nomenclature chemical names & formulas. introduction to chemical bonding §two types of bonding...
TRANSCRIPT
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Nomenclature
Chemical Names&
Formulas
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Introduction to Chemical Bonding
Two types of Bonding _____________________ - transfer of electrons
_____________________ - sharing of electrons
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Bonding takes place at the __________ energy level, ____ and ____ sublevels.
If there are less than half the electrons between the s and p sublevels, the atom will _________ the electrons.
If there are half or more electrons between the s and p sublevels, the atom will __________ electrons.
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Know the trends on the periodic table for how many electrons will be gained or lost.
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Ionic BondingBecause there is a ____________ of
electrons, elements will lose or gain electrons.
If an element loses or gains electrons, it will then become a charged particle - _________. Positive ion - ________________ Negative ion - _______________
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CationsSubstance that has ________
electrons. The charge is equal to the number of
electrons that are transferred.Ca2+ - calcium that has transferred
two electrons to another substance (anion).
Mg2+ - magnesium that has transferred two electrons to another substance (anion).
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AnionSubstance that has ________ electrons.
The charge is equal to the number of
electrons that are transferred.F1- - fluorine that has accepted one
electron from another substance (cation).
O2- - oxygen that has accepted two electrons from another substance (cation).
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Ionic Size
______________ is a charged particle.All atoms are _________________ – the
protons and electrons are equal to one another.
The only way an atom becomes a charged particle is if it _______________ or ________________ electrons.
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Ionic Size
_______________ – positively charged ions Lost electrons – more _________________ than
______________________ ____________________ tend to lose electrons
________________ – negatively charged ions Gained electrons – more _________________
than ______________________ _______________________ tend to gain
electrons
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Ionic Size - Cations
Cations are ___________ than their parent atoms.
The outermost electron is removed and repulsions are reduced.
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Ionic Size - Anions
Anions are ___________ than their parent atoms.
Electrons are added and repulsions are increased.
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Ions _____________ in size as you go down a column. Due to
increasing value of the energy levels.
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Ionic BondingIonic bonding is the _______________ or _______________ of electrons.
Metals are _______________.Nonmetals are _____________.Hence, ionic bonding will occur between ___________ and _________________.
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Oxidation NumbersPossible _______________ on an element.
Any single element, by itself, has a charge of ____________.
An element takes on a charge when put with other elements.
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Basic Rules of Oxidation NumbersGroup 1 elements are always 1+.Group 2 elements are always 2+.Group 3 elements are always 3+Group 17 elements will be 1-.Group 16 elements will be 2-.Group 15 elements will be 3-.
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Other Elements
Ag = 1+
Zn = 2+ Cd = 2+
Al = 3+ Ga = 3+ In = 3+
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Other Elements with Multiple Charges
Cr2+ and Cr3+
Fe2+ and Fe3+
Co2+ and Co3+
Ni2+ and Ni3+
Cu+ and Cu2+
Sn2+ and Sn4+
Pb2+ and Pb4+
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Writing Formulas from Ions
The total overall charge of a compound is ___________________
Use subscripts to balance the charge to zero.
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Ca2+ and S2-
CaS
Na+ andCl-
NaCl
Ba2+ andN3-
Ba3N2
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Writing Ions from Compounds
Go with what you know.
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MgCl2
Mg2+ and Cl-
CuBr2
Cu2+ and Br-
FeCl3
Fe3+ and Cl-
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Polyatomic IonsMany atomed charged particle
that acts as a single unit.Polyatomic ions have specific
names. Use the names.Common polyatomic ions include:
Nitrate ____________ Sulfate ____________ Phosphate ____________ Carbonate ____________ Hydroxide ____________ Chlorate ____________
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Other Polyatomic Ions
Ammonium NH4+
Permanganate MnO4-
Bromate BrO3-
Iodate IO3-
Acetate C2H3O2-
Chromate CrO42-
Dichromate Cr2O72-
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Changing the Oxygen
Per - _____ - ate _____ -
ate _____ - iteHypo - _____ - ite _____ -
ide
Move down – lose 1 oxygen each step
Move up – gain 1 oxygen each step
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Ba2+ andSO42-
BaSO4
Na+ andClO3-
NaClO3
Fe2+andCO32-
FeCO3
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KNO3
K+ and NO3-
CoSO4
Co2+ and SO42-
LiClO3
Li+ and ClO3-
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More than one of the Polyatomic Ion Needed to
Balance the Charge
If more than one of the polyatomic ions is needed to balance the charge, you must use parentheses ( ) around the ion.
Ba(NO3)2
Ba2+ and NO3-
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Mg2+ and ClO3-
Mg(ClO3)2
Fe3+and SO42-
Fe2(SO4)3
Co3+ and NO3-
Co(NO3)2
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Naming Ionic Compounds
Binary Ionic Compounds - Types 1 & 2 A compound that contains a positive ion (______________) and a negative ion (_______________).
