Transcript Slide 1

Chemistry
Chapter 3
Atoms and Moles
Chapter 3 Atoms and Moles
Section 1 – Substances are made of atoms
The atomic Theory: states that atoms are the building blocks of all matter
What do you think an atom looks like?
Incorrect
More Accurate
Chapter 3 Atoms and Moles
Section 1 – Substances are made of atoms
The Law of Definite Proportions
states that two samples of a given compound are made of the same
elements in exactly the same proportions by mass regardless of the
sizes or sources of the samples.
Table salt (sodium chloride) is an example that shows the law of definite
proportions. Any sample of table salt consists of two elements in the
following proportions by mass:
60.66% chlorine and 39.34% sodium
Chapter 3 Atoms and Moles
Section 1 – Substances are made of atoms
The Law of Conservation of Mass
states that the mass of the reactants in a reaction equals the
mass of the products
Chapter 3 Atoms and Moles
Section 1 – Substances are made of atoms
The Law of Multiple Proportions
the law that states that when two elements combine to form two
or more compounds, the mass of one element that combines with
a given mass of the other is in the ratio of small whole numbers
Chapter 3 Atoms and Moles
Section 1 – Substances are made of atoms
Dalton’s Atomic Theory
According to Dalton, elements are composed of only one kind of
atom and compounds are made from two or more kinds of atoms.
Chapter 3 Atoms and Moles
Section 1 – Substances are made of atoms
Dalton’s atomic theory can be summarized by the following statements:
1. All matter is composed of extremely small particles called atoms,
which cannot be subdivided, created, or destroyed.
2. Atoms of a given element are identical in their physical and
chemical properties.
3. Atoms of different elements differ in their physical and chemical
properties.
4. Atoms of different elements combine in simple, whole-number
ratios to form compounds.
5. In chemical reactions, atoms are combined, separated, or rearranged
but never created, destroyed, or changed.
Chapter 3 Atoms and Moles
Section 1 – Substances are made of atoms
Because some parts of Dalton’s theory
have been shown to be incorrect, his
theory has been modified and expanded as
scientists learn more about atoms.
Chapter 3 Atoms and Moles
For Homework:
1. Do Concept Review:
Section 1 – Substances are made of atoms
2. Read Chapter 3, Section 2 - Structure of Atoms
Chapter 3 Atoms and Moles
Section 2 – Structure of Atoms
Experiments by several scientists in the mid-1800s led to the first change
to Dalton’s atomic theory.
Chapter 3 Atoms and Moles
Section 2 – Structure of Atoms
The Discovery of Electrons by J.J. Thompson
Mid 1800’s
To study current, Thomson pumped most of the air out of a glass tube.
He then applied a voltage to two metal plates, called electrodes, which
were placed at either end of the tube. One electrode, called the anode,
was attached to the positive terminal of the voltage source, so it had a
positive charge. The other electrode, called a cathode, had a negative
charge because it was attached to the negative terminal of the voltage
source.
Thomson observed a glowing beam that came out of the cathode and
struck the anode and the nearby glass walls of the tube. So, he called these
rays cathode rays.
Thomson knew the rays must have come from the atoms of the cathode
because most of the atoms in the air had been pumped out of the tube.
Thomson also observed that when a small paddle wheel was placed in
the path of the rays, the wheel would turn. This observation suggested that
the cathode rays consisted of tiny particles that were hitting the paddles
of the wheel.
Chapter 3 Atoms and Moles
Section 2 – Structure of Atoms
Thomson’s experiments showed that a cathode ray consists of particles
that have mass and a negative charge.
Chapter 3 Atoms and Moles
Section 2 – Structure of Atoms
Thomson’s experiments showed that a cathode ray consists of particles
that have mass and a negative charge. These particles are called electrons
Chapter 3 Atoms and Moles
Section 2 – Structure of Atoms
Thomson proposed that the electrons of an atom were embedded in a
Positively charged ball of matter. His picture of an atom, which is shown
in was named the plum-pudding model
Chapter 3 Atoms and Moles
Section 2 – Structure of Atoms
The Discovery of Nucleus by Ernest Rutherford
1909
Rutherford’s team of researchers carried out the experiment where a
beam of small, positively charged particles, called alpha particles,
was directed at a thin gold foil. The team measured the angles at which
the particles were deflected from their former straight-line paths as they
came out of the foil.
