Section 1.1 What is Matter?
Chapter 1
Matter, Measurements, and Calculations
Section 8 Section 9 Section 10 Section 11
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Section 1.1 What is Matter? |
1. Chemistry is the scientific study of matter.
A
scientific discipline that studies matter is ________.
2.
Matter is defined as anything that has mass and occupies space.
a) Anything
that has mass and occupies ________ is said to be matter.
b) The amount of ________ an object occupies is known as its volume.
3.
An
actual measurement of the amount of matter contained in an object is known
as the mass.
Mass
is a measurement of the amount of ________ within an object.
4.
An
object’s weight is a measurement of gravitational force pulling on that
object.
a) ________
is a measure of gravitational force acting on an object.
b) Jupiter has a stronger gravitational force than Earth. On Jupiter, an object would have (more, less, the same) weight as on Earth, and the mass would be (more, less, the same) as on on Earth.
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Section 1.2 Properties and Changes |
5. Physical properties of matter are those characteristics that
can be observed or measured without changing the composition of matter.
Properties
of matter that can be observed or measured without changing the composition of
the matter are said to be ________ properties.
6.
The properties matter demonstrates when attempting to change the matter into a
new substance is called chemical properties.
________
properties can be noted when one tries to change matter into another substance.
7.
Matter can undergo two types of changes; physical or chemical.
The
two types of changes matter can experience are: chemical and ________.
8. In a physical change you do not change what a substance is made up of. Examples include crushing, boiling, freezing, melting, etc. In a chemical change, a substance is changed into some completely new substance or substances and cannot be changed back into the original substance unless some other chemical change is performed. Examples include burning, some color changes when substances are mixed together, fizzing (a gas is given off) when substances are mixed together.
What
is the type of change that matter experiences that alters the composition of the
substance? (physical/chemical)
9.
Classify each of the following changes as physical or chemical: (Write “c”
for chemical and “p” for physical)
a)
Electricity produced from a battery.
b)
Yellow sulfur is melted and changes to a black liquid.
c)
A steel bridge expands on a hot day.
d)
Your stomach is no longer upset after taking an antacid.
e)
Vinegar is used to clean lime deposits in showers.
f)
A copper wire is bent.
g)
Un-refrigerated meat spoils
h)
A snow bank disappears on a sunny day without leaving a puddle of water.
i)
Your car rusts.
j)
Wood burning in a campfire
k)
Gas is released when you open a soda can.
l)
Water freezes
10.
Changes in state are among the most common physical changes.
This includes the melting of solids into liquids, the sublimation of
solids into gases, or the evaporation of liquids to form gases.
The
changing of a solid directly into a gas without passing through the liquid phase
is called ________.
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Section
1.3 |
11.
Explanations for observed behavior in nature are known as scientific models.
Scientists
often use scientific ________ to explain behavior that is observed in nature.
12.
A molecule is the smallest particle of a pure substance that has properties of
that substance and is capable of independent existence.
Therefore, it is the limit of the physical subdivision of a substance.
________
represent the limit to the physical subdivision of pure substances.
13.
Molecules are made up of even smaller particles.
These particles, known as atoms, cannot be chemically broken down into
smaller constituents.
a) ________
are the very small particles that make up molecules.
b) Atoms are the limit of the ________ subdivision of matter.
14.
There are two main categories of molecules; homoatomic and heteroatomic. Homoatomic designates molecules that are made of only one
kind of atom, while heteroatomic suggests that the molecule is made up of two or
more types of atoms.
The
type of molecules that consist of two or more types of atoms are called ________
molecules.
15.
Another way of classifying molecules is by the number of atoms each contains.
Molecules that contain two atoms are known as diatomic, those with three
are called triatomic, and molecules with more that three atoms are called
polyatomic molecules.
a) If
a molecule contains three atoms, it is known as a ________ molecule.
b) Which of the following are examples of heteroatomic molecules? Of diatomic molecules? In this case a capital letter (such as S) or a capital letter followed by a lower case letter (such as Ca) indicate an atom of a specific element (you can look on the periodic table to find the element's name). The subscripted number, such as O3, tells us how many atoms of that element there are; O3 means there are 3 oxygen (O) atoms. If no subscripted number is present, it means there is only one of those atoms. For example: NO2 means there is 1 nitrogen (N) atom and 2 oxygen (O) atoms.
H2O, Br2, HF, S8
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Section 1.4 |
16.
Matter can be divided into two categories; mixtures and pure substances. Matter that is a pure substance has a constant composition
throughout; that is, all the molecules are the same and have a fixed set of
properties. In mixtures, however,
the matter is blended and can be physically separated into two or more
components. (See Figure 1.5)
A bottle full of methanol (CH3OH) would be classified as a ________ ________. Because salt water can be ________ separated by evaporating off the water which leaves the salt remaining behind, it is classified as a ________.
17.
Matter can also be classified as being homogeneous or heterogeneous. Homogeneous matter has a uniform appearance and the same
properties throughout. Heterogeneous
matter has properties and appearances that are not the same throughout the
sample.
A
sample of matter composed of yellow flecks and black granules would be described
as ________.
