PERIODIC TABLE - REVIEW

CHALLENGE #3

PS 16-31 - Ask Mrs. Remis for packet

PERIODIC TABLE - REVIEW

Group 1A	Known as Alkali Metals Very reactive Never found free in nature React readily with water
Group 2A	Known as Alkaline earth elements All are metals Occur only in compounds React with oxygen in the general formula EO (where O is oxygen and E is Group 2A element)
Group 3A	Metalloids Includes Aluminum (the most abundant metal in the earth) Forms oxygen compounds with a X2O3 formula
Group 4A	Includes metals and nonmetals Go from nonmetals at the top of the column to metals at the bottom All oxygen form compounds with a XO2 formula
Group 5A	All elements form an oxygen or sulfur compound with E2O3 or E2S3 formulas
Group 6A	Includes oxygen, one of the most abundant elements. Generally, oxygen compound formulas within this group are EO2 and EO3
Group 7A	Elements combine violently with alkali metals to form salts Called halogens, which mean "salt forming" Are all highly reactive
Group 8A	Least reactive group All elements are gases Not very abundant on earth Given the name noble gas because they are not very reactive

There are two main classifications in the periodic table, "groups" and "periods."

• ·         Groups are the vertical columns that include elements with similar chemical and                 physical properties.
• ·         Periods are the horizontal rows.
• ·         Going from left to right on the periodic table, you will find metals, then metalloids,             and finally nonmetals.
• ·         The 4th, 5th, and 6th periods are called the transition metals. These elements are          all metals and can be found pure in nature. They are known for their beauty and                 durability. The transition metals include two periods known as the lanthanides and           the actinides, which are located at the very bottom of the periodic table. 

CHEMISTRY - PERIODIC TABLE - ACTINIDE #10

ACTINIDE

Actinide Series of Metals

There are two rows under the periodic table: the lanthanide and actinide series. 

• The lanthanide series can be found naturally on Earth. Only one element in the series is radioactive. 
• The actinide series is much different. They are all radioactiveand some are not found in nature. 

Some of the elements with higher atomic numbers have only been made in labs. There are special laboratories across the world that specialize in experimenting on elements. Some of these particle accelerators have pounded atomic particles into elements with lower atomic numbers. The buildup of additional parts creates short-lived, high atomic number elements. 

Meet the Family

The actinide family is comprised of fifteen elements that start with actinium (Ac) at atomic number 89 and finish up with lawrencium (Lr) at number 103.
You have probably heard of plutonium (Pu), since it was used in atomic bombs. Uranium (U) is also well known for its radioactivity. They aren't all used to blow up the world. Some of them help us out every day. You can find americium (Am) is some metal detectors. 

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CHEMISTRY - PERIODIC TABLE - LANTHANIDE #9

LANTHANIDE

Lanthanide Series of Metals

When you look at the periodic table, you will see two rows that kind of sit off to the bottom. They are part of the whole table, but it is easier to print the table when they are on the bottom. One of those rows is called the lanthanide series. 
There are a bunch of names you may hear that describe these 15 elements. Some people say lanthanide, some say rare-earth metals, and some say inner-transition elements. No matter what you choose, everyone will know what you mean if you say lanthanide. 

Meet the Family

The lanthanide family is comprised of fifteen elements starting with lanthanum (La) at atomic number 57 and finishing up with lutetium (Lu) at number 71.
You might find some of these elements in superconductors, glass production, or lasers. 

CHEMISTRY - PERIODIC TABLE - TRANSITION METALS #8

Transitioning

Let's start off by telling you that there are a lot of elements that are considered transition metals. Which metals are the transition metals? 
21 (Scandium) through 29 (Copper)
39 (Yttrium) through 47 (Silver)
57 (Lanthanum) through 79 (Gold)
89 (Actinium) and all higher numbers.

What Makes Them So Special?

It all has to do with their shells/orbitals. We like introducing students to the first eighteen elements, because they are easier to explain. Transition metals are good examples of advanced shell and orbital ideas. They have a lot of electrons and distribute them in different ways. You will usually find that transition metals are shiny, too. Not all of them, but we are sure you've seen pictures of silver (Ag), gold (Au), and platinum (Pt). 

