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Atomic Structure Do you know your atomic structure?

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Atomic Structure. Do you know your atomic structure?. Basic Unit of Matter. ATOM Sodium Atom Animation. What is the charge of each subatomic particle?. Proton neutron electron + O - positive none negative. - PowerPoint PPT Presentation

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Page 1: Atomic Structure

Atomic Structure

Do you know your atomic structure?

Page 2: Atomic Structure

Basic Unit of Matter

•ATOM• Sodium Atom Animation

Page 3: Atomic Structure

What is the charge of each subatomic particle?

• Proton neutron electron

• + O -• positive none negative

Page 4: Atomic Structure

Where are they found in the atom?

Neutron and proton – in the nucleus

Electron –outside the nucleus

Helium atom animation

Page 5: Atomic Structure

Chemical Element

• A pure substance that consists on only one type of atom

Page 6: Atomic Structure

Pure Substance: Iodine

Page 7: Atomic Structure

Atom

• EX: every atom in a gold block looks like all the other gold atoms

Page 8: Atomic Structure

Periodic Table of the Elements

Mendeleev

Page 9: Atomic Structure

Element Song(link)

“The Elements” by Tom Lehrer

• There’s antimony, arsenic, aluminum, selenium,And hydrogen and oxygen and nitrogen and rheniumAnd nickel, neodymium, neptunium, germanium,And iron, americium, ruthenium, uranium,Europium, zirconium, lutetium, vanadiumAnd lanthanum and osmium and astatine and radiumAnd gold, protactinium and indium and galliumAnd iodine and thorium and thulium and thallium.

• There’s yttrium, ytterbium, actinium, rubidiumAnd boron, gadolinium, niobium, iridiumAnd strontium and silicon and silver and samarium,And bismuth, bromine, lithium, beryllium and barium.

• There’s holmium and helium and hafnium and erbium

• And phosphorous and francium and fluorine and terbiumAnd manganese and mercury, molybdinum, magnesium,Dysprosium and scandium and cerium and cesiumAnd lead, praseodymium, platinum, plutonium,Palladium, promethium, potassium, polonium,Tantalum, technetium, titanium, tellurium,And cadmium and calcium and chromium and curium.

• There’s sulfur, californium and fermium, berkeliumAnd also mendelevium, einsteinium and nobeliumAnd argon, krypton, neon, radon, xenon, zinc and rhodiumAnd chlorine, cobalt, carbon, copper,Tungsten, tin and sodium.

• These are the only ones of which the news has come to Harvard,And there may be many others but they haven’t been discovered.

Page 10: Atomic Structure

Symbols of Elements

• 1. First letter is capitalized• 2. Second letter (if there is one) is

always lower case• EXAMPLES:• C F Al• Cl B Mn• Ca H Mg• Cr O Mo

Page 11: Atomic Structure

Which are symbols?Abbreviations for elements

• C CO Mn CO2 Ni Why?

•C Mn Ni

• Only one capital letter

Page 12: Atomic Structure

Trace Elements

Needed by some organisms but only in very small amountsLike iodine, we need only 0.15 mg per dayA deficiency will cause a goiter

Page 13: Atomic Structure

What are trace elements?

• Needed in the body in only small amounts

• Like mg (milligrams)• WHY IMPORTANT IF WE DON’T

NEED SO MUCH?• Minerals act as catalysts (speed up

reactions) for many biological reactions

Page 14: Atomic Structure

EACH ELEMENT: All the same atoms

• Photographic Periodic Table (link)

Page 15: Atomic Structure

Which are elements?

• Cu• C• CO• Co• N• NO• WHY?• Cu C N only

one kind of matter

Page 17: Atomic Structure
Page 18: Atomic Structure

Mass Number

• Protons plus neutrons

• Decimal number

• Will round off the number

• Average of masses of many atoms

Page 19: Atomic Structure

Mass Number

• Mass of nucleus

Page 20: Atomic Structure

What about that decimal for mass number?

= Average of all isotopes of carbon

Page 21: Atomic Structure

• Mass Number • Atomic Number

What is the mass number of Na?

Page 22: Atomic Structure

Atomic Number?Mass Number?

