Chapter 7 Chem: Practice Test

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  • 1. 
    A chemical bond is the attraction between a positive nucleus and negative electrons, or positive and negative ions. True or False?
    • A. 

      True

    • B. 

      False


  • 2. 
    A _____  ______ is a force that holds two atoms together.

  • 3. 
    Atoms that acquired a positive or negative charge are called ____.

  • 4. 
    The energy required to lose an electron is known as __________ ______.

  • 5. 
    Electron affinity is the amount of attraction an atom has for _______.
    • A. 

      Cations

    • B. 

      Anions

    • C. 

      Electrons

    • D. 

      Nuclei

    • E. 

      Photons


  • 6. 
    Noble gases have:
    • A. 

      Low ionization energy and high electron affinity

    • B. 

      High ionization energy and low electron affinity

    • C. 

      The same amount of ionization energy as electron affinity


  • 7. 
    The number of valence electrons can be directly related to the difference in reactivity.
    • A. 

      True

    • B. 

      False


  • 8. 
    An Ionic compound with 2 elements, containing one metal cation and one nonmetal anion, is known as:
    • A. 

      Monoatomic Ionic Compound

    • B. 

      Polyatomic Ionic Compound

    • C. 

      Binary Ionic Compound

    • D. 

      Binary Element


  • 9. 
    Metals are ______, while nonmetals are _______.
    • A. 

      Anion, cation

    • B. 

      Brittle, malleable

    • C. 

      Gypsies, thieves

    • D. 

      Cation, anion


  • 10. 
    The electrostatic force that holds oppositely charged particles together in an ionic compound is known as:
    • A. 

      Electromagnetitivity

    • B. 

      A Cation

    • C. 

      Electron Affinity

    • D. 

      Ionic Bond

    • E. 

      Chemical-Covalent Bond


  • 11. 
    Large numbers of positive ions and negative ions exist together in a ratio determined by the number of electrons transferred from the metal atom to the nonmetal atom. These ions are packed in a regular, repeating pattern that balances the forces of attraction and repulsion between the ions. This regular, repeated pattern in a 3-dimensional geometric arrangement is known as:
    • A. 

      The ionic pyramid of charges

    • B. 

      Crystal Lattice

    • C. 

      Electron Affinity Model

    • D. 

      Sea of Electrons Model


  • 12. 
    What does conductivity of an ionic compound depend upon?
    • A. 

      The cardinal charge of the cation

    • B. 

      The cardinal charge of the anion

    • C. 

      Lattice Energy and how it affects the ionic compound

    • D. 

      Whether the ionic compound is a monoatomic compound or a binary compound

    • E. 

      The free-moving ability of electrons


  • 13. 
    Ionic crystals typically have _____ melting and boiling points because of strong, attracted forces. Similarly, ionic crystals are ______ when solid.
    • A. 

      High, nonmalleable

    • B. 

      Low, nonmalleable

    • C. 

      High, malleable

    • D. 

      Low, nonmalleable


  • 14. 
    An Ionic compound whose acqueous solution conducts an electric current is known as:
    • A. 

      Delocalized Ionic Compound

    • B. 

      Polyatomic Ionic Compound

    • C. 

      Binary Ionic Compond

    • D. 

      Electrolyte

    • E. 

      Crystal Lattice


  • 15. 
    The energy required to separate one mole of the ions of an ionic compound is:
    • A. 

      Electron Affinity

    • B. 

      Lattice Energy

    • C. 

      Ionization Energy

    • D. 

      Electromagnetitivity

    • E. 

      Monoatonomy


  • 16. 
    The _____ the lattice energy, the stronger the force of the attraction is.
    • A. 

      Greater

    • B. 

      Lesser


  • 17. 
    The smaller the ions are, the ________ the lattice energy is because of interionic attraction due to there being a _____ distance between charges
    • A. 

      Greater, greater

    • B. 

      Greater, smaller

    • C. 

      Smaller, greater

    • D. 

      Smaller, smaller


  • 18. 
    A formula unit (chemical formula for an ionic compound) is always ____ in charge.
    • A. 

      Positive

    • B. 

      Negative

    • C. 

      Neutral


  • 19. 
    Note: the characters after the " ^ " are meant to be held up in superscript.Is the following a monoatomic, polyatomic, or binary ion? Mg ^ 2+ 
    • A. 

      Monoatomic

    • B. 

      Polyatomic

    • C. 

      Binary


  • 20. 
    The charge of a monoatomic ion is equal to the number of electrons transferred from the atom to the ion. This is called:
    • A. 

      Lattice energy

    • B. 

      Formula unit

    • C. 

      Electrostatic attraction

    • D. 

      Oxidation number


  • 21. 
    An Ion made of more than 1 atom is:
    • A. 

      Monoatomic

    • B. 

      Binary

    • C. 

