Various tables - related to writing net ionic equations

table 2.4 & 2.5 name of cations & anions

charge	symbol	name		charge	symbol	name
1 +	H	hydrogen		1 -	H	hydride
	Li	lithium			F	fluoride
	Na	sodium			Cl	chloride
	K	potassium			Br	bromide
	Cs	cesium			I	iodide
	Ag	silver			CN	cyanide
	NH4	ammonim			OH	hydroxide
	Cu	copper I or cuprous			C2H3O2 or CH3COO	acetate
					ClO3	chlorate
2 +	Mg	magnesium			ClO4	perchlorate
	Ca	calcium			NO3	nitrate
	Sr	strontium			MnO4	permanganate
	Ba	barium
	Zn	zinc		2 -	O	oxide
	Cd	cadmium			O2	peroxide
	Co	cobalt II or cobaltous			S	sulfide
	Cu	copper II or cupric			CO3	carbonate
	Fe	iron II or ferrous			CrO4	chromate
	Hg2 2+	mercury I or mercurous			Cr2O7	dichromate
	Hg2+	mercury II or mercuric			SO4	sulfate
	Ni	nickel
	Pb	lead II or plumbous		3 -	N	nitride
	Sn	tin II or stannous			PO4	phosphate
3 +	Al	aluminum
	Cr	chromium III or chromic
	Fe	iron III or ferric

table 2.6 prefixes to name covalent compounds

prefix	means
mono-	1
di-	2
tri-	3
tetra-	4
penta-	5
hexa-	6
hepta-	7
octa-	8
nona-	9
deca-	10

 

table 4.1 list of common strong acids & bases

as a strong acid or strong  base completely dissociates, it should be written in terms of its ions (cancell any spectator ions).  on the other hand, a weak acid or weak base should be written as its chemical formula, since it does not dissociate (much)

strong acids	strong bases
Chloric, HClO3	group 1A metal hydroxides [LiOH, NaOH, KOH, RbOH, CsOH]
hydrobromic, HBr	group 2A metal hydroxides [Ca(OH)2, Sr(OH)2, Ba(OH)2 ]
hydrochloric, HCl
hydroiodic, HI
nitric, HNO3
perchloric, HClO4
sulfuric, H2SO4

 

table 4.2 solubility rules - based on anions

soluble compounds; containing	exceptions
NO3 -	none
CH3COO- or C2H3O2-	none
halides: Cl, Br, I	salts of Ag+, Pb2+, Hg2 2+  ["AP & Honors"]
SO42-	salts of Ca2+, Hg22+, Pb2+, Ba2+, Sr2+ ["ch pbs"]
insoluble compounds; containing	exceptions
S2-	salts of NH4+, alkali metal cations, Ca2+, Ba2+, Sr2+  ["cbs"]
CO32-& PO43-	salts of NH4+, alkali metal cations
OH-	salts of alkali metal cations, Ca2+, Ba2+, Sr2+ ["cbs"]

 

table of common oxidizing / reducing agents

common oxidizing agents	products formed
MnO4- in acidic solution	Mn2+ + water
MnO2 in acidic solution	Mn2+ + water
MnO4- in neutral / basic solution	MnO2 + water
Cr2O72- in acidic solution	Cr3+ + water
HNO3, concentrated	NO2 + water
HNO3, dilute	NO + water
H2SO4, hot, concentrated	SO2 + water
metallic ion (higher oxidation #)	metallous ion (lower oxidation #)
free halogen, e.g. I2	halide, e.g. I-
Na2O2	NaOH
HClO4 [perchloric acid]	Cl-
C2O4 2- [oxalic acid]	CO2
H2O2 [hydrogen peroxide]	O2
H2O	H2 + OH-
common reducing agents	products formed
halide ions, I-	free halogen, e.g. I2
free metals	metal ions
SO2 - [sulfite]	SO42- [sulfate ion]
NO2 - [nitrite]	NO3- [ nitrate ion]
free halogen in dilute basic solution	hypohalite ion, e.g. ClO -
free halogen in concentrated basic solution	halate ions, e.g. BrO2 -
metallous ion (lower oxidation #)	metallic ion (higher oxidation #)
water	O2 + H+

 

Subject: Re: Colors
From: Scott H <swhalander@yahoo.com>
Date: Wed, 18 Apr 2007 21:01:41 -0700 (PDT)
X-Message-Number: 5

Here is my list:

flame color test
	Li+	Deep red (crimson)
	Na+	Yellow
	K+	Violet
	Ca2+	Orange-red
	Sr2+	Red
	Ba2+	Green
	Cu2+	Blue-green
Aqueous Ion Colors
	Cu+	green
	Cu2+	blue
	Fe2+	yellow-green (depending on the anion)
	Fe3+	orange-red (depending on the anion)
	Co2+	Pink
	Cr3+	Violet (Cr(NO3)3 to Green (CrCl3)
	Ni2+	green
	Mn2+	pink
	Pb2+   & Pb4+	colorless
	V2+	violet
	V3+	blue-green
	MnO4-	Purple
	CrO42-	Yellow
	Cr2O72-	Orange
	Cu(NH3)42+	Dark Blue
	FeSCN2+	Red-brown, Wine-red to dark orange
	CoCl42-	Blue
	Ti(H2O)63+	Purple
	Al3+, K+, Li+, Mg2+, Na+, Ca2+, Ba2+, Sr2+, Zn2+	colorless
other molecules
	F2	pale yellow gas
	Cl2	green-yellow gas
	Br2	red-brown gas
	I2	dark-violet vapor & dark metallic solid
	S8	yellow, odorous solid
	NO	colorless gas; product of metal & dilute HNO3
	NO2	brown gas; product of metal & conc HNO3
	PbI2	bright yellow
	metallic sulfides	sulfides of transition metals tend to be black
	Fe2O3	reddish brown; rust
	metallic oxides	oxides of transition metals have various colors
pH indicator
	phenolphthalein	colorless @ pH < 8; pink @ pH > 8
	red litmus (paper)	purple in alkaline solution
	blue litmus (paper)	pink in acidic solution

I hope this helps.

-S Halander
Westview HS
SD, CA

table 24.1  common ligands associated with complex ion (partial)

symbol	name
NH3	ammine (not amine)
H2O	aqua
OH-	hydroxo
SCN-	thiocyanato
Cl-	chloro
Br-	bromo
CN-	cyano

table 25.1  alkanes

name	molecular formula	condensed structural formula
methane	CH4	CH4
ethane	C2 H6	CH3 CH3
propane	C3 H8	CH3 (CH2 )CH3
butane	C4 H10	CH3 (CH2 )2 CH3
pentane	C5 H12	CH3 (CH2 )3 CH3
hexane	C6 H14	CH3 (CH2 )4 CH3
heptane	C7 H16	CH3 (CH2 )5 CH3
octane	C8 H18	CH3 (CH2 )6 CH3
nonane	C9 H20	CH3 (CH2 )7 CH3
decane	C10 H22	CH3 (CH2 )8 CH3

 

table 25.4 organic functional groups  [R & R' = alkyl group; may be same or differ]

funtional group	type of compound
C - C	alkane
C = C	alkene
C = C	alkyne
R - O - H	alcohol
R - O - R'	ether
R - X	haloalkane
R - N-        l	amine
O        ll R - C - H	aldehyde
O        ll R - C - R'	ketone
O        ll R - C - O - H	carboxylic acid
O        ll R - C - O - R'	ester
O        ll     l R - C - N -	amide

 

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