Spark

On the blank table in write the formulas for as many elements as possible from memory. Use a pencil so in case you make a mistake. You are not graded on this, so do not bother cheating.

Now look at a table and find your top five favorite elements and label them.

Elements on today's periodic table are arranged byincreasing atomic number...

http://youtu.be/GVoJZkmAAfA

http://youtu.be/uixxJtJPVXk

http://youtu.be/m55kgyApYrY

the lanthanide and actinide series are separated from the main body...

f block

AND the d block elements...

separate the main body elements.

s block p block

1 2 VALENCES 3 4 3 2 1 0

Fluorine is the most active nonmetal

Francium is the most active metal

http://youtu.be/mG6EG_igTGw

http://youtu.be/QSZ-3wScePM

http://youtu.be/pWXQ2tYzJaU http://youtu.be/ii6DmB0cX_w

http://youtu.be/92Mfric7JUc

http://youtu.be/MTcgo46nxNE

http://youtu.be/fLJ4FH7q0EQ

The Nobel GasFamily ischemicallyinactive.

http://youtu.be/QLrofyj6a2s

Vertical columns are Families -

elements with similar properties.

Alkali Metals

Alkaline Earth Metals

Transition Metals

Rare Earth Metals

Boron Family

Carbon Family

Nitrogen Family

Oxygen Family

Halogen Family

Nobel Gas Family

Every element is representedby a single square.

Each square containsthree things:

1. The chemical symbol for the element.

If there are two letters,the first is ALWAYSa capital letter, and the second is ALWAYSa small letter.

1. The chemical symbol for the element.

Solid

The symbols on some tables indicate the physical state at room temperature.

Liquid Gas

Au Hg Ne

2. A whole number representing the atomic number.

The atomic number is notalways in the sameplace on everyperiodic table -but it is ALWAYSa whole number.

2. A whole number representing the atomic number.

The atomic number is definedas the number ofprotons in the atom.

2. A whole number representing the atomic number.

Normal atoms have an equalnumber of protonsand electrons - so,the atomic numberis also equal to theelectrons in an atom.

2. A whole number representing the atomic number.

Chemists can change thenumber of electrons inan atom, but theycan NOT change thenumber of protonsin an atom.

2. A whole number representing the atomic number.

Changing the number ofprotons changes theelement into anotherelement - this canonly happen in anuclear reaction.

3. A decimal fraction number representing the element's average atomic mass.

3. A decimal fraction number representing the element's average atomic mass.

The atomic massof an element isthe sum of itsprotons andneutrons.

Atoms of an element all havethe same numbers of protons,but they can have differentnumbers of neutrons.

H1

1.00794

Hydrogen-1Hydrogen-2Hydrogen-3

Atoms of an element all havethe same numbers of protons,but they can have differentnumbers of neutrons.

H1

1.00794

Hydrogen-1Hydrogen-2Hydrogen-3

How manyneutrons?

Atoms of an element all havethe same numbers of protons,but they can have differentnumbers of neutrons.

H1

1.00794

Hydrogen-1Hydrogen-2Hydrogen-3

0

Atoms of an element all havethe same numbers of protons,but they can have differentnumbers of neutrons.

H1

1.00794

Hydrogen-1Hydrogen-2Hydrogen-3

How manyneutrons?

Atoms of an element all havethe same numbers of protons,but they can have differentnumbers of neutrons.

H1

1.00794

Hydrogen-1Hydrogen-2Hydrogen-3

1

Atoms of an element all havethe same numbers of protons,but they can have differentnumbers of neutrons.

H1

1.00794

Hydrogen-1Hydrogen-2Hydrogen-3

How manyneutrons?

Atoms of an element all havethe same numbers of protons,but they can have differentnumbers of neutrons.

H1

1.00794

Hydrogen-1Hydrogen-2Hydrogen-3

2

Atoms of the same elementwith different numbers of neutrons are called isotopes.

H1

1.00794

Hydrogen-1Hydrogen-2Hydrogen-3

Which of hydrogen's threeisotopes is the most common?

H1

1.00794

Hydrogen-1Hydrogen-2Hydrogen-3

Which of hydrogen's threeisotopes is the most common?

H1

1.00794

Hydrogen-1Hydrogen-2Hydrogen-3

Usually, you can round off all mass numbers to the nearest

WHOLE number.

