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Quizzes > Science

Compound Test: Practice Compounds with 20 Quick Questions

Quick, free compound quiz to check your knowledge. Instant results.

Editorial: Review CompletedCreated By: Levan BaliashviliUpdated Aug 26, 2025
Difficulty: Moderate
Grade: Grade 10
Study OutcomesCheat Sheet
Colorful paper art promoting the Compound Challenge Blitz, a fast-paced chemistry quiz.

This quiz helps you practice compounds with 20 quick questions, clear answers, and short tips to build confidence. For a wider review, try our chemistry basics quiz, challenge yourself with a high school chemistry quiz, or focus your study with a chemistry chapter 2 quiz.

What is a chemical compound?
A physical mixture of elements that can be separated easily.
A substance that consists of only one type of element.
A combination of substances that retains the original properties of its components.
A pure substance formed by chemically combining two or more elements.
A chemical compound is formed when two or more elements chemically combine in fixed proportions, resulting in a substance with new properties. The bonds formed are strong, and the compound exhibits characteristics different from its constituent elements.
Which of the following best describes an ionic bond?
A weak bond that forms due to transient dipoles in atoms.
A bond that forms exclusively between two nonmetals.
A bond formed due to the electrostatic attraction between oppositely charged ions.
A bond formed by the sharing of electrons between atoms.
An ionic bond is created when one atom donates electrons to another, resulting in oppositely charged ions. The strong electrostatic forces between these ions hold the compound together.
What does a chemical formula represent?
The method used to synthesize the compound in the lab.
A description of the physical appearance of a compound.
The process by which elements combine.
The types and ratios of elements present in a compound.
A chemical formula provides a shorthand representation of the elements within a compound and the relative numbers of atoms of each element. It defines the compound's composition and allows one to infer its structure.
In compounds, what does the term 'molecular' typically indicate?
The compound consists of molecules held by covalent bonds.
The compound contains a mixture of different substances.
The compound is formed by ionic bonds.
The compound has a crystalline structure.
Molecular compounds are composed of individual molecules where atoms are connected by covalent bonds. This distinguishes them from ionic compounds, which are formed by the electrostatic attraction between ions.
Which property is generally characteristic of compounds?
Compounds lack any defined chemical bonds.
Compounds are always mixtures of substances.
Compounds have a fixed composition and distinct chemical properties.
Compounds can be separated into elements using physical methods.
Compounds are defined by their fixed composition and unique properties that differ from the individual elements from which they are made. Their chemical bonds create a stable structure that cannot be easily separated by simple physical means.
What is the correct formula for aluminum oxide?
AlO3
Al2O
AlO
Al2O3
Aluminum oxide consists of aluminum and oxygen in a fixed ratio that balances their charges. The formula Al2O3 correctly represents the combination of Al3+ and O2- ions, ensuring charge neutrality.
What is the oxidation state of sulfur in the sulfate ion (SO4^2-)?
+2
âˆ'2
+6
+4
In the sulfate ion, each oxygen typically has an oxidation number of -2. To achieve the overall -2 charge on the ion, sulfur must have an oxidation state of +6.
Which of the following best describes how an ionic bond is formed?
By the mutual exchange of electrons between atoms.
By the sharing of electrons between two nonmetals.
By the attraction of protons between atoms.
By the complete transfer of electrons from a metal to a nonmetal.
Ionic bonds form when a metal donates electrons to a nonmetal, resulting in oppositely charged ions that attract each other. This electron transfer leads to a stable electronic configuration for both atoms.
What is the systematic name for Fe2O3?
Iron(II) oxide
Ferrous oxide
Iron(III) oxide
Dioxide of iron
Fe2O3 contains iron in the +3 oxidation state and oxygen in the -2 state. The correct systematic name, Iron(III) oxide, indicates the oxidation state of iron explicitly, ensuring clarity in chemical nomenclature.
Which of the following is a molecular compound rather than an ionic compound?
KBr
LiF
CO2
NaCl
CO2 is formed by covalent bonds between carbon and oxygen, making it a molecular compound. In contrast, the other listed compounds are formed by ionic bonds between metals and nonmetals.
What distinguishes covalent bonds from ionic bonds in compounds?
Covalent bonds involve the transfer of electrons.
Covalent bonds involve the sharing of electrons.
Covalent bonds result in the formation of ions.
Covalent bonds are always stronger than ionic bonds.
Covalent bonds are characterized by the sharing of electrons between atoms, leading to the formation of molecules. This sharing contrasts with ionic bonds, where electrons are transferred to form ions.
What is the proper name for the compound NaCl?
Chlorosodium
Salt
Sodium chloride
Sodic chloride
NaCl is systematically named sodium chloride based on the elements it contains. This name follows the conventional nomenclature rules for ionic compounds, clarifying its composition.
Given Ca2+ and Cl- ions, what is the correct empirical formula of the compound they form?
Ca2Cl
CaCl
Ca2Cl2
CaCl2
Calcium ions (Ca2+) require two chloride ions (Cl-) to balance the charge in the compound, resulting in the formula CaCl2. This ensures that the overall compound is electrically neutral.
Why do ionic compounds generally have high melting points?
They have weak intermolecular forces.
They form large molecules that require little energy to break.
They are composed of discrete molecules that interact weakly.
Strong electrostatic forces within the ionic lattice require high energy to overcome.
Ionic compounds are structured as a lattice of oppositely charged ions, held together by strong electrostatic forces. A significant amount of energy is necessary to overcome these forces, resulting in high melting points.
What type of bonding is present in CH4 (methane)?
Metallic bonding
Covalent bonding
Hydrogen bonding
Ionic bonding
Methane (CH4) is composed of carbon and hydrogen atoms bonded together by covalent bonds, where electrons are shared. This type of bonding results in the formation of discrete molecules.
When naming binary molecular compounds, which prefix is used to indicate three atoms?
Tetra-
Tri-
Di-
Mono-
In chemical nomenclature, the prefix 'tri-' is used to indicate the presence of three atoms of an element in a molecular compound. This systematic approach helps clearly convey the composition of the compound.
What is the molecular geometry around the central atom in PCl5?
Trigonal bipyramidal
Tetrahedral
Trigonal planar
Octahedral
PCl5 has five bonding regions around the central phosphorus atom. According to VSEPR theory, these regions arrange themselves in a trigonal bipyramidal geometry to minimize electron repulsion.
When iron(III) nitrate, Fe(NO3)3, reacts with sodium hydroxide, NaOH, which of the following is the precipitate formed?
FeO
Fe(OH)3
Fe(OH)2
NaNO3
The reaction between Fe(NO3)3 and NaOH leads to the formation of iron(III) hydroxide, Fe(OH)3, as an insoluble precipitate. This reaction is a common qualitative test for the presence of Fe3+ ions.
Which compound is an example of an amphoteric oxide, capable of reacting with both acids and bases?
MgO
SiO2
CaO
ZnO
Amphoteric oxides react with both acids and bases. Zinc oxide (ZnO) is known for its amphoteric properties, allowing it to behave as either an acid or a base depending on the reacting substance.
How does lattice energy influence the melting point of ionic compounds?
Higher lattice energy typically corresponds to a lower melting point.
Lattice energy has no effect on melting points.
Higher lattice energy leads to higher melting points due to stronger ionic bonds.
Lower lattice energy results in higher melting points.
Lattice energy reflects the strength of the forces holding ions together in an ionic crystal. A higher lattice energy means that more energy is required to break these bonds, thereby increasing the melting point of the compound.
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Study Outcomes

