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Chemistry > Final Exam > Flashcards

Final Exam Flashcards

1
Q 
The SI prefixes micro and kilo represent, respectively: 
A.) 10^6 & 10^-6
B.) 10^-3 & 10^9
C.) 10^-3 & 10^6
D.) 10^-6 & 10^3
E.) 10^3 & 10^-6
A

D.) 10^-6 & 10^3

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2
Q 
The SI base unit of mass
A.) m
B.) kg
C.) km
D.) liter
E.) in
A

B.) kg

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3
Q 
How many milliliters is 0.00055L
A.) 0.55mL
B.) 5.5mL
C.) 0.5mL
D.) 0.0000055mL
E.) 183mL
A

A. 0.55mL

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4
Q 
The average distance between the earth and Mercury is 56,974,000 miles. Explain the distance in kilometers
A.) 6.17 x 10^6 km
B.) 1.52 x 10^5 km
C.) 5.32 x 10^5 km
D.) 9.42 x 10^4 km
E.) 9.17 X 10^7 km
A

E.) 9.17 X 10^7 km

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5
Q 
A patient in the hospital is running a temperature of 102.4 degrees F, what is it in Celsius?
A.) 33.2 C
B.) 39.1 C
C.) 40.1 C
D.) 41.2 C
E.) 43.5 C
A

B.) 39.1 C

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6
Q

If you have a graduated cylinder containing 85.5 mL water, and this volume changes to 93.2 mL after a metal with a mass of 60.06g is dropped into the graduated cylinder then what is the density of this metal?
A.) 3.2g/mL B.) 9.9g/mL C.) 8.7g/mL
D.) 7.8g/mL E.) 0.072g/mL

A

D.) 7.8g/mL

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7
Q

The number 3.05020 X 10^9 has how many dig figs?

A.) 2 B.) 3 C.) 4 D.) 9 E.) 6

A

E.) 6

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8
Q

The result of (4.872 X 3.5630) - 5.98 (all are measured numbers) is properly written as
A.) 0.06236 B.) 11.4 C.) 11.38 D.) 11.37
E.) 11.378936

A

11.38

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9
Q

J.j Thomson studied cathode ray particles(electrons) and was able to measure the mass/charge ratio. His results showed that?
A. The mass/charge ratio varied as the cathode material was changed
B.) the charge was always a whole # multiple of some minimum charge
C.) matter included particles much smaller than the atom
D.) atoms contained dense areas of positive charge
E.) atoms are largely empty space

A

C.) matter included particles much smaller than the atom

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10
Q

Isotopes are
A.) atoms with different number of protons
B.) atoms wth different number of electrons
C.) atoms with the same number of protons but w/ different number of neutrons
D.) atoms with the same number of neutrons but w/ different number of protons
E.) atoms with the same number of neutrons but with different number of electrons

A

C.) atoms with the same number of protons but with different number of neutrons

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11
Q 
An atom of the isotope phosphorus-32 consists of how many protons, neutrons, and electrons
A.) 15p, 17n, 15e
B.) 32p, 31n, 31e
C.) 16p, 15n, 16e
D.) 15p, 16n, 16e
E.) 16p, 31n, 16e
A

A.) 15p, 17n, 15e

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12
Q 
Which of the following is a metalloid? 
A. Carbon, C, Z=6
B.) copper, Cu, Z= 29
C.) sulfur, S, Z=16
D.) bromine, Br, Z= 35
E.) silicon, Si, Z=14
A

E.) silicon, Si,Z=14

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13
Q 
Which of the following is a chemical change?
A.) melting wax
B.) carving a piece of wood
C.) boiling of water
D.) condensing water vapor into rainfall
E.) broiling a steak on a grill
A

E.) broiling a steal on a grill

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14
Q 
Which of the following elements is most likely to form a 2+ ion?
A.) Na
B.) N
C.) Mg
D.) Al
E.) Cl
A

C.) Mg

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15
Q 
Which of the following is a nonmetal?
A.) sodium, Na, Z=11
B.) iridium, Ir, Z=77
C.) sulfur, S, Z=16
D.) copper, Cu, Z=29
E.) germanium, Ge, Z=32
A

