1
Q
What is elemental matter?
A
Matter that is comprised of only 1 type of atom.
2
Q
What is the symbol for iron and its Latin origin?
A
Fe, derived from FERRUM
3
Q
What is the symbol for gold and its Latin origin?
A
Au, derived from AURUM
4
Q
What are macroscopic physical properties?
A
Properties that can be observed using the 5 senses, such as hardness, shape, color, texture, malleability, and ductility.
5
Q
What instrument can help visualize atoms?
A
Atomic Force Microscope (AFM)
6
Q
What does an AFM do?
A
Uses a probe to scan the surface of a piece of matter and record an image.
7
Q
Fill in the blank: The symbol for iron is _______.
A
Fe
8
Q
True or False: All matter on earth is made up of atoms.
A
True
9
Q
What is an example of a macroscopic property of gold?
A
Yellowish hue
10
Q
List two properties that can distinguish iron from gold.
A
- Color
- Hardness
11
Q
How are elements categorized in the Periodic Table?
A
Elements are categorized into metals and non-metals.
Most elements are metals, located on the left-hand side.
12
Q
Where is hydrogen located in the Periodic Table and what is its classification?
A
Hydrogen is in group 1 on the left-hand side but is classified as a nonmetal.
13
Q
What are the three states of matter?
A
Solid, liquid, and gas.
14
Q
What is the physical state of most elements at room temperature?
A
Most elements are solids at room temperature.
15
Q
Which two elements are liquid at room temperature?
A
- Bromine (nonmetal)
- Mercury (metal)
16
Q
What is the microscopic structure of solids?
A
Solids have a definite shape and volume, with particles tightly packed in an organized structure called a lattice structure.
17
Q
What type of motion do particles in a solid exhibit?
A
Particles in a solid exhibit only vibrational motion.
18
Q
How do liquids differ from solids regarding particle movement?
A
Liquids have a definite volume but take the shape of their container, with particles that can move past one another.
19
Q
What types of motion do particles in a liquid exhibit?
A
- Vibrational motion
- Rotational motion
- Translational motion
20
Q
What defines the volume and shape of a gas?
A
The volume and shape of a gas depend on its container.
21
Q
What is the microscopic structure of gases?
A
Gases have no structure and are disordered, with particles in constant linear motion.
22
Q
What is a molecule?
A
A molecule is formed when atoms are linked together.
23
Q
What is the chemical formula for water?
A
H2O.
24
Q
What do the subscripts in a chemical formula indicate?
A
Subscripts indicate the number of each type of atom in a molecule.
25
What does the ball and stick model represent?
Atoms are represented as balls and bonds are represented as sticks.
26
What is the composition of a water molecule?
A water molecule is comprised of 2 hydrogen atoms and 1 oxygen atom.
27
How are water molecules structured in solid form (ice)?
In solid water, molecules are organized into a repeating pattern and vibrate constantly.
28
What is the composition of a methane molecule?
One methane molecule is composed of 1 carbon atom and 4 hydrogen atoms.
29
What happens to the structure of methane molecules in solid form?
Methane molecules are organized into a repeating pattern.
30
What is scientific notation?
A way to represent numbers using the form a x 10^b, where a is the mantissa and b is the exponent.
31
What is the mantissa in scientific notation?
The mantissa is a real number between 1 and 10, not including 10.
32
How do you compare two numbers in scientific notation?
Compare the exponents; the number with the larger exponent is greater.
33
What is the result of multiplying numbers in scientific notation?
Multiply the mantissas and add the exponents.
34
What is the result of dividing numbers in scientific notation?
Divide the mantissas and subtract the exponents.
35
What is the scientific notation for 0.83 x 10^11?
8.3 x 10^10.
36
What does the exponent indicate in scientific notation?
The exponent indicates the power of ten that the mantissa is multiplied by.
37
What is an example of a very small number in scientific notation?
7.2 x 10^-11.
38
What happens when you divide a small number by an even smaller number?
You get a very large number.
