Re-typed from The Ultimate Chemical Equations Handbook by ...

Re-typed from The Ultimate Chemical Equations Handbook by Hague and Smith

SIMPLE INORGANIC FORMULAS AND NOMENCLATURE

Binary Molecules

I. A binary molecule is formed when two nonmetals or metalloids combine. Electrons are shared so thebonding involved is known as CD VQ LJ:::N T bonding.

2. Sometimes these compounds have generic or common names (water) and they also have systemicnames (dihydrogen monoxide). The common names must be memorized. The systemic name is morecomplicated but it has the advantage that the formula of the compound can be deduced from the name.

3. Simple binary compounds consist of only a few atoms. Systemic naming of these compounds followthe rules:

• The elements, except for H, are written in order of increasing group number.

• Prefixes are used to designate the number of each element present in the molecule.

4. The prefixes are:

rl0IJO 6 HE)<A2 DI 7 HEPTA.~-,...3 II( \ 8 otm4 TET12.A 9 "-.ION 1-1

5 Pi.::l'-iTA 10 DECIj

5. Mono is ;Jt'l./l::7L. used in front of the first element. If there is only one atom, the mono isassumed.

***** Name the following binary molecules:

(a) C02 cr·W_mAl DIOX.I])~

(b) N203 DIN IT/106EN T!2IO'IJDl.:;-

(c) P4010 It:"Tf(l::j PHoSPHoR.USiJE(.o)(.1 D i2"

(d) N20 birJ rTQ.0680 SV\otJo '1..1j)t;"

Ionic Compounds

I. Ionic compounds are formed between metals and nonmetals. The electrostatic force of attractionbetween the positive ion (cation) formed by the metal and the negative ion (anion) formed by thenonmetal is what holds the compound together.

OVER

r

2. The cation is named first and written first when writing a formula while the anion is both named andwritten second.

3. Cations can have one or more charges. These charges are known as oxidation numbers, or valences.

4. The transition metals and representative elements in Groups 13, 14, 15, and 16 have multiple oxidationnumbers.

5. Roman numerals, enclosed in parentheses, are used after the name of the cation to designate theoxidation state of the cation - only if the cation has more than one positive oxidation state from which tochoose.

6. This system of nomenclature is known as the Stock system.

7. Here are some simple rules that should help in the determination of the oxidation numbers of cationsfrom the formulas of their compounds.

(a) The oxidation number of any element in its free state (uncombined with other elements) is zero. Fein a bar of iron is zero. 02 and N2 in the atmosphere are zero.

(b) The oxidation number of the alkali metals in a compound is always 1+.

(c) The oxidation number of the alkaline earth metals in a compound is always 2+.

(d) Fluorine in a compound is always assigned an oxidation number of 1-.

(e) The oxidation number of oxygen is almost always 2- in a compound. Exceptions to this rule wouldbe peroxides, oi- where the oxidation number of each oxygen is 1-, and superoxides, Of where theoxidation number of each oxygen is Yz-.

t.\

(0 In covalent compounds (with nonmetals) hydrogen is assigned an oxidation number of 1+ (examplesare HCI, H20, NH3, CH4).

(g) In metallic halides the halogen (F, CI, Br, I, and At) always has an oxidation number equal to 1-.

(h) Sulfide, selenide, telluride, and polonide are always 2- in binary salts.

(i) Nitrides, phosphides, and arsenides are always 3- in binary salts.

U) All other oxidation numbers are assigned so that the sum of the oxidation numbers of each elementequals the net charge on the molecule or polyatomic ion. In neutral compounds, the sum of the positiveand negative charges must equal zero.

***** Determine the oxidation number of the underlined element:

+ 7 t I~

(b) NaCI04 +3


7. Free elements, no matter how complex the molecule, have an oxidation number (valence or charge)equal to zero.

OJ. Fe. T~

He < /1 1~~ L-td.

8. The following are diatomic or polyatomic elements in nature which must be committed to memory.These elements exist as neutral molecules in nature:

(a) i3r,J. (g) r,(b) J:'l (h) 03

(c) J\J.1 (i) fy

(d) CJa (j) Sl?

