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CHEMISTRY I - HONORS MIDTERM REVIEW
Chapter 2
Measurement & Calculations
Describe the purpose of the scientific method
Distinguish between qualitative and quantitative measurements
Describe the differences between the hypotheses, theories and models
Distinguish between a quantity, unit, and a standard measurement
Name & use SI units for length, mass, time, volume & density
Distinguish between mass & weight
Perform density calculations
Distinguish between accuracy and precision
Determine the number of significant figures in measurements & perform operations
Convert measurements into scientific notation
Distinguish between inversely and directly proportional relationships
Vocabulary:
Scientific measurement
System
Hypothesis
Theory
Model
Accuracy
Precision
Percentage error
Significant figures
Scientific notation
Directly proportional
Indirectly proportional
Chapter 1
Matter and Change
Distinguish between physical properties and chemical properties of matter
Classify changes of matter as physical or chemical
Explain gas, liquid & solid states in terms of particles
Explain how conservation of matter applies to changes of matter
Distinguish between a mixture & a pure substance
Vocabulary:
Mass
Matter
Atom
Element
Compound
Extensive properties
Intensive properties
Physical properties
Physical change
Change of state
Solid
Liquid
Gas
Plasma
Chapter 3
Atoms: the Building Blocks of Matter
Explain the Conservation of Mass, the Law of Definite Proportions, & Law of Multiple Proportions
Summarize the 5 essential points of Dalton's atomic theory
Summarize the properties of the cathode ray tube that led to the discovery of the electron Summarize the
experiment carried out be Rutherford that led to the discovery of the nucleus
List the properties of the proton, neutron, electron
Define the atom
Explain what isotopes are
Define atomic number & mass number, describe how they apply to isotopes
Vocabulary:
Law of Conservation Mass
Law of Definite Proportions
Law of Multiple Proportions
Atom
Nuclear forces
Atomic number
Isotope
Mass number
Nuclide
Atomic mass unit
Average atomic mass
Chapter 21
Nuclear Chemistry
Explain what a nuclide is, and describe the different ways nuclides can be represented.
Define and relate the terms mass defect and nuclear binding energy.
Explain the relationship between nucleon number and stability of nuclei.
Explain why nuclear reactions occur and know how to balance a nuclear equation. Define and relate the terms
radioactive decay and nuclear radiation.
Describe the different types of radioactive decay and their effects on the nucleus. Define the term half-life, and
explain how it relates to the stability of a nucleus. Define and relate the terms decay series, parent nuclide, and
daughter nuclide. Explain how artificial radioactive nuclides are made, and discuss their significance.
Compare the penetrating ability and shielding requirements of alpha particles, beta particles, and gamma rays.
Describe three devices used in radiation detection.
Discuss applications of radioactive nuclides.
Define nuclear fission, chain reaction, and nuclear fusion, and distinguish between them. Explain how a
fission reaction is used to generate power.
Discuss the possible benefits and the current difficulty of controlling fusion reactions.
