3.) Determine the number of protons, neutrons, and electrons, and the mass of an element using the periodic table. Locating metals, nonmetals, metalloids, and noble gases on the periodic table Locating metals, nonmetals, metalloids, and noble gases on the periodic table Using data about the number of electrons in the outer shell of an atom to determine its reactivity Using data about the number of electrons in the outer shell of an atom to determine its reactivity

Give the elemental symbol for the elements below: Give the elemental symbol for the elements below: 1Hydrogen 2Sulfur 3Flourine 4Helium 5Silicon 6Boron 7Carbon 8Nitrogen 9Sodium 10Calcium

Give the elemental symbol for the elements below: Give the elemental symbol for the elements below: 1HydrogenH 2SulfurS 3FluorineF 4HeliumHe 5SiliconSi 6BoronB 7CarbonC 8NitrogenN 9SodiumNa 10CalciumCa

  You are going to create a seating chart for the students in this class. The purpose is to organize the class in rows or groups.  You can group them any way that you want, but you must have a reason for placing each student where you place them.  Write the name of each of your classmates in the place that you think they should sit.  Now, explain why/how you grouped the students the way that you did. Start-Up Activity

  Suppose that you went to a movie store and all the dvd’s were mixed together. How could you tell the comedies from the action movies? If the dvd’s were not arranged in a pattern, you wouldn’t know what kind of movie you had chosen! Arranging the Elements

  I need 3 volunteers!  Two stand that the front next to each other.  Let’s list characteristics that they share.  Swap one student out for the third.  Let’s list characteristics that they share.  Now, let’s compare the two lists.  What are the similarities and differences? Demonstration

  The Puzzle The Puzzle Jot Notes

  Scientists in the early 1860s had a problem.  At that time, scientists knew of some of the *properties of more than 60 elements.  No one had organized the elements according to these properties.  Organizing the elements according to their properties would help scientists understand how elements interact with each other. *property-An attribute, characteristic, or quality

  1869….Dmitri Mendeleev  (Russian teacher and chemist)  Discovered a pattern in the elements  Wrote the names and properties of the elements on cards  Arranged them in many different ways (density, appearance, melting point, etc.)  After much thought, he arranged them in order of increasing atomic mass Mendeleev’s Periodic Table

  Mendeleev had arranged elements based on increasing atomic mass. How had Mendeleev arranged elements when he noticed a pattern?

  Mendeleev saw that when the elements were arranged in order of increasing atomic mass, those that had similar properties occurred in a repeating pattern.  This is the pattern that was periodic.  Periodic means “happening at regular intervals”  Example:  The days of the week are periodic. They repeat in the same order every 7 days.  Similarly, Mendeleev found that the elements’ properties followed a pattern that repeated every 7 elements.  His table became known as the periodic table of the elements. Periodic Properties of the Elements

  The Genius The Genius Jot Notes

He called this element eka-Aluminum. Later it was renamed Gallium after its discovery in 1875 Mendeleev’s first try at arranging the elements.

  In approximately twenty words, explain what we discussed today. GIST

  Who was credited with the development of the periodic table? Bell Ringer

  The question marks show gaps in the pattern.  Mendeleev predicted elements that had not been found yet.  He used the pattern he found to predict their properties.  By 1886, all of the gaps had been filled.  His predictions were right. Predicting Properties of Missing Elements

  1914, Henry Moseley  British Scientist  Determined the number of protons –the atomic number-in an atom  Redesigned the periodic table to be arranged by atomic number

 “Periodic” - Repeating patterns  Listed in order of increasing number of protons (atomic #)  Properties of elements repeat  Periodic Law-  Periodic Law- when elements arranged by increasing number of protons, properties repeat in pattern The Modern Periodic Table

  Turn to page in your book.  You are going to work in a small group to answer the following questions.  1. What information does each square on the periodic table show?  2. How many elements are liquid at room temperature?  3. How many elements are gases at room temperature?  4. How many elements are metals?  5. How many elements are metalloids?  6. How many elements are nonmetals?  7. How many groups are the elements divided into?  8. How many periods are the elements divided into? Co-op Learning Activity Worksheet

  What are periods in regards to the periodic table?  Who came up with the modern version of the periodic table?  What did he do differently? Exit Slip

  What is the atomic number for Chlorine?  How many protons are in an atom of Na? Bell Ringer

  At first glance, you might think studying the periodic table is like trying to explore a thick jungle without a guide– you can easily get lost! However, the table itself contains a lot of information that will help you along the way.  Elements are classified as metals, nonmetals, and metalloids, according to their properties.  The number of electrons in the outer energy level of an atom is one characteristic that helps determine which category an element belongs in.  The zigzag line on the periodic table can help you recognize which elements are metals, which are nonmetals, and which are metalloids. The Periodic Table and Classes of Elements

Metals, Nonmetals, Metalloids

Foldable  Create a 3 Panel Flip Chart  Fold your paper hot dog style  Make two cuts on one side only  Label the flaps Metal, Nonmetal, and Metalloid

