Transcript of Common Polyatomic Ions Names of Common Polyatomic Ions Ion Name Ion Name NH 4 + ammoniumCO 3 2-...
- Slide 1
- Slide 2
- Common Polyatomic Ions Names of Common Polyatomic Ions Ion Name
Ion Name NH 4 + ammoniumCO 3 2- carbonate *NO 2 - *nitriteHCO 3 -
bicarbonate NO 3 - nitrate*IO 3 - *iodate *SO 3 2- *sulfite*IO 4 -
*periodate SO 4 2- sulfate *ClO - *hypochlorite HSO 4 - hydrogen
sulfate*ClO 2 - *chlorite OH - hydroxide ClO 3 - chlorate CN -
cyanide *ClO 4 - *perchlorate C 2 H 3 O 2 - acetate *BrO 3 -
*bromate MnO 4 - permanganateC 2 O 4 2- oxalate PO 4 3- phosphateCr
2 O 7 2- dichromate *PO 3 3- *phosphiteCrO 4 2- chromate H 2 PO 4 -
dihydrogen phosphateO 2 2- peroxide Zumdahl, Zumdahl, DeCoste,
World of Chemistry 2002, page 100 Memorize the BOLD ions * = you
will be responsible for knowing these
- Slide 3
- Polyatomic Ion Trends *Charges NEVER change between different
forms Normal ate form BrO 3 - bromate ClO 3 - chlorate IO 3 -
iodate NO 3 - nitrate CO 3 2- carbonate SO 4 2- sulfate PO 4 3-
phosphate BrO 2 - ClO 2 - IO 2 - NO 2 - CO 2 2- SO 3 2- PO 3 3- BrO
- ClO - IO - BrO 4 - ClO 4 - IO 4 - -1 oxygen -ite form -2 oxygens
hypo___ite +1 oxygen Per____ate bromite chlorite iodite nitrite
sulfite phosphite hypobromite hypochlorite hypoiodite perbromate
perchlorate periodate carbonite
- Slide 4
- Atomic Theory Review
- Slide 5
- Electron Cloud Model Orbital (electron cloud) instead of orbits
Region in space where there is 90% probability of finding an
electron Courtesy Christy Johannesson
www.nisd.net/communicationsarts/pages/chem Electron Probability vs.
Distance Electron Probability (%) Distance from the Nucleus (pm)
100150200250500 0 10 20 30 40 Orbital 90% probability of finding
the electron Orbital Shape
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- Shapes of s, p, and d-Orbitals each holds 2 electrons (s 2 )
each of 5 orbitals holds 2 e - = 10 total d electrons (d 10 ) each
of 3 orbitals holds 2 e - = 6 total p electrons (p 6 )
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- s, p, and d-orbitals s orbitals: Each holds 2 electrons (outer
orbitals of Groups 1 and 2) p orbitals: Each of 3 sets holds 2
electrons = 6 electrons (outer orbitals of Groups 3 to 8) d
orbitals: Each of 5 sets holds 2 electrons = 10 electrons (found in
elements in third period and higher) Orbital Filling Video
- Slide 8
- Copyright 2006 Pearson Benjamin Cummings. All rights reserved.
Orbitals overlap each other as you get farther from the
nucleus
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- f-orbitals 7 f orbitals @ 2 e- each = 14 e-
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- s, p, d and f orbitals How many g orbitals could exist?
