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Quizzes > Science

Ions Quick Check: Charges and Symbols Quiz

Quick, free ion quiz to test your knowledge. Instant results.

Editorial: Review CompletedCreated By: Maria RiveraUpdated Aug 25, 2025
Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Paper art illustration for ions quiz on teal background

This quiz helps you practice ion charges and symbols so you can spot Ag+, Fe3+, and common polyatomic groups with confidence. For extra practice, try our common polyatomic ions quiz and a polyatomic ions charge quiz, or brush up on element abbreviations with a chemical symbols quiz.

What is the charge on a sodium ion (Na)?
+2
-2
-1
+1
A sodium atom loses one electron to achieve a noble gas configuration, forming Na+. This results in a +1 charge. Monovalent sodium ions are common in salts like table salt. For more details see .
What is the charge on a chloride ion (Cl)?
+1
+2
-2
-1
A chlorine atom gains one electron to fill its valence shell, resulting in a -1 charged anion. Chloride ions are abundant in salt and biological systems. This is a common monatomic anion. See for more.
What is the charge on a magnesium ion (Mg)?
+2
-2
+1
-1
Magnesium loses two electrons to attain a stable electron configuration, forming Mg2+. This divalent cation is common in minerals and biological processes. Mg2+ often interacts with phosphate groups. For more info see .
What is the charge on an oxide ion (O)?
-2
-1
+1
+2
An oxygen atom gains two electrons to complete its valence shell, forming O2-. This oxide ion is fundamental in many metal oxides. It has a -2 oxidation state in most compounds. Learn more at .
What is the charge on a calcium ion (Ca)?
-1
-2
+2
+1
Calcium loses two electrons to form Ca2+. This divalent cation is essential for biological systems like bone formation. Ca2+ also plays roles in signaling pathways. See .
What is the charge on an aluminum ion (Al)?
+1
-3
+3
+2
Aluminum loses three electrons to achieve a stable electron configuration, forming Al3+. This trivalent cation is common in many compounds like aluminum oxide. It often participates in coordination chemistry. More at .
What is the charge on a potassium ion (K)?
+1
-1
-2
+2
Potassium loses one electron to form K+, achieving a noble gas electron configuration. This monovalent cation is vital for nerve function and ionic balance. It is abundant in salts. Details at .
What is the charge on a fluoride ion (F)?
-2
+2
+1
-1
Fluorine gains one electron to complete its valence shell, forming F-. This monovalent anion is highly electronegative. Fluoride ions are used in dental care. More at .
What is the charge on a lithium ion (Li)?
+2
-1
+1
-2
Lithium loses one electron to form Li+ and achieve a noble gas configuration. This monovalent cation is used in batteries and psychiatric medications. It is highly reactive in water. See .
What is the charge on a sulfate ion (SO4)?
+2
-2
+1
-1
The sulfate ion has one sulfur atom centrally bonded to four oxygens and carries a net -2 charge. Two extra electrons are delocalized over the oxygens. It is a common polyatomic ion in salts like gypsum. Learn more at .
What is the charge on a nitrate ion (NO3)?
+1
-2
+2
-1
The nitrate ion consists of one nitrogen bonded to three oxygens with a -1 charge due to one extra electron. This is stabilized by resonance. It is widely used in fertilizers. More info at .
What is the charge on an ammonium ion (NH4)?
+2
+1
-1
-2
Ammonium is formed by protonation of ammonia, giving NH4+ a +1 charge. It acts as a cation in many salts like ammonium chloride. It plays a role in acid-base chemistry. See .
What is the charge on a phosphate ion (PO4)?
-1
-2
-3
+1
The phosphate ion has one phosphorus atom surrounded by four oxygens and carries a -3 charge. Three extra electrons are delocalized over the oxygens. It is vital in biological molecules like DNA. More at .
What is the charge on a hydroxide ion (OH)?
+1
-1
-2
+2
Hydroxide forms when water loses a proton, giving OH- a -1 charge. It is a strong base in aqueous solutions. It is common in alkali metal hydroxides. Details at .
What is the charge on a silver ion (Ag)?
-2
+2
-1
+1
Silver most commonly loses one electron to form the Ag+ ion. This monovalent cation is stable and occurs in silver salts. Silver(II) is much less common. More information at .
What is the charge on an iron(II) ion (Fe)?
2-
2+
3+
1+
Iron(II) or ferrous ion has lost two electrons, giving Fe2+. It is common in compounds like iron(II) sulfate. Fe2+ can be oxidized to Fe3+. See .
What is the charge on an iron(III) ion (Fe)?
2+
1+
3+
3-
Iron(III) or ferric ion forms when iron loses three electrons, giving Fe3+. It is found in compounds like iron(III) oxide. Fe3+ is more oxidizing than Fe2+. Details at .
What is the charge on a copper(I) ion (Cu)?
1-
2+
1+
2-
Copper(I), also called cuprous, loses one electron to form Cu+. It is less stable than Cu2+ but occurs in some salts. It often disproportionates in aqueous solution. More at .
What is the charge on a copper(II) ion (Cu)?
2+
1+
2-
1-
Copper(II), or cupric, loses two electrons to form Cu2+. This is the most common oxidation state of copper in compounds like copper sulfate. It plays key roles in redox chemistry. See .
What is the charge on a zinc ion (Zn)?
2-
0
1+
2+
Zinc loses two electrons to achieve a filled d10 configuration, forming Zn2+. This divalent cation is found in many enzymes. It does not exhibit other common oxidation states. See .
