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Quizzes > Science

Electronegativity Practice Problems: Covalent Bond Polarity Quiz

Quick, free covalent bond polarity quiz with instant feedback and answer checks.

Editorial: Review CompletedCreated By: Grant MccroskeyUpdated Aug 23, 2025
Difficulty: Moderate
2-5mins
Learning OutcomesCheat Sheet
Paper art illustration shows stylized atoms and bonds on dark blue background for electronegativity quiz

Use this quiz to compare electronegativity values, spot periodic trends, and predict covalent bond polarity in molecules. Get instant scoring with brief explanations so you see what to review before a test. When you are done, check your understanding with our ionic and covalent bonds quiz, explore ionic covalent and metallic bonds, or try a vsepr theory quiz.

What electronegativity difference between two atoms generally indicates a nonpolar covalent bond?
Exactly 2.0
Between 0.5 and 1.7
Greater than 1.7
Less than 0.5
Nonpolar covalent bonds form when the electronegativity difference is very small, typically less than 0.5, because the electrons are shared almost equally. When the difference is larger, one atom attracts electrons significantly more, resulting in polar or ionic character. This threshold is a guideline used in general chemistry to predict bond type. For more details on electronegativity and bond types, see .
Which element has the highest electronegativity on the Pauling scale?
Chlorine
Oxygen
Hydrogen
Fluorine
Fluorine has the highest electronegativity of all elements at 3.98 on the Pauling scale. Its small atomic radius and high effective nuclear charge strongly attract bonding electrons. No other element on the periodic table exceeds fluorine's ability to attract shared electrons. For further information, see .
How does electronegativity change as you move from left to right across a period in the periodic table?
It stays the same
It varies unpredictably
It decreases
It increases
Electronegativity generally increases across a period due to increasing nuclear charge and a decreasing atomic radius, which draws bonding electrons closer. As the protons increase, the effective nuclear pull on shared electrons becomes stronger. This periodic trend helps predict bond polarity in compounds. You can read more on periodic trends at .
Given hydrogen (EN = 2.20) and chlorine (EN = 3.16), what type of bond do they form based on their electronegativity difference?
Nonpolar covalent
Metallic
Ionic
Polar covalent
The electronegativity difference between H and Cl is 0.96, which falls in the polar covalent range (0.5 - 1.7). In a polar covalent bond, electrons are shared unequally but not completely transferred. This unequal sharing gives one end a partial negative charge and the other a partial positive charge. More on this can be found at .
Which of the following bonds is the most polar?
H - F
C - O
C - N
H - H
Hydrogen - fluorine has an electronegativity difference of about 1.78, which is higher than the differences for C - O or C - N. The larger the difference, the more polar the bond, and H - F is the most polar among these choices. H - H is nonpolar because the atoms are identical. For more details, see .
What is the bond polarity of a carbon - hydrogen bond, given EN(C) = 2.55 and EN(H) = 2.20?
Nonpolar covalent
Coordinate covalent
Ionic
Polar covalent
The difference in electronegativity between carbon and hydrogen is 0.35, which falls below 0.5 and indicates a nonpolar covalent bond. In such bonds, electrons are shared almost equally. This is why many hydrocarbons are considered nonpolar molecules. More on C - H bond character can be found at .
Which element is more electronegative: selenium (EN = 2.55) or sulfur (EN = 2.58)?
Sulfur
Selenium
They are equal
Depends on the compound
Sulfur has a slightly higher electronegativity (2.58) than selenium (2.55) on the Pauling scale. As you move up a group in the periodic table, electronegativity generally increases due to decreasing atomic radius. The small numerical difference reflects their positions in the same group. See more at .
A bond between atoms A and B has an electronegativity difference of 2.2. What type of bond is this most likely?
Polar covalent
Coordinate covalent
Nonpolar covalent
Ionic
An electronegativity difference greater than about 1.7 typically indicates an ionic bond, where electrons are transferred rather than shared. At a difference of 2.2, A and B would form ions, leading to an ionic lattice. Ionic bonds have high melting and boiling points and conduct electricity in molten form. For deeper context, visit .
Rank the following bonds in order of decreasing bond polarity: B - F, N - O, C - F.
B - F > N - O > C - F
N - O > C - F > B - F
B - F > C - F > N - O
C - F > B - F > N - O
Electronegativity differences: B - F is about 1.94, C - F is 1.43, and N - O is 0.40. Thus, the bond polarity decreases in the order B - F > C - F > N - O. The greater the electronegativity difference, the more polarized the bond becomes. For more on ranking bond polarities, see .
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Study Outcomes

  1. Understand Electronegativity Concepts -

    Grasp the definition of electronegativity and its role in chemical bonding to build a solid foundation for practice problems.

  2. Compare Elemental Electronegativity -

    Analyze and rank elements such as carbon, oxygen, and bromine by their electron-attracting tendencies.

  3. Predict Bond Polarity -

    Apply electronegativity differences to determine bond type and polarity in various compounds.

  4. Apply Periodic Trends -

    Infer electronegativity patterns across periods and groups to predict trends for untested elements.

  5. Tackle Practice Problems -

    Employ strategies for solving electronegativity practice problems and tricky electronegativity questions efficiently.

  6. Evaluate Quiz Performance -

    Use the electronegativity quiz results to pinpoint strengths and areas for further study.

Cheat Sheet

  1. Periodic Trends in Electronegativity -

    Electronegativity generally increases across a period and decreases down a group, with fluorine (4.0 on the Pauling scale) being the most electronegative element and cesium (~0.7) the least. Referencing University of California publications, you can practice spotting trends in electronegativity practice problems by comparing elements like oxygen vs. sulfur. Familiarity with these trends is essential for any chemical bonding quiz or electronegativity test.

  2. Calculating Electronegativity Differences -

    Use the formula ΔEN = |χA - χB| (Pauling scale) to determine bond character; most textbooks (e.g., Brown & LeMay) cite a threshold of 1.7 for ionic vs. covalent bonds. For example, ΔEN(H - Cl) = |2.20 - 3.16| ≈ 0.96 indicates a polar covalent bond. Regularly solving electronegativity practice problems with this formula boosts your accuracy in electronegativity quiz scenarios.

  3. Bond Polarity and Classification -

    Based on ΔEN, classify bonds as nonpolar (<0.5), polar (0.5 - 1.7), or ionic (>1.7) according to IUPAC guidelines. For instance, ΔEN(C - H) ≈ 0.35 yields a nonpolar covalent bond, while ΔEN(Na - Cl) ≈ 2.23 is ionic. Practicing these distinctions in electronegativity questions enhances your grasp of molecular polarity for any chemical bonding quiz.

  4. Comparing Electronegativity Scales -

    While the Pauling scale is most common, the Mulliken scale (average of ionization energy and electron affinity) and Allred-Rochow scale offer alternative views (J. Am. Chem. Soc.). Knowing these helps you tackle advanced electronegativity practice problems and cross-reference values. For example, Mulliken's χ = (IE + EA)/2 can clarify why some values differ slightly from Pauling's.

  5. Mnemonic Tricks for Trend Recall -

    Use catchy phrases like "FONClBrISCHP" (fluorine, oxygen, nitrogen, chlorine, bromine, iodine, sulfur, carbon, hydrogen, phosphorus) to memorize the highest-to-lowest electronegative elements. This trick, endorsed by many university study guides, makes rapid recall effortless when facing timed electronegativity quiz questions. Combining mnemonics with drill problems ensures confidence in any electronegativity test!

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