Q of the day

1
Q of the day
Day 3 11-14
1. One of Daltons ideas that we still believe
today
2. How are x-rays and radiation different?
2
We have Atoms! 1899 Ernest Rutherford
radiation

• Analyzed ________ to determine its ___________.
• ______________, ? , are fairly heavy with a
  ________ charge.
• _____________, ? , are very tiny with a
  ________ charge.

composition
Alpha particles
positive
Beta particles
negative
3
We have Atoms! 1899 Ernest Rutherford
Beta particles

• _____________, ? , are very tiny with a
  ________ charge.
• ____________, g , have no mass with a _______
  charge.

negative
Gamma rays
neutral
4
Radiation Penetration
5
Radiation Separation

• What does this separation pattern indicate about
  charges and masses of these types of radiation?
• a ______ mass and ________ charge
• ß ________ mass and _________ charge

larger
positive
smaller
negative
6
Radiation Separation

• What does this separation pattern indicate about
  charges and masses of these types of radiation?
• ß ________ mass and _________ charge
• ? ___ mass and ___ charge

smaller
negative
no
no
7
Atoms defy what we thought we knew! - 1900
Max Planck realized that atoms
_________________.
have their own rules
Good-bye, Newtonian physics!
Hello, Quantum Physics!
8
Quick Talk
Catalyst Exothermic reaction Law of conservation
of mass Proton Gold Neutron
Alchemist Law of Definite Proportions Democritus E
lectron Precipitate Reactantsmass
Productsmass Proton
9
Assignment
Page 109 s 9-15
10
Q of the day
Use your jigsaw notes

1. Which atomic model showed the probable locations
   of electrons?
2. Which atomic model was the first to show the
   nucleus of an atom?
3. Which atomic model was first to show energy
   levels?

Day 4 11-17
11
Atoms defy what we thought we knew! 1902

• Ernest Rutherford and Frederick Soddy discovered
  that radioactivity produces new __________
• Nuclear decay of uranium-238

elements
12
Atoms defy what we thought we knew! 1902

• Nuclear decay of uranium-238

Mass
234
Th
238U ? 4He
90
2
92
Atomic
uranium-238 ? thorium-234 a particle
13
Mass protons neutrons
Atomic protons periodic table
Write the nuclear symbol for Carbon with 6
neutrons
Write the nuclear symbol for Carbon with 8
neutrons
14
Practice
For Neon with 9 neutrons Mass ? _____ of
protons? _____ atomic ? _____ Write the
nuclear symbol
19
10
10
15
Practice
If an atom has 7 protons 9 neutrons Mass ?
_____ element ? _________ atomic ?
____ Write the nuclear symbol
16
nitrogen
7
16
Practice
Uranium-239 Mass ? _____ protons?
____ atomic ? ____ Write the nuclear symbol
239
92
92
17
Review
1. What 2 important things did the cathode ray
tubes prove (demonstrate) about electrons?
2. What was Mendeleevs contribution to
Chemistry?
3. How did Thomsons plum pudding model explain
the structure of an atom?
18
Assignments
Page 109 s 9-15 due NOW Practice Assignment 1
AND read section 4.3 and complete s 29, 30, 31
for period 9 due tomorrow
19
Q of the day
Day 5 11-18
How did Rutherfords model explain the structure
of an atom?
20
Review
1. What 2 important things did the cathode ray
tubes prove (demonstrate) about electrons?
2. What was Mendeleevs contribution to
Chemistry?
3. How did Thomsons plum pudding model explain
the structure of an atom?
21
Objective / Essential Question
What does the inside of an atom look like, and
how do we know?
22
Practice
If an atom has 17 protons 18 neutrons Mass
? _____ element ? __________ atomic ?
____ Write the nuclear symbol
35
chlorine
17
23
Atoms defy what we thought we knew!
1909-1910
Gold Foil Experiment

• Ernest Rutherfords
• Experiment applet 1
• Experiment applet 2

24

• Ernest Rutherfords
• Atoms appearance
• ____________________
• ____________________________________
• ________________________________

Gold Foil Experiment
Hollow sphere
Dense center with positive charge
Electrons occupy empty space
25
Atoms defy what we thought we knew! 1912
- 1913

• Neils Bohr - modified Rutherfords atomic model.
• Electrons are located in _______ ______ ______.
• Used this model to explain _________
  __________

specific
energy levels
emission spectra
26
Atoms defy what we thought we knew! 1912
- 1913

• Neils Bohr - modified Rutherfords atomic model.
• When an electron becomes excited (gains energy)
  it can jump up to a new energy level.
• When it falls back down
• to its ground state it
• emits energy (light).

27
Review

• Draw a nuclear symbol for an element with 17
  protons, 18 neutrons, and 18 electrons
• What element is it?
• What is the atomic ?
• What is the mass ?
• What is the charge?

28
Atoms defy what we thought we knew! 1913

• Frederick Soddy coined the term _______
• Atoms of the same ________
• Differ in ____
• Differ in ___________
• Examples
• ________________________
• _________________________

isotope
element
mass
radioactivity
Carbon-12 and Carbon-13
Uranium-236 and Uranium-238
29
Atoms defy what we thought we knew! 1913

• Henry Moseley
• Assigned ______ ________ to each element
• Realized that something in
  the _______ of
  an atom
  determines

atomic numbers
nucleus
30
Atoms defy what we thought we knew! 1913

• Henry Moseley
• Realized that something in
  the _______ of
  an atom
  determines its
  position on the
  _______ _____.

nucleus
Periodic Table
31
Atoms defy what we thought we knew! 1919

• Ernest Rutherford discovered _______
• Carry a _______ charge and are found in the
  ______.
• The number of _______ is the atoms ______
  _______.
• Conducted the first _______ ____________
  reaction,

protons
positive
nucleus
protons
atomic number
artificial
transmutation
32
Atoms defy what we thought we knew! 1919

• Ernest Rutherford discovered _______
• Conducted the first _______ ____________
  reaction, changing the element __________ into
  the element ________

protons
artificial
transmutation
nitrogen-14
oxygen-17
17
14N 4He ? 1H
O
2
7
1
8
33
Assignments
Practice Assignment 1 AND read section 4.3 and
complete s 29, 30, 31 for period 9 due NOW
34
Q of the day
Use your jigsaw notes

• Compare and contrast Rutherfords and Thomsons
  atomic model
• Difference ?
• Similarity ?

Day 6 11-19
35
Review
Use your notes

1. Which type of radiation is the most dangerous
   (penetrating)?
2. Which type of radiation is made up of high speed
   electrons?

36
Objective / Essential Question
1. What does the inside of an atom look like?
37
Atoms defy what we thought we knew! 1926

• Neils Bohrs ________model of the atom
• ______ _____
• _______ is dense center with ______ _______
• ________ found in specific energy levels

quantum
Empty sphere
Nucleus
protons
positive
Electrons
38
Atoms defy what we thought we knew! 1926

• Neils Bohrs ________model of the atom
• ________ found in specific energy levels
• Formula for the maximum number of e- per level

quantum
Electrons
Max e- 2n2
n number of energy level
39
Practice 2 due tomorrow