Unit 4: Electron Configuration, Periodic Trends and ... · PDF fileThis is the electron...
Transcript of Unit 4: Electron Configuration, Periodic Trends and ... · PDF fileThis is the electron...
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Do Now:
Pick up sheets by the door (note
packet and homework packet if you
didn’t pick one up last week)
Take out completed homework #1
Take out Atoms Book
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Review before the quiz
_____1) Bohr’s model of the atom says that electrons
a) are mixed in evenly with positive charge
b) are found orbiting a positively-charged nucleus
c) are found orbiting a positively-charged nucleus in energy levels (shells)
d) are found in regions of probability around the nucleus called orbitals
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Review Before the Quiz
_____5) Dalton’s model of the atom
states that atoms
e) have positive particles called protons
and negative particles called electrons
f) have a positively-charged nucleus
g) have a positively-charged nucleus with
electrons in energy levels (shells)
h) are hard solid indivisible spheres
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Review Before the Quiz
One model of the atom states that atoms are tiny particles composed of a uniform mixture of positive and negative charges. Scientists conducted an experiment where alpha particles were aimed at a thin layer of gold atoms. Most of the alpha particles passed directly through the gold atoms. A few alpha particles were deflected from their straight-line paths. (This question was taken directly from a Regents Exam).
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Review before the quiz
Most of the alpha particles passed
directly through the gold atoms
undisturbed. What does this evidence
suggest about the structure of gold
atoms?
Atoms are mostly empty space
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Review before the quiz
A few of the alpha particles were
deflected. What does this evidence
suggest about the structure of the gold
atoms?
The nucleus must be positive since it
deflects positively charged alpha
particles
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Quiz-E-Poo time
9.5 minutes
Can use your notes/atom book. Turn
ALL OF IT IN when you are done
Atom Book
Homework
Quiz
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Quiz
Name
Answers ¼ sheet of paper
Name that model!
1) Atoms look like solid spheres
2) Atoms are mostly empty space
3)Electrons are found in distinct levels similar
to the path of planets around the sun
4) The most ‘up-to-date’ model
5) The first model to include electrons
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Objective
Describe the difference between a full
and an occupied energy level
What is an energy level?
When is it full?
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I. The Bohr Atom
Bohr was the first to propose that the
electrons were located in energy levels
A lower case “n” is used to denote
these principle energy levels (also
called principle quantum numbers).
The level closest to the nucleus is
labeled n = 1. The next level is labeled
n = 2 and so forth.
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I. The Bohr Atom
Each principle energy level had a certain
energy value associated with the level.
The closer the level was to the nucleus,
the lower the energy of the level.
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I. The Bohr Atom
As long as the electrons were in these
levels, the electrons do not give off
energy.
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Number the principle Energy levels
1
2
3
4 5
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2. Electron Configuration and the
Periodic Table
Each principle energy level can only
hold so many electrons before the level
is full.
A quick and easy way to determine the
maximum number of electrons (max e-)
that a principle energy level can hold is
given by the following:
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max e- = 2 n2.
First square the principle energy level
number (n) then multiply by 2
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2n2 Trick
Principle Energy
Level (n)
Maximum
Electrons
1
2
3
4
5
6
2
8
18
32
50
72
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Electron Configuration
Electrons are arranged around the
nucleus by filling up the first principle
energy level (n=1), then the second
energy level, etc. (with some exceptions
that we will get to later in the unit…)
This is the electron configuration given
on your periodic table.
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Electron Configuration
The number of electrons
are listed for each level with
a dash between levels:
for oxygen (O) which has a
total of 8 electrons, the
configuration is 2–6
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Electron Configuration
2 electrons are located in
the first principle energy
level
6 electrons are located in
the second principle
energy level.
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Look up the electron config. on
the PT for the element given &
fill in the chart.
Element n = 1 n = 2 n = 3 n = 4
Ca 2 8 8 2
Na
F
B
2 8 1
2 7 2 3
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Look up the electron config. on
the PT for the element given &
fill in the chart.
Element n = 1 n = 2 n = 3 n = 4
Al
C
H
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Side Bar: Look up # 72 Hf
What does the ** mean?
So the electron configuration of Hf is…..
