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CHEMISTRY 107: FUNDAMENTALS > EXAM 1 - PREP > Flashcards

EXAM 1 - PREP Flashcards

MAJOR TOPICS ARE: SIG FIGS, SCIENTIFIC METHOD, DIMENSIONAL ANALYSIS, UNIC CONVERSIONS, DEFINITIONS, PROPERTIES OF MATTER AND THE STRUCTURE AND PROPERTIES OF ATOMS,

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1
Q

(Q:1.1)What the definition of a Scientific Law?

A) A law is a number of similar observations generalized into a brief statement summarizing past observations and predicting new ones.

B) A law is the underlying reason for scientific theory

C) A law is a way of learning that emphasizes observation and experimentation

A

A) A law is a number of similar observations generalized into a brief statement summarizing past observations and predicting new ones.

LAWS PREDICT WHILE THEORIES TRY TO EXPLAIN

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2
Q

what is kinetic energy definition?

A

kinetic energy is the energy of motion

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3
Q

(Q:1.1)What is the definition of a scientific theory?

A) A brief statement that summarizes past observations and predicts future ones

B) It is a model that explains the underlying reasons for observations and laws

C) It is a method of learning that emphasizes reason as the way to understand the world

A

B)it is a model that explains the underlying reasons for observations and laws

THEORIES ATTEMPT TO EXPLAIN OBSERVATIONS

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4
Q

(Q:1.1)Which of the following statements best describes the purpose of performing experiments?

A) Experiments are designed to produce the results predicted by a theory or hypothesis.

B) Experiments can be replaced by logical reasoning based on the known facts

A

A) Experiments are designed to produce the results predicted by a theory or hypothesis.

SCIENTIFIC METHOD IS A CYCLE AND RELIES ON OBSERVATIONS

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5
Q

(Q:1.1)Which of the following would be considered a hypothesis?

A) Birds can fly because they have hollow bones

B) Spiders have eight legs

C) Fresh Lava from a volcano is hot

D) None of the choices can be considered a hypothesis

A

A) Birds can fly because they have hollow bones.
++BECAUSE EMPHASIZES AN ATTEMPT TO EXPLAIN IF THIS.. THEN THAT..
++A HYP IS TESTABLE AND TENTATIVE EXPLANATION FOR AN OBSERVATION

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6
Q

(Q:1.1)Which of the statements below is NOT part of the Scientific method?

A) Observations and measurement

B) Formation of a hypothesis

C) Testing of a hypothesis by experimentation

D) Refinement of a hypothesis
as needed

E) All of the above steps are part of the scientific method

A

E) All of the above steps are part of the scientific method

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7
Q

(Q:1.1)Which of the following is false?

A) Experiments can be used show that a theory is somewhat limited in scope.

B) A hypothesis which has successfully withstood many tests eventually can become a theory

C) In general, a theory can be proven to be absolutely true

A

C) In general, a theory can be proven to be absolutely true

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8
Q

(Q1.1)TRUE OR FALSE: Science is the same as Technology?

A

FALSE

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9
Q

(Q1.1)TRUE OR FALSE: There is much overlap between science and technology

A

TRUE

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10
Q

(Q:1.1) Explain the similarities between a scientific Law and scientific theory as they relate to the scientific method:

A

A scientific Law and scientific theory are both based on the scientific foundation of observing and experimentation. They both trying to describe conditions that are happening based on information gathered. However a Law does not explain why, just the conditions for which a certain phenomenon is observed. A theory tries to predict and explain WHY.

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11
Q

(PS:1)
“In the scientific method, a ______________ is a tentative interpretation, or an initial explanation.

A

Hypothesis

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12
Q

(PS:1)
“___________________ are garnered from experiments in order to test an explanation or theory.”

A

Observations

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13
Q

(PS:1) “You may be able to make a brief statement that will only predict a future event, this is called a ___________”

A

Law

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14
Q

(PS:1) “It is possible that after enough testing and scrutiny, you have a well-supported explanation of a phenomenon that also makes predictions, this is called a ________________”

A

Theory

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15
Q

(HW:1.1) Which of the following is NOT part of the scientific method?

A) observation and measurement

B) formation of a hypothesis

C) testing of a hypothesis by experimentation

D) refinement of a hypothesis as needed

E) All of the above are parts of the scientific method

A

E) All of the above are parts of the scientific method

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16
Q

(H.W:1.1) Which Statement about the scientific method is TRUE?

A)The scientific method emphasizes reason as the way to understand the world

B)The scientific method emphasizes observations and experimentation as the way to understand the world

A

B) The scientific method emphasizes observations and experimentation as the way to understand the world

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17
Q

(H.W:1.1) Which of the statements below can be classified as an observation?

A)The universe began as a cosmic explosion called the Big Bang

B) All Matter is made up of atoms

C) When wood is burned in a closed container, the mass of the container and its contents are the same before and after burning

A

C) When wood is burned in a closed container, the mass of the container and its contents are the same before and after burning.

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18
Q

(HW:1.1)Which of the following statements best describes the purpose of performing experiments?

A) Experiments can be replaced by logical reasoning based on the known facts

B) Experiments attempt to produce other observations that support or refute a theory or hypothesis

A

A) Experiments can be replaced by logical reasoning based on the known facts

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19
Q

(1.1) TRUE/FALSE All Leading Zeros are significant
i.e 000002.00

A

FALSE
leading zeroes are never sig figs

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20
Q

(HW:1.1) What is the definition of a scientific theory?

A) It is a brief statement that summarizes past observations and predicts future ones.

B) It is a model that explains the underlying reasons for observations and laws

C) It is a method of learning that emphasizes reason as the way to understand the world.

