Download - Compounds and Molecules
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Compounds and Molecules
4.1vid
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What are compounds?
Two or more elements chemically combined to form new substances.
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What are compounds?
Chemical Bonds – the attractive forces that hold different atoms or ions together
Bonds distinguish compounds from mixtures.
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Chemical FormulaC12H22O11 can only be sugar
H20 can only be water
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Parts to the Formulas
2H2O
Coefficient Subscript
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Parts to the Formulas
Coefficient – gives the amount of molecules or moles
Subscript – tells the number of atoms or ions
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Chemical StructureBond length
-the distance between two bonded atoms
Bond angle-the angle formed between two bonded atoms
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Models of compounds
Ball and stick model-atoms are represented balls, bonds are represented by sticks.
O
H H
Bond length
Bond Angle
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Models of compounds
Structural formulas-chemical symbols represent the atoms.
H HO
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Models of compounds
Space-filling-show the space occupied by each atom represented in the compound. Hydrogen
Oxygen
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Structure of Compounds Network Structures = strong solids
Molecules= weak solids, liquids, or gases
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Ionic and Covalent Bonding
4.2
fun
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Why Bond?Atoms bond so they can become stable!
They want to achieve a full outer energy level
They want 8 electrons.
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1. Ionic bond
A bond formed by the attraction between oppositely charge ions.
The joining of a positive metal ion and a negative nonmetal ionNa+ + Cl- NaCl
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Ionic bond Formed by transferring electrons
Now each ion will have 8 valence electrons
Na+ + Cl- NaCl
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Ionic bond PropertiesThey form network structureshigh melting pointsGood conductors of electricity when dissolved or melted because of their ions
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Metallic bond
Formed by the attraction between positively charged metal ions and the electrons around them.
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Metallic bond
Held together by free flowing electrons
Hold metallic elements together
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Covalent Bonds
Formed when atoms share one or more valence electrons
Formed between non-metals
May form single, double, or triple bonds
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Covalent Properties
They are poor conductors of electricity (no ions)
Low melting points.form molecules
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Polyatomic ion An ion made of two or more atoms
that are covalently bonded and that act like a single ion.
A molecule with a charge Examples: carbonate (CO3)-2
Nitrate (NO3)-1
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Fun
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Compound Names and Formulas
4.3
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REMEMBER!!!!!!!! If it starts with metal it is an ionic
compound If it starts with a nonmetal it is a covalent
compound If the formula contains a parentheses
(polyatomic ion) it contains both ionic and covalent bonds
If it is just a metal it is metallic
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Writing Ionic FormulasCalcium Fluoride Step 1 - Look up both positive and negative ions
Ca2+ F-1
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Writing Ionic CompoundsStep 2Criss-cross numbers down, making subscripts
Ca2+ F-1
Ca1 F2
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Writing Ionic Compounds
Step 3Combine your new compound.
Ca1 + F2 Ca1F2
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Polyatomic ion
Al+3 (CO3)-2
Al2 (CO3)3
Al2(CO3)3
Aluminum Carbonate
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Naming Ionic Compounds
Step one – Name the first ion in the formulaEx. CaCl2 – calcium
Na2(SO4) - sodium
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Naming Ionic Compounds
Step two – Name the second ion Ex. CaCl2 –Calcium Chloride Na2(SO4)-sodium sulfate
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PROBLEMEx. Fe2O3 and FeO are different compounds from different ions
Fe3+ O2- = Fe2O3
Fe2+ O2- = FeO
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Solution-Roman Numerals
Same naming schemeAdd a Roman Numeral to
identify the charge of the metal ion.
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Solution-Roman Numerals Fe2O3 = iron(III)Oxide
FeO = iron(II)OxideRemember!!!
R.N. is the charge, not the subscript of the metal.
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Naming Covalent Compounds
Mono – 1 Di - 2 Tri - 3 Tetra - 4 Penta - 5
Hexa – 6Hepta - 7Octa - 8Nona - 9Deca - 10
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Naming Covalent Compounds
Step 1Identify the number of atoms in the first elementEx. H2O two H atoms
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Naming Covalent Compounds
Step 2Identify the number of atoms in the 2nd element.
Ex. H2O one O atom
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Naming Covalent Compounds
Step 3Name the compound with the appropriate prefixes. Ex. H2O
dihydrogen monoxygen
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Naming Covalent Compounds
Step 4 add an -ide ending to the second element
Ex. Dihydrogen monoxide
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Empirical FormulaThe simplest chemical formula
of a compound.Different covalent compounds
can have same empirical formula
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Ch. 4.4