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Nomenclature and writing chemical equations
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Naming Binary Compounds
TYPE 1 – if the compounds contain a metal and a non-metal The cation is always named first and the anion second. The cation takes its name from the name of the element (ex: Na+ is sodium) The anion is named by taking its root name and adding “ide”. (ex: Cl- is chloride)
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Examples of Type 1 binary compounds
Ions present Name NaCl Na+, Cl- Sodium Chloride KI K+ , I- Potassium Iodide CaS Ca2+, S2- Calcium sulfide CsBr Cs+, Br- Cesium Bromide MgO Mg2+, O2- Magnesium oxide
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Name the following compounds:
CsF AlCl3 MgI2 ZnS Al2S3 Write the formula of the following compounds: Lithium bromide Magnesium phosphide Strontium oxide Barium chloride
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The cation is named first, the anion is named second.
TYPE 2- if compound contains a metal that can form more than one type of cations (the transitions metals). Examples: Fe2+, Fe3+, Cu2+, Cu1+ The cation is named first, the anion is named second. Because the cation can assume more than one charge, the charge is specified by a Roman numeral in parenthesis. The anion is named as it is with type 1 where the anion ends with “ide”. Examples: Compound Ions present name CuCl Cu+1, Cl-1 Copper (I) Chloride HgO Hg2+, O2- Mercury (II) oxide Fe2O3 Fe3+, O2- Iron (III) oxide
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Name the following compounds:
CoCl3 CuI SnBr4 HgCl2 PbS Write the formula of the following compounds Iron (II) chloride Chromium (III) oxide Gold(III) chloride Lead (IV) bromide
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TYPE 3: compounds that contain only nonmetals
1 Mono 2 Di 3 Tri 4 Tetra 5 Penta 6 Hexa 7 Hepta 8 Octa TYPE 3: compounds that contain only nonmetals RULES The first element is named first, and the full element name is used. The second element is named as though it were an anion. Prefixes are used to denote the number of atoms present. The prefix mono- is never used for naming the first element. Ex: CO is called carbon monoxide, NOT monocarbon monoxide Examples BF3 Boron trifluoride NO Nitrogen monoxide N2O5 Dinitrogen pentoxide
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Naming compounds that contain polyatomic ions
Naming compounds that contain polyatomic ions. These are a group of atoms bound together, with a single overall charge. Examples: NH4+1 – ammonium ion SO sulfate ion NO3-1 – nitrate ion Naming of these compounds follow the same rules as naming type I and type II ionic compounds. Examples: Na2SO4 – sodium sulfate Fe(NO3)3 – Iron (III) nitrate NH4ClO3 – ammonium chlorate
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Name the following compounds:
NH4Cl NaCN K3PO4 Fe2(SO4)3 NaC2H3O2 Write the formula for the following compounds Barium sulfate Copper(II) sulfite Iron (III) nitrate Calcium carbonate Ammonium dichromate
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Naming Acids- In all acids, the cation is always the hydrogen ion, H+
Ternary acids- contains H+ and a polyatomic ion Rule1: If the polyatomic ion ends with “ate”, change the “ate” to “ic” then add the word acid. Example: HNO3- nitric acid Rule2: if it ends with “ite”, change “ite” to “ous” then add the word acid. HNO2- nitrous acid Binary acids- contains H+ and a simple anion Rule: Hydro + name of anion ending in “ic” + “acid” Examples: HCl- hydrochloric acid HF- hydrofluoric acid
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Name the following acids:
HI H2SO4 H3PO4 H2CO3 HF Write the formula of the following compounds: Sulfurous acid Permanganic acid Acetic acid Hypochlorous acid Hydrobromic acid
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OF2 is oxygen difluoride
What are the names of the following compounds? OF2 S4N4 BCl3 OF2 is oxygen difluoride S4N4 is tetrasulfur tetranitride BCl3 is boron trichloride Copyright © Cengage Learning. All rights reserved.
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The formula for carbon disulfide is CS2.
What are the formulas for the following binary molecular compounds? carbon disulfide nitrogen tribromide dinitrogen tetrafluoride The formula for carbon disulfide is CS2. The formula for nitrogen tribromide is NBr3. The formula for dinitrogen tetrafluoride is N2F4. Copyright © Cengage Learning. All rights reserved.
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The anion corresponding to HBrO2 is bromite, BrO2-.
Bromine has an oxoacid, HBrO2, bromous acid (compare to HClO2, chlorous acid). What are the name and formula of the corresponding anion? The anion corresponding to HBrO2 is bromite, BrO2-. Copyright © Cengage Learning. All rights reserved.
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Hydrate A compound that contains water molecules weakly bound in the crystals. The formula of a hydrate is written with a dot before the water molecule(s) included. For example: CuSO45H2O Copyright © Cengage Learning. All rights reserved.
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Hydrates are named using the anhydrous (without water) compound name followed by the prefix for the number of water molecules included and the word “hydrate.” For example: CuSO45H2O is named copper(II) sulfate pentahydrate. Copyright © Cengage Learning. All rights reserved.
