Chem 109 Final Exam Review

What is the mass in grams of 1.00 gal of water? The density of water is 1.00 g/mL

3.78x10^3

Convert 2.5 miles to kilometers (1 mile - 1.609 km)

4.0 km

An isotope of Na has a mass number of 23. The Na+ ion of this isotope contains Protons. Electrons. Neutrons a) 11 10 11 b) 11 10 12 c) 11 11 12 d) 12 11 11

B) 11, 10, 12

how many militers of concentrate Hal (12 M) are needed to prepare 250 mL of 0.10 M Hal solution? a) 1.2 mL b) 2.1 mL c) 25 mL d) 30 mL

B) 2.1 mL

you are given the electronegativity values 2.1, 2.5, 3.0, and 3.5 but do not know to which element (O, P, S, and Cl) these values correspond. Which must be the electronegativity value of S? a) 2.1 b) 2.5 c) 3.0 d) 3.5

B) 2.5

a sulfure molecule has the structure shown, where O (circle shaded in) represents a sulfur atom. Calculate the mass of a single sulfur molecule. a) 5.32x10^-23 b) 4.26x10^-22 c) 32.1 g d) 257 g

B) 4.26x10^-22

A hot piece of metal is placed in 50.00 g of water at a temperature of 18.3 ℃. The temperature rises to 54.7℃. How much heat did the water absorb? a) 11,400 J b) 7610 J c) 3830 J d) 11.4 J

B) 7610 J

Which has more atoms, 10.0g Mg or 10.0 g Ca?

Ca would have more atoms

What types of substance and bonds are in each substance below? a) CCl4 b) NH4Cl c) Al2O3 d) Ar

a) molecular, covalent b) ionic, both ionic and covalent c) ionic, ionic d) atomic, neither ionic nor covalent

Write the molecular ionic and net ionic equations for the combination of Fe(NO3)2(aq) with NA2CO3(aq)

- Fe(NO3)2(aq) + Na2CO3(aq) → FeCO3(s) + 2NaNo3(aq) - Fe2+(aq)+Co3-(aq) → FeCO3(s)

How Many moles of H are in 2.5 g of water? How many H atoms?

1.7x10^23 H atoms

The average speed of nitrogen molecule in air at 25℃ is 515 m/s. Convert this speed to miles per hour

1.15x10^3 mi/hr

calculate the number of copper atoms in 2.45 mol of copper

1.48x10^24

The width, length, and height of a small box are 15.5, 27.3, and 5.4 cm, respectively. Calculate the volume of the box, using the correct number of significant figures in your answer.

15.5 x 27.3 x 5.4 = 2285.01 cm^3 ⇒ 2.3x10^3

calculate the amount of carbon (in moles) contained in a 0.0265 g pencil "lead" (Assume that the pencil lead is made of pure graphite, a form of carbon)

2.21x10^-3

How many copper atoms are in a copper penny with a mass of 3.10g? (assume that the penny is composed of pure copper)

2.94x10^22

The US food and drug administration (FDA) recommends that a person consume less than 2.4 g of sodium per fay. What mass of sodium chloride (in grams) can you consume and still be within the FDA guidelines? Sodium chrlodie is 39% sodium by mass

6.2 g NaCL

Calculate the mass percent of Cl in freon-112 (C2Cl4F2),a CFC refrigerant

69.58%

Which fertilizer has the highest percent nitrogen by mass? Formula. Molar Mass a) (NH2)2CO = 60.06 b) NH4NO3 = 80.05 c) (NH4)2CO3 = 96.09 d) (NH4)3PO4 = 149.1

A) (NH2)2CO

Calculate ΔH at 25℃ for 2HCl(g) + 1/2O2(g) → Cl2(g) + H2O(g) given a) -57 kJ b) -150 kJ c) -306 kJ d) -427 kJ

A) -57 kJ

what volume of 0.300 M HCL must be used to react completely with 8.00 g of zinc? Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) a) 815 mL b) 408 mL c) 245 mL d) 204 mL

A) 815 mL

which has the greatest first ionization energy? a) Ar b) Cl c) K d) S

A) Ar

in which compound does the central element fail to follow the octet rule? a) BF3 b) CF4 c) H2O d) NH3

A) BF3

Which is an exothermic process? a) H2O(g) → H2O(l) b) H2O(l) → H+(aq) + OH-(aq) c) H2O(l) → H2)(g) d) H2O(l) → H2(g) + 1/2O2(g)

A) H2O(g) → H2O (l)

Which bond does not result from the sharing of electrons? a) ionic b) pi c) polar covalent d) sigma

A) Ionic

a bond in which two atoms share a pair of electrons provide by only one of the atoms is a) a coordinate covalent bond c) a non polar covalent bond c) a polar covalent bond d) an ionic bond

