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1 ©Prof. Zvi C. Koren 24.10.07
'חלק ב -3נושא
ונוסחאות, יונים, תרכובות, מולקולות
2 ©Prof. Zvi C. Koren 24.10.07
NOT composed of ions
(but consist of partial charges: δ+ and δ–)
Covalent Compounds(between Nonmetals)
3 ©Prof. Zvi C. Koren 24.10.07
C2H6O
Formulas - Representations
Molecular Formula
Condensed Structural Formula
Expanded Structural Formula
Stereo Projection Formula
Molecular Model
CH3CH2OH
OH
H
H
H
H H
CC
Example: Ethanol or Ethyl Alcohol
HO
H
H
H
H
H
CC
(ball & stick) (spacefill)
4 ©Prof. Zvi C. Koren 09.11.09
Go to the website: www.acdlabs.com/download/chemsketch
1. Fill out the form at the bottom of the window – Submit Form.
2. Accept the conditions.
3. Download only this program (from the choices that are given): chemsk12.exe
(This program will download a number of folders/files into the main folder on your
computer.)
4. Draw molecular structures with the program named “ChemSketch” (see next slide).
Drawing 3-D Molecular Structures
ACD/ChemSketch 12.0 Freeware
(ball & stick) (spacefill)
Advanced Chemistry Development Labs:
OH
CH2
CH3
(continued)
5 ©Prof. Zvi C. Koren 09.11.09
ChemSketch: Drawing 3-D Molecular Structures1. To always show C and H atoms:
Click on “Tools”, “Structure Properties”; “Properties” window appears:Click on “Atom”:
With C highlighted, check-off “Show” (twice) until appears.Highlight “H”, “Show” should be checked () already.Click on “Set Default”, and close that window.
2. To start drawing:Click anywhere on the window pane, the formula CH4 appears.
3. To substitute H with another element:Click on the element symbol (on the left), or on the small periodic table icon on the upper left side and
hit “OK”. Click on the pane (a non-metal will always appear with the correct number of H’s.)Click on one of the structures (without releasing the mouse) and drag a line to connect the 2 formulas. (Note: The program ‘knows’ that it needs to eliminate H’s.)
4. To clean the structure:Click on “Tools”, “Clean Structure”
5. To draw the 3-D structure:Click on the “3D Viewer”, which appears as an icon at top right menu.Click on the “3D Optimization” icon (5th from right).Click on the “Balls and Sticks” icon.
6. To rotate the molecule:Click and drag the structure in any direction.
7. To Change Colors: Click “Options”, “Colors”:To change background color from black (to any color, white preferred): Choose white color.To change colors of atoms: Choose the atom and its new color.
8. To copy structure and paste it into Word or PowerPoint:Click “Edit”, “Copy”. Go to Word or PowerPoint and Click “Paste Special”, “ACD 3D Object”.
Have Fun!!!
6 ©Prof. Zvi C. Koren 24.10.07
Nomenclature of Binary Nonmetal Compounds: AaBb
prefix#
mono1
di2
tri3
tetra4
penta5
hexa6
hepta7
octa8
nona9
deca10
EXAMPLES:
NF3
NO
NO2
N2O
N2O4
PCl5
SF6
S2F10
IF7
HCl
H2S
H3As
What do these molecules look like?
General Rule for AaBb:
With no H’s: (prefix mono)(Element name for A) (prefix)(name of B as an ide)
With H’s: same as above without any prefixes
H2O water
NH3 ammonia
N2H4 hydrazine
PH3 phosphine
NO nitric oxide
N2O nitrous oxide
Compounds
with
Historical Names
(do not follow the rules):
nitrogen trifluoride
nitrogen monoxide
nitrogen dioxide
dinitrogen monoxide
dinitrogen tetraoxide
phosphorus pentachloride
sulfur hexafluoride
disulfur decafluoride
iodine heptafluoride
hydrogen chloride
hydrogen sulfide
hydrogen arsenide
7 ©Prof. Zvi C. Koren 24.10.07
Nomenclature of Polyatomic Anions – Group 4A - C
6A5A4A
ONC
Si
1A
H
Without “O”: as an –ideCN–, CN– cyanide
For Oxyanion: suffix is –ateOCN– cyanate
SCN– thiocyanateO
C
O-
O
C
O-
HO-
O
O
C
C2H3O2 – acetate
CH3CO2–
Ac– O-CH3
O
C
O-O-
O
C
HCO3– hydrogen carbonate
(or bicarbonate)
CO32– carbonate
SiO32– silicate
C2O42– oxalate
Prefix “thio” is used when O S
Example: OCN– SCN–