Transition metals are able to put more than eight electrons in the shell that is one in from the outermost shell. Think about argon (Ar). It has 18 electrons set up in a 2-8-8 order. Scandium (Sc) is only 3 spots away with 21 electrons, but it has a configuration of 2-8-9-2. Wow! This is where it starts. This is the point in the periodic table where you can place more than 8 electrons in a shell. You need to remember that those electrons are added to the second-to-last shells. 

The transition metals are able to put up to 32 electrons in their second-to-last shell. Something like gold (Au), with an atomic number of 79, has an organization of 2-8-18-32-18-1. Of course, there are still some rules. No shell can have more than 32 electrons. You will find it's usually 2, 8, 18 or 32 for the maximum number of electrons in an orbital. 

One More Thing

Most elements can only use electrons from their outer orbital to bond with other elements. Transition metals can use the two outermost shells/orbitals to bond with other elements. It's achemical trait that allows them to bond with many elements in a variety of shapes. Why can they do that? As you learn more, you will discover that most transition elements actually have two shells that are not happy. Whenever you have a shell that is not happy, the electrons want to bond with other elements. Example: Molybdenum (Mo), with 42 electrons. The configuration is 2-8-18-13-1. The shells with 13 and 1 are not happy. Those two orbitals can use the electrons to bond with other atoms. 

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CHEMISTRY - PERIODIC TABLE - ALKALINE EARTH METALS #7

ALKALINE METALS

Heading to Group Two

So we just covered the alkali metals in Group I. You will find the alkaline earth metals right next door in Group II. This is the second most reactivefamily of elements in the periodic table. 
Do you know why they are called alkaline? When these compounds are mixed in solutions, they are likely to form solutions with a pH greater than 7. Those higher pH levels means that they are defined as "basic" or "alkaline" solutions. 

A Family Portrait

Who's in the family? 
The members of the alkaline earth metals include: 

• beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba) and radium (Ra). 

As with all families, these elements share traits. While not as reactive as the alkali metals, this family knows how to make bonds very easily. Each of them has two electrons in their outer shell. They are ready to give up those two electrons in electrovalent/ionic bonds. Sometimes you will see them with two halogen atoms, as with beryllium fluoride (BeF₂), and sometimes they might form a double bond, as with calcium oxide (CaO). It's all about giving up those electrons to have a full outer shell. 

As you get to the bottom of the list, you will find the radioactive radium. While radium is not found around your house anymore, it used to be an ingredient in glow-in-the-dark paints. It was originally mixed with zinc sulfide (ZnS). The other elements are found in many items, including fireworks, batteries, flashbulbs, and special alloys. The lighter alkaline earth metals, such as magnesium and calcium, are very important in animal and plant physiology. You all know that calcium helps build your bones. Magnesium can be found in chlorophyll molecules. 

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CHEMISTRY - PERIODIC TABLE - ALKALI METALS #6

ALKALI METALS

Alkali Metals to the Left

Let's go to the left side of the periodic table. When looking for families, the first one you will find is the alkali metal family of elements. They are also known as the alkaline metals. 
You should remember that there is a separate group called the alkaline earth metals in Group Two. They are a very different family, even though they have a similar name. That far left column is Group One (Group I). When we talk about the groups of the periodic table, scientists use Roman numerals when they write them out. The "one" in this case refers to having one electron in the outermost orbital. 

A Family Portrait

Who's in the family? Starting at the top we find hydrogen (H). But wait. That element is NOT in the family. When we told you about families, we said that they were groups of elements that react in similar ways. Hydrogen is a very special element of the periodic table and doesn't belong to any family. While hydrogen sits in Group I, it is NOT an alkali metal. 

Family Bonding

Now that we've covered that exception, the members of the family include:

• lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs) and francium (Fr). As with all families, these elements share traits. They are very reactive. Why? They all have one electrons in their outer shell. That's one electron away from being happy (full shells). When you are that close to having a full shell, you want to bond with other elements and lose that electron. An increased desire to bond means you are more reactive. In fact, when you put some of these pure elements in water (H₂O), they can cause huge explosions. 