- Slide 11
- theoretical g-orbitals 9 g orbitals @ 2 e- each = 18 e-
- Slide 12
- s p d f 6767 Periodic Patterns for Electron Config 1s1s1s1s
2s2s2s2s 3s3s3s3s 4s4s4s4s 5s5s5s5s 6s6s6s6s 7s7s7s7s 3d3d3d3d
4d4d4d4d 5d5d5d5d 6d6d6d6d 1s1s1s1s 2p2p2p2p 3p3p3p3p 4p4p4p4p
5p5p5p5p 6p6p6p6p 7p7p7p7p 4f4f4f4f 5f5f5f5f 12345671234567 1 2
(n-1) (n-2) n 3 5 6 7 8 4
- Slide 13
- s-block1st Period 1s 1 # of e- in that orbital(s) Periodic
Patterns Example - Hydrogen Courtesy Christy Johannesson
www.nisd.net/communicationsarts/pages/chem
- Slide 14
- Shorthand Configuration S 16e - Valence Electrons (Highest
energy level) Core Electrons S16e - [Ne] 3s 2 3p 4 1s 2 2s 2 2p 6
3s23s2 3p43p4 Electron Configuration Review Longhand Configuration
Courtesy Christy Johannesson
www.nisd.net/communicationsarts/pages/chem S 32.066 16
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- [Ar]4s 2 3d 10 4p 2 Periodic Patterns GermaniumExample -
Germanium Courtesy Christy Johannesson
www.nisd.net/communicationsarts/pages/chem Ge 72.61 32
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- [ ] neon's electron configuration(1s 2 2s 2 2p 6 ) Shorthand
Configuration [Ne] 3s 1 3rd energy level (or 3 rd period) 1
electron in the s orbital orbital shape (s,p,d,fetc.) 1s 2 2s 2 2p
6 3s 1 electron configuration A B C D Na = [Ne]
- Slide 17
- Shorthand Configuration Practice [Ar] 4s 2 Electron
configurationElement symbol [Ar] 4s 2 3d 3 [Rn] 7s 2 5f 14 6d 4
[He] 2s 2 2p 5 [Kr] 5s 2 4d 9 [Kr] 5s 2 4d 10 5p 5 [Kr] 5s 2 4d 10
5p 6 [He] 2s 2 2p 6 3s 2 3p 6 4s 2 3d 6 Ca V Sg F Ag I Xe Fe [Ar]
4s 2 3d 6
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- Periodic Patterns Review Period # (1-7) energy level (subtract
for d & f) Group # (1-8excluding d block) total # of valence e
- Column within Sublevel block # of e - in sublevel/orbital
Courtesy Christy Johannesson
www.nisd.net/communicationsarts/pages/chem
- Slide 19
- s p d f 6767 Periodic Patterns and Charge Trends 1s1s1s1s
12345671234567 +1 +2 (n-2) n +3 - 3 - 2 - 1 Variable Charge METALS
NON- METALS
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- Electron Configurations for Cations Metals lose e - to attain a
noble gas configuration Metals form positive ions Cations are
pawsitive Metal ions will lose e - from configuration Na: 1s 2 2s 2
2p 6 3s 1 Na + : 1s 2 2s 2 2p 6 noble gas configuration
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- Formation of a Cation 11p + sodium atom Na [Ne] 3s 1 e-e- loss
of one valence electron e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e-
e-e- e-e- sodium ion Na + [Ne] 11p + e-e- e-e- e-e- e-e- e-e- e-e-
e-e- e-e- e-e- e-e- e-e-
- Slide 22
- Electron Configurations for Anions Non-metals gain electrons to
attain a noble gas configuration They form negative ions Take a
look at the e - configuration S 1s 2 2s 2 2p 6 3s 2 3p 4 (6 valence
electrons) + 2e - S 2- 1s 2 2s 2 2p 6 3s 2 3p 6 ( noble gas
configuration)
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- Formation of an Anion 17p + chlorine atom Cl [Ne]3s 2 3p 5 e-e-
e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e-
e-e- e-e- e-e- e-e- gain of one valence electron chloride ion Cl
[Ne]3s 2 3p 6 or [Ar] e-e- 17p + e-e- e-e- e-e- e-e- e-e- e-e- e-e-
e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e-
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- Stable Electron Configurations All atoms react to achieve noble
gas configuration Noble gases have two s and six p electrons Eight
valence electrons Also called the octet rule Ar
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- Bonding Review and Writing Ionic Formulas Table salt
- Slide 26
- Formation of Ionic Bond sodium ion Na + 11p + e-e- e-e- e-e-
e-e- e-e- e-e- e-e- e-e- e-e- e-e- chloride ion Cl - 17p + e-e-
e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e- e-e-
e-e- e-e- e-e- e-e- + -
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- Ionic Bonding Anions and cations are held together by opposite
charges All ionic compounds are called salts Simplest ratio is
called the formula unit The bond is formed through the transfer of
electrons Electrons are transferred to fill all available orbitals,
or achieve a noble gas configuration
- Slide 28
- O 2- K+K+ K+K+ Mg 2+ Br - K Br potassium atom bromine atom e-e-
e-e- Br - K+K+ potassium ion bromide ion potassium bromide KBr MgBr
2 K2OK2O magnesium bromide potassium oxide
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- Bonding Practice Ca 2+ Al 3+ Na + Pb 4+ OH - N 3- Mg 2+ OH - N
3- Pb 4+ N 3- Pb 4+ N 3- Pb 4+ N 3- ? Pb 4+ N 3- Pb 3 N 4 lead (IV)
nitride or plumbic nitride NaOH Mg(OH) 2 AlN CaBr 2 Ca(OH) 2
CaO
- Slide 30
- Fe 2+ Ca 2+ PO 4 3- NH 4 + O 2- Al 3+ O 2- Ca 3 (PO 4 ) 2 (NH 4
) 3 PO 4 FeO Al 2 O 3
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- Subscripts, Superscripts and Coefficients Mg 3 (PO 4 ) 2
coefficient subscripts superscripts MAGNESIUM PHOSPHATE PO 4 3- Mg
2+ 5
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- Writing Formulas of Ionic Compounds chemical formula: has
neutral charge; shows types of atoms and how many of each To write
an ionic compounds formula, we need: 1. the two types of ions 2.
