Classifying the Elements
Squares in the Periodic Table

P.T. displays the _____________________ and __________________ of the elements, along
with information about the structure of their atoms

The different colors of squares differentiates the groups of elements

◦
Group 1A -> _____________________
◦
Group 2A –> ____________________
◦
Group 7A-> _____________________
Electron Configuration in Groups
◦
Elements can be sorted ___________________, _________________ elements,
___________________ metals, or ________________________ metals based on their
electron configuration

Noble Gases

Group 8A



All end with an __________________ orbital
Representative Elements

Display a wide range of __________________and
___________________ properties

Some are
_____________________________________________

s & p orbitals are not ______________________
Compare the 2 below: which is a noble gas and which is a representative element?
1s2 2s2 2p6 3s2 3p6 4s2
1s22s22p63s23p4

Transition Elements
◦
Group B
◦
2 types


◦
Transition metal

Highest occupied ___________ sublevel and a nearby ______________
sublevel contains electrons

Characterized by having the ___________orbital
Inner transition metal

Highest occupied __________ sublevel and nearby ______ sublevel
generally contain electrons

Characterized by ________ orbitals that contain electrons
Blocks of Elements

P.T. can be divided into different blocks
Orange= ______ orbital
Green= _______ orbital
Purple=_______ orbital
Blue=________orbital
Periodic Trends
Trends in Atomic Size

Size is expressed as the ___________________________
 It is ______________________________ between the nuclei of 2 atoms of the same
element when the atoms are joined (picometers)
 Generally ___________________________ from moving
___________________________within a group and ___________________________
from ___________________________across the p.t.
 Group Trends in Atomic Size

Atomic radius ___________________________ as atomic number increases

As the
______________________________________________________withi
n a group, the charge on the ___________________________and the
number occupied energy levels increases.
 The ___________________________of nucleus makes ___________________________
 Periodic Trends in Atomic Size


Atomic size ___________________________ going left to right on p.t.

When # of p+ ___________________________, so does the
___________________________

An increasing nuclear charge pulls the e- in the highest occupied energy
level closer to the nucleus and the atomic size decreases
Ions
 An atom or group of atoms that has a positive or negative charge

An atom is neutral when ___________________________
 Ions form when e- are transferred between atoms


Cation= + charged ion
______________________________________________________

Anion= - charged ion
______________________________________________________
Trends in Ionization Energy
 ________________________________________________________________________
_______________________________________________________________
 1st ionization tends to ___________________________ from
___________________________within a group and ___________________________
from __________________________across a period
 Group Trends in Ionization Energy

As the size of the atom ___________________________, nuclear charge has a
___________________________ effect on the electrons in the highest occupied
energy level

___________________________is required
___________________________- from this energy level and the first
ionization energy is lower
 Periodic Trends in Ionization Energy

___________________________of representative elements tends to
___________________________ from ___________________________across a
period

This trend can be explained by the nuclear charge, which increases, and
the shielding effect, which remains constant


Making there be an increase in the attraction of the nucleus for
an e- ___________________________
Ionic Size
 During reactions, ______________________________________________________.
This can be predicted
 For metals:

Cations are ___________________________than the atoms from which they
form.

Anions are ___________________________than the atoms from which they
form

This happens b/c e- are drawn closer to nucleus so they tend to lose their
outermost energy levels
 For nonmetals:

The opposite:

Cations are ___________________________

Anions are ___________________________


This happens b/c as the number of e- increases, the attraction of
the nucleus for any 1 e- decreases
Trends in Electronegativity
 ________________________________________________________________________
_______________________________________________________________
 Generally, electronegativity ___________________________ from
___________________________ within a group.

For representative elements, the values tend to ___________________________
from ___________________________ across the period