Ultimate Equations Handbook

Ultimate Equations Handbook
Nomenclature-a system of naming and writing formulas for chemical compounds using the “chemical alphabet”; the symbols of elements. Exercise 1-1 and 1-2; answer these from the reading of pages You may write on the copies, but the answer sheet only will be accepted at the end of each assignment.

I.U.P.A.C. recommendations
Because new elements are being synthesized and disagreement exists among chemists regarding new names, a system for new element names has been proposed. Latin prefixes are used with the –ium suffix See pages 6-7 in handout. Would this system be a better way to name all elements and compounds? What would the name of table salt (NaCl) be? Ununium unseptide!

Most elements do not exist in their elemental state
Most elements do not exist in their elemental state! We have to be able to name their compounds Mercury is a natural component of the earth, with an average abundance of approximately 0.05 mg/kg in the earth’s crust, with significant local variations. Mercury ores that are mined generally contain about one percent mercury, although the strata mined in Spain typically contain up to percent mercury. While about 25 principal mercury minerals are known, virtually the only deposits that have been harvested for the extraction of mercury are cinnabar (HgS).

Inorganic Formulas and Nomenclature….handbook Ch. 2
Binary Molecules (nonmetal + nonmetal) Naming: use prefixes on page 9 to specify the number of atoms in the formula. DO NOT use the prefix mono- for the first element. Add the suffix -ide to the second element Examples; CO2 carbon dioxide N2O4 dinitrogen tetraoxide P4S10 tetraphosphorous decasulfide

Inorganic Formulas and Nomenclature
3. Writing formulas: write symbols with subscripts that equal the number specified by the prefixes in the name. 4. Examples: silicon dioxide SiO2 diarsenic tritelluride As2Te3 bromine monochloride BrCl

Nonmetal “stems” Element Stem (add –ide) oxygen ox chlorine chlor
Carbon carb iodine iod bromine brom selenium selen nitrogen nitr phosphorus phosph fluorine fluor sulfur sulf silicon silic arsenic arsen tellurium tellur astatine astat boron bor

Polyatomic elements Some nonmetals combine with each other to form diatomic molecules, these are the H-O-F-Br-I-N-Cl elements. O Must show that two atoms are combined 2 Natural form of sulfur is S8, phosphorus is P4

Molecules only practice:
1. As4O10 tetraarsenic decaoxide 2. N2O5 Dinitrogen pentaoxide 3. ICl3 Iodine trichloride 4. PCl5 Phosphorous pentachloride 5. CCl4 Carbon tetrachloride

6. CCl4 Carbon tetrachloride 7. CO Carbon monoxide 8. N2O Dinitrogen monoxide 9. SiI4 Silicon tetraiodide 10. P3N5 Phosphorous pentanitride

11. NI3 Nitrogen triiodide 12. P4S10 Phosphorous decasulfide 13. SiS Silicon disulfide 14. Cl2O7 Dichlorine heptoxide 15. BF3 Boron trifluoride

Salts vs. Molecules Metals easily lose electrons, this makes a metallic atom into an ion with a _____charge. These are called cations. Nonmetals easily gain electrons, this makes a nonmetallic atom into an ion with a _____charge. These are called anions. In a salt, the opposite charges of the cations and anions create an attractive force between the ions, an ionic bond.

Salts vs. Molecules The charged end of an ionic unit attracts other units and forms a large crystal. Salts exist in this form: many ionic units attracting one another in a crystal. In a molecule, the atoms of each nonmetal share electrons, so neither end of the molecule is “+” or “”. A Covalent bond is formed. Usually, less attraction exists between molecules and they can exist independently.

