Periodic Table Notes

1
Periodic Table Notes

• Put these on the back of your table

2

• Columns (vertical)
• 1-18 (groups or families)
• Have similar but not identical properties
• Rows (horizontal)
• 1-7 (periods)
• Elements in a period are not alike in properties
• Patterns from left to right
• First elements in column (left) very reactive
• Last elements in column (right) always an
  un-reactive gas
• Elements become less metallic from left to right

3
Valence

• Valence number is the number of electrons in the
  outermost energy level. This number will
  indicate how many bonds an elements is able to
  make.
• Roman numeral number on periodic table
• Family
• 1 1 v.e. 14 4 v.e. 17 7 v.e.
• 2 2 v.e. 15 5 v.e. 18 8 v.e.
• 13 3 v.e. 16 6 v.e.

4
Metals (95 of 118 elements) middle/left side of
periodic table

• Properties
• Luster, ductility (ability to bend into a wire),
  malleability (ability to pound into thin sheets),
  good conductors of heat and electricity
• Valence of 1,2,3,4. Tend to lose electrons (thus
  becoming cations
• Most corrode- react chemically

5
Nonmetals (right side of periodic table)

• Properties
• No luster, dull, do not conduct heat/electricity
• Brittle- break easily, not ductile or malleable
• Valence 5,6,7,8 will gain 3,2, or 1 electron
  (s), thus becoming an anion

6
Metalloids- both sides of the zigzag line on the
periodic table

• Properties
• Properties of both metals and nonmetals
• Solids can be dull or shiny
• Will conduct electricity/heat, but not as well as
  metals

7
Rare Earth elements (transition metals)

• Lanthanoid series
• Soft, high luster and conductivity
• Actinoid series
• All radioactive, all except for first 4 are
  manmade

8
Alkali Metals (family 1) BROWN

• Valence number of 1. Very reactive, especially
  with water
• So reactive, that if touched they will burn skin
• Easily form salts with halogens. They are never
  found in their pure forms in nature.
• Soft, silver-white, low melting points. Good
  conductors.
• Each metal gives off a different color when
  burned. (Licrimson color, Na yellow, Kviolet,
  Rb red/violet, Csblue.)

9
Alkali Metals cont

• Little is known about Fr because it is so rare
  and radioactive
• Uses Li-grease/lubricants, aircraft parts, and
  batteries. Na salt, gasoline. K- fertilizer,
  photography (more expensive than Na, so is less
  widely used.

10
Alkaline Earth Metals (family 2) ORANGE

• Valence of 2-lose electrons, not as reactive as
  family 1
• Soft silver-white, high melting points, high
  densities. Reactive and will react with water.
• Will oxidize or tarnish in the air
• Never found in pure forms.
• Good conductor of electricity.
• Each element burns a different color Mgwhite,
  Caorange/red, Sr bright red, Ba yellow/green,
  Ra crimson

11
Alkaline Earth metals cont..

• Uses fireworks, Be is often added to other
  metals to make hard metal alloys, rocket cones,
  and nuclear reactors. Mg aircraft and
  photographic equipment. Ca used with other
  metals to make reactive alloys. Ra radioactive
  so used in cancer treatment.

12
Transition elements/ Metals (family 3-12) PINK

• Largest family on the periodic table. All are
  metals.
• Most are hard, strong, shiny metals with high
  melting and boiling points. (Hg is the exception,
  since it is liquid at room temperature)
• Most are good conductors of heat/electricity
• Most will dissolve in acid (Au is the exception
  because it resists acids)

13
Transition Metals cont

• Most can bond with oxygen in more than one way
  making different compounds (ex. Fe bonds with O
  to form the ores hermanite and magnetite)
• Most are ductile and malleable
• Uses due to their ability to form strong metal
  alloys, ductility, and malleability these
  elements are used in construction materials,
  pipes, wires, coins, jewelry, aircraft, cars,
  bicycles, cooking utensils etc
• Widely used compounds such as cleaners, catalytic
  converters and added to paint for color.

14
Boron Family (family 13) BLUE and PURPLE

• Valence of 3 electrons. B metalloid, Al most
  abundant metal and is the 3rd most abundant
  element in the Earths crust.
• Carbon Family ( family 14) GREEN, BLUE, PURPLE
• Valence of 4 electrons, Carbon is basis of life
  and makes carbon compounds like sugars and
  starches
• Si (metalloid) is 2nd most abundant element in
  Earths crust, used for glass, cement and
  electronics

15
Nitrogen Family (family 15) GREEN, BLUE, and
PURPLE

• Valence of 5 electrons. N makes up 78 of the
  atmosphere. Stable and not easily bonded with
  others. Used for fertilizers, explosives,
  medicines, and dyes.
• Oxygen Family (family 16) GREEN and BLUE
• Valence of 6 electrons. O is most abundant
  element in Earths crust, 2nd most abundant in
  atmosphere. O will combine with almost every
  other element. O3 is ozone( protective layer of
  atmosphere)

16
Halogen Family (family 17) PEACH

• Valence of 7 electrons, family of poisonous
  non-metals, very reactive, never found in their
  pure form. Reactivity decreases as atomic number
  increases.
• Poor conductors of electricity. Will combine
  with alkali metals to form a family of salts

17
Halogens cont

• Uses F added to toothpaste and water to prevent
  tooth decay. Will combine to form nuclear fuel.
  Cl used in bleach and salts. Br is a gasoline
  additive, photo developer, fire retardant, kills
  germs in water. I added to salts to reduce
  thyroid disease, film developer disinfectant. At
  is very rare and radioactive with no uses

18
Noble Gases (family 18) YELLOW

• Valence of 8 electrons, all are colorless,
  odorless, and tasteless gases.
• Extremely un-reactive. He, Ne, Ar will not
  combine with other elements. Xe, Kr, Rn will
  combine, but its difficult.
• When electric current is passed through Neon it
  glows.
• He is lighter than air and floats.