improvements more info about the people, but take only 1-2 days to cover them

Improvements

• More info about the people, but take only 1-2 days to cover them

Bell Work 12/9/13

• Start new bellwork titled “Atoms”

1.What do you remember about atoms? (their structure, the subatomic particles, the charges…)

2.W5SAYWoS

Happy 16Happy 16thth Birthday Kendle Birthday Kendle Rivera!Rivera!

Atoms: Atoms: The Building The Building Blocks of Matter Blocks of Matter

• Prior knowledge

Schedule• Today

– Elements to memorize– Notes on history of atom– Worksheet

• Monday– Electron configuration

• Tuesday– Isotope quiz!

Elements to Memorize• 1-20, 26-30, 47, 50, 78-80, 82

# Name Symbol How remember

Today you are going to…take notes on the history of the atom.

So you can…explain how & by whom the parts of the atom have been discovered.

You’ll know you’ve got it when you can • List the scientists of the atom and their achievements

History of Atom Overview Video

• http://www.youtube.com/watch?v=B2aFTNhgyII&feature=related

http://www.youtube.com/watch?v=B2aFTNhgyII&feature=related

http://www.youtube.com/watch?v=B2aFTNhgyII&feature=related

Leucippus & Democritus

• Democritus 460 BC - 370 BC460 BC - 370 BC– Student of Leucippus– Believed all matter is made up of various

imperishable, indivisible things which he indivisible things which he called atoma, or “indivisible units”called atoma, or “indivisible units”

– Basically, they named the atomnamed the atom!

Aristotle Aristotle • 384 BC – 322 BC

• Believed matter consisted of 4 basic elementsBelieved matter consisted of 4 basic elements

• Wrong, but peopleWrong, but people

believedbelieved

him because he him because he

was popular withwas popular with

important peopleimportant people

& the church.& the church.

AlchemistsAlchemists• 1100’s

• European “scientists” that tried to make gold from other metals– Couldn’t be done

• Added ideas of observation & experimentation!

• Recorded info on properties of matter

Bell Work 12/10/13

1.What did Democritus think?

2.What did Aristotle think?

3.What did alchemist try to do? How did this advance science?

John DaltonJohn Dalton

• 1766 – 18441766 – 1844

• Had a theory…

Dalton’s Atomic Theory1. All matter is composed of atoms2. Atoms of a given element are identical in size,

mass, and other properties; atoms of different elements are different

3. Atoms cannot be subdivided, created, or destroyed

4. Atoms of different elements combine in simple whole-number ratios to form compounds

5. In chemical reactions, atoms are combined, separated, or rearranged.

Dalton’s Atomic Theory(Simplified)

1.1. All matter is composed of atomsAll matter is composed of atoms2.2. Atoms of same element are identical; atoms of Atoms of same element are identical; atoms of

different elements are differentdifferent elements are different3.3. Atoms cannot be subdivided, created, nor Atoms cannot be subdivided, created, nor

destroyeddestroyed4.4. Atoms of different elements combine to form Atoms of different elements combine to form

compoundscompounds5.5. In chemical reactions, atoms are rearranged.In chemical reactions, atoms are rearranged.

Modern Atomic Theory

• Still True…– All matter is composed of atoms– Atoms of any one element differ in properties

from atoms of another.

• DifferentDifferent– Atoms of the same element may have Atoms of the same element may have

different masses! (Called isotopes)different masses! (Called isotopes)– Atoms Atoms areare divisible divisible (not by ordinary chem. means). (not by ordinary chem. means).

• Nuclear reactions!Nuclear reactions!

Discovery of the ElectronDiscovery of the ElectronIn 1897, J.J. Thomson 1897, J.J. Thomson used a cathode ray cathode ray tube tube to deduce the presence of a negatively charged particle...DISCOVERED THE DISCOVERED THE ELECTRONELECTRON!!

Cathode ray tubes pass electricity through a gas that is contained at a very low pressure.

