Modul Kimia

58
1. Khoirinisak 2. Riski Yudatama 3. Harlely Rianavita 4. Seri Dwiwati 5. Tria Yussanti Atoms, Molecules and Ions

Transcript of Modul Kimia

Page 1: Modul Kimia

Kelompok 2:

1. Khoirinisak

2. Riski Yudatama

3. Harlely Rianavita

4. Seri Dwiwati

5. Tria Yussanti

, Molecules and Ions

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1.1 Basic competencies

Explaining the concept of atoms, theori of atoms, structure atoms, mass number

atoms, elektron configuration, periodic table unsure

1.2 Indicator

Comparing the development of atomic theory

Determine the number of protons, electrons and neutrons of an element by its

atomic number and mass number.

Determine the isotope, Isobars and isoton an element

Determining the atomic structure based on the periodic table

Determine the properties of elements relative atomic mass

Determine the valence electron and the electron configuration of elements

from the periodic table

ATOMS

1.1. Particle Concept

Sand is one example of the object in the form of granules. However, a grain of sand

can still be broken down and keep the sand fractions. Imagine a grain of sand with a

mass about 10 mg (regular sand grains) if grains of sand were split into two, you will

get two grains of sand, each mass of 5 mg. If each grain is broken up into two more,

then 4 grains of sand will be obtained each 2.5 mg mass. Suppose that the cleavage

can be carried out continuously, it will obtain a very small grains, but still the same

with sand. So is the smallest particle of matter is part of the material still has

properties similar to those materials.

ATOMS

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Sand sand particles called molecules. Sand molecules composed of one silicon atom

bonded with two oxygen atoms. This molecule can also be broken down, but the

results are no longer the sand, but two types of atoms, ie atoms of silicon and oxygen

atoms. Oxygen atom is the smallest part of the oxygen that still has the same

properties with oxygen. Likewise with the silicon atom is the smallest piece of silicon

that still has the same properties with silicon. Oxygen and silicon is the substance that

was in the form of atomic particles.

1.2 THEORY ATOMS

1.2.1 Democritus

In the fifth century SM, Greek philosopher Democritus expressing his belief that

all matter consists of particles of very small and can not be on for longer, which he

calls atomos (can not be shared). This opinion is rejected by Aristotle (384-322

BC), who argued that matter is continuous (the material can be cut continuously

until no finite). But this theory remained, at that time experimental evidence

supports the concept of "atomism" is and gradually produce a modern definition of

elements and compounds.

1.2.2 John Dalton (1803)

In 1803, John Dalton expressed the opinion expressed about the atom. Dalton

expressed the opinion of the atoms as follows:

1. The element is composed of very small particles, called atoms. all the atoms of

certain elements is the identity, which has the size, mass and chemical properties

of the same. Certain elements of different atoms with atoms of other elements.

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2. compound consists of atoms of two elements or more. In each compound the

ratio between the number of atoms of any two elements there can be an integer or

simple fraction.

3. chemical reactions that occur in just a separation, merger, or rearrangements of

atoms; so that the atoms can not be created or destroyed.

Hypothesis Dalton atomic model as illustrated by solid balls as in shot-put. As the

picture below:

1.2.3 Josep John Thomson (1900)

Based on the discovery of a better cathode tube by William Crookers, then JJ

Thomson further research on cathode rays and can be ascertained that the cathode

rays are particles, because it can turn a propeller that is placed between the cathode

and anode. From the results of this experiment, Thomson stated that cathode rays

are particles making up atoms (subatomic particles) which are negatively charged

and hereinafter referred to as electrons.

Atoms are neutral particles, because negatively charged electrons, then there must

be other positively charged particles to neutralize the negative charge of the

electron. From these discoveries, Thomson improve weaknesses of daltons atomic

theory and atomic theory put forward known as Thomson Atomic Theory. Which

states that:

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"Atom is a solid ball is positively charged and negatively charged electrons

scattered therein"

Thomson atomic model analogous to the positive ball solid. Thomson atomic

model can be described as follows

1.2.4 Rutherford

Rutherford with two of his disciples (Hans Geigerdan Erners Masreden)

conducted an experiment known as the scattering of alpha rays (λ) of thin plates

of gold. Previously been found to the alpha particle, the particle is positively

charged and move straight, large translucent power so it can penetrate thin sheets

of paper. The experiment was actually intended to test the opinion of Thomson,

namely whether this atom is a ball really solid when subjected to a positive alpha

particles will be reflected or deflected. From their observations, found the fact

that when alpha particles were fired at a very thin gold plate, then most of the

alpha particles passed (there is a deviation angle of less than 1 °), but from the

observations obtained Marsden fact that one in 20,000 alpha particles will turn

angle of 90 · Even more.

Based on the symptoms that occur, obtained following conclusions:

1. Atom is not a solid ball, because almost all the alpha particles passed

2. If the gold plate is considered as a single layer of atoms of gold, the gold

atoms contained in very small particles which are positively charged.

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3. Such particles are particles that make up an atomic nucleus, based on the fact

that 1 in 20,000 alpha particles will be deflected. When the ratio of 1:20,000 is a

comparison of the diameter, the size of the nuclei obtained approximately 10,000

smaller than the overall size of the atom.