Binary salts (metal + nonmetal) IONIC 1. Naming: prefixes used for giving the number of atoms of each element are NEVER used to name a salt. Name the first element (the metal) followed by the second element with the -ide suffix. 2. Examples: CaCl2 calcium chloride MgO magnesium oxide Al2S3 aluminum sulfide

3. Writing formulas: the name will tell you what elements to write symbols for, but it will NOT tell you how many of each atom are present. Salts are always composed of cations and anions and charges must balance out in the formula. A shortcut is the “criss- cross” method to get the right formula. You can find the charges on the p-table if you have labeled it with “typical”  charges. Calcium nitride; From the p-table 2+ 3- Ca N (6+) (6-) 3 2

Loss or gain of electrons by atoms leads to full, more stable energy levels as found in the noble gases (He, Ne, Ar, Kr, Xe, Rn). This loss or gain leads to the formation of cations and anions. 1+ 2+ 3+ 4+/- 3- 2- 1-

4. Examples: strontium iodide SrI2 lithium oxide Li2O gallium arsenide GaAs

Rules for binary formulas:
Does name contain prefixes and 2 nonmetals? Yes…….. Write symbols FOLLOWED by prefix numbers as SUBSCRIPTS No……… Write symbols and look up cation/anion charges on p-table “criss-cross” charge numbers to become subscripts and reduce if possible

Exercise 2-1 additional practice:
1. AlN I Aluminum nitride 2. BeBr2 I Beryllium bromide 3. As4O10 M tetrarsenic decaoxide 4. Ba2Si I Barium silicide 5. CaPo I calcium polonide 6. N2O5 M Dinitrogen pentaoxide 7. Cs3As I Cesium arsenide

Practice ICl3 M iodine trichloride StS I Strontium sulfide CaSe
I Calcium selenide Rb3P I Rubidium phosphide PCl5 M Phosphorus pentachloride HF I hydrogen fluoride AlP I Aluminum phosphide

Practice LiH I lithium hydride CCl4 M carbon tetrachloride CO
M Carbon monoxide ZnI2 I Zinc iodide CaO I Calcium oxide RaBr2 I radium bromide N2O M Dinitrogen monoxide

Practice SiI4 M silicon tetraiodide P3N5 M Triphosphorus pentanitride
K4Si I Potassium silicide NaAt I Sodium astatide NI3 M nitrogen triiodide Ga2Te3 I gallium telluride Ag2O I silver oxide

Indium iodide I InI3 Sulfur hexafluoride M SF6 Ca3N2 I calcium nitride P4S10 M tetraphosphorus decaoxide Aluminum arsenide I AlAs Silver chloride I AgCl CH4 M carbon tetrahydride Hydrogen sulfide M H2S Potassium phosphide I K3P NCl3 M nitrogen trichloride More practice…on white sheet: turn over when done, hold up when prompted

Exercise 2-1 I calcium fluoride M tetraphosphorous decaoxide
I potassium sulfide I sodium hydride I aluminum selenide M dinitrogen monoxide M dioxygen monofluoride M sulfur hexabromide I lithium telluride

Exercise 2-1 10. I Strontium iodide 11. M Carbon monoxide
12. I Cesium polonide 13. I Zinc astatide 14. M Diphosphorus trisulfide 15. I Silver chloride 16. I Sodium nitride 17. I Magnesium phosphide 18. M Xenon hexafluoride

Quiz 1: Like Exercise 2-1 but you will also have to write formulas!
UE Book Quiz #1 Quiz 1: Like Exercise 2-1 but you will also have to write formulas! Quiz 2: You will write formulas ONLY!

Transition metals with variable charge
Note: several elements outside the “transition metal” columns carry more than one charge….see page 14 in UE handbook for these This table shows some of the oxidation states found in compounds of the transition-metal elements. A solid circle represents a common oxidation state, and a ring represents a less common (less energetically favourable) oxidation state.

Handbook Ch. 3 = 7+ KMnO4 2-(4) = 8- 1+ ?
Many element charges (oxidation states) can vary when combined with two or more elements. NOTE: the charges you have labeled on your periodic table are the MOST COMMON for BINARY SALTS ONLY! The formula below is NOT a binary salt! To determine the charge of one element, use the common charge of the other elements: KMnO4 2-(4) = 8- 1+ = 7+ ?