C.) sulfur, S, Z=16

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16
Q 
Which of the following elements is most likely to form a 2- ion?
A.) O
B.) N
C.) Mg
D.) Na
E.) Cl
A

A.) O

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17
Q 
Which of the following is the empirical formula for hexane, C6H6?
A.) C3H3
B.) C2H2
C.) CH
D.) CH2.3
E.) C0.4H0.4
A

C.) CH

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18
Q 
What is the name of BBr3
A.) boron bromide
B.) tribromoboride
C.) boric bromide
D.) bromine triboride
E.) boron tribromide
A

E.) boron tribromide

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19
Q 
What is the formula for lead(III) oxide
A.) PbO
B.) PbO2
C.) Pb2O
D.) PbO4
E.) Pb2O3
A

A.) PbO

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20
Q 
Which one of the following combinations of names and formulas is incorrect
A.) H3PO4 phosphoric acid
B.) H2CO3 carbonic acid
C.) HNO3 nitric acid
D.) KOH potassium hydroxide 
E.) NaHCO3 sodium carbonate
A

E.) NaHCO3 sodium carbonate

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21
Q

The combustion of butane is expressed by the following chemical equation

A

D.) 2C4H10 + 13 O2 = 8CO2 + 10 H2O

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22
Q 
What is the molar mass of butane C4H10?
A.) 17.02g/mole
B.) 34.09g/mole
C.) 58.12g/mole
D.) 12.01g/mole
E.) 46.06g/mole
A

C.) 58.12g/mole

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23
Q 
How many moles of CO2 are formed from 4.205g C4H10?
A.) 0.1758moles
B.) .2894 moles
C.) 6.615 moles
D.) .1694 moles
E.) .01673 moles
A

B.) .2894 moles

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24
Q 
How many molecules of CO2 are formed from 4.205 g C4H10?
A.) 8
B.) 9.032 X 10^23
C.) 6.022 X 10 ^23
D.) 1.743 X 10^23 
E.) 7.984 X 10^24
A

1.743 x 10^23

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25
Q 
Household sugar, sucrose, has the molecular formula C12H22O11. What is the mass % of the carbon in sucrose 
A.) 26.7%
B.) 33.3%
C.) 41.4%
D.) 42.1%
E.) 52.8%
A

D.) 42.1%

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26
Q 
The elements in group VIIA are collectively called
A.) alkali metals
B.) transition metals
C.) alkaline earth metals
D.) noble gases
E.) halogens
A

E.) halogens

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27
Q

Balancing the following equation

B2O3 + HF = BF3 + H2O

A

A.) B2O3 + 6HF= 2BF3 + 3H2O

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28
Q

Ammonia an important source of fixed nitrogen that can be metabolized by plants, is produced using the shaver process in which nitrogen and hydrogen combine N2+3H2=2NH3. How many grams of nitrogen are needed to produce 325 grams of ammonia
A.) 1070g B.) 535g C.) 267g D.) 178g
E.) 108g

A

C.) 267g

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29
Q

What is the percent yield for the reaction PCl3 + Cl2 = PCl5. If 119.3g of PCl5 (M= 208.2g/mol) are formed when 61.3g of Cl2 (M= 70.91g/mol) react with excess PCl3
A.) 195% B.) 85.0% C.) 66.3% D.) 51.4%
E.) 43.7%

A

66.3%

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30
Q

Lithium hydroxide is used in alkaline batteries. Calculate the molarity of a solution prepared by dissolving 1.495 miles of LiOH in enough water to give final volume of 750. mL
A.) 1.99 M B.) 1.50 M C.) 1.12 M
D.) .502 M E.) .00199M

A

A.) 1.99 M

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31
Q

What will be the final volume of a solution prepared by diluting 25 mL of 8.25M sodium hydroxide to a concentration of 2.40 M
A.) 330 mL B.) 210mL C.) 86mL
D.) 60 mL E.) 7.3mL