Rutherford found that most of the alpha particles shot at the foil passed
straight through the foil. But a very small number of particles were
deflected, in some cases backward.
He went on to reason that only a very concentrated positive charge in a
tiny space within the gold atom could possibly repel the fast-moving,
positively charged alpha particles enough to reverse the alpha particles’
direction of travel.
Rutherford also hypothesized that the mass of this positive-charge
containing region, called the nucleus, must be larger than the mass of the
alpha particle.
Chapter 3 Atoms and Moles
Section 2 – Structure of Atoms
Chapter 3 Atoms and Moles
Section 2 – Structure of Atoms
This part of the model of the atom is still considered true today. The nucleus
is the dense, central portion of the atom. The nucleus has all of the
positive charge, nearly all of the mass, but only a very small fraction of
The volume of the atom.
Chapter 3 Atoms and Moles
Section 2 – Structure of Atoms
By measuring the numbers of alpha particles that were deflected and the
angles of deflection, scientists calculated the radius of the nucleus to be
less than 1/10,000 of the radius of the whole atom.
If the nucleus of an atom were the size of a marble, then the
whole atom would be about the size of a football stadium.
Chapter 3 Atoms and Moles
Section 2 – Structure of Atoms
The positively charged particles that repelled the alpha particles in
the gold foil experiments and that compose the nucleus of an atom are
called protons. The charge of a proton was calculated to be exactly equal
in magnitude but opposite in sign to the charge of an electron. Later
experiments showed that the proton’s mass is almost 2000 times the mass
of an electron.
Chapter 3 Atoms and Moles
Section 2 – Structure of Atoms
About 30 years after the discovery of the electron, Irene Joliot-Curie
Discovered that when alpha particles hit a sample of beryllium, a beam
that could go through almost anything was produced.
The British scientist James Chadwick found that this beam was not
deflected by electric or magnetic fields. He concluded that the particles
Carried no electric charge. Further investigation showed that these neutral
particles, which were named neutrons are part of all atomic nuclei
Chapter 3 Atoms and Moles
Section 2 – Structure of Atoms
All atoms consist of protons and electrons. Most atoms also have neutrons.
Protons and neutrons make up the small, dense nuclei of atoms. The
electrons occupy the space surrounding the nucleus. For example, an oxygen
atom has protons and neutrons surrounded by electrons. But that
description fits all other atoms, such as atoms of carbon, nitrogen, silver,
and gold.
Elements differ from each other in the number of protons
their atoms contain.
Chapter 3 Atoms and Moles
Section 2 – Structure of Atoms
Atomic Number and Mass Number
The number of protons that an atom has is known as the
atom’s atomic number
The mass number is equal to the total number of particles of
the nucleus, that is protons plus neutrons
Unlike the atomic number, which is the same for all atoms of an
element, mass number can vary among atoms of a single element. In
other words, all atoms of an element have the same number of
protons, but they can have different numbers of neutrons. These atoms
of the same element are called isotopes.
Chapter 3 Atoms and Moles
Section 2 – Structure of Atoms
Calculating Proton, Electron and Neutron quantity
Proton Quantity is always equal to your atomic number.
How many protons are in a silver atom?
47 protons
Which element has 25 protons in the nucleus?
Manganese
Chapter 3 Atoms and Moles
Section 2 – Structure of Atoms
Calculating Proton, Electron and Neutron quantity
Neutron Quantity is always equal to your mass – atomic number
How many neutrons in an aluminum atom that has a
mass of 27amu?
14 neutrons
What is the mass of an atom of Iron that contains 30 neutrons?
