Name:
Aim 35: Electron Configuration
Date:
Scientists use the periodic table to draw diagrams of elements.
Each element has a unique electron configuration
a) What is electron configuration?
b) How many electrons can each level hold?
c) How do you know how many energy levels are in each element?
d) How do you know how many electrons are in each energy level?
e) What term is used for the electrons in the outermost shell or energy level? ________________________________

Elements in the same ________________ have the ______________ number of valence electrons

Atoms are most __________ when there are

The number of valence electrons affects the ability of an element to

Atoms will
,
other atom to reach a

Group
valence electrons
, or
to other elements
electrons from
number of valence electrons
(the noble gases) are
because they have
valence electrons (stable)

Atoms that are close to achieving a
valence (by losing or gaining an electron) are
___________________________. This is why as you move to the right on the periodic table, the
reactivity decreases (the elements are closer to being stable)
12. How many electrons can each level hold? 1st = _____ 2nd = _____ 3rd = _____
Electron
13. Part
WhatC:
term
is usedConfiguration
for the electrons in the outermost shell or energy level? ____________________
13. What
termuse
is used
theofelectrons
intotheshow
outermost
shell or energy level?
____________________
two for
types
diagrams
Bohr
model and the Lewis model
12.Scientists
How many
electrons
can
each
level tohold?
= electron
_____ configuration:
2nd
= _____ 3rd
= atoms.
_____
14. f)
Scientists
use two
types
of diagrams
show1st
theelectron
configuration
for
Follow your teacher’s directions to14.
complete
the use
diagrams.
Scientists
two types of diagrams to show the electron configuration for atoms. Follow your teacher’s directions 13. What term is used for the electrons in the outermost shell or energy level? ____________________
to complete the diagrams.
Bohr Diagram
Lewis Structure
Sulfur
14. Scientists use two types of diagrams to showShows
theBohr
electron
configuration for atoms.Shows
Follow
yourStructure
teacher’s
directions allDiagram
electrons
valence
electrons
Lewis
Sulfurthe
Atomic
# =diagrams.
16
to complete
Shows all electrons
Shows valence electrons
AtomicMass
# = 16
Atomic
= 32
Bohr Diagram
Lewis Structure
Sulfur
Shows
all
electrons
Shows
valence electrons
Atomic=Mass
Protons
____ = 32
Atomic # = 16
Protons = ____
Neutrons
Atomic Mass = 32
S
S
S
Neutrons
= ____
Electron
= ____
Protons
= ____
Electron = ____
Neutrons = ____
15. Calculate
the missing
Electron
= ____information and then draw the Bohr Diagram and Lewis Structure for each element.
15.g)Calculate
information
then
draw the
Bohr
Diagram
and
Lewis
for each element.
Practice: the
Fillmissing
in the information
forand
each
element.
Then,
complete
each
Bohr
andStructure
Lewis diagram
15. Calculate the missing
information
and then draw the Bohr Atomic
Diagram
Atomic
#=3
# =and
10 Lewis Structure for each element.
Atomic # = 12
Li
Li
Li
Mass
# = 7# = 3
Atomic
Mass
# = 20
Atomic
# = 10
Mass
# = 24
Atomic
# = 12
# Mass
ofAtomic
P =#____
=#7= 3
#Atomic
of
P =#____
Mass
#==20
10
# #ofMass
ofNP==#____
____
=
7
#Mass
of
N P=
# of
____
#=
=____
20
# of
P =##____
Mass
24
Atomic
==12
# of
N# =
# of
P
= ____
Mass
= ____
24
##of
EPN
==____
#ofof
=____
____
of
E==N____
____
# Pof
= ____
## of
# #of#ofE
=P =
____
ofN
= ____
____
##ofofEN==____
____
# of E = ____
Ne
Ne
Ne
____
##ofofNE==____
# of E = ____
Mg
Mg
Mg
of=E____
= ____
# of# N
# of E = ____
Atomic # = 17
Atomic # = 2
Atomic # = 14
Mass
# = 35
Atomic
# = 17
= 17
# Mass
ofAtomic
P =#____
=#35
Mass
# = 4# = 2
Atomic
#==42
#Atomic
of
P =#____
Mass
Mass
# = 28
Atomic
# = 14
Atomic
==14
# of
P =##____
Mass
28
=
35
# #ofMass
ofNP==#____
____
#=
=____
4____
#Mass
of
N P=
# of
Mass
28
# of
N# =
# of
P ____
= ____
ofN
= ____
____
# #of#ofE
=P =
____
# of N = ____
# of E = ____
# of E = ____
##of
EPN
==____
#ofof
=____
____
# of N = ____
# of E = ____
# of E = ____
## of
of
E==N____
____
# Pof
= ____
# of N = ____
# of E = ____
# of E = ____
Cl
He
Cl
He
He in question #15.
16. AnswerCl
the questions below based on the elements
Si
Si
Si
16.Which
Answer
the questions
below
based onshell?
the elements
in question #15.
(1)
elements
had a filled
outermost
_____ _____
16. Answer
questions
based onabove:
the elements
in question #15.
Based
on thethe
elements
in below
the diagrams
(1)Which
Whichelement
elements
had abefilled
shell?
_____ _____
(2)
would
mostoutermost
likely to lose
electrons
a chemical bond? _____
(1) Which
elements
had a filled
outermost
shell?
_____ in
_____
(2)Which
Whichelement
elementwould
wouldbebemost
mostlikely
likelytotogain
lose electronsinina achemical
chemical bond?_____
_____
(3)
(2) Which
element would
be most
likely to loseelectrons
electrons in a chemicalbond?
bond? _____
(3)Which
Whichelements
element are
would
be most
to gain
electrons
in a chemical
bond? ______________________________
(4)
not likely
to likely
bond
other
elements?
_____ _____
(3) Which
element would
be most
likelywith
to gain
electrons
in a chemical
bond? Why?
_____
(4)(4)
Which
elements are not likely to bond with other elements? _____ _____ Why? _________________________
Which elements are not likely to bond with other elements? _____ _____ Why? _________________________
T. Trimpe 2007
T.
2007
T. Trimpe
Trimpe 2007
http://sciencespot.net/
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