General Chemistry Chapter 2: The Periodic Table

Question 1

What are the rows in the periodic table called?

Answer 1

Periods

Question 2

What are the columns in the periodic table called?

Answer 2

Groups

Question 3

What do all the elements in a group have in common?

Answer 3

They all have the same valence shell electron configuration.

Question 4

What are the three types of elements on the periodic table?

Answer 4

Metals, nonmetals and metalloids

Question 5

Describe properties of metals

Answer 5

Metals are shiny (lustrous), conduct electricity well and are malleable

Question 6

Describe properties of nonmetals

Answer 6

Nonmetals are dull, poor conductors of electricity and are brittle.

Question 7

Describe properties of metalloids

Answer 7

Metalloids possess characteristics of both metals and nonmetals and are found in a stair-step pattern starting with boron.

Question 8

What is the effective nuclear charge?

Answer 8

The effective nuclear charge is the net positive charge experienced by electrons in the valence shell and forms the foundation for all other periodic trends.

Question 9

What is the trend for effective nuclear charge?

Answer 9

Zeff increases from left to right across a period with little change in the value from top to bottom in a group. Valence electrons become increasingly separated from the nucleus as the principal energy level, n, increases from top to bottom.

Question 10

What is the trend for atomic radius in a periodic table?

Answer 10

The trend is that it decreases from left to right across a period and increases from top to bottom.

Question 11

What is the trend for ionic radius?

Answer 11

Cations are smaller than their corresponding neutral atom, anions are larger than their corresponding neutral atom.

Question 12

Where do the largest nonmetallic ionic radii and the smallest metallic ionic radii exist?

Answer 12

At the metalloid boundary.

Question 13

What is the ionization energy and what is its periodic trend?

Answer 13

It is the amount of energy necessary to remove an electron from the valence shell of a gaseous species; it increases from left to right across a period and decreases from top to bottom within a group.

Question 14

What is the electron affinity and what is its periodic trend?

Answer 14

It is the amount of energy released when a gaseous species gains an electron in its valence shell; it increases from left to right across a period and decreases from top to bottom in a group.

Question 15

What is electronegativity and what is its periodic trend?

Answer 15

It is a measure of the attractive force of the nucleus for electrons within a bond; it increases from left to right across a period and decreases from top to bottom in a group.

Question 16

What are specific chemical properties of the alkali metals?

Answer 16

Oxidation state of +1
Prefer to lose an electron to achieve noble gas-like configurations
W/AEM, they are the most reactive

Question 17

What are specific chemical properties of the alkaline earth metals?

Answer 17

Oxidation state of +2
Prefer to lose 2 electrons
Highly reactive

Question 18

What are specific chemical properties of the chalcogens?

Answer 18

Oxidation states of -2 or +6

Very biologically important

Question 19

What are specific chemical properties of the noble gases?

Answer 19

fully filled valence shell in their standard state and prefer not to give up or take on additional electrons.
Very high ionization energies & virtually nonexistent electronegativities and electron affinities.

Question 20

What are the specific chemical properties of the transition metals?

Answer 20

Take on multiple oxidation states and can form colorful complexes with nonmetals in solution.