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Ionic Compound Naming Flashcards: Names, Formulas & Charge Balance

Practice ionic compound naming with 56 English flashcards on neutral formulas, Roman numerals, polyatomic-ion parentheses, and common errors.

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À propos de ce paquet

Practice ionic compound names and neutral formulas with 56 English flashcards. This focused deck is for high-school and introductory-college learners who know basic ions and want to apply charge balance consistently.

The cards practice names to formulas, selected formulas back to names, metal-charge inference, one polyatomic-group count, and short repairs of incorrect formulas or missing naming information. Ion charges and polyatomic-ion names are supplied where the target is applying a rule. This is compound-naming practice rather than a table of isolated ions; use the polyatomic ion flashcards for that prerequisite.

The sequence begins with neutrality, cation-first order, subscripts, and the smallest whole-number ratio of intact ions. Fixed-charge binary salts come next, followed by iron, copper, and tin Stock names. Polyatomic groups and ammonium then lead into mixed formula, naming, and error-repair prompts. Selected reverse directions and closely related variants are separated. Every card carries the ionic-naming tag; the review scheduler handles longer-term spacing.

Names follow the usual introductory convention: fixed-charge cations without Roman numerals, variable-charge monatomic metals with Stock Roman numerals, and familiar polyatomic-ion names. Aluminum and aluminium are accepted spelling variants; sodium hydrogen carbonate and sodium bicarbonate are both accepted. This convention does not exhaust all valid systematic names. Arbitrary name-to-example prompts and exhaustive reversals are omitted because they add ambiguity or repetition. Covalent naming, acids, hydrates, organic compounds, coordination complexes, peroxide and mercury(I) special cases, reactions, and solubility are outside this deck. No full-course or examination alignment is claimed.

The questions, explanations, order, and metadata were written independently with AI assistance. Naming and ion facts were checked against Purdue University’s ionic-naming rules and ion reference tables. No competitor cards, source exercise wording, examination questions, or source diagrams were copied. Reference works retain their own rights, and chemical facts are not claimed as proprietary. Original material, including the AI-generated decorative charge-symbol cover, is dedicated under CC0 1.0 to the extent applicable rights exist. This is independent study material without institutional endorsement.

Cartes de ce paquet

  1. Carte 1

    Question

    In a neutral ionic formula unit, what must the total ionic charge be?

    Réponse

    Zero. The positive and negative charges must cancel.

  2. Carte 2

    Question

    When naming a simple ionic compound, which ion is named first?

    Réponse

    The cation, followed by the anion.

  3. Carte 3

    Question

    Write the formula for lithium fluoride using Li⁺ and F⁻.

    Réponse

    LiF. One ion of each kind gives +1 − 1 = 0.

  4. Carte 4

    Question

    In CaCl₂, what does the subscript 2 count?

    Réponse

    Two chloride ions for each calcium ion. It does not mean that each chloride ion has a charge of −2.

  5. Carte 5

    Question

    Name MgO using the usual fixed-charge ionic naming convention.

    Réponse

    Magnesium oxide. The ions are Mg²⁺ and O²⁻.

  6. Carte 6

    Question

    What is the smallest neutral ratio of Al³⁺ ions to O²⁻ ions?

    Réponse

    Two Al³⁺ ions to three O²⁻ ions: +6 and −6 cancel.

  7. Carte 7

    Question

    Write the formula for magnesium bromide using Mg²⁺ and Br⁻.

    Réponse

    MgBr₂. Two bromide ions balance one magnesium ion.

  8. Carte 8

    Question

    Name Na₂S using the usual fixed-charge ionic naming convention.

    Réponse

    Sodium sulfide. The sulfur anion is called sulfide.

  9. Carte 9

    Question

    Write the simplest formula for calcium oxide using Ca²⁺ and O²⁻.

    Réponse

    CaO. Equal and opposite charges give a 1:1 ion ratio.

  10. Carte 10

    Question

    Write the formula for aluminum nitride using Al³⁺ and N³⁻.

    Réponse

    AlN. One ion of each kind is neutral. Aluminium nitride is the same compound, with the British spelling.

  11. Carte 11

    Question

    Name Mg₃N₂ using the usual fixed-charge ionic naming convention.

    Réponse

    Magnesium nitride. Three Mg²⁺ ions balance two N³⁻ ions.

  12. Carte 12

    Question

    Write the formula for lithium oxide using Li⁺ and O²⁻.

    Réponse

    Li₂O. Two lithium ions balance one oxide ion.

  13. Carte 13

    Question

    Name CaF₂ using the usual fixed-charge ionic naming convention.

    Réponse

    Calcium fluoride. This convention uses the ion names without a di- prefix for the two fluoride ions.

  14. Carte 14

    Question

    A student writes Mg₂O₂ for magnesium oxide, using Mg²⁺ and O²⁻. What is the simplest formula?

    Réponse

    MgO. The 2:2 ion ratio is neutral but reduces to 1:1.

  15. Carte 15

    Question

    Name Al₂S₃ using the usual fixed-charge ionic naming convention.

