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The History of your Periodic Table
Ch. 5.1
The History of your Periodic Table
Dmitri Mendeleev- (father of the periodic table)
-Grouped elements in order of atomic mass
-Elements with similar properties were placed in
same column
-HIS MOST IMPORTANT CONTRIBUTION
1. He left spaces open for undiscovered elements
(big jumps in mass)
2. Predicted properties in those spaces with
amazing accuracy

The History of your Periodic Table



Sir William Ramsay discovered three Noble
Gases and added the group to Mendeleev’s
table.
Why were these elements hard to discover
compared to the others?
Lanthanides and the Actinides were the last
elements added to the table.
The History of your Periodic Table
Henry Mosely-Grouped elements in order of atomic
number
-credited with modern periodic table
Period Law-physical and chemical properties of
elements are a periodic function of
their atomic numbers

Inner Transition Metal Placement
Ch. 1.3 Periodic Table
 Periods
-a horizontal row of elements.
-Tells you the electron energy
levels.
Periodic Table
 Groups
(families)
-a vertical column of elements.
-Tells us the # of valence electrons
and the elements’ chemical
properties for “A Main Group”(s,p)
-d and f block makes up B Groups
Ch. 1.3 Periodic Table
4 types of elements
1. metals

2. nonmetals
3. metalloids
4. Noble Gases
Ch. 5.2
Families of the Periodic Table
Periodic Table - Regions
Transition Metals
Inner Transition Metals
Alkali Metals Group 1
 Most
reactive metals (one valence e-)
 Found as compounds (salts).
 Soft metals
 S-block
Alkaline-earth Metals Group 2
 Similar
to Alkali but less
reactive because they have
2 valence electrons
 Mostly found as compounds
 S-block
Calcium
Transition Metals Group 3-12
 d-block
 Less
reactive than group 1 and 2
 Good conductors
 High Luster
Transition Metals
 Hosts
the only liquid metal
mercury
 You can also find some of
the most sample metals:
gold, platinum, and
palladium
Inner Transition Metals
 Two
rows at the bottom
 Rare earth reactive metals
 Actinoids are all radioactive
 93 and above are manmade
 f-block
Uranium
P-Block


Contain all four types of elements
Other metals:


Aluminum most abundant metal on Earth.
More reactive than transition metals
Metalloids
(Semiconductors)
7
elements on the step
 Properties of both metals and non-metals.
 Silicon the most abundant element in
Earth’s crust (computer chips)
 Arsenic
is rat poison
Silicon
Arsenic Exposure
Non Metals
 Are
not able to conduct
electricity or heat very well.
 Found in groups 13-17 with the
exception of hydrogen.
HYDROGEN
It is not an alkali metal
 It is a nonmetal
 A very explosive gas.
 It is located in group one because it
has one valence electron

Carbon

Found as an element (coal, diamond, graphite)


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Allotrophes
Found in millions of different compounds
Called Organic Compounds
Oxygen and Nitrogen

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Oxygen is the most common atom found on
Earth
Nitrogen most common gas found in the
atmosphere
Halogens Group 17
 Highly
reactive
 Form salts with group 1
 Used to kill bacteria (Cl, F, I)
 Bromine the only liquid
nonmetal
Noble Gases Group 18
 Stable
and inert gases
 Don’t form compounds.
 Full valence shell.
 Fun with He
Xenon Bulbs
Neon
Krypton a stable violet colored gas?
Ch. 5.3 Periodic Trends
A
pattern of characteristics
that occur over and over again

Ex days of the weeks
 There
are many trends on the
Periodic Table
 d-block does vary as much as
s,p-blocks
Metallic Trends
 Going
left to right elements
become less metallic
 Going Down elements become
more metallic
Atomic Radii
 Atomic
Radii is measured by
taking the distance from the
nucleus to the outer energy level
Can you tell me the trend?
Atomic Radii

As you go down a group you are adding
an energy level, or another layer of
electrons
Atomic Radii
As you go across the period, your atomic
number increases
 When more protons exist in the nucleus,
more positive charge produces stronger
attractive forces on the electrons

Ionization Energy (kJ/mol)
 The
energy required to remove
the most loosely held electron in
the outer energy level of an atom.
 The less energy required, the
more reactive the metal
Ionization Energy
Atomic Radii
Needs more energy to be lost
+
+
eeNeeds less energy to be lost
Shielding Effect
Ionization Energy–Why increase across period?

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The more valence electrons the atom has,
the more energy it will need to lose its outer
electron.
Remember only metals want to lose electrons
st
1 ,
nd
2 ,
rd
3
IE
Reactivity for Metals

Going down a group reactivity
increases because the atom is more
willing to give away its electron and
react. (Ionization energy decreased)
Brainiac Video
Electronegativity/Electron Affinity
 Measure
of an atoms attraction
for an electron.
 Nonmetals have high attraction
for electrons
 The higher the attraction the more
reactive the nonmetal
Electronegativity
Electronegativity/Electron Affinity
 One
exception- noble gases
 Why?
 They don’t want electrons, they
are happy and full already
Reactivity for nonmetals
 Going
UP a group for nonmetals
increases their reactivity
 The reason more electron affinity
 Flourine is the most reactive
nonmetal.
Ionic Radii
Ions aren't the same size as the atoms
they come from.
 Cations are smaller than the parent atom
 Anions are bigger than the parent atom

Ionic Radii – Why Cations Smaller?
 By
losing electrons, they also
lose a whole energy level,
therefore, becoming smaller
in size
Ionic Radii – Why anions bigger?

When they gain electrons, the
outermost becomes full. So less force
is felt by the nucleus, the electrons
spreads out. (becoming stable)
Periodic Table Review