Chapter 5: Molecules and Compounds – Structure, Classification, and Nomenclature

{"type":"doc","content":[{"type":"heading","attrs":{"textAlign":null,"level":2},"content":[{"type":"text","text":"Molecules and Compounds"}]},{"type":"heading","attrs":{"textAlign":null,"level":3},"content":[{"type":"text","text":"Introduction to Compounds and Their Properties"}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"Compounds are substances formed from two or more elements combined in fixed, definite proportions. The properties of compounds are often very different from those of the elements that compose them. For example, sucrose (table sugar) is made of carbon, hydrogen, and oxygen, yet its properties differ greatly from those of its constituent elements."}]},{"type":"bulletList","content":[{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Compound:"},{"type":"text","text":" A substance composed of two or more elements chemically combined in fixed ratios."}]}]},{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Element:"},{"type":"text","text":" A pure substance consisting of only one type of atom."}]}]},{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Mixture:"},{"type":"text","text":" A combination of two or more substances in variable proportions, not chemically bonded."}]}]},{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Example:"},{"type":"text","text":" Sucrose contains C, H, and O atoms, but its properties are distinct from graphite (carbon), hydrogen gas, or oxygen gas."}]}]}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"image","attrs":{"src":"https://static.studychannel.pearsonprd.tech/study_guide_files/general-chemistry/sub_images/2fab7f92_image_1.png","alt":"Sucrose molecule and its constituent elements","title":null,"width":null,"height":null}}]},{"type":"heading","attrs":{"textAlign":null,"level":3},"content":[{"type":"text","text":"Properties of Compounds vs. Elements"}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"Compounds display unique properties that are not simply a blend of their constituent elements. For instance, sodium chloride (table salt) is formed from sodium (a reactive metal) and chlorine (a poisonous gas), yet salt is safe and stable."}]},{"type":"bulletList","content":[{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Sodium:"},{"type":"text","text":" Highly reactive metal."}]}]},{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Chlorine:"},{"type":"text","text":" Poisonous yellow gas."}]}]},{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Sodium chloride:"},{"type":"text","text":" Stable, edible compound."}]}]}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"image","attrs":{"src":"https://static.studychannel.pearsonprd.tech/study_guide_files/general-chemistry/sub_images/2fab7f92_image_2.png","alt":"Elemental sodium","title":null,"width":null,"height":null}},{"type":"image","attrs":{"src":"https://static.studychannel.pearsonprd.tech/study_guide_files/general-chemistry/sub_images/2fab7f92_image_3.png","alt":"Elemental chlorine","title":null,"width":null,"height":null}},{"type":"image","attrs":{"src":"https://static.studychannel.pearsonprd.tech/study_guide_files/general-chemistry/sub_images/2fab7f92_image_4.png","alt":"Sodium chloride (table salt)","title":null,"width":null,"height":null}}]},{"type":"heading","attrs":{"textAlign":null,"level":2},"content":[{"type":"text","text":"Law of Constant Composition"}]},{"type":"heading","attrs":{"textAlign":null,"level":3},"content":[{"type":"text","text":"Compounds Display Constant Composition"}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"All samples of a given compound have the same proportions of their constituent elements. This is known as the "},{"type":"text","marks":[{"type":"bold"}],"text":"law of constant composition"},{"type":"text","text":" (Proust's Law)."}]},{"type":"bulletList","content":[{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Mixture:"},{"type":"text","text":" Variable proportions (e.g., a balloon filled with hydrogen and oxygen)."}]}]},{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Compound:"},{"type":"text","text":" Fixed proportions (e.g., water always has a 2:1 ratio of hydrogen to oxygen)."}]}]}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"image","attrs":{"src":"https://static.studychannel.pearsonprd.tech/study_guide_files/general-chemistry/sub_images/2fab7f92_image_5.png","alt":"Mixture of hydrogen and oxygen","title":null,"width":null,"height":null}},{"type":"image","attrs":{"src":"https://static.studychannel.pearsonprd.tech/study_guide_files/general-chemistry/sub_images/2fab7f92_image_6.png","alt":"Water with fixed ratio of hydrogen to oxygen","title":null,"width":null,"height":null}}]},{"type":"heading","attrs":{"textAlign":null,"level":3},"content":[{"type":"text","text":"Mass Ratios in Compounds"}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"The mass ratio of elements in a compound is constant. For example, water decomposes to 16.0 g of oxygen and 2.0 g of hydrogen, giving a mass ratio of 8.0:1."