science

1. ATOMS
IONS MOLECHULES

2. ATOMS
lost/get
electrons
may form
IONS
CATION
ANION
composed
by
Atomic
core
Electrons
Protons
Neutrons
MOLECHULES
merged to form
ELEMENT
MOLECHULES
COMPOUND
MOLECHULES

3. WHAT IS ATOM?
Atom is the smallest part of an
element which still has the initial
properties of the element.

4. ATOMIC
STRUCTURE BY
RUTHERFORD
Components of atom:
Neutrons (neutral)
Protons (positive charged)
Electrons (negative charged)

5. X
A
Z
X = ELEMENT SYMBOL
A = ATOMIC MASS
Z = ATOMIC NUMBER = THE AMOUNT OF PROTONS = THE
ELEMENT OF ELECTRONS
A-Z = THE AMOUNT OF NEUTRONS
EXAMPLE
O
16
8
Atomic mass = 16
Atomic number = 8
Protons = 8
Electrons = 8
Neutrons = 16 -8 = 8
ATOMIC STRUCTURE
Ar
40
18

6. Isotops, Isobars, Isotones, Isomers
Isotopes
Atoms having the same
number of protons (Z) but
different number of neutrons
(N)
Isobars
Atoms having the same mass
number (A)
Isotones
Atoms having the same
number of neutrons (N) but a
different number of protons
(Z)
Isomers
Atoms of the same element
(same Z and N) but which are
in different excited states

7. CONFIGURATION OF
ELECTRONS
Skin Skin Number
(n)
Maximum Amount of
Electrons
K 1 2
L 2 8
M 3 18
N 4 36
According to Bohr, electrons circle the atomic core
on several lines in certain levels of energy. Those
lines are then called atomic skins. + K L M N
1 2 3 4
Example :
Na
23
11
Electrons = 11
Configuration of N:
2)8)1)

11. CONFIGURATION OF
ELECTRONS
Ato
m
Electron’s
Amount
Electron’s
Configuration
Group Period
H 1 1 1 1
N 7 2 5 5 2
Cl 17 2 8 7 7 3
Ga 31 2 8 18 3 3 4
Example :
The number at the outer layer also shows
the group of atom.
The amount of layers show the period of
atom.

12. WHAI IS IONS?
Ions is atoms which have positive
charged (cations) or negative
charges (anions)
CATIONS
Na+ Ca2+
ANIONS
I- O2-

13. How the form positive and negative ions?
Formation of positive ions
By releases the electron
11 e-
11 p+
12 n0
Atomic Sodium (Na)
10 e-
11 p+
12 n0
Ionic Sodium (Na+)
1e-
Formation of negative ions
By catches the electron
17 e-
17 p+
18 n0
Atomic Chlorine (Cl)
18e-
17p+
18 n0
Ionic Chlorine (Cl-)
1e-
The purpose of releasing or catching charged is to reach the stability

14. Ionic Compound
Positive and negative ions are tied up to form a neutral
compound.
Na+ + Cl-  NaCl
H+ + O2-  H2O
The charged should exchange at the result.

15. WHAI IS MOLECHULES?
Molechules is the chemical
combination of two atoms or
more.
Element
Molechules
Compound
Molechules

16. Element
Molechules
Compound
Molechules
Molechule from the atoms of same
element chemically merged.
Diatomic
molechules
Poliatomic
molechules
O O
O2
N N
N2
O O
O3
O
P P
P P
P4
Molechule which are composed by more
than one type of atomic shaper.
H
Cl
HCl
H H
O
H2O

17. Element
Molechules
How element molechules are formed?
The formation of O2
1) Oxygen molechules are composed by
two atomic oxygen.
2) The configuration of atomic oxygen is
2,6.
3) To achive the electrons configuration 2 8,
atomic oxygen uses 4 electrons in the
same time so that it can make two
covalent bonds. The bonds formed can
be written down as O = O
What is covalent?
1) If electrons are used in the same time,
they can form a bond which is called
covalent bond.
2) Covalent bond is not as strong as ionic
bond.
3) If there is one pair of atoms which are
used in the same time, then it is called
single covalent bond.
4) If there is two pairs of atoms which are
used in the same time, then it is called
double covalent bond.
5) Covalent compound is not an electric
transmitter because it can’t produce ions
which have electric charged.

21. ISOTON, ISOTOP, ISOBAR,
ISOELECTRON
ISOTON : TWO ATOMS WITH SAME NEUTRON NUMBERS
ISOTOP : TWO ATOMS WITH SAME PROTON NUMBERS
ISOBAR : TWO ATOMS WITH SAME ATOMIC MASS