Discovery of the ElectronDiscovery of the ElectronTV Demo!TV Demo!Cathode rays – stream of electronsCathode rays – stream of electronsee- - moved ______________ the positive moved ______________ the positive charged platecharged plate

Some ModernSome ModernCCathode athode RRay ay TTubesubes

ConclusionsConclusions from the Study from the Study of the Electronof the Electron

Cathode rays have identical properties regardless of the element used to produce them. All elements must contain identically charged All elements must contain identically charged electrons. electrons. Atoms are neutral, so there must bemust be positive positive particles particles in the atom to balance the negative to balance the negative charge charge of the electrons

J.J. Thomson’s Atomic J.J. Thomson’s Atomic ModelModel

Discovered all electrons have equal charge, but couldn’t measure mass or charge of the electrons.

Thomson believed that the electrons were like electrons were like plums embedded in a positively charged plums embedded in a positively charged “pudding,” “pudding,” thus it was called the “plum “plum pudding” model.pudding” model.

I love me some plum puddin’!

Mass of the ElectronMass of the Electron

1909 – Robert 1909 – Robert Millikan determines Millikan determines the mass of the the mass of the electron.electron.

Enables him to calculate the charge too!The oil drop

apparatus Mass of the electron is 9.109 x 10-31 kg

Conclusions from the Study Conclusions from the Study of the Electronof the Electron

Electrons have so little mass that atoms must contain other particles that account for most of the mass

1911: Rutherford’s Gold Foil 1911: Rutherford’s Gold Foil ExperimentExperiment

Fired alpha particles (helium nuclei, ___ charge) Fired alpha particles (helium nuclei, ___ charge) Particles were fired at a Particles were fired at a thinthin sheet of gold foil sheet of gold foil Particle hits on the detecting screen (film) are Particle hits on the detecting screen (film) are recordedrecorded “ “Gold foil” demoGold foil” demo

Rutherford’s FindingsRutherford’s Findings

The nucleus is small The nucleus is small The nucleus is dense The nucleus is dense The nucleus is positively chargedThe nucleus is positively charged

MostMost of the particles passed right passed right through through A fewfew particles were deflected deflected VERY FEW VERY FEW were greatly deflectedgreatly deflected

“Like howitzer shells bouncing off of tissue paper!”

Conclusions:

Top of worksheet

Bohr Model of AtomBohr Model of Atomaka “planetary modelplanetary model”

1. Electrons assume only certain orbitsorbits around the nucleusnucleus. These orbits are stable and called "stationary" orbits.

2. Each orbit has an energy levelEach orbit has an energy level associated with it. For example the orbit closest to the nucleus has an energy E1, the next closest E2 and so on.

3. Light is emitted when an electron jumps from a higher orbit to a lower orbit and absorbed when it jumps from a lower to higher orbit.

4. Energy of light emitted is the difference between the two orbit energies.

Bohr Model of AtomBohr Model of Atomaka “planetary model”1st shell 2 e-

2nd shell 8 e-

3rd shell 8 e-

4th shell 18 e-

5th shell 18 e-

6th shell 32 e-

7th shell 32 e-

Electron Cloud• More accurate

• e- don’t travel in simple, specific orbits

• e- travel around nucleus in random, unpredictable orbits at superfast speeds

• Can’t tell exactly where they are, but they’re somewhere in the “e- cloud”

OrbitalsOrbitalsElectrons can be in 4 types of orbitals within an energy level…

Named s, p, d, or f

Don’t worry about them for now…we’ll talk more about them later.

Bell Work 11/27/121.Discovered the nucleus

2.Planetary model of atom

3.Plum pudding model of atom

4.Discovered most of the atom is empty space

5.Cathode rays

6.Discovered electron

7.Gold foil experiment

8.W5SAYBoS

Today you are going to…take notes on the parts of an atom & isotopes.

So you can…explain the basic structure of an atom, which will help you to predict bonds in the future.

You’ll know you’ve got it when you can • Identify all parts of an atom, their relative masses,

charges, and location. (complete chart)• Determine the mass of an isotope

Atom – smallest particle of an element that retains the chemical properties of that element.