• The alkali metals are also metals. That seems obvious from the name. Often, in chemistry, characteristics are assigned by the way elements look. 
• You will find that the alkali group is shiny and light in weight. Their light weight and physical properties separate them from other metals. 
• They are malleable (bendable) and sometimes soft enough to be cut with a dull knife. 
• Alkali metals are not the type of metals you would use for coins or houses. 

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CHEMISTRY - PERIODIC TABLE - METALS #5

Metal Basics

We wanted to give you a big overview of metals before we get into details about specific families. 
Almost 75% of all elements are classified as metals. 

They are not all like silver (Ag), gold (Au), or platinum (Pt). Those are the very cool and shiny ones. There are other metals like potassium (K) and iridium (Ir) that you might not think about right away. 

Many Kinds of Metals

How many kinds of metals are there? So many. Don't even try to memorize them all. Just remember the ones you might need in class. 
Here's a quick list: 

• Actinide Metals, Lanthanide Metals, Alkali Metals, Alkaline-Earth Metals, Rare Metals, Rare-Earth Metals, and Transition Metals. 
• Remember, that's the easy list. Lucky for you, the periodic table is excellent at organizing elements, and you will find each of these groups in specific areas of the periodic table. 

How Do You Identify a Metal?

What are the characteristics of metals? We've got four traits that will help you identify whether an element is a metal or not: 

1. Conduction: Metals are good at conducting electricity. Silver (Ag) and copper (Cu) are some of the most efficient metals and are often used in electronics. 

2. Reactivity: Metals are very reactive, some more than others, but most form compounds with other elements quite easily. Sodium (Na) and potassium (K) are some of the most reactive metals. A metal like iron (Fe) forms iron oxide (Fe₂O₃), which you know as rust. 

3. Chemical: It gets a little complex here. Metals usually make positive ions when the compounds are dissolved in solution. Also, their metallic oxides make hydroxides (bases) (OH^-), and not acids, when in solution. Think about this example: When sodium chloride (NaCl) is dissolved in water (H₂O), it breaks apart into sodium (Na+) and chlorine (Cl^-) ions. Do you see how that sodium is the positive ion? Sodium is the metal. It works that way for other metals. Potassium chlorine (KCl) works the same way. When it is dissolved, the potassium ion (K⁺) is the positive ion. 

4. Alloys: Metals are easily combined. Mixtures of many metallic elements are called alloys. Examples of alloys are steel and bronze. 

CHEMISTRY -PERIODIC TABLE - NOBLE GASES #4

The Noble Gases

We love the noble gases. Some scientists used to call them the inert gases. It didn't really work because there are a few other gases that are basically inert but not noble gases.
Nitrogen (N₂) might be considered an inert gas, but it is not a noble gas. 

The noble gases are another family of elements, and all of them are located in the far right column of the periodic table. For all of you budding chemists, the far right is also known as Group Zero (Group 0) or Group Eighteen (Group XVIII). This family has the happiest elements of all. 

Why Are They Happy?

Using the Bohr description of electron shells, happy atoms have full shells. All of the noble gases have full outer shells with eight electrons. 
Oh, wait! That's not totally correct. At the top of the noble gases is little helium (He), with a shell that is full with only two electrons. The fact that their outer shells are full means they are quite happy and don't need to react with other elements. In fact, they rarely combine with other elements. That non-reactivity is why they are called inert. 

Who's in the Family?

All of the elements in Group Zero are noble gases. The list includes helium, neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), and radon (Rn). Don't think that, because these elements don't like to react, we don't use them. You will find noble gases all over our world. Neon is used in advertising signs. Argon is used in light bulbs. Helium is used in balloons and to cool things. Xenon is used in headlights for new cars. Because of their chemical properties, these gases are also used in the laboratory to help stabilize reactions that would usually proceed too quickly. When you move down the periodic table, as the atomic numbers increase, the elements become rarer. They are not just rare in nature, but rare as useful elements, too. 

