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Chemistry Monday, October 31, 2016

Do-Now: “Ch. 5 Quiz Review Do-Now” 1. Write down today’s FLT 2.  Explain or diagram the Bohr model of the

atom 3.  List the four quantum numbers and their

symbols 4.  Explain what 3d means. 5. Write the electron configuration for sodium.

Take out your planner and ToC

Planner: •  Read Ch. 6, Section 1 •  Turn in ToC#2 •  Finish lab reports

Table of Contents #2: 24. Quantum Kahoot Do-Now 25. Ch. 5 Quiz Day Do-Now

Quiz • Noiselevel0• Eyesonyourownpaper• Flipoverwhenfinished• Wewillcorrecta9erthequiz

Chemistry Tuesday, November 1 – Wednesday,

November 2, 2016

Do-Now: “6.1 Cornell Notes” 1. Write down today’s FLT

Bear Wolf Cat Lion Puppy Tarantula Tiger Lamb

2. Organize the above organisms into at least three different groups.

3.  Name and describe each group. How did you organize them?

4.  Now, organize the organisms into completely DIFFERENT groups.

5. What did you change and why? Take out your planner and ToC

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Planner: •  Finish WS •  Turn in lab with purpose and conclusion sections •  Mon à even period day •  Progress report grades submitted next Wed AM

Table of Contents #3: 1.  6.1 Cornell Notes 2.  Periodic Table Coloring WS

FLT •  I will be able to explain how elements

are organized in a periodic table by completing 6.1 Cornell Notes

Standard HS-PS1-1:Usetheperiodictableasamodeltopredicttherela;veproper;esofelementsbasedonthepa?ernsofelectronsintheoutermostenergylevelofatoms.

6.1: Organizing the Elements Organizing the Elements •  While some elements have been known for

thousands of years (such as gold), there were still only 13 identified by 1700.

•  As scientists began discovering more and more elements, they realized that they needed to organize the elements.

Organizing the Elements How did chemists begin to organize the known elements?

Organizing the Elements •  Chemists used

the properties of elements to sort them into groups. –  In 1829,

Dobereiner tried arranging elements into groups of three with similar properties.

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Organizing the Elements •  Chlorine, bromine, and iodine have very

similar chemical properties.

Mendeleev

Mendeleev�s Periodic Table

•  By the mid-1800s, about 70 elements were known to exist

•  Dmitri Mendeleev, a Russian chemist, designed the first “Periodic Table”

6.1

Mendeleev’s Periodic Table •  Mendeleev’s Periodic Table = arranged

the elements in order of increasing atomic mass.

•  The periodic table can be used to predict the properties of undiscovered elements.

Mendeleev�s Periodic Table • An Early Version of Mendeleev�s Periodic Table

6.1

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Mendeleev’s Periodic Table •  Mendeleev noticed patterns among

elements, and left blanks in his table for undiscovered elements – He knew there were elements that fit certain

properties that were not yet known

Mendeleev’s Periodic Table •  However, there were some issues with using

atomic mass. •  For example, iodine has a lower relative

atomic mass than tellurium, but a higher atomic number.

Periodic Law

Periodic Law •  In 1913, Henry Moseley arranged elements

according to increasing atomic number.

The Periodic Law •  Periodic Law = When elements are

arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties.

6.1 The Periodic Law •  Periods = Horizontal rows

– There are 7 periods

6.1

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The Periodic Law •  Groups = Vertical columns

– Similar physical and chemical properties – Identified by number and letter (1A, IIA, etc)

6.1 The Periodic Law – The properties of the elements within a

period change as you move across a period from left to right.

– The pattern of properties within a period repeats as you move from one period to the next.

6.1

Classes of Elements

Metals, Nonmetals, and Metalloids •  Three classes of elements: •  Metals, Nonmetals, and Metalloids •  Across a period, the properties of elements

become less metallic and more nonmetallic.

6.1

Metals, Nonmetals, and Metalloids •  Metals, Metalloids, and Nonmetals in the

Periodic Table

6.1

Metals, Nonmetals, and Metalloids •  Metals, Metalloids, and Nonmetals in the

Periodic Table

6.1

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Metals, Nonmetals, and Metalloids •  Metals, Metalloids, and Nonmetals in the

Periodic Table

6.1

Metals, Nonmetals, and Metalloids •  Metals, Metalloids, and Nonmetals in the

Periodic Table

6.1

Metals, Nonmetals, and Metalloids •  Metals

– Metals are good conductors of heat and electricity. • 80% of elements are metals. • Metals have a high luster, are ductile, and are malleable.

