Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
53 Cards in this Set
- Front
- Back
Ammonium
|
NH4 +
Cation (+1 Charge) |
|
Bicarbonate or Hydrogen Carbonate
|
HCO3 -
Anion (-1 Charge) |
|
Hydronium
|
H3O +
Cation (+1 Charge) |
|
Cyanide
|
CN -
Anion (-1 Charge) |
|
Hydrogen Sulfate
|
HSO4 -
Anion (-1 Charge) |
|
Hydroxide
|
OH -
Anion -1 charge |
|
Nitrate
|
NO3 -
Anion 1- charge |
|
Nitrite
|
NO2 -
(Anion 1- charge) |
|
Hyponitrite
|
NO -
(Anion 1- charge) |
|
Perchlorate
|
ClO4 -
(Anion 1- charge) |
|
Permanganate
|
MnO4 -
(Anion 1- charge) |
|
Carbonate
|
CO3 2-
Anion (2- Charge) |
|
Chromate
|
CrO4 2-
Anion (2- Charge) |
|
Dichromate
|
Cr2O7 2-
Anion (2- Charge) |
|
Monohydrogen Phosphate
|
HPO4 2-
Anion (2- Charge) |
|
Sulfate
|
SO4 2-
anion charge 2- |
|
Sulfite
|
SO3 2-
anion charge 2- |
|
Thiosulfate
|
S2O3 2-
anion charge 2- |
|
Phosphate
|
PO4 3-
Anion (-3 Charge) |
|
Silver ion
|
Ag +
|
|
Zinc
|
Zn 2+
|
|
Cadium
|
Cd 2+
|
|
Aluminum
|
Al 3+
|
|
What "other" metals always form the same ion
|
Ag (+1), Zn (2+), Cd (2+), Al (3+)
|
|
Variable Charge Metal Ions
|
Fe 2+ iron (II) ion
Fe 3+ iron (III) ion Cu + copper (I) ion Cu 2+ copper (II) ion Pb 2+ lead (II) ion Pb 4+ lead (IV) ion Sn 2+ tin (II) ion Sn 4+ tin (IV) ion Hg2 2+ mercury (I) ion Hg 2+ mercury (II) ion |
|
2 forms if Iron ion
|
Fe 2+ iron (II) ion
Fe 3+ iron (III) ion |
|
2 Forms of Copper Ion
|
Cu + copper (I) ion
Cu 2+ copper (II) ion |
|
2 Forms of Lead ion
|
Pb 2+ lead (II) ion
Pb 4+ lead (IV) ion |
|
2 Forms of Tin Ion
|
Sn 2+ tin (II) ion
Sn 4+ tin (IV) ion |
|
2 Forms of Mercury Ion
|
Hg2 2+ mercury (I) ion
Hg 2+ mercury (II) ion |
|
Ternary Compounds
|
2 different types of atoms
|
|
Dihydrogen phosphate
|
H2PO4 1-
|
|
Peroxide
|
O2 2-
|
|
Acetate
|
C2H3O2 1-
|
|
Dichromate
|
Cr2O7 2-
|
|
Hypochlorite
|
ClO 1-
|
|
Acetate
|
C2H3O2 1-
|
|
Dichromate
|
Cr2O7 2-
|
|
Hypochlorite
|
ClO 1-
|
|
Bisulfate
|
HSO4 -
|
|
Bicarbonate/ hydrogen carbonate and Bisulfate/ hydrogen sulfate
|
same as polyatomic with an extra poisitve charge so CO3 2- and SO4 2-
add a hydrogen and subtract one negative charge HCO3 1- HSO4 1- |
|
Permanganate
|
MnO4 1-
|
|
Monohydrogen Phosphate and Dihydrogen Phosphate
|
By adding Hydrogen to any polyatomic ion adjust the charge
PO4 3- Monohydrogen Phosphate HPO4 2- Dihydrogen Phosphate H2PO2 1- |
|
Two main Groups of Acids
|
Binary and Oxy acids (ternary acids)
|
|
Naming Binary Acids
|
Binary acids contain H and one other element.
HCl(aq), HBr(aq) |
|
Naming conventions for Binary (H + one other element) Acids
|
They are named with a pattern:
Hydro------ic Acid HCl: hydrochloric acid HBr: hydrobromic acid |
|
Naming Oxy Acids
|
Oxy acids contain a polyatomic ion.
HNO3 H2SO4 |
|
What is the measure of Hydrogens based on dealing with an Oxy (an acid that contains a polyatomic ion) Acids
|
The amount of Hydrogens depends on the charge of the polyatomic ion
|
|
The different naming conventions used for -ate and -ite
|
-ate changed to -ic
---------ic acid HNO3 is nitric acid (one hydrogen matches the negative 1 charge of the anion) -ite changes to -ous ----------ous acid HNO2 is nitrous acid. In either case, do not use the “hydro” prefix. |
|
What are teh namin conventions for Oxy acids that end in -ate or -ite
|
= change -ate to -ic acid
= change -ite to -ous acid DO NOT PREFIX WITH HYDRO!!! |
|
What does the Hydro prefix in naming acids refer to?
|
-It refers to binary acids
- to distinguish between oxy and binary acids the hydro- prefix is used ...ex. chloric acid and hydrochloric acid |
|
Difference between HSO4 -
and H2SO4 |
bisulfate and sulfuric acid
the charge changes the compound completely |
|
Hydrates
|
Hydrates are ionic compounds with an exact number of water molecules bound to each crystal (formula) unit:
MgSO4 • 7 H2O They are named using the Greek prefixes to indicate the number of H2O’s Magnesium sulfate heptahydrate |