Chem Test Prep Ch 8-13

A gas is __________ and assumes __________ of its container whereas a liquid is __________ and assumes __________ of its container. A) compressible, the shape, not compressible, the volume and shape B) compressible, the volume and shape, not compressible, the shape of a portion C) compressible, the volume and shape, compressible, the volume D) condensed, the volume and shape, condensed, the volume and shape E) condensed, the shape, compressible, the volume and shape

A

An alloy is a...... A) metallic material that is composed of two or more elements. B) pure metal. C) heterogeneous mixture of two metals. D) nonmetal with some properties of a metal. E) a mineral containing two or more metals

A

Calculate the mole fraction of phosphoric acid (H3PO4) in a 25.4% (by mass) aqueous solution. A) 0.0589 B) 0.0626 C) 0.259 D) 1.00 E) 4.14

A

Crystalline solids __________. A) have highly ordered structures B) have their particles arranged randomly C) are usually very soft D) exist only at high temperatures E) exist only at very low temperatures

A

For a given arrangement of ions, the lattice energy increases as ionic radius __________ and as ionic charge __________. A) decreases, increases B) increases, decreases C) increases, increases D) decreases, decreases E) This cannot be predicted

A

Given that the average bond energies for C-H and CBr bonds are 413 and 276 kJ/mol, respectively, the heat of atomization of bromoform (CHBr3) is__________ kJ/mol. A) 1241 B) 689 C) -689 D) 1378 E) -1378

A

If the electronic structure of a solid substance consists of a valence band that is completely filled with electrons and there is a large energy gap to the next set of orbitals, then this substance will be a(n) __________. A) insulator B) alloy C) conductor D) semiconductor E) nonmetal

A

In the generation of most anions, the energy change {kJ/mol} that ______ and electron is ________. A) adds, negative B) removes, negative C) adds, positive D) removes, positive E) none of the above

A

Of the following substances, only __________ has London dispersion forces as its only intermolecular force. A) CH4 B) NH3 C) H2S D) CH3OH E) HCl

A

Sodium bicarbonate is reacted with concentrated hydrochloric acid at 37.0°C and 1.00 atm. The reaction of 6.00 kg of bicarbonate with excess hydrochloric acid under these conditions will produce __________ L of CO2. A) 1.82 × 10^3 B) 8.70 × 10^2 C) 2.85 × 10^4 D) 1.09 × 10^2 E) 1.82 × 10^4

A

The Lewis structure of carbon dioxide is given below. The hybridization of the carbon atom in carbon dioxide is __________. A) sp B) sp2d C) sp2d2 D) sp3 E) sp2

A

The density of __________ is 0.900 g/L at STP. A) Ne B) CO C) NO D) CH4 E) N2

A

The electron domain and molecular geometry of BrO2- is __________. A) tetrahedral, bent B) trigonal planar, trigonal planar C) trigonal pyramidal, seesaw D) tetrahedral, trigonal planar E) trigonal pyramidal, linear

A

The phase diagram of a substance is given above. The region that corresponds to the solid phase is ____. A) w B) x C) y D) z E) x and y

A

The type of compound that is most likely to contain a covalent bond is __________. A) one that is composed of only nonmetals B) held together by the electrostatic forces between oppositely charged ions C) a solid metal D) There is no general rule to predict covalency in bonds. E) one that is composed of a metal from the far left of the periodic table and a nonmetal from the far right of the periodic table

A

Which ion below has a noble gas electron configuration? A) Be +2 B) B +2 C) Li +2 D) C +2 E) N -2

A

Which of the following does not have eight valence electrons? A) Ca+ B) Rb+ C) Xe D) Br E) All of the above have eight valence electrons

A

Which of the following statements about gases is false? A) All gases are colorless and odorless at room temperature. B) Distances between molecules of gas are very large compared to bond distances within molecules. C) Non-reacting gas mixtures are homogeneous. D) Gases expand spontaneously to fill the container they are placed in. E) Gases are highly compressible.

A

Which property of metals cannot be explained with the electron-sea model? A) trends in melting points B) high thermal conductivity C) high electric conductivity D) malleability and ductility E) shine

A

Why don't we draw double bonds between the Be atom and the Cl atoms in BeCl2? A) That would give positive formal charges to the chlorine atoms and a negative formal charge to the beryllium atom. B) There aren't enough electrons. C) That would result in more than eight electrons around beryllium. D) That would result in more than eight electrons around each chlorine atom. E) That would result in the formal charges not adding upto zero.

