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The Periodic Table and Periodic Law
Section 6.1 Development of the
Modern Periodic Table
Section 6.2 Classification of the
Elements
Section 6.3 Periodic Trends
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Section 6.1 Development of the Modern
Periodic Table (cont.)
periodic law
group
period
representative elements
transition elements
metal
alkali metals
alkaline earth metals
transition metal
inner transition metal
lanthanide series
actinide series
nonmetals
halogen
noble gas
metalloid
Section 6.1 Development of the Modern
Periodic Table
• Trace the development of the periodic table.
• Identify key features of the periodic table.
atomic number: the number of protons in an atom
The periodic table evolved over
time as scientists discovered more
useful ways to compare and
organize the elements.
Development of the Periodic Table
• In the 1700s, Lavoisier compiled a list of all
the known elements of the time.
Development of the Periodic Table (cont.)
• The 1800s brought large amounts of
information and scientists needed a way to
organize knowledge about elements.
• John Newlands proposed an arrangement
where elements were ordered by increasing
atomic mass.
Development of the Periodic Table (cont.)
• Newlands noticed
when the elements
were arranged by
increasing atomic
mass, their
properties repeated
every eighth
element. This was
called the law of
octaves.
Development of the Periodic Table (cont.)
• Meyer and Mendeleev both demonstrated
a connection between atomic mass and
elemental properties.
• When creating his periodic table, Mendeleev
left blank spaces for elements that had not
yet been discovered.
• Using periodic properties of the other
elements, he correctly predicted the
properties of scandium, gallium, and
germanium.
Development of the Periodic Table (cont.)
• Moseley rearranged the table by
increasing atomic number, and resulted
in a clear periodic pattern – our modern
periodic table.
• Periodic repetition of chemical and
physical properties of the elements when
they are arranged by increasing atomic
number is called periodic law.
Development of the Periodic Table (cont.)
The Modern Periodic Table
• The modern periodic table contains boxes
which contain the element's name, symbol,
atomic number, and atomic mass.
http://periodictable.com/
The Modern Periodic Table (cont.)
• Columns of elements are called groups.
• Rows of elements are called periods.
• Elements in groups 1,2, and 13-18 possess a
wide variety of chemical and physical
properties and are called the representative
elements.
• Elements are classified as metals,
non-metals, and metalloids.
Metals
• Metals are elements that are generally shiny
when smooth and clean, solid at room
temperature, good conductors of heat and
electricity, malleable, and ductile.
• Alkali metals are all the elements in group 1
except hydrogen, and are very reactive.
• Alkaline earth metals are in group 2, and
are also highly reactive.
Metals (cont.)
• Groups 3-12 are called the transition
metals.
• The two rows under the periodic table are
called the inner transition metals.
Nonmetals
• Non-metals are elements that are
generally gases or brittle, dull-looking
solids, and poor conductors of heat and
electricity.
• Group 17 is composed of highly reactive
elements called halogens.
• Group 18 gases are extremely unreactive and
commonly called noble gases.
Metalloids
• Metalloids have physical and chemical
properties of both metals and non-metals,
such as silicon and germanium.
• The metalloids form a staircase that
separates the metals from the nonmetals,
with the exception of aluminum which is a
metal.
• Metalloids: B, Si, Ge, As, Sb, Te, Po, & At
The Modern Periodic Table
Section 6.1 Assessment
What is a row of elements on the periodic
table called?
A. octave
B. period
D
A
0%
C
D. transition
A. A
B. B
C. C
0%
0%
0%
D. D
B
C. group
Section 6.1 Assessment
What is silicon an example of?
A. metal
B. non-metal
C. inner transition metal
D
C
A
0%
B
D. metalloid
A. A
B. B
C. C
0%
0%
0%
D. D
Section 6.2 Classification of the Elements
• Explain why elements in
the same group have
similar properties.
• Identify the four blocks
of the periodic table
based on their electron
configuration.
valence electron:
electron in an atom's
outermost orbitals;
determines the chemical
properties of an atom
Elements are organized into different
blocks in the periodic table according
to their electron configurations.
