This PowerPoint roadmap is one small part of my Atoms and Periodic Table Unit. This unit includes a four part 2000+ slide PowerPoint roadmap. 13 page bundled homework that chronologically follows slideshow 14 pages of unit notes with visuals. 3 PowerPoint review games. Activity sheets, rubrics, advice page, curriculum guide, materials list, and much more. http://sciencepowerpoint.com/Atoms_Periodic_Table_of_Elements_Unit.html

Purchase the entire four curriculum, 35,000 slides, hundreds of pages of homework, lesson notes, review games, and much more. http://sciencepowerpoint.com/Atoms_Periodic_Table_of_Elements_Unit.html Please feel free to contact me with any questions you may have. Thanks again for your interest in this curriculum.\ Sincerely, Ryan Murphy M.Ed www.sciencepowerpoint@gmail.com

Balancing Chemical Equations. Atomic Bonding, Balancing Chemical Equations. Part IV

RED SLIDE: These are notes that are very important and should be recorded in your science journal. Copyright © 2010 Ryan P. Murphy

-Nice neat notes that are legible and use indents when appropriate -Nice neat notes that are legible and use indents when appropriate. -Example of indent. Proton Electron Neutron

-Nice neat notes that are legible and use indents when appropriate -Nice neat notes that are legible and use indents when appropriate. -Example of indent. -Skip a line between topics Proton Electron Neutron

-Nice neat notes that are legible and use indents when appropriate -Nice neat notes that are legible and use indents when appropriate. -Example of indent. -Skip a line between topics --Make visuals clear and well drawn. Label please. Proton Electron Neutron

RED SLIDE: These are notes that are very important and should be recorded in your science journal. BLACK SLIDE: Pay attention, follow directions, complete projects as described and answer required questions neatly. Copyright © 2010 Ryan P. Murphy

Keep an eye out for “The-Owl” and raise your hand as soon as you see him. He will be hiding somewhere in the slideshow Copyright © 2010 Ryan P. Murphy

“Hoot, Hoot” “Good Luck!” Copyright © 2010 Ryan P. Murphy

Balancing Chemical Equations. Atomic Bonding, Balancing Chemical Equations. Part IV

New Area of focus: Atomic Bonding Copyright © 2010 Ryan P. Murphy

New Area of focus: Atomic Bonding Copyright © 2010 Ryan P. Murphy

Chemical Bonding: The attraction that holds atoms close to each other. Copyright © 2010 Ryan P. Murphy

Chemical Bonding: The attraction that holds atoms close to each other. Copyright © 2010 Ryan P. Murphy

Ionic, Covalent, Metallic Copyright © 2010 Ryan P. Murphy

Ionic, Covalent, Metallic Copyright © 2010 Ryan P. Murphy

Ionic, Covalent, Metallic Covalent – Share electrons Copyright © 2010 Ryan P. Murphy

Ionic, Covalent, Metallic Covalent – Share electrons Copyright © 2010 Ryan P. Murphy

Ionic, Covalent, Metallic Covalent – Share electrons Ionic – Gain or lose electrons (transfer) Copyright © 2010 Ryan P. Murphy

Ionic, Covalent, Metallic Covalent – Share electrons Ionic – Gain or lose electrons (transfer) Copyright © 2010 Ryan P. Murphy

Ionic, Covalent, Metallic Covalent – Share electrons Ionic – Gain or lose electrons (transfer) Metallic- Many free electrons Copyright © 2010 Ryan P. Murphy

“My name is Bond.” Copyright © 2010 Ryan P. Murphy

“Covalent Bond.” Copyright © 2010 Ryan P. Murphy

Covalent bonding occurs by a sharing of valence electrons Copyright © 2010 Ryan P. Murphy

Covalent bonding occurs by a sharing of valence electrons Copyright © 2010 Ryan P. Murphy

Covalent bonding occurs by a sharing of valence electrons (Strongest) Copyright © 2010 Ryan P. Murphy

Covalent bonding occurs by a sharing of valence electrons (Strongest) (SPONCH). Copyright © 2010 Ryan P. Murphy

occurs on the next slide. Make an electrostatic sound when the bond occurs on the next slide.

Ionic bonding (+/-) Bonds created by the attraction of opposite charges. Copyright © 2010 Ryan P. Murphy

“Ionic Please.” “Transferred.” “Not shared.”

