BELL RINGER What subatomic particle is not located in the nucleus?
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BELL RINGER
What subatomic particle is not located in the
nucleus?
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Atomic History Research
Chapter 3
Chapter 1
Review Book – Topic 1
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BELL RINGER
What are the nucleons (things in
the nucleus)?
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1. Who did the gold foil experiment?2. Who first named an atom?3. According to Bohr, where are
electrons located?4. Draw an atom according to
Democritus.5. Who discovered the electron?
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A. Ancient Greece (2000+ years ago)
Democritus - believed that matter could not be continuously divided- Matter consists of small indivisible particles“Atomos” = Atom indivisible
Particles are in continuous motion
Four elements make up all matter and energy
Earth, Wind, Water, Fire!
No scientific evidence to show this.
- Aristotle did not agree his teacher
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by 1700s (scientific revolution), all chemists agreed: on the existence of atoms that atoms combined to make
compounds
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B. Dalton’s Atomic Theory - 1803
1. All matter is composed of small particles which cannot be broken down (atoms) same as Democritus
2. All atoms of the same element are identical in size, mass and properties. Atoms of different elements are different in size, mass and properties
3.Atoms of different element combine in simple ratios to make compounds
4. In chemical reactions, atoms are combined, separated, or rearranged (No atoms are created or destroyed)
So at this point, we believe that an atom is like a small solid ball of matter that cannot be split up
H2S PbO2
Hydrogen Sulfur
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Some parts of Dalton’s theory were wrong: AMENDMENTS atoms are divisible into smaller particles
(subatomic particles) atoms of the same element can have
different masses (isotopes) Matter can be lost - Nuclear
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C. J.J. Thomson - 1897
Experimented with cathode rays
Used electric field to show that cathode rays are negatively charged particles
DISCOVORED THE ELECTRONAfter discovery of the proton, Thomson assumed an atom was a mixture of + and – charged particles, all mixed up
Plum-Pudding Model+ - + -- + -
- + - +
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D. Rutherford Ernest Rutherford wanted to determine what an atom looked like.Fired (+) charged alpha particles at a very thin piece of gold (Gold foil)Put a screen behind the foil to determine what happens to the rays
Gold foil
Screen
Most of the rays went straight through the foilSome rays deflectedA very few rays came straight back
Radioactive source
Click on me!!!
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Rutherford explained this by stating thata. Atoms have mostly empty space
This is why most rays went straight throughb. There must be a dense positive center to an atom
This is why the positive rays deflected. (Positive rays are repelled by positive charged objects)
Later experiments showed that electrons exist in the space between nuclei
- - - - - -
+
Rutherford model
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includes all particles inside atom proton electron neutron
charge on protons and electrons are equal but opposite
to make an atom neutral, need equal numbers of protons and electrons
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number of protons identifies the atom as a certain element
protons and neutrons are about same size
electrons are much smaller
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# protons = atomic number# electrons = # of protons (for now)# neutrons =
mass number– atomic number
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26
4
11
3
p n e4 3
1112
5 4
30 26
Li37
Na1123
Be49
Fe2656
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BELL RINGER
Give the p, n, and e in a neutral atom of
Silver.
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22
54
80
17
p n e
18 17
121 80
77 54
26 22
Cl17
Hg201
Xe
X22
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Nucleus: contains protons
and neutrons takes up very little
space Electron Cloud:
contains electrons takes up most of
space
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e- e-
E. Bohr - looked at the arrangement of electrons
Electrons exist in definite areas around the nucleus
Further from the nucleus, an electron has more energy
Electrons can gain energy and “jump” to higher levels
They can then give off the energy as they jump back down
Energy levels are numbered 1,2,3,4,5,6,7 • With 1 being closest to the nucleus and
having the least amount of energy
All atoms have the same types of energy levels
nucleus
e-Energy levelse-
3 2 1
Planetary model
+ - - -
- - -
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F. Wave Mechanical Model
Aka – ‘Electron Cloud’
Electrons are not in circular orbits, but exist in specific spaces around the nucleus
Pattern is random, unpredictable• most dense near nucleus
levellevel
Energy levels contain sublevels
nucleus
Dr. Wave Mechanical
Modified Bohr’s model
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Review of Atoms
Democritus
Dalton
Thompson
Rutherford
Bohr
Wave Mechanical
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Electron Location• Located in energy levels outside of the nucleus
• The closer to the nucleus = less energy
• The farther away from the nucleus = more energy
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Electrons are located in energy levels or shells. There are a bunch of energy levels and each level can “fit” only a limited number of electrons.
