FINAL EXAM REVIEW
*CHEM 111*
THINGS TO KNOW ABOUT THE FINAL EXAM
My son is 1.1 meters tall, Can he ride the coaster by himself?
(rules for the ride: must be at least 48’’)
My son is 1.1 meters tall, Can he ride the coaster by himself?
(rules for the ride: must be at least 48’’)
What is 375 K in degrees celsius?
What is 375 K in degrees celsius?
Determine the amount of significant figures in each of the following measurements...
0.006 L
0.0605 dm
60.5 mg
9.60 x 10^3 g
2900 g
Determine the amount of significant figures in each of the following measurements...
0.006 L (1)
0.0605 dm (3)
60.5 mg (3)
9.60 x 10^3 g (3)
2900 g (2)
What is the mass in kg of a gold bar that is 25 cm long, 7.5 cm wide, and 3.5 cm thick?
density of gold: 19.32 g/cm3
1 in = 2.54 cm (exactly)
12 in = 1 foot
What is the mass in kg of a gold bar that is 25 cm long, 7.5 cm wide, and 3.5 cm thick?
Answer: 13 kg of gold density of gold: 19.32 g/cm3
1 in = 2.54 cm (exactly)
12 in = 1 foot
The density of water at 40 C is 0.992 g/mL. What is
the volume of 2.50 g of water at this temperature?
The density of water at 40 C is 0.992 g/mL. What is
the volume of 2.50 g of water at this temperature?
What subatomic particles are found in a typical gold (Au) atom, gold-197?
A. 79 protons, 118 neutrons, 78 electrons
B. 197 protons, 118 neutrons, 197 electrons
C.118 protons, 79 neutrons, 79 electrons
D. 79 protons, 118 neutrons, 79 electrons
What subatomic particles are found in a typical gold (Au) atom, gold-197?
A. 79 protons, 118 neutrons, 78 electrons
B. 197 protons, 118 neutrons, 197 electrons
C.118 protons, 79 neutrons, 79 electrons
D. 79 protons, 118 neutrons, 79 electrons
The most common isotopes of Potassium are K - 39 & K - 41. K - 39 has a natural abundance of 93.26% and a mass of 38.96371 amu. K - 41 has a natural abundance of 6.73% and a mass of 40.96183 amu. What is the average atomic mass of Potassium?
The most common isotopes of Potassium are K - 39 & K - 41. K - 39 has a natural abundance of 93.26% and a mass of 38.96371 amu. K - 41 has a natural abundance of 6.73% and a mass of 40.96183 amu. What is the average atomic mass of Potassium?
Name the seven diatomic elements and their standard states of matter
Name the seven diatomic elements and their standard states of matter
H2 (g) N2(g) O2(g) F2(g)
Cl2 (g)
Br2 (l)
I2 (s)
What is the other element that is not solid at room temp at standard state?
How many atoms of magnesium are in 69.3 g of Mg?
How many atoms of magnesium are in 69.3 g of Mg?
Which of these values could be used to represent the potential energy of the system when a proton and electron are nearer to eachother?
Which of these values could be used to represent the potential energy of the system when a proton and electron are nearer to eachother?
What is the frequency of violet light with a wavelength of 420 nm?
What is the frequency of violet light with a wavelength of 420 nm?
Answer: 7.1 X 10^14 Hz
Find the energy of a photon of 290. nm UV light.
Find the energy of a photon of 290. nm UV light.
Answer: 6.85x 10^-19 joules
What is the energy change for n=3 to n=5
What is the energy change for n=3 to n=5
Answer: 1.6 X 10 ^-19 Joules
Which statement is correct?
a. There are 3 subshells in a p orbital.
b. There are 3 shells(n) in a p subshell.
c. Electrons travel along the surface of an orbital.
d. A p subshell can hold up to 6 electrons.
e. Two of these are correct.
Which statement is correct?
a. There are 3 subshells in a p orbital.
b. There are 3 shells(n) in a p subshell.
c. Electrons travel along the surface of an orbital.
d. A p subshell can hold up to 6 electrons.
e. Two of these are correct.
Which statement is false?
A . Comparing 2px → 2py → 2pz orbitals: energies arent the same.
b. Comparing 2p → 3p → 4p subshells: size increases.
c. Comparing 2p → 3p → 4p subshells: energies increase.
d. Comparing 3s → 3p → 3d subshells in a H atom: energies are the same.
e. Comparing 3s → 3p → 3d subshells in a multielectron atom: energies increase.
