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Honors Chemistry Final Exam Review
Honors Chemistry Final Exam Review
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Final Exam
Flashcards
38 cards
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Practice quiz
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Questions
38
Answers
1
The electron sea model of bonding represents....
Ionic Bonding
Polar Covalent Bonding
Non Polar Covalent Bonding
Metallic Bonding
2
Which sequence is in the order: noble gas, alkaline earth metal, chalcogen, alkali metal
He, Sr, O, K
Rn, Sr, S, Al
Ne, Ca, Cl, Na
Ar, Li, F, Ba
3
What is the strongest type of IMF that exists between molecules of the substance below?
London dispersion forces
ionic bonds
dipole-dipole
hydrogen bonding
4
Which metal will undergo the greatest ΔT if equal masses are heated with 50.0 J?
Lead - 0.128 J/goC
Zinc - 0.387 J/goC
Silver - 0.233 J/goC
Aluminum - 0.900 J/goC
5
Whose model of the atom is shown in the image?
Dalton
Rutherford
Thomson
Bohr
6
A compound represented by X2Y3. Oxidation number of Y is 2-, what is the oxidation number of X?
3+
2-
2+
3-
7
The electrons involved in the formation of a chemical bond are called...
Dipoles
Valance Electrons
Lewis Electrons
Electrons
8
What law is represented in the image?
Avogadro's Law
Ideal Gas Law
Charles' Law
Boyle's Law
9
Which of the following molecules has trigonal planar geometry?
XeF3+
NH3
CH2O
IF3
10
What is the molecular formula of the compound - empirical formula CH
2
O, molar mass 150 g/mol?
C3H6O3
C4H8O4
C6H12O6
C5H10O5
11
100.0 g of which of the following elements would contain the most atoms?
carbon
lithium
oxygen
nitrogen
12
How many grams of aluminum fluoride are in 2.34 x 10
23
formula units?
22.7 g
36.5 g
333 g
50.3 g
13
How many significant figures are in the measurement 0.0045060 g?
7
4
8
5
14
How many protons, neutrons and electrons are in the ion
238
U
+2
?
92 protons, 238 neutrons, 90 electrons
92 protons, 146 neutrons, 94 electrons
92 protons, 238 neutrons, 90 electrons
92 protons, 146 neutrons, 90 electrons
15
Which of the following statements is FALSE?
Isotopes have different mass numbers.
N-13 and N-14 are isotopes.
Isotopes have the same atomic number.
N-14 and C-14 are isotopes
16
Which is an example of an endothermic process?
water boiling
clouds forming from water vapor
alcohol freezing
combustion of methane
17
Which of these is an organic compound?
CaCl2
CH4
NH3
H2O
18
Whose atomic model is shown in the image?
Rutherford
Thomson
Bohr
Quantum Mechanical
19
Which of the following is NOT an electrolyte?
NaCl
C6H12O6
Ca(C2H3O2)2
HNO3
20
What type of reaction is pictured in this image?
Synthesis
Decomposition
Single replacement
Double replacement
21
Atoms that share electrons unequally are said to have a __________ type of bond.
Polar Covalent
Non Polar Covalent
Metallic
Ionic
22
Which of the following gives the correct answer to the correct sig figs? 20.10 g / 4.30 mL =
4.6744 g/mL
4.67 g/mL
4.7 mL
4.674 g/mL
23
What is the oxidation number of fluorine in 0F
2
?
-1
+2
-2
+1
24
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
2.7 g/cm3, 3.7 g/cm3, 1.7 g/cm3
1.68 g/cm3, 2.70 g/cm3, 2.45 g/cm3
25
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
23
46
26
Which is inversely proportional to the pressure of a gas?
temperature
moles
volume
velocity
27
Pressure is ...
Mass/Volume
Force/Area
Mass Acceleration
Distance/Time
28
The ______________ state is composed of negative and positive particles
Gas
Plasma
Liquid
Solid
29
Which of the formulas is INCORRECT?
AlSO4
Na2S
CaSO4
CaS
30
What rule is being illustrated in the image?
Orbital Principle
Pauli Exclusion Principle
Aufbau Principle
Hund's Rule
31
The scuba diver in the image has a mass of 14.5 g. What is its density?
0.552 g/cm3
3.625 g/cm3
1.81 g/cm3
1.16 g/cm3
32
What is the molar mass of a gas if 2.50 g occupies a volume of 2.78 L at STP?
31.0 g/mol
24.9 g/mol
24.8 g/mol
20.2 g/mol
33
Which of the following is a chemical change?
potassium chloride dissolving in water
potassium chloride evaporating
potassium chloride decomposing
potassium chloride melting
34
Air is classified as a(n)
solution
compound
heterogeneous mixture
element
35
What is the limiting reactant when 4.5 moles of sulfur react with 6.5 moles of silver?
sulfur
silver sulfide
water
silver
36
A chemical substance that can not be broken down further by chemical means is a(n)
compound
mixture
element
solution
37
Give the correct molecular geometry for the SF
4
molecule.
tetrahedral
square planar
see-saw
trigonal by-pyramidal
38
Branch of chemistry relating mass of reactants and products
Organic Chemistry
Stoichiometry
Biochemistry
Nuclear Chemistry