But Wait, They Do Bond!

Some do. As of about 40 years ago, scientists have been able to make some compounds with noble gases. Some have been used in compounds to make explosives, and others just form compounds in a lab. The thing to remember is that they were forced. When going about their natural lives, you will never (well, never say never, because there may be an exception) find the noble gases bonded to other elements. 

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CHEMISTRY - PERIODIC TABLE - HALOGENS #3

Halogens on the Right

In the second column from the right side of the periodic table, you will find Group Seventeen (Group XVII). 

This column is the home of theHalogen family of elements. 

Who is in this family? The elements included are fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At). 

What Makes Them Similar?

When you look at our descriptions of the elements fluorine and chlorine, you will see that they both have seven electrons in their outer shell. That seven-electron trait applies to all of the halogens. They are all just one electron shy of having full shells. Because they are so close to being happy, they have the trait of combining with many different elements. They are very reactive. You will often find them bonding with metals and elements from Group One of the periodic table. The elements in the column on the left each have one electron that they like to donate. 

We've just told you how reactive the halogens are. Not all halogens react with the same intensity or enthusiasm. Fluorine is the most reactive and combines with most elements from around the periodic table. Reactivity decreases as you move down the column. As you learn more about the table, you will find this pattern true for other families. As the atomic number increases, the atoms get bigger. Their chemical properties change just a little bit when compared to the element right above them on the table. 

What is a Halide?

The elements we are talking about in this section are called halogens. When a halogen combines with another element, the resulting compound is called a halide. One of the best examples of a halide is sodium chloride (NaCl). Don't think that the halogens always make ionic compounds and salts. Some halides of the world are a part of molecules with covalent bonds. 

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QUIZ - HALOGENS

PERIODIC TABLE - FAMILIES #2

FAMILIES OF THE PERIODIC TABLE

Families Stick Together We just covered the columns and rows of the periodic table. There are also other, less specific, groups of elements. These groups are all over the table. Scientists group these families of elements by their chemical properties. Each family reacts in a different way with the outside world. Metals behave differently than gases, and there are even different types of metals. Some elements don't react, while others are very reactive, and some are good conductors of electricity. The columns of the periodic table are often used to define families. The noble gases are all located in the far right column of the table. That column is labeled Group Zero. Other families can be made of elements in a series. A good example of a series of elements is the transition metal family. The thing to remember is that a family of elements can be found in several ways. You need to run tests and study the elements to determine their properties. Only after that testing can you determine what family an element belongs in. Examples of Families - Alkali Metals - Alkaline Earth Metals - Transition Metals - Halogen Gases - Noble Gases Examples of Physical Properties - Density - Boiling Point - Melting Point - Conductivity - Heat Capacity Examples of Chemical Properties - Valence - Reactivity - Radioactivity PUZZLE PRACTICE

PERIODIC TABLE - INTRODUCTION #1

PERIODIC TABLE MODULES This set of modules are on the design & use of the Periodic  Table.  Proceed through each module's readings & watching the video clips for details.  Take notes as needed!!! COMPLETE the "ELEMENT of the DAY" COMPLETE the 5 (FIVE) SUPERHERO ELEMENTAL  TRADING CARDS.

INTRODUCTION TO PERIODIC TABLE CHART

The most important chemistry chart there is, and the cornerstone of science since 1869

• The Periodic Table is a chart which arranges the chemical elements in a useful, logical manner.   
• Elements are listed in order of increasing atomic number, lined up so that elements which exhibit similar properties are arranged in the same row or column as each other. 
• The Periodic Table is one of the most useful tools of chemistry and the other sciences. 