56 amu
Chapter 3 Atoms and Moles
Section 2 – Structure of Atoms
Calculating Proton, Electron and Neutron quantity
Electron Quantity using the following rules:
For neutral atom:
Electron quantity is equal to proton quantity
For positively charged atoms:
Electron quantity is equal to proton quantity
minus the charge
For negatively charged atoms:
Electron quantity is equal to proton quantity
plus the charge
Chapter 3 Atoms and Moles
Section 2 – Structure of Atoms
Calculating Proton, Electron and Neutron quantity
How many electrons are in an oxygen atom with a -2 charge?
10
How many electron in an atom of Potassium with a +1 charge?
18
What is the charge of a fluorine atom with 10 electrons?
Negative 1
What is the charge of a titanium atom with 22 electrons?
Neutral
Chapter 3 Atoms and Moles
Section 2 – Structure of Atoms
Mass
Charge
Protons
Electrons
1 amu
1+
0 amu
1-
Neutrons
1 amu
Neutral
How to display atoms with
mass and charge
Mass number
Atomic Charge
22
Na
+
10
Atomic Number
Carbon – 14 or 14C or C-14 is a carbon atom with a mass of 14amu
N-3 is a nitrogen atom with a charge of negative 3
Symbol
# of
Protons
# of Electrons
# of Neutrons
Atomic Mass
Atomic
Number
Atomic Charge
Mn
25
18
30
55
25
+7
I
53
54
74
127
53
-1
Zn
30
28
37
67
30
+2
Symbol
# of
Protons
# of
# of
Electrons Neutrons
Atomic
Mass
Atomic
Number
Atomic
Charge
Xe
54
54
77
131
54
Neutral
Sr
38
76
36
50
88
38
+2
72
10
114
190
76
+4
10
36
18
8
-2
65
29
+2
58
103
45
+3
Os
O
Cu
Rh
8
29
45
27
42
Cd
48
46
64
112
48
+2
As
33
30
42
75
33
Mg
12
10
14
26
12
+3
+2
Ca
20
21
41
20
+2
U
Fr
92
18
86
146
92
+6
87
87
136
238
223
87
0
All atoms of an element have the same atomic number and the
same number of protons. However, atoms do not necessarily
have the same number of neutrons. Atoms of the same element
that have different numbers of neutrons are called isotopes
How to calculate the average atomic mass on an element.
Use the formula below:
(mass of atom1 x % quantity1) + (mass of atom2 x % quantity2) +……..
Average Atomic Mass =
100
Average Atomic Mass = (204 x 1.4) + (206 x 24.1) + (207 x 22.1) + (208 x 52.4)
100
Answer = 207.2 amu
Sample Questions
In a sample of the element potassium, each atom has
1. 19 protons
2. 20 neutrons
3. 39 protons and neutrons
4. 39 neutrons
In a sample of neutral copper, all atoms have atomic numbers which are
1. the same and the atoms have the same number of electrons
2. the same, but the atoms have a different number of electrons
3. different, but the atoms have the same number of electrons
4. different and the atoms have a different number of electrons
What is the mass number of an atom which contains 28 protons, 28 electrons
and 34 neutrons?
1. 28
2. 56
3. 62
4. 90
Sample Questions
Which of the following atoms has the greatest nuclear charge?
1. Al
2. Ar
3. Si
4. Na
An atom of carbon-14 contains
1. 8 protons, 6 neutrons and 6 electrons
2. 6 protons, 6 neutrons and 8 electrons
3. 6 protons, 8 neutrons and 8 electrons
4. 6 protons, 8 neutrons and 6 electrons
Which particle contains the greatest number of electrons?
1. Na
2. Na+
3. F
4. F-
Sample Questions
An electron has a charge of
1. -1 and the same mass as a proton
2. +1 and the same mass as a proton
3. -1 and a smaller mass than a proton
4. +1 and a smaller mass than a proton
What is the total number of electrons in a Cr3+ ion?
