Download 1st block atomic structure ppts.

ChemI Block-1st: 3.4.15
Infinite Campus:
• Matter and Energy Exam-32 pts.
• Mapping Atomic Structure Lab-10pts.
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
1. What question(s) were you able to answer
correctly using your background knowledge?
2. What question(s) did you have trouble with
using your background knowledge? What
did you learn from your research last night?
Include the sources you used.
Atomic Ranking Task Worksheet
Answer qts. using:
1. Background Knowledge
2. Resources(textbook)-marker
Atomic Structure: Ranking Task
Atomic Number
Mass Number
Isotopes
Atomic Mass
ChemI Block-1st: 3.9.15
Due:
Define the following vocabulary words: atomic
number, mass number, and isotopes.
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 Structure: Bell Ringer
1. What is the atomic number for an atom?
2. Rank the following atoms from smallest to
largest based on atomic number?
a. N
b. H
c. F
d. O
3 . What is an atom’s 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?
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
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
Atomic Structure Lab
education.jlab.org
Mass Number?
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.
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
Element’s Atomic Numbers
ChemI Block-1st: 3.10.15
Due:
• Elements Subatomic Differences 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.)
Elements: Subatomic Differences
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)?
Isotope Worksheet
Homework:
• Annotate the passage on isotopes.
• Complete the worksheet (front and back)
ChemI Block-1st: 3.11.15
Due:
• Isotope 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.)
• I can calculate atomic mass for an element.
Elements :Isotopes
Isotopes
• What is an isotope?
ChemI Block : 2.25.15
Due:
• Mapping Atomic Structure Lab-Post Lab Qts.
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.)
• I can distinguish between mass number and atomic mass.
Isotopic Symbols
Isotope Applications
1. Calculate the number of protons, neutrons, and
electrons in each neutral isotope below.
Na-18
and
Na-23
ChemI Block-1st: 3.12.15
Due:
• Kandium Lab
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.)
• I can calculate atomic mass for an element.
• I can investigate the evolution of the atom.
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
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. O-16 and O-17
b. B-10 and B-11
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.
Kandium Lab
Purpose: To investigate an new element’s isotopes
and to calculate its atomic mass
Mass Number vs. Atomic Mass
• Mass Number:
• Atomic Mass:
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.
Calculating Atomic Mass of an Element
Atomic mass:
• It is an average mass calculated from all the isotopes
of a particular element.
• The average mass is weighted because there is NOT
an equal amount of each isotope in a sample.
• How do you calculate a weighted average 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
Isotope
Natural Abundance (%)
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.
ChemI Block : 3.13.15
Due:
• Kandium Lab
• Isotopes and Atomic Mass Worksheet
Objectives:
• Atomic Structure Quiz
• I can identify forces within an atom.
• I can investigate the evolution of the atom.
Homework:
Atomic Structure Study Guide-Test Tuesday
Element’s Isotopes and Atomic Mass
• Questions?
Atomic Structure Quiz
• Quiz includes the ranking task worksheet.
ChemI Block : 3.16.15
Due:
• Ranking Task Worksheet
• Atomic Structure Study Guide-reviewed
Objectives:
• I can identify forces within an atom.
• I can investigate the evolution of the atom.
• Atomic Structure Test-Wednesday!
Bell Ringer: Atomic Structure
1. If most of the atom is empty space, why is it matter
(made of atoms) does not pass through one another?
2. What keeps the protons from leaving the nucleus and
hooking up with the electrons?
Atomic Properties
• If most of the atom is empty space, why doesn’t
matter pass through one another?
• “The Space Between Atoms” video clip.
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.
Evolution of the Atom
• Rank the models of the atom from earliest to most
recent. (only use your background; context clues).
Evolution of the Atom
• Rank the models of the atom from earliest to most
recent. (only use your background; context clues).
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
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
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)