Chemistry Final Exam
temperature of absolute zero measured in C
-273 C
In the following unbalanced reaction, what is the total decrease in oxidation number for the reduced element? HNO3 + HBr --> NO + Br2 + H2O
-3
In the following unbalanced reaction, what is the total decrease in oxidation number for the reduced element? HNO3 + HI --> NO + I2+ H2O
-3
What is the change in oxidation number of chromium when Na2Cr2O7 becomes CrI3?
-3
What is the change in the oxidation number of chromium when K2Cr2O7 becomes CrCl3?
-3
What is the freezing point of a solution of 0.5 mol of LiBr in 500 mL of water? (Kf= 1.86 C/m)
-3.72 C
C3H5OH
...
How many valence electrons are transferred from the nitrogen atom to potassium in the formation of the compound potassium nitride?
0
The oxidation number of bromine in bromine gas...
0
calcium dihydrogen phosphate
Ca(H2PO4)2
calcium hydroxide
Ca(OH)2
What are quanta of light called?
photons
What is the sum of the oxidation numbers in calcium carbonate?
0
What is the sum of the oxidation numbers in lithium carbonate?
0
The temperature at which the motion of particles theoretically ceases
0 K
molecular compounds
composed of two or more nonmetallic elements
What is the number of moles of solute in a 0.3 molal solution containing 0.10 kg of solvent?
0.3 moles
What is the density of an object having a mass of 8.0 g and a volume of 25 cm^3?
0.32 g
composed of two or more substances chemically combined in a fixed proposition
compound
if 1 mL of 6M HCl is added to 499 mL of water to give exactly a 500 mL solution, what is the molarity of the dilute solution?
0.01M
If 2.0 mL of 6.0M HCl is used to make a 500 mL aqueous solution, what is the molarity of the dilute solution?
0.024M
A 500-g sample of Al2(SO4)3 is reacted with 450 g of Ca(OH)2. A total of 596 g of CaSO4 is produced. (i) What is the limiting reagent in this reaction? (ii) How many moles of excess reagent are unreacted? Al2(SO4)3 + 3Ca(OH)2 --> 2Al(OH)3 + 3CaSO4
(i) Al2(SO4)3 (ii) 1.69 moles
In the following unbalanced reaction, what is the total increase in oxidation number for the oxidized element? H2O + Cl2 + SO2 --> HCl + H2SO4
+2
The oxidation number of magnesium in magnesium chloride is...
+2
What is the oxidation number of magnesium in magnesium iodide?
+2
What is the total increase in oxidation number for the atom that is oxidized in the following balanced redox equation? Cr2O7^-2 + 8H+ + 3SO3^-2 --> 2Cr^+3 + 3SO4^-2 + 4H2O
+2
What is the molarity of 200 mL of solution in which 2.0 moles of sodium bromide is dissolved?
10M
How many moles of N2 are in a flask with a volume of 250 mL at a pressure of 300.0 kPa and a temperature of 300 K?
0.03 moles
charge of the strontium ion
+2
charge on the cation CuSO4
+2
What is the change in oxidation number of aluminum in the reaction of aluminum with oxygen gas to make aluminum oxide?
+3
ionic charge on zirconium ion in the ionic compound ZrO2?
+4
What is the change in oxidation number of manganese when MnO2 becomes Mn2O3?
-1
What is the sum of the oxidation numbers in the chlorate ion?
-1
charge of a chloride ion
-1
charge on the polyatomic ions nitrite and chlorite
-1
What is the temperature of 128 K expressed in degrees Celsius?
-145 C
what is the freezing point of a solution that has 5 moles of NaI in 1250 g of water? (Kf= 1.86 C/m)
-15 C
A 55 g piece of copper wire is heated, and the temperature of the wire changes from 19 C to 86 C. The amount of heat absorbed is 343 cal. What is the specific heat of copper?
0.093 cal/g x C
What is the concentration of undissociated acid if the hydrogen-ion concentration is 0.001 M and the acid dissociation constant is 0.0000001?
0.1 M
A gas occupies a volume of 140 mL at 35 C and 97 kPa. What is the volume of the gas at STP?
0.12 L
It takes 770 joules of energy to raise the temperature of 50 g of mercury by 110 C. What is the specific heat of mercury?
0.14 J/g X C
calculate the number of moles of Al2O3 that are produced when 0.60 mol of Fe is produced in the following reaction. 2Al + 3FeO --> 3Fe + Al2O3
0.20 mol
What is the number of moles of solute in 650 mL of a 0.4M solution?
0.26 moles
What is the mole faction of ethanol in a solution of 3 moles of ethanol and 5 moles of water?
0.375
When 45 g of an alloy, at 25 C, are dropped into 100 g of water, the alloy absorbs 956 J of heat. If the final temperature of the alloy is 37 C, what is its specific heat?
0.423
If the solubility of a gas in water is 4.0 g/L when the pressure of the gas above the water is 3.0 atm, what is the pressure of the gas above the water when the solubility of the gas is 1.0 g/L?
0.75 atm
how many liters of a 0.3M solution are needed to give 2.7 moles of solute?
0.9 L
How many iron (II) ions combine with oxygen to form iron (II) oxide?
1
How many pi bonds are formed when sp2 hybridization occurs in the ethene, C2H4?
1
how many half-filled orbitals are in a bromine atom?
1
how many valence electrons are in rubidium?
1
If the [H+] in a solution is 1 x 10^-1 mol/L, what is the [OH-]?
1 x 10^-13
Calculate the hydrogen ion concentration [H+] for an aqueous solution in which [OH-] is 1 x 10^-11 mol/L. Is this solution acidic, basic, or neutral?
1 x 10^-3 M; acidic
If the pH is 9, what is the concentration of hydroxide ion?
1 x 10^-5 M
What is the ion-product constant for water?
