Download Chapter 4, 5, 6 - Campbell County Schools

Atomic Structure
Chapter 4
Mr. Hines
Part A – Standard model of the atom
Learning Targets and “I can” statements
1
2
3
4
I CAN
List, label, and describe the parts of an atom.
Identify the atomic number and the atomic mass of all elements and explain what they
mean.
Describe atoms using the classical model.
Describe atoms using the “Marble in the football stadium” model.
Part B – Electrons and the Periodic Table
5
6
7
8
9
10
Define energy levels and explain how electrons are organized into energy levels.
Determine how many electrons can be held in each energy level.
Explain how electrons fill energy levels (aufbau principle).
Draw atomic models with proper amounts of subatomic particles.
Define valence electrons and determine the amount for each element.
Identify groups on the periodic table and explain the relationship between valence
electrons and groups.
11 Determine the amount of energy levels for each element.
12 Identify periods on the periodic table and explain the relationship between energy levels
and periods.
13 Compare and contrast the various elements on the periodic table.
Part C - Isotopes
14
15
16
17
18
19
20
21
Define isotopes and write proper isotope notation.
Determine the number of all subatomic particles of an element when given the atomic
mass of an isotope.
Compare and contrast isotopes of the same element.
Convert a percent to a decimal.
Calculate the atomic mass of each element from known scientific data.
Explain why the atomic mass of most elements is written as a decimal.
Name and draw the isotopes of Hydrogen.
Evaluate the placement of hydrogen and helium on the periodic table.
Vocabulary
Matter
Atomic
mass units
Neutral
charge
Nucleus
Mass
Isotope
Atoms
Subatomic
particles
Electron
cloud
Bike
Period
Average
Protons
Negative
charge
Energy
Level
symbol
Group
Hydrogen
Neutrons
Positive
charge
Vertical
column
Space
Abundance
Decimal
Electrons
Atomic
number
Horizontal
row
Model
Big Mac
Deuterium
Amu
Atomic
mass
Lewis dot
structure
Volume
Percent
Tritium
Exist
Periodic Table
Natural percent
abundance
Valence Electron
Aufbau principle
PART A – STANDARD MODEL OF THE ATOM
Target 1 – List, label, and describe the parts of an atom.
A. Remember from earlier that matter is anything made of _________________.
B. Atoms are the basic building blocks of all matter.
C. Atoms are made of smaller _________________________. These are listed below.
1. Protons – positive charge (+) and found in nucleus (center) of atom.
2. Neutrons – neutral or zero charge (0) and found in nucleus of atom. Collectively, protons and
neutrons are referred to as _______________________________(amu) – term meaning that they
are found in the nucleus.
3. Electrons – negative charge (-) and found moving around the nucleus of an
atom. Electrons have such a small ________________ that we don’t even consider them when
measuring mass.
.
 Questions
1. List the parts of an atom. (3 parts)
a. _________________
b. _________________
c. _________________
2. Describe where the parts of an atom are located.
a. _________________________________________________
b. _________________________________________________
c. _________________________________________________
3. Indicate the charge on each part of the atom.
a. __________________________________
b. __________________________________
c. __________________________________
Target 2 - Identify the atomic number and the atomic mass of all elements and
explain what they mean.
A. All of the elements are listed on the ___________________________ of Elements.
B. Elements are different kinds of atoms with a name, symbol, and unique properties.
C. The Periodic Table lists the elements in the order based on the number of ___________________.
D. The atomic number is written above the symbol and tells you the number of protons.
E. The number of protons identifies each individual element.
F. The ____________________ _____will also tell you the number of electrons.*
G. The atomic mass is written below the symbol and tells you the total number of protons and neutrons.
H. If you want to know the number of neutrons, you can subtract the atomic number from the atomic mass.
I. Protons, neutrons, and electrons are collectively referred to as ________________________________.
J. Subatomic particles found in the nucleus (protons and neutrons) are more specifically called atomic
mass units.
