Download Unit 03 Packet - Whitwell High School

Note Taking Guide: Episode 301
Name___________________
Model: A __________ idea used to explain __________ facts __________ in
__________.
Theory: An __________ of __________ facts and __________.
To remain valid, models and theories must:
•
•
__________ all known __________
enable __________ to make correct __________
Democritus:
• proposed the __________ of an __________
• word comes from the __________ word __________ which means
__________ __________ __________ or “indivisible”
Aristotle
• __________ the __________ of the __________
• said __________ could be __________ __________
Dalton’s
•
•
•
•
•
theory proposed that atoms:
are __________ __________ of __________
are __________
of the __________ __________ are __________
of __________ __________ are __________
__________ in __________, __________ __________ ratios to form
__________
J.J. Thomson
• credited with __________ of __________: a blow to __________
__________ atom
• proposed the __________ __________ model of the __________:
__________ charged __________ embedded in a ball of __________
__________
CHEMISTRY: A Study of Matter
© 2004, GPB
3.1
Rutherford’s Gold-foil Experiment:
• aimed __________ __________ at __________ __________
• __________ passed __________
• a __________ particles were __________
• __________ particles even __________ __________
Conclusions of Rutherford's experiment:
• __________ of the __________ is __________ __________
• __________ ____________ charged __________
The Chemistry Quiz
CR1._____
CR2._____
3._____
1._____
4._____
CHEMISTRY: A Study of Matter
© 2004, GPB
3.2
2._____
5._____
Worksheet: Development of Atomic Theory
Name___________________
True-False: place a "+" in the blank if the statement is true, and a "O" in the blank
if the statement is false.
1. Dalton's atomic theory stated:
a. atoms are indivisible.
b. all atoms of the same element are alike.
c. atoms unite in small, whole number ratios
to form compounds.
_____
_____
_____
2. The Greek philosopher Democritus was one of the first
to suggest the existence of atoms.
_____
3. The word "atom" means invisible.
_____
4. A theory is an explanation of observable facts and
phenomena.
_____
5. Aristotle supported the idea of the atom.
_____
6. From the "gold-foil" experiment it was concluded that
the atom is mostly empty space.
_____
Short Answer and Fill in the Blanks:
1. What must models and theories do in order to remain valid?
a.
b.
2. The "gold-foil" experiment had the following results: ____________ of the
alpha particles were deflected, ______________ of the alpha particles
were reflected, and _____________ of the alpha particles passed through
the gold foil.
CHEMISTRY: A Study of Matter
© 2004, GPB
3.3
Note Taking Guide: Episode 302
Name___________________
Nucleons- __________ in the __________ of __________
• __________
• __________
Atomic Number- __________ of __________ in the __________ of an
__________
Neutral atom- # of __________ (+) = # of __________ (-)
Isotope- __________ of an __________ that have __________ __________
of __________.
Isotopes of Hydrogen
Hydrogen-1
 _______ proton and _______ neutrons
Hydrogen-2
 _______ proton and _______ neutrons
Hydrogen-3
 _______ proton and _______ neutrons
Mass Number- __________ number of __________ and __________ in an
__________.
Example: Carbon-14 _________________ Neon-20 _________________
Particle
Proton
Charge
Mass
Location
Neutron
Electron
Atomic Mass- __________ of the __________ of all the element’s __________
CHEMISTRY: A Study of Matter
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3.4
Subatomic Particles
# of protons =__________ __________
# of electrons = __________ __________
# of neutrons = __________ __________ - __________ __________
26
Fe
iron:
55.8
__________ protons
__________ electrons
__________ neutrons
8
oxygen-17:
O
15.994
__________ protons
__________ electrons
__________ neutrons
4
2
He
__________ protons
__________ electrons
__________ neutrons
The Chemistry Quiz
CR1._____
CR2._____
3._____
1._____
4._____
CHEMISTRY: A Study of Matter
© 2004, GPB
3.5
2._____
5._____
Worksheet: Atomic Structure
Name___________________
Use your notes from the Atomic Structure program to answer the following
questions.
1. The atomic number tells the number of positively charged ________ in the
nucleus of an atom. The atom is __________ because this is also the number
of __________ charged __________ in the atom.
2. The mass number tells the total number of________ and _________ in the
nucleus of an atom. These particles collectively are called ___________ since
both are located in the nucleus.
