STAAR Chemistry Review
Topic: Periodic Table
TEKS 5 – The student understands
the historical development of the
Periodic Table and can apply its
predictive power. (5 A-C)
Student Expectation (SE) – 5A
• Explain the use of chemical and
physical properties in the historical
development of the Periodic Table.
INDEX CARD TIME!
• Title: History of Periodic Table
• Front:
1. Mendeleev
2. Moseley
• Back: Write a statement that
explains how each man organized
the Periodic Table
Mini - Review
• In 1869, Mendeleev published a
table of the elements organized by
increasing atomic mass.
• Through his work with X-rays, Moseley
determined the actual nuclear charge (atomic
number) of the elements. He rearranged the
elements in order of increasing atomic
number.
• Periodic Law states: When elements are
arranged in order of increasing atomic
number, there is a periodic pattern in their
physical and chemical properties.
Student Expectation (SE) – 5B
• Use the Periodic Table to identify and
explain the properties of chemical
families, including alkali metals,
alkaline earth metals, halogens,
noble gases, and transition metals.
INDEX CARD TIME!
• Title: Periodic Table
• Front: Definitions
»1. Periodic Table
»2. Valence electrons
• Back: Define each term
Mini - Review
• Periodic Table – Chart of elements
ordered by atomic number and grouped by
valence electrons
• Atomic number is the key to the organization of the
periodic table. Elements are listed by atomic number!
• Valence Electrons – Electrons in an atom’s
outermost shell; can be gained, lost or shared
• A full outermost shell is 8 electrons (except for He
which has 2) – known as octet rule for elements with an
atomic number of less than 20
INDEX CARD TIME!
• Title: Periodic Table
• Front: Definitions
»1. Row or Period
»2. Column or Group (family)
• Back: Define each term
Mini - Review
• Row or Period - The horizontal rows
of the periodic table; elements
are in order of increasing atomic number
atomic number = # of protons = # electrons (in a neutral atom)
• Column or Group (Family) – The vertical rows of
the periodic table; elements in a group have the
same number of valence electrons and have similar
physical and chemical properties
INDEX CARD TIME!
• Title: Periodic Table
• Front: Definitions
»1. Oxidation number
»2. Anion
»3. Cation
• Back: Define each term
Mini - Review
• Oxidation number- number assigned
to an atom or ion that represents the number
of electrons gained or lost
• Anion – gains electrons; oxidation number is
negative
• Ex. F gains one electron → F- → oxidation # is -1
• Cation – loses electrons; oxidation number is
positive
• Ex. Ca loses 2 electrons → Ca+2 → oxidation # is +2
INDEX CARD TIME!
• Title: Physical Properties of Elements
• Front: 1. Metals
2. Nonmetals
3. Metalloids
• Back: Draw and label the periodic
table showing where each
of these is located
Mini - Review
INDEX CARD TIME!
• Title : Properties of Chemical Families
• Front: Alkali Metals
• Back: Draw a diagram showing the location of
the Alkali Metals and list their
properties
Mini - Review
• The Alkali Metals – Group 1
– the first column of the periodic table on the left
– have only one electron in their outer shell
– very reactive metals; wants to
lose one electron
– do not occur freely in nature
– silvery-colored metals
– soft, and can be cut easily with
a knife
– Malleable
– good conductors of heat and
electricity
– have low densities
– can explode if they are exposed to water
INDEX CARD TIME!
• Title : Properties of Chemical Families
• Front: Alkaline Earth Metals
• Back: Draw a diagram showing the location of
the Alkaline Earth Metals and list their
properties
Mini - Review
• Alkaline Earth Metals – Group 2
– found in the second group of
the periodic table
– 2 electrons in their outer
energy shell
– very reactive - although not
as reactive as the alkali metals;
wants to lose 2 electrons
– not found freely in nature
– are shiny, silvery white metals
– each of the metals will give a
different colored flame
INDEX CARD TIME!
