Download Chemistry (CP) Final Exam Study Guide 1

Chemistry (CP) Final Exam Study Guide 1
Matching
Match each item with the correct statement below.
a. organic chemistry
d. analytical chemistry
b. inorganic chemistry
e. physical chemistry
c. biochemistry
____
____
____
____
____
1.
2.
3.
4.
5.
the study of the processes that take place in organisms
concerned with the mechanism, rate, and energy transfer that occurs when matter undergoes a change
the study of all chemicals containing carbon
the study of chemicals that, in general, do not contain carbon
the study of the composition of matter
Match each item with the correct statement below.
a. mixture
d. reactant
b. product
e. heterogeneous mixture
c. phase
f. vapor
____ 6. gaseous state of substance that is a liquid or solid at room temperature
____ 7. a physical blend of two or more components
____ 8. part of a sample having uniform composition and properties
____ 9. not uniform in composition
____ 10. a substance formed in a chemical reaction
____ 11. starting substance in a chemical reaction
Match each item with the correct statement below.
a. atomic emission spectrum
d. photon
b. frequency
e. quantum
c. wavelength
f. spectrum
____
____
____
____
____
12.
13.
14.
15.
16.
discrete bundle of electromagnetic energy
energy needed to move an electron from one energy level to another
number of wave cycles passing a point per unit of time
distance between wave crests
separation of light into different wavelengths
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____ 17. Which of the following would a chemist be most likely to study?
a. a leaf floating on water
c. a leaf being blown by the wind
b. a leaf changing color in autumn
d. a leaf being eaten by insects
____ 18. Which of the following statements is false?
a. Knowledge of chemistry allows the public to make informed decisions.
b. Studying chemistry ensures that officials make correct choices in funding technology.
c. Knowledge of chemistry helps prepare people for careers in soil science.
d. Chemistry explains many aspects of nature.
____ 19. Which of the following is an example of a current research focus in chemistry?
a. development of smoke detectors for common use
b. using hook-and-loop tape in the clothing industry
c. applying gene therapy to treat certain diseases
d. studying coal combustion as an energy source
____ 20. How do conceptual problems differ from numeric problems?
a. Solutions to conceptual problems involve analysis, while numeric solutions do not.
b. Logic is not usually involved in solving numeric problems.
c. A plan is necessary to solve numeric problems, but is not necessary for conceptual
problems.
d. Solutions to conceptual problems normally do not involve calculations.
____ 21. All of the following are physical properties of matter EXCEPT ____.
a. mass
c. melting point
b. color
d. ability to rust
____ 22. Which of the following is NOT a physical property of water?
a. It has a boiling point of 100 C.
b. It is a colorless liquid.
c. It is composed of hydrogen and oxygen.
d. Sugar dissolves in it.
____ 23. A vapor is which state of matter?
a. solid
c. gas
b. liquid
d. all of the above
____ 24. Which state of matter takes both the shape and volume of its container?
a. solid
c. gas
b. liquid
d. both b and c
____ 25. Which of the following CANNOT be classified as a substance?
a. table salt
c. nitrogen
b. air
d. gold
____ 26. Which of the following items is NOT a compound?
a. baking soda
c. sucrose
b. salad dressing
d. table salt
____ 27. Which of the following is a chemical property?
a. color
c. freezing point
b. hardness
d. ability to react with oxygen
____ 28. Which of the following is a chemical property of water at 4 C?
a. its color
b. its state
c. its temperature
d. its ability to decompose into hydrogen and oxygen
____ 29. Which of the following measurements contains two significant figures?
a. 0.004 00 L
c. 0.000 44 L
b. 0.004 04 L
d. 0.004 40 L
____ 30. Which group of measurements is the most precise? (Each group of measurements is for a different object.)
a. 2 g, 3 g, 4 g
c. 2 g, 2.5 g, 3 g
b. 2.0 g, 3.0 g, 4.0 g
d. 1 g, 3 g, 5 g
____ 31. Which of the following measurements is expressed to three significant figures?
a. 0.007 m
c. 7.30 10 km
b. 7077 mg
d. 0.070 mm
____ 32. What is the measurement 111.009 mm rounded off to four significant digits?
a. 111 mm
c. 111.01 mm
b. 111.0 mm
d. 110 mm
____ 33. What is the measurement 1042 L rounded off to two significant digits?
a. 1.0 10 L
c. 1050 L
b. 1040 L
d. 1.1 10 L
____ 34. What is the metric system prefix for the quantity 0.000 001?
a. centic. kilob. decid. micro____ 35. Which of the following units is NOT an official SI unit?
a. kilogram
c. mole
b. ampere
d. liter
____ 36. What is the boiling point of water in kelvins?
a. 0 K
c. 273 K
b. 100 K
d. 373 K
____ 37. What is the temperature –34 C expressed in kelvins?
a. 139 K
c. 239 K
b. 207 K
d. 339 K
____ 38. What is the volume of 45.6 g of silver if the density of silver is 10.5 g/mL?
a. 0.23 mL
c. 479 mL
b. 4.34 mL
d. none of the above
____ 39. Which hypothesis led to the discovery of the proton?
a. When a neutral hydrogen atom loses an electron, a positively-charged particle should
remain.
b. A proton should be 1840 times heavier than an electron.
c. Cathode rays should be attracted to a positively-charged plate.
d. The nucleus of an atom should contain neutrons.
