unit 5: the periodic table chemistry 2014-2015. agenda 11/3/14 today’s objectives: - hand back...

UNIT 5: THE PERIODIC TABLE

CHEMISTRY 2014-2015

AGENDA 11/3/14

Today’s Objectives:

- Hand back spectra labs

- Introduction to the Periodic Table

- Periodic Table Activity

HW: Finish the questions from the table structure activity

Now: Quietly read the unit 5 learning targets,

Highlighting words you may not be familiar with

STRUCTURE OF THE TABLE• Using a blank Periodic Table create your own table

following the guidelines in the activity directions.

• Be sure to pay attention to what each section is called.

• Do not answer the questions for this lab yet, we will have time at the end of the class period to work on the questions.

CRYSTAL LAKE CENTRAL NOBEL PRIZE CONTEST

WE HAVE DISCOVERED NEW ELEMENTS!!

It is your job to take the data you are given and arrange it in a way that organizes all of the data.

You will slowly get more information as scientists discover it.

You will have to present your table to the other scientists in the class upon your final draft, be sure to have a reason for your setup!!

THE FIRST SET OF DATA

**The elements are named after the famous scientists who discovered them at The University of Iowa

Element Symbol Mass # (Top Right)

Meekeron Em 30.97

Bernardine Bp 19.00

Sonntagium Js 14.01

Baldinic Mb 79.90

Ballentite Kb 32.07

Kreiterite Ck 20.18

Leonardium Ln 35.45

Olsonium Om 16.00

Schmiederon Sh 74.92

Soderlous Sd 28.09


Energy Levels (Bottom Right)

Meekeron Em 30.97 3

Bernardine Bp 19.00 2

Sonntagium Js 14.01 2

Baldinic Mb 79.90 4

Ballentite Kb 32.07 3

Kreiterite Ck 20.18 2

Leonardium Ln 35.45 3

Olsonium Om 16.00 2

Schmiederon Sh 74.92 4

Soderlous Sd 28.09 3



# protons (Top Left)

Meekeron Em 30.97 3 15

Bernardine Bp 19.00 2 9

Sonntagium Js 14.01 2 7

Baldinic Mb 79.90 4 35

Ballentite Kb 32.07 3 16

Kreiterite Ck 20.18 2 10

Leonardium Ln 35.45 3 17

Olsonium Om 16.00 2 8

Schmiederon Sh 74.92 4 33

Soderlous Sd 28.09 3 14



# protons (Top Left)

Valence electrons (Bottom Left)

Meekeron Em 30.97 3 15 5

Bernardine Bp 19.00 2 9 7

Sonntagium Js 14.01 2 7 5

Baldinic Mb 79.90 4 35 7

Ballentite Kb 32.07 3 16 6

Kreiterite Ck 20.18 2 10 8

Leonardium Ln 35.45 3 17 7

Olsonium Om 16.00 2 8 6

Schmiederon Sh 74.92 4 33 5

Soderlous Sd 28.09 3 14 4

OUR PERIODIC TABLE

Is organized so that the properties of elements repeat themselves in each row.

Mendeleev was able to predict properties of elements before they were discovered!!

Can you predict the properties of an element that would fit in the hole in your periodic table??

Fake Element Real Element

Meekeron (Em) Phosphorus

Bernardine (Bp) Fluorine

Sonntagium (Js) Nitrogen

Baldinic (Mb) Bromine

Ballentite (Kb) Sulfur

Kreiterite (Ck) Neon

Leonardium (Ln) Chlorine

Olsonium (Om) Oxygen

Schmiederon (Sh) Arsenic

Soderlous (Sd) Silicon

Element Fake Symbol

Mass # Orbital Shells

# protons Valence electrons

Phosphorus Em 30.97 3 15 5

Fluorine Bp 19.00 2 9 7

Nitrogen Js 14.01 2 7 5

Bromine Mb 79.90 4 35 7

Sulfur Kb 32.07 3 16 6

Neon Ck 20.18 2 10 8

Chlorine Ln 35.45 3 17 7

Oxygen Om 16.00 2 8 6

Arsenic Sh 74.92 4 33 5

Silicon Sd 28.09 3 14 4

AGENDA 11/4/14 HAPPY ELECTION DAYToday’s Objectives:

- Recap Yesterday

- What are metals and non-metals?

- Begin analyzing the Periodic Table

Now: Take out your homework from last night

OUR ROADMAP TO THE CHEMICAL WORLD

• Where are the transition metals located?• Where are the metalloids located?• Where are the Non-metals located?• Where are the Metals located?

