1. Polyatomic Ions

2. -ate and -ite NO3- nitrate NO2- nitrite
-ate is great, -ite is slight -ate has one more oxygen than –ite
hypo- under one less
per- completely one more

3. Name other ions by analogy with element above
SeO42- selenate
BrO3- bromate
HSe- hydrogen selenide
H2AsO4- dihydrogen arsenate

4. Permanganate is?
MnO2-
MgO4-
MnO42-
MnO4-
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5. IO- is?
hypoiodite
iodite
iodide
iodate
iodine monoxide
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6. Hydrogen selenite is?
H2Se
H2SeO3
HSeO3-
HSeO2-
HSeO4-
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7. Names of Ionic Compounds
1. Name the metal first.
For all metals except groups 1,2, Ag, Zn, Al use Roman numerals in parentheses for charge.
2. Then name the polyatomic ion or non-metal,
changing the ending of the non-metal to
-ide.
3. For hydrates use Greek prefixes to specify the number of water molecules e.g. dihydrate

8. Some Common Hydrated Ionic Compounds

9. Simple Salts Ti3N4 titanium(IV) nitride Fe2O3 iron(III) oxide Ag2O
silver oxide
SnCl4.5H2O
tin(IV) chloride pentahydrate
Mg3N2
magnesium nitride
ZnI2
zinc iodide
No roman numerals needed for Ag, Zn, Al Using roman numerals is only wrong for groups 1 and 2

10. Salts with Polyatomic Ions
NH4NO3
ammonium nitrate
KBrO3
potassium bromate
Mg(MnO4)2.6H2O
magnesium permanganate hexahydrate
Cu(OH)2
copper(II) hydroxide

11. Iron(II) phosphate is?
Fe2PO4
FePO3
Fe3(PO4)2
Fe2(PO4)3
Fe(PO4)2
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12. Zinc iodate is?
ZnIO4
ZnIO3
Zn(IO4)2
Zn(IO3)2
ZnI2 10
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13. Naming Acids Non-oxy acids hydro___ic acid Oxy acids -ate  __ic acid
-ite  __ous acid
Always in aqueous solution
HCN (aq) hydrocyanic acid
H2TeO4 (aq) telluric acid
HBrO2 (aq) bromous acid
HCN hydrogen cyanide

14. Hydrosulfuric acid is H2SO4 (aq) H2SO3 (aq) H2OS (aq) HSO4- (aq)
H2S (aq) 9
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16. Which substance is named correctly?
ZnCl2 zinc chloride
SCl2 sulfur chloride
FeCl2 iron chloride
HCl (aq) hydrogen chloride
HClO3 (aq) hydrochloric acid 10
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17. Properties of Molecular & Ionic Compounds

18. Electrical Conductivity Ionic Solution

19. Molar Mass Sum atomic masses represented by formula
atomic masses in amu  molecular mass in amu
element molar masses in g/mol  compound molar mass in g/mol
Numerical values are the same

20. Percentage Composition
Chemical formula gives the relative proportions by atom or mole
Percentage composition gives the relative proportions by g (out of 100 g total)

21. EXAMPLE: What is the percent composition of chloroform, CHCl3, a substance once used as an anesthetic?
Molecular mass
= (  )amu
= amu
1(12.011)
%C =  100% = % C
1( )
%H =  100 = 0.844% H
3(35.453)
%Cl =  100 = % Cl

22. EXAMPLE: What is the percent composition of chloroform, CHCl3, a substance once used as an anesthetic?
%C = % C
%H = 0.844% H
%Cl = % Cl
Total = = 

23. Simplest (Empirical) Formula
Simplest integer ratio of the atoms in a compound
Assume 100 g of compound, %element is then g element in sample
g element x 1 mol element = mol element
g element
CHCl g C x 1 mol C = mol C
g C
Determine simplest integer mole ratio

24. EXAMPLE: Phosphorus burns in air to produce a white compound that is 43.7% P and 56.3% O by mass. What is the empirical formula of the compound?
Assume 100 g of compound
Relative Number of Atoms
Multiply
by Integer
mass
43.7g P
56.3g O
(mass/atomic mass)
Divide by Smaller
43.7/ = 1.41
56.3/ = 3.52
2  1.00  2
2  2.50  5
1.41/1.41 = 1.00
3.52/1.41 = 2.50
.25, .33, .5, .67, .75
¼, ⅓, ½, ⅔, ¾
1:1.25 = 4:5
Empirical Formula  P2O5

25. Molecular Formula
The exact proportions of the elements that are contained in a molecule
An integer multiple (X) of the empirical formula

26. Molecular Formula from Simplest Formula
empirical formula mass  FM
sum of the atomic weights represented by the empirical formula
molar mass = MM = X  FM

27. Molecular Formula from Simplest Formula
first, knowing MM and FM
X = MM/FM
then
MF = X  EF

28. EXAMPLE: Our phosphorus compound has a molar mass of ~285
EXAMPLE: Our phosphorus compound has a molar mass of ~285. What is the molecular formula?
FM = 2 x x = MM
X = = = 2 FM
thus MF = 2  EF
P4O10

29. The empirical formula of a substance is found to be CH3O and its molecular weight is found to be roughly 61 g/mol. What is the true molecular weight of the substance?
30.5 g/mol
31.0 g/mol
61.0 g/mol
62.0 g/mol
124.0 g/mol
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