The Language Of Chemistry

1

• Falasifah Aulia• 4301410044

2

• Ulfa Pandu Dewanti• 4301410030

3

• Selvia Anggraeni• 4301410029

Members :

2.1 Dalton’s Atomic Theory

Aristotle and Plato The matter could be infinitely divided.

Democritus all matter was composed of small, finite

particles that called atomos.

Dalton’s Theory :

Dalton’s Theory

Matter is composed of exceedingly small particles called atom.

An Element consists of only one type of atome.

Atoms of one element differ in properties from atoms of all other

elements.

Matter is composed of exceedingly small particles called atom.

An Element consists of only one type of atome.

Atoms of one element differ in properties from atoms of all other elements.

A compound consists of a combination of atoms of two or more elements.

Atoms are neither created nor destroyed during a chemical change.

2.2 The composition of Atoms Proton

(+1)(1.0073 amu

)

Electron (-1)

(0.00055 amu)

Neutron (0)

(1.0087 amu)

The composition of Atoms

Nukleus (d = 10-13

cm)

Atom ( d = 10-8

cm)

2.3 Symbols And Formulas

Element Symbol

Aluminium Al

Bromine Br

Calcium Ca

Carbon C

Chlorine Cl

Cobalt Co

Copper Cu ( from Cuprum)

Elements Symbol

Hydrogen H2

Oxygen O2

Nitrogen N2

Fluorine F2

Chlorine Cl2

Bromine Br2

Iodine I2

A molecular formula is a symbolic representation of a molecule that uses chemical symbols to indicate the types of atoms and uses subscripts to show the numbers of atoms of each type in the molecule.Ex : CH4 ( represent a molecule that contains one carbon atom and four hydrogen atoms ).

Empirical Formula is indicated as the types of atoms present and the simplest whole-number ratio of atoms in the compound ( just for ionic compound ).

The structure Formula, shows how the atoms are connected in the molecule.

Example :C2H4O2

H

O

H C C

O H

H

2.4 IsotopesExplanations :A = the AtomX = the mass

NumberZ = the atomic

number = proton = electrone

Isotopes is atoms of a particular element that differ only in the number of neutrons in the nucleus

For the example is isotopes from Magnesium, there isotopes are 12

24Mg, 1225Mg, 12

26Mg.

AX

Z

2.5 The Periodic Table

Advantages of Periodic Table1. Electron configuration from metal elements can

be found.2. Characteristic all of the element can be known

easily.

Radius >> radius <<

Electron Afinity << Electron Afinity >>Acid << Acid >>Base << Base >>ionisation Energi << Ionisation Energi >>

sodium atom

X

XXX

X

X

X

X

X

XX

2.6 Formation of ions

chlorine atom

11Na 2, 8, 1 17Cl 2, 8, 7

X

+

sodium

11Na+

X

X

X -

one electron transferred

2.7 Ionic and Covalent Compoud

Ionic bonds are electrostatic forces of attraction between ions of opposite charge.

covalent bonds are The attractive force that result from the sharing of electrons among atoms.

metal Non metal

Ionic compoud

nonmetal nonmetal Covalent compound

• Groups of metal : group IA – IVA• Groups of non metal : group VA – VIIIA

2.8 Chemical Equations Is a shorthand type of expression when

the atoms, molecules, or ions in one set of substances regroup to form other substances.

Example : CH4 + 2O2 CO2 + 2H2O

Balancing Equations

Balanced chemical equation is indicate that the coefficient of the substance is same with mole its substance.

We must balancing the number of atoms in the reaction and also the charge of substance.

Other Information in Equations

In equations there are information about the condition of the substance like :

1. (s) solid2. (l) liquid3. (g) gass4. (aq) substance that is dissolve in

water

Above or below the arrow there is information about condition of the reaction, such as :

1. Elect. Is for electrolysis2. ∆ is for that reaction carried out by

heating. ∆

CaCO3 (s) CaO (s) + CO2 (g)

2.9 Equations for Ionic Reaction

For an ionic equation, the sum of total charges on each side, as well as the number of kind of atom on each side, must balance.

Example :

NaCl (aq) + AgNO3(aq) NaNO3(aq) + AgCl(s)

The ionic equation is

Na+(aq) + Cl-(aq) + Ag+

(aq) + NO3-(aq) Na+

(aq) + NO3-(aq) + AgCl(s)

solution of NaCl Solution of AgNO3 solution of NaNO3 Solid AgCl

2.10 Classification of Chemical Reactions

1. Addition Reactions or combination reaction occures when two or more substances combine to form another substance.Example :S(s) + O2(g) 2 Mg

2. Decomposition Reactions occurs when one compound breaks down (decomposes) into two or more substances.Example : 2 HgO (s) 2Hg(l) + O2(g)

3. Metathesis Reactions or double displacement reaction, is a rection in which two compound exchange parts – usually ions.example :CaCl2 (aq) + 2AgNO3(aq) 2AgCl(s) + Ca(NO3)2(aq)

4. Combution Reactions is a reaction of element or a cmpound with oxygen that produck heat and, often, light.example :C6H12O6(s) + 6O2(g) 6CO2(g) + 6H2O(l)

5. Neutralization Reactions is a reaction between a solution of an acid and a solution of a base ; it produses a salt and water.HCl (g) + KOH(aq) KCl (aq) + H2O(l)

2.11 Naming Inorganic Compound ( Nomenclature )

3. Binary covalent compouds containing two

nonmetals

4. Binary acids and ternary oxyacids

Binary Ionic Compound

containing a metal ion and

nonmetal

1. A fixed Charge

2. A variable charge

1. A fixed Charge Consist of metals ( IA, IIA, IIIA )

combine with a nonmetal ( VIA, VIIA). Rule :

The name of cations followed by the name of the anion ( it.s ending by the suffix – ide )

Ex :NaCl sodium ClorideKBr Potassium Bromide

2. Variable Charge Consist of metal ( IIIB – VA) and

nonmetal . Rules :

1. the name of the cation ( metal ) followed by charge than the name of the anion ( ending by - ide)2. we may use ending –ic for the higher charge of metal and – ous for lower charge.

Ex :FeCl2 iron (II) chloride or ferrous chlorideFeCl3 iron (III) chloride or ferric chloride

3. Nomenclature containing two nonmetals

Consist of the name of the less nonmetallic element followed by the name of the more nonmetallic element.

Rule : 1. As in the foregoing two categories, the second

name nonmetal is given the suffix – ide.2. The number of atoms of each nonmetal in the

formula is given prefix – mono, di, tri, etc ( sometimes mono is omitted )

Ex :N2O4 dinitrogen tetroxide

Acids and Ternary OxyacidsIf the condition is gas (g) the name is

hidrogen followed by the second atom with the –ide suffix.

If the condition is aqueous (aq) we use preffix hydro- and the suffix –ic and ending with acid.

Ex :HF (g) hydrogen fluoride

HF (aq) hydrofluoric acid

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