Handbook Ch. 3 Determine unknown charge from KNOWN charges, look at your periodic table! Be careful with parentheses: Mg(BF4)2 2+ 4(1-) x 2 = 8- The B would have to = 3+ (x2 = 6+)

Metals with variable charge…handbook Ch. 3
Many transition metals and metals such as tin and lead exhibit multiple valences; they can have more than one positive charge. Stock system (older) was a way of identifying which charge was present. NOTE TYPO ON GREEN SHEET! 3+ Fe is ferric Fe is ferrous 2+

Metals with variable charge
In the newer system, roman numerals are used in the name to indicate the charge of the metal cation: 2+ Fe is iron(II) Fe is iron(III) 3+

One can always determine the charge of a transition metal in a compound by knowing the charge of the other element. What is the charge of the copper cation, +1 or +2? 2- Charge ? We know from the p-table that oxygen is a 2- CuO “copper (II) oxide” What would the charge of the copper have to be to “balance” the oxygen? 2+

3+ 2- FeS 2 3 Which iron is it? Iron(II) or Iron(III)? Figure it out from the nonmetal (sulfur). You can also criss-cross from the bottom up. SEE PAGE 14 FOR LIST!

When naming compounds, ask……
Is the first element a nonmetal? If yes, use prefixes and end in –ide If no, is it a metal from page 14? If yes, use a roman numeral in the name for the charge of the element and end in –ide. If not on page 14, it is an ionic salt, name it with an –ide ending.

When writing formulas, ask……..
Is the first element a nonmetal? If so, use the prefixes in the name to write formula. If the first element is a metal followed by a roman numeral in parentheses, the roman numeral is the charge of the metal. Cross this charge with the nonmetal charge. If the first element is a metal NOT followed by a roman numeral, look up and cross the metal/nonmetal charges.

Binary compounds flowchart
Type I: M-NM Type II: TM-NM Type III: NM-NM Will ALWAYS end with nonmetal name and –ide suffix You can tell if it does, it’s a TM, it is on page 14!

TM salt formulas from names
The metal charge (always first element) will be given by the roman numeral Look up the nonmetal charge on your p-table and cross them. Reduce if possible Bismuth(V)sulfide Bi S Bi2S5 5+ 2-

Sample quiz items CeO2 Cerium(IV)oxide 2. W3N5 Tungsten(V)nitride
3. MnCl3 Manganese(III)chloride 4. CoTe Cobalt(II)telluride 5. PbS Lead(II)sulfide

Sample quiz items Iron(III)silicide Fe4Si3 Bismuth(V)selenide Bi2Se5
Gold(III)phosphide AuP Zirconium(IV)astatide ZrAt4 Titanium(II)bromide TiBr2

Sample quiz items Cu3P2 Copper(II)phosphide Hg2S Mercury(I)sulfide
InI3 Indium(III)iodide VN Vanadium(III)nitride SnO Tin(II)oxide

Sample quiz items Thallium(II)oxide TlO Chromium(III)phosphide CrP
Platinum(IV)selenide PtSe2 Antimony(III)fluoride SbF3 Iridium(IV)phosphide Ir3P4

Sample quiz items U2Te5 Uranium(V)telluride CeBr3 Cerium(III)bromide
CuCl Copper(I)chloride Pt2Si Platinum(II)silicide PbO2 Lead(IV)oxide

Sample quiz items Manganese(II)astatide MnAt2 Bismuth(III)arsenide
BiAs Gold(I)sulfide Au2S

Handbook Ch. 3 You should now be able to do exercise 3-1, 3-2 (3, 4, 9, 16) and 3-3 (1, 14) Next quiz will be Transition metal salts ONLY: 3-2: 3, 4, 9, 16 and 3-3: 1,14. (You must use a roman numeral in the name) Use page 14!

