PS Exam Review Fall 15-16 Chapter 6,7

1. Typically, atoms gain or lose electrons to achieve

A) an exchange of energy
B) a stable electron configuration
C) vaporization
D) an exchange of energy

2. Often atoms join so that each atom will have

A) an equal number of protons and electrons.
B) an outermost energy level that is full of electrons
C) an even number 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 and valence electrons
B) the nucleus and all non-valence electrons.
C) the nucleus and all electrons.
D) the nucleus.

4. The formation of an ionic bond involves the

A) sharing of electrons.
B) transfer of neutrons.
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) four valence electrons.
C) no protons in its nucleus.
D) two inner energy levels.

6. The forces that hold different atoms or ions together are

A) chemical bonds.
B) physical bonds.
C) nuclear forces.
D) electric currents.

7. An ionic bond is a bond that forms between

A) one atom’s nucleus and another atom’s electrons.
B) atoms with neutral charges
C) the electrons of two different atoms
D) ions with opposite charges

8. In the compound MgCl2, the subscript 2 indicates that

A) there are two magnesium ions for each ion of chlorine
B) magnesium and chlorine form a double covalent bond.
C) the chloride ion is twice the size of the magnesium ion.
D) there are two chloride ions for each magnesium ion.

9. Each molecule of hydrochloric acid, HCl, contains one atom of hydrogen and

A) two atoms of oxygen.
B) two atoms of chlorine
C) one atom of oxygen.
D) one atom of chlorine.

10. Solid ionic compounds have very high melting points because they

A) contain metallic elements
B) are positively charged.
C) contain charged ions that are locked tightly together
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) OO
B) O3
C) NN
D) SO3

12. The elements most likely to form more than one type of ion are the

A) alkaline earth metals
B) halogens.
C) alkali metals.
D) transition metals.

13. Fluorine, F, forms a binary ionic compound with lithium, Li. What is the name of this compound?

A) fluorine lithide
B) lithium fluoride
C) fluorine lithium
D) lithium fluorine

14. The name iron(II) indicates that a compound contains

A) iron ions with a negative charge.
B) two types of iron ions.
C) iron ions with a 2+ charge.
D) iron ions with an 11+ charge.

15. Alkali metals, alkaline earth metals, and aluminum all form ions with positive charges equal to the

A) period
B) group number
C) atomic number
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) 2BeCl
B) Be2Cl
C) BeCl2
D) Be2Cl2

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) a polyatomic ion
C) two oxygen atoms
D) two carbon atoms

18. Metallic bonding is similar to ionic bonding because

A) electrons are shared between atoms
B) there is an attraction between positively charged and negatively charged particles
C) electrons are transferred between atoms
D) the lattice that forms contains anions and cations

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) HCl and NaCl
C) NaOH and HCl
D) NaCl and H2O

20. Which of the following is a balanced chemical equation for the synthesis of NaBr from Na and Br2?

A) 2Na + Br2  NaBr
B) Na + Br2  NaBr
C) 2Na + Br2  2NaBr
D) Na + Br2  2NaBr

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 + O2  H2O + CO2
B) CH4 + 4O  2H2O + CO2
C) CH4 + 2O2  2H2O + CO2
D) CH4 + O  H2O + CO2

22. Which of the following takes place during a redox reaction?

A) Electrons are neither gained nor lost
B) Electrons are gained only
C) Electrons are both gained and lost
D) Electrons are lost only

23. In a chemical reaction, an iron atom became the ion Fe2+. What happened to the iron atom

A) It lost electrons and was reduced.
B) It gained electrons and was reduced.
C) It lost electrons and was oxidized.
D) It gained electrons and was oxidized

24. In a compound, chemical energy is contained in the

A) nuclei of the atoms.
B) movement of the electrons.
C) unbonded electrons.
D) bonds.

25. Which of the following statements is true about what happens during a chemical reaction

A) The bonds of both the reactants and the products are broken.
B) Bonds of the reactants are broken, and bonds of the products are formed.
C) The bonds of both the reactants and the products are formed.
D) Bonds of the reactants are formed, and bonds of the products are broken.

26. In terms of energy, how would you classify the following chemical reaction? 2Cu + O2  2CuO + 315 kJ

A) exothermic
B) endothermic
C) both endothermic and exothermic
D) neither endothermic nor 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) reactant is greater than the chemical energy of the products.
C) products is greater than the chemical energy of the reactant.
D) reaction is conserved.

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