Bi- means two Positive ion is written ___________, negative ion is written ______________ in a chemical formula.
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Type 1 - Binary Ionic Compound
The cation of a Type 1 has only ________ possible charge.
Name the first element (cation) as is.
Name the second element (anion) as is with an ending of “-ide”.
Example: CaCl2
Calcium chloride
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More Examples:
NaBr - ________________MgO - ________________KBr - ________________BaS - ________________
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Type 2 - Binary Ionic CompoundsThe cation has multiple charges -
copper can have a charge of 1+ or 2+.
Determine which charge is being used. Use the anion as the guide.
Name the element as is.Use a Roman numeral to indicate
the charge being used.
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Name the anion as is, using an ending of “-ide” as with Type 1 compounds.
Example: CuCl2
Copper (II) chloride
MnO2 - Manganese (IV) oxide
NiO - Nickel (II) oxide
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Naming Type 1 & 2 with Polyatomic Ions
Form compounds called ______________ compounds - compound that contains atoms of three different elements.
______________________ - many atomed charged particle acting as a single unit. poly - many atomic - atom ion - charged particle
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Type 1 & 2 Compounds with Polyatomic Ions
Name the cation using the rules for Type 1 or Type 2 compounds.
Name the polyatomic ion as is - use the name on the chart.
Examples: NaNO3 - ______________ BaSO4 - ______________
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Name these:LiOH - ________________Mg(NO3)2 - ________________
CrCl3 - ________________
Al2O3 - ________________
CoBr2 - ________________
Fe2O3 - ________________
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Covalent BondingCovalent bonding involves the
________________ of electrons between substances.
________________ - smallest neutral unit of a substance that still has the properties of the substance.
________________ - shows the kinds of numbers of atoms present in a molecule of a compound.
Occurs between ________________ and ________________.
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Because these are molecules and are covalently bonded, ions are ________________ - there is no transferring of electrons to form ions.
Prefixes are used in naming nonmetal-nonmetal compounds.
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Prefixesmono - 1di- - 2tri- - 3tetra- - 4penta- - 5hexa- - 6hepta- - 7octa- - 8nona- - 9deca- - 10
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Prefixes:Only used for nonmetal-nonmetal compounds.
Mono- is never used on the first element.
Second element always has a prefix.
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Naming Molecular CompoundsName the first element as is. If
there is more than one of the first element, you must use a prefix.
Name the second element with a prefix to indicate how many atoms there are and add the ending “-ide”.
Example: CO2 - carbon dioxide
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Name these:N2O- ____________________
PCl3- ____________________
SF6 - ____________________
P4O6 - ____________________
SO2 - ____________________
NO3 - ____________________
SO4 - ____________________
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Naming AcidsWhen dissolved in water, certain
molecules produce ____________________ - H+.
These substances are called ____________________.
An acid can be viewed as a molecule with one or more H+ ions attached to an anion.
The rules for naming acids depend on whether the anion contains ____________________.
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Naming AcidsIdentify the compound as being
an acid - the first element is hydrogen (two exceptions are H2O and H2O2)
Find the anion on the chart.Name the anion.Following across to the name of
the acid.Name the acid.
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Naming Acids
If you move up the chart, you ____________________ oxygen.
If you move down the chart, you ____________________ an oxygen.
Start with what you know - usually the -ate group.
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Examples:HCl
The chloride ion (anion) is a single element and ends in “-ide”.
It is at the bottom of the chart.
Move across and the name of this acid is hydrochloric acid.
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H3PO4
The anion is phosphate. Move across to the acids and the name of this acid is phosphoric acid.
H2SO4
The anion is sulfate. Move across to the acids and the name of this acid is sulfuric acid.
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HClO2
Identified as an acid. The anion is ClO2
1-, which is one less oxygen than chlorate, ClO3
1-. Lose an oxygen, move down the chart.
Move down the chart and the name of the anion is chlorite.
Move across to the acid and the name of this acid is chlorous acid.
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Name these:HNO3 - ________________
H2CO3 - ________________
H2SO3 - ________________
HNO2 - ________________
HC2H3O2- ________________
HClO4 - ________________
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Name these Compounds
LiOH ___________________CuBr2 ___________________
H2S ___________________
Na2SO3 ___________________KI ___________________CCl4 ___________________
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Na2SO4
Cu(ClO4)2
N2O5
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MgI2
Sr(NO2)2
HgCl2
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CaCO3
PbC2O4
Cr2(Cr2O7)3
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Iron (III) chromate
Potassium hydroxide
Triphosphorus hexaoxide
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Potassium thiocyanate
Silver nitrate
Aluminum sulfite
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Carbon disulfide
Ammonium sulfate
Nickel (II) chromate
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Xenon tetraoxide
Phosphorus trihydride
Potassium carbonate
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Disulfur dichloride
Lithium oxide
Cobalt (III) hydroxide
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Sodium hydroxide
Dinitrogen monoxide
Ammonium nitrate