Download 6.1 Organizing the Elements

6.1 Organizing the Elements >
Chapter 6
The Periodic Table
6.1 Organizing the Elements
6.2 Classifying the Elements
6.3 Periodic Trends
1
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6.1 Organizing the Elements >
CHEMISTRY
& YOU
How can you organize and classify
elements?
2
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6.1 Organizing the Elements > Searching for an
Organizing Principle
Objectives
• Discuss how early chemists organized
the known elements.
• Describe how the modern periodic table
is organized.
• Identify three broad classes of elements
3
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6.1 Organizing the Elements > Searching for an
Organizing Principle
A few elements, including copper,
silver, and gold, have been known for
thousands of years.
• There were only 13 elements identified by the
year 1700.
– Chemists suspected that other elements existed.
– In one decade (1765–1775), chemists discovered
five new elements.
4
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6.1 Organizing the Elements > Searching for an
Organizing Principle
Early chemists attempted to organize the
known elements.
o Some used the properties of the elements
• Dobereiner, a German chemist, published a
classification system for elements.
o He organized and grouped the known elements into
triads.
5
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6.1 Organizing the Elements > Today’s Periodic Table
Today’s Periodic Table
How is the modern periodic table
organized?
6
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6.1 Organizing the Elements > Today’s Periodic Table
In the modern periodic table, elements
are arranged in order of increasing
atomic number.
7
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6.1 Organizing the Elements > Today’s Periodic Table
• Henry Moseley modified Mendeleev’s table
o **He arranged the elements by increasing
atomic number.
o **Elements that have similar chemical and
physical properties end up in the same
column in the periodic table.
8
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6.1 Organizing the Elements > Today’s Periodic Table
• This led to the Periodic Law
o When the elements are arranged in order of
increasing atomic number, there is a periodic
repetition of their physical and chemical
properties.
9
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6.1 Organizing the Elements > Today’s Periodic Table
• There are seven horizontal rows or periods
in the table
o Each period corresponds to the energy
level
• There are eighteen vertical columns or
groups in the table
10
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6.1 Organizing the Elements > Today’s Periodic Table
• Today’s table has 118 elements
11
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6.1 Organizing the Elements > Today’s Periodic Table
• Periodicity can be observed in the periodic
table
o *Each group has similar properties
o The electron configuration tells an element’s
position in the periodic table
12
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6.1 Organizing the Elements >
Warm-up
1. What is the electron configuration of Phosphorus?
2. Determine the element from the atomic model
pictured below. Find the number of valence electrons.
13
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6.1 Organizing the Elements >
Chapter 6
The Periodic Table
6.1 Organizing the Elements
6.2 Classifying the Elements
6.3 Periodic Trends
14
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6.1 Organizing the Elements > Electron Configurations in
Groups
Objectives
• Describe the information in a periodic
table.
• Classify elements based on electron
configuration.
15
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6.1 Organizing the Elements >
16
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6.1 Organizing the Elements >
Blocks of Elements
The periodic table is divided into sections,
or blocks, that correspond to the highest
occupied sublevels.
17
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6.1 Organizing the Elements > Electron Configurations in
Groups
Electron Configurations in Groups
•
18
How can elements be classified
based on electron configurations?
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6.1 Organizing the Elements > Electron Configurations in
Groups
• Electrons play a key role in determining
the properties of elements.
Elements can be sorted into noble
gases, halogens, transition metals, or
inner transition metals based on their
electron configurations.