A

B) It is a model that explains the underlying reasons for observations and laws

**A LAW PROVIDES PREDICTIONS BASED ON OBSERVATIONS. IT CAN PREDICT NEW OBSERVATIONS

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21
Q

(HW:1.1) Which of the following items does NOT contain chemicals?

A) drain cleaner

B) organically grown vegetables

C) air

D) All of the above contain chemicals

A

D) all of the above contains chemicals

++ALL SUBSTANCES CONTAIN CHEMICALS BC ALL CONTAIN MASS = ATOMIC STRUCTURE

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22
Q

(HW:1.1) Which of the following statements is true?

A) Nanotechnology employs devices that are generally greater than 100nm

B) Nanotechnology works with devices that are always less than 1 nm

C) Nanotechnology deals with dimensions that are less than 100nm

D) Nanotechnology deals with dimensions at any size

A

C) Nanotechnology deals with dimensions that are less than 100nm

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23
Q

(HW:1.1) TRUE/FALSE Science is the pursuit of knowledge of the world around us, whereas technology is the application of scientific knowledge for practical purposes.

A

TRUE

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24
Q

(1.1) TRUE/FALSE The Scientific method is a systematic approach to gaining knowledge

A

TRUE

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25
Q

(1.1)”When wood is burned in a closed container, the mass of the container before burning remains the same after burning.” Is an example of an _____________

A

Observation

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26
Q

(1.1) “John’s blue T-Shirt is blue because it reflects light.” This is an example of ______________

A

Hypothesis

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27
Q

(1.1) “When objects fall, they accelerate towards the earth’s surface.” This is an example of _______________

A

Law

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28
Q

(1.1) TRUE/FALSE Experiments attempt to produce other observations that support or refute a theory or hypothesis.

A

TRUE

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29
Q

(1.1) TRUE/FALSE A control experiment differs from a test experiment in only one variable.

A

TRUE

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30
Q

(1.1)Nanotechnology is the understanding and control of matter at the _________. Nanotechnology deals with dimensions between approximately __________ and ___________ nanometers where unique phenomena enable novel applications.

A

Nanoscale……. 1…… 100

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31
Q

(1.1)When a hypothesis is thoroughly ________. It may become a ___________.

A

Tested….Theory

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32
Q

(1.2) How many SIG FIGS would be used in calculations with the measurement:

2.34m

A

3 SF in 2.34m

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33
Q

(1.2) How many SF would be used in calculations with the measurement: 2.3467 x 10^6 in

A

5SF in 2.3467 x 10^6

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34
Q

(1.2) How many SF would be used in calculations with the measurement: 44,200g

A

3SF in 44,200

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35
Q

(1.2) How many SF would be used in calculations with the measurement:
0.003 L

A

1 SF in 0.003

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36
Q

12.3454 +84.23

A

13.07

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37
Q

(1.2) Convert
2.34 x 10^-3 meters to kilometers

A

2.34 x 10^-6 km

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38
Q

(1.2) Convert
0.00345km to μm

A

3.45 x 10^6 μm

( https://youtu.be/EwsCiRcNi3M)

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39
Q

(1.2) Titanium is a metal used to make golf clubs. A rectangular bar of this metal measuring 1.84cm x 2.24 cm x 2.24 cm was found to have a mass of 45.7g. What is the density of the titanium in the g/cm3?

A

4.95 g/cm^3

(https://youtu.be/msjYwHzxDzQ )

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40
Q

(1.2) What is the number 3606 expressed in scientific notation?

A) 36.06 x 10^2
B) 3.606 x 10^3

A

C) 3.606 x 10^3

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41
Q

(1.2) TRUE/FALSE
The exponents in scientific notation must be positive if the number is greater than 1

A

TRUE

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42
Q

(1.2)Complete the Base Units of the SI System :
length: Meter (m)
mass: _______
time: ________
temperature: __________
amount of substance: mole (mol)

A

mass: kilogram (kg)
time: second (s)
temperature: kelvin (K)

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43
Q

(1.2) Complete the conversion map:
1 Gallon : ____ quarts
1 Quart : _____pints

A

4 quarts…. 1/2 (.5) pints…

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44
Q

(1.2) Common unit prefixes:
Kilo (k)

A

K 10^3 or 1000

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45
Q

(1.2) Common unit prefixes:
Nano (n)

A

n 10^-9
/9 places behind the decimal
ie 4 nanograms = 0.000000004 g

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46
Q

(1.2) Common unit prefixes:
centi (c)

A

10^-2
ie. 7 cm is 0.07m

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47
Q

(1.2) Common unit prefixes:
micro (µ)

A

10^-6
ie microliter µL = 0.000001 L

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48
Q

(1.2) Common unit prefixes:
deci (d)

A

10^-1
ie
deciliter (dL) = 0.1 L

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49
Q

(1.2) Common unit prefixes:
mega (M)

A

10^6
ie
3 megahertz (MHz) = 3,000,000Hz

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50
Q

(1.2) Common unit prefixes:
mili (m)

A

10^-3
i.e 2 milimoles (mmol) o.oo2 mol

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51
Q

(1.2)100cm is 1 _______

A

1 meter

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52
Q

1000g is 1 ________.

A

kilogram

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53
Q

a millionth of the base unit is a _________ unit.
(in the SI system)

A

micro

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54
Q

(1.2) TRUE/FALSE “All certain digits along with the first uncertain digit in measurements are called significant figures or significant digits (or sig. figs.).”

A

TRUE

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55
Q

(1.2) TRUE/FALSE “Exact numbers have no uncertainty as measured numbers do. Hence, exact numbers have an unlimited number of significant figures”

A

TRUE

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56
Q

(1.2) TRUE/FALSE Only some non zero numbers are significant.

A

FALSE.
all numbers 1-9 are significant numbers (all non zeroes).