Spark 10/24/2011

• Please complete the chart using your periodic table as quickly as possible! We have a lot to do today!

The first group done will get the most points with later groups earning fewer.

The emphasis is doing this type of activity quickly!

Why does the periodic table stop?Can we make new elements? How?

Is Seaborg a “creator” or elemental “god”?

Remember the physicist building materials for the Universe…

http://www.pbs.org/wgbh/nova/physics/stability-elements.html

A final word about Mendeleev’s Table…

• Mendeleev’s combining powers or valences• Metals do not form compounds with other

metals• Metals and non-metals react as do non-metals

with non-metals • How?• Why?• Who cares? • http://youtu.be/zGM-wSKFBpo

Just when you thought it was only

Protons Neutrons And Electrons…

“HA HA HA! It never stops! Never! There’s always more!You will never know it all! MUAH HAH HAH HAH! Always more!”

- THE ATOMIC THEORY

Vertical columns are Families -

elements with similar properties.

Alkali Metals

Alkaline Earth Metals

Transition Metals

Rare Earth Metals

Boron Family

Carbon Family

Nitrogen Family

Oxygen Family

Halogen Family

Nobel Gas Family

Spark No Computers!• How do you study something that is invisible?

“Ya throw stuff at it n’see how it bounces off, duh!” -Sam “Bhatman” Bhat,

atomic researcher, politician, toe nail enthusiast

• Complete the projectile activity by using a straightedge and common sense to determine the shape of the invisible object inside the box.

– Some projectiles pass straight through in one side and out the other (they hit nothing).

– Some projectiles go in, hit something, and are reflected back out (dbl sided arrow)

– Some projectiles go in, hit something, and are deflected out at an angle. Retrace the paths and see where they intersect.

http://mogk12.2ya.com/rutherford

http://library.thinkquest.org/19662/low/eng/index.html

Atom – The Incredible World (Thinkquest)

Record what you observed, what you changed/did, what you learned for each virtual lab!

Download the worksheets and complete the lab and questions. Turn it in when you are done.

Virtual Labs• Interactives: http://phet.colorado.edu/ • Click “play with sims” then “chemistry” then “Run

Now”– States of Matter– Balloons and static electricity– Rutherford Scattering– Build an Atom – Tutorial and Game– Isotopes and Atomic Mass– Atomic Interactions– Models of the Hydrogen Atom

Record what you observed, what you changed/did, what you learned for each virtual lab!

You will hand in your labs!

Virtual Labs• http://www.rsc.org/chemsoc/visualelements/

pages/pertable_fla.htm (Visual Elements Periodic Table)

Dalton’s Model

• In the early 1800s, the English Chemist John Dalton performed a number of experiments that eventually led to the acceptance of the idea of atoms.

Dalton’s Theory

• He deduced that all elements are composed of atoms. Atoms are indivisible and indestructible particles.

• Atoms of the same element are exactly alike.

• Atoms of different elements are different.

• Compounds are formed by the joining of atoms of two or more elements.

.

• This theory became one of the foundations of modern chemistry.

Thomson’s Plum Pudding Model

• In 1897, the English scientist J.J. Thomson provided the first hint that an atom is made of even smaller particles.

Thomson Model

• He proposed a model of the atom that is sometimes called the “Plum Pudding” model.

• Atoms were made from a positively charged substance with negatively charged electrons scattered about, like raisins in a pudding.

Thomson Model• Thomson studied

the passage of an electric current through a gas.

• As the current passed through the gas, it gave off rays of negatively charged particles.

Cathode Ray Tube

Thomson Model

• This surprised Thomson, because the atoms of the gas were uncharged. Where had the negative charges come from?

Where did they come from?

Thomson concluded that the negative charges came from within the atom.

A particle smaller than an atom had to exist.

The atom was divisible!

Thomson called the negatively charged “corpuscles,” today known as electrons.

Since the gas was known to be neutral, having no charge, he reasoned that there must be positively charged particles in the atom.

But he could never find them.

Cathode Rays

Had mass – albeit a very small amount; they pushed a lightweight paddlewheel up an incline.

They could do work!

