ASIMILASI 1.pdf

7/25/2019 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


* X is the symbol of the element


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21

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)


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


Electron transferred fromsodium to chlorine


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Formation of ionic bond in MgO

2.8.2 2.6

Mg2+

2.8

O2

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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.


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


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


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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ASIMILASI 1.pdf