A

A saturated solution __________. A) will rapidly precipitate if a seed crystal is added B) contains dissolved solute in equilibrium with undissolved solute C) cannot be attained D) contains no double bonds E) contains as much solvent as it can hold

B

A valid Lewis structure of __________ cannot be drawn without violating the octet rule. A) NF3 B) IF3 C) PF3 D) SbF3 E) SO4 2-

B

According to MO theory, overlap of two p atomic orbitals produces __________. A) two bonding molecular orbitals B) one bonding molecular orbital and one antibonding molecular orbital C) two bonding molecular orbitals and two antibonding molecular orbitals D) two bonding molecular orbitals and one antibonding molecular orbital E) three bonding molecular orbitals and three antibonding molecular orbitals

B

As a solid element melts, the atoms become __________ and they have __________ attraction for one another. A) more separated, more B) more separated, less C) closer together, more D) closer together, less E) larger, greater

B

Automobile air bags use the decomposition of sodium azide as their source of gas for rapid inflation: 2NaN3(s) → 2Na (s) + 3N2 (g). What mass (g) of NaN3 is required to provide 40.0 L of N2 at 25.0°C and 763 torr? A) 71.1 B) 1.64 C) 1.09 D) 107 E) 17.1

B

Heat of sublimation can be approximated by adding together __________ and __________. A) heat of fusion, heat of condensation B) heat of fusion, heat of vaporization C) heat of freezing (solidification), heat of condensation D) heat of freezing (solidification), heat of vaporization E) heat of deposition, heat of vaporization

B

How many moles of gas are there in a 45.0 L container at 25.0°C and 500.0 mm Hg? A) 207 B) 1.21 C) 6.11 D) 18.4 E) 0.630

B

In comparing the same two atoms bonded together, the _______ the bond order, the _ ______ the bond length, and the __________ the bond energy. A) greater, longer, greater B) smaller, longer, smaller C) smaller, greater, greater D) greater, shorter, greater E) greater, greater, greater

B

In general, the vapor pressure of a substance increases as __________ increases. A) surface tension B) temperature C) molecular weight D) hydrogen bonding E) viscosity

B

Of the following gases, __________ will have the greatest rate of effusion at a given temperature. A) NH3 B) CH4 C) Ar D) HBr E) HCl

B

The molecular geometry of the BeCl2 molecule is __________, and this molecule is __________. A) linear, polar B) linear, nonpolar C) bent, nonpolar D) bent, polar E) trigonal planar, polar

B

The phrase "like dissolves like" refers to the fact that __________. A) gases can only dissolve other gases B) polar solvents dissolve polar solutes and nonpolar solvents dissolve nonpolar solutes C) solvents can only dissolve solutes of similar molar mass D) condensed phases can only dissolve other condensed phases E) polar solvents dissolve nonpolar solutes and vice versa

B

There are __________ valence electrons in the Lewis structure of CH3OCH2CH3. A) 32 B) 26 C) 18 D) 36 E) 20

B

What species has the electron configuration [Ar]3d4? A) Mn +2 B) Cr +2 C) V +3 D) Fe +3 E) K+

B

Which of the following has the bonds correctly arranged in order of increasing polarity? A) Be--F, Mg--F, N--F, O--F B) O--F, N--F, Be--F, Mg--F C) O--F, Be--F, Mg--F, N--F D) N--F, Be--F, Mg--F, O--F E) Mg--F, Be--F, N--F, O--F

B

__________ is the energy required to expand the surface area of a liquid by a unit amount of area. A) Viscosity B) Surface tension C) Volatility D) Meniscus E) Capillary action

B

The formal charge of phosphorus in PF3 is __________. A) -2 B) +1 C) +3 D) 0 E) -3

D

10.0 grams of argon and 20.0 grams of neon are placed in a 1200.0 ml container at 25.0°C. The partial pressure of neon is __________ atm. A) 3.40 B) 5.60 C) 20.4 D) 8.70 E) 0.700

C

The molar volume of a gas at STP is __________ L. A) 0.08206 B) 62.36 C) 1.00 D) 22.4 E) 14.7

D

A sample of a gas (5.0 mol) at 1.0 atm is expanded at constant temperature from 10 L to 15 L. The final pressure is __________ atm. A) 1.5 B) 7.5 C) 0.67 D) 3.3 E) 15

C

A solid has a very high melting point, great hardness, and poor electrical conduction. This is a(n) __________ solid. A) ionic B) covalent network C) metallic D) molecular E) metallic and covalent network