Based on the facts obtained from this experiment, Rutherford proposed a model

of the atom, known as Rutherford Atom Model which states that the Atomic

nuclei are composed of very small and positively charged, surrounded by

negatively charged electrons. Rutherford assumed that the particles contained in

the nuclei of neutral particles binding function of positive order not to repel each

other.

Rutherford atomic model can be described as follows:

1.2.5 Neils Bohr

1913, Danish physicist named Neils Bohr atom Rutherford repair failures through

experiments on the hydrogen atom spectrum. Bohr on atomic hydrogen involves a

combination of the classical theory of Rutherford and of Planck's quantum theory,

expressed by four postulates, as follows:

1. There are only a certain set of orbits are allowed for one electron in a hydrogen

atom. Orbit is known as a state of stationary motion (settling) of electrons and is a

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EXERCISE

circular path around the core.

2. As long as the electrons are in stationary trajectory, the electron energy remains

so there is no energy in the form of radiation emitted or absorbed.

3. Electrons can only move from one stationary trajectory into another stationary

trajectory. In this transition, a certain amount of energy involved, the amount in

accordance with Planck equation, ΔE = hv.

4. Stationary trajectory is allowed to have the scale with certain properties,

especially a property called angular momentum. The amount of angular

momentum is a multiple of h/2Π or nh/2Π, where n is an integer and h Planck

constant.

According to Bohr's atomic model, the electrons surrounding the nucleus in certain

paths called electron shells or energy levels. Lowest energy level is the electron

shell which is located in, getting out of her skin and the greater the number the

higher the energy level.

1. How the atomic theory by John Dalton,?

2. Describe the atomic model according to what jj thomson.dan particles arranged?

3. What is the difference borhdan atomic theory atomic theory of quantum

mechanics?

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Quiz

In this section you have mastered the competencies is to know the type and model

type of atomic theory and structure of an atom. based on the description of the

various experiments the scientists in search of something that make up atoms.

complete the following table!

Summary of events and personalities

involved

The results obtained

- Use of the term atomic

- The mass of the electron

John dalton atomic theory put forward -

Gold plate experiment -

- Bohr's atomic model

- The discovery of the neutron

1.3 ATOMS STRUCTURE

massa (kg) Massa relatif Muatan listrik (C)

Proton 1,672623×10-27 1836 1,602189×10-19

Neutron 1,674929×10-27 1839 0

Electron 9,109390×10-31 1 -1,602189×10-19

1.3.1 Elektron

Electrons are found through the cathode tube experiment was first performed by

William Crookes. Joseph John Thomson (1897) continue the experiments of William

Crookes that the influence of electric field and magnetic field in the cathode ray tube.

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In the experiment, when the two metal plates connected by a high voltage source,

negatively charged plate called the cathode, which emits invisible light. cathode ray is

attracted to the positively charged plate, called the anode, where the rays iti going

through a hole and climb on to the other end of the tube. When these rays hit the

surface that has been coated in particular, the cathode ray luminescence yield strong

or bright light.

Because the cathode ray is attracted by positively charged plate and was rejected by

the negatively charged plate, the ray must consist of particles are negatively charged.

These negatively charged particles that is what we know as electrons.

1.3.2 Proton and nucleus

The discovery of the proton beam is a continuation of the cathode ray tube (CRT). Its

positive pole away from those found by Goldstein in 1886. And supported by the

Rutherford prediction.

Rutherford conducted experiments using α-rays to determine the atomic structure, α-

rays by firing a very thin gold leaf. Then he observed that most of the particles

penetrate the sheet without turning or only slightly banked. He also observed that

there is a waste of α particles (or dibelokan) with a large angle. On several occasions,

returned towards the coming of α particles.

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To explain the results of light scattering experiment, Rutherford made a new

model for the structure of atoms, assuming that most of the atom must be empty

space. He also predicted that the positive charge accumulated in the nucleus of all

atoms b (nucleus), which is a dense central core of which lies within the atom. 

The particles are positively charged protons in the nucleus is called. In a separate

experiment, found that the proton has a charge yiap magnitude (large) the electron

and its mass equal to 1.67262 × 〖10 〗 ^ (-24). 

1.3.3. Neutron 

Rutherford atomic model leaves important issues unresolved. when comparing the

mass of hydrogen that has one proton with a mass of helium has 2 protons. So the

ratio of the mass of hydrogen atoms with helium atoms is 2:1. But in reality its mass

ratio of hydrogen atoms with helium atoms is 4:1. 

Rutherford and his colleagues postulated that there must be other types of subatomic

particles in atomic nuclei; proof is given by James Chadwik, in 1932. When Chadwik

α particles fired into a thin sheet of beryllium, the metal emits a very high-energy

radiation similar γ-ray view. Subsequent experiments showed that the light is actually

composed of neutral particles that have a mass slightly larger than the proton

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mass. Chadwik named this particle the neutron. 

