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JLH Chem 1 > chem 1st pp > Flashcards

chem 1st pp Flashcards

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1
Q

Chemistry

A

the study of matter including it’s
composition, transformations and properties

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2
Q

Some everyday examples of chemistry

A

 Adding salt to water when boiling pasta (change the
boiling point)
 Bath Fizzies or Alka Seltzer tabs (chemical reaction)
 Rust of equipment made of iron (chemical reaction)
 Gas stove (chemical reaction)
 Cooking and baking (chemical reactions)
 Shampoo (solubility)

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3
Q

Matter

A

anything that has mass and takes up
space.
 Naturally occurring
 Synthetic – produced in lab.

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4
Q

States/phases of substances

A

Solids

Liquids

Gases

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5
Q

Can substances move between states without change to chemical composition?

A

yes

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6
Q

What does the state of substances depend on?

A

energy of atoms or molecules

More energy = more motion = less order

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7
Q

Solid

A

Very ordered;
molecules/atoms
close together.

Lowest energy

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8
Q

Liquid

A

More distance
between particles than solids.
More energy.

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9
Q

Gas

A

Largest distance
between particles
and the most energy.

Assumes shape and
volume of container.

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10
Q

We characterize matter by what properties?

A
  • Physical properties
  • Chemical properties
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11
Q

Physical properties

A

can be measured without
changing the composition of the matter.
 Boiling point.
 Color
 Feel
 Flame tests (not combustion)

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12
Q

Chemical property

A

the composition of the
matter can be changed during a reaction.
 Combustion analysis

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13
Q

Physical change

A

occurs without changing the
composition of the matter. Just a change in state.
 Melting of iron ore
 Boiling of water

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14
Q

Chemical change

A

changes the composition.
This is a chemical reaction. The matter you
started with is replaced with a different
substance.
 Rusting of iron (4Fe + 3O2 → 2Fe2O3)
 Burning of wood (wood + O2 → CO2 + H2O)
 Electrolysis of water. (H2O → H2 + O2)

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15
Q

How do you recognize that a chemical change has
occurred?

A

 Change in color, odor or temperature (without
external heating or cooling)

 Formation of a gas (bubbles)

 Formation of a solid (precipitate)

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16
Q

Matter can be classified as what?

A

Substance
or
Mixture

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17
Q

Pure Substance

A

 Has constant composition and distinct properties
 One component
Can be elements or compounds
 Can’t be broken down into another pure substance by physical change.

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18
Q

Mixture

A

 Contains more than one component

 Can be separated into it’s individual components by physical separation

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19
Q

Most elements are _________ occurring.

A

natural

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20
Q

Elements can be polyatomic. Give some examples

A

N2

O2

O3

S8

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21
Q

compounds

A

 Chemical combination of elements in fixed ratios.

  • water (H2O), table salt (NaCl), sugar

 Consistent, distinct properties

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22
Q

Compounds require what in order to be broken down into elements?

A

requires a chemical process

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23
Q

Which one of these is a compound?

H2

O2

H2O

A

H2O

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24
Q

Mixtures can be broken down into their individual components by physical means.

What is a homogeneous mixture?

A

Composition is constant throughout

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25
Q

Mixtures can be broken down into their individual components by physical means.

What is a heterogeneous mixture?

A

Composition not uniform

Individual parts are distinct and discernible.

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26
Q

All measurements contain what two things?

A

number and unit

3g

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27
Q

some examples of the English measurement system

A
  • lbs., ounces
  • Inches, feet, miles
  • Fluid ounces
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28
Q

examples of the metric system

A

Length→ meter (m)

Mass→ gram (g)

Volume →Liter (L)

Time→ second (s)

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29
Q
A
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30
Q

Kilo-

A

1000 X the base unit

1 kg = 1000g

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31
Q

Centi-

A

0.01 x the base unit

1 cm = 0.01 m

1 m = 100 cm

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32
Q

Milli-

A

0.001 x the base unit

1 ml = 0.001L

1000 ml = 1 L

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33
Q

Micro-

A

0.000001 x the base unit (1 X 10-6)

1 μl = 0.000001L

1000000 μl = 1L

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34
Q

SI system

A

International System of Units)

Based on Metric system

Recommends some base units over others.

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35
Q

Some SI units

A

Amount of substance = mole (mol)

Length = meter (m)

Mass = kilogram (kg)

Time = second (s)

Thermodynamic termperature = kelvin (K)

Electric current = ampere (A)

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36
Q

Mass vs. weight

A

Mass: amount of matter

Weight: force that matter feels due to gravity

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37
Q

how do we measure volume?

A

length X width X height

(square or rectangle)

1L is equal to a cube that is 10 cm on each side.

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38
Q

What do we typically use in science & medicine instead of liters?

A

mL (.001 L)

dL (.1 L)

(smaller amounts)

<i>(remember, cm = .01)</i>

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39
Q

One unit commonly used in medicine is the “cc” , which stands for what?

A

cubic centimeter

1 cc = 1 cm3 = 1 mL

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40
Q

What is a good way to measure volume with irregularly shaped objects?

