revised naming and chemical formula writing

7/30/2019 Revised Naming and Chemical Formula Writing

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Naming andChemical Formula

Writing


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facts about thePERIODIC TABLE

It was arranged by

Mendeleev according to

their atomic number

The vertical columns arecalled Groups or Families.

The horizontal columns are

called Periods

The elements are divided

into three categories --metals, nonmetals and

metalloids


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Elements

substances that cannot be decomposed by

simple chemical change into two or more

different substances.
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Compounds

substances of definite composition that can

be decomposed by simple chemical

change into two or more differentsubstances.
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Mixtures

materials that contain two or more different

substances more or less jumbled together
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Elements

Elements can occur in nature as:

a. Monatomic form

All metals and noble gasesexist in their simplest form or

as atoms.b. Diatomic molecule

H2, O2, N2, F2, Cl2, Br2, and I2

c. Polyatomic molecule

Elements containing morethan two atoms

phosphorus (P4) and sulfur(S8)

the only elements that existin liquid state are mercury(Hg) and bromine (Br2).

elements that exist ingaseous state are H2, O2, N2,F2, Cl2, and noble gases.

All other elements that existin solid state including

phosphorus (P4) and sulfur(S8) and I2


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Ions

charged species formed from a neutral

atom or molecule when electrons are

gained or lost as the result of a chemicalchange

Cation

Na+Anion

Cl-


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Cation

Metals tend to form cations by losing

electrons

Na Na+ + e-

0 +1 -1


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Anion

Nonmetals tend to gain electrons to form

anions

Cl + e- Cl-0 -1 -1

Cl2 + 2e- 2 Cl-0 -2 -2


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Oxidation number/Oxidation states

number of charges the atom would have in a

molecule (or in an ionic compound)

Group 1A +1 Group 5A -3



Group 4A -4 Group 8A 0

Charges does not apply to metalloids


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.for Transition Metal

Sc Ti V Cr Mn Fe Co Ni Cu

+7

+6 +6 +6+5 +5 +5 +5

+4 +4 +4 +4 +4 +4

+3 +3 +3 +3 +3 +3 +3 +3 +3

+2 +2 +2 +2 +2 +2 +2 +2

+1


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In formula writing..

The subscript of the cation is numerically

equal to the charge on the anion, and the

subscript of the anion is numerically equal

to the charge on the cation

Al2O3

Al 3+ O 2-

Note:Cation are written first then the anion


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Formula writing

How do we compute the sum of the charges?

Al2O3

2(+3) + 3(-2) = 0

Subscriptof Cation

Charge of

Cation

Subscript

of Anion

Charge of

Anion


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Compounds

formed when atoms of 2 or more different

elements chemically combine in ratios of

whole numbers

Types: Binary Compounds

Ternary Compounds


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Naming Compounds

Element Name of Cation

Na Sodium Na+ Sodium ion

K Potassium K+ Potassium

ion

Mg Magnesium Mg2+ Magnesiumion

Al aluminum Al3+ Aluminum

ion

Ionic compounds


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Naming Compounds

Ionic compounds (Anion)

Group 4A Group 5A Group 6A Group 7A

C Carbide (C4-) N Nitride (N3-) O Oxide (O2-) F Fluoride (F-)

Si Silicide(Si4-) P Phosphide

(P3-)

S Sulfide (S2-) Cl Chloride (Cl-

)

Se Selenide

(Se2-)

Br Bromide

(Br-)Te Telluride

(Te2-)

I Iodide (I-)

The suffix -ide is added to the root word of the anion


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Binary Compounds

Contains two (2) elements only

Types:

Metal (cation) + Nonmetal (anion)

a. Cations with fixed oxidation state + Anion derived

from nonmetals

b. Cations with Variable oxidation state + Anion derivedfrom nonmetals

Hydrogen (cation) + Nonmetal (anion)

Nonmetal + Nonmetal


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Cations with fixed oxidation state + Anion derived

from nonmetals

Fixed oxidation states refers to theelements belonging to group A

NaCl Sodium Chloride


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Binary Compounds

BaCl2

Al2O3

AgBr NaF

CaCl2

Cations with fixed oxidation state + Anion

derived from nonmetals

Example:


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Cations with Variable oxidation state + Anion


Variable oxidation states refers to theelements belonging to group B

Copper Cu+ Cu2+

Cuprous Cupric

Copper (I) Copper (II)


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Binary Compounds

Cations with Variable oxidation state + Anion


CuCl2

CuCl Copper (I) Chloride

Copper (II) ChlorideExample:

FeBr2

FeBr3 Manganese (III) oxide


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Hydrogen (cation) + Nonmetal (anion)

Formula Name (pure subs) Name (aqueous soln)

HX Hydrogen + ____ -ide Hydro + ___ic acid

HF Hydrogen fluoride Hydrofluoric acid

HCl Hydrogen chloride Hydrochloric acid

HBr Hydrogen bromide Hydrobromic acid

HI Hydrogen iodide Hydroiodic acid

H2SHydrogen sulfide Hydrosulfuric acid


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Nonmetal + Nonmetal

Prefix Meaning Prefix Meaning

Mono- 1 Hexa- 6

Di- 2 Hepta- 7

Tri- 3 Octa- 8

Tetra- 4 Nona- 9

Penta- 5 Deca- 10

Format: (Prefix + first element) + (Prefix + root of second

element +ide)


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Nonmetal + Nonmetal

Format: (Prefix + first element) + (Prefix + root of

second element +ide)

Exceptions:

1. When the subscript of the first element is one (1)

then the prefix monois omitted.

