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Chapter 12Chapter 12
Introduction to AtomsIntroduction to Atoms
Development of the Atomic Theory
Development of the Atomic Theory
Atom - the smallest particle into which an element can be divided and still be the same substance It still retains its characteristic properties
Atoms make up elements Elements combine to form compounds
Because all matter is made up of elements or compounds, atoms are considered the building blocks of matter.
Atom - the smallest particle into which an element can be divided and still be the same substance It still retains its characteristic properties
Atoms make up elements Elements combine to form compounds
Because all matter is made up of elements or compounds, atoms are considered the building blocks of matter.
Democritus Proposes the Atom
Democritus Proposes the Atom
In 440 B.C. Democritus believed that there was a point where a particle could not be divided any further. This was against popular belief held by
Aristotle He called this particle an atomos (Greek
for atom), which means indivisible He believed these particles were
constantly moving and they form different materials by joining together
In 440 B.C. Democritus believed that there was a point where a particle could not be divided any further. This was against popular belief held by
Aristotle He called this particle an atomos (Greek
for atom), which means indivisible He believed these particles were
constantly moving and they form different materials by joining together
Dalton Creates an Atomic Theory Based on
Experiments
Dalton Creates an Atomic Theory Based on
Experiments John Dalton, a British chemist,
wanted to know why elements combine in specific proportions to form compounds i.e. water (H2O) always has two hydrogen
and one oxygen atoms bound togetherHe performed experiments on
compounds and concluded that they combined in specific proportions because of atoms
John Dalton, a British chemist, wanted to know why elements combine in specific proportions to form compounds i.e. water (H2O) always has two hydrogen
and one oxygen atoms bound togetherHe performed experiments on
compounds and concluded that they combined in specific proportions because of atoms
After many experiments and observations Dalton published his atomic theory in 1803.
He stated the following: 1) All substances are made of atoms.
ATOMS Are small particles that cannot be created, divided, or destroyed
2) Atoms of the same element are exactly alike, and atoms of different elements are different
3) Atoms join with other atoms to make new substances
This was the first step in our understanding of the atom and our current atomic theory
After many experiments and observations Dalton published his atomic theory in 1803.
He stated the following: 1) All substances are made of atoms.
ATOMS Are small particles that cannot be created, divided, or destroyed
2) Atoms of the same element are exactly alike, and atoms of different elements are different
3) Atoms join with other atoms to make new substances
This was the first step in our understanding of the atom and our current atomic theory
Thomson Finds Electrons in the Atom
Thomson Finds Electrons in the Atom
In 1897, a British scientist named J. J. Thomson discovered that atoms are made of small particles. This was contrary to Daltons atomic theory
Thomson experimented with a cathod ray
He noticed that the ray was affected (bent) by a positive charge
He concluded that the ray contained negatively charged particles
In 1897, a British scientist named J. J. Thomson discovered that atoms are made of small particles. This was contrary to Daltons atomic theory
Thomson experimented with a cathod ray
He noticed that the ray was affected (bent) by a positive charge
He concluded that the ray contained negatively charged particles
These negatively charged particles are now called electrons
Thomson revised Dalton's atomic theory to include the presence of electrons even though he did not know how they were arranged in the atom
He came up with the plum pudding modelModel - is a representation of an object or
systemThomson’s model illustrated positively
charged material with negatively charged particles located throughout.
These negatively charged particles are now called electrons
Thomson revised Dalton's atomic theory to include the presence of electrons even though he did not know how they were arranged in the atom
He came up with the plum pudding modelModel - is a representation of an object or
systemThomson’s model illustrated positively
charged material with negatively charged particles located throughout.