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57
Q

(1.2) Sigfig rules about zeros:
Leading zeros (zeros to the left of the first nonzero digit) are __________________. (For example, 0823 contains three significant figures.)

A

Not significant

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58
Q

(1.2) Trailing zeros that fall before a decimal point __________________. (For example, 6000. contains four significant figures, the 6 and the three zeros before the decimal point. Note that there is nothing after the decimal point.)

A

signifigant

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59
Q

(1.2)Captive/Interior Zeros are always ______________.

A

significant.

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60
Q

(1.2)Trailing zeros (zeros to the right of a nonzero digit) that fall after a decimal point are _________________. (For example, 745.00 contains five significant figures.)

A

significant.

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61
Q

In which of the following are all the zeros significant?

A) 0.002g ; 100g; 250.0g

B) 1.500 x 10^4 mL; 058 mL; 0.50 mL

C) 3.00 m; 405 m; 60.00m

A

C) 3.00m;405m;60.00m

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62
Q

How many sig figs?
2.000 x 10^3

A

4 SF

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63
Q

How many sig figs?
2.00 x 10^3

A

3 SF

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64
Q

(Q1.2) The correct scientific notation for the number 0.00050210 is:

A) 5.0210 x 10^4
B) 5.021 x 10^-4
C) 5.0210 x 10^-4

A

C) 5.0210 x 10^-4

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65
Q

(Q1.2) The correct scientific notation for the number 500.0 is?

A

5.000 x 10^2

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66
Q

(Q1.2) The correct decimal representation of 1.201 x 10^-7 is:

A) 12010000
B) 0.0000001201

A

B) 0.0000001201

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67
Q

(Q1.2) How many liters are in 333 mL?

A

0.333 L
divide by 1000 (mili means divide by 1000 or multiply by .001)

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68
Q

How many mililiters are in 17.5 L
(expressed in scientific notation)

A

1.75 x 10^4 mL
multiple by 1000
product is 17500
convert to scientific notation (3SF)
1.7500 (move decimal 4 places)

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69
Q

Convert 17.40 ft^2 to in^2. Your answer must by given with the correct number of significant figures

A

2505.6
SF is 4.
but remember the rules. all non zeros and captive zeros are sigfig

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70
Q

(1.2)
When _________ or ____________ numbers, round the result to the same number of digits as the number with the least number of significant figures (the least
certain value in terms of multiplication and division).

A

When MULTIPLYING or DIVIDING

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71
Q

(1.2) When doing ___________________ apply the two previous rules sequentially. For example, what is the
answer or the following: (4.89 + 5.58) ÷ 1.327?

A

MIXED OPERATIONS

the sum will have 2 sigfig past the decimal
4.89 + 5.58 = 10.47.
then divide
final answer will have 4 SF 7.890

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72
Q

(1.2) If you add or subtract two ______________, the answer is ____________. If you add or subtract two ____________ digits, the result is ____________. Therefore, if you add or subtract a certain and an uncertain digit the result is ________________.

A

TWO CERTAIN…. ANSWER IS CERTAIN.

UNCERTAIN,
…..THE RESULT IS UNCERTAIN

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73
Q

(2.1)The Formula for providing information about the accuracy of a measurement , is calculated using
_______________ = error / true value * 100

A

Percent Error

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74
Q

(2.1)The Formula for
____________ = experimental value - true value

A

Error

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75
Q

(2.1)Precision is determined by the _________ of the experimental value from the average value (rather than true value) it’s as follows:
Average _______________ from the Mean Formula:

(Sum of Deviations) / (number of deviations)

A

Deviations

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76
Q

(1.2)Deviation from the ____________ = (experimental value - mean)

A

Mean

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77
Q

(1.2)To indicate the precision relative to the mean in terms of percentage:

_________________ = (deviation) / (mean) * 100

A

Percent Deviation

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78
Q

(1.2)Two types of problem solving in Chemistry calculations are:

A

Specific equation type
Unit conversion type

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79
Q

(1.2)The formula:
(Mass)/(Volume) is

A

Density

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80
Q

(1.2)Dimensional analysis uses ______________ as a guide to solve problems. The _________ and ____________ must be subjected to the same mathematical operations as their associated numbers.

A

UNITS
UNITS AND QUANTITIES

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81
Q

(1.2)Dimensional analysis involves the use of one of more ________ conversion factors. A conversion factor is a _________ of two equivalent quantities expressed with different measurements.

A

UNITS.
RATIO

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82
Q

(1.2) ______________________ is a method that can be applied to computations ranging from simple unit conversions to more complex, multi-step calculations involving several different quantities.

A

DIMENSIONAL ANALYSIS

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83
Q

(1.2) Convert 168 in. to meters. [1in. = 2.54 cm]

A

4.27m

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84
Q

(1.2)1meter = ____ yard

A

1.0936yd

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85
Q

(1.2)1in. = _____ cm

A

2.54cm

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86
Q

(1.2)
1mile = ____meters

A

1609.3m

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87
Q

(1.2)
1lb = 453.59 ____

A

grams

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88
Q

(1.2)
1kg = 2.2046 ______

A

lbs (pounds)

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89
Q

(1.2)
km = 1000 ____

A

meters

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90
Q

(1.2)
1meter = 100 _____

A

centimeters (cm)

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91
Q

(1.2)
1yd = _____ ft

A

3 feet (ft)

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92
Q

(1.2)
1cm = 10 ______

A

milimeters (mm)

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93
Q

(1.2) What is the number 0.0001870 expressed in scientific notation?