1.0 x 10^-14
What is the measurement 1042 L rounded off to two significant digits?
1.0 x 10^3
What is the frequency of ultraviolet light with wavelength 2.94 x 10^-8 m? (c=3.00 x 10^8)
1.02 x 10^16 s^-1
What is the frequency of a radar photon with energy 6.80 x 10^-25 J? (h=6.63 x 10^-34)
1.03 x 10^9 Hz
What is the molality of a solution containing 15 g of solute in 0.5 kg of solvent? (molar mass of solute= 24 g)
1.25m
the diameter of a carbon atom 0.000000000154 m. What is this number expressed in scientific notion?
1.54 x 10^-10 m
What is the molality of a solution containing 5 moles of solute in 3.2 kg of solvent?
1.56m
The volume of a gas is 250 mL at 340.0 kPa pressure. What will the volume be when the pressure is reduced to 50.0 kPa, assuming the temperature remains constant?
1.7 L
The molality of a solution containing 8.1 moles of solute in 4847 g of solvent is...
1.7m
What is the hydrogen-ion concentration if the pH is 3.7?
1.99 x 10^-4 M
If [OH-]= 1 x 10^-4 M, what is the pH of the solution?
10
How many liters of hydrogen gas are needed to react with CS2 to produce 2.50 L of CH4 at stp? 4H2 + CS2 --> CH4 + 2H2S
10.0 L
boiling point of water
100
What is the boiling point of a solution of 0.1 mole of glucose in 200 mL of water? (Kb= 0.512 C/m)
100.26 C
What is the boiling point of a solution that contains 3 moles of KBr in 2000 g of water? (Kb= 0.512 C/m)
101.4 C
What is the bond angle in a water molecule?
105
What is the pressure exerted by 32 g of O2 in a 22 L container at 30 C?
114.45 kPa
How much heat is required to raise the temperature of 5.5 x 10^2 g of aluminum by 10 C? (specific heat= 0.21)
1155 cal
Express the sum of 7.68 m and 5.0 m using the correct number of significant digits
12.7 m
bond angles in ethene, C2H4, are... (90, 109.5, 120, 180)
120
A rigid container of O2 has a pressure of 340 kPa at a temperature of 713 K. What is the pressure at 273 K?
130.18 kPa
Express the sum of 1111 km and 222 km using the correct number of significant digits
1333 km
how many grams of CO are needed to react with an excess of Fe2O3 to produce 209.7 g Fe? Fe2O3 + 3CO --> 3CO2 + 2Fe
157.75 g
What is the mass number for an oxygen atom that has 10 neutrons in its nucleus?
18
Consider an element Z that has two naturally occurring isotopes with the following percent abundances: the isotope with a mass number of 19.0 is 55% abundant; the isotope with a mass number of 21 is 45% abundant. What is the average atomic mass for element Z?
19.9 amu
how many electrons are in the highest occupied energy level of copper?
1e-
give the electron configuration for a neutral atom of beryllium
1s2 2s2
give the electron configuration for a neutral atom of chlorine
1s2, 2s2, 2p6, 3s2, 3p5
Electron configuration of the calcium ion
1s2, 2s2, 2p6, 3s2, 3p6
electron configuration of the gallium ion
1s2, 2s2, 2p6, 3s2, 3p6, 3d10
What is the electron configuration of potassium?
1s2, 2s2, 2p6, 3s2, 3p6, 4s1
write the electron configuration for chromium
1s2, 2s2, 2p6, 3s2, 3p6, 4s1, 3d5
give the electron configuration for a neutral atom of selenium
1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p4
Determine the subscript for ammonium in the chemical formula for ammonium dichromate
2
How many electrons are shared in a single covalent bond?
2
How many electrons does barium have to give up to achieve a noble-gas electron configuration?
2
How many energy sublevels are in the second principal energy level?
2
How many unpaired electrons are in a sulfur atom?
2
What is the pH of a solution with a concentration of 0.01 M hydrochloric acid?
2
What will the coefficient of HNO3 be when the following equation is compltely balanced using the smallest whole-number coefficients? HNO3 + MnCl2 + HCl --> NO + MnCl4 + H2O
2
how many nonbonding pairs of electrons are in a water molecule?
2
how many phases are present in a colloid?
2
If the volume of solute is 6 mL and the volume of solution is 300 mL, what is the solute's percent by volume?
2& v/v
What is the pH when the hydrogen ion concentration is 7.0 x 10^-3M?
2.15
What is the molarity of a solution containing 56 grams of solute in 959 mL of solution? (molar mass of solute= 26 g)
2.2M
The specific heat of silver is 0.24. How many joules of energy are needed to warm 4.37 g of silver from 25 C to 27.5 C?
2.62 J
Convert 6 feet to mm
203.3898 mm
the density of osmium, which is the densest metal, is 22.57 g/cm^3. What is the mass of a block of osmium that measures 1.00 cm x 4.00 cm x 2.50 cm?
226 grams
A mixture of gases at a total pressure of 95 kPa contains N2, CO2, and O2. The partial pressure of the CO2 is 24 kPa and the partial pressure of the N2 is 48 kPa. What is the partial pressure of the O2?
23 kPa
Balance: Ag2(NO3)2 + CuCl2 -->
2AgNO3 + CuCl2 --> 2AgCl + Cu(NO3)2
Balance C2H6 + O2 -->
2C2H6 + 7O2 --> 4CO2 + 6H2O
Balance: C2H6 + O2-->
2C2H6 + 7O2 --> 4CO2 + 6H2O
Balance: propanol is combusted
2C3H7OH + 9O2 --> 6CO2 + 8H2O
Balance: C4H10 + O2 -->
2C4H10 + 13O2 --> 10H2O + 8CO2
Balance: pentanol is combusted
2C5H11OH + 15O2 --> 10CO2 + 12H2O
Balance: hydrochloric acid is added to limestone
2HCl + CaCO3 --> CaCl2 + H2O + CO2
Balance: potassium is added to water
2K + 2H2O --> 2KOH + H2
Balance: Li + H2O-->
2Li + 2H2O --> 2LiOH + H2
Balance: lithium is placed in water
2Li + 2H2O --> 2LiOH + H2
Balance: magnessium is combusted
2Mg + O2 --> 2MgO
Balance Na + H2O -->
2Na + 2H2O --> 2NaOH + H2
Balance: solid sodium is placed in sulfuric acid
2Na + H2SO4 --> Na2SO4 + H2
how many electrons are in the highest occupied energy level of a neutral strontium atom?
