Section 1 - Chemical Names and Formulas
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| To describe the atomic makeup of compounds, chemists use what | Systematic methods for naming compounds and for writing chemical formulas
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| Chemical formula indicates | The relative number of atoms of each kind in a chemical compound
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| What does the chemical formula reveal in a molecular compound | The number of atoms of each element contained in a single molecule of teh ocmpound
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| The ionic compounds consists of | Lattice of positive and negative ions held together by mutual attraction
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| The chemical formula for an ionic compound represents what one formula | The simplest ratio of the compound's positive ions (cations) and its negative ions (anions).
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| When there is no subscript written next to an atom's symbol, the value of the subscript is | 1
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| By gaining or losing electrons many main-group elements form | ions with noble-gas configurations.
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| Ions formed from a single atom | monatomic ions
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| Rather than gain or lose electrons, atoms of carbon and silicon form | covalent bonds in which they share electrons with other atoms
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| Monoatomic cations are identified by | The element's name
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| How is monatomic anionss named | The ending of the element's name is dropped. The ending ide is added to the root name
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| How is the names and symbols of the common monatomic cations and anions organized | According to their charges
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| Compounds composed of two elements are known as | binary compounds
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| In a binary compound the total number of positive charges and negative charges must | Be equal
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| When writing the formulas for binary ionic compounds the charges of the ions are | Not included in the formula
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| Another name for naming system is | nomenclature
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| The naming system of binary ionic compounds involves | Combining teh names of the compound's positive and negative ions. The name of teh cation is given first, followed by the name of the anion.
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| Write the formula for the binary ionic compound: Potassium and iodine | KI
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| Write the formula for the binary ionic compound: Magnesium and chlorine | MgCl2
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| Write the formula for the binary ionic compound: Sodium and sulfur | Na2S
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| Write the formula for the binary ionic compound: aluminum and sulfur | AI2S3
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| Write the formula for the binary ionic compound: aluminum and nitrogen | AIN
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| Name the binary ionic compounds indicated by: AgCI | silver chloride
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| Name the binary ionic compounds indicated by: ZnO | zinc oxide
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| Name the binary ionic compounds indicated by: CaBr2 | calcium bromide
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| Name the binary ionic compounds indicated by: SrF2 | strontium fluoride
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| Name the binary ionic compounds indicated by: BaO | barium oxide
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| Name the binary ionic compounds indicated by: CaCI2 | calcium chloride
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| To distinquish the ions that are formed from elements that form two or more cations scientists use | The Stock System of nomenclature
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| The Stock System uses what to indicate an ion's charge | A Roman numeral
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| Where is the Roman numeral placed in the Stock System when indicating a charge | The numeral is enclosed in parentheses and placed immediately after teh metal name
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| Names of metals that commonly form only one cation do not include | a Roman Numeral
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| There is no element that commonly forms more than one | monatomic anion
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| Write the formula and give the name for the compounds formed between: Cu2+ and Br- | CuBr2, cooper (II) bromide
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| Write the formula and give the name for the compounds formed between: Fe2+ and O2- | FeO, iron (II) oxide
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| Write the formula and give the name for the compounds formed between: Pb2+ and CI- | PbCI2, lead (II) chloride
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| Write the formula and give the name for the compounds formed between: Hg2+ and S2 | HgS, mercury (II) sulfide
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| Write the formula and give the name for the compounds formed between: Sn2+ and F- | SnF2, tin (II) fluoride
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| Write the formula and give the name for the compounds formed between: Fe3+ and O2-Fe2 | Fe2O3, iron (III) oxide
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| Give the names for the compounds: CuO | copper (II) oxide
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| Give the names for the compounds: CoF3 | cobalt (III) fluoride
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| Give the names for the compounds: SnI4 | tin (IV) iodide
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| Give the names for the compounds: FeS | iron (II) sulfide
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| Polyatomic ions that contain oxygen | oxyanions
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| The name of the ion with the greater number of oxygen atoms ends in | -ate
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| The name of the ion with the smaller number of oxygen atoms ends in | -ite
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| An anion that has one fewer oxygen atom than the -ite anion has is given the prefix | hypo-
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| An anion that has one more oxygen atom than the -ate anion has is given the prefix | per-
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| When multiples of a polyatomic ion are present in a compound the formula for the polyatomic ion is | Enclosed in parentheses
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| Write formula for: sodium iodide | NaI
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| Write formula for: calcium chloride | CaCI2
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| Write formula for: potassium sulfide | K2S
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| Write formula for: lithium nitrate | LiNO3
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| Write formula for: copper (II) sulfate | CuSO4
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| Write formula for: Sodium carbonate | Na2CO3
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| Write formula for: calcium nitrite | Ca(NO2)2
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| Write formula for: potassium perchlorate | KCIO4
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| Ag2 Ag2O | Silver oxide
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| Ca(OH)2 | calcium hydroxide
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| KCIO3 | potassium chlorate
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| NH4OH | ammonium hydroxide
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| Fe2(CrO4)3 | iron (III) chromate
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| KCIO | potassium hypochlorite
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| What do chemist use to nae binary molecules | Two nomenclature systemss
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| The prefix mono- indicates | one oxygen atom
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| The prefix di- indicates | two oxygen atoms
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| The prefix tri - indicates | three
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| The prefix tetra- | Four
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| The prefix penta- | Five
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| The prefix hexa- | Six
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| The prefix hepta- | Seven
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| The prefix octa- | Eight
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| The prefix mona- | Nine
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| The prefix deca- | Ten
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| Name the binary molecular compound: SO3 | sulfur trioxide
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| Name the binary molecular compound: ICI3 | iodine Trichloride
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| Name the binary molecular compound: PBr5 | phosphorus pentabromide
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| Carbon tetraiodide | CI4
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| phosphorus trichloride | PCI3
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| dinitrogen trioxide | N2O3
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| Acids that consist of two elements, usually hydrogen and one of the halogens | Binary acids
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| Acids that contain hydrogen, oxygen, and a third element (usually a nonmetal) | Oxyacids
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| An ionic compound composed of a cation and the anion from an acid is referred to as | salt
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