the atom for middle school - miss little's classroom...
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Table of Contents
1. Accessing Prior Knowledge Activity
2. The Atomic Model Worksheet and Key
3. The Atomic Model of Matter Graphic Organizer and key
4. Atomic Model of Matter Worksheet and key
5. Atom Notes
6. Complete Model of Atom Graphic Organizer and Key
7. Vocabulary Review and Key
8. Periodic Table
9. Understanding the Atom – Finding Numbers of Protons, Neutrons, Electrons and
Key
10. Drawing Bohr Models of Atoms 1 – 20 and Key
11. I Have You Have –game reviewing concepts of atoms
12. Rules for Counting Atoms
13. Counting Atoms Worksheet and Key
14. Counting Atoms Review and Key
15. spdf Energy Levels Diagram and Periodic Table for Orbital Arrangement
16. Electron Arrangement Practice and Key
17. Electron Arrangement Worksheet and Key
18. Formula Weights
What You Already Know About the About the Structure of the Atom
1. Take out a piece of lined paper.
2. Number 1 to 7.
3. Write down one fact you know about the atom.
4. Turn paper over.
5. You have 1 minute to circulate the classroom asking as many classmates as
possible what they wrote down. You must remember this. You may not write
anything down.
6. After one minute back to your desk.
7. Write down as many responses from memory as you can.
8. How many responses can you recall
My Fact
________________________________________________________________________
________________________________________________________________________
1_______________________________________________________________________
2_______________________________________________________________________
3_______________________________________________________________________
4_______________________________________________________________________
5_______________________________________________________________________
6_______________________________________________________________________
7_______________________________________________________________________
Post Unit Reflection – What I learned about the atom
________________________________________________________________________
________________________________________________________________________
________________________________________________________________________
________________________________________________________________________
________________________________________________________________________
________________________________________________________________________
________________________________________________________________________
________________________________________________________________________
Name________________
The Atomic Model of Matter
Name______________________
Block_______________
More than ____________thousand years ago, A Greek philosopher
named____________ led a group of scientists now known as ‘atomists’.
These early Greeks thought that the atom was the ____________ possible
piece of matter that could be obtained. They guessed that the atom was a
small, ____________particle, and that all the atoms were made of the
same material. They also thought that different atoms were different
shapes and sizes, that the atoms were infinite in number, always
____________ and capable of joining together.
In 1803, ____________ proposed an atomic theory. The theory stated
that all elements were made of atoms and that the atoms were
____________ and indestructible particles. Dalton’s theory also said that
atoms of the same element were the same, while atoms of different
elements were ____________. The theory also said that____________
were made by joining the atoms of two or more elements together.
In 1897, J.J. Thomson discovered a particle even smaller than the atom. He
named it the ____________, but today we call it the ____________. As a
result of his discovery, Thomson proposed a new atomic ____________.
According to Thomson’s model, the atom was like a plum ____________ it
was mostly a thick, positively charged material, with negative electrons
scattered about it like ____________ in a pudding.
In 908, Ernest Rutherford took an extremely thin sheet of ____________
and bombarded it with electrons. Much to his surprise, most of the
electrons went right through the foil, and the occasional ____________
was seriously deflected. To him, this seemed as likely as a baseball going
through a brick wall. He theorized that the gold foil must be mostly empty
____________, or else the electrons would bounce off most of the time.
He figured that the atom was made up of a small, dense, positively charged
center, called the ____________. Rutherford’s theory has the electrons
scattered around the atom’s edge.
In1913, Neil Bohr narrowed down the actual location of the electrons. Bohr’s
model was similar to Rutherford’s in that it had a ____________ made up
of positively charged material. Bohr went on to propose that the negative
particles (____________) orbited the nucleus much like the planets
____________ the sun.
Today the atomic model is very similar to Bohr’s model. The modern atomic
model, the Wave model, does not have exact orbits like Bohr did. Instead
the modern model has a scatter region surrounding the ____________
where an ____________ will probably, but not certainly, be found.
The Atomic Model of Matter Key
More than 2000 thousand years ago, A Greek philosopher namedDemocritus
led a group of scientists now known as ‘atomists’. These early Greeks
thought that the atom was the smallest possible piece of matter that could
be obtained. They guessed that the atom was a small, hard particle, and
that all the atoms were made of the same material. They also thought that
different atoms were different shapes and sizes, that the atoms were
infinite in number, always movingand capable of joining together.
In 1803,Dalton proposed an atomic theory. The theory stated that all
elements were made of atoms and that the atoms were indivisible and
indestructible particles. Dalton’s theory also said that atoms of the same
element were the same, while atoms of different elements were different.
The theory also said that compounds were made by joining the atoms of two
or more elements together.