2e-
From which orbital in a lithium atom is an electron transferred to form Li+ ?
2s
How many electrons does nitrogen gain in order to achieve a noble-gas electron configuration?
3
How many unshared pairs of electrons are in a molecule of hydrogen iodide?
3
how many electrons does a gallium atom give up when it becomes an ion?
3
how many electrons does a nitrogen atom need to gain in order to attain a noble-gas electron configuration?
3
in how many physical states does water exist
3
in the measurement of 0.503 L, which digit is the estimated digit?
3
The gaseous product of a reaction is collected in a 25 L container at 27 C. The pressure in the container is 300 kPa and the gas has a mass of 96 g. HOw many moles of the gas are in the container?
3.01 moles
A 0.500M solution of a weak acid, HX, is only partially ionized. The [H+] was found to be 4.02 x 10^-3. Find the dissociation constant for this acid
3.21 x 10^-5
A gas storage tank has a volume of 3.5 x 10^5 m^3 when the temperature is 27 C and the pressure is 101 kPa. What is the new volume of the tank if the temperature drops to -10 C and the pressure drops to 95 kPa?
3.26 x 10^8
What is the acid dissociation constant of a weak acid if a concentration of 0.3M gives a hydrogen-ion concentration of 0.001 M
3.34 x 10^-6
when a mixture of sulfur and metallic silver is heated, silver sulfide is produced. What mass of silver sulfide is produced from a mixture of 3.0 g Ag and 3.0 g S8? 16Ag + S8 --> 6Ag2S
3.45 g
What is the product of the number 1000 and the measurement 0.00357 m expressed in the correct number of significant layers?
3.57 m
what is the molarity of a solution containing 9 moles of solute in 2500 mL of solution?
3.6M
If the solubility of a gas is 7.5 g/L at 404 kPa pressure, what is the solubility of a gas when the pressure is 202 kPa?
3.75 g/L
How many kilocalories of heat are required to raise the temperature of 225 g of aluminum from 20 C to 100 C? (specific heat= 0.21)
3.8 kcal
A 10-g mass of krypton occupies 15.0 L at a pressure of 210 kPa. Find the volume of the krypton when the pressure is increased to 790 kPa.
3.99 L
if 5.0 g of H2 are reacted with excess CO, how many grams of CH3OH are produced, based on a yield of 86%? CO + 2H2 --> CH3OH
34.12 g
What mass of sucrose, C12H22O11, is needed to make 500 mL of a 0.200M solution?
34.2 g
A balloon filled with helium has a volume of 30.0 L at a pressure of 100 kPa and a temperature of 15.0 C. What will the volume of the balloon be if the temperature is increased to 80 C and the pressure remains constant?
36.77 L
boiling point of water in K
373 K
What is the pressure of 0.520 atm equal to in mm of Hg?
395.2 mm Hg
What is the molarity of a solution that contains 6 moles of solute in 2 liters of solution?
3M
Balance the following reaction that occurs in an acidic solution using the redox method. S + NO3- --> SO2 + NO
3S + 4NO3- + 4H+ --> 3SO2 + 4NO + 2H2O
If the hydroxide ion concentration is 10^-10 M, what is the pH of the solution?
4
What coefficient of H+ balances the atoms in the following half-reaction?
4
What coefficient of H+ balances the atoms in the following half-reaction? H+ + MnO2 --> Mn^+2 + H2O
4
What is the total number of covalent bonds normally associated with a single carbon atom in a compound?
4
how many electrons are shared in a double covalent bond?
4
how many valence electrons are in a silicon atom?
4
At what temperature does liquid water have its maximum density?
4 C
How many protons are present in an atom of Be-9?
4 protons
What is the volume of 45.6 g of silver if the density of silver is 10.5 g/mL?
4.34 mL
A gas has a pressure of 710 kPa at 227 C. What will its pressure be at 27 C, if the volume does not change?
426 kPa
What is the percentage of water in the hydrate CoCl2 • 6H2O?
45.42%
Calculate the energy required to produce 7 mol Cl2O7 on the basis of the following balanced equation. 2Cl2 + 7O2 + 130 kcal --> 2Cl2O7
455 kcal
what electron configuration of the 4f energy sublevel is most stable
4f14
What is the maximum number of d orbitals in a principal energy level?
5
how many valence electrons are in an atom of phosphorus?
5
If the percent by volume is 2% and the volume of solution is 250 mL, what is the volume of solute in solution?
5 mL
express 0.05 grams in kilograms
5 x 10^-5 kg
the expression of 5008 km in scientific notation is...
5.008 x 10^3 km
what is the sum of 2.7 g and 2.47 g expressed in the correct number of significant digits?
5.2 g
How many mL of a 2.0M NaBr solution are needed to make 200 mL of 0.5M NaBr?
50 mL
how many electrons are there in the highest occupied energy level of atoms in Group 5A elements?
5e-
Which orbital is filled when iodine gains an electron to become a negative ion?
