Chm 1.2. Matter: Properties and Change - Understand the Bonding That Occurs in Simple

Chm 1.2. Matter: Properties and Change - Understand the Bonding that occurs in Simple Compounds in terms of Bond Type, Strength and Properties - Chapter 6 and 7

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

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

____3.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.

____4.If two covalently bonded atoms are identical, the bond is

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

____5.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.

____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.What are shared in a covalent bond?

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

____8.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

____9.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.

____10.In the three molecules, O2, HCl, and F2, what atom would have a partial negative charge?

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

____11.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.

____12.A neutral group of atoms held together by covalent bonds is a

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

____13.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

____14.In a molecule of fluorine, the two shared electrons give each fluorine atom how many electron(s) in the outer energy level?

a. / 1 / c. / 8
b. / 2 / d. / 32

____15.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

____16.What group of elements satisfies the octet rule without forming compounds?

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

____17.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.

____18.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.

____19.After drawing a Lewis structure, one should

a. / determine the number of each type of atom in the molecule.
b. / add unshared pairs of electrons around nonmetal atoms.
c. / confirm that the total number of valence electrons used equals the number available.
d. / determine the electronegativity of each atom.

____20.The substance whose Lewis structure shows three covalent bonds is

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

____21.What is the correct Lewis structure for hydrogen chloride, HCl?

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

____22.The chemical formula for an ionic compound represents the

a. / number of atoms in each molecule.
b. / number of ions in each molecule.
c. / ratio of the combined ions present in a sample.
d. / total number of ions in the crystal lattice.

____23.Compared with ionic compounds, molecular compounds

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

____24.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.

____25.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.

____26.The Lewis structure for the ammonium ion, NH4, has

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

____27.How many extra electrons are in the Lewis structure of the phosphate ion, PO43–?

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

____28.How many electrons must be shown in the Lewis structure of the hydroxide ion, OH–?

a. / 1 / c. / 9
b. / 8 / d. / 10

____29.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.

____30.According to VSEPR theory, an AB2 molecule is

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

____31.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.

____32.The concept that electrostatic repulsion between electron pairs surrounding an atom causes these pairs to be separated as far as possible is the foundation of

a. / VSEPR theory. / c. / the electron-sea model.
b. / the hybridization model. / d. / Lewis theory.

____33.According to VSEPR theory, the shape of an AB3 molecule is

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

____34.According to VSEPR theory, the structure of the ammonia molecule, NH3, is

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

____35.Use VSEPR theory to predict the shape of the hydrogen chloride molecule, HCl.

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

____36.Use VSEPR theory to predict the shape of the carbon tetraiodide molecule, CI4.

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

____37.Use VSEPR theory to predict the shape of the chlorate ion, ClO3–.

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

____38.Use VSEPR theory to predict the shape of carbon dioxide, CO2.

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

____39.The reason the boiling point of water (H2O) is higher than the boiling point of hydrogen sulfide (H2S) is partially explained by

a. / London forces. / c. / ionic bonding.
b. / covalent bonding. / d. / hydrogen bonding.

____40.The following molecules contain polar bonds. The only polar molecule is

a. / CCl4. / c. / NH3.
b. / CO2. / d. / CH4.

____41.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.

____42.What type of compounds might exhibit the following characteristics?

- conducts heat and electricity as a solid

- insoluble

- solid at room temperature

- malleable and ductile

a. / metallic / c. / molecular
b. / ionic / d. / diatomic

____43.What type of compounds might exhibit the following characteristics?

- brittle solid at room temperature

- does not conduct electricity as a solid or in a solution

- lower boiling point and melting point

- soluble in water

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

____44.What type of bond is associated with compounds that have the following characteristics?

- soluble in water

- crystal solid structure at room temperature

- will conduct electricity when dissolved in water

- high boiling point

a. / metallic / c. / molecular
b. / ionic / d. / covalent

____45.The following data was obtained when students measured the melting points and boiling points of metallic, ionic and covalent compounds.

Substance Melting Point (K) Boiling Point (K)

hydrogen gas (H2) 25 70

calcium oxide (CaO) 1,287 1,996

water (H2O) 273 373

Zinc (Zn) 1,544 2,523

Predict which compound may have london dispersion intermolecular forces between molecules.

a. / hydrogen / c. / water
b. / calcium oxide / d. / zinc

____46.Refer to the table in question #45 . Which of the substances is an ionic compound?

a. / hydrogen gas / c. / zinc
b. / calcium oxide / d. / water

____47.Refer the the table in question #45 . Predict which compound may contain the strongest bond or force.

a. / hydrogen / c. / water
b. / calcium oxide / d. / zinc

____48.How many atoms of fluorine are present in a molecule of carbon tetrafluoride, CF4?

a. / 1 / c. / 4
b. / 2 / d. / 5

____49.What is the formula for zinc fluoride?

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

____50.What is the formula for the compound formed by calcium ions and chloride ions?

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

____51.What is the formula for the compound formed by lead(II) ions and chromate ions?

a. / PbCrO4 / c. / Pb2(CrO4)3
b. / Pb2CrO4 / d. / Pb(CrO4)2

____52.What is the formula for aluminum sulfate?

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

____53.What is the formula for barium hydroxide?

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

____54.Name the compound Ni(ClO3)2.

a. / nickel(II) chlorate / c. / nickel(II) chlorite
b. / nickel(II) chloride / d. / nickel(II) peroxide

____55.Name the compound Zn3(PO4)2.

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

____56.Name the compound KClO3.

a. / potassium chloride / c. / potassium chlorate
b. / potassium trioxychlorite / d. / hypochlorite

____57.Name the compound Fe(NO3)2.

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

____58.Name the compound Al2S3.

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

____59.Name the compound CF4.

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

____60.Name the compound SiO2.

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

____61.Name the compound SO3.

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

____62.Name the compound N2O3.

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

____63.What is the formula for silicon dioxide?

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

____64.What is the formula for dinitrogen trioxide?

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

____65.What is the formula for sulfur dichloride?

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

____66.What is the formula for diphosphorus pentoxide?

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

____67.What is the formula for hydrochloric acid?

a. / HF / c. / HClO
b. / HCl / d. / H2CO3

Short Answer

68.Why do most atoms form chemical bonds?

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

Chm 1.2. Matter: Properties and Change - Understand the Bonding that occurs in Simple Compounds in terms of Bond Type, Strength and Properties - Chapter 6 and 7

Answer Section

MULTIPLE CHOICE

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SHORT ANSWER

68.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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69.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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