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Quizzes > High School Quizzes > Science

Polyatomic Ions Practice Quiz

Master polyatomic ions with flashcards and quizzes

Difficulty: Moderate
Grade: Grade 10
Study OutcomesCheat Sheet
Colorful paper art promoting a Polyatomic Ion Pop Quiz for high school chemistry students.

Use this 20-question flashcards quiz to practice polyatomic ions - names, formulas, and charges - so you remember them fast. Work through quick prompts, spot weak spots before a chem exam, and lock in common groups like sulfate, nitrate, acetate, and ammonium. Play it as a short warm-up or repeat rounds until each card sticks.

What is the chemical formula for the nitrate ion?
N3O
NO2^-
NO4^-
NO3^-
The nitrate ion consists of one nitrogen atom and three oxygen atoms, giving it the formula NO3^- . This is a fundamental fact about nitrate that students must remember.
What is the charge on the sulfate ion?
0
3-
2-
1-
Sulfate is made up of one sulfur atom and four oxygen atoms carrying an overall charge of 2-. This charge is essential for balancing compounds that include sulfate.
Which polyatomic ion contains 4 oxygen atoms and has a -2 charge?
Ammonium (NH4^+)
Sulfate (SO4^2-)
Phosphate (PO4^3-)
Nitrate (NO3^-)
Sulfate is characterized by its composition of one sulfur atom and four oxygen atoms with a -2 charge. This clearly distinguishes it from other polyatomic ions.
What is the chemical formula for the ammonium ion?
NH4^-
NH4^+
N2H4
NH3
The ammonium ion is a positively charged polyatomic ion with the formula NH4^+. It is commonly encountered in many ionic compounds and is vital for charge balancing.
Which ion is represented by the formula PO4^3-?
Phosphate
Nitrate
Carbonate
Sulfate
Phosphate is the polyatomic ion with the formula PO4^3-. It plays a significant role in both inorganic and biological chemistry.
What is the chemical name for the ion HCO3^-?
Carbonate
Bicarbonate
Hydroxide
Acetate
HCO3^- is known as the bicarbonate ion. It is an important part of acid-base equilibria and buffering systems in both natural and industrial processes.
What is the formula for the dichromate ion?
Cr2O4^2-
CrO7^-
CrO4^2-
Cr2O7^2-
The dichromate ion is composed of two chromium atoms and seven oxygen atoms with a 2- charge. This distinguishes it from the chromate ion, which has the formula CrO4^2-.
Which of the following is the correct formula for the perchlorate ion?
ClO^-
ClO4^-
ClO3^-
ClO2^-
Perchlorate consists of one chlorine atom bonded to four oxygen atoms and carries a negative charge. This formula is distinct from other chlorine-oxygen ions such as chlorate and hypochlorite.
What is the common name for the ion HSO4^-?
Bisulfate
Sulfite
Hydrogen sulfate
Sulfate
HSO4^- is commonly known as hydrogen sulfate. This ion is formed from sulfuric acid when one proton is lost and plays a key role in polyprotic acid behavior.
What is the charge on the phosphate ion?
0
-1
-3
-2
The phosphate ion (PO4^3-) carries a -3 charge, which is crucial for forming balanced chemical compounds. This ion is a common constituent in many minerals and biological molecules.
Which polyatomic ion is represented by the formula CO3^2-?
Nitrate
Bicarbonate
Sulfate
Carbonate
CO3^2- is the formula for the carbonate ion, an important ion in geological and environmental chemistry. Recognizing its structure is key to understanding many mineral-based reactions.
Identify the ion with the formula CrO4^2-.
Oxalate
Dichromate
Chromate
Sulfate
CrO4^2- is the chromate ion, which consists of one chromium atom and four oxygen atoms. This ion is different from dichromate (Cr2O7^2-) both in composition and in chemical behavior.
Which polyatomic ion contains nitrogen and two oxygen atoms and has a -1 charge?
Nitride (N^3-)
Nitrite (NO2^-)
Ammonium (NH4^+)
Nitrate (NO3^-)
The nitrite ion (NO2^-) is composed of one nitrogen atom and two oxygen atoms with a -1 charge. This distinguishes it clearly from the nitrate ion, which contains an extra oxygen atom.
Which of the following best describes the nitrate ion (NO3^-)?
It contains a central oxygen atom bonded to three nitrogen atoms.
It has alternating single and double bonds with distinct bond lengths.
It is a linear molecule.
It has three equivalent N-O bonds due to resonance.
The nitrate ion exhibits resonance, which results in three equivalent N-O bonds. This delocalization of electrons is a key factor in the ion's stability.
How does the nitrite ion (NO2^-) differ from the nitrate ion (NO3^-)?
Nitrite has a higher negative charge than nitrate.
Nitrite is a cation, whereas nitrate is an anion.
Nitrite has one fewer oxygen than nitrate.
Nitrite contains sulfur instead of nitrogen.
The nitrite ion has two oxygen atoms compared to nitrate's three, while both carry a -1 charge. This difference in oxygen count is the main distinction between the two ions.
Which polyatomic ion exhibits resonance stabilization resulting in equal bond lengths among its oxygen atoms?
Ammonium (NH4^+)
Sulfate (SO4^2-)
Dichromate (Cr2O7^2-)
Nitrate (NO3^-)
The nitrate ion has its negative charge delocalized equally over its three oxygen atoms, leading to equal bond lengths. This phenomenon, known as resonance stabilization, is crucial for the ion's stability.
Carbonate (CO3^2-) and sulfate (SO4^2-) ions share tetrahedral geometry, but what is the primary difference in their structures?
Carbonate has a higher overall charge than sulfate.
Sulfate is linear while carbonate is bent.
Carbonate has three oxygen atoms while sulfate has four.
Carbonate contains sulfur whereas sulfate contains carbon.
The key structural difference is that the carbonate ion contains three oxygen atoms, whereas the sulfate ion contains four. Despite both having tetrahedral shapes, this difference fundamentally affects their bonding and chemical properties.
When a compound containing bicarbonate (HCO3^-) is heated, which gas is most likely released?
Carbon dioxide (CO2)
Hydrogen (H2)
Nitrogen (N2)
Oxygen (O2)
Heating bicarbonate compounds typically leads to the decomposition of HCO3^- to release carbon dioxide. This reaction is commonly observed in various chemical and culinary processes.
How does resonance stabilization in polyatomic ions, such as the nitrate ion, affect their chemical reactivity?
It decreases reactivity by delocalizing charge.
It makes the ions unstable in solution.
It increases reactivity by concentrating charge on one atom.
It has no effect on reactivity.
Resonance stabilization spreads the negative charge over several atoms, reducing localized charge density and thus reactivity. This delocalization makes these ions more stable and less prone to react in ways that disrupt the electron distribution.
Why is it important to consider multiple resonance structures when drawing the Lewis structure for polyatomic ions like dichromate (Cr2O7^2-)?
It provides a more accurate depiction of electron delocalization.
It indicates the ion does not have any formal charges.
It helps to determine the exact shape of the ion as linear.
It simplifies the understanding of bonding by showing only one possible configuration.
Drawing multiple resonance structures shows how electrons are delocalized across the ion, offering a more complete picture of its bonding environment. This approach is essential for understanding the stability and reactivity of polyatomic ions.
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Study Outcomes

