.

      Iron: 1s ² 2s ² 2p ⁶3s ² 3p ⁶4s ² 3d ⁶

      Cobalt: 1s ² 2s ² 2p ⁶3s ² 3p ⁶4s ² 3d ⁷

      Nickel: 1s ² 2s ² 2p ⁶3s ² 3p ⁶4s ² 3d ⁸

      Copper: 1s ² 2s ² 2p ⁶3s ² 3p ⁶4s ¹ 3d ¹⁰

      Zinc: 1s ² 2s ² 2p ⁶3s ² 3p ⁶4s ² 3d ¹⁰

      Gallium: 1s ² 2s ² 2p ⁶3s ² 3p ⁶4s ² 3d ¹⁰ 4p ¹

      What is interesting is that Vanadium has 3d³ 4S² electrons and the next element, Chromium (Cr), should have 3d⁴ 4S² electrons, but actually it has 3d⁵4S¹ electrons. One electron passed from the 4S orbital to the 3d orbital.

      Nickel has 8 electrons on the d orbital. The next element, Copper (Cu), should have 9 electrons on the 3d orbital and 2 electrons on the 4S orbital, but actually Copper has 10 electrons on the 3d orbital and 1 on the 4S orbital. One electron passed from the 4S orbital to the 3d orbital. The electronic configuration of Copper is [Ar] 3d¹⁰4S¹.

      The complete list of electronic configurations of all the chemical

      elements cab be found in Wikipedia:

      http://en.wikipedia.org/wiki/Electron_configurations_of_the_elements_%28data_page%29

      All elements can be divided into metals and nonmetals.

      In the periodic table, metals are on the left, nonmetals are on the right.

      Group number shows how many electrons are in the outermost orbital. These electrons are called valence electrons. For example, Na (sodium) is in the first group. It has one electron on the outermost orbital Na can easily give this electron to Cl (chlorine). Cl is in the seventh group. It has 7 electrons and it takes one electron from Na. As a result Na becomes a positive ion Na+ and Cl becomes negative ion Cl -. Ions with opposite charge form ionic bonds.

      Ionic bonds usually form crystal structures. That is why salt is made of crystals.

      Carbon C, is located in the 4th group. It has four valence electrons. As a result C forms four covalent bonds with four atoms of Cl. C does not give its electrons to Cl. Carbon and chlorine share electrons. When atoms share electrons, they form covalent bonds.

      Oxides

      Oxides are produced when metals or nonmetals react with oxygen.

      Oxygen is located in the 6th group and has 6 valence electrons. It tends to gain 2 more electrons to become a complete octet and its valence is 2.

      2Ca + O2 = 2CaO

      In nature, metal oxides exist in clay. Clay is a mixture of the oxides

      SiO2

      Al2O3

      K2O

      Na2O

      MgO

      CaO

      Fe2O3

      TiO2

      Bases

      In reaction with water metals or metal oxides produce a base:

      2Na +2H2O = 2NaOH + H2

      CaO + H2O = Ca (OH) 2

      Bases dissociate in water and produce a negative hydroxide OH – ion.

      Acids

      Non metal oxides are NO2, SO3, P2O5

      In reaction with water non metal oxides produce acids:

      H2O + SO3 = H2SO4 – sulfuric acid

      H2O + NO2 = HNO3 – nitric acid

      H2O + CO2 = H2CO3 – Carbonic acid

      Acids dissociate in water and produce proton of hydrogen H+.

      Salts

      When an acid reacts with a base, a salt is produced.

      NaOH + HNO3 = NaNO3 + H2O

      To calculate the percentage composition of NaNO3, find the molecular mass of NaNO3

      23 (Na) +12 (N) +16*3 (O3) = 83

      The molecular weight of NaNO3 = 83

      83 – 100%

      23 (Na) – X%

      X = 23 * 100 /83 = 27.7% of Na

      83 – 100%

      12 (N) – X %

      X = 12 * 100/83 = 14.5% of N

      83 – 100%

      48 (O) – X %

      X = 48 * 100/83 = 57.8% of O

      Some salts are more soluble in water; some are less soluble or not soluble at all. When a non-soluble salt is produced as a result of an acid and base reaction, a precipitate is formed.

      Ca (OH) 2 + H2CO3 = CaCO3 +2H2O

      CaCO3 is not soluble in water. A white precipitate is formed.

      Salts may react with each other and new salts are produced:

      Equivalent proportions

      All chemical reactions occur in equivalent proportions.

      1. How many grams of Ca Cl2 are spent in the following reaction:

      10g?g

      Na2CO3 + Ca Cl2 = CaCO3 +2NaCl

      All compounds react with each other in certain proportions. In a given reaction one mole of Na2CO3 reacts with one mole of CaCl2

      A mole is MW (Molecular mass) in grams.

      For Na2CO3 MW is 23 *2 +12 +48 = 106 g. = 1 mole

      For CaCl2 MW is 40 +35*2 = 110g. = 1 mole.

      106 g Na2CO3 react with 110g CaCl2

      10g Na2CO3 react with X g CaCl2

      X= 10 * 110 / 106 = 10.38 g CaCl2

      2. How many grams of CaCO3 are produced if 100 ml of 0.5 M solution of Na2CO3 reacts with an unlimited volume of solution CaCl2?

      0.5 M

      2. Na2CO3 + Ca Cl2 = CaCO3 +2 NaCL

      100 ml

      1 liter of I M solution of Na2CO3 contains 106 g

      How many grams of Na2CO3 in 1 liter of 0.5 M solution?

      1 M – 106 g

      0.5 M – X g

      X