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Atoms - Molecules - Ions. Molecular Basis of Substances. Substances. Compounds. Elements. Atoms. Molecules. Molecules. Ion. Ions. Periodic Table of the Elements. Hydrogen – 1 proton per atom. Carbon – 6 protons per atom. Elements.

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slide1
Atoms - Molecules - Ions

Molecular Basis of Substances

Substances

Compounds

Elements

Atoms

Molecules

Molecules

Ion

Ions

elements
Hydrogen – 1 proton per atom

Carbon – 6 protons per atom

Elements

Elements contain one or more of the same type of atom!

Examples include:

Oxygen – 8 protons per atom

Copper – 29 protons per atom

Gold – 79 protons per atom

why is the periodic table important to me
Why is the Periodic Table important to me?
  • The periodic table is the most useful tool to a chemist.
  • You get to use it on every test.
  • It organizes lots of information about all the known elements.
pre periodic table chemistry
Pre-Periodic Table Chemistry …
  • …was a mess!!!
  • No organization of elements.
  • Imagine going to a grocery store with no organization!!
  • Difficult to find information.
  • Chemistry didn’t make sense.
slide7
Here are some of the symbols Dalton used for atoms of elements and molecules of compounds. He probably used a circle for each because, like the ancient Greeks, he thought of atoms as tiny, round hard spheres.
dmitri mendeleev father of the table
HOW HIS WORKED…

Put elements in rows by increasing atomic weight.

Put elements in columns by the way they reacted.

SOME PROBLEMS…

He left blank spaces for what he said were undiscovered elements. (Turned out he was right!)

He broke the pattern of increasing atomic weight to keep similar reacting elements together.

Dmitri Mendeleev: Father of the Table
slide9
Dmitri Medeleev gave us a functional scheme with which to classify elements.
    • Mendeleev’s scheme was based on chemical properties of the elements.
    • It was noticed that the chemical properties of elements increased in a periodic manner.
    • The periodicity of the elements was demonstrated by Medeleev when he used the table to predict to occurrence and chemical properties of elements which had not yet been discovered.
slide10
Mendeleev left blank spaces in his table when the properties of the elements above and below did not seem to match. The existence of unknown elements was predicted by Mendeleev on the basis of the blank spaces. When the unknown elements were discovered, it was found that Mendeleev had closely predicted the properties of the elements as well as their discovery.
the current periodic table
The Current Periodic Table
  • Mendeleev wasn’t too far off.
  • Now the elements are put in rows by increasing ATOMIC NUMBER!!
  • The horizontal rows are called periods and are labeled from 1 to 7.
  • The vertical columns are called groups are labeled from 1 to 18.
periodic table
Non-metals

Periods

Groups

Transition metals

Metalloids

B,Si,Ge,As,Sb,Te

Metals

Periodic Table
groups here s where the periodic table gets useful
Groups…Here’s Where the Periodic Table Gets Useful!!
  • Elements in the same group have similar chemical and physical properties!!
  • (Mendeleev did that on purpose.)
  • Why??
  • They have the same number of valence electrons.
  • They will form the same kinds of ions.
families on the periodic table
Families on the Periodic Table
  • Columns are also grouped into families.
  • Families may be one column, or several columns put together.
  • Families have names rather than numbers. (Just like your family has a common last name.)
slide15
The Periodic Law
    • Similar physical and chemical properties recur periodically when the elements are listed in order of increasing atomic number.
slide16
Introduction
    • The periodic table is made up of rows of elements and columns.
    • An element is identified by its chemical symbol.
    • The number above the symbol is the atomic number
    • The number below the symbol is the rounded atomic weight of the element.
    • A row is called a period
    • A column is called a group
slide18
Periodic Patterns
    • The chemical behavior of elements is determined by its electron configuration
    • Energy levels are quantized so roughly correspond to layers of electrons around the nucleus.
    • A shell is all the electrons with the same value of n.
      • n is a row in the periodic table.
    • Each period begins with a new outer electron shell
slide19
Each period ends with a completely filled outer shell that has the maximum number of electrons for that shell.
  • The number identifying the A families identifies the number of electrons in the outer shell, except helium
  • The outer shell electrons are responsible for chemical reactions.
  • Group A elements are called representative elements
  • Group B elements are called transition elements.
slide20
Chemical “Families”
    • IA are called alkali metals because the react with water to from an alkaline solution
    • Group IIA are called the alkali earth metals because they are reactive, but not as reactive as Group IA.
      • They are also soft metals like Earth.
    • Group VIIA are the halogens
      • These need only one electron to fill their outer shell
      • They are very reactive.
    • Group VIIIA are the noble gases as they have completely filled outer shells
      • They are almost non reactive.
slide21
Four chemical families of the periodic table: the alkali metals (IA), the alkaline earth metals (IIA), halogens (VII), and the noble gases (VIIIA).
slide22
Atoms - Molecules - Ions