39
What do numbers in science usually represent?
An amount of something
## Footnote
Examples include distance, mass, and energy.
40
What are the components of a quantity in science?
A number and a unit
## Footnote
Each quantity must be accompanied by a measurement unit.
41
What system do scientists use for standard units?
SI system
## Footnote
SI stands for the International System of Units.
42
What does the SI unit for mass represent?
Kilograms
## Footnote
1 kg is approximately 2.2 pounds.
43
What does the SI unit for length represent?
Meters
## Footnote
Example: The Empire State Building is 443 meters tall.
44
What does the SI unit for volume represent?
Liters
## Footnote
A typical water bottle holds a liter.
45
What does the SI unit for energy represent?
Joules
## Footnote
Energy is measured in joules in the SI system.
46
What is the average weight of a 10-year-old child in kilograms?
About 35 kg
## Footnote
This is a typical weight reference for children.
47
How many milliliters are in a liter?
1000 milliliters
## Footnote
Milliliters are often used for measuring liquids in lab settings.
48
True or False: The British system is preferred in scientific measurements.
False
## Footnote
The metric system (SI) is preferred over the outdated British system.
49
Fill in the blank: The amount of substance is an important _______ in science.
quantity
## Footnote
Understanding the amount of substance is crucial in various scientific contexts.
50
List the four base units in the SI system.
* Mass (kilograms)
* Length (meters)
* Volume (liters)
* Energy (joules)
## Footnote
These units form the foundation for measurement in science.
51
What is the energy required to lift a little book one meter into the air?
About one joule
## Footnote
This serves as a practical example of energy measurement in physics.
52
How much energy is consumed by enjoying a candy bar?
About 1.3 x 10^8 joules
## Footnote
This illustrates a large quantity of energy in everyday terms.
53
What is the challenge with measuring physical quantities?
They are often not measured or reported in base units
## Footnote
This highlights the importance of understanding conversions.
54
What must you recognize and memorize regarding metric prefixes?
All the metric prefixes and the units shown in green
## Footnote
This is essential for converting numerical quantities among prefixes.
55
Fill in the blank: The unit you might be least comfortable with is the _______.
joule
56
True or False: The joule is a base unit of energy.
True
57
What mathematical operation is used to isolate x in the equation?
Algebra
## Footnote
Algebraic manipulation is necessary to solve for the unknown variable.
58
What is the conversion factor for gigabytes to bytes?
1 GByte = 10^9 bytes
## Footnote
This conversion factor is crucial for converting larger data units.
59
How is the proportion equation set up for converting GB to bytes?
1 GB/10^9 B = 2.2 GB/x B
## Footnote
This equation helps in finding the value of x which represents bytes.
60
What does x equal when converting 2.2 GB to bytes?
2.2 x 10^9 B
## Footnote
This result shows the total number of bytes in 2.2 gigabytes.
61
Is the ratio or proportion for unit conversions always the same?
True
## Footnote
The consistency of ratios simplifies the conversion process across different units.
62
Fill in the blank: The general method for any conversion problem involves setting up a _______.
proportion equation
## Footnote
This method allows for systematic conversion between different units.
63
What is indicated when conversions are described as complex?
Another method may be easier to use
## Footnote
Complex conversions might require alternative strategies beyond simple proportions.
64
What is the starting unit in the gigabyte conversion example?
2.2 GB
## Footnote
The starting unit is the unit we want to convert.
65
What is the desired unit in the gigabyte conversion example?
Bytes
## Footnote
The desired unit is the unit we want to convert to.
66
What conversion factor is used to convert GB to Bytes?
10^9 bytes per GB
## Footnote
This factor is used to cancel the GB dimension.
67
What method is used to perform conversions when multiple steps are required?
Dimensional analysis
## Footnote
This method involves using conversion factors to cancel units.
68
True or False: We can use the terms 'dimensions' and 'units' interchangeably.
True
## Footnote
Both terms refer to the same concept in dimensional analysis.
69
What is the SI unit for mass?
