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Domain 3 Structure and Properties of Matter
I. Matter-any substance that occupies space and has
mass
A. States of matter
State
Shape
Solid Definite
shape
Liquid Assumes
shape of
container
Gas
Fills
container
Volume
Definite
volume
Definite
volume
Indefinite
volume
Video Clip
B. Element
1. simplest form of matter; cannot be broken down
into a simpler substance
2. made of atoms
3. represented by a symbol made of one or two
letters. Example Na, C, Au, Ne
C. Compound
1. a substance made of two or more elements that
are chemically combined
2. represented by a chemical formula. ExampleNaCl, H2O, C6H12O6
3. the properties of the compound are different from
the properties of the elements that make up the
compound
4. can be separated only by a chemical reaction
5. two types of compounds
a. ionic
i. formed by the attraction between two or
more elements that transfer electrons
known as ions
ii. example - NaCl (one metal ion and one
nonmetal ion)
b. Covalent (molecular)
i. formed when two or more elements share
electrons
ii. example - H2O Video Clip
D. Mixtures
1. different substances that are simply mixed
together
2. can be separated by physical means (such as
filtration, distillation, and chromatography)
3. Two types
i. heterogeneous-does not have uniform
composition; individual substances
remain distinct. Examples are colloids and
suspensions such as muddy water
ii. homogeneous-has a uniform composition
throughout. Example is a solution which is
made up of a solvent and a solute such as koolaid or salt water
E. Ions
1. Ions are atoms which have gained or lost
electrons.
2. examples include Na+, Cl-, Mg2+, O2Try this online quiz on the organization of matter
II. Physical and Chemical Properties
A. Physical properties
1. properties that are determined by observation,
either looking or measuring
2. examples include color, mass, density, odor,
luster, malleable, ductile
B. Chemical Properties
1. can only be found through testing
2. example includes flammability
III. Chemical and Physical Changes Video Clip
A. In a physical change, the original substance still
exists.
1. Any change in size, shape, or phase is a physical
change. It has only changed form.
2. There are six phase changes.
Phase change What happens
Melting
Solid becomes
liquid
Vaporization
Liquid
(boiling or
becomes gas
evaporation)
Sublimation
Solid become
gas
Freezing
Liquid
becomes solid
Condensation Gas becomes
liquid
Deposition
Gas becomes
a solid
3.
Energy change
Absorbs
Endothermic
heat
Absorbs
Endothermic
heat
Absorbs
heat
Releases
heat
Releases
heat
Releases
heat
Endothermic
Exothermic
Exothermic
Exothermic
4. Other examples of physical changes include
dissolving, crushing, mixing.
B. In a chemical change, a new substance is
produced.
1. Energy changes always accompany chemical
changes.
2. Chemical changes can be accompanied by
physical changes.
3. Identification of a chemical change involve careful
examination of the original reactants to see if new
substances (products) are produced.
i. a gas is formed
ii. temperature change
iii. precipitate forms
iv. appearance of a new color or odor
4. Examples of chemical changes include
fermentation, metabolism, electrolysis.
IV. Atomic Structure
A. Atom
1. the smallest particle of an element that retains
the properties of that element
2. Models of the atom through history
a. Dalton’s model-solid and indivisible
b. Thomson-plum pudding model
c. Rutherford-gold foil experiment-the electrons
orbit around the dense nucleus
Click here for animation of the gold foil
experiment
d. Bohr model
In the Bohr model there were distinct energy
levels where electrons could exist.
•1st energy level holds 2 electrons
•2nd energy level holds 8 electrons
•3rd energy level holds 8 then 18 after 4th
level gets 2 electrons.
Which
element is
this?
e. Modern View of the Atom
 The atom is mostly empty space.
 Two regions
•Nucleus- center region; positively
charged, contains most of the atom’s
mass
•Electron cloud- region where you might
find an electron.
3. Subatomic particles
a. nucleus-center region; positively charged;
contains most of the atom’s mass Video Clip
i. proton –positive particle
ii. neutron-neutral particle (no charge)
b. electron cloud
i. outer region of the atom; mostly empty
space
ii. electron-the negative particle located in
energy levels in the electron cloud;
involved in bonding
electron
neutron
proton
Video Clip
4. Neutral atoms have the same number of protons
and electrons.
5. Isotopes are atoms that have the same number of
protons but different numbers of neutrons. They
have the same atomic number but different
masses.
Click here for video clip
Click here for tutorial on isotopes
6. The atomic number of an element is the number of
protons it has in the nucleus. Video Clip
7. The mass number is the number of protons plus
the number of neutrons.
8. Atomic mass is the average mass of an atom of
a particular element.
Summary
Click here to practice calculating protons, neutrons, and
electrons
Subatomic Charge
Particle
Proton, p+
positive
Nucleus
Neutron, no neutral
Nucleus
Electron, e-
Electron
cloud
negative
Location
Mass
(amu)
1
Number in atom
Same as atomic
number
1
Mass number –
atomic number
1/1840 Same as number
of protons
II. Periodic Table (remember there is of one in your test
booklet)
A. Organization
1. The periodic table is organized by increasing
atomic number and is read from left to right.
2. Each vertical column is called a group or family.
All the elements in a family have the same number
of valence electrons
3. Each horizontal row is called a period. All
elements in the same period have the same
ending energy level (where electrons are found).
Video Clip
B. Get to know the arrangement
1 2 3
4
5
6
1.
2.
3.
4.
5.
6.
7.
8.
8
7
metals
nonmetals
metalloids
Alkali metals (most reactive metals)
Alkaline Earth metals
Transition metals
Halogens (most reactive nonmetals)
Noble gases (most unreactive elements)
C. Valence electrons are the electrons in the
outermost energy level of an atom.
III. Solutions
A. Solutions are homogeneous mixtures of two or
more elements and/or compounds. The major
component is called solvent, and the minor
components are called solute.
1. A solute is the dissolved substance in a
solution. There is less of it.
salt in salt water
sugar in soda
carbon dioxide in soda
2. A solvent is the dissolving medium. You have
more of it.
water in salt water water in sodas
Solutions Video Clip
3. Soluble – describes any substance that will
dissolve in a solvent
4. Insoluble – any substance that will not dissolve
in a solvent
Solubility video clip
B. Concentration-amount of solute dissolved in the
solvent
1. Concentrated vs. dilute
2. Saturation of solutions
a. Saturated – contains the maximum amount
of dissolved solute in a given amount of
solvent at a specific temperature and
pressure
b. Unsaturated – contains less than the
maximum amount of dissolved solute in a
given amount of solvent at a specific
temperature and pressure
c. Supersaturated – contains more than the
maximum amount of dissolved solute in a
given amount of solvent at a specific
temperature and pressure
C. Conductivity refers to the ability of a solution to
conduct electricity.
1. Electrolytes are substances that dissolve in water to
produce ions. These ions carry the electrical
current through the solution.
a. Strong electrolytes ionize completely in aqueous
(water) solutions.
b. Weak electrolytes are only partially converted to
ions in aqueous solution.
c. Examples of electrolytes
 ionic compounds such as NaCl (sodium chloride)
 acids and bases such as HCl (hydrochloric acid)
and NaOH
(sodium hydroxide)
2. Nonelectrolytes are substance whose aqueous
solutions do not contain ions and do not conduct an
electrical current. Click here to see NaCl dissolve