In 1897, J.J. Thomson discovered a particle even smaller than the atom. He
named it the corpuscle, but today we call it the electron As a result of his
discovery, Thomson proposed a new atomic model. According to Thomson’s
model, the atom was like a plum pudding it was mostly a thick, positively
charged material, with negative electrons scattered about it like plumsin a
pudding.
In 908, Ernest Rutherford took an extremely thin sheet of gold foil and
bombarded it with electrons. Much to his surprise, most of the electrons
went right through the foil, and the occasional bullet or electron was
seriously deflected. To him, this seemed as likely as a baseball going
through a brick wall. He theorized that the gold foil must be mostly empty
space or else the electrons would bounce off most of the time. He figured
that the atom was made up of a small, dense, positively charged center,
called the nucleus. Rutherford’s theory has the electrons scattered around
the atom’s edge.
In1913, Neil Bohr narrowed down the actual location of the electrons. Bohr’s
model was similar to Rutherford’s in that it had a nucleus made up of
positively charged material. Bohr went on to propose that the negative
particles (electrons) orbited the nucleus much like the planets orbit the sun.
Today the atomic model is very similar to Bohr’s model. The modern atomic
model, the Wave model, does not have exact orbits like Bohr did. Instead
the modern model has a scatter region surrounding the nucleus where an
electron will probably, but not certainly, be found
Dalton Model - 1803 Democritus Model – 2000 yrs ago Thomson Model - 1897
Rutherford Model - 1908 Bohr Model - 1913 Wave Model - Modern
Name
The Atomic Model of Matter
On the graphic organizer provided summarize and illustrate the features of
the atom for each model, and state the problem with each model.
The Atomic Model of Matter
Name_____________
Block______
Match the statement to the different atomic model. Write the letter for
the atomic model in front of the statement.
1. _____ Atoms are indivisible.
2. _____ An atom is the smallest piece of matter.
3. _____ In an atom, electrons are located in energy levels that are a
certain distance from the nucleus.
4. _____ Atoms are small, hard particles.
5. _____ An atom has a small, positively charged nucleus surrounded by
a large region in which scientists can predict where an
electron is likely to be found.
6. _____ In an atom, electrons move in definite orbits around the
nucleus.
7. _____ Atoms of the same element are exactly alike.
8. _____ An atom is made of positively charged pudding-like material
through which negatively charged particles are scattered.
9. _____ An atom is mostly empty space with a dense, positively
charged nucleus in the center.
10. _____ An atom contains negatively charged particles called
corpuscles.
A - Democritus
B - Dalton
C - Rutherford
D - Thomson
E - Bohr
F - Modern Wave Model
What is an element?
What is a compound?
What is an atom?
What are subatomic
particles?
What is a proton?
What is a neutron?
-pure substance where all
atoms are the same
-cannot be broken down
-can be a molecule
-made up of two or more
kinds of atoms [molecule]
-atoms can be separated if
enough energy is supplied
-the smallest unit of matter
consisting of protons,
neutrons, electrons
-particles that are smaller
than an atom and make up
the atom. They include
protons, neutrons, and
electrons
-subatomic particle with a
positive electric charge that
are found within the nucleus
at the center of the atom.
The relative mass of the
proton is 1 amu.
-subatomic particle with a
zero electric charge that are
found within the nucleus at
the center of an atom. The
relative mass of the neutron
is 1 amu.
The Atom
What is an electron?
What is the atomic number?
What is the atomic mass
number?
How do you calculate the
number of electrons?
.
-subatomic particles with a
negative charge that are
found orbiting around the
nucleus of an atom. The
relative mass of the electron
is 1/1840 amu therefore the
mass of an electron is
considered to be neglible.
-the number of protons in
the nucleus of an atom
Atomic # = # of protons
-is the total number of
protons and neutrons in the
nucleus of an atom.
Mass # = # of neutrons + # of
protons
-In a neutral atom the
atomic number is also equal
to the number of electrons.
Atomic # = # of protons
= # of electrons
What is the atomic mass?
What is an isotope?
-The quantity of matter that
makes up an atom. The
total mass of the protons,
neutrons and electrons that
make up an atom. It is the
average mass of an element’s
naturally occurring isotopes,
taking into account the
percentage of occurrence on
Earth of each isotope.
-There can be more than one
version [isotope] of a
particular element. Each
version [isotope] has the
same number of protons and
electrons therefore the same
atomic #, but each version
has a different # of neutrons
therefore a different mass #.
The Complete Model of the Atom
Name_____________
Block_____
Dalton’s Atomic Theory _________________________________________________________
_________________________________________________________
_________________________________________________________
_________________________________________________________
_________________________________________________________
________________________________________
The Complete Model of the Atom Key
Dalton’s Atomic Theory
1. All matter is made up of atoms. 2. All elements that are the same have the same
mass. Different elements have different masses. 3. Atoms of different elements bond to form
compounds. 4. Matter cannot be created or destroyed.
