Practice Test for Test #4: Bonding

Practice Test for Test #4: Bonding

Multiple Choice

Identify 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.The electrons involved in the formation of a chemical bond are called

a. / dipoles. / c. / Lewis electrons.
b. / s electrons. / d. / valence electrons.

____3.The electrostatic attraction between positively charged nuclei and negatively charged electrons permits two atoms to be held together by a(n)

a. / chemical bond. / c. / neutron.
b. / London force. / d. / ion.

____4.Atoms naturally move

a. / toward high potential energy. / c. / toward less stability.
b. / toward low potential energy. / d. / away from each other.

____5.As atoms bond with each other, they

a. / increase their potential energy, thus creating less-stable arrangements of matter.
b. / decrease their potential energy, thus creating less-stable arrangements of matter.
c. / increase their potential energy, thus creating more-stable arrangements of matter.
d. / decrease their potential energy, thus creating more-stable arrangements of matter.

____6.If two covalently bonded atoms are identical, the bond is

a. / nonpolar covalent. / c. / dipole covalent.
b. / polar covalent. / d. / coordinate covalent.

____7.When atoms share electrons, the electrical attraction of an atom for the shared electrons is called the atom's

a. / electron affinity. / c. / resonance.
b. / electronegativity. / d. / hybridization.

____8.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.

____9.What are shared in a covalent bond?

a. / ions / c. / electrons
b. / Lewis structures / d. / dipoles

____10.Most chemical bonds are

a. / purely ionic. / c. / partly ionic and partly covalent.
b. / purely covalent. / d. / metallic.

____11.Nonpolar covalent bonds are not common because

a. / one atom usually attracts electrons more strongly than the other.
b. / ions always form when atoms join.
c. / the electrons usually remain equally distant from both atoms.
d. / dipoles are rare in nature.

____12.The greater the electronegativity difference between two bonded atoms, the greater the percentage of ____ in the bond.

a. / ionic character / c. / metallic character
b. / covalent character / d. / electron sharing

____13.The pair of elements that forms a bond with the least ionic character is

a. / Na and Cl. / c. / O and Cl.
b. / K and Cl. / d. / Mg and Cl.

____14.The B—F bond in BF3 (electronegativity for B is 2.0; electronegativity for F is 4.0) is

a. / polar covalent. / c. / nonpolar covalent.
b. / ionic. / d. / metallic.

____15.In the three molecules, O2, HCl, and F2, what atom would have a partial negative charge?

a. / oxygen / c. / chlorine
b. / hydrogen / d. / fluorine

____16.The percentage ionic character and the type of bond in Br2 (electronegativity for Br is 2.8) is

a. / 0%; nonpolar covalent. / c. / 0%; pure ionic.
b. / 100%; polar covalent. / d. / 100%; pure ionic.

____17.A neutral group of atoms held together by covalent bonds is a

a. / molecular formula. / c. / polyatomic ion.
b. / chemical formula. / d. / molecule.

____18.Which of the following shows the types and numbers of atoms joined in a single molecule of a molecular compound?

a. / molecular formula / c. / covalent bond
b. / potential energy diagram / d. / ionic bond

____19.Which of the following is not an example of a molecular formula?

a. / H2O / c. / NH3
b. / B / d. / O2

____20.When a stable covalent bond forms, the potential energy of the atoms

a. / increases. / c. / remains constant.
b. / decreases. / d. / becomes zero.

____21.The electron configuration of nitrogen is 1s2 2s2 2p3. How many more electrons does nitrogen need to satisfy the octet rule?

a. / 1 / c. / 5
b. / 3 / d. / 8

____22.What group of elements satisfies the octet rule without forming compounds?

a. / halogen / c. / alkali metal
b. / noble gas / d. / alkaline-earth metal

____23.In drawing a Lewis structure, each nonmetal atom except hydrogen should be surrounded by

a. / 2 electrons. / c. / 8 electrons.
b. / 4 electrons. / d. / 10 electrons.

