Covalent & Ionic Bonding, Electronegativity Quiz

10 Questions | Total Attempts: 209

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Covalent & Ionic Bonding, Electronegativity Quiz

Covalent & Ionic Bonding, Electronegativity Flash Quiz


Questions and Answers
  • 1. 
    Identify the statement that is correct about the number of protons and electrons in an atom:
    • A. 

      The number of protons and the number of electrons in an atom are always equal.

    • B. 

      The number of protons is always greater than the number of electrons in an atom.

    • C. 

      The number of protons is always less than the number of electrons in an atom.

    • D. 

      The number of protons and electrons equals the mass of an atom.

  • 2. 
    Choose the statement that best explains: Why do hydrogen atoms usually exist as molecules, H2?
    • A. 

      Hydrogen has an atomic number of one and is unsatisfied when the outermost orbital is unfilled. A hydrogen molecule of two hydrogen atoms is more stable than two individual hydrogen atoms

    • B. 

      Hydrogen has an atomic number of two and does not need to share

    • C. 

      Hydrogen usually combines with other atoms to form covalent bonds

    • D. 

      Hydrogen has one proton and is in search of one neutron

  • 3. 
    What is a valence electron?
    • A. 

      Electrons in the outer cloud of an atom

    • B. 

      A negatively charge ion

    • C. 

      A positively charge ion

    • D. 

      Ionically bonded electrons

  • 4. 
    What is electronegativity?
    • A. 

      How many electrons are in a valence.

    • B. 

      The strength of an atoms' electrons.

    • C. 

      The electrical charge of a polar molecule.

    • D. 

      The exchange of electrons in ionic bonding.

  • 5. 
    This diagram represents H2.  What does the Hsymbol mean?
    • A. 

      The H2 symbol represents two atoms of Hydrogen.

    • B. 

      The H2 symbol represents a Hydrogen atom.

    • C. 

      The H2 symbol represents a water molecule.

    • D. 

      The H2 symbol represents an ionic bond.

  • 6. 
    In this diagram, the e- represents:
    • A. 

      The e- represents the covalent Hydrogen electrons in this Hydrogen molecule.

    • B. 

      The pair of e- represents the double covalent Hydrogen electrons in the Hydrogen molecule.

    • C. 

      The pair of e- represents the ionic Hydrogen electrons in this Hydrogen molecule.

    • D. 

      The e- represents the single shared Hydrogen electron in this Hydrogen molecule.

  • 7. 
    Why are Hydrogen covalent bonds non-polar?
    • A. 

      Hydrogen bonds are non-polar because electrons in the bonds between identical atoms (H-H) are shared uniformly. This means electrons spend equal amounts of time around each atomic center.

    • B. 

      Hydrogen bonds are non-polar because protons in the bonds between identical atoms (H-H) are shared uniformly. This means electrons spend equal amounts of time around each atomic center.

    • C. 

      Hydrogen bonds are non-polar because protons in the bonds between identical atoms (H-H) are not shared uniformly. This means electrons do not spend equal amounts of time around each atomic center.

    • D. 

      Hydrogen bonds are non-polar because protons and electrons in the atom of identical atoms (H-H) are shared uniformly. This means electrons do not spend equal amounts of time around each atomic center.

  • 8. 
    What is an ion?
    • A. 

      An ion is an atom that has been charged due to the loss or gain of electrons.

    • B. 

      An ion is an electronegative charge.

    • C. 

      An ion is a positively or negatively charged atom.

    • D. 

      An ion is a neutral atom.

  • 9. 
    How are covalent and ionic bonds different?
    • A. 

      Covalent bonds share electrons in the valence. Ionic bonds are formed when one atom loses an electron and it becomes a positive ion and the atom that gains the electron becomes a negatively charged ion because it has gained an electron.

    • B. 

      Covalent bonds are formed when one atom loses an electron and it becomes a positive ion and the atom that gains the electron becomes a negatively charged ion because it has gained an electron. Ionic bonds share electrons in the valence.

    • C. 

      Covalent bonds have a neutral electronegativity. Ionic bonds create anions.

    • D. 

      Covalent bonds make new elements. Ionic bonds create cations and anions.

  • 10. 
    Which is the correct explanation for how table salt, Na+Cl-, ionically bonds?
    • A. 

      The strong electron attraction that causes the pairing of a loss and a gain is the ionic bond. Sodium (Na) has 11 electrons with 1 valance electron. Chlorine (Cl) has 17 electrons with 7 in its valence outer orbit. If Sodium looses its valance electron, its next shell will be full (with 8 electrons). That would make Sodium a positive ion. If Chlorine gains that 1 valance electron, its shell would be full with a maximum of 8 electrons, and it would then be a negative ion.

    • B. 

      The uneven electron attraction that causes the pairing of a loss and a gain is the ionic bond. Sodium (Na) has 17 electrons with 7 in its outer orbit. Chlorine has 11 electrons with 1 valance electron. If Sodium gains one electron it fills it’s valance and is a negative ion. If Chlorine looses 1 electron to Sodium, its next shell is full with 8 electrons and it becomes a positive ion.

    • C. 

      The attraction balance of electrons causes ionic bonding. Sodium (Na) has 8 electrons with 6 in its outer orbit. Chlorine has 12 electrons with 2 in its outer orbit. If Sodium gains two electrons it fills it’s valance and is a negative ion. If Chlorine looses 2 electrons to Sodium, it's next shell is full with 8 electrons and becomes a positive ion.

    • D. 

      An ionic bond occurs whenever an atom with s low electronegativity pairs with an atom of a higher electronegativity. Sodium has a strong electronegativity and Chlorine does not, so they can form an ionic bond.

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