6.1

Metals, Nonmetals, and Metalloids •  Nonmetals

– In general, nonmetals are poor conductors of heat and electricity • Most (not all) nonmetals are gases at

room temperature. • A few nonmetals are solids, such as sulfur and

phosphorus. • One nonmetal, bromine, is a dark-red liquid.

6.1

Metals, Nonmetals, and Metalloids •  Metalloids

– B, Si, Ge, As, Sb, Te, and Po* – Properties between metals and

nonmetals – Ex/ Silicon is lustrous, but a poor conductor

6.1

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Pair-Share-Respond1.   HowdidMendeleevarrangehis

periodictable?2.   WhydidMendeleevleaveblanksinhis

periodictable?3.   Whatistheperiodiclaw?4.   DisInguishbetweenaperiodanda

group5.   IdenIfythethreeclassesofelements,

andbrieflylistapropertyofeach

CW • PeriodicTableWS

– Followthestepsinorder– Useyourbook!Pgs161-163

• ToCorreadCh.6

Chemistry Thursday, November 3 – Friday, November 4,

2016

Do-Now: “BrainPOP: Periodic Table” 1. Write down today’s FLT

2. Who was Mendeleev, and what did he do? 3. What was wrong with Mendeleev’s idea? 4.  Distinguish between periods and groups. 5.  Use at least one pro-talk sentence frame to

explain what metals, nonmetals, and metalloids are.

Take out your planner and ToC

Planner: •  Finish Section Assessment •  Study! Ch. 6 Quiz Mon/Tues

Table of Contents #3: 3.  BrainPOP: Periodic Table 4.  6.2 Cornell Notes

BrainPOP:PeriodicTable• WatchtheBrainPOPvideo• A9erthevideo,answerthequesIonsinyourgroup–everymembermustcopydownthesameanswer

• Thegroupwiththemostcorrectanswersà+5dojopointseach

h?ps://www.brainpop.com/science/ma?erandchemistry/periodictableofelements/

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FLT •  I will be able to classify elements based

on their electron configurations by completing 6.2 Cornell Notes

Standard HS-PS1-1:Usetheperiodictableasamodeltopredicttherela;veproper;esofelementsbasedonthepa?ernsofelectronsintheoutermostenergylevelofatoms.

6.2: Classifying the Elements

Recall

Periodic Table 6.1

Periodic Table Squares •  The periodic table displays the symbols and

names of the elements, along with information about the structure of their atoms. – Atomic number (Z) and average atomic mass

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Squares in the Periodic Table 6.2

Valence Electrons

•  Valence electrons (vse-s) = e-s in the outermost shell (highest s and p orbitals) that can participate in chemical bonding

Periodic Groups

Groups •  On our periodic table, we can look at (1)

Noble Gases (2) Representative Elements (3) Transition Metals and (4) Inner Transition Metals

Groups •  Group 1A: Alkali Metals

–  Highly reactive –  1 vse- (ns1) –  Ex/ Na: 1s22s22p63s1

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Groups •  Group IIA: Alkaline Earth Metals

–  Very reactive –  2 vse- (ns2) –  Ex/ Ca: 1s22s22p63s23p64s2

Groups •  Group VIIA: Halogens

–  Very reactive nonmetals that form salts –  7 vse- (ns2np5) –  Ex/ F: 1s22s22p5

Groups •  Group VIIIA: Noble Gases

–  Very nonreactive gases with full outer shells –  Eight vse- (ns2np6) –  Ex/ Ar: 1s22s22p63s23p6

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Groups •  Transition Metals

–  Groups 3-12 (B’s) –  Contain e-s in their d orbitals –  Ex/Fe: 1s22s22p63s23p64s23d6

Groups •  Inner Transition Metals

–  Lanthanides and actinides –  Contain e-s in their f orbitals

1A

2A 3A 4A 5A 6A 7A

8A•  Elements in the 1A-7A groups

are called the representative elements

outer s or p filling Electron Configurations

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•  Each row (or period) is the energy level for s and p orbitals.

1

2

3

4

5

6

7

Period Number

•  The �d� orbitals fill up in levels 1 less than the period number, so the first d is 3d even though it�s in row 4.

1

2

3

4

5

6

7

3d

4d 5d

6.2

Try Writing Just Using your Periodic Table: •  Ex 1/ Be

•  Ex 2/ C •  Ex 3/ Si

CW1.   P.167#10-152.   THENwriteelectronfiguraIonsforthe

following:a.   Lib.   Oc.   Asd.   Cu

3.   Finished?ReadCh.7Quietly