Mystery of the mass ratio of hydrogen atoms with an atomic mass of helium can

already be described. In the helium nucleus has two protons and two neutrons,

whereas in the hydrogen nucleus there is only one proton only. So that the mass ratio

of hydrogen atoms into helium atoms with a mass of 4:1

1.4 Number of atoms and Number of mass

The number of protons in an atom is called the atomic number or proton number. The

number of protons are characteristic of an element. This means that the atoms of a

particular element has an atomic number that distinguishes it from atoms of other

elements. Given the symbol Z. The atomic number For neutral atoms the number of

protons in the nucleus is equal to the number of electrons so the atomic number is

also the number of electrons that orbit around the atomic nucleus. The number of

protons and neutrons in atomic nuclei is called the mass number, which given the

symbol A. So, if the atomic symbol is X then the writing of an atom is:

XZA

Description:

X = the atomic symbol

Z = atomic number = number of protons = number of electrons

A = mass number = number of protons + number of neutrons.

or

Number of mass (A) =total of protons + total of neutron

Total of neutron = number of mass – number of atoms

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EXAMPLE

Atoms having the same atomic number but have different mass numbers called isotopes. Examples of isotopes: 

Each isotope of an element have the same chemical properties as the number of electrons equal. These isotopes can be used to determine the relative atomic mass (Ar), the atom is based on isotopic abundance and atomic masses of all isotopes. 

Isobars are elements that have the same mass number. The existence of isotopes that make the Isobars. 

  

Isoton are atoms that have equal numbers of neutrons but different number of protons. As we have learned before, that the neutron is the difference between the number of atomic mass number; then isoton can not occur for the same element.

1. How many protons, electrons, neutrons, atoms following the

a. 12 6 c b. 23

11 N+

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2. An atom has 19 protons 20 neutrons and 19 electrons. What the numbers and atomic numbers? What is the cargo?

Solution :

1. a. Atom 12 6 C

Number of atoms : total proton : total elektron : 6

Number of mass : 12

Number of neutron : 12-6 :6

So,total proton : 6,

Total elektron : 6 ,

Total neutron,:12

b.Atom 23 11

N+

Number of atoms : total proton :total elektron : 11

Number of mass : 23

Total of neutron : 12

Total elektron :Z-muatan :11-1:10

So, ,total proton : 11,

Total elektron : 12

Total ,neutron,:10

2. Number of mass : total proton + total Neutron :19 + 20 :39

Number of atoms : total proton : total elektron : 19

1.5Periodic Table

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Periodic systems have evolved along with the increasing number of elements

that are found. Making periodic table preceded by Dobereiner proposed

system triads. Then further developed by Newland with oktafnya system.

Further preparation of the periodic table is done by Lothar Meyer and

Mendeleev. Mendeleev who first suggested the periodic table, then he is

regarded as the inventor of the periodic table is often referred to as short-

periodic system of elements. Moseley managed to find errors in the

Mendeleev periodic table there is an inverse element is located.

Modern periodic system can be regarded as Mendeleev periodic system

improvements. Modern periodic system, also known as long-form periodic

system, composed of increasing atomic number and similarity of properties.

In the modern periodic system, there are horizontal rows called periods and

vertical columns called groups. Periodic system has to do with the electron

configuration. Group together with the valence electrons and period equal to

the amount of skin atom.Unsur elements that make up the periodic system

have kelogaman properties. In general, these elements exist that have the

properties of metals, non metals, and metalloids. If we look at the periodic

table, metal elements located on the left, and non-metallic elements located on

the right. The properties of the periodic system, among others, atomic radii,

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EXERCISE

which have a tendency in one group is getting bigger and smaller in one

period. This is the opposite of ionization energy, electron affinity, and

electronegativity that have a tendency in one group gets smaller and in a

period greater

1. periodic structure based on modern

a. chemical properties of elements

b. the atoms of the element

c. physical properties of elements

d. electron configuration

e. atomic weight of element

2. atom consists of positively charged material that was scattered electrons in

electron bagaiakan raisins in bread kismis.model atoms was presented by

a. R. Milikan

b. jj Thomson

c. N, Borh

d. Goldsten

e. E, Rutherford

3. atomic nuclei proposed by

a. jj Thomson

b. E, Rutherford

c. Goldsten

d. H. Begruerel

e. marie curie

4. elements are elements that the said group how

a. 1A

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b. 11A

c. 111A

d. 1VA

e. VA

5. what is the atomic number elements of potassium

a. 4

b. 8

c. 19

d. 38

e. 58

6. the number of atoms of element X that its nucleus contains 20 neutrons while

the X + ion contains 18 electrons

a. 18

b. 20

c. 38

d. 39

e. 40

7. known 6530Zn Zn 2 + ions mengndung

a. 28 electrons in the core

b. 28 protons in the nucleus

c. 28 protons around the core

d. 8 electrons around the nucleus

e. 30 protons around the core

Electron configuration and valence electron

8. A period of 31 numbered element has the electron configuration as follows

K L M

2 8 5

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Each atomic element has

a. 15 electrons 15 neutrons

b. 15 protons 15 neutrons

c. 15 protons 16 neutrons

d. 15 electrons 31 neutrons

e. 31 electrons 31 protons

9. Here is the symbol of an element 20A

Electron configuration for the A2 + ion is

a. 2 8 8 2

b. 2 8 10

c. 2 8 8

d. 2 8 8 4

e. 2 8 12

10. The number of valence electrons in the 54X is

a. 4

b. 5

c. 6

d. 7

e. 8

ESAI1. explain the Rutherford atomic model. particles of what is found Rutherford

2. specify the period and class of each element below

a. 8o

b. 10Ne

c. 17Cl

d. 20Ca

e. 11Na

3. A third of an atom has an atomic number 53 and number 129 times

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a. Make the filling electron configuration then draw each skin electron

b. How many valence electrons

c. Berapakan isotopes, Isobars, and isoton atom A is!

