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WorksheetsThou Shalt Not Forget AP Chem
Total questions: 95
Worksheet time: 3625secs
What type of alloy is made when the radii of the atoms are similar in size?
interstitial
substitutional
Which atom has the negative dipole in this molecule?
Hydrogen
Fluorine
Neither
What type of bond forms between hydrogen and chlorine?
polar covalent
non-polar covalent
ionic
hydrogen bond
What type of alloy is this?
Interstitial
Substitutional
What is the total # of covalent bonds carbon can form when drawing a Lewis structure?
12
6
4
8
Are asymmetrical molecules polar or nonpolar?
Polar
non-polar
neither
What is the hybridization of carbon in CH4?
sp3
sp
sp2
Count the number of sigma and pi bonds in this molecule:
13 sigma, 1 pi
14 sigma, 2 pi
1 sigma, 14 pi
2 sigma, 13 pi
Choose the correct shape for this molecule:
Trigonal planar
Trigonal pyramidal
Tetrahedral
Linear
When an electron is in a higher energy level, it is farther away from the nucleus and has less Coulombic attraction to the nucleus and is therefore easier to remove
True
False
The greater the electronegativity difference between 2 atoms, the more polar the bond becomes.
True
False
When calculating ΔH from chemical equations with known enthalpies, if you double reaction coefficients, what happens to the overall ΔH value?
it doubles
it is squared
the sign changes
nothing
When calculating ΔH from chemical equations with known enthalpies, if you reverse the reaction, what happens to the overall ΔH value?
the sign for ΔH changes
it doubles
it is squared
nothing
A triple bond is composed of
1 sigma bond
1 pi bond
2 pi bonds
1 sigma and 2 pi bonds
Which of these is false in terms of speeding up reactions?
Adding a catalyst lowers the activation energy
increasing reactant concentration increases collisions
increasing surface area decreases collisions
increasing temperature increases collisions
When calculating ΔH from chemical equations with known enthalpies, if you double reaction coefficients, what happens to the overall ΔH value?
it doubles
it is squared
the sign changes
nothing
If the pressure of a system is increased, which direction will equilibrium shift?
toward the side with less moles of gas
toward the side with more moles of gas
it will not shift
Which of the following is a strong acid?
Hydrochloric acid
Acetic acid
Ammonia
Water
What is the pH of a neutral solution at 25°C?
7
0
14
1
What is the main product of the combustion of hydrocarbons?
Carbon dioxide and water
Oxygen and water
Hydrogen and carbon monoxide
Nitrogen and water
Which element is most electronegative?
Fluorine
Oxygen
Chlorine
Nitrogen
What is the primary intermolecular force in water?
Hydrogen bonding
Ionic bonding
Van der Waals forces
Dipole-dipole interactions
What is the oxidation state of oxygen in most compounds?
-2
+2
0
-1
What is the main characteristic of a buffer solution?
It resists changes in pH
It changes color with pH
It has a pH of 7
It is a strong acid
Which of the following is an example of an exothermic process?
Combustion of gasoline
Melting of ice
Evaporation of water
Photosynthesis
What is the role of a catalyst in a chemical reaction?
It lowers the activation energy
It increases the activation energy
It is consumed in the reaction
It changes the equilibrium position
What is the half-life of a 1st order reaction process?
t1/2 = 0.693/k
t1/2 = k/0.693
t1/2 = k
t1/2 = 1/k
What is the effect of increasing the temperature on the rate of a reaction?
Decreases the number of collisions
Decreases the concentration of reactants
Increases the number of effective collisions
No effect on the rate of reaction
What is the sign for ΔH in an exothermic reaction?
Positive
Negative
Zero
Variable
Which of the following is a strong acid?
HNO_3
CH_3COOH
NH_3
H_2O
What is the relationship between the strength of an acid and the strength of its conjugate base?
The stronger the acid, the stronger its conjugate base
The stronger the acid, the weaker its conjugate base
The strength of the acid does not affect the strength of its conjugate base
The weaker the acid, the stronger its conjugate base, but only for strong acids
What is the pH of a solution if [H^+] = 10^-4 M?
