Download Midterm Review

Midterm Review 2013
1. the logical approach to the solution of scientific problems.
2. the study of the chemistry of living organism.
3. branch of chemistry concerned with the composition of substances.
4. an educated guess.
5. a broad and extensively tested explanation of why experiments give certain results.
6. the study of the composition of matter and the changes that it undergoes.
7. the means to test a hypothesis.
8. uses your senses to obtain information directly.
9. the study of essentially all substances containing carbon.
10. branch of chemistry concerned with theories and experiments that describe the behavior of
chemicals.
11. Matter that flows but has a definite volume
12. Amount of matter that an object contains
13. Starting substances in a chemical reaction
14. a type of homogeneous mixture
15. The simplest forms of matter
16. Alters a substance without changing its chemical composition
17. Matter with a definite shape and volume
18. Substances formed in a chemical reaction
19. Anything that takes up space and has mass
20. In the chemical reaction iron + oxygen  iron oxide: What is the product?
21. Three states of matter
22. chemical symbol for sodium
23. The chemical symbol for chlorine is
24. A gas is a form of matter that:
25. Homogeneous mixtures are:
26. Heterogeneous mixtures are:
27. A compound is:
28. List physical properties of a substance:
29. When iron and oxygen combine to form iron oxide (rust), is this a Chemical or physical change?
30. During chemical and physical changes, substances absorb or give off
31. During
32.
.
, a liquid is boiled to produce a vapor that is then condensed again to a liquid.
mixtures differ from pure substances because these mixtures are not uniform.
33. When iron and sulfur combine to form iron sulfide, a
34. A
change takes place.
property is a quality of a substance that can be observed or measured without
changing the composition of the substance.
35. Elements combine chemically to form
.
36. Fe is the chemical symbol for what element?
37. A
mixture has a completely uniform composition.
