Chemistry: Matter and Change

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Chapter Menu
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
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
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Section 6-1
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.
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Section 6-1
Development of the Periodic Table

• In the 1700s, Lavoisier compiled a list of all
  the known elements of the time.

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Section 6-1
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.

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Section 6-1
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.

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Section 6-1
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.

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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.

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Section 6-1
Development of the Periodic Table (cont.)
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Section 6-1
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/
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Section 6-1
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.

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Section 6-1
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.

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Section 6-1
Metals (cont.)

• Groups 3-12 are called the transition metals.

• The two rows under the periodic table are called
  the inner transition metals.

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Section 6-1
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.

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Section 6-1
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

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Section 6-1
The Modern Periodic Table
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Section 6-1
Section 6.1 Assessment
What is a row of elements on the periodic table
called? A. octave B. period C. group
D. transition

1. A
2. B
3. C
4. D

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Section 6-1
Section 6.1 Assessment
What is silicon an example of? A. metal
B. non-metal C. inner transition metal
D. metalloid

1. A
2. B
3. C
4. D

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End of Section 6-1
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Section 6-2
Section 6.2 Classification of the Elements

• Explain why elements in the same group have
  similar properties.

valence electron electron in an atom's outermost
orbitals determines the chemical properties of
an atom

• Identify the four blocks of the periodic table
  based on their electron configuration.

Elements are organized into different blocks in
the periodic table according to their electron
configurations.
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Section 6-2
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.

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Section 6-2
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.

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Section 6-2
Organizing the Elements by Electron Configuration
(cont.)
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Section 6-2
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.

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Section 6-2
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 C. g-block D. f-block

1. A
2. B
3. C
4. D

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Section 6-2
Section 6.2 Assessment
Which block spans 14 elemental groups?
A. s-block B. p-block C. f-block D. g-block

1. A
2. B
3. C
4. D

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End of Section 6-2
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Section 6-3
Section 6.3 Periodic Trends

• Compare period and group trends of several
  properties.

principal energy level the major energy level of
an atom

• Relate period and group trends in atomic radii to
  electron configuration.

ion ionization energy octet rule electronegativity
Trends among elements in the periodic table
include their size and their ability to lose or
attract electrons
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Section 6-3
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.

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Section 6-3
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.

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Section 6-3
Atomic Radius (cont.)

• Atomic radius generally increases as you move
  down a group because energy levels are being
  added.

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Section 6-3
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.

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Section 6-3
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.

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Section 6-3
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.

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Section 6-3
Ionic Radius (cont.)

• Both positive and negative ions increase in size
  moving down a group.

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Section 6-3
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.

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Section 6-3
Ionization Energy (cont.)
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Section 6-3
Ionization Energy (cont.)
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Section 6-3
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.

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Section 6-3
Ionization Energy (cont.)
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Section 6-3
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.

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Section 6-3
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.

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Section 6-3
Electronegativity (cont.)
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Section 6-3
Section 6.3 Assessment
The lowest ionization energy is the ____.
A. first B. second C. third D. fourth

1. A
2. B
3. C
4. D

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Section 6-3
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 C. moving down a group
D. the ion loses electrons

1. A
2. B
3. C
4. D

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End of Section 6-3
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Resources Menu
Chemistry Online Study Guide Chapter
Assessment Standardized Test Practice Image
Bank Concepts in Motion
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Study Guide 1
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.

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Study Guide 1
Section 6.1 Development of the Modern Periodic
Table (contd.)
Key Concepts

• Elements are classified as either metals,
  nonmetals, or metalloids.

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Study Guide 2
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 elements number of valence electrons.
• The energy level of an atoms valence electrons
  equals its period number.

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Study Guide 3
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.

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Chapter Assessment 1
The actinide series is part of the A. s-block
elements. B. inner transition metals. C. non-meta
ls. D. alkali metals.

1. A
2. B
3. C
4. D

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Chapter Assessment 2
In their elemental state, which group has a
complete octet of valence electrons? A. alkali
metals B. alkaline earth metals C. halogens
D. noble gases

1. A
2. B
3. C
4. D

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Chapter Assessment 3
Which block contains the transition metals?
A. s-block B. p-block C. d-block D. f-block

1. A
2. B
3. C
4. D

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Chapter Assessment 4
An element with a full octet has how many valence
electrons? A. two B. six C. eight D. ten

1. A
2. B
3. C
4. D

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Chapter Assessment 5
How many groups of elements are there? A. 8
B. 16 C. 18 D. 4

1. A
2. B
3. C
4. D

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STP 1
Which group of elements are the least reactive?
A. alkali metals B. inner transition metals
C. halogens D. noble gases

1. A
2. B
3. C
4. D

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STP 2
On the modern periodic table, alkaline earth
metals are found only in ____. A. group 1
B. s-block C. p-block D. groups 1318

1. A
2. B
3. C
4. D

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STP 3
Unreactive gases are mostly found where on the
periodic table? A. halogens B. group 1 and 2
C. group 18 D. f-block

1. A
2. B
3. C
4. D

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STP 4
Bromine is a member of the A. noble gases.
B. inner transition metals. C. earth metals.
D. halogens.

1. A
2. B
3. C
4. D

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STP 5
How many groups does the d-block span? A. two
B. six C. ten D. fourteen

1. A
2. B
3. C
4. D

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CIM
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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