Orbits or energy levels
1st orbit holds 2 electrons
2nd
orbit holds 8 electrons
3rd
orbit holds 8 electrons
Electrons have - charge
Outer orbit
Holds valence electrons
which are involved in
chemical bonding
Nucleus
Positively charged center
Contains Protons and
Neutrons
Protons + charge
Neurons no charge
Atom has no charge
The Atomic Number = Number of Protons
Number of Protons = Number of Electrons
Atomic Mass = Number of Protons + Number of Neutrons
Vocabulary Review Name_______________
Block_______________
_____________: the smallest particle of an element that has all the
properties of that element.
The atom has ___________ charge.
The 3 main subatomic particles that make up the atom are the
___________, ____________ and ____________.
_____________: small, dense positively charged center of an atom.
____________ and ____________ are found in the nucleus.
_____________: positively charged particles in the nucleus.
_____________: neutral particles in the nucleus.
_____________: negatively charged particles orbiting the nucleus.
The atomic mass of a neutron and a proton is __________.
The atomic mass of an electron is ____________.
Number of ____________ = number of electrons
Atomic mass subtract atomic number = number of ______________.
Label the following.
13
aluminum
26.98
Al
Vocabulary Review Key
atom: the smallest particle of an element that has all the properties of
that element.
The atom has nocharge.
The 3 main subatomic particles that make up the atom are the proton,
neutron and electron.
nucleus: small, dense positively charged center of an atom.
protons and neutrons are found in the nucleus.
protons: positively charged particles in the nucleus.
neutrons: neutral particles in the nucleus.
electrons: negatively charged particles orbiting the nucleus.
The atomic mass of a neutron and a proton is 1 amu.
The atomic mass of an electron is 0 amu.
Number of protons = number of electrons
Atomic mass subtract atomic number = number of neutrons.
Label the following.
13
aluminum
26.98
Al
Atomic Number
Chemical Symbol
Element Name
Atomic Mass
Understanding the Atom
Finding Atomic Number
Recall Atomic Number = Number of Protons
Element Symbol Atomic Number
Number of Protons
Hydrogen 1 Beryllium 4
Carbon 6 Cobalt 27
Krypton 36
Finding Atomic Mass Recall Mass Number = Number of Protons + Number of Neutrons
Element Symbol Mass
Number Number of Protons
Number of Neutrons
Hydrogen 1 0 Chromium 24 28 Beryllium 4 5 Carbon 12 6 Gold 197 118 Cobalt 59 27 Barium 56 81 Iron 56 26
Particle Location Charge Mass
Proton
Neutron
Electron
Key
Finding Atomic Number
Recall Atomic Number = Number of Protons
Element Symbol Atomic
Number Number of
Protons Hydrogen H 1 1 Beryllium Be 4 4
Carbon C 6 6 Cobalt Co 27 27
Krypton Kr 36 36
Finding Atomic Mass Recall Mass Number = Number of Protons + Number of Neutrons
Element Symbol Mass
Number Number of Protons
Number of Neutrons
Hydrogen H 1 1 0 Chromium Cr 52 24 28 Beryllium Be 9 4 5 Carbon C 12 6 6 Gold Au 197 79 118 Cobalt Co 59 27 32 Barium Ba 137 56 81 Iron Fe 56 26 30
Particle Location Charge Mass
Proton nucleus + 1 amu
Neutron nucleus - 1 amu
Electron orbits No charge 0 amu
Finding the Number of Electrons
Recall Atomic Number = Number of Protons = Number of Electrons
Element Symbol Atomic Number
Number of Protons
Number of Electrons
Number of Neutrons
Mass Number
Oxygen 8 16 Sodium 11 11 23 Carbon 6 12 Phosphorus 15 16 Potassium 20 39 Iron 26 30 Copper 29 35 Chlorine 17 35 Boron 5 5 11 Aluminum 13 27
Maximum Number of Electrons in First Three Orbits The orbit closest to the nucleus must be full before electrons
can be place on the next orbit. 1st Orbit 2nd Orbit 3rd Orbit
Maximum Number of
Electron
2
8
8
Look at your periodic table. Notice in period 1 there are only two elements and that the 1st orbit only holds 2 electrons. In period 2 and 3 there are eight elements and notice that the 2nd and 3rd orbit holds 8 electrons. In the 4th level the placement of electrons becomes more complex.
