Match Directions: Vertical Axis With Horizontal Axis

Directions Match The Vertical Axis With The Horizontal Axis To Write

Directions: Match the vertical axis with the horizontal axis to write the formulas. I did the first row and a select few for you. When you are finished, go to the discussion board and ask a question, add a comment or give some help.

OH- | H2CO3

NO3- | HNO3

CO32- | H2CO3

SO42- | H2SO4

PO43- | H3PO4

H+ | HOH

Na+ | Na+

Mg2+ | Mg(NO3)2

NH4+ | (NH4)2SO4

Ca2+ | Ca(OH)2

K+ | K2CO3

Al3+ | AlPO4

Pb4+ | to be matched accordingly based on context

Paper For Above instruction

The task of matching the vertical axes (ions or compounds) with the horizontal axes (counter ions, acids, or bases) to correctly form chemical formulas is fundamental in understanding ionic compounds and chemical reactions. This process involves recognizing the charges of ions and pairing them appropriately to satisfy electrical neutrality, which is essential in both inorganic chemistry and solution chemistry.

First, understanding the nature of ions such as hydroxide (OH-), nitrate (NO3-), carbonate (CO32-), sulfate (SO42-), phosphate (PO43-), hydrogen ion (H+), and other cations like sodium (Na+), magnesium (Mg2+), ammonium (NH4+), calcium (Ca2+), potassium (K+), aluminum (Al3+), and lead (Pb4+) is crucial for proper pairing.

For instance, in the case of hydroxide (OH-) paired with H2CO3 (carbonic acid), the formulas may represent bases and acids that react to form salts or neutralization products. Similarly, pairing Na+ with Cl- (not present here but often used in examples) results in sodium chloride. In this worksheet, the goal is to pair polyatomic ions and simple ions with acids and bases to construct valid formulas.

An illustrative example is Mg2+ pairing with NO3- to form magnesium nitrate, Mg(NO3)2. This shows the importance of charge balancing—two nitrates balancing one magnesium cation. Likewise, pairing NH4+ with sulfate (SO42-) produces ammonium sulfate, which requires two ammonium ions to balance one sulfate ion, resulting in (NH4)2SO4.

The comprehension of these pairing principles enables students to predict formulas accurately and understand chemical reactions better, especially in aqueous solutions where ionic interactions are common. These skills are vital for applications in pharmaceuticals, environmental science, and industrial chemistry where formulation and reaction prediction are routine.

References

  • Zumdahl, S. S., & Zumdahl, S. A. (2014). Chemistry: An Atoms First Approach. Cengage Learning.
  • Brown, T. L., LeMay, H. E., Bursten, B. E., Murphy, C., & Woodward, A. (2012). Chemistry: The Central Science. Pearson.
  • Atkins, P., & de Paula, J. (2010). Physical Chemistry. Oxford University Press.
  • Chang, R., & Goldsby, K. (2016). Chemistry (12th Ed.). McGraw-Hill Education.
  • Petrucci, R. H., Herring, F. G., Madura, J. D., & Bissonnette, C. (2017). General Chemistry: Principles & Modern Applications. Pearson.
  • Laing, D. (2018). Principles of Inorganic Chemistry. University Science Books.
  • House, J. E. (2012). Inorganic Chemistry. Academic Press.
  • Holleman, A. F., Wiberg, E., & Wiberg, N. (2013). Inorganic Chemistry. Academic Press.
  • Das, P. K., & Kumar, M. (2013). Practice of Inorganic Chemistry. Narosa Publishing House.
  • Chang, R. (2010). Chemistry: The Central Science. McGraw-Hill Education.

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