the atom for middle school - miss little's classroom...

Understanding

the

Atom for

Middle School

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


On the graphic organizer provided summarize and illustrate the features of

the atom for each model, and state the problem with each model.


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

The Atomic Model of Matter Key

1. A

2. A

3. E

4. A

5. F

6. E

7. B

8. D

9. C

10. D

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

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


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


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______

http://www.google.ca/imgres?hl=en&sa=X&biw=751&bih=437&tbm=isch&prmd=imvns&tbnid=6V7G2Qows66XGM:&imgrefurl=http://www1.assumption.edu/users/bniece/spectra/tutorials/as_bohr.html&docid=bmlcxwexc8dH2M&imgurl=http://www1.assumption.edu/users/bniece/spectra/tutorials/Images/BohrAtom.gif&w=326&h=326&ei=aEJ6UKmBKKbEigL87ICoDA&zoom=1&iact=hc&vpx=213&vpy=83&dur=4078&hovh=225&hovw=225&tx=136&ty=140&sig=100160477650376609534&page=4&tbnh=125&tbnw=125&start=34&ndsp=12&ved=1t:429,r:1,s:34,i:257













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.

Sodium Na

Complete the Chart Fluorine F

11 P

12 N

9 P

10 N

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.


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.


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


Formula Weight______________ Barium Nitrate Ba(NO3)2


Formula Weight______________

Formula Weights Sodium chloride NaCl


sodium

1

23

23

chlorine

1

35

35

Formula Weight 58 amu Zinc nitride Zn3N2


zinc

3

65

195

nitrogen

2

14

28

Formula Weight 223 amu Barium Nitrate Ba(NO3)2


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


Sodium bicarbonate NaHCO3 Element # of atoms Atomic weight Total weight of

atoms


Lead IV arsenate Pb3(AsO4)4 Element # of atoms Atomic weight Total weight of

atoms

Formula Weight_____________

Iron II nitrate Fe(NO3)2



Aluminum sulphate Al2(SO4)3 Element # of atoms Atomic weight Total weight of

atoms


Chromium sulphate Cr(SO4)3 Element # of atoms Atomic weight Total weight of

atoms


Lead III chromate 2{Fe2(CrO4)3 Element # of atoms Atomic weight Total weight of

atoms


Scandium bicarbonate Sc(HCO3)3 Element # of atoms Atomic weight Total weight of

atoms


Iridium dichromate Ir2(CrO7)3 Element # of atoms Atomic weight Total weight of

atoms


Calculating Formula Weights KEY

Hydrogen sulphate H2SO4


hydrogen

2

1

2

sulfur

1

32

32

oxygen

4

16

64


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


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


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


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


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


Lead III chromate 2{Fe2(CrO4)3


lead 4 56 224

chromium 6 52 312

oxygen 24 16 384


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


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


Thanks for purchasing this product.

See other products designed by Merry in the Middle

http://www.teacherspayteachers.com/Store/Merry-In-The-Middle

the atom for middle school - miss little's classroom...

Documents