2-8-18-32-10-2
What is the electron configuration of gold (Au)
# 79?
2-8-18-32-18-1
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ADDITIONAL INFORMATION
Ions: atoms with a charge because of
gaining or losing an electron
Gained an electron (-) charge
Lost an electron (+) charge
How would an Ion’s configuration
compare to a neutral atoms?
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Ion Electron configuration
Al Configuration :
Al+3 Configuration:
Na Configuration:
Na+1 configuration:
Cl configuration:
Cl-1 configuration:
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Ion Configuration
Negative charge gained that many
more electrons
Positive charge lost that many
electrons
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Completely Filled vs. Occupied Principle
Energy Levels
Is this room occupied?
Is this room filled?
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Completely Filled vs. Occupied Principle
Energy Levels
Occupied means that
there is at least one
electron in the Principle
Energy Levels (PEL)
Li: 2 – 1 has 2 occupied
PELs
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Completely Filled vs. Occupied Principle
Energy Levels
Completely Filled means that each level has its maximum number of electrons which can be determined by the 2n2 rule.
n =1 then 2(1)2 =2
& n = 2 then 2(2)2=8
Li: 2 – 1 has only 1 Completely Filled PEL
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To help you review the 2n2 rule
complete the following chart
PEL
(n)
1 2 3 4 5 6 7
Max
e- 2 8 18 32 50 72 98
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In the chart:
Copy the electron configuration from the
Periodic Table
Determine the number of Occupied
Principle Energy Levels (PEL)
Determine the number of Completely
Filled Principle Energy Levels
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Max e-: 2-8-18-32-50-72-98
Elemen
t
Electron Conf. #
ocup
p
#
compl
filled
C 2 1 2-4
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Max e-: 2-8-18-32-50-72-98
Elemen
t
Electron Conf. #
ocup
p
#
compl
filled
Na
O
Cl
2-8-1
2-6
2-8-7
3 2
2 1
3 2
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Max e-: 2-8-18-32-50-72-98
Elemen
t
Electron Conf. #
ocup
p
#
compl
filled
He
F
Ne
2
2-7
2-8
1 1
2 1
2 2
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Max e-: 2-8-18-32-50-72-98
Elemen
t
Electron Conf. #
ocup
p
#
compl
filled
Si
Zn
Au
2-8-4
2-8-18-2
2-8-18-32-18-1
3 2
4 3
6 4
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Ticket out
How many full energy levels are there in
an atom of Gold (Au)?
Done: Do homework #2, all except the
last problem
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Do Now
Take out your notes packet (page 4)
Read how to draw bohr diagrams and
attempt the first box (For F: Atomic #__)
OBJECTIVE: Draw accurate bohr
models of atoms
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3. Drawing Bohr Diagrams of
Atoms:
1) A circle is used for the nucleus- the
# protons (# p or +) and the # of
neutrons (#n) are placed in the circle.
2) A ring is drawn around the nucleus
for each energy level.
3) The electrons for each energy level
are placed in pairs symmetrically
around the nucleus
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For Fluorine (F)
atomic # = _________
atomic mass = ______
electron configuration:
__________________
_
# p =
______________
# n
=_______________
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For Aluminum (Al)
atomic # = _________
atomic mass = ______
electron configuration:
__________________
# p =
______________
# n
=_______________
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Going Backwards:
Determining the identity
of an element from the
Bohr diagram:
# p = _____________
# n =______________
atomic # = _____________
atomic mass = # p + # n =
________________
electron configuration:
_______________________
Isotopic Notation:
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Going Backwards:
Determining the identity
of an element from the
Bohr diagram:
# p = _____________
# n =______________
atomic # = _____________
atomic mass = # p + # n =
________________
electron configuration:
_______________________
Isotopic Notation:
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To review:
To draw a Bohr Model:
Look up the atomic #, atomic mass & the electron configuration
Determine the # of neutrons (atomic mass-atomic #)
Draw nucleus & write the # p & #n in nucleus
Draw rings around the nucleus equal to the # of PEL in atom (# of numbers in electron configuration)
Place electrons for each level symmetrically in the rings in pairs
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Going Backwards writing Isotopic
Notation:
# of protons = atomic number so look up the
atomic # to get symbol
Add the # of protons and neutrons to get the
atomic mass (mass #)
Atomic mass is the top number
10Ne20
Atomic # is the bottom number
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Now it is your turn!
Complete the Bohr
Model worksheet.
When done, show
me and turn in.
If not done, it
becomes
homework along
with homework #2.