the charge on each ion Na + and F Ba 2+ and O 2 Na + and O 2 Ba 2+
and F NaF BaO Na 2 O BaF 2
- Slide 33
- ide Calcium hydrox ide Ca 2+ OH - CaOH 2 Ca(OH) 2 Ca - O H H HO
- Ca - OH vs. The Importance of Parentheses The formulas imply two
totally different compounds!
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- (NH 4 ) 3 N Fe 2 (Cr 2 O 7 ) 3 Sn(SO 4 ) 2 NH 4 ClO 3 Mg(NO 2 )
2 BaSO 4 Writing Formulas w /Polyatomic Ions Parentheses are
required only when you need more than one bunch of a particular
polyatomic ion Ba 2+ and SO 4 2 Mg 2+ and NO 2 NH 4 + andClO 3 Sn
4+ andSO 4 2 Fe 3+ andCr 2 O 7 2 NH 4 + andN 3
- Slide 35
- Element Latin root -ic -ous gold, Auaur- Au 3+ Au 1+ lead,
Pbplumb- Pb 4+ Pb 2+ tin, Snstann- Sn 4+ Sn 2+ copper, Cucupr- Cu
2+ Cu 1+ iron, Feferr- Fe 3+ Fe 2+ Traditional (OLD) System of
Nomenclature used historically (and still some today) to name
compounds w /multiple-charge cations To use: 1. Use Latin root of
cation. 2. Use -ic ending for higher charge -ous lower 3. Then say
name of anion, as usual. ; (icky food is good for you!) ;
(delicious food is not good for you!)
- Slide 36
- Cu 2 S AuN FeF 2 plumbic phosphide plumbous phosphide stannic
chloride Fe 2+ Write formulas:Write names: cuprous sulfide auric
nitride ferrous fluoride Pb 3 P 4 3 Pb ? 4 P 3 Cu 1+ Pb 3 P 2 3 Pb
? 2 P 3 Au 3+ SnCl 4 Sn ? 4 Cl 1 S 2 N 3 F 1
- Slide 37
- Nomenclature - Humor Ferrous Wheel Fe = iron (Latin = ferrum)
Fe 2+ = lower oxidation state = ferrous Fe 3+ = higher oxidation
state = ferric BaNa 2 BaNaNa Fe 2+ What weapon can you make from
the elements nickel, potassium and iron? A KNiFe
- Slide 38
- Teacher: What is the formula for water? Student: H, I, J, K, L,
M, N, O Teacher: Thats not what I taught you. Student: But you said
the formula for water wasH to O. Website: Dihydrogen monoxide
Information Campaign mis Little Johnny took a drink, Now he shall
drink no more. For what he thought was H 2 O, Was H 2 SO 4. Under
aged Pb walks into a bar and the bartender turns to the gold
Bouncer and says, Au, get the lead out! "H-O-H"?! WHAT'S THAT
SPELL?! WATER?
