Unit 2 - Atomic Structure - Blanks

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Unit 2 – Atomic Structure
Section 1 – Standards and Vocabulary
A. Standards
PS-2.1 Compare the subatomic particles (protons, neutrons, electrons) of an atom with regard to
mass, location, and charge, and explain how these particles affect the properties of an atom
(including identity, mass, volume, and reactivity).
PS-2.2 Illustrate the fact that the atoms of elements exist as stable or unstable isotopes.
PS-2.3 Explain the trends of the periodic table based on the elements’ valence electrons and atomic
numbers.
PS-2.4 Use the atomic number and the mass number to calculate the number of protons, neutrons,
and/or electrons for a given isotope of an element.
PS-2.5 Predict the charge that a representative element will acquire according to the arrangement of
electrons in its outer energy level.
PS-2.6 Compare fission and fusion (including the basic processes and the fact that both fission and
fusion convert a fraction of the mass of interacting particles into energy and release a great
amount of energy).
PS-2.7 Explain the consequences that the use of nuclear applications (including medical
technologies, nuclear power plants, and nuclear weapons) can have.
B. Vocabulary
• Atomic Mass
• Atomic Number
• Chain Reaction
• Chemical Reaction
• Chemically Stable
• Chemically Unstable
• Compound
• Critical Mass
• Electron
• Electron Cloud
• Energy Level
• Family
• Group
• Ion
• Isotope
• Mass Number
• Metal
• Metalloid
• Neutron
• Nonmetal
• Nuclear Decay
• Nuclear Fission
• Nuclear Fusion
• Nuclear Medicine
• Nuclear Power
Reactors
• Nuclear Weapons
• Nucleus
• Period
• Periodic Table
• Proton
• Radiation
• Sub-Atomic Particle
• Valence Electron
C. Book Correlations
• Chapter 18
• Chapter 19
• Chapter 22 (Section 1 only)

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Unit 2 – Atomic Structure
Section 2 – Atoms & Subatomic Particles
A. Atoms
1. Atoms are the building blocks of matter.
2. Everything on Earth is made up of atoms.
3. Atoms are the smallest particle that is still considered matter – meaning it has all the
properties of matter.
4. Atoms are made up of Subatomic particles
a. _____________________
b. _____________________
c. _____________________
5. Have an area called a nucleus and area called the electron cloud
a. ______________ – contains the protons and neutrons
1. Has a _____________ charge
b. ______________ – contains the electrons
1. Has a _____________ charge
c. Nucleus and electron cloud area are attracted to one another because one is
negative and the other is positive.
B. Subatomic Particles
1. ____________________
a. Mass = ______________
b. Charge = ________________
c. Location = ________________________
d. Electrons are what cause the atoms to combine with one another
e. They are attracted to the nucleus, which is positive and why they do not fly away.
f. Electrons determine the reactivity of the atom / element. They are given up or
shared.

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2. Neutron - n o
a. Mass = ____________________
b. Charge = ___________________
c. Location = ___________________
d. Can be as many neutrons or as few as the atom desires, they have no charge,
only mass.
3. Proton – p +
a. Mass = _______________
b. Charge = ________________
c. Location = __________________
d. Proton number determines the identity of the atom
e. All elements that are the same, have the same number of protons
Sub-Atomic Particle Mass Charge Location
Electron
Neutron
Proton
C. Periodic Table
• Where can you find one?
o Page 8 of your agenda
o On the back of your yellow equation sheet
1. Contains all the information you need about an atom, you just have to know how to read
the periodic table.
2. Important Parts
a. __________ – This is a capital letter or a Capital letter and lower case letter.
1. H
2. He
3. O
4. Cu
5. Fe
6. Sn
b. ______________ – this is the whole number that is in an individual block
1. Tells you how many protons there are in a stable atom.
2. Tells you how many electrons there are in a stable atom
3. Tells you the location on the periodic table (read like a book).
c. ________________ – this is the decimal number that is in an individual block
1. You round this number to the nearest whole number using math rounding
rules.
2. This will help you determine the number of neutrons that are in the element
a. Mass Number – Number of Protons = Number of Neutrons

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3. Example:
8
O
Oxygen
16.008
Atomic Number _______
Symbol __________
Atomic Mass ___________
Protons ______
Neutrons _______
Electrons _______
Element
Wavelength of Spectral Lines (nm)
Hydrogen 434, 486, 656
Helium 447, 468, 501, 587, 668
Mercury 405, 436, 546, 577, 579
Sodium 589, 590
Calcium 393, 397
Iron 517,
Neon 438-452, 585, 587, 588, 594-598, 603-693
Oxygen 687