5p
express 0.06 liters in cubic meters
6 x 10^-5 m^3
solid sodium reacts violently with water, producing heat, hydrogen gas, and sodium hydroxide. How many molecules of hydrogen gas are formed when 48.7 g of sodium are added to water? 2Na + 2H2O --> 2NaOH + H2
6.38 x 10^23 molecules
how many grams of liquid water are produced when 60 grams of ice melt
60 grams
how many joules are in 148 calories? (1 cal= 4.18 J)
619 J
when glucose is consumed, it reacts with oxygen in the body to produce carbon dioxide, water, and energy. How many grams of carbon dioxide would be produced if 45 g of C6H12O6 completely reacted with oxygen?
66 g
How many liters of O2 are needed to react completely with 45.0 L of H2S at STP? 2H2S + 3O2 --> 2SO2 + 2H2O
67.5 L
What is the volume of an object with a density of 7.73 g/cm^3 and a mass of 5.40 x 10^2 g?
69.9 cm^3
How many valence electrons does an iodine atom have?
7
If the hydrogen ion concentration is 10^-7 M, what is the pH of the solution?
7
Which of the following measurements is expressed to 3 significant figures? (0.007, 7077, 7.30 x 10^-7, 0.070)
7.30 x 10^-7
What mass of Na2SO4 is needed to make 2.5 L of 2.0M solution?
710 g
How many water molecules are in 39 formula units of calcium chloride dihydrate (CaCl2 • 2H2O)?
78
how many electrons are in the highest occupied energy level of a neutral chlorine atom?
7e-
What is the approximate frequency of a photon having an energy 5 x 10^-24 J? (h= 6.6 x 10^-34 J•s)
8 x 10^9 Hz
What is the result of multiplying 2.5 x 10^10 by 3.5 x 10^-7?
8.75 x 10^3
How many grams of copper sulfate pentahydrate (CuSO4 • 5H2O) would you heat to produce 29.8 g of water?
82.62 g
What is the sum of 6.210 L and 3 L expressed in the correct number of significant digits?
9 L
Aluminum Oxide
Al2O3
Aluminum is a group 3A metal. Which ion does Al typically form?
Al^+3
the first step in balancing a redox reaction by the oxidation number change method
Assign oxidation numbers
Which was originally a tenet of Dalton's atomic theory, but had to be revised about a century ago?
Atoms are tiny indivisible particles
Dalton's atomic theory included which idea? (all atoms of all elements are the same size, atoms of different elements always combine in one-to-one ratios, atoms of the same element are always identical, individual atoms can be seen with a microscope)
Atoms of the same element are always identical
barium chlorate
Ba(ClO3)2
for a given mass of gas at constant temperature, the volume of the gas varies inversely with pressure
Boyle's law
chaotic movement of colloidal particles
Brownian motion
ethene
C2H4
ethanol
C2H5OH
Balance: C2H5OH + O2-->
C2H5OH + 3O2 --> 2CO2 + 3H2O
Balance: Ethanol is combusted
C2H5OH + 3O2 --> 2CO2 + 3H2O
butanoic acid
C3H7COOH
Propanol
C3H7OH
propanol
C3H7OH
Balance: C3H8 + O2 -->
C3H8 + 5O2 --> 3CO2 + 4H2O
Balance: C3H8 + O2-->
C3H8 + 5O2 --> 3CO2 + 4H2O
butane
C4H10
Butanol
C4H9OH
Balance: butanol is combusted in oxygen
C4H9OH + 6O2 --> 4CO2 + 5H2O
pentane
C5H12
Balance: pentane is combusted in oxygen
C5H12 + 8O2 --> 5CO2 + 6H2O
cyclohexane
C6H12
Which of the following substances is NOT an electrolyte? (KCl, CCl4, LiCl, Na2SO4)
CCl4
Predict which one of the following compounds would be insoluble in water. (NaCl, HCl, CF4, CuSO4)
CF4
Which of the following substances dissolves most readily in gasoline? (CH4, HCl, NH3, NaBr)
CH4
Which of these would you expect to be soluble in the non polar solvent carbon disulfide, CS2?
CI4
Which of the following substances is less soluble in hot water than in cold water? (CO2, NaCl, NaNO3, KBr)
CO2
Balance: calcium hydroxide reacts with hydrochloric acid
Ca(OH)2 + 2HCl --> CaCl2 + 2H2O
the non-SI scale for temperature
Celsius temperature scale
the volume of a fixed mass of gas is directly proportional to its Kelvin temperature, if the pressure is kept constant
Charle's Law
Chlorine has two naturally occurring isotopes, Cl-35 and Cl-37. The atomic mass of chlorine is 35.45. Which of these two isotopes of chlorine is more abundant?
Cl-35
CuCl2
Copper (II) Chloride
copper (II) bicarbonate
Cu(HCO3)2
At constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases
Dalton's Law
this man lived from 460 BC-370 BC and was among the first to suggest the idea of atoms
Democritus
Use Graham's law to calculate how much faster flourine gas, F2, will effuse than chlorine gas, Cl2, will. The molar mass of F2= 38; the molar mass of Cl2= 70.9
F2 effuses 1.366 faster
chemical symbol for iron
Fe
iron (III) oxide
Fe2O3
Iron (III) Chloride
FeCl3
Iron (II) Oxide
FeO
the pressure of a gas is directly proportional to its Kelvin temperature if the volume is kept constant
Gay-Lussac's law
The rate at which a gas will effuse is inversely proportional to the square root of the gas's molar mass
Graham's Law
Which of the following covalent bonds is the most polar? (H-F, H-C, H-H, H-N)
H-F
what is the limiting reagent when 150.0 g of nitrogen react with 32.1 g of hydrogen? N2 + 3H2 --> 2NH3
H2
Which of the following represents a compound (H, H-3, H2O, O-16)?
