Chemical Bonding Quiz

Grade 11 · Science · Quiz

10 questions covering bond types, VSEPR geometry, electronegativity, Lewis structures, and bonding properties.

Questions

1. Which element has the highest electronegativity?

   1. Oxygen
   2. Nitrogen
   3. Fluorine
   4. Chlorine
   Show answer

   Answer: Fluorine

   Fluorine (3.98 on the Pauling scale) is the most electronegative element, in the upper-right of the periodic table.

2. What type of bond holds sodium chloride (NaCl) together?

   1. Polar covalent
   2. Nonpolar covalent
   3. Ionic
   4. Metallic
   Show answer

   Answer: Ionic

   Na transfers its valence electron to Cl, forming Na⁺ and Cl⁻ held by electrostatic attraction.

3. How many bonding pairs of electrons are in a triple bond?

   1. 1
   2. 2
   3. 3
   4. 6
   Show answer

   Answer: 3

   A triple bond has 3 shared pairs of electrons (6 electrons total), as in N₂ (N≡N).

4. According to VSEPR, what is the geometry of CH₄?

   1. Linear
   2. Trigonal planar
   3. Bent
   4. Tetrahedral
   Show answer

   Answer: Tetrahedral

   Carbon has 4 bonding pairs and 0 lone pairs in CH₄ — tetrahedral geometry, 109.5° bond angles.

5. Which property of metals is BEST explained by the electron sea model?

   1. High melting point
   2. Electrical conductivity
   3. Brittleness
   4. Low density
   Show answer

   Answer: Electrical conductivity

   Delocalized electrons in the metallic electron sea carry charge freely through the metal.

6. A molecule has 2 bonding pairs and 2 lone pairs around its central atom. What is the molecular geometry?

   1. Linear
   2. Tetrahedral
   3. Trigonal pyramidal
   4. Bent
   Show answer

   Answer: Bent

   2 bonding + 2 lone pairs = tetrahedral electron geometry, but molecular shape (bonded atoms only) is bent.

7. Which pair would most likely form an ionic compound?

   1. C and O
   2. N and H
   3. Na and Cl
   4. S and O
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   Answer: Na and Cl

   Ionic bonds form with large electronegativity differences — Na (metal) and Cl (nonmetal) differ by ~2.1.

8. In a Lewis structure, what does a lone pair represent?

   1. Two electrons in a bond
   2. Two nonbonding electrons on an atom
   3. A double bond
   4. An ionic charge
   Show answer

   Answer: Two nonbonding electrons on an atom

   Lone pairs are nonbonding electron pairs associated with one atom and not shared with another.

9. CO₂ is nonpolar despite having polar C=O bonds. Why?

   1. Bond angles are 90°
   2. Dipoles cancel due to linear symmetrical geometry
   3. C and O have equal electronegativity
   4. Lone pairs cancel the charge
   Show answer

   Answer: Dipoles cancel due to linear symmetrical geometry

   CO₂ is linear (180°). The two C=O dipoles point in opposite directions and cancel, making the molecule nonpolar overall.

10. The octet rule states that atoms tend to form bonds until they have how many valence electrons?

    1. 2
    2. 4
    3. 8
    4. 18
    Show answer

    Answer: 8

    Most main-group atoms achieve stability with 8 valence electrons. Hydrogen is an exception, needing only 2 (duet rule).

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