2 e-8 e-18 e-32 e-
2n2
Energy level 1 can have -Energy level 2 can have -Energy level 3 can have -Energy level 4 can have -
Electron Location
Where ‘n’ represents the energy level
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Bohr DiagramsGives the location and the number of the p, n, and e.
p=
n=
Draw the Bohr diagram for Oxygen:
8
8
Valence e- = 6
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Answer
p=
n=
9
10
Valence e- = 7
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BELL RINGER
What did Rutherford contribute to the
development of the atom?
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1. Ge2. Manganese3. As4. Phosphorus5. Ti
6. Sodium7. Cr8. Krypton9. Be10.Boron
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The above is an example of a ground state electron configuration
(=the configuration on your R.T.’s)
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Each electron in an atom has its own distinct amount of energy. Electrons in the first energy level have the lowest potential energy since they are located closest to the nucleus.
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Ground State
e- Configuration for Ne
2-8
As an electron gains a specific bunch of energy, the electron “jumps” to a higher energy state (excited state).
p=
n=
10
10
p=
n=
10
10
Excited State
e- Configuration for Ne
2-7-1
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Giv
es o
ff Ground State
e- Configuration for Ne
2-8
How is light produced?
p=
n=
10
10
p=
n=
10
10
Excited State
e- Configuration for Ne
2-7-1
Releases nrg
Absorbs nrg
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When an electron returns from a higher
energy state to a lower energy state, a specific amount of
energy is given off --> RELEASED
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Each element gives off a
certain color or spectrum
of colors.
You can identify unknown elements by
the color of light that they give off.Bohr Animation
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Ions So far we have only talked about electrically
neutral atoms, atoms with no positive or negative charge on them.
Atoms, however, can have electrical charges – They can gain/lose e-. Some atoms can either gain or lose electrons
The number of protons never changes in an atom.
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Ions If an atom gains electrons, the atom becomes
negatively charged.
If the atom loses electrons, the atom becomes
positively charged (because the number of positively charged protons will exceed the number of electrons).
An atom that carries an electrical charge is called
an ion.
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Ions Listed below are three forms of hydrogen; 2
ions and the electrically neutral form.
H+ : a positively charged hydrogen ion H : the
hydrogen atom
H- : a negatively charged hydrogen ion
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Ions Neither the number of protons nor neutrons changes
in any of these ions, therefore both the atomic number and the atomic mass remain the same.
H+ : a positively charged hydrogen ion
H : the hydrogen atom
H- : a negatively charged hydrogen ion
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IonsIdentify the number of subatomic
particles in the following ions:
A.) Na+ B.) F- C.) O-2
p
n
e
11
12
10
9
10
10
8
8
10
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BELL RINGER
Which is the electron configuration of an atom in the excited state?
1)2-8-2
2)2-8-1
3)2-7-1
4)2-8-3
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Timeline Activity
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When subjected to a flame, solutions containing certain metals have characteristic colors corresponding to the energy released when excited electrons return to lower energy levels.
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IonsIdentify the number of subatomic
particles in the following ions:
A.) Mg+2 B.) Br- C.) K+
p
n
e
12
12
10
35
45
36
19
20
18
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BELL RINGER
Draw the Bohr diagram for a F-1 ion.
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atoms of the same element with different numbers of neutrons
most elements exist as a mixture of isotopes Disproves Dalton’s theory
What do the Carbon isotopes below have in common? What is different about them?
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sum of the particles in nucleus = #p + #n This is a whole number!!!
How many protons do each of the hydrogen atoms below have?
