Download Atom Internet Scavenger Hunt

Atom Internet Scavenger Hunt
The Atom and Its Structure Answer Key
In the 5th century B.C., a Greek philosopher named Democritus proposed
that matter was made up of smaller particles and was the first person to write it
down. But he had no experimental proof. A number of scientists after this
attempted to prove Democritus’ theory. It wasn’t until the late 1700’s/ early
1800’s that John Dalton proposed that matter was composed of atoms and
conducted a number of experiments calculating atomic weights of elements.
Dalton still had not proved the existence of the atom. It wasn’t until Rutherford
and C.T.R. Wilson created an experiment using a cloud chamber. They noticed
that when gold foil was bombarded the helium nuclei deflected the particles. This
was proof gold was made up of atoms and the collision was the nucleus colliding
with a particle. Today we know the atom is the smallest known particle that keeps
its properties. Within atoms are different parts. These parts relate to patterns in
the Periodic table, are instrumental for drawing a Bohr model and a Lewis
electron dot diagram. To help you learn more about atoms and their relationship
to the Periodic Table, please print out this form then go to each website and
research the questions. All answers must be in complete sentences.
For questions 1 and 2 go to http://science-class.net/.
1. What are the three parts of an atom? (Remembering)
The atom is made up of three parts; the proton which has a positive charge (p+) and it
found in the nucleus. Also in the nucleus is the neutron which has a neutral charge (0). An
electron has a negative charge (e-) and is found in electron clouds circling the nucleus.
Science-class net. (n.d.). Atomic Structure. Retrieved from http://scienceclass.net/PowerPoints/Atomic%20Structure_files/frames.htm.
2. Draw a diagram of an atom, label each part including the nucleus and include the charges.
(Applying)
nucleus
e- = electron
0= neutron
p+ = proton
Science-class.net. (n.d.). Atomic Structure. Retrieved from
http://science- class.net/PowerPoints/Atomic%20Structure_files/frame.htm.
For questions 3 and 4 go to http://www.particleadventure.org/.
3. Describe how “quarks” got their name. (Understanding)
A quark is the smallest particle found in a proton and neutron. Murry Gell-Mann chose
the name quark which he got from James Joyce’s book, Finnegan’s Wake: “Three quarks for
Muster Mark!”
Particle Adventure Group. (2012). The naming of quarks. Retrieved from
http://www.particleadventure.org/quarknaming.html.
Continued on next page.
4. Construct a flavor chart for the 6 types of quarks and include their fractional electrical
charges. (Creating)
Up
Charm
Top
-
-
-
Down-anti-matter
Strange-anti-matter
Bottom-anti-matter
Particle Adventure Group. (2012). The Standard Model - What is the world made of? – Quarks.
Retrieved from http://www.particleadventure.org/quarks.html.
For questions 5 and 6 go to: http://www.ndt-ed.org.
5. Compare the atomic mass number of an atom to the atomic number of an atom. (Analyze)
The atomic mass number of an atom is the number of neutrons and the number of
protons in the nucleus. The atomic number is the number of protons in the nucleus.
NDT Education Resource Center. (2012). Atomic Mass and Mass Numbers. Retrieved from
http://www.ndt-ed.org/EducationResources/HighSchool/ Radiography/
atomicmassnumber.htm
6. This element is an alkali earth metal. It has 12 electrons and 12 protons. Demonstrate
your understanding of atomic mass and the atomic number by determining each and then
name the element. Then what is the relationship of the atomic number and the number of
protons? (Applying)
Atomic mass: 24
Atomic number: 12
The element is: Magnesium
This number is represented on the Periodic Table of an element at the top of the
element box and is used to identify an element.
NDT Education Resource Center. (2012). Atomic Mass and Mass Numbers. Retrieved from
http://www.ndt-ed.org/EducationResources/HighSchool/ Radiography/
atomicmassnumber.htm.
For questions 7 and 8 go to http://www.colorado.edu/physics/2000/TOC.html.
7. Define valence electrons: (Remembering)
Valence electrons are the number of electrons in the outer shell (energy level) of an
atom. They are needed to create chemical bonds.
Physics 2000. (n.d.).Atomic Structure and Chemical Reactions. Retrieved from
http://www.colorado.edu/physics/2000/periodic_table/chemical_props.html.
8. Evaluate the following statement: Atoms get bigger as you move down a Group and small
as you move to the right in a Period. If it is true explain why. If it is false explain why.
(Evaluating)
This statement is true. As you move down a Group you add an energy level. The
reason the atoms get smaller is due to the increase in the atomic number. Each element has
one more proton than its neighbor to the left. The more protons in the nucleus, the more
strongly the valence electrons are pulled in.
