Starter: Breaking Down
Misconceptions
 Determine which of the following are true or false.
Justify the statements you consider to be false.
1. The Modern Periodic Table organizes the
elements based on atomic weight (mass).
2. Longitude is to GROUPS as Latitude is to
PERIODS.
3. Although over 100 elements are found on the
Periodic Table, several of them do not really
exist.
Mendeleev Activity
(The Hoya Table)
 Organize yourselves into columns according to your
similar physical properties and rows based on your age.
 Mendeleev and Moseley will facilitate. All students
should help!
 The only rule is that Girls must be on the left side of
the room and Boys on the left. The middle row can be
mixed.
 Possible properties that you could use: shirt color, hair
color, glasses, shoe types, shirt type
 You have 8 minutes to get as many of your classmates
seated as possible. May the best Hoya Table win!
Pre-Periodic Table Chemistry
…
 …was a mess!!!
 No organization of
elements.
 Imagine going to a
grocery store with no
organization!!
 Difficult to find
information.
 Chemistry didn’t make
sense.
History of the Periodic Table:
Mendeleev vs Moseley
MENDELEEV
 Arranged the elements by
MOSELEY
 Developed a new
understanding of periodic law
increasing ATOMIC
and REVISED Mendeleev’s
WEIGHT
organization of the PT
 Put elements in columns by  Realized that atomic mass
the way they reacted.
(weight) was NOT as
 He left blank spaces for what
important in the organization
he said were undiscovered
of the elements as the
elements. (Turned out he
ATOMIC NUMBER
was right!)
 Arranged the elements in
order of increasing ATOMIC
NUMBER
Background: The Periodic Law
The Periodic Law states that there
is a recurring pattern in the
PROPERTIES of elements when
they are arranged in order of
INCREASING ATOMIC NUMBER.
This pattern can be seen every 8
representative elements
The Periodic Road Map
GROUPS
PERIODS
 Groups are the COLUMNS found  Periods are the ROWS on
on the PT
 Elements in the same GROUP:
 Apart of the same FAMILY
 Have the SAME number of
valence electrons
 Form the same kinds of IONS
What would this say about their
properties?
 They demonstrate SIMILAR
properties
the PT
 There are 7 periods on the
PT that represent the 7
principal energy levels
within the atom
 Elements in the same
PERIOD:
 Valence Electrons exist
within the SAME principal
energy level
What BLOCK do you stay on?
 The PT can also be broken down into a BLOCK
SYSTEM
 Elements on the PT reside in certain blocks which are
reflected at the end of their electron configuration
 The block system is based on the SUBLEVELS that
electrons can be found in within the atom. What are
they?
 S, P, D, F
What BLOCK do you stay on?
S block: blue
D block: red
P block: yellow
F block: green
To Be or Not To Be…
 Elements on the PT are either Metal, Non-metal or
Metalloid
 These differences affect the properties of the elements
 METALS: solid at room temp, tend to LOSE electrons to
become more stable (+ IONs), on the LEFT SIDE of the
PT, good conductors of energy
 NON-Metals: typically your gases, tend to GAIN
electrons to become more stable (- IONs), on the RIGHT
SIDE of the PT, poor conductors of energy
 METALLOIDS: found in between metals and nonmetals and so are their properties, on the STAIRCASE in
the middle right of the table
To Be or Not To Be…
Metals = Blue
Metalloids = Pink
Non-metals = Yellow
Starter: PT Anatomy CFU
 Explain the difference between
Mendeleev’s and Moseley’s organization of
the Periodic Table.
 What are the columns and rows on the
Periodic Table called and what
information can you pull from them?
 Which element would conduct electricity
better, Phosphorus or Sodium? Why?
Families on the Periodic Table
 Elements on the periodic table can be grouped into
families bases on their chemical properties.
 Each family has a specific name to differentiate it
from the other families in the periodic table.
 Elements in each family have a stronger reactions as
you move down the table. Why?
Their valence electrons have more energy (on a higher
energy level)
ALKALI METALS
Group 1
 Hydrogen is not a member, it is
a non-metal
 1 electron in the outer shell
 Soft and silvery metals
 Very reactive, esp. with water
 Conduct electricity
Image: http://www.learner.org/interactives/periodic/groups2.html
ALKALINE EARTH METALS
Group 2
 2 electrons in the
outer shell
 White and
malleable
 Reactive, but less
than Alkali metals
 Conduct electricity
TRANSITION METALS
Groups in the middle
 Good conductors of
heat and electricity.
 Some are used for
jewelry.
 The transition metals
are able to put up to 32
electrons in their
second to last shell.
 Can bond with many
elements in a variety of
shapes.
BORON FAMILY
Group 3
 3 electrons in the
outer shell
 Most are metals
 Boron is a
metalloid
CARBON FAMILY
Group 4
 4 electrons in the
outer shell
 Contains metals,
metalloids, and a
non-metal Carbon
(C)
NITROGEN FAMILY
Group 5
 5 electrons in the
outer shell
 Can share electrons
to form compounds
 Contains metals,
metalloids, and
non-metals
OXYGEN FAMILY
Group 6
 6 electrons in the
outer shell
 Contains metals,
metalloids, and
non-metals
 Reactive
Halogens
Group 7
 7 electrons in the
outer shell
 All are non-metals
 Very reactive are
often bonded with
elements from
Group 1
Noble Gases
Group 8
 Exist as gases
 Non-metals
 8 electrons in the
outer shell = Full
 Helium (He) has
only 2 electrons in
the outer shell =
Full
 Not reactive with
other elements
 Do NOT lose or
gain electrons;
They’re already
stable
Rare Earth Metals:
Lanthanides and Actinides
 Some are
Radioactive
 The rare earths
are silver, silverywhite, or gray
metals.
