Polyatomic Ions, Naming Conventions, and more Flashcards
Ammonium cation
NH4^(+)
Hydronium cation
H3O^(+)
Hydroxide anion
OH^(-)
Acetate anion
CH3CO2^(-)
OR
C2H3O2^(-)
Cyanide anion
CN^(-)
Peroxide anion
O2^(2-)
Carbonate anion
CO3^(2-)
Nitrate anion
NO3^(-)
Phosphate anion
PO4^(3-)
Sulfate anion
SO4^(2-)
Chlorate anion
ClO3^(-)
Bromate anion
BrO3^(-)
Iodate anion
IO3^(-)
Peroxide anion
O2^(2-)
Carbonate anion
CO3^(2-)
Nitrate anion
NO3^(-)
Phosphate anion
PO4^(3-)
Sulfate anion
SO4^(2-)
Chlorate anion
CLO3^(-)
Bromate anion
BrO3^(-)
Iodate anion
IO3^(-)
Chromate anion
CrO4^(2-)
Permanganate anion
MnO4^(-)
Chlorite anion
ClO2^(-)
Hypochlorite anion
ClO^(-)
H^+ + F^- (acid)
HF
hydrofluoric acid
H^+ + Cl^- (acid)
HCl
hydrochloric acid
Naming conventions
-ate > -ite (number of oxygens in polyatomic ion)
-ide + Greek number prefixes (covalent)
Binary Acid naming convention
Contains hydrogen + nonmetal element
[hydro + anion root + -ic] + acid
Oxyacid naming convention
Contains hydrogen + oxygen + other element (usu. nonmetal)
[oxoanion root + -ic/-ous] + acid
-ic for oxoanion ending in -ate
-ous for oxoanion ending in -ite
Alkane naming convention
carbon number prefix + -ane
Carbon number prefix: 1
meth-
Carbon number prefix: 2
eth-
Carbon number prefix: 3
prop-
Carbon number prefix: 4
but-
Carbon number prefix: 5
pent-
Carbon number prefix: 6
hex-
Carbon number prefix: 7
hept-
Carbon number prefix: 8
oct-
Carbon number prefix: 9
non-
Carbon number prefix: 10
dec-
Ionic Compounds are
atomic cations + atomic anions
Ionic Compound naming convention
cation name + anion name
*note: no number prefix on cation
Oxoanion naming convention
[number prefix + hydrogen] + oxoanion name
Law of Multiple Proportions
Atoms within a pure substance can be represented with fixed whole number ratios.
Ex) In CO, there is 1. g C and 1.33 g O. While in CO2, there is 1. g C and 2.66 g O.
The different masses of O are proportional to each other.
Using Law of Multiple Proportions to determine if a substance is a pure substance, using given masses of another pure substance
E1 = mass of 1 element in Pure Substance
E2 = mass of another element in substance
m1 = proportion
A1, A2 = E1, E2 masses of another pure substance
m = (E1/E2) * 100g
(A1/A2)100m = number
if number is or can be rounded to a whole number, substance A is a Pure Substance
Acids
Molecular compounds that release H^+ cations when dissolved in water
Ex) HCl(aq) > H^+(aq) + Cl^-(aq)
Usu. have H (e.g. HF) in front of chemical formula.
Bases
Substance that releases hydroxide (OH^-) ions when dissolved in water.
Hydrates
Ionic compound in which one or more water molecules are included per formula unit area of a crystal.
Looks like this:
Ex) Na2CO3*H2O
Note: * (in place to represent multiplication dot)
Hydrates: naming and formula
Formula:
ionic compound + (#)H2O
Ex) Al2(SO4)36H2O
Name:
name of ionic compound + [# in Greek prefix] + hydrate]
Ex) nickel(II) sulfate pentahydrate*
* not a real example
Molecular compounds when dissolved-
Break into individual molecules. Molecules are not further broken down.
Ionic compounds when dissolved-
Break into cations and anions from which they are formed.
Formula unit of ionic compound comes apart.
Formal Charge
FC = Valence electrons - (non-bonded electrons + bonds)
Thiosulfate
S2O3^2-
Thiocyanate
SCN^-
Bicarbonate
HCO3^-
