• Study Resource
• Explore

Survey

* Your assessment is very important for improving the work of artificial intelligence, which forms the content of this project

Document related concepts

History of molecular theory wikipedia, lookup

Unbinilium wikipedia, lookup

Ununennium wikipedia, lookup

Chemical element wikipedia, lookup

Valley of stability wikipedia, lookup

Isotope wikipedia, lookup

Transcript
```SYLLABUS
*Demonstrate an understanding of the terms atom, element, ion, molecule, compound, empirical and molecular
formulae
*Write balanced equations for simple reactions including the use of state symbols
*Demonstrate an understanding of the terms relative atomic mass, amount of substance, molar mass and parts
per million
*Calculate the amount of substance in a solution of known concentration
*Use chemical equations to calculate reacting masses
*Use chemical equations to calculate volumes of gases
*Use chemical equations to calculate volumes of gases and vice versa using the concepts of amount of substance
and molar volume of gases
*Use chemical equations and experimental results to deduce percentage yields
*Demonstrate an understanding of and be able to perform calculation using the Avogadro constant.
*Analyze and evaluate the results obtained from finding a formula of confirming an equation by experiment.
*Calculate the percentage yield of product.
*Carry out and interpret the results of simple test tube reactions, such as displacements, reactions of acids,
precipitations to relate the observations to state symbols used in equations and to practice writing full and ionic
equations.
PARTICLES AND STRUCTURE
The particles
The atomic model consists of protons and neutrons in the nucleus, and electrons in shells around the nucleus.
Particle
Mass
Charge
Acual/kg
Relative to proton
Actual/C
Relative to proton
-27
-19
Proton
1.6726 X 10
1
+ 1.6 X 10
+1
Neutron
1.6750 X 10-27
Just over 1
0
0
Electron
9.1095 X 10-31
1/1836
-1.6 X 10-19
-1
The nucleus
The protons and neutrons constitute the nucleus. As the number of protons increase, the number of neutrons
increase relatively faster, so small atoms have proton and neutron numbers which are comparable, whereas large
atoms have many more neutrons than protons. The ration of protons to neutrons is fairly critical, and any
departure from the optimum range will lead to nuclear instability and thus radioactivity.
Atom
………………………………………………………………………………………………………………………
………………………………………………………………………………………………………………………
…………………………………………………………………………..................................................................
Element
………………………………………………………………………………………………………………………
………………………………………………………………………………………………………………………
……………………………………………………………………………………………………………………...
1
Ihavandhoo school/A level note/ Formulae and equations ?
Atomic number
………………………………………………………………………………………………………………………
………………………………………………………………………………………………………………………
…………………………………………………………………………………………………………………….
Mass number
………………………………………………………………………………………………………………………
………………………………………………………………………………………………………………………
……………………………………………………………………………………………………………………..
Isotopes
………………………………………………………………………………………………………………………
………………………………………………………………………………………………………………………
…………………………………………………………………………………………….......................................
All atoms have isotopes. The word comes from the Greek for the same place because all the isotopes of a given
atom occupy the same place in the periodic Table defined by the atomic number. Isotopes arise because of
changes in neutron number
Compound
………………………………………………………………………………………………………………………
………………………………………………………………………………………………………………………
………………………………………………………………………………………………………………………
………………………………………………………………………………………………………………………
Molecule
………………………………………………………………………………………………………………………
………………………………………………………………………………………………………………………
………………………………………………………………………………………………………………………
………………………………………………………………………………………………………………...........
Relative atomic mass
The relative atomic mass, Ar, of an element is defined as the average mass of an atom of the element divided by
the mass of 1/12 of the mass of an atom of C-12.
Molecular mass
Relative molecular mass for a compound is the sum of all the relative atomic masses of the elements which
make up the compound`s formula.
Molar mass and moles
Molecular mass can be expressed in grams. This value is called 1mole.
2
Ihavandhoo school/A level note/ Formulae and equations ?
Number of particles present in one mole of a substance is called Avogadro constant or Avogadro number. It is
6.02 X 1023
Reacting masses
Amount of substance in moles = Mass of substance
Molar mass
Equations enable you to calculate how much material to use to get a desired amount of product, whatever the
scale.
Empirical formula
It represent ration of atoms present in a compound.
Empirical formula of hydrogen peroxide is HO.
Molecular formula
It represents number of atoms present in the compound.
Molecular formula of hydrogen peroxide is H2O2.
Calculation from the equations
Amount of the substance of unknown quantity can calculate from known quantity by relating the equations.
(Refer the problems)
Parts per million
Parts per million (PPM). Parts per million works like percent by mass, but is more convenient when there is
only a small amount of solute present. PPM is defined as the mass of the component in solution divided by the
total mass of the solution multiplied by 106 (one million):
Gas
xenon
ozone
nitrogen dioxide
Parts per million by volume
Volume
0.09 ppmv (9x10-6%)
0.0 to 0.07 ppmv (0%-7x10-6%)
0.02 ppmv (2x10-6%)
Greenhouse gases frequently express the concentration of fertilizers, in terms of parts per million
(ppm).
3
Ihavandhoo school/A level note/ Formulae and equations ?
Could you find out?
1. Write the ionic equations of the following reactions including state symbols.

AgNO3 + KCl →
AgCl + KNO3.
………………………………………………………………………………………………………….

NaOH + HCl →
NaCl + H2O.
………………………………………………………………………………………………………….

CaCl2 + 2NaOH →
Ca(OH)2 + 2NaCl
…………………………………………………………………………………………………………..
2. 0.00005% nitrous acid present in atmosphere. Find out presence of nitrous acid in parts per million.
…………………………………………………………………………………………………………….
…………………………………………………………………………………………………………....
……………………………………………………………………………………………………………
……………………………………………………………………………………………………………
3. A weighed piece of marble is reacted with hydrochloric acid, and is dried and reweighed when all
action has ceased. The mass loss was 2.33g; the volume of carbondioxide evolved was 550cm 3.
What is the percentage yield of the reaction?
CaCO3(s) + 2HCl (aq) →
CaCl2(aq) + CO2(g) + H2O(l)
………………………………………………………………………………………………………
………………………………………………………………………………………………………
………………………………………………………………………………………………………
………………………………………………………………………………………………………
………………………………………………………………………………………………………
………………………………………………………………………………………………………
………………………………………………………………………………………………………
………………………………………………………………………………………………………
4. Accuracy of the mass of the weighed substances was ±0.03g, find out the percentage error occurs
due to the using this balance.
……………………………………………………………………………………………………………
…………………………………………………………………………………………………
………………………………………………………………………………………………………
………………………………………………………………………………………………………
………………………………………………………………………………………………………
5. Name the following reactions.

BaCl2 + NaOH →
Ba(OH)2 + 2NaCl
………………………………………………………………………………………………………
2NaCl + ZnSO4 →
Na2SO4 + ZnCl2
………………………………………………………………………………………………………

4
Ihavandhoo school/A level note/ Formulae and equations ?
```
Related documents