Page 23: Atomic Structure

HOW TO FIND

• Number of Protons = Atomic Number

• Number of Electrons = Number of Protons = Atomic Number

• Number of Neutrons = Mass Number - Atomic Number

Page 24: Atomic Structure

How many?

• Protons electrons neutrons

• Carbon

6 6 6• Chlorine

• 17 17 18

Page 25: Atomic Structure

What’s a neutral atom?

• Number of protons = number of electrons

• Example: carbon has 6 e-and 6 p+

Page 27: Atomic Structure

Same Number of electrons as protons

• WHY?

• So the atom will be neutral (no excess charge)

Page 28: Atomic Structure

What is the mass number of…?

• Carbon nitrogen hydrogen

• WHY?

• 12 14 1

• Decimal number on periodic table

• Not other number in succession

• Number of p + n

Page 29: Atomic Structure

What is the atomic number of?

• Silicon fluorine sodium WHY?

• 14 9 11• Number in succession (not

a decimal)• Number of protons

Page 30: Atomic Structure

How do you find the number of…?

• Protons electrons neutrons

• Atomic atomic mass no.

Number number minus

(if neutral) At. No.

Page 31: Atomic Structure

YOU NEED TO KNOW

• The Names (spelled correctly) and the Symbols (written correctly)

• “Naturally Occurring Elements in the Human Body”

Page 32: Atomic Structure

Radioisotopes

• All elements with atomic numbers greater than 83 are radioisotopes meaning that these elements have unstable nuclei and are radioactive and some under 83 have isotope forms.

Page 33: Atomic Structure

Isotope: form of an element with a different number of neutrons

Page 34: Atomic Structure

What makes atoms radioactive?Their nuclei are unstable and

they break down at a constant rate over time…and they have uneven numbers of protons and neutrons. Radioactive Decay of Uranium

Page 35: Atomic Structure

Some Radioactive Elements

Page 36: Atomic Structure

Radioactive Particles Given Off

Page 38: Atomic Structure

Isotopes

• Are atoms of the same element that differ in the number of neutrons!

Page 39: Atomic Structure

Number of neutrons? Isotopes? Which is the neutral form?

Page 40: Atomic Structure
Page 41: Atomic Structure

Which has more uneven number of protons and neutrons?

Number of Protons

Page 42: Atomic Structure

Positive Uses of Radioisotopes

PET SCAN

Iodine-131 treat thyroid cancer

Sr 89 treat bone and prostate cancer

Page 43: Atomic Structure

Uses of Radioisotopes

• Positron Emission Tomography

Sterillizing food and medical equipment

Radioactive dating

tracers

Cancer treatment

Page 44: Atomic Structure

Technetium-99m

has become the most widely used (80%) radioisotope for diagnosing diseased organs (especially brain, heart, and bone)

Page 45: Atomic Structure

Which are isotopes?

• 16 20 38 128 12 O F K I C

8 9 19 53 6 WHY?

20 38 128 F K I 9 19 53 different # neutrons

Page 46: Atomic Structure

Formula

• Abbreviation for a compound

• A COMPOUND is two or more elements chemically bound:

Page 47: Atomic Structure

Which are formulas?Abbreviation for a compound

• H2SO4 Cl2 H20 Al Why?

H2SO4 H20 abbreviations for compounds (2 or more different kinds of elements)

Page 48: Atomic Structure

What is a compound?

• 2 or more different elements chemically joined (2+ diff.

capital letters)

• HCl H2O

• H2SO4 NOT O2

Page 49: Atomic Structure

Which are atoms?

• C N N2 H20 Why?

• C and N only one in number

Page 50: Atomic Structure

Using The Correct Term(get handout)

• Element• Compound

• Symbol• Formula

• Atom• Molecule

• 1 kind of Atom, Na, H• 2 or more different kinds of

elements chemically joined, NaCl• Abbreviation of an element, H, Cl

• Abbreviation of a compound Na2S

• 1 unit of matter H Na Cl• 2 or more atoms chemically

joined H2, NaCl

Page 51: Atomic Structure

Which are compounds?

• Na N H2 NO2 H2O Why?

• NO2

• H2O

• 2 or more different elements chemically joined (2+ diff. capital letters)

Page 52: Atomic Structure

What’s the difference?

