Mendeleev

1867- A scientist who arranged the elements in order of increasing atomic mass. The "father" of the modern periodic table

Atmosphere

List the major components

A shell of gases surrounding the earth.

COMPOSED OF- mostly N₂, and O₂. Also contains Ar, CO₂, H₂, and H₂O vapor

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Nitrogen

Major component of air (78%). Obtained by fractional distillation of liquid air. Inert and stable.

Compounds- NH₃, HNO₃, NO

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Oxygen

Most abundant element on earth (20% of air, 89% of H₂O) obtained by fraction distillation of liquid air or electrolysis of water. Reactive at high temperatures

1. Period
2. Colum or family

1. A horizontal row of elements in the periodic table. All the same number of shells of e-. Across the period, the elements' properties change

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Hydrogen

Free hydrogen is rare commercially obtained from H₂O. Reactive at high temperatures

compounds- H₂O, acids and bases, organic compunds, H₂O₂

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Noble gases

Non-reactive gases:

He, Ne, Ar, Kr, Xe, Rn

Uses: in neon signs, Rn- cure cancer, He- fill balloons, Kr- flourescent lamps

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Flourine

Elemental gas is poisonous.

Component of freon (refrigerator gas), plastic, toothpaste, insecticides

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Chlorine

• Kills bacteria in H₂O.
• Component of gastric juice in stomach (HCl)
• Table salt (NaCl)
• Produced by electrolysis of seawater

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Bromine

Liquid at room temperature. Prepared from seawater. Used in the petroleum, drug and photographic industries.

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Iodine

Obtained from nitrate and seawater deposits. Used in the drug industry (iodine solution, iodoform) and in table salt.

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Sulfur

Not active at room temperature. Large amounts occur in nature. Occurs in 3 alotropic forms.

Compounds: H₂SO₄, SO₂, Sulfa drugs, gunpowder, matches

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Phosphorus

• 2 allotropes: white and red
• Can combine with oxygen and hydrogen
• Used in: matched, rat poison, grenades
• Compounds: H₃PO₄, "Phospahates"

1. Nitrogen fixation
2. Haber process

1.The process of including nitrogen to combine chemically with other elements.

(Example: 3Mg + N₂ ↔ Mg₃N₂)

 2. The fixation of nitrigen to hydrogen in  the  presence of metal catalyst at high temperature and pressure to form ammonia

(N₂ + 3H₂ ↔ 2NH₃)

Combustion

Write the equation for the combustion of methane.

A reaction where O₂ combines with another substance so rapidly that heat and light are released.

CH₄+2O → CO₂ + 2H₂O

Allotrope

List an example

The same elemental subtance in different molecualer forms and possessing different properties.

(Oxygen- O₂, O₃; carbon diamond, graphite)

Ionic Hydride

Give examples

Hydrogen combines with active metals to form ionic compounds where the valence of hydrogen is -1

(NaH, CaH₂, LiH)

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Carbon

• allotropic: diamond, graphite, fullerene
• "backbone" of molecules in plants and animals
• Compounds: fats, sugars, gasoline

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Silicon

Second to oygen in abundance.

(25% Of earth's crust)

found in silicate rocks - clay, mica, SiO₂, quartz, sand

Hard and brittle; SiO₂ forms glass

1. Deionization
2. Distillation

1. A process used to separate water from its solutes. Water flows through resins which absorb the ions.
2. A process used to separate a miture based on different boiling points of the components. Componensts are separately vaporized the condensed

Halogens

A family of elements with 7 electrons in their outer shell. They are abundant and chemically active.

(F, Cl, Br, I, At)

Metalloid

List 5 examples

An element with the properties of both metals and non-metals.

Example: Si, As, Ge, Sb, Te

Noble Metals

The few metals which occur uncombined in nature.

(Gold, silver, platinum, copper)

1. Ore
2. Alloy

(List 2 examples)

1. A natural mineral deposit from which a metal can be extracted profitably
2. Alloys are composed of a solution of 2 or more metals and have metallic properties. (Steel, bronze)

1. Steel
2. Alloy steel

1. An alloy of iron and carbon containing less than 2% carbon. use: building material
2. By combining a transition metal with steel an endless varirty of "alloy steels" can be produced. common metals used: Cr, Co, Ni, W, Sn, Ti, V

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Chromium

bluish-white, brittle transition metal, hard, corrosion - resistant.

