Download Basic atomic structure

BASIC ATOMIC
STRUCTURE
You’ll need a periodic table to
follow the lesson!
Chem-To-Go
Lesson 5
Unit 2
ANATOMY OF THE ATOM
Nucleus: dense + core near
the center of the atom
containing protons and
neutrons
Electron cloud: sparse area
with – charge surrounding
the nucleus containing
electrons
PROTON
VS
NEUTRON
VS
ELECTRON
PROTON
NEUTRON
ELECTRON
 + Charge
 Used to identify an
atom
 Equal to atomic
number
 Included in mass
number
 Same mass as a
neutron
 Change in protons
[RARE!] = change
in element name
and atomic mass
 NO Charge
 Same mass as a
proton
 Change in
neutrons =
change in atomic
mass
 - Charge
 Gives chemical
properties
 Sometimes equal
to atomic number
 Nearly no mass
 Change in
electrons=
change in charge
and stability
IMPORTANT NUMBERS
ATOMIC
NUMBER
 Displayed on the
periodic table
 Always equal to
the number of
protons
 Always used to
identify an atom
MASS
NUMBER
ATOMIC
MASS
 NOT displayed on
the periodic table
 Add the # of
protons and the #
of neutrons
 Displayed on the
periodic table
 Calculated using
abundance and
mass of each
isotope of the
element
ISOTOPIC NOTATION
Example 2
Use a periodic table to help!
Write the isotopic notation for an atom with
50 protons, 69 neutrons, and 48 electrons.
Example 1
How many protons, neutrons, and
electrons are in the sodium atom above?
Example 3
Use a periodic table to help!
Write the isotopic notation for an atom with
16 protons, 16 neutrons, and 18 electrons.