Ch 2 - The Periodic Table

Question 1

What is the difference between representative (A) elements and nonrepresentative (B) elements?

Answer 1

• A: group 1-8

- B: transition metals, lanthanide and actinide series

Question 2

What are metal characteristics?

Answer 2

• shiny (lustrous)
• conduct electricity well because they have valence electrons that can move freely
• malleable (ability to be hammered into shapes) and ductile (ability to be pulled or drawn into wires)

Question 3

What are the nonmetal characteristics?

Answer 3

• dull
• poor conductors of electricity
• brittle

Question 4

What are metalloid characteristics?

Answer 4

• characteristics of both metals and nonmetals

- found at the zig zag starting under Boron, but not aluminum and oganesson

Question 5

What are the periodic trends L–>R ?

Answer 5

• decreased atomic radius
• increased ionization energy
• increased electron affinity
• increased electronegativity

Question 6

What are the periodic trends top –> bottom?

Answer 6

• increased atomic radius
• decreased ionization energy
• decreased electron affinity
• decreased electronegativity

Question 7

What is the effective nuclear charge (Zeff) and its trend?

Answer 7

• the net positive charge experienced by electrons in the valence shell and forms the foundation for all periodic trends
• increase from left to right with little change from top to bottom
• valence electrons become increasingly separated from the nucleus as the principal energy level, n, increases from top to bottom

Question 8

What is the atomic radius? How does it compare between anions and cations?

Answer 8

• size
  + < 0 < -
  increases

Question 9

What is ionization energy?

Answer 9

• amount of energy needed to remove an electron from the valence shell of a gaseous species
• increases –> and bottom to top

Question 10

What is electron affinity?

Answer 10

• amount of energy released when a gaseous species gains an electron in its valence shell
• increases –> and bottom to top

Question 11

What is electronegativity?

Answer 11

• measure of the attractive force of the nucleus for electrons within a bond
• increases –> and bottom to top

Question 12

What are the characteristics of alkali metals?

Answer 12

• typically take on oxidation state of +1
• prefer to lose an electron to achieve a noble gas like configuration
• most reactive to metals

Question 13

What are the characteristics of alkaline earth metals?

Answer 13

• take on oxidation state of +2

- can lose 2 electrons to achieve noble gas like configuration

Question 14

What are the characteristics of chalcogens?

Answer 14

• group 16
• take on oxidation states of -2 to +6 (depending on whether nonmetals or metals) in order to achieve noble gas like configuration
• biologically important

Question 15

What are the characteristics of halogens?

Answer 15

• typically oxidation state of -1
• prefer to gain an electron to achieve noble gas like configurations
• have the highest electronegativities

Question 16

What are the characteristics of noble gases?

Answer 16

• have a fully filled valence shell in their standard state and prefer not to give up o take on additional electrons
• very high ionization energies
• virtually non existent electronegativies and electron affinities

Question 17

What are the characteristics of transition metals?

Answer 17

• unique with multiple oxidation states, which explains their ability to form colorful complexes with nonmetals in solution and their utility in certain biological systems

Question 18

When dissolved in water, which ions are most likley to form a complex ion with water?

Answer 18

transition metals

Question 19

What is an effective nuclear charge?

Answer 19

• the strength with which the protons in the nucleus can pull on electrons