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FeSO47H2O is iron(II) sulfate heptahydrate.
A compound whose common name is green vitriol has the chemical formula FeSO47H2O. What is the chemical name of this compound? FeSO47H2O is iron(II) sulfate heptahydrate. Copyright © Cengage Learning. All rights reserved.
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For example: 2Na + Cl2 2NaCl
A chemical equation is the symbolic representation of a chemical reaction in terms of chemical formulas. For example: 2Na + Cl2 2NaCl Reactants are the starting materials; they are written on the left of the equation. Products are the materials at the end of the reaction; they are written on the right of the equation. Copyright © Cengage Learning. All rights reserved.
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This is called balancing the equation.
Because a reaction must accurately describe the chemical reaction, it must be consistent with the law of conservation of mass. When this is not the case, after correct formulas are written for each reactant and product, the coefficients are adjusted so that the same number of each atom is present in both the reactants and the products. This is called balancing the equation. Copyright © Cengage Learning. All rights reserved.
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First, we determine the correct formula for each compound.
For example, the reaction of sodium with chlorine produced sodium chloride. First, we determine the correct formula for each compound. Sodium is Na. Chlorine is Cl2. Sodium chloride is NaCl. Copyright © Cengage Learning. All rights reserved.
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Second, we write the reaction. Na + Cl2 NaCl
Third, we check the number of each atom on each side of the equation. This equation shows two Cl atoms on the reactant side and only one Cl atom on the product side. To balance the Cl atoms, we insert a coefficient of “2” before NaCl on the product side. Na + Cl2 2NaCl Copyright © Cengage Learning. All rights reserved.
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The reaction is now balanced!
Na + Cl2 2NaCl Now the Na are not balanced: there is one on the reactant side and there are two on the product side. To balance Na, we insert the coefficient “2” before Na on the reactant side. 2Na + Cl2 2NaCl The reaction is now balanced! Copyright © Cengage Learning. All rights reserved.
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Tally the number of each atom on each side:
Balance the following equation: CS2 + O2 CO2 + SO2 Tally the number of each atom on each side: C 1 on reactant side; 1 on product side S 2 on reactant side; 1 on product side O 2 on reactant side; 4 on product side Begin by inserting the coefficient “2” before SO2 on the product side. We leave O2 until later because it is an element. Copyright © Cengage Learning. All rights reserved.
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Balance the following equation: NH3 + O2 NO + H2O
Tally the number of each atom on each side: N 1 on reactant side; 1 on product side H 3 on reactant side; 2 on product side O 2 on reactant side; 2 on product side Begin by inserting the coefficient “2” before NH3 on the reactant side and the coefficient “3” before H2O on the product side. We leave O2 until later because it is an element. Copyright © Cengage Learning. All rights reserved.
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N 2 on reactant side; 1 on product side
2NH3 + O2 NO + 3H2O Tally the atoms again: N 2 on reactant side; 1 on product side H 6 on reactant side; 6 on product side O 2 on reactant side; 4 on product side To balance N, insert a “2” before NO: 2NH3 + O2 2NO + 3H2O Copyright © Cengage Learning. All rights reserved.
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Tally the atoms again to double check: 4NH3 + 5O2 4NO + 6H2O
N 4 on reactant side; 4 on product side H 12 on reactant side; 12 on product side O 10 on reactant side; 10 on product side The reaction is now balanced! Copyright © Cengage Learning. All rights reserved.
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Tally the number of each atom on each side:
Balance the following equation: C2H5OH + O2 CO2 + H2O Tally the number of each atom on each side: C 2 on reactant side; 1 on product side H 6 on reactant side; 2 on product side O 3 on reactant side; 3 on product side Begin by balancing H. Insert the coefficient “3” before H2O on the product side. We leave O2 until later because it is an element. Copyright © Cengage Learning. All rights reserved.
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Tally the number of each atom on each side:
C2H5OH + O2 CO2 + 3H2O Tally the number of each atom on each side: C 2 on reactant side; 1 on product side H 6 on reactant side; 6 on product side O 3 on reactant side; 5 on product side To balance C, insert a “2” before CO2. Copyright © Cengage Learning. All rights reserved.
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Tally the number of each atom on each side:
C2H5OH + O2 2CO2 + 3H2O Tally the number of each atom on each side: C 2 on reactant side; 2 on product side H 6 on reactant side; 6 on product side O 3 on reactant side; 7 on product side To balance O, insert a “3” before O2. Copyright © Cengage Learning. All rights reserved.
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Tally the number of each atom on each side:
C2H5OH + 3O2 2CO2 + 3H2O Tally the number of each atom on each side: C 2 on reactant side; 2 on product side H 6 on reactant side; 6 on product side O 7 on reactant side; 7 on product side The reaction is now balanced! Copyright © Cengage Learning. All rights reserved.
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