4-1 Chapter 5 - Ionic Bonding 4-2 Bonds Chemical bond - forces of attraction that hold atoms...
-
Upload
bathsheba-webb -
Category
Documents
-
view
218 -
download
1
Transcript of 4-1 Chapter 5 - Ionic Bonding 4-2 Bonds Chemical bond - forces of attraction that hold atoms...
4-2
BondsBonds• Chemical bond - forces of attraction that hold
atoms together. • The molecule is more stable than the separate
ions/ atoms. • Bond energy - the energy required to break (or
form) a chemical bond. • Energy is released when the bond is formed.• Ionic bonds - bond formed by the attraction
between oppositely charged particles (anion and cation)• The transfer of one or more electrons from one atom
to another
4-3
Ionic CompoundsIonic Compounds
• Ionic compounds - a chemical compound that has an equal amount of positive and negative charges so the compound is electrically neutral. Formed by ionic bonds.
• Salt - an inorganic compound containing cations other than H+ and anions other than OH- and O2-.
4-4
Properties of SaltsProperties of Salts
• All salts are made of ions and are held together by ionic bonds.
• Salts form a crystal lattice - an ordered packing 3-dimensional arrangement of atoms or ions in a crystal
• Crystalline versus amorphous- crystalline solids have a fixed arrangement of atoms while amorphous solids like talcum powder have haphazard/ random arrangement.
4-5
Properties of SaltsProperties of Salts
• Salts do not melt or boil easily because of the strong attraction between ions
• Salts are hard and brittle
• Salts conduct electricity when melted or dissolved to form an aqueous solution (in water- aq.)
4-6
Energy and Ionic BondingEnergy and Ionic Bonding
• Removing an electron from an atom requires an input of energy- Ionization energy
• Adding an electron to an atom releases energy- Electron Affinity
• Lattice energy - the energy released when the crystal lattice of an ionic solid is formed
4-7
NomenclaturePOPO44
3-3-
phosphate ionphosphate ion
CC22HH33OO22--
acetate ionacetate ion
HC2H3O2
Acetic Acid
4-8
Forms of Chemical Forms of Chemical BondsBonds
• There are 3 forms of There are 3 forms of bonding between atoms:bonding between atoms:
• IonicIonic—complete —complete transfer transfer of of 1 or more electrons from 1 or more electrons from one atom to another (one one atom to another (one loses, the other gains)loses, the other gains)
• CovalentCovalent——some valence some valence electrons electrons sharedshared between between atomsatoms
• MetallicMetallic – holds atoms of a – holds atoms of a metal together. Electrons metal together. Electrons form a common pool called form a common pool called sea of electrons. sea of electrons.
Most bonds are Most bonds are somewhere in somewhere in between ionic between ionic and covalent.and covalent.
4-9
Common NamesCommon Names• A lot of chemicals have common A lot of chemicals have common
names as well as the proper names as well as the proper IUPAC name.IUPAC name.
• Chemicals that should always be Chemicals that should always be named by common name and named by common name and never named by the IUPAC never named by the IUPAC method are:method are:
• HH22OO water, not dihydrogen water, not dihydrogen
monoxidemonoxide
• NHNH33 ammonia, not nitrogen ammonia, not nitrogen
trihydridetrihydride
4-10
CATIONCATION + + ANIONANION ---> --->
COMPOUNDCOMPOUND
CATIONCATION + + ANIONANION ---> --->
COMPOUNDCOMPOUND
A neutral compound A neutral compound requiresrequires
equal number of + equal number of + and - charges.and - charges.
A neutral compound A neutral compound requiresrequires
equal number of + equal number of + and - charges.and - charges.
COMPOUNDS COMPOUNDS FORMED FROM FORMED FROM
IONSIONS
COMPOUNDS COMPOUNDS FORMED FROM FORMED FROM
IONSIONSNaNa++ + Cl + Cl- - --> NaCl--> NaCl
4-11
Predicting Charges on Monatomic IonsPredicting Charges on Monatomic IonsKNOW THESE !!!!KNOW THESE !!!!
