Give a Formula for these names: 51. Sodium iodite 52. Chromium (VI) oxide 53. Potassium bromate 54. Potassium perbromate 55. Sodium hypofluorite 56. Potassium fluorate 57. Dinitrogen tetrasulfide 58. Nitrogen disulfide 59. Hydrobromic acid 60. Hydrogen bromide 61. Perbromric acid 62. Bromic acid 63. Bromous acid 64. Hypobromous acid 65. Tin (II) nitrate 66. Tin (IV) nitrate 67. Aluminum carbide 68. Barium carbonate 69. Tungsten (IV) carbonate 70. Sodium hydrogen carbonate 71. Perfluoric acid 72. fluoric acid 73. Fluorous acid 74. Hypofluorous acid 75. Hydrofluoric acid 76. Hydrogen fluoride 77. Sulfuric acid 78. Hydrosulfuric acid 79. Sulfurous acid 80. Iron (II) phosphate 81. Iron (II) hydrogen phosphate 82. Iron (II) dihydrogen phosphate 83. Iron (III) phosphate 84. Iron (III) hydrogen phosphate 85. Iron (III) dihydrogen phosphate 86. Magnesium iodide 87. periodic acid 88. iodic acid 89. lodous acid 90. hypolodous acid 91. hydroiodic acid 92. Zinc periodate 93. Zinc iodate 94. Zinc iodite 95. Zinc hypoidoite 96. Hypofluorous acid 97. Periodic Acid 98. Tin (IV) hypoiodite 99. Tin (II) hypoiodite 100. Calcium hypoiodite 101. hydrocyanic acid
The Correct Answer and Explanation is:
Formulas:
- Sodium iodite – NaIO₂
- Chromium (VI) oxide – CrO₃
- Potassium bromate – KBrO₃
- Potassium perbromate – KBrO₄
- Sodium hypofluorite – NaFO
- Potassium fluorate – KFO₃
- Dinitrogen tetrasulfide – N₂S₄
- Nitrogen disulfide – NS₂
- Hydrobromic acid – HBr (aq)
- Hydrogen bromide – HBr (g)
- Perbromic acid – HBrO₄
- Bromic acid – HBrO₃
- Bromous acid – HBrO₂
- Hypobromous acid – HBrO
- Tin (II) nitrate – Sn(NO₃)₂
- Tin (IV) nitrate – Sn(NO₃)₄
- Aluminum carbide – Al₄C₃
- Barium carbonate – BaCO₃
- Tungsten (IV) carbonate – W(CO₃)₂
- Sodium hydrogen carbonate – NaHCO₃
- Perfluoric acid – HFO₄
- Fluoric acid – HFO₃
- Fluorous acid – HFO₂
- Hypofluorous acid – HFO
- Hydrofluoric acid – HF (aq)
- Hydrogen fluoride – HF (g)
- Sulfuric acid – H₂SO₄
- Hydrosulfuric acid – H₂S (aq)
- Sulfurous acid – H₂SO₃
- Iron (II) phosphate – Fe₃(PO₄)₂
- Iron (II) hydrogen phosphate – FeHPO₄
- Iron (II) dihydrogen phosphate – Fe(H₂PO₄)₂
- Iron (III) phosphate – FePO₄
- Iron (III) hydrogen phosphate – Fe(HPO₄)₃
- Iron (III) dihydrogen phosphate – Fe(H₂PO₄)₃
- Magnesium iodide – MgI₂
- Periodic acid – HIO₄
- Iodic acid – HIO₃
- Iodous acid – HIO₂
- Hypoiodous acid – HIO
- Hydroiodic acid – HI (aq)
- Zinc periodate – Zn(IO₄)₂
- Zinc iodate – Zn(IO₃)₂
- Zinc iodite – Zn(IO₂)₂
- Zinc hypoiodite – Zn(IO)₂
- Hypofluorous acid – HFO
- Periodic acid – HIO₄
- Tin (IV) hypoiodite – Sn(IO)₄
- Tin (II) hypoiodite – Sn(IO)₂
- Calcium hypoiodite – Ca(IO)₂
- Hydrocyanic acid – HCN (aq)
Explanation:
In inorganic chemistry, the naming and writing of chemical formulas follow systematic rules set by IUPAC. These rules depend on whether a compound is ionic, molecular, or acidic.
Ionic compounds consist of a metal and a nonmetal. The cation (metal) is written first, followed by the anion. Transition metals may have multiple oxidation states; their charges are indicated with Roman numerals (e.g., Sn(IV) = Sn⁴⁺). Polyatomic ions, like nitrate (NO₃⁻) or phosphate (PO₄³⁻), retain their names and are combined with cations based on charge balance. For example, tin(IV) nitrate becomes Sn(NO₃)₄ because Sn⁴⁺ requires four NO₃⁻ ions to balance the charge.
Molecular compounds, formed between nonmetals, use Greek prefixes (mono-, di-, tri-, etc.) to indicate the number of atoms. For instance, dinitrogen tetrasulfide (N₂S₄) directly reflects the number of atoms.
Acids are named based on the anion they contain. Binary acids (hydrogen + one other element) use the prefix “hydro-” and the suffix “-ic” (e.g., HBr = hydrobromic acid). Oxyacids, which contain hydrogen, oxygen, and another element (typically a nonmetal), are named from their polyatomic ions. If the ion ends in:
- -ate → acid ends in -ic (e.g., HBrO₃ = bromic acid)
- -ite → acid ends in -ous (e.g., HBrO₂ = bromous acid)
- per-…-ate → acid is per-…-ic (e.g., HBrO₄ = perbromic acid)
- hypo-…-ite → acid is hypo-…-ous (e.g., HBrO = hypobromous acid)
Understanding oxidation states and ion charges is crucial for writing correct formulas.
