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Test Review Chapter 6
(Chemical Bonding)
The first page of the test will be matching. Any or all definitions given in the notes or book are fair game.
Any of the questions or type of problems from the home work or book are also fair game for the test.
For sure you should be able to :
1. Correctly assign oxidation numbers
Ex: Work sheet 6-1
2. Find % Ionic Character for any bond and state if the bond is ionic, polar covalent, or non-polar covalent.
Ex: Work sheet 6-2
3. Identify any of the molecular models that you have been shown in class.
Ex: Mr. Sapp will have them set out for you.
4. Sketch any of the molecules from number 3.
Ex: Sketching of molecules we did in class
5. Explain how and why water is polar.
6. Explain why salt crystals are so brittle.
7. Be able to answer any questions from the rest of this review.
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
____ 1. A mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together is called a(n)
a. / dipole. / c. / chemical bond.b. / Lewis structure. / d. / London force.
____ 2. A chemical bond results from the mutual attraction of the nuclei of atoms and
a. / electrons. / c. / neutrons.b. / protons. / d. / dipoles.
____ 3. The electrons involved in the formation of a chemical bond are called
a. / dipoles. / c. / Lewis electrons.b. / s electrons. / d. / valence electrons.
____ 4. The chemical bond formed when two atoms share electrons is called a(n)
a. / ionic bond. / c. / Lewis structure.b. / orbital bond. / d. / covalent bond.
____ 5. If two covalently bonded atoms are identical, the bond is
a. / nonpolar covalent. / c. / nonionic.b. / polar covalent. / d. / coordinate covalent.
____ 6. If the atoms that share electrons have an unequal attraction for the electrons, the bond is called
a. / nonpolar. / c. / ionic.b. / polar. / d. / dipolar.
____ 7. The electrostatic attraction between ____ forms an ionic bond.
a. / ions / c. / electronsb. / dipoles / d. / orbitals
____ 8. A covalent bond results when ____ are shared.
a. / ions / c. / electronsb. / Lewis structures / d. / dipoles
____ 9. The greater the electronegativity difference between two bonded atoms, the greater the percentage of
a. / ionic character. / c. / metallic character.b. / covalent character. / d. / electron sharing.
____ 10. Bonds that are between 5% and 50% ionic are considered
a. / ionic. / c. / polar covalent.b. / pure covalent. / d. / nonpolar covalent.
____ 11. Bonds that are more than 50% ionic are considered
a. / polyatomic. / c. / ionic.b. / polar covalent. / d. / nonpolar covalent.
____ 12. A bond that is less than 5% ionic is considered
a. / polar covalent. / c. / nonpolar covalent.b. / ionic. / d. / metallic.
____ 13. A neutral group of atoms held together by covalent bonds is a
a. / molecular formula. / c. / compound.b. / chemical formula. / d. / molecule.
____ 14. Bond energy is the energy
a. / required to break a chemical bond. / c. / required to form a chemical bond.b. / released when a chemical bond breaks. / d. / absorbed when a chemical bond forms.
____ 15. In a molecule of fluorine, the two shared electrons give each fluorine atom ____ electron(s) in the outer energy level.
a. / 1 / c. / 8b. / 2 / d. / 32
____ 16. In many compounds, atoms of main-group elements form bonds so that the number of electrons in the outermost energy levels of each atom is
a. / 2. / c. / 8.b. / 6. / d. / 10.
____ 17. The octet rule states that chemical compounds tend to form so that each atom has an octet of electrons in
a. / its highest occupied energy level. / c. / its d orbitals.b. / the 1s orbital. / d. / its p orbitals.
____ 18. The electron configuration of nitrogen is 1s2 2s2 2p3. How many more electrons does nitrogen need to satisfy the octet rule?
a. / 1 / c. / 5b. / 3 / d. / 8
____ 19. The elements of the ____ group satisfy the octet rule without forming compounds.
a. / main / c. / alkali metalb. / noble gas / d. / alkaline-earth metal
____ 20. To draw a Lewis structure, one must know the
a. / number of valence electrons in each atom.b. / atomic mass of each atom.
c. / bond length of each atom.
d. / ionization energy of each atom.
____ 21. The Lewis structure for the ammonium ion has
a. / 2 valence electrons. / c. / 8 valence electrons.b. / 4 valence electrons. / d. / 12 valence electrons.
____ 22. Multiple covalent bonds may occur in atoms that contain carbon, nitrogen, or
a. / chlorine. / c. / oxygen.b. / hydrogen. / d. / helium.
____ 23. Bonding in molecules or ions that cannot be correctly represented by a single Lewis structure is
a. / covalent bonding. / c. / single bonding.b. / resonance. / d. / double bonding.
____ 24. In the NaCl crystal, each Na+ and Cl– ion has clustered around it ____ of the oppositely charged ions.
a. / 1 / c. / 4b. / 2 / d. / 6
____ 25. The ions in an ionic compound are organized into a(n)
a. / molecule. / c. / polyatomic ion.b. / Lewis structure. / d. / crystal.
____ 26. Ionic compounds are brittle because the strong attractive forces
a. / allow the layers to shift easily.b. / cause the compound to vaporize easily.
c. / keep the surface dull.
d. / hold the layers in relatively fixed positions.
____ 27. Compared with nonmetals, the number of valence electrons in metals is generally
a. / smaller. / c. / about the same.b. / greater. / d. / almost triple that of nonmetals.
____ 28. If a material can be shaped or extended by physical pressure, such as hammering, which property does the material have?
a. / conductivity / c. / ductilityb. / malleability / d. / luster
____ 29. Shifting the layers of an ionic crystal causes the crystal to
a. / be drawn into a wire. / c. / become metallic.b. / shatter. / d. / freeze.
____ 30. The model for predicting the shape of a molecule that is based on the repulsion of electrons for each other is called
a. / hybridization. / c. / London force model.b. / Lewis structure. / d. / VSEPR theory.
____ 31. The intermolecular attraction between a hydrogen atom bonded to a strongly electronegative atom and the unshared pair of electrons on another strongly electronegative atom is called
a. / electron affinity. / c. / hydrogen bonding.b. / covalent bonding. / d. / electronegativity.
____ 32. The equal but opposite charges present in the two regions of a polar molecule create a(n)
a. / electron sea. / c. / crystal lattice.b. / dipole. / d. / ionic bond.
____ 33. A polar molecule contains
a. / ions.b. / a region of positive charge and a region of negative charge.
c. / only London forces.
d. / no bonds.
____ 34. A molecule of hydrogen chloride is polar because
a. / it is composed of ions.b. / it is magnetic.
c. / it contains metallic bonds.
d. / the chlorine attracts the shared electrons more strongly than does the hydrogen atom.
Short Answer
35. Why do most atoms form chemical bonds?
36. Differentiate between an ionic compound and a molecular compound.