Download UNIT 4 NOTES: THE PERIODIC TABLE

UNIT 4 NOTES: THE PERIODIC TABLE
SECTION 1 : PERIODIC LAW
Periodic Law states that the properties of elements are
_________________________ functions of their ___________________
_______________________. This means when the elements are listed
according to their atomic number, the properties repeat periodically.
SECTION 2: ARRANGEMENT OF THE PERIODIC TABLE
The periodic table is arranged in order of increasing
__________________________________________________.
The location of an element can be described by indicating what vertical
____________ or horizontal __________________ it is in. The columns
and rows on the table are numbered.
1. VERTICAL COLUMNS: The vertical columns on the table are also known
as __________________ or __________________. Some of them have
specific names, such as:
Group 1: ____________________________
Group 2:_____________________________
Groups 3-11__________________________
Group 17: ____________________________
Group 18: ____________________________
Elements located in the same group on the table the same number of
_________________ _____________________.
Because of this they have the same ________________________.
There are a few exceptions (see group 18)
18
He
2
Ne
2,8
Ar
2,8,8
Kr
2,8,18,8
Xe
2,8,18
18,8
Rn
2,8,18
32,18,8
2. Horizontal Rows- The horizontal rows on the table are also known as:
_______________________________________.
Elements located in the same period have the same number of occupied
____________________________ _______________________. Another
way to say this is that they all have their _____________________
_________________ in the same __________________.
As you go across a period the number of valence electrons
___________________ and the properties of the elements also
__________________ systematically. We will look at some of these
properties later.
Section 3: Atomic Radius
Atomic radius is really the ____________ of the atom. It is defined as
____________of the distance between two adjacent nuclei. It is usually
measured in the units of ____________________. Values of atomic radii
are found in __________________.
1.
Atomic radius down a group:
As you proceed down a group atomic radius generally
_____________________. This is because as you go down you
_____________________
the
number
of
_______________
______________ _______________. More energy levels mean a
_________________ atom.
2.
Atomic radius across a period:
As you proceed across a period atomic radius generally
_____________________________. This may not make sense at first
because the atoms get more ________________ , more
________________ and a greater mass, yet they get
__________________. This is because the ___________________
____________________ of the elements are all in the same
___________________ __________________, but the number of
_______________________ in the nucleus attracting them
________________________, causing the radii to _________________.
SECTION 4: IONIC RADIUS
1. Becoming an ion: Atoms become ions either by ________________
or by losing _______________________. If you gain electrons to
become an ion you are called a _________________. If you lose
electrons to become an ion you are known as a _________________.
2. Definition of ionic radius: Ionic radius is defined at the distance from
the_______________ of an ion to the _______________________
energy level.
3. Metal ions: Metals are located to the _______________ of the stairs.
They form ions by ______________ their valence electrons.
Therefore in metals, the _________________ radius is always smaller
than the ______________ radius. Another way to say this is that the
____________ radius is always ______________ than that of the
parent atom.
4. Nonmetal ions: Nonmetals are located to the _____________ of the
stairs. Nonmetals form ions by ______________________ electrons
until they have ___________ in their valence shell.
The
___________ electrons are not as strongly attracted as the native
electrons and are located a bit ______________ from the nucleus. As
a result nonmetal ions are always _________________ than their
parent atoms. In other words, in nonmetals, the ionic radius is
____________ than the atomic radius.
SECTION 5: IONIZATION ENERGY AND ELECTRONEGATIVITY
1. ELECTRONEGATIVITY is defined as the measure of an atom’s
ability to ____________________ _______________________.
 An atom with a low Electronegativity- like ____ ________________ attract electrons well.
 An atom with a high Electronegativity- like _____________________ attract electrons well.
Electronegativity values are given in reference table _________________.
 As you proceed down
____________________.
 As you proceed across
____________________.
a
group
electronegativity
a
period
electronegativity
2. IONIZATION ENERGY is defined as the _________________ that
must be added to an atom to ________________________ it’s
outermost electron.
 An atom with a low Ionization Energy- like ______________requires _________ of energy to remove its valence electron.
 An atom with a high Ionization Energy- like ______________only requires _________________ of energy to remove its
valence electron.
Ionization energy values are given in reference table __________________.
 As you proceed down the group
_________________________.
 As you proceed across a period
________________________.
Ionization
energy
ionization
energy
SECTION 6: METALS
1. Metals are located on the periodic table to the ____________ of the
_______________.
2. Some examples of metals include ____________________ and
_______________________ and _____________________ and
________________. Even though __________________ is to the
left of the stairs it is _______________ considered a metal.