Rutherford Opens an Atomic “Shooting Gallery”
Rutherford Opens an Atomic “Shooting Gallery”
In 1909, a former student of Thomson’s named Ernest Rutherford tested Thomson’s theory
He aimed positively charged particles, larger than protons, at gold foil
Most particles passed straight through But to Rutherford’s amazement;
Some were deflected at various angles And a few were bounced straight back
It became obvious to Rutherford that Thomson’s model was wrong
In 1909, a former student of Thomson’s named Ernest Rutherford tested Thomson’s theory
He aimed positively charged particles, larger than protons, at gold foil
Most particles passed straight through But to Rutherford’s amazement;
Some were deflected at various angles And a few were bounced straight back
It became obvious to Rutherford that Thomson’s model was wrong
Rutherford Presents a New Atomic Model
Rutherford Presents a New Atomic Model
In 1911 Rutherford revised the atomic theory
He concluded that atoms are mostly empty space with lightweight negative electrons moving around
And in the center of the atom is a tiny, extremely dense, positively charged region - Nucleus
He calculated that the diameter of the nucleus was 100,000 times smaller than
the atom itself
In 1911 Rutherford revised the atomic theory
He concluded that atoms are mostly empty space with lightweight negative electrons moving around
And in the center of the atom is a tiny, extremely dense, positively charged region - Nucleus
He calculated that the diameter of the nucleus was 100,000 times smaller than
the atom itself
Bohr States That Electrons Can Jump Between LevelsBohr States That Electrons Can Jump Between Levels
In 1913 a Danish scientist who worked with Rutherford, Niels Bohr, suggested that electrons travel around the nucleus in definite paths These paths are located at levels at certain
distances from the nucleus He also believe that electrons could jump
from one level to the next Bohr’s model was valuable in predicting
some atomic behavior, but was too simple to explain all atomic behavior
In 1913 a Danish scientist who worked with Rutherford, Niels Bohr, suggested that electrons travel around the nucleus in definite paths These paths are located at levels at certain
distances from the nucleus He also believe that electrons could jump
from one level to the next Bohr’s model was valuable in predicting
some atomic behavior, but was too simple to explain all atomic behavior
The Modern Theory: Electron Clouds Surround
the Nucleus
The Modern Theory: Electron Clouds Surround
the Nucleus Many scientists have contributed
to our current understanding of the atom
This led to the following change to the atomic theory; Electrons do not travel in definite
paths around the nucleusThe exact paths cannot be predicted
The regions around the nucleus where electrons are likely to be found are called - Electron Clouds
Many scientists have contributed to our current understanding of the atom
This led to the following change to the atomic theory; Electrons do not travel in definite
paths around the nucleusThe exact paths cannot be predicted
The regions around the nucleus where electrons are likely to be found are called - Electron Clouds
www.csmate.colostate.edu/#A1D07www.csmate.colostate.edu/#A1D07
Chapter 12 Quiz 1Chapter 12 Quiz 1 1) __________is the smallest particle into
which an element can be divided and still be that element
2) __________ is a unifying explanation for a broad range of hypothesis and observations that have been supported by testing
3) __________ are the negatively charged particles found in all atoms
4) ___________ discovered the nucleus 5) ___________ are regions where electrons
are likely to be found Bonus) __________ are atoms that have the
same number of protons, but different numbers of neutrons
1) __________is the smallest particle into which an element can be divided and still be that element
2) __________ is a unifying explanation for a broad range of hypothesis and observations that have been supported by testing
3) __________ are the negatively charged particles found in all atoms
4) ___________ discovered the nucleus 5) ___________ are regions where electrons
are likely to be found Bonus) __________ are atoms that have the
same number of protons, but different numbers of neutrons
Section 2: The AtomSection 2: The Atom
How Small Is an Atom?How Small Is an Atom? An average sized atom (i.e. aluminum)
has a diameter of 0.00000003 cm That’s three hundred millionths of a
centimeter It would take a stack of 50,000 aluminum
atoms to equal the thickness of a sheet of aluminum foil
There are 2 x 1022 atoms in one penny! 20,000,000,000,000,000,000,000 atoms That’s twenty thousand billion billion atoms That is 4,000,000,000,000 times more atoms
than people on Earth!
An average sized atom (i.e. aluminum) has a diameter of 0.00000003 cm That’s three hundred millionths of a
centimeter It would take a stack of 50,000 aluminum
atoms to equal the thickness of a sheet of aluminum foil
There are 2 x 1022 atoms in one penny! 20,000,000,000,000,000,000,000 atoms That’s twenty thousand billion billion atoms That is 4,000,000,000,000 times more atoms
than people on Earth!
What’s Inside an Atom?What’s Inside an Atom?
As tiny as an atom is, it consists of even smaller particlesProtons, Neutrons, and Electrons
Protons and Neutrons make up the nucleus, which is at the center of the atom
As tiny as an atom is, it consists of even smaller particlesProtons, Neutrons, and Electrons
Protons and Neutrons make up the nucleus, which is at the center of the atom
Protons - the positively charged particles of the nucleusAll protons are identicalEach has an approximate mass of 1.7 x
10-24 grams or 1 amu Neutrons - particles of the nucleus
that have no chargeNeutrons have a slightly greater mass
than protons The nucleus of the atom is small, but
very dense
Protons - the positively charged particles of the nucleusAll protons are identicalEach has an approximate mass of 1.7 x
10-24 grams or 1 amu Neutrons - particles of the nucleus
that have no chargeNeutrons have a slightly greater mass
than protons The nucleus of the atom is small, but
very dense
Outside the NucleusOutside the Nucleus
Electrons - negatively charged particles in atomsElectrons are found moving around
the nucleus within electron cloudsElectrons are very small in mass
compared to protons and neutrons (0.000546 amu)
It takes more than 1,800 electrons to equal the mass of one proton
Electrons - negatively charged particles in atomsElectrons are found moving around
the nucleus within electron cloudsElectrons are very small in mass
compared to protons and neutrons (0.000546 amu)
It takes more than 1,800 electrons to equal the mass of one proton
The charges of protons and electrons are opposite, but equal in strength
Therefore if there are equal amounts of protons and electrons, the overall charge of the atom is zero - neutral i.e. 10 protons - 10 electrons = 0
If the number of protons and electrons differ, the atom becomes a charged particle - Ion
Positively charged atoms are CationsNegatively charged atoms are Anions
The charges of protons and electrons are opposite, but equal in strength
Therefore if there are equal amounts of protons and electrons, the overall charge of the atom is zero - neutral i.e. 10 protons - 10 electrons = 0
If the number of protons and electrons differ, the atom becomes a charged particle - Ion
Positively charged atoms are CationsNegatively charged atoms are Anions
How Do Atoms of Different Elements Differ?