H2O
What are the acids in the following equilibrium reaction? CN- + H2O -->HCN + OH-
H2O and HCN
Sulfurous acid
H2SO3
sulfurous acid
H2SO3
Balance: H2SO4 + NaOH -->
H2SO4 + 2NaOH --> 2H2O + Na2SO4
Balance: H2SO4 + NaOH-->
H2SO4 + 2NaOH --> 2H2O + Na2SO4
Balance: sulfuric acid reacts with sodium hydroxide
H2SO4 + 2NaOH --> 2H2O + Na2SO4
phosphoric acid
H3PO4
Which of the following shows both the correct formula and correct name of an acid? (HClO2 chloric acid, HNO2 hydronitrous acid, H3PO4 phosphoric acid, HI iodic acid)
H3PO4 phosphoric acid
hydrochloric acid
HCl
Balance: chloric acid reacts with sodium hydroxide
HClO3 + NaOH --> H2O + NaClO3
hypoiodous acid
HIO
iodic acid
HIO3
nitric acid
HNO3
states the impossibility of knowing both velocity and position of a moving particle at the same time
Heisenberg uncertainty principle
at a given temperature, the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid
Henry's law
states that if you add two or more thermochemical equations to give a final equation, you can also add the heats of reaction to give the final heat of reaction
Hess's law of heat summation
FeCl2
Iron (II) Chloride
FeO
Iron (II) oxide
If oxygen is removed from a sample of air as iron rusts, what happens to the total pressure of the air?
It decreases
What happens to the temperature of a liquid as it evaporates?
It decreases
What is the formula of the ion formed when potassium achieves noble-gas electron configuration?
K+
potassium sulfite
K2SO3
Which temperature scale is directly proportional to average kinetic energy?
Kelvin
the SI scale for temperature
Kelvin temperature scale
Of the elements Pt, V, Li, and Kr, which is a nonmetal?
Kr
can accept an electron pair
Lewis acid
Lithium nitrate
LiNO3
MgCl2
Magnesium chloride
Who arranged the elements according to atomic mass and used the arrangement to predict the properties of missing elements?
Mendeleev
Balance: Mg + H2SO4
Mg + H2SO4 --> MgSO4 + H2
Magnessium sulfate
MgSO4
Who conducted experiments to determine the quantity of charge carried by an electron?
Millikan
Identify the atom that increases in oxidation number in the following redox reaction: 2MnO2 + 2K2CO3 + O2 --> 2KMnO4 + 2CO2
Mn
Which of the following compounds contains the Mn+3 ion? (MnS, MnBr2, Mn2O3, MnO)
Mn2O3
what is the oxidizing agent in the following reaction: I- + MnO4- --> I2 + MnO2
MnO4-
Which of the following substances dissolves most readily in water? (BaSO4, CaCO3, NH3, CH4)
NH3
What is the reducing agent in the following reaction: 2Na + S --> Na2S
Na
Balance: sodium carbonate reacts with magnessium chloride
Na2CO3 + MgCl2 --> 2NaCl + MgCO3
sodium sulfate
Na2SO4
Balance: sodium sulfate reacts with strontium chloride
Na2SO4 + SrCl2 --> 2NaCl +SrSO4
What is the formula unit of sodium nitride?
Na3N
sodium bicarbonate
NaHCO3
sodium hydroxide
NaOH
Which of the following compounds contains the lead(II) ion? (PbO, PbCl4, Pb2O, Pb2S)
PbO
Which of these elements does not exist as a diatomic molecule? (Ne, F, H, I)
Ne
Which of the following elements has the smallest ionic radius? (Li, K, O, S)
O
melting point of water
O degrees Celsius
Oxygen gas
O2
Which of the following diatomic molecules is joined by a double covalent bond? (O2, Cl2, N2, He2)
O2
Phosphorous diflouride
PF2
each orbital has at most two electrons
Pauli exclusion principle
Lead (II) Nitrate
Pb(NO3)2
Balance Pb(NO3)2 + KCl -->
Pb(NO3)2 + 2KCl --> PbCl2 + 2KNO3
write the formula for the compound rubidium phosphide
Rb3P
The oxidation number of sulfur in each of the following is +6 EXCEPT for... (SO3, Na2SO4, SO4^-2, S2O4^-2)
S2O4^-2
In which of the following compounds is the octet expanded to include 12 electrons? (H2S, PCl3, PCl5, SF6)
SF6
Sulfur hexaflouride
SF6
Which of the following represents a molecular compound? (ZnO, Xe, SO2, BeF2)
SO2
What is the formula of the ion formed when tin achieves a stable electron configuration?
Sn^+4
Which of the following is true about subatomic particles? (electrons are negatively charged and are the heaviest subatomic particle, protons are positively charged and the lightest subatomic particle, neutrons have no charge and are the lightest subatomic particle, the mass of a neutron nearly equals the mass of a proton)
The mass of a neutron nearly equals the mass of a proton
Which of the following is correct concerning subatomic particles? (electron was discovered by Goldstein in 1886, neutron was discovered by Chadwick in 1932, proton was discovered by Thomson in 1880, cathode rays were found to be made of protons)
The neutron was discovered by Chadwick in 1932
If 4 moles of gas are added to a container that already holds 1 mole of gas, how will the pressure change inside the container?