(e) I--b (k) C &0

(f) 0) (I) C/oCharges and the Periodic Table

1. The periodic table can be used to help determine charges on many ions. Cations come from metalsthat lose electrons ( 0 -y: I IJ tCl, TI 0 J-J ) in order to become .ISO 8-ECTl20 tJ' Cwith a noble gas. Anions come from nonmetals that gain electrons ( lZ..Ebucno Iv ) inorder to become r50E1£ CIlLo,.) f c.. with a noble gas.

*****Group 1 +1 Group 17 -I

Group 2 +~ Group 16 - .)

Group 3 +-3 Group IS -3

Group 14 -~ s« +t..J

2. Transition metals, representative metals with +and ~ sublevels, and the inner transition metalstypically have more than one oxidation state.

3. Electrons for these metallic elements are lost in the following order: ei S) J.... . Suchelements are ;...fa T isoelectronic with a noble gas when the outermost (valence) electrons are lost.

4. Inner transition elements are also known as the lanthanides, the actinides, the rare earth elements, andthe transuranium elements. These elements are rare and many exist for short periods of time.

5. Both inner transition elements and transition elements are known for their variable oxidation numbers.The most common oxidation number for transition elements is f ~

OVER

r6. The d: sublevel in transition elements is responsible for the various oxidation numbers that result.Incomplete d sublevels are also responsible for the many colorful transition compounds that are known toexist. Complete d sublevels in cations of silver and zinc result in white compounds. ! '

SUMMARY OF CATIONS WITH VARIABLE OXIDATION NUMBERS- STOCK SYSTEM

1+,2+ copper (I), Cu"; copper (II), Cu2+mercury (I), Hgr"; mercury (II), Hg2+

gold (I), Au"; gold (Ill), Au3+1+,3+ indium 0), In"; indium (III), £n3+

thallium (0, TI+; thallium ([II), T13+chromium (II), Cr2+;chromium (III), cr3+

2+,3+ cobalt (Il), C02+;cobalt (III), C03+iron (II), Fez+; iron (III), Fe3+lead (II), Pb2+; lead (IV), Pb4+

2+,4+platinum (II), peT; platinum (IV), pt+tin (II), Sn2+;tin (IV), Sn4+zirconium (II), z>. zirconium(lV), Zr4+

3+,4+ cerium (III), Ce3+;cerium (IV), Ce4+

antimony (1II),Sb3\ antimony (V), Sb5+

3+,5+arsenic (III), As3+; arsenic (V), As5+bismuth(III), Bi3+; bismuth (V), Bi5+phosphorus (III), p3+;phosphorus (V), p5+iridium (II), Ir2+;iridium (III), Ir3+;iridium (IV), Ir4+

2+,3+,4+ titanium (II), Ti2+;titanium (HI), Ti3+; titanium (IV), Ti4+manganese (II), Mnl+; manganese (III), Mn3+;manganese (IV), Mn4+

2+,4+,5+ tungsten (II), W2+; tungsten (IV), W4+; tungsten (V), W5+

3+,4+,5+ uranium (III), U3+;uranium (IV), U4+; uranium (V), U5+

2+,3+,4+, 5+ vanadium (II), VZ+; vanadium (III), V3+;vanadium (IV), V4:;

vanadium (V), V5+-

,.r\


Polyatomic Ions

I. Polyatomic ions are a group of atoms that behave as a single ion.

2. The bonding within a polyatomic ion is covalent, but because there is either an excess or a shortage ofelectrons compared to the number of protons present, an ion results.

3. This short list of polyatomic ions must be MEMORIZED.

NH4+ ammonium OR hydroxide

NOf nitrite P043- phosphate

N03- nitrate CIO- hypochlorite

so> sulfite CIOf chlorite

S042- sulfate C103• chlorate

C032• carbonate CI04- perchlorate

HC03- bicarbonate Cr042- chromate

C2H)Of acetate Cr20l· dichromate

CN- cyanide SCN- thiocyanate

You also need to know the common Group ions such as (but not limited to) the ions in Groups 1 &2, the halogens, 0, S, N, P, and "the triangle": Ag, Zn, Cd, AI, Ga, and In.

OVER

© Adrian Dingle's Chemistry Pages 2004. All rights reserved.These materials may NOT be copied or redistributed in any way, except for individual class instruction.