A

1.870 x 10^-4

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94
Q

(1.2)Compute the following with the correct SF:
(2.057 x 0.0450 x 132)

A

12.2

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95
Q

Set A Measurements:
8.84g, 8.69g, 8.75g

Set B Measurements:
8.62g, 8.66g, 8.69g

Which set of measurements are more precise if the true value for the object is 8.76g

A

SET B is more precise because the values are closer together (less variation)

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96
Q

What is 3.67kg expressed in lb? [1 lb = 453.59g]

A) 8.09lb
B)1.66lb
C)8.09 x 19^-6 lb

A

A) 8.09lb

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97
Q

(Q1.2) How many meters are in 7528 cm?

A

75.28 m

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98
Q

(1.2)What is 55mi/hr expressed in km/hr? [i mi = 1.609km]

A

88 km/hr

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99
Q

(1.2)What is 35.0m^2 expressed in ft^2? [1in. = 2.54cm]

A

377ft^2

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100
Q

(1.2)What is the mass of 25 cm^3 of gold? The density of gold is 19.3 g/cm^3

A

4.8 x 10^2 g

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101
Q

(1.2) A metric ruler has markings of 0.1cm, which measurement is accurately reported by this ruler?

A

5.55cm

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102
Q

(Q1.3) Which of the following items is a pure substance?

A) air
B) brass
C) ice

A

C) ice
water is H2O molecule containing a controlled ratio of ONLY Hydrogen and Oxygen

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103
Q

(Q1.3) Which of the following statements is true about compound?

A) A compound is always made up different types of atoms bonded together in proportions that may vary.

B) A compound is always made up of different types of atoms bonded together in proportions that are fixed

A

B) A compound is always made up of different types of atoms bonded together in proportions that are fixed

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104
Q

(Q1.3) Which of the following is physical property?

A) The corrosive action of acid rain on granite

B) The tarnishing of a copper statue

C) The odor of spearmint gum

A

C) The odor of spearmint gum
b/c the smell does not change the chemical properties or change the substance

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105
Q

(Q1.3) Which of the following items is a chemical property?

A) The melting and boiling point of water

B) The tarnishing of a copper statue

C) The odor of spearmint gum

A

C) The tarnishing of a copper stature
Tarnishing is caused by a chemical reaction between the metal and oxygen and changes the atomic level

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106
Q

(Q1.3) If you hold a solid piece of pure gallium metal in your hand, your body heat will melt the gallium into its liquid form. This illustrates which of the following:

A) Distillation

B) Physical change

C) Chemical Change or a Chemical Property

A

B) Physical change
melting does not induce any chemical or atomic changes in the elements (no bonding and no breaking)

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107
Q

(Q1.3) How many joules are there in a 255 Calories snack bar?
1 cal = 4.184 J
1 Cal = 1000 cals

A

1.07 x 10^6 J

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108
Q

Convert 68853 milijoules (mJ) to Calories [1 cal = 4.184 J
and 1000 mJ in 1 J J

A) 0.01646 Cal
B) 60.77 Cal
C) 164.6 Cal
D) 16.46

A

D) 16.46

To convert millijoules to Calories, divide by 1000 to convert millijoules to joules and then divide by 4.184 to convert joules to Calories. 68852 millijoules is approximately equal to 16.47 Calories.

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109
Q

If the monthly electricity consumption of a household in 6619 kWh, what is this consumption expressed in KJ? [1kWh = 3.60 x 10^6J]

A) 2.38 x 10^7 kJ]
B) 2.38 x 10^10 kJ

A

A) 2.38 x 10^7 kJ

110
Q

What is the value of 98 degrees F in units of C degrees

A) 35 degrees Cels
B) 37 degrees Cels
C) 46 degrees Cels

A

B) 37 degrees Cels

111
Q

(Q1.3)What is 18 degrees Farenheit in terms of K (kelvin)?

A) 251 K
B) 265 K
C) 301 K

A

B) 265K

112
Q

(Q1.3)In an exothermic reaction:
A) The surroundings absorb heat from the reaction mixture
B) The surroundings release heat to the reaction mixture
B) Both the reaction mixture and surroundings release heat.

A

A) The surroundings absorb heat from the reaction mixture
(Exo- exterior. Heat is absorbed by the surrounds or exterior surroundings)

113
Q

(1,3)In an endothermic:
A) The energy of the reactants is higher than the energy of the products

B) The energy of the reactants is lower than the energy of the products

A

B) The energy of the reactants is lower than the energy of the products

114
Q

(HW1.3) The rusting of iron is due to its reaction with oxygen. An iron nail weighing 8.531 g was left outdoors for a period of one year. After the year, it was found to have a mass of 12.197 g. How much oxygen did the nail combine with?’

A) 3.666g
B) 0.699g

A

A) 3.666g

115
Q

(HW1.3) Which statement is NOT part of the atomic theory?

A) All atoms of an element have the same mass and other properties

B) All elements are made up of indestructible particles called atoms

D) Atoms are made up of protons, neutrons, and electrons

A

%%D maybe double check

116
Q

(HW1.3) According to Dalton’s atomic theory:

A) An atom cannot be subdivided into smaller particles

B) An atom can be subdivided into smaller particles

C) The nucleus is made up of protons and neutrons

D) Electrons are lighter than protons

A

A) An atom cannot be subdivided into smaller particles

117
Q

(HW1.3) For most atoms, the nucleus consists of:

A

protons and neutrons

118
Q

The number of _____________ in an atom represented by the symbol Z, is used to identify the atom as a particular element, it and is the same for all atoms of a particular element.

A

protons
the number of protons…

119
Q

If a calcium atom loses two electrons, how many electrons does it have?

A) 18
B) 20
C) 22
D) not enough information

A

A) 18

120
Q

Atoms have no charge because their numbers of protons and electrons are ___________.

A

equal

121
Q

In general ________________ have the greatest effect on the size of an atom.

A

Electrons have….

122
Q

(3.1)What is matter?

A

matter is defined as anything that has mass and occupies space.

