Unit 5: Bonding and Inorganic Nomenclature Chemistry NaClO 3 Fe(ClO 3 ) 2 lithium nitrate lithium nitride lithium nitrite lead (II) sulfide barium sulfide sulfur dioxide Fe(ClO 3 ) 3 NO 2 N 2 O 4 N 2 O 5
Transcript
Slide 1
Slide 2
Unit 5: Bonding and Inorganic Nomenclature Chemistry NaClO 3
Fe(ClO 3 ) 2 lithium nitrate lithium nitride lithium nitrite lead
(II) sulfide barium sulfide sulfur dioxide Fe(ClO 3 ) 3 NO 2 N 2 O
4 N 2 O 5
Slide 3
Bonding Types 1.Ionic Bonding with ions (+/- charges) atoms
gaining/losing e- M + NM 2.Covalent Bonding atoms sharing e- NM +
NM 3.Metallic Bonding metals share e- freely sea of e- good
conductors
Slide 4
Chemical Bonding Ionic Bonds: atoms give up or gain e and are
attracted to each other by coulombic attraction Na Na + Cl Cl loses
e gains e Na + + Cl NaCl K + + NO 3 KNO 3 ionic compounds = salts
where NO 3 is a polyatomic ion: a charged group of atoms that stay
together ionic bonds: M + NM cation + anion
Slide 5
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 also be responsible for knowing these
Slide 6
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 7
Properties of Ionic Salts 1. very hard 2. high melting points
3. brittle each ion is bonded to several oppositely charged ions
many bonds must be broken with sufficient force, like atoms are
brought next to each other and repel calcite
Slide 8
Writing Formulas of Ionic Compounds chemical formula: 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 shows types of atoms and how many of each NaF BaO Na 2 O BaF
2 (i.e., cations and anions) has neutral charge;
Slide 9
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 Notice that the pink
pieces are cations (metals) and the blue are anions (non-metals) 1
Mg 2+ 2 Br -
Slide 10
Chemical Bonding Activity Examples Na + Pb 4+ OH - 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 1 Mg 2+ 2
OH - Mg OH 2 1 Na + 1 OH - NaOH
Slide 11
charge on cation / anion becomes subscript of anion / cation **
Warning: Al 3+ and O 2 Ba 2+ and S 2 In 3+ and Br 1 Reduce to
lowest terms Al O Ba S In Br 2 3 2 2 3 1 Al 2 O 3 BaS InBr 3
criss-cross rule:
Slide 12
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 + and ClO 3 Sn 4+ and SO 4
2 Fe 3+ and Cr 2 O 7 2 NH 4 + and N 3 BaSO 4 Mg(NO 2 ) 2 NH 4 ClO 3
Sn(SO 4 ) 2 Fe 2 (Cr 2 O 7 ) 3 (NH 4 ) 3 N
Slide 13
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!
