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WorksheetsAP Chem units 1-5 Review
Total questions: 80
Worksheet time: 1hrs 10mins
A 5.00 g sample of a compound consisting of calcium and chlorine contains 1.82 g of calcium and 3.23 g of chlorine. What is the empirical formula?
CaCl2
Ca2Cl4
Ca2Cl2
Ca4Cl2
How many molecules are in 2.5 mol of NaCl?
1.5 x 1024 molecules
1.5 molecules
4.15 molecules
1.5 x 1023 molecules
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
In this molecule, Carbon has a formal charge of ____ and Nitrogen has a formal charge of _____.
0, 0
1, 0
0, -1
-1, 0
Combustion reactions produce what two substances?
Water Vapor and Carbon Dioxide
Carbon Dioxide and Oxygen
Oxygen and Water Vapor
As the electronegativity difference between 2 atoms increases, the polarity of the bond ____________________
increases
decreases
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
What is the bond angle in BF3?
90
120
109.5
180
What is the bond angle in H2O?
120
90
180
104.5
Are asymmetrical molecules polar or nonpolar?
Polar
non-polar
neither
What is the bond angle in NH3
120
107.3
180
90
What is the hybridization of carbon in CH4?
sp3
sp
sp2
What is the hybridization for carbon in CO2
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
Why are asymmetrical molecules polar?
Their dipoles do not cancel
Their dipoles cancel
What is the hybridization for an oxygen in CO2
sp3
sp
sp2
When a molecular solid melts or boils, which breaks?
Intermolecular forces
Intramolecular bonds
What is the total # of covalent bonds carbon has to make when drawing a Lewis structure?
12
6
4
8
Which of these molecules could best be represented by the ball-and-stick model shown?
BeH2
CO2
H2O
SO2
Which of the following substances contains both ionic and
covalent bonds?
NH3
CH4
NaOH
C2H5OH
What type of bonding is found within a water molecule?
ionic bonding
polar covalent bonding
nonpolar covalent bonding
hydrogen bonding
Dinitrogen monoxide, N20, has two double bonds. The general structure is N=N=O. What is the formal charge on the oxygen atom in this molecule?
zero
positive one (+1)
positive two (+2)
negative one (-1)
The Lewis structure of which compound is best represented with resonance structures?
MgCl2
CO2
SO3 2-
OCl2
The molecule shown above represents alanine, one of the simplest amino acids. This amino acid is considered nonessential to the human diet as it can be synthesized in the body from other compounds.
Which statement is correct concerning alanine?
Each carbon atom is sp3 hybridized.
The hybridization of the nitrogen atom is sp2.
All bond angles are approximately 109.50.
The molecule contains 12 sigma and 6 pi bonds.
How many unbonded pairs of electrons are found on the alanine molecule?
0
1
3
5
How many of the following molecules have a measurable dipole moment?
S03 CCl4 PF3 BH3
1
2
3
4
Which best describes the bonding in the cyanide ion (CN-)?
3 (sigma) bonds
2 (sigma) bonds and I (pi) bond
1 (sigma) bond and 2 (pi) bonds
3 (pi) bonds
Which is correct for the hybridization and molecular geometry of phosphorus tribromide?
sp3, tetrahedral
sp3, trigonal pyramidal
sp2, trigonal pyramidal
sp2, trigonal planar
Which bond is the most polar?
F-O
H-O
Na -O
Sn-O
The effect of lone pairs of electrons on molecular geometry is
to push other atoms closer together because lone pairs are
localized on only one nucleus, so they spread out more.
to allow the other atoms to be further apart because lone pairs
take up less space than bonding pairs.
to create an aysmmetical distribution of the electrons within
the atom, thus creating a polar molecule by creating dipoles.
to help to create resonance structures through the formation of
pi bonds.
Why can a molecule with the structure of NBr5 not exist?
Nitrogen only has two energy levels and is thus unable to expand its octet.
Bromine is much larger than nitrogen and cannot be a terminal atom in this molecule
It is impossible to complete the octets for all six atoms using only valence electrons.
Nitrogen does not have a low enough electronegativity to be the central atom of this molecule.
Which of the following compounds would have the highest lattice energy?
