UNENE Chemistry Primer · 2020-03-19 · UNENE Chemistry Primer Lecture 1: Atoms, Molecules and...
Transcript of UNENE Chemistry Primer · 2020-03-19 · UNENE Chemistry Primer Lecture 1: Atoms, Molecules and...
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UNENE Chemistry Primer
Lecture 1:
Atoms, Molecules and Ions
Derek Lister & William Cook
University of New Brunswick
Course Textbook:
Chemistry, The Central Science, 10th edition, Pearson Education Inc., 2006
Theodore L. Brown, H. Eugene LeMay Jr. and Bruce E. Bursten
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To understand chemistry, we have to know how matter
(i.e., solids, liquids and gases) is constructed and
how the fundamental building blocks of matter (i.e.,
atoms and molecules) interact.
Essentially, we must understand the behaviour of
electrons in matter.
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Atomic Theory of Matter
The theory that atoms
are the fundamental
building blocks of
matter reemerged in
the early 19th century,
championed by John
Dalton.
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Dalton’s Postulates
• Each element is composed of extremely small
particles called atoms.
• All atoms of a given element are identical to one
another in mass and other properties, but the
atoms of one element are different from the atoms
of all other elements.
• Atoms of an element are not changed into atoms of
a different element by chemical reactions; atoms
are neither created nor destroyed in chemical
reactions.
• Compounds are formed when atoms of more than
one element combine; a given compound always
has the same relative number and kind of atoms.
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Law of Conservation of Mass
The total mass of substances present at the end of a
chemical process is the same as the mass of
substances present before the process took place.
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The Electron
• Streams of negatively charged particles were found to
emanate from cathode tubes.
• J. J. Thompson is credited with their discovery (1897).
• Thompson measured the charge/mass ratio of the
electron to be 1.76 x 108 coulombs/g.
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Millikan Oil Drop Experiment
Once the charge/mass
ratio of the electron
was known,
determination of either
the charge or the mass
of an electron would
yield the other.
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Millikan Oil Drop Experiment
Robert Millikan
(University of Chicago)
determined the charge
on the electron in
1909.
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Radioactivity:
• The spontaneous emission of radiation by an atom.
• First observed by Henri Becquerel.
• Also studied by Marie and Pierre Curie.
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Radioactivity
• Three types of radiation were discovered by
Ernest Rutherford:
particles
particles
rays
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The Atom, circa 1900:
• “Plum pudding” model,
put forward by
Thompson.
• Positive sphere of matter
with negative electrons
imbedded in it.
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Discovery of the Nucleus
Ernest Rutherford
shot α-particles at a
thin sheet of gold foil
and observed the
pattern of scatter of
the particles.
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The Nuclear Atom
Since some particles
were deflected at large
angles, Thompson’s
model could not be
correct.
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The Nuclear Atom
• Rutherford postulated a very small, dense nucleus with the electrons around the outside of the atom.
• Most of the volume of the atom is empty space.
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Other Subatomic Particles
• Protons were discovered by Rutherford in 1919.
• Neutrons were discovered by James Chadwick in
1932.
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Subatomic Particles
• Protons and electrons are the only particles that have a
charge.
• Protons and neutrons have essentially the same mass.
• The mass of an electron is so small we ignore it.
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Symbols of Elements
Elements are symbolized by one or two letters.
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Atomic Number
All atoms of the same element have the same
number of protons: the atomic number (Z).
Note that Z for an ion does not indicate the number of
electrons (positive ions have a dearth of electrons,
negative ions have an excess).
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Atomic Mass
The mass of an atom in atomic mass units (amu) is
the total number of protons and neutrons in the atom.
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Isotopes:
• Atoms of the same element with different masses.
• Isotopes have different numbers of neutrons.
11
6 C 12
6 C 13
6 C 14
6 C
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Isotopes of Hydrogen
• All three are isotopes of
hydrogen and have the
atomic number A = 1;
• Deuterium has a neutron in
its nucleus, still has atomic
number A = 1 but has a
mass number Z = 2. It is
stable and has about
0.015% abundance in
nature.
• Tritium has two neutrons in
its nucleus, thus: A=1; Z=3.
It is radioactive and decays
by beta particle emission.
Hydrogen
Deuterium
Tritium
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Atomic Mass
Atomic and molecular
masses can be
measured with great
accuracy with a mass
spectrometer.
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Average Mass
• Because in the real world we use large amounts of
atoms and molecules, we use average masses in
calculations.
