Mr. Bouyer

Day 1 | Day 2 - 3 | Lab | 11th Grade TAKS Test

In this chapter our book revisits the periodic table for an even closer look. Most should be a review for you, but there will be a few new concepts developed. Review of things you should already know. Know the history of the development of the periodic table. Know the chemical symbols and names of the 50 most commonly used elements. Use atomic numbers and mass numbers to determine the number of electrons, protons, and neutrons in an atom. Read the following information directly from the periodic table: Whether an element occurs naturally or is man-made. The physical state of an element at room temperature. Whether and element is a metal or nonmetal. How the chemical activity of one element relates to another element. The members of each family of elements. The oxidation number of an atom. Electron energy levels, sublevels, and orbitals. The electron configuration of an atom. New Information: Periodic Properties

The 1954
Periodic Table
showing elements 1-98

The 1964 edition added
elements 99-103

The 1994 edition added
elements 104-109

168 elements??

Review the development of the periodic table from physical science class.
The table is based on current atomic theory. Review how the atomic theory has changed.

The periodic table contains a wealth of chemistry information, if you know how to read it. Freshman physical science students begin learning to read the periodic table. Chemistry students must expand their understanding of the information on the table. Your science facilitator will provide a periodic table that may be used in any way you wish. Make notes on the front and back and use it at any time to make your life easier this year. If you forget to bring it to class, or if it is lost, it may not be replaced. This paper table and the class wall table are the only ones that are always available for use during class. You may keep the table in a pocket of your portfolio, but do not fasten it into the portfolio. Do not share your table with anyone during class.

Ask Mr. Bouyer for a periodic table and begin making careful study notes on it. Do not fasten the periodic table into the clips of your portfolio.

This periodic table is linked at the bottom of each of the chemistry class nine-weeks pages and this periodic table is at the bottom of the physical science class nine-weeks pages. These websites have a wealth of information about each element, but are not available during the times you have been asked to keep your computers turned off.

• Element name:

  Many periodic tables do not have the name of the elements in each square. For this reason you should be familiar with the names and symbols of the most commonly used elements.

• Chemical symbol:

  The one or two letter symbol. The first letter always capital case, the second letter always small case. Do not be sloppy as you write chemical symbols.

• Atomic number:

  The whole number in every square. There is no standard for the location of the information in each square. Different periodic tables may have a different arrangement.

• Mass number:

  The number with a decimal fraction in most sqares. In most squares, this number represents the average of all isotopes. If the number is a whole number, it represents the most stable isotope. In our class, always round off the decimal fraction to the nearest whole number for any question about the mass number of an element.

• Number of protons in atom:

  Always equal to the atomic number. If the number of protons change, the element becomes another element.

• Number of electrons in atom:

  Equal to the atomic number in a normal atom. The numbers of electrons are easily changed within an atom. If the chemical symbol is written with a charge, representing an ion, the charge indicates the number of electrons that have been added or removed.

• Number of neutrons in atom:

  Subtract the atomic number from the mass number to find the number of neutrons. To do this calculation in our class, round off the average mass number to the nearest whole number before doing the subtraction. There is never a fraction of a neutron in an atom.

• Review the quark model of subatomic particles from Physical Science Class.

  The actual mass of subatomic particles is so small that it is usually expressed in a unit known as electron volts. An electron volt is a measure of energy equal to the energy gained by a single electron when it is accelerated across an electric potential difference of 1 volt: 1 eV = 1.602 X 10 ^-19 joules. Because this unit is so small, it is commonly expressed as keV (thousand), MeV (million), or GeV (billion).

  Since Einstein showed that mass and energy are interchangeable, dividing electron volts by the square of the speed of light gives a mass. By substituting 1 for the constant speed of light, electron volts becomes a mass. While this substitution may seem odd, it is commonly done with constants (natural units) in complicated calculations. The exact numbers can be replaced at the end of the calculation to give a numerical value to the final answer.

  The mass of an average sized person would be 4 X 10 ³¹ MeV, which is another way of saying that the average person is made up of about 4 X 10 ²⁸ baryons.

  • The mass of an electron is 0.5110 MeV.
  • The mass of a proton is 938.2796 MeV.
  • The mass of a neutron is 939.5729 MeV.

Homework Assignment 031:
This assignment must be turned in by the beginning of class tomorrow to receive credit.
Scoring criteria

1. Where did the word "atom" come from?
2. How do Mendeleev's and Meyer's Tables differ?
3. Why is today's periodic table shaped the way it is?
4. What would cause the shape of the periodic table to be changed again?
5. Use the periodic table to fill in the blank squares on the following table:

Day 2 - 3

• Natural and manmade elements:

  There are different colors of chemical symbols on some periodic tables. Our class wall table shows manmade elements with a white (black outline) chemical symbol. All other elements are naturally occuring elements.

• Physical state of the element at room temperature:

  There are different colors of chemical symbols on some periodic tables. Our class wall table shows solid elements with black chemical symbols, liquid elements with blue chemical symbols, and gas elements with red chemical symbols.