Finding the Number of Electrons Key
Recall Atomic Number = Number of Protons = Number of Electrons
Element Symbol Atomic Number
Number of Protons
Number of Electrons
Number of Neutrons
Mass Number
Oxygen O 8 8 8 8 16 Sodium Na 11 11 11 12 23 Carbon C 6 6 6 6 12 Phosphorus P 15 15 15 16 31 Potassium K 19 19 19 20 39 Iron Fe 26 26 26 30 56 Copper Cu 29 29 29 35 64 Chlorine Cl 17 17 17 18 35 Boron B 5 5 5 6 11 Aluminum Al 13 13 13 14 27
Maximum Number of Electrons in First Three Orbits The orbit closest to the nucleus must be full before electrons
can be place on the next orbit. 1st Orbit 2nd Orbit 3rd Orbit
Maximum Number of
Electron
2
8
8
Look at your periodic table. Notice in period 1 there are only two elements and that orbit one only holds 2 electrons. In period 2 and 3 there are eight elements and notice that the 2nd and 3rd orbit holds 8 electrons. In the 4th level the placement of electrons becomes more complex. We will work first with elements 1 to 20.
Drawing Bohr Models
1. Write down element name and symbol. 2. Draw circle to represent nucleus. 3. Atomic number = number of protons. 4. Record protons in nucleus as __P 5. Round the atomic mass and subtract atomic
number. This is the number of neutrons. Record in nucleus as __N
6. The number of protons = the number of electrons. 7. Fill 1st orbit with 2 electrons. 8. Remaining electrons to 2nd orbit. Fill only to 8. 9. Remaining electrons to 3rd orbit. Fill only to 8.
Example – Sodium Na
11 P
12 N
Drawing Bohr Model of Atoms 1 to 20
Write the name of the element and calculate the number of protons and neutrons and draw the electrons on the orbits,
Name____________
Block______
Further Practice
Element Atomic Number
Mass Number
Protons
Electron
Neutrons
1st orbit
2nd orbit
3rd orbit
Sodium 23 11 Aluminum 13 14 Sulfur 16 32 Chlorine 35 17 Magnesium 12 12 2 Phosphorus 31 2 8 5
Key Element Symbol Protons Neutrons 1st 2nd 3rd 4th
Hydrogen H 1 0 1
Helium He 2 2 2
Lithium Li 3 4 2 1
Beryllium Be 4 5 2 2
Boron B 5 6 2 3
Carbon C 6 6 2 4
Nitrogen N 7 7 2 5
Oxygen O 8 8 2 6
Fluorine F 9 10 2 7
Neon Ne 10 10 2 8
Sodium Na 11 12 2 8 1
Magnesium Mg 12 12 2 8 2
Aluminum Al 13 14 2 8 3
Silicon Si 14 14 2 8 4
Phosphorus P 15 16 2 8 5
Sulfur S 16 16 2 8 6
Chlorine Cl 17 18 2 8 7
Argon Ar 18 22 2 8 8
Potassium K 19 20 2 8 8 1
Calcium Ca 20 20 2 8 8 2
Further Practice
Element Atomic Number
Mass Number
Protons
Electron
Neutrons
1st orbit
2nd orbit
3rd orbit
Sodium 11 23 11 11 12 2 8 1 Aluminum 13 27 13 13 14 2 8 3 Sulfur 16 32 16 16 16 2 8 6 Chlorine 17 35 17 17 18 2 8 7 Magnesium 12 24 12 12 12 2 8 2 Phosphorus 15 31 15 15 16 2 8 5
Understanding the Atom Review
Name_______________
Block_________
Completion - Fill in the missing word Element Composition
The smallest part of an element with the properties of that element is
called the ____________. There are three parts that make up an atom.
Given the charge, identify the particle: [+] ____________, [-]
____________, [0] ____________. The center of the atom is called the
____________. It contains the ___________ and the protons. The
____________ circle around the center in paths called __________. The
charge on the nucleus of an atom is always ____________. Two subatomic
particles must always have the same numbers. The __________ must
always equal the ____________. Any substance with only one kind of atom,
and it cannot be further broken down, is called: ____________. Any
substance that consists of two or more atoms [same or different] is called a
____________. Any substance that consists of two or more different
types of atoms is called a ____________.
Draw Bohr models of fluorine and sodium.
P
N
P
N
Complete the Chart Element Symbol Atomic
Number Mass Number
# of Protons
# of Neutrons
# of Electrons
Helium
Mg
30
80
13
92
11
Ca
Silver
26
6
Fl
80
14 7
Gold
1. _____atom
2. _____electron
3. _____nucleus
4. _____proton
5. _____neutrons
6. _____shell
7. _____atomic number
8. _____atomic mass
9. _____no charge
10. ____Bohr diagram
A. A positively-charged
particle in the center of an
atom.
B. The atom’s charge.
C. Flattened picture of the
electrons in an atom.
D. The neutral particles in the
center of an atom.
E. The empty space between
the electrons and the
nucleus.
F. The combination of atoms to
form a compound.