A

C.) 86mL

32
Q

In 0.20 mole of phosphoric acid, H3PO4
A.) how many H atoms are there?
B.) what is the total number of atoms
C.) how many miles of O atoms are there

A

A.) 3.61 x 10^23 atoms
B.) 9.61 X 10^23 atoms
C.) .80 moles

33
Q

How many milliliters of 1.58 M HCl are needed to react completely with 23.2 g of NaHCO3 (M=84.02g/mol)
A.) 638mL B.) 572mL C.) 536mL
D.) 276mL E.) 175mL

A

E.) 175mL

34
Q

How many miles of H+ (aq) ions are present in 750mL of .65M hydrochloric acid
A.) 1.2 mol B.) .98 mol C.) .87mol
D.) .65 mol E.).49 mol

A

E.) .49 mol

35
Q

Select the precipitate that forms when the following reactants are mixed Na2CO3+ BaCl2=
A.) Ba2CO3 B.) BaCO3 C.) NaCl
D.) NaCl2 E.) BaO

A

B.) BaCO3

36
Q 
Which of the following solutions will be the poorest conductor of electrical current
A.) sucrose C12H22O11
B.) sodium chloride, NaCl
C.) potassium nitrate KNO3
D.) lithium hydroxide LiOH
E.) sulfuric acid H2SO4
A

A.) sucrose C12H22O11

37
Q

Calculate the oxidation number of sulfur in sodium metabisulfate Na2S2O5
A.) -2 B.) +2 C.) +4 D.) +5 E.) none

A

C.) +4

38
Q

Select the net ionic equation for the reaction between sodium chloride and Mercury nitrate

A

Hg2^2+ + 2Cl-= Hg2Cl2

39
Q 
Identify the oxidizing agent in the following redox reaction 
Hg^2+(aq)+Cu(s)=Cu^2+(aq) +Hg(L)
A.) Hg2+(aq)
B.) Cu(s)
C.) Cu2+(aq) 
D.) Hg(L) 
E.) Hg2+(aq) and Cu2+(aq)
A

A.) Hg2+ (aq)

40
Q 
A sample of an ideal gas has its volume doubled while its temperature remains constant. If the original pressure was 100torr, what is the new pressure. 
A.) 10torr
B.) 50torr
C.) 100 torr
D.) 200 torr
E.) 1000torr
A

B.) 50torr

41
Q 
Hydrogen gas exerts a pressure of 466 torr in a container. What is this pressure in atmospheres?
A.) .217 atm
B.) .466 atm
C.) .613 atm
D.) 1.63 atm
E.) 4.60 atm
A

C.) .613 atm

42
Q 
Nitrogen dioxide is a red brown has that is responsible for the color of photochemical smog. A sample of nitrogen dioxide has a volume of 28.6L at 45.3 C and 89.9kPa. What is the volume at STP?
A.) 21.7 L
B.) 27.6 L
C.) 29.6L
D.) 37.6 L
E.) 153 L
A

A.) 21.8 L

43
Q 
Assuming the ideal behavior, what is the density of argon gas at STP in g/L
A.) .0176g/L
B.) .0250g/L
C.) .0561g/L
D.) 1.78g/L
E.) 181. g/L
A

D.) 1.78g/L

44
Q

If .750L of argon at 1.50 atm and 177C and .235L of sulfur dioxide at 95.0 kpa and 63.0 C are added to a 1.00L flask and the flasks temperature is adjusted to 25.0 C what is the resulting pressure in the flask?
A.) .0851 atm B.) .244atm C.) .946atm
D.) 1.74atm E.) 1.86atm

A

C.) .946atm

45
Q 
Which of the following gases will be the slowest to diffuse through a room
A.) methane, CH4
B.) hydrogen sulfide, H2S
C.) carbon dioxide CO2
D.) water H2O
E.) neon Ne
A

C.) carbon dioxide CO2

46
Q

A system which undergoes an adiabatic change (I.e, q=0) and does work on the surroundings has
A.) w0, ΔE>0
C.) w>0, ΔE0
E.) w

