have No Overall Charge, continued _________ Mg 2+ cations are needed for every _____ N 3− anions for electroneutrality. That way, there are ____ positive charges and ____ negative charges. Subscripts are used to denote ion ____________. Therefore, the formula for magnesium nitride is Mg 3 N 2. Section 3 Names and Formulas of Ionic Compounds Chapter 5

55. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Writing Ionic Formulas, continued Writing the Formula of an Ionic Compound Follow the following steps when writing the formula of a binary ionic compound: Write the __________ and __________ for the cation and anion. The roman numeral shows which cation. Write the symbols for the ions side by side, beginning with the __________. To show it is a neutral compound, look for the ____________ common multiple of the charges on the ions. Section 3 Names and Formulas of Ionic Compounds Chapter 5

56. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Polyatomic Ions Instead of having ions made of a single atom, many ionic compounds have ______ of atoms that are ions. Many Atoms Can Form One Ion A simple ion is _________, which means “one-atom.” A __________ ion is a charged group of two or more bonded atoms that can be considered a single ion. Unlike simple ions, most polyatomic ions are made of atoms of several _______________. Like simple ions, polyatomic ions are either positive or negative charge. Section 3 Names and Formulas of Ionic Compounds Chapter 5

57. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Polyatomic Ions, continued Many Atoms Can Form One Ion, continued Consider the polyatomic ion ammonium, NH 4 +. Ammonium is made of one nitrogen and four hydrogen atoms. They have a total of __ protons but only __ electrons. So the ammonium ion has a ___+ charge overall. This charge is not found on any one atom. Instead, it is __________ across this group of bonded atoms. Section 3 Names and Formulas of Ionic Compounds Chapter 5

58. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Polyatomic Ions, continued The Names of Polyatomic Ions Can Be Complicated The endings -____ and -____ in the name for a polyatomic indicate the presence of oxygen and the number of oxygen atoms present. For example, the formulas for two polyatomic ions made from sulfur and oxygen are Section 3 Names and Formulas of Ionic Compounds Chapter 5 and. The one with less oxygen takes the -____ ending, is named __________. The ion with more oxygen takes the -____ ending, so is named __________.

59. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Polyatomic Ions, continued The Names of Polyatomic Ions Can Be Complicated, continued Section 3 Names and Formulas of Ionic Compounds Chapter 5 The presence of hydrogen is often indicated by an ion’s name starting with hydrogen. The prefixes _______- and _______- are also used. is _____hydrogen phosphate. is ____hydrogen phosphate. The prefix _______- means “replace an oxygen with a sulfur.” K 2 S 2 O 3 is potassium thiosulfate.

60. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Polyatomic Ions, continued Naming Compounds with Polyatomic Ions Follow these steps when naming an ionic compound that contains one or more polyatomic ions: Name the cation. Recall that a cation is simply the name of the _______________. Name the anion. Recall that salts are electrically _________. Name the salt. Recall that the name of a salt is just the names of the _____________ and _____________. Section 3 Names and Formulas of Ionic Compounds Chapter 5

61. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Formula of a Compound with a Polyatomic Ion Sample Problem A What is the formula for iron(III) chromate? Section 3 Names and Formulas of Ionic Compounds Chapter 5

62. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 1.Which of the following can achieve the same electron configuration as a noble gas when the atom forms an ion? A.argon B.iron C.nickel D.potassium Standardized Test Preparation Understanding Concepts Chapter 5

63. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 2.Why is an input of energy needed when forming NaCl? F.to change chlorine to a gas G.to add an electron to the chlorine atom H.to remove an electron from the sodium atom I.to bring together the sodium and the chloride ions Standardized Test Preparation Understanding Concepts Chapter 5

64. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 3.Which of the following is a characteristic of a salt? A.bends but does not shatter when struck sharply B.has the ability to conduct electric current in the solid state C.has the ability to conduct electric current in the liquid state D.melts at temperatures that are slightly higher than room temperature Standardized Test Preparation Understanding Concepts Chapter 5

65. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 4.Which of the following pairs of elements are most likely to form an ionic bond? F.Br and Ca G.Br and N H.Ca and Mg I.Ca and Fe Standardized Test Preparation Understanding Concepts Chapter 5

66. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 5.Explain why only a few metals are found in nature in their pure form, while most exist only as ores, which are metal-containing compounds. Standardized Test Preparation Understanding Concepts Chapter 5

67. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 6.How can you tell from the number of valence electrons whether an element is more likely to form a cation or an anion? Standardized Test Preparation Understanding Concepts Chapter 5

68. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Read the passage below. Then answer questions 7 and 8. In 1980, an oil drilling rig in Lake Peignur in Louisiana opened a hole from the lake to a salt mine 1,300 feet below ground. As the lake water flowed into the mine, it dissolved the salt pillars that were left behind to hold up the ceiling. When the entire mine collapsed, the resulting whirlpool swallowed a number of barges, a tugboat, trucks, and a large portion of an island in the middle of the lake. Eventually, the hole filled with water from a canal, leaving a much deeper lake. Standardized Test Preparation Reading Skills Chapter 5

69. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 7.What was the most likely cause of the collapse of the salt mine? A.The salt melted due to the temperature of the water. B.Water dissolved the ionic sodium chloride, leaving no supports. C.Water is denser than salt, so the salt began to float, moving the columns. D.The open hole exposed the salt pillars to the air and they had a chemical reaction with oxygen. Standardized Test Preparation Reading Skills Chapter 5

70. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 8.When there is no water present, the pillars in a salt mine are capable of holding the weight of the ceiling because F.salt is held together by strong ionic bonds. G.salt melts as it is mined and then reforms to a hard crystal. H.salt contains sodium, which gives it the properties of metal. I.salt does not crumble due to the low temperatures found below ground level. Standardized Test Preparation Reading Skills Chapter 5

71. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Many transition metals are capable of forming more than one type of stable ion. The properties of compounds formed by one ion are often different from those formed by an ion of the same element have a different charge. Use the table below to answer questions 9–12. Standardized Test Preparation Interpreting Graphics Chapter 5

72. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Standardized Test Preparation Interpreting Graphics Chapter 5 9.How do the cations formed by transition metals differ from those formed by metals in the first two columns of the periodic table? A.Transition metals lose more electrons. B.All of the transition metal ions have a positive charge. C.Transition metals generally do not ionize to a noble gas configuration. D.All of the transition metals are capable of forming several different ions.