3. Isotopes are atoms of the same element with different numbers of _________
which results in different _______ numbers.
4. Write the hyphen notation of the three isotopes of hydrogen:
a.
b.
c.
5. Fill in the following chart (Hint: Isotopes may have different masses than the
periodic table lists!):
Symbol
Atomic
#
Mass
#
Hg
80
201
Mo
42
96
# of
protons
# of
electrons
# of
neutrons
29
35
29
C
14
15
Pb
Na
31
208
82
11
13
CHEMISTRY: A Study of Matter
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3.6
Lab: Atoms and Eggs—Datasheet
Name___________________
Inside the nucleus of an atom are ______________ and _______________. The
__________ ______________ of an atom is the sum of these two particles.
The atomic number is equal to the number of __________________ present in
the nucleus of the atom, and because the atom is neutral, the atomic number is also
the number of ________________ outside the nucleus of the atom.
Procedure: In this activity an “egg” will represent the nucleus of an atom and
different colors of candy will represent the subatomic particles within the nucleus.
Write the description of the candy used to represent the subatomic particles
based on your teacher’s instructions below:
Particle
Description
__________________ ________________________________
__________________ ________________________________
The “atoms” have been numbered. In the data table, write the number of the
“atom”, the number of each subatomic particle present, the mass number, and the
nuclear symbol for the element represented by the “atom” as well as the hyphen
notation for that atom.
# of
Atom
# of
protons
# of
neutrons
Mass
number
Nuclear
Symbol
CHEMISTRY: A Study of Matter
© 2004, GPB
3.7
Hyphen
Notation
Lab: Isotopes—Datasheet
Name______________
Purpose: A new element has been discovered and it is your responsibility to learn
the following about the element:
• the number of naturally occurring isotopes present in the element
• the percentage of each isotope present in your sample of the element
• the atomic mass of the element
Procedure:
1. Obtain a sample of the element from your teacher and record its ID number
above the chart.
2. Count the total number of atoms in your sample and record in the space labeled
as such beside the blank for the ID#.
3. Separate the element into its different isotopes. Assign each isotope a letter
to identify it and record this letter in the first column of the chart.
4. Count the number of atoms of each isotope and record in the second column of
the chart.
5. Calculate the percentage of each isotope present in your element (# of atoms
of isotope/total # of atoms in sample) and record in the last column of the
chart.
6. Mass each isotope group of atoms and record in the third column under "Mass
of Isotope Group”.
7. Calculate the average mass of one atom of that isotope (Mass of Isotope
Group/ # of atoms of that isotope) and record under "Average Mass of Isotope
Group."
ID #______________
Total # of Atoms in Sample ________
Isotope
# of atoms in
Isotope Group
Mass of
Isotope Group
Average Mass of
Isotope Group
Percentage of
Isotope Group
8. On the back of this worksheet, determine the average atomic mass of your
element using this equation: Be sure to show your work!
Average atomic mass = (avg. mass of isotope)(%) + (avg. mass of
isotope)(%) + ...
(Remember that % means "per 100". In a calculation, 50% becomes 50/100 or
0.50.)
9. Give your element a name and symbol and record the information here.
Remember that this is a new element so you, as a scientist, get to name this
element whatever you want!
Element Name:______________ Symbol_____ Atomic Mass_________
CHEMISTRY: A Study of Matter
© 2004, GPB
3.8
Worksheet: Isotope Problems
Name___________________
1. A student looked up the naturally occurring isotopes of bromine and found the
following information:
50.54% of the naturally occurring isotopes of bromine have an atomic mass
of 78.92 u while 49.46% of the naturally occurring isotopes of bromine have
an atomic mass of 80.92 u.
Calculate the average atomic mass of bromine, showing all work:
2. Using the following data, calculate the average atomic mass of magnesium (give
your answer to the nearest .01 u) : Show all work!
Isotope:
Percent abundance:
78.70%
25
Isotope: 12
Mg
Percent abundance:
10.13%
26
Isotope: 12
Mg
Percent abundance:
11.17%
24
12
Mg
3. Using the periodic table,
What is the average atomic mass of bromine? ____________
What is the average atomic mass of magnesium? __________
How do your calculated answers in #1 and #2 compare to those on the
periodic table?