Revised June 2005

AP Common Ions

CAT10NS (+ve)Name Symbol Alternative"

Aluminum At'+

Ammonium NH:Arsenic (III) As3+

Arsenic (V) As~

Barium Ba2+

Bismuth (III) 8i3+

Bismuth (V) Bi~

Cadmium c<f+Calcium Ca2+Chromium (II) Cr·

Chromium (III) Cr+

Cobalt (II) C02+

Cobalt (III) Co'·Copper (I) Cu+ (Cuprous)Copper (II) Cu2+ (Cupric)Hydrogen H+

Hydronium H,O+

Iron (II) Fe2+ (Ferrous)Iron (III) Fe'+ (Ferric)Lead (II) ptf+ (Plumbous)Lead (IV) Pb" (Plumbic)lithium L(

Magnesium Mg1+

Manganese (II) Mn~+

Manganese (IV) Mn.•.•

Mercury (I) H!hz+ (Mercurous)Mercury (II) Hg2• (Mercuric)Nickel (II) Ni2+

Potassium K'"

Silver Ag+

Sodium Na+

Strontium Sr+

,Tin (II) Snz+ (Stannous)Tin (IV) Sn'" (Stannic)Zinc Znz+

ANIONS (-ve)Name Symbol Alternatlve~

Bromide BfBromate (I) BrO' (Hypobromite)Bromate (III) BrOz' (Bromite)Bromate (V) BrO,' (Bromate)Bromate (V") BrO•. (Perbromate)Carbonate C0,2'

Chlorate (I) CIO' (Hypochlortte)" Chlomte (III) CI02' (Chlorite): Chlorate (V) CIO; (Chlorate),Chlorate (VII) CIO" (Perchlorate). Chloride cr

Chromate crO.2,

, Cyanide CN"Dichromate CrzOr2,

Dihydrogen Phosphate H2POiEthanoate CzH,Oi (Acetate)Ruoride F"Hydride H'Hydrogen Carbonate He03' (Bicarbonate) /:Hydrogen Oxalate HCzO" (Binoxalate) (Hydrogen Phosphate HPO/'

\''~

,,Hydrogen Sulfate HSOi (Bisulfate )..Hydrogen Sulfide HS' (Bisulfide)

Hydrogen Sulrrte HSO)' (Bisulfite)Hydroxide OH'Iodate (I) 10' (Hypoiodile)Iodate (III) 102' (Iodite)Iodate (V) 10; (Iodate)Iodate (VII) 10. (Periodate)Iodide rManganate (V") MnO•. (Permanganate)

, Nitrote NO,'Nitride N""NiDite NOz'

Oxalate CzO/' (Ethandioate)Oxide ry-Peroxide 0/'Phosphate PO.3-Phosphide p""Phosphite PO/'Sulfate SO.z,Sulfide S1'

Sulfite 5032-

Thiosulfate S20)2-

Thiocyanate SCN"

• In the case of the cations, the alternative names are genemlly redundant in modem chemistry, but the anions sometimesuse the older, alternate names, For example, the oxyhatogen ions (bromate, chlorate, iodate stc.) are usually referred toby the altemate names, but HSOJ' is much more likely 10be called Hydrogen Sulfrte rather than Bisufite,

,---,------- ~-----


Ternary Nomenclature: Acids and salts Containing Halogens and/or Oxygen

1. The halogens, with their variable oxidation numbers, allow for a great variety of compounds.

2. A good way to learn ternary nomenclature is to start with a certain HOI'\<lE !3/1~£"polyatomic ion. This is polyatomic ion ending with the suffix - C~te

Number of Oxygen Atoms Polyatomic Ion Name(compared to home base)

Plus one oxygen atom Cl04' perchlorate ion

Home base CI03' ch lorate ion

Minus one oxygen atom CI02' chlorite ion

Minus two oxygen atoms ClO' hypochlorite ion

No oxygen atoms CI' chloride ion

3, Water solutions of binary hydrides form acids. The root derived from the hydride is given the prefixli'/ Dr2..0 - and the suffix - Ie and the name ends with the word ACt D

4. The binary hydride HCl is known as H'I Dt2.0GeJ CI-ILo.e.IOlE'when aqueous it is known as 14 'f D1200-l W.e.IL !~C ID

(hydrogen monochloride) gas, but

5. Many common acids contain only oxygen, hydrogen, and a nonmetallic ion or polyatomic ion. Theseacids are called _-=O...:..Y--...:'1..:.,i-\,!.,:C:..;I.::::.b..=S=-- _

6, If the name of the polyatomic ion ends in - ['L+e , the suffixthe word acid.

