Download Do-now

Do-now
 Get into Lab Groups! Take out
a piece of paper!
 Periodic Table of the Aliens!Figure out what your missing
aliens should look like

First group to finish gets an EXTRA 5
points! ( Classwork Grade)
HINT 1: Look for a pattern on each alien, try to arrange in a
grid
HINT 2: There should be two ways in which each alien
changes
HINT 3: Look at the amount of fingers on each alien! Group
similar ones together and look for another pattern
Chapter 6
THE PERIODIC TABLE
Objectives
 6.1a Explain how chemists began to organize the known
elements.
 6.1b Describe how Mendeleev organized his periodic table.
 6.1c Describe how the modern periodic table is organized.
 6.1d Identify three broad classes of elements.
QUESTION
 What makes one element different
from another?
The
number of protons in the nucleus!
Organizing the elements
 Early Chemists, such as
JW Dobereiner, used
properties of elements to
sort them into groups
 “triads” were sets of
three elements with the
same properties

For instance- Chlorine,
Bromine, and Iodine
Mendeleev
 Dmitri Mendeleev was a
Russian chemistry teacher
who published his own
table of the elements
 In his table he arranged
each element by increasing
atomic mass and noticed
patterns
 There were unknown
elements in his table that
had not been discovered
yet!
The modern periodic table- p. 162
 Unlike Mendeleev’s
table, the modern
periodic table is not
measured by increasing
atomic mass

Instead, atomic number is
used
 We see a new pattern,
the periodic law,
where as the elements
are listed in increasing
atomic number, there
properties will repeat
periodically.
Atomic number increases down and to the right
A closer look
Three classes of elements
Metals
2. Nonmetals
3. Metalloids
1.
Metals
 Metals- good conductors of heat and
electric current



High luster or “sheen”
Solid at room temperature, except for
mercury
Ductile and malleable
How it’s made- Aluminum
Nonmetals
 Nonmetals- poor conductors of heat
and electric current



Carbon is an exception to this rule
Typically gases at room temperature
Solid nonmetals are typically brittle
Periodic Videos- Chlorine
https://www.youtube.com/watch?v=BXCf
Bl4rmh0
Metalloid
 Metalloid- has properties similar to
those of metals and nonmetals

Under some conditions behave as a metal,
under others, behave as a nonmetal
How it’s made- computer chips
https://www.youtube.com/watch?v=aWVywhzuHnQ
Homework
 Worksheet 6.1
Do-now
 Hand in Homework!
 Write the electron configurations for Helium, Neon,
Argon, and Krypton in your notes.
Objectives
 6.2a Describe the information in a periodic table.
 6.2b Classify elements based on electron
configuration.
Relating to electron configuration
 Write the electron configuration for Helium, Neon,
Argon, and Krypton




Helium
Neon
Argon
Krypton
 What do each of these have in common?
Groups of Elements
Groups of Elements
 Alkali Metals (1A)
 Alkaline Earth Metals (2A)
 Halogens (7A)
 Noble Gases (8A)
Alkali Metals
Noble Gases
Blocks of Elements
“s”
block1A-2A
“p” block- 3A-8A
“d” block- all B groups
“f” block
Electron Configuration Groups
 All noble gases have completely filled electron
configurations
 Elements in groups 1A through 7A (s and p blocks)
are usually referred to as representative
elements

Sometimes called “main group elements”
 The B group elements (d block) are called
transition metals.
 The lower block elements (f block) are called inner
transition metals.
Blocks of Elements
“s”
block1A-2A
“p” block- 3A-8A
“d” block- all B groups
“f” block
Electron Configuration Groups
Representative
Elements
Transition Metals
Inner Transition Metals
Noble Gases
Repre
sentat
ive
NOBLE GAS CONFIGURATION
 Selenium
 Barium
 Iron
 Copper
Electron configuration in groups
WHERE IS ELEMENT:
1s2, 2s2, 2p6, 3s2, 3p6, 4s1?
[Xe] 6s2, 4f5 ?
Battleship!
 Rules:



Set up your fleet.
Player 1 calls out an
element by stating its
noble gas configuration
Player 2 confirms this by
stating “hit” or “miss”


If a hit, player 1 gets
another shot!
Play until someone’s
whole fleet has been sunk!
 Have fun!
Homework
 Read section 6.2
 Lesson Check, p. 171
 Quiz Tomorrow
 Lab Tomorrow
 Projects due tomorrow
Activity- Periodic Trends
 Download a periodic table app on your phone
 Your will be given a property for that element
 Atomic radius (size)
 Ionization energy or First Ionization energy
 Ionic radius (size)
 Electronegativity
 Find the values for elements 1-36 (H-Kr), arrange
in a table form.
 Graph those elements as property vs. atomic
number. (2 graphs!)
 Put a title on the graph and label the axes
Objectives
 6.3a Describe trends among elements for atomic size
 6.3b Explain how ions form
 6.3c Describe periodic trends for first ionization
energy, ionic size, and electronegativity
Trends in the Periodic Table
 The periodic table is organized by atomic number
and by electron configuration
 Other patterns begin to occur!



Ionization Energy
Atomic Radius
Electronegativity
Atomic Radius
 Atomic Radius tends to
increase from top to
bottom in a group and
decreases from left to
right in a period
Ions
 Ions are atoms that have
either a positive or negative
charge

They have an unequal amount
of protons and electrons
 Positive and negative ions
form when electrons are
transferred in between
atoms


Cations: Ions with a positive
charge
Anions: Ions with a negative
charge
Sodium and Chlorine
HTTPS://WWW.YOUTUBE.COM/WATCH?V=MX
5JJWI2AAW
Cations vs Anions
 An atom will lose an
electron to become a
cation
 An atom will gain an
electron to become an
anion
Demo
I NEED 3 POSITIVE STUDENTS AND 3
NEGATIVE STUDENS
Ionization Energy
 The ionization energy
is the energy required to
remove the first electron
from an atom
 Table on p. 177
 Will decrease from top to
bottom in a group and
increase from left to right
across a period
Demos
 Sodium in Water
 Potassium in Water
 Rubidium in Water
 Cesium in Water
 Cesium in Water (slow-mo)
Ionic Size
 The size of ions tends to increase from top
to bottom within a group. They will
decrease from left to right across a period
Electronegativity
 Electronegativity is
the ability of an atom of
an element to attract
electrons when the
element is in a
compound

Defined by Linus Pauling
 Electronegativity values
tend to decrease from
top to bottom in a group,
and increase from left to
right in a period
Review
 How does ionization energy increase?
 What will produce larger ions, Oxygen or Nitrogen?
 What has a larger atomic radius, Cesium or Potassium?
 Which is more likely to attract more electrons, Silicon or
Sulfur?
Homework
 Finish Graph- to be handed in