1.6 Electron Configuration

Persebaran elektron dalam atom disebut konfigurasi elektron. Persebaran

elektron pada kulit-kulit atom mengikuti pola tertentu.

Pengisian elektron dimulai dari kulit K, L, dan M

1.6.1 Relationship between the electron configuration with Period

In the periodic system, the period shows the number of skin that has been filled

electron in an atom.

So according to the amount of skin that is K, L, M, N, O, P, Q then the periodic

system has seven periods.

1,6,2 Relationships Between Group With Electron Configuration

Element which is located on one group has chemical properties that are

similar (almost identical).

The elements of class A is called the primary group, while the elements of

group B is called a transition element (transition), all elements of the

transition given the symbol B triads except for iron, palladium and platinum

are called "class VIII''

1.6.3 SYMBOL ELEMENTS OF GROUP A

Coat Type NAME TYPE Configuration Elektron outer Orbital

I - A Alkali ns1

II - A Alkali tanah ns2

III - A Boron ns2 - np1

IV - A Karbon - ns2 - np2

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Silikon

V - A Nitogen - Posphor

ns2 - np3

VI - A Oksigen ns2 - np4

VII - A Halogen ns2 - np5

VIII - A Gas mulia ns2 - np6

SYMBOL ELEMENTS OF GROUP B

Elektron Configuration

Coat Type

(n - 1) d1 ns2 III - B(n - 1) d2 ns2 IV - B(n - 1) d3 ns2 V - B(n - 1) d4 ns2 VI - B(n - 1) d5 ns2 VII - B(n - 1) d6-8 ns2 VIII(n - 1) d9 ns2 I - B(n - 1) d10 ns2 II - B

1.6.4 Determination Period And How To Type A Elements

1. The element with atomic number 11, the configuration: 1s2 2s2 2p6 3s1

- N = 3, means a period of 3 (skin M).

- Valence electrons (outermost) 3s as much as an electron, means including

class IA.

2. Ga elements with atomic number 31, the configuration: 1s2 2s2 2p6 3s2

3p6 4s2 3d10 4p1

- N = 4, means the period 4 (skin N).

- Elektronvalensi 4s2 4p1, meaning class IIIA.

3. Sc element with atomic number 21, the configuration: 1s2 2s2 2p6 3s2 3p6

4s2 3d1

- N = 4, means the period 4 (skin N).

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EXERCISE

- 3d1 4s2 means the group IIIB.

 

4. Fe element with atomic number 26, the configuration: 1s2 2s2 2p6 3s2 3p6

4s2 3d10

- N = 4, means the period 4 (skin N).

- 3d6 4s2, means the group VIII.

A. Choose one correct answer!

1. Nucleus of an atom consists of .......

a. protons and neutrons c. protons, electrons and neutrons

b. protons and electrons d. neutrons and electrons

2. Atom will become positive ions or cations when .......

a. receiving proton c. loss of proton

b. accept electrons d. loss of electrons

3. Atom consists of positively charged material and the electrons are scattered

Inside. This is a model of the atom by .......

a. John Dalton c. Thomson J.J

b. Rutherford d. Niels Bohr

4. An atom has three orbits of the electrons with the number of electrons in the

outermost orbit 2 electrons. Element's atomic number is .......

a. 8 b. 12 c. 14 d. 16

5. What is meant by the atomic number is .......

a. the number of protons in the nucleus

b. the number of electrons in atomic nuclei

c. number of neutrons in atomic nuclei

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d. the number of protons and neutrons

6. The number of neutrons contained in the atom 2311Na is .......

a. 6 b. 8 c. 10 d. 12

7. Distribution of electrons in an atom is called .......

a. elektronisasi c. electron configuration

b. ionization d. isotope

8. Ion consisting of two or more atoms is called .......

a. cation c. polyatomic

b. anion d. single ion

9. These particles are not electrically charged is .......

a. protons c. electron

b. atom d. ion

10. Of the following chemical formula that considered the molecular compound is

.......a. H2 b. O3 c. CO d. P4

B. Answer the questions below with a brief and clear!

1. According to Democritus, the material is discontinuous, explain what it

means!

Answer:.......................................................................................................................................

..................................................................................................................................................

..................................................................................................................................................

2. Atom consists of protons, electrons and neutrons. How does the layout of the

subatomic particles in atoms?

Answer::.....................................................................................................................................

..................................................................................................................................................

..................................................................................................................................................

3. Write the electron configuration of elements with atomic numbers

a. 7 b. 14 c. 18

Answer:....................................................................................................................................

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Standard Competens : 3. Discribing about Ions

Indicator : Distinguish between the anion and cation charge

..................................................................................................................................................