A) a coordinate covalent bond

Which best describe the carbon-carbon bond distance in benzene, if a typical C-C single bond length is 154 pm and a typical C=C bond length is 133 pm? a) all are between 133 and 154 pm b) half are 133 pm and half are 154 pm c) all alternate between 133 and 154 pm d) all are 154 pm

A) all are between 133 and 154 pm

The observation that 20 g of hydrogen gas always combines with 160 g of oxygen gas to form 180 g of water, even when there is more than 160 g of oxygen present in the reaction container, illustrates the law of: a) definite proportions b) multiple proportions c) ideal gases d) excess reactants e) conservation of mass

A) definite proportions

what is the net ionic equation for the reaction that occurs when a solution of magnesium chloride, MgCl2, is added to a solution of silver nitrate, AgNO3, and a white precipitate is formed? a) Cl2^-2(aq) + 2Ag+(aq) → 2AgCl(s) b) Cl-(aq) + Ag+(aq) → AgCl(s) c) MgCl2(aq) + 2Ag+(aq) → 2AgCl(s) + Mg2+(aq) d) 2Cl-(aq) + 2AgNO3(aq) → 2AgCl(s) + 2NO3-(aq)

B) Cl-(aq) + Ag+(aq) → AgCl(s)

When Fe(NO3)2 (a strong electrolyte) dissolves in water, the particles in solution are: a) Fe and(NO3)2- b) Fe2+ and 2NO3- c) Fe and 2NO3 d) Fe and N2 and 3O2

B) Fe2 and 2NO3-

what is the empirical formula for Na2S2O3 x 5H2O? a) HNaO2S b) H5NaO4S c) H5Na2O4S2 d) H10Na2O8S2

B) H5NaO4S

an aqueous solution of Mg(NO3)2 contains a) Mg(NO3)2 molecules b) Mg2+ ions and NO3- ions c) Mg atoms andNO3 molecules d) Mg2+ ions and (NO3)2^2- ions

B) Mg2+ ions and NO3- ions

which scientist described the atoms as "a positively charged core (nucleus) in the middle of a lot of empty space"? a) Chadwick b) rutherford c) thomson d) Bohr

B) Rutherford

Which element; W, X, Y, or Z; has the largest atomic mass? W = 24.31 g mol^-1 X2 = 70.90 g mol^-1 Y4 = 123.9 g mol^-1 Z8= 256.6 g mol^-1 a) W b) X c) Y d) Z

B) X

Which postulate of Dalton's theory explains the observation that when 100 g of solid calcium carbonate is heated, 44 g of carbon dioxide and 56 g of calcium oxide are produced? a) compounds contain atoms of two different types b) atoms do not change during chemical reactions; they rearrange c) matter is composed of small individual particles called atoms d) atoms of one element are different from atoms of another element

B) atoms do not change during chemical reactions; they rearrange.

a bond order increases, what is the effect on bond length and bond dissociation energy a) both decease b) bond length decreases and bond dissociation energy increases c) bond length increases and bind dissociation energy decreases d) there is no correlation between bond order, bond length and/or bond dissociation energies

B) bond length decreases and bond dissociation energy increase

Which of these elements is chemically similar to magnesium? a) Sulfur b) calcium c) iron d) nickel e) potassium

B) calcium

in an atom, orbital I and orbital II must differ in (I) o (II) (><) a) n, the principle quantum number b) l, the angular momentum (azimuthal) quantum number c) mt, the magnetic quantum number d) ms, the spin quantum number

B) l, the angular momentum (azimuthal) quantum number

Ammonia has a melting point of 196 K and a normal boiling point of 240 K. At 225 K and 1 atm, ammonia exists primarily as a a) gas b) liquid c) solid d) mixture of solid and liquid

B) liquid

Which of the following is the best description of how potassium and bromine are bonded together in order to make potassium bromide (KBr)? a) the -2 charge on the K is attracted to the +2 charge on the Br. b) the -1 charge on the K is attracted to the +1 charge on the Br c) the +1 charge on the K is attracted to the -1 charge on the Br d) the +2 charge on the K is attracted the the -2 charge on the Br e) The K and Br atoms share electrons

C) the +1 charge on the K is attracted to the -1 charge on the Br

what is the oxidation number of arsenic in H2AsO3? a) -3 b) 0 c) +3 d) +5

C) +3

How much of a reactant in excess remains when solutions containing 0.50 mol AgNO3 and 0.50 mol K2CrO4 are mixed? 2AgNO3(aq) + K2CrO4(aq) → Ag2CrO4(s) + 2KNO3(aq) a) 0.25 mol AgNO3 b) 0.50 mol AgNO3 c) 0.25 mol K2CrO4 d) neither reactant is in excess; both are completely consumed