________________________________________
CHEMISTRY: A Study of Matter
© 2004, GPB
3.9
Note Taking Guide: Episode 303
Name___________________
Bohr's Energy Levels
• Electrons in __________ __________ __________
• __________ energy levels: __________ to __________
• __________ energy levels: __________ from __________
• Ground State: __________ in __________ __________ __________
possible
Excited Atom
• Atom has __________ __________.
• __________ state is __________.
• __________ soon __________ same amount of __________ __________.
• __________ seen as __________ __________.
Wave Description of Light
Wavelength (_____): __________ between __________ __________ on
__________ waves
Frequency (_____): the __________ of __________ passing a given
__________ in a given __________
c = __________
c = _______________ : speed of ___________
Sample problem #1:
What is the frequency of light if the wavelength is
6.0 x 10 -7 m?
CHEMISTRY: A Study of Matter
© 2004, GPB
3.10
Sample problem #2:
What is the wavelength of light if its frequency is
5.0 x 1014 Hz?
Particle Description of Light
__________ exists as __________ called __________
E = ____________
•
•
The Modern View of Light
__________ has a __________ __________.
Light may __________ as a __________.
Light may __________ as a __________ of __________ called
__________ or __________.
Spectroscopy
• __________ lines represent __________ __________ as __________
returns to __________ __________ __________.
• __________ lines __________ an __________.
• Called the __________ __________ ____________ of an __________.
Orbital
__________ of __________ where an __________ is __________ to be
__________
The Chemistry Quiz
CR1._____
CR2._____
3._____
1._____
4._____
© 2004, GPB
3.11
2._____
5._____
Worksheet: Electrons in Atoms
I.
Name___________________
Fill in the blanks with the most appropriate term:
In Bohr’s model of the atom, electrons are in certain ___________ levels,
with the levels closest to the nucleus of __________ energy than those
farther from the nucleus. In the _____________ state of the atom, the
electrons are in the lowest _____________ level possible. When an atom
absorbs energy, it is said to be in the _______________ state, which is
unstable. The atom will soon _______ the same amount of energy absorbed
which may be seen as visible light. In the study of ________________,
this visible light is seen as the ________ __________ spectrum of an
element, which is also called an element’s “fingerprints”.
The modern view of light is that it has a _____________ nature. In other
words, light may behave as a stream of particles called ____________ or
___________, or light may behave as a ______________. Modern
scientists suggest that the nature of light depends on the experiment!
In the wave view of light, the wave equation is often used to determine a
wave’s frequency or wavelength. The ____________ is the distance
between corresponding points on adjacent waves while the
_______________ is the number of waves passing a given point in a given
time. The wave equation is: ____________
II.
1.
Use the wave equation to solve the following:
What is the frequency of light with a wavelength of 1.87 x 10-14 m?
2.
What is the wavelength of light with a frequency of 5.6 x 1014 Hz?
III.
1.
Short Answer:
According to Planck’s equation, E = hf , what is the relationship between the
frequency and the energy of light?
2.
According to the wave equation, ________________, what is the
relationship between the frequency and wavelength of light?
CHEMISTRY: A Study of Matter
© 2004, GPB
3.12
Note Taking Guide: Episode 304
Name___________________
Quantum Numbers
• ___________________________________
• Used to __________ an __________ in an __________
n
•
•
__________ __________ __________
Represents __________ energy level of __________
__________ # of __________ in an
__________ __________ = __________
Example: What is the maximum number of electrons that can be in the
_____ main energy level?
l
•
•
•
The __________ __________ __________
Describes the __________ __________ within an __________
__________
__________ of orbital __________ possible in __________
__________ = __________
Orbital Shapes
designated __________________
• level 1: __________
• level 2: __________
• level 3: __________
• level 4: __________
How many electrons can each sublevel hold?
s = 1 orbital x 2 e-/orbital = _______ep = 3 orbitals x 2 e-/orbital = _______ed = 5 orbitals x 2 e-/orbital = _______ef = 7 orbitals x 2 e-/orbital = _______e-
CHEMISTRY: A Study of Matter
© 2004, GPB
3.13
m
•
•
s
•
•
The __________ __________ __________
describes __________ of __________ in __________
The __________ __________ __________
describes __________ of __________ in __________
Ground State: __________ energy arrangement of __________
Diagonal Rule
Examples—
hydrogen _______________
lithium_________________
nitrogen ________________
Orbital Notation
Examples—
hydrogen
nitrogen
CHEMISTRY: A Study of Matter
© 2004, GPB
3.14
Hund's Rule:
