WorksheetsIB Chemistry HL 11 Spring Final Review (Revised 2024)
Total questions: 22
Worksheet time: 1hrs 10mins
Which of the following molecules has a trigonal pyramidal geometry?
BF3
SO3
SO3-2
CO3-2
What is the formal charge for carbon in H-C≡N: ?
-1
0
1
2
Which of the following is a network covalent compound?
NaCl
CH4
SiO2
Fe
Which of the following would have the weakest London dispersion forces?
I2
Br2
Cl2
F2
Which of the following organic molecules has hydrogen bonding?
Ether
Ketone
Halocarbon
Alcohol
Which of the following would make a real gas least like an ideal gas?
Low Pressure
High Temperature
Strong Intermolecular Forces
Infinitely large container
In relation to the triple point, when is a substance guaranteed to be a vapor?
At pressures lower than, and temperatures higher than the triple point.
At pressures lower than, and temperatures lower than the triple point.
At pressures higher than, and temperatures higher than the triple point.
At pressures higher than, and temperatures lower than the triple point.
Write the equilibrium constant expression for the following reaction. I2 (s) + H2 (g) ↔ 2 HI (g)
K = [HI]2 / [H2][I2]
K = [HI]2 / [H2]
K = [H2][I2] / [HI]2
K = [H2] / [HI]2
How would the value of an equilibrium constant change if the reaction was reversed and cut in half?
Take the square root of the value and change the sign.
Take the square of the inverse of the value.
Take the square root of the inverse of the value.
Take the square of the value and change the sign.
What does a really small equilibrium constant mean?
At equilibrium the system is mostly reactants, and very few products.
At equilibrium the system is mostly products, and very few reactants.
At equilibrium the system has nearly equal amounts of reactants, and products.
At equilibrium both the forward and reverse reactions slow down to an imperceptible speed.
N2 (g) + 3 H2 (g) --> 2 NH3 (g) ΔH= -200 kJ
What temperature and pressure combination would maximize the yield of ammonia?
High temperature and pressure.
Low temperature and pressure.
High temperature and low pressure.
Low temperature and high pressure.
For the reaction AgCl (s) <--> Ag+1 (aq) + Cl-1 (aq), what does it mean if Q is larger than K?
The solution is unsaturated.
The solution is saturated.
The solution is supersaturated
What is the conjugate base of H2PO4-1?
H3PO4
H2PO4-1
HPO4-2
PO4-3
Which of the following is not true for a pH of 2.0 at 25 °C?
The solution is acidic.
[H3O+1] > [OH-1]
[H3O+1] = 1.0 x 102 M
pOH = 12.0
Which of the following salts would lower the pH of a solution?
NaCl
KNO3
NH4Cl
K2CO3
Which of the following would produce a buffer solution?
100 mL of 1.0 M KOH with 100 mL of 1.0 M HF
100 mL of 1.0 M KOH with 50 mL of 1.0 M HF
50 mL of 1.0 M KOH with 100 mL of 1.0 M HF
50 mL of 1.0 M KOH with 50 mL of 1.0 M HF
At what point on the titration curve does pH = pKa ?
A
B
C
D
What is the oxidation number of Cr in Cr2O7-2 ?
+7
+6
+3
+2
When the half-reaction Ag (s) --> Ag2O (aq) is balanced in acidic solution, where do the electrons and hydrogen ions show up?
Both electrons and hydrogen ions are added to the reactant side.
Both electrons and hydrogen ions are added to the product side.
Electrons are added to the product side and hydrogen ions to the reactant side.
Electrons are added to the reactant side and hydrogen ions to the product side.
What is the voltage when the following half-cells are connected to form a voltaic cell?
Na+ + e- → Na E = -2.71 V
Zn+2 + 2 e- → Zn E = -0.76 V
6.18 V
3.47 V
4.66 V
1.95 V
In the cell Na | Na+1 || Zn+2 | Zn , how would increasing the concentration of Na+1 affect the voltage of the cell?
The voltage would increase
The voltage would decrease
The voltage would stay the same
An object has a mass of 2.00 ± 0.01 g and a volume of 4.00 ± 0.05 mL. What is the density of this object in g/mL with respect to uncertainties?
0.500 ± 0.009 g/mL
0.50 ± 0.09 g/mL
0.50 ± 0.01 g/mL
0.500 ± 0.001 g/mL
