Bell Work

1
Bell Work

• 1) Describe how to test palladium to see if it is
  a metal.
• 2) Think Critically If X stands for a metal, how
  can you tell from the following formulas XCl
  and XCl2 which compound contains an alkali
  metal and which contains an alkali earth metal?

2
Groups of the Periodic Table
3
Metals

• Good conductors of heat and electricity
• Solid at room temperature (except mercury)
• Reflect light (luster)
• Are malleable can be hammered or rolled into
  sheets
• Are ductile can be drawn into wires
• Because of these characteristics metals are
  suitable for use in a variety of objects

4
Metals

• Can form ionic bonds to become more stable
• They generally have 1 to 3 electrons in their
  outer energy levels which they give up to form
  positive ion

5
Alkali Metals

• The elements in Group 1 of the periodic table ?
  have 1 electron in their outer energy level
• Shiny, ductile, malleable
• Conduct heat and electricity
• Most reactive of all the metals. Why?
• Only have 1 electron in their outer energy level
  that they like to get rid of
• Dont occur in nature in their elemental form
• Form positive ions when ionic bonds are formed
• NaCl, KBr

6
Alkaline Earth Metals

• Make up Group 2 of the periodic table ? have 2
  electrons in their outer energy level
• Very reactive ? not founds as free elements in
  nature
• Form positive ions in ionic compounds
• CaF2

7
Transition Metals

• Elements in Groups 3-12
• Unlike the alkali metals and alkaline earth
  metals, transition metals are often found as
  uncombined elements. Why?
• They are more stable than the alkali metals and
  alkaline earth metals

8
Inner Transition Metals

• Elements found between Groups 3 and 4 in Periods
  6 and 7
• Usually located below the main table

9
Inner Transition Metals

• Lanthanide Series
• First row of inner transition metals atomic
  number 58-71
• Actinide Series
• Second row of inner transition metals atomic
  number
• All are radioactive and unstable
• radioactive element nucleus breaks down and
  gives off particles of energy

10
Nonmetals

• Are usually gasses or brittle solids at room
  temperature ? so they are not malleable or
  ductile
• Do not conduct heat or electricity well
• Located to the right of the stair-step line in
  Groups 14-18 (except hydrogen)
• Form ionic and covalent bonds

11
Halogens

• Very reactive in their elemental form
• Located in Group 17
• Have 7 electrons in their outer energy levels ?
  only 1 electron is needed to complete this energy
  level
• Form salts when ionic compounds are formed
• Form diatomic covalent compounds

12
Noble Gasses

• Are very stable - Why?
• Their outer energy level is full of electrons
• No naturally occurring noble gas compounds are
  known

13
Metalloids

• Can form ionic and covalent bonds
• Can have metallic and nonmetallic properties
• Known a semiconductors because some conduct
  electricity better than most nonmetals but not as
  well as some metals
• Located along the stair-step line

14
Boron Group

• Elements in Group 13
• 3 electrons in the outer shell
• Boron is a metalloid, the rest are metals

15
Carbon Group

• Elements in Group 14
• 4 electrons in the outer energy level

16
Nitrogen Group

• Elements in Group 15
• 5 electrons in the outer energy level
• Tend to share electrons to form covalent
  compounds

17
Oxygen Group

• Elements in Group 16
• 6 electrons in the outer energy level