Kilogram (kg)
70
What is the SI unit for length?
Meter (m)
71
What is the SI unit for volume?
liter (l)
72
What is the SI unit for energy?
Joule (J)
73
What is the SI unit for time?
Second (s)
74
What is the SI unit for temperature?
Kelvin (deg celsius) K (deg C)
75
True or False: The liter (L) is an SI unit of volume.
True
76
True or False: The SI unit for mass is the gram (g).
False
77
What is the SI unit for amount of substance?
Mole (mol)
78
Fill in the blank: The SI unit for work is the _____ (J).
Joule
79
True or False: The SI unit for temperature is Celsius.
False
80
What is the base unit for quantity of substance in the SI system?
Mole (mol)
81
True or False: The SI unit for length is the kilometer.
False
82
What is the SI unit for surface area?
Square meter (m²)
83
True or False: The SI unit for volume is the cubic centimeter.
False
84
What is the SI unit for molar mass?
Kilogram per mole (kg/mol)
85
Fill in the blank: The SI unit for work done is the _____ (J).
Joule
86
What is the SI unit for the rate of radioactive decay?
Becquerel (Bq)
87
True or False: The SI unit for the amount of substance is the liter.
False
88
What is the SI unit for enzyme activity?
Katal (kat)
89
True or False: The SI unit for work is measured in joules.
True
90
Fill in the blank: The SI unit for specific energy is _____ (J/kg).
Joule per kilogram
91
What is the SI unit for the measure of temperature difference?
Kelvin (K)
92
What is the SI unit for the measure of energy in a system?
Joule (J)
93
Fill in the blank: The SI unit for the measure of radioactivity is the _____ (Bq).
Becquerel
94
What prefix represents one million in the metric system? (10 6)
Mega
95
True or False: The prefix 'deci' represents one-tenth.
True
96
Fill in the blank: The prefix 'kilo' means _____ times the base unit.
1000
97
Which prefix corresponds to a factor of 10?
Deka
98
What is the prefix for one billion? 10 9
Giga
99
True or False: The prefix 'centi' indicates one-hundredth.
True
100
What does the prefix 'milli' represent?
One-thousandth
101
Which prefix is used to denote a factor of 10^-6?
Micro
102
Fill in the blank: The prefix 'nano' indicates _____ times the base unit.
10^-9
103
What is the metric prefix for one thousandth?
Milli
104
Which prefix means one hundred? )10 2
Hecto
105
What is the meaning of the prefix 'pico'?
10^-12
106
What prefix represents a factor of 10^3?
Kilo
107
Fill in the blank: The prefix 'giga' means _____ times the base unit.
10^9
108
True or False: The prefix 'femto' denotes one quadrillionth. 10 -15
True
109
What is the prefix for one hundredth?
Centi
110
Which prefix represents a factor of 10^6?
Mega
111
What prefix corresponds to ten?
Deca
112
True or False: Ductility is a measure of a material's ability to undergo significant plastic deformation before rupture.
True
113
Fill in the blank: Materials that are highly ductile can be drawn into ______.
wires
114
Which of the following materials is known for high ductility? A) Glass B) Copper C) Ceramics
B) Copper
115
What is the opposite of ductility?
Brittleness
116
True or False: Ductility can be affected by temperature.
True
117
What type of stress is primarily associated with ductility?
Tensile stress
118
What is a common application of ductile materials?
Electrical wiring
118
Multiple Choice: Which of the following processes benefits from ductility? A) Casting B) Forging C) Machining
B) Forging
119
What term describes the maximum amount a material can stretch before breaking?
Ultimate tensile strength
120
True or False: Ductility is only relevant for metals.
False
121
What is the definition of malleability?
Malleability is the ability of a material to deform under compressive stress, often characterized by the material's capacity to be shaped or molded.
122
True or False: Malleability refers to the ability of a material to be stretched into a wire.
