Chapter 7 Chem: Practice Test
48
Questions
I
By Konlee
Question Excerpt
| 1. | A chemical bond is the attraction between a positive nucleus and negative electrons, or positive and negative ions. True or False? |
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| 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 _______. |
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| 6. | Noble gases have: |
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| 7. | The number of valence electrons can be directly related to the difference in reactivity. |
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| 8. | An Ionic compound with 2 elements, containing one metal cation and one nonmetal anion, is known as: |
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| 9. | Metals are ______, while nonmetals are _______. |
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| 10. | The electrostatic force that holds oppositely charged particles together in an ionic compound is known as: |
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| 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: |
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| 12. | What does conductivity of an ionic compound depend upon? |
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| 13. | Ionic crystals typically have _____ melting and boiling points because of strong, attracted forces. Similarly, ionic crystals are ______ when solid. |
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| 14. | An Ionic compound whose acqueous solution conducts an electric current is known as: |
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| 15. | The energy required to separate one mole of the ions of an ionic compound is: |
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| 16. | The _____ the lattice energy, the stronger the force of the attraction is. |
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| 17. | The smaller the ions are, the ________ the lattice energy is because of interionic attraction due to there being a _____ distance between charges |
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| 18. | A formula unit (chemical formula for an ionic compound) is always ____ in charge. |
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| 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+ |
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| 20. | The charge of a monoatomic ion is equal to the number of electrons transferred from the atom to the ion. This is called: |
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| 21. | An Ion made of more than 1 atom is: |
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| 22. | A(n) _____ is a polyatomic ionic compound composed of an element, usually a nometal, bonded to one or more oxygen atoms. |
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| 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? |
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| 24. | ___________ Ionic compounds always end in "ide." |
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| 25. | What is the name of CsBr? |
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| 26. | Ionic compounds that are liquid conduct electricity because: |
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| 27. | The attraction of a metallic cation for delocalized electrons is known as a(n): |
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| 28. | What is the difference between a substitutional and an interstitial alloy? |
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| 29. | Nonmetals form a stable outer electron configuration by losing electrons and becoming anions. |
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| 30. | A Cl - ion is an example of a cation. |
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| 31. | A sodium atom tends to lose one electron when it reacts. |
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| 32. | Elements in group 1 lose their one valence electron, forming an ion with a 1+ charge. |
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| 33. | A positively charged ion is called an anion. |
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| 34. | Elements tend to react so that they can acquire the electron struture of a noble gas. |
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| 35. | The ending "ide" is used to designate an anion. |
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| 36. | H+ would be called a Hydrogen ion and not hydride. |
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| 37. | N+ would be called nitride and not a nitrogen ion. |
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| 38. | When naming ions, a positive ion would be called [insert element here] anion, while a negative ion would be given the suffix "ide." |
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| 39. | Salts are examples of ionic compounds. |
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| 40. | The crystal lattice of ionic compounds affect their melting and boiling points. |
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| 41. | The lattice energy is the energy required to separate the ions of an ionic compound. |
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| 42. | The energy of an ionic compound is higher than that of the separate elements that formed it. |
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| 43. | Large ions tend to produce a more negative value for lattice energy than smaller ions do. |
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| 44. | Ions that have larger charges tend to produce a more negative lattice energy than ions with smaller charges do. |
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| 45. | Steel is an example of an ____ alloy. |
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| 46. | Why do we "criss-cross"? |
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| 47. | Higher oxidation state = ____ Lattice Energy. |
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| 48. | Ionic compounds are conductive only when a liquid/acqueous. |
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