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Honors Chemistry: Final Exam Review Flashcards | StudBud
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Honors Chemistry: Final Exam Review
Honors Chemistry: Final Exam Review
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General review of high school honors chemistry material.
Flashcards
72 cards
F
Practice quiz
P
Host live
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Questions
72
Answers
1
Is the bond formed between the pair of atoms nonpolar, polar, or ionic?
Ionic
Nonpolar
Huh?
Polar
2
What is the percent by mass of hydrogen in pentane?
15.0 %
83.2 %
70.6 %
16.8 %
3
If 1.0 mol of pentanol has 6.02 x 10
25
atoms of hydrogen, how many moles of H are there?
100
10
1000
1
4
Which hydrocarbon, CH
4
or C
2
H
6
, has the higher boiling point?
C2H6
CH4
5
True or False: Ionization energy decreases when going from left to right.
False
True
6
A compound has a MM of 60.10g/mol: 39.97% C; 13.41% H; 46.62% N. Find the molecular formula.
CH4N
C2HN2
C2H8N2
CHN
7
What happens to the pressure of a gas in a closed container if the temperature increases?
the pressure cannot be predicted
the pressure increases
the pressure decreases
the pressure does not change
8
What is the name of this piece of lab equipment?
weigh boat
crucible
evaporating dish
pouring bowl
9
An x-ray has a wavelength of 1.2 x 10
-8
. Calculate the energy of one photon of this radiation.
1.66 x 10-17 J
3.32 x 10 -14 J
1.66 x 10-13 J
3.32 x 10-16 J
10
Define excess reactant.
The reactant that is left over
H2
The reactant that determines the amount of product formed
The reactant that determines the amount of reactant formed
11
What is the formula to find percent yield?
Actual yield / theoretical yield x 100
Actual yield x 100
Theoretical yield x 100
Theoretical yield / actual yield x 100
12
Dipole-dipole forces exist in all ... molecules.
Covalent
Nonpolar
Ionic
Polar
13
What is the volume, in liters, of 1.55 mol of ammonia at STP?
34.7 L
can not be determined
6.20 L
1.55 L
14
How many moles of aluminum oxide can be produced from 12.5 grams of O
2
?
0.365 mol
0.125 mol
0.150 mol
0.260 mol
15
Ground state
Stat of an atom which the electron occupy the highest energy
State of an atom which the electron occupy the lowest energy
16
Lewis dot structure: How many dots will magnesium have surrounding it?
5
1
2
7
17
Ionic compounds consist of...
other combination
metals and nonmetals
nonmetals only
metals only
18
Is the following picture correct of NF
3
lewis structure?
No
Yes
19
1s
2
2s
2
2p
6
3s
2
3p
3
is the electron configuration for...
phosphorus
bromine
potassium
silicon
20
Which of the following is NOT an ionic compound?
NaCl
NaF
LiMg
MgO
21
Excited state
State of an atom which the electron occupy high energy
State of an atom which the electron occupy the lowest energy
22
How many valence electrons are transferred from bromine to lithium in the formation of LiBr?
2
3
1
0
23
What is the percent composition of Ba in BaO if a sample contains 7.58 g Ba and 10.5 g O?
41.9 %
50.1 %
36.5%
58.1 %
24
How many neutrons are in the following element?
48
26
22
70
25
Is the bond formed between the pair of atoms nonpolar, polar, or ionic?
Nonpolar
This is an L
Ionic
Polar
26
At what temperature will 0.654 moles of neon gas occupy 12.30 liters at 1.95 atm?
446 oC
174 oC
230 K
540 K
27
Which of the following describes an example of pure chemistry?
developing a cure for arthritis
studying chemicals containing carbon
developing a medication for a new virus
testing effects of medications on the brain
28
What is the formula for calcium phosphite?
Ca3(PO3)2
Ca2(PO3)
CaPO4
Ca3(PO4)2
29
Which electron configuration of the 3d orbital is the most stable?
3d10
3d2
3d14
3d5
30
What measurement contains three significant figures?
10.55
100
10.0
10
31
What is the electron configuration of Ca? (short hand)
[Ar]2p6
[Ne]5d5
1s2
[Ar]4s2
32
Molecular compounds consist of...
Other combination
Nonmetal only
Nonmetal and metal
Metal only
33
What is the formula for ideal gas law?
V1T1 / V2T2
PV = nRT
None
P1V1 / T1 = P2V2 / T2
34
Does the following picture correctly demonstrate the lewis theory for Na and Cl?
