BLOCK DAY BELLWORK
1. Pick up your textbook, the notes slip and the
PowerPoint notes handout.
2. Either glue into your comp book or staple to your
packet the 2 notes sheets.
3. Take out your packet and finish page 2 and the
Periodic Table coloring and labeling activity.
4. Make sure you have re-read all of the information I
gave to you on pages 2-4 in the packet.
5. Read the PowerPoint handout on the groups/families
of the periodic table, then think about how each
group is different.
6. Read Chapter 5 in your textbook.
7. Pick up an extra credit sheet from the front counter
called “An Alien Periodic Table”
Scientist
Discovery
Picture
Democritis The 1st person Around 430BC
to propose the
idea of the
atom
John
Proposed
Dalton - the ATOMIC
1802
theory
Thompson- Discovered that
1897
atoms have
negative
ELECTRONS and
thought they were
spread throughout
a positive ball
Rutherford- Discovered that
1909
positive PROTONS
are in a NUCLEUS
and electrons
move around them
Bohr-1913 Electrons
move in rings
around the
nucleus
Schroding Electrons are
er-1920
in a “cloud”
around the
nucleus
Chadwic Discovered
k-1932
NEUTRONS
in the
nucleus
Dalton’s Atomic Theory
Although two centuries old, Dalton's atomic theory remains
valid in modern chemical thought. Modern atomic theory is,
of course, a little more involved than Dalton's theory but the
essence of Dalton's theory remains valid.
1) All matter is made of atoms. Atoms
are indivisible and indestructible.
2) All atoms of a given element are
identical in mass and properties
3) Compounds are formed by a
combination of two or more different
kinds of atoms.
4) A chemical reaction is a
rearrangement of atoms
Metals, Nonmetals
and Metalloids
Coloring in the Periodic Table
Notice the difference between the appearance of the
metals and nonmetals.
Click here for a better view of each of the elements.
Physical properties of METALS
• Metals are SOLIDS.
(except mercury)
• Metals are HARD.
(except Lithium, Potassium, Sodium)
Physical Properties of METALS
Metals have shiny luster. (or metallic luster)
LUSTER – the way an object’s surface
reflects light
When you leave a spoon in a cup of hot drink, the bit
poking out of the drink gets hot. Why? Conduction!
METALS are the best conductors of heat.
This is because the electrons in metals move more freely than
in non-metals, allowing the heat energy to travel across the
metal.
For example, when the spoon touches the hot drink, the heat
from the drink excites the electrons in the metal, and the
electrons transfer the energy from one electron to another,
carrying the heat all the way up the spoon quickly.
Best conductors:
silver and copper
Physical Properties of METALS
• Metals are good conductors of electricity.
Copper, silver, and gold are good electrical
conductors. In a conductor, electric current
can flow freely. Since metals have free
electrons, they can carry a charge easily.
Copper Wiring
Physical Properties of METALS
Metals are malleable.
Malleable or Malleability - metals ability to be
shaped or formed as by hammering or pressure; can be
beaten into thin sheets
Aluminum is malleable.
Physical Properties of METALS
Metals are ductile.
Ductility or ductile – can be drawn into
a wire
Examples of NONMETALS
Non metals may be solids, liquids or gases.
Examples:
Solids – Carbon, Sulfur, Phosphorus
Liquid – Bromine
Gases – Oxygen, Hydrogen, Nitrogen
Physical Properties of
NONMETALS
Nonmetals have a dull luster.
(They are not shiny!)
Example: Phosphorus
Physical Properties of NONMETALS
Nonmetals are insulators.
They do not conduct electricity or
heat well.
The atoms in nonmetals do not have
loose electrons. Therefore, when
electricity, or something hot touches a
non-metal, the energy does not move
quickly through the material.
What would you rather stir a hot pot
with—a wooden spoon or a metal spoon?
Physical Properties of
NONMETALS
Nonmetals are soft (except for diamonds
and brittle.
Example: Sulfur
An interesting element: Carbon
Ever break the point of your
pencil? That’s because it’s
made of graphite, a substance
made up completely of
Carbon—a brittle nonmetal.
However diamonds, the hardest
material of all, are made of the
same element: Carbon. Look at
how the carbon atoms are
arranged in diamonds—why do
you think diamonds are harder
than graphite?