4
7
10
14
What is the percent ionization of a weak acid in terms of hydrogen ion concentration and acid molarity?
[H⁺] / Mₐ
Mₐ / [H⁺]
[H⁺] * Mₐ
[H⁺] + Mₐ
If a salt contains a conjugate base of a weak acid, what is the resulting pH of the solution likely to be?
Neutral
Slightly acidic
Slightly basic
Highly acidic
What is the pH at the half equivalence point for a titration between a weak acid and a strong base?
Equal to the pKa of the weak acid
Greater than the pKa of the weak acid
Less than the pKa of the weak acid
Equal to 7
Thermodynamically favorable reactions have what sign for ΔG?
Positive (+ΔG)
Negative (−ΔG)
Zero (ΔG = 0)
ΔG is not related to thermodynamic favorability
What is the relationship between ΔG and the equilibrium constant (Keq) when ΔG is negative?
Keq < 1
Keq = 1
Keq > 1
Keq = 0
What is the value of ΔG at equilibrium?
Positive (+ΔG)
Negative (−ΔG)
Zero (ΔG = 0)
ΔG cannot be determined at equilibrium
When using the equation ΔG° = −RT lnK, what is the unit for the gas constant R?
J/mol
J/mol K
kJ/mol
kJ/mol K
Where does oxidation always occur in an electrochemical cell?
At the cathode
At the anode
In the salt bridge
In the external circuit
In an electrochemical cell, how do electrons flow?
From anode to cathode
From cathode to anode
From the salt bridge to the anode
From the external circuit to the cathode
What happens to the mass of the cathode and the anode when a battery is discharged?
The cathode gains mass and the anode loses mass.
The cathode loses mass and the anode gains mass.
Both the cathode and anode gain mass.
Both the cathode and anode lose mass.
If the cell potential (E° cell) of the battery decreases, what is the effect on the Gibbs free energy (ΔG°)?
ΔG° becomes positive.
ΔG° becomes negative.
ΔG° remains the same.
ΔG° becomes zero.
What is the order of a reaction if doubling the concentration of a reactant quadruples the rate?
Zero
First
Second
Third
What is the unit for the rate constant (k) for a first-order reaction?
s^-1
M/s
M^-1s^-1
M^2s^-1
In a reaction mechanism, what is the role of the intermediate?
It speeds up the reaction
It is consumed in one step and regenerated in another
It is the final product
It is the reactant
Which curve represents the most particles in this Maxwell-Boltzmann curve (# of particles vs. speed)?
Black (peak on the left)
Red (peak in the middle)
Blue (peak on the right)
They all have the same number of particles
What is NOT a way to speed up a reaction
Add a catalyst
Decrease the volume
Increase the concentration of reactants
Increase surface area of the solid
Decrease the pressure
What is the rate law for the reaction with this slow elementary step? A --> B + C
rate = k[A]2
rate = k[B]2
rate = k[A][B]
rate = k[A]
What is the rate law for the reaction with this slow elementary step? A + 2B --> D + C
rate = k[A]2
rate = k[A][B]2
rate = k[A][B]
rate = k[A]
What order is the half life of Carbon14?
Zero
First
Second
If you quadruple the concentration and the rate quadruples, what order is this reaction?
zero
first
second
At equilibrium, rates of the forward and reverse reaction are...
The same
Not the same
A system at equilibrium
Must have reactants and products
Must have products only
Must have reactants only
At what time does the system first reach equilibrium?
24s
40s
60s
80s
If a K value is greater than 1,
more products are present at equilibrium
more reactants are present at equilibrium
If a K value is VERY large,
the reaction has essentially gone to completion
there are more reactants present at equilibrium
If K < Q, the reaction will proceed in the...
reverse direction to reach equilibrium
forward direction to reach equilibrium
To calculate the K of an overall reaction from individual reaction K values, the individual K values are
added
subtracted
multiplied
divided
Given the following equilibrium equation,
A (g) + 2B (g) ⇄ AB2 (g) ΔH > 0, which of the following changes will increase the amount of AB2 in the vessel?
