Unit 4The Incredible Periodic Table

Today…• Turn in:

–Get out PT Basics Poster

• Our Plan:

–PT Basics Questions with group

–Introduce Personal PT Project

• Homework (Write in Planner):–Personal PT Project

• Choose topic and how to organize

Block A B C D F Ave High Score

1 5 3 5 5 4 74 962 6 2 5 4 5 74 945 1 5 4 5 6 66 94

6 8 3 9 5 3 77 100

TOTAL22%

14% 25% 20%19%

Daily Challenge

• PT Basics Inquiry Activity–Answer the questions on the

back of your PT Basics Handout with your group.

–Turn in your poster and your questions when finished.

Wrap Up

• As a group, come up with 3 things that you learned today about the Periodic Table and be prepared to share.

Today…• Turn in:

–Nothing

• Our Plan:

–Work on your Personal Periodic Table

–Wrap Up – Questions about project?

• Homework (Write in Planner):

–Personal PT Project – due Monday• Don’t forget a title and key!

Wrap Up•What questions do you have about your Periodic Table project?

Today…• Turn in:

– Periodic Table Project

• Our Plan:

– Crash Course Video

– PT Card Sort

– Alphabet Brainstorm

• Homework (Write in Planner):

– Stop the Process due NEXT class

Crash Course on the Periodic Table• http://www.youtube.com/watch?v=0RRVV

4Diomg

• First 5 minutes

Game Time• In your team of 3 or 4, complete

the Periodic Table Card Sort and complete the worksheet as a team.

• Be sure to follow the requirements in the instructions for how many things you have to list.

Activity Discussion• Where are the metals?• Where are the nonmetals?• Where are the metalloids?• What do things in a column have in

common?• What do things in a row have in

common?• What is the trend in size?• What is the trend in reactivity?

Wrap Up

• Alphabet Brainstorm – as a group of 4, come up with one word for each letter of the alphabet that relates to the Periodic Table. Don’t forget to look at the Word Wall!

Homework

• Complete p. 3 of your notes by next class. Read your textbook to answer the questions.

Today…• Turn in:

– Get out Stop the Process– Grade Reflections

• Our Plan:– PT Puns– Notes/Label Your PT– Family Sort/Crossword Puzzle– Wrap Up – Family Clicker Review

• Homework (Write in Planner):– Family Sort/Crossword Puzzle due next class

Modern Periodic Table

• The table is called the “Periodic Table” because elements have similar properties that occur periodically.

Periods• Rows (left to

right) are called periods.

• All of the elements in a period have the same number of energy levels.

Periods Relate to Atoms

• As we increase the atomic number, the electrons fill the energy levels

• Energy levels are labeled K, L, M, N, O, P, Q (or 1-7)

1. Label on your PT

Label Your PT

Energy Levels

GROUPS• The columns (top to bottom) of the periodic table

GROUPS• The elements in a group have the

same number of valence electrons.

• Valence electrons are the electrons found in the outermost energy level of the atom

• They are VERY important to bonding and reactions!

GROUPS• Every element in the first

column (Group 1) has one electron in its outer shell. Every element in the second column (Group 2) has two electrons in its outer shell. ETC.

2. Label the group #s and valence electrons

Label Your PT

Symbols on the PT

19K

39.1

Atomic Number= number of protons

Symbols on the PT

19K

39.1Symbol

Symbols on the PT

19K

39.1

Average Atomic Mass= average mass of the naturally occurring isotopes

Let’s Label the PT3. Oxidation Number = charge

– Relates to how many electrons needed to become stable

– To become stable an atom wants 8 electrons (THE OCTET RULE)

– “Eight is great, except for hydrogen and helium, 2 will do”!

Label Your PT

Let’s Label the PT4. Multivalent= elements with 2

or more possible charges

+1 only = Ag

+1, +2 = Cu, Hg

+2, +3 = Cr, Ni, Fe, Co

+2, +4 = Pb, Sn

Label Your PT

Let’s Label the PT5. Diatomic Molecules

– Atoms that exist in nature as pairs

– Only diatomic when ALONE!

H2, O2, Cl2, I2, N2, F2, Br2

Label Your PT

Let’s Label the PT6. Metals, Nonmetals, & MetalloidsType Location Properties

Metals Left-side PT

(80% of elements)

Shiny, malleable, ductile, good conductor of heat & electricity

Nonmetals Upper Right Corner

Colorless, gases @ room temp, Poor conductors

Metalloids Stair-Step Line Properties of both metals & nonmetals,

semiconductors

Label Your PT

Groups• Group 1: Alkali

Metals–Most reactive

metals–Do not occur in

nature–Very soft–Explode in Water

Groups• Group 2:

Alkaline Earth Elements

–Very reactive

–Not found in nature

Groups• Group 3-10: Transition

Metals–Unreactive – used in

coins and jewelry–Electrons they use to

bond are in more than one energy level(MULTIVALENT)

–Iron, Cobalt, and Nickel are Magnetic

Groups

• Metalloids

–On the stair-step line

–Properties of metals & non-metals

–Semiconductors

Groups• Group 17: Halogens

–Most reactive non-metals–Exist as all three states of

matter at room temperature–Compounds with them are

called “salts”

Groups

• Group 18: Noble Gases–Contain 8 electrons in outer shell (oxidation # 0) = stable

–Unreactive

Groups

• 57-71: Lanthanides• 89-103: Actinides

–Most are synthetic, or man-made

–Actually in Period 6 & 7–Actinides are Radioactive

Assignment Time…

• Complete the Family Sort and the Crossword Puzzle. It is due next class!

