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Dmitri Mendeleev
Professor Dmitri Mendeleev published the first Periodic Table of the Atomic Elements in 1869 based on properties
which appeared with some regularity as he laid out the elements from lightest to heaviest. When Mendeleev
proposed his periodic table, he noted gaps in the table, and predicted that as-of-yet unknown elements existed
with properties appropriate to fill those gap.
He wrote names and properties of elements on cards. Then he arranged the cards by properties, such as density,
appearance, and melting point.
Mendeleev then ordered the elements by increasing atomic mass, a pattern began to appear.
–
When arranged by increasing atomic mass, those elements with similar properties occurred in
repeating patterns.
The Periodic Table
The periodic table of elements is a chart that provides valuable
information about all of Earth’s known elements.
There are eighteen columns on the periodic table. These columns
are called families or groups. Elements in the same family or
group have similar characteristics.
Families of the Periodic Table
There are 8 families on the periodic table that have specific names:
Family 1 – Alkali Metals
Family 2 – Alkaline Earth Metals
Family 13 – Boron Family
Family 14 – Carbon Family
Family 15 – Nitrogen Family
Family 16 – Oxygen Family
Family 17 – Halogens
Family 18 – Noble Gases (this family contains only gases)
Families 13-16 get their name from the first element in the family.
The other ten families (3-12) are called the transition metals.
The Periodic Table

The Elements:

Elements 1 (hydrogen) through 92 (Uranium) are the Natural Elements.


Building blocks of matter on earth.

43 (Technetium) and 84 (Polonium) are not found naturally on earth.
Elements 43, 84, and all elements beyond 92 are Artificial or Synthetic Elements.

Produced by nuclear reactions in the laboratory.
Vocabulary
Element – A substance that cannot be broken
down into smaller substances.
Atom – The smallest unit of an element.
Family – a column on the periodic table.
Group – another name for a family on the
periodic table.
Periodic Table
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Vocabulary
Family – a column on the periodic table.
Group – another name for a family on the periodic table.
Element – A substance that cannot be broken down into
smaller substances.
Atom – The smallest unit of an element.
Atoms are made up of subatomic particles.

Protons

Neutrons

Electrons
6
C
Carbon
12.011
Atomic Number – The number
of protons. Also the number of
electrons in an uncharged atom.
Symbol
Atomic Mass – The average total
mass of protons, neutrons, &
electrons.
Subatomic Particles
Protons – Have a positive (+) charge and are
located in the nucleus or center area of the
atom.
Neutrons – Have no charge/ or are neutral and
are located in the nucleus of the atom.
Electrons – Have a negative (-) charge and are
located outside of the nucleus.
Electrons are very small and move very fast making
their location difficult to pin point. The general area
where they are located is called an electron cloud or
orbital.
The Big Question
How are atoms of one element different from the
atoms of another element?
The atoms of each element has a different
number of protons.
This is distinguished by the atomic number – the
number of protons in the nucleus of the
atom/element.
Compounds
Compound - When two or more elements are held together by
chemical force or bond.


Ionic Bonds – A bond where electrons are transferred from one atom to
another.
Covalent Bonds – A bond where atoms share electrons.
Bonding – The combining of atoms.
Molecule – 1. The smallest particle of a substance that retains the chemical
and physical properties of the substance and is composed of two or more
atoms. 2. A group of like or different atoms held together by chemical
forces.
Ionic & Covalent Bonds
Atomic Charge & Ions
When an atom gains or looses an electron, the
atom is no longer neutral and therefore has a
charge.
An atom with a charge is an Ion.
The number of protons never change in an atom.
Water Molecule
Compound of Water
H2O


Hydrogen (H) – Colorless, odorless gas. Very light and
highly explosive when it meets air.
Oxygen (O) – A clear, colorless gas. Very flammable.
Water (H2O) – A nonflammable liquid.
The number of atoms in each compound are fixed in
ratio.
Water cannot be separated into H & O by physical methods – only a chemical
reaction can separate a molecule into it's component elements.
Metals
Non-Metals & Metalloids
States of Matter
Water can be found in solid, liquid and gas forms. How does this
happen?
Solid, liquid and gas are the names of different physical forms or
phases of matter. Also called States of Matter.
- Solids – Made of closely-packed atoms or molecules and
maintain a rigid form without a container.
–
Incompressible – Cannot be 'squeezed' down to a
smaller size.
States of Matter
- Solids
- Liquids – Made of closely associated atoms or molecules and
will flow to conform to the shape of the container.
–
Liquids are mostly incompressible.
- Gases – Made of mostly unassociated atoms or molecules and
will expand to fill a container.
–
Gases are compressible, their volume can be reduced
by applying force.
Solids
Solids are formed when attractive forces between
atoms are greater that the energy causing them
to move apart. The atoms are locked in position
near each other.
Crystalline Solid – A solid where atoms are in a
fixed, structured position.
–
Examples: Salt, diamond, quartz, ice.
Amorphous Solid – A solid with no structure.
–
Examples: Wax, many foods, like cotton candy.
Solids
In the solid phase, atoms cannot move past one
another. Even in this state, atoms still have
energy and move. Atoms in the solid phase
vibrate.
- As the temperature of a solid increases, the amount of vibration
increases. The solid will keep its shape until the amount of
energy added is greater than the attractive forces between the
atoms. Now the atoms start to move more freely... forming a
liquid.
The temperature at which a solid become a liquid
is called it's?
Melting Point
Liquids
In liquids, atoms can move past on another and
bump into each other. This is why liquids can
“flow” to take the shape of their container. Atoms
in a liquid still stay relatively close together.
-
As the temperature of a liquid and motion of the atoms is
increases, the amount of movement of individual atoms
increases. They bump into each other with increasing thermal
energy. Eventually some particles have enough energy to
“escape.” These atoms have entered the gas phase.
The temperature at which a liquid become a gas is
called it's?
Boiling Point
Gases
Atoms and molecules in the gas phase have little interaction with
each other. Gases have low density, meaning there are few
particles occupying a given space.
- Increasing the temperature of a gas increases the movement of
the gas particles. When in a fixed container the increased
movement of the gas will cause them to hit the walls of the
container with greater frequency and force. This creates
increased pressure.
Thermal Energy
Physical & Chemical Changes
Chemical Change – When one substance is
changed into something else. Irreversible.
Physical Change – A change in a substance
where the substance stays the SAME.
Reversible.
Mixtures and Compounds
Homogeneous & Heterogeneous
Mixtures
Examples of Mixtures
Chemical Changes
Possible Signs of a Chemical Change:
- Heat is produced that was not there before.
- Light is produced that was not there before.
- Fumes or smoke are produced.
- The substance fizz (means a gas phase material is being
produced.)
- Solid substances appear. Percipitate.
- Substances change color.
- Substances smell different.
Chemical Reactions
Factors that affect a chemical reaction:
- Increasing temperature
- Increasing pressure
- Increasing concentration
- Increasing particle movement (thermal energy)
- Increasing surface area.