ASIMILASI 1.pdf
Transcript of ASIMILASI 1.pdf
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WHAT IS MATTER ?
Anything that has mass, volume or occupy
space
Matter consist of atoms, molecules or ions
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ATOM
Tiny particles of an element that cannot be
created or destroyed
Example :
Copper metal consist of copper atoms, Cu
WHAT IS ATOM,
MOLECULE AND ION ?
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Example :
Aluminium metal consist of aluminium atom, Al
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MOLECULE
Two or more atoms that are chemically
bound together
Example :
One chlorine molecule, Cl2consist of two Cl atoms
Cl Cl
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Example :
One carbon dioxide molecule, CO2 consist of onecarbon atom and two oxygen atoms
CO O
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ION
A charged particle (cation or anion) that
forms from an atom when it loses or gains
one or more electrons
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HOW THE CATION FORM?
Example :
A neutral lithium, Li atom contains 3 electrons.
When it loses one electron, it forms Li+ion.
Li Li+
+ e
Li Li+
Electron configuration : 2.1 Electron configuration : 2
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Example :
A neutral fluorine, F atom contains 9 electrons.
However, in chemical reactions a fluorine atom
gains one electron to form fluoride, F- ion.
F + e F-
HOW THE ANION FORM?
F F
F with 9 electrons Fwith 10 electronsElectron configuration : 2.7 Electron configuration : 2.8
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Classification of Matter According to Its Composition:
Elements, Compounds and Mixtures
MATTER
PURE SUBSTANCES MIXTURES
ELEMENTS COMPOUNDS HOMOGENEOUS
HETEROGENOUS
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MATTER
Anything that has mass, volume and occupy
space
Example :
Air
WaterChair
Almonds
Salt
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ELEMENT
Substance that consist of only one kind of
atom.
The element can be atom or molecule
Example : Na, C(graphite), O2, O3, Cl2
Elements cannot be decomposed into simpler
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COMPOUND
A substance that is composed of two or
more elements that are chemically
combined in fixed proportions.
Example : water, H2O
sodium chloride, NaCl
butane,C4H10
They contain two or more kinds of atoms
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MIXTURE
Combination of two or more substances in
which the substances retain their distinct
identities.
Two types of mixtures:
Homogeneous
Heterogeneous
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Homogeneous Mixture
Composition of the mixture is the same throughout.
Example :
A spoonful of sugar dissolves in water
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Milk
Tea
Blood
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Heterogeneous Mixture
Composition of the mixture is not uniform.
Example :
Iron filings and sand
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Mixture of oil,
water and sand
Mixture of oil and water
Mixture of fruits
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EXERCISE 1
Classify each substance as an element or acompound.
a) Aluminium, Al
b) Sulphur, S8c) Chlorine, Cl2d) Methanol, CH3OH
e) Carbon, C
f) Baking soda, NaHCO3g) Nickel, Ni
h) Gold, Au
i) Carbon monoxide, CO
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Elements & The Periodic Table
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What are the information
that can be derived fromthe isotope notation ?
Proton number (Z)
Nucleon number (A)
Number of electrons
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* X is the symbol of the element
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1
2
3
45
6
7
All known elements are listed in the periodic table
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In periodic table, elementsare arranged in
order of increasingproton number (Z).
Each element is represented by a unique
chemical symbol.
Example :
Helium He
Aluminium Al
Silver Ag
Tin Sn
Copper Cu Uranium U
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There are seven horizontal rows of elements
called per iods.
The vertical columns of elements are
called groups.
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The periods are numbered 1 through 7 on
the left-hand side of the table.
PERIODS
In each period (horizontal row), the atomic
number increases from left to right.
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GROUPS
The group in the Periodic Table are
numbered from 1 to 18.
Elements in the same group have the
same number of valence electron.
Number of valence electrons indicate the
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Groups of elements in the periodic table
The elements are arranged in the same group according
to their chemical behavior and number of valenceelectrons.