False
123
Fill in the blank: Malleability is a property often associated with __________ materials.
ductile
124
Which of the following materials is known for its high malleability? A) Glass B) Gold C) Wood D) Plastic
B) Gold
125
What factors can affect the malleability of a material?
Temperature, composition, and the presence of impurities can affect the malleability of a material.
126
What is the definition of hardness in materials science?
Hardness is the measure of a material's resistance to deformation, particularly permanent deformation, scratching, cutting, or abrasion.
127
Scientific notation includes 1 and 10. True or False
False
128
Which two elements are liquid at room temperature?
Mercury (Hg) and Bromine (Br)
129
When multiplying numbers how many significant digits should the product have?
the same as the number with the least amount of significant figures
130
What is the order of magnitude in a scientific number?
the exponent
131
The reactivity of metals increases as you move across a
period and increases as you move down a group.
False
The reactivity of metals decreases as you move across a
period and increases as you move down a group.
132
When adhering to the rules of significant figures, the answer from adding or subtracting numbers must be written how?
the decimal places must be equal to the number with the least amount of decimal places.
Remember: brackets first
133
When adhering to the rules of significant figures, the answer from multiplying or dividing numbers must be written how?
the number of significant figures must be equal to the number with the least amount of significant figures
Remember: brackets first
134
What is Group 1 in the periodic table commonly known as?
Alkali metals
135
Which group in the periodic table contains the noble gases?
Group 18
136
True or False: Group 2 elements are called alkaline earth metals.
True
137
Fill in the blank: Group 17 elements are known as ______.
Halogens
138
What is the common characteristic of the elements in Group 1?
They are highly reactive and have one electron in their outer shell.
139
Which group contains the transition metals?
Groups 3 to 12
140
Which group in the periodic table is known for having a complete valence shell?
Group 18 (Noble gases)
141
Multiple choice: Which of the following is not a halogen? A) Fluorine B) Chlorine C) Oxygen D) Iodine
C) Oxygen
142
What is the primary characteristic of alkaline earth metals in Group 2?
They have two electrons in their outer shell.
143
Which group is known for its reactivity with alkali metals to form salts?
Group 17 (Halogens)
144
What are the two rows of elements placed below the main body of the periodic table called?
Lanthanides and Actinides
145
Multiple choice: Which group contains elements that are typically good conductors of electricity? A) Group 1 B) Group 17 C) Group 18 D) Group 14
A) Group 1
146
What is a common property of noble gases in Group 18?
They are inert and do not readily form compounds.
147
The elements in group 2 are called ?
earth alkali metals
148
Is selenium a metal or nonmetal?
Selenium is a non metal
149
Boron is a non metal
False, boron is a metalloid
150
Silicon is a nonmetal like phosphorus.
False, silicon is categorized as a metalloid (semimetal)
151
What group name are the following elements categorized under? Gallium, Germanium, Arsenic, Selenium
Metals (metalloids): Gallium, Germanium, Arsenic
Nonmetal: Selenium
152
What group name are the following elements categorized under? Germanium, Arsenic, Selenium, Antimony, Tellurium
Metals (metalloids) : Germanium, Arsenic
Antimony, Tellurium
nonmetal: Selenium
Chem 1
flashcards
Decks in class (18)
# Cards
-
Polyatomic ions29
-
Elements And Their Names60
-
Topic 1 Matter Models Math153
-
Topic 6 Energy Consideration10
-
Topic 2 Atoms and Orbitals79
-
Topic 3 Basic Bonding Principles174
-
Topic 10 Molecular Geometry111
-
Topic 11 Valence Bond Theory63
-
Topic 12 Molecular Orbital Theory72
-
Topic 7 Periodic Trends70
-
Topic 8 Atomic Spectroscopy65
-
Topic 9 The Electron96
-
Topic 13 The Mole18
-
Topic 14 Stoichiometry Calculations10
-
Topic 15 Empirical and Molecular Formula15
-
Topic 16 Phase Change and IMFs148
-
Topic 17 Gases84
-
Topic 18 Applications of Stoichiometry37