8 ©Prof. Zvi C. Koren 24.10.07
Nomenclature of Polyatomic Anions – Group 5A
1A
H6A5A
ON
P
As
Also for As replacing P
nitrite ion NO2–
nitrate NO3–
phosphite PO33–
phosphate PO43–
hydrogen phosphate HPO42–
dihydrogen phosphate H2PO4–
hydrogen phosphite HPO32–
dihydrogen phosphite H2PO3–
O
3
Polyatomic Cation
NH4+ ammonium
XOn–1 = -ite
XOn = -ate
9 ©Prof. Zvi C. Koren 24.10.07
Nomenclature of Polyatomic Anions – Group 6A
1A
H
XOn–1 = -ite
XOn = -ate
hydroxide ion OH–
sulfite SO32–
thiosulfite S2O22–
sulfate SO42–
thiosulfate S2O32–
hydrogen sulfate HSO4–
(or bisulfate)
6A
O
S
Se
Te
oxide ion O2–
peroxide O22–
superoxide O2–
hydrogen sulfite HSO3–
(or bisulfite)
Prefix “thio” is used when O S
Example: OCN– SCN–
What are the names of the following
anions:
SeO32–
TeO42–
SeSO22–
TeSO32–
10 ©Prof. Zvi C. Koren 24.10.07
Nomenclature of Polyatomic Anions – Group 7A
1A
H
chlorite ClO2–
chlorate ClO3–
7A6A
FO
Cl
Br
I
At
perchlorate ClO4–
hypochlorite ClO–
XOn–1 = hypo- -ite
XOn–1 = -ite
XOn = -ate
XOn+1 = per- -ate
X = halogen
11 ©Prof. Zvi C. Koren 24.10.07
Nomenclature of Transition Metal Polyatomic Anions
chromate CrO42–
6A
O
7B6B
MnCr
dichromate Cr2O72–
permanganate MnO4–
12 ©Prof. Zvi C. Koren 24.10.07
Substance with an ionizable proton in an aqueous solution: HCl(aq) H+ + Cl–
Naming Acids
• If anion’s suffix is ide, the acid’s name is: hydro(anion root name)ic acid:
Compound(aq), AcidPure CompoundAnion
HCl(aq), hydrochloric acidHCl(g), hydrogen chlorideCl– chloride
HBr(aq), hydrobromic acidHBr(g), hydrogen bromideBr– bromide
H2S(aq), hydrosulfuric acidH2S(g), hydrogen sulfideS2– sulfide
HCN(aq), hydrocyanic acidHCN, hydrogen cyanideCN– cyanide
• For oxyacids (oxoacids):if anion’s suffix is ate, the acid’s name is: (anion root name)ic acidif anion’s suffix is ite, the acid’s name is: (anion root name)ous acid
HNO3(aq) nitric acidNO3– nitrate
HNO2(aq) nitrous acidNO2– nitrite
H2SO3(aq) sulfurous acidSO32– sulfite
H2SO4(aq) sulfuric acidSO42– sulfate
HOCl(aq) hypochlorous acidClO– hypochlorite
HClO2(aq) chlorous acidClO2– chlorite
HClO3(aq) chloric acidClO3– chlorate
HClO4(aq) perchloric acidClO4– perchlorate
H3PO4(aq) phosphoric acidPO43– phosphate
H3PO3(aq) phosphorous acidPO33– phosphite
13 ©Prof. Zvi C. Koren 24.10.07
Nomenclature of Selected Inorganic Compounds
Ionic Compound Covalent Compound
Cation Anion
Metal(or NH4
+)monatomic
(or -ide)oxyanion(-ate, -ite)
metal nameor
ammonium(root)ide (root)ate (root)ite+
Ba(NO2)2Na2Cr2O7MgCl2
barium nitrite
sodium dichromate magnesium
chloride
AgOBrHg2(ClO4)2Fe2S3
silver hypobromite
mercury(I) perchloratemercurous “
iron(III) sulfideferric “
Na2SO3Ca(OCN)2KO2
sodium sulfite
calcium cyanatepotassium superoxide
Binary (without H)
AaBb
(#a1)(A name)(#b)(B root)ide
HNO2(aq)H2CrO4(aq)HI(aq)H2SN2O5
nitrous acidchromic acidhydroiodic
acid
hydrogen
sulfide
dinitrogen
pentoxide
H2SO3(aq)H2C2O4(aq)H2Se(aq)HC2H3O2SF6
sulfurous
acidoxalic acid
hydroselenic
acid
hydrogen
acetate
sulfur
hexafluoride
HClO(aq)HC2H3O2(aq)H2S(aq)HNO2CO
hypochlorous
acidacetic acid
hydrosulfuric
acid
hydrogen
nitrite
carbon
monoxide
With H
HnX(pure)
X = -ide, -ate, or -itehydrogen (root)(suffix)
HnX(aq) = acid
if X = -idehydro(root)ic
acid
if X = -ate(root)ic
acid
if X = -ite(root)ous
acid
14 ©Prof. Zvi C. Koren 24.10.07
Hydrated Compounds
15 ©Prof. Zvi C. Koren 24.10.07
Nomenclature of Selected Compounds
Formula Name
MgCl2 magnesium chloride
Fe(ClO3)3 iron(III) chlorate ALSO ferric chlorate
Fe(ClO2)2 iron(II) chlorite ALSO ferrous chlorite
Mg(SCN)2 magnesium thiocyanate
N2O5 dinitrogen pentoxide
HCl(g) hydrogen chloride
HCl(aq) hydrochloric acid
HClO3(aq) chloric acid
HClO2(aq) chlorous acid
הטבלה הבאה תינתן בבוחן
16 ©Prof. Zvi C. Koren 24.10.07
Impossible (?) Formulas
HIJKLMNO
BaNa2
NAg
MgNiV
13Al–1H–19K–9F–19K
S H NU K Ra
Au
L )ארגון אשלגן חנקן הליום גופרית R):