Chemistry Chapter 2: The Periodic Table (2 Stars)

Question 1

The Periodic Table of the Elements organizes the elements according to their _______ and reveals a pattern of similar chemical and physical properties among elements.

Answer 1

atomic numbers

Question 2

Rows are called ______ and are based on the same principal energy level, n.

Answer 2

periods

Question 3

______ are called groups. Elements in the same group have the same valence shell electron configuration.

Answer 3

Columns

Question 4

_____ are shiny (lustrous), conduct electricity well, and are malleable and ductile. Found on left side and middle of the periodic table.

Answer 4

Metals

Question 5

_______ are dull, poor conductors of electricity, and are brittle. Right side of the periodic table.

Answer 5

Nonmetals

Question 6

______ possess characteristics of both metals and nonmetals and are found in a stair-step pattern starting with boron (B).

Answer 6

Metalloids

Question 7

Effective nuclear charge (Zeff) is the net _____ charge experienced by electrons in the valence shell and forms the foundation for all periodic trends.

Answer 7

positive

Question 8

Zeff increases from ___to ____ across a period, with little change in value from top to bottom in a group.

Answer 8

left to right

Question 9

Valence electrons become increasingly separated from the nucleus as the principal energy level, n, increases from ___ to ____ in a group.

Answer 9

top to bottom

Question 10

Atomic radius _____ from left to right across a period and increases from top to bottom in a group.

Answer 10

decreases

Question 11

_____ is the size of a charged species.

Answer 11

Ionic radius

The largest nonmetallic ionic radii and the smallest metallic ionic radii exist at the metalloid boundary.

Question 12

______ are generally smaller than their corresponding neutral atom.

Answer 12

Cations

Question 13

______ are generally larger than their corresponding neutral atom.

Answer 13

Anions

Question 14

Ionization energy is the amount of energy necessary to ______ 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 in a group.

Answer 14

remove

Question 15

______ 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.

Answer 15

Electron affinity

Question 16

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

Answer 16

nucleus

Question 17

______ typically take on an oxidation state of +1 and prefer to lose an electron to achieve a noble gas-like configuration; they and the alkaline earth metals are the most reactive of all metals.

Answer 17

Alkali metals

Question 18

Alkaline earth metals take on an oxidation state of ____and can lose two electrons to achieve noble gas-like configurations.

Answer 18

+2

Question 19

______ take on oxidation states of –2 or +6 (depending on whether they are nonmetals or metals, respectively) in order to achieve noble gas configuration. They are very biologically important.

Answer 19

Chalcogens

Question 20

_____ typically take on an oxidation state of –1 and prefer to gain an electron to achieve noble gas-like configurations; these nonmetals have the highest electronegativities.

Answer 20

Halogens

Question 21

_______ have a fully filled valence shell in their standard state and prefer not to give up or take on additional electrons;

Answer 21

Noble gases
They have very high ionization energies and (for He, Ne, and Ar), virtually nonexistent electronegativities and electron affinities.

Question 22

________are unique because they take on multiple oxidation states, which explains their ability to form colorful complexes with nonmetals in solution and their utility in certain biological systems

Answer 22

Transition metals