Nomenclature Guide (inorganic) Case 1 1. 2. 3.
Greek prefixes:
- Nonmetal + Nonmetal First element retains its name. Second element gets -ide ending. Use Greek prefixes to identify the # of atoms (ignore the 1st one if it's a '1')
Examples:
N2O = ______________________
1-
6-
2-
7-
3-
8-
4-
9-
5-
101/2-
SO3 = ______________________ Now Try These: carbon dioxide
__________
BrF3 ________________________
diphosphorus pentasulfide __________
N2O 4 ________________________
Case 2 - fixed metal + nonmetal 1. Metal retains its name. 2. Non-metal retains its ionic name.
• make sure ions join to form a neutral compound •
Examples
Na+
Ca+2
+ Cl- ---> ___________
+ Cl- ---> ___________
name = __________________________
name = __________________________
+
---> ___________
name = ___________________________
+
---> ___________
name = ___________________________
+
---> ___________
name = ___________________________
Now Try These: lithium bromide
____________
Al2S 3___________________________
magnesium hydroxide____________
(NH4)2S O3 _______________________
aluminum acetate
Ba(NO3)2 _________________________
____________
Case 3 - variable charge metal + nonmetal 1. Metal gets its charge written w/ Roman # in ( ) after name 2. Non-metal retains its ionic name. Examples: Fe+2
+
Cl-
---> __________
name = _________________________
Fe+3
+
Cl-
---> __________
name = _________________________
+
---> _________
name = _________________________
+
---> _________
name = _________________________
Now Try These: manganese (IV) chloride __________
Cr(OH)3 ______________________
nickel (III) carbonate __________
CuCO3 ______________________
Case 4
- Acids (positive ion = "H+")
1. Drop the ending on the negative ion. The -ate ending changes to -ic acid. The -ite ending changes to -ous acid. The -ide ending uses the prefix hydro- and the suffix -ic acid
Examples:
H2CrO4 = ______________________ HNO2 = ______________________ HCl = ______________________
Now Try These: hydrobromic acid __________ perchloric acid ____________
H3PO3
_____________________
HI __________________________
“hydrates” when ionic substances have water molecules attached, theyʼre called “hydrates” MgSO4 • 3 H2O =
__________________________________
Now Try These: calcium phosphate tetrahydrate = _________________ NaC2H3O2 • 2 H20 = ______________________________________________
Packet #3+ Objectives (know these for quiz...) • know how to name covalent molecules ("case 1") • know the first 10 Greek prefixes • know how to name ionic compounds ("case 2 & 3") as well as hydrates • know how to name acids (need to know those endings!) ("case 4") • know how to determine the # of e- transferred during ionic bonding • know differences between ionic and covalent bonding • know how to draw Lewis dot structures for molecules & ions, including exceptions to octet rule • know the definition of electronegativity, who developed it, and how to calculate ΔEN • know what a "dipole arrow" is, and how to draw them on molecules • know how to determine the geometry and polarity of molecules WS 3.2 answer bank
ammonium hydroxide, ammonium sulfide, boric acid, bromine trifluoride, calcium nitrite, calcium carbonate, calcium fluoride, carbon tetrachloride, copper (II) chloride hexahydrate, hydrosulphuric acid, iron (II) iodate, iron (II) phosphate, lithium oxalate, magnesium sulfate heptahydrate, magnesium thiosulfate, nitric acid, phosphite ion, phosphorus trioxide, potassium bicarbonate, potassium nitrate, sodium bisulfite, sulphur tetrachloride, sulphur trioxide, tin (II) iodide, tin (II) phosphate, vanadium (V) bromate Al(C2H3O2)3, AlI3, BCl3, Ba(CN)2, BrF7, CaH2, Co(NO3)3•4 H2O, CO, CO2, CS2, Cu3(PO4)2, H2C2O4, HClO3, HNO2, H3PO3, Hg3(BO3)2, KClO3, KCN, KOH, NaCl, NaC2H3O2•5 H2O, NH4C2H3O2, PbS, SeS2, Si2O3, Sr(NO3)2, ZnSO4
Video Questions- Bonding
Name ________________________
1. Why are the noble gases chemically inert? ____________________________________________________ 2. How many valence electrons are in sodium? _______ 3. What charge does sodium get when it forms an ion? ________ 4. Chlorine needs to _______ (gain / lose) how many electrons in order to achieve a noble gas configuration? _____ 5. When salt is viewed with an electron microscope, what basic shape does it have? ________________________ 6. When the bulb slowly lights, what does Don Showalter say? (guess:_____ ) a) "Wow!"
b) "Look at that bulb!"
(actual:______ )
c) "Here we go; the bulb is lit"
d) "How about that!"
7. Which of the crystalline substances conducted electricity when in solution? ____________________ 8. The formation of a covalent bond is an __________________ (endothermic / exothermic) process. 9. The N-N triple bond is _______________ (stronger / weaker) than the single N-I bonds in NI3 10. When the nitrogen triiodide ("small brownish pile") explodes, what does Don Showalter say? ______ a) "There it goes!"
b) "Wow, what a reaction!"
c) "Did you see that!?!"
d) "Now my eyebrows are really spiked!"
11. Today's explosive of choice, which is also a fertilizer, is _____________________________________.
Octet Rule:
What Is An Ionic Bond?
How Does An Ionic Bond Form?
Ionic Bonding Diagrams NaCl
CaCl2
Single Covalent Bond
Double Covalent Bond
Al2O 3
Triple Covalent Bond
electronegativity:
developed by: _____________________________________
Δ EN
structure
0.0
0.4
nonpolar covalent
2.0 polar covalent
bond type
4.0 ionic
Valence Shell Electron Pair Repulsion Theory (VSPER) # of e- pairs (regions)
e - geometry
bond angle: _______
bond angle: _______
bond angle: _______
bonding diagram
molecular geometry
(pull the ropes) polarity
example
Exceptions To The Octet Rule
Common Ions To Memorize For Quiz, Honors Chemistry: 1+ ions
1- ions
H+1 hydrogen L i+1 lithium +1 Na sodium K +1 potassium
F -1 C l-1 B r-1 I -1
N H4 + 1
NO2 - 1
nitrite
NO3 - 1
nitrate
C l O- 1 C l O2 - 1
hypochlorite chlorite
C l O3 -1
chlorate
ammonium 2+ ions
Mg2+ magnesium Ca2+ calcium Ba2+ barium
3+ ion Al3+
aluminum
fluoride chloride bromide iodide
C l O4 - 1
perchlorate
I O3 - 1
iodate
OH- 1 C N- 1 HCO3 - 1
hydroxide cyanide bicarbonate
H S O3 - 1
bisulfite
H S O4 - 1
bisulfate
C 2 H 3 O2 - 1
acetate
2- ions O2S2-
oxide sulfide
C O3 2 -
carbonate
S O3 2 -
sulfite
S O4 2 -
sulfate
3- ions N3P 3-
nitride phosphide
P O3 3 -
phosphite
P O4 3 -
phosphate
