Download Notes: Unit 4: Periodic Table - Mr. Palermo`s Flipped Chemistry

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Regents Chemistry: Mr. Palermo
Notes: Unit 4: Periodic
Table
MIND BLOWN!!!!
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Key Ideas:
The placement or location of elements on the Periodic Table gives an indication of
physical and chemical properties of that element. The elements on the Periodic
Table are arranged in order of increasing atomic number. (3.1y)
Elements can be classified by their properties and located on the Periodic Table as
metals, nonmetals, metalloids (B, Si, Ge, As, Sb, Te), and noble gases. (3.1v)
Elements can be differentiated by their physical properties. Physical properties of
substances, such as density, conductivity, malleability, solubility, and hardness,
differ among elements. (3.1w)
Elements can be differentiated by chemical properties. Chemical properties describe
how an element behaves during a chemical reaction. (3.1x)
Some elements exist in two or more forms in the same phase. These forms differ in
their molecular or crystal structure, and hence in their properties. (5.2f)
For Groups 1, 2, and 13-18 on the Periodic Table, elements within the same group
have the same number of valence electrons (helium is an exception) and therefore
similar chemical properties. (3.1z)
The succession of elements within the same group demonstrates characteristic
trends: differences in atomic radius, ionic radius, electronegativity, first ionization
energy, metallic/nonmetallic properties. (3.1aa)
The succession of elements across the same period demonstrates characteristic
trends: differences in atomic radius, ionic radius, electronegativity, first ionization
energy, metallic/nonmetallic properties. (3.1bb)
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10/31/15&
UNIT 4: PERIODIC TABLE
LESSON 4.1 DEVELOPMENT
OF THE PERIODIC TABLE
W W W. M R PA L E R M O . C O M
MENDELEEV
•  Organized the elements based upon
ATOMIC MASS
PERIODIC LAW
•  The properties of elements are
periodic functions of their atomic
numbers.
MOSLEY
•  Developed the Modern Day Table
•  Organized elements by # of PROTONS
(Atomic Number)
THE RESULT…..
•  Can fill in gaps to predict
undiscovered elements and their
properties
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HOW IS THE TABLE ORGANIZED?
Period
Group
•  PERIODS (horizontal rows)
-  Equal to the # of energy levels (shells)
•  GROUPS (vertical columns)
-  elements have the SAME # of VALENCE
ELECTRONS resulting in similar chemical
properties
•  # of period tells us the # of e- SHELLS
(AKA principal energy level)
•  properties of elements change
drastically ACROSS A PERIOD (metals
! metalloids/semi-metals !
nonmetals)
•  # of VALENCE ELECTRONS increases
from left to right (1 ! 8)
•  Ex: K is in period 4
REACTIVITY OF ELEMENTS
•  Determined by # of valence
electrons
•  All atoms (except Hydrogen) want 8
VALENCE ELECTRONS to become
STABLE (full valence shell)
•  Called a STABLE OCTET
EXAMPLE:
•  The closer to a stable octet the MORE
REACTIVE the element is.
Which element is in Group 2
and has 4 energy levels?
****Period 1 elements need 2 electrons
to have a full valence shell NOT 8
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EXAMPLE:
•  Which two elements have similar
chemical properties and why? Na, K,
Li, Be
•  Na & K are in the same group and
have the same number of valence
electrons
1
METALS, NONMETALS,
METALLOIDS
H
3
4
5
6
7
2
Li
Be
B
C
N
O
F
Ne
3
4
5
6
7
8
9
10
Al
Si
PNonmetals
S Cl Ar
13
14
15
16
Na Mg
11
12
17
18
K
Ca Sc
Ti
V
Cr Mn Fe Co
Ni Cu Zn Ga Ge As Se Br
Kr
19
20
21
22
23
24
28
Y
39
Rb Sr
37
W W W. M R PA L E R M O . C O M
He
1
2
LESSON 4.2 CATEGORIES &
PROPERTIES OF ELEMENTS
38
25
31
32
Zr Nb Mo Tc Ru Rh Pd Ag Cd
In
Sn Sb Te
40
49
50
51
27
29
30
METALS
41
42
43
Cs Ba
He Ta
W
55
56
72
74
Fr
Ra
87
88
Ω
26
73
44
36
I
Xe
53
54
Re Os
Ir
Pt Au Hg
Tl
Pb
Bi Po At Rn
75
77
78
81
82
83
80
52
35
46
79
48
34
45
76
47
33
84
85
86
ELEMENT GROUPS
Rf Db Sg Bh Hs Mt
104
105
106
107
108
Metalloids
109
La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
57
• 
• 
• 
• 
58
59
60
Ac Th Pa
U
89
92
90
91
61
62
63
64
65
66
Np Pu Am Cm Bk Cf
93
94
95
96
97
98
67
68
69
70
71
Es Fm Md No Lr
99
100
101
102
103
GROUP 1: ALKALINE METALS
GROUP 2: ALKALINE EARTH METALS
1 valence electron
Lose 1 electron to form +1 ions
Extremely reactive with water
Most REACTIVE metal is Fr
•  2 valence electrons
•  Lose 2 electrons to form +2 ions
•  Fairly reactive in water
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GROUPS 3-12: TRANSITION METALS
•  Least reactive metals
•  Form COLORED IONS in solution
GROUP 18: NOBLE GASES
•  Unreactive or INERT
•  Stable octet (8 valence electrons)
-  Exception is He which has 2 valence
electrons
-  monoatomic
PROPERTIES OF METALS
GROUP 17: HALOGENS
•  7 valence electrons
•  Gain 1 electron to for -1 ions
•  Most REACTIVE nonmetal is F
HYDROGEN
•  Not officially part of a group
•  Nonmetal
•  Gas at STP
METALS HAVE A “SEA” OF MOBILE
ELECTRONS….RESULTS IN
ELECTRICAL CONDUCTIVITY
•  Malleable (can be hammered or rolled into
thin sheets)
•  Ductile (can be drawn into a wire)
•  Excellent conductors of heat and electricity
•  Luster (shiny)
•  Lose electrons to
form cations
•  Solid @ STP (except Hg)
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WHY DO METALS HAVE LUSTER?