__________ of __________ __________ are each __________ by one
__________ before any __________ is occupied by a __________
__________.
Pauli Exclusion Principle:
No two __________ in the __________ __________ can have the __________
__________ of __________ __________ __________.
The Chemistry Quiz
CR1._____
CR2._____
3._____
1._____
4._____
CHEMISTRY: A Study of Matter
© 2004, GPB
3.15
2._____
5._____
Worksheet: Energy Levels, Sublevels, Orbitals
Name___________________
Energy Level
n
# of e- in
Sublevel
E Sublevel
(type of orbital)
# of Orbitals in
Sublevel
1
2
3
4
CHEMISTRY: A Study of Matter
© 2004, GPB
3.16
Total # of ein E level
(2n2)
Worksheet: The Diagonal Rule
To determine the order in which electrons will fill orbitals in an atom,
use the diagonal rule below.
Start at the top
1s
and when you reach the end of one arrow,
return to the next, working your way down.
2s
2p
3s
3p
3d
4s
4p
4d
4f
5s
5p
5d
5f
6s
6p
6d
6f
7s
7p
7d
7f
CHEMISTRY: A Study of Matter
© 2004, GPB
3.17
Worksheet: Electron Distributions
Name___________________
1.
There are four types of orbitals:
s :
shaped like a ___________
An E level can contain only _____ s orbital, making up the “s sublevel”.
p :
shaped like ____________
An E level can contain _____ p orbitals, making up the “p sublevel”.
d:
shaped like double dumbbells
An E level can contain _____ d orbitals, making up the “d sublevel”.
f:
too complex to draw or describe
An E level can contain _____ f orbitals, making up the “f sublevel”.
2.
Each orbital can hold a maximum of _____ electrons. Since both electrons
have a __________ charge, they __________. What keeps them from
flying apart?
Each electron _______ on its axis. One spins __________
and the other spins _____________. When charged particles spin,
they act like tiny magnets. Since the two electrons spin
in ___________ directions, one acts like the north pole of a magnet
and the other acts like the south pole. This makes the electrons
_____________ .
3.
Since each orbital can hold _____ electrons:
The “s sublevel” can hold ______ electrons.
The “p sublevel” can hold ______ electrons.
The “d sublevel” can hold ______ electrons.
The “f sublevel” can hold ______ electrons.
We use this notation to describe an electron:
main _______ level
3p5
# of e- in __________
__________
How are electrons distributed within a sublevel?
According to Hund’s Rule, each __________ within a sublevel is
half-filled before any is __________.
CHEMISTRY: A Study of Matter
© 2004, GPB
3.18
We draw orbital diagrams to show the distribution of electrons in a sublevel.
Circles are used to represent the individual ________. __________ are used to
represent electrons in the orbital. The first electron in an orbital is represented
by a ! and the second by a ! .
A set of four ______________ numbers is assigned to each __________ to
describe its energy and location within the atom. The quantum numbers use the
symbols _______, _______, _______, and _______.
_______ is the principle quantum number and represents the ________ level of
the electron.
_______ represents the sublevel of the electron, which depends on the type of
_____________.
Pauli’s Exclusion Principle states that within an atom, no two electrons can have
the same set of _____________ _____________. If two electrons have the
same n, l, and m numbers, they are in the same _______ level, the same
___________, and the same _____________. They must then have
____________spins! So, the s quantum numbers must be different.
Practice: Write electron distributions and do the orbital notation for the
following:
1.
P:
2.
Ca:
Only do the electron distributions for the following:
1.
Co:
2.
Eu:
3.
Tc:
CHEMISTRY: A Study of Matter
© 2004, GPB
3.19
Worksheet: Electron Distributions Review
Name___________________
I. Fill in the blanks:
1. The orbital shaped like a "dumb-bell" is the _____ orbital, while the orbital
shaped spherically is the ______ orbital.
2. How many sublevels are present in the third main energy level?_____
3. What is the maximum number of orbitals in the "d" sublevel?_____
4. The maximum number of electrons that can occupy an orbital is _____,
provided they have ____________ _________.
5. The maximum number of electrons that can occupy an energy level is
represented by the formula _________.
6. The highly probable location of an electron within the atom is a(n) _________.
II. Write the electron configuration for the following:
1. Mg:______________________________
2. As:______________________________
III.