Decreasing the temperature
Increasing the concentration of A
Removing a small amount of B
Decreasing the pressure
The following system at equilibrium is exothermic. If the temperature is increased...
A (g) + 2B (g) ⇄ AB2 (g)
[A] will increase the most
[B] will increase the most
[AB2] will increase the most
In a Ksp expression, we always assume that the reactant is made up of
the solid precipitate
the aqueous ions
If Ksp >1, we say the salt is...
soluble
insoluble
What is the oxidation number of N in NO21-?
0
-1
2
3
Chose the salts that are soluble:
sodium
potassium
nitrates
ammonium
Losing electrons is ________________, gaining electrons is ________________
oxidation, reduction
reduction, oxidation
Bases
donate electrons
accept electrons
donate protons
accept protons
Acids
donate electrons
donate protons
accept protons
donate protons
What formula do we use for dilution calculations?
M1V1=M2V2
D=m/V
V1=M2
Total Volume/Partial Volume
1.What type of reaction is this?
3O2 + 2FeCl3 --> 2Fe2O3 + 3Cl2
Single Displacement
Decomposition
Double Displacement
Combustion
What is a limiting reactant?
The reactant that runs out first
The reactant that has the lowest mass
The reactant with the smallest coefficient
The reactant with the lowest molar mass
What is the formula for calculating % yield?
actual/theoretical *100
theoretical/actual *100
In an exothermic reaction, the sign of ΔH is ____ and the reaction feels ______
(-), hot
(+), hot
(-), cold
(+), cold
Freezing is an _________________________ process
Endothermic
Exothermic
Breaking bonds is _________________. Forming bonds is ______________________
endothermic, exothermic
exothermic, endothermic
According to Hess' Law, if you double the coefficients of a reaction, ΔH will ________________________
Stay the same
Double
Quadruple
Halve
According to Hess' Law, if you reverse a reaction, ΔH will ________________________
Change signs
Double
Be inversed
Halve
_____ Hydrogen-Hydrogen single bond/s are broken and _____ Carbon-Hydrogen single bond/s formed
6; 8
2; 8
2; 10
6; 10
Bond enthalpy is the amount of energy is takes to break __________ of a bond.
one mole
one gram
the activation energy
the binding energy
What are the units of ΔHrxn?
kJ
J
kJ/mol
J/mol
Endothermic
absorb energy
release energy
On a potential energy diagram for an endothermic reaction,
the potential energy of the reactants is greater than the potential energy of the products
the potential energy of the reactants is less than the potential energy of the products
the potential energy of the reactants is equal to the potential energy of the products
Using bond energies to solve for enthalpy,
ΔH = Bond broken - bonds formed
undefined = Bond formed- bonds broken
undefined = products - reactants
undefined = reactants- products
When a molecular solid melts or boils, which breaks?
Intermolecular forces
Intramolecular bonds
Name a property that increases as Intermolecular Forces increase.
Vapor pressure
Conductivity
Melting point
Solubility
“More polarizable” refers to which Intermolecular Force?
hydrogen bonding
london dispersion
dipole dipole
What is an example of a covalent network solid?
Salt
Diamond
Sugar
Water
P and V are ___________________ related?
inversely
directly
The greater the molar mass of a gas, the_________________ it moves.
faster
slower
Fill in the blanks: germanium is a ________________, hydrogen is a _________________ and uranium is a ________________
metal, non-metal, metalloid
metalloid, non-metal, metal
non-metal, metal, metalloid
List ALL the Intermolecular forces that exist in PCl3
hydrogen bonding, london dispersion
london dispersion, hydrogen bonding, dipole dipole
london dispersion, dipole dipole
london dispersion
Name a property that decreases as Intermolecular Forces increase.
Vapor pressure
Conductivity
Melting point
Solubility
Real gases behave most like an ideal gas at what conditions of temperature and pressure?
High T, Low P
High P, Low T
High V, Low T
This is a representation of a hydrogen bond.
True
False
SiO2 (quartz) and diamonds are ____________________, and they have very high boiling/melting points.
covalent network solids
ionic solids
molecular solids
interstitial alloys