}]},{"type":"bulletList","content":[{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Water:"},{"type":"text","text":" "},{"type":"inlineMath","attrs":{"latex":"\\text{Mass ratio} = \\frac{16.0\\ \\text{g O}}{2.0\\ \\text{g H}} = 8.0"}},{"type":"text","text":" or "},{"type":"inlineMath","attrs":{"latex":"8.0:1"}}]}]},{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Ammonia:"},{"type":"text","text":" "},{"type":"inlineMath","attrs":{"latex":"\\text{Mass ratio} = \\frac{14.0\\ \\text{g N}}{3.0\\ \\text{g H}} = 4.7"}},{"type":"text","text":" or "},{"type":"inlineMath","attrs":{"latex":"4.7:1"}}]}]}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"image","attrs":{"src":"https://static.studychannel.pearsonprd.tech/study_guide_files/general-chemistry/sub_images/2fab7f92_image_7.png","alt":"Mass ratio of elements in water","title":null,"width":null,"height":null}},{"type":"image","attrs":{"src":"https://static.studychannel.pearsonprd.tech/study_guide_files/general-chemistry/sub_images/2fab7f92_image_8.png","alt":"Mass ratio of elements in ammonia","title":null,"width":null,"height":null}}]},{"type":"heading","attrs":{"textAlign":null,"level":2},"content":[{"type":"text","text":"Chemical Formulas"}]},{"type":"heading","attrs":{"textAlign":null,"level":3},"content":[{"type":"text","text":"How to Represent Compounds"}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"Chemical formulas indicate the elements present in a compound and the relative number of atoms of each. Subscripts show the number of atoms; a subscript of 1 is omitted by convention."}]},{"type":"bulletList","content":[{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Example:"},{"type":"text","text":" H2O (water) – 2 hydrogen atoms, 1 oxygen atom."}]}]},{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Example:"},{"type":"text","text":" NaCl (table salt) – 1 sodium atom, 1 chlorine atom."}]}]},{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Example:"},{"type":"text","text":" CO2 (carbon dioxide) – 1 carbon atom, 2 oxygen atoms."}]}]}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"image","attrs":{"src":"https://static.studychannel.pearsonprd.tech/study_guide_files/general-chemistry/sub_images/2fab7f92_image_9.png","alt":"Chemical formula for water","title":null,"width":null,"height":null}}]},{"type":"heading","attrs":{"textAlign":null,"level":3},"content":[{"type":"text","text":"Changing Subscripts Changes the Compound"}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"The subscripts in a chemical formula define the compound. Changing them results in a different compound with different properties."}]},{"type":"bulletList","content":[{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"CO:"},{"type":"text","text":" Carbon monoxide (toxic)."}]}]},{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"CO2:"},{"type":"text","text":" Carbon dioxide (relatively harmless)."}]}]}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"image","attrs":{"src":"https://static.studychannel.pearsonprd.tech/study_guide_files/general-chemistry/sub_images/2fab7f92_image_10.png","alt":"CO and CO2 molecular models","title":null,"width":null,"height":null}}]},{"type":"heading","attrs":{"textAlign":null,"level":3},"content":[{"type":"text","text":"Order of Elements in Chemical Formulas"}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"Formulas list the most metallic element first. In compounds without metals, the more metal-like element is listed first. Table 5.1 shows the order for listing nonmetal elements."}]},{"type":"bulletList","content":[{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Metals:"},{"type":"text","text":" Listed first (e.g., NaCl)."}]}]},{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Nonmetals:"},{"type":"text","text":" Order based on periodic table position."}]}]}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"image","attrs":{"src":"https://static.studychannel.pearsonprd.tech/study_guide_files/general-chemistry/sub_images/2fab7f92_image_11.png","alt":"Order of listing nonmetal elements in a chemical formula","title":null,"width":null,"height":null}}]},{"type":"heading","attrs":{"textAlign":null,"level":3},"content":[{"type":"text","text":"Polyatomic Ions in Chemical Formulas"}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"Some compounds contain groups of atoms (polyatomic ions) that act as a unit. Parentheses and subscripts indicate the number of each group."}]},{"type":"bulletList","content":[{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Example:"},{"type":"text","text":" Mg(NO3)2 contains 1 Mg, 2 NO3 groups (2 N, 6 O)."}]}]}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"image","attrs":{"src":"https://static.studychannel.pearsonprd.tech/study_guide_files/general-chemistry/sub_images/2fab7f92_image_12.png","alt":"Chemical formula for Mg(NO3)2","title":null,"width":null,"height":null}}]},{"type":"heading","attrs":{"textAlign":null,"level":3},"content":[{"type":"text","text":"Types of Chemical Formulas"}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"There are three main types of chemical formulas:"}]},{"type":"bulletList","content":[{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Empirical formula:"},{"type":"text","text":" Shows the simplest ratio of elements (e.g., HO for hydrogen peroxide)."