Transcript 5-2%20Using%20the%20Periodic%20Table[1]

2.2 Using the Periodic Table
 Elements can be divided into three broad classes based
on their general properties:
 metals, nonmetals and metalloids.
 Most elements are metals.
 Metals
 Are good conductors of electricity
 Are able to reflect light when cleaned or cut
 All metals, except mercury, are solid at room
temperature.
 Most metals are ductile and malleable
 Nonmetals are elements that tend to have
properties that are the opposite of metals.
 Most non metals are gasses at room temperature
 Sulfur & Phosphorous are solids at room
temperature
 Bromine is a brown liquid.
 Nonmetals are generally poor conductors of
electricity and heat.
 Solid nonmetals are brittle
 Metalloids are elements that have properties that
are similar to both metals and nonmetals.
 The behavior of metalloids is dependent on the
conditions that they are exposed to.
 The boiling points, melting points, and densities of
the metalloids vary widely.
, possesses a metallic luster, yet it is an
inefficient conductor and is brittle.
 The reactivity of the metalloids depends on the
element with which they are reacting.

 For example,
acts as a nonmetal when reacting
with sodium yet as a metal when reacting with fluorine.
 The intermediate (in between) conductivity of
metalloids means they tend to make good
semiconductors.
 Most elements are __________.
 List 3 properties of each, metals, non-metals and
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metalloids.
Give three examples of each, metals, non-metals and
metalloids.(Not in the presentation)
If they are generally poor conductors, they are
members of which group?
Are all metals solids at room temperature? Explain.
Identify the properties of each of the following:
 Niobium(Nb), Palladium(Pd), Krypton(Kr), Fluorine(F),
Silicon(Si)
 The color of the element symbol gives information on the
physical state of the element at room temperature.
 Black = solid @ room temp
 Red = Liquid@ room temp
 Blue = Gas @ room temp
 Elements printed in black, red or blue are found in
nature.
 Those printed in 0utline are not found in nature
Squares in the Periodic Table
 Background colors are used to distinguish groups of
elements.
 We now know that there are 3 major classes of
elements: __________, __________, ____________.
 We also know that there are 8 groups of elements:
__________, _________, ___________, __________,
__________, _________, ___________, ___________.
 We know that the color of the element symbols can
communicate something to us, like;
 We know that the background colors can also tell us
something, like;
 Work in pairs around your table.(2 people)
 Have one person get a computer
 While the other gets 2 copies of the handout with
instructions.
 Read through all of the instructions before beginning
the activity.
 Collect all of the data and record it on your sheet.
 You will be given 2 class periods to complete the
activity, but it will take that long so do not waste
time!
Trends in Atomic Size
 Group Trends in Atomic Size
 As one moves down a group the size of the atom’s atomic
radius increases.
 Periodic Trends in Atomic Size
 Atomic size decreases across a period from left to right.
Ions
 An ion is an atom or group of atoms that have a
positive or a negative charge.
 Ions form when electrons are transferred
between atoms.
 An ion with a positive charge is called a cation.
 Metallic elements form cations by loosing one or
more electrons
 An ion with a negative charge is called an anion.
 Nonmetallic elements form anions by gaining one
or more electrons
Trends in Ionization Energy
 Ionization energy is the energy required to remove
an electron from an atom in its gaseous state.
 First ionization energy tends to decrease from
top to bottom in a group and increase from left
to right across a period.
 The energy required to remove the first
electron is called the first ionization energy.
Trends in Ionic Size
 Cations ( pos. change) are always smaller than the
atoms from which they form.
 Anions ( neg. charge) are always larger than the atoms
from which they form.
 This change in atomic size is due to the change in the
force of attraction between the protons and between
the electrons.
 Spread out
Trends in Electronegativity
 Electronegativity is the ability of an atom of an
element to attract electrons when an element is in
a compound.
 In general, Electronegativity values decrease from
top to bottom within a group.
 For representative elements ( s- and p- block
elements), the values tend to increase from left o
right across a period.
Electron Configurations in Groups
 Elements can be sorted into
 noble gases,
 representative elements,
 transition metals, or
 inner transition metals based on their electron
configurations.
Electron Configurations in Groups
 The Noble Gasses (Group 8 A)
 The noble gasses are non metals whose s and p sublevels
of the highest occupied energy level are filled
 These gasses are also called the inert gasses because they
rarely take part in chemical reactions.
Electron Configuration in Groups
 The representative elements
occupy groups 1A through 7A in
the periodic table.
 The representative elements
display a wide range of physical
and chemical properties.
 The s and p sublevels of the
highest occupied energy level
are not filled.
 The group number equals the
number of electrons in the
highest occupied energy level
Electron Configuration in Groups
 The transition elements in the B groups separate
the A groups.
 The transition metals are one of the B Group
elements in which the highest occupied s
sublevel and a nearby d sublevel generally
contain elections
 The inner transition metals are B Group element
which have f orbitals that are occupied by
electrons.
 These elements are sometimes called the rareearth elements