Ionization: The process of removing electrons from an atom to form ions. Copyright © 2010 Ryan P. Murphy

Ionic - One atom strips electron from the other so both are now stable Ionic - One atom strips electron from the other so both are now stable. Held then by + / - charge Copyright © 2010 Ryan P. Murphy

Ionic - One atom strips electron from the other so both are now stable Ionic - One atom strips electron from the other so both are now stable. Held then by + / - charge Copyright © 2010 Ryan P. Murphy

Ionic - One atom strips electron from the other so both are now stable Ionic - One atom strips electron from the other so both are now stable. Held then by + / - charge Copyright © 2010 Ryan P. Murphy

Ionic Bonding: Forms crystal lattice. Copyright © 2010 Ryan P. Murphy

Learn more: http://web.jjay.cuny.edu/~acarpi/NSC/5-bonds.htm

Video: Ionic and Covalent Bonds http://www.youtube.com/watch?v=Kj3o0XvhVqQ&feature=results_main&playnext=1&list=PL85B1E4851BDEE325

Metallic bonding: The bonding between atoms within metals Metallic bonding: The bonding between atoms within metals. The sharing of many free electrons. Copyright © 2010 Ryan P. Murphy

Metallic bonding: The bonding between atoms within metals Metallic bonding: The bonding between atoms within metals. The sharing of many free electrons. Learn more: http://www.chemguide.co.uk/atoms/bonding/metallic.html Copyright © 2010 Ryan P. Murphy

Activity! Generating heat by breaking metallic bonds. Copyright © 2010 Ryan P. Murphy

Activity. Generating heat by breaking metallic bonds Activity! Generating heat by breaking metallic bonds. Wear Safety Goggles. Copyright © 2010 Ryan P. Murphy

Activity! Generating heat by breaking metallic bonds. Bend spoon back and forth to generate very hot temperatures, WATCH OUT! Copyright © 2010 Ryan P. Murphy

Activity! Generating heat by breaking metallic bonds. Bend spoon back and forth to generate very hot temperatures, WATCH OUT! Do not try this in the lunchroom! Copyright © 2010 Ryan P. Murphy

Video! Ionic and Covalent Bonding. http://www.youtube.com/watch?v=QqjcCvzWwww

Video Link! (Optional) Khan Academy, Atomic Bonding. http://www.khanacademy.org/video/ionic--covalent--and-metallic-bonds?playlist=Chemistry

Ion: A charged atom. When an atom strips an electron, now one atom has 1+ (cation), and the other has 1 – (anion), Copyright © 2010 Ryan P. Murphy

Ion: A charged atom. When an atom strips an electron, now one atom has 1+ (cation), and the other has 1 – (anion), Copyright © 2010 Ryan P. Murphy

Cats. I love cats, Cats are positive. Ion: A charged atom. When an atom strips an electron, now one atom has 1+ (cation), and the other has 1 – (anion), “+1 Cation, Animal hoarding adds Cats. I love cats, Cats are positive. Copyright © 2010 Ryan P. Murphy

Ion: A charged atom. When an atom strips an electron, now one atom has 1+ (cation), and the other has 1 – (anion), Copyright © 2010 Ryan P. Murphy

Ion: A charged atom. When an atom strips an electron, now one atom has 1+ (cation), and the other has 1 – (anion), Copyright © 2010 Ryan P. Murphy

“Hoot” “Hoot” “Did anybody see me on that charged atom.” Ion: A charged atom. When an atom strips an electron, now one atom has 1+ (cation), and the other has 1 – (anion), “Hoot” “Hoot” “Did anybody see me on that charged atom.” Copyright © 2010 Ryan P. Murphy

“Hoot” “Hoot” “Did anybody see me on that charged atom.” Ion: A charged atom. When an atom strips an electron, now one atom has 1+ (cation), and the other has 1 – (anion), “Hoot” “Hoot” “Did anybody see me on that charged atom.” Copyright © 2010 Ryan P. Murphy

The closer and more tightly bound an electron is to the nucleus, the more difficult it will be to remove, and the higher its ionization energy will be.

Nightmare Protons stink! This is the worst. I hate being in this shell.

Electrons are negative - Nightmare Protons stink! This is the worst. I hate being in this shell.

Electrons are negative - Nightmare Protons stink! I’m so happy. This is the worst. This is so nice I hate being in this shell.