____ 40. All atoms are ____.
a. positively charged, with the number of protons exceeding the number of electrons
b. negatively charged, with the number of electrons exceeding the number of protons
c. neutral, with the number of protons equaling the number of electrons
d. neutral, with the number of protons equaling the number of electrons, which is equal to the
number of neutrons
____ 41. As a consequence of the discovery of the nucleus by Rutherford, which model of the atom is thought to be
true?
a. Protons, electrons, and neutrons are evenly distributed throughout the volume of the atom.
b. The nucleus is made of protons, electrons, and neutrons.
c. Electrons are distributed around the nucleus and occupy almost all the volume of the atom.
d. The nucleus is made of electrons and protons.
____ 42. Isotopes of the same element have different ____.
a. positions on the periodic table
c. atomic numbers
b. chemical behavior
d. mass numbers
____ 43. In which of the following sets is the symbol of the element, the number of protons, and the number of
electrons given correctly?
a. In, 49 protons, 49 electrons
c. Cs, 55 protons, 132.9 electrons
b. Zn, 30 protons, 60 electrons
d. F, 19 protons, 19 electrons
____ 44. Using the periodic table, determine the number of neutrons in O.
a. 4
c. 16
b. 8
d. 24
____ 45. Which of the following statements is NOT true?
a. Atoms of the same element can have different masses.
b. Atoms of isotopes of an element have different numbers of protons.
c. The nucleus of an atom has a positive charge.
d. Atoms are mostly empty space.
____ 46. Select the correct symbol for an atom of tritium.
a. n
c. H
b. H
d. H
____ 47. How is the number of neutrons in the nucleus of an atom calculated?
a. Add the number of electrons and protons together.
b. Subtract the number of electrons from the number of protons.
c. Subtract the number of protons from the mass number.
d. Add the mass number to the number of electrons.
____ 48. What unit is used to measure weighted average atomic mass?
a. amu
c. angstrom
b. gram
d. nanogram
____ 49. Which of the following statements is NOT true?
a. Protons have a positive charge.
b. Electrons are negatively charged and have a mass of 1 amu.
c. The nucleus of an atom is positively charged.
d. Neutrons are located in the nucleus of an atom.
____ 50. What is the maximum number of d orbitals in a principal energy level?
a. 1
c. 3
b. 2
d. 5
____ 51. What types of atomic orbitals are in the third principal energy level?
a. s and p only
c. s, p, and d only
b. p and d only
d. s, p, d, and f
____ 52. What is the next atomic orbital in the series 1s, 2s, 2p, 3s, 3p?
a. 2d
c. 3f
b. 3d
d. 4s
____ 53. According to the aufbau principle, ____.
a. an orbital may be occupied by only two electrons
b. electrons in the same orbital must have opposite spins
c. electrons enter orbitals of highest energy first
d. electrons enter orbitals of lowest energy first
____ 54. Which type of electromagnetic radiation includes the wavelength 10
a. gamma ray
c. radio wave
b. microwave
d. visible light
m?
____ 55. What is the wavelength of an electromagnetic wave that travels at 3
MHz? (1 MHz = 1,000,000 Hz)
a.
b. 60 MHz
c.
____ 56.
____ 57.
____ 58.
____ 59.
____ 60.
10 m/s and has a frequency of 60
300,000,000 m/s
d. No answer can be determined from the information given.
The atomic emission spectra of a sodium atom on Earth and of a sodium atom in the sun would be ____.
a. the same
b. different from each other
c. the same as those of several other elements
d. the same as each other only in the ultraviolet range
What are quanta of light called?
a. charms
c. muons
b. excitons
d. photons
Who predicted that all matter can behave as waves as well as particles?
a. Albert Einstein
c. Max Planck
b. Erwin Schrodinger
d. Louis de Broglie
According to the Heisenberg uncertainty principle, if the position of a moving particle is known, what other
quantity CANNOT be known?
a. mass
c. spin
b. charge
d. velocity
How can the position of a particle be determined?
a. by analyzing its interactions with another particle
b. by measuring its velocity
c. by measuring its mass
d. by determining its charge