A

water displacement method

41
Q

How to use water displacement method

A
  1. Measure amount of water in graduated cylinder.
  2. Drop in object and measure the volume again.
  3. Final volume minus initial volume equals the volume of the object.
42
Q

Data in chemistry is either exact or inexact.

how are exact numbers obtained?

Inexact numbers?

A

Exact numbers – obtained from counting.

Inexact numbers – measured by anything else.

43
Q

Accuracy vs. Precision

A

Accuracy – how close to real number

Precision – how close multiple measurements are to each other (not necessarily correct).

44
Q

what do we know about significant numbers with all non-zero digits?

A

All non-zero digits are significant

111.1 (4 sig. figures)

3,456.892 (7 sig. figures)

45
Q

Are zeros between non-zero digits significant or not?

  1. 003 (how many sig digits?)
  2. 8 (how many sig digits?)
A

Zeros between non-zero digits are significant

  1. 003 (4 sig. figures)
  2. 8 (4 sig. figures)
46
Q

How many digits are significant in 0.006?

0.045?

A
  1. 006 (1 sig. fig)
  2. 045 (2 sig. fig)

Zeros to the left of the first non-zero digit ARE NOT significant. They are place holders.

47
Q

How many significant digits are there in 165.0?

20.0?

A
  1. 0 (4 sig. fig)
  2. 0 (3 sig. fig)

Zero to the right of the last non-zero are significant only IF there is a decimal point.

48
Q

put 14,000,000 in scientific notation

A

1.4 x 107

49
Q

How many significant digits are in 1.400?

A

4 significant digits

Zeros to right of non-zero without decimal are not significant (1400 would only have 2 sig digits)

50
Q

Some rules for significant digits

A
  1. Non-zero digits are always significant
  2. Any zeros between two significant digits are significant
  3. A final zero or trailing zeros in the decimal portion ONLY are significant

Example: .500 or .632000 the zeros are significant

.006 or .000968 the zeros are NOT significant

51
Q

Some rules for addition & subtraction with significant digits

A
  1. Count the number of significant figures in the decimal portion ONLY of each number in the problem
  2. Add or subtract in the normal fashion
  3. Your final answer may have no more significant figures to the right of the decimal than the LEAST number of significant figures in any number in the problem.
52
Q

Some rules for significant digits with multiplication

A
  1. The LEAST number of significant figures in any number of the problem determines the number of significant figures in the answer. (You are now looking at the entire number, not just the decimal portion)

*This means you have to be able to recognize significant figures in order to use this rule*

Example: 5.26 has 3 significant figures

6.1 has 2 significant figures

53
Q

1.535 + 0.36 =

A

1.90

54
Q

10.6/0.32 =

A

33

The number of significant figures in the final product (or quotient) is determined by the original number that has the smallest number of significant figures.

55
Q

Exact numbers

A

Exact numbers are either defined numbers or the result of a count. For example, a dozen is defined as 12 objects, and a pound is defined as 16 ounces. An exact number can only be expressed in one way and cannot be simplified any further.

Conversions between English and Metric system are generally NOT exact. Exceptions will be pointed out to you. e.g. 1 in = 2.54 cm exactly (1 and 2.54 are both exact.)

56
Q

how do you do multi-step calculations?

A

keep at least one more significant figure in intermediate results than needed in your final answer. For example, if a final answer requires two significant figures, then carry at least three significant figures in all calculations.

57
Q

what are the steps in writing scientific notation?

A
  1. Move the decimal point so that you get a number with one digit before the decimal (y) 602,200,000,000,000,000,000,000 → 6.02,200,000,000,000,000,000,000
  2. Count the number of places you moved. This will be the exponent (x). 6.022 x 1023
  3. If you moved the decimal to the left the exponent is positive, if you moved it to the right the exponent is negative.
58
Q

given (y x 10x ), if you make y larger, then x must get

A

smaller

The opposite is also true: if you make y smaller, then x must get larger.

59
Q

some examples of scientific notation written in expanded form

A
60
Q

Factor-label method

(Dimensional Analysis or Unit Analysis)

A
61
Q

What is the order to setting up a story problem?

A
  1. What is the question asking you to find.
  2. What unit(s) will be used to express the answer.
  3. What conversion factors will be needed (including units).
62
Q

factor-label method pic from pp

44/67

A
63
Q

Using the factor-label method, convert 4.5 meters to feet.

2.54 cm = 1 inch, 12 inches = 1 ft.

A

15 ft

64
Q

Is temperature a measurement of heat?

A

No. Temperature is a measure of how hot or cold an object is. It is related to the average heat content.

65
Q

To measure temperature we used to use mercury thermometers. What is used now?

A

alcohol or digital thermometers.

66
Q

What are different temperature scales?

A

Fahrenheit (oF)

Celsius (oC)

Kelvin (K)

67
Q

How do you convert oC to K?

A

K = oC + 273

68
Q

How do you convert oF to oC?

A

oC = (oF-32)/1.8

Do work in parentheses first

69
Q

How do you convert oC to oF?

