AP Chemistry Semester 1 Final
Lithium and nitrogen react to produce lithium nitride: 6Li (s) + N2 (g) → 2Li3N (s) How many moles of N2 are needed to react with 0.500 mol of lithium?
0.0833
The molarity of a solution prepared by diluting 43.72 mL of 1.005 M aqueous K2Cr2O7 to 500. mL is ________.
0.0879
Silver ions can be precipitated from aqueous solutions by the addition of aqueous chloride: Ag+ (aq) + Cl- (aq) → AgCl (s) Silver chloride is virtually insoluble in water so that the reaction appears to go to completion. How many grams of solid NaCl must be added to 25.0 mL of 0.149 M AgNO3 solution to completely precipitate the silver?
0.218
Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg (s) + O2(g) → 2MgO (s) How many moles of O2 are consumed when 0.550 mol of magnesium burns?
0.275
An object will sink in a liquid if the density of the object is greater than that of the liquid. The mass of a sphere is 4.69 g. If the volume of this sphere is less than ________ cm3, then the sphere will sink in liquid mercury (density = 13.6 g/cm3).
0.345
A 17.5 mL sample of an acetic acid (CH3CO2H) solution required 29.6 mL of 0.250 M NaOH for neutralization. The concentration of acetic acid was ________ M.
0.423
A 26.9-g sample of ammonium carbonate contains ________ mol of ammonium ions.
0.559
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.
0.67
What is the molarity of a NaOH solution if 48.0 mL of a 0.220 M H2SO4 solution is required to neutralize a 25.0-mL sample of the NaOH solution?
0.845
How many moles of Na+ are present in 343 mL of a 1.27 M solution of Na2SO4?
0.871
For molecules with only one central atom, how many lone pairs on the central atom guarantees molecular polarity?
1
Which of the following are chemical processes? 1. rusting of a nail 2. freezing of water 3. decomposition of water into hydrogen and oxygen gases 4. compression of oxygen gas
1,3
When the following equation is balanced, the coefficients are ________. C8H18+O2→CO2+H2O
1,5,2,2
(i) Viscosity increases as temperature ___________. (ii) Viscosity increases as molecular weight ___________. (iii) Viscosity increases as intermolecular forces __________.
1. decreases 2. increases 3. increase
Which of the following equations shows an incorrect relationship between pressures given in terms of different units? 1.20 atm = 122 kPa 152 mm Hg = 2.03 ⋅ 104 Pa 1.0 torr = 2.00 mm Hg 0.760 atm = 578 mm Hg 1.00 atm = 760 torr
1.0 torr = 2.00 mm Hg
A sample of a gas (1.50 mol) is contained in a 15.0 L cylinder. The temperature is increased from 100 °C to 150 °C. The ratio of final pressure to initial pressure [P2P1] is ________.
1.13
How many moles of carbon dioxide are there in 52.06 g of carbon dioxide?
1.183
What are the respective concentrations (M) of Cu2+ and Cl- afforded by dissolving 0.554mol CuCl2 in water and diluting to 380mL?
1.46 and 2.92
What is the concentration (M) of CH3OH in a solution prepared by dissolving 11.7 g of CH3OH in sufficient water to give exactly 230. mL of solution?
1.59
A sample of a gas originally at 29 °C and 1.25 atm pressure in a 3.0 L container is allowed to contract until the volume is 2.2 L and the temperature is 11 °C. The final pressure of the gas is ________ atm.
1.6
The density of NO2 in a 4.50 L tank at 760.0 torr and 25.0 °C is ________ g/L.
1.88
Which member of the following pairs has the larger London dispersion forces? 1. H2S or H20 2.CO2 or CO 3.SiH4 or GeH4
1.H2S 2.CO2 3.GeH4
Approximately how many elements are there?
100
The combustion of ammonia in the presence of oxygen yields NO2 and H2O: 4 NH3 (g) + 7 O2 (g) → 4 NO2 (g) + 6 H2O (g) The combustion of 43.9 g of ammonia with 258 g of oxygen produces ________ g of NO2.
119
The formula of nitrobenzene is C6H5NO2. The molecular weight of this compound is ________ amu.
123.11
What is the correct number of protons, electrons, and neutrons in the isotope 36Cl, respectively?
17 protons, 17 electrons, 19 neutrons
The molecular weight of a gas that has a density of 7.10 g/L at 25.0 °C and 1.00 atm pressure is ________ g/mol.
174
The volume occupied by 1.5 mol of gas at 35 °C and 2.0 atm pressure is ________ L.
