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Chemistry 105 > Chapter 1 > Flashcards

Chapter 1 Flashcards

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1
Q

What is the definition of significant figures?

A

Expressing a measurement with the correct number of digits.

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2
Q

What is scientific notation?

A

A way to express numbers as a coefficient between 1 and 10 multiplied by 10 raised to an exponent.

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3
Q

What does the coefficient represent in scientific notation?

A

A number between 1 and 10.

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4
Q

What does the exponent represent in scientific notation?

A

Any positive or negative whole number.

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5
Q

What is the first step in using the scientific method?

A

Make observations about nature and ask questions about what you observe.

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6
Q

What is a hypothesis?

A

A possible explanation of the observations.

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7
Q

What is the purpose of experiments in the scientific method?

A

To test the hypothesis.

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8
Q

What is concluded when the results of experiments are analyzed?

A

A conclusion is made as to whether the hypothesis may be true or false.

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9
Q

What happens if the results of the experiments do not support the hypothesis?

A

The hypothesis is modified.

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10
Q

What is matter?

A

Anything that has mass and takes up volume.

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11
Q

What is the classification of matter?

A

Elements and compounds, atoms and molecules, pure and impure, states of matter, physical and chemical properties.

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12
Q

Which of the following contain chemicals? A. Sunlight, B. Fruit, C. Milk, D. Breakfast cereal

A

B. Fruit, C. Milk, D. Breakfast cereal.

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13
Q

True or False: Numbers with negative exponents in scientific notation are decimal numbers less than one.

A

True.

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14
Q

What is the scientific notation for the number 3097?

A

3.097 x 10^3.

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15
Q

What is the scientific notation for 0.000138?

A

1.38 x 10^-4.

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16
Q

What is the scientific method?

A

A set of general principles that helps to describe how a scientist thinks.

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17
Q

What type of change is melting ice?

A

Physical change.

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18
Q

What is the difference between a compound and an element?

A

A compound is formed by chemically joining two or more elements; an element cannot be broken down by a chemical change.

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19
Q

What is the definition of a homogeneous mixture?

A

The composition is uniform throughout this mixture.

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20
Q

What is the definition of a heterogeneous mixture?

A

A mixture composed of more than one component with varying composition.

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21
Q

What is the metric system’s base unit for length?

A

Meter.

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22
Q

What is a physical property?

A

A property that can be observed or measured without changing the composition of the material.

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23
Q

What is a chemical property?

A

A property that determines how a substance can be converted into another substance.

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24
Q

Fill in the blank: The number of molecules of CO2 exhaled in one breath is approximately ______.

A

320,000,000,000,000,000,000.