Which statement is false?
A . Comparing 2px → 2py → 2pz orbitals: energies arent the same.
b. Comparing 2p → 3p → 4p subshells: size increases.
c. Comparing 2p → 3p → 4p subshells: energies increase.
d. Comparing 3s → 3p → 3d subshells in a H atom: energies are the same.
e. Comparing 3s → 3p → 3d subshells in a multielectron atom: energies increase.
Go over how to determine electron configuration
Write the full and condensed/noble gas configuration of phosphorus.
Write the full and condensed/noble gas configuration of phosphorus.
Full: 1s2 2s2 2p6 3s2 3p3
Condensed: [Ne] 3s2 3p3
Which of these statements correctly describe(s) shielding?
I. Electrons shield each other from experiencing the full charge of the nucleus
II. Valence electrons are most shielded by core electrons
III. Valence electrons are most shielded by other valence electrons
a. I
b. II
c. III
d. I and II
e. I and III
Which of these statements correctly describe(s) shielding?
I. Electrons shield each other from experiencing the full charge of the nucleus
II. Valence electrons are most shielded by core electrons
III. Valence electrons are most shielded by other valence electrons
a. I
b. II
c. III
d. I and II
e. I and III
Which are related to a process in which energy is absorbed by the atom
Which are related to a process in which energy is absorbed by the atom
Write the full electron configuration for Mn4+ ion
Write the full electron configuration for Mn4+ ion
Answer: 1s2 2s2 2p6 3s2 3p6 3d3
Arrange these species in increasing radius:
a. Cl − < Ar < K+
b. Ar < K+ < Cl −
c. Cl − < K+ < Ar
d. K+ < Ar < Cl −
e. Ar < Cl − < K+
Arrange these species in increasing radius:
a. Cl − < Ar < K+
b. Ar < K+ < Cl −
c. Cl − < K+ < Ar
d. K+ < Ar < Cl −
e. Ar < Cl − < K+
Which compound has the greatest lattice energy?
Which compound has the greatest lattice energy?
Name these five compounds...
Name these five compounds...
A 360 mL (12 oz ) serving of coke contains 39. G of sucrose, how many molecules of sucrose are in the 2.0 L bottle? Sucrose: C12H22O11
A 360 mL (12 oz ) serving of coke contains 39. G of sucrose, how many molecules of sucrose are in the 2.0 L bottle? Sucrose: C12H22O11
Answer: 3.8 x 10^23 molecules
In a 100-g sample of ibuprofen, there are 75.69 g C, 8.80 g H, and 15.51 g O. What is the empirical formula of ibuprofen?
In a 100-g sample of ibuprofen, there are 75.69 g C, 8.80 g H, and 15.51 g O. What is the empirical formula of ibuprofen?
Answer: C13H18O2
Ascorbic acid (vitamin C) has mass 40.92% C 4.58% H 54.50% O. Absorbic acid has a molar mass of 176.12 g/mol. What is its molecular formula?
Ascorbic acid (vitamin C) has mass 40.92% C 4.58% H 54.50% O. Absorbic acid has a molar mass of 176.12 g/mol. What is its molecular formula?
Answer: C6H8O6
What is the increasing order for bond strength?
What is the increasing order for bond strength?
What is the best structure for formaldehyde( CH2O)?
What is the best structure for formaldehyde( CH2O)?
Draw the resonance structures for the nitrate ion, NO3 – , found in some fertilizers. How many equivalent resonance structures are there?
a. 1
b. 2
c. 3
d. 4
e. 5
Draw the resonance structures for the nitrate ion, NO3 – , found in some fertilizers. How many equivalent resonance structures are there?
a. 1
b. 2
c. 3
d. 4
e. 5
Which compound does not have an expanded octet?
Which compound does not have an expanded octet?
What are the other two exceptions to the octet rule other than expanded octet?
Review bond line structures
Acetic acid makes vinegar sour. For the three central atoms in acetic acid, identify the electron geometry, molecular geometry, and bond angles.
Acetic acid makes vinegar sour. For the three central atoms in acetic acid, identify the electron geometry, molecular geometry, and bond angles.