19
A double bond consists of ________ pairs of electrons shared between two atoms.
2
The combination of two atomic orbitals results in the formation of ________ molecular orbitals.
2
When the following equation is balanced, the coefficient of Al is ________. Al (s) + H2O (l) → Al(OH)3 (s) + H2 (g)
2
There are ________ paired and ________ unpaired electrons in the Lewis symbol for a nitrogen atom.
2,3
The energy of a photon that has a wavelength of 9.0 m is ________ J.
2.2 × 10^-26
The thermal decomposition of potassium chlorate can be used to produce oxygen in the laboratory. 2KClO3 (s) → 2KCl (s) + 3O2 (g) What volume (L) of O2 gas at 25 °C and 1.00 atm pressure is produced by the decomposition of 7.5 g of KClO3 (s)?
2.3
The wavelength of light that has a frequency of 1.20 × 1013 s-1 is ________ m.
2.50 × 10^-5
10.0 grams of argon and 20.0 grams of neon are placed in a 1160.0 ml container at 31.0 °C. The partial pressure of neon is ________ atm.
21.3
How many grams of CH3OH must be added to water to prepare 150 mL of a solution that is 4.5 M CH3OH?
22
The molar volume of a gas at STP is ________ L.
22.4
The element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is ________ amu. Isotope Abundance Mass 221X 82.900 220.90 220X 13.200 220.00 218X 3.9000 218.10
220.67
A vessel contained N2, Ar, He, and Ne. The total pressure in the vessel was 987 torr. The partial pressures of nitrogen, argon, and helium were 44.0, 486, and 218 torr, respectively. The partial pressure of neon in the vessel was ________ torr.
239
If 50.75 g of a gas occupies 10.0 L at STP, 129.3 g of the gas will occupy ________ L at STP.
25.5
The pressure exerted by 1.3 mol of gas in a 13 L flask at 22 °C is ________ kPa.
250
A certain mass of carbon reacts with 128 g of oxygen to form carbon monoxide. ________ grams of oxygen would react with that same mass of carbon to form carbon dioxide, according to the law of multiple proportions.
256
What volume (mL) of a concentrated solution of sodium hydroxide (6.00 M) must be diluted to 497 mL to make a 3.12 M solution of sodium hydroxide?
258
What volume (mL) of a concentrated solution of sodium hydroxide (6.00 M) must be diluted to 200.0 mL to make a 0.880 M solution of sodium hydroxide?
29.3
Which periodic table group contains only metals? 6A 5A 8A 2A 7A
2A
The wavelength of a photon that has an energy of 6.33 × 10-18 J is ________ m.
3.10 × 10^-8
Part complete What is the mass % of carbon in dimethylsulfoxide (C2H6SO) rounded to three significant figures?
30.7
The ion PO43- has ________ valence electrons.
32
How many grams of NaOH (MW = 40.0) are there in 500.0 mL of a 0.200 M NaOH solution?
4
What mass of Xe is needed to fill a 400 L tank with Xe gas and produce a pressure of 200 atm at 25 0C? Assume ideal behavior.
429.5 kg Xe
The frequency of a photon that has an energy of 3.7 × 10-18 J is ________ s-1.
5.6*10^15
The reaction of 50 mL of Cl2 gas with 50 mL of C2H4 gas via the equation: Cl2 (g) + C2H4 (g) → C2H4Cl2 (g) will produce a total of ________ mL of products if pressure and temperature are kept constant.
50
Propane (C3H8) reacts with oxygen in the air to produce carbon dioxide and water. In a particular experiment, 38.0 grams of carbon dioxide are produced from the reaction of 22.05 grams of propane with excess oxygen. What is the % yield in this reaction?
57.6
How many p-orbitals are occupied in a K atom?
6
In the symbol shown below, x = ________. (14/x)C (thing w atomic number and isotopes-couldn't get formatting right)
6
Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg (s) + O2 (g) → 2MgO (s) When 4.00 g of magnesium burns, the theoretical yield of magnesium oxide is ________ g.
6.63
An atom of 128Xe contains ________ neutrons
74
Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s) + 3O2 (g) → 2Al2O3 (s) In a particular experiment, the reaction of 2.5 g of Al with 2.5 g of O2 produced 3.5 g of Al2O3. The % yield of the reaction is ________.
74
The molecular weight of butanol (C4H9OH), rounded to one decimal place, is ________ amu.
74.1
A pressure of 1.00 atm is the same as a pressure of ________ of mm Hg.