The pressure will be 5 times higher
phenomenon observed when beam of light passes through a colloid
Tyndall effect
Zinc metal
Zn
An ionic bond is a bond between what?
a cation and an anion
each period in the periodic table corresponds to...
a principal energy level
All of the following are physical properties of matter EXCEPT... (mass, color, melting point, ability to rust)
ability to rust
the lowest point on the Kelvin scale
absolute zero
When an electron moves from a lower to a higher energy level, the electron ____________
absorbs a quantum of energy
Lewis acid is a substance that...
accepts a pair of electrons
closeness to true value
accuracy
the closeness of a measurement to its true value is a measure of its what?
accuracy
ratio of the concentration of the dissociated to the undissociated form
acid dissociation constant
the amount of product formed when a reaction is carried out in the laboratory
actual yield
If the hydrogen ion concentration of a solution is 10^-10 M, is the solution acidic, alkaline, or neutral?
alkaline
Which of the following are considered physical properties of a substance... (color and odor, melting and boiling points, malleability and hardness, all of the above)
all of the above
Which of the following statements is part of the kinetic theory? (the particles of a gas move independently of each other, the particles in a gas move rapidly, the particles in a gas are relatively far apart, all of the above)
all of the above
what type of ions have names ending -ide?
anions
homogeneous mixture of water and dissolved substances
aqueous solution
the pressure resulting from the collision of atoms and molecules with objects
atmospheric pressure
the smallest particle of an element that retains the properties of that element
atom
frequencies of light emitted by an element
atomic emission spectrum
region of high probability of finding an electron
atomic orbital
one-half the distance between the nuclei of two atoms when the atoms are joined
atomic radius
tendency of electrons to enter orbitals of lowest energy first
aufbau principle
a device used to measure atmospheric pressure
barometer
What is the best description for a solution with a hydroxide ion concentration of 1 x 10^-4 M?
basic
shape of NO2
bent
shape of O3
bent
shape of a water molecule
bent
sulfur hexaflouride is an example of a... (monoatomic ion, polyatomic ion, binary compound, polyatomic compound)
binary compound
a colligative property related to a decrease in the vapor pressure of a solution
boiling point elevation
In the following unbalanced reaction, which atom is oxidized? HNO3 + HBr --> NO + Br2 + H2O
bromine
mixture in which particle size averages between 1 nm and 1000 nm
colloid
Ca(OH)2
calcium hydroxide
CaO
calcium oxide
device used to measure the heat absorbed or released during a chemical or physical process
calorimeter
CO
carbon monoxide
Which of the following compounds is a nonelectrolyte? (sodium bromide, magnesium sulfate, copper chloride, carbon tetrachloride)
carbon tetrachloride
type of ion formed by Group 2A elements
cation
element with lowest electronegativity value
cesium
process in which substances are changed into different substances
chemical reaction
in the reaction of calcium with chlorine, which atom is the oxidizing agent?
chlorine
ClO2
chlorine dioxide
the next to the last step in balancing a redox reaction by the oxidation number change method
choose coefficients to make the change in oxidation number equal to 0
CoCl2
cobalt (II) chloride
measure of the amount of solute dissolved in a specified quantity of solvent
concentration
An ideal gas CANNOT be... (condensed, cooled, heated, compressed)
condensed
a covalent bond in which the shared electron pair comes from only one of the atoms
coordinate covalent bond
the number of ions of opposite charge surrounding each ion in a crystal
coordination number
a repetition of properties occurs when elements are arranged in order of increasing atomic number
periodic law
Which of the following does NOT involve a physical change? (mixing, melting, grinding, decomposing)
decomposing
As the density of a substance increases, then the volume of a mass....
decreases
N2O
dinitrogen monoxide
N2O5
dinitrogen pentaoxide
N2O4
dinitrogen tetraoxide
What type of acid is sulfuric acid ? (monoprotic, diprotic, triprotic, none of the above)
diprotic
acid with two ionizable protons
diprotic acid
colloidal particles spread throughout a suspension
dispersed phase
a process in which a liquid is boiled to produce a vapor that is condensed again into a liquid
distillation
separating a solid from a liquid by evaporating the liquid
distillation
a covalent bond in which two pairs of electrons are shared
double covalent bond
What is the shape of the 3p atomic orbital?
dumbbell
MnO4-
permanganate
compound that will conduct current in the liquid state or in the aqueous solution
electrolyte
a negatively charged subatomic particle
electron
arrangement of electrons around atomic nucleus
electron configuration
a depiction of valence electrons around the symbol of an electron
electron dot structure
ability of an atom to attract electrons when the atom is in a compound
electronegativity
Which of the following are free to drift in metals (protons, electrons, neutrons, cations)?
electrons
subatomic particles that are transferred to form positive and negative ions
electrons
What causes the shielding effect to remain constant across a period? (electrons are added to the same principal energy level, electrons are added to different principal energy levels, the charge on the nucleus is constant, the atomic radius increases)
electrons are added to the same principle energy level
substance that cannot be changed into simpler substances by chemical means
element
colloid of a liquid in a liquid
emulsion
in the Bohr model of the atom, the electron in an orbit has a fixed what?
energy
The principal quantum number indicates what property of an electron?
energy level
another name for the acid dissociation constant
equilibrium constant
C2H6
ethane
which of the following is a physical change... (corrosion, explosion, evaporation, rotting of food)
evaporation
the reactant that is not completely used up in a reaction
excess reagent
a colligative property related to the fact that ice will form at higher temperatures in the Great Lakes than in the ocean
freezing point depression
number of wave cycles passing a point per unit of time
frequency
Which of the following electromagnetic waves have the highest frequencies? (ultraviolet light waves, x-rays, microwaves, gamma rays)
gamma rays
what state of matter is a vapor
gas
what state of matter takes both the shape and volume of its container?
gas
What expression is generally used for solubility?
grams of solute per 100 grams of solvent
lowest energy level
ground state
vertical column in the periodic table
group
Elements that are characterized by the filling of p orbitals are classified as...
groups 3A-8A
part of a sample having uniform composition and properties
phase
reaction showing either the reduction or the oxidation reaction
half-reaction
an anion of chlorine or other halogen
halide ion
Which of the following is NOT an example of matter? (air, heat, smoke, water vapor)
heat
heat content of a system at constant pressure
heat capacity
the change in enthalpy that accompanies the formation of a compound from its elements
heat of formation
the energy required to melt a solid at its melting point
heat of fusion
the enthalpy change for a chemical reaction exactly as it is written
heat of reaction
the enthalpy change caused by dissolving a substance
heat of solution
not uniform in composition
heterogeneous mixture
which of the following cannot be considered a single phase? (pure solid, pure liquid, homogeneous mixture, heterogeneous mixture)
heterogeneous mixture
describes mixture with a uniform composition
homogeneous
HBr
hydrobromic acid
HCl
hydrochloric acid
in the reaction of hydrogen with iodine, which atom is oxidized?