Composed of: protonsneutronselectrons

Subatomic ParticlesProtonsPositive charge

In nucleus (tiny, dense, center of atom)

Mass of 1 amu (atomic mass unit)

NeutronsNeutral (no charge)

In nucleus

Mass of 1 amu

Electrons Negative charge

In “electron cloud” around nucleus (“orbit” nucleus)

Very little mass (about 1/2000 P, or 0.0006 amu)

Atomic ParticlesAtomic ParticlesParticle Charge Mass (kg) Location

Electron

-1 9.109 x 10-31 Electron cloud

Proton +1 1.673 x 10-27 Nucleus

Neutron

0 1.675 x 10-27 Nucleus

Force in the Nucleus Force in the Nucleus •Two protons extremely close to each other attract

•(indirect effect of strong nuclear force, the strongest force in the universe!)

•Over 100 protons can exist together in a nucleus!•Strong nuclear force has same effect on neutrons.

ElectroElectronn

NeutronsNeutrons

ProtonsProtons

+ charge+ charge““pp++””

chargedcharged

about same about same massmass

- charge- charge

very little very little massmass

orbits nucleusorbits nucleus

““nnoo”” cathode rayscathode rays

no chargeno charge

subatomic subatomic particlesparticles

found in atomfound in atom

in nucleusin nucleus

““ee--””

Determines what Determines what element atom iselement atom is

Understanding Isotopes

Atomic Number

• Number of protons in an atom

• Tells which element atom is– Atoms of the same element ALWAYS have

the same number of protons.

• Above atom on periodic table

• What subatomic particles have the most mass?• What subatomic particle has hardly any mass?• Therefore, an atom’s mass depends on how

many ___ and ___ it has.• All atoms of the same element have the same

____ ____, which means they have the same number of _____.

• Do all atoms of the same element have the same mass?

• What must be different about these atoms?• Atoms of the same element with a different

number of neutrons are called isotopes.

IsotopeIsotopess

Elements occur in nature as mixtures of isotopes.Isotopes are atoms of the same element that differ in the number of neutrons

Isotopes are named by their mass number

IsotopesIsotopesatoms of same element with different number of neutrons and, therefore, different masses

Isotope Protons

Electrons

Neutrons

Nucleus

Hydrogen–1

(protium)

1 1 0

Hydrogen-2

(deuterium)

1 1 1

Hydrogen-3

(tritium)

1 1 2

Mass NumberMass Number•number of protons and neutrons in the nucleus of an atom.•measured in atomic mass units (amu)• 1 proton = 1 amu 1 neutron = 1 amuMass # = p+ + n0

Isotope p+ n0 e- Mass #

Oxygen - 10

- 33 42

- 31 15

8 8 1818

Arsenic 75 33 75

Phosphorus 15 3116

Assume the particles below are atoms, meaning they have no charge.

Atomic MassAtomic Mass

Isotope Symbol Composition of the nucleus

% in nature

Carbon-12

12C 6 protons 6 neutrons

98.89%

Carbon-13


1.11%

Carbon-14


<0.01%

• average mass of all the naturally isotopes of that element• Found under symbol on periodic tableAtomic mass of Carbon = 12.011

Atomic Mass

• average mass of all the naturally isotopes of that element

• Also the mass of 1 mole of an element!

There are two isotopic notations

Element name – mass # or mass#

Symbol

atomic #

Chlorine – 37 108

___ protons Ag

___ electrons 47

___ neutrons

___ protons

___ electrons

___ neutrons

Carbon – 10 13___ protons C___ electrons 6___ neutrons ___ protons ___ electrons ___ neutrons

Gold -200 197___ protons Au___ electrons 79___ neutrons ___ protons ___ electrons ___ neutrons

Sulfur-31 197

___ protons Hg

___ electrons 80

___ neutrons

___ protons

___ electrons

___ neutrons

Calcium-39 19

___ protons F

___ electrons 9

___ neutrons

Strontium-87 119

___ protons Sn

___ electrons 50

___ neutrons

Ions – charged atoms!

• Charge of –2 has 2 more electrons than protons

• Charge of +3 has 3 more protons than electrons

Bell Ringer 12/5/12

4. W5SAYW

Sulfur-31 197 ___ protons___ protons Hg ___ electrons___ electrons 80 ___ neutrons___ neutrons

Quiz answers

Bell Work 12/7/12

1. What do you know about electron configuration?

Bell Work 12/11/12 – 3 min

Determine the number of electrons, protons, and neutrons in the following neutral atoms.

1. Helium-5

2. Sulphur-34

Bonus!