Electrons are negative - Nightmare Protons stink! I’m so happy. This is the worst. This is so nice I hate being in this shell. Protons are positive +

Electrons are negative - Protons are positive +

Electrons are negative - The atom has a neutral charge when the number is the same. Protons are positive +

Electrons are negative - The atom has a neutral charge when the number is the same. When you remove an electron Protons are positive +

Electrons are negative - The atom has a neutral charge when the number is the same. When you remove an electron the atom becomes more positive Protons are positive +

Electrons are negative - The atom has a neutral charge when the number is the same. Yay, we lost Grumpy. I feel so more positive. When you remove an electron the atom becomes more positive Protons are positive +

Electrons are negative - The atom has a neutral charge when the number is the same. Yay, we lost Grumpy. I feel so more positive. When you remove an electron the atom becomes more positive (Cation +) Protons are positive +

Electrons are negative - The atom has a neutral charge when the number is the same. When you remove an electron the atom becomes more positive (Cation +) Protons are positive +

Electrons are negative - The atom has a neutral charge when the number is the same. When you remove an electron the atom becomes more positive (Cation +) Protons are positive +

Electrons are negative - The atom has a neutral charge when the number is the same. When you add an electron the atom becomes more negative. When you remove an electron the atom becomes more positive (Cation +) Protons are positive +

Electrons are negative - The atom has a neutral charge when the number is the same. When you add an electron the atom becomes more negative. Anion - When you remove an electron the atom becomes more positive (Cation +) Protons are positive +

Electrons are negative - The atom has a neutral charge when the number is the same. When you add an electron the atom becomes more negative. Anion - More negativity When you remove an electron the atom becomes more positive (Cation +) Protons are positive +

Which atom below is the anion, and which is the cation?

Sodium formed a cation because it lost 1 electron and became positive.

Sodium formed a cation because it lost 1 electron and became positive. Add cats, Cats are +

Chlorine formed an anion because it gained -1 electron. More negative. Add cats, Cats are + Anion

Which atom below formed a cation, and which formed an anion?

Which atom below formed a cation, and which formed an anion?

Which atom below formed a cation, and which formed an anion?

Which atom below formed a cation, and which formed an anion?

Which atom below formed a cation, and which formed an anion?

Which Gnome is the Cation, and which Gnome is the Anion? Copyright © 2010 Ryan P. Murphy

Which Gnome is the Cation, and which Gnome is the Anion? Cation +1 gives an electron Copyright © 2010 Ryan P. Murphy

Which Gnome is the Cation, and which Gnome is the Anion? Cation +1 gives an electron Copyright © 2010 Ryan P. Murphy

Which Gnome is the Cation, and which Gnome is the Anion? Cation +1 gives an electron Anion -1 accepts an electron Copyright © 2010 Ryan P. Murphy

Electron Affinity: The amount of energy required to detach an electron from a singly charged negative ion. Copyright © 2010 Ryan P. Murphy

Will this atom want to lose this valence electron, or gain many electrons to have a full outer shell? Copyright © 2010 Ryan P. Murphy

Answer: This Potassium atom will want to lose this electron Answer: This Potassium atom will want to lose this electron. It has a low electron affinity. Copyright © 2010 Ryan P. Murphy

Who wants it? Copyright © 2010 Ryan P. Murphy

Who wants it? Copyright © 2010 Ryan P. Murphy

Is this Ionic, Covalent, or Metallic Bond? Who wants it? Copyright © 2010 Ryan P. Murphy

Is this Ionic, Covalent, or Metallic Bond? Who wants it? Copyright © 2010 Ryan P. Murphy

Is this Ionic, Covalent, or Metallic Bond? Who wants it? It is ionic because it's a bond between a metal(potassium) and a non-metal(chlorine). Potassium has one electron in its valence shell, and chlorine has seven electrons in its valence shell. Following the octet rule, the potassium gives an electron to the chlorine. Then the negatively charged chlorine ion and the positively charged potassium ion stick together because of their opposite charges. Ionic bonds give electrons, covalent bonds share electrons Who wants it? Is this Ionic, Covalent, or Metallic Bond? Copyright © 2010 Ryan P. Murphy

Will this atom want to lose these valence electrons, or gain one electron to have a full outer shell? Copyright © 2010 Ryan P. Murphy

Answer: This Chlorine atom will want to gain one electron rather than lose seven. Copyright © 2010 Ryan P. Murphy

Answer: This Chlorine atom will want to gain one electron rather than lose seven. It has a high electron affinity. Copyright © 2010 Ryan P. Murphy

