2.20 Oxidization

By -
Oxidization 
Metals and metal oxides 



Example 

 Magnesium + copper oxide --> magnesium oxide + copper

Magnesium has been oxidized to magnesium oxide 
Copper has been reduced to copper

Copper oxide is the oxidizing agent
- it oxidizes but gets reduced in the process

Mg is the reducing agent
- it reduces the CuO to Cu but gets oxidized in the process

e.g. Ca + ZnO --> CaO + Zn

Comments

Post a Comment

Popular posts from this blog

1.33 calculate empirical and molecular formulae from experimental data

By Anonymous -
Calculating Molecular Formula 1 Write the element symbols S O 2  Write the masses or the % of the elements  3.2 g 6.4 g – 3.2 g = 3.2 g 3  Write the A r values of each element 32 16 4  Divide masses by At   3.2 ÷ 32 = 0.1 3.2 ÷ 16 = 0.2 5 Divide by the smallest number 0.1 ÷ 0.1 = 1 0.2 ÷ 0.1 = 2 6 Write the formula SO 2 Calculating Molecular Formula From the empirical formula, you can work out the molecular formula from the relative formula mass (M r ) of the compound. Add up the atomic masses of the atoms in the empirical formula. For example, the empirical formula of a hydrocarbon is CH 2 and its M r is 42. The mass of the atoms in the empirical formula is 14 42 ÷ 14 = 3 so you need to multiply the numbers in the empirical formula by 3 The molecular formula of the hydrocarbon is therefore C 3 H 6 .
Read more

1.27 know that the mole (mol) is the unit for the amount of a substance

By Anonymous -
A mole is that amount of substance that contains 6.02 x 10 23 atoms, molecules etc. This number is known as the Avogadro constant Molar masses A mole of an element will have a mass equal to its Ar but in grams A mole of a compound will have a mass equal to its Mr but in grams Moles tell you how many particles are present, and the ratio of moles tells you the ratio of particles that are represented by an equation.  You can find out how many moles are present by dividing the mass by the Mr: number of moles = mass ÷ Mr                                      
Read more

1.16 know what is meant by the terms atomic number, mass number, isotopes and relative atomic mass (Ar)

By Anonymous -
Atomic number - the number of protons in the nucleus of an atom, which determines the chemical properties of an element and its place in the periodic table. Mass number - the total number of protons and neutrons in a nucleus. The larger number shown on the periodic table.  Isotopes - each of two or more forms of the same element that contain equal numbers of protons but different numbers of neutrons in their nuclei, and hence differ in relative atomic mass. Relative atomic mass (Ar) - the mass of an atom of a chemical element expressed in atomic mass units. It is approximately equivalent to the number of protons and neutrons in the atom (the mass number). 
Read more