Slide 14
1+ Charges Reminder! Group 1: Group 2: Group 3: Group 5: Group
6: Group 7: Group 8: 2+ 3+ 3 2 1 0 1+ 2+ 3+ 3 2 1 0
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 17
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. 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 18
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 19
Ionic Compounds (cation/anion combos) Fixed-Charge Cations with
Elemental Anions The fixed-charge cations are: groups 1, 2, 13, Ag
+ and Zn 2+ i.e., pulled off the Table anions 1+ 2+ 3+ 3 2 1
Slide 20
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 21
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 22
A. To name, given the formula: 2. Use name of anion (it has the
ending ide) 1. Use name of cation NaF BaO Na 2 O BaF 2 sodium
fluoride barium oxide sodium oxide barium fluoride Na Ba 1+ 2+ 3 2
1 3+
Slide 23
1. Write symbols for the two types of ions 2. Balance charges
to write formula silver sulfide zinc phosphide calcium iodide B. To
write formula, given the name: Ag + S 2 Ag 2 S Zn 2+ P 3 Zn 3 P 2 I
Ca 2+ CaI 2 Ca Ag Zn 1+ 2+ 3 2 1 3+
Slide 24
Variable-Charge Cations with Elemental Anions The
variable-charge cations are: i.e., pulled off the Table anions Pb,
Sn, and the transition metals (but of course! not Ag or Zn)
Slide 25
iron oxide A. 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. 4. Write name of anion. FeO Fe 2 O 3 CuBr
CuBr 2 iron oxide Cu Fe Stock System of nomenclature Fe ? O 2 iron
(II) oxide Fe ? O 2 iron (III) oxide copper bromide copper bromide
Cu ? Br copper (I) bromide Cu 2+ Br copper (II) bromide Fe ? Br O 2
O 2 Fe 2+ Fe 3+ Cu + Cu ? - 6
Slide 26
Roman Numeral Review Greek Number Roman Numeral 1I 2II 3III 4IV
5V 6VI 7VII 8VIII 9IX 10X NumberRoman Numeral 50L 100C 500D
1000M
Slide 27
B. To find the formula, given the name: 1. Write symbols for
the two types of ions. 2. Balance charges to write formula. cobalt
(III) chloride tin (IV) oxide tin (II) oxide Co Sn Co 3+ Cl CoCl 3
Sn 4+ O 2 O 2 Sn 2+ SnO 2 SnO
Slide 28
Ionic Nomenclature Practice 1.sodium hydroxide 2.HgSO 4 3. lead
(II) phosphate 4. (NH 4 ) 2 S 5. aluminum chlorate 6. Cu 2 CO 3
7.manganese (IV) oxide 8.MnSO 4 9. iron (III) oxide 10. Mg(NO 3 ) 2
11. calcium sulfide 12. K 2 O 13. magnesium chloride 14. Cr 2 O 3
15. gold (III) bromide 16. Zn(NO 2 ) 2 NaOH mercury (II) sulfate Pb
3 (PO 4 ) 2 ammonium sulfide Al(ClO 3 ) 3 copper (I) carbonate MnO
2 manganese (II) sulfate Fe 2 O 3 magnesium nitrate CaS potassium
oxide MgCl 2 chromium (III) oxide AuBr 3 zinc nitrite
Slide 29
Traditional 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
ending for lower charge. 3. Then say name of anion, as usual.
Slide 30
ElementLatin root-ic-ous gold, Auaur-Au 3+ Au + lead,
Pbplumb-Pb 4+ Pb 2+ tin, Snstann-Sn 4+ Sn 2+ copper, Cucupr-Cu 2+
Cu + iron, Feferr-Fe 3+ Fe 2+ Write formulas: cuprous sulfide auric
nitride ferrous fluoride Write names: Pb 3 P 4 Pb 3 P 2 SnCl 4 Cu +
S 2 Cu 2 S Au 3+ N 3- AuN Fe 2+ FF FeF 2 cuprous sulfide auric
ferrous fluoride Pb 3 P 4 Pb 3 P 2 Sn P 3 Pb ? Pb ? P 3 Pb 4+
plumbic phosphide Pb 2+ plumbous phosphide Cl Sn 4+ Sn ? stannic
chloride
Slide 31
Compounds Containing Polyatomic Ions Insert name of ion where
it should go in the compounds name. Write formulas: iron (III)
nitrite ammonium phosphide ammonium chlorate zinc phosphate lead
(II) permanganate iron (III) nitrite ammonium phosphide ammonium
chlorate zinc phosphate lead (II) permanganate Fe 3+ NO 2 Fe(NO 2 )
3 NH 4 + NH 4 + P 3 (NH 4 ) 3 P ClO 3 NH 4 ClO 3 Zn 2+ PO 4 3 Zn 3
(PO 4 ) 2 Pb 2+ MnO 4 Pb(MnO 4 ) 2
Slide 32
Write names: (NH 4 ) 2 S 2 O 3 AgBrO 3 (NH 4 ) 3 N U(CrO 4 ) 3
Cr 2 (SO 3 ) 3 (NH 4 ) 2 S 2 O 3 AgBrO 3 (NH 4 ) 3 N U(CrO 4 ) 3 Cr
2 (SO 3 ) 3 ammonium thiosulfate silver bromate ammonium nitride U
? CrO 4 2 CrO 4 2 CrO 4 2 uranium (VI) chromate Cr ? Cr ? Cr 3+ SO
3 2 SO 3 2 SO 3 2 chromium (III) sulfite U 6+
Slide 33
4. NaClO 3 5. Fe(ClO 3 ) 2 1. lithium nitrate 2. lithium
nitride 3. lithium nitrite 7. lead(II) sulfide 8. barium sulfide 6.
