Chapter No. 4 (notes).docx

Chemistry Chapter no.4 Atomic Structure Notes What is an atom? An atom is the smallest component of an element having the chemical properties of the element.

Basic Structure of an atom:

     

An atom has a nucleus at the center containing neutrons and protons with one or more electrons circulating around the nucleus in electron shells or at different energy levels. Protons are positively charged. Neutrons have no charge. Electrons are negatively charged. The electrons are held by an electrostatic force of attraction by its negative charge and positive charge of protons. An atom is electrically neutral because the same proton number (positive charge) in the nucleus is balanced by the electron number (negative charge) in the shells.

How to identify atoms of different elements  Proton number also called atomic number.  The atomic number (proton number) determines the identity of an element.  Each element has different proton number and no two different elements have the same proton number.  For examples, hydrogen has one proton number, carbon has six proton number and chlorine has seventeen proton number (see image below).

Hydrogen has one (proton number) atomic number

Carbon has six (proton number) atomic number

Chlorine has 17 (proton number) atomic number



In the Periodic Table, the elements are arranged in order of increasing atomic number.

Periodic Table

Relative charges and approximate relative masses of protons, neutrons and electrons  used.

Since an atom is too light to be measured with a weighing scale, relative atomic mass (amu, symbol Ar ) is

 The relative atomic mass is the average mass of the atom of an element, relative to the mass of an atom of carbon-12. 

1 amu = 1/12 the mass of a carbon-12 atom The relative mass of a carbon-12 atom = 12 ( 6 protons + 6 neutrons ) The relative mass of a hydrogen atom = 1 ( 1 proton + 0 neutron ) Meaning, the average mass of a hydrogen atom is 1/12 of the mass of a carbon-12 atom. The relative mass of a magnesium atom = 24 (12 protons + 12 neutrons)



Meaning, the average mass of a magnesium atom is twice the mass of a carbon-12 atom. In fact, the relative mass of an atom are the total number of protons and neutrons in the nucleus.



Electrons are omitted because their mass is so tiny.

 A proton and a neutron weighted almost the same with a relative mass of 1 but an electron weights only 1/1837 of a proton.

Sub-atomic Particle Proton

Relative Mass

Relative Charge

Symbol

1 amu

+1

p

Neutron

1 amu

0

n

Electron

1/1837 amu

-1

e-

 Protons and neutrons are in the nucleus of the atom, so they are called nucleons. Nucleon number (mass number/ atomic mass) = protons + neutrons



The proton number and nucleon number of an element are often expressed in a short way as the following:

Example 1: A hydrogen element

An atomic structure of hydrogen element

Hydrogen element written on a short way

Example 2: A helium element

List of the atoms of the first 20 elements in the Periodic Table, arranged in order of increasing atomic number. Element

Symbol number

hydrogen helium lithium beryllium boron carbon nitrogen oxygen fluorine neon sodium magnesium aluminum silicon phosphorus sulphur chlorine argon potassium calcium

H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca

Atomic (Protons)

1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20

Electrons

1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20

Neutrons

0 2 4 5 6 6 7 8 10 10 12 12 14 14 16 16 18 22 20 20

Nucleon number (protons + neutrons) 1 4 7 9 11 12 14 16 19 20 23 24 27 28 31 32 35 40 39 40

Electron Configuration/ Electron Structure Electrons move very fast circulating the nucleus. Electrons can only occupy certain energy levels (shells) and cannot exist between different levels (shells) at the same time. Each energy levels (shells) can hold only up to a certain number of electrons.

Chlorine atom, electron configuration: 2,8,7 First shell, the closest to the nucleus, has the lowest energy level, holds up to 2 electrons. Second shell, has higher energy level, holds up to 8 electrons. Third shell can also holds up to 8 electrons. The further a shell is from the nucleus, the higher the energy level. Electron configuration means the arrangement of electrons in an atoms.

For any atom, the electrons fill the energy levels starting from the lowest energy (innermost shell). When the first shell is full with two electrons, the remaining electrons start filling the second energy level (second shell) up to a maximum of 8 electrons. Then, electrons continue filling the third energy level and so-on. As the picture shown above, chlorine atom contains 17 electrons. 2 of its electrons fill the first shell, then the next 8 electrons fill the second shell and the remainder seven electrons fill the third shell. The electron configuration for chlorine can be written as 2,8,7

Electron Configuration/ Electronic Structure (first 20 atoms)

Electron Configuration and the Periodic Table The horizontal raw defined as Period. Atoms of the same Period have the same number of shells.



All atoms of Period 1 have one shell

 All atoms of Period 2 has two shells and so-on. The vertical column defined as Group. Atoms of the same Group have the same number of valency electrons (the same number of electrons in the outermost shell or the last shell).  All atoms of Group 1 have one valency electron (one electron in the outermost shell or the last shell).  All atoms of Group 2 have two valency electrons (two electrons in the outermost shell or the last shell).

Define Isotopes 

Isotopes are atoms of the same element with the same proton number but different neutron number

or  The atoms of the same elements with different nucleon numbers or mass numbers due to different neutron number.

Isotopes of Hydrogen: Hydrogen Atomic Mass 1 1 proton, 0 neutron, 1 electron

Tritium, an isotope of Hydrogen Atomic Mass 2 1 proton, 1 neutron, 1 electron Deuterium, an isotope of Hydrogen Atomic Mass 3 1 proton, 2 neutrons, 1 electron

Isotopes of Carbon:

Isotopes: Identical Chemical Properties Isotopes of the same element have identical chemical properties. This is because isotopes of the same element have the same electron distribution. In other words, they have the same proton number and same number of electrons. There are two types of isotopes. 1. Stable isotopes 2. Unstable isotopes which is called radioisotopes 

Unstable isotopes due to extra neutrons in the nuclei which are radioactive.

 Examples: cobalt-60 used in radiotherapy treatment and uranium-235 used as a source of nuclear power.

Use of Radioisotopes in industry (Note: Not carbon dating) 1. 2. 3. 4. 5. 6.

Detection of leaks Monitor of thickness of paper production Nuclear fuel for generating electricity Radiographs of welds Measuring wear Sterilizing food (food preservation)

Use of Radioisotopes in Medical Practice 1. 2. 3. 4. 5. 6. 7.

Medical treatment of cancer Radiotherapy Treatment of thyroid gland X rays Tracer studies in body Sterilizing equipment Locating tumours