Transcript Week 13 Chemistry

Week 13 Chemistry
Nuclear Chemistry
Warm Up: 4 Minutes
Stay in your own seat
Write the Learning
Target
You should be working SILENTLY
89
In the atom, 39𝑌 , how many protons
and neutrons are in the nucleus?
Agenda

Warm Up – 7 minutes

Test Recap– 1 minutes

Cornell Style Notes/ Examples – 15 minutes

Guided Practice – 12 minutes

Independent Practice -15 minutes

Closing – 3 minutes
Test Scores
Period
Period
Period
Period
Period
Period
1:
3:
4:
5:
6:
7:
54%
58%
69%
69%
54%
60%
This Week
Monday
Tuesday
Thursday
Types of
Nuclear
Radiation
Nuclear
Equations
Fission and
Fusion
Nuclear Chemistry
Nuclear Chemistry
Changes
in matter originating in
the nucleus of an atom.
Applications:
Energy  Nuclear Energy
Life  The Sun is an example of nuclear
chemistry at work
Medicine  X-rays, MRI
Jobs in Nuclear Chemistry

Energy research, production (Nuclear Engineer)

Cancer Treatment (Oncologist)

Medical Imaging (Radiologist)

Radioactive Tracing (Medicine)

Radioactive Dating (Geology)
Alpha
Symbol
Beta
Gamma
Let’s Review the Parts of a Chemical
Symbol
Mass
number
X
Atomic
number
Alpha Radiation
An alpha particle is identical to that of a helium nucleus.
It contains two protons and two neutrons.
Alpha Radiation
222
226
Ra
88
Rn
86
4
α
2
Alpha
Symbol
4
2𝛼
Beta
Gamma
Beta Radiation
A beta particle is a fast moving electron which is
emitted from the nucleus of an atom undergoing
radioactive decay.
Beta decay occurs when a neutron changes into a
proton and an electron.
Beta Radiation
218
218
Po
84
At
85
b
-1
0
Alpha
Symbol
4
2𝛼
Beta
0
−1𝛽
Gamma
Alpha
Symbol
4
2𝛼
Beta
Gamma
0
−1𝛽
0
0𝛾
Alpha
Symbol
Charge
4
2𝛼
Beta
Gamma
0
−1𝛽
0
0𝛾
Alpha
Symbol
2𝛼
Charge
+2
4
Beta
Gamma
0
−1𝛽
0
0𝛾
Alpha
Symbol
2𝛼
Charge
+2
4
Beta
Gamma
0
−1𝛽
-1
0
0𝛾
Alpha
Symbol
2𝛼
Charge
+2
4
Beta
Gamma
0
−1𝛽
-1
0
0𝛾
0
Alpha
Symbol
2𝛼
Charge
+2
Relative
Mass
4
Beta
Gamma
0
−1𝛽
-1
0
0𝛾
0
Alpha
Symbol
2𝛼
Charge
+2
Relative
Mass
Heavy
4
Beta
Gamma
0
−1𝛽
-1
0
0𝛾
0
Alpha
Beta
Gamma
0
0𝛾
0
Symbol
2𝛼
Charge
+2
0
−1𝛽
-1
Relative
Mass
Heavy
Light
4
Alpha
Beta
Gamma
0
0𝛾
0
No Mass
Symbol
2𝛼
Charge
+2
0
−1𝛽
-1
Relative
Mass
Heavy
Light
4
Let’s look at Penetration Power
Alpha
Beta
Gamma
0
0𝛾
0
No Mass
Symbol
2𝛼
Charge
+2
0
−1𝛽
-1
Relative
Mass
Penetration
Power
Heavy
Light
4
Alpha
Beta
Gamma
0
0𝛾
0
No Mass
Symbol
2𝛼
Charge
+2
0
−1𝛽
-1
Relative
Mass
Penetration
Power
Heavy
Light
4
Low
Alpha
Beta
Gamma
0
0𝛾
0
No Mass
Symbol
2𝛼
Charge
+2
0
−1𝛽
-1
Relative
Mass
Penetration
Power
Heavy
Light
Low
Medium
4
Alpha
Beta
Gamma
0
0𝛾
0
Symbol
2𝛼
Charge
+2
0
−1𝛽
-1
Relative
Mass
Penetration
Power
Heavy
Light
No Mass
Low
Medium
High
4
Check point
 Which
type of nuclear radiation has a
negative charge?
Beta
Check point
 Which
type of nuclear radiation produces
the most massive particle?
Alpha
Check point
 Which
type of nuclear radiation has the
highest penetrating power?
Gamma
Guided Practice
Mr. Ghosh: Project a multiple question
Student will:
1. SILENTLY read the question to your self and pick
an answer [19 seconds]
2. Take 42 seconds to speak with your shoulder
partner to chose the correct answer and discuss
why it is the correct answer. [42 seconds]
3. When Mr. Ghosh says “SWAG” all students should
be SILENT