7. If the name of the polyatomic ion ends in - / te. , the suffix - OUSis substituted followed bythe word acid.

1/

- f c..- is substituted followed by

8, The mnemonic aid is: (cfe- ic. ('fe - OU.5

***** Name the following compounds:

(a) HI04 (aq) PERIOble. I~( 11)

(b) NaBr04Sdb \vyt, eEQ8~Oi!~\(~TE

OVER

***** Write the formulas for the following compounds:

(a) calcium hypochlorite Cl\. ( OD)::I (c) cyanic acidIi (NO O!L iioe iJ

(b) hydrotelluric acid H.)Ie (d) chlorous acid

HC~O,;!

BALANCING EQUATIONS HINTSSYNTHESIS & DECOMPOSITION

Chemists write balanced equations to illustrate what is happening during a chemical reaction. Bonds arebroken, atoms are rearranged, and new bonds are formed. Every chemical reaction supports the Law ofconservation of Matter. This means that in every reaction, the number of atoms of each type of elementcontained within the reactants must be the same as the number of atoms of each type of element containedwithin the products.

Balancing equations is a process which assures that equations are written properly to support the Law ofConservation of Matter; however, balancing cannot be done until each reactant and product formula iswritten correctly. It is important to properly write the seven elements that are diatomic in their elementalform and also use subscripts and parentheses appropriately when considering the oxidation number ofions. All compounds must be made neutral before beginning to balance the atoms.

Balancing is accomplished by adding coefficients that multiply the number of atoms represented by theformula. For example, a coefficient of2 in front of oxygen (e.g., 2 02) means that 4 oxygen atoms arerepresented. Unlike algebra, in chemistry a coefficient does not need to be outside parentheses orbrackets to b distributed. A coefficient applies to the complete substance; however, it no longer applieswhen a plus sign (+) or arrow (--+) is encountered. For example:

3 (NH4)2C03 shows 6 nitrogen, 24 hydrogen, 3 carbon, and 9 oxygen atoms.

3 MgCb + NaBr indicates 3 magnesium, 6 chlorine, 1 sodium, and 1 bromine atom.

PREREQUISITE KNOWLEDGE

Before you do anything, you must know and understand the following areas of nomenclature and formulawriting:

I. Ionic compounds

2. Covalent compounds

3. Acids and bases

4. Complex ions (coordination chemistry)

5. Organic nomenclature


TIPS FOR BALANCING EQUATIONS

I. Ensure each molecular formula is written correctly and each compound is neutral.

2. Mentally count or tally how many of each type of atom is present on each side of the equation.

3. Begin by balancing elements that are only found in one substance on each side.

4. Balance oxygen and hydrogen LAST - they usually balance out at the end or perhaps only the numberof water molecules needs to be adjusted.

5. If there is an odd number of an element on one side and an even number on the other, the odd numberwill need to be evened out - so use a coefficient of 2 for that substance.

6. Ifthere are polyatomic ions that remain together as a unit during the reaction, count the polyatomic ionas a unit.

7. When tallying, be sure to adjust the count for each and every element that an added coefficient affects.

8. Combustion reactions that don't seem to balance will often come out better if a coefficient of 2 is usedfor the hydrocarbon.

SYNTHESIS REACTIONS

Synthesis reactions occur when two or more reactants combine to form a single product. There areseveral types of synthesis reactions.

I . A metal combines with a nonmetal to form a binary salt.

Example: A piece of lithium metal is dropped into a container of nitrogen gas.

2. Metallic oxides and water form bases (metallic hydroxides)

Example: Solid magnesium oxide is added to water.

MgO + 2 HOH -+ Mg(OH)2

3. Nonmetallic oxides and water form acids. The nonmetal retains its oxidation number.

Example: Dinitrogen pentoxide is bubbled into water.