LiF
MgCl2
CaBr2
C2H6
The six carbon atoms in a benzene molecule are shown in different resonance forms as three single bonds and three double bonds. If the length of a single carbon—carbon
bond is 154 pm and the length of a double carbon—carbon bond is 133 pm, what length would be expected for the carbon—carbon bonds in benzene?
126 pm
133 pm
140 pm
154pm
What is the molecular geometry in the structure A?
Tetrahedral
Trigonal Planar
Trigonal Pyramidal
Octahedral
Which of the following statements regarding the structure B is true?
The double bonds must be located opposite of each other due to additional electron repulsion.
It is a more polar molecule than the molecule represented by structure A.
The bonds in the molecule are weaker than those in structure A.
All bonds in the molecule are identical to each other.
Which structure is more likely to correspond with the actual Lewis diagram for the sulfate ion?
Structure A; single bonds are more stable than double bonds
Structure A; it has the most unshared pairs of electrons
Structure B; there are more possible resonance structures
Structure B; fewer atoms have formal charges
Is this a chemical or physical process? CO2(g) → C(s) + O2(g)
chemical
physical
both chemical and physical
Is this a chemical or physical process? H2O(s) → H2O(l)
chemical
physical
both chemical and physical
Is this a chemical or physical process? MgCl2(s) → Mg+2(aq) + 2Cl-1(aq)
chemical
physical
both chemical and physical
What are the spectator ions in this reaction? Fe+3(aq) + 3Cl-1(aq) + Na+1(aq) + OH-1(aq) → Fe(OH)3(s) + Na+1(aq) + Cl-1(aq)
Fe+3 and Cl-1
Na+1 and Cl-1
Fe+3 and Na+
Na+1 and OH-1
What is the net ionic equation for this reaction? Fe+3(aq) + 3Cl-1(aq) + Na+1(aq) + OH-1(aq) → Fe(OH)3(s) + Na+1(aq) + Cl-1(aq)
Fe+3 (aq) + OH-1(aq) → Fe(OH)3(s)
Na+1(aq) + Cl-1(aq) → NaCl(aq)
Fe+3(aq) + 3Cl-1(aq) + Na+1(aq) + OH-1(aq) → Fe(OH)3(s) + Na+1(aq) + Cl-
Precipitates are ____________________________ in solution.
miscible
soluble
insoluble
In this reaction...
CH3NH2 + H2O ↔ CH3NH3+ + OH-
CH3NH2 can be classified as which of the following? (HINT...follow the H+!!!)
A Brønsted-Lowry base
A Brønsted-Lowry acid
An Arrhenius acid
An Arrhenius base
Balance this equation:
____ Zn + _____HCl → _____ ZnCl2 + _______H2
1,2,1,2
2,1,1,2
1,2,1,1
1,3,1,2
NH3 + H2O ↔ NH4+ + OH-
What is H2O in this reaction?
acid
base
conjugate acid
conjugate base
What order is this graph?
Zero
First
Second
Third
What order is this graph?
Zero
First
Second
Third
If you quadruple the concentration and the rate quadruples, what order is this reaction?
zero
first
second
The particles under the purple curve (middle) have an average Kinetic Energy that is proportional to of 500K
True
False
Which step of a reaction mechanism determines the rate?
the slow step
the fast step
the first step
the second step
What order is the half life of Carbon14?
Zero
First
Second
What is the unit for the rate constant (k) for 2nd order reactions?
s-1
M/s
M-1s-1
How does a catalyst speed up a reaction?
Adding more reactant
Providing a pathway that has a lower activation energy
Increasing the activation energy
Increasing binding energy
___________ are produced in one step and used up in a later step and __________________ are present and unchanged in the reactants and the products
intermediates, catalysts
catalysts, intermediates
If a “reaction profile” has a taller ‘hill’ (or activation energy) then the reaction is ____________________?
Faster
Slower
What are the 2 characteristics that an effective collision must have? SELECT TWO
Enough energy to overcome Ea
Molecules in the correct orientations
High enough temperature
Apporpriate intermediates present
What is the rate law for the reaction with this slow elementary step? A + A --> B + B
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 --> 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 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
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
Which curve in this Maxwell-Boltzmann distribution represents the highest proportion of particles moving the fastest (# of particles vs. speed)?
Black (peak on the left)
Red (peak in the middle)
Blue (peak on the right)
All particles are moving at the same speed
What order of reaction has a half-life that does not change regardless of the initial concentration?
Zero
First
Second
Third