18.
Pure substances are always homogeneous. Mixtures
can be either homogeneous or heterogeneous. (See figure 1.10)
Brass is composed of copper and zinc. Brass is a (homogeneous/heterogeneous) (pure substance/mixture). Copper is a (homogeneous/heterogeneous) (pure substance/mixture).
19.
Solutions are homogeneous mixtures of two or more pure substances.
A
homogeneous mixture of two or more pure substances is called a ________.
20.
The two sub-categories of pure substances are: elements and compounds.
a) Elements
and compounds are the two divisions of ________ ________.
b) Which of the following are examples of elements? Of compounds?
Cl2, FeSO4, P5, CaO
21.
Elements are individual atoms or homoatomic molecules of one kind and cannot be
chemically subdivided into simpler pure substances.
However, compounds consist of heteroatomic molecules or two or more kinds
of atoms and can be chemically subdivided into simpler substances. (See fig
1.10)
What
type of matter is composed of molecules in a uniform composition and are homoatomic as well?
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SECTION: 1.6 The Metric System |
22.
The metric system is the measurement system used primarily everywhere but in the
U.S. It is based on a decimal system where larger and smaller units are related
by factors of 10.
Within
the metric system, units of measurement have factors of ________ in common.
23.
In the metric system, common prefixes are used to indicate their relationship to
the basic unit. Some of the most
commonly used prefixes are: kilo- 1000 x basic unit, deci – 1/10 x basic unit,
centi – 1/100 x basic unit, milli – 1/1,000 x basic unit, and micro –
1/1,000,000 x basic unit. (See Table 1.2 and Example 1.6)
Convert
each of the following into the desired units:
a)
1.54 m = ________ cm
b)
5.6 g = ________ mg
c)
8,695 g = ________ kg
d) 647 mm = ________ km
e) 4837 mL = _____ L
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24.
There are three scales on which temperature can be measured; Celsius,
Fahrenheit, and Kelvin. The
relationship between the scales can be found in Equations 1.1-1.4.
Using
the formulas in your text and Example 1.7 as a guide, convert each of the
following into the desired units. Round
answers to the nearest whole number.
a)
(normal body temperature) 98.6o F = ________o C
b)
37o C = ________ K
c)
10o C = ________o F
25.
In the metric system, different units are used to measure different quantities.
For measuring length, the basic unit is the meter (m),
volume = cubic decimeter (dm 3) or liter (L),
mass = kilogram (kg), and temperature = Kelvin (K).
What
is the basic unit used for measuring length?
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SECTION: 1.7 Large and Small Numbers |
26.
When dealing with very large or small numbers, using scientific notation can be
very helpful. Scientific notation
is a way to represent numbers in which a number is multiplied by 10 raised to a
positive or negative exponent. The
exponent to which 10 is raised is used to indicate how many positions the
decimal point will move and the sign of the exponent indicates in what
direction. When changing a number from scientific notation to regular numbers,
if the exponent is negative, move the decimal to the left.
If it is positive, move the decimal to the right.
(See Example 1.8) For example 5.88 x 10 2 is another way to
write 588.
Take
the following number out of scientific notation: 3.72 x 10-5.
27.
When changing a number from regular numerical form into scientific notation, the
goal is to have the first non-zero number then the decimal followed by any
trailing numbers. The position
directly to the right of the first non-zero number is known as the standard
position. If, when moving the
decimal to the standard position, it is moved to the right, the exponent on the
ten will be negative. If the
decimal is moved to the left, the exponent is positive.
Also, as discussed above, the number of positions the decimal is moved
indicates the number of the exponent. (See Example 1.9)
Change
the following numbers to correct scientific notation:
a) 5,830,000 =
b) 0.00181
c) 0.0068 x 10-2
d) 0.097 x 107
Note: It is highly advisable to use a scientific calculator!!
28. When multiplying numbers in scientific notation, do regular multiplication with the nonexponential numbers and then add the exponents of 10 for the final answer. (See Example 1.11)
Complete the following calculation, and express the result in correct scientific notation:
(4.6 X 10-7) (5.0 X 103) =
29.
When dividing numbers in scientific notation, divide the nonexponential numbers
as regular and then subtract the bottom exponent from the top one.
Complete the following calculation, and express the result in correct scientific notation:
1.2 x 103/3.0 x 10-2 =
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SECTION: 1.8 Significant Figures |
30.
Significant figures are the numbers within a measurement that represent the
certainty of the measurement, plus one number that represents an estimate for an
uncertain number.
The
numbers that represent the certainty of a measurement plus one number that is an
estimate are known as _______ figures.
31.
The rules for determining the number of significant figures within a number are
as follows (See Example 1.12):
1)
All non-zero numbers are significant.
2)
Leading zeros, or zeros not preceded by nonzero numbers are not
significant.
3)
Confined zeros or zeros between nonzero numbers are significant.
4)
Trailing zeros or zeros at the end of numbers are significant.
How
many significant figures are found in the following measurements?
a)
0.00180 m
b)
16.5o C
c)
25.0 L
32. When using scientific notation, only the numbers that precede the "x 10exp" are significant. All of the zeros that are expressed by the "x 10exp" are not considered significant.
