Unit 2 Chapter 4 Day 1 OBJECTIVE:

Explain how the Study of Atoms has changed in the last century and identify subatomic particles

• Do Now:• The Elements in the Body – a graph• TURN IN: Current Events

Today: • Chapter 4 Notes – Part 1

• Atoms and Atomic Structure• Thomson’s and Rutherford’s experiments

• P-N-E worksheets• Homework:

• Read Chapter 4.1 & complete 4.1 GRWS

New Chapter New Notebook

Unit 2 Chapter 4 Day 2 OBJECTIVE:

Explain how the Study of Atoms has changed in the last century and identify subatomic particles

• Do Now:• The Atom – Graphic Organizer

• Today: • Homework check and review 4.1 GRWS

• More P-N-E practice• What is Matter?

• Video: Bill Nye-Atoms & Molecules• Chapter 4 Notes – Part 2

• Ions, Isotopes and Excited Electrons• Homework:

• Chapter 4.2 GRWS

Unit 2 Chapter 4 Day 3 OBJECTIVE:

Discuss variations of atoms and Investigate the structural differences of hydrogen isotopes

• Do Now:• Atoms and Parts crossword puzzle

• Today: • Homework check and review 4.2 GRWS• Finish Chapter 4 Notes – Part 2

• Ions, Isotopes and Excited Electrons• LAB: Modeling Isotopes of Hydrogen• R & R Structure of the Atom

• Homework:• Finish R & R

Unit 2 Chapter 4 Day 4OBJECTIVE:

Construct and interpret Bohr’s models and Lewis dot diagrams for multiple elements

• Do Now:• What happens to Carbon if…• TURN IN HOMEWORK

• Today: • Return Unit 1 Test – Corrections Due TOMORROW• Intro - Chemistry Unit Project - Due Date = 4/1/15• Bohr and Lewis - Electron Models of the Atom

• “Bohr”ing practice and Making Lewis Dot Diagrams

• Homework:• Advertise-the-Elements project – Select your Elements!• Read Chapter 4.3 & complete GRWS• Progress Reports signed

Unit 2 Chapter 4 Day 5 OBJECTIVE:

Construct and interpret Bohr’s models and Lewis dot diagrams for multiple elements.

• Do Now:• Word Wise Chapter 4

• What are YOUR Elements?• Today:

• Homework check and Review 4.3 GRWS• Element Practice

• What Atom am I? Review Bohr’s /Lewis Models• LAB: Modeling the Location of an Electron in a Cloud

• Homework:• Textbook Chapter 4 Assessment pg 121+

#1 – 32 Complete sentences

PARCC BREAK

5 days of PARCC testing – no instructional classes!

Unit 2 Chapter 4 Day 6 OBJECTIVE:

Demonstrate understanding of atomic structure basics.

• Do Now:• Chapter Assessment Homework Check and Review

• Today: • Atomic Basics – Chapter 4 Quiz

• Homework:• Everyday Elements!• Advertise-the-Elements project Due 4/1/15

POP

Chapter 4

ATOMS and

AtomicStructure

Matter•The term matter describes all of the physical substances around us: your table, your body, a pencil, water, and so forth•Anything that has mass and takes up space (has volume)•Made up of different kinds of atoms•Includes all things that can be seen, tasted, smelled, or touched

Matter is made of atoms

Models

Models are often used for things that are too small or too

large to be observed or that are too difficult to be understood easily

Early Models of the Atom Democritus

Universe was made of empty space and tiny bits of stuff

Called these tiny bits of stuff atomos

Atoms could not be divided

Early Models of the Atom Dalton

All elements are composed of indivisible particles. Atoms of the same element are the sameAtoms of different elements are different. Compounds consisted of atoms of different elements combined together

Early Models of the AtomThomson

Plum pudding model

Atom made of a positively charged material with the negatively charged electrons scattered through it.

He discovered the ELECTRON!

Early Models of the Atom Rutherford

Mostly empty space

Small, positive nucleus

Contained protons

Negative electrons scattered around the outside

He discovered the PROTON!

Early Models of the Atom Bohr

Atom as a planetary arrangement

Electrons move in definite orbits around the nucleus

Modern Model of the AtomThe Electron Cloud

Sometimes called the wave modelSpherical cloud of varying density Shows where an electron is more or less likely to be (quantum mechanics)

Atomic Structure

Nucleus –Protons–Neutrons

Electrons

Electrons Tiny, very light particles

Have a negative electrical charge (-)

Move around the outside of the nucleus

Always moving – can move in any direction within their shell

Is equal to the number of protons

Protons Much larger and heavier than electrons

Protons have a positive charge (+)

Located in the nucleus of the atom 

Identifies the Atomic Number

Made up of smaller particles called quarks

NeutronsLarge and heavy like protons– 1840 times the mass of an electron

Neutrons have no electrical charge

Located in the nucleus of the atom

Made up of smaller particles called quarks

 

Describing Atoms

Atomic Number = number of protons

Mass Number = number of protons plus neutrons.

