Bellringer 9/27
 Write the Bohr model for Calcium
Periodic Table
 Periodic Table – arrangement of elements in
order of increasing atomic number with
elements having similar properties in
vertical columns
 Groups – vertical columns
 Periods – horizontal rows
ALKALI METALS
Group 1
 Hydrogen is not a member, it is
a non-metal
 1 electron in the outer shell
 Soft and silvery metals
 Very reactive, esp. with water
 Conduct electricity
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ALKALINE EARTH METALS
Group 2
 2 electrons in the
outer shell
 White and
malleable
 Reactive, but less
than Alkali metals
 Conduct electricity
TRANSITION METALS
Groups in the middle
 Good conductors of
heat and electricity.
 Some are used for
jewelry.
 The transition metals
are able to put up to 32
electrons in their
second to last shell.
 Can bond with many
elements in a variety of
shapes.
BORON FAMILY
Group 3
 3 electrons in the
outer shell
 Most are metals
 Boron is a
metalloid
CARBON FAMILY
Group 4
 4 electrons in the
outer shell
 Contains metals,
metalloids, and a
non-metal Carbon
(C)
NITROGEN FAMILY
Group 5
 5 electrons in the
outer shell
 Can share electrons
to form compounds
 Contains metals,
metalloids, and
non-metals
OXYGEN FAMILY
Group 6
 6 electrons in the
outer shell
 Contains metals,
metalloids, and
non-metals
 Reactive
Halogens
Group 7
 7 electrons in the
outer shell
 All are non-metals
 Very reactive are
often bonded with
elements from
Group 1
Noble Gases
Group 8
 Exist as gases
 Non-metals
 8 electrons in the
outer shell = Full
 Helium (He) has only
2 electrons in the
outer shell = Full
 Not reactive with
other elements
Rare Earth Metals
 Some are
Radioactive
 The rare
earths are
silver, silverywhite, or gray
metals.
 Conduct
electricity
Groups
 Representative elements – group A elements
 Transition elements – group B elements
 Lanthanide and actinide series = inner transition
metals
Groups (reminder)
 The group = number of valence electrons that the
element has
 Valence electrons are electrons in the outermost shell
of the atom
 All group 1A elements have 1 valence electron.
Likewise, all group 8A elements have 8 valence
electrons.
Charges
 Every element wants 8 valence electrons to become stable.
They will gain or lose valence electrons to form an octet
 For example…Group 1A elements have 1 valence electron.
They can either gain 7 electrons to have an octet or lose 1.
 What is easier?
Lose 1
 If an element loses 1 electron (1 negative charge) what
charge will the resulting ion have?
+1
Oxidation numbers
 The charge an element would have if it released or
obtained electrons to look like a noble gas.
 Metals release electrons
 Nonmetals obtain electrons
Characteristics
 Elements in the same group exhibit similar chemical
characteristics due to the fact that they all have the
same number of valence electrons.
 The most stable number of valence electrons is 8
 called an octet
 Predict the oxidation numbers for the following
 A. Al
 B. Mg
 C. N
 D. Na
 E. Cl
Physical States and Classes of the
Elements
 Majority of the elements are metals.
 They occupy the entire left side and center of the
periodic table.
 Nonmetals occupy the upper-right-hand corner.
 Metalloids are located along the boundary between
metals and nonmetals
Metals
 Metals
 elements that have luster,
 conduct heat and electricity,
 and usually bend without breaking.
Transition Metals
 The elements in Groups 3 through 12 of the periodic
table are called the transition elements.
 All transition elements are metals.
 Many transition metals can have more than one charge
Inner Transition Metals
 In the periodic table, two series of elements,
atomic numbers 58-71 and 90-103, are placed
below the main body of the table.
 These elements are separated from the main table
because putting them in their proper position
would make the table very wide.
 The elements in these two series are known as the
inner transition elements.
Inner Transition Metals
 Lanthanides
 First series of inner transition element
 follow element number 57, lanthanum.
 actinides,
 2nd series of inner transition elements
 have atomic numbers ranging from 90 (thorium, Th) to
103 (lawrencium, Lr).
Non Metals
 Although the majority of the elements in the
periodic table are metals, many nonmetals are
abundant in nature
 Most nonmetals
 don’t conduct electricity,
 are much poorer conductors of heat than
metals,
 brittle when solid.
 Many are gases at room temperature; those that
are solids lack the luster of metals.
Properties of Metals and Nonmetals
Metalloids
 Metalloids
 have some chemical and physical properties of metals
and other properties of nonmetals.
 In the periodic table, the metalloids lie along the
border between metals and nonmetals.
Bellringer 9/28
 Given: iodine, helium, sulfur, or hydrogen, which is a
halogen?
Periodic Trends
 Periodic Trends are trends that occur across the
periodic table and down the periodic table
 They include:
 atomic radius,
 Ionization energy,
 electro negativity,
 metallic character
 ionic radius
Atomic Radius
Decreases
Increases


 Atomic Radius – size of the atom
Atomic radius
 The distance from the outer edge of the electron cloud
to the nucleus.
 The radius increases as the principle quantum number
increases. So elements increase going from top to
bottom.
 The period they are in increased, radius increases.
 As you move from left to right across the period things
change.
 The # of protons in the nucleus increases. This causes
the electrons to be attracted to the nucleus more and
the size of the elements decrease.
 As you move from left to right radius decreases.
 Which element in the pair is larger?
 A. Sn, Sr
 B. Cl, I
 C. S,P
 D. Ac, U
 E. Na, Rb
 F. B, Al
Determining the Atomic Radius of a Nonmetal (Chlorine)
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Determining the Atomic Radius of a Metal (Molybdenum)
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Ionization Energy
Increases
Decreases


 Ionization energy – the ability to pull off 1 electron
Ionization energy
 The energy required to remove the most loosely held
electron from an element.
 Large radii elements lose electrons easily
 Small radii elements require energy to remove
electrons.
 Metals- don’t like electrons lose them easily
 Nonmetals – like electrons, want to keep them, require
energy to remove them.

Electro negativity
 Electro negativity – the ability of an atom to
Increases
Decreases


attract another atom
Metallic Character
 Metallic character – how much like a metal the
Decreases
Increases


element is
Electron affinity
 The ability of an atom to attract electrons to itself.
 Metal = low affinity
 Nonmetals = high affinity
 Large radius = low affinity
 Small radius – high affinity
Metals and nonmetals
 Metals tend to lose electrons.
 Nonmetals tend to gain electrons.
 The goal is to get enough electrons in the outer energy
level to look like a noble gas.
 Every electron lost leaves behind a net + charge.
 Energy electron gained causes a net – charge.
 These charges effect the radius of the elements.
 Elements with charges are called ions
Ionic radius
 The more + charge an ion has the greater the ability to
attract electrons to itself and is therefore smaller.
 The more – charge an ion has the more electrons it has
pulling away from the nucleus and therefore they are
larger.
Ionic Radius
 When you talk about ionic radius, you are comparing
an atom and its ion
 When an atom has a negative charge, you have added
electrons
 Which makes it bigger
 For example, which will be larger:
 Cl or Cl-1
Ionic Radius
 When an atom has a positive charge, you have taken
away electrons
 Which makes it smaller
 For example, which will be larger:
 Na or Na+1
 Which is larger?
 A. Ca, Ca+2
 B. Cl, Cl-
 C. Br-, F D. Pb, Pb+4
Periodic Table Trends
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Ionic Radii
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