- Slide 39
- Four Types of Naming Fixed Charge Ionic Compounds Variable
Charge Ionic Compounds Acidic Compounds Covalent Molecules Contain
a metal with a fixed charge and a non- metal (ionic) Contain H +
with various anions (ionic when aqueous) Contain 2 or more
nonmetals only Contain a metal with a variable charge and a non-
metal (ionic)
- Slide 40
- Li 3 H1H1 He 2 C6C6 N7N7 O8O8 F9F9 Ne 10 Na 11 B5B5 Be 4 H1H1
Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 K 19 Ca 20 Sc 21 Ti 22 V 23 Cr 24
Mn 25 Fe 26 Co 27 Ni 28 Cu 29 Zn 30 Ga 31 Ge 32 As 33 Se 34 Br 35
Kr 36 Rb 37 Sr 38 Y 39 Zr 40 Nb 41 Mo 42 Tc 43 Ru 44 Rh 45 Pd 46 Ag
47 Cd 48 In 49 Sn 50 Sb 51 Te 52 I 53 Xe 54 Cs 55 Ba 56 Hf 72 Ta 73
W 74 Re 75 Os 76 Ir 77 Pt 78 Au 79 Hg 80 Tl 81 Pb 82 Bi 83 Po 84 At
85 Rn 86 Fr 87 Ra 88 Rf 104 Db 105 Sg 106 Bh 107 Hs 108 Mt 109 Mg
12 Ce 58 Pr 59 Nd 60 Pm 61 Sm 62 Eu 63 Gd 64 Tb 65 Dy 66 Ho 67 Er
68 Tm 69 Yb 70 Lu 71 Th 90 Pa 91 U 92 Np 93 Pu 94 Am 95 Cm 96 Bk 97
Cf 98 Es 99 Fm 100 Md 101 No 102 Lr 103 La 57 Ac 89 1 2 3 4 5 6 7
Fixed charge cations Variable charge cations Elemental anions 1+ 2+
3+1-2-3-
- Slide 41
- Fixed Charge Exceptions Start with Al Go backwards down the
stairs Decrease the charge after each stair Al 13 Zn 30 Ag 47 3+ 2+
+ 3+
- Slide 42
- Fixed Charge Compound Nomenclature Metals (fixed charge) +
Nonmetals
- Slide 43
- Fixed Charge Compounds Compounds that contain a metal with a
fixed charge (group 1, 2, and 3, with Zn 2+, Ag +, etc.), and a
non-metal To name these compounds, use the name of metal and the
name of the non-metal with the ending replaced by the suffix ide
Examples: NaCl (Na + Cl - ) CaS (Ca 2+ S 2- ) AlI 3 (Al 3+ 3I - )
sodium chloride calcium sulfide aluminum iodide
- Slide 44
- Cations and Anions Common Simple Cations and Anions CationName
AnionName* H + hydrogen H - hydride Li + lithium F - fluoride Na +
sodium Cl - chloride K + potassium Br - bromide Cs + cesium I -
iodide Be 2+ beryllium O 2- oxide Mg 2+ magnesium S 2- sulfide Al
3+ aluminum N 3- nitride Ag + silver P 3- phosphide Zn 2+ zinc *
The root is given in color Zumdahl, Zumdahl, DeCoste, World of
Chemistry 2002, page 86 EXCEPTIONS
- Slide 45
- Perhaps one of you gentlemen would mind telling me just what is
outside the window that you find so attractive..? Image courtesy
NearingZero.net
- Slide 46
- Fixed Charge Naming Practice FormulaName 1
BaO____________________ 2________________ sodium bromide 3 MgI 2
____________________ 4 KCl____________________ 5________________
strontium fluoride 6________________ cesium fluoride barium oxide
NaBr magnesium iodide potassium chloride SrF 2 CsF
- Slide 47
- (NH 4 ) 3 N Na 2 Cr 2 O 7 Al 2 (SO 4 ) 3 NH 4 ClO 3 Mg(NO 2 ) 2
BaSO 4 Fixed Charge Nomenclature w /Polyatomic Ions Simply insert
the name of the polyatomic ion into the final name Ba 2+ and SO 4 2
Mg 2+ and NO 2 NH 4 + andClO 3 Al 3+ andSO 4 2 Na + andCr 2 O 7 2
NH 4 + andN 3 barium sulfate magnesium nitrite ammonium chlorate
alumnium sulfate sodium dichromate ammonium nitride
- Slide 48
- Polyatomic Ions Quiz phosphate sulfate dichromate permanganate
acetate PO 4 3- SO 4 2- Cr 2 O 7 2- .. MnO 4 - .. CH 3 COO - .