• Metals and nonmetals:

  Some periodic tables have a line dividing these two, our class wall table does not. The dividing line begins between boron and aluminum and stair-steps down and to the right, one square at a time. Metals are left of the line, nonmetals are to the right.

• Chemical activity:

  • Metals increase in chemical activity as you go from right to left on a horizontal row and from top to bottom in a vertical column.
  • Nonmetals increase in chemical activity as you go from left to right on a horizontal row and from bottom to top in a vertical column.
  • The elements in the far right-hand column on the periodic table are chemically inert.

  
   
• Families of elements:

  Families contain elements with similar characteristics, usually determined by the number of electrons in the outer electron energy level. Families on the periodic table are in vertical columns called "groups". Some resources will identify 10 families. We will recognize only 9 families in this class. The difference involves the placement of the Lanthanoid Series (elements 57 - 71) and Actinoid Series (elements 89 - 103). Some references will place these two series in a family known as the "Rare-earth Metals". We will consider them as part of the "Transition Metal Family".

Group #	Family Name & Notes	Elements in the Family
1	Alkali Metals	H, Li, Na, K, Rb, Cs, Fr
2	Alkaline Earth Metals	Be, Mg, Ca, Sr, Ba, Ra
3 - 12	Transition Metals Including the Lanthanoid and Actinoid Series (Rare Earth Metals)	See this periodic table
This family includes the "precious metals". Current New York Prices.
13	Boron Group	B, Al, Ga, In, Tl
14	Carbon Group	C, Si, Ge, Sn, Pb
15	Nitrogen Group	N, P, As, Sb, Bi
16	Oxygen Group	O, S, Se, Te, Po
17	Halogens	F, Cl, Br, I, At
18	Noble Gases	He, Ne, Ar, Kr, Xe, Rn

• Oxidation number:

  The table below shows the elements and oxidation numbers that can be read from the periodic table.

  Column #	Elements	Oxidation #
  1	All	+ 1
  2	All	+ 2
  3 - 12	Silver	+ 1
  13	Aluminum	+ 3
  14	Carbon & Silicon	+ or - 4
  15	Nitrogen & Phosphorus	- 3
  16	Oxygen & Sulfur	- 2
  17	All	- 1
  18	All	0

  
  An element's oxidation number, sometimes called valence, is the number of electrons gained or lost by an atom when forming compounds. This characteristic is controlled by the electrons in the outer energy level. Atoms gain or lose electrons to get eight electrons in their outer shell. Elements with a positive oxidation (usually metals) number lose electrons when forming compounds. Elements with a negative oxidation number (usually nonmetals) gain electrons when forming compounds.

• Electron energy levels:

  The number of electron energy levels in an atom is indicated by the horizontal row on which the element is found on the periodic table. The horizontal rows are numbered 1 to 7, at the extreme left of the table.

• Electron energy sublevels:

  The shape of the periodic table makes the four sublevels easy to see.

  

  • s sublevel - the two tall columns on the left.

    Helium is at the far right because it is inert. For the purpose of reading sublevels, it should be thought of as sitting in the second column beside hydrogen.

  • p sublevel - the six tall columns on the right, without helium.
  • d sublevel - the ten short columns in the middle of the table.
  • f sublevel - the fourteen columns of two below the body of the table.

  One thing that does not show on the periodic table is the overlap of some sublevels. Both the d and f sublevels overlap the s sublevel of the next lowest electron energy level.

  • Even though the first elements in the d sublevel on the periodic table are on the fourth row, the first electron energy level to have a d sublevel is the third energy level.
  • Even though the first elements in the f sublevel on the periodic table are on the fifth row, the first electron energy level to have an f sublevel is the fourth energy level.

• Orbitals within sublevels:

  An orbital can hold two electrons. Within an electron energy sublevel on the periodic table, each orbital is represented by two element squares.

• Electron configuration:

  Electron configurations can be read directly from the periodic table. This concept will be covered in detail next week.

• Element name:

  Many periodic tables, including our class table, do not have element names on them. You already know many element names and you will learn more as you use them this year. However, you might find it worth your time to write the names into the element squares on your periodic table.

In-class Assignment 033:
This assignment must be turned in by the end of class tomorrow to receive credit.
Scoring criteria

1. What is the first nonmetal on the fourth row of the periodic table?
2. What is the man-made element with the lowest atomic number?
3. Name one element that is a liquid at room temperature.
4. Determine which element in each of these pairs is the most active:
   1. magnesium or barium
   2. chlorine or bromine
   3. manganese or iron
   4. lithium or potassium
   5. nitrogen or phosphorus
5. Is silicon a metal or nonmetal?
6. To what chemical family does iodine belong?
7. What transition metal can be trusted to always have only one valence electron?
8. How many electron energy levels are in an atom of tin?
9. How many columns on the periodic table represent p sublevel electrons?
10. How many orbitals are in the d sublevel?

Research Links:

• A Periodic Table - Quick and Easy
• A Periodic Table - Lots of display options
• Interactive Periodic Table - Chemical Elements.Com
• Fill in a blank table - University of Kentucky