• Empty 2 liter bottles

• Big pop cans (the bigger the better)

• Now lets review chart!

Today you are going to…take notes on and begin writing the electron configuration of atoms

So you can…better understand the structure of an atom and predict ionic bonds

You’ll know you’ve got it when you can

• Write the electron configurations and draw the Bohr models for– All elements to calcium– All atoms up to barium– All elements!

Valence electrons

• electrons in the outermost shell of an atom.

• IMPORTANT! - determine many of the properties of an atom

• What row?

• What orbital (letter)?

• How many over?

Bell Work 12/13/12• Turn in bonus

• Write the electron configuration for

1.Bromine

2.Iodine

3.Astatine

Valence electrons

• electrons in the outermost shell of an atom.

• IMPORTANT! - determine many of the properties of an atom

Electron Configurations• Electron “locations”

• Identifies which energy level the electrons are in

• There are 4 orbitals – s, p, d, & f– s orbital, holds up to 2 electrons– p orbital, holds up to 6 electrons– d orbital, holds up to 10 electrons– f orbital, holds up to 14 electrons

Electron Configuration

1s2

Energy Level

Orbital

# of electrons

Bell Work 12/14/12 – 5 min• Turn in bonus

• Write the electron configuration & Bohr diagram for

1. Fluorine-19

2. Bromine-80

3. Astatine-210

4.What are valence electrons?

Schedule• Bell work/check homework

• Grades

• Review homework

• Electron dot diagram

Today you are going to…take notes on and begin writing the electron dot diagram of atoms

So you can…better understand the structure of an atom and predict ionic bonds

You’ll know you’ve got it when you can

• Write the electron configurations, draw the Bohr models, and electron dot diagrams for– All elements!


3s1

Energy Level

Orbital

# of electrons


2p4

Energy level?

Orbital?# of electrons?

Beryllium (Be) – Atomic # 4

1s2, 2s2

Sulfur (S)

1s2, 2s2,2p6, 3s2, 3p4

Iron (Fe) – Atomic # 26

1s2, 2s2,2p6, 3s2, 3p6, 4s2, 3d6

Bohr Models

• Where are the valence electrons?

Homework (or Homeroom work)Write the electron configuration AND draw the

following atoms

• Helium-5

• Nitrogen-15

• Iron- 54

• Antimony-123 (symbol Sb)

• BONUS CHART!

Bell Work 12/11/12Put your homework upside-down on your desk.

Write the electron configuration AND draw the following atoms

1. Phosphorus-30

2. Cobalt-56

Bell Work 12/10/12

Put your homework upside-down on your desk.

1. Chlorine-36

2. Nickel-56

Electron Dot Diagram

1s2

Bell Work 12/20/12

Which numbers go together?

1.Discovered the nucleus

2.Planetary model of atom

3.Plum pudding model of atom

4.Discovered most of the atom is empty space

5.Cathode rays

6.Gold foil experiment

7.Discovered electron

+ charge+ charge

““pp++””

chargedcharged

about same massabout same mass

- charge- charge

very little massvery little mass


““nnoo””

cathode rayscathode raysno chargeno charge

subatomic particlessubatomic particles



““ee--””

Which subatomic particles…Which subatomic particles…

Atom & Solar System Similar

little stuff (planets n e-) orbits big stuff

both mostly empty space

orbiting things are always moving

Different

orbits less precise in space

solar system bigger!

solar system has life

some atomic particles have charges!

planets have moons

Atomic structureProton - +, has mass of 1amu, in nucleus,

always same # in atom!

Neutron – neutral (no charge), 1 amu, in nucleus, different # in different atoms (isotopes)

Electron – orbits nucleus, negative charge, 1/2000 mass of proton/nutron, can be lost through bonding

Dalton’s Atomic Theory(Simplified)

1. All matter is composed of atoms2. Atoms of same element are identical; atoms of

different elements are different3. Atoms cannot be subdivided, created, nor

destroyed4. Atoms of different elements combine to form

compounds5. In chemical reactions, atoms are rearranged.