#1
Which of the following statements accurately
describes beta particles in terms of charge and mass?
A.
B.
C.
D.
Beta particles are positively charged and less
massive than alpha particles.
Beta particles are negatively charged and less
massive than alpha particles.
Beta particles are positively charged and more
massive than alpha particles.
Beta particles are negatively charged and more
massive than alpha particles.
#2
Which of the following statements describes an
alpha particle?
A.
An alpha particle has no mass.
B.
An alpha particle has a negative charge.
C.
An alpha particle has low penetrating power
D.
An alpha particle has a symbol of −𝟏𝟎𝜶
#3
The three main types of nuclear radiation are alpha,
beta, and gamma. Which of the following lists these
types of radiation from lowest penetrating power to
highest penetrating power?
A.
Alpha, beta, gamma
B.
Beta, gamma, alpha
C.
Beta, alpha, gamma
D.
Gamma, alpha, beta
#4
Which of the following best describes alpha particles, beta
particles, and gamma rays?
A.
Beta particles are negatively charged and are easy to stop
B.
Alpha particles have no charge and are easy to stop
C.
Gamma rays are positively charged and are hard to stop
D.
Alpha particles are positively charged and are easy to
stop
Independent Practice
 Practice Makes Perfect 
85%
Closing
What are the three types of nuclear
radiation?
Which one is the most powerful?
Warm Up: 4 Minutes
Write the Learning
Target
Stay in your own seat
You should be working SILENTLY
Type of Nuclear
Radiation
Gamma
Alpha
Beta
Symbol
[Include Mass # & Atomic #]
Warm Up: 4 Minutes
Type of Nuclear
Radiation
Gamma
Alpha
Beta
Symbol
[Include Mass # & Atomic #]
0
γ
0
Warm Up: 4 Minutes
Type of Nuclear
Radiation
Symbol
[Include Mass # & Atomic #]
Gamma
Alpha
Beta
0
γ
0
4
α
2
or 42He
Warm Up: 4 Minutes
Type of Nuclear
Radiation
Symbol
[Include Mass # & Atomic #]
Gamma
Alpha
Beta
0
γ
0
4
α
2
or 42He
0
β
−1
Agenda

Warm Up: 7 Minutes

Cornell Style Notes and Examples: 15 Minutes

Guided Practice: 13 Minutes

Independent Practice: 15 Minutes

Closing: 3 Minutes
Announcement
We have had complaints from the Janitors about the
trash being left in the desks.
Before you leave each day, I will check EVERY
SINGLE DESK for trash.
NOBODY WILL LEAVE UNTIL ALL TRASH IS CLEANED UP
This Week
Monday
Tuesday
Thursday
Types of
Nuclear
Radiation
Nuclear
Equations
Fission and
Fusion
Take out paper for notes
BLUE
RED
Nuclear reactions
A
change in the identity or
characteristics of an atomic
nucleus
 Results due to an energetic
particle, as in fission, fusion, or
radioactive decay.
Let’s Review the Parts of a Chemical
Symbol
Mass
number
X
Atomic
number
How to Compose Chemical Symbols

Begin with Element symbol

Put mass number on top

Find atomic number of element on periodic table, put it
on the bottom
Example: Compose the Chemical Symbol for Polonium-212
212
84
Po
Requirements of a nuclear reaction

Sum of the mass numbers is the same on both sides of the
equation.

Sum of the atomic numbers is the same on both sides of the
equation.
Alpha Decay Nuclear Reactions
A
A-4
4
226
222
4
X
Z
Ra
88
Y
+
Z-2
Rn
+
86
He
2
He
2
Beta Decay Nuclear Reactions
A
X
Z
218
Po
84
A
b
-1
218
b
-1
Y
+
Z+1
Rn
+
85
0
0
Gamma Radiation Nuclear Reactions
230
Th
90
234
Th
90
He
Ra
+
+

2
88
226
234
Pa
+
91
4
0
-1 b +

Example: Complete the nuclear equation
210
𝑃𝑜
84
→
206
𝑃𝑏
82
+ ___________
Example: Complete the nuclear equation
239
93𝑁𝑝
→ ___________ +
0
−1𝛽
Example: Complete the nuclear equation
60
0
0
_______  Ni +
β+ 
28
0
−1
Check point
What is true of the sum of the mass numbers on both sides of the
equation?
They are equal
Check point
What is true of the sum of the atomic numbers on both sides of
the equation?
They are equal
Guided Practice
Teacher:
1. Will show the problem on the board
 Students:
1. Take 31 seconds to read the question SILENTLY and
compose an answer.
2. Take 63 seconds to speak with your shoulder partner
to solve the problem and discuss how to do it
3. When Mr. Ghosh says “SWAG” all students should be
SILENT

