Transcript Chapter 1 – Matter and Change

Chapter 1 – Matter and Change
Taken from Modern Chemistry
written by Davis, Metcalfe, Williams
& Castka
Chemistry is a Physical Science
Section 1 - Objectives
– Define chemistry
– List examples of the branches of chemistry
– Compare and Contrast
• Basic research
• Applied research
• Technological development
Section 1-1
Chemistry is the study of the composition,
structure, and properties of matter and the
changes it undergoes.
What is it made of?
Makeup and internal arrangement?
What happens when we
heat?
cool?
Mix with other materials?
Why does this behavior occur?
Section 1-1 (continued)
Six main Branches of Chemistry
Organic – deals with carbon containing compounds
Inorganic – study of substances not classified as organic, mainly those
that don’t contain carbon
Physical – study of properties, changes and relationship between energy
and matter
Analytical – identification of components and composition of materials
Biochemistry – study of substances and processes occurring in living
things
Theoretical – using math and computers to design and predict the
properties of new compounds
Section 1-1 (continued)
A Chemical is any substance that has a
definite composition.
Section 1-1
(continued)
The 3 often overlap –
understanding of
crystals and basic light
allowed lazers to be
created which lead to
fiber optics
Basic Research
- carried out for the sake of
increasing knowledge (ex.
Teflon, sticky notes)
Applied research – is
carried out to solve
problems (ex ozone
depletion)
Technological
developments –
production of
products to improve
our lives
(ex biodegradable
material)
Matter and Its Properties
Section 2 - Objectives
– Distinguish between the physical properties and
chemical properties of matter.
– Classify changes of matter as physical or chemical.
– Explain the . . . states in terms of particles
• Gas
• Liquid
• Solid
– Distinguish between a mixture and a pure
substance
Section 1-2
M&M
Mass is a measure of the amount of matter.
Measured in Kg, g and for the
less educated ☺in lbs and ozs.
So . . .Matter is anything that has mass and takes up
space.
Section 1-2 (continued)
Basic Building Blocks of Matter
An Atom is the smallest unit of an element that
maintains the properties of that element.
and . . .an element is a pure substance made of one
only kind of atom.
and . . .a compound is a substance that is made from
the atoms of two or more elements that are
chemically bonded.
Section 1-2 (continued)
Basic Building Blocks of Matter (continued)
An molecule is the smallest unit of an element or
compound that retains the properties of that element
or compound .
EXAMPLES
O2
H2O
Section 1-2 (continued)
Properties and Changes in Matter
Extensive properties
depend on the amount
of matter present
– Volume
– Mass
– Amount of Energy
Intensive properties do
not depend on the
amount of matter
present
– Melting pt.
– Boiling pt.
– Density
– Ability to conduct:
– Heat
– Electricity
Section 1-2 (continued)
Physical Properties and Physical Changes
Physical property is a characteristic that can be
observed without changing the identity of the
substance
– Melting pt.
– Boiling pt.
A change in a substance that does not involve a change in
the identity of the substance is called a physical change
– Grinding
– Cutting
– Melting & Boiling
Section 1-2 (continued)
Physical Properties and Physical Changes (continued)
Change of state is a physical change of a substance
from one state to another.
Solid has definite volume and definite shape
Liquid has definite volume but an indefinite state
Gas has neither a definite volume or a definite shape
Section 1-2 (continued)
Chemical Properties and Chemical Changes
A Chemical property relates to a substances ability to
undergo changes that transform it into different
substances.
– Ability to burn in air
– Iron rusting by combining with the oxygen in air
A change in which one or more substances are
converted into different substances is called a
chemical change.
Section 1-2 (continued)
Chemical Properties and Chemical Changes (continued)
The substances that
react in a chemical
change are called the
reactants.
The substances that
are formed in a
chemical change are
called the products.
Carbon plus oxygen yields (or forms) carbon-dioxide
Carbon + oxygen  carbon-dioxide
C + O2  CO2
Section 1-2 (continued)
Chemical Properties and Chemical Changes (continued)
Chemical changes and reactions, such as combustion
and decomposition, form products whose properties
differ greatly from those of the reactants.
However, chemical changes do not affect the
total amount of matter present before and
after a reaction. The amount of matter, and
therefore the total mass, remains the same.
Section 1-2 (continued)
Energy and Changes in Matter
When physical or chemical changes occur,
energy is almost always involved.
The energy can take several different forms,
such as heat or light.
Although energy can be absorbed or released in
a change, it is not created or destroyed. It
simply assumes a different form.
Section 1-2 (continued)
Classification of Matter - Mixture
A mixture is a blend of two or more kinds of matter,
each of which retains its own identity and
properties.