1. 18
2. 21
3. 24
4. 27
A particle of matter contains six protons, seven neutrons, and six
electrons. This particle must be a
1. neutral carbon atom
2. neutral nitrogen atom
3. positively charged carbon ion
4. positively charged nitrogen ion
Sample Questions
If 75.0% of the isotopes of an element have a mass of 35.0 amu
and 25.0% of the isotopes have a mass of 37.0 amu, what is the
atomic mass of the element?
1. 35.0 amu
2. 35.5 amu
3. 36.0 amu
4. 37.0 amu
Which symbol represents an isotope of carbon?
Sample Questions
All isotopes of a given element must have the same
1. atomic mass
2. atomic number
3. mass number
4. number of neutrons
As the number of neutrons in the nucleus of a given atom of an
element increases, the atomic number of that element
1. decreases
2. increases
3. remains the same
Which symbols represent atoms that are isotopes of each other?
Chapter 3 Atoms and Moles
Section 3 Electron Configuration
Rutherford’s Model Proposed Electron Orbits
The experiments of Rutherford’s team led to the replacement of the
Plumpudding model of the atom with a nuclear model of the atom.
Rutherford suggested that electrons, like planets orbiting the sun, revolve
around the nucleus in circular or elliptical orbits.
Chapter 3 Atoms and Moles
Section 3 Electron Configuration
Bohr’s Model Confines Electrons to Energy Levels
The Rutherford model of the atom, in turn, was replaced only two
years later by a model developed by Niels Bohr, a Danish
physicist. The Bohr model describes electrons in terms of
their energy levels.
According to Bohr’s model, electrons can be only certain distances from
the nucleus. Each distance corresponds to a certain quantity of energy
that an electron can have.
Chapter 3 Atoms and Moles
Section 3 Electron Configuration
Electrons Act Like Both Particles and Waves
In 1924, Louis de Broglie pointed out that the behavior of
electrons according to Bohr’s model was similar to the behavior of
waves.
The present-day model of the atom, which takes into account both the particle
and wave properties of electrons. According to this model, electrons are
located in regions called Orbitals around a nucleus that correspond to specific
energy levels. Orbitals are regions where electrons are likely to be found.
Orbitals are sometimes called electron clouds because they do not have sharp
boundaries. When an orbital is drawn, it shows where electrons are most likely
to be. Because electrons can be in other places, the orbital has a fuzzy
boundary like a cloud.
Chapter 3 Atoms and Moles
Section 3 Electron Configuration
Electron Configurations
The arrangement of electrons in an atom is usually shown by writing
an electron configuration. Like all systems in nature, electrons in atoms
tend to assume arrangements that have the lowest possible energies. An
electron configuration of an atom shows the lowest-energy arrangement
of the electrons for the element.
Chapter 3 Atoms and Moles
Section 3 Electron Configuration
Principle Energy Levels
(electron shells)
Name
Max # of e-
1
2
2
8
3
18
4
32
5
32
6
32
7
32
Chapter 3 Atoms and Moles
Section 3 Electron Configuration
Two types of electron configuration:
Ground state: When electrons are all found in the lowest possible
principle energy levels (electron shell).
Excited state: When one or more electrons have “jumped” to a
higher principle energy level (electron shell).
Valence electrons: The electrons found in the outermost principle
energy level (electron shell)
Octet Rule: Atoms will gain or lose electrons to try to have only 8 electrons
in the last principle energy level (electron shell). Very small atoms only need 2
electrons to satisfy this rule.
Chapter 3 Atoms and Moles
Section 3 Electron Configuration
Sample Questions
Which electron configuration is correct for a sodium with a 1+ charge?
1. 2-7
2. 2-8
3. 2-8-1
4. 2-8-2
How many electrons are in an Fe2+ ion?
1. 24
2. 26
3. 28
4. 56
Chapter 3 Atoms and Moles
Section 3 Electron Configuration
Sample Questions
Which ion has the same electron configuration as an H- ion?
1. Cl2. F3. K+
4. Li+
What is the total number of electrons in the valence shell of an atom of
aluminum in the ground state?
1. 8
2. 13
3. 3
4. 10
Chapter 3 Atoms and Moles
Section 3 Electron Configuration
Sample Questions
Which element has an atom with the electron configuration 2-8-8-2?