• Co CO co

• Symbol formula nuttin

Page 53: Atomic Structure

Which are molecules?

• Co CO CO2 O2 Why?

• CO CO2 O2 two or more atoms (alike or not alike, it doesn’t matter) bonded together

Page 54: Atomic Structure

What are the four…• Most abundant elements in living

matter?

C H O N

Page 55: Atomic Structure

What is the relative size?

• Proton neutron electron

• 1 amu 1 amu ~1/2000

• amu

• AMU=atomic mass unit= 1/12 CARBON ATOM

Page 56: Atomic Structure
Page 57: Atomic Structure

How do electrons arrange?

• In the outer shells?

• 2, 8, 8• Fill inner shell first, then

go to next shell out

Page 58: Atomic Structure

Get kinda complicated beyond 2,8,8…so that’s all

we’ll do for now!

Page 59: Atomic Structure

Atoms that have the same number of electrons have the same

chemical properties.

Page 60: Atomic Structure

How many electrons in each shell?

• C O F Na

• 2,4 2,6 2,7 2,8,1

Page 61: Atomic Structure

What are ions?

• Charged atoms

• Have lost or gained

an electron

Page 62: Atomic Structure

Lost or Gained How Many e-?

• H+ Li+ Na+ K+

• Be+2 Mg+2 Ca+2

• Al+3

• F- Cl- Br- I-

• S-2

• Lost one e-

• Lost 2 e-

• Lost 3 e-

• Gained one e-

• Gained 2 e-

Page 63: Atomic Structure

Note Ions and Formulas

• Na+ Cl-+1 -1 NaCl 1:1

• Mg2+ Cl-+2 -1 MgCl2 1:2

• Na+ S 2-+1 -2 Na2S 2:1

• Mg2+ S 2-+2 -2 MgS 1:1

Page 64: Atomic Structure

Which are ions?

• Cl O-2 Na+1 N2

Why?

• O-2 Na+1

• Charged atoms (lost or gained electrons)

• show charges as superscripts

Page 65: Atomic Structure

Which electrons determine…

• The chemical properties of the atom?

• Outermost shell

Page 66: Atomic Structure

Periodic Table Hint:

• You can tell how many electrons are in an atom’s outermost shell by just looking at its position on the periodic table!!!!!

Page 67: Atomic Structure

1 2

3 4 5 6 7 8

e- in outer shells

Page 68: Atomic Structure

Which atoms combine…

• with other atoms?

• Ones that do not have filled outer electron shells

Page 69: Atomic Structure

What is the driving force to make atoms join with other atoms to form compounds?

• TO HAVE FILLED OUTER ELECTRON SHELLS!!!!!!!!!!!!!!!!!!!!!!!!

Page 70: Atomic Structure

How does an atom…

• Get a filled outer electron shell?

• Gaining, losing, or sharing electrons

Page 71: Atomic Structure

If one electron is…

• Lost what charge will the ion have?

•+1

Page 72: Atomic Structure

If one electron is gained…

• What charge will the ion have?

•-1

Page 73: Atomic Structure

If 2 electrons are lost…

• What charge will the ion have?

•+2

Page 74: Atomic Structure

If two electrons are gained…

• What charge will the ion have?

•-2

Page 75: Atomic Structure

Making Correct Formulas:

• Note how the ion charge becomes the subscript of the other ion

• Na+ Cl- NaCl

• Mg2+ Cl- MgCl2

• Na+ S-2 Na2S

• Mg2+ S-2 MgS

Page 76: Atomic Structure

What do we call the forces that…

• Hold atoms together in a molecule?

• Chemical bonds…not to be confused with James Bond

Page 77: Atomic Structure

IONIC BOND

• What makes up ionic bonds?

• IONS

• WHY?

• Opposite charged ions attract

Page 78: Atomic Structure

Covalent Bond

• What makes up covalent bonds?

• Atoms that are sharing electrons

Page 79: Atomic Structure

Comparing Bonds

IONIC BOND (gain or lose e-)

COVALENT BOND (sharing e-)

Page 80: Atomic Structure

How can covalent bonds be written?

• Single bond double bond triple bond

• C-C C=C C=C• C:C C::C C:::C