Chem I: 2/24Due:• Heat Calculation Problems Gallery Walk• Extra Energy Calculation Problems• Atomic Structure Ranking Task Worksheet Objectives:• I can locate and calculate subatomic particles in an atom.• I can predict properties of an atom based on subatomic

particles. • I can identify and compare isotopes of the same element. Homework:• Element’s Subatomic Particles Worksheet

Atomic Structure: Ranking Task Worksheet

• For each answer, rank the elements in increasing order. Ignore highest to lowest.

• Using textbook, make corrections to ranking task worksheet. Make sure to include evidence to support your answer. Use a colored pencil or pen to make corrections.

Atoms

What are we going to study about the atom?•History •Structure•Properties•Forces

Subatomic Particle

symbol charge location Mass (g)

mass # (amu)

proton 1.674 x 10 -24 1

electron 9.11 x 10-28 0

neutron 1.675 x 10 -24 1

Subatomic Particles in an Atom

Distinguishing Atoms

• What distinguishes one element’s atom from another element’s atom?

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What distinguishes each element below from one another?

Distinguishing AtomsAtomic number • The number of protons within an atom’s nucleus.• Its an atom’s I.D.• Atoms of the same element always have the same

number of protons.

• Do you notice any patterns with atomic numbers on the periodic table?

Element’s Atomic Numbers

What is the mass number for an atom?Subatomic Particle

symbol charge location Mass (g)

mass # (amu)

proton p+ +1 nucleus 1.674 x 10 -24 1

electron e- - 1 electron cloud

9.11 x 10-28 0

neutron n0 0 nucleus 1.675 x 10 -24 1

Chem I: 2/25Infinite Campus Update• Matter and Energy Exam (37pts.)• Heat Energy Problems-Gallery Walk (6pts.)• Extra Heat Energy Problems (10pts.)Due:• Ranking Task: Atomic Structure(yesterday’s modification clearly distinguished from initial

thoughts. )• Elements Subatomic Differences Wksht.

Element’s Subatomic Differences

Element AtomicSymbol

Atomic Number

Mass #(amu)

# of p+ # of n0 # of e-

What is the mass number for an atom?Subatomic Particle

symbol charge location Mass (g)

mass # (amu)

proton p+ +1 nucleus 1.674 x 10 -24 1

electron e- - 1 electron cloud

9.11 x 10-28 0

neutron n0 0 nucleus 1.675 x 10 -24 1

An Atom’s MassMass number : • The mass of a single atom.

• Sum of the p+ and n0 within an atom.

• Common unit: atomic mass unit (amu)

*The mass number is NOT the same as atomic mass located on your periodic table.

Atom’s Subatomic ParticlesProblem A: A cesium (Cs) atom has a mass of 133

amu and an atomic number of 55. a. How many p+, e-, and n0 are there?b.Illustrate a Cs atom, identifying where the

subatomic particles would be located. Problem B: An iron atom has an atomic number of

26 and consists of 30 neutrons. a. How many p+ and e- are there?b.What is iron’s mass number (amu)?

Matter and Energy Exam Evaluation• Class Average on Exam = 65%• How much time did you prepare for this exam?

• How did you prepare for this exam?

• What changes do you plan on making to improve your test scores?

• What grade do you want to earn in chemistry?

• What can I do to help you reach your goals?

Matter and Energy Exam • Make-up Assessment: Friday, Feb. 28th• Earn up to 5 points on original exam.• If made less than a B must take the make-up

assessment.

Isotope Worksheet

Homework:• Annotate the passage on isotopes.• Complete the worksheet (front and back)

Atomic Structure

• What do you predict the size difference is between an atom’s nucleus and its electron cloud?

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Isotope Worksheet

Homework: Due Wed., Feb. 26th• Annotate the passage on isotopes.• Complete the worksheet (front and back)

Chem I: 2/26Infinite Campus Update• Atomic Structure Bell RingerDue:• Isotope WorksheetObjectives:• I can locate and calculate subatomic particles in an atom.• I can predict properties of an atom based on subatomic

particles. • Complete “Mapping Atomic Structure Lab”• I can identify and compare isotopes of the same element.Homework: Analyzing and Illustrating Elements Isotopes

Mapping Atomic Structure LabData Section: • Need to include units with measurements.• Show work with calculations for credit. • Draw radius of atom on map.