G. Bohr’s explanation of
electron orbits around the
nucleus.
H. The number of protons in
the nucleus.
I. Negatively-charged particle
discovered by J. J.
Thomson.
J. Total number of protons and
neutrons in the nucleus.
K. Positively charged particles
that orbit in shells around
the nucleus.
L. The center of an atom.
M. The smallest piece of an
element.
N. Moving up to a higher
electron shell
Choose the Best Description for the Vocabulary Term and Place the Letter in front of the Term.
Understanding the Atom Review Key Element Composition
The smallest part of an element with the properties of that element is
called the atom There are three parts that make up an atom. Given the
charge, identify the particle: [+] proton, [-] electron [0] neutron. The
center of the atom is called the nucleus. It contains the netrons and the
protons. The electrons circle around the center in paths called orbits.
Shells, energy levels. The charge on the nucleus of an atom is always
positive. Two subatomic particles must always have the same numbers. The
protons must always equal the electrons. Any substance with only one kind
of atom, and it cannot be further broken down, is called: element. Any
substance that consists of two or more atoms [same or different] is called a
molecule. Any substance that consists of two or more different types of
atoms is called a compound.
Element Symbol Atomic
Number Mass Number
# of Protons
# of Neutrons
# of Electrons
Helium He 2 4 2 2 2
Magnesium Mg 12 24 12 12 12
Zinc Zn 30 65 30 35 30
Bromine Br 35 80 35 45 35
Aluminum Al 13 27 13 14 13
Uranium U 92 238 92 146 92
Sodium Na 11 23 11 12 11
Calcium Ca 20 40 20 20 20
Silver Ag 47 108 47 61 47
Iron Fe 26 56 26 30 26
Carbon C 6 12 6 6 6
Fluorine Fl 9 19 9 10 9
Mercury Hg 80 201 80 121 80
Nitrogen N 7 14 7 7 7
Gold Au 79 199 79 120 79
1. M 6. G
2. I 7. H
3. L 8 J
4. A 9. B
5. D 10. C
I Have You Have
Cut out the cards and distribute one to each student. The student with the first card begins.
They pose the question and the student with the card with answer stands and answers. They
then pose the question at the bottom of their card.
This game is designed to be used by students using their Periodic Tables.
I have the first
card.
Who has the element with
20 protons
I have
calcium.
Who has matter made up of only one type
of atom?
I have
Element.
Who has the positive
electric charge within the atom
nucleus?
I have
proton.
Who has chart listing all
the known elements?
I have
the Periodic Table.
Who has
the element with 26
electrons?
I have
iron.
Who has the element with 2 neutrons and 2
protons?
I have helium.
Who has
the element used in thermometers?
I have
mercury.
Who has the negative
electric charge which orbits the
nucleus?
I have
electron.
Who has the element with atomic number 6?
I have
carbon.
Who has the smallest piece
of matter?
I have
the atom.
Who has the element with
55 protons?
I have cesium.
Who has the second
element in the Noble gas family?
I have neon.
Who has
the total number of protons + the total number of
neutrons?
I have
the atomic mass.
Who has the neutral
electric charge found in the
nucleus?
I have
neutrons.
Who has the most abundant element in
Earth’s crust?
I have oxygen.
Who has
the element with symbol Na?
I have sodium.
Who has
the element used for fancy
serving sets and tarnishes?
I have silver.
Who has
the abbreviation for the element
name
I have
a chemical symbol.
Who has
the element with 19 protons?
I have
potassium.
Who has the lightest
element?
I have
hydrogen.
Who has the electric
charge on the entire atom?
I have
no charge.
Who has the term by which
elements are listed on the
Periodic Table?
I have
the atomic number
Who has
the element with chemical
symbol K?
I have
potassium.
Who has the element with
symbol Au?
I have gold.
Who has
the element with 5 protons
and 6 neutrons?
I have boron.
Who has
the element which is the most abundant gas in
air?
I have
nitrogen.
Who has the unit for
measurement for subatomic particles?
I have
atomic mass units or amu.
Who has
the element with the atomic number 53?
I have iodine.
Who has
the term for the most numerous elements on the periodic table?
I have metals.
And I have the
last card!
3(Ca3P
2)
Ca
3P
2 Add the subscripts.
Answer = 5 atoms
Na(OH) We never write 1 as a subscript.
1 sodium + 1 oxygen + 1 hydrogen = 3 atoms
3(Ca3P
2) Add the subscripts and multiply by
the coefficient. 5 atoms x 3 = 15 atoms
Au3(PO
4) Some atoms are grouped in a
bracket. Just add them up.
3 gold+ 1 phosphorus + 4 oxygen = 8 atoms
Ca3(PO
3)2
A subscript to the right of a bracket
multiplies all the atoms within the
bracket to the left.
