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Advanced Physical Science B. Chemistry in Review: The Ions Chemical Formulas Chemical Equations Stoichiometry. The Ions. Ions. In general ions are formed from that lose or gain enough electrons to gain a full octet in their valence shell.

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Advanced Physical Science B

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Advanced physical science b

Advanced Physical Science B

Chemistry in Review:

The Ions

Chemical Formulas

Chemical Equations

Stoichiometry


The ions

The Ions


Advanced physical science b

Ions

  • In general ions are formed from that lose or gain enough electrons to gain a full octet in their valence shell.

  • Elements that lose electrons become a positive CATION.

  • Elements that gain electrons become a negative ANION.


Oxidation numbers

Oxidation Numbers


Monatomic cations

Monatomic Cations

  • Monatomic- one type of atom.

  • Most metals make monatomic cations, with a positive charge.

  • Usually the group number indicates the oxidation number of the elements in that group.

  • The cation simply has the same name as the element.

  • Transition Metals have multiple oxidation numbers.


Elements with multiple charge

Cu+1, Cu+2

Fe+2, Fe+3

Pb+2, Pb+4

Sn+2, Sn+4

Hg2+2, Hg+2

Cuprous, cupric

Ferrous, ferric

Plumbous, plumbic

Stannous, stannic

Mercurous, mercurric

High -ic and Low -ous!

Elements with Multiple Charge


Monatomic anion

Monatomic Anion

  • Monatomic- single type of atom.

  • Anions are usually made from Nonmetals, groups 15, 16, and 17. They gain electrons in their Valence.

  • All Anions end with a suffix.

  • Most monatomic anions end with a “-ide”.


Polyatomic cations

Polyatomic Cations

  • Polyatomic- more than one atom.

  • There just a few polyatomic cations.

    • NH4+, ammonium

    • Hg2+2, mercury(I)


Polyatomic anions

Polyatomic Anions

  • Polyatomic anions have more than one atom.

  • A nonmetal plus oxygen or oxygen and hydrogen.

    • Sometimes called an “oxyanion.”

  • Anions end with a suffix.

    • Most end with “-ate”

    • Polyatomic anions with less oxygens end with “-ite”

  • “ite” anions usually have one less oxygen then “ate” anions.

  • “ate” ate the “ite”!


Chemical formulas

Chemical Formulas

The building blocks.


Symbols and formulas

Symbols and Formulas

  • Names of Elements - 109 elements, >10 million known compounds

  • Compounds are represented by formulas combining chemical symbols and numeric subscripts.

  • Some elements are named for their properties.

    • Nitrogen-“niter forming”

    • Plumbic (lead)-shiny

  • Some elements are named for their place of origin.


Symbols and formulas cont 2

Symbols and Formulas (cont.2)

  • Some elements are named for the minerals they are found in.

    • Tungsten-Swedish name for “heavy stone”

  • Some elements are named in honor of a person.

  • Symbols for the elements

  • One or two letters, the first letter is capitalized

  • In 1813, JJ Berzelius, a Swedish chemist developed the modern symbols for designated elements.


Chemical formulas1

Chemical Formulas

  • Are a combination of symbols that represent the composition of a compound.

  • Molecular Compounds and Ionic Compounds.


Ionic compounds

Ionic Compounds

  • Are compounds composed of charged particles.

  • In general: the electrons are shared between the ions. Metals tend to give up their electrons to an incomplete nonmetal.

  • All Ionic compounds are represented by their empirical formulas. They are always in the smallest whole number ratios.


Other types of molecules

Other Types of Molecules

  • Diatomic Molecules:these 7 elements must exist in nature paired with itself or other elements.

    • Br2, Bromine - O2, Oxygen

    • I2, Iodine - H2, Hydrogen

    • Cl2, Chlorine - N2, Nitrogen

    • F2, Fluorine

  • “BrIClFOHN”


Other types of molecules cont 2

Other Types of Molecules (cont.2)

  • Hydrates:Ionic Molecules attached to water molecules.

  • Organic Molecules:contains carbon as it’s central element.

  • Alloys: metals form these molecules where atoms are held together by a “sea” of electrons.


Predicting formulas of ionic compounds

Predicting Formulas of Ionic Compounds

  • Write the symbols for the elements in the compound

    • Always write the CATION first.

  • Determine the charge on each ion.

    • Na+1=+1, O-2=-2

  • From the charge on each ion use subscripts to indicate the multiplier for the ions.

