Chapter 7 Chem: Practice Test

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Practice Test Quizzes & Trivia

Yay, this practice test will determine if you're ready to take the real thing. Questions are taken right out of the book/packet and review lotsa vocab.


Questions and Answers
  • 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

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