Transcript Chapter 6 The Periodic Table

Chapter 6
The Periodic Table
Stylish Shoes
What is in common with all the pictures below?
Which one does not belong?
Which one does not belong?
Which one does not belong?
Which one does not belong?
History of the Periodic Table
 1869
- Mendeleev published a
classification scheme of all the
currently known elements
 Organized
elements
based on
similar
characteristics.
 Left
blank spaces in table for
undiscovered
elements.
Mendeleev’s Periodic Table (1869)
Mendeleev arranged the elements on his
table in order of increasing
atomic mass.
Many scientist suggested other periodic
tables.
Albert Tarantola’s
Orbital Table
Timothy Stowe – Table for Physicists
Theodor Benfey
Emil Zmaczynski
Vocational Exile Periodic Table
The Periodic Law

In the modern periodic
table, elements are arranged
in order of
increasing
atomic number
Periodic Law –
when elements are arranged in order of
increasing
atomic number,
there is a trend in their physical and
chemical properties
Metals, Metalloids and Nonmetals
 Elements
can be grouped into
three broad classes based on their
general properties
Metals
Nonmetals
Metalloids
 Metals:
 Generally
solid at room temp.
 Ductile – drawn into wires.
 Malleable – hammered into sheets
 Shiny surface
 Conduct heat and electricity
Metals
• Nonmetals:
• Varying properties, but are generally
poor conductors
of heat and electricity
• Brittle
Non-metals

Nonconductors
• Metalloids:
• some properties
of metals and nonmetals
• Intermediate
Metalloids or Semimetals

Properties of both
Practice

Tell me all you can about the
following elements:
1. Titanium (Ti)
2. Germanium (Ge)
3. Calcium (Ca)
4. Fluorine (F)
Section 6.2 - Classifying the Elements
 The
periodic table displays the
symbols and names of
the elements, along with
information
about the structure of their atoms (# of
protons, neutrons, and electrons)
Black symbol = solid
 Green = gas
 Blue = liquid

Electron Configurations in Groups

Elements can be sorted into 4 different
groupings based on their electron
configurations:
1) Noble gases
2) Representative elements
3) Transition metals
4) Inner transition metals
Representative
Noble Gases
Transition
Inner Trans.
Electron Configurations in Groups
1) Noble gases
elements in Group 8A
2) Very stable = do not react
•
Noble gases have an electron
configuration that has the outer s
and p sublevels completely full
Circle the Noble Gases
Ci
Electron Configurations in Groups
2) Representative Elements
are in Groups 1A through 7A
• Display wide range of
properties, thus a good
“representative”
• Include metals, nonmetals,
metalloids, solids, gases, or liquids
• Their outer s and p electron
configurations are NOT filled
Circle the Representative Elements
Ci
Electron Configurations in Groups
3) Transition metals are in the “B”
columns of the periodic table
•
Electron configuration has
outer s sublevel full
Elements in the “d” sublevel
•
•
A “transition” between the metal area and
the nonmetal area
Circle the Transition Metals
Ci
Electron Configurations in Groups
4) Inner Transition Metals are
located below the main body of
the table, in two horizontal rows
•
•
Electron configuration has the
outer s sublevel full
Elements in the f sublevel
Circle the Inner Transition Metals
Ci
1A
 Elements
2A
in the 1A-7A groups
are called the representative
3A 4A 5A 6A 7A
elements
outer s or p filling
8A
The group B are called the
transition elements
 These
are called the inner
transition elements, and they
belong here
Groups of elements - family names
1A – alkali metals
 Forms a “base” (or alkali) when reacting
with water
Exception is Hydrogen
 Group 2A – alkaline earth metals
 Also form bases with water; do not
dissolve well, hence “earth metals”
 Group 7A – halogens
 Means “salt-forming”
 Group
Group 1A - alkali metals (but NOT H)
Group 2A - alkaline earth metals
H
 Group
8A are the noble gases
 Group 7A is called the halogens
The Groups of the Periodic Table
 Groups
of the periodic table:
 Representative
Elements
 Noble
Gases
 Transition Metals
 Inner Transition Metals
 Family
 Alkali
names:
metals
 Alkaline earth metals
 Halogens
Practice

Tell me all you can about the
following elements:
1. Titanium (Ti)
2. Germanium (Ge)
3. Calcium (Ca)
4. Fluorine (F)
Section 6.3 – Periodic Trends


Properties of elements are related to
their location on the periodic table
We will be studying 3 periodic trends:
–Atomic Radius
–Ionization Energy
–Electronegativity
1. Atomic Radius or Atomic Size
 One-half
the distance from
center to center
of two atoms
Atomic
Radius
Atomic Radius or Atomic Size
What do you notice about the atomic radii
of the elements on the periodic table?
Atomic Radius increases towards the
bottom left corner of the PT
Atomic Radius/Size Practice
 Which
element has a greater atomic
radius?
F or Cs
Ga or K
Kr or Rb
Ba or Si
Fr or W
O or Ag
Ions
 Normally,
atoms are neutral because
they have the same number
of protons and electrons
 When
elements combine in
compounds, they transfer electrons.
 Ions
are atoms that have a
positive or negative charge.
Transfer of
an electron
forms two
ions:
a cation
and anion
Na+
Cations

Cation – an ion with a
positive charge (lost electrons)
Circle the
cation
Na+
Anions
 Anion
– an ion with a
negative charge
gained electrons)
Circle the
anion
Na+
Ionic Size
 Cations
are always
smaller than the atoms
from which they form
 Anions
are always
larger than the atoms
from which they form
Before
After
• Does this make sense?
• Where are electrons located in the
atom?
• Around the nucleus
• The more electrons
around the nucleus,
the larger the atom
will be.
Practice
 Which
Na
of the following is larger?
or Na+
Al or Al3+
I or ICa2+ or Ca
S or S2O2- or O
2. Ionization Energy

The energy required to
remove an electron
from an atom
Ionization Energy

What trend do you notice about the ionization
energy of the elements on the periodic table?
Ionization Energy increases
towards the top right
corner of the PT
• Does this make sense?
• Which elements are the most
stable?
• Elements with full orbitals
• The more stable
the elements is,
the harder it will be
to remove an electron.
Ionization Energy Practice
 Which
of these elements has a
greater ionization energy?
Kr or Ar
Al or Na
S or Rb
Si or Cs
He or Ca
P or O
3. Electronegativity (EN)
 The
ability of an atom to
attract electrons
to itself when in a compound
Electronegativity
What trend do you notice about the electronegativity of
the elements on the periodic table?
Electronegativity increases
towards the top right
corner of the PT
• Does this make sense?
• Which elements want electrons?
• Elements closest to
filling their orbitals
• The closer the
elements is to filling its orbital,
the more it will
attract electrons.
Electronegativity Practice
 Which
element has greater
electronegativity?
Na or F
Ca or C
Al or Mg
Sr or Al
Ca or K
Cl or F
Draw a diagonal arrow showing
increasing atomic size
Draw a diagonal arrow showing
increasing ionization energy
Draw a diagonal arrow showing
increasing electronegativity