760
There are ________ mol of carbon atoms in 4 mol of dimethylsulfoxide (C2H6SO).
8
In ideal gas equation calculations, expressing pressure in Pascals (Pa), necessitates the use of the gas constant, R, equal to ________.
8.314 m3-Pa/mol-K
Calculate the percentage by mass of nitrogen in PtCl2(NH3)2.
9.34
Which of the following is soluble in water at 25∘C?
AgNO3
The net ionic equation for formation of an aqueous solution of Al(NO3)3 via mixing solid Al(OH)3 and aqueous nitric acid is ________.
Al(OH)3 (s) + 3H+ (aq) → 3H2O (l) + Al3+ (aq)
Which of the following correctly represents the third ionization of aluminum?
Al2+ (g) → Al3+ (g) + e-
The ________ ion has a noble gas electron configuration. B3- Li Al3+ B2+ Al4
Al3+
Which one of the following substances is the product of this combination reaction? Al (s) + I2(s) → ________
AlI3
Which of the following statements about gases is false? All gases are colorless and odorless at room temperature. Gases expand spontaneously to fill the container they are placed in. Distances between molecules of gas are very large compared to bond distances within molecules. Gases are highly compressible. Non-reacting gas mixtures are homogeneous.
All gases are colorless and odorless at room temperature.
Of the species below, only ________ is not an electrolyte. NaOH RbCl Ar KNO3 HF
Ar
Of the choices below, which gives the order for first ionization energies? S > Si > Cl > Al > Ar Cl > S > Al > Ar > Si Cl > S > Al > Si > Ar Ar > Cl > S > Si > Al Al > Si > S > Cl > Ar
Ar > Cl > S > Si > Al
Consider the following species when answering the following question: (i) NF3 (ii) BF3 (iii) IF3 (iv) PBr3 (v) BrCl3 Of the molecules below, only ________ is nonpolar.
BF3
Which of the following statements best explains why a closed balloon filled with helium gas rises in air?
Because the helium atoms are of lower mass than the average air molecule, the helium gas is less dense than air. The balloon thus weighs less than the air displaced by its volume.
Which hydrocarbon pair below has identical mass percentage of C?
C2H4 and C3H6
What is the empirical formula of a compound that is 66.6 % C, 11.2 % H, and 22.2 % O by mass?
C4H8O
Based on molecular mass and dipole moment of the five compounds in the table below, which should have the highest boiling point? Substance Molecular Mass (amu) Dipole Moment (D) Propane, CH3CH2CH3 44 0.1 Dimethylether, CH3OCH3 46 1.3 Methylchloride, CH3Cl 50 1.9 Acetaldehyde,CH3CHO 44 2.7 Acetonitrile, CH3CN 41 3.9
CH3CN
Of the following, ________ is the most volatile. CBr4 CH4 CH2Br2 CHBr3 CH3Br
CH4
In which of the following species does chlorine have an oxidation number of zero? HCl HClO4 Cl2 NaClO3 Cl−
Cl2
T or F: A gas is considered "ideal" if one mole of it in a one-liter container exerts a pressure of exactly 1 atm at room temperature.
F
T or F: The main component of air is oxygen
F
T or F:The principal source of the difference in the normal boiling points of ICl (97 °C; molecular mass 162 amu) and Br2 (59 °C; molecular mass 160 amu) is both dipole-dipole interactions and London dispersion forces.
F
Why are the electron affinities of the Group 4A elements more negative than those of the Group 5A elements?
Group 5A half-filled p-subshells discourage addition of an electron.
When H2SO4 is neutralized by NaOH in aqueous solution, the net ionic equation is ________.
H+ (aq) + OH- (aq) → H2O (l)
The substance ________ is always produced when an active metal reacts with water.
H2
The balanced molecular equation for complete neutralization of H2SO4 by KOH in aqueous solution is ________.
H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (aq)
In which species does chlorine have the highest oxidation number? HClO4 Cl− HCl NaClO3 Cl2
HClO4
Of the molecules below, the bond in ________ is the most polar. HF HCl HI H2 HBr
HF
Of the following substances, ________ has the highest boiling point. O2 Cl2 CH3CH2CH2OH HOCH2CH2OH C2H6
HOCH2CH2OH
Which nonmetal exists as a diatomic solid? bromine boron phosphorus antimony iodine
Iodine
If compound A has an equal number of oxygen and carbon atoms, what can we conclude about the composition of compound B?
It has twice as many oxygen than carbon atoms
What are the spectator ions in the reaction between KOH (aq) and HNO3 (aq)?