STOPSTOP

Bromine-81 40___ protons Ar___ electrons 18___ neutrons ___

protons ___

electrons ___

neutrons

Bell Ringer 11/14 – 5 minutes

1. The number of ___________ an atom has; gives it it’s identity.

2. Atoms of the same element that have a different number of neutrons are called ______________.

3. W5SAYW

4. Study

Element Poster Project (33 pts)

Chemical Symbol, average atomic mass, & atomic number _______ 3 points

Electron configuration _______ 3 points

All known isotopes ______ 2 points

Electron Dot Diagram ______ 2 points

At least 3 uses ______ 3 points

Atomic ParticlesAtomic ParticlesParticle Charge Mass (kg) Location

Electron

-1 9.109 x 10-31 Electron cloud

Proton +1 1.673 x 10-27 Nucleus

Neutron

0 1.675 x 10-27 Nucleus

Bell WorkBell Work•number of protons and neutrons in the nucleus of an atom.•measured in atomic mass units (amu)

Mass # = p+ + n0

Nuclide (new clyde)

p+ n0 e- Mass #

Oxygen - 9

- 33 40

- 34 15

8 8 1717

Arsenic 73 33 73

Phosphorus 15 3419

Assume the particles below are atoms, meaning they have no charge.

Bell Work 12/41. Atoms of the same element may have different

numbers of ____________, and they may gain or lose ____________, but they ALWAYS have the same number of _____________.

Bell Work 11/3Bell Work 11/3ElectronElectron

ss

NeutronsNeutrons

ProtonsProtonssubatomic particlessubatomic particles

chargedcharged+ charge+ charge- charge- charge

no chargeno chargeabout same massabout same massvery little massvery little mass

in nucleusin nucleus orbits nucleusorbits nucleusfound in atomfound in atomcathode rayscathode rays

““ee--””“n“n00””““pp++””

subatomic subatomic particlesparticles

chargedcharged

+ charge+ charge- charge- charge

no chargeno charge

about same about same massmass

sum gives sum gives atomic massatomic mass

very little massvery little mass




cathode rayscathode rays

““ee--””

““nn00””

““pp++””

ElectroElectronn

NeutronsNeutrons

ProtonsProtons

subatomic particlessubatomic particleschargedcharged+ charge+ charge- charge- charge



““ee--””“n“n00””““pp++””



in nucleusin nucleus orbits nucleusorbits nucleusfound in atomfound in atom

sum gives atomic masssum gives atomic masscathode rayscathode rays

““ee--””“n“n00””““pp++””

The Atomic The Atomic ScaleScale

Most of the mass of the atom is in the nucleus (protons and neutrons) Electrons are found outside of the nucleus (the electron cloud) Most of the volume of the atom is empty space

“q” is a particle called a “quark”

http://vimeo.com/819138

Bell Work 11/4/10Bell Work 11/4/10

1. How much would 1 gallon of mercury weigh?2. If a 185 lb man on mercury, how much volume

would you displace? (This is individual as it depends on your mass.)

3. How many m&m’s do you think are in the jar?

Mercury has a density of 13.5 cm3.Use your conversion factors…

ChargeChargeCharged atoms have an unequal number of protons & electrons and are called ions.Charge = p+ - e-

Ion p+ N0 e- Charge

Oxygen 7

11 12

56

8 10

Sodium 10

Barium +265

Size of AtomsSize of Atoms

We think of the area occupied by electrons as an “electron cloud”. Radius of atom – distance from center of nucleus to outer part of e- cloud.

Measured in picometers (pm)1 pm = 10-12 m = 1/1,000,000,000,000 meter

pm is to cm as cm is to km

Nuclei are extremely dense… 200,000,000 metric ton/cm3

= 200,000,000,000 kg/cm3

weighs 440,000,000,000 lb/cm3

Bohr Model of AtomBohr Model of Atom

1. Helium – 52. Beryllium – 113. Neon – 204. Carbon – 145. Potassium – 41

1. Find element’s atomic number on p. table.

2. Draw nucleus & write # of p+ & n0

• Mass # = p+ + n0

3. Draw electrons in orbitals

1st shell 2 e-

2nd shell 8 e-

3rd shell 8 e-

4th shell 18 e-

5th shell 18 e-

6th shell 32 e-

7th shell 32 e-

The Elements!The Elements!

1 dozen =1 gross =

1 ream =

1 mole =

12

144

500

6.02 x 1023

There are exactly 12 grams of carbon-12 in one mole of carbon-12.