K. Atomic mass units are abbreviated as amu.
Notes
12
Mg
24.30
 Questions
1. What is listed on the periodic table? ____________________________________________
2. What is the difference between an element and an atom? ____________________________
3. What determines the order in which elements are listed on the periodic table?
____________________________________________________________________________
4. Where is the atomic number listed on the periodic table? ____________________________
5. Where is the atomic mass listed on the periodic table? ______________________________
6. What does the atomic number tell you about an element? ____________________________
7. What does the atomic mass tell you about an element? ______________________________
8. How do you determine the amount of neutrons in an element? ________________________
9. How many protons does Potassium have? _____
10. How many neutrons does Potassium have? _____
11. How many electrons does Potassium have? _____
12 How many subatomic particles does Potassium have? _____
13. How many atomic mass units does Potassium have? _____
Target 3 – Describe atoms using the classical model - Pg 129
A. The classical model of the atom.
1. Protons and neutrons are particles located in the nucleus.
2. Electrons _________________ around the nucleus.
3. It is known that electrons occupy a very large amount of space around the nucleus.
4. Since the electrons occupy a large ___________around the nucleus, we call that space the electron cloud.
5. The electron cloud simply refers to the space where the electrons exist.
6. Label the electron cloud on the next illustration.
Target 4 - Explain the “Marble in the football stadium” model of an atom
A. The classical model of the electron is commonly used around the world, but is not _____________________.
B. A more accurate model of the atom is known as the marble in the football stadium.
1. If an atom were the size of a football stadium, the nucleus would be about the size of a marble.
2. Therefore, the electrons pretty much occupy all of the __________________ in the stadium.
3. In other words, atoms are 99.99% empty space!
4. Draw a marble in the center this stadium.
PART B – ELECTRONS AND THE PERIODIC TABLE
Target 5 – Define energy levels and explain how electrons are organized into
energy levels
1. Energy Level - Specific location around the nucleus where electrons exist
2. Electrons are well organized in the electron cloud into _________________________
3. Energy levels can be visualized similar to planets orbiting around the sun – each planet is further away
from the sun and do not leave their orbits
Solar system with planets revolving around sun Atom with electrons revolving around the nucleus
4. Energy levels around the nucleus are sort of like layers of an onion.
5. Energy levels can also be compared to rungs on a ladder – if you climb a ladder, your feet will
on the rungs of the ladder. Pg 129
6. There are a total of 7 energy levels.
be
Target 6 - Determine how many electrons can be held in each energy level.
A. Energy levels can only hold so many electrons
Notes box (drawing)
Energy
Amount of
level
electrons held
1
2
2
8
3
8
4
18
5
18
6
32
7
32
 Questions
1. What particles are found in the nucleus of an atom? _______________________________________________
2. Where are the electrons of an atom? ___________________________________________________________
3. Explain the marble in the stadium model of the atom. _____________________________________________
4. What is meant by the electron cloud? __________________________________________________________
5. What is an energy level of the electron cloud? ___________________________________________________
6. How many electrons can be held in the 1st energy level? _____
7. How many electrons can be held in the 2nd energy level? _____
8. How many electrons can be held in the 3rd energy level? _____
9. How many electrons can be held in the 5th energy level? _____
Target 7 - Explain how electrons fill energy levels
A. Electrons will fill the innermost energy levels first (aufbau principle).
B. When the innermost energy levels are filled, electrons must fill ______________________ energy levels.
C. This is similar to people filling around a boxing match – once the front rows are filled, outer seating will fill up.
D. For example – ___________________ has 3 electrons.
1. The first 2 electrons will fill the first energy level
2. The third electron will therefore be forced to exist in the second energy level.
E. This concept is best learned through drawings.
Target 8 - Draw atomic models with proper amounts of subatomic particles.
Table Z
Hydrogen
Helium
Lithium
Protons =
Neutrons =
Electrons =
Protons =
Neutrons =
Electrons =
Protons =
Neutrons =
Electrons =
Beryllium
Boron
Protons =
Neutrons =
Electrons =
Carbon
Protons =
Neutrons =
Electrons =
Nitrogen
Protons =
Neutrons =
Electrons =
Oxygen
Protons =
Neutrons =
Electrons =
Fluorine
Protons =
Neutrons =
Electrons =
Neon
Protons =
Neutrons =
Electrons =
Sodium
Protons =
Neutrons =
Electrons =
Magnesium
Protons =
Neutrons =
Electrons =
Aluminum
Protons =
Neutrons =
Electrons =
Protons =
Neutrons =
Electrons =
Silicon
Phosphorus
Protons =
Neutrons =
Electrons =
Sulfur
Protons =
Neutrons =
Electrons =
Chlorine
Protons =
Neutrons =
Electrons =
Argon
Protons =
Neutrons =
Electrons =
Potassium
Protons =
Neutrons =
Electrons =
Protons =
Neutrons =
Electrons =
Target 9 - Define valence electrons and determine the amount for each element.
A. Valence electrons – electrons that are located in the outermost energy level.
B. From the drawings on Table Z, determine the amount of valence electrons for each element.
1. Hydrogen = ____
2. Helium = ____
3. Lithium = ____
4. Beryllium = ____
5. Boron = ____
6. Carbon = ____
7. Nitrogen = ____
8. Oxygen = ____
9. Fluorine = ____
10. Neon = ____
11. Sodium = ____
12. Magnesium = ____
13. Aluminum = ____
14. Silicon = ____
15. Phosphorus = ____
16. Sulfur = ____
17. Chlorine = ____
18. Argon = ____
Einstein moment - can you explain the arrangement of the
elements on the periodic table based on valence
electrons?
Target 10 - Identify groups on the periodic table and explain the relationship
between valence electrons and groups. (Pg 118)
1. Groups on the periodic table are ______________ columns - draw a vertical line over here →
2. For example, Sodium, Lithium and Hydrogen are all in the same group (group 1)
3. Groups on the periodic table are divided into 2 catagories.
a. Group A
b. Group B
4. In this chemistry class, we will mostly speak of _________________. (Group B for advanced studies)
5. Label the groups on your periodic table as demonstrated in class
Target 11 – Determine the amount of energy levels for each element.