K+ and NO3-
Compound A contains 0.4020 g of oxygen per gram of carbon, whereas compound B contains 0.8040 g of oxygen per gram of carbon. What chemical law do these data illustrate?
Law of multiple proportions
Which type of intermolecular attractive force operates between all molecules?
London-dispersion forces
1 mole of which of the following will have the largest mass? Neon Boron Mercury Lithium
Mercury
Based on the octet rule, magnesium most likely forms a ________ ion.
Mg^2+
Methane and ethane are both made up of carbon and hydrogen. In methane, there are 12.0 g of carbon for every 4.00 g of hydrogen, a ratio of 3:1 by mass. In ethane, there are 24.0 g of carbon for every 6.00 g of hydrogen, a ratio of 4:1 by mass. This is an illustration of the law of ________.
Multiple Proportions
________ is the chemical symbol for elemental sodium.
Na
Of the following metals, ________ exhibits multiple oxidation states. Ni Cs Rb Al Mg
Ni
When aqueous solutions of which of the following are mixed, a precipitate forms: Li2CO3 and CsI K2SO4 and CrCl3 NiBr2 and AgNO3 NaI and KBr KOH and Ba(NO3)2
NiBr2 and AgNO3
Which of the following would have to gain two electrons in order to achieve a noble gas electron configuration? O Sr Na Se Br
O,Se
What is the empirical formula of a compound that contains 27.0% S, 13.4% O, and 59.6% Cl by mass?
SOCl2
Which one of the following is a metalloid? Sb H C Ca Cd
Sb
Element M reacts with chlorine to form a compound with the formula MCl2. Element M is more reactive than magnesium and has a smaller radius than barium. This element is ________.
Sr
Which element would be expected to have chemical and physical properties closest to those of calcium? S Sr Si Cu Fe
Sr
For a given element that does not form diatomic molecules, the number of peaks in the spectrum is equal to the number of naturally occurring isotopes of that element.
T
T or F: According to the kinetic-molecular theory, molecules of different gases at the same temperature always have the same average kinetic energy.
T
T or F: The atomic radius of iodine is one-half the distance separating the iodine nuclei.
T
T or F: The height of each peak in the mass spectrum is directly proportional to the relative abundance of the isotope
T
T or F: The paths of neutral (uncharged) atoms are not affected by the magnet in a mass spectrometer
T
In general, the vapor pressure of a substance increases as ________ increases.
Temperature
Electrolysis of water. Water decomposes into its component elements, hydrogen and oxygen, when an electrical current is passed through it. The volume of hydrogen, collected in the right test tube, is twice the volume of oxygen: How are the relative gas volumes collected in the two tubes related to the relative number of gas molecules in the tubes?
They are the same
The valence shell of the element X contains 2 electrons in a 5s subshell. Below that shell, element X has a partially filled 4d subshell. What type of element is X?
Transition metal
Which of the following is an illustration of the law of constant composition?
Water is 11% hydrogen and 89% oxygen by mass.
The element xenon has the symbol _______
Xe
The molecular geometry of ________ is square planar. XeF4 PH3 ICl3 CCl4 XeF2
XeF4
The condensed electron configuration of potassium, element 19, is ________.
[Ar]4s1
What is the electron configuration for the Fe3+ ion?
[Ar]4s^0 3d^5
One significant difference between gases and liquids is that ________.
a gas expands to fill its container
Oxides of most nonmetals combine with water to form ________.
an acid
The hybridization of the carbon atom in carbon dioxide is ________.
ap
What submicroscopic particles are the building blocks of matter?
atoms
The molecular geometry consists of ________. a) a nonbonding pair of electrons b) a single bond c) a multiple bond
b and c
The kinetic-molecular theory predicts that pressure rises as the temperature of a gas increases because ________
both the gas molecules collide more frequently with the wall and the gas molecules collide more energetically with the wall
If matter is uniform throughout and cannot be separated into other substances by physical processes, but can be decomposed into other substances by chemical processes, it is called a(n) ________.
compound
The law of constant composition applies to ________.
compounds
As the temperature increases, do you expect the surface tension of a liquid to increase, decrease, or stay the same?
decrease
In general, as you go across a period in the periodic table from left to right: (1) the atomic radius ________; (2) the electron affinity becomes ________ negative; and (3) the first ionization energy ________.
decreases, increasingly, increases
Part complete Which type of intermolecular attractive force operates only between polar molecules?
dipole-dipole
What is the predominant intermolecular force in CH3Br?