123
Q

(3.1) matter is classified based on
_______, size, ________, and methods of separation.

A

state….composition

124
Q

Matter is classified into different states based on the following:
The _______ between the particles.
The ______ movement of the particles.
The ________ of the sample
The __________
The _________ of the sample.

A

spacing….
movements…
shape….
volume…
compressibility

125
Q

Summarize the properties that distinguist the states of matter:
Solids….
Liquids….
Gases….

A

Solid substances have a rigid shape and volume.

Liquids flow and posesses a definite volume but not a definite shape. Liquids take the shape of its container (except that it forms a flat or slightly curve upper surface when acted upon by gravity)

Gases are COMPRESSIBLE and take the shape and volume of their container. Gases are volumes are depended on pressure conditions.

126
Q

The spacing of particles in each state of matter:

Solid…
Liquid….
Gas…

A

Solids particles are spaced VERY CLOSE TOGETHER

Liquids are spaced CLOSE TOGETHER

Gases are spaced FAR APART

127
Q

Movement of the particles of each state of Matter:

Solids…
Liquid…
Gas…

A

Particles in
Solids VIBRATE

Liquids MOVE RELATIVE TO EACH OTHER

Gases MOVE INDEPENDENTLY OF EACH OTHER

128
Q

The THEORY that states matter is comprised of tiny particles that are in random motion.

A

Kinetic molecular theory

129
Q

Gas Laws describe the behavior of gases by showing the relationships between a gases’s volume, temperature, and _____________.

A

pressure.

130
Q

The gas law that states the volume of a gas is inversely proportional to applied pressure ((if temperature and moles of gas (n) are constant))

A

Boyle’s Law

131
Q

The gas law that states the volume of a gas is directly proportional to the kelvin temperature ((if pressure and number of moles are constant))

A

Charles’s Law

132
Q

What’s an Ideal Gas?

A

An ideal gas is not a real gas. It’s a hypothetical gas that obeys the gas laws at all temperatures and pressures perfectly. The construct of an Ideal gas help to calculate what real gases may do at HIGH TEMPERATURES and LOW PRESSURES

133
Q

PV = nRT

A

The ideal Gas Law equation
P= gas pressure
V= gas volume
n = moles of gas
R = gas constant
T = kelvin in temp

134
Q

Name an example of the Boyle’s law in application

A

When a diver experiences the “bends” or “decompression sickness” if they rise to quickly from a lower depth because it will make their lungs (which holds O2 and Co2 ) expands out into the blood stream to quickly

135
Q

Name an example of Charles’s law in application

A

When the gas in a hot air balloon is heated, the expansion of the hot gas leads to a LOWERING of the density of the balloon. the balloon becomes less dense than the surrounding air, allowing the hot air balloon to rise.

136
Q

A sample of gas will increase in VOLUME if it is heated at a constant pressure…. _______ law

A

Charles’s law

137
Q

At high altitudes, the air pressure is lower than at sea level….. _______ law

A

Boyle’s law

138
Q

(1.3) Name examples of matter classified PARTICULATE (diameters less than 1nm):

A

Virus
Protein molecule
Aspirin molecule
water molecule
atom
(descending order)

139
Q

(1.3) Name examples of matter classified as MICROSCOPIC (diameters ranging from 1mm to 10nm):

A

plant cell
animal cell
bacterial cell

140
Q

(1.3) name examples of matter classified as MACROSCOPIC

A

Height of a human
sheet of paper
wedding ring
thickness of a CD
grain of sand

141
Q

Matter with constant properties and composition such as Ice cubes is a __________substance

A

Pure substance

142
Q

Matter without constant properties/composition/fixed ration are a __________.

A

mixture

143
Q

TRUE/FALSE all pure substances are heterogeneous mixture.

A

FALSE
pure substances are homogeneous and uniform throughout (having fixed properties and ratio).

144
Q

Examples of a heterogenous mixture are:

A

tossed salad,
pizza,
oil in watter,
coffee

145
Q

A Pure substance that can be simplified chemically is a _______

A

COMPOUND
because its made of multiple parts but fixed ratios. Therefore a compound can be broken down into base elements

146
Q

A Pure substance that CANNOT be simplified chemically is an _______________

A

ELEMENT
one type of atom makes up the substance. cannot be chemically brokendown/ simplified

147
Q

Examples of compounds

A

Salt, Sugar, Water, Oxygen, Carbon

148
Q

examples of elements

A

Hydrogen, copper, helium, argon,

149
Q

Elements on the periodic table are organized in 7 rows called ___________ and 18 columns called ____________.

A

7 periods across…. 18 groups vertical…

150
Q

(3.1)Whats the element in group 1 period 1?

A

Hydrogen

151
Q

Mixtures can be seperated by physical means such as,
Filtration, _________,
magnetism, and chromatography

A

Distillation

152
Q

Color is a _________ property.

A

Physical property

153
Q

Density is a _______ (chemical/physical) property and ______
(intensive/extensive) property

A

Physical property : there is no chemical change

intensive because : When a property, like density, is independent of the amount of sample measured, it is known as an “intensive” property.

154
Q

Odor is a _________ property.

A

Physical property

155
Q

Boiling point of a substance is a _________.

A

Physical property

156
Q

burning of a log is an example of a ___________________.

A

chemical change

157
Q

Which one is NOT chemical change
A) rusting of iron
B) decomposition of milk
C) melting iron

A

C) melting iron is a physical change because the atomic/chemical bonds are not changed

158
Q

Which one is NOT physical property?
A) color
B) odor
C) rusting of iron

A

C) the rusting of iron is an oxidation process. thus it’s a chemical change

159
Q

TRUE/FALSE
The following:
filtering a mixture,
boiling water,
melting iron,
seperating the components of dyes in a mixture,
is a list of chemical changes.

