Polyatomic Ions, Naming Conventions, and more Flashcards
1
Q
Ammonium cation
A
NH4^(+)
2
Q
Hydronium cation
A
H3O^(+)
3
Q
Hydroxide anion
A
OH^(-)
4
Q
Acetate anion
A
CH3CO2^(-)
OR
C2H3O2^(-)
5
Q
Cyanide anion
A
CN^(-)
6
Q
Peroxide anion
A
O2^(2-)
7
Q
Carbonate anion
A
CO3^(2-)
8
Q
Nitrate anion
A
NO3^(-)
9
Q
Phosphate anion
A
PO4^(3-)
10
Q
Sulfate anion
A
SO4^(2-)
11
Q
Chlorate anion
A
ClO3^(-)
12
Q
Bromate anion
A
BrO3^(-)
13
Q
Iodate anion
A
IO3^(-)
14
Q
Peroxide anion
A
O2^(2-)
15
Q
Carbonate anion
A
CO3^(2-)
16
Q
Nitrate anion
A
NO3^(-)
17
Q
Phosphate anion
A
PO4^(3-)
18
Q
Sulfate anion
A
SO4^(2-)
19
Q
Chlorate anion
A
CLO3^(-)
20
Q
Bromate anion
A
BrO3^(-)
21
Q
Iodate anion
A
IO3^(-)
22
Q
Chromate anion
A
CrO4^(2-)
23
Q
Permanganate anion
A
MnO4^(-)
24
Q
Chlorite anion
A
ClO2^(-)
25
Hypochlorite anion
ClO^(-)
26
H^+ + F^- (acid)
HF
hydrofluoric acid
27
H^+ + Cl^- (acid)
HCl
hydrochloric acid
28
Naming conventions
-ate > -ite (number of oxygens in polyatomic ion)
-ide + Greek number prefixes (covalent)
29
Binary Acid naming convention
Contains hydrogen + nonmetal element
[hydro + anion root + -ic] + acid
30
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
31
Alkane naming convention
carbon number prefix + -ane
32
Carbon number prefix: 1
meth-
33
Carbon number prefix: 2
eth-
34
Carbon number prefix: 3
prop-
35
Carbon number prefix: 4
but-
36
Carbon number prefix: 5
pent-
37
Carbon number prefix: 6
hex-
38
Carbon number prefix: 7
hept-
39
Carbon number prefix: 8
oct-
40
Carbon number prefix: 9
non-
41
Carbon number prefix: 10
dec-
42
Ionic Compounds are
atomic cations + atomic anions
43
Ionic Compound naming convention
cation name + anion name
*note: no number prefix on cation
44
Oxoanion naming convention
[number prefix + hydrogen] + oxoanion name
45
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.
46
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)*100*m = number
if number is or can be rounded to a whole number, substance A is a Pure Substance
47
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.
48
Bases
Substance that releases hydroxide (OH^-) ions when dissolved in water.
49
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)
50
Hydrates: naming and formula
Formula:
ionic compound + (#)H2O
Ex) Al2(SO4)3*6H2O
Name:
name of ionic compound* + [# in Greek prefix] + hydrate]
Ex) nickel(II) sulfate pentahydrate*
* not a real example
51
Molecular compounds when dissolved-
Break into individual molecules. Molecules are not further broken down.
52
Ionic compounds when dissolved-
Break into cations and anions from which they are formed.
Formula unit of ionic compound comes apart.
53
Formal Charge
FC = Valence electrons - (non-bonded electrons + bonds)
54
Thiosulfate
S2O3^2-
55
Thiocyanate
SCN^-
56
Bicarbonate
HCO3^-
