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A comprehensive list of common ions, including their charges and names. It explains how to determine the charge of an element based on the charge of its corresponding negative ion. The document also covers common negative ion pairs and their differences in oxygen atoms. It is a useful resource for students studying chemistry, particularly those learning about ions.
What you will learn
Typology: Study notes
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Positive ions (cations) Negative ions (anions)
1+ 1- Ammonium (NH 4 +) Acetate (C 2 H 3 O 2 - ) Cesium (Cs+) Azide (N 3 - ) Copper (I) or cuprous (Cu+) Bromide (Br-) Hydrogen (H+) Chlorate (ClO 3 - ) Lithium (Li+) Chloride (Cl-) Potassium (K+) Cyanide (CN-) Silver (Ag+) Dihydrogen phosphate (H 2 PO 4 - ) Sodium (Na+) Fluoride (F-) Hydride (H-) 2 +^ Bicarbonate Barium (Ba2+) Bisulfate Cadmium (Cd2+) Hydroxide (OH-) Calcium (Ca2+) Iodide (I-) Cobalt (II) or cobaltous (Co2+) Nitrate (NO 3 - ) Copper (II) or cupric (Cu2+) Nitrite (NO 2 - ) Iron (II) or ferrous (Fe2+) Perchlorate (ClO 4 - ) Lead (II) or plumbous (Pb2+) Permanganate (MnO 4 - ) Magnesium (Mg2+) Thiocyanate (SCN-) Manganese (II) or Manganous (Mn2+) Mercury (I) or mercurous (Hg 2 2+) 2- Mercury (II) or mercuric (Hg2+) Carbonate (CO 3 2-) Nickel (Ni2+) Chromate (CrO 4 2-) Strontium (Sr2+) Dichromate (Cr 2 O 7 2-) Tin (II) or stannous (Sn2+) Hydrogen Phosphate (HPO 4 2-) Zinc (Zn2+) Oxide (O2-) Peroxide (O 2 2-) 3+ Sulfate (SO 4 2-) Aluminum (Al3+) Sulfide (S2-) Chromium (III) or chromic (Cr3+) Sulfite (SO 3 2-) Iron (III) or ferric (Fe3+) 3- Arsenate (AsO 4 3-) Nitride (N3-) Phosphate (PO 4 3-) Phosphide (P3-)
The list of common ions may seem impossible to learn; however, by using the Periodic Table a
sizable chunk of the list is easily conquered.
Each row is called a period ; whereas, each column is referred to as a group. Group has similar chemical properties mainly because of the electrons in their outer shell.
Each atom wants eight electrons in its valence shell (outer-most shell). This is the most stable structure of the atom. Thus Group 8 A, the Noble Gases, all have eight electrons and rarely react. The other elements will either gain electrons or lose their electrons to gain a full valence shell.
The Method
First of all, photocopy the list given in class by your professor, or photocopy the list in your book.
*** Now by using a highlighter, pencil, or color coding, cross out the following groups:**
The negative ions:
Group 7 A: F, Cl, Br, I and At are -1.
Group 6 A: O, S, Se and Te are -2.
Group 5 A: N, and P are -3.
All these negative ions have the ending "-ide".
In addition, hydrogen can be -1 (and, thus, "hydride").
The positive ions:
Group 1 A: The first column is + 1 charge. That takes care of Li, Na, K, Rb, CS, and Fr.
Group 2 A: The following are + 2 charge: Be, Mg, Ca, Sr, Ba, and Ra.
Group 3 A: Alumninum is +3.
Hydrogen is an element that is either +1 (and simply "hydrogen") or -1 (hydride).
The remaining positive ions to be learned (preferably using notecards) are the Transition metals:
+1 Ag (Silver) +2 Cd (Cadmium), Ni (Nickle), and Zn (Zinc)
Ammnonium (NH 4 +) Hydronium (H 3 O+)
Since Phosphate is -3 adding one hydrogen (+1) would give Hydrogen phospate WITH a charge of -2.
One more hydrogen gives Dihydrogen phosphate WITH a charge of -1.
The following have "historical" names also:
Bicarbonate: Add one hydrogen (+1) to Carbonate (-2) to get HCO3-.
Bisulfate: Add one hydrogen (+1) to Sulfate (-2) to get HSO4-.
THIS IS NOT A COMPLETE LISTING OF KNOWN IONS BUT SHOULD BE A START AND HOPEFULLY LOGICAL TOOL TO ABSORB, UTILIZE, AND LEARN SOME CHEMISTRY.
Revised: Spring 1995 Edited by: Senovio R. Rodriguez, Spring 1995 Source: Brown, LeMay, Bursten 5th Ed. 1991, Chemistry: The Central Science STUDENT LEARNING ASSISTANCE CENTER (SLAC) Texas State University-San Marcos