Had direction – they passed from the negative to the positive electrode

Had charge they bent in an electric field (towards the positive plate) and in a magnetic field

Rutherford’s Gold Foil Experiment

• In 1908, the English physicist Ernest Rutherford was hard at work on an experiment that seemed to have little to do with unraveling the mysteries of the atomic structure.

• Rutherford’s experiment Involved firing a stream of tiny positively charged particles at a thin sheet of gold foil (2000 atoms thick)

• http://chemmovies.unl.edu/ChemAnime/RUTHERFD/RUTHERFD.html

http://chemmovies.unl.edu/ChemAnime/http://chemmovies.unl.edu/ChemAnime/RUTHERFD/RUTHERFD.htmlRUTHERFD/RUTHERFD.html

Alpha Particles = He nucleus2p+ + 2no

– Most of the positively charged “bullets” passed right through the gold atoms in the sheet of gold foil without changing course at all.

– Some of the positively charged “bullets,” however, did bounce away from the gold sheet as if they had hit something solid. He knew that positive charges repel positive charges.

You Try

• The radius of a hydrogen atom is 5 x 10-11

meters. The radius of a single proton is 5 x 10-

16 meters. Assuming that atoms take the most size – efficient shape, a sphere, determine how much of an atom is truly empty space free of matter.

• Vsphere = 4/3 π r3

Rutherford vs Thomson

• This could only mean that the gold atoms in the sheet were mostly open space. Atoms were not a pudding filled with a positively charged material.

• Rutherford concluded that an atom had a small, dense, positively charged center that repelled his positively charged “bullets.”

• He called the center of the atom the “nucleus”• The nucleus is tiny compared to the atom as a whole.

Crammin’ Spark

You will have a quiz on the correct placement of elements on the table from memory.

You Try

• The radius of a hydrogen atom is 5 x 10-11

meters. The radius of a single proton is 5 x 10-

16 meters. Assuming that atoms take the most size – efficient shape, a sphere, determine how much of an atom is truly empty space free of matter.

• Vsphere = 4/3 π r3

Rutherford• Rutherford reasoned

that all of an atom’s positively charged particles were contained in the nucleus.

• The negatively charged particles were scattered outside the nucleus around the atom’s edge.

Bohr Model• In 1913, the Danish

scientist Niels Bohr proposed an improvement. In his model, he placed each electron in a specific energy level.

Where did I put my electrons?

Bohr Model• According to Bohr’s

atomic model, electrons move in definite orbits around the nucleus, much like planets circle the sun. These orbits, or energy levels, are located at certain distances from the nucleus.

The Wave Model

• Today’s atomic model is based on the principles of wave mechanics.

• According to the theory of wave mechanics, electrons do not move about an atom in a definite path, like the planets around the sun.

Wave Model

Electrons are defined by 3-D regions of probability where electrons are found “most” often

But where are they when they’re not where we expect?

A final word about Mendeleev’s Table…

• Mendeleev’s combining powers or valences• Metals do not form compounds with other

metals• Metals and non-metals react as do non-

metals with non-metals • How?• Why?• Who cares?

It’s the electrons

• The nucleus does not change.• The number of electrons do change

– Atoms become “ions” and they are attracted to oppositely charged particles

– Ions are named according to Faraday and his study of electrolytes (salt water) and conduction

• The combining powers that Mendeleev found reflect the amount of negative charge lost or gained during a reaction

The oxidation number of an element indicates the number of electrons gained or lost when forming compounds.

Elements with positive oxidation numbers lose electrons. (cation)

Elements with negative oxidation numbers gain electrons. (anion)

+1

+2

+1, +2, +3

+3

+4 or -4

-3

-2

-1

Electron energy levels, from 1 to 7

Electron energy sublevels

Electron energy sublevel s

Electron energy sublevel p

Electron energy sublevel d

Electron energy sublevel f

Each "pair" of boxes in a sublevelindicates an orbital. Each orbital can hold up to 2 electrons…

How many electrons fit in the 3rd energy level? What about the 4th?Count the boxes to find your answer…

3

4

8

18

An Electron Configuration showsthe exact location of every electronin an atom.1s2 2s2 2p6 = Configuration for Neon

With very few exceptions, theelectron configuration of an atomcan be read directly from the Table.

S block

P block

D Block

F block

Electron Energy Levels Match Up with the Rows of the Periodic Table