CHAPTER 2Atoms, Molecules, and Ions
History of the Atom
Democritus (400 BC)
• Proposed that matter was composed of tiny, invisible particles.
• Gr. atomos
Aristotle
• Said that all substances are composed of four elements: Earth, Wind, Fire, and Water.
John Dalton (1803 AD)• the first coherent atomic theory
• Matter is composed of small particles called atoms.
• All atoms of an element are identical.
• During chemical reactions, atoms are neither created nor destroyed, but are simply rearranged.
J.J. Thompson (1897 AD)
• Used cathode rays to calculate the atomic mass of atoms.
Cathode Ray Tube Experiment
Ernest Rutherford (1910 AD)
• alpha particles (He nuclei) were shot at a thin piece of gold foil.
• most of the particles passed through the foil with little or no deflection, some were deflected to a great degree.
Gold Foil Experiment
History400 -370 BC - Democritus thought that there
must be atoms, “invisible particles”.
384-322 BC – Aristotle refused this theory.
1700 – Isaac Newton again favored the idea of smaller invisible particles.
1800 – John Dalton formed the atomic theory.
Dalton’s Atomic Theory Elements composed of small particles called
atoms. All atoms of the same element are identical in
physical properties but different from atoms of other elements.
Atoms of one element can not change into atoms of different elements with chemical reactions.
Compounds are composed of atoms of different elements and are consistent in number and type of elements.
Dalton’s Atomic TheoryVocabulary Atom – the smallest particle of an element that
retains the chemical identity of the element.
Compound – contains atoms of two or more elements.
Conservation of matter – atoms can neither be created nor destroyed in a chemical reaction.
Continuing History1897 – J. J. Thomson – using a cathode ray determined
the presence of negative particles, electrons, and the “plum pudding” model.
1911 –Ernest Rutherford – using alpha particles through gold foil determined electrons were not evenly spaced and determined the presence of a nucleus.
1919 – Rutherford- determined the presence of protons.
1932 – James Chadwick – determined the presence of neutrons.
Modern Atomic StructureAtoms consist of subatomic particles:
Particle Charge Mass (amu)
Location
Proton Positive 1.0073 Nucleus
Neutron Neutral 1.0087 Nucleus
Electron negative 5.486 x 10-4
Electron cloud
Atomic NumberThe number of protons in an atom of an
element.
Each element has a different atomic number or number of protons.
Each element has no charge.
Each element has the same number of electrons as protons to keep neutral.
Periodic Table of Elements 1750 only 17 elements 1800 – 31 elements 1865 – 63 elements Today – 117 elements
Antoine Lavoisier – categorized elements into metals, nonmetals, gases, and earths
Dmitri Mendeleev (Russia)- 1865 – categorized 63 elements according to atomic weight along with Lothar Meyer (Germany).
Modeled chart of elements after the solitaire card game.
Arranged the elements into rows in the order of increasing mass so that elements with similar properties were in the same column like suits in the card game.
Within columns, atomic masses increased from top to bottom leading to the periodic table.
Mendeleev
Mendeleev Since many elements were still
undiscovered, he left gaps in the chart where he thought the undiscovered elements should be.
The structure of the table lead to the prediction and discovery of gallium which had similar properties as aluminum.
1913 Rutherford’s nuclear model of the atom lead to atomic numbers, verification of Mendeleev’s table.
Periodic Table Organized by increasing atomic number. Basic Info:
17 = atomic numberCl = symbol
35.453 = atomic mass
17Cl
35.453
OrganizationTable is configured into: Periods – rows on the periodic table. Groups – columns on the table with elements
in the same group having similar physical properties.
Further organized into: Metals Metalloids Nonmetals
OrganizationMetals good conductors of heat and electricity Malleable (hammered into thin sheets) Ductile (drawn into thin wires) Lustrous (shiny)
Nonmetals Poor conductors Mostly gases If metal then brittle
Metalloid Demonstrate both metal and nonmetal properties
OrganizationGroups Group 1 – Alkali metals Group 2 – Alkaline earth metals Group 7 – Halogens Group 8 – Noble gases Group B – Transition metals
OrganizationAlkali metals – very reactive with water
and oxygen. They have low densities and melting points. They all have 1 valence electron so readily give away 1 electron in s orbital.
Ex. Sodium and potassium react violently with water such that they will react with the water in human skin igniting the hydrogen molecules and burn the skin.
OrganizationAlkaline earth metals – have 2 valence
electrons. Differences in reactivity along these elements is shown by the ways they react with water. More dense and higher melting temperatures
Ex. Calcium, strontium and barium react easily with water. Magnesium reacts with hot water. Beryllium has no reaction in water.
