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Chapter 4
The Periodic Table
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4.1 Element Organization
Patterns in Element Properties
groups of elements havemuch in common
discovery (invention) ofperiodic table
1861
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4.1 Element Organization
Patterns in Element Properties
discovery (invention) ofperiodic table
1865: John Newlands (Englishchemist) noticed repeatingchemical and physical
properties every eightelements when arranged byincreasing atomic mass
thought to be absurd
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4.1 Element Organization
Patterns in Element Properties
1869: Dmitri Mendeleev madefirst periodic table
arranged elements byincreasing atomic mass
switched problem elements
made predictions for gapshe was right
nominated for Nobel prize
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4.1 Element Organization
Patterns in Element Properties
Henry Moseley (Englishchemist) found that pattern
of table was due to atomicnumber, not atomic mass
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Periodic Table
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Symbols in Table
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4.1 Element Organization
The Periodic Law
similar properties are due tosimilar electron configuration
each column (group) containselements with the samenumber of electrons in the
outer energy level (valenceelectrons)
valence electrons participate
in reactions (bonding)
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4.1 Element Organization
The Periodic Law
similar properties are due tosimilar electron configuration
each row (period) containselements with the samenumber of occupied energy
levels
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4.2 Table Tour
Main-Group Elements
elements in groups 1,2,13-18
s-and p-blocks
electron configuration variesconsistently
examples
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Main-Group Elements
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4.2 Table Tour
Main-Group Elements
Group 2: alkaline-earthmetals
also very reactive, but lessthan Group 1
usually found as compounds
harder, higher melting pointsthan alkali metals
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4.2 Table Tour
Main-Group Elements
Group 18: noble gases
unreactive; full set of
electrons in outer energy levelused to be called inert, butxenon was found to react
good for electric lights
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4.2 Table Tour
Main-Group Elements
Hydrogen
about 75% of the universe
behaves unlike any otherelement
reactive
major component in organiccompounds (carbs, proteins,lipids, nucleic acids)
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4.2 Table Tour
Metals
excellent conductors ofelectricity
100 000 x better than mostconductive nonmetal
excellent conductors of heat
l
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Metals
bl
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4.2 Table Tour
Metals
often ductile (can besqueezed into a wire)
often malleable (can behammered into a sheet)
often shiny
2 bl
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4.2 Table Tour
Metals
Transition Metals (Groups 3-12)
d-block
electron configuration is notidentical in each group
do not always lose the samenumbers of valence electronsin each reaction (depends onother element
4 2 T bl T
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4.2 Table Tour
Metals
Transition Metals (Groups 3-12)
can be found as pureelements (e.g., gold,platinum)
good conductors (both heatand electricity)
ductile and malleable
4 2 T bl T
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4.2 Table Tour
Metals
Lanthanides and Actinides
f-block
lanthanides: atomic numbersfollow lanthanum
actinides: atomic numbers
follow actinium
shiny metals
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4.2 Table Tour
Metals
Lanthanides and Actinides
reactive like alkaline-earth
metalsall actinides are radioactive(e.g., uranium)
4 2 T bl T
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4.2 Table Tour
Metals
melting points vary widely
metals can be mixed with
other metals to form alloysexamples: brass (copper andzinc), sterling silver (silver and
copper), steel (iron, carbon,manganese, nickel, chromium)
4 3 T d i P i di T bl
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4.3 Trends in Periodic Table
Trend: predictable change in
a particular direction Ionization Energy
Ionization: removing anelectron from an atom or ion
Ionization energy: energyrequired to remove anelectron from an atom or ion
must overcome attraction
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4 3 T d i P i di T bl
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4.3 Trends in Periodic Table
Ionization Energy
decreases as you move downa group
due to electron shielding(inner electrons shield outerelectrons from the full
attractive force of the nucleus) increases as you moveacross a period
I i ti E T d
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Ionization Energy Trends
I i ti E G h
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Ionization Energy Graph
4 3 T d i P i di T bl
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4.3 Trends in Periodic Table
Atomic Radius
bond radius: half thedistance from center to
center of two like atoms thatare bonded
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4 3 Trends in Periodic Table
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4.3 Trends in Periodic Table
Atomic Radius
increases as you move downa group
due partly to electronshielding
decreases as you move
across a periodlevels as electrons get close to
one another
Atomic Radii Trends
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Atomic Radii Trends
Atomic Radii Graph
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Atomic Radii Graph
4 3 Trends in Periodic Table
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4.3 Trends in Periodic Table
Electronegativity
measure of the ability of anatom in a compound to
attract electrons is calledelectronegativity
higher electronegativity means
a stronger pull on electrons
4 3 Trends in Periodic Table
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4.3 Trends in Periodic Table
Electronegativity
decreases as you move downa group
due to electron shielding increases as you moveacross a period
not adding electrons to innerlevels, so stronger effective
nuclear charge
Electronegativity Trends
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Electronegativity Trends
Electronegativity Graph
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Electronegativity Graph
4 3 Trends in Periodic Table
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4.3 Trends in Periodic Table
Ionic Size
increases as you move downa group
due to electron shieldingdecreases as you moveacross a period
due to increasing nuclearcharge, whether the ion is
positive or negative
Ionic Radii Trends
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Ionic Radii Trends
4 3 Trends in Periodic Table
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4.3 Trends in Periodic Table
Electron Affinity
the energy change thatoccurs when a neutral atom
gains an electron is calledthe atoms electron affinity
decreases as you move down
a group due totake a guess
increases as you move
across a period Electron Affinity Trends
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Electron Affinity Trends
4 3 Trends in Periodic Table
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4.3 Trends in Periodic Table
Melting and Boiling Points
peak as dand porbitals fill
bonds are stronger with half-
filled orbitals
Melting and Boiling Points
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Melting and Boiling Points