Transcript Chapter 6- The Periodic Table

Chapter 6- The Periodic Table
• Vocabulary-Atomic Mass, Atomic number,
macronutrient, trace element, trace
amount, periodic table, periodic properties,
electronegativity, ionization energy, orbital,
transition metal, noble gas, alkali metal,
alkali earth metal, atomic radius, valence,
electron shell, electron configuration,
bonding, Lewis dot diagrams
The state says you need to
• 3.01 Analyze periodic trends in chemical
properties and use the periodic table to
predict properties of elements.
• Groups (families).
• Periods.
• Representative elements (main group) and
transition elements.
More
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Electron configuration and energy levels.
Ionization energy.
Atomic and ionic radii.
Electronegativity.
New way to examine
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Chm.1.3 Understand the physical and
chemical properties of atoms
based on their position in the
Periodic Table.
• Chm.1.3.1 Classify the components
of a periodic table (period, group,
metal, metalloid, nonmetal,
transition).
• Chm.1.3.2 Infer the physical
properties (atomic radius, metallic
and nonmetallic characteristics) of an
element based on its position on the
Periodic Table.
Chm.1.3.3 Infer the atomic
size, reactivity,
electronegativity, and
ionization energy of an
element from its position in
the Periodic Table.
What is the universe made of?
• The materials the universe first developed
were few, mainly hydrogen and helium
• Where did the rest come from?
• (explain the process of fusion that
happens in stars)
• Pressure causes nuclei to fuse together
The periodic table
• Gregor Mendeleev notice patterns in the
mass and reactions of elements
• (Scientists notice patterns and anomolies)
• Periodic means repeating
Size of atoms
• The Strong nuclear force keeps the
protons and neutrons together.
• The more protons and more neutrons you
have, the stronger the attraction between
the nucleus and the electrons.
• This is what makes the atom radius
smaller as you cross the periodic table.
Electronegativity
• Electronegativity is the measure of how
well an atom can attract electrons from
another atom to which it is bonded.
• They are already bonded...what does it do
to the electrons. The more electronegative
it is, the more likely it is to pull off electrons
of its partner.
Ionization energy
• ionization energy - the energy required to
remove an electron from its atom.
• Almost, but not quite like electronegativity
• Electronegativity is how well it takes
someone else’s electron
• Ionization energy is how well it holds on to
its own electrons
6.2 Properties of groups
• Columns on the periodic table are called
groups or families. Each member of the
group would have the same number of
electrons in the outside orbital. Thus, they
would be similar chemically
Group I- Alkali Metals
• (Hydrogen not actually considered a part
of it)
• Soft Metals. lose the one electron on its
outer orbital easily. React explosively with
water.
• In your body used in nerve signaling.
(electrolytes)
Group II-Alkaline Earth metals
• 2 outer electrons, they lose them easily
(ions are B 2+ , Ca 2+ , etc)
• CaO, CaCl2, etc
Transition Metals
• The low part of the periodic table
• Outer electrons are in the d orbital
• Can bond in different ways, both FeO and
Fe2O3.
• Traditional metals, good conductors of
electricity
Carbon, Nitrogen, Oxygen
• Very flexible in bonding, especially carbon
• 4, 5, and 6 electrons in their outer orbitals
Halogens
• Group 17
• 7 of 8 possible electrons in the outer
orbital
• Tend to pull an electron off another atom to
form ionic bonds.
• Form diatomic molecules (F2, Cl2, etc.)
• Form acids with H (HCl, HBr, HF)
• Form salts with metals (NaCl)
Noble Gases
• Don’t normally form bonds!
• Outer orbitals are full!~
Compounds
• Compounds give each participating atom a
full outer orbital. This makes it more
stable.
• CH4, H2O
Section 6.3 Valence
• Reactions only occur in the highest unfilled
electron level.
• Atoms react to have a full or empty outer
level
• The total possible valence electrons is 8
• Each group or family has the same
number of electrons in every member’s
outer shell.
Lewis Dots
• Lewis Dots represent the number of
electrons in the outer orbits. These
electrons are referred to as Valence
electrons
• Notice that each family looks the same in
Lewis Dots
• You need to be able to make Lewis dots
for each group or family
Notes
• Make sure you read 189 to 191
Faculty Periodic Table
• Arrange at least 30 of the staff at Paisley
into a periodic table.
• Remember that “Periodic” means having
patterns.
• Explain your reasoning for your
arrangement (75%)
• Creativity with symbols and appearance is
appreciated (25%)
Included
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Reason for groups (10 pt)
Reason for families (10)
At least two other “periodic” traits (10)
Creativity and appropriateness (10)
• To help you with patterns and the periodic
table:
• 6A
• 6B
Feb 9
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How are the projects coming?
6C
Collect work
Lewis Dots