19
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6.1 Organizing the Elements > Electron Configurations in
Groups
Remember:
• s block – groups 1 & 2
• p block – groups 13 – 18
• d block – groups 3 – 12
• f block – bottom two rows
20
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6.1 Organizing the Elements >
•
s block
o Group 1 – Alkali metals (s1)
- Most reactive metals
-
So reactive, not found in nature as elements
1 valence electron
https://www.youtube.com/watch?v=m55kgyApYrY
Lithium (Li)
1s22s1
Sodium (Na)
1s22s22p63s1
Potassium (K) 1s22s22p63s23p64s1
21
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6.1 Organizing the Elements >
•
s block
o Group 2 – Alkaline Earth metals (s2)
- Less reactive than group 1 metals
- 2 valence electrons
Beryllium (Be)
Magnesium (Mg)
Calcium (Ca)
22
1s22s2
1s22s22p63s2
1s22s22p63s23p64s2
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6.1 Organizing the Elements >
•
p block
o Group 13 – Mixed group (s2p1)
- Even less reactive than groups 1 & 2
- 3 valence electrons
Boron (B)
Aluminum (Al)
Gallium (Ga)
23
1s22s22p1
1s22s22p63s23p1
1s22s22p63s23p64s23d104p1
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6.1 Organizing the Elements >
•
p block
o Group 14 – Mixed group (s2p2)
- 4 valence electrons
o Group 15 – Mixed group (s2p3)
- 5 valence electrons
24
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6.1 Organizing the Elements >
p block
Group 16 – Nonmetals (s2p4)
- 6 valence electrons
Group 17 – Halogens (s2p5)
- Most reactive nonmetals
- 7 valence electrons
- Example Fluorine: 1s22s22p5
Video1
Video2
Group 18 – Noble Gases (s2p6)
- 8 valence electrons (with the exception of
helium)
- Completely unreactive nonmetals
25
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6.1 Organizing the Elements > Electron Configurations
in Groups
Halogens
• There are seven
electrons in the highest
occupied energy level (7
valence electrons).
26
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6.1 Organizing the Elements > Electron Configurations in
Groups
The Noble Gases
• There are eight electrons in
the highest occupied
energy level.
o These eight electrons are
called valence electrons
27
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6.1 Organizing the Elements >
d block
Groups 3 – 12 – Transition metals
- Have usually 2 or 3 valence electrons
- Less reactive than groups 1 & 2
- Have the ability to move their electrons from s and d
orbitals
f block
Bottom two rows
- Known as the lanthanides and actinides (inner transition
metals or rare earth metals)
- Have usually 2 or 3 valence electrons
- Have the ability to move their electrons from s and f
orbitals
28
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6.1 Organizing the Elements >
Sample Problem 6.1
1 Analyze Identify the relevant concepts.
• For all elements, the atomic number is equal
to the total number of electrons.
• For a representative element, the highest
occupied energy level is the same as the
number of the period in which the element is
located.
• You can tell how many electrons are in this
energy level from the group in which the
element is located.
29
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6.1 Organizing the Elements > Sample Problem 6.1
2 Calculate Apply the concepts to this problem.
Use Figure 6.9 to identify where the atom is
in the periodic table and the number of
electrons in the atom.
1. This element ends in 3s23p2
Ans: Silicon
2. This element ends in 5s24d2
Ans: Zirconium
3. This element ends in 5s25p5
Ans: Iodine
30
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6.1 Organizing the Elements > Section 6-1
Section 6.1 Assessment
What is a row of elements on the periodic
table called?
A. octave
B. period
31
D
A
0%
C
D. transition
B
C. group
A. A
B. B
C. C
0%
0%
0%
D. D
6.1 Organizing the Elements > Section 6-1
Section 6.1 Assessment
What is silicon an example of?
A. metal
B. non-metal
32
D
A
0%
C
D. metalloid
A. A
B. B
C. C
0%
0%
0%
D. D
B
C. inner transition metal
6.1 Organizing the Elements > Key Concepts
• Elements can be sorted into noble
gases, representative elements,
transition metals, or inner transition
metals based on their electron
configurations.
33
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6.1 Organizing the Elements >
Three broad classes of elements are
metals, nonmetals, and metalloids.
• The elements can be grouped into one of
these three classes based on their
general properties.
34
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6.1 Organizing the Elements > Metals, Nonmetals, and
Metalloids
Periodic tables are sometimes color-coded
to classify types of elements.
