Midterm Review Flashcards
(165 cards)
0
Q
Give an example of qualitative data?
A
Color of a shirt
1
Q
What is the goal of science and it’s models?
A
Workability
2
Q
When a hypothesis makes as few assumptions and is as simple as possible, what principle of logic has been followed?
A
Ockham’s razor
3
Q
What is a simple, testable statement of a prediction based on available information?
A
Hypothesis
4
Q
Who discovered the element oxygen?
A
Joseph Priestly
5
Q
Which branch of chemistry primarily studies compounds contained carbon?
A
Organic chemistry
6
Q
Alchemists were known for trying to convent ordinary metals into __________.
A
Gold
7
Q
What is anything that occupies space and mass?
A
Matter
8
Q
The Sumerians were skilled in the science of obtaining metals from ores. What is this science called?
A
Metallurgy
9
Q
What were the four basic elements the Greeks believed made up the universe?
A
Earth
Air
Fire
Water
10
Q
The logical thinking demanded by a course in chemistry helps Christians to further develop the ability to think critically.
T/F
A
True
11
Q
Alchemists were known for their experimentations.
T/F
A
True
12
Q
The Greeks desired knowledge rather than practical skills.
T/F
A
True
13
Q
Scientific theories should be accepted without question because they have results from thorough investigation.
T/F
A
False
14
Q
The scientific method, when used properly, can lead a person to determine absolute truth.
T/F
A
False
15
Q
As Christians, we all believe were all created how?
A
In God’s image
16
Q
What science explorers natural products and processes for specific purposes and applications?
A
Applied science
17
Q
What physical property explains materials that can be drawn into long, thin wires?
A
Ductility
18
Q
What is the most conductive metal?
A
Silver
19
Q
The measure of disorder or randomness of particles is also known as ______________.
A
Entropy
20
Q
What is the change from a gas to a liquid called?
A
Condensation
21
Q
Identify each of the following chemical formula: 5H2O
A
5- coefficient
2- subscript
H&O- element
Chemical symbol
22
Q
What is matter?
A
Is anything that takes up space and has mass
23
Q
Identify three characteristics of a solid:
A
Definite volume
Definite shape
Difficult to compress
24
What is the study of movement and conservation of energy?
Thermodynamics
25
What are changes that result in changes of the identity of a material?
Chemical change
26
What is a pure substance that cannot be broken down into a simpler substance by ordinary chemical means?
Element
27
What is an example of a molecule that occurs naturally as a monatomic element?
Xenon
28
What is the operation definition of energy?
The ability to do work
29
What energy is responsible for the forming of breaking bonds with other elements?
Chemical energy
30
What is the sum of the kinetic energy of an objects parities?
Thermal energy
31
What temperature is absolute zero?
-273.15 C
32
What is the standard SI unit for measuring energy and work?
Joules (J)
33
The first professor of chemistry in the United States
Benjamin Rush
34
Identify the three characteristics for each of the following:
Solids
Liquids
Gases
Solids:
Definite shape
Definite volume
Incompressible
Gases
No definite shape
Do definite volume
Highly compressible
Liquids
Shape of container
Definite volume
Nearly incompressible
35
Give an example of quantitative data.
The amount of fish in a bowl
36
List 3 of the six major branches of chemistry.
Organic chemistry
Inorganic chemistry
Nuclear chemistry
37
What is matter?
Anything that takes up space and has mass
38
What distinguishes mixtures from pure substances?
Type of change or bonding
39
Identify two homogeneous and two heterogeneous mixtures.
Homogeneous- cake and air
Heterogeneous- oil&vinegar dressing and granite
40
Physical or chemical property:
Colorless
Physical
41
Physical or chemical property:
Flammable
Chemical
42
Physical or chemical property:
Freezes at 34K
Physical
43
Physical or chemical property:
Magnetic
Physical
44
Physical or chemical property:
Explosive
Chemical
45
Physical or chemical property:
Sinks in water
Physical
46
The second letter in a chemical symbol is always capitalized.
T/F
Why
False
| The first letter is always capitalized
47
Kelvin temperatures cannot be negative.
T/F
Why
True
48
Reactions that release energy are exothermic.
T/F
Why
True
49
Everything in the universe is composed of chemicals.
T/F
Why
True
50
Temperature measures the total kinetic emery in a sample.
T/F
Why
False
| Thermal energy
51
What is the base unit for the dimension of mass and length?