What is the charge on a lead(II) ion (Pb)?
4+
2+
2-
1+
Lead(II), or plumbous ion, loses two electrons to form Pb2+. It is more stable than lead(IV) in many compounds. Common in lead salts. More at .
What is the charge on a lead(IV) ion (Pb)?
2+
1+
4+
3+
Lead(IV), or plumbic ion, loses four electrons to form Pb4+. It is a strong oxidizer found in lead dioxide. Less stable in aqueous solution. See .
What is the charge on a tin(II) ion (Sn)?
3+
4+
1+
2+
Tin(II), or stannous ion, loses two electrons to form Sn2+. It is more stable than stannic (Sn4+) in certain conditions. Occurs in tin(II) chloride. More at .
What is the charge on a tin(IV) ion (Sn)?
4+
3+
2-
2+
Tin(IV), or stannic ion, loses four electrons giving Sn4+. It is found in tin(IV) oxide. It is a strong oxidizing agent. See .
What is the charge on a cobalt(II) ion (Co)?
2-
3+
2+
1+
Cobalt(II) loses two electrons to form Co2+. It is common in vitamin B12 analogs. Co2+ can oxidize to Co3+. More at .
What is the charge on a cobalt(III) ion (Co)?
3+
1+
2+
3-
Cobalt(III) loses three electrons, forming Co3+. It is found in complexes like cobalamin. Co3+ is more oxidizing than Co2+. See .
What is the charge on a permanganate ion (MnO4)?
+1
-2
0
-1
Permanganate has manganese in the +7 oxidation state and four oxygens at -2 each, totaling -8+7 = -1. This gives MnO4- a net -1 charge. It is a strong oxidizing agent. More at .
What is the charge on an acetate ion (C2H3O2)?
-2
-1
0
+1
Acetate has two carbons and three hydrogens with two oxygens, carrying a net -1 charge. It is the conjugate base of acetic acid. Common in salts like sodium acetate. See .
What is the charge on a dichromate ion (Cr2O7)?
-1
-2
-3
+2
Dichromate has two Cr atoms each +6 and seven oxygens each -2: total 12 -14 = -2. Hence Cr2O7 2-. It is in equilibrium with chromate in solution. See .
What is the charge on a chromate ion (CrO4)?
0
-2
+2
-1
Chromate has Cr +6 and four oxygens at -2 each, giving +6 -8 = -2 net charge. Chromate and dichromate are pH-dependent. More at .
What is the charge on a peroxide ion (O2)?
-1
0
-3
-2
Peroxide consists of two oxygens sharing a -2 charge divided between them, giving O2 2-. Each oxygen has an oxidation state of -1. Common in hydrogen peroxide. See .
What is the charge on a superoxide ion (O2)?
-3
0
-2
-1
Superoxide contains two oxygens with a total -1 charge (O2-). Each oxygen has an oxidation state of -½. It is reactive in biological systems. More at .
What is the charge on a carbonate ion (CO3)?
-2
-3
0
-1
Carbonate has one C at +4 and three O at -2 each: +4 -6 = -2 net. CO3 2- is common in minerals and buffers. See .
What is the charge on a hydrogen carbonate ion (HCO3)?
+1
0
-2
-1
Bicarbonate contains H+ and carbonate, giving net -1 charge for HCO3-. It is a key buffer in blood. See .
What is the charge on a hydrogen phosphate ion (HPO4)?
-1
-3
0
-2
Hydrogen phosphate has one H (+1), P +5, and four O at -2 each: +1+5-8 = -2. It is intermediate in phosphate buffers. See .
What is the charge on a dihydrogen phosphate ion (H2PO4)?
-3
-1
-2
0
Dihydrogen phosphate has two H (+2), P +5, and O4 -8: +2+5-8 = -1. It is another phosphate buffer species. See .
What is the charge on a sulfite ion (SO3)?
-2
0
-1
-3
Sulfite has S +4 and three O at -2 each: +4-6 = -2 net. It is used as a preservative in food. See .
What is the charge on a bisulfite ion (HSO3)?
0
+1
-2
-1
Bisulfite has one H (+1), S +4, and O3 -6: +1+4-6 = -1. It acts as a reducing agent. See .
What is the charge on a cyanide ion (CN)?
-1
+1
-2
0
Cyanide is composed of carbon (usually +2) and nitrogen (-3), net -1. It is highly toxic due to inhibition of cytochrome c oxidase. More at .
What is the charge on a thiocyanate ion (SCN)?
0
-2
-1
+1
Thiocyanate has S, C, N with overall -1 charge. It binds to metals in coordination complexes. It is isoelectronic with cyanate. See .
What is the charge on a hypochlorite ion (ClO)?
0
-1
+1
-2
Hypochlorite has Cl +1 and O -2: +1-2 = -1 net. It is the active component in bleach. See .
What is the charge on a perchlorate ion (ClO4)?
-1
-3
-2
0
Perchlorate has Cl +7 and O4 -8: +7-8 = -1. It is a strong oxidizer used in propellants. More at .
What is the charge on the chromyl cation (CrO2)?
1+
3+
2+
4+
The chromyl cation CrO2+ has chromium at +6 and two oxygens at -2 each: +6-4 = +2 overall. It appears in chromyl chloride equilibria. See .
What is the charge on the peroxydisulfate ion (S2O8)?
0
-2
-1
-3
Peroxydisulfate has two S at +6 each and eight O at -2 each plus the peroxide linkage adds no extra charge, giving +12-16 = -4 but the O - O bond yields net -2. Hence S2O8 2-. See .
What is the charge on the thiosulfate ion (S2O3)?
0
1+
-1
-2
Thiosulfate replaces one O with S in sulfate; S2O3 has net -2 like sulfate. The two S atoms share oxidation states, with one at +6 and the other at -2 effectively. More at .
What is the charge on the periodate ion (IO4)?
-3
-2
-1
0
Periodate has iodine in +7 oxidation state and four oxygens at -2: +7-8 = -1 net. It is a powerful oxidizer. See .
What is the charge on the hexacyanoferrate(III) ion ([Fe(CN)6])?
-2
-3
-4
-6
In [Fe(CN)6]3-, each cyanide has -1 charge (total -6) and Fe is +3, yielding net -3. This complex is known as ferricyanide. More at .
What is the charge on the hexachloroplatinate(IV) ion ([PtCl6])?
-4
-1
0
-2
In [PtCl6]2-, platinum is in +4 oxidation state and six chlorides each -1 give -6. +4-6 = -2 net. This complex is called hexachloroplatinate(IV). See .
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Study Outcomes

