The Periodic Table Test Review

Dmitri Mendeleev

Ordered the periodic table by atomic mass and predicted undiscovered elements.

Henry Mosely

Ordered the periodic table by atomic number, which is the current organization.

Groups

Vertical columns on the periodic table, also called families, correlate to valence electron number.

Periods

Horizontal rows on the periodic table, correlate to principal energy levels (rings).

Metals

Elements located on the left side of the metalloids on the periodic table.

Nonmetals

Elements located on the right side of the metalloids, except for hydrogen.

Metalloids

Elements that have properties of both metals and nonmetals, including B, Si, Ge, As, Sb, Te, Po.

Alkali Metals

Group 1 elements on the periodic table.

Alkaline Earth Metals

Group 2 elements on the periodic table.

Transition Metals

Elements found in groups 3-12 of the periodic table.

Halogens

Group 7 elements on the periodic table.

Noble Gases

Group 8 elements on the periodic table.

Representative Elements

Elements in the A column of the periodic table.

Transition Elements

Elements in the B column of the periodic table.

S Block

Groups 1-2 on the periodic table.

D Block

Groups 3-12 on the periodic table.

P Block

Groups 13-18 on the periodic table.

F Block

The two bottom rows on the periodic table, often referred to as "the moat."

Total Groups

18 groups on the periodic table.

Total Periods

7 periods on the periodic table.

Electron Configuration

The long-hand version of electron arrangement in an atom (e.g., 1s² 2s² 2p⁶).

Noble Gas Configuration

The short-hand version of electron arrangement using the nearest noble gas symbol in brackets (e.g., [Ne] 3s²).

Atomic Radius

The size of an atom, which can vary based on the number of electron shells and protons.

Ionic Radius

The size of an ion, which can differ from its parent atom based on electron loss or gain.

Ionization Energy

The energy required to remove the outermost electron from an atom.

Shielding Effect

The repulsive force on valence electrons by core electrons, affecting atomic size and ionization energy.

Effective Nuclear Charge (Zeff)

The net positive charge experienced by valence electrons, calculated as Zeff = Z - S.

Electronegativity

The ability of an atom to attract electrons to itself.

Trends in Atomic Radius

Increases down a group and decreases left to right across a period.

Trends in Ionization Energy

Decreases down a group and increases left to right across a period.

Trends in Electronegativity

Decreases down a group and increases left to right across a period.

Cations

Positively charged ions that are smaller than their neutral atoms.

1. Electronegativity is the ___________ of an atom to _____________ electrons to itself. 

ability, attract

1. Which has the larger electronegativity? why? Sr  or  Mg

Mg, protons are closer to the electrons, ie stronger hold on them, smaller atom and less orbitals