Name _____________________ Block___ Date ________ Handout# ___
Chemistry Quest
Part 1. Subatomic Particles
Objective: To create a chart that summarizes the characteristics of the three types of subatomic
particles. Include, location, charge, mass, relative mass and function.
Materials: ruler, unlined paper, pencil.
Assignment 1-1
a. On a separate sheet of unlined paper, use a ruler and pencil to draw a chart summarizing
the characteristics of the three subatomic particles – protons, neutrons and electrons.
Include location, charge, mass, relative mass and function.
b. Create a chart in WORD or Excel as per instructions in part a.
Characteristics of Protons, Electrons and Neutrons
ATOM
Fundamental particles of atom are electron, proton and neutron – AKA subatomic particles
The center of an atom is called the nucleus. The nucleus contains the protons and neutrons.
The electrons circle around the nucleus of an atom in different orbits or shells
These subatomic particles
CHARACTERISTICS
OF ELECTRONS
Charge: It is a negatively charged particle.
Mass of electron: Mass of electron is 0.000548597 a.m.u.
Comparative mass: For our purposes the mass is so small it doesn’t factor
into the atomic mass of the atom! About 1/1800 the size of a proton.
Location in the atom: Electrons revolve around the nucleus of atom in different orbits.
Function: The most outer electrons are responsible for the bonding with other atoms.
CHARACTERISTICS
OF PROTONS
Charge: Proton is a positively charged particle.
Mass of proton: Mass of proton is 1.0 amu (atomic mass unit)
Comparative mass: Proton is about 1800 times heavier than an electron.
Position in atom: Protons are present in the nucleus of atom.
Function: The number of protons in an atom determines its identity.
CHARACTERISTICS
OF NEUTRONS
charge: It is a neutral particle because it has no charge.
Mass of neutron: Mass of neutron is 1.0 amu
Comparative mass: Neutron is 1800 times heavier than an electron.
Location in the atom: Neutrons are present in the nucleus of an atom.
Function: Neutrons act like “glue” holding the nucleus together.
Adapted from - (http://www.citycollegiate.com/atomic_structureXIg.htm)
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Assignment 1-2: Quiz yourself for homework: Copy and paste the link below. Watch the
video, take notes and test yourself. Print the final page with your score!
http://studyjams.scholastic.com/studyjams/jams/science/matter/atoms.htm
Part 2- How many PENS’ inside an atom?
Objective: To be able to determine the number of protons, neutrons and electrons in any atom
on the PTE.
Materials – Paper, pencil, PTE.
Procedure: To find the number of protons, electrons and neutrons in an atom, just follow these
easy steps:
Step 1 - Gather Information
The first thing you will need to do is find some information about your element.
Use the Table of Elements to find your element's atomic number and atomic mass. The atomic
number is the number located in the upper left corner, top center or sometime right-hand corner
of a PTE. The atomic mass (weight) is the number located on the bottom, as in this example for
krypton: It is easily distinguished from the atomic number because it contains a decimal and is
always larger.
Step 2 - The Number of Protons is...
The atomic number is equal to the number of protons in an atom of an element. In our
example, krypton's atomic number is 36. This tells us that an atom of krypton has 36 protons in
its nucleus.
The interesting thing here is that every atom of krypton contains 36 protons. If an atom
doesn't have 36 protons, it can't be an atom of krypton. Adding or removing protons from the
nucleus of an atom creates a different element. For example, removing one proton from an
atom of krypton creates an atom of bromine.
Step 3 - The Number of Electrons is...
By definition, atoms have no overall electrical charge. That means that there must be a
balance between the positively charged protons and the negatively charged electrons. Atoms
must have equal numbers of protons and electrons. In our example, an atom of krypton must
contain 36 electrons since it contains 36 protons.
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Step 4 - The Number of Neutrons is...
The atomic weight is basically a measurement of the total number of particles in an atom's
nucleus.
The mass number is a count of the number of particles in an atom's nucleus. Remember that
the nucleus is made up of protons and neutrons and that the mass of a single proton or neutron
is 1 amu (atomic mass unit).
Mass Number = (Number of Protons) + (Number of Neutrons)
For krypton, this equation becomes:
84 = (Number of Protons) + (Number of Neutrons)
If we only knew how many protons krypton has, we could figure out how many
neutrons it has. Wait a minute... We do know how many protons krypton has! We
did that back in Step 2! The atomic number (36) is the number of protons in
krypton. Putting this into the equation, we get:
84 = 36 + (Number of Neutrons)
What number added to 36 makes 84? Hopefully, you said 48. That is the number
of neutrons in an atom of krypton.
The interesting thing here is that adding or removing neutrons from an atom does
not create a different element. Rather, it creates a heavier or lighter version of that
element. These different versions are called isotopes and most elements are
actually a mixture of different isotopes.
If you could grab atoms of krypton and count the number of neutrons each one
had, you would find that most would have 48, others would have 47, some would
have 50, some others would have 46, a few would have 44 and a very few would
have 42. You would count different numbers of neutrons because krypton is a
mixture of six isotopes. This explains why the atomic mass number is a decimal –
it’s the average number of neutrons in any given sample of that element.