    • The total positive must equal the total negative.

    • The “total” charge of the compound must be zero.

    • Ex. Na2O


Predicting formulas of ionic compounds cont 2

Predicting Formulas of Ionic Compounds (cont.2)

  • When using subscripts for polyatomic ions, the ion is placed in parentheses, and the subscript is placed on the outside to indicate “x” ion units.

    • The subscript applies to all the elements in the parentheses.

  • If the subscript is “1”, it is understood and not written.

    • For monatomic ions no parentheses is used.


Naming ionic compounds

Naming Ionic Compounds

  • Naming Binary Ionic Compounds:

  • The cation is listed first, then the monatomic anion.

  • For stock names include the oxidation number of the cation in parantheses.

  • For traditional names use the “-ous” or “-ic” name for the cation.


Naming ionic compounds cont 2

Naming Ionic Compounds (cont.2)

  • Naming Ternary Ionic Compounds:

  • Made up with a cation and a polyatomic anion.

  • The suffix tells which anion.

    • “-ate” for more oxygen's

    • “-ite” for less oxygen's.


Chemical equations

Chemical Equations

A chemical recipe


Types of chemical reactions

Types of Chemical Reactions

  • There are 5 fundamental types of Chemical Reactions.

    • Synthesis (Direct Combination)

    • Decomposition (Analysis)

    • Single Replacement

    • Double Replacement

    • Combustion


Synthesis direct combination

Synthesis(Direct Combination)

  • “joining together”

    • The general form of reaction:

      • A + B AB

      • element+element compound

      • Two reactants One product


Synthesis cont 2

Synthesis (cont.2)

O2 + 2NO2NO2


Decomposition analysis

Decomposition (Analysis)

  • “breaking down”

    • The general form of reaction:

      • AB A + B

      • compound element + element

      • One reactant Two products


Decomposition cont 2

Decomposition (cont.2)

2NI3 N2 + 3I2


Single replacement

Single Replacement

  • “Like ions must displace like ions”

    • The general form of reaction:

      • A + BC AC + B

      • element + compound compound + element

      • Two reactants Two products


Single replacement cont 2

Single Replacement (cont.2)

Fe2O3 + 2Al Al2O3 + 2Fe


Double replacement

Double Replacement

  • “Exchanging ions”

    • The general form of reaction:

      • AC + BD AD + BC

      • compound+compound compound+compound

      • Two reactants Two products


Double replacement cont 2

Double Replacement (cont.2)

AgNO3 + NaCl AgCl + NaNO3


Combustion

Combustion

  • Special form of a decomposition rxn.

  • Burning hydrocarbons.

    • Metabolism

    • The general form of reaction:

      • hydrocarbon + oxygen CO2 + H2O

      • Presence of oxygen in the form, O2

      • Products are always CO2 and H2O


Combustion cont 2

Combustion (cont.2)

2C8H18 + 17O2 18H2O + 8CO2


Special considerations for replacement reactions

Special Considerations for Replacement Reactions

  • Single Replacement Reactions: follow the “Activity Series” of elements.

    • Cations displace cations.

    • Anions displace anions.

    • Li+1 is the most reactive cation.

    • F-1 is the most reactive anion.

  • Double Replacement Reactions: must show evidence of a chemical reaction.

    • “God Punishes Chemistry Teachers”

    • Gas, Precipitate, Color change, Temperature change.


Atom accounting

Atom Accounting

  • Reactants-a starting substance in a chemical reaction.

  • Products-a substance produced in a chemical reaction.

  • Atoms in the reactants must equal the atoms in the products.


Balancing chemical equations

Balancing Chemical Equations

  • Do an “Atom Accounting”

    • H2 + N2 NH3

      H=2H=3

      N=2N=1

    • Li + Al2(SO4)3 Li2SO4 + Al

      Li=1Li=2

      Al=2Al=1

      S=3S=1

      O=12O=4


Balancing basics

Balancing Basics

  • Rules for Balancing Chemical Equations:

    • Law of Conservations of Matter: “What goes IN must come OUT”

      • Be sure the elements in the products are in the reactants.

    • Make sure COMPOUNDS are good chemical formulas.

      • Use subscripts to make formulas.


Balancing basics cont 2

Balancing Basics (cont.2)

  • Balance the atoms on each side of the equation using COEFFICIENTS.

    • Do NOT Touch the Subscripts!

  • Keep the coefficients in the lowest whole numbered ratios.