Carbon
atoms in
graphite
METALLOIDS
The elements contained in the classification of Metalloids:
METALLOIDS
• Elements classified as Metalloids have physical
properties of both metals and non-metals.
• Some are shiny, some are dull, they are
somewhat malleable and ductile, and can
conduct heat and electricity at a lesser level than
metals.
SILICON
BORON
ARSENIC
METALLOIDS
• Some metalloids are useful semiconductors,
which are used in electronics (radio, computers,
telephones, etc.)
• They are useful because they conduct just the
right amount of electricity or heat.
Where do we find METALS?
Some metals like gold, silver, and platinum are
found as pure substances in the earth’s crust
because they are least reactive.
Most metals are reactive and are found as oxides
(react with oxygen), carbonates (react with carbon),
sulfides (react with sulfur).
Minerals : are elements or compounds which
occur naturally inside the earth’s crust.
Ore : is a mineral from which metals can be
extracted profitably.
In your packet…
• There are 2 charts to fill out classifying
properties of metals, nonmetals and
metalloids
Important Vocabulary
• Valence Electrons
• Bohr Diagram
• Lewis Dot Diagram/Lewis Structure
• https://www.youtube.com/watch?v=rSwnO
DMNULI&feature=youtu.be
Bohr Diagrams
and
Lewis Dot Structures
What you’ve already learned
in class and from readings
• You learned that Electrons can exist
in different energy levels
• You learned that the # of Electrons in
an atom are equal to the # of Protons
in an atom
• You learned that the # of Valence
Electrons are the outermost Electrons
of an Atom
What You’re about to learn
(Find it in your Packet!)
1. How to draw the Electrons
around an Atom in a Bohr
Diagram
2. How many Electrons are
found in any Element’s
Valence Shell
3. How to draw a Lewis Structure
Notes
• A Bohr Diagram is the model of an atom
with the Nucleus at the center, and the
Electrons drawn around it on different
energy levels.
First Steps in Bohr Model
• Find the amount of each subatomic
particle in the atom
p=
e=
n=
• Know how many electrons can fit in each
ring and write the electron configuration
– 2-8-18-32
Now for some practice
•
•
•
•
For an Atom of Hydrogen:
1 Electron!
The electron configuration is just 1
Simple, you just draw the first Electron here
• The number of protons and neutrons get
written in the nucleus.
Next
• For an Atom of Helium:
• 2 Electrons! The electron configuration is 2
• Simple, you just draw the second Electron
here
More
• For an Atom of Lithium:
• 3 Electrons!
• But wait a minute…We said that only 2
Electrons can fit into the first level
• So What do we do when it’s full????
WE ADD ANOTHER LEVEL!!!
• That’s right, the first energy level is full
• Now we add another level!!!
• This new level can hold up to 8
Electrons!!!
So
• For an Atom of Lithium:
• 3 Electrons! The electron configuration is 2-1
• Simple, you just draw the third Electron here
Then What?
• When you run out of room on
the second level, you add a
third that can hold another 18
Electrons, then a fourth that
can hold another 32 Electrons,
(but we won’t worry about that
level right now)
You should Know by Now
• How to draw a Bohr Diagram
• That the
–1st energy level can hold 2 e–The 2nd can hold 8 e–The 3rd can hold 18 e-
Finally: Lewis Structures
• All you have to do for a
Lewis Structure is draw
Dots around an Element’s
Symbol
• But How Many????
What you are about to learn
1. How many Electrons are
found in any Element’s
Valence Shell
2. How to draw a Lewis
Structure
So…
• The amount of dots you
draw for a Lewis Structure
(LS for short) is equal to the
# of Valence Electrons in an
Atom
Valence Electrons
• The # of Valence e- an
atom has is dictated by the
Group the Element is in
• Groups are the Vertical
Columns on the Periodic
Table!!! It’s So Simple!!!!
Review of Terms
(make sure in notes!)
•
•
•
•
Electron configuration
Valence electrons
Bohr Diagram
Lewis Dot Diagram/Lewis Structure
To Do
1. Finish all of pages 1-5 in your packet.
Make sure you understand all content – ask
questions if you need to.
2. Read and complete Chapter 5 in your
textbook.
3. Alien Periodic Table Extra Credit Challenge
If time, we will do an element matching card
activity and go over pages 1-5 after I check
them in your packet – show me when