Download Orbital - Uplift Education

Criteria
Quality of
work
Quantity of
work
Unacceptable
1
Work was not usable,
or regularly needed
major rework
Marginal
2
Work often had flaws
and omissions that
needed fixing
Did hardly any work.
Contributed OK,
somewhat less than
their share.
Usually met
commitments. Needed
some reminders or
follow-up.
Some interaction
problems,
unhelpfulness, or
failure to communicate.
Dependability Could not be counted
and meeting
on at all.
commitments
Very good
3
Generally high quality
of work, only
occasional fixes
needed
Worked hard, carried
their share of the load.
Outstanding
4
Amazingly good
output, well beyond
expectations
Drew out others and
ensured that everyone
participated, used and
encouraged the team
to use the class
meeting time
efficiently
Did everything well
and added some
outstanding
contributions
Considerable extra
work, more than their
share.
Conscientious about
Went out of the way to
commitments. Very
pick up slack for
dependable.
others who miss
commitments.
Interacted well with
Went out of the way to
others, helpful, flexible, help teammates and
pleasure to work with. enable them to
contribute.
Interaction,
supporting
other team
members,
sharing
information
Team
meetings:
participation,
use of team
time
Was a major problem
to interact and work
with.
Little participation in
discussions and
activities, wasted the
class team time.
Participation spotty:
not always
participative, did not
always use class team
time effectively
Participated fully in all
team activities, used
the class team time
wisely
Overall
Contributions
Rating
Often failed to
complete assigned
work, was difficult to
work with and made no
real contributions to
the team.
Sometimes failed to
complete assigned
work, was often
unprepared, but made
some contributions
Consistently good
contributions, valuable
member of the team,
and usually prepared
1. What is the definition of atomic number?
Number of protons in the nucleus
2. What is the definition of atomic mass?
Neutrons + Protons; mass of an
atom
D, E, Q
1
3
compare
and contrast
Mendeleev and Moseley’s
periodic tables.
explain the benefits and
drawbacks of the Bohr model of
the atom, and describe the
currently accepted theory of the
locations of electrons around an
atom.
By
1860, more than 60 elements
had been discovered
(How should we organize
all of these elements!?)
 Mendeleev
is
credited with
developing the
periodic table
(father of the PT!)
 Created
1869
his table in
 Mendeleev
arranged
the elements in order
of increasing atomic
mass and noticed
that certain similarities
in element’s properties
appeared at regular
intervals
Arranged
in
order of
increasing
atomic mass
Rows
and
columns
switched
 In
1911, Henry Moseley created a
periodic table that was arranged by
increasing atomic
number.
How is the PT organized today?
What is the main difference
between Mendeleev and
Moseley’s periodic table?
What are some similarities
between the two tables?
Natural States of the Elements
(solid/liquid/gas)
 explain
the benefits and drawbacks of
the Bohr model of the atom, and describe
the currently accepted theory of the
locations of electrons around an atom.

describe the
organization of the
electron cloud into
energy levels and
sublevels
 list
the amount of
electrons that can
fill each energy
level
What Bohr Did Right…
 Electrons
of increasing energy occupy orbits
farther and farther from the nucleus
 Electrons exist in quantized orbits (specific
energy levels).
 Electrons can’t exist between energy levels
Electrons can’t exist between energy levels, just like
people can’t stand between stair steps
With the partner who is sitting
next to you, create an analogy
about quantized energy
• Both partners need to contribute
to the final product
• Conversation should be on task
• 2 minute time limit!!
Draw your analogy/something
brilliant below:
Draw your analogy/something
brilliant below:
 Electrons
do not travel in neat,
planet-like orbits
This will blow your
mind!
+
Energy level= stair
Stairs contain shapes
Shapes contain orbitals
4.
3.
2.
1.
Orbital: a
three-dimensional
region around the nucleus
Each
orbital contains 2 electrons;
where the electrons spend 90%
of their time
Orbital
(Subshell)
Shape
Number of
Orbitals
Total number
of electrons
S
Sphere
1
2
P
D
F
Orbital
(Subshell)
Shape
Number of
Orbitals
Total number
of electrons
S
Sphere
Peanut
1
3
2
6
P
D
F
Orbital
(Subshell)
Shape
Number of
Orbitals
Total number
of electrons
S
Sphere
Peanut
Clover
1
3
5
2
6
10
P
D
F
Orbital
Shape
Shape
Number of
Orbitals
Total number
of electrons
S
Sphere
1
2
P
Peanut
3
6
D
Clover
5
10
F
Flower?
7
14
Whiteboard
directions/expectations
How many electrons can an orbital
hold?
How many electrons can an orbital
hold?
2
True or false?
Each energy level
contains shapes.
True or false?
Each energy level
contains shapes.
Answer: TRUE
How many electrons can the
S orbital shape hold?
How many electrons can the
S orbital shape hold?
Answer: 2
What is the shape of d
orbitals?
What is the shape of d
orbitals?
Answer: Clover
Name that orbital:
This orbital shape can hold
6 electrons and is shaped
like a peanut/dumbbell.
Name that orbital:
This orbital can hold 6
electrons and is shaped
like a peanut/dumbbell.
Answer: p orbital
Put your notes away!
How many orbitals does the f
orbital shape contain?
How many orbitals does the
f orbital shape contain?
Answer: 7
How many electrons does
the f orbital shape contain?
How many electrons does the
f orbital shape contain?
Answer: 14
What is the number of
orbitals in the p-shape?
What is the number of
electrons total in the pshape?
What is the number of orbitals in
the p-shape? What is the
number of electrons total in the
p-shape?
Answer: 3 orbitals; 6
electrons
Why was Bohr’s model
wrong?
Why was Bohr’s model wrong?
Electrons do not orbit the
nucleus on singular paths
(like planets around the sun)
Where do electrons have
more energy?
Closer or farther from the
nucleus?
Where do electrons have
more energy?
Closer or farther from the
nucleus?
Which electron has more
energy?
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