Organizing the Elements by Electron
Configuration
• Recall electrons in the highest principal
energy level are called valence electrons.
• Groups can help determine how many
valence electrons an atom has.
Organizing the Elements by Electron
Configuration (cont.)
• Group 1 elements have 1 valence e- and
group 2 elements have 2 valence e-.
• The number of valence electrons for
elements in groups 13-18 is ten less than
their group number.
• Remember, the maximum number of valence
e- is 8.
Organizing the Elements by Electron
Configuration (cont.)
The s-, p-, d-, and f-Block Elements (cont.)
• The Noble Gases are the only elements that
have completely filled orbitals. He has 2
valence e- and the other noble gases all have
8 valence e-.
• Since they have a full valence, the Noble
Gases are very unreactive.
Section 6.2 Assessment
Which of the following is NOT one of the
elemental blocks of the periodic table?
A. s-block
B. d-block
D
A
0%
C
D. f-block
A. A
B. B
C. C
0%
0%
0%
D. D
B
C. g-block
Section 6.2 Assessment
Which block spans 14 elemental groups?
A. s-block
B. p-block
C. f-block
D
C
A
0%
B
D. g-block
A. A
B. B
C. C
0%
0%
0%
D. D
Section 6.3 Periodic Trends
• Compare period and
group trends of several
properties.
• Relate period and group
trends in atomic radii to
electron configuration.
principal energy level:
the major energy level of
an atom
ion
ionization energy
octet rule
electronegativity
Trends among elements in the periodic
table include their size and their ability
to lose or attract electrons
Atomic Radius
• Atomic size is influenced by the
arrangement of electrons around the
nucleus..
• Atomic radius is the ½ the distance between
two adjacent nuclei.
Atomic Radius (cont.)
• There is a
general
decrease in
atomic
radius from
left to right,
as protons
are added
the nucleus
pulls the
electrons in
tighter.
Atomic Radius (cont.)
• Atomic radius generally increases as you
move down a group because energy levels
are being added.
Ionic Radius
• An ion is an atom or bonded group of
atoms with a positive or negative charge.
• When atoms lose electrons, a positively
charged ion is formed.
• It will be smaller because the remaining
electrons are pulled closer to the nucleus.
Ionic Radius (cont.)
• When atoms gain electrons, a negatively
charged ion is formed.
• It will be larger because the electrons repel
each other more and must spread out.
Ionic Radius (cont.)
• The ionic radii of positive ions generally
decrease from left to right.
• The ionic radii of negative ions generally
decrease from left to right, beginning with
group 15 or 16.
Ionic Radius (cont.)
• Both positive and negative ions increase
in size moving down a group.
Ionization Energy
• Ionization energy is defined as the energy
required to remove an electron from a
gaseous atom.
• Noble Gases have the highest IE since they
do not want to lose any electrons from their
full valence.
• Each time an electron is removed, more IE is
required.
Ionization Energy (cont.)
Ionization Energy (cont.)
Ionization Energy (cont.)
• The ionization at which the large increase
in energy occurs is related to the number of
valence electrons.
• First ionization energy increases from left to
right across a period.
• First ionization energy decreases down a
group because less energy is required to
remove an electron farther from the nucleus.
• Metals have low IE and nonmetals have
high IE.
Ionization Energy (cont.)
Ionization Energy (cont.)
• The octet rule states that atoms tend to
gain, lose or share electrons in order to
acquire a full set of eight valence electrons.
• The octet rule is useful for predicting what
types of ions an element is likely to form.
Electronegativity
• The electronegativity of an element
indicates its relative ability to attract
electrons in a chemical bond.
• Electronegativity increases left to right
across a period and decreases down a
group .
• Metals have low EN and nonmetals have
high EN.
• There are no EN values given for the Noble
gases because they already have a full
valence.
Electronegativity (cont.)
Section 6.3 Assessment
The lowest ionization energy is the ____.