- Slide 49
- Variable Charge Compound Nomenclature Metals (variable charge)
+ Nonmetals
- Slide 50
- Roman Numeral Review Greek Number Roman Numeral 1I 2II 3III 4IV
5V 6VI 7VII 8VIII 9IX 10X NumberRoman Numeral 1I 5V 10X 50L
100C
- Slide 51
- Li 3 H1H1 He 2 C6C6 N7N7 O8O8 F9F9 Ne 10 Na 11 B5B5 Be 4 H1H1
Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 K 19 Ca 20 Sc 21 Ti 22 V 23 Cr 24
Mn 25 Fe 26 Co 27 Ni 28 Cu 29 Zn 30 Ga 31 Ge 32 As 33 Se 34 Br 35
Kr 36 Rb 37 Sr 38 Y 39 Zr 40 Nb 41 Mo 42 Tc 43 Ru 44 Rh 45 Pd 46 Ag
47 Cd 48 In 49 Sn 50 Sb 51 Te 52 I 53 Xe 54 Cs 55 Ba 56 Hf 72 Ta 73
W 74 Re 75 Os 76 Ir 77 Pt 78 Au 79 Hg 80 Tl 81 Pb 82 Bi 83 Po 84 At
85 Rn 86 Fr 87 Ra 88 Rf 104 Db 105 Sg 106 Bh 107 Hs 108 Mt 109 Mg
12 Ce 58 Pr 59 Nd 60 Pm 61 Sm 62 Eu 63 Gd 64 Tb 65 Dy 66 Ho 67 Er
68 Tm 69 Yb 70 Lu 71 Th 90 Pa 91 U 92 Np 93 Pu 94 Am 95 Cm 96 Bk 97
Cf 98 Es 99 Fm 100 Md 101 No 102 Lr 103 La 57 Ac 89 1 2 3 4 5 6 7
Single charge cations Variable charge cations Elemental anions 1+
2+3+1-2-3-
- Slide 52
- Stock System of nomenclature Variable Charge Ionic Compounds To
name, given the formula: 1. Figure out charge on cation 2. Write
name of cation 3. Write Roman numerals in ( ) to show cations
charge Compounds that contain a metal with variable charge (Pb, Sn,
and the transition metalsnot including Ag or Zn), and a
non-metal
- Slide 53
- Variable charge Naming Practice 4. Write name of anion: FeOFe ?
O 2 Fe 2 O 3 2 Fe ? 3 O 2 CuBrCu ? Br CuBr 2 Cu ? 2 Br iron(II)
oxide iron(III) oxide copper(I) bromide copper(II) bromide
- Slide 54
- Variable Charge Cations Common Type II Cations IonStock System
Traditional System Fe 3+ iron (III)ferric Fe 2+ iron (II)ferrous Cu
2+ copper (II)cupric Cu 1+ copper (I)cuprous Co 3+ cobalt
(III)cobaltic Co 2+ cobalt (II)cobaltous Sn 4+ tin (IV)stannic Sn
2+ tin (II)stannous Pb 4+ lead (IV)plumbic Pb 2+ lead (II)plumbous
Hg 2+ mercury (II)mercuric Hg 2 2+ mercury (I)mercurous * Mercury
(I) ions are always bonded together in pairs to form Hg 2 2+
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 90
- Slide 55
- To find the formula, given the name: 2. Balance charges to
write formula cobalt (III) chlorideCo 3+ Cl tin (IV) oxideSn 4+ O 2
tin (II) oxideSn 2+ O 2 1. Write symbols for the two types of ions
Variable Charge Ionic Compounds SnO SnO 2 CoCl 3
- Slide 56
- Naming Variable Charge Ionic Compounds FormulaName 1 Hg 2
O____________________ 2 HgO____________________ 3________________
copper (II) fluoride 4________________ copper (I) sulfide 5 Cr 2 O
3 ____________________ 6________________ lead (IV) oxide mercury
(I) oxide PbO 2 mercury (II) oxide CuF 2 Cu 2 S chromium (III)
oxide
- Slide 57
- Ionic Compounds with Polyatomic Ions 1.________________ iron
(II) phosphate 2.________________ ammonium carbonate
3.________________ aluminum sulfate 4. V 2 SO 3
____________________ 5. AgCN____________________ 6. Ba(ClO 3 ) 2
____________________ 7.________________ copper (II) hydroxide Fe 3
(PO 4 ) 2 (NH 4 ) 2 CO 3 Al 2 (SO 4 ) 3 vanadium (I) sulfite silver
cyanide barium chlorate Cu(OH) 2
- Slide 58
- Acidic Compounds Oxysalts + H 2 O Oxyacids
- Slide 59
- Acidic Compounds (Nonmetals Dissolved in Water) The prefix
hydro- is used to represent hydrogen, followed by the root name of
the nonmetal with its ending replaced by the suffix ic acid.