Metals – Nonmetals - Metalloids

Metals: A material that has a characteristic luster or shine

and that is a relatively good conductor of heat and

electricity (Metal oxides react with water to form

bases and are located on the left side of the table)

Nonmetals: A element that does not exhibit the properties

of a metal. (Nonmetal oxides react with water to

form acids and are on the right side of the table)

Metalloids: Elements with properties intermediate

between those of metals and nonmetals.

periodic table 1a
Periodic Table: 1A

Alkali metals

Very reactive

Metals never occur in nature as pure elements

hydrogen
Hydrogen
  • Hydrogen belongs to a family of its own.
  • Hydrogen is a diatomic, reactive gas.
  • Hydrogen was involved in the explosion of the Hindenberg.
  • Hydrogen is promising as an alternative fuel source for automobiles
alkali metals
Alkali Metals
  • 1st column on the periodic table (Group 1) not including hydrogen.
  • Very reactive metals, always combined with something else in nature (like in salt).
  • Soft enough to cut with a butter knife
periodic table 2a
Periodic Table: 2A

Alkaline Earth metals

alkaline earth metals
Alkaline Earth Metals
  • Second column on the periodic table. (Group 2)
  • Reactive metals that are always combined with nonmetals in nature.
  • Several of these elements are important mineral nutrients (such as Mg and Ca
boron family
Boron Family
  • Elements in group 13
  • Aluminum metal was once rare and expensive, not a “disposable metal.”
periodic table 4a
Periodic Table: 4A

allotropes of carbon

carbon family
Carbon Family
  • Elements in group 14
  • Contains elements important to life and computers.
  • Carbon is the basis for an entire branch of chemistry.
  • Silicon and Germanium are important semiconductors.
nitrogen family
Nitrogen Family
  • Elements in group 15
  • Nitrogen makes up over ¾ of the atmosphere.
  • Nitrogen and phosphorus are both important in living things.
  • Most of the world’s nitrogen is not available to living things.
  • The red stuff on the tip of matches is phosphorus.
oxygen family or chalcogens
Oxygen Family or Chalcogens
  • Elements in group 16
  • Oxygen is necessary for respiration.
  • Many things that stink, contain sulfur (rotten eggs, garlic, skunks,etc.)
periodic table 7a
Periodic Table: 7A

Halogens

Greek for “salt-forming”

Very reactive

halogens
Halogens
  • Elements in group 17
  • Very reactive, volatile, diatomic, nonmetals
  • Always found combined with other element in nature .
  • Used as disinfectants and to strengthen teeth.
the noble gases41
The Noble Gases
  • Elements in group 18
  • VERY unreactive, monatomic gases
  • Used in lighted “neon” signs
  • Used in blimps to fix the Hindenberg problem.
  • Have a full valence shell.
transition metals
Transition Metals
  • Elements in groups 3-12
  • Less reactive harder metals
  • Includes metals used in jewelry and construction.
  • Metals used “as metal.”
slide45
Names of Elements
    • The first 103 elements have internationally accepted names, which are derived from:
      • The compound or substance in which the element was discovered
      • An unusual or identifying property of the element
      • Places, cities, and countries
      • Famous scientists
      • Greek mythology
      • Astronomical objects.
slide46
What is a chemical symbol?
  • Chemical symbol tells us what atom it is
  • Always a CAPITAL LETTER, sometimes followed by a lower case letter
  • Ex: Oxygen O Nitrogen N Sodium Na
  • *Cobalt – Co *Carbon Monoxide – CO
  • (Co is an element, CO is a compound)
slide47
Chemical Symbols
    • There are about a dozen common elements that have s single capitalized letter for their symbol
    • The rest, that have permanent names have two letters.
      • the first is capitalized and the second is lower case.
    • Some elements have symbols from their Latin names.
    • Ten of the elements have symbols from their Latin or German names.
slide48
Charge (if ion)

Atomic Mass

Symbol

Atomic Number

slide49
Hydrogen

Protons: 1

Neutrons: 0

Electrons: 1

H

1

1

slide50
Sodium

Protons: 11

Neutrons: 12

Electrons: 11

Na

23

11

slide51
Rhenium

Protons: 75

Neutrons: 111

Electrons: 75

Re

186

75

slide52
Rhenium isotope

Protons: 75

Neutrons: 112

Electrons: 75

Re

187

75

slide53
133

55

EXAMPLE

How many protons, neutrons and electrons are found in an atom of

Cs

Atomic number = protons and electrons

There are 55 protons and 55 electrons

Mass number = sum of protons and neutrons

133 – 55 = 78

There are 78 neutrons

kinds of atoms
Kinds of Atoms
  • Ninety-two naturally occurring elements
    • Periodic table arranged by grouping atoms based on valence electrons (electrons in the outer energy levels).
      • Octet rule
        • Inert atoms have outer level filled.
        • Reactive atoms do not have outer level filled.
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