Learn more: Ionization. http://www.wisegeek.com/what-is-ionization.htm Answer: This Chlorine atom will want to gain one electron rather than lose seven. It has a high electron affinity. Learn more: Ionization. http://www.wisegeek.com/what-is-ionization.htm Copyright © 2010 Ryan P. Murphy

Which atom below has a high electron affinity, and which has a low electron affinity? Fluorine Sodium High Electron Affinity Low Electron Affinity A B Fluorine Sodium Copyright © 2010 Ryan P. Murphy

A B Fluorine Sodium Answers: Fluorine Sodium High Electron Affinity Low Electron Affinity A B Fluorine Sodium Copyright © 2010 Ryan P. Murphy

A B Fluorine Sodium Answers: Fluorine Sodium High Electron Affinity Low Electron Affinity A B Fluorine Sodium Copyright © 2010 Ryan P. Murphy

A B Fluorine Sodium Answers: Fluorine Sodium High Electron Affinity Low Electron Affinity A B Fluorine Sodium Copyright © 2010 Ryan P. Murphy

A B Fluorine Sodium Answers: Fluorine Sodium High Electron Affinity Low Electron Affinity A B Fluorine Sodium Copyright © 2010 Ryan P. Murphy

A B Fluorine Sodium Answers: Fluorine Sodium High Electron Affinity Low Electron Affinity A B Fluorine Sodium Copyright © 2010 Ryan P. Murphy

A B Fluorine Sodium Answers: Fluorine Sodium High Electron Affinity Low Electron Affinity A B Fluorine Sodium Copyright © 2010 Ryan P. Murphy

Electronegativity increases from lower left to upper right. Copyright © 2010 Ryan P. Murphy

Electronegativity increases from lower left to upper right. Moving top to bottom down the periodic table, electronegativity decreases. Copyright © 2010 Ryan P. Murphy

H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Sc Ti Ga Ge As Se Br Kr Electronegativity Copyright © 2010 Ryan P. Murphy

Note: Noble gases are missing. Copyright © 2010 Ryan P. Murphy

Copyright © 2010 Ryan P. Murphy

The most strongly electronegative element, Fluorine (F). Copyright © 2010 Ryan P. Murphy

The most strongly electronegative element, Fluorine (F). “I want electrons.” Copyright © 2010 Ryan P. Murphy

The most strongly electronegative element, Fluorine (F). The least electronegative element is Francium (Fr). Copyright © 2010 Ryan P. Murphy

“I want to give away electrons.” The most strongly electronegative element, Fluorine (F). The least electronegative element is Francium (Fr). “I want to give away electrons.” Copyright © 2010 Ryan P. Murphy

“I want to give away electrons.” The most strongly electronegative element, Fluorine (F). The least electronegative element is Francium (Fr). “I want to gain electrons” “I want to give away electrons.” Copyright © 2010 Ryan P. Murphy

“I want to give away electrons.” The most strongly electronegative element, Fluorine (F). The least electronegative element is Francium (Fr). “I want to gain electrons” “I want to give away electrons.” “You guys should get together.” Copyright © 2010 Ryan P. Murphy

Electronegativity is a measure of the attraction of an atom for the electrons in a chemical bond. Copyright © 2010 Ryan P. Murphy

Electronegativity is a measure of the attraction of an atom for the electrons in a chemical bond. The higher the electronegativity of an atom, the greater its attraction for bonding electrons. Copyright © 2010 Ryan P. Murphy

Electronegativity is a measure of the attraction of an atom for the electrons in a chemical bond. The higher the electronegativity of an atom, the greater its attraction for bonding electrons. “Those elements attract electrons like wicked.” Copyright © 2010 Ryan P. Murphy

Electronegativity is a measure of the attraction of an atom for the electrons in a chemical bond. The higher the electronegativity of an atom, the greater its attraction for bonding electrons. “Not the Noble Gases however.” Copyright © 2010 Ryan P. Murphy

Electronegativity is a measure of the attraction of an atom for the electrons in a chemical bond. The higher the electronegativity of an atom, the greater its attraction for bonding electrons. “Not the Noble Gases however.” “They’re wicked different.” Copyright © 2010 Ryan P. Murphy

Electrons with low ionization energies have a low electronegativity because their nuclei do not exert a strong attractive force on electrons. Elements with high ionization energies have a high electronegativity due to the strong pull exerted on electrons by the nucleus. and Ions) Ionization energy is the energy required to remove an electron. (Gases and Ions) Copyright © 2010 Ryan P. Murphy