IONS Ion is an atom or group of atoms that have a positive or negative net charge. The number of positively charged protons remain the same preformance of an atom, but the number of negative charged electrons can be increased or decreased. Neutral atom loses one or more of its electrons will produce a cation, ion with a positive total charge. For example, atoms (Na) can easily lose its one electron to become kationn sodium, which recorded for Na +. 

Atom Na Ion Na+

11 proton 11 proton11 elektron 10 elektron

On the other hand, the neutral atoms receive electrons will produce an anion, the total negative ion charge due to the addition of the number of its electrons. for example, atomic chlorine (Cl) may receive an additional electron to become ions clorida. 

Atom Cl Ion Cl-

17 proton 17 proton17 proton 18 elektron

Atoms can lose or receive more than one electron. For example, Mg2+, Fe3+ and others. These ions also Na+ and Cl- can be called monatomic ions because only composed of one atom. While ion consisting of two or more atoms in the polyatomic ion called. Such as, OH-, NH4

+ , CN- and others. 

Ionic Formulas compound

Ionic compound is a compound formed by cations and anions. For example NaCl is

composed of ions Na + and Cl-ions. In order for ionic compounds are electrically

neutral, the amount of charge on the cations and anions in each unit of the formula

must be zero. If the charge on the anions and cations are different, we apply the

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EXAMPLE

exerciseESAI

following rules to create electrically neutral formula: cations subscript numbers equal

to the charge on the anion, and the numbers subscript equal to the charge on the

anion-cation.

Potassium Bromide k + cations and the anions Br-ionic compounds combine

to form potassium bromide. The amount of the charge is +1 + (-1) = 0, so it is

not in need subscript. The formula KBr.

Zinc Iodide Zn2 + cations and anions I-combine to form zinc iodide, the

amount of the charge +2 + (-1) = +1, so that the charge be zero we must

multiply charge anions-1 by 2 and adding the subscript 2 on iodine. So the

formula for ionic zinc iodide is ZnI2.

Aluminum Oxide Al3+ dan anion O2- -joined to form aluminum oxide, the

charge +3 + (-2) = +1, in order to charge the non-2 (+3) +3 (-2) = 0 and add

subskrit 2 on Al , the subscript 3 on O.

1. Among the following properties are not properties of ionic compounds are ....     A. fragile     B. high melting point     C. the solution can deliver electricity     D. lelehannya can deliver electricity     E. the solid can deliver electricity

2. Among these substances, which have an ionic bond is .... A. ice B. limestone C. silicon D. sugar

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E. bronze

3. Na atoms with atomic numbers 11 to form the ion ... .     A. +1 B. -1 C. +2 D. -2 E. +3

4. An element with atomic number 12 can form ionic bonds with atoms unsurbernomor ... .     A. 3 B. 18 C. 11 D. 20 E. 17

5. Electron configuration of element X with 2, 8, 8, one can form ionic bonds with elements     Electron configuration ... .     A. 2, 8, 1 B. 2, 8, 2 C. 2, 8, 7 D. 2, 8 E. 2

6. Most ionic bond can form between pairs of elements ... .    A. K and F B. Li and C. C. Na and Cl D. Na and Li E. K and Mg

7. Here are the properties of ionic compounds, except ... .    A. water-soluble C. soft and fragile B. can conduct electricity of melt D. the solution can conduct electricity   E. high melting point

8. The couple elements - elements of the following groups that can form an ionic bond is an element of class .... A. IA & VIIIA B. B. IA & IIA

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C. C. IIA & VIIA D. VIA & VIIA E. IIIA & IIIA

 9. The following pairs of compounds which have an ionic bond is ....  A. KCl & CaF2                             C. CaF2 & HF                             E. NH3 & KNO3

   B. NaCl & CCl4                            D. KCl & CCl4

15. Each element of X & Y - each having 6 & 7 electrons. Formulas & type of the corresponding bond if both element is ....   A. XY6, ionic B. X2Y, covalently C. XY2, covalently D. XY2, ionic. E. X2Y, ionic

16. The following pairs of compounds that bind covalently coordinate ion & is ....   A. NaCl & CO2 B. SO2 & CCl4 C. NaCl & HCl D. NH4

+ & MgCl2 E.. KOH & O2

17. Type of bond that is not likely to occur between non-metallic & non-metal is ... .   A. Ionic bond C. Single covalent bond    B. Triple covalent bonds D. Coordinate covalent bond E. Double covalent bond

18. Statements are true about an ionic bond is .... .   A. Occurs between the elements in group VIIA & VA D. Occur with the use of electron   B. Have an electrostatic attraction force E. Can draw objects - metal objects   C. Having a small electron negativity difference

19. 11Na & 35Br elements can form .... .   A. Ionic bonding, the formula Na2Br D. Ionic bonding, the formula NaBr   B. Covalent bonding, the formula NaBr E. Covalent bonding, the formula Na2Br   C. Covalent bonding, the formula NaBr2

20. The following group of compounds that have ionic bonds are ....   A. H2O, CO2, CH4 D. CO2, CH4, NH3

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ESAI

   B. . NaCl, HI, H2O E. K2O, NaBr, MgCl2

C. HCl, H2SO4, NaOH

21. Element with electron configuration 1s2 2s2 2p6 3s2 can form ionic bonds with the elements .... A. 1A B. 4B C. 17C D. 19D E. 20E