C

A solution is prepared by dissolving calcium chloride in water and diluting to 500.0 mL If this solution contains 44 ppm chloride ions, the concentration of calcium ions is __________ ppm. A) 44 B) 88 C) 22 D) 11 E) 500

C

As a gaseous element condenses, the atoms become __________ and they have __________ attraction for one another. A) more separated, more B) more separated, less C) closer together, more D) closer together, less E) larger, greater

C

In the nitrite ion (NO2-), __________. A) both bonds are double bonds B) one bond is a double bond and the other is a single bond C) both bonds are the same D) there are 20 valence electrons E) both bonds are single bonds

C

Inorganic compounds that are semiconductors have an average of __________ valence electrons. A) 2 B) 1 C) 4 D) 3 E) 5

C

Lattice energy is _________. A) the sum of electron affinities of the components in an ionic solid B) the energy required to produce one mole of an ionic compound from its constituent elements in their standard states C) the energy required to convert a mole of ionic solid into its constituent ions in the gas phase D) the sum of ionization energies of the components in an ionic solid E) the energy given off when gaseous ions combine to form one mole of an ionic solid

C

Of the bonds C-C, C=C, and C≡C, the C-C bond is __________. A) strongest/shortest B) strongest/longest C) weakest/longest D) weakest/shortest E) intermediate in both strength and length

C

Of the following elements, ________ has the most negative electron affinity. A) Li B) Na C) F D) N E) Be

C

Of the molecules below, only _______ is polar. A) I2 B) CH4 C) AsH3 D) SbF5 E) Sf6

C

Of the molecules below, the bond in _________ is the most polar. A) F2 B) HBr C) HF D) HCl E) H2

C

The O-C-O bond angle in the CO3 2- ion is approximately __________. A) 60° B) 90° C) 120° D) 109.5° E) 180°

C

The carbon-carbon σ bond in ethylene, H2C=CH2, results from the overlap of __________. A) sp hybrid orbitals B) sp3 hybrid orbitals C) sp2 hybrid orbitals D) s atomic orbitals E) p atomic orbitals

C

The electron configuration [Kr]4d^10 represents____. A) Sr+2 B) Sn+2 C) Ag+1 D) Te+2 E) Rb+1

C

The formal charge on nitrogen in NO3- is __________. A) -1 B) 0 C) +1 D) +2 E) -2

C

The halogens, alkali metals, and alkaline earth metals have _______ valence electrons, respectively. A) 2, 7, and 4 B) 7, 4, and 6 C) 7, 1, and 2 D) 1, 5, and 7 E) 8, 2, and 3

C

The kinetic-molecular theory predicts that pressure rises as the temperature of a gas increases because __________. A) the gas molecules collide less frequently with the wall B) the gas molecules collide more energetically with the wall C) both the gas molecules collide more frequently with the wall and the gas molecules collide more energetically with the wall D) the average kinetic energy of the gas molecules decreases E) the gas molecules collide more frequently with the wall

C

The molecular-orbital model for Ge shows it to be A) a conductor, because all the lower energy band orbitals are filled and the gap between the lower and higher bands is large. B) an insulator, because all the lower energy band orbitals are filled and the gap between the lower and higher bands is large. C) a semiconductor, because the gap between the filled lower and empty higher energy bands is relatively small. D) a semiconductor, because the gap between the filled lower and empty higher energy bands is large. E) a conductor, because its lower energy band orbitals are only partially filled.

C

The oxidation number of phosphorus in PF3 is _____. A) -2 B) +1 C) +3 D) +2 E) -3

C

To convert from one resonance structure to another, __________. A) only atoms can be moved B) electrons and atoms can both be moved C) only electrons can be moved D) neither electrons nor atoms can be moved E) electrons must be added

C

Using the Born-Haber cycle, the ΔHf° of KBr is equal to __________. A) ΔHf°[K (g)] - ΔHf°[Br (g)] - Il(K) - E(Br) - ΔHlattice B) ΔHf°[K (g)] + ΔHf°[Br (g)] - Il- E(Br) + ΔHlattice C) ΔHf°[K (g)] + ΔHf°[Br (g)] + Il(K) + E(Br) - ΔHlattice D) ΔHf°[K (g)] + ΔHf°[Br (g)] + Il(K) + E(Br) + ΔHlattice E) ΔHf°[K (g)] - ΔHf°[Br (g)] + Il(K) - E(Br) + ΔHlattice

C

Using the table of bond dissociation energies, the ΔH for the following reaction is __________ kJ. 2HCl (g) + F2(g) → 2HF (g) + Cl2(g) A) -359 B) -223 C) 359 D) 223 E) 208

C

Which statement about atmospheric pressure is false? A) As air becomes thinner, its density decreases. B) Air actually has weight. C) With an increase in altitude, atmospheric pressure increases as well. D) The warmer the air, the lower the atmospheric pressure. E) Atmospheric pressure prevents water in lakes, rivers, and oceans from boiling away.