Increasing Ionization Energies Electrons with low ionization energies have a low electronegativity because their nuclei do not exert a strong attractive force on electrons. Elements with high ionization energies have a high electronegativity due to the strong pull exerted on electrons by the nucleus. Increasing Ionization Energies and Ions) Ionization energy is the energy required to remove an electron. (Gases and Ions) Copyright © 2010 Ryan P. Murphy

Increasing Ionization Energies Electrons with low ionization energies have a low electronegativity because their nuclei do not exert a strong attractive force on electrons. Elements with high ionization energies have a high electronegativity due to the strong pull exerted on electrons by the nucleus. Increasing Ionization Energies and Ions) Ionization energy is the energy required to remove an electron. (Gases and Ions) Copyright © 2010 Ryan P. Murphy

Increasing Ionization Energies Electrons with low ionization energies have a low electronegativity because their nuclei do not exert a strong attractive force on electrons. Elements with high ionization energies have a high electronegativity due to the strong pull exerted on electrons by the nucleus. Increasing Ionization Energies and Ions) Ionization energy is the energy required to remove an electron. (Gases and Ions) Copyright © 2010 Ryan P. Murphy

A polar bond: Results in the unequal sharing of the electrons in the bond. Copyright © 2010 Ryan P. Murphy

A polar bond: Results in the unequal sharing of the electrons in the bond. When two unlike atoms are covalently bonded, the shared electrons will be more strongly attracted to the atom of greater electronegativity Copyright © 2010 Ryan P. Murphy

A polar bond: Results in the unequal sharing of the electrons in the bond. When two unlike atoms are covalently bonded, the shared electrons will be more strongly attracted to the atom of greater electronegativity The presence or absence of polar bonds within a molecule plays a very important part in determining chemical and physical properties of those molecules. Some of these properties are melting points, boiling points, viscosity and solubility in solvents. Copyright © 2010 Ryan P. Murphy

The three classes of bonds

The three classes of bonds Nonpolar Covalent

The three classes of bonds Nonpolar Covalent Polar Covalent

The three classes of bonds Nonpolar Covalent Polar Covalent Ionic

The three classes of bonds Nonpolar Covalent Polar Covalent Ionic The most commonly used electronegativity scale is Pauling's. Most Periodic Tables gives the value for each element.

The three classes of bonds Nonpolar Covalent Polar Covalent Ionic The most commonly used electronegativity scale is Pauling's. Most Periodic Tables gives the value for each element. Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar.

The three classes of bonds Nonpolar Covalent Polar Covalent Ionic The most commonly used electronegativity scale is Pauling's. Most Periodic Tables gives the value for each element. Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar. H2O Electron Negativity Difference

The three classes of bonds Nonpolar Covalent Polar Covalent Ionic The most commonly used electronegativity scale is Pauling's. Most Periodic Tables gives the value for each element. Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar. H2O Electron Negativity Difference Hydrogen = 2.20 Oxygen = 3.44

The three classes of bonds Nonpolar Covalent Polar Covalent Ionic The most commonly used electronegativity scale is Pauling's. Most Periodic Tables gives the value for each element. Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar. H2O Electron Negativity Difference Hydrogen = 2.20 Oxygen = 3.44 3.44 – 2.20 =

The three classes of bonds Nonpolar Covalent Polar Covalent Ionic The most commonly used electronegativity scale is Pauling's. Most Periodic Tables gives the value for each element. Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar. H2O Electron Negativity Difference Hydrogen = 2.20 Oxygen = 3.44 3.44 – 2.20 = 1.24

The three classes of bonds Nonpolar Covalent Polar Covalent Ionic The most commonly used electronegativity scale is Pauling's. Most Periodic Tables gives the value for each element. Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar. H2O Electron Negativity Difference Hydrogen = 2.20 Oxygen = 3.44 3.44 – 2.20 = 1.24

The three classes of bonds Nonpolar Covalent Polar Covalent Ionic The most commonly used electronegativity scale is Pauling's. Most Periodic Tables gives the value for each element. Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar. H2O Electron Negativity Difference Hydrogen = 2.20 Oxygen = 3.44 3.44 – 2.20 = 1.24

Try Ethane C2H6?

Try Ethane C2H6?