Group 1: Alkali metals
Group 2 : Alkali earth metals
Group 13
Group 14
Group 15
Group 16 : Chalcogen
Group 17 : Halogens
Group 18 : Noble gases
Group 3 4 : Transition elements
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1 2 18
17
Elements
in the
same
group have
similar
properties
2
3
4
5
6
7
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Metalloids :
(elements that have properties between those metals
and nonmetals)
Boron (B), Silicon (Si), Arsenic (As) and etc
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Determining the Group & Period
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Example :
Na, sodiumProton number, Z = 11
Electron configuration = 2.8.1
Valence electron = 1
Group = 1Period = 3
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Mg, magnesium
Proton number, Z = 12
Electron configuration = 2.8.2Valence electron = 2
Group = 2
Period = 3
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F, fluorine
Proton number, Z = 9
Electron configuration = 2.7Valence electron = 7
Group = 17
Period = 2
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EXERCISE 2
Which group and period do these elements
belong to?
a) Nitrogen, N (Z = 7)b) Potassium, K (Z=19)
c) Lithium, Li (Z = 3)
d) Boron, B (Z = 5)
e) Calcium, Ca (Z = 20)
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METALS NON METALS
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METALS, NON-METALS,
METALLOIDS
Metalsare located on the leftsideand in
the middleof the periodic table.
Nonmetalsare located on the upper right
quarterof the table
Metalloidsare elements that lie along the line
that separates metal from nonmetal.
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EXERCISE 3
Classify each elements as metal, nonmetal ormetalloid.
a) Barium, Ba
b) Iodine, Ic) Oxygen, O
d) Sulphur, S
e) Chorine, Cl
f) Iron, Fe
g) Chromium, Cr
h) Silicon, Si
i) Boron, B
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Ions & The Periodic Table
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Group 1, 2, 13 to 17tends to form ionsthat
have the same number of valence electrons as
the nearest noble gas
Group 1elements (alkali metals) tend to
lose 1 electron and form 1+ ions.
Group 2elements (alkali earth metals) tend
to lose 2 electronsand form 2+ ions.
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Example :
Lithium, Li loses one valence electron toattain the same number of valence
electrons as Helium, He
Li Li+ + e
Magnesium, Mg loses its two valence
electrons to attain the same number of
valence electrons as Neon, Ne
Mg Mg2+ + 2e
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Group 17(the halogens) tend to gain 1 electron
and form 1ions.
Group 15tend to gain 3 electronsand form3ions.
Group 16tend to gain 2 electronsand form
2ions.
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Example :
When fluorine, F ionizes, it accepts one
additional electron for a total of 8 valenceelectrons the same number of electrons
as Neon, Ne.
F + e
F-
Oxygen accepts two additional electrons
for a total of 8 valence electrons the samenumber of electrons as Neon, Ne.
O + 2e O2
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EXERCISE 4
Based on their position in the periodic table,
what are the ions these elements tend to
form?
a) Barium, Ba
b) Chlorine, Cl
c) Potassium, Kd) Nitrogen, N
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Type of Elements
&The Type of Bonds Formed
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A MOLECULAR VIEW OF ELEMENTS AND COMPOUNDS
PURE SUBSTANCES
ELEMENTS COMPOUNDS
ATOMIC MOLECULAR MOLECULAR
(COVALENT)
IONIC
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Elements
ATOMIC MOLECULAR
Have single
atom astheir basic
unit
Example :
Copper, Cu Sodium, Na
Helium, He
Does not
exist assingle atom
Example :
Chlorine, Cl2 Bromine, Br2 Oxygen, O2
Phosphorus, P4 Sulphur, S8
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Example :
Bromine exist
as diatomic
molecule
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Molecular Compounds (Covalent)
Compounds that are composed from two ormore nonmetal atoms.
Type of bond formed is covalent bond
Example : H2O, CO2, SO2and etc
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Example :
Water (liquid)
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Ionic Compounds
Compounds that are composed of one or
more cations paired with one or more
anions.
In most cases, the cations are metals and
the anions are nonmetals.
Example : NaCl, LiF, CaCl2and etc.
Type of bond formed between cations and
anions is called ionic bond
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Na
+
Cl-
Example :
Table Salt
(NaCl)
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Ionic Bond, Covalent Bond
and Metallic Bond
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Ionic Bond (Electrovalent Bond)
Chemical bond formed when metal combine
with nonmetal by electron transfer.
Metal atom transfer its valence electrons tononmetal atom and form cation.
Nonmetal atom accept electrons from metal
atom and form anion
The electrostatic force between cation and
anion forms ionic bond.
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Example :
Formation of ionic bond in NaCl
Na+
2.8Cl
2.8.82.8.12.8.7
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Electron transferred fromsodium to chlorine
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Formation of ionic bond in MgO
2.8.2 2.6
Mg2+
2.8
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Covalent Bond
Chemical bond formed when nonmetal atoms
combine.
