Today in ScienceYou will Need:1)Pencil, Colored Pencils, Highlighters or Markers2)Power Notes – Atomic Structure– 1 page 2 sides -Bookshelf

Final JeopardyYou will Need:1)Pencil

FINAL JEOPARDY• ANSWER: Complete the Chart

Item Has Mass

Definite Volume

Definite Shape

Takes the shape of container

What is it at room temp:Solid, Liquid, Gas, Plasma

Helium

H2O at 32 degrees C

Pencil

The element Mercury

FINAL JEOPARDY• ANSWER: Complete the Chart

Item Has Mass

Definite Volume

Definite Shape

Takes the shape of container

At room temp:Solid, Liquid, Gas, Plasma

Helium X X Gas

H2O at 32 degrees C

X X X Liquid

Pencil X X X Solid

The element Mercury

X X X Liquid

1.MANAGER– Log in to LearningPoint – Lead discussion

2. MATERIALS MANAGER– Organize Table Box

3. TIMER/DESIGNER– “Highlighting Patrol”

4.ORAL PRESENTER– Communicator, Asks Questions for the group

We are Changing Seats!!! !!

1.MANAGER– Log in to LearningPoint – Lead discussion

2. MATERIALS MANAGER– Organize Table Box (Colored Pencils, Markers, 4 rulers, glue sticks, tape, scissors, post-it notes)

3. TIMER/DESIGNER– “Highlighting Patrol”

4.ORAL PRESENTER– Communicator, Asks Questions for the group

Topic:

Power Notes- Atomic Structure

Do we understand everything????

Democritus 400 BC

Lavoisier 1789

• 1st idea of “atoms”• Believed all matter is made

up of tiny particles separated by space

• Named particles “atomos” which means indivisible.

• Founder of modern chemistry• 1st carefully controlled

experiments providing evidence to the Law of Conservation of Mass

France - provided the formula for the conservation of matter in chemical reactions, and also distinguished between an element and a compound

Greece - stated that all matter is made up of atoms.  He also stated that atoms are eternal and invisible and so small that they can’t be divided, and they entirely fill up the space they’re in

Dalton 1766-1844 1st MODERN Atomic Theory1.All matter made up of tiny indivisible particles called atoms2.Atoms of the same element have identical properties3.Atoms of different elements have different properties4.Atoms combine in a specific ratio to form compounds5.A specific compound is always made up of atoms in a specific proportion.

England - formed the 1st atomic theory, which states that all matter is composed of tiny, indestructible particles called atoms that are all alike and have the same atomic weight. 

Thomson 1897

Rutherford 1898

Plum Pudding Model1.Negative particles scrambled into the “dough” of the positive particles.

Gold Foil Experiment1.Atoms are mostly empty space2.All the Mass of an atom is in the positively charged ball in the center of the structure.

England - discovered the electron and developed the plum-pudding model of the atom.

England - used the results of his gold-foil experiment to state that all the mass of an atom was in a small posit ively-charged ball at the center of the atom. 

What is the difference between the EXPECTED RESULTS &OBSERVED RESULTS?

•Scientists look for patterns in data and passed experiments to PREDICT what they think might happen.•When scientists actually do an experiment their observed results may be different than what they EXPECT to happen because of passed information.•However, many times the expected results are in fact, what is observed.

Bohr 1922

Schrödinger (Schroedinger )

1930

“Planetary” atom model1.Believed the atom structure was like our solar system2. Nucleus in the middle like the sun and the electrons orbiting like the planets.

Wave Mechanic Model1.Planetary model was too specific2.Rather: electrons vibrate around the outside of the nucleus- can only predict where they are most like to be3.QUARKS – protons, neutrons and electrons made up of some of these smaller particles.4.http://library.thinkquest.org/05aug/01087/quarks.html

Denmark - stated that the electrons moved around the nucleus in successively large orbits. He also presented the Bohr atomic model which stated that atoms absorb or emit radiation only when the electrons abruptly jump between allowed, or stationary, states. 

Austria - introduced the Shroedinger Equation, a wave equation that describes the  form of the probability waves that govern the motion of small particles and how these waves are altered by external influences.

Basic Atomic Structure

Bohr Model for Lithium(not to scale)

Where is most of the mass in the Atom?

Where is most of the volume in the Atom?

Today scientists agree on the three basic subatomic particles that make up all atoms.

P= 3 +N = 3 0

Electron = 3

NUCLEUS

Outside the Nucleus; Electron Cloud

Make sure to include these question next to your model Answer

s

Nucleus

Electron

• Contains protons(+) and Neutrons (0)

• Holds most of the mass of the atom

• Very small compared to the entire size of the atom

• Most dense part of the atom

• Negatively charged subatomic particle

• Found outside the nucleus in the electron cloud

• Smallest particle; mass = 1/1836th of the atom

No need to include words…just i l lustration

Proton

Neutron

• Positively charged subatomic particle, Found in the nucleus

• Mass = 1 amu (atomic mass unit)• # of protons in an atom IDENTIFIES the

atom (which element)• # of protons in the nucleus of an atom

called the atomic number

• Zero charge• Mass = 1 amu• Do NOT affect the identity of the atom• Found in the nucleus• Same atom of an element can have

varying amounts of neutrons (isotope)• Adding the total number of protons &

neutrons = Atomic Mass Number

http://www.sawyerscience.com/Units/unit2/atoms_compounds.html

1. Atomic Number1. Number of PROTONS (Unique

to each element)2. Number of ELECTRONS (IF

Atom is NEUTRAL)2. Chemical Symbol

1. Abbreviation of element (some from LATIN name)

3. Element Name1. Full name provided below

symbol4. Atomic Mass Number

1. Sum of the particles in the nucleus

2. Represents total count of protons and neutrons

3. Positively charged because neutrons have no charge and protons are positive

Atomic Mass on the Periodic Table represents a “weighted average” of the mass of all the naturally occurring ISOTOPES of each element. (based on mass & abundance of each isotope.)

All atoms found on the Periodic Table are

Isotope

Hydrogen has 3 natural occurring ISOTOPES: Protium, Deuterium and Tritium

• NEUTRAL– same # of protons(+) and # of electrons(-)

• Atoms of the same element with same number of protons and different number of neutrons.

All ISOTOPES of Hydrogen are neutral because they have 1 electron as well . Make sure to include the electron in your i l lustration. (Did you put the electron in the right place?)

Al l are

HYDROGEN

because al l have

1 proton.

IONS

Review

REVIEW & REFLECT

• When atoms gain or lose electrons they become charged. (number of protons (+) and electrons (-) particles are NOT EQUAL)

• Atoms that do not have equal amounts of protons (+) and electrons (-) particles are called IONS

Draw atoms of hydrogen that are charged because of the UNEQUAL amounts of protons and electrons.

Short answer, no complete sentences. All answers are located in your notes.

+ - On ALL pages – Please do this with a colored pen, pencil or marker.

Homework1)None Unless you owe me something (We will continue working on Monday and Tuesday of next week)

2)Have a good weekend!

Do You see HOW the periodic table and the Atomic Structure are RELATED?