2. If the second element is oxygen and the last letterof the prefix is a letteraor a lettero, these letters

are omitted.


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.example

N2O4

___nitrogen _____oxidedi tetr

Example:

CCl4 CBr4 Phosphorus pentachloride


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Exercises

Write the chemical

symbols of the ff :

ocalcium nitrideo phosphorus pentachloride

o lithium sulfide

o cesium iodide

o barium phosphide


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Ternary Compounds

A. Metal (cation) + Polyatomic ion (anion)

Polyatomic ion (cation) + Monoatomic Anion

Polyatomic ion (cation) + Polyatomic Anion

NaNO3

NH4Br

NH4NO3

Sodium Nitrate

Ammonium bromide

Ammonium nitrate

Contains 3 elements only.


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Must know..Ammonium NH4

+

Carbonate CO32-

Chlorate ClO3-

Hydrogen carbonate HCO3-

Hydrogen sulfate HSO4-

Hydroxide OH-

Nitrate NO3-

Phosphate PO43-

Sulfate SO42-

Sulfite SO32-


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Thiocyanate SCN-

Permanganate MnO4-

Hydrogen Phosphate HPO4-

Dihydrogen Phosphate H2PO4-

Chromate CrO4

2-

Dichromate Cr2O72-

Cyanide CN-

Diborane B2H6

Silane SiH4

Phosphine PH3


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Some Acids

Nitric Acid HNO3Sulfuric Acid H2SO4

Hydrochloric Acid HCl

Carbonic Acid H2CO3

Chloric Acid HClO3

Phosphoric Acid H3PO4

Phosphorous Acid H3PO3

Sulfurous Acid H2SO3

Nitrous Acid HNO2


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B. H + oxyanions (oxyacids)

Formula of

Oxoacids

Naming of

Oxoacids

Formula of

Oxoanion

Name of

Oxoanion

HClO4 Perchloric

acid

ClO4- Perchlorate

HClO3 Chloric acid ClO3- Chlorate

HClO2 Chlorous acid ClO2- Chlorite

HClO Hypochlorous

acid

ClO- Hypochlorite

HNO3 Nitric acid NO3- Nitrate

HNO2 Nitrous acid NO2- Nitrite

Only halogens Cl, Br, I have four names


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Balancing Chemical Equations

Chemical Equation summarizes the

molecular changes involved in a

chemical reaction

A + B C + D

Reactants

ProductsSTARTINGMATERIAL

Formed substances


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Examples:

a) Evaporation of water

H2O(l) H2O(g)

b) Combustion of carbon to form carbon

dioxideC(s) + O2 (g) CO2 (g)


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Steps in writing Chemical Equation:Step 1: write the formulas of the reactants

Step 2: write the formulas of the products by

writing the oxidation numbers of the two

combined elements and applying the criss-cross

Step 3: it is very important to balance the

equation. (the number of atoms of each

element in the reactant side should be equal

to the number of atoms of the said element in

the product side.


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Balance the following chemical

equations:

a) N2 + O2

NO2b) P + Cl2 PCl3

c) Zn + AgCl ZnCl2 + Ag

d) Cl2 + NaI NaCl + I2e) CO + O2 CO2


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Types of Chemical Reactions:

1. Combination/Synthesis

2. Decomposition

3. Single Displacement4. Double Decomposition

Chemical Reactiona process in which a

substance is changed into one or more new

substances


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Combination/Synthesis

A single substance is formed by union of

two substances

A. Rule: A + B ABSodium + Iodine

Step 1: Na + I2

Step 2: Na+1 I-1

Step 3: 2Na + I22NaI


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A. Rule: A + B AB

Combustionprocess of burning; requires oxygen

a. Metal + oxygen metallic oxide

b. nonmetal + oxygen non-metallic oxide

2Ba + O2 2BaO

2S + 3O2 2SO3


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B. Rule: A + O2 C + D

Complete combustion

CH4 + 2O2 CO2 + 2H2O

Incomplete combustion

2CH4 + 3O2 2CO+ 4H2O


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C. Rule: Metall ic oxide + H2O Base

MgO + H2O Mg(OH)2

D. Rule: Non-metal l ic oxide + H2O Acid

SO2 + H2O H2SO3

E. Rule: Active Metal + H2O Base + H

2

2Na + 2H2O 2NaOH + H2


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Decomposition

A reaction that involves using of heat or

electric current. It is the opposite reaction of

synthesis

also known as Metathesis

General Rule:AB A + B


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Single Displacement

The possibility of the positive part of a

compound may interact with the negative

part of the second compound

Also known as Single Substitution, Single

replacement

AB + C CB + A

Where A and C are metals and C is more active thanA. if not there is no reaction

CaCl2 + 2Na 2NaCl + Ca


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Metal Metal

K Sn

Na Pb

Ca H

Mg Cu

Al Bi

Mn Sb

Zn Hg

Cr Ag

Fe Pt

Ni Au

dec

dec

Activity Series


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Single Displacement

Rule: AB + C AC + B

BaCl2 + F2 BaF2 + Cl2

Where B and C are non-metals and C is more activethan B. if not there is no reaction


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Single Displacement

Non-metals

F

O

Cl

Br

I

S

dec


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Double decomposition

Also known as Double Displacement,

Double Substitution

General Rule: AB + CD AD + CB

HCl + NaOH NaCl + H2O

Strong

Acid

Strong

Base


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Double Decomposition

Also known as Double Displacement, Double

Substitution

General Rule: AB + CD AD + CB

Neutralization reaction between an acid anda base that produces a salt and water

HCl + NaOH NaCl + H2OStrongAcid Strong

Base

revised naming and chemical formula writing

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