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