Mass- kilogram(kg)
| Length- meter (m)
52
What is the comparison of the actual measurement and the numerical evaluation of the instrument?1
Accuracy
53
When adding and subtracting measurements, what must be taken into consideration when dealing with significant digits?
Precision
54
What is the formula for density?
d=m/v
55
What is the scale or a measuring instrument which is the accurately subdivided measuring units?
Calibrated scale
56
What is the prefix that represents million? Millionth?
Million- mega (m)
| Millionth- micro (u)
57
In order to deal with significant digits of a measurement, what two things must be present?
Number & unit
58
SI unit that represents the amount of particles of a substance
Mole
59
Your calculators answer is read from this type of screen
Digital
60
A fraction equal to one that contains both the original unit and it's equivalent value in a new unit
Conversion factor
61
Indicates the precision of an instrument and helps scientists report measurements honestly
Significant digits
62
System of measurement based on a decimal scale
Metric
63
The accurately subdivided measuring units
Calibrated
64
The result of comparing an unknown quantity to a standard unit
Measurement
65
Any artificial device made for the purpose of refining, extending, or substituting for the human senses when measuring
Instrument
66
The number 0.00800 has three significant digits
T/F
Why
True
67
When determining significant digits in multiplication and division problems, the answer cannot contain more significant digits than the measurement with the least number of significant digits.
T/F
Why
True
68
If a scientist is extremely careful and uses precise instruments, a perfect measurement can be obtained.
T/F
Why
False
| There is always going to be uncertainty with measurements, there is no perfect measurement.
69
The unit for volume is derived from the SI unit for length, the meter.
T/F
Why
True
70
The first step in problem solving is choosing the specific tools to use.
T/F
Why
False
| Read the statement of problem
71
When wolfing problems that involve compost calculations, it is nest to round off at each of the intermediate steps.
T/F
Why
False
| Don't round until the end
72
Give four of the seven base units for SI and the basic dimension that each represents.
Length- meter (m)
Time- seconds (s)
Mass- kilogram (kg)
Temperature- kelvin (K)
73
Explain the difference between accuracy and precision.
Accuracy is how close your measurement is to the actual measurement. Precision is how close a repeated number of measurements are to each other.
74
Hundredth
Centi
75
Million
Mega
76
Tenth
Deci
77
Billionth
Nano
78
Thousandth
Milli
79
Thousand
Kilo
80
Millionth
Micro
81
What is the maximum numbers of electrons that can be found in any atom's second principle energy level?
8
82
Who was the first to refer to the smallest particles composing matter as atoms?
Democritus
83
What rule describes how electrons fill an orbital?
Hund's rule
84
The following equals the number of protons and neutrons:
Mass number (A)
85
What charge does an atom have if it loses an electron?
Positive=cation
86
Who discovered the electron?
Thompson
87
An atom that gains three electrons will have a +3 charge.
T/F
False
88
An electron can behave either as a wave of a particle.
T/F
True
89
What are the names and values for the four sublevels?
S-0
P-1
D-2
F-3
90
Isotopic atoms have different number of __________, while ions have a differing number of _____________.
Neutrons
| Electrons
91
Philosophical atomism
Democritus
92
First experimental atomic model
John dalton
93
Cathode rays
J. J Thomas
94
X rays
Wilhelmina roentgen
95
Neutrons
James Chadwick
96
Protons
Ernest Rutherford
97
God foil experiment
Hans Geiger
98
What is the idea that any sample of water always contains 8 g of oxygen for every 1 g of hydrogen.
Law of definite composition
99
The type of sublevel found in all principle energy levels is the ____ level.
S
100
The s, p, d, and f sublevels are identified by _________ quantum numbers.
Azimuthal
101
Two different isotopes of a single element will have the same number of _________ but different number of ___________.
Protons
| Neutrons
102
The general region of space where an electron is most probably found is known as it's orbital.
T/F
True
103
Dalton based his atomic model on both experiments and logic.
T/F
True
104
Neutrons contribute to an atom's mass and it's charge.
T/F
False
105
An electron can behave as either a wave or particle.
T/F
True
106
Each atom can be identified by the number of protons in its nuecleus.
T/F
True
107
The first quantum number identifies the principle energy level of an electron.
T/F
True
108
Compare three different atomic models.
Dalton's atomic model, Thompsons plum pudding model, and rutherford's nuclear model all dealt with uncertainty and enhanced in later years.
109
First model to include atoms of each element having different masses.