 Most elements are metals.  They can be found to the left of the zigzag line on the table.  Atoms of most metals have few electrons in their outer energy level.  Most are solid at room temperature.  Mercury is a liquid at room temperature. Metals

  Metals are usually shiny ( luster ).  Mirrors have a thin coat of silver  Ductile -can be drawn into thin wires  Conductors - good for electricity and thermal energy  Malleable -can be flattened with a hammer and will not shatter Properties of Metals

 Found to the right of the zigzag line on the table  Atoms of most nonmetals have an almost complete set of electrons in their outer level.  Atoms of the elements in Group 18, the noble gases, have a complete set of electrons.  More than half of the nonmetals are gases at room temperature. (low boiling point)  Properties are generally opposite of metals Non-Metals

  Poor conductors of heat and electricity  Low boiling points  Many are gases at room temperature but can be found in solid or liquid form also  Not Malleable -Solid, non- metals are brittle (break easily)  Not Lustrous- not shiny  Chemical properties vary Non-Metals

 Also called Semiconductors  conduct electric current more easily than nonmetals but less easily than metals  Border the zigzag line on the table  Have a bout half of a complete set of electrons in their outer energy level  Have properties similar to metals and non-metals Metalloids

  Tellurium is shiny, but it is brittle and can be easily smashed into a powder.  Boron is almost as hard as a diamond, but it is also very brittle. At high temperatures, it is a good conductor of electrical current. Metalloids

 Decoding the Periodic Table

Element Key Important information about an element is given in each square of the periodic table:  its atomic number  chemical symbol  element name  average atomic mass 6 C Carbon For example: Carbon has atomic # 6 (or has 6 protons), an average atomic mass of and a symbol of C

One Pager  You have one page to summarize what we have learned today.  Be accurate.

Bell Ringer  What is the atomic mass for Boron?  How many electrons are in an atom of Cl?

Periods vs. Groups

 Physical and Chemical properties of elements in a row follow a repeating or periodic pattern as you move across the period.  Metallic properties decrease as we move to the right  Ability to lose an electron decreases  Ability to gain electrons increases Variation Across a Period: Left to Right



-horizontal (left – right) -called a period -properties change greatly across period -first element in period is very active metal -last element in most periods is noble gas -7 periods (number them on your periodic table) Rows in the Periodic Table

-vertical (top to bottom) -called groups or families -numbered 1-18 or 1A through 8A -elements in same family have similar properties Columns in the Periodic Table

  Mendeleev developed the first periodic table by listing the elements in order of increasing atomic mass.  He used his table to predict that elements with certain properties would be discovered later. Summary

  Properties of elements repeat in a regular, or periodic, pattern. Summary

  Moseley rearranged the elements in order of increasing atomic number. Summary

  The periodic law states that the repeating chemical and physical properties of elements relate to and depend on elements’ atomic numbers. Summary

  Elements in the periodic table are classified as metals, nonmetals, and metalloids. Summary

  Each element has a chemical symbol.  A horizontal row of elements is called a period.  Physical and chemical properties of elements change across each period. Summary

  A vertical column of elements is called a group or family.  Elements in a group usually have similar properties. Summary

  Complete the worksheet. Directed Reading B Worksheet

How do you know that a bird is a bird, that a kangaroo is a kangaroo, and that a shark is a shark? What characteristics of each animal help you to tell the animal apart?

  Write what you know about how the groups on the periodic table are organized.  Write what you would like to know more about. K-W-L chart

  You probably know a family with several members who look a lot alike. The elements in a family or group in the periodic table often—but not always— have similar properties. Grouping the Elements

 outermost e-’s  Responsible for chemical properties  Elements in same group have same # of VE  ALL atoms want full outer energy level (usually 8 VE)  To get full outer energy level, some elements:  lose e- (metals)  gain e- (non-metals)  share electrons (some non-metals & metalloids) What exactly are Valence electrons?

  Atoms will often take, give, or share electrons with other atoms in order to have a complete set of electrons in their outer energy level. (We called these ions.)  Elements whose atoms undergo such processes are called reactive and can combine to form compounds.

Introducing the 18 major groups (families) on the modern Periodic Table:

Alkali Metals (1) -Group Contains: metals -1 valence electron (VE) -very reactive because they like to give electron away -soft, silver-white, shiny metals -Low density -never found pure in nature -When in their pure form, they are stored in oil to keep them from reacting with water and oxygen in the air. -*Although the element hydrogen appears above the alkali metals on the periodic table, it is not considered a member of Group 1. reactivity increases potassium

Label the Alkali Metals to your PT

Alkaline-Earth Metals (2) -Group contains: metals -2 Valence Electrons -Very reactive but not as reactive as alkali metals -Color of silver -Higher Density than Alkali metals -It is more difficult for atoms to give two atoms than to give one when joining with other atoms. -often mixed with Aluminum -forms strong/light weight alloys magnesium

 Magnesium  Used to make steel (light metal w/o losing strength)  photosynthesis (chlorophyll)  Calcium  bones & teeth  Chalk, limestone, pearls, plaster

Label the Alkaline Earth Metals to your PT

  Write what you have learned today about how the groups of elements on the periodic table are grouped? K-W-L