38. In any physical or chemical change, mass is
39. In a chemical reaction, the new substances formed are called
40. A measure of the pull of gravity on a given mass.
41. Being able to reproduce a measurement or out come.
42. The ratio of the mass of an object to its volume.
43. The difference between the accepted value and the experimental value.
44. The degree of hotness or coldness of an object.
45. The closeness of a measurement to the true value.
46. The space occupied by matter.
47. List all the SI units and what they measure
48. Measurements that have a definite values and numbers are called.
49. When results are given in a descriptive form, they are called.
50. How many significant figures are in the measurement 2103.2 g?
51. How many of the zeros in the measurement 0.000 040 200 m are significant (should be counted)?
52. How many significant figures are in 2.50 kg?
53. The closeness of a measurement to its true value is a measure of its:
54. List three measurements in which the number is expressed to three significant figures?
55. List the metric prefixes and their values
56. What is the formula for density?
57. What is the volume of 60.0 g of ether if the density of ether is 0.70 g/mL?
58. What is the formula for converting from Celsius to Kelvin?
59. What is the formula for converting from Kelvin to Celsius?
60. An acid has a density of 1.19 g/mL. What is the mass, in grams, of 2000 mL of this acid?
61. What is the mass, in grams, of 1000.0 cm3 of balsa wood if the density is 0.20 g/cm3 ?
62. Chlorine boils at 239 K. What is the boiling point of chlorine expressed in degrees Celsius?
63. The total number of protons and neutrons in the nucleus of an atom
64. The weighted average mass of the atoms in a naturally occurring sample of an element
65. The mass of a carbon-12 atom
66. The number of protons in the nucleus of an element
67. Atoms with the same number of protons but different numbers of neutrons
68. Negatively charged subatomic particles
69. The smallest particle of an element that retains the properties of that element
70. Subatomic particle with no charge
71. Positively charged subatomic particles
72. The nucleus of an atom is:
73. Dalton theorized that atoms are indivisible and that all atoms of an element are identical.
Scientists now know that:
74. The number of neutrons in the nucleus of an atom can be calculated by:
75. All atoms of the same element have the same:
76. These elements are found in Group 0.
77. Who came up with the “plum pudding” model of the atom?
78. Who discovered the nucleus?
79. The periodic law states that:
80. Relative atomic masses are measured in:
81. He got credit over Meyers for the first periodic table.
82. Lines of colored light obtained by passing the light emitted by an element through a prism
83. The region around an atomic nucleus where an electron is likely to be moving
84. A range of colors seen when light passes through a prism
85. Rule/Law that states that electrons enter orbitals of lowest energy first.
86. A region outside the nucleus where there is high probability of finding an electron
87. The p sublevel has how many orbitals:
88. If the electron configuration of an element is 1s2 2s2 2p6 3s2 3p5, name the element .
89. The maximum number of electrons that can occupy the third principal energy level is:
90. In the formula 2p6, the 2 represents:
91. In order to occupy the same orbital, two electrons must have:
92. According to Hund’s rule, when electrons occupy orbitals of equal energy, one electron enters
each orbit until:
93. Identify the elements that have the following electron configurations:
a. 1s2 2s2 2p6 3s2 3p1
b. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6
c. 1s2 2s2 2p6 3s2 3p6 4s2 3d7
94. Consider the elements neon, bromine, and phosphorus. Which has:
a. three electrons in its 3p sublevel?
b. its highest energy level completely filled?
c. the highest occupied energy level?
95. An element whose outermost s or d sublevels are only partially filled.
96. The NRG needed to remove an electron from a gaseous atom
97. A horizontal row on the periodic table
98. The electrons in the outermost NRG level are called
99. Any of a family of nonmetals including fluorine and chlorine are called
100.
The tendency of an atom to attract electrons to itself when it is chemically combined with
another element
101.
An element in which the outermost s and p sublevels are completely filled
102.
An element found in the f block.
103.
Which orbital corresponds to the transition metals in the periodic table?
104.
The representative elements are usually called:
105.
The vertical columns of the periodic table are called:
106.
When a strontium atom loses two electrons to form a Sr2+ ion, the electrons are lost from which
orbital?
107.
The element iodine, I, is what type of element:
, found in which group and period:
,
108.
How many diatomic elements are there? Name all of them.
109.
The subatomic particle that plays the greatest role in determining the physical and chemical
properties of an element is the:
110.
a. I
Which of the following atoms would you expect to have the largest atomic radius?
b. Na
c. Ca
d. Sr
111.
Which element is the most electronegative:
112.
Group B elements are also known as the
113.
How do you determine the atomic radius of an element?
114.
A polyatomic anion consists of
115.
In the Lewis Dot Structure, what is the maximum number of dots that can be used?
116.
Write Lewis Dot Structure for all the elements in Period 2 of the Periodic Table
117.
A metallic bond is a bond between:
118.
What is meant by one lone pair of electrons?
119.
Know the number of valence electrons found in each group of the Representative elements
120.
In forming chemical bonds, atoms are trying to attain the configuration of a
121.
If a bonding pair of electrons is unequally shared between two atoms, the bond is:
122.
The electron configuration of a fluoride ion, F-1, is:
123.
Metals are good conductors of electricity because they:
124.
Molecule in which one end has a partial positive charge and the other end has a partial
negative charge is called a(n)
True or False (Write the entire word on your lined paper)
125.
The chemical properties of an element are largely determined by the number of valence
electrons the element has.
126.
Fluorine and chlorine each have one valence electron.
127.
Non-metals acquire the stable electron structure of a noble gas by losing electrons.
128.
An alloy is a mixture of two or more elements, in which at least one is a metal.
129.
The crystal structure of ionic compounds such as sodium chloride is very unstable.
130.
Ionic compounds conduct electricity only when in a molten/melted state.
131.
During the formation of ionic compounds, electrons are transferred from one atom to another.
132.
