ChemI Block : 2.23.14
Due:
• 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 Worksheet
Answer qts. using:
1. Background Knowledge
Atomic Ranking Task Worksheet
Answer qts. using:
1. Background Knowledge
2. Resources(textbook)-marker
Atomic Structure: Ranking Task
Atomic # ?
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 Particles in an Atom
Subatomic symbol charge
Particle
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
Mass Number
Mass 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 Knowledge
2. *Peer Collaboration*
3. Resources (text/internet)
Atomic Number ?
Atomic Structure: Ranking Task
Atomic # ?
1. # of p+ in an
atom.
2. # of (p+) and (n0)
in an atom.
3. # of p+, n0, and ein an atom.
4.
atomic mass- protons.
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?
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 Number
Mass 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 Particles in an Atom
Subatomic symbol charge
Particle
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 symbol charge
Particle
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
Isotopes?
ChemI Block : 2.24.14
Due:
• 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 Particles in an Atom
Subatomic symbol charge
Particle
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
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 Number
Mass 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 Particles in an Atom
Subatomic symbol charge
Particle
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
Isotopes
• What are isotopes?
Bell Ringer: Atom’s Subatomic Particles
1. : 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 Particles
1. : 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: Homework
1. 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-7
b. H-1 and H-2
c. O-16 and O-17
d. B-10 and B-11
2. Research and state the difference between the following
atomic terms: mass number and atomic mass.
*Record answers on separate sheet.
Chem I: Homework
1. 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-7
b. H-1 and H-2
c. O-16 and O-17
d. B-10 and B-11
2. Research and state the difference between the following
atomic terms: mass number and atomic mass.
*Record answers on separate sheet.
Mapping Atomic Structure Lab
Purpose:
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
education.jlab.org
• What distinguishes one element’s atom from another
element’s atom?
Atom’s Subatomic Particles
Problem 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: Homework
1. 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-7
b. H-1 and H-2
c. O-16 and O-17
d. B-10 and B-11
2. Research and state the difference between the following
atomic terms: mass number and atomic mass.
*Record answers on separate sheet.
Atomic Structure
education.jlab.org
• What do you predict the size difference is between
an atom’s nucleus and its electron cloud?
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 Lab
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?
What is the mass number for an atom?
Subatomic symbol charge location
Particle
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 symbol charge location
Particle
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 Mass
Mass 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 Properties
If most of the atom is empty space, why doesn’t
matter pass through one another?
spiff.rit.edu
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: 9/29
Due:
• 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 Applications
3. Calculate the number of protons, neutrons, and
electrons in each neutral isotope below.
Na-18
and
Na-23
4. 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:
Calculating Atomic Mass of an Element
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
Gold’s Isotopes
Natural Abundance (%)
Homework:
• Review for Matter and Energy Make-up Exam
• Complete Atomic Mass Worksheet
Chem I: 2/28
Due:
• 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: 9.30.14
Due:
• 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
Rubidium’s Isotopes
Natural Abundance (%)
Rb-86
72.2
Rb-87
27.8
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.
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: 10/01.14
Due:
• 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: 10/02.14
Due:
• 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
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.
Thomson’s Plum Pudding Model
Thomson’s Cathode Tube Experiment
l-esperimento-piu-bello-della-fisica.bo.imm.c...
Subatomic Particle: Electron
J.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
chemed.chem.purdue.edu
reich-chemistry.wikispaces.com
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 Experiment
If 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
Subatomic Particle: Neutron
•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.
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
•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)
http://micro.magnet.fsu.edu/
Current Atomic Model
Erwin Schrodinger
Current Atomic Model
Erwin Schrodinger
blogs.stsci.edu
science.howstuffworks.com
Current Atomic Model
Electrons 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: 10/02.14
Due:
• Evolution of the Atom Packet
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-Test Friday
Atomic Models
Atomic Model
Dalton’s Model
Thomson’s Model
Rutherford’s
Model
Bohr’s Model
Schrodinger’s
Model
Illustration
Description
Atomic Models
Dalton’s Atomic Model
Bohr’s Planetary Model
Thomson’s Plum Pudding Model
Rutherford’s
Nuclear Model
Schrodinger’s Atomic Model
(current model)