C) 0.25 mol K2CrO4

what is the density of CO2 at 25℃ and 0.850 atm? a) 44.0 g L^-1 b) 22.4 g L^-1 c) 1.53 g L^-1 d) 0.0347 g L^-1

C) 1.53 g L^-1

How many 1-L bottles are required to contain 1 m^3 of liquid? a) 10 b) 100 c) 1000 d) 10000

C) 1000

In another universe the physical laws are almost identical to ours except that there are three spin states allowed for electrons, rather than two. How many elements constitute the second row of the reiodic table in this universe? a) 3 b) 8 c) 12 d) 18

C) 12

an electron has these quantum numbers: n= 4 l=2 mt = -2 ms = -1/2 which set of quantum numbers could describe another electron in the same orbital? n,l,mt,ms a) 4,-2,-2,+1/2 b) 4,2,-2,-1/5 c)4,2,-2,+1/2 d)4,2,+2,-1/2

C) 4,2,-2,+1/2

What is the smallest whole number coefficient for BF3 when this equation is balanced? ____BF3(g) + ____H2O(l) → _____H3BO3(aq) + ______HBF4(aq) a) 2 b) 3 c) 4 d) 5

C) 5

What madd of ethanol can be produced from 2.27x10^3 g of glucose, if the yield is 85.0%? C6H12O6(s) → 2C2H5OH(l) + 2CO2(g) a) 1.37x10^3 g b) 1.16x10^3 g c) 987 g d) 290 g

C) 987 g

the formula for iron(III) sulfate is a) Fe2S3 b) Fe2(SO3)3 c) Fe2(SO4)3 d) Fe3(SO4)2

C) Fe2(SO4)3

Which of the following allows scientist to explain a broad range of observations and even make predictions? a) laws b) facts c) theories d) hypothesis

C) Theories

Soluble ionic compounds are a) always non-electrolytes b) always week electrolytes c) always strong electrolytes d) sometimes weak electrolytes e) sometimes strong electrolytes

C) always strong electrolytes

The complete Lewis structure of OCCl2 will have: a) resonance forms b) only single bonds c) at least one double bond d) at least one lone pair on each atom

C) at least one double bond

What element represented by the following data? Protons: Neutrons: ⚫️⚫️⚫️⚫️⚫️⚫️⚫️⚫️ Electrons: 🔵🔵🔵🔵🔵🔵 a) carbon-12 b) carbon-14 c) oxygen-14 d) more than one of these

C) oxygen-14

What is the geometry around each aluminum atom in the aluminum chloride dimer? [image given] a) square planar b) square pyramidal c) tetrahedral d) trigonal planar

C) tetrahedral

determine the oxidation state of S in Na2SO4 a) -4 b) +2 c) +4 d) +6 e) -2

D) +6

Which is the electron affinity of chlorine given that the electron affinities of sulfur and bromine are -200 kJ mol^-1 and -325 kJ mol^-1, respectively? a) -151 kJ mol^-1 b) -200 kJ mol^-1 c) -262 kJ mol^-1 d) -349 kJ mol^-1

D) -349 kJ mol^-1

How many grams of O2 are needed to prepare 55.9 g of PbO? 2PbS(s) + 3O2(g) → 2Pb(s) + 2SO2(g) a) 2.67 g b) 5.33 g c) 6.00 g d) 12.0 g

D) 12.0 g

According to the law of conservation of mass, how much zinc was present in the zinc carbonate (assume no gases are formed)? 64 g Ca + 192 g CaC → 152 g CaC + ? g Zn a) 40 g b) 88 g c) 104 g d) 356 g

D) 256 g

What is the coefficient preceding O2 when the following combustion reaction of a fatty acid is properly balanced using the smallest set of whole numbers? ___C18H36O2 + _____ O2 → ____CO2 + H2O a) 1 b) 8 c) 9 d) 26 e) 27

D) 26

What is the approximate average mass of an argon atom in this sample? 36Ar, 38Ar, 40Ar, 36Ar a) 40 amu b) 36 amu c) 38 amu d) 37.5 amu

D) 37.5 amu

a metal sample has a mass of 24.6g. When it is simmered in oil in a graduated cylinder, it causes the volume reading to rise from 18.7 to 22.3 mL. Identify the metal a) Li 0.534 g cm^-3 b) K 0.862 g cm^-3 c) Ca 1.55 g cm^-3 d) Bi 9.75 g cm^-3