Exercise 3-2, 3-3 Teams 1, 3, 5 do… Teams 2, 4, 6 do… 3-2: 3, 4, 9, 13
3-2: 3, 4, 9, 13 3-3: 1, 2, 5 Teams 2, 4, 6 do… 3-2: 14, 15, 16, 19, 20 3-3: 9, 14

Informal “quiz” banana BaNa2 Ba/Na2 banana split
banana split with a cherry on top CH2O sea water

Informal “quiz” HIJKLMNO water HIOAg hi-o-silver H2OGa8 watergate
(GON)5 pentagon

Informal “quiz” Co3La co-co-co-la Co(Fe)2 coffee K9P dog pee

Exercise 3-1 2- 7+ 1+ 4+ 2+ 6+

Exercise 3-1 3+ 4+ 5+ 6+

Exercise 3-2 and 3-3 binary or elemental compounds
3. Mercury(I)chloride 4. Silver bromide Tin(IV)oxide Dinitrogen tetraoxide Rubidium phosphide Sulfur Iron(III)oxide Phosphorus pentafluoride Lithium hydride

Exercise 3-2 and 3-3 Binary or elemental compounds
V2O5 H2O P4O10 O2 Mn2O7

Individual practice-HOMEWORK
Create a table/grid to write the formulas of each metal below with group 15, 16, 17 nonmetals Copper(II), Mercury(I), Mercury(II), Gold(III), Chromium(II), Iron(III), Lead(IV), Tungsten(V)

WRITE FORMULA AND NAME IN EACH BOX!
Homework table N P As O S Se Te F Cl Br I- Cu2+ Hg2+ Hg22+ Au3+ Cr2+ Fe3+ Pb4+ W5+ Zn2+ Cu3N2 Copper(II) nitride WRITE FORMULA AND NAME IN EACH BOX!

Quiz 2 from Ch. 1-4 Handout This quiz will be much like exercises 3-1, 3-2 and 3-3[3-2 (3, 4, 9, 16) and 3-3 (1, 14)] You will determine the charge of elements by deduction. (3-1) You will name transition metal salts by writing the metal name first followed by a roman numeral (unless it is silver or zinc) then the nonmetal with the ending –ide. 3-2 (3, 4, 9, 13-16, 19, 20) USE PAGE 14! You will write the formulas of transition metal salts by listing the metal symbol followed by the nonmetal symbol with their charges canceling out as subscripts (criss-cross). Remember that the roman numeral in the name is the charge of the transition metal. 3-3 (1, 2, 5, 9, 14, 17) NOTE: ALL CHEMICAL NAMES AND FORMULAS ON THIS QUIZ WILL BEGIN WITH A METAL FROM PAGE 14(MUST USE ROMAN NUMERAL IN NAME): I, II, III, IV, V, VI, VII, VIII, IX, X

Polyatomic ions MnO 4 1- “leftover” 7+ 2-
Some elements combine to form ions, not molecules. These are called polyatomic ions. See page 16. When they react, they form ternary compounds. Note page 16 in handout and reference sheet. Nearly all of these end in –ate or –ite. Poly anions/cations by charge and those which end in -ide Permanganate ion: 1- “leftover” MnO 4 7+ 2-

Polyatomic ions ClO4 perchlorate ClO3 chlorate ClO2 chlorite
These groups of atoms behave as single ions. There is no simple way to learn these, other than seeing the patterns in their families. For example, Cl and O can be “parent” ions…… see page 16 ClO4 perchlorate ClO3 chlorate ClO2 chlorite ClO hypochlorite # of oxygen atoms

Oxygen “family” of ions
Oxide = O2 Peroxide = O22…..each “O” is a 1- Superoxide = O21…one “O” is neutral and one “O” is a 1- Hydroxide = OH1−…“O” is 2- and H is 1+

Organic ions Carbon atoms are the “central” atoms with surrounding hydrogen and oxygen atoms: Can be written CH3COO or C2H3O2 (Acetate ion)

Ternary formulas and names….. I do, we do
When naming, simply use the periodic table and page 16 to combine the names of the element or ion(s). NEVER CHANGE THEIR SUFFIX ENDINGS! ALSO USE REFERENCE TABLE “POLYATOMIC IONS” MgCO3 Magnesium carbonate Cu(OH)2 Copper(II)hydroxide NH4Cl Ammonium chloride

