Download Still placed in the 6th and 7th periods, respectively (even though 4f

Periodic Trend
• Horizontal rows are called _________
• Vertical columns are called ________
• There are __ periods, __ groups
Element Arrangement
• Elements in each ______have different electron
energy shell level
• Elements in each column of table have same
number of __________ in their _________ level
– _____________
• Group 1 or 1A– one valence electron
• Group 2 or 2A– two valence electron
• Group 13 or 3A– has three valence electron and
so on.
• Groups 3/ 3B to 12 / 12B have different number
of valence electron
Periodic Table
• Periodic Table
A. Metallic Character
• Metals
• Nonmetals
• Metalloids
– Metals- 80%, ___ of stair-step line, excellent
– Nonmetals- ____ of stair-step line, generally
poor
– Metalloids- ______ stair-step line;
» Stair-step line aka. “zig-zag”
• We can also look at the periodic table in
terms of ________________, the
arrangement of electrons in an atom
Take a look at Pg 119
• What is the electron configuration of C?
• What is the electron configuration of Pb?
– s-block elements: chemically reactive metals,
• alkali metals- group ___
• alkaline earth metals- group __
– d-Block elements:
• transition metals- group ____,
– p-Block elements: part of main block
• halogens- group ___,
• noble gases- group ___,
– f-Block elements: To save space the lanthanides
and actinides are set off below the main portion of
the Table.
• inner transition metals-aka ____-____ ________
• Lanthanide
Still placed in the 6th and 7th periods, respectively (even
• Actinide
though 4f and 5f)
Periodic Trend
• As you go from ____ to ____, the number
of _____________.
• As you go from ____ to _____, the
____________ in the same energy level
___________.
• As you go from _____ to _______, more
_______ are added.
• As you go from _____ to _______, ______
are farther away.
Effective Nuclear Charge
• Nucleus is _________.
• Positive charge of the nucleus
____________
• Electrons closer are ________ effectively
drawn to nucleus
• Electrons farther away are _______ drawn to
nucleus
• Attractive force from the nucleus is canceled
out by inner electrons. Outermost shell feel
less attraction – _________________
Atomic Radius
• Hard to determine- electron clouds
• ___________- the length that is half the
distance between the nuclei of two bonded
atoms. Figure 19.
• _________, _________  more pulling 
closer to the nucleus  smaller the bond
radius  _____________________
• _________, _____________  electrons are
farther away  ____________  bigger the
bond radius  __________________
Atomic size increases, (shielding
constant across a period)
Ionic size increases
Ionization Energy
• The energy needed to __________ an
electron from the shell
• ___________, more protons  stronger
pulling  tighter the atom  more energy
needed to remove an electron 
_______________
• ____________, more electron shells 
electron shielding  farther electrons feel
less attraction  less energy to remove an
electron  _____________________
Ionization energy, Electronegativity,
Electron affinity INCREASE
Electronegativity
• A measure ability to __________ electrons
• __________, more protons  more pulling
from nucleus  easier to attract another
electron  ________________________
• ________, more electron shells  farther
away  less effective pulling 
______________________________
Atomic Size
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Radius
• Atomic Radius = half the distance between
two nuclei of a diatomic molecule