The three classes of bonds Nonpolar Covalent Polar Covalent Ionic The most commonly used electronegativity scale is Pauling's. Most Periodic Tables gives the value for each element. Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar. C2H6 Ethane Electron Negativity Diff.

The three classes of bonds Nonpolar Covalent Polar Covalent Ionic The most commonly used electronegativity scale is Pauling's. Most Periodic Tables gives the value for each element. Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar. C2H6 Ethane Electron Negativity Diff. Hydrogen = 2.20 Carbon = 2.55

The three classes of bonds Nonpolar Covalent Polar Covalent Ionic The most commonly used electronegativity scale is Pauling's. Most Periodic Tables gives the value for each element. Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar. C2H6 Ethane Electron Negativity Diff. Hydrogen = 2.20 Carbon = 2.55 2.55 – 2.20 =

The three classes of bonds Nonpolar Covalent Polar Covalent Ionic The most commonly used electronegativity scale is Pauling's. Most Periodic Tables gives the value for each element. Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar. C2H6 Ethane Electron Negativity Diff. Hydrogen = 2.20 Carbon = 2.55 2.55 – 2.20 = .35

The three classes of bonds Nonpolar Covalent Polar Covalent Ionic The most commonly used electronegativity scale is Pauling's. Most Periodic Tables gives the value for each element. Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar. C2H6 Ethane Electron Negativity Diff. Hydrogen = 2.20 Carbon = 2.55 2.55 – 2.20 = .35

Oil

Oil Water

Oil Water Polar

Oil Nonpolar Water Polar

Which one is polar covalent and which one nonpolar? B

Which one is polar covalent and which one nonpolar? B

Which one is polar covalent and which one nonpolar? B

Which one is polar covalent and which one nonpolar? B

Which one is polar covalent and which one nonpolar? B

Which one is polar covalent and which one nonpolar? = 1.24 B

Which one is polar covalent and which one nonpolar? = 1.24 B = .35

Vegetable Oil Water Corn Syrup Layering liquids with different densities. Use a clear container and add the following in this order…. Corn Syrup Water (food Coloring) Vegetable Oil Vegetable Oil Water Corn Syrup

Polar Non-Polar or Vegetable Oil Water Corn Syrup Layering liquids with different densities. Use a clear container and add the following in this order…. Corn Syrup Water (food Coloring) Vegetable Oil Polar Non-Polar or Vegetable Oil Water Corn Syrup

Polar Non-Polar or Non-Polar Vegetable Oil Water Corn Syrup Layering liquids with different densities. Use a clear container and add the following in this order…. Corn Syrup Water (food Coloring) Vegetable Oil Polar Non-Polar or Non-Polar Vegetable Oil Water Corn Syrup

Polar Non-Polar or Non-Polar Vegetable Oil Water Corn Syrup Layering liquids with different densities. Use a clear container and add the following in this order…. Corn Syrup Water (food Coloring) Vegetable Oil Polar Non-Polar or Non-Polar Vegetable Oil Water Corn Syrup

Polar Non-Polar or Non-Polar Vegetable Oil Polar Water Corn Syrup Layering liquids with different densities. Use a clear container and add the following in this order…. Corn Syrup Water (food Coloring) Vegetable Oil Polar Non-Polar or Non-Polar Vegetable Oil Polar Water Corn Syrup

Polar Non-Polar or Non-Polar Vegetable Oil Polar Water Corn Syrup Layering liquids with different densities. Use a clear container and add the following in this order…. Corn Syrup Water (food Coloring) Vegetable Oil Polar Non-Polar or Non-Polar Vegetable Oil Polar Water Corn Syrup

Polar Non-Polar or Non-Polar Vegetable Oil Polar Water Corn Syrup Layering liquids with different densities. Use a clear container and add the following in this order…. Corn Syrup Water (food Coloring) Vegetable Oil Polar Non-Polar or Non-Polar Vegetable Oil Polar Water Corn Syrup

I would recommend completing these questions right away.