Conclusion: • What does your data section inform you about the size

difference between the electron cloud and nucleus of an atom?

Atomic Model and Properties• If most of the atom is empty space, why doesn’t

matter (atoms) pass through one another?

• What keeps the protons from leaving the nucleus and being drawn towards the electrons?

Atomic Properties• “The Space Between Atoms” video clip.

spiff.rit.edu

Atomic Properties• “The Space Between Atoms” video clip.• Dr. Michio Kaku will be speaking at WKU on March

17th in the evening. If interested in seeing him let me know know. (getting seats reserved for Science Club).

spiff.rit.eduen.wikipedia.org

Atomic PropertiesIf most of the atom is empty space, why doesn’t

matter pass through one another?

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Atomic Model and Properties• If most of the atom is empty space, why doesn’t

matter (atoms) pass through one another?

• What keeps the protons from leaving the nucleus and being drawn towards the electrons?

Atomic Forces• Electrostatic Forces :- Forces between charged particles.Types of electrostatic forces:a. Attractive: (p+ and e-)b. Repulsion: (p+ and p+ e- and e-)• Nuclear Forces:Forces that holds p+ and n0 together in nucleus.

Chem I: 2/27Due:• Isotope Practice Problems

Objectives:• I can illustrate the difference between isotopes of the same

element.• I can distinguish between mass number and atomic mass.• I can calculate atomic mass for an element.

Homework: Review Matter and Energy concepts-Make-up tomorrow.

Isotopes• Atoms of the same element that differ in their

number of neutrons.

• What else is different about isotopes? They have different mass numbers (weights)

• They are observed to have similar chemical properties with one another.

Why?

Atomic Forces

1.What are the two types of forces within an atom?

2. Which force is stronger and how do you know this?

Chem I: Homework1. Calculate subatomic particles in each set of isotopes and

illustrate each isotope with correct location and number of subatomic particles.

a. Li-6 and Li-7b. H-1 and H-2c. O-16 and O-17d. B-10 and B-112. Research and state the difference between the following

atomic terms: mass number and atomic mass. *Record answers on separate sheet.

Illustrating Element’s Isotopes• Use gallery walk to ensure understanding of

differences between element’s isotopes.

• Assess peers understanding of element’s isotopes.

• Off-task or unproductive students will get a zero for assignment and receive additional work.

Isotope Applications1. Calculate the number of protons, neutrons, and

electrons in each neutral isotope below. Na-18 and Na-232. For each isotope, illustrate the location and

quantity of each subatomic particle in the atom.

3. Does Na-18 and Na-23 isotopes have similar chemical properties? Explain.

4. What did you learn is the difference between mass number and atomic mass?

Isotope Applications1. Calculate the number of protons, neutrons, and

electrons in each neutral isotope below. Na-18 and Na-232. For each isotope, illustrate the location and

quantity of each subatomic particle in the atom.

3. Does Na-18 and Na-23 isotopes have similar chemical properties? Explain.

4. What did you learn is the difference between mass number and atomic mass?

Isotope Applications

1. Calculate the number of protons, neutrons, and electrons in each neutral isotope below.

Na-18 and Na-23

2. For each isotope, illustrate the location and quantity of each subatomic particle in the atom.

3. Does Na-18 and Na-23 isotopes have similar chemical properties? Explain.

Isotopic Symbols• There are two isotopic symbols you need to know:

Mass Number vs. Atomic Mass• Mass Number:

• Atomic Mass:

Atomic mass:• It is an average mass calculated from all the isotopes

of a particular element. • It is a weighted average mass due to their being a

possible unequal distribution of isotopes in matter. • Located on the periodic table.How do you calculate atomic mass? 1. For each isotope, multiple its mass (mass #) by its

natural abundance (decimal form) to get the weighted mass for each isotope.