____24.In drawing a Lewis structure, the central atom is generally the

a. / atom with the greatest mass.
b. / atom with the highest atomic number.
c. / atom with the fewest electrons.
d. / least electronegative atom.

____25.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.

____26.The substance whose Lewis structure shows three covalent bonds is

a. / H2O. / c. / NH3.
b. / CH2Cl2. / d. / CCl4.

____27.What is the correct Lewis structure for hydrogen chloride, HCl?

a. / A / c. / C
b. / B / d. / D

____28.Bonding in molecules or ions that cannot be correctly represented by a single Lewis structure is

a. / polyatomic. / c. / single bonding.
b. / resonance. / d. / double bonding.

____29.What is placed between a molecule's resonance structures to indicate resonance?

a. / double-headed arrow / c. / series of dots
b. / single-headed arrow / d. / Lewis structure

____30.In an ionic compound, the orderly arrangement of ions in a crystal is the state of

a. / maximum potential energy. / c. / average potential energy.
b. / minimum potential energy. / d. / zero potential energy.

____31.The ions in most ionic compounds are organized into a

a. / molecule. / c. / polyatomic ion.
b. / Lewis structure. / d. / crystal.

____32.Compared with energies of neutral atoms, a crystal lattice has

a. / higher potential energy. / c. / equal potential energy.
b. / lower potential energy. / d. / less stability.

____33.Compared with ionic compounds, molecular compounds

a. / have higher boiling points. / c. / have lower melting points.
b. / are brittle. / d. / are harder.

____34.The forces of attraction between molecules in a molecular compound are

a. / stronger than the forces among formula units in ionic bonding.
b. / weaker than the forces among formula units in ionic bonding.
c. / approximately equal to the forces among formula units in ionic bonding.
d. / zero.

____35.The properties of both ionic and molecular compounds are related to the

a. / lattice energies of the compounds.
b. / strengths of attraction between the particles in the compounds.
c. / number of covalent bonds each contains.
d. / mobile electrons that they contain.

____36.How many extra electrons are in the Lewis structure of the phosphate ion, PO43–?

a. / 0 / c. / 3
b. / 2 / d. / 4

____37.A chemical bond formed by the attraction between positive ions and surrounding mobile electrons is a(n)

a. / nonpolar covalent bond. / c. / polar covalent bond.
b. / ionic bond. / d. / metallic bond.

____38.In metallic bonds, the mobile electrons surrounding the positive ions are called a(n)

a. / Lewis structure. / c. / electron cloud.
b. / electron sea. / d. / dipole.

____39.Metals are malleable because the metallic bonding

a. / holds the layers of ions in rigid positions.
b. / maximizes the repulsive forces within the metal.
c. / allows one plane of ions to slide past another.
d. / is easily broken.

____40.VSEPR theory is a model for predicting

a. / the strength of metallic bonds. / c. / lattice energy values.
b. / the shape of molecules. / d. / ionization energy.

____41.According to VSEPR theory, the structure of the ammonia molecule, NH3, is

a. / trigonal-planar. / c. / trigonal-pyramidal.
b. / bent. / d. / tetrahedral.

____42.Use VSEPR theory to predict the shape of the carbon tetraiodide molecule, CI4.

a. / tetrahedral / c. / bent
b. / linear / d. / trigonal-planar

____43.Use VSEPR theory to predict the shape of carbon dioxide, CO2.

a. / tetrahedral / c. / bent
b. / linear / d. / octahedral

____44.A chemical formula includes the symbols of the elements in the compound and subscripts that indicate

a. / atomic mass of each element.
b. / number of atoms or ions of each element that are combined in the compound.
c. / formula mass.
d. / charges on the elements or ions.

____45.A chemical formula for a molecular compound represents the composition of

a. / a molecule. / c. / the ions that make up the compound.
b. / an atom. / d. / the crystal lattice.