Carbon = 2.55 Hydrogen = 2.20 Carbon = 2.55 Oxygen = 3.44 Hydrogen = 2.20 Oxygen = 3.44

Hydrogen = 2.20 Carbon = 2.55 2.55 – 2.20 = .35 Oxygen = 3.44 Carbon = 2.55 3.44 – 2.55 = .89 Hydrogen = 2.20 Oxygen = 3.44 3.44 – 2.20 = 1.24 Do we want to see the answers? Do we want to see the answers? Do we want to see the answers? Carbon = 2.55 Hydrogen = 2.20 Carbon = 2.55 Oxygen = 3.44 Hydrogen = 2.20 Oxygen = 3.44

Hydrogen = 2.20 Carbon = 2.55 2.55 – 2.20 = .35 Oxygen = 3.44 Carbon = 2.55 3.44 – 2.55 = .89 Hydrogen = 2.20 Oxygen = 3.44 3.44 – 2.20 = 1.24 Do we want to see the answers? Do we want to see the answers? Do we want to see the answers? Carbon = 2.55 Hydrogen = 2.20 Carbon = 2.55 Oxygen = 3.44 Hydrogen = 2.20 Oxygen = 3.44

Hydrogen = 2.20 Carbon = 2.55 2.55 – 2.20 = .35 Oxygen = 3.44 Carbon = 2.55 3.44 – 2.55 = .89 Hydrogen = 2.20 Oxygen = 3.44 3.44 – 2.20 = 1.24 Do we want to see the answers? Do we want to see the answers? Carbon = 2.55 Hydrogen = 2.20 Carbon = 2.55 Oxygen = 3.44 Hydrogen = 2.20 Oxygen = 3.44

Hydrogen = 2.20 Carbon = 2.55 2.55 – 2.20 = .35 Oxygen = 3.44 Carbon = 2.55 3.44 – 2.55 = .89 Hydrogen = 2.20 Oxygen = 3.44 3.44 – 2.20 = 1.24 Do we want to see the answers? Do we want to see the answers? Carbon = 2.55 Hydrogen = 2.20 Carbon = 2.55 Oxygen = 3.44 Hydrogen = 2.20 Oxygen = 3.44 Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar.

Hydrogen = 2.20 Carbon = 2.55 2.55 – 2.20 = .35 Oxygen = 3.44 Carbon = 2.55 3.44 – 2.55 = .89 Hydrogen = 2.20 Oxygen = 3.44 3.44 – 2.20 = 1.24 Do we want to see the answers? Do we want to see the answers? Carbon = 2.55 Hydrogen = 2.20 Carbon = 2.55 Oxygen = 3.44 Hydrogen = 2.20 Oxygen = 3.44 Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar.

Nonpolar Covalent Hydrogen = 2.20 Carbon = 2.55 2.55 – 2.20 = .35 Oxygen = 3.44 Carbon = 2.55 3.44 – 2.55 = .89 Hydrogen = 2.20 Oxygen = 3.44 3.44 – 2.20 = 1.24 Do we want to see the answers? Do we want to see the answers? Carbon = 2.55 Hydrogen = 2.20 Carbon = 2.55 Oxygen = 3.44 Hydrogen = 2.20 Oxygen = 3.44 Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar.

Nonpolar Covalent Hydrogen = 2.20 Carbon = 2.55 2.55 – 2.20 = .35 Oxygen = 3.44 Carbon = 2.55 3.44 – 2.55 = .89 Hydrogen = 2.20 Oxygen = 3.44 3.44 – 2.20 = 1.24 Do we want to see the answers? Do we want to see the answers? Carbon = 2.55 Hydrogen = 2.20 Carbon = 2.55 Oxygen = 3.44 Hydrogen = 2.20 Oxygen = 3.44 Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar.

Nonpolar Covalent Hydrogen = 2.20 Carbon = 2.55 2.55 – 2.20 = .35 Oxygen = 3.44 Carbon = 2.55 3.44 – 2.55 = .89 Hydrogen = 2.20 Oxygen = 3.44 3.44 – 2.20 = 1.24 Do we want to see the answers? Carbon = 2.55 Hydrogen = 2.20 Carbon = 2.55 Oxygen = 3.44 Hydrogen = 2.20 Oxygen = 3.44 Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar.

Nonpolar Covalent Hydrogen = 2.20 Carbon = 2.55 2.55 – 2.20 = .35 Oxygen = 3.44 Carbon = 2.55 3.44 – 2.55 = .89 Hydrogen = 2.20 Oxygen = 3.44 3.44 – 2.20 = 1.24 Do we want to see the answers? Carbon = 2.55 Hydrogen = 2.20 Carbon = 2.55 Oxygen = 3.44 Hydrogen = 2.20 Oxygen = 3.44 Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar.