35
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6.1 Organizing the Elements > Today’s Periodic Table
Metals
• The majority of elements
are metals
• Metals have three key
properties
1) Shiny or luster
2) Flexible (malleable – hammer into a sheet and
ductile – drawn into a wire)
3) Good conductor of energy (electricity and heat)
36
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6.1 Organizing the Elements > Metals, Nonmetals, and
Metalloids
Nonmetals
• Although there are fewer nonmetals,
they are more abundant on Earth
• Nonmetals have three key properties
1) Dull
2) Brittle
3) Poor conductor of heat and electricity
37
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6.1 Organizing the Elements > Metals, Nonmetals, and
Metalloids
Nonmetals
The variation among nonmetals makes it
difficult to describe one set of general properties
that will apply to all nonmetals.
• A diamond, which is
composed of carbon,
is very hard.
38
• Some match heads are
coated with phosphorus,
a brittle solid.
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6.1 Organizing the Elements > Metals, Nonmetals, and
Metalloids
Metalloids
There is a heavy stair-step line that separates the
metals from the nonmetals.
• Most of the
elements that
border this
line are
shaded green.
• These
elements are
metalloids.
39
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6.1 Organizing the Elements > Metals, Nonmetals, and
Metalloids
Metalloids
• A metalloid generally has properties that
are similar to those of metals and
nonmetals.
o Their properties can be changed by
conditions
o Silicon is the most famous metalloid
-It is responsible for computer chips
40
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6.1 Organizing the Elements > Metals, Nonmetals, and
Metalloids
Metalloids
• Silicon is also
present as the
compound
silicon dioxide
in glass items.
• Silicon can be cut into wafers and
used to make computer chips.
41
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6.1 Organizing the Elements >
CHEMISTRY
& YOU
All of the known elements are listed in
the periodic table. What are different
ways you could use the periodic table to
classify elements?
42
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6.1 Organizing the Elements >
CHEMISTRY
& YOU
All of the known elements are listed in
the periodic table. What are different
ways you could use the periodic table to
classify elements?
You can use the periodic table to classify
elements by their atomic weight, by their
chemical properties, by their physical
properties, or by their electron
configuration.
43
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6.1 Organizing the Elements > Key Concepts
Early chemists used the properties of
elements to sort them into groups.
Mendeleev arranged the elements in his
periodic table in order of increasing
atomic mass.
In the modern periodic table, elements are
arranged in order of increasing atomic
number.
Three classes of elements are metals,
nonmetals, and metalloids.
44
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6.1 Organizing the Elements > Glossary Terms
• periodic law: when the elements are
arranged in order of increasing atomic
number, there is a periodic repetition of their
physical and chemical properties
• metal: one of a class of elements that are
good conductors of heat and electric
current; metals tend to be ductile,
malleable, and shiny
45
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6.1 Organizing the Elements > Glossary Terms
• nonmetal: an element that tends to be a
poor conductor of heat and electric current;
nonmetals generally have properties
opposite to those of metals
• metalloid: an element that tends to have
properties that are similar to those of metals
and nonmetals
46
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6.1 Organizing the Elements >
Do Now
1. ___ ion
a. The ability of an atom to attract
electrons when in a compound
2. ___ atomic radius
a. Atom that has a positive or
negative charge
3. ___ ionization energy
4. ___ electronegativity
47
b. one-half the distance between
the nuclei of two atoms when
atoms are joined
c. The energy required to remove
an electron from an atom
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6.1 Organizing the Elements >
Terrence Howard Wears Diamonds
https://www.youtube.com/watch?v=gWTE
Xtx8mQA
48
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6.1 Organizing the Elements >
Chapter 6
The Periodic Table
6.1 Organizing the Elements
6.2 Classifying the Elements
6.3 Periodic Trends
49
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6.1 Organizing the Elements >
Objectives
• Describe trends among elements for
atomic size (radii), ionization energy,
electron affinity, and electronegativity.
• Explain how ions form.
