1. Chem I
Semester 1 Review

2. All of the following are general characteristics of a substance in the liquid state except
definite volume.
not easily compressed.
able to flow.
definite shape.
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3. In the chemical reaction iron plus oxygen →iron oxide,
iron oxide is a reactant.
oxygen is a product.
iron is a reactant.
iron is a product.
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4. Which term does not fit with the others listed?
Solid
Gas
Reactant
Liquid
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5. The chemical symbol for sodium is
NA.
SO.
Na.
So.
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6. A basketball has more mass than a golf ball because:
the basketball takes up more space.
the basketball contains more matter.
the golf ball contains a different kind of matter.
the golf ball has an indefinite composition.
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7. A gas is a form of matter that
has a definite volume.
is generally a liquid or solid at room temperature.
takes the shape and volume of its container.
is difficult to compress.
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8. Homogeneous mixtures are always liquids.
consist of two or more phases.
have a composition that is fixed.
are known as solutions.
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9. A compound is a pure substance. has a composition that varies.
can be physically separated into its elements.
has properties similar to those of its elements.
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10. Physical properties of a substance include
color and odor.
malleability.
melting & boiling points.
all of the above.
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11. When iron and oxygen combine to form iron oxide,
a physical change occurs.
a change of state occurs.
a change in mass occurs.
a chemical change occurs.
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12. How many significant figures are in the measurement 2103.2 g?4 5 3
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13. Which of these equalities is not correct?
10 kg= 1 g
100 cg= 1 g
1 cm3= 1 mL
1000 mm= 1 m
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14. How many of the zeros in the measurement 0
How many of the zeros in the measurement m are significant? 2 7 3 8
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15. How many milligrams are in 2.5 kg?
2.5 x 106 mg
2.5 x 104 mg
25 mg
2.5 x 102 mg
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16. The closeness of a measurement to its true value is a measure of its:
usefulness.
accuracy.
precision.
reproducibility.
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17. Which of these measurements is expressed to three significant figures?
0.070 mm
7007 mg
7.30 x 107 km
0.007 m
both C and D
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18. A metric unit of volume is the:
km.
mg. K.
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19. The number of seconds in a 40-hour work week can be calculated as follows:
Picture Choice 1
Picture Choice 2
Picture Choice 3
Picture Choice 4 A. B. C.
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20. The metric prefix kilo- means:
100 times smaller.
1000 times smaller.
1000 times larger.
100 times larger.
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21. What is the volume of 60. 0 g of ether if the density of ether is 0
What is the volume of 60.0 g of ether if the density of ether is 0.70 g/mL?
86 mL
2.4 x102 mL
1.2 x 102 mL
42 mL
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22. Concentrated hydrochloric acid has a density of 1. 19 g/mL
Concentrated hydrochloric acid has a density of 1.19 g/mL. What is the mass, in grams, of 2.00 liters of this acid?
2.38 x 103 g
4.20 x 10-4 g
2.38 g
4.20 x 104 g
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23. A conversion factor: is equal to 1.
is a ratio of equivalent measurements.
does not change the value of a measurement.
all of the above
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24. Which of the following is not a part of Dalton’s atomic theory?
All elements are composed of atoms.
Atoms of the same element are alike.
Atoms are always in motion.
Atoms that combine do so in simple whole-number ratios.
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25. The nucleus of an atom is
negatively charged and has a low density.
negatively charged and has a high density.
positively charged and has a low density.
positively charged and has a high density.
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26. Dalton theorized that atoms are indivisible and that all atoms of an element are identical. Scientists now know that
Dalton’s theories are completely correct.
atoms of an element can have different numbers of protons.
atoms are all divisible.
all atoms of an element are not identical but they all have the same mass.
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27. The number of neutrons in the nucleus of an atom can be calculated by
adding together the numbers of electrons and protons.
subtracting the number of protons from the mass number.
subtracting the number of protons from the number of electrons.
adding the mass number to the number of protons.
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28. The sum of the protons and neutrons in an atom equals the
atomic number.
atomic mass.
number of electrons.
mass number.
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29. All atoms of the same element have the same:
number of protons.
mass number.
number of neutrons.
mass.
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30. Which of these statements is false?
Electrons have a negative charge.
Electrons have a mass of 1 amu.
The nucleus of an atom is positively charged.
The neutron is found in the nucleus of an atom.
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31. An atom of an element with atomic number 48 and mass number 120 contains
48 protons, 48 electrons, and 72 neutrons.
72 protons, 48 electrons, and 48 neutrons.
120 protons, 48 electrons, and 72 neutrons.
72 protons, 72 electrons, and 48 neutrons.
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32. The number 80 in the name bromine-80 represents
the atomic number.
the mass number.
the sum of protons and electrons.
none of the above
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33. Which of these statements is not true?
Atoms of the same elements can have different masses.
The nucleus of an atom has a positive charge.
Atoms of isotopes of an element have different numbers of protons.
Atoms are mostly empty space.
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34. If E is the symbol for an element, which two of the following symbols represent isotopes of the same element?
1 and 2
3 and 4
1 and 4
2 and 3
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35. The fourth principal energy level has
4 orbitals.