D) Bi 9.75 g cm^-3

which is a correct representation for the ground state atom? a) C [He] 2s ↑↓ 2p ↑↓ b) V [Ar] 2s ↑↓ 2p ↑ c) Cr [Ar] 4s ↑↓ 3d ↑↓ ↑↓ d) Co [Ar} 4s ↑↓ 3d ↑↓ ↑↓ ↑↑↑

D) Co [Ar} 4s ↑↓ 3d ↑↓ ↑↓ ↑↑↑

Which is insoluble in water? a) K3PO4 b) Ca(OH)2 c) ZnSO4 d) Hg2Br2 e) (NH4)2S

D) Hg2Br2

which substance contains both ionic and covalent bonds? a) KF b) PCl3 C) CHCl3 d) KNO3

D) KNO3

arrange the species K, Na, Mg, and Mg+2 in order of smallest to largest radius a) K < Na < Mg < Mg+2 b) Na < Mg < Mg+2 < K c) Na < Mg+2 < Mg < K d) Mg+2 < Mg < Na < K

D) Mg2 < Mg < Na < K

Arrange the molecules in order of increasing bond polarity a) PF3 < PCl3 < PBr3 < PI3 b) PBr3 < PCl3 < PF3 < PI3 c) PI3 < PF3 < PCl3 < PBr3 d) PI3 < PBr3 < PCl3 < PF3

D) PI3 < PBr3 < PCl3 < PF3

Silicone, Si, combines with hydrogen to form silane, SiH4. What other element, X, is likely to combine with hydrogen to form XH4? a) Br b) N c) P d) Sn

D) Sn

which is the best representation of the electron configuration of element 107? a) [Rn] 6d^7 b) [Rn] 6d^5/7s^2 c) [Rn] 5f^14/6d^7 d) [Rn] 5f^14/6d^5/7s^2

D) [Rn] 5f^14/6d^5/7s^2

The elements in Group 2A are known by what name? a) Transition metals b) halogens c) alkali metals d) alkaline earth metals e) noble gases

D) alkaline earth metals

which of the following is NOT a part of Dalton's Atomic Theory? a) all matter is composed of extremely small particle called atoms b) in chemical reactions, atoms are combined, separated, or rearranged c) atoms of different elements combine in simple whole-number rations d) atoms can be subdivided, created, or destroyed

D) atoms can be subdivided, created, or destroyed

The two 10.0 L flask contain O2 and N2, respectively. Both are at 292 K and 0.963 atm. Which response is supported by the kinetic molecular theory? a) both flask contain the same mass of gas b) both flasks contain the same number of molecules. c) both cases have the same average kinetic energy d) both B and C are correct

D) both B and C are correct

Which is a transition metal? a) calcium b) carbon c) cesium d) cobalt

D) cobalt

the shape of the molecule NH3 is _____ and the H-N-H bond angles are approximately _____ a) planar, 120 b) tetrahedral, 109 c) pyramidal, 120 d) pyramidal, 109

D) pyramidal, 109

xenon in XeF4 has four single bonds and two lone electron pairs. What is the hybridization of xenon? a) sp2 b) sp3 c)sp3d d) sp3d2

D) sp3d2

Give the correct name or formula a) CaSO3 b) diphospofrus tetrabromide c) Li3P d) nickel (II) nitrate hexahydrate e) HC2H3O2 (aq)

a) Calcium Sulfite b) P2Br4 c) lithium phosphide d) Ni(NO3)2*6H20 e) acetic acid

Perform each a conversion a) 101,000 ns to seconds b) 32.08 kg to grams

a) 1.01x10^-4 b) 32080 g

What is the total pressure go a gas mixture composed of 0.200 mol CO2, 0.360 mol N2, and 0.450 mol O2 in a 1.00 L container at 25℃? a) 24.5 atm b) 22.4 atm c) 2.05 atm d) 1.00 atm

a) 24.5 atm

If the volume of a mole of a gas is tripled and the Kelvin temperature is doubled, then the pressure will be...(PV=nRT) a) 1/6 of the original pressure b) 2/3 of the original pressure c) 3/2 of the original pressure d) 6 times the original pressure

b) 2/3 of the original pressure

which name is paired correctly with its formula? a) N2O4 → nitrogen tetroxide b) HN)3 → nitrous acid c) KBrO3 → potassium bromate d) NAHCO3 → sodium carbonate

c) KBrO3

Sodium azide, NaN3, is used in the air bags of automobiles. What is the volume of N2 gas at 25℃ and 1.0 atm released from 100 g of NaN3? 2NaN3(s)→2Na(s)+3N2(g) a) 34 L b) 38 L c) 52 L d) 56 L

d) 56 L

The boiling point of H2O is higher than that of CCl4 because of a) London forces b) ion-ion attractions c) ion-dipole attractions d) hydrogen bonding

d) hydrogen bonding