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Honors Chemistry Final Exam Review
Honors Chemistry Final Exam Review
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Final Exam
Flashcards
35 cards
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Practice quiz
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Questions
35
Answers
1
What type of IMFs are present in the molecule shown (C
6
H
14
)?
Dipole-dipole
London Dispersion Forces
ionic bonds
H-bonding
2
A chemical substance that can not be broken down further by chemical means is a(n)
solution
compound
mixture
element
3
When this equation is balanced, what is the sum of the coefficients? C
6
H
14
+ O
2
--> CO
2
+ H
2
O
24
47
46
23
4
Which of the following statements is FALSE?
Isotopes have the same atomic number.
N-14 and C-14 are isotopes
Isotopes have different mass numbers.
N-13 and N-14 are isotopes.
5
What is the molar mass of a gas if 2.50 g occupies a volume of 2.78 L at STP?
81.6 g/mol
20.2 g/mol
6.95 g/mol
0.0496 g/mol
6
How many grams of aluminum fluoride (AlF
3
) are in 2.34 x 10
23
formula units?
32.7 g
17.9 g
0.389 g
84.0 g
7
Whose atomic model is shown in the image?
Bohr
Thomson
Rutherford
Quantum Mechanical
8
What rule is being illustrated in the image?
Hund's Rule
Orbital Principle
Pauli Exclusion Principle
Aufbau Principle
9
How many protons, neutrons and electrons are in the ion
238
U
+2
?
92 protons, 146 neutrons, 94 electrons
92 protons, 238 neutrons, 90 electrons
92 protons, 146 neutrons, 90 electrons
92 protons, 238 neutrons, 90 electrons
10
Whose model of the atom is shown in the image?
Bohr
Thomson
Rutherford
Dalton
11
What is the strongest type of IMF that exists between molecules of the substance below?
dipole-dipole
London dispersion forces
ionic bonds
hydrogen bonding
12
What is the molecular formula of the compound - empirical formula CH
2
O, molar mass 150 g/mol?
C5H10O5
C4H8O4
C3H6O3
C6H12O6
13
What is the charge of Fe in FePO
4
?
+4
+2
+3
-3
14
Which electron configuration is not possible ever?
1s22s22p63s23p64s23d4
1s22s22p63s1
1s22s22p63s23p64s23d104p3
1s22s22p63s23p7
15
Which of the following is a chemical change?
potassium chloride decomposing
potassium chloride dissolving in water
potassium chloride melting
potassium chloride evaporating
16
Which of the following gives the correct answer to the correct sig figs? 20.10 g / 4.30 mL =
4.67 g/mL
4.7 mL
4.674 g/mL
4.6744 g/mL
17
Which metal will undergo the greatest ΔT if equal masses are heated with 50.0 J?
Zinc: 0.387 J/goC
Lead: 0.128 J/goC
Silver: 0.233 J/goC
Aluminum: 0.900 J/goC
18
Which of the following molecules has trigonal planar geometry?
CH2O
H2O
NH3
CH4
19
What is the pH of a 0.30M NaOH solution?
13.47
0.501
0.523
12.57
20
Which is an example of an endothermic process?
alcohol freezing
clouds forming from water vapor
combustion of methane
water boiling
21
Air is classified as a(n)
element
solution
heterogeneous mixture
compound
22
Which of the following is a true statement?
The value of Keq is affected by a catalyst
The value of Keq is affected by changes in temperature
Q>Keq means reaction needs more products to hit equilibrium
Keq > 1 means more reactants than products at equilibrium
23
What type of reaction is pictured in this image?
Double replacement
Decomposition
Single replacement
Synthesis
24
100.0 g of which of the following elements would contain the most atoms?
carbon, C
nitrogen, N2
oxygen, O2
lithium, Li
25
The scuba diver in the image has a mass of 14.5 g. What is its density?
1.81 g/cm3
0.55 g/cm3
0.552 g/cm3
1.8 g/cm3
26
Which molecule would you predict to have the highest boiling point?
CH3OH
C2H5OH
HCl
C2H6
27
Which of the following is NOT an electrolyte?
NaCl
C6H12O6
Ca(C2H3O2)2
HNO3
28
Which sequence is in the order smallest to largest radius?
Rn, Sr, S, Al
F, O, Ca, Rb
Ar, Li, F, Ba
He, Sr, O, K
29
Which of the formulas is INCORRECT?
AlSO4
Na2S
CaS
CaSO4
30
Which of the following changes will NOT increase rate of reaction?
increasing concentration
adding a catalyst
decreasing temperature
increasing surface area of solid reactant
31
How many significant figures are in the measurement 0.0045060 g?
5
4
8
7
32
Which is inversely proportional to the pressure of a gas?
volume
temperature
velocity
moles
33
What law is represented in the image?
Charles' Law
Ideal Gas Law
Avogadro's Law
Boyle's Law
34
Which of the following is a weak acid?
HF
HI
HCl
HBr
35
What is the limiting reactant when 4.5 mol of sulfur react w/ 6.5 mol of silver? 2Ag + S → Ag
2
S
water
silver sulfide
sulfur
silver