Fe(ClO 3 ) 3 9. Never show charges in a compounds formula. (T/F)
10. When writing names with Group 9 cations, you need to use Roman
numerals. (T/F) 11. When using an anion off the polyatomic ion
sheet, change names ending to -ide. (T/F) 12. A Roman numeral
indicates the charge on the anion. (T/F) Self-Test Quiz
9. Never show charges in a compounds formula. 10. When writing
names with Group 9 cations, you need to use Roman numerals. 11.
When using an anion off the polyatomic ion sheet, change the names
ending to -ide. 12. A Roman numeral indicates the charge on the
anion. Self-Test Quiz Answers T T F F
Slide 36
Covalent Bonds (2 nonmetals) atoms share e to get a full
valence shell C1s 2 2s 2 2p 2 F1s 2 2s 2 2p 5 Both need 8 valence e
- for a full outer shell otherwise known as the octet rule o 4
valence e- 7 valence e- o x o o C x x x x x x F
Slide 37
Draw the Lewis dot structure for the following elements: Si O P
B Ar Br 1s 2 2s 2 2p 6 3s 2 3p 3 1s 2 2s 2 2p 4 1s 2 2s 2 2p 1 1s 2
2s 2 2p 6 3s 2 3p 6 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 5 1s 2
2s 2 2p 6 3s 2 3p 2 4 valence e- 6 valence e- 5 valence e- 3
valence e- 8 valence e- 7 valence e-
Slide 38
Notice any trends?
Slide 39
Drawing Lewis Structures Lewis structure: 1. Two shared e make
a single covalent bond, four make a double bond, etc. 2. unshared
pairs: pairs of unbonded valence e 3. Each atom needs a full outer
shell, i.e., 8 e . Exception: H needs 2 e a model of a covalent
molecule that shows all of the valence e
Slide 40
C F F F F Lets bond two F atoms together Each F has 7 v.e. and
each needs 1 more e- F F F F Now lets bond C and F atoms together C
F F F F carbon tetrafluoride (CF 4 ) F2F2
Slide 41
And now, a video break
Slide 42
oo o o N o nitrogen triiodide (NI 3 ) carbon dioxide (CO 2 ) x
x x x xx I x x xx x xx I x x xx x xx I x x xx xx I x x x xx x xx I
x x xx x xx I x oo o o N oN o o C o o ox xx x x O x x xx x x O x x
xx x x O x o C o o o O = C = O x x x xx x x O x
Slide 43
butter (consist of two or more nonmetal elements) covalent
compounds = molecular compounds -- have lower melting points than
do ionic compounds
Slide 44
Dihydrogen Monoxide: A Tale of Danger and Irresponsibility
major component of acid rain found in all cancer cells inhalation
can be deadly excessive ingestion results in acute physical
symptoms: e.g., frequent urination, bloated sensation, profuse
sweating often an industrial byproduct of chemical reactions;
dumped wholesale into rivers and lakes
Slide 45
mono Covalent Compounds -- contain two types of ** Key: Use
Greek prefixes to indicate how many atoms of each element, but dont
use mono on first element. nonmetals FORGET CHARGES! What to do: 1
2 3 4 5 6 7 8 9 10 di tri tetra penta hexa hepta octa nona
deca
Slide 46
EXAMPLES: carbon dioxide CO dinitrogen trioxide N2O5N2O5 carbon
tetrachloride NI 3 CO 2 carbon monoxide N 2 O 3 dinitrogen
pentoxide CCl 4 nitrogen triiodide
Slide 47
In insulators (like wood), the v.e are attached to particular
atoms. Metallic Bonds In metals, valence shells of atoms overlap,
so v.e are free to travel between atoms through material. Not so in
metals.