In the space below, show the orbital notation for Mg:
CHEMISTRY: A Study of Matter
© 2004, GPB
3.20
Review Sheet: Unit 3
Name___________________
I.
Short Answer and Fill in the Blanks:
1.
_____________ are a familiar idea used to explain unfamiliar facts
observed in nature while a ______________ is an explanation of observable
facts and phenomena.
To remain valid, models and theories must:
a.
b.
The existence of the atom was proposed by the Greek philosopher
______________. The word “atom” comes from the Greek word “atomos”
which means ________________.
____________ was a Greek philosopher who rejected the idea of the atom.
__________ __________ was an English schoolmaster who explained the
Law of Conservation of Mass, the Law of Definite Proportions, and the Law
of Multiple Proportions using an atomic theory. His theory proposed that
atoms:
a.
b.
c.
d.
e.
The discovery of the atom’s nucleus can be credited to __________, whose
_______-foil experiment provided experimental detail about the atom’s
structure. In his experiment, Rutherford aimed _______ particles at a
piece of _______ foil. _________ of the particles passed through the foil,
but a few were ___________, and some even bounced back (were
reflected). He concluded that most of the atom is _________
__________. He also concluded that the atom has a dense,
____________ charged core we call the nucleus.
The particles that make up the nucleus of the atom are called
____________ and are comprised of the __________ and ____________
in an atom.
Atoms are ___________ because the number of _________ charged
protons equals the number of ___________ charged electrons.
2.
3.
4.
5.
6.
7.
8.
CHEMISTRY: A Study of Matter
© 2004, GPB
3.21
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
__________ are atoms of an element that have different numbers of
neutrons, and consequently, different atomic ___________.
The _________ _________ of an atom is the sum of all the nucleons of an
atom.
Rutherford’s planetary model of the atom faced a major problem. Classical
physics predicted that the electron, as it circled the nucleus, would
________ energy so eventually the atom would collapse!
Bohr placed e- in _________ levels, assuming that the electron won’t lose
energy as long as it stays in the allowed level.
Bohr suggested that electrons can ________ a quantum or ________ of
energy, and then jump to a __________ energy level. This is called the
____________ state. This is an unstable state, and the atom soon gives
off the same amount of energy absorbed. Some of this energy is in the
form of __________ light.
The science of studying visible light through the use of a spectroscope is
called _______________. The ___________ lines identify an element and
are called the element’s __________ _________ spectrum.
The modern view of light is that it has a ___________ nature, behaving as
both a ___________ and a stream of ___________. It simply depends on
the experiment!
Four _________ ___________ are used to describe the location of an
electron in an atom. They are _____, _____, ____, and ____. The
principal quantum number, _____, represents the main ________ level of
the electron. The maximum number of electrons in this level is found using
the formula: ________. The second quantum number, _____, describes the
_________ shape.
In the electron distribution 1s2, the “1” represents the ________
_________ level, the “s” represents the __________, and the “2”
represents the number of __________ in the ___________.
_________ Rule states that orbitals of equal energy are each occupied by
_________ electron before any orbital is occupied by a __________
electron.
The _____________ Exclusion Principle states that no two electrons in the
________ atom can have the ________ set of four ________
________________.
CHEMISTRY: A Study of Matter
© 2004, GPB
3.22
II.
1.
Charts and Problems: Show all work if applicable.
Complete the following table:
Hyphen
Notation
Nuclear
Symbol
Carbon - 12
Atomic
Number
Mass
Number
# of
Protons
# of
Electrons
# of
Neutrons
6
40
19
K
5
2.
6
The relative abundance of the isotopes of oxygen are:
Oxygen-16: 99.760%
Oxygen-17:
0.037%
Oxygen-18:
Calculate the average atomic mass of oxygen:
0.204%
3.
In a bright-line spectrum, the wavelength of a particular line is
6.0 x 10-7m. What is the frequency of this color of light?
4.
The maximum number of electrons in a main energy level is calculated using
the formula ___________. Therefore, the maximum number of electrons in
the 5th main energy level is:
5.
How many sublevels are present in the 4th main energy level?_____
What are they?_______________
6.
The maximum number of electrons that can occupy an orbital is ____, if
they have __________ ____________.
7.
Do the electron distribution and the orbital notation for:
Li:
O:
CHEMISTRY: A Study of Matter
© 2004, GPB
3.23