Vocabulary:
Mass defect
Nuclear binding energy
radioactive decay
nuclear radiation
half-life
decay series
parent nuclide
daughter nuclide
Nuclear fission
Chain reaction
Nuclear fusion
Chapter 4 Arrangement of Electrons
Explain the mathematical relationship among the speed, wavelength & frequency of electromagnetic
radiation
Discuss the dual wave-particle nature of light
Discuss the significance of the photoelectric effect & line-emission spectrum
Describe the Bohr model of the hydrogen atom
Discuss the development of the quantum model of the atom
Explain the Heisenberg Uncertainty Principle
List the 4 quantum numbers & describe their significance
Relate the number of sublevels to an atom’s energy levels, orbitals per sub-level
List the total number of electrons needed to fully occupy each energy level
State Aufbau principle, the Pauli Exclusion Principle, & Hund’s Rule
Describe electron configurations using, orbital notation, electron configuration or noble-gas notation
Vocabulary:
Electromagnetic radiation
Electromagnetic spectrum
Wavelength
Frequency
Photoelectric effect
Quantum
Photon
Ground state
Excited state
Line-emission spectrum
Continous spectrum
Heisenberg Uncertainty Principle
Quantum theory
Orbital
Quantum number
Principle quantum number
Angular momentum quantum number
Magnetic quantum number
Spin quantum number
Electron configuration
Aufbau Principle
Pauli Exclusion Principle
Hund’s Rule
Noble-gas
Noble-gas configuration
Chapter 5
The Periodic Law
Describe the roles of Mendeleev and Moseley in the development of the periodic table
Describe the modern periodic table
Explain how periodic law can be used to predict physical and chemical properties
Describe how elements belonging to a group are interrelated
Locate and name the four blocks of the periodic table
Discuss the relationship between group configurations and group numbers
Describe the locations in the periodic table and the general properties of the alkalai metals, the alkaline
earth metals, the halogens, and the noble gases
Define and compare the periodic trends atomic radii, ionization energy, electron affinity &
electronegativity
Define valance electrons and state how many are present in each main group element
Compare the periodic trends of the d-block elements with those of the main block elements
Vocabulary:
Periodic law
Periodic table
Lanthanide
Actinide
Alkalai metal
Alkaline earth metal
Transition metal
Main group elements
Halogens
Atomic radius
Ion
Ionization Ionization energy
Electron affinity
Cation
Anion
Valence electrons
Electronegativity
Chapter 6 Bonding
Know how to tell if a bond is polar or nonpolar.
Know how to tell if a bond is ionic or covalent.
Be able to count valence electrons and understand their importance in bonding.
Be able to draw Lewis Dot Structures.
Be able tot use VSEPR theory to predict the molecular geometry (shape) of molecules.
Be able to use VSEPR theory to predict polarity of a molecule.
Chemistry Midterm review –random extra questions *Test may cover other topics not included on
this review, yet have been covered throughout the semester.
1.
2.
What are the two main branches of science? And how do they relate to each other?
What is the difference between scientific law and scientific theory? Which can be
changed or replaced and when can this happen?
3.
Describe the relationship between science and technology?
4.
What is the first step in the scientific method?
5.
When are scientific models used? Give 2 examples.
6.
How do scientists test a hypothesis?
7.
Explain why no experiment should be called a failure?
8.
What is the difference between an SI base unit and a derived unit?
9.
What are the 3 types of graphs used? And when are each of them used?
10. Explain in your own words the difference between accuracy and precision?
11. Copy table 1, table 2, table 3 on page 16. (your SI base Units and the prefixes)
12. What is the rule for significant figures for adding/subtracting? And
multiplying/dividing?
13. Convert 3.5 sec to milliseconds.
14. Convert 40 cm to m.
15. Convert 1.5 kg to g.
16. Convert 24 ml to L.
17. Write the following in scientific notation
a.
0.00345 m
b. 60,200 mg c. 0.000044 L
18. Write the measurements in long form. (take out of scientific notation)
a.
4.5 x 103 g
b.
1.67 x 10‐8 cm
c.
4.55 x 106 km
19. Perform the calculations and write the answer with the correct number of
significant figures.
a.
12.34 m x 40.3 m
b.
3.05 cm x 6.70 cm x 8.222 cm
c.
3.5 g +
4.56 g
d.
3.123 L / 1.3 L
e.
5.78 g ‐ 2.3 g
20. How many significant figures are in the following numbers:
a. 45
b. 640
c. 0.046 d. 1.0023
21. Explain the relationship between matter, atoms, and elements.
22. Which is the most abundant element on Earth?
23. What are the two types of pure substances?
24. Sketch a flow chart with these words: Matter, Mixtures, Pure Substances, Elements,
Compounds, Homogeneous Mixture, and Heterogeneous Mixture.
25. Compare and contrast mixtures and pure substances. Give an example of each.
26. Describe the differences between physical and chemical properties. List some of
these properties and explain why they are important.
