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WorksheetsCHEM 241 Exam 1
Total questions: 51
Worksheet time: 13hrs 45mins
How many valence electrons are in C?
(a)
How many valence electrons are in Se?
(a)
How many valence electrons are in Mg?
(a)
How many valence electrons are in P?
(a)
How many valence electrons are in F-?
(a)
How many valence electrons are in K+?
(a)
What is the molecular shape of BF3?
bent
trigonal planar
trigonal pyramidal
tetrahedral
What is the molecular shape of this molecule
tetrahedral
trigonal pyramidal
trigonal planar
linear
What are the hybridization and geometry of the carbon atom?
sp2
geometry: tetrahedral
sp3
geometry: trigonal planar
geometry: square planar
What are the hybridization and geometry of the N atom
geometry: tetrahedral
geometry: trigonal planar
sp3
sp2
geometry: trigonal pyramidal
What is the hybridization
sp
sp2
sp3
sp3 has 4 sets of bonds or lone pairs
true
false
how many pi bonds are in each?
(a)
Polar or nonpolar and what is the hybridization
polar
nonpolar
sp
sp3
sp2
What are the valid skeletal structures for C5H11N
A
B
C
E
F
Classify as same (S), isomer (I), or different (D)
(a)
Use electronegativity values to evaluate the polarity of the bonds between the two atoms shown. Then classify each bond as either nonpolar covalent (NP), polar covalent (PC), or ionic (ION)
a. C-H b. Li-Cl c. N-S d. Al-C
(a)
What is the hybridization and the molecular shape
polar
nonpolar
bent
tertrahedral
trigonal pyramidal
Which skeletal structure is consistent for the molecular formula C5H10O
A
B
C
D
Which illustrate hydrogen bonding
1
2
3
Which can undergo hydrogen bonding
1
2
3
4
What is the strongest molecular force for A-D?
1 for hydrogen-bonding, 2 for dipole-dipole force, 3 for London dispersion force
(a)
What are the strongest intermolecular forces for E-H?
1 for hydrogen-bonding, 2 for dipole-dipole force, 3 for London dispersion force
(a)
Rank the atoms in order of decreasing electronegativity
I>IV>II>III
III>IV>II>I
II>III>IV>I
III>II>IV>I
Order in decreasing boiling point
III>IV>II>I
I>II>III>IV
III>II>IV>I
I>IV>II>III
Rank in order of increasing melting point
III<II<I
II<I<III
I<II<III
I<III<II
Rank in decreasing strength of intermolecular forces
IV>II>I>III
I>IV>II>III
I>III>IV>II
IV>I>III>II
Which is expected to be least soluble in H2O?
I
II
III
IV
Which is expected to be the most soluble in H2O?
I
II
III
IV
Which of the following bonds has the largest dipole moment?
C-H
C-O
H-F
C-C
Which of the following does NOT have a net dipole of zero?
BF3
CO2
NH3
CCl4
Which of the following has the SMALLEST dipole moment?
HCl
CO2
H2O
NH3
Determine the geometry around the indicated atom in each species.
I = Trigonal planar; II = linear; III = tetrahedral; IV = trigonal planar
I = Linear; II = tetrahedral; III = trigonal planar; IV = linear
I = Linear; II = tetrahedral; III = trigonal planar; IV = tetrahedral
I = Tetrahedral; II = trigonal planar; III = linear; IV = tetrahedral
What is the hybridization for each of the indicated atoms in the following compound?
I = sp2; II = sp3; III = sp3.
I = sp; II = sp2; III = sp3.
I = sp2; II = sp2; III = sp2.
I = sp2; II = sp2; III = sp3.
Which of the following Lewis structures is correct?
I
IV
II
III
Convert the following skeletal (or bond-line) structure to a condensed structure.
I
II
III
IV
Which compound contains the most polar bond?
I
II
III
IV
Which one of the following molecules has non-polar covalent bonds?
CO2
N2
CCl4
HF
Which of the following statements about resonance are correct? Select all that apply.
Resonance structures are separated by a double-headed arrow:
Resonance generally involved lone pairs, pi bonds, and formal charges.
Electrons can move between different resonance structures.
Each resonance structure must be a valid Lewis structure.
Atoms can move between different resonance structures.
Which of the structures below represent a pair of valid resonance structures? Select all that apply.
a
b
c
d
Consider the following structures I-IV. Which two species represent resonance structures?
I and II
I and IV
I and III
II and IV
For the first reaction: Which compound is the acid?
For the first reaction: Which compound is the conjugate base?
For the second reaction: Which compound is the base?
For the second reaction: Which compound is the conjugate base?
(a)
In the two reactions shown below, which compounds (A-H) are acting as acids?
A
B
E
F
In the two reactions shown below, which compounds are acting as bases?
A
B
E
F
Which of the two reactions shown below could be considered an example of a Lewis acid-Lewis base reaction? (Enter 1 for the first reaction or 2 for the second reaction.)
Give the letter of the compound (A-G) acting as the Lewis acid.
(a)
For the acid-base reaction shown below, indicate which TWO structures (A-F) will be the expected products.
(a)
Classify each of the reactions below as either Bronsted acid-base (B), Lewis acid-base (L), or neither (N). List in the order of reactions (1, 2, 3, (a) )
Which one of the following statements explains why H2O is a stronger acid than CH4?
H2O forms a more stable conjugate base, HO-.
H2O forms a less stable conjugate base, HO-.
CH4 forms a more stable conjugate base, CH3-.
H2O can form hydrogen bonds while CH4 cannot.
Which molecule/ion (I-IV) is the conjugate base in the following reaction?
I
II
III
IV
Rank the following compounds (I-III) in order of decreasing acidity, putting the most acidic first.
III>I>II
I>II>III
III>II>I
II>III>I
For the acid-base reaction below, indicate which of the TWO structures (A-F) will be the expected products.
(a)
