CH 3

Question 1

Dalton

Answer 1

• hook & eye method (drove Pauling to write Nature of Chemical Bond)

Question 2

Hook & eye atomic attachment

Answer 2

Argued that atoms of solids were hooked & stuck to one another

Question 3

G.N. Lewis

Answer 3

• Used Thomson’s discovery of electron
• Recognized valence electrons fundamental to bonding
  
  • electron transfer = IONIC bond
  • sharing electrons = COVALENT bonds
  • atoms tend to acquire noble-gas electronic configs
• lewis theory & dot structure

Question 4

chemical bonds

Answer 4

the attraction between electrons of 1 atom to the nucleus of another atom

Question 5

Alkali metals

Answer 5

• group 1
• most reactive metals
• monovalent when react w/nonmetals

Question 6

halogens

Answer 6

• group 7a or 17
• most reactive nonmetals
• monovalent when react with metals

Question 7

Abegg’s law of valence

Answer 7

the diff btwn the max pos & neg valences of an element is frequently 8

Question 8

Noble gases

Answer 8

• inert (will not form compounds)
• unreactive
• no unpaired electrons

Question 9

Lewis theory

Answer 9

• emphasizes role of valences in bonding
  1. every atom has core of electrons (unchanged) that contains excess of positive charges
  2. atom has an outer shell, which, in the neutral atom, contains negative elctrons = to pos charges of core
• # of electrons in outer shell may vary during chemical change btwn 0 & 8
  3. the atom tends to hold an even # of electrons in outer shell
  4. 2 atomic shells are mutually interpenetrable (overlap). valence electrons may pass completely into another atom to form shared electron pairs
  5. electrons can readily pass from one position in outer shell to another (held by electrostatic forces)
  6. Electrostatic forces btwn electrons @ very close distances don’t obey simple law of electrostatic potential. electrons will instead follow Quantum Mechanics & may pair-up to form a bond