____46.What is the formula for zinc fluoride?

a. / ZnF / c. / Zn2F
b. / ZnF2 / d. / Zn2F3

____47.What is the formula for the compound formed by calcium ions and chloride ions?

a. / CaCl / c. / CaCl3
b. / Ca2Cl / d. / CaCl2

____48.What is the formula for aluminum sulfate?

a. / AlSO4 / c. / Al2(SO4)3
b. / Al2SO4 / d. / Al(SO4)3

____49.What is the formula for barium hydroxide?

a. / BaOH / c. / Ba(OH)2
b. / BaOH2 / d. / Ba(OH)

____50.Name the compound Zn3(PO4)2.

a. / zinc potassium oxide / c. / zinc phosphate
b. / trizinc polyoxide / d. / zinc phosphite

____51.Name the compound Fe(NO3)2.

a. / iron(II) nitrate / c. / iron(III) nitrate
b. / iron(II) nitrite / d. / iron(III) nitride

____52.Name the compound Al2S3.

a. / aluminum sulfate / c. / aluminum(II) sulfate
b. / aluminum sulfur / d. / aluminum sulfide

____53.Name the compound CF4.

a. / calcium fluoride / c. / carbon tetrafluoride
b. / carbon fluoride / d. / monocalcium quadrafluoride

____54.Name the compound SiO2.

a. / silver oxide / c. / silicon dioxide
b. / silicon oxide / d. / monosilver dioxide

____55.Name the compound SO3.

a. / sulfur trioxide / c. / selenium trioxide
b. / silver trioxide / d. / sodium trioxide

____56.Name the compound N2O3.

a. / dinitrogen oxide / c. / nitric oxide
b. / nitrogen trioxide / d. / dinitrogen trioxide

____57.What is the formula for silicon dioxide?

a. / SO2 / c. / Si2O
b. / SiO2 / d. / S2O

____58.What is the formula for dinitrogen trioxide?

a. / Ni2O3 / c. / N2O6
b. / NO3 / d. / N2O3

____59.What is the formula for sulfur dichloride?

a. / SCl / c. / S2Cl
b. / SCl2 / d. / S2Cl2

____60.What is the formula for diphosphorus pentoxide?

a. / P2PeO5 / c. / P2O4
b. / PO5 / d. / P2O5

Short Answer

61.Why do most atoms form chemical bonds?

62.Differentiate between an ionic compound and a molecular compound.

63.Explain why metals are good conductors of electricity.

Problem

64.Draw a Lewis structure for the oxalate ion, C2O42–.

65.Draw a Lewis structure for carbon disulfide, CS2.

66.Draw a Lewis structure for the nitrate ion, . Use VSEPR theory to predict its molecular geometry.

67.Draw a ball-and-stick model of a water molecule. Label the atoms, include the polarities of the bonds using dipole vectors, and indicate molecular polarity.

Completion

Complete each statement.

68.The name and formula for the compound formed by strontium ions and sulfite ions are ______.

69.The Stock name for the compound P2O5 is ______.

Practice Test for Test #4: Bonding

Answer Section

MULTIPLE CHOICE

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SHORT ANSWER

61.ANS:

Atoms form chemical bonds to establish a more-stable arrangement. As independent particles, they are at high potential energy. By bonding, they decrease their potential energy, thus becoming more stable.

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62.ANS:

Atoms in a molecular compound share electrons to achieve stability. Atoms in an ionic compound gain or lose electrons to form ions, which combine so that the number of positive and negative charges is equal.

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63.ANS:

The valence electrons in a metal's structure are delocalized, so they can move freely and carry an electric charge throughout the metal.

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PROBLEM

64.ANS:

PTS:1DIF:IIIREF:3OBJ:5

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65.ANS:

PTS:1DIF:IIIREF:3OBJ:5

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66.ANS:

trigonal-planar

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67.ANS:

Polar molecule

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COMPLETION

68.ANS:strontium sulfite, SrSO3

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69.ANS:phosphorus(V) oxide

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