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)

Friday 4-5pm

Tutoring

Quiz

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

DEMO

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