Electrons are shared between nonmetal atoms
The shared electrons that appear in the space
between the two atoms are counted as the
octets (or duplet) of both atoms
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Example :
Formation of covalent bond in H2molecule
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Example :
Formation of covalent bond in O2molecule
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Metallic Bond
All metal atoms in the sample contributetheir valence e-to form an electron sea
that is delocalizedthroughout the
substance
Electrostatic attraction between the
positively charged metal ions and the
seaof delocalised valence electrons
forms metallic bond.
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Example: Electron sea Model
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Example: Electron-sea Model
Na+ Na+ Na+
Na+ Na+ Na+
Na+ Na+ Na+
e- e-
e-
e- e-
e-
e- e-
e-
Group 1
Mg2+ Mg2+ Mg2+
Mg2+ Mg2+ Mg2+
Mg2+ Mg2+ Mg2+
e- e-
e-
e-
e-
e-
e-
Group 2
e- e-
e-e- e-
e- e-e- e-
e- e-
Sodium, Na Magnesium, Mg
nucleus
Delocalised
Valence
electrons
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Writing The Chemical Formula
&Naming the Ionic and Covalent
Compounds
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Chemical formula
A notation of atomic symbols and numerical
subscripts that shows the type and number
of each atom in a molecule or formula unit
of a substance.
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Compounds Formed from Monatomic Ions
The name of the cation is the same as the name
of the metal.Many metalsname end with i um.
The name of the anion takes the root of thenonmetal and adds the suffix ide
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Common Monatomic Ions
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Common Monatomic Ions
Charge Formula Name
Cations
1+ H+ Hydrogen
Li+ Lithium
Na+ Sodium
K+ Potassium
Cs+ Cesium
Ag+ Silver
2+ Mg2+ Magnesium
Ca2+ Calcium
Ba2+ Barium
Zn2+ Zinc
3+ Al3+ Aluminium
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Charge Formula Name
Anions
1 H Hydride
F Fluoride
Cl Chloride
Br Bromide
I Iodide
2 O2 Oxide
S2 Sulphide
3 N3 Nitride
P3 Phosphide
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Writing Formulas & Naming Ionic Compounds
Ionic compounds always contain positive
and negative ions.
In the chemical formula, the sum of positivecharges (cations) must always cancel
exactly the sum of negative charges
(anions).
(net charge = 0)
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Example :
Write formula for the ionic compound that formsfrom sodium, Na and chlorine, Cl.
Step 1 :
Write the symbol for the metal and its charge
followed by the symbol of the nonmetal and its
charge.
Na+ Cl
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Step 2 :
Equalize the net charge. The overall net charge is
equal to zero.
Na+ Cl
1 1
Cation = 1(1+) = 1+
Anion = 1(1)= 1= 0
Overall net
charge = 0Step 3 :
Write the formula. The formula is NaCl.
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Step 4 :
The name of this compound issodium chloride
Write the name of the ionic compound.
Name of cation :
metal
Base name of anion :
Nonmetal, ending
with ide
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Ionic Compounds Containing a Polyatomic Ion
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Ionic Compounds Containing a Polyatomic Ion
Most polyatomic ions are oxoanions; anions
containing oxygen.
Example : Oxoanions Name
NO3 nitrate
NO2 nitrite
SO42 sulphate
ClO hypochlorite
ClO2 chlorite
ClO3 chlorate
ClO4 perchlorate
CrO42 chromate
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Example :
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Example :
KNO3
NH4NO3
CuSO4
potassium nitrate
ammonium nitrate
Copper(II) sulphate
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EXERCISE 5
Write the formula for the ionic compound that
forms from:
a) Magnesium, Mg and Oxygen, Ob) Aluminium, Al and Oxygen, O
c) Sodium, Na and fluorine, F
d) Calcium, Ca and chlorine, Cl
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EXERCISE 6
Give the name for each of the following
compounds :
a) NaNO3b) CuSO4c) Na2CO3d) K2CrO4e) Fe2(SO4)3
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Naming Molecular Compounds
For binary molecular compounds, their names
have the form :
prefixName of first
elementprefix
Base name of second
element + ide
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The prefixes given to each element indicate the
number of atoms present.
mono 1
d i 2
t r i 3
tetra 4
penta 5
hexa 6
hepta 7
octa 8
nona 9
deca 10
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Example :
CO2 Carbon dioxide
N2O dinitrogen monoxide
CCl4 Carbon tetrachloride
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EXERCISE 7
Name each compound :
a) BCl3
b) SF6c) P2O5
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