Download Fall 2015 Review-2

Fall Semester Review - 2
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1. What is the SI unit of measurement for mass?
a. gram
b. kilogram
c. milligram
d. pound
2. An example of an extensive property of matter is ____.
a. temperature
c. mass
b. pressure
d. hardness
3. Which state of matter expands when heated and is easy to compress?
a. gas
c. solid
b. liquid
d. all of the above
4. All of the following are physical properties of a substance in the liquid state EXCEPT ____.
a. indefinite volume
c. not easily compressed
b. definite mass
d. indefinite shape
5. Which of the following is true about compounds?
a. They can be physically separated into their component elements.
b. They have compositions that vary.
c. They are substances.
d. They have properties similar to those of their component elements.
6. A substance that can be separated into two or more substances only by a chemical change is a(n) ____.
a. solution
c. mixture
b. element
d. compound
7. What is one difference between a mixture and a compound?
a. A compound consists of more than one phase.
b. A compound can only be separated into its components by chemical means.
c. A mixture can only be separated into its components by chemical means.
d. A mixture must be uniform in composition.
8. What must occur for a change to be a chemical reaction?
a. There must be a change in chemical properties.
b. There must be a change in physical properties.
c. The change must involve a change in mass.
d. The change must involve a change in volume.
9. A chemical change occurs when a piece of wood ____.
a. is split
c. decays
b. is painted
d. is cut
10. What must be done to be certain that a chemical change has taken place?
a. Check for the production of bubbles before and after the change.
b. Demonstrate that a release of energy occurred after the change.
c. Check the composition of the sample before and after the change.
d. Demonstrate that energy was absorbed by the reactants after the change.
11. How many protons, electrons, and neutrons does an atom with atomic number 50 and mass number 125
contain?
a. 50 protons, 50 electrons, 75 neutrons
c. 120 neutrons, 50 protons, 75 electrons
b. 75 electrons, 50 protons, 50 neutrons
d. 70 neutrons, 75 protons, 50 electrons
12. Isotopes of the same element have different ____.
a. numbers of neutrons
c. numbers of electrons
b. numbers of protons
d. atomic numbers
13. Which of the following sets of symbols represents isotopes of the same element?
a.
c.
J
J
J
M
M
M
b.
d.
L
L
L
Q
Q
Q
Fall Semester Review - 2
____ 14. The atomic mass of an element is the ____.
a. total number of subatomic particles in its nucleus
b. weighted average of the masses of the isotopes of the element
c. total mass of the isotopes of the element
d. average of the mass number and the atomic number for the element
____ 15. If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed in
the three orbitals?
a. one electron in each orbital
b. two electrons in one orbital, one in another, none in the third
c. three in one orbital, none in the other two
d. Three electrons cannot fill three empty 2p atomic orbitals.
____ 16. What unit is used to measure weighted average atomic mass?
a. amu
c. angstrom
b. gram
d. nanogram
____ 17. What is the maximum number of electrons in the s, p, and d sublevels respectively?
a. 1, 3, 5
c. 6, 2, 10
b. 2, 2, 6
d. 2, 6, 10
____ 18. Which of the following is correct concerning subatomic particles?
a. The electron was discovered by Goldstein in 1886.
b. The neutron was discovered by Chadwick in 1932.
c. The proton was discovered by Thomson in 1880.
d. Cathode rays were found to be made of protons.
____ 19. In which of the following is the number of neutrons correctly represented?
a.
c.
F has 0 neutrons.
Mg has 24 neutrons.
b.
d.
As has 108 neutrons.
U has 146 neutrons.
____ 20. Which of the following was originally a tenet of Dalton's atomic theory, but had to be revised about a century
ago?
a. Atoms are tiny indivisible particles.
b. Atoms of the same element are identical.
c. Compounds are made by combining atoms.
d. Atoms of different elements can combine with one another in simple whole number ratios.
____ 21. Which of the following is true about subatomic particles?
a. Electrons are negatively charged and are the heaviest subatomic particle.
b. Protons are positively charged and the lightest subatomic particle.
c. Neutrons have no charge and are the lightest subatomic particle.
d. The mass of a neutron nearly equals the mass of a proton.