Bell Work 11/10 – 5 minBell Work 11/10 – 5 min

1 mole O2 = 31.9988 g 1 mole = 6.02 x 1023

Take out yesterday’s work.How many molecules of O2 are in 85.02 g of O2? (Use dimensional analysis to find your answer.)

Avogadro’s NumberAvogadro’s Number6.02 x 1023 is called “Avogadro’s Number” in honor of the Italian chemist Amadeo Avogadro (1776-1855).

Amadeo Avogadro

I didn’t discover it. Its just named after me! (Probably cuz

I’m hot.)

Calculations with Moles:Calculations with Moles:Converting moles to gramsConverting moles to grams

How many grams of lithium are in 3.50 moles of lithium?

3.50 mol Li= g Li

1 mol Li

6.941 g Li24.2935

24.3 g Li

Calculations with Moles:Calculations with Moles:Converting grams to molesConverting grams to moles

How many moles of lithium are in 18.2 grams of lithium?

18.2 g Li= mol Li

6.941 g Li

1 mol Li2.62247

2.62 mol Li

Calculations with Moles:Calculations with Moles:Using Avogadro’s NumberUsing Avogadro’s Number

How many atoms of lithium are in 3.50 moles of lithium?

3.50 mol Li =

1 mol Li

6.022 x 1023 atoms Li 21.077 x 1023

2.1077 x 1024

2.11 x 1024

2.11 x 1024 atoms Li


How many atoms of lithium are in 18.2 g of lithium?

18.2 g Li

= atoms Li

1 mol Li 6.022 x 1023 atoms Li

1.58 x 1024

6.94 g Li 1 mol Li

(18.2)(6.022 x 1023)/6.94

Bell Work 11/11 – 5 minBell Work 11/11 – 5 minTake out your homework.How many molecules of H2O are in 6,022 g of H2O? (Use dimensional analysis to find your answer.)

Bell Work 11/15 – 5 minBell Work 11/15 – 5 min

1. During photosythesis, a 1000 leaved plant produces about 1.429 g of O2 in an hour. Convert this to moles.

2. W5SAYW

6CO2 + 6H2O (+ light energy) C6H12O6 + 6O2

Mole RatioMole Ratio

According to the above equation...if 6 mol carbon dioxide are combined with 6 mol water, how many moles of glucose will be produced?How many moles of oxygen will be produced?

This is called the mole ratio!Moles of one substance: moles of

another

6CO2 + 6H2O (+ light energy) C6H12O6 + 6O2

Mole RatioMole Ratio

In an experiment where nitric acid reacts with a penny, 3.100 g of copper (Cu) are lost and 4.489 g of nitrogen dioxide (NO2) are produced. What is the mole ratio of this reaction?

To find the mole ratio, calculate how many moles of each participate in the reaction.

Cu(s) + 4HNO3(aq) Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l)

Law of Conservation of MassLaw of Conservation of Mass

Total mass of reactants =

Total mass of products

Antoine Lavoisier

Mass is neither created nor destroyed during chemical or physical reactions.

Bell Work 11/17 – 5 minBell Work 11/17 – 5 minTake out mole conversions wksts 1 & 2.Turn your lab in if you haven’t already.1. Calculate the number of molecules in 32.47 g of water.