+1 +2 -3 -2 -1 0
Cd+2
4-12
Properties of Ionic CompoundsProperties of Ionic CompoundsForming NaCl from Na and ClForming NaCl from Na and Cl22
Properties of Ionic CompoundsProperties of Ionic CompoundsForming NaCl from Na and ClForming NaCl from Na and Cl22
• A metal atom can A metal atom can transfer an electron transfer an electron to a nonmetal.to a nonmetal.
• The resulting cation The resulting cation and anion are and anion are attracted to each attracted to each other by other by electrostatic electrostatic forcesforces..
4-13
IONIC COMPOUNDSIONIC COMPOUNDSIONIC COMPOUNDSIONIC COMPOUNDS
NH4+
Cl-
ammonium chloride, NHammonium chloride, NH44ClCl
4-14
Some Ionic CompoundsSome Ionic CompoundsSome Ionic CompoundsSome Ionic Compounds
MgMg2+2+ + N + N-3-3 ----> ---->
MgMg33NN22
magnesiummagnesium nitridenitride
SnSn4+4+ + O + O2-2- ----> ---->
SnOSnO22
Tin (IV) oxideTin (IV) oxide
calcium fluoridecalcium fluoride
CaCa2+2+ + 2 F + 2 F-- ---> ---> CaFCaF22
4-15
Formulas of Ionic CompoundsFormulas of Ionic Compounds
Formulas of ionic compounds are determined from the charges on the ions
atoms ions
–
Na + F : Na+ : F : NaF
sodium + fluorine sodium fluoride formula
Charge balance: 1+ 1- = 0
4-17
Writing a FormulaWriting a Formula
Write the formula for the ionic compound that will form between Ba2+ and Cl.
Solution:
1. Balance charge with + and – ions
2. Write the positive ion of metal first, and the
negative ion Ba2+ Cl
Cl3. Write the number of ions needed as
subscripts BaCl2
4-18
• Writing BINARY FORMULAS
• 1. CANCEL CHARGES TO GET A TOTAL CHARGE OF ZERO.
• 2. CROSS- MULTIPLY TILL YOU GET THE LOWEST COMMON MULTIPLE.
• 3. WHAT YOU MULTIPLIED WITH IS YOUR SUBSCRIPT.
• 4. DO NOT WRITE CHARGES ON YOUR FINAL FORMULA.
• 5. METAL IS WRITTEN FIRST AND THEN NON- METAL.
• SIMPLEST FORMULA IS WRITTEN
4-19
Learning Check Learning Check
Write the correct formula for the compounds containing the following ions:
1. Na+, S2-
a) NaS b) Na2S c) NaS2
2. Al3+, Cl-
a) AlCl3 b) AlCl c) Al3Cl
3. Mg2+, N3-
a) MgN b) Mg2N3 c) Mg3N2
4-21
Naming CompoundsNaming CompoundsNaming CompoundsNaming Compounds
• 1. Cation first, then anion
• 2. Monatomic cation = name of the element
• Ca2+ = calcium ion
• 3. Monatomic anion = root + -ide• Cl = chloride
• CaCl2 = calcium chloride
Binary Ionic Compounds:Binary Ionic Compounds:
4-22
Naming Binary Ionic CompoundsNaming Binary Ionic Compounds
Examples:
NaCl
ZnI2
Al2O3
sodium chloride
zinc iodide
aluminum oxide
4-23
Learning Check Learning Check
Complete the names of the following binary compounds:
Na3N sodium ________________
KBr potassium ________________
Al2O3 aluminum ________________
MgS _________________________
4-24
1. BaCl22. NaF
3. Ag2O4. CuBr
5. CuBr2
6. FeO
7. Fe2O3
8. MgS
9. Al2O3
10. CaI2
1. BaCl22. NaF
3. Ag2O4. CuBr
5. CuBr2
6. FeO
7. Fe2O3
8. MgS
9. Al2O3
10. CaI2
11. K2S
12. CrCl213. CrCl314. CaO
15. Ba3P2
16. Hg2I2
17. Na2O18. BeS19. MnO
20. Mn2O3
11. K2S
12. CrCl213. CrCl314. CaO
15. Ba3P2
16. Hg2I2
17. Na2O18. BeS19. MnO
20. Mn2O3
Name the ionic compoundsName the ionic compoundsName the ionic compoundsName the ionic compounds
4-25
Transition MetalsTransition Metals
Elements that can have more than one possible
charge MUST have a Roman Numeral to
indicate the charge on the individual ion.