Examples: *HCl(aq) HBr(aq) *The name of this gas would be hydrogen
monochloride if it was NOT dissolved in water. Acids(aq) without
oxygen Hydrochloric acid Hydrobromic acid (aq) = aqueous or
dissolved in water
- Slide 60
- Acidic Compounds Nonmetals Dissolved in Water Start with the
name of the polyatomic ion (with oxygen), and change the ending
based on the following rule: If the ion ends in ate, change the
suffix to ic acid. If the ion ends in ite, change the suffix to ous
acid. Retain any prefixes such as per or hypo in front of the acid
name. NEVER use hydro! Examples: HClO 3 (aq) HBrO(aq) Acids(aq)
WITH oxygen (oxyacids) Chloric acid Hypobromous acid ClO 3 - =
chlorate BrO - = hypobromite
- Slide 61
- An acid with a name ending in An ion with a name ending in -ic
-ous -ate -ite Hill, Petrucci, General Chemistry An Integrated
Approach 1999, page 60 Oxyacid Naming Rules
- Slide 62
- Common Oxyacid Names The following table lists the most common
families of oxy acids. one more oxygen atom most common one less
oxygen two fewer oxygens HClO 4 perchloric acid HClO 3 chloric acid
HClO 2 chlorous acid HClO hypochlorous acid H 2 SO 4 sulfuric acid
H 2 SO 3 sulfurous acid H 3 PO 4 phosphoric acid H 3 PO 3
phosphorous acid H 3 PO 2 hypophosphorous acid HNO 3 nitric acid
HNO 2 nitrous acid
- Slide 63
- Acid Nomenclature Practice FormulaName 1
HCl____________________ 2 HClO____________________
3________________ sulfuric acid 4________________ hydrofluoric acid
5 H 3 N____________________ 6________________ periodic acid
hydrochloric acid HIO 4 hypochlorous acid H 2 SO 4 HF hydronitric
acid
- Slide 64
- Covalent Compounds Nonmetal + Nonmetal
- Slide 65
- Writing Formulas of Covalent Compounds Covalent Compounds
contain two or more non-metals (NO METALS!) Key: FORGET CHARGES To
Name, given the formula: 1. Use Greek prefixes to indicate how many
atoms of each element, but dont use mono on first element (least
electronegative, excluding H) 2. Add the suffix ide to the second
element (most electronegative) 1 mono 6 hexa 2 di7 hepta 3 tri8
octa 4 tetra9 nona 5 penta10 deca Prefixes to memorize!
- Slide 66
- Covalent Nomenclature Practice EXAMPLES: 1. carbon dioxide 2.
