Chemistry !!The study of the composition,

__________, and properties of matter

and the ____________________

Chemists make measurements to ________________ of matter. To keep things consistent, we all work in __________

Matter?

Matter is anything that occupies space and has mass. Chemistry is the study of matter and how it changes

Volume - _____________

(even air !)

measured in ____and ____

Matter

Mass - measure of __________.

____in ____________

Any substance that has a definite composition

Chemical

Examples:

The smallest unit of an

Element that _____________

Properties of that element

Atom

Classification of Matter

Elements _____ be separated into simpler substances by chemical means. Example: __________ Smallest part is an ______

Elements/Compounds

Compounds are composed of atoms of _________ elements. Examples:_________________

Phases of Matter

There are three common phases of matter:

•____ – closely spaced and _____

•____ – closely spaced but _____

•____ – large separation; mostly _____________

3 States of Water

Phase Atom Movement

Shape Volume Energy

Solid

Liquid

Gas

Properties

An ________ property _______ on __________ matter is being considered. Example:

An _________ property _______ depend on __________ matter there is. Example:

Properties?

In Chemistry we study of matter and how it changes; we need to be able accurately observe properties to do this!

Properties

A __________ property is a characteristic that can be observed or measured _______ changing the identity of the substance.

Examples include

A _________ property is a characteristic that describes the _______ of a substance to undergo changes that alter its identity.

Examples include the _____ of coal ______ and the _____ of iron _______.

Properties

Properties

A _______ change is when a substance changes physical condition but ________ involve a change in composition.

A _______ change is when a substance changes a substance ______________________ of substances.

Properties

Classify each of the following as either a physical change or a chemical change:

• Tearing a sheet of paper

• Melting a piece of wax

• Burning a log

• Milk turns sour

-

Mixtures contain two or more substances and generally can be __________________.

Pure substances have a _______ _____________ and distinct properties.

Mixtures/Substances

Homogeneous means the ______ throughout. ________ separate by filtering. Ex.

Mixtures

Heterogeneous means that it is ___________. ____ separate by filtering. Ex.

Scientific Method

Definitions•___________ – a testable

statement•______ – an explanation of how

phenomena occur and how data and events are related

•_________ – a broad generalization that explains a body of facts

EquipmentCommonly used for liquid

measures

Liquid Volumes

Volume read to the bottom of the _________

SI Units?

Measurements can be made in many different units. To be consistent, all scientists use the metric system to report measurements. Metric system units are called ________

_________________

SI Units ExamplesMeasureme

ntUnit Abbrev.

mass gram

length meter

volume liter

time second

temperature Kelvin

energy JouleAmount of

sampleMoles

Label each instrument with the SI correct units

Temperature Conversions

Like most measurements, temperature has many forms. There are three common ways to report temperature: Fahrenheit (F ), Celsius (C ), and Kelvin (K ).

K = C + 273 or C = K - 273

F = (1.8)(C ) + 32

Temperature Conversion?

So, if it is 35 C , would you go skiing or swimming?

What is the temperature inF ?

In K ?

____ F

____ K

SI SubunitsPrefix Abbrev. Factor

Mega M- 1 x 106

Kilo K- 1 x 103

Hecto H- 1 x 102

Deka D- 1 x 101

Base Unit – meter (m), liter (l), or grams (g)

deci- d- 1 x 10-1

centi- c- 1 x 10-2

milli m- 1 x 10-3

micro- 1 x 10-6

nano- n- 1 x 10-9

pico- p- 1 x 10-12

Metric Conversions

Meter (m)Liter (l)Gram (g)Joule (J)

Unit Conversion?In Chemistry, we can make measurements in many different units. So, we often need to convert to another set of units. We need three things:

1. where you are __________ 2. where you are _______, and 3. the __________________ to get you there.

Converting Units ExampleTo convert units you need to know

where you are starting, finishing, and the conversion factor.

Find the number of cm in 2.1 meters.

We know: 1 m = 100 cm 2.1 m 100 cm = ____ cm 1 m

Find the number of g in 8,200 g.

We know: 1000 g = 1 g

8,200 g 1 g = ____ g 1000 g

Converting Units

SI Subunits Conversions

10.5 g= _________ kg

1.57 km = _______ m

3.54 mg = __________ g

3.5 J = _________ DJ

1.2 L = _____ ml

358 cm3 = _________ m3

How many cm are in 2.8 inches.