22. Among the elements below which has a tendency to accept electrons form a configuration      electron is stable ... .   A. 10X C. 17Z B. 11Y D. 18A E. 19b

23. The following elements are very difficult to chemically bind is ....   A. Fe, Au C. Cl, P B. Na, Mg D. H, He E. Ne, Ar

24. The following statement is not a characteristic ionic bond is ....   A. Formed between the metal & non-metallic D. There are positive & negative ions ion   B. Has a tensile strength - attractive electrostatic    C. Handover occurs electron D. There are positive & negative ions ion E. Occurs between the elements of group IVA & VIA

25. The following group of compounds that have ionic bonds are ....   A. H2O, CO2, CH4 D. K2O, NaBr, MgCl2    B. NaCl, HI, H2O E. HCl, H2SO4, NaOH C. CO2, CH4, NH3

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Standard Competens : 3. 3. Comparing between molekules unsure dan molekules element.

Indicator :

discribing about molekules comparing between molekules and element Distinguishing unsure and element differentiateing molekules unsure and molekules element.

1.. Determine the ionic compounds formed from reactions between these atoms

a 11Na dan 10S

b. 13Al dan 10S

2. Choose couples the following elements that can form ionic compounds!

a. 19K dan 2He

b. 19K dan 17Cl

c. 16S dan 8O

4. Determine the formula of ionic compound element pairs of the following elements a. Na with O b. Ca with N

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MOLEKULESMolecule (molecule) has the same meaning as the compound (compound), which is a

combination of several elements / atoms.

Examples of compounds / molecules that exist in nature such as: water (H2O), carbon dioxide

(CO2), carbon monoxide (CO2), and others.

So, what's different compounds and molecules?

In terms of meaning it makes no difference. But its use is different. Molecules including

nouns (objective) while the compound is an adjective (adjective). Let us see the following

figure:

H2O CO2

H2O

Sentence / statement can be made based on the picture above are:

• In the picture there are two types of compounds, namely water (H2O ) and carbon dioxide

(CO2).

• In the picture there are three molecules, namely two molecules of water (H2O) and one

molecule of carbon dioxide (CO2).

Molecule formation occurs from non-metallic elements which reacted with similar non-

metals, non-metallic element with other non-metallic elements or non-metallic elements with

metal elements

chemical formulaChemists use chemical formulas to express the composition of the

molecular and ionic compounds in chemical symbols. Here we will discuss about the

molecular formula, empirical formulas and formulas of chemical compounds.

molecular formula

Molecular formula shows the exact number of atoms of each element in the

smallest unit of a substance. For example H2 is the formula for the hydrogen

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molecule, O2 for oxygen, O3 for ozone, H2O for water and others. Subscript

numbers mark the number of atoms of an element. Molecular formula shows the

exact number of atoms of each element in the smallest unit of a substance. For

example H2 is the formula for the hydrogen molecule, O2 for oxygen, O3 for ozone,

H2O for water and others. Subscript numbers mark the number of atoms of an

element present in the molecule. For example H2O, no subkrip on O because it only

contained one O atom in water molecules, whereas for H subscripts 2 because there

are two H atoms in water molecules.

3.1 Diatomic Molecules

Diatomic molecule is formed from two similar atoms. Are you able to cite the

example of a diatomic molecule? Yes I do.

Examples of diatomic molecules is molecular oxygen, molecular hydrogen and

molecular nitrogen.

 

3.2 Tetraatomic molecules

Tetraatomik molecule is formed of four similar atoms. Are you able to cite

examples of molecules tetraatomik? Yes I do. Examples tetraatomik molecule is

a molecule of phosphorus.

 

3.3 Oktaatomic molecules

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Oktaatomik molecule is formed from eight similar atoms. Are you able to cite

examples of molecules oktaatomik? Yes I do. Examples tetraatomik molecule is

a molecule of sulfur (sulfur).

 

Quiz

Fill in the blank in the table of molecular elements in the column name and the number of elements, such as number 1.

NO Unsure name Lambang Rumus Molekul

Compiler Name and Number of Elements

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1

2

3

4

5

6

7

8

9

10

11

Hidrogen

Florida

Oksigen

Oksigen

Nitrogen

Klorida

Bromide

Iodide

astatin

phosphor

sulfur

H

F

O

O

N

Cl

Br

I

At

P

S

H2

F2

O2

O3

N2

Cl2

Br2

I2

At2

P4

S8

Consists of two atoms of hydrogen ……………………………………………

……………………………………………

…………………………………………..

…………………………………………….

…………………………………………..

………………………………………….

……………………………………………

…………………………………………

…………………………………………

………………………………………..