hydrogen
a type of bond that is very important in determining the properties of water and of important biological molecules such as proteins and DNA
hydrogen bond
What causes water's low vapor pressure?
hydrogen bonding
What is responsible for the high thermal energy required to melt ice?
hydrogen bonding
bonds between adjacent water molecules
hydrogen bonds
primarily responsible for holding water molecules together in the liquid state
hydrogen bonds
When dissolved in water, acids produce... (negative ions, polyatomic ions, hydrogen ions, oxide ions)
hydrogen ions
H2O2
hydrogen peroxide
Bronsted-Lowry acid
hydrogen-ion donor
HI
hydroiodic acid
a crystal that absorbs water vapor from the air
hygroscopic
why is ice less dense than water?
ice has a molecular structure that is an open framework held together by hydrogen bonds
PV=nRT
ideal gas law
describes liquids that are insoluble in one another
immiscible
how is the modern periodic table arranged?
increasing atomic number
What is the key difference between a liquid and a gas?
intermolecular attractions
HIO3
iodic acid
Which of the following elements has the ability to undergo sublimation? (Oxygen, carbon, sodium, iodine)
iodine
the force of attraction binding oppositely charged ions together
ionic bond
Which of the following are weak electrolytes in water? (ionic compounds that partially dissassociate in water, ionic compounds that are soluble, polar compounds that ionize, nonpolar compounds that do not ionize)
ionic compounds that partially dissociate in water
Which of the following decreases with increasing atomic number in Group 2A? (shielding effect, ionic size, ionization energy, number of electrons)
ionization energy
energy required to remove an electron from an atom
ionization energy
When the vapor pressure of a liquid is equal to the atmospheric pressure, what happens to the liquid?
it begins to boil
How does the energy of an electron change when the electron moves closer to the nucleus?
it decreases
How does the surface tension of water compare with the surface tension of most other liquids?
it is higher
During a phase change, what happens to the temperature of a substance?
it remains constant
When an iron is ground into powder, what happens to its mass?
it stays the same
How does atomic radius change from top to bottom in a group in the periodic table?
it tends to increase
SI unit of energy
joule
the energy an object has due to its motion
kinetic energy
all matter consists of tiny particles that are in constant motion
kinetic theory
N2O
laughing gas
the reactant that determines the amount of product that can be formed in a reaction
limiting reagent
What element in the second period has the largest atomic radius?
lithium
Li2O
lithium oxide
Mg(OH)2
magnesium hydroxide
Which hydroxide compound yields the lowest concentration of hydroxide ions in aqueous solution? (sodium hydroxide, potassium hydroxide, calcium hydroxide, magnesium hydroxide)
magnesium hydroxide
the next to the last step in balancing a redox reaction by the half reaction method
make the electron changes equal
MnO2
manganese (IV) oxide
An example of an extensive property of matter is... (temperature, pressure, mass, hardness)
mass
amount of matter an object contains
mass
the heat capacity of an object depends on its...
mass
the quantity of matter an object contains
mass
this is conserved in every ordinary chemical reaction
mass
type of element that is a good conductor of heat and electric current
metal
the attraction of valence electrons for metal ions
metallic bond
What is the metric system prefix for the quantity 0.000001?
micro-
a physical blend of two or more components
mixture
number of moles of solute dissolved in 1 kg of solvent
molality
The amount of heat needed to melt one mole of a solid at a constant temperature
molar heat of fusion
number of moles of solute dissolved in 1 L of solution
molarity
ratio of moles of solute in solution to total number of moles of both solvent and solute
mole faction
Which type of solid has the highest melting point?
network solid
a subatomic particle with no charge
neutron
What is the correct name for the N^-3 ion?
nitride ion
HNO2
nitrous acid
the central part of an atom, containing protons and neutrons
nucleus
this quantity can always be used in the same way as moles when interpreting balanced chemical equations
number of molecules
What does NOT change when a solution is diluted by the addition of solvent? (volume of solvent, mass of solvent, number of moles of solute, molarity of solution)
number of moles of solute
What do colligative properties depend upon?
number of solute particles in a solution
Isotopes of the same element have different...
numbers of neutrons
atoms react so as to acquire the stable electron structure of a noble gas
octet rule
How many hydrogen bonds can be formed between one hydrogen atom in a water molecule and oxygen atoms of surrounding water molecules?
one
How is an emulsifying agent characterized?
one polar end and one nonpolar end
under what conditions can potassium bromide conduct electricity?
only when melted or dissolved in water
the letter "p" in the symbol 4p3 indicates what?
orbital shape
Cu--> Cu^+2 + 2e-... wat type of reaction is this?
oxidation
integer related to the number of electrons under an atom's control
oxidation number
substance that accepts electrons (agent)
oxidizing agent
Which atom in a water molecule has the greatest electronegativity?
oxygen atom
negative logarithm of the hydrogen ion concentration
pH
If the hydroxide-ion concentration is 1 x 10^-12 M, what is the pH of the solution?
pH=2
SI unit of pressure
pascal
the ratio of the actual yield to the theoretical yield
percent yield
HClO4
perchloric acid
horizontal row in the periodic table
period
a covalent bond between two atoms of significantly different electronegativities
polar bond
The Ka of carbonic acid is 4.3 x 10^-7. H2CO3 --> H+ + HCO3-... this means that H2CO3 is...
poor hydrogen-ion donor
What is the charge of a cation?
