Module 1: Measurement, Matter, and Atomic Theory

Chemistry

1.1 Behavior of matter and energy in the _____ domains provide different ways of considering and describing ___________ behavior

3; chemical

1.1 Macroscopic Domain

The realm of everyday things that are large enough to be sensed directly by human sight or touch

1.1 Microscopic Domain

Most aspects are too small to be seen and often visited in the imagination or by a microscope

1.1 Symbolic Domain

Uses specialized language to represent composition of the macroscopic and microscopic domains. Eg: symbols, formulas, equations, graphs, drawings, and calculations

1.2 The 3 things a measurement provides

1. Size or magnitude of the measurement (a number)

2. A standard of comparison for the measurement (a unit)

3. An indication of the uncertainty of the measurement

1.2 Numbers

can be represented in different ways, including decimal form and scientific notation

1.2 Units

Standards of comparison for measurements, without numbers can be meaningless, confusing, or life-threatening

1.2 The International System of Units (SI)

The standard system of measurements that the scientific community uses. An updated version of the metric system composed of 7 fundamental properties

1.2 The 7 fundamental properties of the SI system

Length, Mass, Time, Temperature, Electric Current, Amount of substance, and Luminous intensity

1.2 What is the name of the SI unit for length?

meter

1.2 What is the name of the SI unit for mass?

kilogram

1.2 What is the name of the SI unit for time?

second

1.2 What is the name of the SI unit for temperature?

kelvin

1.2 What is the name of the SI unit for electric current?

ampere

1.2 What is the name of the SI unit for amount of substance?

mole

1.2 What is the name of the SI unit for luminous intensity?

candela

1.2 What is the name of the SI unit for density?

kilogram per cubic meter

1.2 What is the name of the SI unit for volume

cubic meter

1.2 What is the symbol for the SI unit for length?

m

1.2 What is the symbol for the SI unit for mass?

kg

1.2 What is the symbol for the SI unit for time?

s

1.2 What is the symbol for the SI unit for temperature?

K

1.2 What is the symbol for the SI unit for electric current?

A

1.2 What is the symbol for the SI unit for amount of substance?

mol

1.2 What is the symbol for the SI unit for density?

kg/m³

1.2 What is the symbol for the SI unit for volume

m³

1.2 how many pounds is the kilogram (kg)

2.2

1.2 How are kelvin and Celsius related?

They have the same magnitude, but on a different scale.

1.2 How can you write cm³ differently?

cc or mL

1.2 What does dm³ also equal

1 liter (L)

1.2 What is the equation for density?

density = mass/volume

1.2 What is the equation for volume

volume = mass/density

1.2 What is the equation for mass?

mass = density x volume

1.2 femto

f, 10^-15

1.2 pico

p, 10^-12

1.2 nano

n, 10^-9

1.2 micro

µ, 10⁻⁶

1.2 milli

m, 10⁻³

1.2 centi

c, 10⁻²

1.2 deci

d, 10⁻¹

1.2 kilo

k, 10³

1.2 mega

M, 10⁶

1.2 giga

G, 10⁹

1.2 tera

T, 10¹²

1.3 In general, numerical scales will permit measurements to _____________ of the small scale division. aka, one __________ number.

one-thenth; estimated

1.3 Significant figures/digits

All of the digits in a measurement, including the uncertain last digit

1.3 Leading zeros

These zeros tell us where the decimal is located and not measured and are not significant. Eg- 0.008020

1.3 Captive Zeros

These zeros appear between two non-zero numbers and are always measured. Eg- 0.008020

1.3 Trailing Zeros

These zeros appear after all of the non-zero numbers. If there is a decimal, they are significant. If there is not a decimal, they are not significant. Eg- 0.008020

1.4 Dimensional Analysis aka Factor-label Method

When some quantities may not be easy or possible to measure directly but must be calculated from other measured properties and appropriate relationships.