Any part of a system with uniform composition and properties is called a phase.
133.
A pure substance can be a mixture.
134.
A heterogeneous mixture consists of two or more substances.
135.
A vapor is a gaseous substance.
136.
A compound can be chemically separated into its elements.
137.
Precise measurements are also accurate measurements.
138.
All zeros in a measurement are significant.
139.
Yesterday was a cool fall day. This is a qualitative measurement.
140.
One cubic centimeter is the same as one milliliter.
141.
The weight of an object changes with its location.
142.
A kilogram is the mass of 1mL of water at 4 °C.
143.
The density of a substance decreases at its temperature increases.
144.
Heat transfers from objects at high temperatures to objects at low temperatures.
145.
Oil floats on water, therefore, water’s density is greater than oil.
146.
The periodic table is an arrangement of elements according to similarities in their properties.
147.
Relative atomic masses are expressed in amus.
148.
The atomic number of an element is the sum of the protons and electrons in an atom of that
element.
149.
According to Dalton’s atomic theory, atoms are composed of protons, electrons, and neutrons.
150.
The charge on all protons is the same.
151.
A cathode ray is a beam that travels from a cathode to an anode.
152.
The position and velocity of an electron in an atom can be determined with great certainty.
153.
The photoelectric effect will occur no matter what energy of light strikes a metal.
154.
The outermost s orbital of an atom contains two electrons.
On the periodic table, how are the following terms effected as you move down a group.
Explain why.
155.
Electronegativity generally
156.
Atomic size generally
157.
Ionization NRG generally
On the periodic table, how are the following terms effected as you move across a period.
Explain why.
158.
Electronegativity generally
159.
Atomic size generally
160.
Ionization NRG generally
161.
For the elements whose outermost electron configurations are given below, tell the period and
the group to which each belongs.
3s 2
a.
162.
b.
5s 2 5p 4
c.
2s 2 2p 1
Write the FULL electron configurations and orbital diagram/notation for each of the following
elements.
a.
He
c.
Al
b.
K
d.
P
e.
O
Answer the following:
163.
Chart the characteristics of ionic and covalent compounds.
164.
Why does atomic size generally increase as you move down a group of the periodic table and
decrease as you move from left to right across a period?
165.
Define valence electrons.
166.
State Dalton’s Atomic theory.
167.
Compare and contrast metals and non-metals and metalloids give 1 element example for
each.
168.
A cube of gold-colored metal with a volume of 64 cm3 has a mass of 980 g. The density of
pure gold is 19.3 g/cm3. Is this metal pure gold?
169.
When a glass blower shapes molten glass into an ornament, does a chemical reaction occur?
Explain.
170.
Find the density of a rock, if its mass is 25 g and if displaces 30 mL of water.
171.
Distinguish between physical changes and chemical changes and give two examples of each.
172.
List all things that are often indications of a chemical change or reaction.
173.
Describe how you would separate a mixture of salt, water, and sand.
174.
What are the electronegativity differences between non-polar covalent, polar covalent, and
ionic bonds?
175.
Find the electronegativity difference and label the bond type for the following:
a. NaCl
c. HF
e. H2O
b. O2
d. SiO2
f. MgCl2
176.
Make a chart to describe the physical properties of solids, liquids and gases.
177.
What is the difference between a single covalent, double covalent and triple covalent bond?
Name or write formula of the following compounds
178.
Fe2O3
188.
N2O4
179.
NH4Cl
189.
CS2
180.
CoBr2
190.
P2O5
181.
Calcium chloride
191.
Phosphorus trichloride
182.
Sodium iodide
192.
Sulfur dioxide
183.
Aluminum nitrate
193.
Carbon dioxide
184.
Iron (II) oxide
194.
Dihydrogen monoxide
185.
Lead (IV) oxide
195.
NaI
186.
Mg3(PO4)2
187.
Ag2S
196.
List the prefixes used in naming covalent compounds.