• Title : Properties of Chemical Families
• Front: Halogens
• Back: Draw a diagram showing the location of
the Halogens and list their properties
Mini - Review
• Halogens
–
–
–
–
have 7 electrons in their outer-most energy level
very reactive
found in nature as diatomic molecules
physical appearances of the halogens is very different
between elements
INDEX CARD TIME!
• Title : Properties of Chemical Families
• Front: Noble Gases
• Back: Draw a diagram showing the location of
the Noble Gases and list their properties
Mini - Review
• Noble Gases
– have full outer electron shell (8 valence electrons except
for He which has 2)
– inert; will not readily react with other elements
– found at room temperature as gasses, and they have very
low boiling points
INDEX CARD TIME!
• Title : Properties of Chemical Families
• Front: Transition Metals
• Back: Draw a diagram showing the location of
the Transition Metals and list their
properties
Mini - Review
• Transition Metals
–
–
–
–
38 elements in groups 3 through 12
Metals in table’s center
Has partially filled shell
have different numbers of
valance electrons in their outer
energy level (variable oxidation
numbers) ex. Cu1+ or Cu2+
– mallable
– conduct electricity and heat
– iron, cobalt, and nickel are the only
elements known to produce a magnetic field
Student Expectation (SE) – 5C
• Use the Periodic table to identify and explain
periodic trends, including atomic and ionic
radii, electronegativity, and ionization energy
INDEX CARD TIME!
• Title: Periodic Trends
• Front: Atomic Radius
• Back:
1.Draw a periodic table and label
with arrows the trend for atomic
radius.
2. In a short sentence describe
what is happening.
Mini - Review
• More electrons = fatter = larger radius (attraction
from nucleus felt less)
• Size of the Atom
– Measured as half the distance between the nuclei of two
atoms of the element
• Decreases Left to Right
– Within the energy level adding more electrons and protons
increases the attraction between the nucleus and the
electrons causing the electrons to be pulled in tighter
• Increases Top to Bottom
– Adding more levels further out from the nucleus makes
the atom bigger
Here is a graph of atomic radius
INDEX CARD TIME!
• Title: Periodic Trends
• Front: Ionic Radii
• Back:
1.Draw a periodic table and label
with arrows the trend for ionic
radii.
2. In a short sentence describe
what is happening.
Mini - Review
• Size of the ion (atoms that have lost
or gained an electron)
• Decreases Left to Right
– Positive Ions decrease & Negative Ions decrease
– There is a “jump” crossing from Positive to
Negative Ions
• Increases Top to Bottom
– Adding more levels further out from the nucleus
makes the Ions bigger
Ionic Radius
Decreases *
I
n
c
r
e
a
s
e
s
* Jumps
between + ions
and – ions
then gets
smaller again
INDEX CARD TIME!
• Title: Periodic Trends
• Front: Ionization Energy
• Back:
1.Draw a periodic table and label
with arrows the trend for
ionization energy
2. In a short sentence describe
what is happening.
Mini - Review
• Energy needed to take an electron away
• Increases Left to Right
– These atoms are smaller and have a greater pull from the nucleus and
will require more energy to take an electron away (they usually want
more electrons)
• Decreases Top to Bottom
– Electrons are further away from the nucleus and will require less
energy to take an electron away
• Low ionization energy means that the electron removed is
not held tightly
Ionization Energy
Increases
D
e
c
r
e
a
s
e
s
INDEX CARD TIME!
• Title: Periodic Trends
• Front: Electronegativity
• Back:
1.Draw a periodic table and label
with arrows the trend for
electronegativity
2. In a short sentence describe
what is happening.
Mini - Review
• How much it “loves” it electrons
• Ability of an atom to attract electrons
• Increases Left to Right
– These atoms are smaller and have a greater pull
from the nucleus and will have a higher attraction
for more electrons
• Decreases Top to Bottom
– Electrons are further away from the nucleus and
will have less attraction for more electrons
Electronegativity
Increases
D
e
c
r
e
a
s
e
s
Here is a graph of electronegativity