AP Chem: Elements – Flashcards

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Mendeleev

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

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Atmosphere

List the major components

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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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List some basic facts about:

Nitrogen

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

Compounds- NH3, HNO3, NO

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List some facts about:

Oxygen

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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

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  1. Period
  2. Colum or family
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  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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List some basic facts about:

Hydrogen

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

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

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List some basic facts about:

Noble gases

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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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List some basic facts about:

Flourine

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Elemental gas is poisonous.

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

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List some basic facts about:

Chlorine

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  • Kills bacteria in H2O.
  • Component of gastric juice in stomach (HCl)
  • Table salt (NaCl)
  • Produced by electrolysis of seawater
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List some basic facts about:

Bromine

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

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List some basic facts about:

Iodine

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

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List some basic facts about:

Sulfur

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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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List some basic facts about:

Phosphorus

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  • 2 allotropes: white and red
  • Can combine with oxygen and hydrogen
  • Used in: matched, rat poison, grenades
  • Compounds: H3PO4, "Phospahates"
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  1. Nitrogen fixation
  2. Haber process
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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)

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Combustion

Write the equation for the combustion of methane.

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

CH4+2O ; CO2 + 2H2O

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Allotrope

List an example

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

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

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Ionic Hydride

Give examples

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

(NaH, CaH2, LiH)

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List some facts about:

Carbon

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  • allotropic: diamond, graphite, fullerene
  • "backbone" of molecules in plants and animals
  • Compounds: fats, sugars, gasoline
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List some basic facts about:

Silicon

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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

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  1. Deionization
  2. Distillation
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  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
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Halogens

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

(F, Cl, Br, I, At)

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Metalloid

List 5 examples

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

Example: Si, As, Ge, Sb, Te

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Noble Metals

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The few metals which occur uncombined in nature.

(Gold, silver, platinum, copper)

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  1. Ore
  2. Alloy

(List 2 examples)

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  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)
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  1. Steel
  2. Alloy steel
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  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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List some basic facts about:

Chromium

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

Chief ore: chromite

use: chromium plating, paint pigment

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Metals

List 6 characteristics

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

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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)

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  1. Describe the change in electronegativity across the periodic table.
  2. Describe the change in metallic activity across the periodic table
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  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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List some basic facts about:

Nickel

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A hard, white metal which resists tarnish. Ferromagnetic

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

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Non-metals

List 7 characteristics

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  • 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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List some basic facts about:

Copper 

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principal ores:

chalcocite, cuprite chalcopyrite

soft, red-brown, ductile, malleable

use: wires, brass, bronze

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List some basic facts about:

Zinc

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principal ores: sphalerite, smithsonite, zincite

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

 

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List some basic facts about:

Mercury

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The only liquid metal at room temperature.

Uses: thermometers, Hg vapor lamps, alloys- amalgams

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List some basic facts about:

Tin

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soft white low-melting metal

use: tinplates- to protect steel and in alloys

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List some basic facts about:

Alkali metals

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  • 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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List some basic facts about:

Lead

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

uses: piping, telephone cables, alloys

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List some basic facts about:

Silver

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

uses: silver plating, jewelry, photographic film and paper

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List some basic facts about:

Gold

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Found uncombined as nuggets or grains.

uses: coins, jewelry, alloys

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List some basic facts about:

Platinum metals

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

Inert and occur free in nature, rare, and expensive

uses of Pt: dentistry, jewelry, industrial catalyst

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Lanthanide and actinide series

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

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Describe the change in Atomic Radius across the periodic table

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

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List some basic facts about:

Ammonium Ion

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

use: fertilizers, baking powder, soldering flu, explosives

 

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Alkaline earth metals

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  • 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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List some basic facts about:

Magnesium

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

uses: structural metal, flashbulbs, milk of magnesia

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List some basic facts about:

Calcium

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  • 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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List some basic facts about:

Aluminum

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

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

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  1. Malleable
  2. Ductile
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  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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List some basic facts about:

Iron

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

uses: structural, magnetic, dyes

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Transition element

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  • 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  

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Describe the change in Nonmetallic activity across the periodic table

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

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Compare the ionic radii of

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

What is the reason for the different sizes?

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  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.
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Ionization energy

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

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