50
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6.1 Organizing the Elements >
There are several trends in the periodic
table
o
o
o
o
o
o
51
Valence electrons
Atomic radii
Ionic radii
Ionization energy
Electron affinity
Electronegativity
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6.1 Organizing the Elements > Trends in Atomic Size
Trends in Atomic Radii
• The distance between the nuclei of two identical atoms
(i.e. two chlorine atoms) that are bonded together can
be used to estimate the size of the atoms.
• Atomic radii is one half the distance between the nuclei
of two atoms of the same element
52
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Trends in> Atomic Size
6.1 Organizing the Elements
Atomic Radius Trend:
Down a group – atomic radii increases

-This happens because of the increased
number of energy levels
-The energy levels shield the electrons from
the attraction of protons in the nucleus
53
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Trends in> Atomic Size
6.1 Organizing the Elements
Atomic Radius Trend:
oAcross a period – atomic radii decreases
-This happens because as more electrons are
added to the same energy level, those
electrons are pulled closer due to the
increased number of protons in the nucleus
oLargest atomic radii – francium
Smallest atomic radii – fluorine
54
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6.1 Organizing the Elements > Trends in Atomic Size
The figure below summarizes the group
and period trends in atomic size.
55
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6.1 Organizing the Elements > Trends in Atomic Size
Periodic Trends in Atomic Size
Atomic radius (pm)
Across a period, the electrons are added to the
same principal energy level.
56
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AtomicCopyright
number
.
Interpret>Graphs
6.1 Organizing the Elements
Group Trends in Atomic Size
The atomic radius within these groups increases
as the atomic number increases.
Atomic radius (pm)
• This increase
is an example
of a trend.
Atomic number
57
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6.1 Organizing the Elements >
What are the trends for atomic
radii?
In general, atomic radius increases
from top to bottom within a group
and decreases from left to right
across a period.
58
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6.1 Organizing the Elements > Trends in Atomic Size
Valence electrons are the electrons found in
the outermost energy level
o These are the electrons available to be
gained, lost, or shared
59
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6.1 Organizing the Elements >
All atoms want 8 valence electrons or a full
outer energy level
-
Noble gas electron configuration
Valence electrons determine the chemical
properties of the atom
Valence electrons can be represented using
Lewis Dot Diagrams
60
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6.1 Organizing the Elements > Trends in Atomic Size
Valence electrons can
be represented using
Lewis Dot Diagrams
61
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6.1 Organizing the Elements >
Do Now
1. What is the trend in atomic radii going down
a group?
2. Explain your answer for #1.
3. What is the trend in atomic radii going left to
right across the periodic table?
4. Draw the Lewis Dot Diagram for Boron.
62
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6.1 Organizing the Elements >
Atoms are neutral because there are equal
numbers of both protons and electrons
o Example: Sodium (Na) 11 positively charged protons
11 negatively charged electrons
o The net charge on a sodium atom is zero
[(+11) + (-11) = 0].
Sometimes atoms can gain or lose electrons to
form ions
63
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6.1 Organizing the Elements >
An ion is an atom or group of atoms that
has a positive or negative charge
o Losing electrons results in a positive ion
called a cation
o Gaining electrons results in a negative
ion called an anion
64
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6.1 Organizing the Elements > Ions
Ions
How do ions form?
http://education-portal.com/academy/lesson/ionspredicting-formation-charge-and-formulas-ofions.html#lesson
65
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6.1 Organizing the Elements >
Metals (left side of the table) form cations
Cations are smaller than their atom counterparts
because they are losing an electron (and
sometimes an energy level)
• More positive charges have a greater pull on
less negative charges
66
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6.1 Organizing the Elements >
Nonmetals (right side of the table) form anions
Anions are larger than their atom counterparts
because they are gaining an electron
• Less positive charges cannot pull in the
greater number of negative charges
67
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6.1 Organizing the Elements >
What type of element tends to
form anions? What type tends to
form cations?
Nonmetals tend to form anions.
Metals tend to form cations.