3.4 UNSURE

The element is a single substance that can not be described again into other

substances are much simpler with ordinary chemical reactions. The universe contains

countless elements. It turned out that all substances are composed of basic substances

called elements. Inspired by the many elements that exist in the universe is Jons

Jakob Berzelius (1779-1848) who came from Sweden states that any given element

symbol in the form of letters of the name element in the Latin language with the

following provisions:

1. The emblem consists of a single element must use uppercase letters

2. Coat terdir elements of the two letters should be put on the first letter uppercase

and lowercase letters in the second letter

Some element name and symbol

NAMA LATIN

NAMA INDONESIA LAMBANG

Argentum Perak Ag

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Aluminium Aluminium AlArgon Argon Ar

Arsenicum Arsen AsAurum Emas AuBorium Boron BBarium Barium Ba

Bismuthum Bismut BiBromium Bromin Br

Carbonium Karbon CCalsium Kalsium Ca

Chlorium Klorin ClCobaltum Kobal CoChromium Kromium Cr

Cuprum Tembaga CuFluorium Fluorin FFerrum Besi Fe

Hydrogenium

Hydrogen H

Helium Helium He

Symbols of the elements listed above is only a small fraction of the elements

contained in this universe.

3.5 Compounds

Compounds are substances that emerged from two or more elements through chemical

reactions. Each compound has unique properties, different from the properties of its

constituent elements. Examples of Hydrogen and Oxygen is a gas, are the combined

results of the second element is the clear liquid, colorless, and no sense that we know as

water.

The compound is a substance that can be used to chemically decompose into substances

that are more modest. Compound composed of two or more elements of different types

with a fixed and certain comparisons with the incorporation of chemically

Compound name and formula of compounds

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NAMA SENYAWA

RUMUS SENYAWA

Glukosa C6H12O6

Sukrosa C11H22O11

Garam Dapur

NaCl

Asam Cuka CH3COOHUrea CO(NH2)2

Asam Sulfat

H2SO4

Soda Kue NaHCO3

Amoniak NH3

Aseton CH3COCH3

The molecule is a particle consisting of two or more atoms, either type of atom or

different atoms. The molecule consists of molecules of elements and molecular

compounds, to distinguish the molecular elements and molecular compounds are as

follows.

3.7 Moleculas unsure

Molecular elements are generally formed from non-metallic elements. Some non-

metallic element found naturally as molecules, atoms rather than as a stand-alone. One

example is oxygen. Oxygen gas contained in the air consists of molecules of O2. This

happens because the more stable form of oxygen molecules from the atoms as a stand-

alone. When heated at high temperatures, the molecules will break down into oxygen

atoms. Some examples of elements (non metallic) which exist as molecules are as

follows:

Elements that exist as molecules and molecular formula.

Nama Unsur

Lambang Unsur Rumus Molekul

Hidrogen H H2

Nitrogen N N2

Oksigen O O2

Fluorin F F2

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Klorin Cl Cl2

Bromin Br Br2

Iodin I I2

Fosforus P P4

Belerang S S8

The formula states melekol arrangement of molecules, O2 stated that each

molecule consists of two atoms, P4 means that each molecule consists of four requi

3.8 Compound molecules

Molecules of compounds consisting of two or more kinds of atoms. Examples of

water molecules that have been mentioned in the previous section. Another example of

a molecule of ammonia (NH3) and methane molecule (CH4).

          Various types of molecules we have seen in the discussion above. All the examples

given is a simple molecule, composed of two atua are three types of elements and

consists of only a few atoms only. Many also include a very complex molecule is a

molecule compounds found in living things, such as vitamin B2, Protein, and DNA.

Many of the molecules of compounds that play a role in living systems that are used to

address various health issues, including genetic engineering.

Quiz

. Below is a few pictures of molecules. for these molecules is by filling in the blanks

available with the molecule compound or molecular elements.

Page 35: Modul Kimia

exercise

Choose one correct answer!

1. Substances that can not be described again into other substances by ordinary

chemical reaction called .......

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a. element c. molecule

b. d. compoun d ion

2. Substances that are composed of multiple elements with a fixed ratio is

called .......

a. solution of c. compound

b.combine d. mixture element

3. The lightest element is .......

a. . hydrogen c. carbon

b.. oxygen d uranium

4. The most serious element is .......

a. uranium c. oxygen

b. hydrogen d. carbon

5. The symbol of the element zinc is .......

a. Al b.Cu. C. Zn D Fe

6. The person who first gave the letter symbols on each element is .......

a. John Dalton c. Thomson

b. Jons Jakob Berzelius d. Rutherford

7. Substances that may decompose through chemical reactions used to be the

substances that are more sedehana called .......

a. element c. atom

b. molecules d. compound

8. Below that is not an element molecule is .......

a.. N2 B. Br2 c. Cl 2 d. HNO

9. Known molecular formula of alcohol is C2H5OH, Means in 2 molecules of

alcohol are .......

a. 2 atom b. 8 atoms c. 9 atom d. 18 atom

10. Here is a molecule-molecule compounds, except .......

a. O2 b.H2SO4 C.NaNO3 d. HNO3

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example

3.9 Empirical formula

Empirical formula shows us that there are elements and the simplest integer ratio

of the atoms, but do not always have to show the true value in a molecule. For

example, hydrogen peroxide has the molecular formula of H2O2. This formula

indicates that the ratio of hydrogen atoms with oxygen atoms in the molecule is 2:2 or

1:1, so the empirical formula HO.

