ChemI Block : 2.23.14Due: •Atomic Structure Ranking Task Worksheet

Objectives:•I can illustrate the composition and size of an atom. (Ranking Task Wksht. /Basketball Lab)•I can predict properties of an atom based on its atomic structure. (Ranking Task Wksht.)•I can distinguish between isotopes of the same element. (Atomic Structure Wkshts.)

Atomic Ranking Task WorksheetAnswer qts. using:1.Background Knowledge

Atomic Ranking Task Worksheet

Answer qts. using:1.Background Knowledge2.Resources(textbook)-marker

Atomic Structure: Ranking TaskAtomic # ? Mass # ? Atom I.D. ? Istopes ?

Atomic 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?

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

Mass NumberMass 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.

Atomic Structure: Ranking Task Worksheet

Answered Qts. using….1.Background Knowledge2.*Peer Collaboration*3. Resources (text/internet)

Atomic Number ?

Atomic Structure: Ranking TaskAtomic # ? Mass # ? Atom I.D. ? Istopes ?

1. # of p+ in an atom.

2. # of (p+) and (n0) in an atom.

3. # of p+, n0, and e- in an atom.

4. atomic mass- protons.

Atomic 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

Mass Number?

Atomic 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?

Mass NumberMass 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.

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

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

Isotopes?

ChemI Block : 2.24.14Due: •Atomic Structure Ranking Task Worksheet

Objectives:•I can illustrate the composition and size of an atom. (Ranking Task Wksht. /Basketball Lab)•I can predict properties of an atom based on its atomic structure. (Ranking Task Wksht.)•I can distinguish between isotopes of the same element. (Atomic Structure Wkshts.)

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

Atomic Structure• Atomic Number?

• Mass Number?

• Isotopes?

Atomic 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?

Mass NumberMass 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.

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

Isotopes

• What are isotopes?

Bell Ringer: Atom’s Subatomic Particles1. : 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 where the subatomic particles are

located within the cesium atom. 2.: An iron(Fe) 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)?

Bell Ringer: Atom’s Subatomic Particles1. : 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 where the subatomic particles are

located within the cesium atom. 2.: An iron(Fe) 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)?

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.

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.

Mapping Atomic Structure LabPurpose: Model the size difference between the nucleus and the electron

cloud. Data 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?

Chem I Block : 9.25.14

Objectives:•I can illustrate the composition and size of an atom. (Ranking Task Wksht. /Basketball Lab)•I can predict properties of an atom based on its atomic structure. •I can distinguish between isotopes of the same element.

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.

What distinguishes each element below from one another?

Distinguishing Atoms

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

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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)?

Isotopes

• Annotate resource and complete practice problems on front.

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.

Atomic Structure

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

education.jlab.org

ICP: 9/29

Due:• Isotope Worksheet Objectives:• I can distinguish between isotopes of the same element. • I can illustrate the composition and size of an atom.

(Ranking Task Wksht. /Basketball Lab)• I can predict properties of an atom based on its atomic

structure.

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?

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

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.

Isotope Worksheet

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

Isotope Worksheet

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

Chem I: 9/26

Due:• Mapping Atomic Structure Lab • Atomic Mass Worksheet Objectives:• I can illustrate the composition and size of an atom.

(Ranking Task Wksht. /Basketball Lab)• I can predict properties of an atom based on its atomic

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

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

matter pass through one another?

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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: 9/29Due:• Isotope Worksheet• Kandium Lab• Evolution of the Atom (qts. 1)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. • I can investigate the evolution of the atom.

Homework:

Isotope Applications3. Calculate the number of protons, neutrons, and electrons in each neutral isotope below. Na-18 and Na-234. For each isotope, illustrate the location and quantity of each subatomic particle in the atom. 5. Does Na-18 and Na-23 isotopes have similar chemical properties? Explain.

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

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, multiply 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.

Chemistry I Block: 9.30.14Due: • Kandium Lab• Evolution of the Atom packet

Objectives:• 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.

Atomic Structure Review: Bell Ringer

1. Identify the number of protons, neutrons, and electrons for each isotope of Rb. 2.Does Rb-86 and Rb-87 isotopes have similar chemical properties? Explain how you know this. 3.a.Calculate the atomic mass of Rubidium. b. What is the difference between mass number and atomic mass? 4.a. Distinguish between the two types of forces within an atom. b. Which force is stronger? Explain how you know this.

Rubidium’s Isotopes Natural Abundance (%)

Rb-86 72.2

Rb-87 27.8

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?

Chem I: 10/01.14Due:• Evolution of the Atom (qts. 1)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. • I can investigate the evolution of the atom.

Homework: Atomic Structure Study Guide

Evolution of the Atom

Chem I: 10/02.14Due:• Subatomic Particles Wksht. 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. • I can investigate the evolution of the atom.

Homework: • Review for Atomic Structure Test

History of the Atom

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.

4) 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

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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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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

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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

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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

Chem I: 10/02.14Due:• Evolution of the Atom PacketObjectives:• 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. • I can investigate the evolution of the atom.

Homework: Atomic Structure Study Guide-Test Friday

Atomic ModelsAtomic Model Illustration Description

Dalton’s Model

Thomson’s Model

Rutherford’s Model

Bohr’s Model

Schrodinger’s 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)