Dalton
110
States that it is impossible to know both the energy and the exact position of an electron at the same time.
Uncertainty principle
111
Describes how electrons fill orbitals.
Hunds
112
Describes now electrons fill sublevels
Aufbua
113
Equals the numbers of protons and neutrons.
Mass number
114
Electrons in the outermost energy level that are important in bonding.
Valence electrons
115
Negatively charged ions.
Anions
116
Charge of an atom if it loses an electron.
Positive
117
What is determined by the weighted averages of isotopes on an element?
AMU
118
What is the minimum energy required to remove the first electron form it's outermost shell to make it a cation?
First ionization energy
119
Helium, neon, argon, and krypton are all examples of what family of elements?
Noble gases
120
What group of elements conduct electricity only under certain conditions therefore are known as semiconductors.
Metalloids
121
What is the measured attraction between the nucleus and the valence electrons?
Electronegativity
122
Who was the Nobel Prize winning chemist who devised an electronegativity scale?
Linus Pauling
123
What states that the properties of elements vary with their atomic numbers in a periodic way?
Periodicity
124
Which element has a larger atomic radius: potassium or helium?
Potassium
125
Which element has a higher first ionization energies: calcium or krypton?
Krypton
126
What is the tasteless, odorless gas that accounts for 21% of the earth's ato sooner and is the most abundant element in the earth's crust. It is also essential for the life of animals and humans.
Oxygen
127
The two elements that are the major constituents of hard water and magnesium and ____________.
Calcium
128
Mendeleev's periodic table was arranged by elements what?
First mass, then atomic number
129
Who arranged a number of elements in triads based on similar properties?
Dobreiner
130
Whose work resulted in the revision in of the periodic law and the atomic number being used as the organizing factor for the elements of the periodic table?
Moseley
131
What chemist arranged the elements according to increasing atomic masses and thereby discovered the relationship he called the law of octaves?
Newlands
132
It is the lightest and most abundant element in the universe is extremely flammable in the air, and is used in the industrial production of ammonia.
Hydrogen
133
Existing as diatomic molecules, this gas is tasteless, colorless, odorless and it accounts for approximately 78% of the earths atmosphere.
Nitrogen
134
According to the Big Bang theory, the very first elements would problem have been....?
H and He
135
The presence of calcium and magnesium ions in water makes it "hard" water.
T/F
True
136
Graphite and diamonds are both composed of the same element, carbon.
T/F
True
137
Halogens are easily obtainable in their elemental form.
T/F
False
138
High electronegativity is are associated with large ionization energies and high electron affinities.
T/F
True
139
Under normal conditions, noble gases form compounds with other elements easily.
T/F
False
140
Mendeleev's work sets him apart from other scientists because of his obsessiveness about his work.
T/F
True
141
Helium, neon, argon, xenon, radon
Noble gases
142
Oxygen, nitrogen, carbon, sulfur
Nonmetal
143
Flourine, chlorine, iodine, bromine
Halogens
144
Boron, silicon, arsenic, germanium
Metalloids
145
Semiconductors
Metalloids
146
Good conductors of heat and electricity, usually hard, lustrous, malleable, and ductile
Metals
147
Contains characteristics of both metals and nonmetals.
Metalloids
148
Generally gases or soft solids
Nonmetals
149
Negative ion
Anion
150
The minimum energy required to remove the first electron from its outermost shell to make it a cation
First ionization energy
151
Distance from the center of an atom's nucleus to its outermost electron.
Atomic radius
152
Positive ion
Cation
153
Amount of energy required to add an electron to a neutral atom to form a negative ion
Electron affinity
154
The electron-sea theory applies to what bonds?
Metallic
155
What bond is between the attraction of oppositely charged ions?
Ionic
156
What is the ultimate purpose of why atoms bond?
Octet rule
157
In the Lewis structure, how many electrons does the dash represent?
Two
158
When one or two pairs of shared electrons bond, what bond occurs?
Covalent
159
What is the mixture of metal atoms with another element resulting in a mixture with metallic properties?
Alloys
160
Examples of network covalent substances
Diamonds
Silicate
Quartz
161
Diatomic molecules
H2 N2 O2 Cl2 F2 Br2 I2
162
What is the tendency of an object to form two localized regions of opposite character?
Polarity
163
What are the two-dimensional diagrams that show the bonds between different atoms?
Lewis structures
164
What is the force exerted between electrical charges of two atoms?
Electrostatic force