68
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6.1 Organizing the Elements >
Ionization Energy
video
Ionization energy is the energy required to remove
an electron from an atom
o a low IE means it is easier to remove the
electron
o Atoms can lose an electron, to form an ion
They do this to achieve noble gas electron
configuration (or 8 valence electrons)
o When an atom easily loses electrons, it is said
to be active
o Metals tend to lose electrons
69
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6.1 Organizing the Elements >
Ionization Energy
oDown a group – ionization energy decreases
•As the valence electrons are farther from the
nucleus, the atom gives them up easily,
requiring little energy to remove them
70
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6.1 Organizing the Elements >
Ionization Energy
oAcross a period – ionization energy increases
•As the number of valence electrons increases
in the same energy level, the atom is more
resistant to giving up an electron (more energy)
oGreatest IE – fluorine
oLeast IE - francium
71
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6.1 Organizing the Elements >
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6.1 Organizing the Elements >
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6.1 Organizing the Elements >
Electronegativity
Electronegativity is the measure of the ability
of an atom in a chemical compound to attract
electrons
o All values are based on fluorine
- Fluorine is most electronegative atom - 4.0
- The trend decreases in either direction
from fluorine
74
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Interpret>Data
6.1 Organizing the Elements
This table lists electronegativity values for
representative elements in Groups 1A through 7A.
Electronegativity Values for Selected Elements
H
2.1
75
Li
1.0
Be
1.5
B
2.0
C
2.5
N
3.0
O
3.5
F
4.0
Na
0.9
Mg
1.2
Al
1.5
Si
1.8
P
2.1
S
2.5
Cl
3.0
K
0.8
Ca
1.0
Ga
1.6
Ge
1.8
As
2.0
Se
2.4
Br
2.8
Rb
0.8
Sr
1.0
In
1.7
Sn
1.8
Sb
1.9
Te
2.1
I
2.5
Cs
0.7
Ba
0.9
Tl
1.8
Pb
1.9
Bi
1.9
• The data
in this
table is
expressed
in Pauling
units.
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6.1 Organizing the Elements >
Electronegativity Trend
76
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6.1 Organizing the Elements > Trends in
Electronegativity
This figure summarizes several trends that
exist among the elements.
77
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6.1 Organizing the Elements > Key Concepts
In general, atomic size increases from
top to bottom within a group and
decreases from left to right across a
period.
Positive and negative ions form when
electrons are transferred between
atoms.
First ionization energy tends to
decrease from top to bottom within a
group and decrease from left to right
across a period.
78
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6.1 Organizing the Elements > Key Concepts
In general, electronegativity values
decrease from top to bottom within a
group. For representative elements,
the values tend to increase from left
to right across a period.
79
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6.1 Organizing the Elements >
END OF 6.3
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6.1 Organizing the Elements >
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6.1 Organizing the Elements >
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6.1 Organizing the Elements >
Atoms are neutral because there are equal
numbers of both protons and electrons
Ex. Carbon C
6 protons
6 electrons
o Sometimes atoms can gain or lose
electrons to form ions
• An ion is an atom or group of atoms
that has a positive or negative charge
83
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6.1 Organizing the Elements >
o Losing electrons results in a positive
ion called a cation
• Metals (left side of the table) form
cations
Example: K1+
o Gaining electrons results in a negative
ion called an anion
• Nonmetals (right side of the table)
form anions
Example: Cl184
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6.1 Organizing the Elements >
Practice
Lithium
Oxygen
Li
# ___ protons
# ___ electrons
Li1+
# ___ protons
# ___ electrons
O
# ___ protons
# ___ electrons
O285
# ___ protons
# ___ electrons
6.1 Organizing the Elements >
BIG IDEA
Electrons and the Structure of Atoms
• Periodic tables may contain each
element’s name, symbol, atomic number,
atomic mass, and number of electrons in
each energy level.
• The electron configuration of an element
can be determined based on the location
of an element in the periodic table.
86
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6.1 Organizing the Elements >
END OF 6.2
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6.1 Organizing the Elements >
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6.1 Organizing the Elements >
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6.1 Organizing the Elements >
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6.1 Organizing the Elements >
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6.1 Organizing the Elements >
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