•  Metals easily absorb light energy
which excites the delocalized
electrons and when they fall back to
lower energy levels they emit light
(luster)
WHY ARE ALLOYS (MIXTURES OF
METALS) STRONGER THAN PURE
METALS?
•  Alloys such as brass (a mixture of
copper and zinc) are harder than the
original metals because the
irregularity in the structure helps to
stop rows of atoms from slipping over
each other
WHY ARE METALS MALLEABLE AND
DUCTILE?
•  Metals consist of layers of atoms that
can slide over each other
METALLIC CHARACTER
•  How much “like a metal” an element is
•  Franicium is most metallic
-  Closer to Fr more metallic…further from Fr
least metallic
PROPERTIES OF METALLOIDS
•  Semiconductors (Good/moderate
conductor)
•  Luster (like metals) and Brittle (like
nommetals)
•  Used for making computer
microchips
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PROPERTIES OF NON-METALS
SUMMARY OF THE CATEGORIES
OF ELEMENTS
•  Poor conductors of heat and
electricity
•  Brittle (shatter when struck)
•  Dull
•  Tend to gain electrons to form anions
ATOMIC RADIUS
•  SIZE of the atom
•  Located on Table S
LESSON 4.3 TRENDS IN
ATOMIC RADIUS
W W W. M R PA L E R M O . C O M
ACROSS A PERIOD
TREND IN ATOMIC RADIUS
•  Trend: DECREASES
•  Why?
•  Nuclei have greater NUCLEAR PULL
(larger positive charges) which PULL
electrons CLOSER
Atomic radius decreases
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13 +
DOWN A GROUP
Greater nuclear
charge
17 +
Cl
Al
•  Trend: INCREASES
•  Why?
•  GREATER number of ENERGY SHELLS
(indicated by the PERIOD #)
Atomic Radius increases
Less nuclear charge
TO FIGURE OUT:
•  Pick a Period (row) or Group (column)
and note the values of the elements
USING TABLE “S” TO DETERMINE
TRENDS IN ATOMIC RADIUS
•  Example: Going across a period
what is the trend in atomic radius?
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•  Pick an element on the left side of the
periodic table and pick another
element on the right side of the same
period.
130 pm
"
60 pm
Trend is decreasing
ION SIZE- METALS
Ion radius SMALLER than
atomic radius
Why?
•  Metal ions LOSE electrons to
form Cations
• 
RECALL…..
ION SIZE- NONMETALS
Ion radius LARGER than
atomic radius
•  Why?
•  Nonmetal ions GAIN electrons to for
anions.
• 
© 2002 Prentice-Hall, Inc.
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RECALL……REACTIVITY
Metals
• 
LESSON 4.4 TRENDS IN
IONIZATION
ENERGY & ELECTRONEGATIVITY
• 
• 
Non Metals
Decreases across
period
Increases down group
• 
Reason: The larger
the atom the weaker
the nuclear pull and
the more easily you
lose electrons and
become stable
• 
• 
Increases across
period
Decreases down
group
Reason: The smaller
the atom the greater
the nuclear pull (+)
and the more easily it
attracts electrons (-)
IONIZATION ENERGY
e
-
+
e
-
+
Smaller atom
•  Energy required to REMOVE the most
loosely bound ELECTRON in the
valence shell
•  Located on Table S
Larger atom
TREND IN IONIZATION ENERGY
•  INCREASES across a PERIOD
•  Why?
•  Stronger NUCLEAR PULL makes it more
difficult to remove electrons
Less nuclear charge
e
-
Greater nuclear
charge
e
-
13 +
17 +
Cl
Al
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TREND IN IONIZATION ENERGY
e
-
•  DECREASES down a GROUP
•  Why?
•  Larger atomic radius means LESS
NUCLEAR PULL on outer electrons
e
-
+
+
EXAMPLE
•  What is trend in atomic radius going
down a group?
•  Why does this trend occur?
•  496
•  419
•  403
Trend is decreasing
larger atomic radius
equals less nuclear
pull on valence e-
ELECTRONEGATIVITY
•  Measure of the ATTRACTION
for electrons
•  Located on Table S
•  FLUORINE most electronegative (4.0)
•  The closer an atom is to Fluorine the
HIGHER the electronegativity
•  Scale of 0 - 4
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TREND IN ELECTRONEGATIVITY
•  INCREASES across period
•  Why?
Less nuclear charge
e
-
Greater nuclear
charge
e
-
-  Greater NUCLEAR PULL(charge) to attract
electrons
17 +
13 +
Cl
Al
TREND IN ELECTRONEGATIVITY
•  DECREASES down group
•  Why?
-  Larger atomic radius means LESS
NUCLEAR PULL to attract electrons to the
valence shell
e
e
-
+
+
The Trend is INCREASING
EXAMPLE
a.  What is the trend in electronegativity
across a period?
b.  Why does this trend occur?
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Summary
Periodic Property
Variation across
a Period
Variation down
a Group
Metallic
Character
Decreases
Increases
Atomic Radius
Decreases
Increases
Ionization Energy
Increases
Decreases
Electronegativity
Increases
Decreases
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