Mendeleev summarized these observations in the periodic law:

(a)  

Mendeleev arranged the known elements in rows so that

(a)  

Mendeleev’s Periodic Table included some gaps, which

(a)  

The elements are listed in order of

(a)  

Rows on the periodic table are referred to as

(a)  

Columns in the table are referred to as

(a)  

Elements in a group or family have

(a)  

Elements in the periodic table are classified as

(a)  

The periodic table can be divided into

(a)  

Main-group elements properties tend to be

(a)  

In the periodic table, main-group elements are labeled by

(a)  

Transition elements and inner transition elements properties tend to be

(a)  

In the periodic table, transition elements and inner transition elements are labeled by a

(a)  

Quantum-mechanical theory describes the

(a)  

The electrons in atoms exist in

(a)  

A description of the orbitals occupied by electrons is called an

(a)  

The Pauli Exclusion Principle

(a)  

Aufbau Principle

(a)  

Orbitals that are in the same sublevel have the same

(a)  

There can be no more than two electrons per

(a)  

Hund’s rule

(a)  

Electrons in singly occupied orbitals spin in the

(a)  

Electron configuration that result in unpaired electrons mean that

(a)  

Electron configuration with unpaired electrons with a net magnetic field

(a)  

Paramagnetism

(a)  

Electron configurations that result in all paired electrons mean that

(a)  

Electron configurations where all electrons are paired with no magnetic field

(a)  

Diamagnetism

(a)  

The electrons in all the sublevels with the highest principal energy shell are called the

(a)  

Electrons in lower energy shells are called

(a)  

One of the most important factors in the way an atom behaves, both chemically and physically, is the

(a)  

The group number corresponds to the

(a)  

The length of each “block” is the

(a)  

The period number corresponds to the

(a)  

Transition metals (d block) and inner transition metals (f block) exhibit trends differing from those of

(a)  

Some of the transition metals have irregular electron configurations in high

(a)  

Ion formation can be predicted by

(a)  

These atoms form ions that will result in an electron configuration that is the same as that of the nearest

(a)  

Metals form

(a)  

Main group metals will lose electrons to obtain the same electron configuration as

(a)  

Transition, inner transition, and p-block form

(a)  

Nonmetals form

(a)  

Nonmetals gain electrons to obtain the

(a)  

Cations

(a)  

Anions

(a)  

Atomic radius decreases across a

(a)  

As atomic radius decreases, it adds

(a)  

As atomic radius decrease, effective nuclear charge

(a)  

As atomic radius decreases, valence shell is

(a)  

Atomic radius increase

(a)  

As atomic radius increases

(a)  

Cations are always smaller than

(a)  

Anions are always larger than

(a)  

It is the minimum energy needed to remove an electron from an atom or ion in the gas phase

(a)  

Ionization is an (a)   process

Endothermic process

(a)  

The valence electron with the lowest ionization energy is the

(a)  

First ionization energy =

(a)  

M(g)+IE1 ->

(a)  

Second IE=

(a)  

M+1(g) + IE2 ->

(a)  

First IE (a)   down the group

During the first IE, the valence electron is

(a)  

First IE generally (a)   across the period

When IE increases, effective nuclear charge

(a)  

Electron Affinity

(a)  

M(g) + 1e- ->

(a)  

Exothermic (-)

(a)  

Endothermic (+)

(a)  

Some alkaline earth metals’ and all noble gases’ electron affinities are

(a)  

The more energy that is released, the

(a)  

The more negative the number, the larger the

(a)  

General Trend for Main-Group Elements

(a)  

Halogens have the highest (a)   for any period

Moving down a group, atomic radii

(a)  

Moving down a group, ionization energy

(a)  

Moving down a group, electron affinity

(a)  

Moving across a period, atomic radii

(a)  

Moving across a period, ionization energy

(a)  

Moving across a period, electron affinity

(a)