positive
Which of the following elements has the smallest first ionization energy? (sodium, calcium, potassium, magnesium)
potassium
Which of the following compounds is a strong electrolyte? (ammonia, acetic acid, sugar, potassium sulfate)
potassium sulfate
narrowness of range of measurements
precision
a substance formed in a chemical reaction
product
C3H8
propane
C3H7OH
propanol
a positively charged subatomic particle
proton
particles that are found in the nucleus of an atom
protons and neutrons
energy needed to move an electron from one energy level to another
quantum
starting substance in a chemical reaction
reactant
substance that donates electrons (agent)
reducing agent
A compound held together by ionic bonds is called....
salt
When an acid reacts with a base, what compounds are formed?
salt and water
solution containing maximum amount of solute
saturated solution
known or estimated in a measurement
significant figure
a covalent bond in which only one pair of electrons is shared
single covalent bond
Which element increases its oxidation number in the following reaction? 2Na + 2H2O --> 2NaOH + H2
sodium
NaHCO3
sodium bicarbonate
Which of the following substances is the most soluble in water? (sodium chloride, methane, bromine, carbon)
sodium chloride
Which of the following compounds is an electrolyte? (rubbing alcohol, sugar, carbon tetrachloride, sodium hydroxide)
sodium hydroxide
Na2O
sodium oxide
Na2SO4
sodium sulfate
which state of matter is characterized by having a definite shape and definite volume?
solid
Which of the following occurs as temperature increases? (solubility decreases, solubility increases, solubility remains the same, molarity doubles)
solubility increases
dissolved particle
solute
solute ions or molecules are surrounded by solvent molecules
solvation
dissolving medium
solvent
What occurs in salvation?
solvent molecules surround solute ions
the ∆Hsoln is... (always negative, always positive, sometimes both, always 0)
sometimes positive, sometimes negative
quantity of heat required to change the temperature of 1 g of a substance by 1 C
specific heat
discrete bundle of electromagnetic energy
spectrum
shape of XeF4
square planar
law of conservation of mass
states that the mass of the reactants is equal to the mass of the products
average kinetic energy of water molecules is greatest in... (steam at 100 C, liquid water at 90 C, liquid water at 373 K, ice at O C)
steam at 100 C
a depiction of the arrangement of atoms in molecules and polyatomic ions
structural formula
What is an acid according to Arrhenius?
substance that ionizes to yield protons in aqueous solution
Which of the following is NOT a common hydrate? (epsom salt, borax, sugar, alum)
sugar
Which of the following mixtures is NOT a colloid? (fog, milk, paint, sugar water)
sugar water
Which of the following is NOT a cation? (Iron iii ion, sulfate, Ca+2, mercurous ion)
sulfate
SO2
sulfur dioxide
H2SO4
sulfuric acid
H2SO3
sulfurous acid
how can you calculate the change in enthalpy
sum of products minus sum of reactants
If a chrystal added to an aqueous solution causes many particles to come out of the solution, the original solution was...
supersaturated
solution containing more solute than can theoretically dissolve at a given temperature
supersaturated solution
inward force tending to minimize surface area of a liquid
surface tension
interferes with hydrogen bonding between water molecules
surfactant
mixture in which particle size averages greater than 1000 nm in diameter
suspension
shape of the methane molecule
tetrahedral
What is the basis of a metallic bond?
the attraction of metal ions to mobile electrons
What does the symbol ∆H stand for?
the heat of reaction for a chemical reaction
Which is a typical characteristic of an ionic compound? (electron pairs are shared among atoms, the ionic compound has a low solubility in water, the ionic compound is described as a molecule, the ionic compound has a high melting point)
the ionic compound has a high melting point
What does the number 84 in the name krypton-84 represent?
the mass number
If the volume of a container of gas is reduced, what will happen to the pressure inside the container?
the pressure will increase
What happens to the solubility of a gas, in a liquid, if the partial pressure of the gas above the liquid decreases?
the solubility decreases
For group 2A metals, which electron is the most difficult to remove?
the third
If a liter of water is heated from 20 C to 50 C, what happens to its volume?
the volume increases
the maximum amount of product that could be formed from given amounts of reactants
theoretical yield
Which of the following is NOT a characteristic of most ionic compounds? (they are solids, they have low melting points, when melted they conduct an electric current, they are composed of metallic and nonmetallic elements)
they have low melting points
What characteristic of metals make them good electrical conductors?
they have mobile valence electrons
how many significant figures are in the measurement 40,500 mg?
three
Sn3(PO4)2
tin (II) phosphate
Why do atoms share electrons in covalent bonds?
to attain a noble-gas electron configuration
type of element characterized by the presence of electrons in the d orbital
transition metal
an electron in the highest occupied energy level of an atom
valence electron
What is the name given to the electrons in the highest occupied energy level of an atom?
valence electrons
gaseous state of substance that is a liquid or solid at room temperature
vapor
a measure of the force exerted by a gas above a liquid
vapor pressure
According to the Heisenberg uncertainty principle, if the position of a moving particle is known, what other quantity CANNOT be known?
velocity
this is conserved only in reactions where the temperature is constant and the number of moles of gaseous reactants is the same as that of gaseous products
volume
Which of the following substances has the highest specific heat? (steel, water, alcohol, chloroform)
water
another term for the water of hydration
water of crystallization
Which of the following is an example of a phase? (pressure, water vapor, temperature, triple point)
water vapor
distance between wave crests
wavelength
compound that ionizes incompletely in aqueous solution
weak electrolyte
the force of gravity on an object
weight
the first step in balancing a redox reaciton by the half-reaction method
write the equation showing ions seperately
Use the information below to calculate the enthalpy change for the following reaction. 2NO2 --> N2O4; N2 + 2O2-->2NO2 (∆H=67.7 kJ); N2 + 2O2--> N2O4 (∆H= 9.7 kJ)
∆H= -58