1+ or 2+ 2+ or 3+
Cu+, Cu2+ Fe2+, Fe3+
copper(I) ion iron(II) ion
copper (II) ion iron(III) ion
4-26
Names of Variable IonsNames of Variable Ions
These elements REQUIRE Roman Numerals because they can have more than one possible charge:anything except Group 1A, 2A, Ag, Zn, Cd, and Al
(You should already know the charges on these!)
Or another way to say it is: Transition metals and the metals in groups 4A and
5A (except Ag, Zn, Cd, and Al) require a Roman Numeral.
FeCl3 (Fe3+) iron (III) chlorideCuCl (Cu+ ) copper (I) chlorideSnF4 (Sn4+) tin (IV) fluoridePbCl2 (Pb2+) lead (II) chloride
Fe2S3 (Fe3+)iron (III) sulfide
4-27
Examples of Older Names of Cations Examples of Older Names of Cations formed from Transition Metalsformed from Transition Metals
(you do not have to memorize these)(you do not have to memorize these)
4-28
Learning Check Learning Check
Complete the names of the following binary
compounds with variable metal ions:
FeBr2 iron (_____) bromide
CuCl copper (_____) chloride
SnO2 ___(_____ ) ______________
Fe2O3 ________________________
Hg2S ________________________
4-29
NONO33--
nitrate ionnitrate ion
NONO22--
nitrite ionnitrite ion
Polyatomic Polyatomic IonsIons
Polyatomic Polyatomic IonsIons
4-30
You can make additional polyatomic You can make additional polyatomic ions by adding a Hions by adding a H++ to the ion! to the ion!
COCO33 -2-2 is carbonate is carbonate
HCOHCO33–– is hydrogen carbonate is hydrogen carbonate
HH22POPO44–– is dihydrogen phosphate is dihydrogen phosphate
HSOHSO44–– is hydrogen sulfate is hydrogen sulfate
Polyatomic IonsPolyatomic IonsPolyatomic IonsPolyatomic Ions
4-31
Ternary Ionic NomenclatureTernary Ionic Nomenclature
Writing Formulas
• Write each ion, cation first. Don’t show charges in the final formula.
• Overall charge must equal zero.• If charges cancel, just write symbols.• If not, use subscripts to balance charges.
• Use parentheses to show more than one of a particular polyatomic ion.
• Use Roman numerals indicate the ion’s charge when needed (stock system)
4-32
Ternary Ionic NomenclatureTernary Ionic Nomenclature
Sodium SulfateNa+ and SO4 -2
Na2SO4
Iron (III) hydroxideFe+3 and OH-
Fe(OH)3
Ammonium carbonateNH4
+ and CO3 –2
(NH4)2CO3
4-33
Learning Check Learning Check
1. aluminum nitrate
a) AlNO3 b) Al(NO)3 c) Al(NO3)3
2. copper(II) nitrate
a) CuNO3 b) Cu(NO3)2 c) Cu2(NO3)
3. Iron (III) hydroxide
a) FeOH b) Fe3OH c) Fe(OH)3
4. Tin(IV) hydroxide
a) Sn(OH)4 b) Sn(OH)2 c) Sn4(OH)
4-34
Naming Ternary CompoundsNaming Ternary Compounds
Contains at least 3 elementsThere MUST be at least one polyatomic ion
(it helps to circle the ions)Examples:
NaNO3 Sodium nitrate
K2SO4 Potassium sulfate
Al(HCO3)3 Aluminum bicarbonate
or
Aluminum hydrogen carbonate
4-35
Learning Check Learning Check
Match each set with the correct name:
1. Na2CO3 a) magnesium sulfite
MgSO3 b) magnesium sulfate
MgSO4 c) sodium carbonate
2 . Ca(HCO3)2 a) calcium carbonate
CaCO3 b) calcium phosphate
Ca3(PO4)2 c) calcium bicarbonate
4-36
Mixed Practice!Mixed Practice!