A

E.) w

47
Q

A system that does no work but which transfers heat to the surroundings has
A.) q0
B.) q0,ΔE>0
D.) q>0,ΔE

A

B.) q

48
Q 
A system expands from a volume of 1.00 L to 2.00 L against a constant external pressure of 1.00atm. The work done by the system in jn J
A.) 1.00J
B.) 2.00J
C.) 1.01 X 10^2 J
D.) 1.01 x 10^5 J 
E.) none
A

C.) 1.01 X 10^2 J

49
Q 
A 275 g sample of nickel at 100.0 C is placed in 100.0 mL of water at 22.0C. What is the final temperature of the water? Assume that no heat is lost or gained from the surroundings. Specific heat capacity of nickel.444J(g.k)
A.) 39.6 C
B.) 40.8 C
C.) 61.0 C
D.) 79.2 C
E.) 82.4C
A

A.) 39.6 C

50
Q

Which one of the following equations represents the formation reaction of CH3OH

A

E.) C(graphite) + 2H2(g) + 1/2 O2(g) =CH3 OH(l)

51
Q 
Use hess's law to calculate the enthalpy change for the reaction WO3+ 3H2= W + 3H2O
ΔH=- 1685.4kj
ΔH=- 477.84
A.) 125.9 kj
B.) 252.9 kj
C.) 364.9 kj
D.) 1207.6 kj
E.) none
A

A.) 125.9 kj

52
Q 
Calcium hydroxide which reacts with carbon dioxide to form calcium carbonate, was used by the ancient Romans as mortar stone structures. What is the enthalpy change if 3.8 mol of calcium carbonate is formed
A.) -18kj
B.) -69kj
C.) -73kj
D.) -260kj
E.) none
A

D.) -260kj

53
Q 
Hot packs, whose temperatures are raised when iron(Ii) oxide reacts with oxygen in air, are used to treat muscle pains. Which of the following is true of this reaction
A.) ΔH 0, process is endothermic
C.) ΔH>0, process is Exothermic
D.) ΔH=0, since hot packs are sealed
E.) ΔH
A

A.) ΔH

54
Q 
Which scientist first proposed that particles of matter could have wave particles?
A.) Einstein
B.) plank
C.) de brogile
D.) Compton
E.) Heisenberg
A

C.) de brogile

55
Q 
Select the arrangements of electromagnetic radiation which starts with the lowest wavelength and increases to greatest wavelength
A.) radio,infrared, uv, gamma rays
B.) radio, uv, infrared, gamma rays
C.) gamma, radio, uv, infrared 
D.) gamma, infrared, radio, uv
E,) gamma, uv, infrared, radio
A

E.) gamma rays, uv, infrared, radio

56
Q 
The AM station KBOR plays your favorite music from the 20s and 30s at 1290kHz. Find the wavelength of these waves
A.) 4.30 X 10^-2m
B.) .144m
C.) 6.94m
D.) 232
E.) >10^3
A

D.) 232

57
Q 
Infrared radiation from the sun has a wavelength of 6200nm. Calculate the energy of the photon of that radiation
A.) 4.1 X 10^-39J
B.) 4.1 X 10^-30J
C.) 3.2 X 10^-29J
D.) 3.2 X 10 ^-26 J 
E.) between 10^-20 and 10^-19
A

E.) between 10^-20 and 10^-19

58
Q 
A photon had an energy of 5.53 X 10 ^-17J. What is the frequency in s-1?
A.) 3.66 X 10^-50 s-1
B.) 1.20 x 10^-17 s-1
C.) 3.59 X 10^-9 s-1
D.) 2.78 X 10^8 s-1
E.) 8.35 X 10^16s-1
A

E.) 8.35 X 10^16 s-1

59
Q 
According to the rydberg equation, the longest wavelength (in nm) in the series of H- atom lines with n1=3 is
A.) 1875 nm
B.) 1458 nm
C.) 820nm
D.) 656nm
E.) 365 nm
A

A.) 1875 nm

60
Q 
An electron in the n=6 level emits a photon with a wavelength of 410.2 nm. To what energy level does the electron move?
A.) n=1
B.) n=2 
C.) n=3 
D.) n=4
E.) n=5
A