3 calcium + 2 phosphorus + 6 oxygen = 11 atoms
Coefficient – Indicates
the number of
molecules and
multiplies all atoms in
the formula that follow
Subscript –
Indicates the
number of atoms
of that symbol
Board Practice
NaHCO
3
_____________________________________________________
C2H
4O
2
__________________________________________________________________________________________
(NH4)3PO
4
________________________________________________________________________________________
3H3PO
4
__________________________________________________________________________________________
(NH4)2(CrO
4)
_____________________________________________________
4CaCO3
_____________________________________________________
Board Practice
NaHCO
3
1 sodium + 1 hydrogen + 1 carbon + 3 oxygen = 6 atoms
C2H
4O
2
2 carbon + 4 hydrogen + 2 oxygen = 8 atoms
(NH4)3PO
4
3 nitrogen + 12 hydrogen + 1 phosphorus + 4 oxygen = 24 atoms
3H3PO
4
9 hydrogen + 3 phosphorus + 12 oxygen = 24 atoms
(NH4)2(CrO
4)
2 nitrogen + 8 hydrogen + 1 chromium + 4 oxygen = 15 atoms
4CaCO3
4 calcium + 4 carbon + 12 oxygen = 20 atoms
Counting Atoms Name________________________
Block_______________
1. H20______________________________________________________________
2. NaF______________________________________________________________
3. Rb(NO2)_______________________________ ___________________________
4. H(OH)____________________________________ _______________________
5. Sc2O3____________________________________________________________
6. TiBr4_____________________________________________________________
7. 3(V2O5)____________________________________ ______________________
8. H2(SO4)_____________________________________ _____________________
9. 3[Li(OH)]____________________________________ _____________________
10. 2[H3(PO4)]___________________________________ _____________________
11. Na3(PO3)___________________________________ ______________________
12. Ca3(PO4)2_________________________________________________________
13. Ti(ClO3)3_________________________________________________________
14. Sc(MnO4)3________________________________________________________
15. Fe2(Cr2O7)3_______________________________________________________
16. 2[Al(OH)3]_________________________________ ______________________
17. 4[H(NO3)]___________________________________ _____________________
18. 3(C6H11O6) _______________________________________________________
19. 2[Al(MnO4)3]____________________________ _________________________
20. Pb(CrO4)4________________________________________________________
21. 3[Ti(HCO3)4] _____________________________________________________
22. (NH4)(OH) _______________________________________________________
23. 2[Mg3(AsO4)2] ____________________________________________________
24. 3[Au2(SO3)]_______________________________________________________
25. Co(CN)3 _________________________________________________________
26. 2[(NH4)2(Cr207)]_____________________________ ______________________
27. Sr(ClO3)2_________________________________________________________
28. Pb(CrO4)2________________________________________________________
29. KI______________________________________________________________
30. Pb(NO3)2________________________________________________________
Counting Atoms Key
1. H20 -2 hydrogen, 1 oxygen = 3
2. NaF- 1 sodium, 1 fluorine = 2
3. Rb(NO2) - 1 rubidium, 1 nitrogen, 2 oxygen = 4
4. H(OH)-1 hydrogen, 1 oxygen, 1 hydrogen = 3
5. Sc2O3 - 2 scandium, 3 oxygen = 5 6. TiBr4- 1 titanium, 4 bromine = 5 7. 3(V2O5) – vanadium, 15 oxygen = 21 8. H2(SO4) – 2 hydrogen, 1 sulfur, 4 oxygen = 7 9. 3[Li(OH)] – 3 lithium, 3 oxygen, 3 hydrogen = 9
10. 2[H3(PO4)] – 6 hydrogen, 2 phosphorus, 8 oxygen = 16
11. Na3(PO3) – 3 sodium, 1 phosphorus, 3 oxygen = 7
12. Ca3(PO4)2- 3 calcium, 2 phosphorus, 8 oxygen = 13
13. Ti(ClO3)3 – 1 titanium, 4 chlorine, 12 oxygen = 17
14. Sc(MnO4)3 – 1 scandium, 3 manganese, 12 oxygen = 16
15. Fe2(Cr2O7)3 – 2 iron, 6 chromium, 21 oxygen = 29
16. 2[Al(OH)3] – 2 aluminum, 6 oxygen, 6 hydrogen = 14
17. 4[H(NO3)] – 4 hydrogen, 4 nitrogen, 12 oxygen = 20
18. 3(C6H11O6) - 18 carbon, 33 hydrogen, 18 oxygen = 69
19. 2[Al(MnO4)3] – 2 aluminum, 6 manganese, 24 oxygen = 32
20. Pb(CrO4)4 – 1 lead, 4 chromium, 16 oxygen = 21
21. 3[Ti(HCO3)4] - 3 titanium, 12 hydrogen, 12 carbon, 36 oxygen = 63
22. (NH4)(OH) - 1 nitrogen, 4 hydrogen, 1 oxygen, 1 hydrogen = 7
23. 2[Mg3(AsO4)2] - 6 manganese, 4 arsenic, 16 oxygen = 26
24. 3[Au2(SO3)] – 6 gold, 3 sulfur, 9 oxygen = 18
25. Co(CN)3 – 1 cobalt, 3 carbon, 3 nitrogen = 7
26. 2[(NH4)2(Cr2o7)] – 4 nitrogen, 16 hydrogen, 4 chromium, 14 oxygen = 38
27. Sr(ClO3)2 – 1 strontium, 2 chlorine, 8 oxygen = 9
28. Pb(CrO4)2 – 1 lead, 2 chromium, 8 oxygen = 11
29. KI – 1 potassium, 1 iodine = 2
30. Pb(NO3)2 – 1 lead, 2 nitrogen, 6 oxygen = 9
1.
