atoms want 8ve- to be stable “happy”
DESCRIPTION
Atoms want 8ve- to be stable “happy”. Chemical Bonds / Formulas. Atoms bond to become stable or “happy” – octet rule (full valence shell) When they bond they form compounds. Each compound has a special formula Subscripts show how many of each element is in the compound. FORMULAS. - PowerPoint PPT PresentationTRANSCRIPT
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Atoms want 8ve- to be stable “happy”
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Chemical Bonds / Formulas Atoms bond to become stable or
“happy” – octet rule (full valence shell) When they bond they form
compounds. Each compound has a special
formula Subscripts show how many of each
element is in the compound
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FORMULASMgCl2
The subscript is the number at the bottom of a formula.
There is 1- Mg & 2 – Cl Never use 1 as a subscript!
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IONIC BONDbond formed between
two ions by the transfer of electrons
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Ions Atom that gains or loses electrons
to become stable “happy” Cation: loses e- to form (+)
charged ion Anion: gains e- to form (-)
charged ion
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Formation of Ions from Metals
Ionic compounds result when metals react with nonmetals
Metals lose electrons to form a positive charge Nonmetals gain electrons to form a negative
charge
Metals: Nonmetals: Na+ N -3
Ca+2 S -2
Al+3 Br -
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IONIC BONDS Bonds form from the (+) & (-)
charges. Form a network of ions. – very
strong bonds. Conduct electricity when
melted or dissolved in water.
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Writing Ionic Formulas – binaryRepresentative metals
Calcium & oxygen
Write the metal ion Ca +2
Write the nonmetal ion O -2
If charges cancel – ratio is 1:1 ( 1 of each)
CaO
Magnesium & chlorine
Write the metal ion Mg +2
Write the nonmetal ion Cl -
If charges DO NOT cancel – drop & swap
MgCl2
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Writing Ionic Formulas – binaryTransition metals
Ion charges change – an element can have more than one ion charge
The charge is given as a ROMAN NUMERALEx: Iron (II) Fe+2 / Iron (III) Fe+3
Gold (I) Au + / Gold (III) Au+3
You will never have to memorize all the charges each transition metal forms – the charges will be given to you !!!!!
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Practice Magnesium & iodine
Strontium & bromine
Barium & nitrogen
Aluminum & phosphorus
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Naming Ionic Formula - binary Representative Metals
Name the metalChange the ending of the
nonmetal to – ide
MgCl2 - magnesium chlorideAlP - aluminum phosphide
Cl – chloride C - carbideF – flouride Se - selenideI – iodide N – nitrideP – phosphide S – sulfideBr – bromide O – oxide
Transition MetalsName the metal & Include the
charge using a Roman Numeral
Ex: Iron (II) Fe+2 / Iron (III) Fe+3
Gold (I) Au + / Gold (III) Au+3
Change the ending of the nonmetal ending to –ide
Fe +2 Cl - iron (II) chloride
Au + O -2 gold (I) oxide
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Practice CaBr2
Na3N
BCl3
MgO
FeCl3
Ni3N
ZnO
FeS
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Ternary Ionic Bonds – contain Polyatomic Ions
Polyatomic ion : a group of (covalently) bonded nonmetals that form a charge.
Act as a single ion in an ionic bond
Have special names that DO NOT CHANGE
You need to write down the polyatomic ions and their names on a sheet of paper and DO NOT LOSE IT!!!
You will use your list on all quizzes and tests!
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AmmoniumNH4+
Acetate C2H3O2-
Hypochlorite ClO-
Chlorite ClO2-
Chlorate ClO3-
PerchlorateClO4-
Cyanide CN-
Hydroxide OH-
Nitrite NO2-
Nitrate NO3-
Bicarbonate/Hydrogen Carbonate HCO3-
Carbonate CO3-2
Chromate CrO4-2
Dichromate Cr2O7-2
Oxalate C2O4-2
Sulfate SO4-2
Sulfite SO3-2
Phosphite PO3-3
Phosphate PO4-3
Permanganate MnO4-
Peroxide O2-2
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Writing Ionic Formulas - ternary Write the cation – all metals (only polyatomic cation
is ammonium: NH4+ )
Write the anion – all nonmetals and polyatomic ions
If charges cancel – 1:1 ratio
If charges DO NOT cancel – drop & swap You must use parenthesis if more than one
polyatomic ion is present
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Practice cesium nitrate
barium sulfite
aluminum hydroxide
strontium phosphate
ammonium sulfide
Iron(III) chlorite
Zinc(II) nitrite
Gold(III) carbonate
Silver(I) phosphite
Copper(I) acetate
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Naming ionic formulas - ternaryRepresentative metal Name the cation Use the same name
for the polyatomic ion
If the anion is a nonmetal – change the ending to -ide
Transition metal Name the metal and include
a ROMAN NUMERAL for the charge of the metal
Use the same name for the polyatomic ion
If the anion is a nonmetal – change the ending to -ide
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Group 1 - Alkali Metals
reacts violently with water VERY reactive, one valence e-
to lose; +1 cation
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Alkali metals http://www.youtube.com/watch?v=m55k
gyApYrY&safety_mode=true&persist_safety_mode=1
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Group 2 - Alkaline Earth Metals
2 valence e-; +2 cation reactive
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http://www.youtube.com/watch?v=m55kgyApYrY&safety_mode=true&persist_safety_mode=1
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Transition Metals Groups 3-12 Ions charges change –
changes properties NOT REPRESENTATIVE!
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Halogens -Group 17 -1 ions, highly reactive 7 valence e-
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Noble Gases Group 18 unreactive, 8 valence e- do not form ions exist as single atoms,
don’t bond - inert
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COVALENT BONDbond formed by the sharing of electrons
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Covalent Compounds
Covalent compounds result when nonmetals react with nonmetals
Both nonmetals share their valence electrons to be happy – Octet Rule
Examples:CO2 SCl2
H2O CH4
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Naming Covalent formulas Use prefixes to show the # of atoms of each
element in a covalent compound 1 – mono 6 - hexa 2 – di 7 - hepta 3 – tri 8- octa 4 – tetra 9 - nona 5 – penta 10 – deca
1st element – use prefixes only of the # of atoms is greater than 1
2nd element – use prefixes; change ending to – ide
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Practice CO2
N3F8
Se4Br9
S7O
tetraselenium nonabromide
trinitrogen octaflouride
heptasulfur monoxide
carbon dioxide
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Writing Covalent formulas Use the prefix to identify how many of each
nonmetal atoms are in each molecule The prefix becomes the subscript.
Carbon Tetrahydride Disulfur Hexachloride○ CH4 S2Cl6
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1) Name the following covalent compounds:a) SiF4
b) N2S3
c) H3Br7
d) S5Br9
e) H2O
2) Write the formulas for the following covalent compounds:
a) diboron hexahydrideb) nitrogen tribromidec) sulfur hexachlorided) diphosphorus pentoxide
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