Write a formula for the compound that forms between potassium and each polyatomic ion. a. carbonate b. phosphate c. hydrogen phosphate d. acetate

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insert step 1> Identify the charge of the potassium ion (K^+), which is +1.

insert step 2> Determine the charge of each polyatomic ion: carbonate (CO_3^{2-}), phosphate (PO_4^{3-}), hydrogen phosphate (HPO_4^{2-}), and acetate (C_2H_3O_2^{-}).

insert step 3> Use the criss-cross method to balance the charges between potassium and each polyatomic ion.

insert step 4> For carbonate, combine K^+ and CO_3^{2-} to form K_2CO_3.

insert step 5> For phosphate, combine K^+ and PO_4^{3-} to form K_3PO_4. For hydrogen phosphate, combine K^+ and HPO_4^{2-} to form K_2HPO_4. For acetate, combine K^+ and C_2H_3O_2^{-} to form KC_2H_3O_2.

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주요 개념

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Ionic Compounds

Ionic compounds are formed when metals react with nonmetals, resulting in the transfer of electrons. In this case, potassium (a metal) donates an electron to the polyatomic ions, which are negatively charged. The resulting compound is held together by the electrostatic attraction between the positively charged potassium ions and the negatively charged polyatomic ions.

Polyatomic Ions

Polyatomic ions are ions that consist of two or more atoms bonded together, carrying a net charge. Common examples include carbonate (CO3^2-), phosphate (PO4^3-), hydrogen phosphate (HPO4^2-), and acetate (C2H3O2^-). Understanding the charge and composition of these ions is crucial for writing the correct formulas for the resulting ionic compounds.

Chemical Formula Writing

Writing chemical formulas involves combining the symbols of the elements or ions in a compound, reflecting their ratios and charges. For ionic compounds, the total positive charge must balance the total negative charge. This requires knowledge of the charges of both potassium and the polyatomic ions to ensure the correct stoichiometry in the final formula.