11/14/16
1
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
11/14/16
2
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.
11/14/16
3
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
11/14/16
4
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
11/14/16
5
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
11/14/16
6
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
11/14/16
7
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/
11/14/16
8
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
11/14/16
9
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
11/14/16
10
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
11/14/16
11
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
11/14/16
12
• 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