  1. Analyze chemical compounds and their molecular structures.
  2. Apply stoichiometric principles to solve quantitative problems.
  3. Interpret chemical formulas to deduce compound properties.
  4. Evaluate reaction mechanisms to predict outcomes in chemical reactions.
  5. Synthesize core concepts to tackle advanced compound challenges.

Compound Quiz: Practice & Review Cheat Sheet

  1. Master the periodic table - Think of the periodic table as your treasure map to elements: it reveals trends in reactivity, atomic size, and electron configurations. By memorizing key groups and periods, you'll predict how elements interact and form compounds with ease. Dive into this layout to unlock the secrets of metals, nonmetals, and everything in between.
  2. Learn chemical nomenclature rules - Naming compounds correctly is like speaking the universal language of chemistry: it ensures scientists around the world understand exactly what you mean. From ionic salts to complex organic molecules, mastering prefixes, suffixes, and naming conventions will take you far. Get fluent in IUPAC and never misname a molecule again!
  3. Understand ionic and covalent bonding - Ionic bonds form when electrons are transferred between atoms, while covalent bonds share electrons to build molecules. Knowing which bond type you're dealing with helps predict melting points, solubilities, and conductivity. This knowledge is your key to unlocking compound behavior in everything from salt crystals to plastics.
  4. Familiarize yourself with functional groups - Functional groups are the personality traits of organic molecules: alcohols, carboxylic acids, amines and more each behave in signature ways. Spotting these groups lets you predict reactions and design new compounds for medicines or materials. Practice drawing and naming them until they become second nature!
  5. Practice balancing chemical equations - Balancing equations is like solving a puzzle: you adjust coefficients so mass and charge are conserved on both sides. This skill ensures you understand stoichiometry, reactant limits, and product yields for lab work or exams. The more you practice, the more intuitive reaction stoichiometry becomes!
  6. Use mnemonics for diatomic molecules - Mnemonics like "Have No Fear Of Ice Cold Beer" help you remember Hâ‚‚, Nâ‚‚, Fâ‚‚, Oâ‚‚, Iâ‚‚, Clâ‚‚, Brâ‚‚. A quick mental jingle means you'll never forget which elements exist as pairs in their pure form. Turn study time into song time and watch retention skyrocket!
  7. Study acid-base chemistry - Acids, bases, and pH are everywhere from digestion to industrial processes. Understanding proton donors and acceptors will help you master neutralization reactions, titration curves, and real‑world applications like water treatment. Get ready to mix, measure, and marvel at pH changes!
  8. Explore solubility rules - Predicting which compounds dissolve and which form precipitates is crucial for reactions in solution. Learn the common solubility guidelines for ionic salts and practice applying them to double displacement reactions. This skill saves you time in the lab and on exams!
  9. Review oxidation‑reduction reactions - Redox reactions involve electron transfers that power batteries, corrosion, and metabolic processes. Identifying oxidizing and reducing agents helps you balance redox equations and understand energy flows. Dive into half‑reaction methods and watch electrons in action!
  10. Understand molecular geometry - The 3D shapes of molecules dictate polarity, intermolecular forces, and reactivity. Using VSEPR theory, you'll predict bond angles and molecular shapes - linear, trigonal, tetrahedral and more. This geometric insight explains why water is bent and why carbon dioxide is linear!
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