Chapter 2: The Periodic Table

The periodic table is organized based on increasing atomic ________.

The periodic table is a visual representation of the periodic law, which states: the chemical and physical properties of the elements are dependent, in a periodic way, upon ________.

Groups contain elements that have the same electronic configuration in their ________ ________ and share similar chemical properties.

The electrons in the valence shell, known as the ________ ________, are the farthest away from the nucleus and have the (greatest/least?) amount of potential energy.

The Roman numeral above each group represents what?

The A elements are known as the ________________ elements and they have their valence electrons in which orbitals?

The B elements are known as the ____________________ elements and include both the ________________ elements, which have valence electrons in which subshells? They also include the ________________ and ________________ series, which have valence electrons in which subshells?

________ are found on the left side and in the middle of the table. What 4 types do they include?

Metals are ________, meaning they can be hammered into shapes. They are also ________, meaning they can be pulled or drawn into wires.

Metals have: 1. (high/low?) effective nuclear charge 2. (high/low?) electronegativity 3. (small/large?) atomic radius 4. (small/large?) ionic radius 5. (high/low?) ionization energy 6. (high/low?) electron affinity.

Many transition metals (Group B) elements have 2+ ________________ ________, which are charges when forming bonds with other atoms.

Valence electrons of metals are loosely held onto and are thus free to move, which makes metals good ________________ of electricity and heat.

Valence electrons of the active metals are found in the ____ subshell; those of the transition metals are found in the ____ and ____ subshells; and those of the lanthanide and actinide series elements are in the ____ and ____ subshells.

____________ are found predominantly on the upper right side of the periodic table. They are ____________ (texture) in the solid state and are not very lustrous, if at all.

Nonmetals have: 1. (high/low?) ionization energy 2. (high/low?) electron affinity 3. (high/low?) electronegativity 4. (small/large?) atomic radii 5. (small/large?) ionic radii They are not good conductors.

Separating the metals and nonmetals are a stair-step group of elements called the ________________, also known as semimetals. The electronegativities and ionization energies of the metalloids are inbetween metals and nonmetals.

The electrostatic attraction between the valence shell electrons and nucleus is known as ____________ ____________ ____________ - measure of net positive charge experienced by the outermost eleectrons.

Zeff (decreases/increases?) from left to right. Why?

Elements can gain/lose electrons in order to achieve a stable ____________, representative of the noble (inert) gas.

________ ________ is 1/2 the distance between centers of 2 atoms of an element

Atomic radius (increases/decreases?) from left to right. Why?

Atomic radius (increases/decreases?) going down a group. Why?

________ ________ is the radius of a monatomic ion in an ionic crystal structure

For nonmetals close to the metalloid line, they need to (gain/lose?) more e- to achieve an octet, and thus have a (smaller/larger?) ionic radius.