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Honors Chemistry Review
Honors Chemistry Review
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Final Exam
Flashcards
35 cards
F
Practice quiz
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Host live
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Questions
35
Answers
1
What is the oxidizing agent in the reaction: Na + H
2
O --> NaOH + H
2
H2
H2O
Na
NaOH
2
What rule is being illustrated in the image?
Pauli Exclusion Principle
Hund's Rule
Orbital Principle
Aufbau Principle
3
How many grams of aluminum fluoride are in 2.34 x 10
23
formula units?
36.5 g
22.7 g
50.3 g
333 g
4
How many protons, neutrons and electrons are in the ion
238
U
+2
?
92 protons, 238 neutrons, 90 electrons
92 protons, 238 neutrons, 90 electrons
92 protons, 146 neutrons, 94 electrons
92 protons, 146 neutrons, 90 electrons
5
Which sequence is in the order: noble gas, alkaline earth metal, chalcogen, alkali metal
He, Sr, O, K
Ar, Li, F, Ba
Rn, Sr, S, Al
Ne, Ca, Cl, Na
6
What is the molecular formula of the compound - empirical formula CH
2
O, molar mass 150 g/mol?
C3H6O3
C5H10O5
C4H8O4
C6H12O6
7
What is the limiting reactant when 4.5 moles of sulfur react with 6.5 moles of silver?
water
silver sulfide
sulfur
silver
8
What is the molar mass of a gas if 2.50 g occupies a volume of 2.78 L at STP?
24.9 g/mol
24.8 g/mol
31.0 g/mol
20.2 g/mol
9
Which metal will undergo the greatest ΔT if equal masses are heated with 50.0 J?
Silver - 0.233 J/goC
Lead - 0.128 J/goC
Aluminum - 0.900 J/goC
Zinc - 0.387 J/goC
10
What is the frequency of electromagnetic radiation with a wavelength of 452 nm?
6.64 x 105 Hz
6.64 x 1014 Hz
1.36 x 1014 Hz
1.50 x 10-15 Hz
11
Which of the following gives the correct answer to the correct sig figs? 20.10 g / 4.30 mL =
4.7 mL
4.6744 g/mL
4.67 g/mL
4.674 g/mL
12
How many significant figures are in the measurement 0.0045060 g?
8
4
5
7
13
The scuba diver in the image has a mass of 14.5 g. What is its density?
3.625 g/cm3
0.552 g/cm3
1.16 g/cm3
1.81 g/cm3
14
Which set of data is precise but not accurate, given that the true value is 2.70 g/cm
3
?
2.71 g/cm3, 2.68 g/cm3, 2.69 g/cm3
3.4 g/cm3, 3.3 g/cm3, 3.5 g/cm3
1.68 g/cm3, 2.70 g/cm3, 2.45 g/cm3
2.7 g/cm3, 3.7 g/cm3, 1.7 g/cm3
15
Which is inversely proportional to the pressure of a gas?
moles
volume
velocity
temperature
16
What type of IMFs are present in the molecule shown?
LDFs
H-bonding
ionic bonds
Dipole-dipole
17
What is the strongest type of IMF that exists between molecules of the substance below?
hydrogen bonding
ionic bonds
London dispersion forces
dipole-dipole
18
A chemical substance that can not be broken down further by chemical means is a(n)
element
compound
solution
mixture
19
Which of the formulas is INCORRECT?
Na2S
AlSO4
CaS
CaSO4
20
Air is classified as a(n)
element
compound
solution
heterogeneous mixture
21
What law is represented in the image?
Charles' Law
Ideal Gas Law
Boyle's Law
Avogadro's Law
22
Give the correct molecular geometry for the SF
4
molecule.
trigonal by-pyramidal
tetrahedral
see-saw
square planar
23
What type of reaction is pictured in this image?
Double replacement
Synthesis
Single replacement
Decomposition
24
Which of the following is NOT an electrolyte?
HNO3
NaCl
Ca(C2H3O2)2
C6H12O6
25
Which of the following molecules has trigonal planar geometry?
IF3
XeF3+
NH3
CH2O
26
Which of the following is a chemical change?
potassium chloride dissolving in water
potassium chloride decomposing
potassium chloride melting
potassium chloride evaporating
27
What is the oxidation number of fluorine in 0F
2
?
-2
+1
-1
+2
28
100.0 g of which of the following elements would contain the most atoms?
nitrogen
lithium
oxygen
carbon
29
When this equation is balanced, what is the sum of the coefficients? C
6
H
14
+ O
2
--> CO
2
+ H
2
O
47
46
23
24
30
Whose model of the atom is shown in the image?
Dalton
Thomson
Bohr
Rutherford
31
Which is an example of an endothermic process?
clouds forming from water vapor
alcohol freezing
combustion of methane
water boiling
32
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.
33
Whose atomic model is shown in the image?
Thomson
Quantum Mechanical
Bohr
Rutherford
34
Which of the following is a weak acid?
HCl
HBr
HI
HF
35
What is the pH of a 0.30M NaOH solution?
13.5
0.523
12.6
0.501
