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Quizzes > Science

Ionic Compounds Quiz: Spot what is not an ionic compound

Quick chemistry quiz to spot the non-ionic compound. Instant results.

Editorial: Review CompletedCreated By: Caleb DagnallUpdated Aug 27, 2025
Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Paper art chemistry quiz layout with ionic compounds question on golden yellow background

This ionic compounds quiz helps you spot what is not an ionic compound and confirm which formulas are truly ionic. After each quick question, build skills with ionic formula practice, then compare patterns in an ionic and covalent quiz or broaden your view with ionic covalent and metallic bonds.

All of the following are ionic compounds except:
CO2
CaF2
MgO
NaCl
CO2 is a covalent molecular compound made up of discrete molecules rather than ions. It does not form a crystalline lattice of cations and anions. Ionic compounds rely on electrostatic attraction between positive and negative ions to maintain their structure. .
All of the following are ionic compounds except:
KBr
PCl5
NH4Cl
Li2S
Phosphorus pentachloride (PCl5) is a covalent molecular compound with discrete P - Cl bonds. It does not dissociate into ions in the solid state. Ionic compounds consist of positive and negative ions held by electrostatic forces. .
Which of the following is not an ionic compound?
Na3N
CuSO4
Al2O3
H2O
Water (H2O) is a covalent molecular compound with polar covalent bonds, and it does not form an ionic lattice. Ionic compounds are composed of cations and anions held together by strong electrostatic attraction. .
All of the following are ionic except:
Na3PO4
BaCl2
KI
CS2
Carbon disulfide (CS2) is a covalent molecular compound with nonpolar C - S bonds and exists as discrete molecules. It does not contain ions in a lattice. Ionic compounds consist of charged species held by ionic bonds. .
All of the following are ionic compounds except:
LiOH
NaNO3
NH3
SrF2
Ammonia (NH3) is a covalent molecular compound with polar N - H bonds; it does not consist of cations and anions in a lattice. Ionic compounds are salts formed by electrostatic attraction between ions. .
All of the following are ionic compounds except:
BaSO4
CaO
SiO2
NaCl
Silicon dioxide (SiO2) is a covalent network solid in which each silicon atom bonds to four oxygen atoms, forming a continuous network. It lacks discrete ions in a lattice. Ionic compounds consist of distinct positively and negatively charged ions. .
Which of the following is not ionic?
HF
LiCl
NaBr
CsI
Hydrogen fluoride (HF) is a polar covalent compound that forms discrete HF molecules held together by hydrogen bonding in the liquid state. It does not form an ionic lattice. Ionic compounds are formed by electrostatic attraction between ions. .
All of the following are ionic except:
MgCl2
HCl
K2CrO4
RbBr
Hydrogen chloride (HCl) in its molecular form is a covalent compound composed of H - Cl bonds. It does ionize in water, but the pure substance is covalent. Ionic compounds exist as solids composed of ions in a lattice. .
Identify the non-ionic compound:
MgCO3
CH4
Fe2O3
Ca3(PO4)2
Methane (CH4) is a covalent molecular compound with nonpolar C - H bonds and discrete molecules. It does not form ions. The other options are ionic compounds composed of metal cations and nonmetal anions. .
All of the following are ionic compounds except:
Na2O
CCl4
PbCl2
ZnS
Carbon tetrachloride (CCl4) is a covalent molecular compound with nonpolar C - Cl bonds. It does not consist of ions. Ionic compounds are held together by the electrostatic attraction between positively and negatively charged ions. .
Which is not ionic:
BaO
NH4NO3
NaCl
P4O10
Tetraphosphorus decoxide (P4O10) is a covalent molecular oxide composed of P4O10 molecules. It does not form an ionic lattice. The other listed compounds are ionic salts formed by metal cations and nonmetal anions. .
All of the following are ionic except:
K3PO4
CO2
BeCl2
AgNO3
Carbon dioxide (CO2) is a covalent molecular compound composed of discrete CO2 molecules. It does not consist of charged ions. Ionic compounds are made of positive and negative ions arranged in a crystalline lattice. .
Which is the only non-ionic compound among these?
ThO2
SiO2
UO2
PuO2
Silicon dioxide (SiO2) is a covalent network solid with each silicon atom tetrahedrally bonded to oxygen atoms, forming a continuous network. The actinide dioxides listed are predominantly ionic metal oxides. .
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Study Outcomes

  1. Differentiate Ionic and Covalent Compounds -

    Apply your knowledge of chemical bonding to distinguish ionic compounds from covalent or molecular species based on their formulas and bond types.

  2. Identify Non-Ionic Exceptions -

    Spot which substance does not qualify as an ionic compound when presented with a list, answering 'all of the following are ionic compounds except.'

  3. Recall Two Main Ionic Compound Types -

    Explain the classification of ionic compounds into their two primary categories and cite representative examples for each.

  4. Describe Characteristic Properties -

    List and describe three defining properties of ionic compounds - high melting points, electrical conductivity, and solubility in polar solvents.

  5. Analyze Conductivity and Melting Trends -

    Evaluate how ionic bonding influences melting behavior and electrical conductivity in solid and molten states.

Cheat Sheet

  1. Binary vs. Polyatomic Ionic Compounds -

    The two main types of ionic compounds are binary ionic compounds (formed from one metal and one nonmetal, e.g., NaCl) and polyatomic ionic compounds (containing charged molecular groups, e.g., NH₄NO₃). Use the "BiPo" mnemonic to remember these categories when tackling 4.04 quiz properties of ionic compounds. (Chemistry LibreTexts)

  2. Identifying Exceptions: "All of the Following Are Ionic Compounds Except…" -

    This question tests your ability to distinguish ionic from covalent substances by examining properties like electron transfer vs. sharing. For example, CO₂ is covalent, making it the correct answer in an "all of the following are ionic compounds except" scenario. (Royal Society of Chemistry)

  3. Three Characteristic Properties of Ionic Compounds -

    Ionic compounds typically have high melting/boiling points, conduct electricity when molten or dissolved, and are hard but brittle. Remember "Melts, Conducts, Shatters" (MCS) to quickly recall what are three characteristic properties of ionic compounds in your quiz ionic compounds prep. (American Chemical Society)

  4. Lattice Energy and Crystal Structure -

    The strength of ionic bonds is quantified by lattice energy, which correlates with melting point and solubility. Smaller ions with higher charges (e.g., MgO) have higher lattice energies, so they require more heat to melt. (Journal of Chemical Education)

  5. Solubility Trends in Water -

    Most ionic compounds dissolve in water due to ion - dipole interactions; think of NaCl dissociating into Na❺ and Cl❻. Recognizing solubility rules helps you predict precipitates and answer "quiz ionic compounds" questions with confidence. (International Union of Pure and Applied Chemistry)

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