    Réponse

    Aluminum sulfide (also spelled aluminium sulfide). Two Al³⁺ ions balance three S²⁻ ions.

  16. Carte 16

    Question

    Write the formula for sodium phosphide using Na⁺ and P³⁻.

    Réponse

    Na₃P. Three sodium ions balance one phosphide ion.

  17. Carte 17

    Question

    Name LiF using the usual fixed-charge ionic naming convention.

    Réponse

    Lithium fluoride. Name the lithium cation first and the fluoride anion second.

  18. Carte 18

    Question

    Write the formula for magnesium oxide using Mg²⁺ and O²⁻.

    Réponse

    MgO. The smallest neutral ratio is one magnesium ion to one oxide ion.

  19. Carte 19

    Question

    In the Stock name iron(III) chloride, what does III specify?

    Réponse

    A +3 charge on each iron ion. For this monatomic ion, its charge equals its oxidation state; III is not an atom count.

  20. Carte 20

    Question

    Name FeCl₂ using Stock nomenclature. Chloride is Cl⁻.

    Réponse

    Iron(II) chloride. Two chloride ions total −2, so the iron ion is Fe²⁺.

  21. Carte 21

    Question

    What is the charge on each copper ion in Cu₂O, taking oxide as O²⁻?

    Réponse

    +1. The two copper ions together must supply +2, so each is Cu⁺.

  22. Carte 22

    Question

    Write the formula for tin(IV) oxide, using oxide O²⁻.

    Réponse

    SnO₂. One Sn⁴⁺ ion balances two oxide ions; reduce a crossed 2:4 ratio to 1:2.

  23. Carte 23

    Question

    Name Fe₂O₃ using Stock nomenclature. Oxide is O²⁻.

    Réponse

    Iron(III) oxide. Three oxide ions total −6; divided between two iron ions, that requires Fe³⁺.

  24. Carte 24

    Question

    Write the formula for copper(II) bromide, using bromide Br⁻.

    Réponse

    CuBr₂. One Cu²⁺ ion needs two bromide ions.

  25. Carte 25

    Question

    Name SnCl₂ using Stock nomenclature. Chloride is Cl⁻.

    Réponse

    Tin(II) chloride. Two Cl⁻ ions require one Sn²⁺ ion.

  26. Carte 26

    Question

    Write the formula for iron(II) chloride, using chloride Cl⁻.

    Réponse

    FeCl₂. One Fe²⁺ ion balances two chloride ions.

  27. Carte 27

    Question

    Name CuO using Stock nomenclature. Oxide is O²⁻.

    Réponse

    Copper(II) oxide. The 1:1 ratio requires Cu²⁺ to balance O²⁻.

  28. Carte 28

    Question

    Write the formula for iron(III) sulfide, using sulfide S²⁻.

    Réponse

    Fe₂S₃. Two Fe³⁺ ions supply +6 and three sulfide ions supply −6.

  29. Carte 29

    Question

    Why is the name copper chloride insufficient to choose a single formula in introductory Stock nomenclature?

    Réponse

    It omits the copper oxidation state. Copper(I) chloride is CuCl; copper(II) chloride is CuCl₂.

  30. Carte 30

    Question

    Name SnO₂ using Stock nomenclature. Oxide is O²⁻.

    Réponse

    Tin(IV) oxide. Two oxide ions total −4, so the tin ion is Sn⁴⁺.

  31. Carte 31

    Question

    A student labels Fe₂O₃ as iron(II) oxide. Keeping the name iron(II) oxide, what formula should replace it?

    Réponse

    FeO. Fe²⁺ and O²⁻ balance in a 1:1 ratio; Fe₂O₃ instead corresponds to iron(III) oxide.

  32. Carte 32

    Question

    Name CaCl₂ using the usual introductory fixed-charge convention.

    Réponse

    Calcium chloride. Calcium is treated as Ca²⁺, so this convention omits the Roman numeral. An explicit oxidation-state name is not a different compound.

  33. Carte 33

    Question

    Write the formula for sodium nitrate using Na⁺ and NO₃⁻.

    Réponse

    NaNO₃. One nitrate ion balances one sodium ion; keep the nitrate formula intact.

  34. Carte 34

    Question

    Name K₂CO₃. The polyatomic ion CO₃²⁻ is carbonate.

    Réponse

    Potassium carbonate. Two K⁺ ions balance one carbonate ion.

  35. Carte 35

    Question

    When writing a conventional ionic formula, when do you put a polyatomic ion in parentheses?

    Réponse

    When more than one of that whole ion is needed. Put the count outside the parentheses and leave the ion’s internal subscripts unchanged.

  36. Carte 36

    Question

    Write the formula for calcium hydroxide using Ca²⁺ and OH⁻.

    Réponse

    Ca(OH)₂. Two whole hydroxide ions balance one calcium ion.

  37. Carte 37

    Question

    Name NH₄Cl. NH₄⁺ is ammonium.

    Réponse

    Ammonium chloride. The cation is the whole NH₄⁺ ion, even though it contains no metal.