}]}]},{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Molecular formula:"},{"type":"text","text":" Shows the actual number of atoms (e.g., H2O2)."}]}]},{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Structural formula:"},{"type":"text","text":" Shows how atoms are connected."}]}]}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"image","attrs":{"src":"https://static.studychannel.pearsonprd.tech/study_guide_files/general-chemistry/sub_images/2fab7f92_image_13.png","alt":"Color coding for molecular models","title":null,"width":null,"height":null}}]},{"type":"heading","attrs":{"textAlign":null,"level":3},"content":[{"type":"text","text":"Models for Representing Molecules"}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"Molecular models help visualize the structure and geometry of molecules. Ball-and-stick and space-filling models are commonly used."}]},{"type":"bulletList","content":[{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Ball-and-stick model:"},{"type":"text","text":" Atoms as balls, bonds as sticks."}]}]},{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Space-filling model:"},{"type":"text","text":" Atoms fill the space between each other."}]}]}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"image","attrs":{"src":"https://static.studychannel.pearsonprd.tech/study_guide_files/general-chemistry/sub_images/2fab7f92_image_14.png","alt":"Comparison of formulas and models for methane, CH4","title":null,"width":null,"height":null}}]},{"type":"heading","attrs":{"textAlign":null,"level":3},"content":[{"type":"text","text":"Connecting Macroscopic and Molecular Worlds"}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"Chemists use symbolic representations to connect what we see (macroscopic) with the atomic and molecular world."}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"image","attrs":{"src":"https://static.studychannel.pearsonprd.tech/study_guide_files/general-chemistry/sub_images/2fab7f92_image_15.png","alt":"Macroscopic, molecular, and symbolic view of water","title":null,"width":null,"height":null}}]},{"type":"heading","attrs":{"textAlign":null,"level":2},"content":[{"type":"text","text":"Classification of Elements and Compounds"}]},{"type":"heading","attrs":{"textAlign":null,"level":3},"content":[{"type":"text","text":"Pure Substances: Elements and Compounds"}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"Pure substances can be classified as elements or compounds. Elements may be atomic or molecular, while compounds may be molecular or ionic."}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"image","attrs":{"src":"https://static.studychannel.pearsonprd.tech/study_guide_files/general-chemistry/sub_images/2fab7f92_image_16.png","alt":"Classification of elements and compounds","title":null,"width":null,"height":null}}]},{"type":"heading","attrs":{"textAlign":null,"level":3},"content":[{"type":"text","text":"Atomic vs. Molecular Elements"}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"Atomic elements exist as single atoms (e.g., mercury), while molecular elements exist as diatomic molecules (e.g., chlorine)."}]},{"type":"bulletList","content":[{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Atomic element:"},{"type":"text","text":" Basic unit is a single atom."}]}]},{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Molecular element:"},{"type":"text","text":" Basic unit is a molecule (often diatomic)."}]}]}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"image","attrs":{"src":"https://static.studychannel.pearsonprd.tech/study_guide_files/general-chemistry/sub_images/2fab7f92_image_17.png","alt":"Atomic element: mercury","title":null,"width":null,"height":null}},{"type":"image","attrs":{"src":"https://static.studychannel.pearsonprd.tech/study_guide_files/general-chemistry/sub_images/2fab7f92_image_18.png","alt":"Molecular element: chlorine","title":null,"width":null,"height":null}}]},{"type":"heading","attrs":{"textAlign":null,"level":3},"content":[{"type":"text","text":"Elements That Exist as Diatomic Molecules"}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"Some elements naturally occur as diatomic molecules. These include hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, and iodine."}]},{"type":"table","content":[{"type":"tableRow","content":[{"type":"tableHeader","attrs":{"colspan":1,"rowspan":1,"colwidth":null},"content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"Name of Element"}]}]},{"type":"tableHeader","attrs":{"colspan":1,"rowspan":1,"colwidth":null},"content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"Formula of Basic