The Elements

1
The Elements

• Properties of s-Block Elements
• Properties of p-Block Elements
• Properties of d-Block f-Block Elements

2
Representative Elements

• Groups 1A 8A
• As a group they
• Display a wide range of chemical physical
  properties
• Metals nonmetals
• Highly reactive some hardly reactive
• Solid, liquid, or gas at room temperature

3
Representative Elements

• Group valence electrons
• Similar chemical physical properties
• Valence electrons
• 1 8
• But different number of non-valence elecrtons

4
Shielding electrons

• Add electrons/levels of electrons
• Atomic radius increases
• Shielding effect increases
• Ionization energy decreases
• This makes it easier for and element to lose
  electrons

5
Metals

• Tend to lose electrons
• Lower ionization energy
• More reactive
• Reactivity increases as atomic increases
• Opposite is true for nonmetals
• Tend to gain electrons
• Higher ionization, more reactive
• Reactivity decreases as atomic increases

6
Representative Elements

• Of the representative elements, which is the most
  reactive metal?
• Francium
• Which is the most reactive nonmetal?
• Fluorine
• Trend for ionization energy??

7
Diagonal Relationships

• The close relationship between elements in
  neighboring groups of the periodic table

8
Hydrogen

• 1A?
• 1 valence electron
• Does not mean it has same properties as 1A metals
• Shares more properties with group 7A

9
Hydrogen

• Henry Cavendish
• flammable air
• Antoine Lavoisier
• hydrogen
• Hydro water
• Genes forms
• Hindenburg

10
Hydrogen

• Universe contains more than 90 H
• 3 isotopes of H
• Protium 99.985
• No neutrons
• Deuterium 0.015
• One neutron
• Tritium radioactive
• Two neutrons

11
Hydrogen

• Heavy water
• Deuterium
• Neutrons add mass to water molecules
• Nuclear reactors use heavy water
• Keeps the chain going

12
Hydrogen

• Single valence electron
• Explains metal nonmetal properties
• Nonmetal
• Gains an electron to become stable
• Metal
• Reacts with a nonmetal
• Like Oxygen

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Group 1A Alkali Metals

• Alkali?
• Arabic, al-qili
• Ashes of saltwort plant
• Easily lose a valence electron
• Form an ion with a 1 charge
• Soft enough to cut like butter
• Good conductors of heat electricity

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Lithium

• Lightest alkali metal
• Least reactive alkali metal
• Less likely to dissolve in water
• Closely related to Mg
• Found in
• Batteries, dehumidifiers
• Lithium carbonate
• Glass, prescription drugs
• Metal alloys
• Light strong (Airplane)

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Sodium Potassium

• Most abundant alkali metals
• Sodium
• Sodium lamp vapors heat exchanger in nuclear
  reactors
• Potassium
• Few industrial uses
• K Na gradient
• Sodium chloride (table salt)
• Potassium chloride (salt substitute)

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Rest of the alkali metals

• Rubidium, Cesium, Francium
• The most reactive alkali metals
• Very unstable
• Rb
• M.P. 40 C
• Fr
• Radioactive

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Group 2A Alkaline Earth Metals

• Alchemists classified because
• Did not melt in fire
• Form compounds with oxygen
• Oxides
• Tend to lose 2 e- to form 2 charge

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Beryllium

• Lightest of 2A
• Reacts with Al, Si, O
• Used to
• Moderate neutrons in nuclear reactors
• Tools for petroleum refineries

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Calcium

• Essential for humans
• Bones teeth
• Found in nature
• Limestone, Chalk, Coral
• Calcium carbonate
• Decomposes gt lime
• Steel, paper, glass, mortar

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Magnesium

• Lighter than steel, but equally strong
• Alloys with Al Zn
• Frames
• Backpack, bike, tires
• High melting point
• Line furnaces
• Plants
• Chlorophyll
• Hard water
• Water softener

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Rest of the alkaline earth metals

• Strontium
• Fireworks
• Barium
• Paints glass
• Radium
• Radioactive
• Emits alpha, beta, gamma rays
• Glows in the dark