B.) n=2

61
Q 
The de brogile equation predicts that the wavelength in m of a proton moving at 1000 m/s is
A.) 3.96 X 10^-10m
B.) 3.96 X 10^-7m
C.) 2.52 X 10^6m
D.) 2.52 X 10^9m
E.) >10^10m
A

A.) 3.96 X 10^-10m

62
Q

The size of an atomic orbital is associated with
A.) the principal quantum number n
B.) the angular momentum quantum number l
C.) the magnetic quantum number ml
D.) the spin quantum number ms
E.) the angular momentum and magnetic quantum numbers, together

A

A.) the principal quantum number n

63
Q 
In quantum mechanical treatment of the hydrogen atom, which one of the following combinations of quantum numbers is not allowed
A.) N 3, l 0, ml 0
B.) n 3, l 1, ml -1
C.) n 3, l 2, ml 2
D.) n 3, l 2, ml -1
E.) n 3, l 3, ml 2
A

E.) n 3, l 3, ml 2

64
Q 
The effective nuclear charge for an atom is less than the actual nuclear charge due to
A.) shielding
B.) penetration
C.) paramagnetism
D.) electron pair repulsion
E.) relativity
A

A.) shielding

65
Q 
Electrons added to atomic orbitals of the same energy will remain unpaired wth parallel spins until the subshell is more than half filled is a statement of
A.) the aufbau principle
B.) hunds rule
C.) the Pauli exclusion principle 
D.) the periodic law
E.) the singularity rule
A

B.) hunds rule

66
Q 
Select the correct electron configuration for Te (z=52) 
A.) [Kr] 5s2 5p6 4d8
B.) [Kr] 5s2 5d10 5p4
C.) [Kr] 5s2 4d10 5p6
D.) [Kr] 5s2 4f14
E.) [Kr] 5s2 4d10 5p4
A

E.) [Kr] 5s2 4s10 5p4

67
Q 
An element with the electron configuration [noble gas] ns2 (n-1) d10 np3 has \_\_\_\_\_\_\_\_\_\_\_ valence electrons
A.) 2
B.) 3
C.) 5
D.) 10
E.) 15
A

C.) 5

68
Q 
Which of the following elements has the smallest atomic size
A.) Na
B.) Ar
C.) K
D.) Ca
E.) Kr
A

B.) Ar

69
Q 
Which one of the following equations correctly represents the process relating to the ionization energy of X
A.) X = X+ + e-
B.) x2 = X+ + X -
C.) X + e- = X-
D.) X-= X+ e-
E.) X = X+ +e-
A

E.) X = X+ + e-

70
Q 
Elements with the highest first ionization energies are found in the \_\_\_\_\_ region of the periodic table
A.) lower left
B.) upper left
C.) center
D.) lower right
E.) upper right
A

E.) upper right

71
Q 
Select the element with the least metallic character
A.) Sn
B.) Sr
C.) Ti
D.) Ge
E.) Ga
A

D.) Ge

72
Q 
Which of the following contains ionic bonding
A.) CO
B.) SrF2
C.) Al
D.) OCl 2
E.) HCl
A

B.) SrF2

73
Q 
Which of the following contains covalent bonds
A.) BaO
B.) IBr
C.) Mg
D.) LiBr
E.) Cu
A

B.) IBr

74
Q 
In which of these substances are the atoms held together by polar covalent bonding
A.) SrCl2 
B.) CsCl
C.) ClF
D.) TiF2
E.) S8
A

C.) ClF

75
Q 
Select the compound with the highest lattice energy
A.) CaS
B.) BaO
C.) NaI
D.) LiBr
E.) MgO
A

E.) MgO

76
Q 
Which of the following elements is the most electronegative 
A.) Ne
B.) Rb
C.) P
D.) I
E.) Cl
A

E.) Cl

77
Q 
Select the most polar pond amongst the following 
A.) C-O
B.) Si-F
C.) Cl-F
D.) C-F
E.) C-I
A

B.) Si-F

Chemistry (2 decks)

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