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PS Exam Review Fall 15-16 Chapter 6,7
  • 1. Typically, atoms gain or lose electrons to achieve
A) vaporization
B) an exchange of energy
C) a stable electron configuration
D) an exchange of energy
  • 2. Often atoms join so that each atom will have
A) an even number of electrons
B) an equal number of protons and electrons.
C) an outermost energy level that is full of electrons
D) more electrons than either protons or neutrons.
  • 3. In an electron dot diagram, the symbol for an element is used to represent
A) the nucleus.
B) the nucleus and valence electrons
C) the nucleus and all non-valence electrons.
D) the nucleus and all electrons.
  • 4. The formation of an ionic bond involves the
A) transfer of neutrons.
B) sharing of electrons.
C) transfer of protons.
D) transfer of electrons.
  • 5. A carbon atom can bond to four other atoms because it has
A) four different cations
B) no protons in its nucleus.
C) two inner energy levels.
D) four valence electrons.
  • 6. The forces that hold different atoms or ions together are
A) chemical bonds.
B) nuclear forces.
C) electric currents.
D) physical bonds.
  • 7. An ionic bond is a bond that forms between
A) the electrons of two different atoms
B) atoms with neutral charges
C) ions with opposite charges
D) one atom’s nucleus and another atom’s electrons.
  • 8. In the compound MgCl2, the subscript 2 indicates that
A) magnesium and chlorine form a double covalent bond.
B) the chloride ion is twice the size of the magnesium ion.
C) there are two magnesium ions for each ion of chlorine
D) there are two chloride ions for each magnesium ion.
  • 9. Each molecule of hydrochloric acid, HCl, contains one atom of hydrogen and
A) one atom of chlorine.
B) two atoms of oxygen.
C) two atoms of chlorine
D) one atom of oxygen.
  • 10. Solid ionic compounds have very high melting points because they
A) contain charged ions that are locked tightly together
B) are positively charged.
C) contain metallic elements
D) are made of elements that are solid at room temperature.
  • 11. Which of the following formulas represents a compound whose molecules contain a triple bond?
A) NN
B) OO
C) O3
D) SO3
  • 12. The elements most likely to form more than one type of ion are the
A) alkali metals.
B) halogens.
C) transition metals.
D) alkaline earth metals
  • 13. Fluorine, F, forms a binary ionic compound with lithium, Li. What is the name of this compound?
A) fluorine lithium
B) lithium fluorine
C) fluorine lithide
D) lithium fluoride
  • 14. The name iron(II) indicates that a compound contains
A) iron ions with an 11+ charge.
B) iron ions with a negative charge.
C) two types of iron ions.
D) iron ions with a 2+ charge.
  • 15. Alkali metals, alkaline earth metals, and aluminum all form ions with positive charges equal to the
A) group number
B) atomic number
C) period
D) atomic mass
  • 16. Beryllium, Be, and chlorine, Cl, form a binary ionic compound with a one-to-two ratio of beryllium ions to chloride ions. The formula for the compound is
A) Be2Cl2
B) 2BeCl
C) BeCl2
D) Be2Cl
  • 17. In the name carbon dioxide, the prefix of the second word indicates that a molecule of carbon dioxide contains
A) an ionic bond
B) two oxygen atoms
C) a polyatomic ion
D) two carbon atoms
  • 18. Metallic bonding is similar to ionic bonding because
A) electrons are transferred between atoms
B) electrons are shared between atoms
C) the lattice that forms contains anions and cations
D) there is an attraction between positively charged and negatively charged particles
  • 19. Hydrochloric acid, HCl, is added to solid NaOH. After the reaction is complete, NaCl dissolved in water remains. What are the products of this chemical reaction?
A) NaOH and H2O
B) NaOH and HCl
C) NaCl and H2O
D) HCl and NaCl
  • 20. Which of the following is a balanced chemical equation for the synthesis of NaBr from Na and Br2?
A) Na + Br2  2NaBr
B) 2Na + Br2  2NaBr
C) Na + Br2  NaBr
D) 2Na + Br2  NaBr
  • 21. Methane, CH4, burns in oxygen gas to form water and carbon dioxide. What is the correct balanced chemical equation for this reaction? (
A) CH4 + 4O  2H2O + CO2
B) CH4 + 2O2  2H2O + CO2
C) CH4 + O  H2O + CO2
D) CH4 + O2  H2O + CO2
  • 22. Which of the following takes place during a redox reaction?
A) Electrons are gained only
B) Electrons are neither gained nor lost
C) Electrons are lost only
D) Electrons are both gained and lost
  • 23. In a chemical reaction, an iron atom became the ion Fe2+. What happened to the iron atom
A) It lost electrons and was oxidized.
B) It gained electrons and was oxidized
C) It lost electrons and was reduced.
D) It gained electrons and was reduced.
  • 24. In a compound, chemical energy is contained in the
A) unbonded electrons.
B) bonds.
C) movement of the electrons.
D) nuclei of the atoms.
  • 25. Which of the following statements is true about what happens during a chemical reaction
A) Bonds of the reactants are formed, and bonds of the products are broken.
B) The bonds of both the reactants and the products are formed.
C) The bonds of both the reactants and the products are broken.
D) Bonds of the reactants are broken, and bonds of the products are formed.
  • 26. In terms of energy, how would you classify the following chemical reaction? 2Cu + O2  2CuO + 315 kJ
A) endothermic
B) neither endothermic nor exothermic
C) both endothermic and exothermic
D) exothermic
  • 27. For the chemical reaction C2H6 + 137 kJ  C2H4 + H2, the chemical energy of the
A) reactant and the chemical energy of the products are equal
B) products is greater than the chemical energy of the reactant.
C) reaction is conserved.
D) reactant is greater than the chemical energy of the products.
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