Physics 2000. (n.d.). Atomic Structure and Periodic Properties. Retrieved from
http://www.colorado.edu/physics/2000/periodic_table/atomic_structure.html.
For questions 9 and 10 go to http://chemicalelements.com/.
9. Classify the following elements by their group using the Periodic Table. Include the atomic
number, element symbol, atomic mass, group and period number, element classification, and
the number of valence electrons. Using what you have learned also include a Lewis dot
electron configuration. What pattern do you see? (Understanding)
The Group number tells how many valence electrons in each group.
Lithium
Beryllium
Boron
Carbon
Atomic Number: 3
Atomic Number: 4
Atomic Number: 5
Atomic Number: 6
Element Symbol: Li
Element Symbol: Be
Element Symbol: B
Element Symbol: C
Atomic Mass: 6.941=7
Atomic Mass: 9.012=9
Atomic Mass:10.811=11
Atomic Mass:12.011
Element Classification:
Element Classification:
Element Classification:
Element Classification:
Alkali Metal
Alkaline Metal
Metalloid
Non-metal
Period: 2
Period 2
Period: 2
Period: 2
Group number: 1
Group number: 2
Group number: 13
Group number: 13
Valence electron/s: 1
Valence electron/s: 2
Valence electron/s: 3
Valence electron/s: 3
Lewis dot configuration:
Lewis dot configuration:
Lewis dot configuration:
Lewis dot configuration:
Nitrogen
Oxygen
Fluorine
Neon
Atomic Number: 7
Atomic Number: 8
Atomic Number: 9
Atomic Number: 10
Element Symbol: N
Element Symbol: O
Element Symbol: F
Element Symbol: Ne
Atomic Mass: 14.007
Atomic Mass: 15.999=16
Atomic Mass: 18.998=19
Atomic Mass: 20.180
Element Classification:
Element Classification:
Element Classification:
Element classification:
Non-metal
Non-metal-Chalcogens
Non-metal-Halogen
Non-metal-Noble Gas
Period: 2
Period: 2
Period: 2
Period: 2
Group number: 15
Group number: 16
Group number: 17
Group number: 8
Valence electron/s: 5
Valence electron/s: 6
Valence electron/s: 7
Valence electron/s: 8
Lewis dot configuration:
Lewis dot configuration:
Lewis dot configuration:
Lewis dot configuration:
Chemical Elements.com. (n.d.). Periodic Table: Beryllium. Retrieved from
http://chemicalelements.com/elements/be.html.
Chemical Elements.com. (n.d.). Periodic Table: Boron. Retrieved from
http://chemicalelements.com/elements/b.html.
Chemical Elements.com. (n.d.). Periodic Table: Carbon. Retrieved from
http://chemicalelements.com/elements/c.html.
Chemical Elements.com. (n.d.). Periodic Table: Fluorine. Retrieved from
http://chemicalelements.com/elements/f.html.
Chemical Elements.com. (n.d). Periodic Table: Lithium. Retrieved from
http://chemicalelements.com/elements/li.html.
Chemical Elements.com. (n.d.). Periodic Table: Neon. Retrieved from
http://chemicalelements.com/elements/ne.html.
Chemical Elements.com. (n.d.). Periodic Table: Nitrogen. Retrieved from
http://chemicalelements.com/elements/n.html.
Chemical Elements.com. (n.d.). Periodic Table: Oxygen. Retrieved from
http://chemicalelements.com/elements/o.html.
10. Compare Halogen to Noble Gases. Make sure you include the names elements in each
group, reactivity, and the number of valence electrons. (Analyze)
Halogens are found in Group 17 on the Periodic Table. They are non-metals and are
considered salt compounds. These elements exist in all three states: liquid, solid, and gas.
There are 7 electrons in the outer shell and their oxidation number is -1 and they are
considered to be reactive. Elements in this group are Fluorine (F), Chlorine (Cl), Bromine (B),
Iodine (I), and Astatine (At).
Chemical Elements.com. (n.d.). Periodic Table: Halogens. Retrieved from
http://chemicalelements.com/groups/halogens.html.
Noble gases are found in Group 18 on the Periodic Table. They are non-metals and
are usually gases at room temperature. They are non reactive because they have complete
outer shells with 8 electrons. Due to this they seldom transfer or gain electrons and are
considered stable with an oxidation number of zero. Helium is the exception. Helium has 2
electrons in its outer shell but it is considered to have a complete outer shell. Noble gases
include: Helium (He), Neon (Ne), Argon (Ar), Krypton (Kr), Xenon (Xe), and Radon (Rn).
Chemical Elements.com. (n.d.). Periodic Table: Noble Gases. Retrieved from
http://chemicalelements.com/groups/noblegases.html.