Chemistry of Groups Flashcards

1
Q

Alkali Metals

A
  • Group IA or Group 1
  • posess most of the classical physical properties of metals
    • except densities are lower than those of other metals
  • Typically take on an oxidation state of +1 and prefer to lose an electron to achieve a noble gas like config.
  • Alkali Metals and Alkaline Earth metals are the most reactive of all metals
  • React readily with nonmetals (especially Halogens) ie: NaCl
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2
Q

Alkaline Earth metals

A
  • Group IIA or Group 2
  • take an oxidation state of +2 and can lose 2 electrons to achieve noble gas like config.
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3
Q

Chalcogens

A
  • Group VIA or Group 16
  • Oxygen is the most important element in this group
    • One of the primary constituents of water, carbohydrates and other biological molecules
  • High concentrations of many of these elements can be toxic
  • take on oxidation states of -2 (metals) or +6 (non metals) in order to achieve noble gas config.
  • Very biologically important
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4
Q

Halogens

A
  • Group VIIA or Group 17
  • typically take on an oxidation state of -1 and prefer to gain an electron to achieve noble gas like config
  • highly reactive non-metals
  • have highest electronegativities
  • F has highest electronegativity of all elements
  • Halogens are not naturally found in their elemental (neutral) state but rather as ions called halides or diatomic molecules
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5
Q

Noble Gases

A
  • Group VIIIA or Group 18
  • aka “inert gases”
  • have fully filled valence shell in their standard state and prefer not to give up or take additional electrons
  • very high ionization energies and (for He, Ne, and Ar), virtually nonexistent electronegativities and electron affinities
  • low boiling points and exist as gases at room temp
  • niche as lighting sources
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6
Q

Transition Metals (B)

A
  • Groups IB to VIIIB or Groups 3-12
  • metals
  • very hard, have high melting and boiling points
  • Unique because they take on multiple oxidation states, which explains their ability to form colorful complexes with non metals in solution and their utility in certain biological systems
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7
Q

Active Metals

A
  • Alkali Metals and Alkaline Earth Metals
  • not naturally found in their elemental (neutral) state
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8
Q

Hydrogen Complexes

A
  • solution with molecules of water
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