A. first
B. second
C. third
D
C
A
0%
B
D. fourth
A. A
B. B
C. C
0%
0%
0%
D. D
Section 6.3 Assessment
The ionic radius of a negative ion
becomes larger when:
A. moving up a group
B. moving right to left across period
D
A
0%
C
D. the ion loses electrons
A. A
B. B
C. C
0%
0%
0%
D. D
B
C. moving down a group
Chemistry Online
Study Guide
Chapter Assessment
Standardized Test Practice
Image Bank
Concepts in Motion
Section 6.1 Development of the
Modern Periodic Table
Key Concepts
• The elements were first organized by increasing
atomic mass, which led to inconsistencies. Later,
they were organized by increasing atomic number.
• The periodic law states that when the elements are
arranged by increasing atomic number, there is a
periodic repetition of their chemical and physical
properties.
• The periodic table organizes the elements into periods
(rows) and groups (columns); elements with similar
properties are in the same group.
Section 6.1 Development of the
Modern Periodic Table (contd.)
Key Concepts
• Elements are classified as either metals, nonmetals,
or metalloids.
Section 6.2 Classification of
the Elements
Key Concepts
• The periodic table has four blocks (s, p, d, f).
• Elements within a group have similar chemical
properties.
• The group number for elements in groups 1 and 2
equals the element’s number of valence electrons.
• The energy level of an atom’s valence electrons equals
its period number.
Section 6.3 Periodic Trends
Key Concepts
• Atomic and ionic radii decrease from left to right
across a period, and increase as you move down a
group.
• Ionization energies generally increase from left to right
across a period, and decrease as you move down a
group.
• The octet rule states that atoms gain, lose, or share
electrons to acquire a full set of eight valence electrons.
• Electronegativity generally increases from left to right
across a period, and decreases as you move down a
group.
The actinide series is part of the
A. s-block elements.
B. inner transition metals.
C. non-metals.
D
C
A
0%
B
D. alkali metals.
A. A
B. B
C. C
0%
0%
0%
D. D
In their elemental state, which group has a
complete octet of valence electrons?
A. alkali metals
B. alkaline earth metals
D
A
0%
C
D. noble gases
A. A
B. B
C. C
0%
0%
0%
D. D
B
C. halogens
Which block contains the transition
metals?
A. s-block
B. p-block
D
A
0%
C
D. f-block
A. A
B. B
C. C
0%
0%
0%
D. D
B
C. d-block
An element with a full octet has how many
valence electrons?
A. two
B. six
D
A
0%
C
D. ten
A. A
B. B
C. C
0%
0%
0%
D. D
B
C. eight
How many groups of elements are there?
A. 8
B. 16
C. 18
D
C
A
0%
B
D. 4
A. A
B. B
C. C
0%
0%
0%
D. D
Which group of elements are the least
reactive?
A. alkali metals
B. inner transition metals
D
A
0%
C
D. noble gases
A. A
B. B
C. C
0%
0%
0%
D. D
B
C. halogens
On the modern periodic table, alkaline
earth metals are found only in ____.
A. group 1
B. s-block
D
A
0%
C
D. groups 13–18
A. A
B. B
C. C
0%
0%
0%
D. D
B
C. p-block
Unreactive gases are mostly found where
on the periodic table?
A. halogens
B. group 1 and 2
D
A
0%
C
D. f-block
A. A
B. B
C. C
0%
0%
0%
D. D
B
C. group 18
Bromine is a member of the
A. noble gases.
B. inner transition metals.
C. earth metals.
D
C
A
0%
B
D. halogens.
A. A
B. B
C. C
0%
0%
0%
D. D
How many groups does the d-block span?
A. two
B. six
C. ten
D
C
A
0%
B
D. fourteen
A. A
B. B
C. C
0%
0%
0%
D. D
Click on an image to enlarge.
Table 6.4
Noble Gas Electron
Configuration
Figure 6.5
The Periodic Table
Figure 6.11 Trends in Atomic Radii
Figure 6.18 Trends in Electronegativity
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