aufbau principle - weebly
TRANSCRIPT
Aufbau Principle Electrons occupy the orbitals of lowest energy first.
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It
Na : 152252213635'
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= e-
are selfish
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Chemistry 11 – Atomic Theory Study Guide
The Periodic Table and Its Trends
The modern periodic table, which was designed by Mendeleev, contains all the elements that have been
discovered. It organizes elements according to _____________________.
Classifying elements according to their metallic character:
• There is a ___________________ that separates the metals from non-metals
• On the left are the __________ and on the right are the______________
• __________________________ are elements that are found next to the zig-zag line and have
properties of both metal and non-metal. (e.g., B, Si, Ge, As, Se, Sb, Te)
Arrangement of elements on the periodic table:
Definition:
• Period:____________________________________________________________________
• Group (Family) :____________________________________________________________
Some special groups of elements:
Alkali Metals (Group 1)
• Have ______ e- in the outermost shell and have ______ ions
• Very _____________ (especially with water)
• Reactivity increases as you go ___________________ of the family
o This is generally true for all families
More notes about other families on “Family Ties” worksheet.
Other trends: Atomic Radii, Metallic Character, Ionization Energy, Electronegativity
Definition:
• Atomic radius:________________________________________________________________
As you go from ____________ to _____________, the size of atom _____________ so atomic radii
_________________. As you go from ____________ to _____________, atomic radii _____________
because of increase in ____________________ between protons and electrons. (More protons can
____________ electrons tightly.)
atomic number
Zig-zag line
metals non - metals
Semi - metal ( metalloid )
←
A group of elements found in a row of a p - table .
= a = in a column I = .
↳ Members have the same # Ve ?
= Behave in similar way .
I +1
reactive
down
eg ) K is more reactive
than Na
• →
⑦ The distance between the nucleus Is valence shell
top bottom ITA left right IAble of the new shell
net attraction
hold eg ) B bigger Vs F smaller
s÷. . •a.:!g¥⇐:
Chemistry 11 – Atomic Theory Study Guide
• Metallic character:_____________________________________________________________
OR :______________________________________________________________
As you go from ____________ to _____________, the metallic character _________________. As you
go from ____________ to _____________, the metallic character________________.
Why?
• Ionization Energy:______________________________________________________________
OR :______________________________________________________________
As you go from ____________ to _____________, the ionization energy _________________. As you
go from ____________ to _____________, the IE ________________.
Why?
• Electronegativity:______________________________________________________________
OR :______________________________________________________________
As you go from ____________ to _____________, the electronegativity _________________. As you
go from ____________ to _____________, the EN ________________.
Why?
Summary:
② The set of Chemical properties associated W/ metals
How easily an atom would give up valence e- ( Easy =
Furth )top bottom IT
left right Hv
The bigger the size of an atom , the easier
it is to lose valence e-
= more metal ie
③ Energy required to remove Ie - from valence shell
How easily an atom would give up valence e : CEasy = EE )top bottom He
left right A
The bigger the size of an atom,
the greater the
distance between pt and valence e-
= easier to remove e-
= Low IE
④ Tendency of an atom to attract e- from its neighbour .
How badly does an atom want to steal e- from others
. (MENdhrgn )top bottom I
left right A
The bigger the size of an atom,
the greater the distance
from pt to e-
of other atoms = unlikely to attract e-
= EN TS low .
IE is highest for noble gasEN B = = halogen
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Home Fun
• Complete p 164035 - 39 ,48 - 51
,53,55 ( Hebden )
• Read Hebden p 172 Ionic Bond
P 176 covalent Bond
171179 London Force
• complete HI # 12 to prepare for quiz ¥3
↳ Answer key is posted online