Nonpolar Covalent Polar Covalent Hydrogen = 2.20 Carbon = 2.55 2.55 – 2.20 = .35 Oxygen = 3.44 Carbon = 2.55 3.44 – 2.55 = .89 Hydrogen = 2.20 Oxygen = 3.44 3.44 – 2.20 = 1.24 Do we want to see the answers? Carbon = 2.55 Hydrogen = 2.20 Carbon = 2.55 Oxygen = 3.44 Hydrogen = 2.20 Oxygen = 3.44 Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar.

Nonpolar Covalent Polar Covalent Hydrogen = 2.20 Carbon = 2.55 2.55 – 2.20 = .35 Oxygen = 3.44 Carbon = 2.55 3.44 – 2.55 = .89 Hydrogen = 2.20 Oxygen = 3.44 3.44 – 2.20 = 1.24 Do we want to see the answers? Carbon = 2.55 Hydrogen = 2.20 Carbon = 2.55 Oxygen = 3.44 Hydrogen = 2.20 Oxygen = 3.44 Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar.

Nonpolar Covalent Polar Covalent Hydrogen = 2.20 Carbon = 2.55 2.55 – 2.20 = .35 Oxygen = 3.44 Carbon = 2.55 3.44 – 2.55 = .89 Hydrogen = 2.20 Oxygen = 3.44 3.44 – 2.20 = 1.24 Carbon = 2.55 Hydrogen = 2.20 Carbon = 2.55 Oxygen = 3.44 Hydrogen = 2.20 Oxygen = 3.44 Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar.

Nonpolar Covalent Polar Covalent Hydrogen = 2.20 Carbon = 2.55 2.55 – 2.20 = .35 Oxygen = 3.44 Carbon = 2.55 3.44 – 2.55 = .89 Hydrogen = 2.20 Oxygen = 3.44 3.44 – 2.20 = 1.24 Carbon = 2.55 Hydrogen = 2.20 Carbon = 2.55 Oxygen = 3.44 Hydrogen = 2.20 Oxygen = 3.44 Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar.

Nonpolar Covalent Polar Covalent Polar Covalent Hydrogen = 2.20 Carbon = 2.55 2.55 – 2.20 = .35 Oxygen = 3.44 Carbon = 2.55 3.44 – 2.55 = .89 Hydrogen = 2.20 Oxygen = 3.44 3.44 – 2.20 = 1.24 Carbon = 2.55 Hydrogen = 2.20 Carbon = 2.55 Oxygen = 3.44 Hydrogen = 2.20 Oxygen = 3.44 Differences 1.7 or greater, the bond is usually ionic, Differences Less than 1.7, the bond is usually covalent, Unless the difference is less than 0.5 the bond has some degree of polarity Differences of less than 0.5 are considered to be nonpolar.

Hundreds of more slides, activities, video links, End of Preview Hundreds of more slides, activities, video links, homework package, lesson notes, review games, rubrics, and much more on the full version of this unit and larger curriculum.

This PowerPoint roadmap is one small part of my Atoms and Periodic Table Unit. This unit includes a four part 2000+ slide PowerPoint roadmap. 13 page bundled homework that chronologically follows slideshow 14 pages of unit notes with visuals. 3 PowerPoint review games. Activity sheets, rubrics, advice page, curriculum guide, materials list, and much more. http://sciencepowerpoint.com/Atoms_Periodic_Table_of_Elements_Unit.html

More Units Available at… Earth Science: The Soil Science and Glaciers Unit, The Geology Topics Unit, The Astronomy Topics Unit, The Weather and Climate Unit, and The River Unit, The Water Molecule Unit. Physical Science: The Laws of Motion and Machines Unit, The Atoms and Periodic Table Unit, The Energy and the Environment Unit, and The Science Skills / Metric Unit. Life Science: The Diseases and Cells Unit, The DNA and Genetics Unit, The Life Topics Unit, The Plant Unit, The Taxonomy and Classification Unit, Ecology: Feeding Levels Unit, Ecology: Interactions Unit, Ecology: Abiotic Factors, The Evolution and Natural Selection Unit and the Human Body and Health Topics Unit. Copyright © 2010 Ryan P. Murphy

Purchase the entire four curriculum, 35,000 slides, hundreds of pages of homework, lesson notes, review games, and much more. http://sciencepowerpoint.com/Atoms_Periodic_Table_of_Elements_Unit.html Please feel free to contact me with any questions you may have. Thanks again for your interest in this curriculum.\ Sincerely, Ryan Murphy M.Ed www.sciencepowerpoint@gmail.com