1. Calculate the number of in 32.47 g of water.

32.47 g H2O

=

1 mol Li 6.022 x 1023 atoms H2O

1.085409 x 1024

18.0148 g H2O 1 mol H2O

(32.47)(6.022 x 1023)/ 18.0148

From periodic table:1 mol H = 1.0079 1 mol O =

15.999 1 mol H2O = 2(1.0079 g) + 1(15.999 g) = 18.0148 g

1.085 x 1024 molecules H2O

1. How many moles of silver are in 57.00 g of Ag?

From periodic table: 1 mol Ag = 107.87 g

57.00 g Ag1

1 mol Ag107.87 g Ag

X = 0.5284138

0.5284 mol Ag

2. How many moles of gold are in 89.0 g of Au?

From periodic table: 1 mol Au = 196.97 g

89.0 g Au1

1 mol Au196.97 g Au

X = 0.4518454

0.452 mol Au

3. How many moles of iron are in 2.43 x 1025 atoms of Fe?

From your brain (Av’s #): 1 mol = 6.022 x 1023

2.43 x 1025 atoms Fe 1

1 mol Fe 6.022 x 1023 atoms Fe

X = 0.40352 x 102

4.04 x 101 mol Fe

40.4 mol Fe

4. How many atoms of copper are in 3.1 g of Cu?

From periodic table: 1 mol Cu = 63.546 g


3.1 g Cu1

1 mol Cu63.546 g Cu

X =

0.29377 x 1023

2.9 x 1022 atoms Cu

6.022 x 1023 atoms Cu1 mol Cu

X

5. How many molecules of carbon dioxide are in 86.00 g of CO2?

From periodic table: 1 mol C = 12.011 g

1 mol O = 15.999 g

Therefore: 1 mol CO2 = 1(12.011) + 2(15.999 )

= 44.009 g


86.00 g CO2

1 1 mol CO2

44.009 g CO2

X =

11.77 x 1023

1.177 x 1024 molecules CO2


1 mol CO2

X

6. How many molecules of copper sulfate are in 8 g of CuSO4?

From periodic table: 1 mol Cu = 63.546 g

1 mol S = 32.065 g

1 mol O = 15.999 g

Therefore: 1 mol CuSO4 = 1(63.546) + 1(32.065 ) + 4(15.999)

= 159.607 g


8 g CuSO4

1 1 mol CuSO4

159.607 g CuSO4

X =

0.30184 x 1023

3 x 1022 molecules CuSO4

6.022 x 1023 molecules CuSO4

1 mol CuSO4

X

8. How many atoms of oxygen are in 2.0 mol of CO2?

From chemical formula: there are 2 moles of O atoms for each mole of CO2 molecules

1 mol CO2 = 1 mol C

2.0 mol CO2

1 2 mol C 1 mol CO2

X = 4 mol C

4.0 mol O

7. How many atoms of carbon are in 2.0 mol of CO2?

From chemical formula: there are 1 mole of C atoms for each mole of CO2 molecules

1 mol CO2 = 1 mol C

2.0 mol CO2

1 1 mol C 1 mol CO2

X

1.2 x 1023 atoms

6.022 x 1023 atoms C

1 mol CX

9. How many atoms of oxygen are in 86.00 g of CO2? (See # 5)

From periodic table: 1 mol C = 12.011 g

1 mol O = 15.999 g

Therefore: 1 mol CO2 = 1(12.011) + 2(15.999 )

= 44.009 g


86.00 g CO2

1 1 mol CO2

44.009 g CO2

X

3.9082 x 1023


X


1 mol CO2

X

2 atoms CO2 1 molecule CO2

On QuizOn QuizJust like bohring worksheets!

Test TuesdayLaw of conservation of massAtomDalton’s atomic theoryIsotopesBohring worksheetProtons, neutrons, electrons (chart)Discovery of electron – who & howPlum pudding modelRutherford & gold foil experimentBohring worksheets, # e- in each shellAvagadro’s number (memorized)Mole problems1 mole ratio question

1 atomic mass unit - 1/12 the mass of a carbon-12 atom

Molecular mass (m) of a substance is the mass of one molecule of that substance, in atomic mass units(s) u

http://en.wikipedia.org/wiki/Chemical_compound

http://en.wikipedia.org/wiki/Mass

http://en.wikipedia.org/wiki/Molecule

About Quarks…About Quarks…Protons and neutrons are NOT fundamental particles.Protons are made of two “up” quarks and one “down” quark.Neutrons are made of one “up” quark and two “down” quarks.

Quarks are held together by “gluons”

ElectroElectronn

NeutronsNeutrons

ProtonsProtons




““ee--””“n“n00””““pp++””

Bell Work 11/30/11 – 5 min1. Who discovered the electron?

2. If a substance had a density of 200,000,000,000 kg/cm3, how much mass would be in a 32.7 cm3 sample?

3.One kilogram weighs 2.2 lbs. How much would the sample weigh?


1. 25 m = ? km

2. Who named the atom?

3. W5SAYWorS


1. What did J.J. Thomson discover?

2. Explain J.J. Thomson’s model of the atom.

3. What atom is represented in the Bhor diagram below?

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