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25
How do you convert a number in scientific notation back to a standard number when the exponent is positive?
Move the decimal point x places to the right.
26
How do you convert a number in scientific notation back to a standard number when the exponent is negative?
Move the decimal point x places to the left.
27
What is the volume of 1 liter in milliliters?
1,000 milliliters.
28
What is the relationship between significant figures and inexact numbers?
An inexact number results from a measurement and contains some uncertainty.
29
What is the formula for measuring volume?
Volume = Length x Width x Height.
30
True or False: All matter is made up of basic building blocks called atoms.
True.
31
What is the scientific notation for 520,000 with 3 significant figures?
5.20 x 10^5.
32
What is the relationship between cubic centimeters and milliliters?
1 mL = 1 cm³ ## Footnote This indicates that 1 milliliter is equivalent to 1 cubic centimeter.
33
Define a physical change.
A physical change alters the material without changing its composition ## Footnote Examples include melting ice to form liquid water and boiling liquid water to form steam.
34
What is the SI unit for volume?
Cubic meter (m³) ## Footnote In practice, liters (L) are often used for everyday measurements.
35
Convert 1 kilometer to meters.
1 kilometer = 1,000 meters ## Footnote This is a basic metric conversion.
36
What is the definition of mass?
Mass is a measure of the amount of matter in an object ## Footnote Weight, in contrast, is the force that matter feels due to gravity.
37
What is the SI unit for mass?
Kilogram (kg) ## Footnote 1 kg = 1,000 grams (g).
38
True or False: Significant figures include all the digits in a measured number including one estimated digit.
True ## Footnote Significant figures are important in scientific measurements.
39
What are the three temperature scales commonly used?
Degrees Fahrenheit (°F), Degrees Celsius (°C), Kelvin (K) ## Footnote Each scale has its own conversion formulas.
40
Fill in the blank: 1 centimeter (cm) = _____ meters (m).
0.01 meters
41
What is the formula to convert Celsius to Fahrenheit?
°F = 1.8(°C) + 32 ## Footnote This formula allows for temperature conversion between the two scales.
42
What is density?
Density is the measured relationship between mass and volume of an object ## Footnote It is calculated as Density (d) = Mass (g) / Volume (mL).
43
What is the formula for specific gravity?
Specific gravity = density of substance (g/mL) / density of water (g/mL) ## Footnote Specific gravity is unitless since the units cancel out.
44
What happens to the density of a substance when it is heated?
Generally, density decreases as temperature increases ## Footnote This is due to the expansion of the substance.
45
What is the SI unit for temperature?
Kelvin (K) ## Footnote Celsius (°C) is commonly used in everyday contexts.
46
Fill in the blank: The SI unit of time is the _____
second (s)
47
How do you determine the number of significant figures in a measured value?
All non-zero digits are significant; leading zeros are not; trapped zeros are significant; trailing zeros are significant only if there is a decimal point ## Footnote This rule helps in accurately reporting measurements.
48
What is the conversion factor for mass from kilograms to pounds?
1 kg = 2.20 lb ## Footnote This helps in converting mass measurements between metric and imperial systems.
49
What is the formula for converting Kelvin to Celsius?
°C = K - 273 ## Footnote This formula allows for temperature conversion between the two scales.
50
True or False: The density of a less dense substance will sink in a denser substance.
False ## Footnote Less dense substances float on top of denser substances.
51
List the prefixes used in the metric system.
* Kilo- * Centi- * Milli- ## Footnote These prefixes indicate the scale of measurement relative to the base unit.
52
What are extrinsic properties?
Properties influenced by the amount of substance present ## Footnote Examples include mass, volume, and solubility.
53
What is the average density of an average human brain with a mass of 1.30 kg and a capacity of 1.24 L?
1.05 kg/L ## Footnote Density is calculated as mass divided by volume.
54
What happens to significant figures during addition and subtraction?
The answer has the same number of decimal places as the original number with the fewest decimal places ## Footnote This rule ensures precision in calculations.
55
What is the significance of the number of significant figures in scientific calculations?
They indicate the precision of a measurement ## Footnote Using the correct number of significant figures is critical in scientific reporting.
56
What is the base unit in measurement?
Each type of measurement has a base unit.
57
What does SI stand for?
International System of Units.
58
What is a conversion factor?
A term that converts a quantity in one unit to a quantity in another unit.
59
Give an example of a conversion factor.
2.21 lb = 1 kg
60
What is density?
A physical property that relates the mass of a substance to its volume.
61
What are intrinsic properties?
Properties which are not influenced by the amount of substance present, such as color, boiling point, and melting point.
62
What is the formula for density?
Density = mass / volume.
63
Fill in the blank: To convert volume (mL) to mass (g), use the formula _______.
mL x (g/mL) = g.
64
Fill in the blank: To convert mass (g) to volume (mL), use the formula _______.
g x (mL/g) = mL.
65
True or False: The amount of a substance influences its density.
False.
66
How do you solve a density problem using the factor-label method?
Set up the problem with conversion factors that cancel unwanted units.
67
What is the significance of significant figures in calculations?
The answer must be written with the correct number of significant figures.
68
How would you convert 325 mg to grams using the factor-label method?
325 mg x (1 g / 1000 mg) = 0.325 g.
69
Using the factor-label method, how many liters are in 1.0 pint?
0.47 L.
70
What is the conversion factor for converting pounds to kilograms?
2.21 lb = 1 kg.
71
What is the density of muscle?
1.1 g/cm³.
72
What is the density of fat?
0.9 g/cm³.
73
How do you set up a problem using two or more conversion factors?
Arrange factors so that the denominator in one term cancels the numerator in the preceding term.
74
What is the density of acetic acid?
1.05 g/mL.
75
How do you find the mass of a substance using density?
Mass = Density x Volume.
76
What is the formula to find the volume from mass using density?
Volume = Mass / Density.

Chemistry 105 (1 decks)

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