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Unit 2 – Atomic Structure
Section 3 – Structure of an Atom
A. Nucleus
1. The nucleus contains the neutrons and protons.
2. The nucleus is incredibly small as compared to where you find the electrons.
3. The protons and neutrons are between one another
B. Orbitals
1. This area is known as the electron cloud.
2. The electron cloud has areas called orbitals in which the electrons move.
3. There are a maximum of seven orbitals that range from very close to the nucleus to farther
away.
4. There is a maximum number of electrons that each orbital can hold.
a. 1 st Energy Level – _________________________
b. 2 nd Energy Level – _________________________
c. 3 rd Energy Level – _________________________
d. 4 th Energy Level – _________________________
e. 5 th Energy Level – _________________________
f. 6 th Energy Level – _________________________
g. 7 th Energy Level – _________________________
C. Bohr Model – the accepted model for the electrons
__ p +
__ n o

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Unit 2 – Atomic Structure
Section 4 – Isotopes and Ions
A. Isotope
1. Isotopes are atoms of the same element with a different number of neutrons.
2. They are still neutral atoms because only the neutrons change and neutrons have a
NEUTRAL charge.
3. Only the mass changes because neutrons have a mass of 1.
B. Radioactive Isotopes
1. Atoms that have an incorrect ratio of neutrons to protons are radioactive, meaning they
give off radiation.
2. Radiation is the type of energy that is given off from a substance in the form of high
energy particles released from the atom in question
i. __________________– short range danger – not strong (2 protons & 2 neutrons)
ii. _____________________– stronger than alpha but less the gamma (electrons)
iii. ______________– most dangerous because it has the highest amount of energy
3. All items have radiation that is given off due to Nuclear Decay
i. Nuclear Decay occurs naturally and is the breakdown of the nucleus over time.
ii. Humans use this knowledge to our benefit
1. Nuclear Medicine
Pros
Cons
2. Nuclear Weapons
Pros
Cons

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3. Nuclear Power Reactors
Pros
Cons
C. Determining a Isotope:
1. You have to compare it to the periodic table and see that it is different
Electrons Neutrons Protons Mass
OR
2. You have to be told that you have a change in the mass number. There are two ways
to do this
i. Symbol – Mass Number
Symbol Electrons Neutrons Protons Mass
C-12 6 6 6 12
C-13
C-11
16
15
14
17
18
14

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ii. Mass Number (Symbol)
Atomic Number
Symbol Electrons Neutrons Protons Mass
12 C
6 6 6 6 12
13 C
6
11 C
6
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D. Examples
1. You have found an element that has a mass of 33 AMU and contains 22 neutrons.
i. What is the number of protons in this element? _________________________
ii. What is the number of electrons in this element? _________________________
iii. What is the element? _________________________
iv. Identify this element as an isotope, written correctly. _____________________
2. A student brings you an element with the mass of 8 AMU and 3 neutrons.
i. What is the number of protons in this element? _________________________
ii. What is the number of electrons in this element? _________________________
iii. What is the element? _________________________
iv. Identify this element as an isotope, written correctly. _____________________
3. Zn-57
i. What is the number of electrons in this element? _________________________
ii. What is the number of neutrons in this element? _________________________
iii. What is the number of protons in this element? _________________________
iv. What is the element? _________________________
4. Fe-86
i. What is the number of electrons in this element? _________________________
ii. What is the number of neutrons in this element? _________________________
iii. What is the number of protons in this element? _________________________
iv. What is the element? _________________________
5. 4 H
1
6. 27 Na
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i. What is the number of electrons in this element? _________________________
ii. What is the number of neutrons in this element? _________________________
iii. What is the number of protons in this element? _________________________
iv. What is the element? _________________________
i. What is the number of electrons in this element? _________________________
ii. What is the number of neutrons in this element? _________________________
iii. What is the number of protons in this element? _________________________
iv. What is the element? _________________________

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E. Ions
1. Ions are elements that are charged either positively or negatively due to the gaining or
losing of electrons.
2. This occurs naturally and is very normal
3. If an element gains an electron it is negatively charged.
4. If an element loses an electron it is positively charged.
Symbol Lose/ Gain Electrons Neutrons Protons Mass Notation
Li
Neither
Li Loses 1e -
Li Gains 7e -
O
Neither
O Gains 2e -
O Loses 6e -
5. Examples:
i. An atom of nitrogen gains 3 electrons.
1. What is the number of electrons? _________________________
2. What is the number of neutrons? _________________________
3. What is the number of protons? _________________________
4. Is this a positive or negative atom? _________________________
5. What is the notation? _________________________
ii. At atom of magnesium loses 2 electrons
1. What is the number of electrons? _________________________
2. What is the number of neutrons? _________________________
3. What is the number of protons? _________________________
4. Is this a positive or negative atom? _________________________
5. What is the notation? _________________________

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Unit 2 – Atomic Structure
Section 5 – The Periodic Table
A. Groups
• Vertical Columns
• All have the same number of valence electrons
1. Group 1 – ___________________
i. One valence electron
ii. Very Reactive with other elements
iii. Likes to give away 1 electron
2. Group 2 – _________________________
i. Two valence electrons
ii. Also very reactive
iii. Likes to give away 2 electrons
3. Groups 3-12 – _________________________
i. Most have 1 or 2 valence electrons
ii. These are tricky; they can do different things a lot of times.
4. _________________________
i. These are pulled out from the transition metals and dropped below on the table to be
sure there is room for all the elements.
ii. They follow the same trends as transitional elements.
iii. They are named Lanthanides because where the elements are pulled out is the
element Lanthanum.
5. ____________________________
i. These are pulled out from the transition metals and dropped below on the table to be
sure there is room for all the elements.
ii. They follow the same trends as transitional elements.
iii. They are named Lanthanides because where the elements are pulled out is the
element Actinium.

