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Slide 1
Regents Chemistry Lecture Notes for Topic I The Atom
Slide 2
Elements Elements are an extremely important part of our daily
lives Each element is different and has different properties and
behaviors Since ancient times, humans have used chemical changes to
their advantage Example: processing of ores to produce metals for
ornaments and tools
Slide 3
Elements and Changes early exp. Greeks were the first to try to
explain why chemical changes occur. By 400 B.C., they had proposed
that all matter was composed of four fundamental substances: fire,
earth, water and air The next 2000 yearschemical history was
characterized by alchemy
Slide 4
Elements early pioneers Robert Boyle (1627 1691) the first
scientist to recognize the importance of careful measurements.
Defined the term element in terms of experimentation; a substance
was an element unless it could be broken down into two or more
simpler substances
Slide 5
Elements How many Presently there are 110 different elements,
of which 88 occur naturally (the rest have been made in
laboratories) The elements vary tremendously in abundance For
example, only 9 elements account for most of the compounds found in
the Earths crust See pg. 87 tables 4.1 and 4.2
Slide 6
Elements The term element can used in different ways For
example, element can mean a single atom of an element (microscopic
view) Element can also mean a sample large enough to mass on a
balance; this sample contains many atoms (macroscopic view)
Slide 7
Elements - symbols The names of chemical elements have many
sources; often from Greek, Latin or German languages Example; the
elemental name bromine comes from a Greek word meaning stench We
use abbreviations (symbols) in place of the words
Slide 8
Your Assignment Read trace elements on pg. 88 and answer the
following questions in complete sentences: Name and describe (4)
trace elements and their impacts on our bodies What is Lithium used
for? How does it affect our bodies? What did William Walsh
discover? How? Are aluminum and fluoride good for us? Why or why
not?
Slide 9
Regent Chemistry Evolution of atomic structure
Slide 10
Pre-Dalton the atom is mostly empty space and void : The
Greeks! Said matter was made up of particles from four elemental
substances : Earth, water, air and fire Daltons Postulates
(proposed 1808) 1. All elements are composed of indivisible atoms
2. All atoms of a given element are identical Early Atomic Theory
of Matter
Slide 11
Daltons Postulates 3. Atoms of different atoms are different;
that is, they have different masses 4. Compounds are formed by the
combination of atoms of different elements. Compounds are formed in
definite proportions! Early Atomic Theory of Matter
Slide 12
Law of constant composition relatives numbers/kinds of atom are
constant Law of conservation of mass total mass before = total mass
after Law of multiple proportions (video) For example... What
Daltons Law explains...
Slide 13
Same elements and mass before and after reaction
Slide 14
In the late 1890s J.J. Thomson cathode ray tube with magnetic
fields cathode ray tube Observed nature of rays is the same
regardless of identity of cathode material 1897 concluded that
cathode rays are not rays but are particles with mass Generally
accepted as the discovery of the electron -
Slide 15
J.J High voltage produces radiation within the tube know as
cathode rays Movement in tube can be seen as cathode rays cause
certain materials to fluoresce Can be deflected by magnetic
fields
Slide 16
Shortly after...William Thomson aka Lord Kelvin Concluded atom
is a large positive sphere with electrons floating around like
raisons in pudding
Slide 17
Ernest Rutherford..the famous exp. Disproved Thomsons Plum
Pudding Model How?? Alpha and Beta particle scattering experiment
(video) The famous gold foil experiment (video) Coming up
next..modern atomic structure
Slide 18
Your Assignment Write an essay using the information from this
lecture and pg 90-96 in your textbook. Your essay should be
approximately 500 words in length and compare/contrast the
contributions of JJ Thomson, Lord Kelvin and Ernest Rutherford
Slide 19
Regents Chemistry Modern Atomic Theory
Slide 20
Nucleus electrons The nucleus contains A positive charge..
Electrons surround the nucleus in a cloud
Slide 21
Modern Atomic Theory Modern atomic theory is based on two
models The Bohr Model (planetary model) The Wave Mechanical
Model
Slide 22
The Bohr Model Neils Bohr proposed a model of the atom with a
dense, positive charge in the center and electrons surrounding the
nucleus in specific orbits.. Ask me!
Slide 23
Location of electrons energy levels Electrons are in specific
levels according to the amount of energy they contain There are
maximum numbers of electrons for each level Electrons can jump from
one level to another by absorbing or emitting photons of
energy..
