12/4
• Write your name and class period on your lab
corrections
– Staple your lab correction on the FRONT of your
old lab
• Homework
– Page 4
– Finish page 8
– TEST MONDAY!
Review Homework
Review Homework
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
1.
2.
3.
4.
AgClO
Fe(CN)2
Ca3N2
Ni3PO4
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
Naming Hydrates
Practice
sage-n-scribe – shoulder partner
• For A’s problem: A tells B what to write
• For B’s problem: B tells A what to write
Notice:
There is a dot in the formulas.
There is NO dot in the names.
A: ZnCl2•4H2O
B: CuSO4•5H2O
A: Barium hydroxide hexahydrate
B: Copper(II) chloride dihydrate
Practice
sage-n-scribe
• For A’s problem: A tells B what to write
• For B’s problem: B tells A what to write
A: ZnCl2•4H2O zinc chloride tetrahydrate
B: CuSO4•5H2O copper(II) sulfate pentahydrate
A: Barium hydroxide hexahydrate Ba(OH)2•6H2O
B: Copper(II) chloride dihydrate
CuCl2•2H2O
Turn to page 3 of your packet
• We are going to take notes on three types of
intramolecular forces (metallic, ionic, and
covalent)
Covalent
This is a
covalent bond;
it’s within the
molecule;
intra=within
• bond – when 2 atoms share 2 electrons
• Usually between 2 nonmetals
• Happens when 2 atoms have a similar
electronegativity (neither is strong enough to
take the electrons, so they share)
• Lewis structures depict how electrons are
shared (single bond, double bond, what’s in the
middle, etc.)
• This is a directional bond (it has a direction –
between the two atoms)
• Key point: electrons are shared
Ionic
• not a true bond because electrons aren’t
being shared
• Ionic ‘bond’ is an electrostatic attraction (an
attraction between oppositely charged ions)
Na transfers its 1
valence electron to
chlorine (which has 7)
Notice that both
now have a full
octet and both are
now charged
Ionic, continued
• Because they are oppositely charged, they
stick together in a large, repeating pattern
• Directional force of attraction; notice the
inside Na+ that has Cl- to the left, right, top,
bottom, in front, and behind
Ionic
• Happens when 2 atoms have very different
electronegativies (less EN loses e, more EN
gains e)
• Between a cation (+) and an anion(-)
– We will learn more when we talk about
nomenclature)
• Key point: electrons are transferred
Metallic
• Metal core = the nucleus and core
electrons, positively charged
• A metallic ‘bond’ happens when
the valence electrons dissociate
from the metal core and roam free
as a ‘sea of electrons’
• Not a true bond because electrons
are shared between all the metal
cores
• Nondirectional because all metal
cores share all valence electrons
• Key point: sea of electrons
Notice that the
core electrons and
the nucleus
remain; only
valence electrons
come off the atoms
Page 4
There are 3 types of solids
• Metallic
• Ionic
• Molecular
Each solid has different properties. We are going
to talk about
– Conductor vs insulator
– High vs low melting and boiling points
– Brittle vs malleable
Person 4: get scissors for everyone in
your group and 2 bottles of glue
• Cut out the 12 squares
• Arrange one from each group into the three
columns
• Don’t glue them down yet!
Let’s discuss the properties of each
type of solid
Clean Up
• Person 2 – return the scissors and glue
• Person 1 – recycle ALL scraps of blue paper
Practice! What type of solid am I?
1.
2.
3.
4.
5.
6.
7.
CaO
I’m brittle and have a low melting point
Brass
Sulfur
Potassium nitrate
I conduct heat and am malleable
I have intermolecular forces holding me
together
8. I have intramolecular forces holding me together
• Go back and forth with your shoulder partner
sharing answers
• B starts!
Answers! What type of solid am I?
1.
2.
3.
4.
5.
6.
7.
CaO ionic
I’m brittle and have a low melting point Molecular
Brass metallic
Sulfur Molecular
Potassium nitrate ionic
I conduct heat and am malleable metallic
I have intermolecular forces holding me
together Molecular
8. I have intramolecular forces holding me together
Metallic or ionic
• In 3 words or less, eplain why metals conduct
electricity.