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Entry Task: Nov 5-6th Block 2
Provide the name and formula for the following:
MgP and Lithium nitride
Agenda:Sign off on Binary compounds 1 ws
Notes Formula mass, # of elements and compounds
HW: Formula mass and elements ws
I can…Create binary ionic formulas
Count the # of elements in a compound.
Check my formula with the given formula mass
Describe the properties of ionic substances
Clear off DesksHAVE OUT:
Binary compound wsPeriodic tableWriting utensil
CALCULATOR
Ion Formation ReviewProvide the ions for the following atoms.
Al____ Si_____ S_____
Cu(II)_____ P_____ Mn(V)____
Na____ F_____ Pb(IV)____
Cd(II)____ Rb_____ O______
Ca_____ Cl_____ Ag(I)_____
Al+3 Si+4 S-2
Cu+2 P-3 Mn+5
Na+1 F-1 Pb+4
Cd+2 Rb+1 O-2
Ca+2 Cl-1 Ag+1
Ion Formation ReviewProvide the ions for the following atoms.
Se____ K____ Ba____
N_____ In____ Sr_____
I_____ Au(III)_____ Br_____
Te_____ V(VI)_____ Be_____
F_____ Mg____ Li_____
Bi(III)____ Sc (II)_____ Cs______
Se-2 K+1 Ba+2
N-3 In+3 Sr+2
I-1 Au+3 Br-1
Te-2 V+6 Be+2
F-1 Mg+2 Li+1
Bi+3 Sc+2 Cs+1
Ionic Bonding Basics
Describe what happens to the electrons (cation/anion) when an ionic compound is formed.
What type of elements are involved?
What is the point of ionic bonding?
Cations transfer their valence electron(s) to the anion.
Metals and nonmetals
The cation gives up its ve- to drop to a filled orbit and the anion gets the ve- to fill it orbit to be stable.
F/Mg
Na/Ca
Cs/F
As/Sr
O/N
O/Ba
Mg/Fr
Ionic BondingDetermine if the following will form ionic compounds? If yes, write the correct ionic formula.
Mg+2 F-1 MgF2
Na+1 Ca+2 NO formula
Cs+1 F-1 CsF
Sr+2 As-3 Sr3As2
O-2 N-3 No Formula
Ba+2 O-2 BaOMg+2 Fr+1 No Formula
Li/Cl
At/Rb
S/K
N/Fe(II)
Se/Be
Br/Cs
Ne/Ca
Cl/S
Ionic BondingDetermine if the following will form ionic compounds? If yes, write the correct ionic formula.
Li+1 Cl-1 LiCl
At-1 Rb+1 RbAt
K+1 S-2 K2S
Fe+2 N-3 Fe3N2
Be+2 Se-2 BeSe
Cs+1 Br-1 CsBr
Ne Ca+2 No Formula
Cl-1 S-2 No Formula
1. ZnCl2
2. MgF2
3. FeO
4. CoCl2
5. VCl5
6. AgCl
7. PbS
Cl -1 (2) = -2
F-1 (2) = -2
Iron II oxide
Cobalt II chloride
Vanadium V chloride
Silver I chloride
Lead II sulfide
Zinc II chloride
Magnesium fluoride
Zn = +2
Mg = +2
O-2 (1) = -2 Fe = +2
Cl-1 (2) = -2 Co = +2
Cl-1 (5) = -5 V = +5
Cl-1 (1) = -1 Ag = +1
S-2 (1) = -2 Pb = +2
11. MnO2
12. NiCl3
13. V4C5
14. FeN
15. Co2S3
Mn = +4
Nickel III chloride
Vanadium V carbide
Cobalt III sulfide
Iron III nitride
Iron III sulfide
Aluminum oxide
Gallium bromide
8. Fe2S3
9. Al2O3
10. GaBr3
S-2 (3) = -6 Fe = +6/ (2)= +3
O-2 (3) = -6 Al = +3 (2)= +6
Br-1 (3) = -3 Ga = +3
O-2 (2) = -4 Manganese IV oxide
Cl-1 (3) = -3 Ni = +3
C-4 (5) = -20 V = +20/4 = +5
N-3 (1) = -3 Fe = +3
S-2 (3) = -6 Co = +6/2 = +3
16. Barium nitride
17. Nickel (II) iodide
18. Iron (II) sulfide
19. Chromium (III) chloride
20. Copper (I) oxide
21. Manganese (IV) nitride
22. Iron (III) sulfide
23. Germanium arsenide
= Ba3N2
= NiI2
= FeS
= CrCl3
= Cu2O
= Mn3N4
= Fe2S3
Ba = +2 N = -3
Ni = +2 I = -1
Fe = +2 S = -2
Cr = +3 Cl = -1
Cu = +1 O= -2
Mn = +4 N= -3
Fe = +3 S= -2
= Ge3As4
Ge = +4 As= -3
24. Zinc (II) oxide
25. Aluminum oxide
= ZnO
= Al2O3
26. Cobalt (II) fluoride
27. Zinc (II) carbide
28. Nickel (III) selenide
29. Manganese (IV) arsenide
30. Copper (II) bromide
Zn= +2 O = -2
Al = +3 O= -2
= CoF2
= Zn2C
= Ni2Se3
= Mn3As4
= CuBr2
Co = +2 F = -1
Zn = +2 C= -4
Ni = +3 Se= -2
Mn = +4 As= -3
Cu = +2 Br= -1
Clear OFF Desk!I’ll provide a periodic Table
for the Quiz
Properties of Ionic Compound1. Ions are packed together tightly alternating positive and negative charges in a crystal lattice.