How Do Atoms of Different Elements Differ?
There are 117 different elements, each made of different atoms
The number of Protons determines the elementThis is called the Atomic number
Each element is composed of atoms with the same atomic number
There are 117 different elements, each made of different atoms
The number of Protons determines the elementThis is called the Atomic number
Each element is composed of atoms with the same atomic number
Are All Atoms of an Element the Same?Are All Atoms of an Element the Same?
Isotopes - are atoms that have the same number of protons, but have different number of neutronsAtoms that are isotopes of each other
are the same element because they have the same number of protons
Some isotopes have unstable nuclei and become radioactive
Isotopes - are atoms that have the same number of protons, but have different number of neutronsAtoms that are isotopes of each other
are the same element because they have the same number of protons
Some isotopes have unstable nuclei and become radioactive
How Can You Tell One Isotope from Another?How Can You Tell One Isotope from Another?
You can identify one isotope from another by its mass number Mass number - is the sum of the protons and
neutrons in an atom Electrons are not included in this calculation because
their mass too small to affect it
To identify a specific isotope write the name of the element followed by a hyphen and the mass number i.e. carbon - 12 (C-12) has contains 6 protons
and 6 neutron, while carbon - 13 has 6 protons and 7 neutrons
You can identify one isotope from another by its mass number Mass number - is the sum of the protons and
neutrons in an atom Electrons are not included in this calculation because
their mass too small to affect it
To identify a specific isotope write the name of the element followed by a hyphen and the mass number i.e. carbon - 12 (C-12) has contains 6 protons
and 6 neutron, while carbon - 13 has 6 protons and 7 neutrons
How Do You Calculate the Mass of an Element
How Do You Calculate the Mass of an Element
Most elements found in nature contain a mixture of different isotopes i.e. All copper is composed of copper-63 and
copper-65 atoms Atomic Mass Unit (amu) - is the
weighted average of the masses of of all naturally occurring isotopes
To calculate the amu of an element, multiple the mass of each element by its percentage of abundance (in decimal form)
Most elements found in nature contain a mixture of different isotopes i.e. All copper is composed of copper-63 and
copper-65 atoms Atomic Mass Unit (amu) - is the
weighted average of the masses of of all naturally occurring isotopes
To calculate the amu of an element, multiple the mass of each element by its percentage of abundance (in decimal form)
Copper consists of copper-63 at 69% abundance, and copper-65 at 31% abundance. What is the amu of copper?
(63 x .69) = 43.47 (65 x .31) = 20.17
63.62 amu
* So the amu of copper is 63.62 amu
Copper consists of copper-63 at 69% abundance, and copper-65 at 31% abundance. What is the amu of copper?
(63 x .69) = 43.47 (65 x .31) = 20.17
63.62 amu
* So the amu of copper is 63.62 amu
Now You Try OneNow You Try One
Chlorine consists of chlorine-35 at 76%, and chlorine-37 at 24%. What is the amu of chlorine
(35 x .76)= 26.6 (37 x .24)= 8.9
35.5 amu
Chlorine consists of chlorine-35 at 76%, and chlorine-37 at 24%. What is the amu of chlorine
(35 x .76)= 26.6 (37 x .24)= 8.9
35.5 amu
What Forces Are at Work in Atoms?
What Forces Are at Work in Atoms?
There are four basic forces at work everywhere, including in atoms.
They include: 1) Gravity - the attraction between two
objects based on their masses Because the masses of the particles in atoms is so
small, the gravity between them is small 2) Electromagnetic Force - particles of the
same charge repel, while opposite charges attract.
The electromagnetic force holds electrons around the nucleus
There are four basic forces at work everywhere, including in atoms.
They include: 1) Gravity - the attraction between two
objects based on their masses Because the masses of the particles in atoms is so
small, the gravity between them is small 2) Electromagnetic Force - particles of the
same charge repel, while opposite charges attract.
The electromagnetic force holds electrons around the nucleus
3) Strong Force - At the close distances between protons in the nucleus, the strong force is greater than the electromagnetic force between the protons
This keeps the nucleus together4) Weak Force - In certain unstable, a
neutron can change into a proton and a electron.
It is an important force in radioactive atoms
3) Strong Force - At the close distances between protons in the nucleus, the strong force is greater than the electromagnetic force between the protons
This keeps the nucleus together4) Weak Force - In certain unstable, a
neutron can change into a proton and a electron.
It is an important force in radioactive atoms