Here are 10 fun and interesting Periodic Table facts:

1. While Dmitri Mendeleev is most often cited as the inventor of the modern periodic table, his table was just the first to gain scientific credibility, and not the first table that organized the elements according to periodic properties.
2. There are 90 elements on the periodic table that occur in nature. All of the other elements are strictly man-made.
3. Technetium was the first element to be made artificially.
4. The International Union of Pure Applied Chemistry, IUPAC, revises the periodic table as new data becomes available. At the time of this writing, the most recent version of the periodic table was approved 19 February 2010.
5. The rows of the periodic table are called periods. An element's period number is the highest unexcited energy level for an electron of that element.
6. Columns of elements help to distinguish groups in the periodic table. Elements within a group share several common properties and often have the same outer electron arrangement.
7. Most of the elements on the periodic table are metals. The alkali metals, alkaline earths, basic metals, transition metals, lanthanides and actinides all are groups of metals.
8. The present periodic table has room for 118 elements. Elements aren't discovered or created in order of atomic number. Scientists are working on creating and verifying element 120, which will change the appearance of the table.
9. Although you might expect atoms of an element to get larger as their atomic number increases, this does not always occur because the size of an atom is determined by the diameter of its electron shell. In fact, element atoms usually decrease in size as you move from left to right across a row or period.
10. The main difference between the modern periodic table and Mendeleev's periodic table is that Mendeleev's table arranged the elements in order of increasing atomic weight while the modern table orders the elements by increasing atomic number.

We sometimes use the terms atom and element to mean the same thing.

As far as we know, there are only so many basic elements. Up to this point in time, we have discovered/created over 120. While there may be more out there to discover, the basic elements remain the same.

Iron (Fe) atoms found on Earth are identical to iron atoms found on meteorites. The iron atoms on Mars that make the soil red are the same too. 

With the tools you learn here, you can explore and understand the Universe. You will never stop discovering new reactions and compounds, but the elements will remain the same. 

The List of Elements

Let’s start with 18 ELEMENTS.   "Why start with 18?"  Because the rules for the first eighteen elements are very straightforward: 

1)       Electrons fit nicely into three shells.

·          Remember that the shells are the places you will find the electrons as they spin around the nucleus. 

2)           These elements make up most of the matter in the Universe.

3)           It's a lot easier to remember facts about 18 elements than over 100 elements.

Who are we kidding? We know you want information on more than eighteen elements. We've added the next 18 elements from the fourth period (row) of the periodic table. You need to remember that this is the first row with transition elements. The transition metals have electron configurations that are a little different from the first 18 elements. Make sure you understand the first 18 before you move on to this set. 

Elements as Building Blocks

As you probably saw, the periodic table is organized like a big grid. The elements are placed in specific locations because of the way they look and act. If you have ever looked at a grid, you know that there are rows (left to right) and columns (up and down). The periodic table has rows and columns, and they each mean something different. 

You've got Your Period/Rows...

REVIEW

Even though they skip some squares in between, all of the rows go left to right. When you look at a periodic table, each of the rows is considered to be a different period (Get it? Like PERIODic table.).

In the periodic table,

·          elements have something in common if they are in the same row.

·          All of the elements in a period have the same number of atomic orbitals.

Every element in the top row (the first period) has one orbital for its electrons.

All of the elements in the second row (the second period) have two orbitals for their electrons.

It goes down the periodic table like that. At this time, the maximum number of electron orbitals or electron shells for any element is seven. 

...and Your Groups

Now you know about periods. The periodic table also has a special name for its columns.

·        When a column goes from top to bottom, it's called a group.

·        The elements in a group have the same number of electrons in their outer orbital.

·        Those outer electrons are also called valence electrons. They are the ones involved in chemical bonds with other elements. 

Every element in the first column (group one) has one electron in its outer shell. Every element in the second column (group two) has two electrons in the outer shell. As you keep counting the columns, you'll know how many electrons are in the outer shell. There are some exceptions to the order when you look at the transition elements, but you get the general idea. Transition elements start to add electrons to the second-to-last shell. 

Two at the Top

Hydrogen (H) and helium (He) are special elements. 

Hydrogen can have the talents and electrons of two groups: one and seven. To scientists, hydrogen is sometimes missing an electron, and sometimes has an extra one. 

Helium is different from all of the other elements. It can only have two electrons in its outer shell. Even though it only has two, it is still grouped with elements that have eight (i.e., noble gases).

The noble gases and helium are all "happy," because their outermost electron shell is full. The elements in the center section are called transition elements. They have special electron rules too. 

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