Polyatomic Ions And Periodic Table Reference Sheet

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Polyatomic Ions and Periodic Table Reference Sheet
Constants Use in Calculations!
Stoichiometry Flowchart!
Formulas!
!
!
*see “Constants” section also*!
Q = m c ∆T!
!
Calorimetry!
1 mole:!
atomic mass of element (g)!
Mass (
)!
Given
!
Q = heat, energy (J or cal)!
(mol)! !
formula mass of a compound (g)!
⇣!
!
m = mass (g)!
!
!
6.022 x 10
23
molecules/atoms/particles!
Moles (
)!
Given
!
c = specific heat (J/g
o
C or cal/g
o
C)!
!
!
22.4 L of gas!
⇣*
*
!
!
∆T = change in temperature (
o
C, ∆T = T
- T
)!
———————————————————————————!
final
initial
Moles (
)!
Unknown
————————————————————————————————!
Energy:!
1 calorie = 4.18 Joule (J)!
⇣!
M
V
= M
V
Dilution and Solution Concentration!
!
!
1000 calories = 1 Calorie!
1
1
2
2!
!
!
!
!
M = Molarity (Concentration)!
!
!
Specific Heat of Water: 4.18 J/g
o
C!
solute(g)
Mass (
)!
Unknown
%Conc. =
× 100
———————————————————————————!
solution(g)
moles of solute (mol)
*use ratio from balanced formula*
!
M =!
!
Standard!
1 atm = 760 Torr = 760 mm Hg = 101.3 kPa!
solution = solute + solvent
Liters of solution (L)
Pressure
————————————————————————————————!
PV = nRT!
!
Ideal Gas Law & Triangle!
Dimensional Analysis!
Empirical/Molecular Formula Flowchart!
P
V
!
P = pressure (atm)!
% → mass → moles → mole ratio → Emp. formula!
(T-chart)!
! !
!
V = volume (L)!
desired units
Mass given
!
n = number of moles!
given units ×
T
!
= Multiple of Emp. Formula = Molecular Formula
K
Emp. formula mass
units to cancel given units
!
R = gas constant [0.0821 (L*mol)/(mol*K)]!
!
T = temperature (K)
Example:!
More Formulas!
mass(g)
D =
2.54cm
volume(mL)
Acid-Base Equations!
pH Scale!
! !
30in ×
= 76.2cm
pH = − log[H
+
]
1in
part
Actual
%Comp. =
× 100
%Yield =
× 100
pOH = − log[OH
Theoretical
whole
]
0 1 2 3 4 5 6 7 8 9 10 11 12 13 14
pH + pOH = 14
(NH
)
+!
!
Ammonium*! !
!
(O
)
2-
! !
Peroxide!
4
2
+
] = 1.0 × 10
−14
(C
H
O
)
-!
Acetate*!
!
!
(PO
)
3-!
Phosphate*!
[H
][OH
2
3
2
4
Temp. Conversions!
(AsO
)
3-
!
Arsenate!
!
!
(PO
)
3-!
Phosphite!
+
− pH
4
3
] = 10
[H
°F = (9/5)°C + 32!
(AsO
)
3-
!
Arsenite!
!
!
(SO
)
2-!
Sulfate*!
3
4
°C = (°F - 32)(5/9)!
− pOH
] = 10
[OH
(HCO
)
-
!
Bicarbonate! !
!
(SO
)
2-!
Sulfite!
3
3
K = 273 + °C!
(BrO
)
-!
Bromate!
!
!
(SCN)
-
!
Thiocyanate!
= M
3
M
V
V
°C = K - 273
A
A
B
B
(CO
)
2-!
Carbonate*! !
!
(S
O
)
2-!
Thiosulfate!
3
2
3
(ClO
)
-!
Chlorate*!
!
!
!
* commonly used
Common Prefixes and Conversions!
3
(ClO
)
-!
Chlorite!
10
3!
10
2!
10
1!
10
0!
10
-1!
10
-2!
10
-3
!
2
(CrO
)
2-
!
Chromate!
Kilo!
Hecto! Deca! Base! deci!
centi!
milli!
4
Special Transition Metals:!
1000!
100!
10!
1!
0.1!
0.01! 0.001
(CN)
-
! !
Cyanide!
Silver (Ag)!
+1!
(Cr
O
)
2-
!
Dichromate!
2
7
Zinc (Zn)! !
+2!
Roman Numerals!
Prefixes!
(OH)
-
! !
Hydroxide*!
Cadmium (Cd)!
!
+2!
*for transition metal charges*!
*covalent bonding only!*!
(NO
)
-
!!
Nitrate*!
3
1 - Mono!
6 - Hexa!
I - One!
VI - Six!
(NO
) -!!
Nitrite!
2
These only form one type of ion and
2 - Di! !
7 - Hepta!
II - Two!
VII - Seven!
(C
O
)
2-
!
Oxalate!
Roman numerals are not used in
2
4
3 - Tri! !
8 - Octa!
III - Three!
VIII - Eight!
(ClO
) -!
Perchlorate!
naming
4
4 - Tetra!
9 - Nona!
IV - Four!
IX - Nine!
(MnO
)
-
!
Permanganate
4
5 - Penta!
10 - Deca
V - Five!
X - Ten

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