Boron Family (13)  Group contains: one metalloid and 4 metals  3 VE  Reactivity: reactive  Solids at room temperature Boron (metalloid)  Hard/brittle  never found pure in nature  in borax...used to make detergents & cosmetics

Aluminum  Most common  most abundant metal in earth’s crust  important metal for industry  light, strong, slow to corrode  A coating of aluminum oxide is what makes us able to use this highly reactive metal Boron Family 13 Al Alumin um Aluminum

Label the Boron Family on your PT

Carbon Family (14) -Group contains: one nonmetal, two metalloids, and two metals -4 VE -Can gain 4 e-, lose 4 e-, or share e- -Reactivity: varies -Can be found uncombined or in compounds silicon

 Most compounds in the body contain Carbon  The metalloids Si and Ge are used to make computer chips.  Si 2nd most abundant element in Earth’s crust  Si used to tip saw blades  The metal Tin (Sn) is useful because it is not very reactive.  For example, a tin can is really made of steel coated with tin.  Because the tin is less reactive than steel is, the tin keeps the iron in the steel from rusting.

Label the Carbon Family on your PT

Nitrogen Family (15) -Group contains: two nonmetals, two metalloids, one metal -5 VE -Tend to gain 3 electrons -Reactivity: varies -Solids at room temperature except for Nitrogen -N and P used in fertilizers -P on tips of matches Arsenic

 Nitrogen makes up 80% of the air you breathe.  Nitrogen is not very reactive, however, Phosphorus is.

Label the Nitrogen Family on your PT

Oxygen Family (16) -Group contains: three nonmetals, one metalloid, and one metal -6 VE -Tend to gain 2 e- -Reactivity: Reactive -All but Oxygen are solids at room temperature -O very abundant element -S used in fertilizers -O makes up 20% of air we breathe sulfur

Label the Oxygen Family on your PT

Halogen Family (“salt-former”) (17) -Group contains: nonmetals -7 VE -Reactivity: very reactive -they only need to gain one electron -poor conductors -violent reactions with alkali metals to form salts -never in uncombined form in nature -F most active halogen -Although the chemical properties of halogens are similar, the physical properties are quite different.

 F compounds in toothpaste  Cl kills bacteria  I keeps thyroid gland working properly Halogens cont… bromine

Label the Halogen Group on your Periodic Table

The Noble Gases (Inert Gases) (18) -Group contains: nonmetals - Reactivity: non-reactive -8 VE -They are full so they do not need to lose or gain any electrons. -Normally, they do not react with other elements. -colorless, odorless gas at room temperature -In “neon” lights -in earth’s atmosphere (less than 1%) Neon

Label the Noble Gases on your Periodic Table

Hydrogen Electrons in the outer level: 1 Reactivity: reactive Colorless, odorless gas at room temperature Low density Explosive reactions with oxygen They properties of hydrogen do not match the properties of any single group, so hydrogen is set apart from the other elements. It is above group 1 because atoms of the alkali metals also have only one electron in their outer level. Atoms of hydrogen can give away one electron when they join with other atoms. It’s physical properties are like those of nonmetals. Hydrogen is the most abundant element in the universe.

Transition Metals (3-12) Group contains: metals Electrons in the outer level: 1 or 2 Reactivity: less reactive than alkaline-earth metals Shiny Good conductors Higher density and melting points than Groups 1 and 2 (except for Mercury) Fe, Co, and Ni produce magnetic field mercury

  Groups 3-12 do not have individual names.  Instead they are called transition metals.  They do not give away their electrons as easily as Group 1 and Group 2 do.  Transition metals are less reactive than alkali metals and alkaline-earth metals.

Label the Transition Metals on your periodic table

 Lanthanide series (period 6)  Actinide Series (period 7)  Separated from table to make easy to read/print  silver, silvery-white, or gray metals.  Conduct electricity Rare Earth Elements uranium

  1 st row  Shiny, reactive metals  Used to make steel Lanthanide

Label the Lanthanide Series on your PT

  2 nd row  All are radioactive or unstable  These can be made in labs. Some of these do not exist in nature. Actinide

Label the Actinide Series on your PT

  Alkali metals (Group 1) are the most reactive metals.  Atoms of the alkali metals have one electron in their outer level. Summary

  Alkaline-earth metals (Group 2) are less reactive than the alkali metals are.  Atoms of the alkaline-earth metals have two electrons in their outer level. Summary

  Transition metals (Groups 3-12) include most of the well-known metals and the lanthanides and actinides. Summary

  Groups contain the metalloids and some metals and nonmetals. Summary

  Halogens (Group 17) are very reactive nonmetals.  Atoms of the halogens have seven electrons in their outer level. Summary

  Noble gases (Group 18) are unreactive nonmetals.  Atoms of the noble gases have a full set of electrons in their outer level. Summary

  Hydrogen is set off by itself in the periodic table.  Its properties do not match the properties of any one group. Summary

  Grouping the Elements Directed Reading B

  Placing All Your Elements on the Table Reinforcement Worksheet