Counting Atoms Name____________________ Block_____
1. NaBr____________________________________________________ =_______atoms
2. MgO____________________________________________________ =_______atoms
3. K(MnO4)_________________________________________________ =_______atoms
4. Ni(SO4) _________________________________________________ _=_______atoms
5. Zn(HSO4)2________________________________________________ =_______atoms
6. Na2(SO4) ________________________________________________ _=_______atoms
7. (NH4)(HCO3)_____________________________________________ =_______atoms
8. Ca3(PO4)2________________________________________________ =_______atoms
9. 2[Li3(PO4)] _______________________________________________ =_______atoms
10. 3[Sc(MnO4)3] ____________________________________________ =_______atoms
Counting Atoms KEY Name____________________ Block_____
1. NaBr 1 sodium 1 bromine = 2 atoms
2. MgO 1 magnesium 1 oxygen = 2 atoms
3. K(MnO4) 1 potassium, 1 manganese 4 oxygen = 6 atoms
4. Ni(SO4) 1 nickel, 1 sulfur 4 oxygen = 6 atoms
5. Zn(HSO4)2 1 zinc, 2 hydrogen, 2 sulfur, 8 oxygen = 13 atoms
6. Na2(SO4) 2 sodium, 1 sulfur, 4 oxygen = 7 atoms
7. (NH4)(HCO3) 1 nitrogen, 5 hydrogen, 1 carbon, 3 oxygen = 10 atoms
8. Ca3(PO4)2 3 calcium, 2 phosphorus, 8 oxygen = 13 atoms
9. 2[Li3(PO4)] 6 lithium, 2 phosphorus, 8 oxygen = 16 atoms
10. 3[Sc(MnO4)3] 3 scandium, 9 manganese, 36 oxygen = 48 atoms
Energy Level Diagram for
Quantum Levels, Orbitals, and Related Periods
7p
6d
5f
n = 7______________________________ 7s
6p
5d
4f
n = 6______________________________ 6s
5p
4d
n = 5______________________________ 5s
4p
3d
n = 4______________________________ 4s
Energy 3p
n = 3______________________________ 3s
2p
n = 2______________________________ 2s
n = 1______________________________ 1s
The s, p, d, f orbital blocks of the Periodic Table s orbital
block
d orbital block
f orbital block
p orbital block
Board Practice
Energy levels for the atoms have sublevels.
Sublevels must be completely filled period by period.
Look at the energy level diagram for the pattern.
The sublevels are represented by letters, spdf
Refer to the energy level diagram. Each circle
represents 2 electrons.
When recording the number of electrons in a sublevel,
write the sublevel and follow it with the number of
electrons superscripted.
For example:
Hydrogen Atomic Number 1
1s1
Magnesium Atomic Number 12
1s2
2s2
2p6
3s2
Add the superscripts – Note it equals 12, the same as
the atomic number.
Silver Atomic Number 47
1s2
2s2
2p6
3s2
3p6
4s2
3d10
4p6
5s2
4d9
Now You Try
Element 1st
orbit 2nd
orbit 3rd
orbit 4th
orbit 5th
orbit
Sulfur
(16)
Gallium
(31)
Strontium
(38)
Tin
(50)
Board Practice
Element 1st
orbit 2nd
orbit 3rd
orbit 4th
orbit 5th
orbit
Sulfur
(16)
1s2
2s22p
6
3s23p
2
Gallium
(31)
1s2
2s22p
6
3s23p
6
4s23d
104p
1
Strontium
(38)
1s2
2s22p
6
3s23p
6
4s23d
104p
6
5s2
Tin
(50)
1s2
2s22p
6
3s23p
6
4s23d
104p
5
5s24d
105p
2
Name Symbol Atomic
Number
Mass
Number
Protons Neutron 1st 2nd 3rd 4th 5th
hydrogen
helium
lithium
nitrogen
fluorine
silicon
potassium
calcium
zinc
cobalt
krypton
zirconium
silver
Complete the Following Table. Show the spdf Electron Arrangement.
