Atoms vs. Ions,
Valence Electrons
Topic # 1.3
GPS: 1a, 4b
Part I: Atoms vs. Ions
Date: _____/_____/_____
SPS1. Students will investigate our current understanding of the atom. a.
Examine the structure of the atom in terms of proton, electron, and neutron
locations, atomic mass and atomic number, atoms with different numbers of
neutrons (isotopes), and explain the relationship of the proton number to the
element’s identity. SPS4. Students will investigate the arrangement of the
Periodic Table. a. Determine the trends of the following: number of valence
electrons, types of ions formed by representative elements, location of metals,
nonmetals, and metalloids, and phases at room temperature. b. Use the
Periodic Table to predict the above properties for representative elements.
 atom = an __________ _______ unit of matter
atom: p+ = econtaining protons and electrons in ______ numbers.
cation: p+ > e ion = an atom that has become ______, by the _____ or
anion: p+ < e________ of electrons (never ______!).
 cation = a _______ ion, created when an atom ____ electrons.
 anion = a _______ ion, created when an atom _____ electrons.
 important to note: when an ion is created, it is because the _______ number
changes. If the _______ number were to change, the ________ itself would
change! Take a look:
sodium ____
__ protons
__ electrons
__ charge
sodium ___
__ protons
__ electrons
__ charge
chlorine ____
__ protons
__ electrons
__ charge
chlorine ___
__ protons
__ electrons
__ charge
The number of (protons, neutrons, electrons) changes when an atom becomes an ion.
When forming an ion, sodium (loses, gains) an electron, forming a (cation, anion).
Part II: Valence Electrons
 the ______ of electrons an atom has to ____ or wants to ____ depends on the
number of electrons it has on its ___________ _______ ____.
 valence electrons = an electron that is ________ to be lost or gained in the
formation of _________ __________.
 the periodic table is arranged in such a way as to show the ________
_______ in the number of valence electrons an atom has (see below).
valence
electron
number:
__
__
__
__
__
__
__
__
 only the e- on the __________ _____ ____ are counted as valence e-!
How many valence electrons does nitrogen have? _____ Argon? _____ Aluminum? _____
valence
electron
number:
1
2
3
4
5
6
7
8
 all elements want ___ valence electrons for __________ _______.
 elements in the ____ column of the periodic table, known as the _____ _____,
already have __ valence electrons, so they are very ______.
 due to this, noble gases do ___ ____ _________ with other elements.
 the reason atoms with __ -__ valence electrons form ____ is to ____ like a noble
gas on the _______ (but their _____ number does not change!).
 elements with __, __, or __ valence electrons _____
electrons to make 8:
 7 + __ = 8 (elements with 7 v.e. have a ___ charge)
 6 + __ = 8 (elements with 6 v.e. have a ___ charge)
 5 + __ = 8 (elements with 5 v.e. have a ___ charge)
When forming an ion, oxygen would gain ___ electrons since it has ___ v.e. to start with.
 elements with __, __, or __ valence electrons _____
electrons to leave 8 ________ in the next level _____:
 1 - __ = 8 (elements with 1 v.e. have a ___ charge)
 2 - __ = 8 (elements with 2 v.e. have a ___ charge)
 3 - __ = 8 (elements with 3 v.e. have a ___ charge)
When forming an ion, aluminum would lose ___ electrons since it has ___ v.e. to start with.
 elements with __ valence electrons can either ____ or ____ 4 electrons (they have
a ___ charge).
 elements in the ____ 2 and ____ 6 columns of the periodic table always have a
valence electron number equal to their ______ ______.
 elements not found in the first two or last 6 columns of the table have _______
numbers of valence electrons, so their _______ vary as well.
Ex 1:
Ex 2:
Mg
Mg
ion
S
S
ion