An analysis of the ionic compound indicates that the compound contains 2.82 g of

sodium, 4.35 g of chlorine, 7.83 g of oxygen. Determine the empirical formula of the

compound

Solution

Determine the time of each element of Na Cl O

1.82 4.35 7.83

Numbers with each Ar2.8223

4.3535,5

7,4816

Comparative smallest 0.123 0,123 0,489

So the empirical formula 1 1 2

then in may NaClO2

RELATION BETWEEN ATOM, MOLECULES and IONS IN LIVE

A. The relationship between atoms, ions and molecules

In the foregoing discussion has known how the concept of atoms, ions and

molecules are all interconnected as one example in this case the production of

sugar. We imagine that one tablespoon of granulated sugar is composed of tiny

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grains of sugar. If one spoon of sugar is dissolved in water it will dissolve the

sugar, the sugar particles dispersed into the water with a very small size so can

not be filtered even can not be seen by the eye. Though transformed into particles

whose size is very small nature of the sugar is not lost. Small particles of sugar

still has the same properties with granulated sugar molecule called glucose. The

smallest particle of matter can be shaped constituent atoms, ions and molecules.

So we can conclude that the atom is the smallest part of an element, and the

molecule is the smallest particle of a compound composed of two atoms or more.

Molecules composed of atoms called molecules of different compounds.

Molecules are composed of atoms called molecules of the same element. While

the ion is a collection of atoms that are electrically charged, positively charged

ions can (cations) and negatively charged (anions)

B. The material is composed of atoms, ions and molecules

Basically molekules theories of physics to explain the change, but not necessarily

able to explain the chemical changes, because it developed the atomic theory

which states that all matter consists of particles of very small particles called

atoms. In 1803, John Dalton a British propose a theory which states that matter

consists of atoms. Dalton's atomic theory can be summarized as follows:

1. Each is composed of the smallest particles of matter called atoms

2. Atom can not be broken down into smaller particles with similar properties

3. The atoms of certain elements have identical properties and mass. Different

elements have atoms of different mass.

4. Compounds are formed from two or more kinds of atoms are different.

5. Chemical reactions are merging and splitting the atoms of the element or

compound in the reaction.

So a material composed of several molecules, the molecules are composed of several

atoms of the same or different, for example: Oxygen (O2) is composed of two oxygen

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atoms, water molecules (H2O) is composed of two hydrogen atoms and one oxygen

atom, molecule of sulfuric acid (H2SO4) is composed of two hydrogen atoms, one

sulfur atom and four oxygen atoms.

 Likewise with other chemical products as an example: The production of urea

fertilizer with chemical composition NH2CONH2, NH4NO3, NH4 H2 PO3 dan KCl .

Aspirin C9 Ha O4 NH2CONH2, NPK fertilizer / fertilizer compound with the

composition of the mixture of NH4NO3, NH4 H2 PO3 and KCl. Acetic acid

CH3COOH is used as food vinegar. C11 22 O11 sucrose is used as a sweetener. Ha C9 O4

Aspirin is used to reduce pain.

Compounds of the formula is a combination of symbol element that shows the type of

compound-forming elements and the number of atoms of each element, such as

sucrose with the formula C12H22O11 formula shows that sucrose is composed of 12

carbon, 22 hydrogen and 11 oxygen

.

Table. Examples of that can be consumed by humans directly

Page 40: Modul Kimia

exercise

Answer the question below correctly!

1. Name the following compound-forming elements and determine the amount

Of insur, the atoms in each molecule:

a. Baking soda ( Na HCO3)

a. Caffeine ( C8 H10 N4 O2)

b. Asam cuka ( C2 H2 O4)

2. Explain the relationship between atoms, ions and molecules.

3. Make a concept map classification of the material by completing the

following

Page 41: Modul Kimia

MATERI

chart with the concepts that have been provided.

- Concepts: Homogeneous elements of compound. Heterogeneous mixture of

single substances

- Chart:

REFERENSIChang, Raymond. Tanpa tahun. Kimia Dasar: Konsep-konsep inti. Terjemahan

Lemeda Simarta. 2004. Jakarta: Erlangga.

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Sudarmo, Unggul.2004. Kimia SMA. Jakarta: Erlangga.

Sudarmo, Unggul.2006i.Kimia SMA untuk Kelas X . Jakarta: Phiβeta.

Takeuchi, Yoshito. 2008. Penemuan Elektron.(Online), (http://www.chem-is-

try.org/materi_kimia/kimia_dasar/struktur_atom1/penemuan-elektron/,

diakses 16 Desember 2011).

Utami, Budi.2011. Penemuan Partikel Dasar : Penemuan Elektron. (Online),(

http://www.chem-is-try.org/materi_kimia/kimia-sma-ma/tabel-periodik-unsur-

dan-struktur-atom/penemuan-partikel-dasar-penemuan-elektron/, diakses 16

Desember 2011).

Utami, Budi.2011. Penemuan Partikel Dasar: Penemuan Proton dan Neutron.

(Online), (http://www.chem-is-try.org/materi_kimia/kimia-sma-ma/tabel-

periodik-unsur-dan-struktur-atom/penemuan-partikel-dasar-penemuan-proton-

dan-neutron/, diakses 16 Desember 2011).

Kimiamifkho.2009. Perkrmbangan Teori Atom. (Online),

(http://kimiamifkho.wordpress.com/2009/07/22/perkembangan-teori-atom/,

diakses 16 Desember 2011).