• Average mass is calculated from the isotopes of an
element weighted by their relative abundances.
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Periodic Table:
• A systematic catalog
of elements.
• Elements are
arranged in order of
atomic number.
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Periodicity
When one looks at the chemical properties of
elements, one notices a repeating pattern of
reactivities.
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Periodic Table
• The rows on the periodic
chart are periods.
• Columns are groups.
• Elements in the same
group have similar
chemical properties.
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Groups
These five groups are known by their names.
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Periodic Table
Nonmetals are on the
right side of the periodic
table (with the
exception of H).
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Periodic Table
Metalloids border the
stair-step line (with the
exception of Al and Po).
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Periodic Table
Metals are on the left
side of the chart.
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Chemical Formulas
The subscript to the right of
the symbol of an element tells
the number of atoms of that
element in one molecule of
the compound.
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Molecular Compounds
Molecular compounds are
composed of molecules and
almost always contain only
nonmetals.
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Diatomic Molecules
These seven elements occur naturally as molecules
containing two atoms.
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Types of Formulas
• Empirical formulas give the lowest whole-number
ratio of atoms of each element in a compound.
• Molecular formulas give the exact number of atoms
of each element in a compound.
For example, the empirical formula for hydrazine
would be NH2. Its molecular formula is N2H4.
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Types of Formulas
• Structural formulas show the
order in which atoms are bonded.
• Perspective drawings also show
the three-dimensional array of
atoms in a compound.
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Ions
• When atoms lose or gain electrons, they become
ions.
• Cations are positive and are formed by elements
on the left side of the periodic chart.
• Anions are negative and are formed by elements
on the right side of the periodic chart.
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Mnemonic
Cations are so-called because they seek out the
negative cathode in an electrolytic cell (i.e., they are
positive).
Anions are so-called because they seek out the positive
anode (i.e., they are negative).
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Ionic Bonds
Ionic compounds (such as NaCl) are generally
formed between metals and nonmetals.
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Writing Formulas
• Because compounds are electrically neutral, one can
determine the formula of a compound this way:
• The charge on the cation becomes the subscript
on the anion.
• The charge on the anion becomes the subscript
on the cation.
• If these subscripts are not in the lowest whole-
number ratio, divide them by the greatest common
factor.
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Common Cations
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Common Anions
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Inorganic Nomenclature
• Write the name of the cation.
• If the anion is an element, change its ending to -ide; if
the anion is a polyatomic ion, simply write the name
of the polyatomic ion.
• If the cation can have more than one possible
charge, write the charge as a Roman numeral in
parentheses.
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Patterns in Oxyanion Nomenclature
• The one with the second fewest oxygens ends in –ite
• ClO2− : chlorite
• The one with the second most oxygens ends in –ate
• ClO3− : chlorate
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Patterns in Oxyanion Nomenclature
• When there are two oxyanions involving the same
element:
• The one with fewer oxygens ends in -ite
• NO2− : nitrite; SO3
2− : sulfite
• The one with more oxygens ends in -ate
• NO3− : nitrate; SO4
2− : sulfate
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Patterns in Oxyanion Nomenclature
• The one with the fewest oxygens has the prefix hypo-
and ends in –ite
• ClO− : hypochlorite
• The one with the most oxygens has the prefix per- and
ends in –ate
• ClO4− : perchlorate
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Acid Nomenclature
• If the anion in the acid
ends in -ide, change the
ending to -ic acid and add
the prefix hydro- :
• HCl: hydrochloric acid
• HBr: hydrobromic acid
• HI: hydroiodic acid
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Acid Nomenclature
• If the anion in the acid
ends in -ite, change the
ending to -ous acid:
• HClO: hypochlorous
acid
• HClO2: chlorous acid
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Acid Nomenclature
• If the anion in the acid
ends in -ate, change the
ending to -ic acid:
• HClO3: chloric acid
• HClO4: perchloric acid
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Nomenclature of Binary Compounds
• The less electronegative atom is usually listed first.
• A prefix is used to denote the number of atoms of each element in the compound (mono- is not used on the first element listed, however.)
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Nomenclature of Binary Compounds
• The ending on the more
electronegative element is
changed to -ide.
• CO2: carbon dioxide
• CCl4: carbon tetrachloride
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Nomenclature of Binary Compounds
If the prefix ends with a or o and the name of the element begins with a vowel, the two successive vowels are often elided into one:
N2O5: dinitrogen pentoxide