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p-block Elements

• Many differences in properties of elements
• Metals, nonmetals, metalloids
• Solids or liquids at room temp.
• Get Stable!
• Ions

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Group 3A The Boron Group

• Always found with other elements in nature
• Oxides in Earths crust
• Metals
• Al, Ga, In, Tl
• Metalloid
• B
• Ions
• B, Al, Ga, In (3)
• Tl (1)

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Boron

• Lightest least represented
• Diagonal Relationship with Si
• Used in
• Laboratory Equipment
• Borax
• Cleaning agent
• Boric acid
• Disinfectant

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Aluminum

• Most abundant metal
• 3rd most abundant element in Earths crust
• Commonly with O or Si
• Great deal of E to purify
• Recycle!!!!
• Used in
• Bauxite
• Ceramics
• Gems
• Aluminum sulfate
• Antiperspirants water purification

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Gallium

• Liquid from 30C to 2403C
• Used in
• Gallium arsenide
• Semiconductor chips (solar power calculators)
• More efficient than Si chips
• Gallium nitride
• Blue laser
• More storage capacity on DVD
• Printers
• Cancer detecting

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Group 4A The Carbon Group

• Wide variety of properties
• Nonmetal
• Carbon
• Metalloid
• Si Ge
• Metal
• Sn Pb
• Few rules apply to all elements in group

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Carbon

• Organic chemistry
• Once believed that organic compounds could only
  be produced in organisms
• First synthesized in 1828
• Inorganic chemistry
• Mineral
• Element or inorganic material that
• is found in nature as solid crystals
• Ore
• Material from which a mineral can
• be removed at a reasonable cost

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Graphite vs. Diamond

• Both contain only C
• Allotropes
• Forms of an element in the same physical state
  that have different structures properties

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Silicon

• Second most abundant element in crust
• Used in
• Silicon carbine
• Sharpen tools
• Silicon dioxide (Silica)
• Quartz crystal, sand, glass

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Lead Tin

• Tin is a very soft metal
• Bronze
• Alloy of tin copper
• Pewter
• Alloy of tin zinc
• First isolated low MP
• Toxic
• Used in
• Eating utincils, plumbing, gas, paint
• Car batteries

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Group 5A The Nitrogen Group

• Wide variety of properties
• Nonmetal
• N P
• Metalloid
• As Sb
• Metal
• Bi

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Nitrogen

• Gas
• Colorless, odorless, relatively uncreative
• 78 of Earths atmosphere
• Nitrogen Cycle
• Ammonia
• Cleaning products
• Fertilizer (liquid)
• Nitric acid
• Explosives, dyes, solid fertilizers
• TNT

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Phosphorus

• Phosphoric acid
• Converted to phosphate compounds
• Used in
• Processed cheese
• Laxatives
• Baking powders
• Flame retardant coating
• Fertilizers
• Algae

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Arsenic, Antimony, Bismuth

• Less abundant
• Some of the oldest known elements
• Arsenic (toxic)
• Once used to treat illnesses
• Antimony sulfide
• Cosmetics, eye liner/shadow
• Bismuth
• Pink remedy for nausea diarrhea

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Group 6A The Oxygen Group

• Metals and nonmetals
• Valence electrons?
• Act as nonmetals
• Form 2- ions

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Oxygen

• 2 allotoropes
• 03 (ozone)
• 02
• 21 of atmosphere
• Colorless, odorless gas
• Joseph Priestly
• Mercury oxide
• Most abundant in earths crust
• Forms compounds with all elements
• Except helium, neon, and argon

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Sulfur

• 10 allotropes
• Melting point of 112 C
• Sulfur dioxide
• Preserve fruit and antibacterial agent
• Sulfuric acid
• Fertilizers
• Steel, paper, paints
• Heat vents
• Hydrogen sulfide

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Selenium

• Found in
• Vitamins
• Sodium selenate
• Fish, eggs, grains
• Inhibit growth of cancer cells
• Solar panels
• Toxic in high amounts