Ternary formulas and names
When writing formulas, look up the symbols and charges of the element or ion(s) and cross them. Use parentheses if necessary: Iron(II)phosphate Fe3(PO4)2 Potassium sulfate K2SO4 Sodium hypochlorite NaClO

More I do….we do Na3PO4 2. aluminum hydroxide
CuSO potassium benzoate NH4F 6. zinc acetate CaC rubidium carbonate 9. LiOH iron(III)bicarbonate

Naming Ternary compounds (3 or more elements)
First element will be a metal or NH4+ If metal is not a transition metal (group 1 or 2) name the metal followed by the polyatomic ion name. If metal is from group 3-16, check to see if it is on page 14. If not, name as above. If on page 14, name metal followed by its charge in roman numerals and then name the polyatomic ion.

Formulas of ternary compounds
Look up metal symbol and charge from p-table or use roman numeral if present. Look up polyatomic ion formula and charge. Cross metal charge # to make subscript for poly ion, cross poly ion charge # to make subscript for metal. Reduce charge # if possible.

Exercise 3-2 on white sheet
You do… 3-2: 1, 2, 5, 6, 7, 8 / 10, 11, 12, 17, 18, 21 3-3: 3, 4, 6, 7, 8, 10 / 11, 12, 13, 15-20

Hydrated salts If first dissolved in water, many salts will “take-up” water molecules in their crystals as the water is evaporated. Their chemical formulas and names will indicate this in the following ways: Na2B4O7 • 10 H2O is sodium tetraborate decahydrate, or “borax” CaSO4 • 2 H2O is calcium sulfate dihydrate, or “gypsum” CuSO4 • 5H2O is copper (II) sulfate pentahydrate

Summary of Handbook Ch. 2 and 3
Determining whether or not the first element in the compound is a metal or nonmetal is the most important question. Apply the rules from there. When naming compounds that contain a transition metal (page 14) with variable charge as the first element, use roman numerals to indicate valence. When naming compounds that contain 3 or more elements, a polyatomic ion is present, use page 16 or reference sheet.

Teams on 3-2, 3-3 (poly ions) Team and number:
1; 3-2: 1,2…….3-3: 3,4,6 2; 3-2: 5,6…….3-3: 7,8 3; 3-2: 7,8…….3-3: 10,11 4; 3-2: 10,11….3-3: 12,13 5; 3-2: 12,17….3-3: 15,16,17 6; 3-2: 18,21….3-3: 18,19,20

Exercises 3-2 and 3-3 (with Poly ions)
Iron(II)sulfite Copper(II)nitrate Potassium chlorate Magnesium carbonate Barium peroxide Potassium superoxide (see page 11) Lead(II)hydroxide Nickel(II)phosphate Copper(I)acetate Ammonium sulfite Calcium permanganate 21. Titanium(IV)monohydrogen phosphate

Exercises 3-2 and 3-3 (with Poly ions)
(NH4)2C2O4 Po(SCN)6 Zn(OH)2 KCN Cs2C4H4O6 Hg(CH3COO)2 Ag2CrO4 SnCO3 NaHCO3 Cu(H2PO4)2 Fr2Cr2O7 CaC2 Hg2(NO3)2 Ce(C6H5COO)4 KHC8H4O4

Nomenclature quiz format
Write name and formulas for type I, II, II, and IV Type I Sodium nitride Na3N CaBr2 Calcium bromide

Type II Iron(II)sulfide FeS MnO2 Manganese(IV) oxide

Type III Dichlorine heptasulfide Cl2S7 BrI Bromine monoiodide

Type IV Ammonium chloride NH4Cl Al2(SO4)3 Aluminum sulfate Vanadium(V)carbonate V2(CO3)5 Cu3(PO4)2 Copper(II)phosphate

(see that you may also need page 14)
Quiz 3 over 3-2, 3-3 Questions from exercises 3-2 or 3-3? NO binary compounds…this means you will need page 16 to name and find formulas of ions for EVERY QUESTION ON THE QUIZ!** Name from formula: FeSO4 Iron(II)sulfate (see that you may also need page 14) Formula from name: potassium dichromate K2Cr2O7

Quiz 3-Practice Naming: Follow the rules we have covered so far and use page 16 for polyatomic ion names! Na2CO3 Fe(OH)3 H2O2………be careful with this one!