3. Metals have the following properties:
 Metals have ________________ - this means that they are
__________.
 Metals are ________________. This means they can be
______________ into shapes.
 Metals are ___________________________ conductors of heat
and electricity.
 Metals _____________ electrons easily- this indicates they
have low ________________________ _____________.
 Metals ____________ their own valence electrons and
therefore do not ________________ others. This indicates they
have low _________________________________.
 In metals, their _____________ radius is smaller than their
______________ radius
 Metals are ______________________, this means they can be
_________ into a wire.
 Most metals are _______________ at 25C or 298 K. The only
exception is _____________________, which is a
____________.
 The reactivity of metals _________________ down a group
and _______________ across a period. __________________
is the most active metal.
SECTION 7: NONMETALS
1. Nonmetals are located to the _________________ of the stairs. Even
though the Group 18 elements are to the left- they are not considered
to be ____________________.
2. Some examples of nonmetals include_______________________
and
___________________________
and
_________________________
and
_____________________________.
3. Nonmetals have the following properties:
 Nonmetals do not have ________________- they are
_______________
 Nonmetals are ___________________- they are not
_______________ or ductile.
 Nonmetals _____________ electrons in reactions and form
_______________. They have a strong ability to attract
electrons from other elements. This means they have a
_________________ ___________________________.
 In nonmetals, their _____________ radius is smaller than their
________________ radius.
 Nonmetals are _________________ conductors of heat and
electricity.
 Nonmetals have _____________ ionization energies- this
means it requires ______________ of energy to remove
electrons from them.
 Nonmetals exist as ______________ -like ___________; or as
colored ______________ - like __________________ or as a
__________________ like _________________.
 The reactivity of nonmetals ____________________ down a
group
and
________________
across
a
row.
_________________ is the most active nonmetal.
SECTION 8: SEMI-METALS OR METALLOIDS
1.
Semi-metals are located _____________ the stairs. The following
elements are metalloids:
2.
Semi-metals have properties of both ________________ and
___________________.
SECTION 9: THE GROUP 1 METALS
1. The group 1 metals are known as the ___________________ metals.
2. They have ___________ valence electron.
3. They ___________ one electron to be stable and form ions with a
_________ charge.
4. They have _______ ionization energies and _________
electronegativities.
5. They are the ___________ reactive group of metals- and are so active
they are never found in nature as _____________ only as
________________.
6. They react with water to form _____________ and a _____________.
7. As you go down the group reactivity _____________________.
8. Members include:
SECTION 10: THE GROUP 2 METALS
1. The group 2 metals are known as the ____________________
________________ metals.
2. They have ___________ valence electrons.
3. They ______________ two electrons to be stable and form ions with a
___________ charge.
4. They have _______ ionization energies and _________
electronegativities.
5. They are the ____________-___________ reactive group of metalsand are so active they are never found in nature as _____________
only as ________________.
6. They react with water to form _____________ and a _____________.
7. As you go down the group reactivity _____________________.
8. Members include:
SECTION 11: GROUPS 3-11
1. These are known as the ___________________________ metals.
2. They are __________ at reactive as other metals.
3. They form _______________ solutions when dissolved in water. For
example Cu+2 is ___________, while Fe3+ is ___________. In other
words transition elements have _______________ ions.
4. They have _____________________ positive oxidation states.
5. They can ________ electrons from their _____________________
shell and their ___________________________.
SECTION 12: GROUP 15
1. This group is composed of nonmetals, semi-metals and
_______________.
2. As you proceed down the group non-metallic character
________________ and metallic character __________________.
3. This group contains one diatomic element ________________, that is
________________ bonded to itself.
SECTION 13: GROUP 17
1. These elements are known as the _____________________.
2. The have _________ valence electron.
3. They will ______________ 1 electron to become stable and therefore
have a charge of ____________ as ions.
4. These have___________ ionization energies and electronegativities.
5. These are the _______________ reactive nonmetals and their
reactivity ________________ down a group.
6. These elements are so reactive they are not found in nature as
______________ only as __________________.
7. This is the only group on the periodic table that contains elements in
all three ____________________ of matter. Fluorine and chlorine are
________________. Bromine is a __________________ and iodine
is a ______________.
8. This group also contains four diatomic elements:
SECTION 14: THE GROUP 18 ELEMENTS
1. These elements are called the _____________________________.
2. They have _______________ valence electrons- except for _____ it
only has ____________.
3. These elements are very ________________- they have a _________
outer shell of electrons.
4. These elements do not ______________ in nature, but
_______________. ________________. And _______________ have
been forced to react with fluorine and oxygen in a lab.