Structural Formulas AGENDA: Review Check homework Notes on Structural Formulas Homework: Drawing Formluas

Repetition Ionic Electrons are… Types of elements… Naming Covalent Electrons are… Type of elements Naming

Iron (II) oxide FeO

Carbon monoxide CO

Sodium nitrate NaNO 3

Carbon dioxide CO 2

Na + Sodium ion

Carbon tetrachloride CCl 4

Mg 3 (PO 4 ) 2 Magnesium phosphate

SiF 4 Silicon tetrafluoride

Magnesium chlorate Mg(ClO 3 ) 2

SO 2 Sulfur dioxide

Cl - Chloride

SO 3 Sulfur trioxide

ClO 3 - chlorate

Boron trichloride BCl 3

Sodium chloride NaCl

Germanium tetrafluoride GeF 4

CaCO 3 Calcium carbonate

Aluminum sulfide Al 2 S 3

NI 3 Nitrogen triiodide

(NH 4 ) 2 CrO 4 Ammonium chromate

Iron (II) ion Fe +2

carbonate CO 3 -2

H2OH2O Dihydrogen monoxide water

CoBr 2 Cobalt (II) bromide

Na 2 CO 3 Sodium carbonate

Oxide O -2

H2SH2S Dihydrogen monosulfide

Li 3 PO 3 Lithium phosphite

Barium hydroxide Ba(OH) 2

Na 2 SiO 2 Sodium silicate

Homework Check

Mixed naming 1.Sodium bromide 2.Dinitrogen tetrafluoride 3.Lithium hydroxide 4.Mercury (I) hydroxide 5.Sulfur difluoride 6.Iron (II) chloride 7.Barium acetate 8.Selenium trioxide 9.Ammonium nitrate 10.Copper (I) oxide 11.Aluminum sulfate 12.Ammonium chloride 13.Nitrogen trifluoride 14.Barium phosphate 15.Sodium sulfate 16.Lead (II) hydroxide 17.Nitrogen monoxide 18.Sodium bicarbonate 19.Sulfur trioxide 20.Cadmium nitrite 21.Selenium dioxide

22.CBr 4 23.LiNO 2 24.NH 4 HSO 4 25.ClF 3 26.Hg 2 SO 4 27.Fe 2 O 3 28.Mg 3 (PO 3 ) 2 29.Ni(HCO 3 ) 2 30.H 2 O 31.(NH 4 ) 2 CO 3 32.MgBr 2 33.GaPO 4 34.KC 2 H 3 O 2 35.Cu(NO 2 ) 2 36.Ca(ClO 3 ) 2 37.SnO 2 38.NaClO 4 39.K 2 CO 3 40.Fe(OH) 2 41.Pb(ClO) 4 42.SiO 2

Binary Molecular 1.Carbon monoxide 2.Carbon dioxide 3.Iodine heptafluoride 4.Dinitrogen tetroxide 5.Boron trifluoride 6.Dinitrogen pentoxide 7.Nitrogen monoxide 8.Tetraphosphorus decoxide 9.Tetraphosphorus trisulfide 10.Phosphorus trichloride 11.Phosphorus pentachloride 12.Disulfur decafluoride 13.Disulfur heptoxide 14.P 2 O 3 15.CCl 4 16.P 4 O 6 17.N 2 F 4 18.S 2 Cl PCl 5 20.NO 2 21.N 2 O 3 22.SF 6 23.CBr 4 24.H 2 S 25.SBr 6

Naming Molecular Compounds 1.Carbon dioxide 2.Carbon monoxide 3.Sulfur dioxide 4.Sulfur trioxide 5.Dinitrogen monoxide 6.Nitrogen monoxide 7.Dinitrogen trioxide 8.Nitrogen dioxide 9.Dinitrogen tetroxide 10.Dinitrogen pentoxide 11.Phosphorus trichloride 12.Phosphorus pentachloride 13.Nitrogen trihydride 14.Sulfur hexachloride 15.Diphosphorus pentoxide 16.Carbon tetrachloride 17.Silicon dioxide 18.Carbon disulfide 19.Oxygen difluoride 20.Phosphorus tribromide

Structural Formulas Date:

Geometry of Molecular Bonds Valence Shell Electron Pair Repulsion model (VSEPR) – Electrons repel Draw the bonds as far way from each other as possible. Set structures appear

Build a model 1 black ball 4 white balls 4 short sticks

tetrahedral

Build a model Remove the “top” stick and ball

Trigonal pyramidal

Build a model Remove another stick and ball

Bent

Build a model 1 black ball 2 white balls 2 short sticks 2 long sticks 1 red ball

Trigonal planar 120 o

Build a model 2 red balls 2 long sticks

linear

FamilyOxidation ## bonds Alkali+11 Alkaline earth+22 Boron family+33 Carbon family+44 Nitrogen family-33 (or 4) Chalogens-22 Halogens1 Noble Gases00

Draw F 2, Cl 2, Br 2, I 2, H 2, O 2, N 2

Diatomics 2 atoms bonded to each other There are 7 diatomics, which make a shape of a 7 on column 7.

Bonds Single bond – Like putting desks together Double bond – Putting desks together AND – Fist pounds on either side Triple bond – Putting desks together AND – Fist pounds on either side AND – Putting heads and knees together Single bonds – long and weak Double bonds – Stronger than single – Shorter than single Triple bonds – Strongest bond – Shortest bond

Draw NH 3, CH 4, CH 3 OH

SCl 2, CF 4, COCl 2, NF 3

GeCl 4, AsCl 3, CO, CO 2

SeCl 2, NCl 3,H 2 Se

AsF 3, SF 2, PBr 3