Important Properties of…

Metals: Non-Metals:

STRUCTURE AND REGIONS

Metals

• Largest region – left of staircase

• Solids (except Hg)

• Conduct heat/electricity

• Luster

• Ductile (stretchable)

• Malleable (able to be flattened)

STRUCTURE AND REGIONS• Non-metals

–Right of staircase–Solids, liquids,

gases–Low conductivity

(heat and electricity)

–Low luster–Brittle solids

STRUCTURE AND REGIONS

Metalloids/Semi-Metals

•On staircase•Share properties of metals and nonmetals

•Semi-conductors

SOME VOCAB YOU NEED TO KNOW

Family/Group

Period

BLAST FROM THE PAST!!!Write the electron configuration for:

• Li

• Na

• K

• Do you notice a trend?

• As you go down a family/group, each element gains an energy level.

AGENDA 11/5/14Today’s Objectives: - Review P.T. Basics - Learn the Trends of the Periodic Table

HW: Complete note review of periodic trends

Now: Discuss with your neighbors about the answer to yesterday’s homework question!

THE SHIELDING EFFECT

The ability/tendency of lower energy level electrons to “shield” outer electrons from the pull/attraction of protons in the nucleus.

Which would show a greater “Shielding Effect”?

GREATER SHIELDING

Having a greater shielding effect means that the outer electrons are not as attracted to the nucleus.

Remember our holding hand demo…

ATOMIC SIZE/RADII

ATOMS INCREASE IN SIZE AS YOU GO FROM TOP TO BOTTOM WITHIN A FAMILY/GROUP BECAUSE . . .

“Bottom” elements have electrons in higher principal energy levels ---> greater distance from the nucleus ---> more levels means larger atom!

Plus, each successive element in a group exhibits a greater shielding effect!! Outer electrons feel only a weak pull from the nucleus!

ATOMS DECREASE IN SIZE AS YOU GO FROM LEFT TO RIGHT ACROSS A PERIOD BECAUSE . . .

From left to right, successive elements have more protons & electrons. However, the “extra” electrons do not occupy higher energy levels, so there is no additional shielding effect. With the “extra” protons, all electrons are pulled closer to the nucleus!

ATOMIC RADIUS

Greatest Atomic Radius! (Francium)

Smallest Atomic Radius! (Helium)

Let’s Recap

What are some properties of Metals?

What are some properties of Non-Metals?

What causes the changes in atomic size within a FAMILY?

What causes the changes in atomic size in a PERIOD?

AGENDA 11/6/14Today’s Objectives: - Review P.T. Basics - Discuss Ions

- Ionization Energy

HW: Forming Ions Homework

Now: Find a partner for an activity

Let’s Recap

What are some properties of Metals?

What are some properties of Non-Metals?

What causes the changes in atomic size within a FAMILY?

What causes the changes in atomic size in a PERIOD?

P.T. REVIEW

2. Vertical columns of elements are called groups/families. Horizontal rows are called __________.

3. True or False: Elements in the same row tend to have very similar chemical properties.

4. What is the chemical symbol for the halogen in Period 4?

5. An element’s outermost electrons are found in the 5 th energy level. The Lewis dot structure for the element shows four dots. Give the chemical symbol for this element.

6. Of the elements that have 2 valence electrons, which has the lowest atomic mass? What family is this element a part of?

P.T. REVIEW

2. Vertical columns of elements are called groups/families. Horizontal rows are called periods.

3. True or False: Elements in the same row tend to have very similar chemical properties. False! Elements in the same column have very similar chemical properties!

4. What is the chemical symbol for the halogen in Period 4? Br 5. An element’s outermost electrons are found in the 5 th energy

level. The Lewis structure for the element shows four dots. Give the chemical symbol for this element. Sn

6. Of the elements that typically form ions with a +2 charge, which has the lowest atomic mass? What family is this element a part of? Be; part of Alkali Earth metals

REACTIVITY

METAL REACTIVITY

• Metals react by losing electrons.

• Would it be easier to lose an electron from a smaller or larger atom??

• Think about the shielding effect.

REACTIVITY INCREASES AS YOU GO DOWN A GROUP OF METALS. WHY?

SHIELDING EFFECT! LOWER ELEMENTS HAVE ELECTRONS FURTHER FROM THE NUCLEUS WHICH ARE LESS FIRMLY HELD AND THEREFORE MORE EASILY LOST.

