PS Exam Review Fall 15-16 Chapter 6,7

1. Typically, atoms gain or lose electrons to achieve

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

2. Often atoms join so that each atom will have

A) an even number of electrons
B) more electrons than either protons or neutrons.
C) an outermost energy level that is full of electrons
D) an equal number of protons and electrons.

3. In an electron dot diagram, the symbol for an element is used to represent

A) the nucleus.
B) the nucleus and all non-valence electrons.
C) the nucleus and all electrons.
D) the nucleus and valence electrons

4. The formation of an ionic bond involves the

A) sharing of electrons.
B) transfer of electrons.
C) transfer of neutrons.
D) transfer of protons.

5. A carbon atom can bond to four other atoms because it has

A) four valence electrons.
B) four different cations
C) two inner energy levels.
D) no protons in its nucleus.

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

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

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) ions with opposite charges
D) the electrons of two different atoms

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

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

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

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

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) SO3
B) NN
C) OO
D) O3

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) lithium fluorine
D) fluorine lithium

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

A) iron ions with a negative charge.
B) iron ions with an 11+ 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) atomic number
B) period
C) atomic mass
D) group number

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) BeCl2
B) 2BeCl
C) Be2Cl
D) Be2Cl2

17. In the name carbon dioxide, the prefix of the second word indicates that a molecule of carbon dioxide contains

A) two oxygen atoms
B) two carbon atoms
C) an ionic bond
D) a polyatomic ion

18. Metallic bonding is similar to ionic bonding because

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

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 HCl
B) NaOH and H2O
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) 2Na + Br2  NaBr
B) 2Na + Br2  2NaBr
C) Na + Br2  2NaBr
D) Na + 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 + O2  H2O + CO2
B) CH4 + 4O  2H2O + CO2
C) CH4 + O  H2O + CO2
D) CH4 + 2O2  2H2O + CO2

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

A) Electrons are gained only
B) Electrons are both gained and lost
C) Electrons are lost only
D) Electrons are neither gained nor 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 reduced.
B) It lost electrons and was oxidized.
C) It gained electrons and was oxidized
D) It gained electrons and was reduced.

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

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

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

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

A) both endothermic and exothermic
B) exothermic
C) neither endothermic nor exothermic
D) endothermic

27. For the chemical reaction C2H6 + 137 kJ  C2H4 + H2, the chemical energy of the

A) reactant is greater than the chemical energy of the products.
B) reactant and the chemical energy of the products are equal
C) products is greater than the chemical energy of the reactant.
D) reaction is conserved.

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