Download power point

Assignments
I have found related jognog quizzes you can do for
extra point’s pts. to replace the missing naming HW.
There is also a balancing equations page to use as make
up points on those assignments. Jognog Code JSX4R7F
(All scores have to be greater than 85% to earn
credits.)
In addition I have assigned you three periodic table
jognog quizzes to go along with the power point I have
assigned you for the break. Please have these
completed by the time we are back at school.
Introduction to the
Periodic Table
Atomic Number ● Symbol ● Atomic Weight
Element ● Compound ● Mixture
Periodicity Objectives
Be able to:
 Explain how the early versions of the periodic table was organized by the
following people
– Mendeleev
– Mosley



State the periodic law
Define Periods and groups/families of the table
Identify the following groupings in the table and their tables
– Metals, non-metals, metalloids,
– Alkali metals, Alkali earth metals, transition metals, Halogens, noble gases,
Rare earth elements(Lanthanide and actinide series)

Describe the following trends in the periodic table. (Trends through the
period and the family.)
–
–
–
–

Atomic Radii
Density
Ionization energy
Electron affinity/ electronegativity
List or identify the properties of the metals and non-metals.
Homework
 Take
notes on the previously listed
objectives. You can also color in a
periodic table to identify the areas
required. Use the periodic tables in
your notes or download one and use
your smart phones to label it. Be
resourceful. Also, I have assigned you
two jognog quizzes to complete. You
will only receive credit if you earn 85%
or above.
 Jognog code JSX4R7F
I am Dmitri Mendeleev!
I made the PERIODIC TABLE !
Mendeleev’s Periodic Table
“I began to look about and
write down the elements
with their atomic weights
and typical properties,
analogous elements and
like atomic weights on
separate cards, and this
soon convinced me that the
properties of elements are
in periodic dependence
upon their atomic weights.”
--Mendeleev, Principles of
Chemistry, 1905, Vol. II
What is the PERIODIC TABLE?
o
Shows all known
elements in the universe.
o
Organizes the elements
by chemical properties.
How do you read the
PERIODIC TABLE?
What is the ATOMIC NUMBER?
o
o
The number of
protons found in the
nucleus of an atom
Or
The number of
electrons surrounding
the nucleus of an
atom.
What is the SYMBOL?
o
An abbreviation of
the element name.
What is the ATOMIC WEIGHT?
o
The number of protons
and neutrons in the
nucleus of an atom.
How do I find the number of protons,
electrons, and neutrons in an element
using the periodic table?
o
# of PROTONS
= ATOMIC NUMBER
o
# of ELECTRONS = ATOMIC NUMBER
o
# of NEUTRONS = ATOMIC _ ATOMIC
WEIGHT
NUMBER
Now you are almost as smart as
I am!
But not as handsome!
Man, I look GOOD!
What is an ELEMENT?
o
A substance
composed of a
single kind of atom.
o
Cannot be broken
down into another
substance by
chemical or physical
means.
What is a COMPOUND?
o
A substance in
which two or
more different
elements are
CHEMICALLY
bonded together.
What is a MIXTURE?
o
Two or more
substances that
are mixed
together but are
NOT chemically
bonded.
You are still not as handsome as
the great Mendeleev!
I am working this beard!
Man, I look GOOD!
Henry Moseley (1887-1915)
English chemist
Worked with Rutherford

Proved Mendeleev’s
arrangement of the
periodic table to be correct
– only, the periodic table
was arranged according to
atomic number, not atomic
mass


The Periodic Law
States that when elements are
arranged in order of increasing
atomic number, their physical and
chemical properties show a periodic
pattern

How do we read the table?

The modern periodic table has 118 squares, which
represent a unique element. The distinctive shape of the
periodic table comes in part from the periodic law.
Elements in the same column have similar properties.
These columns are referred to as groups or families of
elements. The horizontal rows of the periodic table are
called periods. The elements in the periodic table are also
grouped as metals, nonmetals, and semimetals. Metals
make up most of the periodic table and are located in the
center and at the left of the table. With the exception of
hydrogen, nonmetals are on the right side, and semimetals
are located between the metals and nonmetals.
metals, nonmetals and metalloids.
METALS
METALLOIDS
NONMETALS

Nonmetals






Good
conductors of
heat and
electricity
Malleable
Ductile
Luster
Typically
solids at room
temperature



Nonmetals
Solids, liquids
and gases at
room
temperature
Solids are
brittle and dull
Poor
conductors of
heat and
electricity




Metalloids
Have
properties of
both metals
and
nonmetals
Mostly brittle
solids
Intermediate
conductors of
electricityAKA
semiconductor
ALKALI METALS
Extremely reactive
Readily react
with water and
air
Silvery in appearance
Soft enough to cut with a
knife
Lower densities than other
metals
Lower melting points than
other metals
ALKALINE-EARTH METALS
Harder & stronger than
alkali metals
Higher densities &
melting points than alkali
metals
Less reactive than alkali
metals
HALOGENS
Most reactive nonmetals
React readily with most
metals to form salts
Most electronegative
elements
NOBLE GASES
Least reactive elements
because their highest
occupied energy levels
are completely filled
with an octet of
electrons (except He,
which only requires 2
electrons to be filled).
TRANSITION METALS
High densities
High melting points
Good conductors of heat
& electricity
High luster
Less reactive than alkali
and alkaline-earth metals
INNER TRANSITION
(Rare Earth) METALS
LANTHANIDES
Soft, silvery metals
Similar reactivity to
alkaline-earth metals
ACTINIDES
All radioactive
The first 4 have
been found
naturally on Earth
PERIODS
GROUPS
Atomic radius - Decreases across a period.
Protons are added to the nucleus moving across
a period from left to right. This increases the
charge of the nucleus and electrons are pulled
closer to the nucleus.
Atomic Radii
Variations in Ionization Energies
Energy vs Atomic
Number
Ionization Energy - The energy required to take an electron and
become ionized. Chemical activity and bonding depends on taking or
sharing electrons Getting to big makes it harder to hold onto E-.
Being smaller allows you to grab E- from other atoms.
Ionization Energy Trends
INCREASES
INCREASES
Electronegativity
A
measure of the ability of an atom
in a chemical compound to attract a
bonding pair of electrons
 NOTE
*Electronegativity is a
property of atoms in compounds and
thus differs from ionization energy
and electron affinity, which are
properties of isolated atoms*
Trends
 Increase
across a period
Effective nuclear charge increases
 Decrease
down a group
Increase in atomic size and increase in electron shielding decreases the
effective nuclear charge
 Electronegativity
depends upon:
The number of protons in the nucleus
The distance from the nucleus
Electron shielding
Electronegativity trends
INCREASES
INCREASES
Big Picture



Fluorine and Francium are the most
reactive elements. How do you asses an
atoms reactivity? Reactivity depends on
# of Protons, The distance from the
nucleus and Electron shielding
Moving towards Fluorine on the table, protons
increase. This means greater attraction to eand grabbing free or weakly held e-.
Moving towards Francium the E- shells
increase. Full electron shells means greater
electron repulsion and less attractive forces to
e- in the outer shell.
Electronegativity Trends
INCREASES
INCREASES