How many significant figures are in the following scientific notation expressions?
a) 1.045 x 105
b) 6.20 x 10-4
c) 3.142 x 10-12
33.
When doing multiplication or division, the answer must have the same number of
significant figures as the quantity with the fewest significant figures used in
the calculation (See Example 1.13)
Do
the following calculation, and round the answer to the correct number of
significant figures:
(6.85)(3.0)/16.1
34.
When adding or subtracting, the answer must have the same number of places to
the right of the decimal as the quantity in the calculation with the fewest
number of places right of the decimal (See Example 1.14)
Do
the following calculation, and round the answer to the correct number of
significant figures:
(8.357
+ 2.6) –13.213
35.
Numbers that have no uncertainty, such as counting numbers, or numbers that are
part of reduced simple fractions are know as exact numbers and are considered to
have an unlimited number of significant digits and are not used to determine the
number of significant figures in solutions for calculations.
Exact
numbers, like one dozen, contain unlimited ________.
36. Self Test
1. How many significant figures are in the following?
a) 0.0040310
b) 5.64 x 105
2. Do the following calculations and express your answers using the correct number of significant figures:
a)
| 1.085 x 6.21 |
| 0.9512 |
b) (8.965 + 0.011) - 0.7
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SECTION: 1.9 Using Units in Calculations |
37.
The Factor-Unit-Method is a technique used for converting measurements from one
unit of measurement to another. It
involves ratios (proportions) taken from fixed relationships between quantities.
To
use the Factor-Unit-Method one must use ratios from fixed relationships
between quantities to convert between different ________ of measurement.
38. Factors are proportions with units. Unlike fractions, factors can be flipped up side down and still have the same meaning. For example:
8 oz =
1 cup 1 cup 8 oz You'll notice that the line does not imply "divided by", but is read as "per". For example, "8 oz per 1 cup".
Practice converting the following relationships into factors. Make two factors for each relationship, as shown above.
a) 36 inches = 1 yard
b) 1 gross = 144 items
c) 1440 minutes are in 24 hours
d) 1 bushel contains 4 pecks
39. A woman has a weight of 136 lbs. A nurse must have the woman's weight in Kilograms to calculate a drug dosage for the woman. What is the woman's weight in Kg? There are 2.20 pounds in 1.00 Kilogram.
Above is an example of a typical problem that uses the Factor-Unit-Method to solve it. Complete the following steps to solve the problem:
- What is the number (value) and units that needs to be converted? What are the units this number needs to be converted to?
- What factor is given? Write the factor in two ways as you did in question 38.
- All Factor-Unit-Method problems use the following format:
number and units to be converted x factor = answer with desired units
To set-up the problem:
Write down the number and units that needs to be converted from (a) above. Put a multiplication sign (X) after it.
Write the factor you will use for the conversion. The factor you choose from part (b) is the one with the units of the number you are converting from on the BOTTOM and the units you wish to convert to on the TOP.
Show the set-up for the problem above:
d. Do the math to solve the problem. To do this, simply multiply the two numbers that are on top and then divide by the bottom number. What is the answer? Don't forget the units!
40. Self Test
a) A toy factory can produce 24 gizmos in 0.845 hours. How many gizmos can the factory produce in 6.50 hours?
(Use the factor-unit method to answer the questions below which will allow you to answer the problem above.)
1) What is the number (and units) that the problem needs to convert?
2) What factor is given to you?
3) Using the factor-unit method, how is the problem set up?
4) What is the answer?
b) You've just completed 56.0 hours of work. Your boss pays you $35.75 for every six hours of work. How much money did you make?
c) You can make 37 cookies from 1.50 pounds of flour. How many cookies can you make from 10.0 pounds of flour?
d) Your basement has a 325 square foot room that needs carpeting. You can buy 9 sq. feet of carpeting for $7.65. How much will it cost to carpet the room (excluding installation)?
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41. The percent, when taken literally, means per one hundred. So, when one is trying to determine what percent a certain group of items is out of all the items, take the part (group of items) divided by the whole (all the items), times 100. (Part/whole) x 100 = % (See Equation 1.6)
The percent of something is found by taking the part divided by the whole, times _____.
42. Percentages are used in many capacities from charting progress within a
group to determining the amount of a reactant used in a reaction. (See Example
1.18)
a)
In a voting district there are 4,237 voters.
927 of these are African-American.
There is ________% African-American voters in this district (answer should have
3 significant figures).
b) A 253g sample of ore is 0.16% gold by weight. How much gold is in the sample?
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SECTION: 1.11 Density |
43. Density is a physical property of matter that basically refers to the heaviness or lightness of an object relative to its size. The formula for determining the exact density of an object is: Density = Mass/Volume (See Equation 1.8). If an object is less dense than a liquid will float on it. If it is more dense it will sink.
Liquid mercury has a density of about 13.5g/mL. Calcium has a density of about 1.5g/mL. Water has a density of about 1.0g/mL. Will a clump of calcium float or sink in mercury? in water?