What effect does a strong bond have on boiling and melting points of a chemical compound?
2. Ionic Compounds have HIGH boiling points and have HIGH melting points
What happens when an ionic compound is placed in water?
3. The ions (cation/anion) separate in water because water is polar (having +/-) ends and ions are +/-.
Summary of Ionic Substances
High melting/boiling point
Dissolves in water
Conduct electricity
Solids at room temperature (think salt)
Brittle – NOT malleable
Energy and Ionic Compounds
WHY do Ionic compounds have these properties?
5. Ionic bonds are STRONG due to the repeated positive-negative lattice pattern.
Polyatomic ionsPolyatomic ions: it’s a group of atoms that are covalently bonded that carry a charge and are dealt with just like monatomic ions.
FLIP your Periodic Table Over-Use your common ion sheet to provide the formula and charge of the following polyatomic ions.
Chloride________ Nitride________ Chlorite ________ Nitrite________ Chlorate________ Nitrate________
Cl-1
ClO2-1
ClO3-1
N-3
NO2-1
NO3-1
Polyatomic ionsPolyatomic ions: it’s a group of atoms that are covalently bonded that carry a charge and are dealt with just like monatomic ions.
FLIP your Periodic Table Over-Use your common ion sheet to provide the formula and charge of the following polyatomic ions.
Phosphide________ Sulfide _________ Phosphite________ Sulfite__________ Phosphate________ Sulfate__________
P-3
PO3-3
PO4-3
S-2
SO3-2
SO4-2
Polyatomic ionsWhat is the difference between –ites and –ate endings?
What is up with Hydronium and Ammonium ion?
acetate carbonate
cyanide dichromate
borate hydroxide
permanganate selenite
Ions with –ites and –ates have oxygen's attached. The –ites have less oxygen compared to –ates.
Hydronium (H3O+) and ammonium (NH4+) ions are
positive polyatomic ions.
C2H3O2-1
CN-1
BO3-3
MnO4-1
CO3-2
Cr2O7-2
OH-1
SeO3-2
When bonding with other ions, more than 1 polyatomic ion maybe needed to balance the charge.
2 chlorate ions
3 hydroxide ions
2 ammonium ions
(ClO3)2
(OH)3
(NH4)2
There are no charges because they bonded.
When dealing with polyatomic ions, treat them just like monatomic ions
K+1
Potassium nitrate
NO3–1
KNO3
Barium sulfate
Ba+2 SO4–2
BaSO4
PO4–3
Iron III phosphateFe+3
FePO4
When dealing with polyatomic ions, treat them just like monatomic ions
NaCN
Sodium cyanide
Ag2SO3
Silver I Sulfite
CuNO2
Copper I nitrite
Use ( ) to group polyatomic ions
Al2(SO3)3
Aluminum sulfite
Ba(NO2)2
Barium nitrite
Cu3(PO4)2
PO4-3
PO4-3
-6
Cu+?
Cu+?
Cu+?
+6Cu+2
Copper II phosphate
In-Class for credit!!
Polyatomic ions- Practice
Silver Oxide
O-2Ag+1 Ag2OK+1 CO3
-2 K2CO3 Potassium Carbonate
Lithium Li+1 Sulfate SO4-2 Lithium sulfate
Sodium Na+1 Bromide Br-1 NaBr
Polyatomic ions- Practice
Polyatomic ions- Practice
Polyatomic ions- Practice