  38. Carte 38

    Question

    Write the formula for aluminum sulfate using Al³⁺ and SO₄²⁻.

    Réponse

    Al₂(SO₄)₃. Two aluminum ions supply +6 and three intact sulfate ions supply −6.

  39. Carte 39

    Question

    Name Mg(NO₃)₂. NO₃⁻ is nitrate.

    Réponse

    Magnesium nitrate. One Mg²⁺ ion is balanced by two nitrate ions.

  40. Carte 40

    Question

    Write the formula for ammonium phosphate using NH₄⁺ and PO₄³⁻.

    Réponse

    (NH₄)₃PO₄. Three ammonium ions balance one phosphate ion; only ammonium needs parentheses.

  41. Carte 41

    Question

    How many whole hydroxide ions are represented in one formula unit of Ba(OH)₂?

    Réponse

    Two hydroxide ions. The outer subscript multiplies the entire OH group, giving two O atoms and two H atoms.

  42. Carte 42

    Question

    Name Fe₂(SO₄)₃ using Stock nomenclature. SO₄²⁻ is sulfate.

    Réponse

    Iron(III) sulfate. Three sulfate ions total −6, so each of the two iron ions has charge +3.

  43. Carte 43

    Question

    Write the formula for calcium nitrate using Ca²⁺ and NO₃⁻.

    Réponse

    Ca(NO₃)₂. Two intact nitrate ions supply −2 to balance calcium’s +2.

  44. Carte 44

    Question

    Name (NH₄)₂SO₄. NH₄⁺ is ammonium and SO₄²⁻ is sulfate.

    Réponse

    Ammonium sulfate. Two ammonium ions balance one sulfate ion.

  45. Carte 45

    Question

    Write the formula for magnesium phosphate using Mg²⁺ and PO₄³⁻.

    Réponse

    Mg₃(PO₄)₂. Three magnesium ions and two phosphate ions give +6 and −6.

  46. Carte 46

    Question

    Name NaHCO₃. HCO₃⁻ is hydrogen carbonate, also called bicarbonate.

    Réponse

    Sodium hydrogen carbonate, also called sodium bicarbonate. HCO₃⁻ is one intact anion.

  47. Carte 47

    Question

    Repair AlOH₃ as the formula for aluminum hydroxide, using Al³⁺ and OH⁻.

    Réponse

    Al(OH)₃. Three whole hydroxide ions are needed. AlOH₃ fails to multiply the oxygen count along with the hydrogen count.

  48. Carte 48

    Question

    Write the formula for ammonium sulfite using NH₄⁺ and SO₃²⁻.

    Réponse

    (NH₄)₂SO₃. Two ammonium ions balance one sulfite ion; sulfite retains its three oxygen atoms.

  49. Carte 49

    Question

    Name Cu(NO₃)₂ using Stock nomenclature. NO₃⁻ is nitrate.

    Réponse

    Copper(II) nitrate. Two nitrate ions total −2, requiring Cu²⁺.

  50. Carte 50

    Question

    Write the formula for iron(III) sulfate, using sulfate SO₄²⁻.

    Réponse

    Fe₂(SO₄)₃. Two Fe³⁺ ions balance three sulfate ions.

  51. Carte 51

    Question

    Repair K(CO₃)₂ as the formula for potassium carbonate, using K⁺ and CO₃²⁻.

    Réponse

    K₂CO₃. Two potassium ions balance one carbonate ion. A single carbonate group needs no parentheses.

  52. Carte 52

    Question

    Can Mg(NO₃)₂ be simplified to MgNO₃ by removing the outer subscript? Use Mg²⁺ and NO₃⁻.

    Réponse

    No. The ion ratio is already 1:2. Removing the outer 2 would leave total charge +1 instead of zero.

  53. Carte 53

    Question

    Name Ca(OH)₂. OH⁻ is hydroxide.

    Réponse

    Calcium hydroxide. The two hydroxide ions balance one Ca²⁺ ion; the ion name stays hydroxide.

  54. Carte 54

    Question

    What is the charge on each copper ion in Cu₃(PO₄)₂, taking phosphate as PO₄³⁻?

    Réponse

    +2. Two phosphate ions total −6, shared equally among three copper ions as +2 each.

  55. Carte 55

    Question

    Write the formula for sodium nitrite using Na⁺ and NO₂⁻.

    Réponse

    NaNO₂. One nitrite ion balances one sodium ion. Keep NO₂⁻ intact; NO₃⁻ would be nitrate.

  56. Carte 56

    Question

    Repair NH₄SO₄ as the formula for ammonium sulfate, using NH₄⁺ and SO₄²⁻.

    Réponse

    (NH₄)₂SO₄. Two whole ammonium ions are required to balance one sulfate ion; the 2 goes outside the ammonium parentheses.

Illustrated study cards with teal plus and coral minus signs, linked by a decorative loop to suggest charge balance.

56 cartes

Ionic Compound Naming Flashcards: Names, Formulas & Charge Balance

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