  1. Understand Ionic Charge Basics -

    Learn how to determine charges for ions by applying the periodic trends and electron configurations that govern ion formation.

  2. Identify Ion Symbols -

    Recognize and write the correct symbol ion notation for various elements, ensuring you know how to display both the element and its charge.

  3. Calculate the Ion Charge of Ag -

    Apply your knowledge to determine the specific charge on the ion of silver (Ag) and compare it with other transition metal ions.

  4. Apply Charge Rules in Compounds -

    Use your understanding of charge on the ion to balance ionic compounds and predict the formulas of salts.

  5. Test and Evaluate Your Skills -

    Challenge yourself with targeted quiz questions to reinforce how to determine charges of ions and solidify your mastery of ionic charge concepts.

Cheat Sheet

  1. Predicting Main-Group Ion Charges -

    Main-group elements follow a simple rule: Group 1 forms +1 ions, Group 2 forms +2, Group 16 forms −2, and Group 17 forms −1 (Chemistry LibreTexts). This pattern makes determining charges for ions as easy as matching the element's group number to its charge on the ion. For example, oxygen (Group 16) consistently forms O2− while sodium (Group 1) forms Na+.

  2. Silver's Unique Ion Charge (Ag+) -

    Unlike many transition metals, silver almost always forms a +1 ion charge of Ag (American Chemical Society). Remember that the ion charge of Ag is virtually always Ag+ in ionic compounds, simplifying how to determine charges of ions when silver is involved. Rare exceptions like Ag2O still reflect this predominant +1 state per atom.

  3. Memorizing Common Polyatomic Ion Symbols -

    Polyatomic ions, such as sulfate (SO42−), nitrate (NO3−), and ammonium (NH4+), have fixed symbol ions that must be memorized (Royal Society of Chemistry). Using flashcards or charts helps you quickly recall both the symbol and charge on the ion. A handy tip: group them by charge (+1, −1, −2) to build mental associations.

  4. Balancing Ionic Formulas by Charge -

    To write a neutral compound, the total positive and negative charges must cancel out (Chemguide, UK). For instance, combining Al3+ and SO42− requires two Al3+ ions and three SO42− ions, yielding Al2(SO4)3. This ensures the net charge of the formula is zero and reinforces how to determine charges of ions in compounds.

  5. Mnemonic Tricks for Ion Charges -

    Use memory aids like "Nick the Camel ate a Clam for Supper in Phoenix" to recall NO3−, CO32−, Cl−, SO42−, and PO43− (University of Wisconsin - Madison). Breaking down the phrase into element symbols and oxidation numbers helps you internalize common polyatomic charges. This fun trick boosts confidence when identifying the charge on the ion during quizzes.

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