Atomic Mass (or Weight) = average mass of the naturally occurring isotopes of an element .

In a neutral atom, the # of protons = # of

electrons

5 6 7 8

B C N O11 12 14 16

Boron Carbon Nitrogen Oxygen

13 14 15 16

Al Si P S27 28 31 32

Aluminum Silicon Phosphorus Sulfur

Chapter 4

Atoms and Atomic Structure

Part 2

IonsAn atom that carries an electrical charge is called an ion– The number of protons does not change

in an ion– The number of neutrons does not

change in an ion

SO…both the atomic number and the atomic mass remain the same

IonsIf the atom loses electrons, the atom becomes positively charged (because the number of positively charged protons will be more the number of electrons)

If an atom gains electrons, the atom becomes negatively charged (more negative charges than positive charges)

IonsThis atom has lost an electron. Now it has one more proton than electron.

One more proton means one more positive charge.

This makes the total charge of the atom POSITIVE.This atom has gained an electron. Now it has one less proton than electron.

One less proton means one less positive charge.

This makes the total charge of the atom NEGATIVE.

IsotopesHave the same atomic number (number of protons) The number of protons for a given atom never changes.

The number of neutrons can change. 

Two atoms with different numbers of neutrons are called isotopes

Have different atomic mass numbers (number of protons + neutrons)

Three Isotopes of Hydrogen

Write symbols for each of the three Isotopes of

Hydrogen?

H H H

Protium Deuterium Tritium

Isotopes

Add or Subtract a PROTON

• NEW ELEMENT

Add or Subtract a NEUTRON • ISOTOPE

Add or Subtract an ELECTRON • ION

Atomic OrbitalsAn orbital is the region of space around the nucleus where an electron is likely to be found

The electron cloud model approximates how electrons behave in their orbitals.

Electrons and Energy Levels

Each electron in an atom has a specific amount of energy

Possible energies that electrons can have in an atom are called energy levels

An electron can move from one energy level to another when the atom gains or loses energy

Electron ConfigurationElectron configuration is the specific arrangement of electrons in orbitals.– Each energy level can only hold a specific

amount of electrons– Each energy level must be completely filled

before electrons fill the next level

The number of electrons in the outermost level are called valence electrons– These are the electrons used for bonding!

Electron Diagrams

Bohr and Lewis

Bohr’s Model of the Atom

Rules for filling the model– Start at the lowest energy level

• 1st energy level = 2 electrons(electrons #1 and 2)Place them opposite each other

• 2nd energy level = 8 electrons(electrons #3 to 10)Place them opposite each other -and-Make pairs for easier counting

• 3rd energy level = 18 electrons(electrons #11 to 28)

Bohr’s Model of the Atom

ELEMENT _____________

# Protons ________

# Neutrons ________

Bohr’s Model of the Atom

ELEMENT _____________

# Protons ________

# Neutrons ________

Lewis Dot Structures

Lewis dot diagrams are a simple way to show how the electrons are arranged in their outer shell.

This is where chemical reactions take place and how elements bond together.

Lewis Dot StructuresRules for filling the model:

ONLY VALENCE ELECTRONS

ARE USED

2

3 1

4

WHAT ARE

VALENCE ELECTRONS

?

Lewis Dot Structures VALENCE ELECTRONS are the electrons found in the OUTERMOST shell of the Bohr’s model.

ELEMENT _____________

# electrons (total) _______

# Valence electrons _______

ELEMENT _____________

# electrons (total) _______

# Valence electrons _______

ELEMENT _____________

# electrons (total) _______

# Valence electrons _______

Lewis Dot StructuresRules for filling the model:

ONLY VALENCE ELECTRONS

ARE USED

2

3 1

4

Lewis Dot Structures

Advertise-the-ElementsGeneral Information

Due date is Wed 4/1 at the beginning of class…Not after you finish gluing this on, or tying that together…Nor after you borrow my scissors and tape…NO…you must walk in here with it ready to turn in or it will be LATE! (Projects turned in after Spring Break cannot earn more than 50% credit MAX)

The Unit Project is worth as much as the Unit Test. Make that work for you.

Internet SourcesWikipedia (or Wiki-anything) is NOT an acceptable scientific source for this project and cannot be used as a source.

Cost for elements can be found on various sites. Try:Periodic Table of Elements: Los Alamos National Laboratory at http://periodic.lanl.gov/

OR even places like…

http://www.elementsales.com/pl_element.htm

Cool interactive periodic tables can be found at lots of sites…Try:

http://www.chemicalelements.com/ http://elements.wlonk.com/ElementUses.htm

http://education.jlab.org/itselemental/

Repeat…wiki-ANYTHING is not acceptable

• Try searching for your element in Science Journals. You could find innovative uses and new discoveries.