Chemical Bonding Exam: Trivia Quiz! MCQ

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  • 1/9 Questions

    Ionic compounds are brittle because _____.

    • They are arranged in a regular shape and therefore cannot be broken apart.
    • They are arranged in a regular shape and force applied would bring ions of the same charge together.
    • They are arranged in a regular shape which shatters easily
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About This Quiz


What can be said about chemical bonding? Chemical bonding is any interaction that accounts for molecules, ions, crystals, and other stable materials that create the familiar substances in our daily lives. Suppose the complete energy of a group of atoms is lower than the sum of the component atoms' energies. In that case, they then bond collectively, and the energy lowering is the bonding energy. This quiz will improve your understanding of chemical bonding. Good luck.

Chemical Bonding Exam: Trivia Quiz! MCQ - Quiz

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  • 2. 

    Which of the following forces is the strongest?

    • Covalent bonds

    • Hydrogen bonds

    • Van der Waals forces

    Correct Answer
    A. Covalent bonds
    Explanation
    Covalent bonds are the strongest forces among the given options. Covalent bonds involve the sharing of electrons between atoms, creating a strong bond that holds the atoms together in a molecule. This sharing of electrons results in a stable configuration for both atoms, making covalent bonds highly stable and difficult to break. On the other hand, hydrogen bonds are weaker than covalent bonds as they involve an electrostatic attraction between a hydrogen atom and an electronegative atom. Van der Waals forces are even weaker than hydrogen bonds, arising from temporary fluctuations in electron distribution.

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  • 3. 

    Metallic compounds can conduct electricity in molten or solid state because of _____.

    • Presence of 'delocalised sea' of electrons

    • Presence of mobile ions

    • Presence of electrons

    • Presence of applied potential difference

    Correct Answer
    A. Presence of 'delocalised sea' of electrons
    Explanation
    Metallic compounds can conduct electricity in both their molten and solid states because of the presence of a 'delocalised sea' of electrons. In metallic bonding, the valence electrons are not localized to specific atoms but instead form a shared electron cloud that is free to move throughout the structure. This delocalized sea of electrons allows for the flow of electric current as the electrons can easily move and carry charge. This is why metallic compounds are good conductors of electricity.

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  • 4. 

    There are four ______ and one ______ in the compound C2H4.

    • A) double covalent bonds b) single covalent bond

    • A) triple covalent bonds b) double covalent bonds

    • A) triple covalent bonds b) single covalent bond

    • A) double covalent bounds b) triple covalent bonds

    • A) single covalent bond b) double covalent bonds

    • A) single covalent bond b) triple covalent bonds

    Correct Answer
    A. A) single covalent bond b) double covalent bonds
    Explanation
    The compound C2H4, also known as ethene, consists of one single covalent bond between the two carbon atoms (C2) and two double covalent bonds between each carbon atom and two hydrogen atoms (H4).

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  • 5. 

    Ionic compounds can conduct electricity in molten or aqueous state because of _____.

    • Presence of 'delocalised sea' of electrons

    • Presence of mobile ions

    • Presence of mobile electrons

    • Presence of applied potential difference

    Correct Answer
    A. Presence of mobile ions
    Explanation
    Ionic compounds can conduct electricity in molten or aqueous state because they contain ions that are free to move. In the molten or aqueous state, the ionic bonds are broken and the ions become mobile. These mobile ions can carry an electric charge and allow the flow of electricity through the compound. The presence of mobile ions enables the transfer of charge and the conduction of electricity in ionic compounds.

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  • 6. 

    For the covalent compound, HCl, the inter-molecular forces that are acting between the molecules are ________.

    • Covalent bonds

    • Permenant dipole-dipole

    • Temporary dipole-dipole

    • Hydrogen Bonding

    Correct Answer
    A. Permenant dipole-dipole
    Explanation
    The correct answer is permanent dipole-dipole. In HCl, the hydrogen atom has a partial positive charge and the chlorine atom has a partial negative charge due to the difference in electronegativity. This creates a permanent dipole in the molecule, and the positive end of one molecule is attracted to the negative end of another molecule, resulting in permanent dipole-dipole interactions between the HCl molecules.

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  • 7. 

    Which of the following are attributes of metals?

    • Generally high boiling and melting point for most metals, Malleable and Ductile, Brittle

    • Gerenrally high boiling and melting point for most metals, Conductor of electricity, Strong but not rigid

    • High Boiling point and Melting point for all metals, Conductor of heat, Conductor of electricity

    Correct Answer
    A. Gerenrally high boiling and melting point for most metals, Conductor of electricity, Strong but not rigid
    Explanation
    Metals generally have high boiling and melting points, making them able to withstand high temperatures. They are also malleable and ductile, meaning they can be easily shaped and stretched without breaking. Additionally, metals are good conductors of electricity, allowing electric current to flow through them easily. However, metals are not brittle; they are strong but not rigid, meaning they can be deformed without breaking.

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  • 8. 

    Sillicon oxide is exists as a giant covalent molecule.

    • True

    • False

    Correct Answer
    A. False
    Explanation
    Sillicon dioxide exists as a giant covalent molecule.

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  • 9. 

    The melting point of HBr is higher than that of HCl. Why is this so? Both substances exist as _________. The molecules of HBr are bigger than Hcl, therefore there is more distortion of the electron cloud and more energy is required to overcome the weak Van der Waals forces between the HBr molecules than to overcome the weaker Van der Waals forces between HCl molecules. Thus, the MP of HBr is higher than HCl.

    Correct Answer
    simple covalent molecules
    simple covalent structures
    Explanation
    The melting point of HBr is higher than that of HCl because both substances exist as simple covalent molecules or simple covalent structures. The molecules of HBr are bigger than HCl, which leads to more distortion of the electron cloud. As a result, more energy is required to overcome the weak Van der Waals forces between the HBr molecules compared to the weaker forces between HCl molecules. This higher energy requirement leads to a higher melting point for HBr.

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  • Mar 20, 2023
    Quiz Edited by
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  • May 15, 2011
    Quiz Created by
    Binhui19
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