Key Learning: The number of valence electrons in an
atom dictates its location on the periodic table as well
as its chemical and physical properties.
UEQ: What is the relationship between an
elements location on the periodic table and
its chemical and physical properties?
 Concept: Introduction to the Periodic Table
 Concept: Periodic Table and Electron Configuration
UEQ: What is the relationship between an elements location on
the periodic table and its chemical and physical properties?
Concept: Introduction to Periodic Table
 Vocabulary:
 Non-metal
 Group/Family
 Halogens
 Period
 Noble Gas
 Metal
 Alkali Metals
 Metalloid
 Alkaline Earth Metals
 Transition Metal
 Lanthanide
 Actinide
Concept: Introduction to Periodic Table
LEQ: What is the general organization of the periodic
table and how was it developed?
 Mendeleev “Father of Periodic Table”
organized elements based on increasing
atomic mass. Found similarities in chemical
properties and published his first periodic
table in 1869.
Concept: Introduction to Periodic Table
LEQ: What is the general organization of the periodic
table and how was it developed?
 Moseley discovered while working with
elements that they fit better into pattern
when arranged by nuclear charge (number
of protons-also known as atomic number).
Concept: Introduction to Periodic Table
LEQ: What is the general organization of the periodic
table and how was it developed?
 Periodic Law states that physical and
chemical properties of the elements are
periodic functions of their atomic numbers.
 This means that when elements are
arranged in order of increasing atomic
number, elements with similar properties
appear at regular intervals.
Concept: Introduction to Periodic Table
LEQ: How are the elements classified and arranged on
the periodic table?
 Periods – rows across, horizontal
 Indicates number of energy levels (Principle
Quantum Number)
 Groups/Families – down, columns
 18
 Indicate number of e- in outer most energy level
(1-2, 13-18 main group elements)
Concept: Introduction to Periodic Table
LEQ: How are the elements classified and arranged on
the periodic table?
 Metals
 Groups 1-12 (except H) and under stair-step groups 13





15
Form ionic and metallic bonds
Good Conductors of heat and electricity because the
outer electrons are not held tightly to the nucleus and
move freely
Solid at room temperature (except for Hg)
Reflects light (luster)
Malleable (hammered into sheets)
Ductile (stretched/drawn into wires)
Concept: Introduction to Periodic Table
LEQ: How are the elements classified and arranged on
the periodic table?
 Group 1 (ns1)
 Alkali metals
 Soft, silvery (pure state), highly reactive
(reacts with O2 and H2O)
 Do not occur in nature in elemental form
 Stored in kerosene
 Lower melting points
Concept: Introduction to Periodic Table
LEQ: How are the elements classified and arranged on
the periodic table?
 Group 2 (ns2)
 Alkaline Earth Metals
 Reactive; but, less than alkali
 Not found as free elements in nature
 Bright fireworks, aircraft
 Harder, denser, and stronger than alkali
metals
 Higher melting points than alkali
Concept: Introduction to Periodic Table
LEQ: How are the elements classified and arranged on
the periodic table?
 Transition Elements (d block, n-1)
 Groups 3-12 (elements in transition)
 Vary in reactivity and can be found as free
elements
 Metal characteristics
 Form colored compounds
 Often occur in nature as uncombined
elements
 Hg – mercury – liquid metal
Concept: Introduction to Periodic Table
LEQ: How are the elements classified and arranged on
the periodic table?
 Inner Transitional Metals (f-block, n-2)
 ALL are radioactive and unstable
 Includes lanthanides (atomic number 58-
71)

Shiny metals, similar in reactivity to alkaline
earth metals
 and actinides (atomic number 90-103)

First 4 are found on earth, the remaining are
synthetic
Concept: Introduction to Periodic Table
LEQ: How are the elements classified and arranged on
the periodic table?
 Nonmetals








