Periodic table Elements are arranged based on similarities in their properties Dmitri Mendeleev is credited with our current periodic table Even predicted the existence of elements that were not yet discoveredie Gallium ID: 701500
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Slide1
Chapter 6
The Periodic TableSlide2
Periodic table
Elements are arranged based on similarities in their properties
Dmitri Mendeleev is credited with our current periodic table
Even predicted the existence of elements that were not yet discovered(i.e. Gallium)
His periodic table was slightly revised a few years later so that the elements were in order of
increasing atomic number
Can be broken down into groups (columns) and periods (rows)Slide3
Periods
Range from 1-7
Indicates the highest occupied energy level in an atom Slide4
Groups
2 numbering systems: 1-18 and A/B elements
We will be using the A/B designation
A-elements are called the representative elements (besides noble gases)
B-elements are the transition and inner transition metals
A-group names:
I A- alkali metals
II A- alkaline earth metals
VII A- halogens
VIII A- noble gasesSlide5
Zig-zag
line
Locate the zig-
zag
line starting at III A
Metals are to the left of the line
Nonmetals are to the right of the line
Metalloids are those elements that border the line (except Al !!)Slide6
Color of the symbol
Black (includes white outlined in black)
solid at room temp.
Blue
liquid at room temp
Red
gas at room tempSlide7
Periodic Trends
Chapter 6Slide8
Standards
Students know
how to use the periodic table to identify trends in ionization energy, electronegativity, and the relative sizes of ions and atoms.Slide9
Definition: Half of the distance between nuclei in covalently bonded diatomic molecule
Radius
decreases
across a period
Increased effective nuclear charge
Radius
increases
down a group
Each row on the periodic table adds a “shell” or energy level to the atom
Atomic RadiusSlide10
Table of
Atomic
RadiiSlide11
Period Trend:
Atomic RadiusSlide12
Tends
to
increase
across a period
As radius decreases across a period, the electron you are removing is closer to the nucleus and harder to remove
Tends
to
decrease
down a group
Outer electrons are farther from the nucleus and easier to remove
Ionization Energy
Definition:
the energy required to remove an electron from an atomSlide13
Periodic Trend:
Ionization EnergySlide14
Electronegativity
Definition:
A measure of the ability of an atom in a chemical compound to attract electrons
Tends to
increase
across a period
As radius decreases, electrons get closer to the bonding atom’s nucleus
Tends
to
decrease
down a group
As
radius increases, electrons are farther from the bonding atom’s nucleusSlide15
Periodic Table of
ElectronegativitiesSlide16
Periodic Trend:
ElectronegativitySlide17
Summary of
Periodic TrendsSlide18
Ionic Radii
Cations
Positively charged ions formed when
an atom of a metal loses one or
more electrons
Smaller than the corresponding
atom
Anions
Negatively charged ions formed
when nonmetallic atoms gain one
or more electrons
Larger than the corresponding
atom Slide19
Table of Ion SizesSlide20
Practice
Identify each of the following:
Which has a larger atomic radius?
F , O
Na , Li
Which has a higher ionization energy?
Li , B
Mg ,
Sr
Which has a higher electronegativity value?
Na , K
C , N
Which particle has to largest radium in each atom/ion pair?
Na , Na
+
S
,
S
-2