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Ions/Isotopes
PRACTICE PROBLEMS
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since masses of atoms are so small, it is more convenient to use relative atomic masses instead of real masses
to set up a scale, we have to pick one atom to be the standard
since 1961, the carbon-12 nuclide is the standard and is assigned a mass of exactly 12 amu (=atomic mass unit)
REFERENCE TABLES
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atomic mass unit (amu)- one is exactly 1/12th of the mass of a carbon-12 atom
mass of proton= 1.007276 amu = 1 amu mass of neutron= 1.008665 amu = 1amu mass of electron= 0.0005486 amu = 0
amu
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weighted relative atomic masses of the isotopes of each element
each isotope has a known natural occurrence (percentage of that elements’ atoms)
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An element has three main isotopes with the following percent occurances: #1: 19.99244 amu, 90.51% #2: 20.99395 amu, 0.27% #3: 21.99138 amu, 9.22%
Find the average atomic mass and determine the element.
=20.179 amu
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Naturally occurring copper consists of: Cu-63 Cu-65
Actual Mass 62.929amu 64.927amu
Percent Abundance
Relative abundance
Relative Mass
69.71% 30.83% 100.54
.6971 .3083 1.0054
43.87 20.02 63.89
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BELL RINGER
Calculate the average atomic mass of Sulfur.
Isotope AMUNatural
Abundance32S 31.97 94.93%33S 32.97 0.76%34S 33.97 4.29%36S 35.97 0.02%
32.06 amu
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There are two isotopes of Silver, Ag-107 and Ag-109. 52% of the isotopes are Ag-107, what is the average atomic mass of silver?
Ag-107
Ag-109
52%48%
=
=
5564523210796
÷100=107.96
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BELL RINGER
Identify the number of p, n, and e in the following:
13717
Cl
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Spectroscopy
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The energy emitted is in the form of radiant or light energy which corresponds to a bright-line spectrum. Each element has its own signature or bright-line spectrum.
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There are several kinds of spectra, such as: continuous & bright line.A continuous spectrum is, as the name implies, a parade of all the colors from the deepest red to the ultraviolet - of which the rainbow in the sky is a good example.
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In the laboratory, a continuous spectrum can be produced by heating a solid - Light from the
electric lamp filament, for example, produces such a spectrum.
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When light emitted by a gas through which an electrical discharge is passing produces a spectrum consisting of a few isolated parallel lines, it is known as a "bright line spectrum"
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The characteristic color of neon signs is due to bright red and orange lines in its spectrum. The typical color of neon signs is due to the great intensity of the red and orange lines.
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Element X
Element Y
Elements X and Y combined
3 different electron jumps
A group of elements would create a combination of spectral lines
Notice how the combination of X and Y is just a combination of the individual spectral lines?
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Some Atomic Emission Spectra
Hydrogen
Mercury
Argon
Helium
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It should be carefully noted that each element always gives the same pattern of lines. Each element, so to speak, has its own fingerprints, possessed by no other element. This fact is utilized in chemical analysis and in many other applied fields.
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BELL RINGER
Identify the number of electrons and neutrons in the following:
1)Ti +3
2)S-2
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Unknown
What element is the unknown?
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Atomic History
DEMOCRITUS named the most basic particle
atom- means “indivisible
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Atomic History
1. Atoms of same element have the same size, mass, and properties
2. Atoms can’t be subdivided, created or destroyed
3. Atoms of different element combine in whole number ratios to make compounds
4. In chemical reactions, atoms are combined, separated, and rearranged.
DALTON
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Atomic History
Some parts of Dalton’s theory were wrong: atoms are divisible into smaller particles
(subatomic particles) atoms of the same element can have different
masses (isotopes) Most important parts of atomic theory:
all matter is made of atoms atoms of different elements have different
properties
DALTON
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Atomic HistoryRUTHERFORD
‘Gold Foil Experiment’ Atom is mostly empty space Small, hard, dense positive part = NUCLEUS
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Atomic HistoryJJ THOMSON
discovered the e-
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Atomic HistoryNEILS BOHR
Electons in ‘orbit’
protons in nucleus
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Atomic HistoryMODERN MODEL
protons in nucleusElectrons in an orbital – most probable location
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Atomic HistorySUMMARY
What we know about the atom has been the work of many scientists over thousands of years!
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WHITE BOARD REVIEW
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BELL RINGER
How much heat energy in joules is released by 25.0 grams of water when it is cooled from
75.2ºC to 31.9 ºC?
Get the formula from Reference Tables
q = mcΔT
q = 25.0g (4.18J/g•ºC) 43.3ºC
q = 4525 J