1.4 What is the Dimensional Analysis aka Factor-label Method is based on?

Units of quantities must e subjected to the same mathematical operations as their associated numbers

1.4 What are the two most common reference values on a thermometer?

Freezing and boiling temperatures

1.5 Matter

Anything that occupies space and has mass

1.5 What are some examples of Matter?

solids, liquids, and gasses

1.5 Describe a solid?

rigid and possesses a definite shape

1.5 Describe a liquid

flows and takes the shape of its container

1.5 Describe a gas

takes both shape and volume of its container

1.5 Which form(s) of matter have volumes that are nearly independent of pressure?

Solid and liquid

1.5 What is the mass of an object?

a measure of the amount of matter in it

1.5 Law of conservation of Matter (Mass)

There is no detectable change in the total quantity of matter present when matter converts from one type to anther (chemical change) or changes among solid, liquid, or gaseous states (physical change)

1.5 Describe a Pure Substance

has a constant composition

1.5 What classes can a Pure Substance be divided into?

Elements and Compounds

1.5 Describe Elements

Pure substances that cannot be broken down into simpler substances by chemical changes

1.5 Describe Compounds

Pure substances that are comprised of two or more elements that can be broken down by chemical changes that yield either elements, compounds, or both

1.5 Properties of __________________ are different from those in the free, or uncombined, state

combined elements

1.5 Describe a Mixture

Composed of two or more types of matter that can that can be present in varying amounts and can be separated by physical changes

1.5 Describe Heterogeneous Mixture

not completely uniform in composition, varying from point to point

1.5 What is an example of a Heterogeneous Mixture?

Italian dressing, chocolate chip cookies, or granite

1.5 Describe Homogeneous Mixture

exhibits a uniform composition and appears visually the same throughout

1.5 What is an example of Homogeneous Mixture?

sports drink, air, maple syrup, gasoline, and a solution of salt in water

1.5 Describe Properties

Characteristics that distinguish one substance from another

1.5 Physical Property

A characteristic of matter that is not associated with a change in its chemical composition

1.5 What is an example of a Physical Property?

density, color, melting and freezing temperatures

1.5 Physical Change

a change in the state of properties of matter without any accompanying change in the chemical identities of the substance contained in the matter

1.5 What is an example of Physical Change?

wax melts, sugar dissolves in coffee, magnetizing and demagnetizing metals

1.5 Chemical Property

Change of one type of matter into another (or inability to change)

1.5 What is an example of a Chemical property

flammability, toxicity, acidity

1.5 Chemical Change

Always produces one or more types of matter that differ from the matter present before the change

1.5 What is an example of a Chemical Change?

combustion, food being cooked, digested, or rotting

1.5 Describe Extensive Property

Depends on the amount of matter present and is directly proportional to the amount of matter in question

1.5 What is an example of an Extensive Property?

Mass, volume, gallon of milk is larger than a cup of milk

1.5 Describe Intensive Property

Does not depend on the amount of matter present

1.5 What is an example of Intensive Property

temperature

1.6 Atom

Smallest particle of an element that has the properties of that element and can enter into chemical combination

1.6 Molecules

consists of two or more atoms joined by strong forces called chemical bonds. The atoms can be identical or different.

1.6 What did JJ Thomson Discover?

the electron

1.6 What did JJ Thomson use to make his discovery?

The cathode Ray Tube

1.6 When did JJ Thomson make his discovery?

Late 1800’s

1.6 What did Robert A. Millikan discover?

The charge of an electron (1.6×10^-19 C)

1.6 How did Robert A. Millikan make his discoveries?

Oil Drop experiments

1.6 When did Robert A. Millikan make his discoveries?

1909

1.6 What did Ernest Rutherford discover?

1. The volume of an atom contains large amount of empty space

2. The Proton is at the center of each atom

1.6 How did Ernest Rutherford and his team make their discoveries?

By shooting alpha particles at a very thin sheet of gold foil

1.6 What is Ernest Rutherford’s famous quote?

“It was quite the most incredible event that has ever happened to me in my life. It was almost as incredible as if you fired a 15-inch shell at a piece of tissue paper and it came back and hit you.”

1.6 Isotopes

atoms of the same element that differ in mass because there is a different amount of neutrons than protons

1.6 Who discovered isotopes

Frederick Soddy, awarded the Nobel prize in chemistry in 1921

1.6 What did James Chadwick discover?

the neutron

1.6 When did James Chadwick make his discovery?

1932

1.7 Atomic Mass Unit (amu) and Fundamental Unit of Charge (e)

The small units of measure used to describe atoms

1.7 Proton

Mass 1.0073 amu, charge +1