Slide 48
All due to free-moving v.e . Properties of Metals ductile
conduct heat and electricity malleable
Slide 49
These are much weaker than ionic, covalent, or metallic bonds,
but very important in determining states of matter, boiling and
melting points, and molecular shape (among other things). Other
Types of Forces/Attractions dipole-dipole forces hydrogen bonds
London dispersion forces ion-dipole forces DNA boiling H 2 O
Slide 50
Empirical Formula and Molecular Formula Compound Molecular
Formula Empirical Formula glucoseC 6 H 12 O 6 propaneC3H8C3H8
butaneC 4 H 10 naphthaleneC 10 H 8 sucroseC 12 H 22 O 11 octaneC 8
H 18 lowest-terms formula shows the true number and type of atoms
in a mcule CH 2 O C3H8C3H8 C2H5C2H5 C5H4C5H4 C 12 H 22 O 11
C4H9C4H9
Slide 51
Nomenclature Review Flow Chart
Slide 52
Metal + Nonmetal? Formula Name? Ionic Covalent Two Nonmetals?
Variable Fixed Use Prefixes! *Mono* Hexa Di Hepta Tri Octa Tetra
Nona Penta Deca 1.Write name of cation (metal) 2.Determine the
charge on the metal by balancing the (-) charge from the anion
3.Write the charge of the metal in Roman Numerals and put in
parentheses 4.Write name of anion (Individual anions need ide
ending!) Steps 1 & 4 ONLY d,f-block Pb,Sn Columns 1, 2, 13 Ag
+, Zn 2+ (Including NH 4 + ) Metal Type? Add ide to 2 nd
element
Slide 53
Name Formula? No Prefixes? Prefixes? 1.Determine the ions
present and the charge on each (Roman Numeral = cation charge,
otherwise use PT) 2.Balance formula (criss-cross) 3.Reduce
subscripts (if needed) 1.FORGET CHARGES!!! 2.Use prefixes to
determine subscripts 3.Do NOT reduce subscripts! Ionic
Covalent
Slide 54
Two nonmetalsVariable-charge cationFixed-charge 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 Covalent Ionic Compounds Dont know the charge from PT Know
the charge from PT
Slide 55
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 56
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 57
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 58
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
Slide 59
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+ ) Answer Key Al 2 S 3
Mg 3 (PO 4 ) 2 barium oxide nickel (III) sulfide LiBr dinitrogen
pentoxide MoN 2 8 21 PbI 4 P3O7P3O7
Slide 60
4. S F 6 5. Fe (NO 3 ) 3 1. Ni 2 S 3 2. N F 3 3. Na BrO 3 6. Sr
SO 4 Writing Chemical Names FormulaRN/GP/neither Use poly. ion
sheet? Name GP RN GP neither no yes no yes sulfur hexafluoride iron
(III) nitrate nickel (III) sulfide nitrogen trifluoride sodium
bromate strontium sulfate
Slide 61
10. oxygen difluoride 4. zinc arsenate 5. silver nitride 1.
copper (II) phosphide 2. lithium phosphate 3. phosphorus triiodide
7. dinitrogen pentasulfide 8. tin (IV) nitride 6. sulfur dibromide
Writing Chemical Formulas 9. rubidium nitrite 11. iron (III)
sulfite 12. ammonium oxide NameCharges matter? Use poly. ion sheet?