    • Ex. 4H2 + 2O2 2H2O

    • Will be:

    • 2H2 + O2 H2O


Balancing basics cont 3

Balancing Basics (cont.3)

  • Balance the equation:

    • 3H2 + N22NH3

      H=2 6H=3 6

      N=2N=1 2


Balancing basics cont 4

Balancing Basics (cont.4)

  • Li + Al2(SO4)3 Li2SO4 + Al

    Li=1Li=2

    Al=2Al=1

    S=3S=1

    O=12O=4

  • 6Li + Al2(SO4)33Li2SO4 + 2Al

    Li=1 6Li=2 6

    Al=2Al=1 2

    S=3S=1 3

    O=12O=4 12


Stoichiometry

Stoichiometry

Mathematical with chemical equations.


Stoichiometry1

Stoichiometry

  • A Chemical Equation gives information about the relative relationship (ratio) between reactants and products in a chemical reaction.

  • Coefficients of a balanced chemical equation gives three pieces of quantitative information about the reactants and the products.

    • The relative number of particles.

    • The relative number of moles.

    • The relative volume of a gas, at the same temperature and pressure.


Stoichiometry cont 2

Stoichiometry (cont.2)

  • When a chemical equation is balanced, the total mass of the reactants equals the total mass of the products. (Law of Conservation of Mass)

    • The coefficients DO NOT give relative ratios of reactants to products by mass.

    • Must convert to MOLE or particles the compare coefficients.


Stoichiometry cont 3

Stoichiometry (cont.3)

  • Organization is critical.

    • Balance the chemical equation, FIRST!

    • Determine the element/compounds that is given and the element/compound that is sought. Make a chart.

    • Place the information given in the problem under the correct element/compound.


Extended mole map

Extended Mole Map


Mixed stoichiometric relationship

Mixed Stoichiometric Relationship

  • In general, this relationship holds:

    • All mixed relationship problems take 3 steps.

    • First, always balance the chemical equation and organize the problem. Determine what is Given and what if Sought.

    • Convert Given to moles, Change Given to Sought, Convert from Sought moles to whatever units asked for.

      • Remember:

      • If changing to/from mass: 1mol=Molar Mass

      • If changing to/from particles: 1mol=6.02x1023parts

      • If changing to/from volume(gases only): 1mol=22.4dm3 at STP


Mixed stoichiometric relationship cont 2

Mixed Stoichiometric Relationship (cont.2)

  • MOLES RULE!!!

  • In One DA Table:

    Xunit,Sought = Given,units CF1 CF2 CF3

    • Where:

      • CF1=converts units Given to moles

      • CF2=converts moles Given to moles Sought. The Mole Bridge.

      • CF3=converts moles Sought to units Sought.


Try this mass mass problem

Try this mass-mass problem:

  • Calculate the mass of oxygen produced if 2.50g of potassium chlorate is completely decomposed to give potassium chloride and oxygen.

    • Balance the Chemical Equation:

      • 2KClO3 2KCl + 3O2

  • Determine the Given and the Sought:

    • Given: 2.50g KClO3

    • Sought: mass of O2 produced

  • Organize the appropriate information:

    • 2.50g KClO3 Xg O2


  • In one step

    In One Step

    • Calculate the mass of oxygen produced if 2.50g of potassium chlorate is completely decomposed to give potassium chloride and oxygen..

      • The balanced chemical equation:

    • 2KClO3 2KCl + 3O2

    • XgSought =Givenmass 1molGiven Mole MolarMassSought

      MolarMassGiven Bridge1mol Sought

    • XgO2 = 2.50gKClO3 1molKClO3 3O2 32gO2

      123gKClO3 2KClO3 1molO2

      = 9.76x10-1gO2


    2 try this

    #2 Try this:

    • How much silver phosphate is produced if 10.0g of silver acetate reacts with sodium phosphate?

      • Balance the Chemical Equation.

      • Organize the problem.

      • Use Three or One Step to solve the problem.


    How much silver phosphate is produced if 10 0g of silver acetate reacts with sodium phosphate

    How much silver phosphate is produced if 10.0g of silver acetate reacts with sodium phosphate?

    3AgC2H3O2+ Na3PO4 Ag3PO4+ 3 NaC2H3O2

    10.0gAgC2H3O2 XgAg3PO4

    XgAg3PO4=10.0gAgAce 1AgAce 1Ag3PO4 418.58gAg3PO4

    166.92gAgAce 3AgAce 1Ag3PO4

    X= 8.36gAg3PO4


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