      Polyatomic


  • 22. 
    A(n) _____ is a polyatomic ionic compound composed of an element, usually a nometal, bonded to one or more oxygen atoms.
    • A. 

      Oxidation state

    • B. 

      Oxyanion

    • C. 

      Oxion

    • D. 

      Oxanion


  • 23. 
    When naming oxyanions, it is likely that you will use "ate" or "ite", like "Nitrate" and "Nitrite."Which of the following statements, knowing this, is true?
    • A. 

      "Ate" will always have a superscript that is 1 greater than "ite".

    • B. 

      "Ite" will always have a superscript that is 1 greater than "ate."

    • C. 

      "Ite" will always have a superscript that is 3 times as that of "ate."


  • 24. 
    ___________ Ionic compounds always end in "ide."
    • A. 

      Monoatomic

    • B. 

      Binary

    • C. 

      Polyatomic


  • 25. 
    What is the name of CsBr?
    • A. 

      Cesium Bromate

    • B. 

      Cesium Bromite

    • C. 

      Celium Bromide

    • D. 

      Cesium Bromide

    • E. 

      Celium Bromite


  • 26. 
    Ionic compounds that are liquid conduct electricity because:
    • A. 

      The difference of the atomic mass between an ion and an atom

    • B. 

      (of) Delocalized electrons

    • C. 

      They are Interstitial alloys

    • D. 

      They are Substitutional alloys


  • 27. 
    The attraction of a metallic cation for delocalized electrons is known as a(n):
    • A. 

      Ionic Bond

    • B. 

      Chemical Bond

    • C. 

      Physical Bond

    • D. 

      Covalent Bond

    • E. 

      Metallic Bond


  • 28. 
    What is the difference between a substitutional and an interstitial alloy?
    • A. 

      Substitutional alloys consist of small holes in a metallic crystal, while interstitial intersect atoms in substitutional alloys.

    • B. 

      Substitutional alloys are replaced by other metals of opposite atomic size, while interstitial alloys intersect the electrons of a substitutional alloy (thus preventing from combining).

    • C. 

      Substitutional alloys are replaced by other metals of similar atomic size, while interstitial alloys have small hols in a metallic crystal that are filled with smaller atoms.

    • D. 

      Substitutional alloys substitute interstitial alloys when the interstitial alloy is not durable enough for the product being manufactured.


  • 29. 
    Nonmetals form a stable outer electron configuration by losing electrons and becoming anions.
    • A. 

      True

    • B. 

      False


  • 30. 
    A Cl - ion is an example of a cation.
    • A. 

      True

    • B. 

      False


  • 31. 
    A sodium atom tends to lose one electron when it reacts.
    • A. 

      True

    • B. 

      False


  • 32. 
    Elements in group 1 lose their one valence electron, forming an ion with a 1+ charge.
    • A. 

      True

    • B. 

      False


  • 33. 
    A positively charged ion is called an anion.
    • A. 

      True

    • B. 

      False


  • 34. 
    Elements tend to react so that they can acquire the electron struture of a noble gas.
    • A. 

      True

    • B. 

      False


  • 35. 
    The ending "ide" is used to designate an anion.
    • A. 

      True

    • B. 

      False


  • 36. 
    H+ would be called a Hydrogen ion and not hydride.
    • A. 

      True

    • B. 

      False


  • 37. 
    N+ would be called nitride and not a nitrogen ion.
    • A. 

      True

    • B. 

      False


  • 38. 
    When naming ions, a positive ion would be called [insert element here] anion, while a negative ion would be given the suffix "ide."
    • A. 

      True

    • B. 

      False


  • 39. 
    Salts are examples of ionic compounds.
    • A. 

      True

    • B. 

      False


  • 40. 
    The crystal lattice of ionic compounds affect their melting and boiling points.
    • A. 

      True

    • B. 

      False


  • 41. 
    The lattice energy is the energy required to separate the ions of an ionic compound.
    • A. 

      True

    • B. 

      False


  • 42. 
    The energy of an ionic compound is higher than that of the separate elements that formed it.
    • A. 

      True

    • B. 

      False


  • 43. 
    Large ions tend to produce a more negative value for lattice energy than smaller ions do.
    • A. 

      True

    • B. 

      False


  • 44. 
    Ions that have larger charges tend to produce a more negative lattice energy than ions with smaller charges do.
    • A. 

      True

    • B. 

      False


  • 45. 
    Steel is an example of an ____ alloy.
    • A. 

      Substitutional

    • B. 

      Interstitial

    • C. 

      Monoatomic


  • 46. 
    Why do we "criss-cross"?
    • A. 

      To get a more negative charge.

    • B. 

      To get a more stable charge.

    • C. 

      To get a more positive charge.


  • 47. 
    Higher oxidation state = ____ Lattice Energy.
    • A. 

      Lower

    • B. 

      Higher


  • 48. 
    Ionic compounds are conductive only when a liquid/acqueous.
    • A. 

      True

    • B. 

      False


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