____ 22. Consider an element Z that has two naturally occurring isotopes with the following percent abundances: the
isotope with a mass number of 19.0 is 55.0% abundant; the isotope with a mass number of 21.0 is 45.0%
abundant. What is the average atomic mass for element Z?
a. 20.0 amu
c. 19.9 amu
b. 1.99 amu
d. 199 amu
____ 23. What is the electron configuration of potassium?
a. 1s 2s 2p 3s 3p 4s
c. 1s 2s 3s 3p 3d
b. 1s 2s 2p 3s 3p
d. 1s 2s 2p 3s 3p 4s
____ 24. What are the number of protons, neutrons, and electrons in a neutral atom of Tin (Sn)?
a. p 50, n 69, e 50
c. p 119, n 69, e 119
b. p 50, n 50, e 50
d. p 50, n 69, e 69
Fall Semester Review - 2
____ 25. Give the electron configuration for a neutral atom of Argon (Ar).
a. 1s2 2s2 3s2 2p6 3p6
c. 1s2 2s2 2p6 3s2 3p6
2
2
10
2
2
b. 1s 2s 2p 3s 3p
d. 1s1 2s1 2p6 3s2 3p8
____ 26. 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
____ 27. What element has the electron configuration 1s 2s 2p 3s 3p ?
a. nitrogen
c. silicon
b. selenium
d. silver
____ 28. 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.
____ 29. Give the electron configuration for a neutral atom of beryllium.
a. 1s2 2s1 2p1
c. 1s1 2s3
2
2
b. 1s 2s
d. 1s1 2s1 2p2
____ 30. The atomic number of an element is the total number of which particles in the nucleus?
a. neutrons
c. electrons
b. protons
d. protons and electrons
____ 31. Dalton's atomic theory included which idea?
a. All atoms of all elements are the same size.
b. Atoms of different elements always combine in one-to-one ratios.
c. Atoms of the same element are always identical.
d. Individual atoms can be seen with a microscope.
___ 32. An element has an atomic number of 76. The number of protons and electrons in a neutral atom of the
element are ____.
a. 152 protons and 76 electrons
c. 38 protons and 38 electrons
b. 76 protons and 0 electrons
d. 76 protons and 76 electrons
____ 33. Who arranged the elements according to atomic mass and used the arrangement to predict the properties of
missing elements?
a. Henry Moseley
c. John Dalton
b. Antoine Lavoisier
d. Dmitri Mendeleev
____ 34. Which of the following is true about the electron configurations of the noble gases?
a. The highest occupied s and p sublevels are completely filled.
b. The highest occupied s and p sublevels are partially filled.
c. The electrons with the highest energy are in a d sublevel.
d. The electrons with the highest energy are in an f sublevel.
____ 35. Which subatomic particle plays the greatest part in determining the properties of an element?
a. proton
c. neutron
b. electron
d. none of the above
____ 36. Which of the following statements is true about ions?
a. Cations form when an atom gains electrons.
b. Cations form when an atom loses electrons.
c. Anions form when an atom gains protons.
d. Anions form when an atom loses protons.
Fall Semester Review - 2
____ 37. The metals in Groups 1A, 2A, and 3A ____.
a. gain electrons when they form ions
c. all have ions with a 1 charge
b. all form ions with a negative charge
d. lose electrons when they form ions
____ 38. Which of the following statements correctly compares the relative size of an ion to its neutral atom?
a. The radius of an anion is greater than the radius of its neutral atom.
b. The radius of an anion is identical to the radius of its neutral atom.
c. The radius of a cation is greater than the radius of its neutral atom.
d. The radius of a cation is identical to the radius of its neutral atom.
____ 39. Give the electron configuration for a neutral atom of selenium.
a. 1s2 2s2 2p6 3s2 3p6 4s2 4d10 4p4
c. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4
b. 1s2 2s2 2p6 3s2 3p6 4d10 4s2 4p4
d. 1s2 2s2 2p6 3s2 3p6 4s2 3d8 4p6
____ 40. Using the table list the following elements in order of increasing ionization energy
a. F, O, Ca
c. O, F, Ca
b. O, Ca, F
d. Ca, O, F
____ 41. Using the table list the following elements in order of decreasing atomic size.
a. S, Se, Rb
c. Rb, S, Se
b. Rb, Se, S
d. Se, Rb, S
____ 42. Using the table list the following elements in order of increasing electronegativity.
a. Fr, Br, F
c. F, Br, Fr
b. Fr, F, Br
d. Br, Fr, F
____ 43. Which of the following elements is the most electronegative?
a. Lithium
c. Helium
b. Radium
d. Fluorine
____ 44. Which of the following represents the Noble Gas Notation for Potassium?
a. [Ne] 3s23p3
c. [Ne] 4s1
b. [Ar] 3s1
d. [Ar] 4s1
____ 45. The modern periodic table is arranged in order of increasing atomic ____.
a. mass
c. number
b. charge
d. radius
____ 46. To what category of elements does an element belong if it is a poor conductor of electricity?
a. transition elements
c. nonmetals
b. metalloids
d. metals
____ 47. How many valence electrons are in an atom of phosphorus?
a. 2
c. 4
b. 3
d. 5
____ 49. The relative ability to attract an another atom’s electrons is known as___________.
a. ionization energy
c. electron affinity
b. electronegativity
d. valence
____ 50. The group soft, highly active metals, all of which have only one valence electron in the outer s orbital, is
known as ____________.
a. Alkaline earth metals
c. transition metals
b. alkali metals
d. inner transition metals