A mixture that is uniform in
composition they are
said to be homogeneous
Examples
salt-water solutions
A mixture that is not
uniform in composition is
said to be heterogeneous
Examples
clay & water
Section 1-2 (continued)
Classification of Matter – Pure substances
A pure substance has a fixed composition and differ
from a mixture in the following ways:
1. Every sample of a pure substance has exactly
the same characteristic properties.
2. Every sample of a given pure substance has
exactly the same composition.
Section 1-2 (continued)
Classification of Matter – Laboratory Chemicals and Purity
Chemicals in laboratories are generally treated as if
they are pure. However all chemicals have some
impurities.
Purity ranking depends on the needs of the users.
Elements
Section 3 - Objectives
– Use a periodic table to name elements, given their
symbols.
– Use a periodic table to write the symbols of
elements given their names.
– Describe the arrangement of the periodic table.
– List the characteristics that distinguish metals,
nonmetals, and metaloids.
Section 1-3
Introduction to the Periodic Table
The vertical columns of the periodic table are called
groups.
The horizontal rows of elements in the periodic table are
called periods.
Section 1-3 (continued)
Oxygen
Introduction to the Periodic Table (continued) Carbon
Seventeen most common Hydrogen
Ten most common
elements in the Human
Nitrogen
elements in the Milky Way
Body
Galaxy
Calcium
Hydrogen
Phosphorus
Ten most common
Helium
Potassium
Oxygen
elements in the
Oxygen
Sulfur
Earth’s Crust
Silicon
Carbon
Chlorine
Aluminum
Neon
Sodium
Iron
Magnesium
Iron
Calcium
Iron
Sodium
Nitrogen
Magnesium
Cobalt
Silicon
Potassium
Copper
Magnesium
Titanium
Zinc
Sulfur
Hydrogen
Iodine
Selenium
Section 1-3
The periodic table is divided into two main
groups – metals and non-metals. Metals to
the left and non-metals to the right.
Types of Elements - Metals
An element that is a good conductor of heat and electricity is a metal.
Most metals are malleable – they can be hammered or rolled into
thin sheets
They are also ductile which means they can be drawn in to fine wire.
Metals that behave this way have a high tensile strength.
Section 1-3
Types of Elements - Nonmetals
A nonmetal is an element that is a poor conductor of heat and
electricity.
Many nonmetals are gas at room temperature , when solid they
tend to be brittle.
Section 1-3
Types of Elements - metalloids
A metalloid is an element that has some characteristics of
metals and some characteristics of nonmetals.
Metalloids tend to be semiconductors.
Section 1-3
Types of Elements – Noble Gases
The elements in group 18 of the periodic table are generally
unreactive.
Chapter Summary Questions
HW – page 26
1 ,5-13 ,17 ,19 , 20 & 23
Chapter Summary Questions
1 - Chemistry is the study of the compostion,
structure and properties of substances and the
changes they under go
5
a) A measure of the amount of matter
b) the amount of space occupied by matter
6
The portions of elements in a pure substance
are fixed.
7
a) A property is any characteristic of a
substance or material.
b) Properties can be compared in order to
classify unknown materials as members of
known groups or subgroups of substances, or
to identify substances directly.
8
Extensive properties depend on the amount of
matter that is present. Intensive properties do
not.
9
a. a characteristic that can be observed or
measured without changing the identity of
the substance.
b. Examples include color, odor, length, size ,
melting point & boiling point.
10
a. a property that describes the ability of a
substance to undergo changes that alter its
identity.
b. Examples include the ability of coal to burn
and the ability of iron (Fe) to rust.
11
A physical change is a change in a substance that
does not involve a change in its identity. A
chemical change is a change in which a
substance is converted into other substances.
12
a. solids, liquids & gases
b. A solid has a definite shape and fixed volume
, whereas a liquid has a fixed volume but
takes the shape of the vessel it is in.
c. A gas has neither fixed volume or definite
shape.
d. Liquids and gases take the shape of the
container they are in.
13
A change of a substance from one state of
matter to another.
17
The reactants are potassium (K) and water (H2O)
and the products are potassium hydroxide
(KOH) and hydrogen (H2)
19
a. physical , wood still wood
b. chemical , composition change think taste
c. physical, butter still butter
20
a.
b.
c.
d.
e.
f.
potassium (K)  metal
Silver (Ag)  metal
Silicon (Si)  metalloid
sodium (Na)  metal
Mercury (Hg)  metal
helium (He)  noble gas
23
a.
b.
c.
d.
e.
f.
Group 14, period 2
Group 18, period 3
Group 6, period 4
Group 2, period 6
Group 17, period 5
Group 11, period 6