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WorksheetsAP Chemistry Unit 2 Review
Total questions: 44
Worksheet time: 44mins
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
What type of alloy is this?
Interstitial
Substitutional
What is the bond angle in BF3?
90
120
109.5
180
What is the hybridization of carbon in CH4?
sp3
sp
sp2
Why are asymmetrical molecules polar?
Their dipoles do not cancel
Their dipoles cancel
What is the hybridization for carbon in CO2
sp3
sp
sp2
As the electronegativity difference between 2 atoms increases, the polarity of the bond ____________________
increases
decreases
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
What is the hybridization of carbon in C2H2?
sp3
sp
sp2
The Lewis structure of the CO32- ion is
The Lewis structure of N2H2 shows __________.
a nitrogen-nitrogen triple bond
a nitrogen-nitrogen single bond
each nitrogen has one lone pair
each nitrogen has two lone pairs
each hydrogen has one lone pair
Resonance structures differ by __________.
number and placement of electrons
number of electrons only
placement of atoms only
number of atoms only
placement of electrons only
As the number of covalent bonds between two atoms increases, the distance between the atoms ______ and the strength of the bond between them ______.
increases, increases
decreases, decreases
increases, decreases
decreases, increases
is unpredictable
The ability of an atom in a molecule to attract electrons is best quantified by the ______.
electronegativity
paramagnetism
diamagnetism
electron change-to-mass ratio
first ionization energy
The ion NO- has _____ valence electrons.
10
12
14
15
16
The formal charge on carbon in the molecule shown is _______.
0
+1
+2
+3
-1
Which of these bonds takes the most energy to break?
single
double
triple
quadruple
Potassium iodide, KI,has the following bonding:
ionic
metallic
nonpolar covalent
polar covalent
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 elements C and Se have the same electronegativity value, 2.55. Which of the following claims about the compound that forms from C and Se is most likely to be true?
The carbon-to-selenium bond is unstable.
The carbon-to-selenium bond is nonpolar covalent.
The compound has the empirical formula CSe.
A molecule of the compound will have a partial negative charge on the carbon atom.
Which of the following correctly indicates whether the solid represented by the particulate model shown above conducts electricity and explains why or why not?
It conducts electricity because it is made of positive and negative ions.
It conducts electricity because it is made of particles of different sizes.
It does not conduct electricity because its ions cannot move freely within the solid.
It does not conduct electricity because there are small spaces between the particles.
Which of the following Lewis diagrams best represents the bonding in the N2O molecule, considering formal charges?
Which atom can accommodate an octet of electrons, but doesn't necessarily have to accommodate an octet?
N
C
H
O
B
Choose the correct shape for H2S
Tetrahedral
Trigonal pyramidal
Bent
Trigonal planar
How many sigma and pi bonds are there in C2H2? (the structure will be ordered HCCH)
1 sigma and 1 pi
3 sigma and 1 pi
3 sigma and 2 pi
2 sigma and 3 pi
Which of the following best explains why copper conducts electricity?
It can have two or three valence electrons
It has delocalized electrons that can flow in a circuit
It is a transition metal
It has a low electronegativity
Which of the following molecular shapes would have a bond angle of 180 Degrees?
Bent
Trigonal Planar
Tetrahedral
Linear
Which one is polar?
BF4−
H2CO
PF5
SeF6
What kind of an alloy is this?
substitutional
interstitial
metallic
nonpolar
Which of these alloys is a substitutional alloy?
Bronze
Steel
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.
Choose the correct Electron Geometry and then Molecular Geometry of this molecule.
Tetrahedral, Trigonal planar
Tetrahedral, Trigonal pyramidal
Tetrahedral, Tetrahedral
Trigonal Bipyramidal, Bent
Which structure consists of a giant lattice of cations and anions held together by strong electrostatic forces of attraction?
ionic bonding
metallic bonding
covalent bonding
Which color graph would be the plot for the molecule with the largest atomic radius
purple graph
blue graph
red graph
The acronym VSEPR stand for
very strong electron pair repulsion.
varied symmetry electrostatic proton reaction.
venomous snakes enjoy pink ribbons.
valence shell electron pair repulsion.
Ionic Compounds are normally Solid at Room Temperature and known as Salts. The lattice energy of a salt is related to the energy required to separate the ions of solid ionic s. For which of the following pairs of ions is the energy that is required to separate the ions largest?
K and F
Fr and I
Ga and O
Al and O