A. From the drawings on Table Z, determine the amount of energy levels for each element.
1. Hydrogen = ____
11. Sodium = ____
2. Helium = ____
12. Magnesium = ____
3. Lithium = ____
13. Aluminum = ____
4. Beryllium = ____
14. Silicon = ____
5. Boron = ____
15. Phosphorus = ____
6. Carbon = ____
16. Sulfur = ____
7. Nitrogen = ____
17. Chlorine = ____
8. Oxygen = ____
18. Argon = ____
9. Fluorine = ____
10. Neon = ____
Einstein moment - can you explain the arrangement of the
elements on the periodic table based on energy levels?
Target 12 - Identify periods on the periodic table and explain the relationship
between energy levels and periods. (Pg 118)
1. Periods on the periodic table are ___________________ columns (draw a horizontal line here) 
2. For example, sodium, magnesium, and aluminum are all in the same period (period 3).
3. This means that elements in period 3 will all have 3 ___________________________
4. Label the periods on your periodic table as demonstrated in class
Practice – Indicate which GROUP each element is in.
Element
Group
Element
Group
Element
Mg
B
C
Ca
Al
Si
Sr
Ga
Ge
Practice – Indicate which PERIOD each element is in.
Element
Period
Element
Period
Element
Li
B
N
Na
Al
P
Ca
Fe
Cu
Group
Element
O
S
Se
Group
Period
Element
Ne
Ar
As
Period
1. What is a group on the periodic table? ________________________________________________
2. What is a period on the periodic table? ________________________________________________
Target 13 - Compare and contrast the various elements on the periodic table.
1. What is the definition of an element?
_____________________________________________________________________
2. What is the definition of the periodic table?
_____________________________________________________________________
3. How are elements alike? (compare)
_____________________________________________________________________
4. How are elements different? (contrast)
_____________________________________________________________________
PART C - ISOTOPES
Target 14 - Define isotope and write proper isotope notation
A. Even though atoms are considered to be the same based on the amount of _________________, they can
have different amounts of neutrons.
B. In nature, _____________________ will contain different amounts of neutrons.
C. Isotope - elements that have different numbers of neutrons
D. If most elements have a different number of neutrons, how can the atomic mass number be determined?
E. Whenever an Isotope is written, it includes the _______________________of the isotope after the
symbol separated by a dash.
Practice – Write the proper isotope notation for each example
Helium –
Carbon Protons = 2
Protons = 6
Neutrons = 1
Neutrons = 6
Electrons = 2
Electrons = 6
Helium Carbon Protons = 2
Protons = 6
Neutrons = 2
Neutrons = 7
Electrons = 2
Electrons = 6
Nitrogen Protons = 7
Neutrons = 7
Electrons = 7
Nitrogen –
Protons = 7
Neutrons = 8
Electrons = 7
Target 15 - Determine the number of all subatomic particles of an element when
given the atomic mass of an isotope
Oxygen – 17
Protons =
Neutrons =
Electrons =
Phosphorus - 33
Protons =
Neutrons =
Electrons =
Fluorine - 21
Protons =
Neutrons =
Electrons =
Copper - 66
Protons =
Neutrons =
Electrons =
Calcium - 42
Protons =
Neutrons =
Electrons =
Potassium - 41
Protons =
Neutrons =
Electrons =
Target 16 – Compare and contrast isotopes of the same element.
Target 17 - Convert a percent to a decimal.
A. A percent can be written as a decimal by moving the decimal point to the left 2 places.
notes
Percent
27%
Decimal
1.2%
Percent
976%
Decimal
.000035%
Percent
4%
Decimal
.56%
Target 18 - Calculate the atomic mass of each element from known scientific
data.
A. Why is the atomic mass for each element written as ________________________?
B. Even though atoms are considered to be the same based on the amount of protons, they can have
different amounts of neutrons.
1. For example, a neon atom will always have 10 ________________. However, neon atoms can
have different amounts of neutrons.
2. Because of this, neon atoms will have different atomic masses.
C. The atomic mass number is calculated by the ______________________ of its abundance in nature.
D. In order to do this, you must know 3 things
1. The number isotopes of the element
2. The mass of each isotope
3. The natural percent abundance of each isotope.
Carbon
1. The number of
stable isotopes of
the element
2. The mass of
each isotope
3. The natural
percent abundance
of each isotope.
C-12
C-13
12.000
13.003
98.89%
1.11%
notes
 The average mass reflects both the mass and the relative abundance of the isotopes as they occur in nature
Calculate the average atomic mass for each element
Natural Percent Abundance of Stable Isotopes of Some Elements
Name
Notation Natural percent Mass
Average atomic mass
abundance
(amu)
Hydrogen
H-1
99.985%
1.0078
H-2
0.015000%
2.0141
H-3
0.000010000%
3.0160
Helium
Nitrogen
He-3
0.00010000%
3.0160
He-4
99.9999%
4.0026
N-14
99.630%
14.003
N-15
0.37000%
15.000
Target 19 – Explain why the atomic mass of most elements is written as a
decimal.
notes
Target 20 - Name and draw the isotopes of Hydrogen
notes
Target 21 - Evaluate the placement of hydrogen and helium on the periodic table
Notes