2. Add up the isotopes weighted masses to get the atomic mass (average mass) for the element.

Calculating Atomic Mass of an Element

Calculating Atomic Mass

Gold’s Isotopes Natural Abundance (%)

Homework:• Review for Matter and Energy Make-up Exam• Complete Atomic Mass Worksheet

Chem I: 2/28Due: • Atomic Mass Worksheet (front side)Objectives:• Chemistry Make-up Exam• I can locate and calculate subatomic particles in an

atom.• I can illustrate the difference between isotopes of

the same element.• I can distinguish between mass number and atomic

mass. • I can apply atomic mass with Kandium Lab.

Atomic Mass Worksheet

Kandium LabPurpose: • To analyze isotopes of Kandium and calculate its

atomic mass. Data:• Must show work for credit.• Don‘t forget to include units.

Conclusion/Post-Lab Sections: • Complete after the lab or homework

Evolution of an Atom

Chem I: 10/18Due: • Kandium LabObjectives:• I can distinguish between mass number and atomic

mass. • I can calculate atomic mass. • I can research the evolution of the atom. Homework:• Evolution of the Atom Worksheet

Kandium LabPurpose: To analyze Kandium’s isotopes and calculate

the atomic mass of this “new” element.

Kandium’s Isotopes:• Tartium• Beanium• Skittlium• Gummium

Chem I: 3/10Infinite Campus Update:• Ice Cream Lab• Ranking Task: Atomic Structure• Matter and Energy Make-up Exam• Mapping Atomic StructureDue: • Element’s Isotopes and Atomic Mass Worksheet• Kandium Lab

Atomic StructureObjectives:• I can identify, illustrate, and calculate subatomic

particles in an atom.• I can assess isotopes of the same element. • I can distinguish between mass number and atomic

mass. • I can investigate the evolution of the atom.

Elements Isotopes and Atomic Structure Worksheet

Element Isotopes NA (%)

AtomicNumber

MassNumber(amu)

protons neutrons electrons

chlorine Cl-35 75.88

chlorine Cl-37 24.22

Chlorine’s Atomic mass

Elements Isotopes and Atomic Structure Worksheet

Element Isotopes NA (%)

AtomicNumber

MassNumber(amu)

protons neutrons electrons

Kandium Lab

Infinite Campus Check-Up

• Assess infinite campus and record any missing or incomplete assignments.

• Discuss how you plan on making up any missing assignments. (RTI/GSH, ESS)

• Record current average.• Signature of student and parent• Due: Wednesday, March 12th.

Evolution of the Atom• Predict the developmental order of the atom. Rank them 1(earliest) to 5(current). Include your

reasoning for credit.

• Discuss ranking with a peer. Report similarities and differences. Were you persuaded to make modifications to your initial ranking, explain?

Evolution of the Atom• Predict the developmental order of the atom. Rank them 1(earliest) to 5(current). Include your

reasoning for credit.

• Discuss ranking with a peer. Report similarities and differences. Were you persuaded to make modifications to your initial ranking, explain?

Homework: • Validate your ranking with online resources. Complete questions 3-4.

Bell Ringer: Evolution of Atom• Who is given credit for the earliest model of the because he applied the scientific method?• What did Thomson’s model contribute to the atom?

• What did Rutherford’s model contribute to the atom?

• What did Bohr’s model contribute to the atom?

• What did Schrodinger’s (current) model contribute to the atom?

History of the Atom

•Great Thinkers (2,000yrs. Ago)

•Age of Reason and Thought

•Democritus vs. Aristotle view on the make-up of matter.

Democritus(400b.c.)Greek Philosopher

Democritus(400b.c.)Greek Philosopher

1) Observed matter to be made up of atoms.

2) Atoms are the smallest form of matter.

3. Atoms cannot be broken down.

3) The types of atoms in matter determine its properties.

Aristotle: Greek Philosopher (300b.c.)

• Aristotle observed matter to be made from four things:

earth, water, air, and fire

John Dalton’s Atomic Model

John Dalton’s Atomic Model

• English school teacher• Proved Democritus atoms

hypothesis using the scientific method.