Name the following:
• Na2O
• CaCO3
• PbS2
• Sn3N2
• Cu3PO4
• HgF2
4-37
Mixed Up… The Other WayMixed Up… The Other Way
Write the formula:
1. Copper (II) chlorate
2. Calcium nitride
3. Aluminum carbonate
4. Potassium bromide
5. Barium fluoride
6. Cesium hydroxide
4-38
Naming Molecular Naming Molecular (Covalent) Compounds(Covalent) Compounds
CH4 methaneBCl3 boron trichloride
CO2 Carbon dioxide
All are formed from two or more nonmetals.
Ionic compounds generally involve a metal and nonmetal (NaCl)
4-39
IONIC BONDING COVALEN T BONDING1. COMPOUNDSFORMED BYTRANSFER OFELECTRONS
COMPOUNDSFORMED BY SHARINGELECTRONS
2. FORMED BETWEENMETALS ANDNONMETALS
FORMED BETWEENNONMETALS
3.IONS ARE FORMED NOT FORMED4. NO CONCEPT OFSINGLE, DOUBLE ORTRIPLE BOND
MOLECULES CAN BEFORMED BY SHARINGONE ELECTRON PAIR(SINGLE BOND), ORDOUBLE OR TRIPLEBOND.
5. COMPOUNDSCONDUCTELECTRICITY INWATER SOLUTION
COMPOUNDS DO NOTCONDUCTELECTRICITY
6. COMPOUNDS HAV EHIGHER BOILINGAND MELTINGPOINTS DUE TONETWORK
LOWER MELTINGAND BOILING POINTSDUE TO SEPARATEMOLECULES
4-40
Molecular (Covalent) NomenclatureMolecular (Covalent) Nomenclaturefor two for two nonnonmetalsmetals
• Prefix System (binary compounds)
1. Less electronegative atom comes first.
2. Add prefixes to indicate # of atoms. Omit mono- prefix on the FIRST element. Mono- is OPTIONAL on the SECOND element .
3. Change the ending of the second element to -ide.
4-41
PREFIXmono-di-tri-tetra-penta-hexa-hepta-octa-nona-deca-
NUMBER12345678910
Molecular Nomenclature PrefixesMolecular Nomenclature Prefixes
4-42
• CCl4
• N2O
• SF6
• carbon tetrachloride
• dinitrogen monoxide
• sulfur hexafluoride
Molecular Nomenclature: ExamplesMolecular Nomenclature: Examples
4-43
• arsenic trichloride
• dinitrogen pentoxide
• tetraphosphorus decoxide
• AsCl3
• N2O5
• P4O10
More Molecular ExamplesMore Molecular Examples
4-44
Learning Check Learning Check
Fill in the blanks to complete the following names of covalent compounds.
