Transcript Quick Atomic Structure Review

Quick Atomic
Structure Review
Review Before The Card Activity
Atomic Number
You may remember
Atomic #
Proton
Electron
Same #
But sometimes
Atomic # ≠ Electron #
(does not equal)
When an atom
becomes more positive
or negative it becomes
a charged atom, or an
ion. This occurs when
an atom gains or loses
an extra electron.
(see next slide)
Formation of Ions
Normal Sodium
Normal Chlorine
Chlorine + extra electron
Chlorine - extra electron
Atomic Mass

Atomic mass is the
weighted average of
many atoms of the
same kind (ie: carbon).
Kind of like if we took the average
mass of all students in this room.

That’s why mass
information on the
periodic table has
decimals.
Subatomic Particles in the
Nucleus
Protons
Neutrons
Same Size (1amu)
Positively Charged
Neutrally Charged
Electrons

Size: Tiny!


Charge: Negative


1876 times smaller than a proton or neutron.
But the charge is as strong as a positive
proton.
Location: Electron cloud outside of nucleus.

Location of an electron is unknown. It’s
always moving.
Card Activity


Your group will receive a
set of cards to fill out.
Let’s fill out one together.
19
20
19
1. Cross out this section. We won’t
do this.
2. Look at the information and fill
out the Bohr model.
3. Draw the electrons in each
energy level to figure out the
number of valence electrons.
4. Draw the lewis dot diagram
Card Activity
Fill out all the cards and organize them in an
explainable way.
Hint: Look for patterns.

You have _____ minutes
Do not reveal until students have
attempted to organize cards.
Remember

Opposite Charges
Attract

Alike Charges Repel
The stronger the charge, the stronger the attraction or repelling force.