1. Mg
2. Ni
3. Ca
4. Ge
Which set of symbols represents atoms with valence electrons in the
same electron shell?
1. Ba, Br, Bi
2. Sr, Sn, I
3. O, S, Te
4. Mn, Hg, Cu
Chapter 3 Atoms and Moles
Section 3 Electron Configuration
Sample Questions
Which symbol represents a particle that has the same total number of
electrons as S2-?
1. O22. Si
3. Se24. Ar
Which of these elements has an atom that completes the octet rule?
1. Ne
2. Cl
3. Ca
4. Na
Chapter 3 Atoms and Moles
Section 3 Electron Configuration
Ions: atoms that have lost or gained an electron
Cation: an atom that has lost at least one electron, thereby
becoming positively charged.
Anion: an atom that has gained at least one electron, thereby
becoming negatively charged.
Chapter 3 Atoms and Moles
Section 3 Electron Configuration
Sample Questions
What is the total number of valence electrons in a fluorine atom in the
ground state?
1. 5
2. 2
3. 7
4. 9
Chapter 3 Atoms and Moles
Section 3 Electron Configuration
By 1900, scientists knew that light could be thought of as moving waves
that have given frequencies, speeds, and wavelengths.
In empty space, light waves travel at 2.998 × 108 m/s. At this speed, light
waves take only 500 s to travel the 150 million kilometers between the sun
and Earth. The wavelength is the distance between two consecutive peaks
or troughs of a wave. The distance of a wavelength is usually measured in
meters. The wavelength of light can vary from 105 m to less than 10−13 m.
This broad range of wavelengths makes up the electromagnetic spectrum.
Our eyes are sensitive to only a small portion of the electromagnetic spectrum.
This sensitivity ranges from 700 nm, which is about the value of wavelengths
of red light, to 400 nm, which is about the value of wavelengths of violet light.
Chapter 3 Atoms and Moles
Section 3 Electron Configuration
Chapter 3 Atoms and Moles
Section 3 Electron Configuration
Chapter 3 Atoms and Moles
Section 3 Electron Configuration
Normally, if an electron is in a state of lowest possible energy, it is in
a ground state. If an electron gains energy, it moves to an excited state. An
electron in an excited state will release a specific quantity of energy as it
quickly “falls” back to its ground state. This energy is emitted as certain
wavelengths of light, which give each element a unique line-emission spectrum.
Chapter 3 Atoms and Moles
Section 3 Electron Configuration
Chapter 3 Atoms and Moles
Section 3 Electron Configuration
http://jersey.uoregon.edu/vlab/elements/Elements.html
Chapter 3 Atoms and Moles
Section 3 Electron Configuration
Chapter 3 Atoms and Moles
Section 3 Electron Configuration
Sample Questions
The diagram shows the characteristic spectral line patterns of four elements.
Also shown are spectral lines produced by an unknown substance. Which
pair of elements is present in the unknown?
1.
2.
3.
4.
lithium and sodium
sodium and hydrogen
lithium and helium
helium and hydrogen
Chapter 3 Atoms and Moles
Section 3 Electron Configuration
Sample Questions
The characteristic bright-line spectrum of an element is produced when
its electrons
1. form a covalent bond
2. form an ionic bond
3. move to a higher energy state
4. return to a lower energy state
When electrons in an atom in the excited state fall to lower energy levels,
energy is
1. absorbed, only
2. released, only
3. neither released nor absorbed
4. both released and absorbed
Chapter 3 Atoms and Moles
Section 3 Electron Configuration
What is the electron configuration of a sulfur atom in the ground state?
1. 2-4
2. 2-6
3. 2-8-4
4. 2-8-6
Which electron transition represents a gain of energy?
1. from 2nd to 3rd shell
2. from 2nd to 1st shell
3. from 3rd to 2nd shell
4. from 3rd to 1st shell
Chapter 3 Atoms and Moles
Section 3 Electron Configuration
Which is an electron configuration for an atom of chlorine in the excited state?
