Table of common polyatomic ions with their chemical formulas and charges.

The user has provided an image showing a table of chemical species (ions) labeled (a) through (l). However, the actual question/task is not explicitly stated in the prompt. The image shows:
(a) NH₄⁺
(b) H₃O⁺
(c) CN⁻
(d) SCN⁻
(e) CO₃²⁻
(f) ClO₃⁻
(g) SO²⁻
(h) PO₄³⁻
(i) SO₃²⁻
(j) NO₂⁻
(k) BF⁻
(l) NO₃⁻

Since no specific task is given, I need to figure out what the likely homework question is. Given these are all ions/polyatomic ions, common questions include:


- Identifying Lewis structures and molecular geometry
- Determining hybridization of central atoms
- Finding conjugate acids or bases
- Calculating formal charges
- Identifying which are acids vs bases

Without seeing the actual question, I should probably work through the most common analysis for these types of problems—likely identifying the molecular geometry and hybridization of each ion's central atom, since that's a standard exercise with this set of polyatomic ions. I'm realizing the question might be asking me to identify which species can act as Lewis acids or bases based on their electron configurations and charges. Let me think through what makes sense here—cations like NH₄ and H₃O⁺ have no lone pairs to donate, while anions like CN⁻, SCN⁻, and the oxyanions have lone pairs available, making them potential Lewis bases. The tetrahedral ions like BF₄⁻ are interesting because boron typically acts as a Lewis acid, but once it's bonded to four fluorines with a negative charge, it's saturated. I'm reconsidering what the actual question might be asking—it could be about identifying which species act as Lewis acids versus bases, or perhaps determining molecular geometries and hybridization states. Since the problem doesn't specify exactly what to find, I should probably work through the most common analyses for these ions: their Lewis structures, VSEPR geometries, and hybridization patterns, which would give a comprehensive answer regardless of the specific focus. I'm working through the Lewis structures and geometries for each ion systematically. For NH₄⁺ and H₃O⁺, I'm calculating valence electrons and determining that both have tetrahedral electron geometries with sp³ hybridization, though H₃O⁺ has a trigonal pyramidal molecular shape due to the lone pair. Now I'm moving on to analyze CN⁻ and the remaining ions. Continuing with the remaining polyatomic ions: carbonate has trigonal planar geometry with sp² hybridization, chlorate is trigonal pyramidal with sp³, sulfate is tetrahedral with sp³, and phosphate also appears to be tetrahedral with sp³ hybridization based on its four bonding domains and no lone pairs on the central atom.

For sulfite, I'm getting trigonal pyramidal geometry with sp³ hybridization due to the lone pair on sulfur. Nitrite bends with sp² hybridization, tetrafluoroborate is tetrahedral with sp³, and nitrate is trigonal planar with sp². Now I'm wondering if the question is actually asking me to identify which species can act as Lewis acids or bases instead.

Looking at the cations and anions, NH₄⁺ and H₃O⁺ are Brønsted acids that can donate protons, while the anions like CN⁻, SCN⁻, CO²⁻, and the others function as Brønsted bases by accepting protons. But I'm realizing the question might be asking something different entirely—maybe about molecular geometry, hybridization, or resonance structures rather than acid-base behavior. Since the original question isn't clearly stated, I should probably provide a comprehensive breakdown covering the key properties of each ion. I'm realizing the question might be asking about molecular geometry and hybridization for each ion, so let me work through that systematically. For each species, I need to count the valence electrons, determine the electron domains around the central atom, and then identify both the electron geometry and molecular geometry along with the hybridization state.