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Group 7A The Halogens

• Ability to form compounds with almost all metals
• Salts
• salt formers
• Differ in physical properties
• Always found with other element in nature
• Except Astatine
• Form 1- ions

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Fluorine

• Greatest electronegativity
• Most active of all elements
• Reacts with all elements except Ne, Ar, He
• Used in
• Toothpaste
• Uranium enrichment
• Fuel for nuclear reactors

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Chlorine

• Reacts with nearly all elements
• As a gas is deadly
• Used in
• Bleach solutions
• Dentists
• Hydrochloric acid
• Polyvinyl Chlorine
• PVC

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Bromine Iodine

• Few commercial uses
• Silver bromine silver iodine
• Coat photographs
• Iodine
• Thyroid gland
• Disinfectant

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Group 8A Noble Gases

• One of the last naturally occurring elements to
  be discovered
• Colorless unreactive
• Neil Bartlett
• Fluorine Xenon
• He, Ne, Ar

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Helium

• Lightest of the noble gases
• Emission spectra from the sun
• Used in
• Blimps, airships, balloons
• Deep sea divers
• Helium Oxygen mix

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Neon

• Neon lights
• Electricity runs though neon gas in tube
• Electrons become excited to higher energy level
• When electrons return to lower energy state
• Atoms emit bright orange light
• Argon
• Blue
• Helium
• yellow

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Argon Krypton

• Argon
• Most abundant of noble gases
• 1 of Earths atmosphere
• Both used in
• Filament in incandescent light bulbs

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d-Block f-Block

• Transition metals
• d-Block
• Inner transition metals
• f-Block
• f-Block
• Lanthanide series
• Period 6
• Actinide series
• Period 7

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Transition Metals

• Share properties in
• Electrical conductivity, luster and malleability
• Little variation in atomic size,
  electronegativity, ionization energy

51
Transition Metals

• Physical properties
• Determined by electron configuration
• Most are hard solids with high melting boiling
  points
• Differences are based on the ability of unpaired
  d electrons to move into the valence shell
• The more unpaired electrons in the d sublevel
• The greater the hardness and higher the melting
  boiling points

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Closer look

• Period 4 transition metals
• Moving left-to-right
• Sc 1, Ti 2, V 3, Mn - 4 unpaired d
  electron(s)
• Cr 6 unpaired electrons, 5 unpaired d electrons
  1 unpaired s electron
• Hardest has the highest melting point
• Fe, Co, N, Cu all form pairs of electrons
• Hardness, melting boiling points decrease
• Zn

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Ions

• Can lose 2 s electrons to form 2 ions
• Unpaired electrons can move to outer level
• Form ions with 3 charge
• Partially filled d sublevel can produce color
• Electrons in levels can absorb specific
  wavelengths of light

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Magnetism

• The ability of a substance to affected by a
  magnetic field
• Moving e- creates a magnetic field
• Paired e- have opposite spins
• Magnetic fields cancel out
• Diamagnetism
• All e- are paired, unaffected or repel magnetic
  field
• Ferromagnetism
• Strong attraction of a substance to a magnetic
  field
• If they stay aligned in the same direction they
  can become a permanent magnet

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Sources of Transition Metals

• Almost all metals are found in nature with
  nonmetals (except Ag, Au, Pt, Pl)
• Metallurgy
• Brach of applied science that studies designs
  methods for extracting metals their compounds
  from ores
• High temps.
• Blast furnace starts iron ore at
• 200C then to molten iron at 2000C
• Turned into steel

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Transition Metal Uses

• Our body needs large amounts of
• C, O, H, N, S, P, Na, K, Ca, Mg, Cl

• Cu
• Electrical wiring
• Zn
• Protective coating
• Alloys
• Jet engines, drill bits, surgical instruments

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Inner Transition Metals

• Lanthanide series
• Silvery metal with relatively high M.P.
• Found in nature with each other
• Hard to separate
• Used in
• Welders goggles
• TV screens
• Movie projectors
• Lasers
• Tinted sunglasses

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Inner Transition Metals

• Actinide Series
• Radioactive elements
• Only 3 exist in nature
• Transuranium