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 What is an ionic bond?  What is a covalent bond?  Draw a picture of an ionic bond for salt (NaCl) DO NOW.

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Presentation on theme: " What is an ionic bond?  What is a covalent bond?  Draw a picture of an ionic bond for salt (NaCl) DO NOW."— Presentation transcript:

1  What is an ionic bond?  What is a covalent bond?  Draw a picture of an ionic bond for salt (NaCl) DO NOW


3  Ionic compounds form crystals  What do you notice about the pictures? IONIC COMPOUNDS

4  Strong attractions between ions of a compound cause it to have  High melting points  Highly brittle (breakable)  Very strong Cation anion IONIC COMPOUNDS

5  How do we form an ion? SPEAKING OF IONS

6  Ions- an atom with either a positive (cation) or a negative (anion) charge caused by the addition or removal of an electron.  Why do we add or remove electrons? IONS

7  ELECTRONS are the reason we have compounds!  All bonding is caused by either the transfer or sharing of electrons!  When electrons are shared it is _________ bonding.  When electrons are transferred it is _________ bonding. BONDING

8  Do you like being unstable?  Think about standing on the side of a cliff….with a very strong wind. Would you be happy?  How do elements gain stability? ALL ELEMENTS WANT TO BE STABLE

9  What is a valence electron?  What is the octet rule? THE OCTET RULE

10  Compounds are most stable when they have eight (8) valence electrons.  Compounds will gain or give up electrons based on how easy it is.  Ionization energy- the amount of energy required to remove an electron. THE OCTET RULE

11  In your notebook explain how ionization energy changes across the periodic table.  You have 3 minutes.  Use full sentences!!!!!!! (I’m serious…I will be checking!) OCTET RULE


13  What ionic charge will Magnesium have?  When is an atom least likely to react?  Define ion, ionization energy, valence electron, octet rule, covalent bond, and ionic bond.  *Bonus* how many protons, neutrons, and electrons does Bromine have? HOMEWORK 12/2/13

14  You need to pick up a white board, dry erase marker, and eraser from the front left corner of the room.  You must be seated with these materials by the time the bell rings or points will be deducted from your grade today. DO NOW

15  Draw a water molecule. Chemical formula H 2 O.  Is water a compound, mixture, or element?  How many elements are in a molecule of water?  What’s an ionic bond, covalent bond? DO NOW CONTINUED

16 LETS BREAK IT DOWN Many water molecules together Pure substance not a mixture

17  The word molecule is ambiguous.  What does ambiguous mean???  You can have a molecule of an element  You can have a molecule of a compound  You can have a molecule of a substance  The word molecule does NOT always mean compound or element. THE WORD MOLECULE

18  Tricky right?  There are elemental forms of all elements.  Air is made mostly of what element? HOW CAN TWO ATOMS TOGETHER BE AN ELEMENT?

19  Just Remember! STABILITY rules the UNIVERSE! All chemical bonding is done to make an element stable. CONFUSED?

20  What is a covalent bond?  You can make one covalent bond for every valence electron you have. COVALENT BONDING

21 Covalent bonds are expressed as lines. Unlike ionic expressed as charges. COH COVALENT BOND

22  The types of atoms in a molecule and its shape affect its polarity.  What do you see when you look in a mirror? NON-POLAR COVALENT

23  For non-polar elements you look for equality in the molecule. NON-POLAR COVALENT

24  To be polar you should look for unequal sharing.  The unequal sharing will cause some charges on molecules  BUT due to the fact there is no electron transfer it is still a covalent bond. POLAR COVALENT

25  Unequal sharing causes slight charges. POLAR COVALENT

26  What is the strongest type of bond?  Polar molecules will attract to one another through intermolecular forces. Which makes polar substances stronger than non-polar. POLARITY AND STRENGTH Intermolecular forces

27 Ionic > polar covalent > non-polar BOND STRENGTH

28  Draw these molecules in your notebook and label them as either polar or non-polar molecules. PRACTICE

29  1. What is ionic bond?  2. What is a covalent bond?  3. Draw a picture of an ionic bond for salt (NaCl).  Today’s Lesson Topic: Chemical Naming DO NOW


31  SWBAT name common mono-atomic and polyatomic ions.  Essential Questions: how do chemical compounds get their name? TODAY’S OBJECTIVE

32 Ionic Bond vs. Covalent Bond  Ionic bond is an electron transfer  Covalent Bond is electron sharing  Which is stronger? Why? REVIEW..

33  How many elements are in the following compound? Na 2 CO 3 LET’S CHECK…

34  There are so many ways to combine atoms.  We must give compounds names.  To do this there are rules….many many rules  Fortunately this is not organic chemistry (you’ll get that in college)  Fewer rules to follow for physical science (yay!)  But, you will need to memorize some rules. NAMING COMPOUNDS

35 HOLD UP…REVIEW  What is a Cation? What is an Anion? A cation is an ion with a positive charge An ion an with a negative charge

36 REVIEW  What are the ions of Na, C, N, O, Cl ?

37  In ionic bonding we join an anion with a cation.  The first step to naming is to determine which is which. IONIC COMPOUND NAMING

38 1. In NaCl which would be the anion? 2. In CaCl 2 which would be the anion? 3. In LiS which would be the anion?  Sensing a pattern? IDENTIFYING THE ANION

39  In ionic bonding the anion is usually listed second in the chemical formula. IONIC COMPOUND NAMING



42 PRACTICE 2: WRITE THESE 1. Sulfide ion 2. iodide ion 3. phosphide ion 4. Fluorine ion

43  This rule is easy.  Use the element name of the cation.  NaCl = sodium chloride  Sodium is the cation  Chloride is the anion CATION RULE

44 1. NaCl 2. CaCl 2 3. MgO 2 PRACTICE 3: NAME THESE

45  To complicate things we have polyatomic ions.  What are they?  Multiple atoms in an ion.  Multiple atoms with a charge  Example: NH 4 + ammonium  Unfortunately, these are ion names you must memorize.  THAT NAMING SYSTEM WORKS FOR MONO-ATOMIC IONS


47  Any trends you see?  Elements ending in –ate? TRENDS?

48 MOLECULAR COMPOUNDS  Molecular compounds are named based on the number of atoms in a molecule.

49 WHAT IS THE COMMON NAME FOR CO2? What about CO3? Carbon Trioxide

50 PRACTICE 4: MOLECULAR COMPOUNDS  In order to name you just add the prefix to the elemental name (with –ide). 1. CO 2. PO 5

51 YOU TRY 3. PO 3 4. SO 4 (careful with this one) 5. N 2 O 4

52 FINAL REVIEW  Name the following compounds: 1. NaCl 2. NaO 3. H2O 4. LiF

53  1. What are anions? What are cations?  2. What is the name of CaCl2?  3. What is the name of NaCl?  4. What is the name of EXIT TICKET

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