Calculate the Molecule Mass Relative of the Compound

Molecular mass relative (Mr) calculated from the atomic mass number (Ar) of the elements in the molecule. Ar express the weight of the element relative to 1/12 atomic mass of C-12 isotope. Here is the example of the Mr NaCl calculation.

Since Ar Na=23 and Ar Cl=35,5
so, Mr NaCl is equal to the sum of that:
Mr NaCl = (1 x Ar Na) + (1 x Ar Cl) = (1 x 23) + (1 x 35,5) = 23 + 35,5 = 58,5

Now, you have to able to calculate the amount of Mr H2SO4 while known that Ar H = 1, Ar S = 32 and Ar O = 16. Right, the answer below.
Mr H2SO4 = (2 x Ar H) + (1 x Ar S) + (4 x Ar O) = (2 x 1) + (1 x 32) + (4 x Ar 16) = 2 + 32 + 64 = 98

The value of atomic mass number of some elements shown below.
H = 1        Li = 7        Mg = 12
C = 12      Na = 23      Ca = 40
O = 16      K = 39        Fe = 56
N = 14      Cl = 35,5    Cu = 63,5

Acid Overview

An acid simply defines as a substance in water solutions dissociate yielding hydrogens ions as only a positive ions. Some acids dissociate in one step yield one hydrogen ion called monobasic acid. Here is the example monobasic acid.

Others acid dissociate yield two or more hydrogen ions through two dissociation steps or more called polybasic acid.

 

Actually, in a aqueous solution, hydrogen ions doesn't exist. This proton combine with a water molecule form a hydronium ions by coordination covalent bond using a free pair electron from oxygen of the water molecule.

Ionic Bonding

The first explanation of chemical bonding was suggested by the properties of salts. Salts are generally crystalline solids that melt at high temperature. Sodium chloride for example, the white crystalline melt at 801^oC. The liquid after melting (molten) salt conduct an electric current. And a salt dissolved in water gives a solution that also conducts and electric current. The electric conductivity of the molten salt and the salt solution is resulted from the motion of ions in the liquid. A salt is formed between two atoms hold by ionic bonding. An ionic bonding corresponds to electrostatic attraction between positive and negative ions. It form between two atoms when one or more electrons are transferred from the valence shell of one atom to the valence shell of the other. The atom that loses electrons becomes positive ion (cation) and the atom that gains electrons becomes negative ion (anion). Any given ion tend to attract as many neighboring ions of opposite charge as possible. When the large number of ion gather together, they form an ionic solid. The losing and gaining electron of the atom cause the electron configuration changing.

The trend of electron configuration changing

The unstable elements tend to reach similar electron configuration with nearly noble gas by electron configuration changing. There are two trends, first the element atom trend to remove valence electrons , and secondly the element atom trend to gain valence electrons.

If the atom of an element removes it’s valence electron the positive charge particle occurs due to differences or proton and electron number in it. The number of electron will decrease and less then the number or proton, so that he atom change to the positive charge particle. We say the elements is electropositive elements.

In the opposite trends, if an atom gains valence electron, the number of electron increase and more than the number of proton, so that the atom change to the negative charge particle. The elements with trends to gain electron is named electronegative elements.

Example 1.1 :

Lithium has atomic number 3. It has electron configuration 2 1. It’s valence electron is 1 so lithium is unstable. To reach stability it must change to duplet system like helium by remove a valence electron and form lithium ion .

Li : 2 1 remove 1 valence electron to be Li ion (Li⁺) : 2

The lithium ion more stable than lithium atom

Example 1.2:

Magnesium has atomic number 12. The electron configuration is 2 8 1. It’s valence electron is 2 so it must change to octet system like neon with 2 8 electron configuration. Magnesium atom must remove two valence electron and form magnesium ion with (2+) number of charge.

Mg : 2 8 2 remove 2 valence electron to be Mg ion (Mg²⁺) : 2 8

Examples 1.3 :

Fluorine atom has atomic number 9. It’s electron configuration is 2 7. It need an electron to reach octet system. If fluorine atom gain an electron will form fluoride ion (F^-) that has 2 8 electron configuration like neon. So that fluoride ion more stable than fluorine atom.

F : 2 7 gain 1 valence electron to be fluoride ion (F^-) : 2 8

The ionic compound that formed between lithium and fluorine is LiF. Lithium loses an electron and fluorine gains it. The Li⁺ and F^- are formed and the attract to form neutral LiF compound. But if the compound is formed between magnesium and fluorine, the magnesium will removes two electrons, so in this case the two fluorine atoms are needed to gain two electrons. The formula of compound formed is MgF₂.

Flame Colour of Group IA (Group 1)

Flame colors are produced from the movement of the electrons in the metal ions present in the compounds.
For example, a sodium ion in an unexcited state has the structure 1s2 2s2 2p6. When you heat it, the electrons gain energy and can jump into any of the empty orbitals at higher levels - for example, into the 7s or 6p or 4d or whatever, depending on how much energy a particular electron happens to absorb from the flame.
Because the electrons are now at a higher and more energetically unstable level, they tend to fall back down to where they were before - but not necessarily all in one go.
An electron which had been excited from the 2p level to an orbital in the 7 level, for example, might jump back to the 2p level in one go. That would release a certain amount of energy which would be seen as light of a particular color.
However, it might jump back in two (or more) stages. For example, first to the 5 level and then back to the 2 level.
Each of these jumps involves a specific amount of energy being released as light energy, and each corresponds to a particular color.
As a result of all these jumps, a spectrum of colored lines will be produced. The color you see will be a combination of all these individual colors.
The exact sizes of the possible jumps in energy terms vary from one metal ion to another. That means that each different ion will have a different pattern of spectral lines, and so a different flame color.

