Transcript Coloring the Periodic Table

The Periodic Table
(Your new best friend!!)
The Periodic Table
 The Periodic Table is a list of all the known elements.
 It is organized by increasing atomic number.
 As you move from the left to the right, the elements
become less metallic with the far right side of the table
consisting of nonmetals.
The Periodic Table
 Elements in the middle of the table are called
“transition” elements because they are changed from
metallic properties to nonmetallic properties.
 Elements who touch the “zigzag” line are called
metalloids because they have both metallic and
nonmetallic properties.
Properties of Metals
Metals are good
conductors of heat and
electricity

 Metals are malleable (can
be hammered into thin
sheets)
 Metals are ductile (can be
pulled into wires)
Metals have luster (shiny)
Examples of Metals
Potassium, K
reacts with
water and
must be
stored in
kerosene or
oil
Copper, Cu, is a relatively soft
metal, and a very good electrical
conductor.
Zinc, Zn, is more
stable than
potassium
Mercury, Hg, is the only
metal that exists as a liquid
at room temperature
Properties of Nonmetals
Carbon, the graphite in “pencil lead” is a
great example of a nonmetallic element.
 Nonmetals are poor conductors of
heat and
electricity
 Nonmetals tend to be brittle
 Nonmetals do not have luster
 Many nonmetals are gases at room
temperature
Examples of Nonmetals
Sulfur, S, was once
known as “brimstone”
Graphite is not the only pure
form of carbon, C. Diamond
is also carbon; the color
comes from impurities
caught within the crystal
structure
Microspheres
of phosphorus,
P, a reactive
nonmetal
Properties of Metalloids
Metalloids straddle
the border between
metals and
nonmetals on the
periodic table.
 They
have properties of both metals and
nonmetals.
Metalloids are more brittle than metals, less
brittle than most nonmetallic solids
 Metalloids are semiconductors of electricity
 Some metalloids possess metallic luster
Silicon, Si – A Metalloid
 Silicon has metallic luster
 Silicon is brittle like a nonmetal
 Silicon is a semiconductor of
electricity
Other metalloids include:
 Boron, B
 Germanium, Ge
 Arsenic, As
 Antimony, Sb
 Tellurium, Te
Period
Group or Family
The Periodic Table
Group or
family
Period
Families on the Periodic Table
 The table is arranged in vertical columns called
“groups” or “families”
 The horizontal rows are called “periods.”
 Elements in each vertical column or group have similar
properties
Families on the Periodic Table
 Elements on the periodic table can be grouped into
families bases on their chemical properties.
 Each family has a specific name to differentiate it
from the other families in the periodic table.
 Elements in each family
react differently with
other elements.
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
Image: http://www.learner.org/interactives/periodic/groups2.html
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, silvery-white,
or gray metals.
 Top row are
lanthanides
 Bottom row are
actinides
Period
Group or Family
The Periodic Table
Group or
family
Period
Describe how to read the periodic
table:
 Every table has:
Describe how to read the periodic
table:
Atomic Symbol:
 One or two letters chosen to represent an element.
 These symbols are used every where in the world
 Usually, abbreviation of the element or the abbreviated
Latin name of the element.
Describe how to read the periodic
table:
Atomic Number
The number of protons in an atom identifies the
element.
Describe how to read the periodic
table:
Atomic Mass:
 The average mass of an element
 Measured in atomic mass units ("amu”)
 Is an average of all the isotopes of an element.
Mass Number:
 protons + neutrons = Mass Number
 Is always a whole number.
What are the 3 major parts of an atom?
 Proton
 Neutron
 Electron
Protons
 Positively charged particles found in the atomic
nucleus.
 Have a mass of 1 AMU
 Are made from other particles called quarks.
Neutrons
 Uncharged particles found in the atomic nucleus
 Have a mass of 1 AMU
 Made from other particles called quarks.
Electron
 Negatively charged particles that surround the atom's
nucleus.
 Have no mass??
 Determine properties of the atom.
 Chemical reactions involve sharing or exchanging
electrons.
Draw a Diagram of an Atom
A diagram showing the location of each
part of the atom.
The Quark
 One of the basic building blocks of matter
 Discovered in experiments done in the late 1960’s
 There are Three families of quarks
 Each family contains two quarks.
The Quark
 Three Families:
1. Consists of Up and Down quarks,

these quarks join together to form protons and
neutrons.
2. Consists of Strange and Charm quarks

Exist only at high energies.
3. Consists of Top and Bottom quarks

Exist only at high energies.
The Nucleus
 The central part of an atom
 Composed of protons and neutrons
 Contains most of an atom's mass
 Discovered by Ernest Rutherford in 1911.
Atomic Symbols
 Some show the mass number and atomic number
in nuclear symbol form
mass number
23 Na
atomic number
11
Isotopes
Atoms that have the same number
of protons but different numbers of
neutrons
Describe Isotope
Example:
http://education.jlab.org/glossary/isotope.html
Naturally occurring carbon consists of three isotopes,
12C, 13C, and 14C. State the number of protons,
neutrons, and electrons in each of these carbon atoms.
12C
13C
14C
6
6
6
#p+ _______
_______
_______
#no _______
_______
_______
#e- _______
_______
_______
Answers
12C
6
6
13C
6
14C
#p+ 6
6
6
#no 6
7
8
#e- 6
6
6
Some quick questions
An atom has 14 protons and 20 neutrons.
A. Its atomic number is
1) 14
2) 16
3) 34
B. Its mass number is
1) 14
2) 16
C. The element is
1) Si
2) Ca
3) 34
3) Se
D. Another isotope of this element is
1) 34X
2) 34X
3) 36X
16
14
14
7 DIATOMIC MOLECULES
• Elements that only exist
as PAIRS.
• Note: when they
combine to make
compounds, they are no
longer elements so they
are no longer in pairs!
• Hydrogen, Nitrogen,
oxygen, fluorine,
chlorine, bromine, iodine
IONS
 IONS are atoms or groups of atoms with a
positive or negative charge.
 Taking away an electron from an atom gives a
CATION with a positive charge
 Adding an electron to an atom gives an
ANION with a negative charge.
 To tell the difference between an atom and an
ion, look to see if there is a charge in the
superscript! Examples: Na+ Ca+2 I- O-2
Na Ca I
O
Forming Cations & Anions
A CATION forms
when an atom
loses one or more
electrons.
An ANION forms
when an atom
gains one or more
electrons
Mg2+
F + e- --> F-
Mg -->
+ 2 e-
PREDICTING ION CHARGES
In general
 metals (Mg) lose electrons ---> cations
 nonmetals (F) gain electrons ---> anions
Learning Check – Counting
State the number of protons, neutrons, and electrons in
each of these ions.
39 K+
16O -2
41Ca +2
19
#p+ ______
8
______
20
_______
#no ______
______
_______
#e- ______
______
_______
A diagram showing the location of each
part of the atom.