K2MnO4 Al(HCO3)3 Na3C6H5O7 NH4Cl

Quiz 3-Practice Writing formulas; follow the rules we have covered so far for metal-nonmetal compounds by crossing charges….use parentheses when you need more than one of a polyatomic ion! Potassium sulfate Ammonium phosphate Aluminum carbonate

mercury(I)cyanide calcium carbide (binary, but with a poly-ion) gallium selenate lead(II)acetate

Sodium carbonate Potassium sulfate Iron(III)acetate Magnesium selenate
TERNARY COMPOUND NAMES/FORMULAS ASSIGNMENT: DUE THURSDAY (use pages 14,16) Sodium carbonate Potassium sulfate Iron(III)acetate Magnesium selenate Copper(II)zincate

6. Ammonium chloride 7. Lithium phosphate 8. Lead(II)chlorate 9. Calcium carbide 10. Zinc phosphite…use phosphate to figure this out

Vanadium (V) peroxide Cerium (IV) benzoate Silver dichromate Manganese(II)nitrate Mercury(I)cyanide

16. Ca(IO3)2 17. Bi2(MnO4)3 18. NaClO 19. Fe(OH)3 20. Cr(ClO3)3

CuS2O3 NaHCO3 Pt(SO3)2 Ir(SCN)3 SrC2O4

26. Bi2(C2O4)5 27. NH4CH3COO 28. Na2O2 29. K2S2O3 30. PbSiO4

H2O(l) + HCl(g) ↓ H3O+(aq) + Cl-(aq)
Acids-notes for Ch. 4 Contain “ionizable” hydrogen ions, H+ When dissolved in water, some or all of the H+ ions separate from the anions and combine with water to form the acidic hydronium ion, H3O+ H2O(l) + HCl(g) ↓ H3O+(aq) + Cl-(aq) The hydrogen monochloride gas, when aqueous, is called hydrochloric acid

Acid Nomenclature…handbook ch. 4
Acids and Salts; Acidic compounds contain H+ ions in solution (aq), basic compounds contain OH in solution. When acids and bases react, they form water and a salt, either binary or ternary. HCl + NaOH  HOH + NaCl Acid Base Water Salt

Acid Nomenclature Inorganic acids-first element always hydrogen in 1+ oxidation state (charges crossed) Are there 3 or more elements? Yes No (these are binary) Name the acid using the polyatomic ion root (see page 16) -ide* ion Name the acid with the hydro- prefix followed by the root of the nonmetal with the –ic suffix -ite ion ends in -ous -ate ion ends in -ic *Cyanide, etc.

Acids………H1+ + any anion = ACID
H+ and Cl …….chloride……………….hydrochloric acid(HCl) H+ and ClO ……hypochlorite………….hypochlorous acid(HClO) H+ and ClO2 ……chlorite………………..chlorous acid(HClO2) H+ and ClO3 ……chlorate……………….chloric acid(HClO3) H+ and ClO4……perchlorate……………perchloric acid(HClO4) NOTE: THE LAST 4 IONS LISTED ABOVE ARE POLYATOMIC, MEANING THEY ARE FOUND ON PAGE 16

Acid Nomenclature Organic acids-carbon linked to –OOH
“R” represents additional hydrogen or carbon links The number of carbon atoms and the ending -anoic are used in naming CH3COOH contains 2-carbon atoms, prefix in organic chemistry for 2 = “eth”. The acid is “ethanoic”

Summary Hydro-root-ic from –ide Root-ic from –ate Root-ous from –ite

Acid names practice HCl Hydrochloric acid H2SO4 Sulfuric acid HF
Hydrofluoric acid CH3COOH Acetic acid HI Hydriodic acid H2Se Hydroselenic acid H2SO3 Sulfurous acid