C

Which statements about viscosity are true? (i) Viscosity increases as temperature decreases. (ii) Viscosity increases as molecular weight increases. (iii)Viscosity increases as intermolecular forces increase. A) (i) only B) (ii) and (iii) C) (i) and (iii) D) none E) all

C

A valid Lewis structure of __________ cannot be drawn without violating the octet rule. A) PO4 -3 B) SiF4 C) CF4 D) SeF4 E) NF3

D

Arrange the following gases in order of increasing average molecular speed at 25°C. He, O2, CO2, N2 A) He < N2< O2< CO2 B) He < O2< N2< CO2 C) CO2< N2< O2< He D) CO2< O2< N2< He E) CO2< He < N2< O2

D

If 50.75 g of a gas occupies 10.0 L at STP, 129.3 g of the gas will occupy __________ L at STP. A) 3.92 B) 50.8 C) 12.9 D) 25.5 E) 5.08

D

In ionic bond formation, the lattice energy of ions_______ as the magnitude of the ion charges________and the radii_______. A) decreases, increase, increase B) increases, decrease, decrease C) increases, decrease, increase D) increases, increase, decrease E) increases, increase, increase

D

Molecular Orbital theory correctly predicts paramagnetism of oxygen gas, O2. This is because __________. A) the bond order in O2 can be shown to be equal to 2. B) there are more electrons in the bonding orbitals than in the antibonding orbitals. C) the energy of the π2p MOs is higher than that of the σ2p MO D) there are two unpaired electrons in the MO electron configuration of O2 E) the O=O bond distance is relatively short

D

Molecular compounds of low molecular weight tend to be gases at room temperature. Which of the following is most likely not a gas at room temperature? A) CH4 B) H2 C) HCl D) LiCl E) Cl2

D

Of the molecules below, only ______ is nonpolar. A)TeCl2 B) H2O C) NH3 D) HCl E) CO2

D

On a phase diagram, the critical pressure is _____. A) the pressure required to melt a solid B) the pressure below which a substance is a solid at all temperatures C) the pressure above which a substance is a liquid at all temperatures D) the pressure at which a liquid changes to a gas E) the pressure required to liquefy a gas at its critical temperature

D

One significant difference between gases and liquids is that __________. A) a gas may consist of both elements and compounds B) gases are always mixtures C) a gas is made up of molecules D) a gas assumes the volume of its container E) All of the above answers are correct.

D

The Lewis structure of N2H2 shows __________. A) each nitrogen has two nonbonding electron pairs B) a nitrogen-nitrogen triple bond C) each nitrogen has one nonbonding electron pair D) each hydrogen has one nonbonding electron pair E) a nitrogen-nitrogen single bond

D

The central atom in __________ violates the octet rule. A) NH3 B) SeF2 C) AsF3 D) BF3 E) CF4

D

The class of semiconductors, known as elemental, has special features. These are __________. A) band gap and individual element valence electrons B) overlapping hybrid orbitals and filed conduction bands C) tetrahedral coordination geometry and sp2 hybrid orbitals D) periodical table grouping and diamond crystal structure E) none of the above

D

The electron configuration of the S2-ion is __________. A) [Ar]3s2 3P6 B) [Ar]3s2 3P2 C) [Ne]3s2 3P2 D) [Ne]3s2 3P6 E) [Kr]3s23P-6

D

The process of doping can produce a __________ which can greatly __________ intrinsic conductivity. A) non-metal, decrease B) p-type semiconductor, decrease C) non-metal, increase D) n-type semiconductor, increase E) allotrope, diminish

D

The volume of a sample of gas (2.49 g) was 752 mL at 1.98 atm and 62°C. The gas is __________. A) NH3 B) SO2 C) SO3 D) NO2 E) Ne

D

Which of the following would have to gain two electrons in order to achieve a noble gas electron configuration? A) Br B) Sr C) Na D) O, Se E) Sr, O, Se

D

Why don't we draw double bonds between the B atom and the Cl atoms in BCl3? A) That would result in more than eight electrons around each chlorine atom. B) That would result in the formal charges not adding up to zero. C) There aren't enough electrons. D) That would result in more than eight electrons around boron. E) That would give positive formal charges to the chlorine atoms and a negative formal charge to the boron atom.

