2: Period Table

Question 1

periodic law

Answer 1

chemical and physical properties of the elements are dependent, in a periodic way, upon their atomic numbers

Question 2

representative elements

Answer 2

A elements which have valence electrons in orbitals of either s or p subshells

Question 3

non-representative elements

Answer 3

B elements which include transition elements and lanthanide and actinide series

• valence electrons in s and d subshells

Question 4

metals

Answer 4

• lustrous
• malleable
• ductile
• high melting points and densities
• low electronegativity… easily give up electrons
• large atomic radius, small ionic radius, low IE, low EA, low effective nuclear charge

Question 5

nonmetals

Answer 5

• high IE, EA, electronegativities
• small atomic radii, large ionic radii
• inability of nonmetals to easily give upelectrons
• upper right of periodic table

Question 6

metals, nonmetals, and metalloids on the periodic table

Answer 6

Question 7

effective nuclear charge

Answer 7

electrostatic attraction between the valence shell electrons and the nucleus… a measure of the net positive charge experienced by the outermost electrons

• increases from left to right within the same period

*somewhat mitigated by nonvalence electrons that reside closer to the nucleus

Question 8

ionization energy (IE)

Answer 8

energy required to remove an electron from a gaseous species… endothermic process

Question 9

electron affinity

Answer 9

energy dissipated by a gaseous species when it gains an electron… exothermic

*opposite of ionization energy

Question 10

electronegativity

Answer 10

measure of the attractive force that an atom will exert on an electron in a chemical bond

Question 11

alkali metals

Answer 11

• very low Zeff because only 1 loosely bound electron in their outermost shells –> lagest atomic radii
• low IE, low electron affinities, low electronegativities
• easily loose an electron to form univalent cations
• most readily react with halogens

Question 12

alkaline earth metals

Answer 12

• valence electrons easily removed to form divalent cations

Question 13

halogens

Answer 13

highly reactive nonmetals with seven valence electrons… desperate to complete octets by gaining one additional electron

• very high electronegativities and electron affinities
• especially reactive toward alkali and alkaline earth metals

Question 14

chalgogens

Answer 14

group 6A or group 16

• very important for biologica functions
  
  • ie. Oxygen
• nonmetals and metalloids
• 6 valence electrons
• small atomic radii and large ionic radii

Question 15

noble gases

Answer 15

inert gases because they have minimal chemical reactivity due to their filled valence shells…

• high IE with little or no tendency to gain or loose electrons
• low boiling points and exist as gases at room temperature

Question 16

transition elements

Answer 16

• metals with low electron affinities and low electronegativites
• good conductors due to loosely held electrons in the d-orbitals of their valence shells
• various positive oxidation states so form many different ionic compounds
  
  • either hydration complexes or with nonmetals

Question 17

subtraction frequencies

Answer 17

the reflected colors of light that are brain mises and leads us to percieve the complementary color of the frequency that was…