Conversion Factor: 1 in = 2.54 cm

2.8 in = ____ cm

How many inches in 12.4 cm?

12.4 cm = ____ in

Converting Units

Unit Conversion Examples

How many ounces in 600 mls?

mls = ______ oz

First we need conversion factor !

12 oz. = 355 ml

Converting TimeHow many days are there in

52,480 minutes?

= ______ days

How many minutes are there in 2.4 months?

= ___________ minutes

Conversions with two units

If you are traveling 20 miles/hour, how many meters/seconds is this?Change one unit at a time. Note, many ways to do this.

Conversions with two units

Convert 25 miles/gallon to km/liter

Convert 10 kg/liter to g/ml

= ______ km/l

= ______ g/ml

Precision vs. Accuracy

Accuracy andPrecision

_________

_______

_______________

_________

Precision

• Refers to the closeness of a set of measurements __________

• Requires that ____________ measuring the same thing be done

• Example:– 2.22,2.23,2.21 shows good precision

Accuracy

•Refers to how close an answer ________ is to __________ or correct value

•Requires that the accepted value is ______

•Use ___________ to express accuracy

Percent Error• _________ = experimental value – accepted value

(value can be _______ or ________)

• ___________ experimental value – accepted value x

100 accepted value(absolute value)

Significant figures?

In most cases it is __________ to obtain the exact value for a measurement. We need to _____________ the significant figures - the meaningful digits in a measured or calculated quantity. The trick is _______ _____________________!

Significant Figures

Rules for determining sig. figs.:

1.All non-zero #’s are sig.

2. Zeros between non-zeros are sig. (a zero sandwich!)

3. Zeros to the left of the first non-zero # are not sig.

-> ______

-> _______

-> ______

Significant Figures Rules

4. Zeros at the end of a number and to the right of a decimal are sig. They are holding a place!

5.For #’s w/out decimals, the trailing zero may or may not be sig. We use Sci. notation on these.

-> ______

1,000,000 years – now 1,000,000.019 years ??

Which zeros are important? Use scientific notation: Could be _________ or ________ or ____________, etc.

Significant Figures

Determine the sig figs & Rule #:

• 6.002 cm

• 0.0020 m

• 10.0500 g

• 7000 kg

-> _____________

-> _____________

-> ______________

-> _______________ _________________

Scientific Notation Examples

1.Distance to Sun:

93,000,000 miles -> _______ miles

2. Vacuum pressure:

0.000000001 torr -> _______ torr

Sci. Not. w/ Calculators

Example: 4 x 1023 x 5 x 10-12 = ?Action Display

Enter “4” 4

Press “EE” 4 00

Enter “23” 4 23

Press “x“ 4 23

Enter “5” 5

Press “EE” 5 00

Enter “-12” 5 -12

Press “=“ 2 12 (2 x 1012)

Significant Figures

Rules for adding and subtracting:

•Answer cannot have more digits to the right of decimal point than the original!!

89.332

+ 1.1

90.432

____round off

Significant Figures

Rules for multiplying and dividing:

•Answer cannot have more significant figures than the original!

2.8 2 s.f.

x 4.5039 5 s.f.

12.61092

___round off

Significant Figures

Report with the correct # of sig. fig.:

• 11,254.1 g + 0.1983 g

• 66.59 L – 3.13 L

• 8.16 m x 5.1355 m

• 0.0154 kg / 88.3 ml

-> ______ g

-> _______ L

-> ____m;__ sf.

-> _________ kg/ml; ___ s.f.

Measurements?

Chemists make measurements to study the properties of matter. To keep things consistent, we all work in SI Units and use significant figures. We also make many conversions between different types of _________ ________. We also make many ________________

Derived Units

•Mathematical combinations of units

•Examples are:

Density?

Density is a common physical property that relates the mass and volume of a substance:

Density =

Units: grams/mlsor

grams/cm3

Density Example

What is the density of a substance that has a mass of 84.7 g and a volume 55.4 cm3.

Density = mass/volume

g = _____ g/cm3

cm3

g cm3 = ___ cm3

g

Density ExampleWhat is the volume of a substance that has a density of 1.73 g/cm3 and a mass of 7.75 g.Density is a conversion factor. 1.73 g = 1.00 cm3 or 1.00 cm3 = 1.73 g