WorksheetsAP Chemistry Unit 2 Review
Total questions: 40
Worksheet time: 45mins
The Lewis structure of the CO32- ion is
In the nitrite ion (NO2-), __________.
both bonds are single bonds
both bonds are double bonds
both bonds are the same because of resonance
there are 20 valence electrons
there is one single and one double bond
Of the possible bonds between carbon atoms (single, double, and triple), _____.
a triple bond is longer than a single bond
a double bond is stronger than a triple bond
a single bond is stronger than a triple bond
a double bond is longer than a triple bond
a single bond is stronger than a double bond
The formal charge on carbon in the molecule shown is _______.
0
+1
+2
+3
-1
In the Lewis structure of ClF, the formal charge on Cl is _______ and the formal charge on F is _______.
0,0
-1, -1
0, -1
-1, 0
+1, -1
In the resonance form of ozone shown, the formal charge on the central oxygen atom is _______.
0
+1
-1
+2
-2
Choose the correct shape for H2S
Tetrahedral
Trigonal pyramidal
Bent
Trigonal planar
Draw the Lewis Dot structure for ICl2- and determine its predicted molecular geometry.
see-saw
trigonal bipyramidal
linear
bent
The carbon atom undergoes what type of hybridization?
sp hybridization
sp2 hybridization
sp3 hybridization
dsp3 hybridization
The nitrogen atom undergoes what type of hybridization?
sp hybridization
sp2 hybridization
sp3 hybridization
dsp3 hybridization
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
The molecule that uses sp3d hybrid orbital on the central atom is
BCl3
NCl3
ICl3
PCl3
What is the molecular geometry of this molecular compound?
Trigonal bypyramidal
Tetrahedral
Trigonal planar
linear
What is the bond angle for the central atom in this molecular compound? *Just type in the number!
(a)
Which of the following Lewis Structures for this molecule is most accurate? Explain your answer.
As two atoms covalently bond to become more stable, what happens to their bond energy?
(a)
Which of these alloys is a substitutional alloy?
Bronze
Steel
The melting point of MgO is higher than that of NaF. Which of the following best explains this observation?
O2- is more negatively charged than F-
Mg2+ is more positively charged than Na+
The O2- ion is smaller than the F- ion
Mg2+ is more positively charged than Na+ and O2- is more negatively charged than F-
The diagram above shows two resonance structures for a molecule of C6H6 . The phenomenon shown in the diagram best supports which of the following claims about the bonding in C6H6?
In the C6H6 molecule, all the bonds between the carbon atoms have the same length.
Because of variable bonding between its carbon atoms, C6H6 is a good conductor of electricity.
The bonds between carbon atoms in C6H6 are unstable, and the compound decomposes quickly.
The C6H6 molecule contains three single bonds between carbon atoms and three double bonds between carbon atoms.
How would coulombic forces affect physical properties of a molecule such as boiling (BP) and melting point(MP)?
Higher coulombic forces would lead to lower BP and MP
Higher coulombic forces would lead to higher BP and MP
Higher coulombic forces would lead to higher BP ,but a lower MP
Lower coulombic forces would lead to higher BP and MP
Which of the following molecular shapes would have a bond angle of 180 Degrees?
Bent
Trigonal Planar
Tetrahedral
Linear
Steel is an alloy containing Fe atoms and C atoms. Which of the following diagrams best represents the particle-level structure of steel?
Which of the following molecules has the shortest bond length?
N2
O2
Cl2
Br2
I2
What is the bond angle in H2S molecule?
107◦
104.5◦
180◦
120◦
Why is the bond angle in NH3 molecule is smaller than that in CH4 molecule?
Among the four electron pairs around the central atom N in NH3
molecule, there are two lone pairs which require more space than bonding pairs and tend to compress the angles between the bonding pairs.
Among the four electron pairs around the central atom N in NH3
molecule, there is one lone pair which requires more space than a bonding pair and tends to compress the angles between the bonding pairs.
Among the four electron pairs around the central atom N in NH3
molecule, there is one lone pair which requires less space than bonding pairs and tend to increase the angles between the bonding pairs.
In reality, bond angle in NH3 molecule is larger than that in CH4 molecule.
Breaking bonds is _________________. Forming bonds is ______________________
endothermic, exothermic
exothermic, endothermic
Use bond energies to determine the energy change for the following reaction and use the information to determine if it is an endothermic or exothermic reaction:
HCN + H2 --> CH3N2
The average bond enthalpies for O-O and O=O are 146 and 496 kJ/mol respectively. What is the enthalpy change, in kJ, for the reaction below?
H2O2(g) → H2O(g) + ½O2(g)
-102
+102
+350
+394
Which has the higher lattice energy: BeCl2 or LiCl?
LiCl because lithium is smaller than beryllium
LiCl because Li has a smaller ionic charge than Be
BeCl2 because there are more chlorine atoms in the bond
BeCl2 because Be has a stronger ionic charge than Li
Choose the ionic compound with the greater magnitude of lattice energy.
NaCl
KCl