The colors
The colors in the table are just a guide. Almost everybody sees and describes colors differently. I have, for example, used the word "red" several times to describe colors which can be quite different from each other. Other people use words like "carmine" or "crimson" or "scarlet", but not everyone knows the differences between these words - particularly if their
Li red
Na strong persistent orange
K lilac (pink)
Rb red (reddish-violet)
Cs blue? violet? (see below)

What do you do if you have a red flame colour for an unknown compound and don't know which of the various reds it is?
Get samples of known lithium, strontium (etc) compounds and repeat the flame test, comparing the colours produced by one of the known compounds and the unknown compound side by side until you have a good match.
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Note: I don't have confidence in the caesium flame colour. There is total disagreement about this on the web and in the books I have looked at, and I have never seen this flame colour myself. However, I have received a helpful email from a student who says: "At my school we did some flame testing experiments, and . . . caesium is actually either blue or violet, depending on the way you look at it. I think it looks more violet than blue, but it sort of changes each time you do it." (Kara Gates, March 2006). If you thought chemistry was clear-cut, you are sadly mistaken!
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Ionization Energy

Ionization energy is the energy required by an atom in the form of gas to remove one electron to form positive ions.

The lower the ionization energy, the easier an electron released an atom to form negative ions.
In the periodic table, ionization energy values showed periodicity. In a period from left to right, the ionization energy increased. In one class, from left to right, ionization energy decreased.

Electron Affinity

Electron affinity is the energy released by an atom (in the form of gas) when an electron capture to form negative ions. Since the energy is released, given the price of the electron affinity of the minus sign.
The greater the energy released, the negative ions are formed more stable. IIA group elements and VIIIA not form a stable negative ions. Prices positive electron affinity.
In one period, from left to right, electron affinity values tend to increase. In one class, from top to bottom, the electron affinity values tend to decrease.

Introduction of Chemical Bonds

An atom consists of the atomic core and the atom's skins. Atomic core consists of proton particles that is positive particles and neutrons that ia neutral particles. Meanwhile, electron skins contains electron that is negative particles. The place where electrons found is called the orbital. Electrons first put themselves on the orbitals which has the lowest energy level.

Two or more atoms can form a chemical bond using the valence electrons in order to form a molecule. If the atoms does not have a strong difference electronegativity (or little difference of electronegativity), valences electron of atoms are used together formed a covalent bond. If the atoms has a large difference of electronegativity, the atoms are formed ion bonds.

The atoms bonded to obtain stable configuration that is formed as electrons configuration of noble gas elements.

In the covalent bond, electrons used together by the atoms so that the atoms has electron configuration such as electron configuration noble gas elements. For example, hydrogen has 1 valence electron and oxygen has 6 valence electrons. Both types of elements are formed of water molecules (H₂O).
If a bond has a pair of electrons used to bond, called single covalent bond. There are also covalent bong type with two pairs of electrons, called double covalent bond. If the covalent bond using three electron pairs, called the triple cobalent bond. In some cases, the electron pair shared come from only one atom of it, called coordination covalent bond or coordinates covalent bond or covalent dativ bond or semipolar covalent bond.

At the ion bond, the atoms has a high value of electronegativity capture elctrons form a negative ion, while the atoms that has a low value of electronegaivity release the valense electrons formed positive ion. With the capture or release electrons, the atoms become stable formed electron configuration like elements configuration of noble gas. Although the atoms in the compound does not use the pair electron together, but the atoms have a strong bond each other because the atoms cargo is different. In an ion compound, all the ions form a crystal lattice structure.

Metal and Non-metallic Elements

Nowadays, more than 100 elements have been found. Elements have certain properties that distinguish between the one elements with the other elements. We can distinguish the elements to the metal elements, metaloid elements and non-metallic elements.

Some of the properties of the metal:
Malleability: the metal can be formed without cracks.
Ductility: the metal can be drawn without a change in the surface.
Toughness: metal can be crooked.
Hardness: resistance to the penetration of metal or other hard objects puncture.

Commonly non-metal elements in gas phase at room temperature. While metaloid elements have the properties between metal elements and non-metallic elements.



In the table of periodic system of the elements, non-metallic elements located on the left side (except hydrogen) and non-metallic elements is located on the right side. Metal and non-metallic elements is separated by the metaloid elements which is located in the middle table of periodic system of the elements.

Metaloid elements are Boron (B), Silicon (Si), Germanium (Ge), Arsenic (As), Antimony (Sb), Tellurium (Te) Polonium (Po), Astatine (At). Some of the metal elements are Sodium (Na), Iron (Fe), Coppre (Cu) etc. Some of the non-metallic elements are hydrogen (H), Helium(He), Oxygen (O), Nitrogen (N) etc.