C1: tetrahedrahl, tetrahedrahl, 109.5 degrees
C2: trigonal planar, trigonal planar, (>120, >120-top/
<120 (bottom)
O: tetrahdedrahl, bent, <109.5 degrees
Is this molecule polar?
List the substances by increasing boiling point: CH3CH3, CH2O, CH3OH
a. CH3OH < CH2O < CH3CH3
b. CH3CH3 < CH2O < CH3OH
c. CH2O < CH3OH < CH3CH3
d. CH3OH < CH3CH3 < CH2O
e. CH2O < CH3CH3 < CH3OH
List the substances by increasing boiling point: CH3CH3, CH2O, CH3OH
a. CH3OH < CH2O < CH3CH3
b. CH3CH3 < CH2O < CH3OH
c. CH2O < CH3OH < CH3CH3
d. CH3OH < CH3CH3 < CH2O
e. CH2O < CH3CH3 < CH3OH
Review hybridization
The bond overlap between C and O in cinnamaldehyde involves the _(i)_ overlap of _(ii)_ orbitals on C and O as well as _(iii)_ overlap of _(iv)_ orbitals on C and O.
(i) (ii) (iii) (iv)
B. End on end hybridized Side by side unhybridized
C. End on end unhybridized Side by side hybridized
D. Side by side hybridized Side by side unhybridized
E. Side by side hybridized End on end unhybridized
The bond overlap between C and O in cinnamaldehyde involves the _(i)_ overlap of _(ii)_ orbitals on C and O as well as _(iii)_ overlap of _(iv)_ orbitals on C and O.
(i) (ii) (iii) (iv)
B. End on end hybridized Side by side unhybridized
C. End on end unhybridized Side by side hybridized
D. Side by side hybridized Side by side unhybridized
E. Side by side hybridized End on end unhybridized
List the coefficents in order for this balanced chemical equation:
__FeBr3 +__H2 (SO4)→ __Fe2 (SO4 )3 + __HBr
List the coefficents in order for this balanced chemical equation:
__FeBr3 +__H2 (SO4)→ __Fe2 (SO4 )3 + __HBr
Answer: 2,3,1,6
How many moles of oxygen are needed to fully react 837.4 grams of C8H18?
How many moles of oxygen are needed to fully react 837.4 grams of C8H18?
Answer: 91.63 moles O2
2.50 g of hydrogen is reacted with 30.0 L of carbon monoxide at STP. What mass of CH3OH is produced?
CO + 2 H2 → CH3OH
2.50 g of hydrogen is reacted with 30.0 L of carbon monoxide at STP. What mass of CH3OH is produced?
CO + 2 H2 → CH3OH
Answer: 19.9 g of CH3OH
How much CO is in excess?
In the reaction below, 7.0 moles of NO reaction with 5.0 moles of O2. This reaction generates 3.0 moles of NO2. What is the percent yeild for the reaction?
In the reaction below, 7.0 moles of NO reaction with 5.0 moles of O2. This reaction generates 3.0 moles of NO2. What is the percent yeild for the reaction?
Answer: 42.9 %
Reveiw of Acids and Bases
Will mixing solutions of (NH4 )2 SO4 and BaBr2 result in a reaction?
Will mixing solutions of (NH4 )2 SO4 and BaBr2 result in a reaction?
If 0.206 L of Ba(OH)2 is required to titrate 0.125 L o 0.22 M of HCl, what is the concentration of the Ba(OH)2 solution?
If 0.206 L of Ba(OH)2 is required to titrate 0.125 L o 0.22 M of HCl, what is the concentration of the Ba(OH)2 solution?
Answer: 0.067 M of Ba(OH)2
A piece of metal weighing 59.047 g was heated to 100.0 °C and then put it into 100.0 mL of water (initially at 23.7 °C). The metal and water were allowed to come to an equilibrium temperature, determined to be 27.8 °C. Assuming no heat lost to the environment, calculate the specific heat of the metal
Remember: specific heat of water is 4.184 j/gC
A piece of metal weighing 59.047 g was heated to 100.0 °C and then put it into 100.0 mL of water (initially at 23.7 °C). The metal and water were allowed to come to an equilibrium temperature, determined to be 27.8 °C. Assuming no heat lost to the environment, calculate the specific heat of the metal
Answer: s metal= 0.402 J/g oC
Remember: specific heat of water is 4.184 j/gC
Calculate DH for the reaction CH4 (g) + NH3 (g) → HCN (g) + 3 H2 (g), from the reactions.