CO 3. dinitrogen trioxide 4. SF 6 5. carbon tetrachloride 6. NI 3
CO 2 carbon monoxide N2O3N2O3 sulfur hexafluoride CCl 4 nitrogen
triiodide
- Slide 67
- More Practice with covalent compounds 1.________________
diarsenic trisulfide 2.________________sulfur dioxide 3. P 2 O 5
____________________ 4.________________ nitrogen trihydride 5. N 2
O 5 ____________________ 6. H 2 O____________________ As 2 S 3 SO 2
diphosphorus pentoxide NH 3 dinitrogen pentoxide dihydrogen
monoxide
- Slide 68
- Naming Simple Chemical Compounds Ionic (metal and
nonmetal)Covalent (2 nonmetals) Metal Forms only one positive ion
Forms more than one positive ion Nonmetal Use the name of element
Use element name followed by a Roman numeral to show the charge
First nonmetal Second nonmetal Before element name use a prefix to
match subscript Use a prefix before element name and end with ide
Single Negative Ion Polyatomic Ion Use the name of the element, but
end with ide Use the name of polyatomic ion (ate or Ite)
- Slide 69
- fluoride sulfide bromide diphosphide iodide tetrachloride oxide
phosphide iridium (III) calcium titanium (IV) hydrochloric acid
barium trinitrogen hydrofluoric acid zinc nitrogen gold (III)
sodium Ir Ca Ti H Ba N 3 H Zn N Au Na F 3 S S 2 Cl(aq) Br 2 P 2
F(aq) I 2 Cl 4 2 O 3 3 P Ionic/variable Ionic/fixed Ionic/variable
Acid Ionic/fixed Covalent Acid Ionic/fixed Covalent Ionic/variable
Ionic/fixed Overall Nomenclature Practice
- Slide 70
- dichromate hydroxide acid acetate acid sulfate cyanide nitrite
chlorate phosphate acid iridium (III) calcium nitric platinum (II)
bromous strontium potassium zinc manganese (IV) gold (III)
sulfurous (Cr 2 O 7 ) 3 (OH) 2 NO 3 (aq) (CH 3 COO) 2 BrO 2 (aq) SO
4 CN (NO 2 ) 2 (ClO 3 ) 4 PO 4 SO 3 (aq) Ir 2 Ca H Pt H Sr K Zn Mn
Au H2H2 Ionic/variable Ionic/fixed Acid Ionic/variable Acid
Ionic/fixed Ionic/variable Acid Ionic Nomenclature Practice
- Slide 71
- Covalent Ionic (M + NM) Two or more NMsVariable charge cation
Fixed charge cation Roman numeral Polyatomic ions OK Roman numeral
for name only Polyatomic ions Greek prefixes Charge Criss-Cross
Rule Roman numeral OK Where would you file these? VCrO 4 BaO CBr 4
Nb(ClO 4 ) 5 SCl 2 Rb 2 SO 4 dinitrogen pentoxide platinum (IV)
iodate ammonium chlorate potassium iodide nitrogen trichloride
manganese (V) sulfide vanadium (II) chromate VCrO 4 N2O5N2O5
dinitrogen pentoxide barium oxide BaO Pt(IO 3 ) 4 platinum (IV)
iodate carbon tetrabromide CBr 4 NH 4 ClO 3 ammonium chlorate
niobium (V) perchlorate Nb(ClO 4 ) 5 KI potassium iodide sulfur
dichloride SCl 2 NCl 3 nitrogen trichloride rubidium sulfate Rb 2
SO 4 Mn 2 S 5 manganese (V) sulfide
- Slide 72
- Suffixes have meaning -idebinary compound sodium chloride
(NaCl) -ite or -atepolyatomic compound sulfite(SO 3 2- ) sulfate
(SO 4 2- )-ate means one more oxygen than -ite -olalcohol methyl
alcohol (methanol) -osesugar sucrose -aseenzyme sucrase
- Slide 73
- Extra Slides H H O S O O O
- Slide 74
- Compounds Containing Polyatomic Ions Insert name of ion where
it should go in the compounds name. Write formulas: iron (III)
nitrate ammonium phosphide ammonium chlorite zinc phosphate lead
(II) permanganate Fe(NO 3 ) 3 (NH 4 ) 3 P NH 4 ClO 2 Zn 3 (PO 4 ) 2
Pb(MnO 4 ) 2 Fe 3+ NO 3 1 NH 4 1+ P 3 NH 4 1+ ClO 2 1 Zn 2+ PO 4 3
Pb 2+ MnO 4 1 3 3 32 2
- Slide 75
- Write names: (NH 4 ) 2 S 2 O 3 AgBrO 3 (NH 4 ) 3 N U(CrO 4 ) 3
Cr 2 (SO 3 ) 3 Writing Formulas of Ionic Compounds ammonium
thiosulfate silver bromate ammonium nitride uranium (VI) chromate
chromium (III) sulfite CrO 4 2 SO 3 2 3 32 Cr U ? ? 6+ 3+
- Slide 76
- Element Latin root -ic -ous gold, Auaur- Au 3+ Au 1+ lead,
Pbplumb- Pb 4+ Pb 2+ tin, Snstann- Sn 4+ Sn 2+ copper, Cucupr- Cu
2+ Cu 1+ iron, Feferr- Fe 3+ Fe 2+ Traditional (OLD) System of
Nomenclature used historically (and still some today) to name
compounds w /multiple-charge cations To use: 1. Use Latin root of
cation. 2. Use -ic ending for higher charge -ous lower 3. Then say
name of anion, as usual. ; (icky food is good for you!) ;
(delicious food is not good for you!)
