Chemistry Chapter 2: The Periodic Table (2 Stars) Flashcards
The Periodic Table of the Elements organizes the elements according to their _______ and reveals a pattern of similar chemical and physical properties among elements.
atomic numbers
Rows are called ______ and are based on the same principal energy level, n.
periods
______ are called groups. Elements in the same group have the same valence shell electron configuration.
Columns
_____ are shiny (lustrous), conduct electricity well, and are malleable and ductile. Found on left side and middle of the periodic table.
Metals
_______ are dull, poor conductors of electricity, and are brittle. Right side of the periodic table.
Nonmetals
______ possess characteristics of both metals and nonmetals and are found in a stair-step pattern starting with boron (B).
Metalloids
Effective nuclear charge (Zeff) is the net _____ charge experienced by electrons in the valence shell and forms the foundation for all periodic trends.
positive
Zeff increases from ___to ____ across a period, with little change in value from top to bottom in a group.
left to right
Valence electrons become increasingly separated from the nucleus as the principal energy level, n, increases from ___ to ____ in a group.
top to bottom
Atomic radius _____ from left to right across a period and increases from top to bottom in a group.
decreases
_____ is the size of a charged species.
Ionic radius
The largest nonmetallic ionic radii and the smallest metallic ionic radii exist at the metalloid boundary.
______ are generally smaller than their corresponding neutral atom.
Cations
______ are generally larger than their corresponding neutral atom.
Anions
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.
remove
______ 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.
Electron affinity
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.
nucleus
______ 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.
Alkali metals
Alkaline earth metals take on an oxidation state of ____and can lose two electrons to achieve noble gas-like configurations.
+2
______ 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.
Chalcogens
_____ 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.
Halogens
_______ have a fully filled valence shell in their standard state and prefer not to give up or take on additional electrons;
Noble gases
They have very high ionization energies and (for He, Ne, and Ar), virtually nonexistent electronegativities and electron affinities.
________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
Transition metals