Wrap Up

•Family Clicker Review

Today…• Turn in:

– Crossword/Family Sort – basket

• Our Plan:

– Crash Course Review

– Clicker Review

– Notes – Trends

– Periodic Trends War

• Homework (Write in Planner):

– Nothing

Quick Crash Course Review

• 5 – 7 minutes

• http://www.youtube.com/watch?v=0RRVV4Diomg

Periodic Trends

•Activity Series of Metals - Reactivity increases right to left and top to bottom

•Most reactive = Fr

Why?

• The further to the left and down you go, the easier it is for electrons to be given or taken away

Periodic Trends• Activity Series of Nonmetals - Reactivity increases left to right and bottom to top

• EXACT OPPOSITE• Most Reactive = F

Why?

• The farther right and up you go, the stronger the element can “grab” other electrons or bond

Atomic Radii

• Calculated by finding 1/2 the distance between the 2 nuclei of 2 atoms of the element when joined

Period Trend

• Atomic Radius DECREASES as you go left to right across a period

• Why?– Determined by the strength of the attraction

between the nucleus and the outermost electrons (protons “suck” the electrons in)

– Stronger the attraction, smaller the size of atom– More Protons = More Nuclear Attractive Force

Group Trend

• Atomic Radius INCREASES as you go down a group

• Why?

–There is a significant jump in the size of the nucleus (protons & neutrons) as well as the number of electron energy levels

Ions

• An atom or group of atoms with a positive or negative charge.

• Form when electrons are transferred between atoms

–Cation – positive charge (Ca+2)

–Anion – negative charge (N-3)

Ionization Energy

• Energy required to remove an electron from the neutral atom to form a positively charged ion (cation)

Period Trend• Ionization Energy INCREASES as you

go from left to right across a period

• Metals (left) WANT to get rid of their electrons, therefore it doesn’t take much energy to ionize

• Non-metals (right) DO NOT WANT to give away electrons, therefore it takes more energy to ionize

Group Trend• Ionization Energy DECREASES as you go

down a group

• Why?

– Shielding Effect - Caused by an increasing number of electrons between the outer level and the nucleus

– Blocks the attraction of the nucleus for the electrons

– Causes large atoms to lose their electrons more freely

Ionization Energy• Ionization energy relates to activity of metals & non-metals

• The highest ionization energy = the most active non-metal (Fluorine)

• The lowest ionization energy = the most active metal (Francium)

Ionization Energy

• As each electron is removed, the ionization energy increases

• Large jumps of energy indicate a removal of an electron from a new shell

Example• For Na the IE for each

successive electron are 496 kJ/mol, 4562 kJ/mole, 4912 kJ/mol, and 5544 kJ/mol. How many valence electrons does Na have?

Example

496 kJ/mol

4562 kJ/mol

4912 kJ/mol

5544 kJ/mol

Large jump in energy here, therefore there is only one valence electron

Ionic Size

• Cations are always SMALLER than the atoms from which they form

• Anions are always LARGER than the atoms from which they form

Ionic Size

Electronegativity• Ability of an

atom to attract electrons when it makes a compound

Electronegativity• Discovered by Linus Pauling

• He won the Nobel Prize for his work

Period Trend• Electronegativity INCREASES as you

go left to right across a period

• WHY?– Elements on the left side have 1-2 valence

electrons that they would rather give away than “grab” another element’s electrons, so they have low electronegativity

– Elements on the right side only need a few electrons so they want to “grab” another atom’s electrons giving them a high electronegativity

Group Trend

• Electronegativity DECREASES as you go down a group

• Why?– Elements near the top of the PT have few electrons

to begin with so they have a stronger desire to acquire more electrons (higher electronegativity)

– Elements near the bottom have so many electrons already, that gaining or losing an electron is no big deal (lower electronegativity)

Summary of Trends

Periodic Trends Music Video

• http://www.youtube.com/watch?v=MGTKVaZcq8Y&feature=related

Periodic Trends War

• You will play “War” with your face partner.

1. Deal out all of the cards so that each of you have half. Keep the cards in a pile face down.

2. Each player will play their top card. The element that is greatest for that trend wins both cards. After going through your deck mix them up and then continue play. Every 3 minutes we will switch trends.

3. The game ends when one person runs out of cards. If that doesn’t happen in the time allotted, the winner is the person with the most cards at the end.

Trends War• Atomic Radius• Electronegativity• Ionization Energy• Valence Electrons (if tie play next

card and winner gets all)• Reactivity (if it is a metal and a

nonmetal the metal wins)

Today…• Turn in:

– Grab a clicker and pull out your lab

• Our Plan:

– PT Worksheet Race

– Periodic Trends Lab

– Test Review

– Clicker Review

– Exit Slip• Homework (Write in Planner):

– Test Review Due next class

– TEST NEXT CLASS

Alkali Metals in Water

Cesium & Rubidium Bathtub

Wrap Up – write on sticky note or index card and give to Mrs. C on your way out…On the Periodic Table, observe the locations of the following elements:

Li, Ca, Co, Cl, Br, Cs1.Which element is the most reactive metal?

2.Which element is the most reactive nonmetal?

3.Which element is the biggest?

4.Which element has the greatest electronegativity?

5.Which element has the smallest ionization energy?

The Answers

1.Cs

2.Cl

3.Cs

4.Cl

5.Cs

Today…• Turn in:

– Get out test review to check

• Our Plan:– Station Review– Questions on Test Review– Unit 4 Test– Fill out Goal Sheet (except test)– Sodium Party Reading/Video

• Homework (Write in Planner):– Sodium Party Reading (due next class)

Sodium Party Video

• http://periodictable.com/Stories/011.2/index.html