Complete the following nuclear equation
73
4
1
Ge + He  H + ____
32
2
1
Complete the following nuclear equation
222
𝑅𝑛
86
→ ___________ +
4
𝐻𝑒
2
Polonium-212 decays directly to
Lead-208. What type of particle
must be emitted during this
radioactive decay?
Thorium-228 decays to Polonium-216
through a series of alpha decays.
How many alpha particles are
emitted in this decay series?
Independent Practice
 Practice Makes Perfect 
85%
Closing
All Students Stand UP
Push Stools Under Desk
Clean ALL trash from your area
Warm Up: 4 Minutes
Complete the following nuclear reactions by
filling in the blank:
1
0
n+
239
94
13
6
Pu → ________ +
C+
4
2
144
57
He → ______ +
1
0
1
0
La + n + n
1
0
n
Agenda

Warm Up: 7 Minutes

Cornell Style Notes and Examples: 13 Minutes

Guided Practice: 15 Minutes

Independent Practice: 15 Minutes

Closing: 3 Minutes
This Week
Monday
Tuesday
Thursday
Types of
Nuclear
Radiation
Nuclear
Equations
Fission and
Fusion
Take out paper for notes
BLUE
RED
Fission reaction
Did you know that?
Fission of 1 GRAM of Uranium…
Releases enough energy to run a light bulb
for 20 YEARS
Fission reaction

Breaking apart of a nucleus into smaller fragment
1
91
142
1
1
1
235
U + n  Kr +
Ba + n + n + n
0
36
56
0
0
0
92

Neutrons emitted cause other (chain) reactions
Question…
Is there a more efficient way to write:
1
1
1
n+ n+ n
0
0
0
What is another way to write 2 + 2 + 2?
3x2
or
3(2)
Using your knowledge from the previous example, how
would you write:
1
1
1
n+ n+ n
0
0
0
3
1
0n
Fusion reactions
Did you know that?
The sun is a giant nuclear fusion power
source
Fusion Reaction

Combining of nuclei to form a nucleus with a greater mass
0
4
1
4 H  He +2
e + energy
+1
2
1

Releases tremendous amount of energy (more than fission)
Check point

Which type of reaction causes a heavy nucleus to
break into lighter nuclei once it is bombarded by
a neutron?
Fission Reaction
Check point
 Both
fusion and fission reaction produce
1
neutrons, n . Which reaction utilizes the
0
neutrons to trigger another set of nuclear
reactions ?
Fission Reaction
Check point
What type of reaction is listed below? Why?
1
268
1
207
58
n+
Mt +  4 n +
Pb + Co
0
109
0
82
27
Fission Reaction
Check point
 What
do both types of reaction release?
Energy
Guided Practice
Teacher:
1. Will show the problem on the board
 Students:
1. Take 31 seconds to read the question SILENTLY and
compose an answer.
2. Take 53 seconds to speak with your shoulder partner
to solve the problem and discuss how to do it
3. When Mr. Ghosh says “SWAG” all students should be
SILENT

#1
Which of the following equations shows a
fusion reaction?
246
12
1
A. 238
U
+
C
→
Cf
+
4
6
0n
92
98
139
93
1
B. 10 n + 235
U
→
I
+
𝑌
+
4
0n
92
39
53
C.
D.
0
24
24
Na
→
𝑀𝑔
+
11
12
−1𝛽 + 𝛾
141
235
92
1
n
+
U
→
𝐵𝑎
+
0
92
36
56
𝐾𝑟 + 3 10 n
#2
Which of the following equations shows a
fission reaction?
246
12
1
A. 238
U
+
C
→
Cf
+
4
6
0n
92
98
139
93
1
B. 10 n + 235
U
→
I
+
Y
+
4
0n
92
39
53
C.
D.
0
24
24
Na
→
Mg
+
11
12
−1β +
3
0
1
2
H
+
H
→
He
+
1
1
2
0γ
γ
#3
Which of the following best describes a
common feature of nuclear fission and
fusion reactions?
A.
Nuclei split during fission and fusion
B.
Fission and fusion both form heavier elements
C.
Fission and fusion both generate energy
D.
Nuclei gain electrons during fission and fusion
#4
Which of the following statements applies
to a nuclear fusion reaction?
A.
Nuclear fusion reactions have no commercial applications
B.
The reaction takes place when a nucleus is bombarded with
neutrons
C.
The reaction releases large amounts of energy when nuclei
are brought together
D.
A chain reaction is involved
Independent Practice
 Practice Makes Perfect 
85%
Closing
 What
are the two types of nuclear
reactions?
 How
are the same?
 How
are they different?
Warm Up: 3 Minutes
Stay in your own seat
Write the Learning
Target
You should be working SILENTLY
Classify the following elements as either a metal or
a nonmetal:
 Carbon
 Aluminum
 Vanadium
 Oxygen
 Iodine
Check Your Answers!!!
•
•
•
•
•
Carbon -Nonmetal
Aluminum -Metal
Vanadium- Metal
Oxygen-Nonmetal
Iodine-Nonmetal
Agenda

