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Atoms and Bonding
Chapter 1 Review
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__Atoms and Bonding Review__
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Multiple Choice
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1. When an atom loses an electron, it becomes a
a. positive ion.
b. negative ion.
c. neutral ion.
d. neutral atom.
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2. Ions that are made of more than one atom are examples of
a. polyatomic ions.
b. negative ions.
c. positive ions.
d. neutral ions.
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3. What is the chemical name for the compound with the formula Li2O?
a. sodium fluoride
b. magnesium sulfide
c. lithium oxide
d. sodium sulfide
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4. Which of the following is a characteristic property of ionic compounds?
a. They have low melting points.
b. They have low boiling points.
c. They form hard, brittle crystals with characteristic shapes.
d. They contain no charged particles.
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5. A chemical bond formed when two atoms share electrons is called a(n)
a. ionic bond.
b. covalent bond.
c. polyatomic bond.
d. crystal bond.
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6. What is a triple bond?
a. a bond between three atoms
b. one pair of electrons shared between three atoms
c. two pairs of electrons shared between two atoms
d. three pairs of electrons shared between three atoms
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7. Which is a property shared by most molecular compounds?
a. high boiling point
b. high melting point
c. low melting point
d. nonpolar bonds
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8. Molecular compounds do not conduct electricity because they
a. break up into ions.
b. do not break up into ions.
c. do not dissolve in water.
d. have high melting points.
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9. Molecules that contain two polar bonds are
a. ionic.
b. always polar.
c. always nonpolar.
d. sometimes polar.
____ 10. The smallest particle of an element is called a(n)
a. compound.
b. mixture.
c. atom.
d. molecule.
____ 11. Which of the following terms means that metals can be pulled into thin strands or wires?
a. polar
b. alloy
c. ductile
d. malleable
____ 12. In the chemical formula for an ionic compound, which item is written first?
a. positive ion
b. negative ion
c. subscript
d. charge
____ 13. Which of the following statements is NOT a part of John Dalton’s atomic theory?
a. All elements are composed of atoms that cannot be divided.
b. All atoms of the same element are exactly alike and have the same mass.
c. Electrons move in specific orbits around the nucleus of an atom.
d. Every compound is composed of atoms of different elements, combined in a specific ratio.
____ 14. In Ernest Rutherford’s gold foil experiment, most positively charged particles passed through the foil, but a
few particles were deflected strongly. This result caused Rutherford to infer
a. that electrons move in specific orbits around the nucleus of an atom.
b. that an atom’s positive charge must be clustered in a tiny region in its center, called the nucleus.
c. that electrons have almost no mass.
d. that an atom consists of negative charges scattered throughout a ball of positive charge—something
like raisins or berries in a muffin.
____ 15. What is the greatest number of valence electrons an atom can have?
a. 2
b. 3
c. 8
d. 12
Element
16.
helium
17.
lithium
18.
bromine
19.
radium
Chemical
Symbol
Group
#
Number of
Valence
Electrons
Ion
Charge
Draw Dot
Diagram
20. The series of electron orbits in _______________________ model resemble planets orbiting the sun or the layers
of an onion.
21. Each family in the periodic table has its own characteristic properties based upon its number of
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22. The attraction between a positive ion and a negative ion results in a ___________________________ bond.
23. Orderly crystal shapes, high melting points, and electrical conductivity when dissolved in water are properties of
____________________________________ compounds.
24. Low melting points and lack of electrical conductivity are properties of _____________________compounds.
25. A ____________________________________ is formed when two atoms share two pairs of electrons.
26. A covalent bond in which electrons are shared unequally is called a _________________________________.
27. A ___________________________ is two or more substances—elements, compounds or both—that are in the
same place but are not chemically combined.
28. A ___________________________ is a pure substance made of two or more elements that are combined
chemically in a specific ratio.
29. _____________________________ described an atom that consisted of negative charges scattered throughout a
ball of positive charges.
30. According to ___________________________ model, an atom was mostly empty space and electrons moved
around a small, positively charged nucleus.
31. A _____________________________________ is the force of attraction that holds two atoms together as a
result of the rearrangement of electrons between them.
32. Ions that are made of more than one atom are called __________________________________.
33. A covalent bond in which electrons are shared equally is a __________________________________.
34. A ___________________________________ is a neutral group of atoms joined by covalent bonds
Ions
35.
Ca2+ N3-
36.
K+ Cl-
37.
Al3+ O2-
38.
Be2+ I-
Ionic Compound
Name of Binary Compound
39. Explain how a bond forms between sodium and chlorine in sodium chloride (NaCl).
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40. Compare a covalent bond and an ionic bond. Give an example of both.
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41. Describe properties that would help you to distinguish an ionic compound from a molecular compound.
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42. Distinguish among elements, compounds, and mixtures. Give examples of each.
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