 Conduct
electricity
 Can also be
called Inner
Transition Metals
Periodicity Part II: TRENDS
 You must know the following trends for on the PT:
Atomic Radius
2. Ionic Radius
3. Electronegativity
4. Ionization Energy
1.
Trend 1: Atomic Radius
 Atomic Radius is
A measure of the size of the atom
half of the distance between the centers
of two atoms of that element that are
just touching each other
 Measured from the nucleus to the
boundary of the farthest (highest)
energy level for the valence
electrons
Trend 2: Ionic Radius
 Ionic Radius is…
A measure of the size of the ion
half of the distance between the centers
of two atoms of that element that are
just touching each other
 Measured from the nucleus to the
boundary of the farthest (highest)
energy level for valence electrons
Trend 3: Electronegativity
 Electronegativity is…
a measure of the tendency of an
atom to attract electrons
 the desire an atom has for
electrons in a bond
 Similar to Electron Affinity
Trend 4: Ionization Energy
 Ionization energy is the amount of
energy REQUIRED to remove an
electron from an atom
The Trends…What you need to
know
 Know what each trend means
 How they change as you move to the…
Right and left of a period
2. Up and down a group
 Be able to compare the elements
according to the trends
1.
PT Trends Activity
Periodic Table Trends
Mendeleev’s Castle
 Google: PT Trends
 Complete the
activity and
lynchburg
 Click on Cool PT
 Use the information that
you find when you click on
each element to complete
the WS
 Important: You will have a
quiz on this on Friday!
correctly answer the
questions
 Important: This
assignment is due at
the end of class!
Starter: Analyzing Trends
 Explain the difference between the 4
trends on the Periodic Table.
 Does Sodium or Chlorine have a higher
electronegativity?
 Does Copper or Gold have a higher atomic
radius?
 Does Potassium or Xenon have a higher 1st
Ionization energy?
Analyzing Trends
 Important:
When analyzing a trend for elements in
different groups and different
periods…
1. consider the trend going down the
group
2. consider the trend going across the
period.
Analyzing the Trends
Atomic Radius
 Increases as you move
Ionic Radius
 Increases as you move
DOWN the PT
DOWN the PT
Why? You’ve added more
Why? You’ve added more
energy levels.
energy levels
 As you move across the PT…
 Decreases as you move to the
- Decreases for Metals because
RIGHT of the PT
they tend to _______
Why? The force of the nucleus
electrons. (+ Ion = Cation)
is stronger and it pulls the
- Increases for Non-metals
electrons closer
because they tend to _______
electrons ( - Ion = Anion)
Analyzing the Trends
Electronegativity
 Decreases as you move
Ionization Energy
 Decreases as you move DOWN
the PT
DOWN the PT
Why? Electrons are farther out
Why? The attraction of the
from the nucleus which has less
positive nucleus decreases as
of a hold; more likely to get
the shell gets farther.
taken because it takes less
 Increases as you move to the
energy
RIGHT across the PT
 Increases as you move to the
Why? Elements want electrons
RIGHT across the PT
more and more to become
Why? As you move to the right
more stable.
the elements really want to
keep their electrons so it
requires more energy to take
them.
Diatomic Molecules
 Why do atoms form ions?
 To Become More STABLE!
 Well…a few elements can also do something else to
become stable.
 They come together and share electrons (or BOND)
with each other. They are called DIATOMIC
MOLECULES.
 Here are the Diatomic Molecules (Pay attention to
which elements can form Diatomic Molecules!)
N2, O2, F2, Cl2, H2, Br2, & I2
Starter:
 Which is larger Ra or Ra+2 ? I or I-? Why?
 Identify at least 1 element in the following
families and what kind of ions they would form:
Halogen, Alkali metals, Alkaline earth metals
 Bromine has less Ionization energy and less
Electronegativity than Fluorine. Explain why
this is.
 Which would have a more violent reaction to
the same stimuli, Potassium or Francium? Why?
Introduction to Halide Lab:
 In this lab, you will explore ions of the elements in
Group 7A. Which family will you be observing?
 Your objective is to mix the solutions containing
these ions with Silver Nitrate and Lead Nitrate.
 Record your observations in the data table
provided. You may write on the lab handout.
 While in the lab area, be sure to wear your goggles
and apron at all times.
 This assignment is graded and will be turned in
today, so be sure to stay on task!
Halide Lab
(Important Information):
 Once you have completed the lab and cleaned
your lab area, put your safety materials away and
begin to answer the Analysis questions.
 You are responsible the following questions: 2, 3
(excluding the equation portion), 4, and the
question below
 Based on your understanding of families on
the Periodic Table, which halide ion would
you expect to have the most reactivity in this
experiment? Least reactivity? Why?
Focus of Study:
 Know the history of the PT (Mendeleev vs Moseley)
 Know the organization of the PT (sublevel blocks,
groups, periods, Metals vs Metalloids vs Nonmetals)
 Know the difference between GROUPS (FAMILY)
and PERIODS; How to determine them…
(Groups – same valence e- = similar activity/properties
and types of IONS; Periods – principal (valence)
energy level)
 Know the 4 trends and their meaning
- Be able to explain WHY the trends occur as they do
Starter: Do You Know the PT
 What is the valence energy level and number of
valence electrons in Silicon?
 Does Copper, Gold, or Cadmium have a higher
atomic radius?
 Does Cesium, Barium, or Francium have a lower
1st ionization energy?
 Does Oxygen, Sulfur or Fluorine have a higher
electronegativity?