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6. Group 13 – _________________________
i. Three valence electrons
ii. Likes to give away three electrons
7. Group 14 – _________________________
i. Four valence electrons
ii. Likes to share electrons
iii. Bonds with MANY things
iv. Likes to gain, lose or share four electrons
8. Group 15 – _________________________
i. Five valence electrons
ii. Likes to gain three electrons
9. Group 16 – _________________________
i. Six valence electrons
ii. Likes to gain two electrons
iii. Very reactive!!
10. Group 17 – _________________________
i. Seven valence electrons
ii. Likes to gain one electron
iii. Very reactive!!
11. Group 18 – _________________________
i. Eight Valence Electrons
ii. These do not react with anything
iii. Helium is the exception, it does not react but
it only has two valence electrons
B. _________________________
1. These are the horizontal rows on the periodic table.
2. There are seven horizontal rows
3. Tells you how many electron orbital’s are being used
C. Major Categories of Elements
1. _________________________
i. Good Conductors of electricity and heat
ii. Have Luster (Shininess)
iii. High Density
iv. High Melting Point
v. Ductile – pulled into wire form
vi. Malleable – fold and bend
2. _________________________
i. Not good conductors of electricity and heat
ii. Lack Luster
iii. Low Density
iv. Low Melting Point
v. Not Ductile
vi. Not Malleable

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3. ____________________ – have characteristics of metals and non-metals
i. Solids
ii. Shiny or Dull
iii. Can conduct electricity and heat but not great conductors
D. Periodic Trends
1. ___________________________
i. The number of valence electrons increases from left right in groups 1-3, and 13-
18
2. ___________________________
i. The number of energy levels/orbital’s increase as the periods increase.
ii. The period number tells you how many energy levels / orbital’s are used
3. Questions?
i. Which element has more valence electrons Ca or S? ____________________
ii. Which element has more valence electrons Si or Al? ____________________
iii. Which element has more valence electrons B or At? ____________________
iv. Which element has more valence electrons F or P? ____________________
v. Which element has less valence electrons Cs or Te? ____________________
vi. Which element has more energy levels Se or Po? ____________________
vii. Which element has more energy levels Ra or S? ____________________

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Unit 2 – Atomic Structure
Section 6 – Nuclear Fission & Fusion
A. _____________________
1. Nuclear fission occurs when a heavy nucleus splits into two or more parts.
2. There is a change in the number of protons and neutrons
3. This is done by using a particle accelerator to bombard particles into atoms to make it split
into two.
4. Examples:
i. ____________________
ii. ____________________
iii. ____________________
B. _____________________________
1. Nuclear fusion occurs when you combine two atom’s nuclei together to create a third type
of nucleus.
2. There is a change in the number of protons and neutrons
3. This is done by using a particle accelerator to bombard particles into atoms to make it fuse
the atoms into one.
4. Example:
i. ____________________
ii. ____________________
iii. ____________________
• Both types of reactions involve very high temperatures and a lot of water to cool the reaction
afterwards. The waste water must be neutralized and some of the water waste cannot be
returned to the earth right away.
• The materials used during these reactions contain high amounts of radiation and must have
special storage.
• This special storage is usually not close to the reactor in case of a meltdown accident. It is
carried away and stored in other places.
C. Remember Pros and Cons
1. Nuclear Medicine
Pros
• Destroy targeted cells to be destroyed, like
cancer cells.
• Mapping the pathway of isotopes in the body,
such as in the digestive or circulatory system.
Cons
• Waste from these tests have to be stored for
LONG periods of time until no longer active.
• When you are destroying bad cells you are
also destroying good cells, however,
treatment has gotten better in the last 10
years.

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2. Nuclear Weapons
Pros
• Some people believe that nuclear weapons
are a deterrent to war since WWII.
• Only need a small amount of fuel (U)
3. Nuclear Power Reactors
Pros
• Energy from nuclear fission reaction heats
water to steam to rotate turbine.
• Lots of energy available.
• No air pollution
• Abundance of Fuel
• Decreases dependence on fossil fuels for
electricity.
Cons
• Specialized technology is required to create
the weapons.
• Only need amount of fuel so easier to
smuggle and hide.
• Destruction Potential
• Contamination to environment
• Waste
• Leakage
Cons
• Specialized technology is required.
• Thermal pollution in lakes and streams
• Waste Storage
• Leakage
• Accidents (Chernobyl, Three Mile Island)
D. Comparison of Chemical and Nuclear Reactions
Chemical Reaction
Nuclear Reaction
What part of the atom is
involved?
How is the reaction started?
What is the outcome of the
reaction?
How much energy is absorbed
or released?
What are some examples?