- Slide 77
- Cu 2 S AuN FeF 2 plumbic phosphide plumbous phosphide stannic
chloride Fe 2+ Write formulas:Write names: cuprous sulfide auric
nitride ferrous fluoride Pb 3 P 4 3 Pb ? 4 P 3 Cu 1+ Pb 3 P 2 3 Pb
? 2 P 3 Au 3+ SnCl 4 Sn ? 4 Cl 1 S 2 N 3 F 1
- Slide 78
- Polyatomic Ion: a group of atoms that stay together and have a
single, overall charge. BrO 4 1- Perbromate ion BrO 3 1- Bromate
ion BrO 2 1- Bromite ion BrO 1- Hypobromite ion CO 4 2- CO 3 2-
Carbonate ion CO 2 2- CO 2- ClO 4 1- ClO 3 1- Chlorate ion ClO 2 1-
ClO 1- IO 4 1- IO 3 1- Iodate ion IO 2 1- IO 1- NO 4 1- NO 3 1-
Nitrate ion NO 2 1- NO 1- PO 5 3- PO 4 3- Phosphate ion PO 3 3- PO
2 3- SO 5 2- SO 4 2- Sulfate ion SO 3 2- SO 2 2- 1 more
oxygennormal1 less oxygen2 less oxygen
- Slide 79
- Two nonmetalsMultiple-charge cationEverything else Roman
numeral Polyatomic ions OK Roman numeral for name only Polyatomic
ions Greek prefixes Charge Criss- Cross Rule Roman numeral OK Where
would you file this? VCrO 4 BaO CBr 4 Nb(ClO 4 ) 5 SCl 2 Rb 2 SO 4
dinitrogen pentoxide platinum (IV) iodate ammonium chlorate
potassium iodide nitrogen trichloride manganese (V) sulfide
vanadium (II) chromate VCrO 4 N2O5N2O5 dinitrogen pentoxide barium
oxide BaO Pt(IO 3 ) 4 platinum (IV) iodate carbon tetrabromide CBr
4 NH 4 ClO 3 ammonium chlorate niobium (V) perchlorate Nb(ClO 4 ) 5
KI potassium iodide sulfur dichloride SCl 2 NCl 3 nitrogen
trichloride rubidium sulfate Rb 2 SO 4 Mn 2 S 5 manganese (V)
sulfide
- Slide 80
- Two nonmetalsMultiple-charge cationEverything else Roman
numeral Polyatomic ions Roman numeral for name only Polyatomic ions
Greek prefixes Charge Criss- Cross Rule Roman numeral OK Where
would you file this? VCrO 4 dinitrogen pentoxide BaO platinum (IV)
iodate CBr 4 ammonium chlorate Nb(ClO 4 ) 5 potassium iodide SCl 2
nitrogen trichloride Rb 2 SO 4 manganese (V) sulfide
- Slide 81
- Write the total number of atoms that make up each compound.
Write the compound formed by the following ions: 1) Al 3+ S 2- 2)
Mg 2+ PO 4 3- When a formula is givenwrite the proper name. When a
name is givenwrite the proper formula. 3) BaO 4) lithium bromide 5)
Ni 2 S 3 6) triphosphorus heptoxide 7) N 2 O 5 8) molybdenum (VI)
nitride 9) trinitrotoluene (TNT) CH 3 C 6 H 2 (NO 2 ) 3 10)
phosphoric acid H 3 PO 4 Extra credit: What is the formula for
plumbic iodide? (Hint: lead is Pb 2+ or Pb 4+ )
- Slide 82
- Write the total number of atoms that make up each compound.
Write the compound formed by the following ions: 1) Al 3+ S 2- 2)
Mg 2+ PO 4 3- When a formula is givenwrite the proper name. When a
name is givenwrite the proper formula. 3) BaO 4) lithium bromide 5)
Ni 2 S 3 6) triphosphorus heptoxide 7) N 2 O 5 8) molybdenum (VI)
nitride 9) trinitrotoluene (TNT) CH 3 C 6 H 2 (NO 2 ) 3 10)
phosphoric acid H 3 PO 4 Extra credit: What is the formula for
plumbic iodide? (Hint: lead is Pb 2+ or Pb 4+ ) POP QUIZ