Podcast
Questions and Answers
What is the name of the acid derived from the anion sulfite (SO3)?
Which of the following acids contains one more oxygen atom than the common acid chloric acid?
What is the correct name for HClO2?
How is the acid with no oxygen, HCl, named?
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What do you call acids that are derived from anions ending in –ite?
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What does the formula H2O represent?
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What is the charge of an atom that loses electrons?
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What is the name for Fe2(SO4)3 using the Stock System?
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Which of the following correctly describes the naming of ionic compounds?
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What is a hydrate?
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Which prefix indicates the presence of five water molecules in copper sulfate?
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Which of the following pairs represents correct application of the crossover rule?
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How is the name of an oxyacid derived from an oxyanion ending in -ite formed?
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When naming ionic compounds with variable oxidation states, what suffix is used for lower oxidation states?
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What is the correct name for CO2 in the context of naming non-metal compounds?
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What is a common property of anhydrous substances?
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Which of the following is the correct name for HCl according to chemical naming conventions?
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What is the oxidation state of iron in Iron (II) chloride?
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In the naming of ionic compounds, how is the name of the anion typically formed?
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What is the suffix change when naming an oxyacid derived from a -ate anion?
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Which of the following compounds contains a tetravalent compound indicated by its prefix?
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Study Notes
Chemical Formulas
- A chemical formula shows the elements present in a compound and their relative proportions.
- The formula H2O represents water, which is composed of hydrogen and oxygen in a 2:1 ratio.
Oxidation Numbers
- Oxidation numbers are positive or negative integers that reflect the charge of an atom in a compound.
- They are used to keep track of the number of valence electrons lost or gained by an atom.
- A positive oxidation number indicates an atom has lost electrons.
- A negative oxidation number signifies an atom has gained electrons.
- For polyatomic ions, the charge of the ion is distinct from the oxidation numbers of the constituent elements.
Naming Ionic Compounds
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Writing Ionic Compound Formulas
- The metal (cation) is written before the non-metal (anion).
- The cross-over rule applies, using the absolute values of the charges (oxidation numbers) of the anion as the subscript for the cation and vice versa.
- Example: NaCl (Sodium chloride), Mg3(PO4)2 (Magnesium phosphate).
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Naming Ionic Compounds
- The name follows the order of the ions in the formula.
- The metal (+ion) name comes first, followed by the non-metal (-ion) name.
- The cation retains the metal's name, while the anion's name is derived by changing the ending to -ide.
- Example: LiBr (Lithium bromide), Na2O (Sodium oxide), AlI3 (Aluminum iodide).
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Naming Ionic Compounds with Variable Oxidation Numbers
- Metals with variable oxidation states can be named using two systems:
- Old System: The Latin name of the cation is modified to end in -ous for the lower oxidation state and -ic for the higher oxidation state.
- Stock System: The English name of the metal is used, with the oxidation state indicated by a Roman numeral enclosed in parentheses.
- Example: FeCl2 (Ferrous chloride or Iron (II) chloride), Fe2(SO4)3 (Ferric sulfate or Iron (III) sulfate).
- Metals with variable oxidation states can be named using two systems:
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Naming Hydrates
- Hydrates are ionic compounds that incorporate water molecules into their solid structures.
- Anhydrous substances are water-free.
- Greek prefixes are used to indicate the number of water molecules in the formula.
- Example: Copper (II) sulfate pentahydrate.
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Naming Compounds with Polyatomic Ions
- Name the first polyatomic ion followed by the second polyatomic ion.
- Example: (NH4)3PO4 (Ammonium phosphate).
Naming Compounds of Non-metals
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Binary Compounds
- The name of the first element (appearing first in the formula) is written first.
- The second part of the name is formed by adding the -ide suffix to the stem of the second non-metal.
- Example: HCl (Hydrogen chloride), H2S (Hydrogen sulfide).
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Compounds with Multiple Non-metals
- Greek prefixes are used to indicate the number of atoms of each element present.
- Example: NO (Nitrogen oxide), CO (Carbon monoxide), NO2 (Nitrogen dioxide), CO2 (Carbon dioxide), N2O (Dinitrogen oxide), CO3 (Carbon trioxide), N2O4 (Dinitrogen tetroxide), SO2 (Sulfur dioxide), SO3 (Sulfur trioxide).
Oxyacids
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Oxyacids are derived from oxyanions.
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Naming Oxyacids
- If the oxyanion name ends in -ate, the oxyacid name will be -ic acid.
- Example: SO42- (Sulfate), H2SO4 (Sulfuric acid)
- If the oxyanion name ends in -ite, the oxyacid name will be -ous acid.
- Example: ClO2- (Chlorite), HClO2 (Chlorous acid)
- If the oxyanion name ends in -ate, the oxyacid name will be -ic acid.
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Prefixes and Suffixes for Oxyacids
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per-ic denotes an acid with one more oxygen atom than the common acid.
- Example: HClO4 (Perchloric acid).
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-ic denotes the common acid.
- Example: HClO3 (Chloric acid).
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-ous denotes an acid with one less oxygen atom than the common acid.
- Example: HClO2 (Chlorous acid).
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hypo--ous denotes an acid with two less oxygen atoms than the common acid.
- Example: HClO (Hypochlorous acid).
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hydro--ic denotes an acid with no oxygen.
- Example: HCl (Hydrochloric acid).
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per-ic denotes an acid with one more oxygen atom than the common acid.
Bases
- Compounds identified by the presence of hydroxide group (OH-)
- To name bases, name the metallic portion first, followed by the word hydroxide.
- Example: KOH (Potassium hydroxide), Fe(OH)2 (Ferrous hydroxide or Iron (II) hydroxide), Fe(OH)3 (Ferric hydroxide or Iron (III) hydroxide).
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Description
This quiz covers essential concepts related to chemical formulas, oxidation numbers, and the naming of ionic compounds. You'll explore how to read and write formulas, understand oxidation states, and apply the cross-over rule in ionic compounds. Ideal for students studying chemistry.