Slide 24
Location of electrons We can identify an elements electrons
distribution by looking at the periodic table These number describe
how many electrons are in each level
Slide 25
Jumping of Electrons Check this outwhat happens when we excite
the electrons of specific metals? Why do we see a color? Why do
different metals show different colors? Can we get any other info
from this demo?
Slide 26
Jumping levels Electrons in a non excited state are said to be
in the ground state We just observed how to excite these
electrons.. But how does this change an elements electrons
distribution Check out your PT
Slide 27
Spectral Lines When electrons are emitted or absorbed from
specific elements, we see the result in two ways.. Emission Spectra
Absorption Spectra
Slide 28
Emission and Absorption Spectra
Slide 29
The Wave Mechanical Model Most current model of electron
behavior Proposes electrons are in orbitals, which are regions of
high probability of finding an electrons Also called the electron
cloud model Why this model?because of wave behavior of
electrons
Slide 30
Classwork Read the attached article regarding protons, neutrons
and electrons. Answer the questions on the handout using this
information. Modern Atomic Theory
Slide 31
Regents Chemistry The Structure of the Atom
Slide 32
The Nucleus A dense centered nucleus contains protons and
neutrons Protons are (+) Neutrons have no charge These have a mass
of 1 amu and make up most of the mass of an atom This mass is
called an elements atomic mass
Slide 33
Subatomic Particles We measure the mass of protons and neutrons
in atomic mass units (amu) The atomic mass unit is based on 1/12
the mass of the C 12 isotope The protons define an element This is
called an elements Atomic Number
Slide 34
Isotopes WE CAN NEVER CHANGE AN ELEMENTS ATOMIC NUMBER (# p) We
does vary is an elements number of neutrons Atoms of the same
element that have different numbers of neutrons are called Isotopes
C 14 and C 12 are isotopes
Slide 35
Isotopes cont An Isotope is an atom that looses or gains
neutrons. It is thus lighter or heavier than the base atom of the
element.
Slide 36
Average Atomic Mass The atomic mass listed on the Periodic
table is actually the average of all known atomic masses for that
element How do we do thiseasy!
Slide 37
Atomic Weights and Isotopes Multiply the exact weight x %
abundance for Each isotope and then add them up!
Slide 38
Regents Chemistry Types of Matter
Slide 39
What is Matter? Matter is the stuff of which the universe is
composed Anything that has mass and occupies space is considered
matter!
Slide 40
Mixtures and Pure Substances A mixture is something that has
variable composition. Example: soil, cereal, air A pure substance
will always have the same composition. Pure substances are elements
or compounds. Example: pure water, table salt, carbon
Slide 41
Mixtures For Example: AIR Mixture of oxygen nitrogen, carbon
dioxide Argon, water, others Elements, which are pure substances
Compounds, which are pure substances
Slide 42
Elements and Compounds Pure substances have an invariable
composition and are composed of either elements or compounds.
Elements "Substances which cannot be decomposed into simpler
substances by chemical means". Compounds Can be decomposed into two
or more elements.
Slide 43
Elements Elements are the basic substances out of which all
matter is composed. Everything in the world is made up from only
110 different elements. 90% of the human body is composed of only
three elements: Oxygen, Carbon and Hydrogen Elements are known by
common names as well as by their abbreviations (symbols).
Slide 44
Compounds Compounds are substances of two or more elements
united chemically in definite proportions by mass. The observation
that the elemental composition of a pure compound is always the
same is known as the law of constant composition (or the law of
definite proportions). For Example...
Slide 45
For example, pure water is composed of the elements hydrogen
(H) and oxygen (O) at the defined ratio of 11 % hydrogen and 89 %
oxygen by mass. Good Old H 2 O Worksheet
Slide 46
Classification of Mixtures Homogeneous Mixtures are the same
throughout (a single phase). ex: table salt and water, air, brass
Heterogeneous Mixtures contain regions that have different
properties from those of other regions (more than 1 phase). ex:
sand in water, cereal Phase - area of uniform composition
Slide 47
Examples of Heterogeneous Mixtures Sand on a beach Cereal sand
in water sugar in lemonade Most of the time you can see the
different substances, hence the mixtures are said to be not well
mixed and can be separated physically
Slide 48
Examples of Homogeneous Mixtures, also called Solutions Air
Table salt in water Solution of Na 2 SO 4 You cannot see the
different substances in the mixture (solution) - can be separated
by chemical or physical means
Slide 49
Means of Separation Use a magnet - physical Ex: Iron and sand
mixture Distillation - physical Ex: salt and water mixture see
distillation apparatus Filtration - physical Ex: sand and water
mixture Electrolysis - chemical Ex: water - see video -
worksheet