The Periodic Table & Periodic Law and The Elements- Chapter 6 & 7, See also pages 70, 72-73
What is the PERIODIC TABLE?
2 Influential Scientists
Arrangement
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Mendeleev (mid 1800’s) |
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Mosely |
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Periodic Law: when elements are
arranged by increasing ________________________, elements with similar
____________________fall into the same column.
v
What is a period?
Antiquity
v
What is a group? 2 ways to
identify it!
Modern
g +1 1 H 1.0079
v
Each block is
represented by a 1 or 2 ___________________ symbol. Period _________ represents
the newest __________________ elements and has a 3 letter symbols like "Une"
while it is being checked out.
3 Classes of Elements
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Metals |
Nonmetals |
Metalloids |
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Location |
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Color |
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Physical state |
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Conducting ability |
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Reflectiveness |
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Strength |
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Formability |
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2 Types of Elements on the Periodic Table
Group A: ___________________________ : Groups 1A, 2A, and 3A-8A
v
Represents the
entire range of ________________ and ___________________ properties
v
The group # next
to the “A” equals the __________________________
Group B : ___________________________
v
Have more than 1
__________________ .
v
Are all
_______________.
v
Typically less
__________________ than 1A and 2A elements.
v
The hardest,
___________________ , and highest melting points of
the table.
v
Great conductors
of heat and ______________________.
Inner transition: lower block
Period 6:
_________________________(rare earth) : Ce – Lu
Period 7:
_____________________ : Th – Lr; all are
__________________________ and unstable; the first 4 are _____________________
found, remaining are ____________________.
Properties of Chemical Families
Alkali metals:
Group 1A
v
React violently
with water to make __________________ gas and a ______________.
v
Reacts
vigorously with __________________ to form _______________ compounds.
v
Stored under
________________ or oil.
v
Not found
_______________ in nature.
v
Low
_________________ and ____________________________.
v
Usually
__________ and _________________ in appearance.
v
Found as
______________ ions in ionic compounds.
Alkaline Earth metals: Group 2A
v
Less reactive
than ________________ metals but still very ____________________.
v
Not found
____________ in nature.
v
Reacts with
_________________ to form a base.
v
Extracted from
mineral __________________.
v
Harder,
_______________, stronger and higher ____________________ than group 1A.
v
Found as
______________ ions in ionic compounds.
Groups 3A to 6A
v
Families are
names by the first element of each group.
v
Ex: Group 6A is
called the __________________ family.
Hydrogen
v
Nonmetal
v
_____________ charge with other nonmetals; ___________ charge with metals.
v
Reacts
___________________; explosive
v
Reacts with
other ____________________, especially the ___________________.
v
Diatomic:
consists of ________ identical atoms
_____________ bonded to one another; others include
_____________________________
Memorizing Tool:
Halogens: Group 7A
v
Most reactive of the __________________.
v
Do not exist ______________ in nature.
v
Most form the
diatomic molecules when by themselves.
v
Found as
____________ ions in ionic compounds.
Noble Gases: Group 8A
v
Non
_________________: rarely form compounds due to their ___________________.
v
Also called
_________________________.
v
Most are used in
__________________.
v
Contain
__________ electrons in their outer energy level
Periodic Trends
Atomic Radii (size)
v
Defined as:
v
Influenced by 2
factors
- Energy level:
- Nuclear Charge:
Period Trend: generally
____________________________
The greater number of protons and __________________
within the same _____________________ create a stronger pull towards the
_____________________
Why?
Group Trend generally
___________________________
_____________________are being added
to ________________ energy levels. Shielding
:electrons between the _________________ and ___________
electrons shield the forces of the nucleus.
Why?
Remember Ions are charges particles. Atom or group of atoms that ___________
electrons (anions) or
lose electrons ( _________________)
Ionization Energy (I.E.)
v
Defined as:
A + energy à ________________
Period Trend: generally ____________________________
The _________________ attraction of the _____________
for the electron, the _________________ it is to remove the electron and the
more energy is used up.
Why?
Group Trend generally
___________________________
**** Exceptions****
The outermost _____________________ are the farthest
away from the nucleus so they are _________________ to remove and less
energy is used up. Think about the
_______________.
Why?
***** Filled and half filled
___________________ have lower energy so achieving them is _______________________
and less I.E. is used up. *****
Metallic Properties
1.
2.
2.
4.
5.
6.
Period trend: generally _________________________
Group trend: generally
________________________
Electron Affinity
v
Defined as:
A
+ e- à
________________________
v
Easiest to add
electrons to group 7A (get to a full energy level quickly)
v
Usually negative
values or zero
Period trend: generally _________________________; becomes
more negative
Atoms who really want an electron will __________ for it
with large amounts of energy.The (-) sign just
means the energy is _______________________.
Why?
Group trend: generally
________________________; not a consistent pattern; becomes more positive
**** Exceptions****
Filled and ___________
filled orbitals( groups 14 & 15)
v
Adding an
electron to C gives a half filled orbital whereas you are forcing one on N who
is already half filled.
Reactivity
v
Defined as:
Metals: the most reactive ones have the
_______________________ionization energy
Period trend =
_________________ Group
trend = __________________
Nonmetals: the most reactive ones have the
highest _________________________(most negative)
Period trend = _________________ Group trend =
__________________
Ionic Size
v
Positive ions
are ___________________ in size than neutral atoms
Na
Na+1
Loss of an outershell
______________ increases the ______________________ for the nucleus.
Why?
v
Negative ions
are ___________________in size than neutral atoms
Cl Cl-1
The increased _____________ of electrons decreases the
attraction of the __________________.
Why?
Period trend:
____________________ for a cation and __________________ for an anion
Group trend: generally ______________________ for both
Electronegativity
v
Defined as the
tendency of an atom to gain an ___________________ when combining with another
element
v
________________
has the highest electronegativity and
__________________ has the lowest
Period trend: generally
_______________________ due to the increase in __________________ charge.
Group trend
: generally ____________________ due to shielding.