Homework
• Page 8
– 1st column for #1 and #2
• Correct lab and resubmit
Lab
• Everyone can improve their grade!
• Answer any questions you got wrong on a
sheet of NOTEBOOK paper (not in lab
notebook)
• Staple to the back of the original lab
• Return next class
• Use notes from today (in addition to POGIL
and page 2 notes) in order to help you
So you know…
• Bonds and forces are different
• NO BONDS WERE BROKEN IN THIS
LAB
Page 2
• Let’s update our notes
• Look at the strength row
– Strength of DD depends on _____
– Strength of LDF depends on _____
So you know…
• The number of atoms in a molecule would
only be important if we were talking about
LDF
– More atoms would mean more electrons
With your face partner, finish
your assigned sentence
B. Strength of LDF depends on…..
A. Strength of DD depends on….
With your face partner, finish
your assigned sentence
B. Strength of LDF depends on the number
of electrons (more electrons means a stronger
LDF)
A. Strength of DD depends on the polarity of
the molecule which depends on the difference
in electronegativity (larger difference, more
polar, stronger DD)
Intra vs Inter Reminder
• Bottom of pg 2
The state a substance is in
depends on the strength of the
intermolecular forces
States of Matter
• Solid
• Liquid
• Gas
• Plasma
Make this chart in your notes
(5 columns, 6 rows)
solids
Kinetic energy
Shape
Volume
Intermolecular
forces
picture
liquids
Gases
Plasma
Solids
– very low KE - particles vibrate
but can’t move around
– fixed shape
– fixed volume – molecules are
very close together
– Very strong attractive forces
between molecules
• Be specific about the ‘force’ type if you
are given a specific substance (LDF,
DD, etc.)
Liquids
– low KE - particles can move
around but are still close together
– variable shape
– fixed volume - atoms and
molecules are touching but can
move throughout container
– strong attractive forces between
molecules
Gases
– high KE - particles can separate and
move throughout container
– variable shape
– variable volume - molecules are moving
in random patterns with varying
amounts of distance between the
particles.
– NO attractive forces between molecules
Plasma
– very high KE - particles collide with enough
energy to break into charged particles (+/-)
– gas-like, variable
shape & volume
– stars, fluorescent
light bulbs, CRTs
– NO attractive forces
You are a molecule
• What would it look like if….
Requires adding energy in order to break
the attractive forces between the molecules.
Remember
• Nonpolar molecules have LDF
• Polar molecules have LDF and DD
– If the polar molecule has H attached to
nitrogen, oxygen, or fluorine, the substance has
LDF, DD, and HB
Example Question & Answer
The normal boiling point of CCl4 is 77°C,
whereas that of CBr4 is 190°C. Explain.
Mention specific IMFs for BOTH substances
Both CCl4 and CBr4 are nonpolar. This means that Explain why
London dispersion forces hold the molecules togetherthe strengths
in the liquid state. To boil the substances, the LDF of the forces
different
must be broken. Since CBr4 has more electrons than
CCl4, a stronger momentary dipole can be formed
when its electrons shift. Therefore, the molecules are
more attracted to each other and more energy is
required to break those attractive LD forces.
Make claim to answer question
Your Turn
• Mention specific IMFs for BOTH substances
• Explain why the strengths of the forces different
• Make claim to answer question
• Ammonia, NH3, has a significantly higher
boiling point than PH3. Both substances are
trigonal pyramidal. Explain.
• Ammonia is a polar molecule that has LDF,
dipole-dipole, and hydrogen bonds. PH3 is
also polar; it has LDF and dipole-dipole
attractions. Since ammonia has an
additional strong type of intermolecular
force, its boiling point will be higher.
•
•
•
•
Ionic Nomenclature
Must be neutral overall
NO PREFIXES!!!!!!
Name the cation first, then the anion
Cation is either a metal or ammonium
– To name a metal cation, use the element name and a roman
numeral to indicate the charge of the cation
•
•
•
•
Tin(II) is Sn2+
Tin(III) is Sn3+
Mercury(II) is Hg2+
Mercury(I) is Hg22+ (it’s diatomic)
– Roman numerals are NOT used for the following because they
only have one charge: Group 1A (+1), Group 2A(+2),
ammonium(+1), or CdZnAgAl 2213 (where 2 is the charge of
Cd, 2 is the charge of Zn, etc.)
• Sodium is Na+
• Magnesium is Mg2+
• Cadmium is Cd2+
Ionic Nomenclature
• Anion is either a nonmetal or a negative polyatomic ion (like
sulfate or phosphite)
• Use the ion name for the nonmetal (Cl- is chloride)
• Some examples for you to look at before we practice
• Zr(NO3)2 = zirconium(II) nitrate
– Since nitrate has a -1 charge and there are 2 of them, zirconium
must have a +2 charge to make the compound neutral overall
• CuCl = copper(I) chloride
• CuCl2 = copper(II) chloride
– the # of Cl- depends on the charge of Cu ion
• Ag3PO4 = silver phosphate (no roman numerals because this
is part of CdZnAgAl 2213)
Quiz-Quiz-Trade
• What’s my roman numeral?
Work with your shoulder partner –
A does #1 and B checks, B does #1 and A checks
A does #2 and B checks, etc.
 the answers will be displayed when everyone is done
These are A’s problems
(B will check them)
These are B’s problems
(A will check them)
1.
2.
3.
4.
1.
2.
3.
4.
Au(ClO)2
MgO
Fe2S3
AlN
If there are groups
of 3, just rotate A,
B, and C
CoP
Ag2CO3
Ca(CN)2
PbF2
Hint: each set has 2 that need roman
numerals and 2 that do not
Answers
These are A’s problems
(B will check them)
These are B’s problems
(A will check them)
1. Au(ClO)2
gold(II) hypochlorite
2. MgO
magnesium oxide
3. Fe2S3
iron(III) sulfide
4. AlN
aluminum nitride
1. CoP
cobalt(III) phosphide
2. Ag2CO3
silver carbonate
3. Ca(CN)2
calcium cyanide
4. PbF2
lead(II) fluoride
1.
2.
3.
4.
Silver hypochlorite
Iron(II) cyanide
Calcium nitride
Nickel(I) phosphate
Work these on your own –
1.
2.
3.
4.
5.
(but ask your partner if you need help)
Careful: I mixed in some covalent….
FeSO4
1. iron(II) sulfate
(NH4)2CrO4
2. ammonium chromate
NI3
3. nitrogen triodide
Fe(HCO3)3
4. iron (III) bicarbonate
Co(C2H3O2)3
5. Cobalt(III) acetate
Exit Ticket
1. Y(OH)2
2. FeBr3
3. ZnSO3
4. Platinum(IV) phosphate
5. Tungsten(VI) cyanide
6. Cadmium oxalate