1. have the rest of the homework packet on periodic table trends out to be stamped 2. take 5 minutes...
TRANSCRIPT
1. Have the rest of the homework packet on periodic table trends out to be stamped
2. Take 5 minutes to prepare for the quiz by answering the questions on the board.
**Lab Thurs/Fri – have comp. book **Test next Thursday/Friday
Bellwork 9-10-2014
Part 1:1. Elements on the left side of the periodic
table have a larger radius because there are LESS protons so they pull on the outer shells LESS making the atom bigger
2. Elements on the bottom of the periodic table have more shells so their radius is larger
3. A. Lithium – less protons, less pull B. Barium – more shells
Homework: Periodic Table Trends
Part 2:1. Elements on the right side of the periodic table
have a higher ionization energy because they have MORE valence electrons meaning it is HARDER to pull them away. They are closer to a full shell or stability
2. Elements on the top of the periodic table have a higher ionization energy because they have less shells so electrons are closer to the nucleus and HARDER to pull away
3. A. Chlorine – more valence e-, harder to take away B. Beryllium – less shells, e- closer to nucleus, harder to take away
Part 3:1. Elements on the right side of the periodic
table have a higher electronegativity because they have more valence electrons and their desire for more is high
2. Elements on the top of the periodic table have a higher electronegativity because they have less shells making the outer electrons MORE attracted to the nucleus
3. A. Fluorine – less shells, e- more attracted to nucleus
B. Bromine – more valence e-, wants more
Steps to Solving Trend Problems
Atomic Radius – size of atom 1. Find the elements on the periodic table2. If Left – Right look at # of protonsa. More protons = more pull = smaller
radiusb. Less protons = less pull = larger radius
3. If Up – Down look at # of shellsa. More shells = larger radiusb. Less shells = smaller radius
Steps to Solving Trend Problems
Ionization Energy – energy needed to remove e-1. Find the elements on the periodic table2. If Left – Right look at # of valence electronsa. More valence electrons = harder to pull away =
higher ionization energy b. Less valence electrons = easier to pull away =
lower ionization energy 3. If Up – Down look at # of shellsa. More shells = lower ionization energy because
electrons farther from nucleus (easier to remove) b. Less shells = higher ionization energy because
electrons closer to nucleus (harder to remove)
Steps to Solving Trend Problems
Electronegativity – desire for or attraction to electrons 1. Find the elements on the periodic table2. If Left – Right look at # of valence electronsa. More valence electrons = more attracted to
electrons = higher electronegativityb. Less valence electrons = less attracted to
electrons = lower electronegativity3. If Up – Down look at # of shellsa. More shells = lower electronegativity because
electrons farther from nucleus (not as attracted)b. Less shells = higher electronegativity because
electrons closer to nucleus (more attracted)
Test next Thurs/Fri will cover:Scientists (4) – who did what and discovered
whatAtomic structure – p+, n0, e
Test Next Thursday/Friday
1. Grab a pair of headphones IF YOU DON’T HAVE ANY
2. What was the hardest thing about the quiz on Wednesday?
3. What was the easiest thing?4. What will you do to prepare better
next time, if need be?
**Pass back quizzes **Test next Thurs/Fri
Bellwork 9-12-2014
1. Bellwork from last two weeks2. Periodic table groups note taker
(stamped)3. Homework: periodic table groups
.
Homework Packet
Station 1 – Small group instruction I will be calling a few students aside to work
on problems with me
Station 2 – IndependentYou will be working on an EduCanon video
silently by yourself with headphones (see instructions on the board)
Stations
Fill us in:1. What were the three groups discussed
in the video?2. What are the major differences between
metals and nonmetals as discussed in the video?
3. Those of you who did not see the video, what would you predict the properties of metalloids (or semi-metals) to be?
Group Discussion
You will be testing three different samples for the characteristics described in the video.
Objective:You will be able to identify a substance
as a metal or a nonmetal given specific properties of that substance.
Metals vs. Nonmetals Mini Lab
Copy Down This Table…
Characteristics
Sample 1: Battery
Sample 2: Pencil
Sample 3: Copper Wire
Is it malleable?
Is it ductile?
Is it brittle?
Does it conduct electricity?
Does it conduct heat?
It is a metal or nonmetal?
***Use the information on the board in green box when using the multi-meters***
Characteristics to think about:1. Malleable – can it be hammered or pressed
permanently out of shape without cracking?2. Ductile – can it deform under stress
without cracking?3. Brittle – does it crack easily? 4. Conductivity – does it conduct electricity
or heat?Use voltage meter to test this
5. Shiny – does it reflect light?
Metals, Nonmetals and Metalloids Mini Lab
They have intermediate properties of metals and nonmetals
Blue zig-zag section on the periodic table
Those of you who did not see the video, label each section of the periodic table as metal, nonmetal or metalloids
So What Are Metalloids?
Check your neighbor’s periodic table and make sure each section is appropriately labeled.
Thumbs up if the property is metal, thumbs down if nonmetal:1. Conducts electricity2. Lustrous – shiny 3. Poor conductor of heat4. Brittle and breaks easily5. Malleable – bends easily6. Dull in appearance
Quick Check