32 orbitals.
16 orbitals.
9 orbitals.
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36. If the electron configuration of an element is 1s22s22p63s23p5, the element is
iron.
chlorine.
bromine.
phosphorus.
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37. The electron configuration of calcium is
1s22s22p23s23p34s2.
1s22s22p103s23p4.
1s22s23s23p6 3d8.
1s22s22p63s23p64s2.
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38. The maximum number of electrons that can occupy the third principal energy level is
18. 2.
32. 8.
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39. As the frequency of light increases, the wavelength
remains the same.
decreases.
approaches the speed of light.
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40. In order to occupy the same orbital, two electrons must have
the same direction of spin.
low energy.
opposite charge.
opposite spin.
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41. Stable electron configurations are likely to contain
high-energy electrons.
unfilled s orbitals.
fewer electrons than unstable configurations.
filled energy sublevels.
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42. According to Hund’s rule, when electrons occupy orbitals of equal energy, one electron enters each orbit until
all the orbitals contain one electron, with spins parallel.
all the orbitals contain one electron, with opposite spins.
there are two electrons in each orbital.
electron velocities become constant.
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43. In the periodic table, there is a periodic pattern in the physical and chemical properties of elements when they are arranged in order of
increasing atomic mass.
increasing electronegativity.
increasing atomic number.
increasing atomic radius.
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44. Which sublevel corresponds to the transition metals in the periodic table?f
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45. Which of the following elements is a metalloid?Br Se As Kr
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46. The element iodine, I, is a
period 5 alkali metal.
period 4 halogen.
period 5 halogen.
period 5 transition metal.
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47. The subatomic particle that plays the greatest role in determining the physical and chemical properties of an element is the
proton.
electron.
neutron.
photon.
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48. Which of the following atoms would you expect to have the largest atomic radius?K Rb Ca
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49. From left to right across the second period of the periodic table,
first ionization energy increases.
atomic radii increase.
electronegativity decreases.
atomic mass decreases.
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50. The category of elements that is characterized by the filling of f orbitals is the
inner transition metals.
alkali metals.
alkali earth metals.
transition metals.
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51. Electronegativity
generally decreases from left to right across a period.
is the energy change that accompanies the loss of an electron from a gaseous atom.
generally decreases from top to bottom within a group.
is generally higher for metals than for nonmetals.
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52. Atomic size generally increases from left to right across a period.
decreases from top to bottom within a group.
remains constant within a period.
decreases from left to right across a period.
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53. The alkali metals do not include
Na.
Ca.
Rb.
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54. How many valence electrons does an atom of any element in Group 16 have?2 6 4 8
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55. The electron dot structure for an atom of phosphorus is
Picture Choice 1
Picture Choice 2
Picture Choice 3
Picture Choice 4 A. B. C. D.
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56. When an aluminum atom loses its valence electrons, what is the charge on the resulting ion?2+ 3+ 2- 1+
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57. 15 The high surface tension of water is due to the:
a. small size of water molecules.
b. low mass of water molecules.
c. hydrogen bonding between water molecules.
d. covalent bonds in water molecules. c.

58. The electron configuration of a fluoride ion, F-, is
1s2 2s2 2p5.
the same as that of the neon atom.
1s2 2s2 2p6 3s1.
the same as that of a potassium ion.
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59. In forming chemical bonds, atoms tend to attain
the electron configuration of noble gas atoms.
a state of higher energy.
the electron configuration of halogen atoms.
all of the above
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60. An ionic compound is electrically neutral.
held together by ionic bonds.
composed of anions and cations.
all of the above
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61. A cation is any atom or group of atoms with
a positive charge.
no charge.
a negative charge.
more electrons than the corresponding atoms.
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62. The cation Fe3+ is formed when
an atom of iron loses two electrons.
an atom of zinc loses two electrons.
an atom of iron loses three electrons.
an atom of iron gains three electrons.
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63. Which of these elements does not exist as a diatomic molecule?
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64. Which one of the following compounds is not covalent?
HCl
KCl
SCl2
S2Cl2
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65. How many valence electrons does an atom of any halogen have?4 2 1 7
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66. If a bonding pair of electrons is unequally shared between two atoms, the bond is
ionic.
coordinate covalent.
nonpolar covalent.
polar covalent.
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67. A covalent bond forms when an element becomes a noble gas.
when atoms share electrons.
between metals and nonmetals.
when electrons are transferred from one atom to another.
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68. The correct name for the N3- ion is the:
nitrate ion.
nitride ion.
nitric ion.
nitrite ion.
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69. A molecular formula: gives information about molecular geometry.
can be written for ionic compounds.
shows the number and kinds of atoms in a molecule of a compound.
uses superscripts to show the number of atoms of each kind.
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70. The metals in Groups 1A, 2A, and 3A:
gain electrons when they form ions.
form ions with a charge found by subtracting 8 from the group number.
all form ions with a 1 charge.
lose electrons when they form ions.
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71. Which of the following is not an empirical formula?
Na2SO4
N2H4
C6H5Cl
Sn3(PO4)4
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