In Summary...
For any element:
Number of Protons = Atomic Number
Number of Electrons = Number of Protons = Atomic Number
Number of Neutrons = Mass Number - Atomic Number
For krypton:
Number of Protons = Atomic Number = 36 3
Number of Electrons = Number of Protons = Atomic Number = 36
Number of Neutrons = Mass Number - Atomic Number = 84 - 36 = 48
Assignment 2-1
Find the number of subatomic particles for each of the following types of atoms
Atom Name___Krypton___ Number _36___ Mass 83.80____
Calculation for N’s
84
- 36
48
a. P= _36___
b. E= _36___
c. N= _48____
Atom Name___Helium___ Number _____ Mass _____
Calculation for N’s
d. P= _____
e. E= ______
f. N= ______
Atom Name _Oxygen_____, Number _____ Mass _______
a. P= _____
Calculation for N’s
b. E= ______
c. N= ______
Atom Name __magnesium_, Number _____ Mass _______
a. P= _____
Calculation for N’s
b. E= ______
c. N= ______
Atom Name _Gold___,
Number _____ Mass _______
a. P= _____
Calculation for N’s
b. E= ______
c. N= ______
Assignment 2-2: Test yourself: http://education.jlab.org/elementmath/question.php?96146754
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Part 3- the Drawing Bohr Model of an Atom
The Bohr Model of an Atom
Orbits or shells
nucleus
Electron Shell Capacity
Electron shell capacity is used to find how many electrons can fit in each shell around an atom.
Electron Shell/Orbit Capacity
Shell Number (Shell letter) Maximum no of Electrons in each Shell (2n2)
1 (K) (closest to nucleus)
2 (1) 2 = 2
2 (L)
2 (2) 2 = 8
3 (M)
2 (3) 2 = 18
4 (N)
2 (4) 2 = 32
5 (O) (farthest from nucleus 2 (5) 2 = 50
Note – Equation for electron shell capacity = 2n2
(n= shell number)
Directions for Drawing Bohr Models
1.
2.
3.
4.
5.
6.
7.
Determine the number of protons, electrons and neutrons of the selected atom
Draw a circle for the nucleus – size of a quarter
Write the number of protons and neutrons in the nucleus using coefficients- see Na.
Using the shell capacity table, add electrons starting with the most inner shell.
Continue filling shells until shell capacity is reached or you have used up the electrons.
For atom less than atomic number 12 (Mg), draw individual electrons.
For atoms with an atomic number 12 or greater, use coefficients for electrons (2e or 7e).
Note- Drawing atoms is usually more complicated than just filling up the orbits from the most inner (1) to the
most outer. However, for our purposes this will suffice. See my website for a more detailed explanation.
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Atomic Numbers 12 or greater Use Coefficients
2e
3e
16P
16N
Assignment 3-1 – Drawing Bohr Models
1. Write your name, block and date across the top of an unlined sheet of paper.
2. Use a ruler to divide the paper into quarters.
3. Use the above framework for each model – draw only as many shells as is needed.
4. Follow the directions on the previous page.
5. DTL a Bohr model diagram of Helium, Oxygen, Magnesium and Gold.
Part 4 -The Periodic Table of Elements
Our current periodic table lists 118 elements. It is arranged according to the
periodic law. The Periodic Law states that the physical and chemical
properties of the elements repeat themselves in a predictable way when the
elements are arranged in order of increasing atomic number.
Basic Arrangement of Elements
1. Elements are arranged in order of increasing atomic number (protons)
2. The most basic categories of elements are the metals, metalloids and nonmetals
3. Elements in the vertical column are called families or groups and have similar
properties as well as the same number of electrons in their most outer shell.
4. Elements in the horizontal rows or periods have different properties but the same
number of shells. The periods are also numbered 1 – 7 (not shown below)
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Assignment 4-1
Materials – periodic table handout page #1 in your binder, pencil and coloring pencils
Part a.
1) Using a pencil draw the “Zig-Zag line onto your own PTE (handout #1)
2) Get teacher okay – then trace the “zig-zag” line with a red coloring pencil.
3) See PTE below and shade in the elements that are metalloids (blue).
4) Shade in nonmetals – red, orange or yellow
5) Shade families/groups 1 - 12 as metals (green)
6) Continue shading in metals that are not metalloids in families 13-16.
7. Outline in red all gases, blue all liquids.
The Periodic Table
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Part b.
8.
9.
10.
11.
12.
On a separate sheet of lined paper, write name block and date.
Title it Families on the Periodic Table
Draw a T- chart as if you are doing Cornell Notes
Topic is Families/Groups
Substopics are
1. Group 1 – Alkali Metals
2. Group 2- Alkaline Metals
3. Groups 3-12 Transition Metals
4. Group 14 – Carbon family
5. Group 18 – Noble gases
13. Use pages 87-101 in Prentic Hall’s, Chemical Building Blocks to find at least two examples of
each group and two characteristic of all elements in that group.
Assignment 4-2
Complete the Alien Periodic Table Assignment on pages 102 and 103 of the text.
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