A

oF = (oC)1.8 + 32

Do multiplication first

70
Q

At the boiling point of water, there is a difference of 112 between C and F. At its freezing point, the difference is 32. The scales are getting closer together as the temperature drops. They cross at -40. So -40 C is the same temperature as -40 F.

A

This formula works for both conversions. Tnew = (Told + 40) × f - 40

This is based on the fact that -40o represents the same temperature in both systems (oF and oC).

“f” is a conversion factor. If converting from F and C, the factor is 5/9; if converting from C and F, the factor is 9/5. The denominator is used to cancel the old unit; the numerator creates the new unit.

71
Q

Density

A

Density- a physical property that relates mass
and volume of a substance

D = m/V

72
Q

What units do we use to find the density for liquids and solids

A

g/ml or g/cm3

Grams per milliliter or grams per centimeter cubed

73
Q

What do we use to find density for gases?

A

g/L

grams per liter

74
Q

What is density dependent on?

A

Temperature

Because D = m/v and temperature affects volume

75
Q

What is a general rule for solids, liquids, and gases in relation to density?

What is the exception?

A

As a general rule solids are more dense that
liquids. Liquids are more dense than gases.

Exception is water. Liquid water is more dense than
steam and ice. That is why ice cubes float.

76
Q

Specific Gravity

A

compares the density of a
substance with the density of water at a given
temperature.

Specific gravity = density of substance (g/L)
Density of water (g/L)

77
Q

Because units cancel, specific gravity has no units.

Give an example.

A

The density of water at 4 oC is 1.00 g/ml. Therefore
at 4 oC specific gravity = density (but without units).

78
Q

How many significant figures in 560,000?

A

2

560,000

79
Q

How many significant figures in 0.04?

A

1

0.04

80
Q

How many significant figures in 4.60 x 10-6

A

3

4.60 x 10-6

3.080 x 103 has 4 sig figs

81
Q

Significant figures examples

A
82
Q

Solve with the correct number of significant figures

56.8 x 0.37 =

A
  1. 8 has 3 sig figures; 0.37 has 2 sig figures (least sig figs)
  2. 8 x 0.37 = 21.016 => 21 (2 sig figs)
83
Q

Solve with the right number of sig figs

(2.075)(0.585) divided by (8.42)(0.0045)

A

(2. 075)(0.585) divided by (8.42)(0.0045) = 32 (the answer must have 2 sign. figures)
2. 057 has 4 sig figures
0. 585 has 3 sig figures
8. 42 has 3 sig figures
0. 0045 has 2 sig figures(←the fewest )

84
Q

Solve with the correct number of significant figures. 27.8 cm + 0.235 cm = ?

A
  1. 8 has 1 decimal place(←the fewest decimal places)
  2. 235 has 3 decimal places 27.8 cm + 0.235 cm = 28.0 cm

(the answer must have 1 decimal place)

85
Q

Speed limit is 65 m/hr.

What is that speed in ft/sec?

A

Remember, we want ft/sec in the answer

86
Q

how do you figure out the average?

A

The average of a set of numbers is simply the sum of the numbers divided by the total number of values in the set. For example, suppose we want the average of 24 , 55 , 17 , 87 and 100 . Simply find the sum of the numbers: 24 + 55 + 17 + 87 + 100 = 283 and divide by 5 to get 56.6

87
Q

Which of the following are correct unit conversion factors involving the gram?

A
88
Q

The metric unit of volume is the liter, which has a volume equal to that of what?

A

a cube measuring 10 cm

89
Q

The general formula for a number written in scientific notation is y x 10x. Which of the following statements about the formula are correct?

A

y is called the coefficient.

  • x* can be any positive or negative whole number.
  • y* is a number whose absolute value is between 1 and 10.
90
Q

Name some volumes that are equal to one liter?

A

1 dm3 (1 cubic dm = 1000 ml)

1000 cm3 (10cm3)

109 nL (nL = 1x10-9)

91
Q

Select all the statements that correctly describe a conversion factor.

A

Conversion factors are used to convert one unit into another.

The conversion factor must be arranged so that the denominator in one term cancels the numerator in another term.

The conversion factor must cancel out the unwanted unit.

92
Q

A student uses the SCI button or mode on his calculator to convert the number 0.00873 to scientific notation. How might the number now display? Select all that apply.

A
  1. 73–03
  2. 73E–3
93
Q

Which of the following statements about temperature scales are correct? Select all that apply.

A

The units of the Celsius and Fahrenheit scales are both called degrees.

Zero on the Kelvin scale corresponds to absolute zero.

94
Q

10 EE 5 means what?

A

10x105

EE = 105

95
Q

The density of palladium is 12.0 g/cm3. What volume in liters would be occupied by 532 g of palladium?

A

0.0443L

96
Q

On the Celsius temperature scale, water freezes at what? and boils at what?

A

water freezes at 0 degrees C and boils at 100 degrees C

97
Q

Which of the following units are possible units for density? Select all that apply.

A

kg/L

mg/dL

g/cc

98
Q

1dm3 =

A

1 Liter

JLH Chem 1 (5 decks)

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