OrganizationHalogens – highly reactive with metals. They
all have 7 valence electrons.
Nobel gases – mostly nonreactive colorless, odorless gas that give off different colors when excited.
Ex. Helium-pinkNeon-orange/redArgon-lavenderKrypton-whiteXenon-blue
Atomic & Ionic Radii Trends Columns of periodic table – radius increases
from top to bottom.
Periods of periodic table – radius decreases from left to right.
Cations have smaller radii than parent elements.
Anions have larger radii than parent elements.
MoleculeAssembly of two or more atoms tightly bound
together with no net charge.Chemical formula - representation of the number
and type of elements in a compound.H2O, CO2, CH4
Molecular formula– actual chemical formula of a molecule indicating the actual number of molecules of each atom
Empirical formula – simplified formula of a molecule indicating the smallest ratio of atoms of elements.
Writing Chemical Formulas1. Each atom (element) is represented
by it symbol.2. The number of atoms of each
element is represented by a subscript.
3. When the number of atoms is 1 then the subscript is not written and understood to be one.
Chemical FormulasExamples of formulas
Ca3(PO4)3 Al(NO3)3 H2SO4 3CO2
Diatomic moleculesMolecules that exist is pairs
Hydrogen Nitrogen Oxygen Fluorine Chlorine Bromine Iodine
IonsA charged entity produced by taking a neutral
atom and adding or removing one or more electrons.
Cation-positively charged particle due to the removal of an electron.K+ , Mg2+
Anion-negatively charged particle due to the acceptance of an electron (tend to be nonmetals).Cl- , S2-
How many electrons are contained in each of the following ions?
Ba2+
P3-
Sn2+
Cl-
Ions
There must be both positive ions (cations) and negative ions (anions) present.
The numbers of cations and anions must have a net charge of zero or the sum of the oxidation numbers is zero.
Cation is first then the anion.
Writing Formulas
Ex. Na and Cl Na+ Cl- → NaClCharge: +1 Charge: -1 Net = 0Oxidation number = charge
Ex. Mg and Cl
Mg2+ Cl - Cl- → MgCl2Charge: +2 2 x (-1) net =0
Writing Formulas
Calcium and chlorine Sodium and sulfur Lithium and nitrogen Phosphorus and Calcium Barium and oxygen Sulfur and Aluminum Potassium and phosphorus
Writing Formulas
Writing Formulas Ionic Compound – a molecule that contains both
a metal and a nonmetallic elements.NaClMgCl2
Molecular Compound – a molecule that contains only nonmetals.CO2
CH4 Polyatomic ions – atoms joined as a molecule
with a charge.
Writing Formulas
Iron (II) and chlorine Cooper (I) and fluorine Calcium and hydroxide Chromium (II) and peroxide Hydrogen and oxygen Hydrogen and phosphate
NomenclatureNaming cations: Metals with single charge – cation is
metal name with “ion” added Metal with multiple charge – cation is
metal name with charge indicated by Roman numeral and “ion” added.
Polyatomic – nonmetal name with “ium” replacing end.
NomenclatureNaming anions: Monatomic – element name with end
replaced with “ide” . Polyatomic –
With oxygen (oxyanion)– element name with end replaced with “ate”.
With hydrogen & oxyanion – polyatomic name prefix “hydrogen” added.
Nomenclature Naming ionic compounds: Cation is named
first using cation name then anion name. Naming molecular compounds:
1. Name element further to left first.2. If same group, name higher atomic number first.3. Anion is named using anion name (ide)4. Atoms are indicated by following prefixes:
One – mono six - hexa Two – di seven - hepta Three – tri eight - octa Four – tetera nine - nona Five - penta ten - deca
NomenclatureNaming acids: If anion name ends in “ide” change to
“ic” and add “hydrogen” to name. These are molecules with no oxygen.
If anion name ends in “ate” change to “ic” and add “acid”.
If anion name ends in “ite” change to “ous” and add “acid”.
Naming Flow Chart
Is it Ionic or molecular?
Ionic Molecularnonmetals
Transition metalWith multiple charges? Use prefixes to tell
number of each atom present
YesMetal – roman numeral
Nonmetal – “ide” endingOr polyatomic ion name
NoMetal – metal name
Nonmetal – “ide” endingOr polyatomic ion name
Isotopes
Radioactive Decay
C14 Decay
Carbon Dating
Carbon Dating VideoClick on the picture above to view.