NFDMS 4/14

For today, answer the following questions using the periodic table site that we created last class period.

1. If a new element is discovered, could it be placed between oxygen and fluorine on the periodic table? Why or why not? (hint: what does the atomic number tell us about an element?)

2. How many valence electrons do the elements in group 1 have?

3. How many valence electrons do the elements in group 2 have?

4. How many valence electrons do the elements in group 13, 14, 15, 16, 17, and 18 have?

5. What is the charge of elements in group 1?

6. What is the charge of elements in group 2?

7. What is the charge of elements in group 13, 14, 15, 16, 17, and 18?

8. A positive charge on an element represents that element's desire to lose an electron. A negative charge represents that element's desire to gain an electron. With this in mind, which group of elements are the happiest the way that they are?



Sometime next week, I will be giving a quiz for the names (spelling counts!) and chemical symbols (capitalization counts!) of the first 20 elements. Basically, if I give you N, you would write Nitrogen. If I give you Sodium, you would write Na. Fairly simple. The quizlet below is a good way to study, but make sure you quiz yourself on both names and symbols.

NFDMS 4/12

Refer to the email that you received about this project to make sure that you are editing the correct element on the wiki. Do not edit any element's page but the one that you are assigned and do not comment on anyone else's element page.

For the element that you have been assigned, you will be editing a page on the "Periodic Table" wiki that I have created. On the table, click on your element and then copy and paste the information below. Then, replace the italicized sections with the information relevant to your element. I have done Xe (found here) for you as an example. If you need help figuring out what any of the sections are talking about, please go to the Periodic Table Help Page

Atomic Number – Your Name
Element Symbol
Element Name
Atomic Mass (2 decimals)

# Electrons
# Protons
# Neutrons

Metal, Semi-metal, or Non-metal (Metalloid)?

Period: Number
Group: Number
Group Name

# Valence Shell Electrons

Dot Structure
. .
: ? :
. .

Charge: ?

ODMS 3/16 & NFDMS 3/17

Today we are going to take a closer look at what different atoms are made of and how to navigate each box found on the periodic table. Please carefully read the passage below and then ask Mrs. Pelkey (ODMS) or Mrs. Oatman (NFDMS) for your handout once you understand what you have read. Please feel free to work with the people around you to figure out what the passage means before getting your handout.

I say this with all the love that I can; you have the right to be confused for no more than 10-15 minutes. After that, you just aren't trying hard enough ;)

Things to remember from the notes:
- Elements are made up of protons, neutrons, and electrons
- Protons and neutrons have the same mass
- Electrons are about 1/2000th the mass of a proton or a neutron, so they are ignored when talking about mass

Reading the Periodic Table: Carbon

To describe the information contained within each individual box we will use a specific example: carbon.
external image carbon.gif

Element Name

The purpose of the element name is obvious. However, many Periodic Tables do not include element names. For those situations you must memorize the symbols that accord to each element name.

Element Symbol

Each element has a specific one or two letter symbol that is used interchangeably with its name. These should be memorized. Most of the time, symbols quite clearly accord to the name of the element they represent, as C accords to carbon. Occasional, however, an element's name and symbol have little relation. For example, the symbol for mercury is Hg.

Atomic Number

As you move across a period the atomic number increases. Similarly, as you move down a group the atomic number increases. In this way, the atomic number represents exactly where in the periodic table an element stands.
More importantly, and the reason why the ordering of the elements according to atomic number yields elements in groups with similar chemical and physical properties, the atomic number is the same as the number of protons in the nucleus of an atom of an element, and also the same as the number of electrons surrounding the nucleus in a neutral state. Carbon, for example, has six protons and six electrons. (Protons and electrons will be discussed in more detail in the Atomic Structure SparkNote)

Atomic Weight

Along with protons, an atom also contains neutrons in its nucleus. The atomic mass (also called atomic weight) of an element is the combined number of protons and neutrons in the nucleus.
Atoms of particular elements generally have different "versions," meaning that elements have atoms with different numbers of neutrons in their nucleus. These different versions are called isotopes. The atomic weight displayed is actually the weighted average of the mass numbers of the various isotopes. The atomic weight for Carbon is 12.01 because around 99% of all carbon is the carbon-12 isotope. To use this number for finding the number of protons, neutrons, or electrons you simply round to the nearest whole number.

So, here are a few things to remember for your assignment:
Atomic mass = protons + neutrons
Atomic number = protons
protons = electrons
neutrons = atomic mass - protons
You will need to use this link to a periodic table, or you may use the one that is on the back cover of your textbook.
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