Unit"}]}]}]},{"type":"tableRow","content":[{"type":"tableCell","attrs":{"colspan":1,"rowspan":1,"colwidth":null},"content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"hydrogen"}]}]},{"type":"tableCell","attrs":{"colspan":1,"rowspan":1,"colwidth":null},"content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"H2"}]}]}]},{"type":"tableRow","content":[{"type":"tableCell","attrs":{"colspan":1,"rowspan":1,"colwidth":null},"content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"nitrogen"}]}]},{"type":"tableCell","attrs":{"colspan":1,"rowspan":1,"colwidth":null},"content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"N2"}]}]}]},{"type":"tableRow","content":[{"type":"tableCell","attrs":{"colspan":1,"rowspan":1,"colwidth":null},"content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"oxygen"}]}]},{"type":"tableCell","attrs":{"colspan":1,"rowspan":1,"colwidth":null},"content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"O2"}]}]}]},{"type":"tableRow","content":[{"type":"tableCell","attrs":{"colspan":1,"rowspan":1,"colwidth":null},"content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"fluorine"}]}]},{"type":"tableCell","attrs":{"colspan":1,"rowspan":1,"colwidth":null},"content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"F2"}]}]}]},{"type":"tableRow","content":[{"type":"tableCell","attrs":{"colspan":1,"rowspan":1,"colwidth":null},"content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"chlorine"}]}]},{"type":"tableCell","attrs":{"colspan":1,"rowspan":1,"colwidth":null},"content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"Cl2"}]}]}]},{"type":"tableRow","content":[{"type":"tableCell","attrs":{"colspan":1,"rowspan":1,"colwidth":null},"content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"bromine"}]}]},{"type":"tableCell","attrs":{"colspan":1,"rowspan":1,"colwidth":null},"content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"Br2"}]}]}]},{"type":"tableRow","content":[{"type":"tableCell","attrs":{"colspan":1,"rowspan":1,"colwidth":null},"content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"iodine"}]}]},{"type":"tableCell","attrs":{"colspan":1,"rowspan":1,"colwidth":null},"content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"I2"}]}]}]}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"image","attrs":{"src":"https://static.studychannel.pearsonprd.tech/study_guide_files/general-chemistry/sub_images/2fab7f92_image_19.png","alt":"Table of diatomic elements","title":null,"width":null,"height":null}}]},{"type":"heading","attrs":{"textAlign":null,"level":3},"content":[{"type":"text","text":"Molecular vs. Ionic Compounds"}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"Molecular compounds are formed from two or more nonmetals and consist of molecules. Ionic compounds contain cations (usually metals) and anions (usually nonmetals) arranged in a three-dimensional array."}]},{"type":"bulletList","content":[{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Molecular compound:"},{"type":"text","text":" Basic unit is a molecule (e.g., CO2)."}]}]},{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Ionic compound:"},{"type":"text","text":" Basic unit is a formula unit (e.g., NaCl)."}]}]}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"image","attrs":{"src":"https://static.studychannel.pearsonprd.tech/study_guide_files/general-chemistry/sub_images/2fab7f92_image_20.png","alt":"Molecular compound: dry ice (CO2)","title":null,"width":null,"height":null}},{"type":"image","attrs":{"src":"https://static.studychannel.pearsonprd.tech/study_guide_files/general-chemistry/sub_images/2fab7f92_image_21.png","alt":"Ionic compound: table salt (NaCl)","title":null,"width":null,"height":null}}]},{"type":"heading","attrs":{"textAlign":null,"level":2},"content":[{"type":"text","text":"Writing Formulas for Ionic Compounds"}]},{"type":"heading","attrs":{"textAlign":null,"level":3},"content":[{"type":"text","text":"Rules for Writing Ionic Compound Formulas"}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"Ionic compounds must be charge-neutral. The sum of the charges of the cations and anions must equal zero. The charge of each ion determines the subscripts in the formula."}]},{"type":"bulletList","content":[{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Step 1:"},{"type":"text","text":" Write the symbol and charge for each ion."}]}]},{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Step 2:"},{"type":"text","text":" Use the charge of one ion as the subscript for the other."}]}]},{"type":"listItem","content":[{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","marks":[{"type":"bold"}],"text":"Step 3:"},{"type":"text","text":" Reduce subscripts to smallest whole numbers."}]}]}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"image","attrs":{"src":"https://static.studychannel.pearsonprd.tech/study_guide_files/general-chemistry/sub_images/2fab7f92_image_22.png","alt":"Formula for aluminum oxide","title":null,"width":null,"height":null}},{"type":"image","attrs":{"src":"https://static.studychannel.pearsonprd.tech/study_guide_files/general-chemistry/sub_images/2fab7f92_image_23.png","alt":"Formula for magnesium oxide","title":null,"width":null,"height":null}}]},{"type":"heading","attrs":{"textAlign":null,"level":3},"content":[{"type":"text","text":"Polyatomic Ions in Ionic Compounds"}]},{"type":"paragraph","attrs":{"textAlign":null},"content":[{"type":"text","text":"Polyatomic ions are groups of atoms with an overall charge. 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