4. Metallic oxides and nonmetallic oxides form salts.

Example: solid calcium oxide is added to sulfur trioxide.

CaO + S03 ~ CaS04

OVER

DECOMPOSITION REACTIONS

Decomposition reactions occur when a single reactant is broken down into two or more products. Ie>

1. Metallic carbonates decompose into metallic oxides and carbon dioxide.

Example: A sample of magnesium carbonate is heated.

2. Metallic chlorates decompose into metallic chlorides and oxygen.

Example: A sample of magnesium chlorate is heated.

3. Ammonium carbonate decomposes into ammonia, water and carbon dioxide.

Example: A sample of ammonium carbonate is heated.

4. Sulfurous acid decomposes into sulfur dioxide and water.

Example: A sample of sulfurous acid is heated.

5. Carbonic acid decomposes into carbon dioxide and water.

Example: A sample of carbonic acid is heated.

6. A binary compound may break down into two elements.

Example: Molten sodium chloride is electrolyzed.

2 NaCI -+ 2 Na + Ch

7. Hydrogen peroxide decomposes into water and oxygen.

8. Ammonium hydroxide decomposes into ammonia and water.

"


NOMENCLA TURE PRACTICE

I. Name each of the following compounds.

(a) CaF2

CALt lIJ M F LUOe.1 Dt=

(h) PFs,:)H O:Sr l-\0LU.s Pt:NTt\ FU) ce. I DE

(i) (NH4hS03

1~i\,nION'viH Si..'LFlll:

(c) NaH

:30 b I Vi'Vl WI Dfll j) l:

U) AU2(C204)3

GeLD (m)

(d) HIO (aq)

H'IpcIO DoLlS I~LI.t)

(k) KSCN

{JOTAS S \v r11 '/l-11 OC'f A A.1 A n=

(e) Hg2Ch

n18Z.. C 1'Q.'( (I) C H L02. IO<i-(I) Pb(C2H302)4

LE'AD (IV) ACETATE

(t) Ba02

rM)'fLl U WI i=t-e.o Y... I .D~(m) LiH

U T\-l h..H1I\ H '11)/2.. \ DE

(g) Mn(HC03)3

rY\ i\NGArJESE ( ill.." H'I DI(OGe-J

(n) H2Cr04 (aq)

CAf2&iJ.RTE

2. Write formulas for the following substances.

(a) vanadium (V) oxide

'Vd. O.s(g) tin (IV) chromate

Sn~ (Cr OLl)'f(b) zinc hydroxide

l'1,(oH)J

(h) nitrous acid

/f,JO(J

(c) silver chromate

Aj ,:J c-o;(d) tungsten (V) thiosulfate

~J~(S.;l 03)S

(i) magnesium hydrogen phosphate

Il1!J /-I1tJ C;

U) calcium carbide

~()(e) cerium (III) nitrate

C e (A103)-3(k) mercury (II) acetate

J/j (C,; 1-/3 Q;J) J

(t) hydroiodic acid(-1-1

(I) perbromic acid

!--I erO 'I

OVER

BALANCING SYNTHESIS AND DECOMPOSITION EQUATIONS

Predict and balance the following synthesis and decomposition reactions. Use abbreviations to indicatethe phase of reactants and products where possible [(aq) (s) (I) (g)]

I. A sample of calcium carbonate is heated.

2. Sulfur dioxide gas is bubbled through water.

3. Solid potassium oxide is added to a container ofcarbon dioxide gas.

4. Liquid hydrogen peroxide is warmed.

5. Solid lithium oxide is added to water.

" "\L ., D (5) /ti 0 to -'7

6. Molten aluminum chloride is electrolyzed.

----- -------------


7. A pea-sized piece of sodium is added to a container of iodine vapor .

.;J J4.(s)+- I,J- Cj) -7 ,J Aft:-...-l. (5)

8. A sample of carbonic acid is heated.

9. A sample of potassium chlorate is heated.

') L.Ji) AQ d. k'tf (5) -I- .J 002 ~J)..v 1\ L..,( .3 (S) -~ ..

10. Solid magnesium oxide is added to sulfur trioxide gas.

OVER

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Re-typed from The Ultimate Chemical Equations Handbook by ...

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