A

FALSE the list is all physical changes

160
Q

TRUE/FALSE
If the property depends on the amount of matter present, it is an extensive property.

A

TRUE

161
Q

TRUE/FALSE
Temperature is an intensive property, because the property (temperature) of a sample of matter does not depend on the amount of matter present.

A

TRUE

162
Q

TRUE/FALSE the mass and volume of a substance are examples of extensive properties

A

TRUE because the value of an extensive property is directly proportional to the amount of matter in question. EX a gallon of milk has a larger mass that a cup of milk.

163
Q

Temperature is intensive property, heat is an ______ extensive property.

A

extensive property.
(when you combine oil at 100 degrees the temperature remains the same). But more oil means more heat (extensive).

164
Q

Changing a substances size or shape is an example of a ______ change.

A

physical change

165
Q

The ________ change affects a composition of the substance. It’s when the substance reacts to another and gives rise to another or more new substances i.e iron rusting

A

chemical

166
Q

(1.3) A candy bar contains 225 Cal of nutritional energy. How many joules does it contain? [1 cal = 4.184 J]

A

9.41 x 10^5 J

solution map:
Cal > cal > J

167
Q

____ cal = 4.184 J
____ cal = 1 Cal
____ cal = 1kcal
____ kWh = 3.60 x 10^6 J

A

1 cal
1000 cal
1000 cal
1 kWh

168
Q

Convert 485 cal to kilojoules. [1 cal = 4.184 J

A

2.03 kJ

169
Q

Energy is neither __________ nor ____________ but it can be changed from one form to another.

A

created….. destroyed

170
Q

(1.3) Kinetic energy is the energy associated with ___________.

A

motion

171
Q

(1.3) Potential energy is the energy associated with ________ and _______ of matter. Objects with high potential energy ten to be unstable. So they have a tendency to change in a way that lowers their potential energy

A

position…. composition

172
Q

______ molecules tend to undergo rapid chemical changes that lower their potential energy, which is why it’s so explosive. (name of molecule that’s explosive)

A

TNT (trinitrotoluene)

173
Q

Energy and Change of States generally involve the ______ or ______ of energy.

A

gain…. loss

174
Q

(1.3) involves the loss of heat in a system. When heat is released the potential energy of the system is lowered and the process is _______________.

A

Exothermic

175
Q

(1.3) When heat is absorbed, the potential energy of the system is increased and the process is said to be _______________.

A

Endothermic

176
Q

Products of an endothermic reaction gain ______ energy.

A

potential
(starting materials have lower potential energy than the products)

177
Q

products of an exothermic reaction ______ potential energy.

A

loss energy.

178
Q

(1.3) Condensation, ________, and deposition involve a loss of heat. When heat is released, the potential energy of the system is _______.

A

Freezing….. Lowered.
(Exothermic)

179
Q

(1.3) Melting (fusion), __________, and sublimation involve a gain of heat in the system. When the system absorbs heat, the potential energy is ___________.

A

Vaporization, increased.
(Endothermic)

180
Q

Complete the blanks:
EXO
Condensation : ____ to liquid
Freezing : _____ to solid
Deposition: ____ to solid

ENDO
Melting : ____ to liquid
Vaporization : _____ to gas
Sublimation : _____ to gas

A

gas to liquid
liquid to solid
gas solid

solid to liquid
liquid to gas
solid to gas

181
Q

Potential energy that is lost during an exothermic process is generally converted to ______.

A

heat

182
Q

Because energy is __________ in a change, an increase in potential energy means that there is a decrease in the kinetic and vice versa.

A

conserved

183
Q

Lower _____ energy content means that temperature is lowered and a higher ______ energy content means that temperature is increased.

A

kinetic, kinetic.

184
Q

(1.3) the degree of hotness or coldness of a body is __________.

A

temperature

185
Q

original and converted temperatures must have the same _________.

A

precision

186
Q

(3.1) approximately twice the degree Celsius

A

degree Fahrenheit

187
Q

Convert 15.5 Fahrenheit into Celsius and Kelvins

F to C: (F-32)* 5 /9
F to K: F-32 * 5 / 9 + 273.15

A

-9.2 Celsius
264.0 Kelvin

188
Q

F = (Celsius x 1.8 ) + 32

A

Converting Fahrenheit to Celsius

189
Q

C = (F - 32 )/1.8

A

Converting Celsius to Fahrenheit

190
Q

K = C + 273.15

A

Converting Celsius to Kelvin

191
Q

C = K - 273.15

A

Converting Celsius to Kelvin

192
Q

According to what Theory is: “Matter is made of extremely small particles called atoms”

A

Dalton’s Atomic Theory

193
Q

According to Dalton’s Atomic Theory: “All atoms of a given element are identical in mass and properties. Atoms of one element ______ in properties from atoms of all other elements.”

A

differ.

194
Q

According to Dalton’s Atomic Theory “____________ are formed by a combination of two or more different kinds of atoms.”

A

Compounds

195
Q

According to Dalton’s Atomic Theory: “Atoms cannot be __________, created, nor ________.”

A

subdivided,
destroyed

196
Q

According to Dalton’s Atomic Theory: Atoms of one element cannot be ________ into atoms of another element. A _________ reaction is a rearrangement of atoms.

A

converted….
chemical

197
Q

Why was the Atomic theory proposed by Dalton so important?

A

It explained two important laws that were established in the 18th century by previous chemists. These two lass was the mass conservation in chemical changes and of definite proportions or constant composition

198
Q

__________ states that in a chemical change mass is conserved. This means that the total number and kinds of atoms present at the start of a chemical process will be the same at the end.