D

A solution contains 28% phosphoric acid by mass. This means that __________. A) 1 mL of this solution contains 28 g of phosphoric acid B) 1 L of this solution has a mass of 28 g C) 1 L of this solution contains 28 mL of phosphoric acid D) the density of this solution is 2.8 g/mL E) 100 g of this solution contains 28 g of phosphoric acid

E

According to MO theory, overlap of two s atomic orbitals produces __________. A) one bonding molecular orbital and one hybrid orbital B) two bonding molecular orbitals C) two bonding molecular orbitals and two antibonding molecular orbitals D) two bonding molecular orbitals and one antibonding molecular orbital E) one bonding molecular orbital and one antibonding molecular orbital

E

As the number of covalent bonds between two atoms increases, the distance between the atoms __________ and the strength of the bond between them __________. A) increases, decreases B) decreases, decreases C) is unpredictable D) increases, increases E) decreases, increases

E

ClF3 has "T-shaped" geometry. There are __________ non-bonding domains in this molecule. A) 3 B) 4 C) 0 D) 1 E) 2

E

Electropositivity __________ from left to right within a period and __________ from top to bottom within a group. A) increases, stays the same B) stays the same, increases C) increases, decreases D) increases, increases E) decreases, increases

E

Sodium hydride reacts with excess water to produce aqueous sodium hydroxide and hydrogen gas: NaH (s) + H2O (l) → NaOH (aq) + H2(g) A sample of NaH weighing __________ g will produce 982 mL of gas at 28.0°C and 765 torr, when the hydrogen is collected over water. The vapor pressure of water at this temperature is 28 torr. A) 2.93 B) 0.960 C) 925 D) 0.0388 E) 0.925

E

The Lewis structure of PF3 shows that the central phosphorus atom has __________ nonbonding and __________ bonding electron pairs. A) 3, 1 B) 1, 2 C) 2, 2 D) 3, 3 E) 1, 3

E

The combination of two atomic orbitals results in the formation of __________ molecular orbitals. A) 3 B) 4 C) 0 D) 1 E) 2

E

The critical temperature and pressure of CS2 are 279°C and 78 atm, respectively. At temperatures above 279°C and pressures above 78 atm, CS2 can only occur as a __________. A) solid B) liquid C) liquid and gas D) gas E) supercritical fluid

E

The ion ICl4- has __________ valence electrons A) 35 B) 34 C) 28 D) 8 E) 36

E

The ion NO- has __________ valence electrons A) 15 B) 14 C) 16 D) 10 E) 12

E

The ion PO4 3- has __________ valence electrons. A) 14 B) 24 C) 27 D) 29 E) 32

E

The more effectively two atomic orbitals overlap, ___. A) the more bonding MOs will be produced by the combination B) the higher will be the energy of the resulting bonding MO and the lower will be the energy of the resulting antibonding MO C) the higher will be the energies of both bonding and antibonding MOs that result D) the fewer antibonding MOs will be produced by the combination E) the lower will be the energy of the resulting bonding MO and the higher will be the energy of the resulting antibonding MO

E

The pressure exerted by a column of liquid is equal to the product of the height of the column times the gravitational constant times the density of the liquid, P = ghd. How high a column of water (d = 1.0 g/mL) would be supported by a pressure that supports a 713 mm column of mercury (d = 13.6 g/mL)? A) 14 mm B) 52 mm C) 713 mm D) 1.2 × 104 mm E) 9.7 × 103 mm

E

The scattering of light waves upon passing through a narrow slit is called __________. A) diffusion B) grating C) incidence D) adhesion E) diffraction

E

What is the typical effect of the addition of an interstitial element on the properties of a metal? A) increase in malleability and corrosion resistance B) increased surface luster C) decrease in melting point and increase in ductility D) decrease in conductivity and increase in brittleness E) increase in hardness and strength, decrease in ductility

E

Which of the following molecules or ions will exhibit delocalized bonding? SO2 SO3 SO3 2- A) SO2 and SO3 B) SO3 and SO3 2- C) None of the above will exhibit delocalized bonding. D) SO2, SO3, and SO3 2- E) SO3 2- only

E

Which one of the following exhibits dipole-dipole attraction between molecules? A) XeF4 B) Cl2 C) CO2 D) BCl3 E) AsH3

E