REACTIVITY DECREASES AS YOU GO LEFT TO RIGHT IN A ROW OF METALS. WHY?

Successive elements have more protons, but no “new” energy levels for electrons. “Extra” protons hold the electrons more tightly (helps that there’s no added shielding effect!).

TREND #2: REACTIVITY THE MOST REACTIVE METALS TEND TO BE LOCATED IN THE LOWER LEFT HAND CORNER OF THE PERIODIC TABLE. WHY?

METALS REACT BY LOSING ELECTRONS. THE EASIER IT IS TO LOSE ELECTRONS, THE MORE REACTIVE THE METAL.

REACTIVITY OF METALS

Most Reactive Metal!! (Francium)

THE MOST REACTIVE METALS

https://www.youtube.com/watch?v=m55kgyApYrY

AGENDA 11/6/14Today’s Objectives: - Review P.T. Basics - Discuss Ions

- Ionization Energy

HW: Forming Ions Homework

Now: Find a partner for an activity

One answers, one explains…

WHICH HAS THE SMALLER ATOMIC RADIUS?

NA OR S ??


WHICH EXHIBITS THE GREATER SHIELDING EFFECT?

F OR I ??


WHICH IS THE LARGER PARTICLE:

N OR AS ???


WHICH IS THE MOST REACTIVE:

RB OR SR ???


WHICH HAS 2 VALENCE ELECTRONS:

HE OR CA ???

IONIZATION ENERGY

The ability for an atom to gain or lose an electron. The ability for an atom to become an ion.

METALS V. NON-METALS• Metals

• Lose electrons in order to become an ion

• Non-metals

• Gain electrons in order to become an ion

Would a smaller atom or a larger atom be able to attract an electron better?

Would a smaller atom or a larger atom be able to release an atom easier?

Generally, ionization energy decreases from top to bottom within a family because….

SHIELDING INCREASES SO THE ELECTRONS ARE ATTRACTED LESS STRONGLY!

Generally, ionization energy increases from left to right across a period because….

EXTRA PROTONS IN NUCLEUS ATTRACT THE VALENCE ELECTRONS MORE STRONGLY!

IONIZATION ENERGY

Highest I.E.(Helium)

AGENDA 11/7/14Today’s Objectives: - Electronegativity Trend - Review all other trends

- Reactivity DemoCOLLECT FORMING IONS

HW: Trends Packet

Now:Take out your Forming Ions Homework

ELECTRONEGATIVITY

The ability for an atom to attract an electron.

Can a smaller or larger atom attract an electron better?

Think about shielding effect.

Generally, electronegativity tends to decrease from top to bottom in a group because….

AS THE SIZE OF THE ATOM INCREASES, THE PULL OF THE NUCLEUS IS LESS STRONG

Generally, electronegativity tends to increase from left to right in a row because….

THE ARE MORE PROTONS IN THE NUCLEUS BUT THE SAME NUMBER OF ENERGY LEVELS.

ELECTRONEGATIVITY

HighestElectronegativity(Fluorine)Note: Noble gases will not attract extra electrons!!

AGENDA 11/10/14Today’s Objectives: - Review the periodic trends - White board review activity

- Periodic Table History Web Quest

HW: Unit 5 Review Packet due Wednesday

Now: Take out your homework from this weekend

BECOME THE EXPERT1. You and your table will select a trend to become the expert

on.

2. It is your job to study this trend from your notes and prepare a 2-3 minute presentation on your trend to the class.

3. You may use a whiteboard to organize your presentation.

4. Your presentation should include:

1. Definition of the trend

2. How the trend changes on the PT

3. How does the shielding effect or atomic size relate to your trend.

4. What is an example question that could be asked on a test about your trend?

The trends are…

1. Reactivity of Metals

2. Ionization Energy

3. Electronegativity

4. Atomic Radius

5. Shielding Effect

DURING PRESENTATIONS…

1. Add to your notes from in class.

2. Think about questions you might have about this trend for the group.

3. Work out the problems on a separate sheet of paper to turn in for credit.

HISTORY OF THE PERIODIC TABLE• Work in groups to answer the questions about each

scientist.

• This document will serve as your notes for this portion of the unit.

• You are accountable to your classmates!

ACC CHEM 3/13/14

Today’s Objectives:

- Study for test tomorrow

H.W. Study for test tomorrow

unit 5: the periodic table chemistry 2014-2015. agenda 11/3/14 today’s objectives: - hand back...

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