Warm Up: 7 Minutes

Cornell Notes and Examples: 15 Minutes

Guided Practice: 12 Minutes

Independent Practice: 10 Minutes

Closing: 1 Minutes
Metal or Nonmetal?
What is a Compound?
Two or more elements that are bonded
together by the interaction of their valence
electrons in order to achieve their octet rule
Ionic vs. Covalent Compounds
PF3
NaCl
Al2S3
CaS
CO2
H2O
N2
NO2
Br2
Compound
Covalent
What is a Covalent Compound?
Two
or more nonmetals bonded
together
COVALENT
Bond:
SHARES valence electrons.
Examples:
N2 or CO2
Check point
Is this a covalent compound?
C6H12O6
YES
Check point
Is this a covalent compound?
KBr
NO
Compound
Covalent
2 or More
Nonmetals
Ionic
What is an Ionic Compound?
Positive
(cations) and negative ions
(anions) that are bonded together
IONIC
bond:
TRANSFERS valence electrons from one
ion to the other
Examples:
NaCl and K2SO4
Compound
Covalent
2 or More
Nonmetals
Ionic
Cation
What is a Cation?
Any
atom or GROUP OF ATOMS with a
positive charge.
Examples:
Metals (Na+1 , Ag+2 ) or NH4 +1
Compound
Covalent
2 or More
Nonmetals
Ionic
Cation
Positive
Anion
What is an Anion?
Any
atom or group of atoms with a negative
charge
Examples:
Nonmetals (F-1 , O-2 )
Polyatomic Ions (NO3 -1 , SO4
-2
)
Compound
Covalent
2 or More
Nonmetals
Ionic
Cation
Positive
Anion
Negative
What is a Polyatomic Ion ?
Any
group of atoms that acts as a single
unit in chemical bonding
Examples:
Anions (NO3-1 , PO4 -3 )
Cations (NH4 +1)

Ammonium, NH4 +1
Acetate:
Nitrite:
Nitrate:
C2H3O2
-1
NO2-1
CN-1
Hydroxide:
OH-1
Permanganate:
Hypochlorite:
Chlorite:
MnO4-1
ClO-1
ClO2-1
ClO3-1
Perchlorate
Oxalate:
NO3-1
Cyanide:
Chlorate:
: ClO4-1
C2O4 -2
Sulfite:
SO3 -2
Sulfate:
SO4-2
Carbonate:
CO3-2
Chromate:
CrO4-2
Phosphate:
PO4-3
Check point
Is this an Ionic or a Covalent compound?
H2
COVALENT
Check point
Is this an Ionic or a Covalent compound?
Na2SO4
IONIC
Recap
Does the compound have a metal?
IONIC
No Metals?
COVALENT
Guided Practice

Teacher:
1. Will show the problem on the board

Students:
1.
2.
3.
Take 38 seconds to look at the set of compounds
SILENTLY and compose your answer.
Take 57 seconds to speak with your shoulder
partner to solve the problem and discuss how to
do it
When Mr. Ghosh says “SWAG” all students should
be SILENT
Compound
NaF
CO
KNO3
Ionic or
Covalent
Compound
NaF
CO
KNO3
Ionic or
Covalent
Ionic
Compound
NaF
CO
KNO3
Ionic or
Covalent
Ionic
Covalent
Compound
NaF
CO
KNO3
Ionic or
Covalent
Ionic
Covalent
Ionic
Compound
N2O
P2O5
K2SO4
Ionic or
Covalent
Compound
N2O
P2O5
K2SO4
Ionic or
Covalent
Covalent
Compound
N2O
P2O5
K2SO4
Ionic or
Covalent
Covalent
Covalent
Compound
N2O
P2O5
K2SO4
Ionic or
Covalent
Covalent
Covalent
Ionic
Compound
SO2
Se2O5
MgCl2
Ionic or
Covalent
Compound
SO2
Se2O5
MgCl2
Ionic or
Covalent
Covalent
Compound
SO2
Se2O5
MgCl2
Ionic or
Covalent
Covalent
Covalent
Compound
SO2
Se2O5
MgCl2
Ionic or
Covalent
Covalent
Covalent
Ionic
Independent Practice
 Practice Makes Perfect 
85%
Closing
 What
was the purpose in learning to
distinguish between ionic and covalent
compounds?