chapter 20
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Chapter 20. Chemical Bonds. Sec. 1: Stability in Bonding. Atoms from different elements can combine to form compounds. When atoms combine, the compound has different properties than the elements. Ex. Sodium Chloride (table salt) is made of sodium & chlorine. - PowerPoint PPT PresentationTRANSCRIPT
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Chapter 20Chemical Bonds
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Sec. 1: Stability in Bonding
Atoms from different elements can combine to form compounds.
When atoms combine, the compound has different properties than the elements.Ex. Sodium Chloride (table salt) is made of
sodium & chlorine. Sodium is a soft metal that reacts violently
with water.Chlorine is a poisonous greenish-yellow gas.
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FormulasChemical Formula—tells what elements
a compound contains and the exact number of the atoms of each element.Ex. NaCl has 1 atom of sodium & 1 atom of
chlorineEx. H2O has 2 atoms of hydrogen and 1 atom
of oxygen.A subscript (small # written below) is
written after a symbol to tell how many atoms of that element are in the compound.
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Atomic StabilityAtoms combine to form a compound that
is more stable than the separate atoms.Noble gases are already stable and do not
form compounds.Their outer energy level is full of electrons.
Atoms can gain, lose, or share electrons to get a full valence electron shell.
Chemical Bond—the force that holds atoms together in a compound.
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Sodium & ChlorineSodium has 1
valence electron.Chlorine has 7, so
it needs 1 more electron to be stable.
If sodium give its 1 valence e- to chlorine, they are both stable with 8 valence e-.
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Water MoleculeIn water, each
hydrogen atom needs 1 e- to fill its outer shell.
Oxygen needs 2 e- to fill its outer shell.
To be stable, the atoms share electrons.
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Types of BondsIonic Bonds
Contain a metal & a nonmetal (at least 1 of each)
Electrons are gained or lostEx. Salt, NaCl
Covalent BondsContain 2 or more nonmetals or
hydrogenElectrons are sharedEx. Water, H2O
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IonsWhen atoms gain or lose electrons in
an ionic bond, they form ions.Ion—an atom with a positive or
negative charge.You can tell the charge of the ion that
an element will form based on its position on the periodic table.
Polyatomic Ions—ions made of more than one atom.
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Write the charges on you periodic table!!!1+
2+ 3+ 3- 2- 1-
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Types of IonsThere are 2 types of ions: cations &
anions.Cations—ions that have a positive
chargeThey form by atoms losing electronsMetals form cations
Anions—ions that have a negative chargeThey form by atoms gaining electronsNonmetals form anions
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Ionic BondingIn an ionic bond, one atoms gives
electrons to another atom.When atoms combine this way, it is
called a formula unit.Ex. NaCl is a formula unit
The charge of a formula unit is always 0.
The positive and negative charges must always balance each other.
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Oxidation number—the charge of an ion
1+
2+ 3+ 3- 2- 1-
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Multiple Oxidation Numbers
Some metals (other metals & transition metals) can have more than 1 oxidation number.
If an element can have more than 1 oxidation number, the charge of the ion is written as a roman numeral in parentheses.Ex. Copper (I) ion is Cu1+
Copper (II) ion is Cu2+
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Writing Formulas for Ionic Compounds
Write the symbol for the cation (either the metal element symbol or polyatomic ion) firstEx. Mg2+ or NH4
+
Write the symbol for the anion (either the element symbol or polyatomic ion) secondEx. Cl- O2-
Use subscripts to balance the charges of the ions.Ex. KCl, (NH4)2O, MgO, MgCl2
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Balancing Chemical Formulas Practice
http://www.chemfiles.com/flash/formulas.html Write the name of the chemical formula, ions
and charges, and the chemical formulas when you get them balanced for 10 problems!!!!!
Don’t forget subscripts and parenthesis!
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Naming Ionic Compounds
Write the name of the cation first (remember cations are metals)Ex. Ca2+ is calcium
Some elements can have more than 1 charge (see table 2 p. 588)If it does put the charge of the ion
using roman numerals and put it in parentheses.
Ex. Cu2+ Copper (II)
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Ionic Naming ContinuedWrite the name of the anion second, but
change the ending to –ide.Ex. Chlorine becomes Chloride
If the anion is a polyatomic ion DO NOT CHANGE THE ENDING.Ex. NO3
- is still named Nitrate
Put the cation & anion together to get the full name.KI is Potassium IodideCuSO4 is Copper (II) Sulfate
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Covalent BondsCovalent bonds share electronsComposed of 2 or more nonmetals (and H)Covalent compounds are called moleculesMolecules can be polar or nonpolarPolar molecule—slightly positive and negative
at parts—but overall neutrale- are unevenly shared
Nonpolar molecule—electrons are shared equally—completely neutral
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Naming Covalent Compounds
Use prefixes to tell how many of each element you have.This is done because you can have
different covalent compounds containing the same elements.
Change the ending of the 2nd element to -ideEx. N2O is dinitrogen monoxide.
You can leave off the prefix mono- on the first element.Ex. NO2 is nitrogen dioxide
Not mononitrogen dioxide
Mono—1Di—2Tri—3Tetra—4Penta—5Hexa—6Hepta—7Octa—8Nona—9Deca—10
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Formulas for Covalent CompoundsUse the prefixes as the subscript
in the formula.Ex. Phosphorus Trichloride
PCl3Dinitrogen Tetrafluoride
N2F4