27. How are mixtures separated? Give 3 examples.
28. Are changes of state, physical or chemical changes? Why?
29. Which is easily reversible, physical or chemical change? Why?
30. List 3 clues that indicate a chemical change has occurred?
31. Is Density a physical or chemical property? Why?
32. Identify whether the following is an element or compound:
a. H2O
b. Fe
c. K
d. C6H12O6
33. In question above, how many Oxygen atoms are in 1a?
1d?
34. What is Density and what kind of property is it?
35. A piece of tin has a mass of 15.52 g and a volume of 2.26 cm3. What is the density of the tin?
36. A piece of titanium metal has a mass of 67.5 g and volume of 15 cm3. What is the
density of the titanium?
37. The density of a piece of brass is 8.4 g/cm3. If the mass of the brass is 510g, find
the volume of the brass.
38. Identify whether the following is a chemical or physical property:
a.
Flammability
b.
Freezing point
c.
Boiling point
d.
Density
e.
Reactivity with air
f.
Color
39.
Identify whether the following is a physical or chemical change:
a.
Change of color
b.
Dissolving sugar in water
c.
Producing a gas
d.
Evaporation
e.
Rusting Iron
f.
Burning paper
g.
Fruit rotting
40. Describe how temperature relates to kinetic energy.
If the temperature goes up or down, what happens to kinetic energy?
41. Name several factors that determine the speed of the atoms and molecules of a
particular substance.
42. What are the four states of matter? Describe them each in terms of having definite or
indefinite shape volume.
43. What were the differences between Bohr’s model of the atom and the modern model of the
atom?
44. What is the order of the periodic table based on?
45. How are the electrons of an element related to the arrangement of the periodic
table?
46. What do valence electrons predict?
47. What group # are the alkali metals and alkaline earth metals located? And list 2
characteristics of each.
48. Where are the semiconductors located on the periodic table? List several
characteristics of them.
49. Do Noble Gases exist as a molecule or a single element? And why?
50. What makes noble gases extremely stable and inert?
51. Do metals tend to lose or gain electrons? Why?
52. Do nonmetals tend to lose or gain electrons? Why?
Where are the transition metals located?
53. In the following problems, how many protons, electrons and neutrons are there:
a. Carbon-14 b. Nitrogen-15 c. Sulfur-35 d. 35 17 Cl
54. Name the element AND the group that the following elements belong to.
a. K
b. Ti
c. Cl
d. Ne
e. Mg
f. Si
55. How many moles are present if you have 56.0 grams of BaBr2?
56. How many grams are present if you have 1.12 E23 atoms of Au?
57. How many grams are present if you have 4.50 moles of KCl?
58. How many molecules are present if you have 6.70 moles of Al2O3?
59. How many grams are present if you have 4.56 E23 molecules of NaOH?
60. How many grams are equal to 12.0 moles of H2?
61. How many moles are equal to 3.50 grams of BaBr2?
62. How many moles are equal to 6.02 E24 molecules of Ca3(PO4)2?
63. What are the differences between Ionic Bonds and Covalent Bond?
64. What bonding is involved with Ionic Compounds and Molecules?
65. Which type of electrons are involved with bonding?
66. How many valence electrons in the following: a. C b. O c. N
67. What are Lewis Dot diagrams?
68. Draw Lewis Dots structures for the following:
a. NH3
b. H2S
c. CCl4
d. BF3
e. F2
69. Predict the shapes for the previous problems and tell whether they are nonpolar or
polar.
70. An AM Radio station broadcasts at a frequency of 1150 KHz. What is its wavelength?
71. The energy of a photon is 3.31 E -18 J. What is the wavelength of this photon?
72. What is the electron configuration of Antimony?
73. What is the orbital notation for sulfur?
74. Which color of light has a higher frequency, blue or green?
75. Which has a longer wavelength, x-rays or microwaves?
76. Which trend typically decreases as you move from left to right across a Period on the
Periodic Table?