• His conclusions produced:

Dalton’s Atomic Theory

1. Atoms are the building blocks of all matter.

2. Atoms cannot be subdivided.

3. Each element has the same kind of atoms.

4. A compound is composed of two or more atoms chemically combined in a fixed amount. Ex. NaCl

5. Atoms cannot be created or destroyed just rearranged during chemical reactions.

Dalton’s Atomic Theory

Thomson’s Plum Pudding Model

Thomson’s Cathode Tube Experiment

l-esperimento-piu-bello-della-fisica.bo.imm.c...

Subatomic Particle: ElectronJ.J. Thomson (pg. 105)• 1897 discovered electrons in gas atoms using a

cathode ray tube. • Determined electrons have a negative charge.• Electrons have the same charge in all atoms.

Robert Millikan: Determined the mass of the electron to be very tiny.

J. J Thomson’s Plum Pudding Model• If atoms are made of electrons how come most

matter does not shock us?• Atoms must have positive particles, too. • He proposed the Plum Pudding Atomic Model

• An atom is equally made up of positive and negative particles.

Goldstein’s Cathode Tube Experiment

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chemed.chem.purdue.edu

He discovered protons using a cathode ray tube. Observe particles moving in the opposite direction.

Subatomic Particles: Protons

• 1886 Eugen Goldstein observed particles traveling in the opposite direction of the cathode rays(electrons).

• He knew these particles must be (+) charged. They were called protons.

• Protons charge is the same for all atoms• Protons have a significant mass compared to

the electron.

Rutherford’s Model of the Atom

green-planet-solar-energy.com

Rutherford’s Gold Foil ExperimentIf positively charged light particles traveled through a sample of matter composed of atoms with protons and electrons evenly distributed throughout the atom, what would happen to the trajectory (path) of the + charged light particles as it passes through these atoms?

Rutherford’s Gold Foil Experiment

Rutherford’s Conclusion

•Most of the atom is empty space.

•Small dense region composed of (+) charged particles.(Nucleus)

Rutherford’s Nuclear Atomic Model

•What keeps the protons within the nucleus ?(Like particles repel each other)

•1932 - James Chadwick discovers that the nucleus also has neutral particles present. He called them neutrons.

Subatomic Particle: Neutron

Chadwick’s Experiments: Neutron

nobelprize.org

Bohr’s Model of the Atom

http://micro.magnet.fsu.edu/

Bohr’s Model of the Atom

http://micro.magnet.fsu.edu/

Bohr’s Model of the Atom

http://micro.magnet.fsu.edu/

•Electrons travel in fixed, circular paths around the nucleus.•Each path has a specific energy requirement.•These circular paths are called energy levels.•Limited number of electrons on each energy level. (2n2 Rule)

Current Atomic Model

Erwin Schrodinger

Current Atomic Model

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science.howstuffworks.com

Erwin Schrodinger

Current Atomic ModelElectrons do not travel in fixed paths around the nucleus

Electrons constantly move to different energy levels in the electron cloud.

Direction of movement is dependent upon how much energy an electron has.

Observed several different paths electrons can take around the nucleus.

Types of electron paths around nucleus

Bell Ringer: History of AtomAtomic Model Illustration Description

Dalton’s Model

Thomson’s Model

Rutherford’s Model

Bohr’s Model

Schrodinger’s Model (current model)

Atomic Models

Dalton’s Atomic Model Thomson’s Plum Pudding Model Rutherford’s Nuclear Model

Bohr’s Planetary ModelSchrodinger’s Atomic Model(current model)

Bell Ringer

1. Compare the different views Aristotle and Democritus had about what matter was made of.

2. Which Greek philosopher was correct ?3. Which later scientist proved his view?

Bell Ringer:4. a. Identify and explain this Atomic Model?

b. Who concluded this atomic model?

Bell Ringer5. Look at the following experiment below.a. What was this experiment called?b. Who developed this experiment?c. Did his experiment prove or disprove the

Plum Pudding Model?

Rutherford’s Conclusion

•Most of the atom was empty space.•Small dense region composed of (+) charged particles. (nuclues)

Rutherford’s Atomic Model

Rutherford’s Nuclear Atom Model

•What keeps the protons within the nucleus ?(Like particles repel each other)

•1932 - James Chadwick discovers the nucleus also has neutral particles present. He called them neutrons.

•Neutrons have a significant mass like protons.

Subatomic Particle: Neutron

Modern Atomic Model