Yes
No
35
Define theoretical yield.
Determines amount of reactant formed
Max amount of product thatcan be made base on limit reactant
None
Determines amount of product formed
36
1 single bond is how many sigma bonds?
3
2
4
1
37
Which of the following is NOT an example of an acid?
NH3
H2SO4
HCl
HNO3
38
How many energy sublevels are in the third principal energy level?
2
1
4
3
39
Which of the following is an anion?
carbonate
magnesium
cesium
ammonium
40
Does the atomic size increase or decrease when going down a group?
Increase
Decrease
41
What is the formula for Boyle's Law?
P1V1 x P2V2
P1V1 = P2V2
P1V1 / P2V2
L
42
What is the following diagram called?
Heating curve
Spongebob meme
Titration curve
Equilibrium
43
Is the bond formed between the pair of atoms nonpolar, polar, or ionic?
Ionic
Nonpolar
Polar
Idk
44
VSEPR Theory: What is the name for 2 bonds and 2 lone pairs?
Linear
Pyramidal
Octahedral
Bent
45
Does the following diagram correctly show a resonance structure for CO
3
2-
?
Yes
No
46
The number of wave cycles that pass through a stationary point
Wavelength
Frequency
Ground state
Excited state
47
VSEPR Theory: What is the name for 2 bonds and no lone pairs?
Trigonal planar
Linear
Bent
Tetrahedral
48
True or False: Ionization energy increases when going up a group.
True
False
49
1 triple bond is how many sigma bonds and pi bonds?
2 sigma bonds, 2 pi bonds
1 sigma bond, 2 pi bonds
2 sigma bonds, 3 pi bonds
1 sigma bond, 3 pi bonds
50
Define actual yield.
The amount of product actually produced
Max amount of product thatcan be made base on limit reactant
The amount of product NOT actually produced
Percentage of theoretical yield that was actually attained
51
Which of the following is NOT an example of an base?
NaOH
HCl
NH3
All of them are bases
52
What is the formula for molarity?
M = mol / grams
M = grams / L
M = mol / mL
M = mol / L
53
A solution is a(n)
heterogeneous mixture
homogeneous mixture
insoluble solute in solvent
a compound composed of two or more substances
54
Which of the following elements is a transition metal?
Be
Mn
Sr
O
55
Identify the type of reaction.
single replacement
combustion
synthesis
decomposition
56
How do you calculate pH when given hydrogen concentration?
[OH-]10
-log[OH-]
-log[H+]
L
57
What is the correct name for the P
-3
ion?
phosphite
phosphide
phosphate
phosphorus
58
What is the net charge of the polyatomic ion sulfate?
+1
-1
-3
-2
59
How many moles are in 372 g of barium nitrate?
1.42 mol
3.72 mol
1.86 mol
2.84 mol
60
Which of the following is true about the Pauli exclusion principle?
No more than 2 electrons can occupy an orbital
The 2 electrons must have opposite spins
None
The 2 electrons must have the same spins
61
Define limiting reactant.
The reactant that determines the amount of reactant formed
H2
The reactant that determines the amount of product formed
The reactant that is left over
62
What is the net charge of the ionic compound magnesium fluoride?
0
1
-1
2
63
VSEPR Theory: What is the name for 3 bonds and no lone pairs?
Linear
Octahedral
Trigonal planar
Bent
64
Does the atomic size increase or decrease when going from left to right?
Decrease
Increase
65
Determine the limiting reactant when 4.0 mol of F
2
react with 3.5 mol FeI
3
.
FeI3
can't be determined
F2
66
1 double bond is how many sigma bonds and pi bonds?
3 sigma, 1 pi
1 sigma, 1 pi
2 sigma, 1 pi
1 sigma, 2 pi
67
What is the following picture an example of?
None
Ionization energy
Electron configuration
Pauli Exclusion Principle
68
The distance between adjacent wave crests in a wave.
Excited state
Ground state
Wavelength
Frequency
69
What is the formula for the combined gas law?
L
P1V1 / T1 x P2V2 / T2
P1V1 / T1 divided by P2V2 / T2
P1V1 / T1 = P2V2 / T2
70
the molar mass of an element corresponds to...
empirical formula
molecular formula
71
The following structure has how many sigma and/or pi bonds?
sigma = 3, pi = 3
sigma = 1, pi = 2
sigma = 3, pi = 1
sigma = 3, pi = 2
72
What is the formula for Charles Law?
V1T1 x V2T2
V1T1 / V2T2
L
V1/T1 = V2/T2