dipole-dipole
Hydrogen bonding is a special case of ________.
dipole-dipole attractions
Discussing this chapter, a classmate says, "Since elements that form cations are metals and elements that form anions are nonmetals, elements that do not form ions are metalloids." Do you agree or disagree?
disagree
What is the predominant intermolecular force in CO2?
dispersion
What types of intermolecular forces exist between HCl molecules?
dispersion and dipole-dipole
A separation process that depends on differing abilities of substances to form gases is called ________.
distillation
The Lewis structure of N2H2 shows ________
each nitrogen has one nonbonding electron pair
The basis of the VSEPR model of molecular bonding is ________.
electron domains in the valence shell of an atom will arrange themselves so as to minimize repulsions
If 42.0 kJ of heat is added to a 32.0-g sample of liquid methane under 1 atm of pressure at a temperature of −170∘C, what is the final state of the methane once the system equilibrates? Assume no heat is lost to the surroundings. The normal boiling point of methane is −161.5 ∘C. The specific heats of liquid and gaseous methane are 3.48 and 2.22 J/g⋅K, respectively. What is the final temperature of the methane once the system equilibrates?
gas-185K
Heat of sublimation can be approximated by adding together ________ and ________
heat of fusion, heat of vaporization
Which type of intermolecular attractive force operates only between the hydrogen atom of a polar bond and a nearby small electronegative atom?
hydrogen bonding
Consider the following electron configurations to answer the question: (i) 1s2 2s2 2p6 3s1 (ii) 1s2 2s2 2p6 3s2 (iii) 1s2 2s2 2p6 3s2 3p1 (iv) 1s2 2s2 2p6 3s2 3p4 (v) 1s2 2s2 2p6 3s2 3p5 The electron configuration belonging to the atom with the highest second ionization energy is ________.
i
In ionic bond formation, the lattice energy of ions ________ as the magnitude of the ion charges _______ and the radii ________.
increases, increase, decrease
A strong electrolyte is one that ________ completely in solution.
ionizes
The gold foil experiment performed in Rutherford's lab ________.
led to the discovery of the atomic nucleus
Which region of the periodic table shown here contains elements that are easiest to oxidize?
left
The hybridization of orbitals on the central atom in a molecule is sp. The electron-domain geometry around this central atom is ________.
linear
For a molecule with the formula AB2, the molecular shape is ________
linear or bent
Ethanol melts at -114 °C and boils at 78 °C at a constant pressure of 1 atm. What state of matter must a sample of ethanol be in at 25°C and 1 atm?
liquid
What is the physical state in which matter has no specific shape but does have a specific volume?
liquid
Oxides of the active metals combine with water to form ________.
metal hydroxides
Most of the elements on the periodic table are ________.
metals
Screening of the nuclear charge by core electrons in atoms is ________.
more efficient than that by valence electrons
Electrons in the 1s subshell are much closer to the nucleus in Ar than in He due to the larger ________ in Ar.
nuclear charge
The type of compound that is most likely to contain a covalent bond is ________.
one that is composed of only nonmetals
The element that corresponds to the electron configuration 1s22s22p4 is ________.
oxygen
Which region of the periodic table contains the least readily oxidized elements?
right
The hybridization of nitrogen in the H - C≡N: molecule is ________.
sp
The hybridization of the central atom in the XeF4 molecule is ________.
sp^3d^2
The molecular geometry of the CHCl3 molecule is ________.
tetrahedral
The molecular geometry of the left-most carbon atom in the molecule below is ________. The figure shows an organic molecule CH3COH, with an oxygen atom double-bonded to the second (from left to right) carbon atom.
tetrahedral
The law of constant composition says ________.
that the composition of a compound is always the same
The photoelectric effect is ________.
the ejection of electrons by a metal when struck with light of sufficient energy
What happens to h the height of the mercury column, if the atmospheric pressure increases?
the height of the mercury column increases
How high a liquid will rise up a narrow tube as a result of capillary action depends on ________.
the magnitudes of cohesive forces in the liquid and adhesive forces between the liquid and the tube, and gravity
The atomic number indicates _______
the number of protons or electrons in a neutral atom
Cathode rays are deflected away from a negatively charged plate because ________.
they are negatively charged particles
The molecular geometry of the PF3 molecule is ________, and this molecule is ________.
trigonal pyramidal, polar
A neutralization reaction between an acid and a metal hydroxide produces ________.
water and a salt
Which one of the following is correct? νλ=c ν+λ=c λ=cν ν÷λ=c ν=cλ
νλ=c