Acid names practice H2S Hydrosulfuric acid HClO4 Perchloric acid HAt
Hydroastatic acid C6H5COOH Benzoic acid HBr Hydrobromic acid H2Te Hydrotelluric acid H2S2O8 Peroxydisulfuric acid

Acid names practice H2O Hydroxic acid H3P Hydrophosphoric acid H4Si
Hydrosilicic acid HCOOH Formic acid H3As Hydroarsenic acid H3AsO4 Arsenic acid H2C4O6 Tartaric acid

Acid Formulas H 1+ I 1- = HI H 1+ CO32- = H2CO3
Acid formulas: must begin* with H cation in the 1+ valence. If the acid begins with hydro- , find the anion and its charge on the p-table-the acid is binary (cyanide exception, etc.) If the acid does not begin with hydro- , find the anion on page 16 or ref. sheet. An –ate anion = -ic acid. An –ite anion = -ous acid. A hypo- root –ite anion = hypo- root –ous acid. Criss-cross the H 1+ with the anion charge Examples: hydriodic acid, carbonic acid H 1+ I 1- = HI H 1+ CO32- = H2CO3

Acid formulas practice – do on white board with partners
Hydrosulfuric H2S Hydrocyanic HCN Cyanic HOCN Nitric HNO3 Selenic acid H2SeO4 Telluric acid H2TeO4 Boric acid H3BO3

Acid formulas practice
Phosphorous acid – H3PO3 Perchloric acid – HClO4 Hydrobromic acid – HBr Hypobromous acid - HBrO Tellurous acid – H2TeO3 Iodous acid – HIO2 Hydroarsenic acid – H3As

Common strong acids you should know…put these on reference sheet or p-table
Hydrochloric-HCl (stomach acid) Hydrobromic-HBr (used to produce metal bromides) Hydroiodic-HI (used to treat asthma) Chloric-HClO3 (an accelerant) Perchloric-HClO4 (produces shock sensitive salts) Periodic-HIO4 (lab reagent) Nitric-HNO3 (fertilizers, explosives, flares) Sulfuric-H2SO4 (car battery acid)

4-1, 4-2 Iodic acid Periodic acid Hydroastatic acid Benzoic acid
Phosphorous acid H2C4H4O6 H2Te H2CO3 HIO HOCN H2C8H4O4

Name of Acid Formula of Acid Name of Anion Hydrochloric acid HCl
Chloride Sulfuric acid H2SO4 Sulfate Hydriodic acid HI Iodide Sulfurous H2SO3 Sulfite Chlorous acid HClO2 Chlorite Nitric acid HNO3 Nitrate Acetic acid HC2H3O2 or CH3COOH Acetate Hydrobromic acid HBr Bromide Hydrosulfuric acid H2S Sulfide Nitrous acid HNO2 Nitrite Chromic acid H2CrO4 Chromate Phosphoric acid H3PO4 Phosphate

Chem Nomenclature Review Organizer

Chemical Nomenclature Quiz Practice (all 4 chapters)
FeCrO4 Iron(II)chromate Na2O Sodium oxide H2CO3 Carbonic acid (hydrogen carbonate) CuS Copper(II)sulfide CF4 Carbon tetrafluoride

Chemical Nomenclature Quiz Practice (all 4 chapters)
Ca(OH)2 Calcium hydroxide Xenon hexafluoride XeF6 Hypochlorous acid HClO Molybdenum(VI)selenide MoSe3 Aluminum phosphide AlP Lead(IV)bromide PbBr4

Chemical nomenclature quiz practice (molecular names/formulas, salt names) thru Ch. 2
Dinitrogen monoxide Na2Se Sodium selenide Xenon hexafluoride XeF6 Iodine trichloride ICl3 ZnF2 Zinc fluoride

Chemical nomenclature quiz practice (molecular names/formulas, salt names) thru Ch. 2
BaS Barium sulfide Silicon dioxide SiO2 Triarsenic pentachloride As3Cl5 BAt3 Boron triastatide Al2N3 Aluminum nitride

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