A

Law of Conservation of Mass

199
Q

_______________ states that all samples of a pure compound contain the same elements in the same proportion by mass. The idea that the numbers of atoms of the elements in a given compound always exist in the same ratio is consistent with these observations.

A

The law of definite proportions (or the law of constant composition)

200
Q

___________________ is applied whenever the chemical formula of a compound is written. For instance, we write the chemical formula for water as H2O regardless of who makes it, where it is made, or the reaction by which it is made. If the substance is water, any sample of it will have a mass ratio of 8 g oxygen to 1 g hydrogen. The laws of conservation of mass and of definite proportions are foundational to the advances in chemistry.

A

The law of constant composition

201
Q

_______________ states that when two elements react to form more than one compound, a fixed mass of one of the elements will react with masses of the other element in a ratio of small, whole numbers.

A

The Law of Multiple Proportions

202
Q

When 0.96g of oxygen and 0.12g of hydrogen combine, 1.08g of water is expected to form is a condition that illustrates the law of _______________.

A

The law of conservation of mass

203
Q

An amount of 0.96g of oxygen is expected to react with 0.12g of hydrogen to form water illustrates the law of ______________________.

A

The law of constant composition

204
Q

A substance that is represented by at least two different types of spheres arranged in an orderly fashion illustrates an example of a _____________

A

compound

205
Q

Each Element is comprised of tiny, indivisible particles illustrates _________ theory.

A

atomic theory

206
Q

The ______ and the neutron have very similar masses and each is nearly two thousand times as heavy as an electron

A

proton

207
Q

The _________ therefore, contains the majority of an atom’s mass, whereas electrons occupy almost all of an atom’s volume

A

nucleus

208
Q

the more __________ an atom has, the greater the volume of space that the electrons will occupy. This means that atoms with more electrons will generally be larger in size than atoms with fewer electrons.

A

Electrons

209
Q

The number of ___________ in the nucleus of an atom is called its atomic number and is denoted as Z. This is the defining trait of an element: Its value determines the identity of the atom

A

protons

210
Q

The _________ of an atom is influenced by the number of electrons i that it has

A

size

211
Q

Consider a sample of H2O, in which form is the average kinetic energy the highest?

A) Steam
B) water
C) Ice

A

A) Steam

212
Q

Identify the property that is both physical and intensive.

A) color
B) odor
C) density
D) all physical and intensive properties

A

D) All are physical and intensive properties

213
Q

Which is the correct temperature in Celsius of 46.8 degrees Fahrenheit
A) 8 degrees Celsius
B) 8.2 degrees Celsius

A

B) 8.2

214
Q

Which of the following statements are NOT true?

A) the law of multiple proportions
B) The atomic theory explains the law of conservation of mass.
C) the atomic theory explains the law of definite proportions

A

A) the law of multiple proportions was known before Dalton proposed the atomic theory

215
Q

O2 (gas)

A

Molecule and Element 2 bonded oxygen atoms

216
Q

Fe (s)

A

Atom, Element (single atom)

217
Q

NaCl(s)

A

Compound, Ionic Compound
ionic compounds are usually metals

218
Q

Melting iron is a ________change.
Browning Marshmellows is a ___________ change.

A

physical , chemical

219
Q

If exactly 441g of propane and 1,600grams of oxygen combust to form 721g of water. How many grams of carbon dioxide are formed?

A

1320g carbon dioxide

220
Q

Convert 285 calories to Joules

A

68.1 Joules

221
Q

Convert 32 degrees F to degrees C

A

0 degrees C

222
Q

10) Convert 30.0 degrees C to degrees K

A

303 degrees Kelvin

223
Q

Convert 2.34 x 10^-3m to km

A

2.34 x 10^-6 km

224
Q

Convert 0.00345 km to μm

A

3.45 x 10^6 μm

225
Q

Calculate the density of magnesium in g/cm^3, in a sample of magnesium has a mass of 14.3g and it has a volume of 8.46 cm^3

A

1.69g/cm^3

226
Q

The density of mercury is 13.6 g/mL. how many pounds lnns does one quart of mercury weigh?

A

28.4lbs

227
Q

what is 1.74935 rounded to 2 SF?

A

1.7

228
Q

What is 0.089510 rounded to 2 SF?

A

0.090

229
Q

What is 100459.7 rounded to 3 SF?

A

1.00 x 10^5

230
Q

What is the sum of 6.289 + 0.52 + 1.3?

A

8.109 rounded to 8.1 as final answer because you one want one uncertain digit in you answer max.

231
Q

Five students (A to E) used the same balance to measure a metal block separately. The true mass of the block is 50.0000 g but the students obtained the following masses:

A: 49.9990

B: 49.9451

C: 50.0025

D: 50.9000

E: 49.9889

CALCULATE THE MEAN OR AVERAGE

A

50.1671g

HOW: (sum of masses) / (number of masses)

232
Q

Five students (A to E) used the same balance to measure a metal block separately. The true mass of the block is 50.0000 g but the students obtained the following masses:

A: 49.9990

B: 49.9451

C: 50.0025

D: 50.9000

E: 49.9889

CALCULATE THE DEVIATION OF ALL STUDENTS AND THE AVG DEVIATION

A

A. 0.1681g

B. 0.2220

C. 0.1681

D. 0.7329

E. 0.1782

AVG: 0.2932

HOW: (measured value - mean)
ex student A:
49.9990g-50.1671g=0.1681g

for average add the list of values and divide by 5 (number of values)

233
Q

Five students (A to E) used the same balance to measure a metal block separately. The true mass of the block is 50.0000 g but the students obtained the following masses:

A: 49.9990

B: 49.9451

C: 50.0025

D: 50.9000

E: 49.9889

CALCULATE THE ERROR OF ALL THE STUDENTS

A

A. 0.0010

B. 0.0549

C. 0.0025

D. 0.9000

E. 0.0111

HOW: (measured value - true value)
ex student A:
49.9990g-50.0000g=0.0010g

234
Q

Five students (A to E) used the same balance to measure a metal block separately. The true mass of the block is 50.0000 g but the students obtained the following masses:

A: 49.9990

B: 49.9451

C: 50.0025

D: 50.9000

E: 49.9889

CALCULATE THE PERCENTAGE ERRORS OF ALL STUDENTS
AND THE PERCENT ERROR OF THE GROUP

A

A: 0.002%

B: 0.110%

C: 0.0050%

D: 1.800%

E: 0.0222%

AVG: 0.3878%

HOW: (error) / (true value) *100
ex student A:
(0.0010g) / (50.0000g)=0.00002g * 100 =0.002%

235
Q

Five students (A to E) used the same balance to measure a metal block separately. The true mass of the block is 50.0000 g but the students obtained the following masses:

A: 49.9990

B: 49.9451

C: 50.0025

D: 50.9000

E: 49.9889

CALCULATE THE PERCENTAGE ERROR ALL THE STUDENTS

A

0.002%

HOW: (error) / (true value) *100
ex student A:
(0.0010g) / (50.0000g)=0.00002g * 100 =0.002%

236
Q

DIMENSIONAL ANALYSIS:
calculate what is the density of a liquid whose mass is 27.2g and the volume is 22.5 mL?

A

1.21g/mL

density = (mass)/(volume)

237
Q

DIMENSIONAL ANALYSIS:

(1inch)/(1inch) = (2.54cm)/(2.54cm) = ______

A

1

because the ratio is an equality relationship illustrating that a unit of 1in. EQUALS 2.54cm

238
Q

What is 1ft^3? a measure of?

A

cubic is a measure of volume.

239
Q

Liters is a measure of units for _________.

A

Volume

240
Q

1L = 1000 ______

A

mL

241
Q

1mL = _____ cm^3

A

1

242
Q

A solution map shows how the ______ will be changed in the conversion process, that calculates a dimensional analysis equation.

A

units

243
Q

What is 194cm converted to ft? [1in = 2.54cm]

A

6.36 ft

Sol map: cm to in. to ft

244
Q

What is 4.86lb in kg? [1lb - 453.59 g]

A

2.20kg
sol map: lb to gram to kg

245
Q

What is 4.89 gal converted to L? [1 L = 1.057 qt]

A

18.5 L

sol map: gal to qt to L

246
Q

What is 3.00 x 10^8 meters/second in miles/hour? [1 mile = 1.609km]

A

6.71 x 108 miles/hr

sol map:
numerator:
m to km to mi
denominator:
s to min to hr

247
Q

What is 125m^3 converted to in^3 [1in = 2.54 cm]

A

7.63 x 10^6 in^3

sol map meters cubed to centimeters cubed to inches cubed

**cube the conversion units so it matches the 125^3 in the original problem.

248
Q

If a liquid substance has a density of 1.32 g/cm^3, what volume (in mL) shoud be measured to obtain a mass of 68.4g?

A

51.8 mL

solmap: g to cm3 to mL

249
Q

Classify each statement as an observation, a law, or a theory:

a) When the pressure on a sample of oxygen has is increased 10%, the volume of the gas decreases by 10%
b) The volume of a gas is inversely proportional to its pressure
c) A gas is composed of small particles in constant motion
d) A gas sample has a mass of 15.8g and a volume of 10.5L

A

observations: a,d
law: b
theory: c

250
Q

convert 27m/s to km/hr

A

97km/hr

251
Q

A graduated cylinder has markings every mililiter. Which measurement is accurately reported for this graduated cylinder?

a) 21mL
b)21.2mL
c)21.23mL

A

b) 21.2mL

252
Q

How many SF are in the number 0.00620?

A

3

253
Q

Perform this multiplication to the correct number of significant figures:
65.20.001512.02

A

1.2

254
Q

The SI units of ________ are units of length raised to the third power; liters or milliliters are often used as well. The density of a substance is its mass divided by its ________.

A

volume

255
Q

Always count the following digits as significant:

_______ digits
interior zeros
__________ zeros after a decimal point
trailing zeros before a ________ point but after a nonzero number.

A

nonzero
trailing zeros
decimal point

256
Q

How many significant figures are in the following numbers?

a) 1.0050
b) 0.00870
c) 100.085
d) 5400

A

a) 5
b)3
c)6
d) impossible to tell in it’s current form

257
Q
A

the result of a multiplication of division should carry the same number of significant figures as the factor with the least number of significant figures

258
Q
A

In calculations involving both addition/subtraction and multiplication/division, do the steps in parentheses first, keeping track of how many significant figure, then proceeding with the remaining steps. DO NOT ROUND UNTIL THE VERY END!!!

259
Q

convert 108 ft to meters
(there are 39.37in in 1 meter)

A
260
Q
A

answer = 26.46 mg/kg

261
Q
A
262
Q
A
263
Q
A
264
Q
A
265
Q
A

54.9 mL

266
Q
A
267
Q

A compound is composed of different atoms that are chemically united (bonded). While a _____________ is composed of different substances that are not chemically united, but simply mixed together.

A

mixture

268
Q

a ________ substance can also be a compound, a substance composed of two or more elements in a fixed definite proportions.

A

pure substance

269
Q

we can classify mixtures according to how uniformly the substances within them are mixed. In a __________________ mixture, such as oil and water the composition varies from one region to another. in a _______________ mixture, the composition is uniform because the atoms or molecules are mixed uniformly.

A

heterogeneous
homogeneous

270
Q

You can classify a pure substance into 2 categories:
__________ and ___________

A

element and compounds

271
Q
A

CHEMISTRY 107: FUNDAMENTALS (5 decks)

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