N2 (g) + 3 H2 (g) → 2 NH3 (g) DH = -91.8 kJ
C (s, graphite) + 2 H2 (g) → CH4 (g) DH = -74.9 kJ/mole
H2 (g) + 2 C (s, graphite) + N2 (g) → 2 HCN (g) DH = +270.3 kJ
Calculate DH for the reaction CH4 (g) + NH3 (g) → HCN (g) + 3 H2 (g), from the reactions.
N2 (g) + 3 H2 (g) → 2 NH3 (g) DH = -91.8 kJ
C (s, graphite) + 2 H2 (g) → CH4 (g) DH = -74.9 kJ/mole
H2 (g) + 2 C (s, graphite) + N2 (g) → 2 HCN (g) DH = +270.3 kJ
Answer: +256.0 KJ
Use ΔHf ° values to determine the enthalpy(ΔH° rxn) for the reaction C₃H₈ (g) + 5 O₂ (g) → 3 CO₂ (g) + 4 H₂O (g)
ΔHf ° (kJ/mol)
C3H3 (g) -108.4
O2 (g) 0
CO2 (g) -393.5
H2O (g) -241.8
Use ΔHf ° values to determine the enthalpy(ΔH° rxn) for the reaction C₃H₈ (g) + 5 O₂ (g) → 3 CO₂ (g) + 4 H₂O (g)
ΔHf ° (kJ/mol)
C3H3 (g) -108.4
O2 (g) 0
CO2 (g) -393.5
H2O (g) -241.8
Answer: -2039 KJ
Based on the bond enthalpies given, What is the enthalpy for the reaction? H2+ N2+ 2C→ 2HCN
Based on the bond enthalpies given, What is the enthalpy for the reaction? H2+ N2+ 2C→ 2HCN
Answer: -1222 KJ
Review Kinetic Molecular Theory of Gases
A gas is heated from 263.0 K to 298.0 K and the volume is increased from 24.0 liters to 35.0 liters by moving a large piston within a cylinder. If the original pressure was 1.00 atm, what would the final pressure be?
A gas is heated from 263.0 K to 298.0 K and the volume is increased from 24.0 liters to 35.0 liters by moving a large piston within a cylinder. If the original pressure was 1.00 atm, what would the final pressure be?
Answer: 0.77 atm
Dry ice is carbon dioxide in the solid state. 1.28 grams of dry ice is placed in a 5.00 L chamber that is maintained at 35.1oC. What is the pressure in the chamber after all of the dry ice has sublimed?
Dry ice is carbon dioxide in the solid state. 1.28 grams of dry ice is placed in a 5.00 L chamber that is maintained at 35.1 degrees celsius. What is the pressure in the chamber after all of the dry ice has sublimed?
Answer: 1.47 atm
How many L of CO2 at 1.00 atm and 298.15 K are released from the car’s engine upon consumption of 60.0 L liquid tank gasoline? (gasoline density 0.77 kg/L, MM of C8H18: 114.2 g/mol)
C8H18 + 25/2 O2 → 8 CO2 + 9 H2O
How many L of CO2 at 1.00 atm and 298.15 K are released from the car’s engine upon consumption of 60.0 L liquid tank gasoline? (gasoline density 0.77 kg/L, MM of C8H18: 114.2 g/mol)
C8H18 + 25/2 O2 → 8 CO2 + 9 H2O
Answer: 7.92 x10 ^4 L
What amount of heat is required to vaporize 115 g of ethanol (C₂H₅OH)? (∆Hvap = 43.3 kJ/mol)
What amount of heat is required to vaporize 115 g of ethanol (C₂H₅OH)? (∆Hvap = 43.3 kJ/mol)
Answer: 108. KJ
If you put 100. g of ice at 0.0ºC into a glass, how much heat is absorbed/released by the ice when it melts and then warms to room temperature, 25.0ºC?
If you put 100. g of ice at 0.0ºC into a glass, how much heat is absorbed/released by the ice when it melts and then warms to room temperature, 25.0ºC?
Answer: 43.8 KJ
Review the difference between unsaturated, saturated, and supersaturated solutions
Which of these vitamins below are water soluble?
Which of these vitamins below are water soluble?