P block
Gases or brittle solids at room temperature
Form ionic and covalent bonds
Not malleable
Not ductile
Most do not conduct heat or electricity
Generally not shiny
All, except H, are found on right of periodic table
Concept: Introduction to Periodic Table
LEQ: How are the elements classified and arranged on
the periodic table?
 Group 17 “halogens”
 Most reactive non-metal
 Interact with alkali metals to form salts
 7 electrons in outer energy level
 Bromine – only liquid nonmetal
 Group 18 “noble gases”
 Full outer energy level
 Relatively un-reactive
Concept: Introduction to Periodic Table
LEQ: How are the elements classified and arranged on
the periodic table?
Metalloids
 P-block
 Elements along stair-step line (except for Al)
 Can form ionic and covalent bonds with
other elements
 Can have metallic and nonmetallic
properties
 Semiconductors
Concept: Introduction to Periodic Table
LEQ: How are the elements classified and arranged on
the periodic table?
Practice – looking for
group number, period
number and name of
element
[Xe] 6s1
[Kr] 5s2
[Ne] 3s2 3p2
[Ar] 3d104s24p5
[He] 2s22p3
Concept: Introduction to Periodic Table
LEQ: How are the elements classified and arranged on
the periodic table?
BOOK WORK
pg. 137 #’s 1 b and c, # 2
Pg. 149 # 2
Pg. 166 #’s 3, 4, 8, 9, 11-16a, 17-19 a-d
UEQ: What is the relationship between an
elements location on the periodic table and its
chemical and physical properties?
UEQ: What is the relationship between an elements
location on the periodic table and its chemical and
physical properties?
Concept: Periodic Table and Electron Configuration
 Vocabulary
 Ion
 Cation
 Anion
 Valence electron
 Lewis-Dot structure
Concept: Periodic Table and Electron Configuration
LEQ: How do we relate the location of an element on
the periodic table to its electron configuration?
 Group 1 = ns1
 Group 2 = ns2
 Groups 13-18 = np1-6
 Groups 3-12 = n-1 (d)1-10
 Lanthanides (period 6) and Actinide
(period7)
 n-2 (f)1-14
Concept: Periodic Table and Electron Configuration
LEQ: How does an elements location on the periodic
table relate to its valence electrons?
 Valence Electrons
 The electrons in the outer most energy
level that are available to chemically
react
 Correlates to the group number for main
group elements
 Groups 13-18 – subtract 10 from group
number to get the number of valence
electrons
Concept: Periodic Table and Electron Configuration
LEQ: How does an elements location on the periodic
table relate to its valence electrons?
 Energy levels correlate to periods. Each
energy level needs to have 8 electrons to
make that level complete and stable (with
exception to period 1)
 Period 1 = up to 2 electrons
 Period 2 = up to 8 electrons
 Period 3 = up to 18 electrons
 Period 4 = up to 32 electrons
Concept: Periodic Table and Electron Configuration
LEQ: How does an elements location on the periodic
table relate to its valence electrons?
 Electron Cloud structure
 Lewis-Dot structure
Concept: Periodic Table and Electron Configuration
LEQ: How do we use an elements location on the
periodic table to determine its ionic charge?
 Atomic Radius (Angstrom)
 ½ the distance from the nuclei to another
 From the nucleus to edge of e- cloud
 Going down a group, Atomic radius increases
because of the increasing number of energy
levels
 Going across a period, atomic radius decreases
because of the increase in positive charge in the
nucleus
Concept: Periodic Table and Electron Configuration
LEQ: How do we use an elements location on the
periodic table to determine its ionic charge?
 Ionization is a process that results in the
formation of an ion
 An ion is an atom or group of atoms that
have a “+” or “-” charge
 Change is created by gain or loss of e Losing an e creates a “+” charge (cation)
Concept: Periodic Table and Electron Configuration
LEQ: How do we use an elements location on the
periodic table to determine its ionic charge?
 Losing the e- requires energy. Energy
required to remove one e- from a neutral
atom is called
IONIZATION ENERGY
(also known as 1st ionization
energy)
Concept: Periodic Table and Electron Configuration
LEQ: How do we use an elements location on the
periodic table to determine its ionic charge?
 Ionization energy decreases as you go
down a group because valence
electrons are farther from the nucleus
 And increases as you go across a period
because of the greater positive charge
leads to greater attraction to electron
Concept: Periodic Table and Electron Configuration
LEQ: How do we use an elements location on the
periodic table to determine its ionic charge?
 Electron Affinity
 Gaining an electron results in an ion with
a “-” charge (anion)
 When an atom gains an e- it causes an
energy change. The energy change when a
neutral atom gains an e- is the
ELECTRON AFFINITY
Concept: Periodic Table and Electron Configuration
LEQ: How do we use an elements location on the
periodic table to determine its ionic charge?
 Electron affinity decreases as you move
down a group
 Increases as you move across a period
Concept: Periodic Table and Electron Configuration
LEQ: How do we use an elements location on the
periodic table to determine its ionic charge?
 Electronegativity (0-4)
 Ability of an atom to attract (or
remove) an e- from another atom
 Fluorine is most electronegative (4)
 Metals have Electronegativity of less
than 2
Concept: Periodic Table and Electron Configuration
LEQ: How do we use an elements location on the
periodic table to determine its ionic charge?
 Electronegativity decreases as you go
down a group because the electrons are
farther from the nucleus
 Electronegativity increases as you go to
the right because atoms are more
inclined to gain electrons in order to
gain a full shell
Concept: Periodic Table and Electron Configuration
Book Work
Pg. 164 #’s 1 and 3
Pg. 167 #’s 22-24c, 25 a, 26 a, 27 a,
28-30
Pg. 168 #’s 40 and 42