  1. Understand the structure and charge of common polyatomic ions.
  2. Identify polyatomic ions in various chemical compounds.
  3. Analyze the nomenclature associated with polyatomic ions.
  4. Apply polyatomic ion knowledge to balance chemical equations.
  5. Evaluate the significance of polyatomic ions in chemical reactions.

Polyatomic Ions Flashcards Cheat Sheet

  1. Polyatomic Ions as Units - Polyatomic ions are groups of atoms that team up, sharing electrons to carry a charge and act as a single chunk in reactions. Treating them like one big atom can simplify balancing equations and writing formulas Learn more
  2. Key Polyatomic Players - You'll meet sulfate (SO₄²❻), nitrate (NO₃❻), and ammonium (NH₄❺) over and over in chemistry class, so get cozy with their shapes and charges. Recognizing these VIP ions by sight and symbol will speed up your problem solving Discover common ions
  3. Naming Conventions: -ate vs -ite - Names ending in "-ate" carry one extra oxygen compared to their "-ite" cousins (for example, sulfate vs sulfite). This tiny suffix swap can change formulas, so listen to the name! Naming guide
  4. Oxygen Prefixes: per- & hypo- - Prefix "per-" means you get an extra oxygen beyond the "-ate" form, while "hypo-" strips one oxygen off the "-ite" form (like perchlorate vs hypochlorite). It's like adding or removing a Lego block from your ion structure. Oxygen prefixes explained
  5. Hydrogen Addition Effects - Slap a hydrogen atom onto a polyatomic ion and you'll reduce its negative charge by one (carbonate CO₃²❻ becomes bicarbonate HCO₃❻). This small change can completely flip how the ion behaves in acids and bases. Hydrogen hacks
  6. Mnemonic Magic for Ion Mastery - Try "Nick The Camel Ate Clams for Supper in Phoenix" to recall elements, oxygens, and charges: consonants = oxygens, vowels = charge. Mnemonics turn boring lists into catchy jingles you won't forget! Use mnemonics
  7. Formula Practice - Combine your polyatomic ions with cations and watch the magic: swap subscripts until the overall charge is zero. Practicing writing out formulas builds speed so you're ready for any quiz. Practice formulas
  8. Acid-Base Behavior - Polyatomic ions like bicarbonate (HCO₃❻) can accept or donate protons, acting as bases or acids in reactions. Understanding this flip‑flop is key to mastering pH and buffer systems. Acid-base guide
  9. Everyday Ion Applications - You encounter ions like phosphate in fertilizers and sulfate in detergents every day - chemistry is literally in your laundry! Seeing these particles in action makes the subject more relevant (and fun). Real-world uses
  10. Flashcards & Quizzes - Testing yourself with flashcards or quick quizzes cements your memory and boosts confidence before exams. The more you practice, the more natural these ions will feel. Study strategies
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