CO carbon ______oxide
CO2 carbon _______________
PCl3 phosphorus _______chloride
CCl4 carbon ________chloride
N2O _____nitrogen _____oxide
4-45
Learning Check Learning Check
1. P2O5 a) phosphorus oxide
b) phosphorus pentoxide
c) diphosphorus pentoxide
2. Cl2O7 a) dichlorine heptoxide
b) dichlorine oxide
c) chlorine heptoxide
3. Cl2 a) chlorine
b) dichlorine
c) dichloride
4-48
Mixed Review Mixed Review
Name the following compounds:1. CaO
a) calcium oxide b) calcium(I) oxidec) calcium (II) oxide
2. SnCl4 a) tin tetrachloride b) tin(II) chloride c) tin(IV) chloride
3. N2O3a) nitrogen oxide b) dinitrogen trioxidec) nitrogen trioxide
4-49
Solution Solution
Name the following compounds:
1. CaO
2. SnCl4
3. N2O3
a) calcium oxide
c) tin(IV) chloride
b) Dinitrogen trioxide
4-50
Mixed PracticeMixed Practice
1. Dinitrogen monoxide
2. Potassium sulfide
3. Copper (II) nitrate
4. Dichlorine heptoxide
5. Chromium (III) sulfate
6. Iron (III) sulfite
7. Calcium oxide
8. Barium carbonate
9. Iodine monochloride
4-51
Mixed PracticeMixed Practice
1.1. BaIBaI22
2.2. PP44SS33
3.3. Ca(OH)Ca(OH)22
4.4. FeCOFeCO33
5.5. NaNa22CrCr22OO77
6.6. II22OO55
7.7. Cu(ClOCu(ClO44))22
8.8. CSCS22
9.9. BB22ClCl44
4-52
Acid NomenclatureAcid Nomenclature
• AcidsAcids
• Compounds that form HCompounds that form H++ in water. in water.
• Formulas usually begin with ‘H’.Formulas usually begin with ‘H’.
• In order to be an acid instead of a gas, binary In order to be an acid instead of a gas, binary
acids must be aqueous (dissolved in water)acids must be aqueous (dissolved in water)
• Ternary acids are ALL aqueousTernary acids are ALL aqueous
• Examples:Examples:
• HCl HCl (aq)(aq) – hydrochloric acid – hydrochloric acid
• HNOHNO33 – nitric acid – nitric acid
• HH22SOSO44 – sulfuric acid – sulfuric acid
4-53
Anion Ending Acid Name
-ide hydro-(stem)-ic acid
-ate (stem)-ic acid
-ite (stem)-ous acid
Acid NomenclatureAcid Nomenclature
Binary Binary
Ternary Ternary
An easy way to remember which goes with which…An easy way to remember which goes with which…
““In the cafeteria, you In the cafeteria, you ATEATE something something ICICky”ky”
4-54
Acid Nomenclature FlowchartAcid Nomenclature Flowchart
hydro- prefix-ic ending
2 elements
-ate endingbecomes-ic ending
-ite endingbecomes
-ous ending
no hydro- prefix
3 elements
ACIDSstart with 'H'
4-55
• HBr HBr (aq)(aq)
• HH22COCO33
• HH22SOSO33
• 2 elements, 2 elements, --ideide
• 3 elements, 3 elements, -ate-ate
• 3 elements, 3 elements, -ite-ite
hydrohydrobromic acidbromic acid
carboncarbonicic acid acid
sulfursulfurousous acid acid
Acid NomenclatureAcid Nomenclature
4-56
• hydrofluoric acidhydrofluoric acid
• sulfuric acidsulfuric acid
• nitrous acidnitrous acid
• 2 elements2 elements
• 3 elements, 3 elements, -ic-ic
• 3 elements, 3 elements, -ous-ous
HF HF (aq)(aq)
HH22SOSO44
HNOHNO22
Acid NomenclatureAcid Nomenclature
HH++ F- F-
HH++ SO SO442-2-
HH++ NO NO22--
4-58
Write the Formula!Write the Formula!
• Hydrobromic acidHydrobromic acid
• Nitrous acidNitrous acid
• Carbonic acidCarbonic acid
• Phosphoric acidPhosphoric acid
• Hydrotelluric acidHydrotelluric acid
4-61
Rainbow Matrix GameRainbow Matrix Game
• Link on Chemistry Geek.com on Chemistry I page
• http://chemistrygeek.com/rainbow
Use [ ] to represent subscripts since you can’t enter subscripts into the computer
So H2O would be H[2]OAnd Al2(SO4)3 would be Al[2](SO[4])[3]
Additional Polyatomic Ions (you do not have to memorize these, but they are in the game!)
Borate = BO3 -3 ; Silicate = SiO4 -4 ;Manganate = MnO4 -2 (permanganate is -1)