1. 2-8-7
2. 2-8-8
3. 2-8-6-1
4. 2-8-7-1
Which electron configuration represents the electrons of an atom
in an excited state?
1. 2-4
2. 2-6
3. 2-7-2
4. 2-8-2
Chapter 3 Atoms and Moles
Section 4 Counting Atoms
Obviously, atoms are so small that the gram is not a very convenient unit
for expressing their masses. Even the picogram (10−12 g) is not very useful.
A special mass unit is used to express this unit has two names—the
atomic mass unit (amu) and the Dalton (Da). In this class, atomic mass unit
will be used.
Most samples of elements have great numbers of atoms. To make working
with these numbers easier, chemists created a new unit called the mole
(mol). A is defined as the number of atoms in exactly 12 grams of
carbon-12.The mole is the SI unit for the amount of a substance.
Chemists use the mole as a counting unit, just as you use the dozen as a
counting unit. Instead of asking for 12 eggs, you ask for 1 dozen eggs.
Similarly, chemists refer to 1 mol of carbon or 2 mol of iron.
Chapter 3 Atoms and Moles
Section 4 Counting Atoms
To convert between moles and grams, chemists use the molar mass of a
substance. The gram molar mass of an element is the mass in grams of one mole
of the element. Molar mass has the unit grams per mol (g/mol). The mass in
grams of 1 mol of an element is numerically equal to the element’s atomic
mass from the periodic table in atomic mass units.
For example, the atomic mass of copper to two decimal places is 63.55 amu.
Therefore, the molar mass of copper is 63.55 g/mol. Meaning that 63.55 grams of
copper is equal to 1 mole of copper.
Chapter 3 Atoms and Moles
Section 4 Counting Atoms
Calculate the gram molar mass the following substances.
H2O
18 g/mol
Bi(ClO3)3
N2O4
459.5 g/mol
92.0 g/mol
Ca(OH)2
Hg2S2O3
74.1 g/mol
513.4 g/mol
180.0 g/mol
C6H12O6
CdO
(NH4)2Cr2O7
128.4 g/mol
252.0 g/mol
Chapter 3 Atoms and Moles
Section 4 Counting Atoms
Converting between gram molar mass and moles.
Chapter 3 Atoms and Moles
Section 4 Counting Atoms
1. How many moles in 125.0 grams of PbI2?
0.27 moles
4.4 moles
2. How many moles in 88.9 grams of Ne?
3. How many moles in 500 grams of H2O?
27.8 moles
4. What is the mass of 5.6 moles of AgBr?
5. What is the mass of 8.5 moles of MgO?
6. What is the number of grams in 0.28 moles of K2O
7. Calculate the mass of 0.058 moles of Hg2S
1051.7 grams
342.6 grams
26.4 grams
25.1 grams
Chapter 3 Atoms and Moles
Section 4 Counting Atoms
Scientists have also determined the number of particles present in 1 mol
of a substance, called Avogadro’s number One mole of pure substance
contains 6.0221367 × 1023 particles.
Avogadro’s number may be used to count any kind of particle, including
atoms and molecules. For calculations in this class ,Avogadro’s number
will be rounded to 6.022 × 1023 particles per mole.
Chapter 3 Atoms and Moles
Section 4 Counting Atoms
Chapter 3 Atoms and Moles
Homework
Pages 107-112
Due Thursday
#1-12, 15-22, 24-36, 38, 42, 43, 45
Due Friday
46a-d, 48a-d, 53a-c, 54a-c,
55a-g, 56a-b, 57
Chapter 3 Atoms and Moles
Chapter Review
Chapter 3 Atoms and Moles
Chapter Review
Chapter 3 Atoms and Moles
Chapter Review
Chapter 3 Atoms and Moles
Chapter Review
Chapter 3 Atoms and Moles
Chapter Review
Chapter 3 Atoms and Moles
Chapter Review
Chapter 3 Atoms and Moles
Chapter Review
Chapter 3 Atoms and Moles
Chapter Review
Chapter 3 Atoms and Moles
Chapter Review