Name
1. Determine the name for each element
from the chemical symbols
2. Write down the number of atoms for
each element.
3. Write down the atomic mass for each
element. Round it to the units place.
4. Calculate the total weight of the atoms
for each element.
Number of atoms x atomic mass
5. Calculate the total weight of the
compound by totaling the weight of each
individual atom.
6. Don’t forget your units.
Formula Weights Sodium chloride NaCl
Element # of atoms Atomic weight Total weight of atoms
Formula Weight______________ Zinc nitride Zn3N2
Element # of atoms Atomic weight Total weight of atoms
Formula Weight______________ Barium Nitrate Ba(NO3)2
Element # of atoms Atomic weight Total weight of atoms
Formula Weight______________
Formula Weights Sodium chloride NaCl
Element # of atoms Atomic weight Total weight of atoms
sodium
1
23
23
chlorine
1
35
35
Formula Weight 58 amu Zinc nitride Zn3N2
Element # of atoms Atomic weight Total weight of atoms
zinc
3
65
195
nitrogen
2
14
28
Formula Weight 223 amu Barium Nitrate Ba(NO3)2
Element # of atoms Atomic weight Total weight of atoms
barium
1
137
137
nitrogen
2
14
28
oxygen
6
16
96
Formula Weight 261 amu
Calculating Formula Weights
Name________________
Block______
Hydrogen sulphate H2SO4 Element # of atoms Atomic weight Total weight of
atoms
Formula Weight______________
Sodium bicarbonate NaHCO3 Element # of atoms Atomic weight Total weight of
atoms
Formula Weight______________
Lead IV arsenate Pb3(AsO4)4 Element # of atoms Atomic weight Total weight of
atoms
Formula Weight_____________
Iron II nitrate Fe(NO3)2
Element # of atoms Atomic weight Total weight of atoms
Formula Weight______________
Aluminum sulphate Al2(SO4)3 Element # of atoms Atomic weight Total weight of
atoms
Formula Weight______________
Chromium sulphate Cr(SO4)3 Element # of atoms Atomic weight Total weight of
atoms
Formula Weight______________
Lead III chromate 2{Fe2(CrO4)3 Element # of atoms Atomic weight Total weight of
atoms
Formula Weight______________
Scandium bicarbonate Sc(HCO3)3 Element # of atoms Atomic weight Total weight of
atoms
Formula Weight______________
Iridium dichromate Ir2(CrO7)3 Element # of atoms Atomic weight Total weight of
atoms
Formula Weight______________
Calculating Formula Weights KEY
Hydrogen sulphate H2SO4
Element # of atoms Atomic weight Total weight of atoms
hydrogen
2
1
2
sulfur
1
32
32
oxygen
4
16
64
Formula Weight 98 amu
Sodium bicarbonate NaHCO3 Element # of atoms Atomic weight Total weight of
atoms sodium 1 23 23
hydrogen 1 1 1
carbon 1 12 12
oxygen 3 16 48
Formula Weight 84 amu
Lead IV arsenate Pb3(AsO4)4 Element # of atoms Atomic weight Total weight of
atoms lead 3 207 621
arsenic 4 75 300
oxygen 16 16 256
Formula Weight 1177 amu
Iron II nitrate Fe(NO3)2 Element # of atoms Atomic weight Total weight of
atoms iron 1 56 56
nitrogen 2 14 28
oxygen 6 16 96
Formula Weight 180 amu
Aluminum sulphate Al2(SO4)3 Element # of atoms Atomic weight Total weight of
atoms aluminum 2 27 54
sulfur 3 32 96
oxygen 12 16 192
Formula Weight 342 amu
Chromium sulphate Cr(SO4)3 Element # of atoms Atomic weight Total weight of
atoms chromium 2 52 104
sulfur 3 32 96
oxygen 12 16 192
Formula Weight 392 amu
Lead III chromate 2{Fe2(CrO4)3
Element # of atoms Atomic weight Total weight of atoms
lead 4 56 224
chromium 6 52 312
oxygen 24 16 384
Formula Weight 920 amu
Scandium bicarbonate Sc(HCO3)3 Element # of atoms Atomic weight Total weight of
atoms scandium 1 45 45
hydrogen 3 1 3
carbon 3 12 36
oxygen 9 16 144
Formula Weight 228 amu
Iridium dichromate Ir2(CrO7)3 Element # of atoms Atomic weight Total weight of
atoms iridium 2 192 384
chromium 3 52 156
oxygen 21 16 336
Formula Weight 876 amu
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