Formula yes no yes no yes no yes no yes no yes no Zn 3 (AsO 4 ) 2
Ag 3 N Cu 3 P 2 Li 3 PO 4 PI 3 N2S5N2S5 Sn 3 N 4 SBr 2 RbNO 2 Fe 2
(SO 3 ) 3 (NH 4 ) 2 O OF 2
Slide 62
7. S O 3 8. Sn Br 4 Writing Chemical Names 9. K 3 PO 4 11. C S
2 12. Cu F 10. NH 4 OH FormulaRN/GP/neither Use poly. ion sheet?
Name GP neither GP RN neither no yes no yes sulfur trioxide tin
(IV) bromide potassium phosphate carbon disulfide copper (I)
fluoride ammonium hydroxideyes
Slide 63
10. oxygen difluoride 4. zinc arsenate 5. silver nitride 1.
copper (II) phosphide 2. lithium phosphate 3. phosphorus triiodide
7. dinitrogen pentasulfide 8. tin (IV) nitride 6. sulfur dibromide
Writing Chemical Formulas 9. rubidium nitrite 11. iron (III)
sulfite 12. ammonium oxide NameCharges matter? Use poly. ion sheet?
Formula yes no yes no yes no yes no yes no yes no Zn 3 (AsO 4 ) 2
Ag 3 N Cu 3 P 2 Li 3 PO 4 PI 3 N2S5N2S5 Sn 3 N 4 SBr 2 RbNO 2 Fe 2
(SO 3 ) 3 (NH 4 ) 2 O OF 2
Slide 64
10. oxygen difluoride 4. zinc arsenate 5. silver nitride 1.
copper (II) phosphide 2. lithium phosphate 3. phosphorus triiodide
7. dinitrogen pentasulfide 8. tin (IV) nitride 6. sulfur dibromide
Writing Chemical Formulas 9. rubidium nitrite 11. iron (III)
sulfite 12. ammonium oxide NameCharges matter? Use poly. ion sheet?
Formula yes no yes no yes no yes no yes no yes no Zn 3 (AsO 4 ) 2
Ag 3 N Cu 3 P 2 Li 3 PO 4 PI 3 N2S5N2S5 Sn 3 N 4 SBr 2 RbNO 2 Fe 2
(SO 3 ) 3 (NH 4 ) 2 O OF 2
Slide 65
4. S F 6 5. Fe (NO 3 ) 3 1. Ni 2 S 3 2. N F 3 3. Na BrO 3 7. S
O 3 8. Sn Br 4 6. Sr SO 4 Writing Chemical Names 9. K 3 PO 4 11. C
S 2 12. Cu F 10. NH 4 OH FormulaRN/GP/neither Use poly. ion sheet?
Name GP RN GP neither GP neither GP RN neither no yes no yes no yes
no yes sulfur hexafluoride iron (III) nitrate nickel (III) sulfide
nitrogen trifluoride sodium bromate sulfur trioxide tin (IV)
bromide strontium sulfate potassium phosphate carbon disulfide
copper (I) fluoride ammonium hydroxide
Slide 66
10. oxygen difluoride 4. zinc arsenate 5. silver nitride 1.
copper (II) phosphide 2. lithium phosphate 3. phosphorus triiodide
7. dinitrogen pentasulfide 8. tin (IV) nitride 6. sulfur dibromide
Writing Chemical Formulas 9. rubidium nitrite 11. iron (III)
sulfite 12. ammonium oxide NameCharges matter? Use poly. ion sheet?
Formula yes no yes no yes no yes no yes no yes no Zn 3 (AsO 4 ) 2
Ag 3 N Cu 3 P 2 Li 3 PO 4 PI 3 N2S5N2S5 Sn 3 N 4 SBr 2 RbNO 2 Fe 2
(SO 3 ) 3 (NH 4 ) 2 O OF 2