The document discusses the language and terminology used in chemistry, including: - Atoms, elements, compounds, and molecules and their representations using symbols and formulas. - Ionic and covalent bonds between atoms and the structures they form. - The periodic table and how it organizes elements and predicts their properties. - Types of chemical reactions like synthesis, decomposition, and acid-base. - Naming conventions for binary ionic compounds, acids, and other substances.

1. The Language Of
Chemistry
• Falasifah Aulia
1 • 4301410044
• Ulfa Pandu Dewanti
2 • 4301410030
• Selvia Anggraeni
3 • 4301410029

2. Aristotle and Plato  The matter could
be infinitely divided.
Democritus  all matter was
composed of small, finite particles that
called atomos.
Dalton’s Theory :

3. Matter is composed of exceedingly small
Matter is composed of exceedingly small
particles called atom.
particles called atom.
An Element consists of only one type of
An Element consists of only one type of
atome.
atome.
Atoms of one element differ in properties
Atoms of one element differ in properties
from atoms of all other elements.
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.

4. Proton
(+1) Nukleus
(1.007 (d = 10-13
3 amu cm)
)
The
composit Electron
ion of (-1)
(0.00055
Atoms amu)
Neutron
(0)
(1.0087 Atom
amu) ( d = 10-8 cm)

5. Element Symbol Elements Symbol
Aluminium Al Hydrogen H2
Bromine Br Oxygen O2
Calcium Ca
Nitrogen N2
Carbon C
Fluorine F2
Chlorine Cl
Chlorine Cl2
Cobalt Co
Bromine Br2
Copper Cu ( from
Cuprum) Iodine I2

6.  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 ).

7.  The structure Formula, shows how the
atoms are connected in the molecule.
 Example :
C2H4O2
H
O
H C C
O H
H

8. Explanations :
A = the Atom
X = the mass Number
Z = 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 1224Mg, 1225Mg, 1226Mg.

10.  Advantages of Periodic Table
1. 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 >>

11. X
one electron transferred
X
X
+
-
X X
XX
XX
X X
X X
XX
sodium atom chlorine atom
11Na+2, 8, 1 17Cl 2, 8, 7

12.  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.

13. Non Ionic
metal
metal compoud
Covalent
nonmetal nonmetal
compound
• Groups of metal : group IA – IVA
• Groups of non metal : group VA – VIIIA

14.  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

15.  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.

16.  In equations there are information about
the condition of the substance like :
1. (s) solid
2. (l) liquid
3. (g) gass
4. (aq) substance that is dissolve in water

17.  Above or below the arrow there is
information about condition of the
reaction, such as :
1. Elect. Is for electrolysis
2. ∆ is for that reaction carried out by
heating.
∆
CaCO3 (s) CaO (s) + CO2 (g)

18. 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

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

20. 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)

21. 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)

22. Binary Ionic
1. A fixed Compound 2. A variable
containing a
Charge metal ion and charge
nonmetal
3. Binary covalent compouds 4. Binary acids and ternary
containing two nonmetals oxyacids

23.  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 Cloride
KBr  Potassium Bromide

24.  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 chloride
FeCl3  iron (III) chloride or ferric chloride

25.  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

26. If 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

27. Fala
Ulfa
Selvi