Chief ore: chromite

use: chromium plating, paint pigment

Metals

List 6 characteristics

• Solid (except Hg)
• Malleable and ductile
• Conduct heat and electricity
• Shiny, relective and lustrous
• Lose e- to form cations
• good reducing agents

Electronegativity

The ability of an atom to attract the e- in a covalent bond to itself.

VAlues range from 0.7 (Cs) to 4.0 (F)

1. Describe the change in electronegativity across the periodic table.
2. Describe the change in metallic activity across the periodic table

1. Electronegativity tends to increase across the table left ot the right and decrease down colums
2. Metallic activity decreases across the table (left to right) and increases down the columns.

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Nickel

A hard, white metal which resists tarnish. Ferromagnetic

Use: catalyst for hydrogenation of fats. Coins, the magnetic alloy is called alnico.

Non-metals

List 7 characteristics

• 1/2 are gases
• solids are brittles
• poor conducters of heat and electricity
• dull and non-flective
• gain e- to form anions good oxidizing agents

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Copper 

principal ores:

chalcocite, cuprite chalcopyrite

soft, red-brown, ductile, malleable

use: wires, brass, bronze

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Zinc

principal ores: sphalerite, smithsonite, zincite

use: galvanized iron, dry cells, electrical connectors, die casting

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Mercury

The only liquid metal at room temperature.

Uses: thermometers, Hg vapor lamps, alloys- amalgams

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Tin

soft white low-melting metal

use: tinplates- to protect steel and in alloys

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Alkali metals

• form +1 cations
• soft metals
• react to light and air
• found in seawater and rocks
• displace hydrogen from water
• found in group IA of the periodic table

use: sodium vapor lamps, salt, lye, postash (Li, Na, K, Rb, Cs)

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Lead

soft, non-elastic, low-melting, blue-white metal. Becomes dark grey in air.

uses: piping, telephone cables, alloys

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Silver

Found uncombined or as Ag₂S, bright, lustrous, soft, malleable

uses: silver plating, jewelry, photographic film and paper

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Gold

Found uncombined as nuggets or grains.

uses: coins, jewelry, alloys

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Platinum metals

They are: Ru, Rh, Pd, Os, Ir, Pt

Inert and occur free in nature, rare, and expensive

uses of Pt: dentistry, jewelry, industrial catalyst

Lanthanide and actinide series

Transition elements #57-71 and #89-103 which have partially filled f orbitals. Only the first four elements occur naturally.

Describe the change in Atomic Radius across the periodic table

The atomic radius tends to decrease from left to right across the table and increase down the columns

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Ammonium Ion

The ammonium ion (NH₄⁺¹) behaves chemically like an alkali metal

use: fertilizers, baking powder, soldering flu, explosives

Alkaline earth metals

• a family of metals which form +2 cations
• chemically active
• their oxides form mildy basic solutions

(Be, Mg, Ca, Sr, Ba)

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Magnesium

• abundant (2% of earth's crust)
• found in seawater, salt beds and silicates

uses: structural metal, flashbulbs, milk of magnesia

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Calcium

• abundant (3% of eath's crust)
• found in limestone marble, chalk and seashells

uses: essential to bones and teeth, concrete, mortar

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Aluminum

• most abundant metal (7% of earth's crust)
• found in mica, feldspar
• bauxite(principal ore)

use: structure (wheels, building) foil, paint, electrical wires

1. Malleable
2. Ductile

1. A physical property of metals; can be asily made into sheets (example: aluminum foil)
2. A physical property of metals; can be drawn into a wire. (example: copper electrical wires)

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Iron

• abundant (5% of earth's crust)
• principal ores: hematite, pyrite, magnetite
• seperated from ore in a blast furnace

uses: structural, magnetic, dyes

Transition element

• A metal having two incomplete shells of electrons
• Many have multiple oxidation states.
• Less active than family IA and IIA

examples: Fe, Ag, Au, Cr, W  

Describe the change in Nonmetallic activity across the periodic table

Non-metallic activity increases across the table (left to right) and decreases down the colums.

Compare the ionic radii of

1. Cl, S, P
2. Na, Mg, Al

What is the reason for the different sizes?

1. Cl^-1 is smallest; P^-3 is the largest, the P atom gained the most e- and has rhe most shells.
2. Na⁺¹ is the largest; Al⁺³ is smallest, the Al atom lost the most e- and has the fewest shells.

Ionization energy

The energy change required for the removal of the outermost electron from the gaseous atom to form a +1 ion.