CHEMY.4M2.4ATOMIC STRUCTURE

ATOMIC STRUCTURE

ATOM:

Is the smallest particle of an element that can take part in a chemical reaction.

Atoms as the smallest particles have ability to exist on its own.

Dalton was the first person to use the word ATOM.

DALTON ATOMIC THEORY

1. All matter are made up of tiny particles called ATOM.

2. Atoms can neither be created nor destroyed.

3. Atoms of a given element are identical. They have the same atomic mass and similar chemical properties

4. Atoms of one elements can combine with atoms of other elements to form molecules.

5. Atoms of given element are different from those of other elements.

MODIFICATION OF DALTON ATOMIC THEORY

1. Atoms are made up of smaller particles called electrons, protons and neutrons.

2. Atom can be created or destroyed or split up by nuclear reaction/ nuclear fission.

3. Some element have atom of more than one type. They are called Isotopes.

4. Atoms of different elements combine together to form complex compound.

SUB ATOMIC PARTICLES

• Atom are made up of 3 particles these are;

              i.        Proton

            ii.        Electron

           iii.        Neutron

• All atoms of an element have both 3 particles except hydrogen which has no Neutron.

A: THE ELECTRON

• This is a negatively charged particle (-ve)

• It's mass is about;1840

• It's symbol is 'e'

• It rotates around the nucleus in a particular patten called shell or energy level

B: THE PROTON

                      i.        This is a positively charged particles (+ve)

                    ii.        It has mass approximately the same as that of hydrogen atom ie atomic mass

                   iii.        It is symbol is (p) or +

                   iv.        It is found in the nucleus of an atom

C: THE NEUTRON

• This is a neutral particle or is a particle which has no charge

• This is a neutral particle or is a particle which has no charge

• The mass is the same as that of protons ie atomic mass unit

• It symbol is (n) ¹₀n

• It is found in the nucleus of an atom

ATOMIC STRUCTURE

Although an atom contain charge particles (protons) and electron is natural because the number of protons (+Ve) are equal to the number of electron (-Ve)

Although an atom contain charge particles (protons) and electron is natural because the number of protons +Ve) are equal to the number of electron (-Ve)

THE ARRANGEMENT OF ELECTRONS IN ATOM

ELECTRONIC CONFIGURATIONS

Is the distribution of electrons in various shell of an atom.

The maximum number of electrons held within each energy level. It can be determined by the formula 2nWhere n is the position of energy level from the nucleus.

      i.        The first shell from the nucleus of an atom have ability of carrying only 2 electron. =(2x12) = 2 electrons

    ii.        The second shell from the nucleus of an atom has ability of carrying only 8 electrons. =( 2x22) = 8 electrons

   iii.        The third shell from the nucleus of an atom have ability of carrying only 8 electronic. = (2x34) =18 electrons

   iv.        The forth shell from the nucleus carry a maximum of 18 electrons. = (2x42) = 32 electrons

NOTE;

But the third energy level is stable with 8 electrons

Arrangement of Energy Levels Around the Nucleus

Example of electron diagrams of an atom;

1. Hydrogen, 1=1

2. Aluminium, 13=2:8:3

3. Chlorine, 17 =2:8:7

4. Oxygen, 8= 2:6

ELECTRONS CONFIGURATIONS OF FIRST ELEMENT

NOTE

1. In the above the element are arranged according to the increase in atomic number

2. The number of proton = number of electron = Atomic number

3. The mass number (A) is the sum of proton (P) and neutron (N): (A=P+N)

ATOMIC NUMBER, MASS NUMBER AND ISOTOPES

       ATOMIC NUMBER (Z)

Is the number of proton in the nucleus of an atom which is equal to the number of electron in the shell.

      i.        It's official symbol is (Z).

    ii.        Atomic number is written on left hand side below the symbol of an element

Therefore atomic number of the following element are written as 6C, 801701, 20Ca

   iii.        Also atomic number = number of proton = number of electron

2. MASS NUMBER / ATOMIC MASS (A)

• It is written on left hand side above the symbol of an element.

.E.g. Carbon atomic mass is 12 written as ¹²C chlorine atomic mass is written as ³⁵Cl

• The official symbol for mass number is A.

• Combination of mass and atomic number are;

e.g.

Carbon ¹²₆C

Chlorine ³⁵₁₇Cl

Oxygen ¹⁶₈0

Therefore Atomic mass = Proton (atomic number)

Example:

Atom R has mass number of 40 and an atomic number of 20. What is it's neutron number, and what is the number of electrons in an atom R?

Solution :

 mass number = 40

atomic number = 20

 (a) Neutron number = mass number - atomic number

= 40 -20

 Neutron number =20

(b) Number of electrons = number of protons = atomic number = 20

ISOTOPES

These are atoms of the same element which have the same atomic number but they differ in mass number

      i.        Isotopes have the same proton electron and atomic number.

    ii.        They have same chemical properties but have slight different physical properties.

   iii.        Isotopes has different mass number because they have different number of neutrons.

Example of element which have the isotopes;

NOTE:

      i.        in the above four examples, the numbers above the element in the isotopes are the mass numbers.

    ii.        The numbers below the element are atomic numbers.

   iii.        From the definition of the isotopes, it is true that mass number are different and atomic number are the same

RELATIVE ATOMIC MASS (RAM)

• The relative atomic mass of an element is the mass of an atom of carbon twelve(12) Isotopes.

¹²₆C has no units

• If an element has several Isotopes its relative atomic mass will be the mass of Isotopes on calculation. The average mass of the proportion (abundance) of each Isotope in the sample of element must be known.

• This is calculated by working out the relative abundance of each isotope

CALCULATING RELATIVE ATOMIC NUMBER

Relative atomic mass (RAM) (Relative abundance x Atomic mass) + (Relative abundance x Atomic mass)

100

Example:

1. A sample of chlorine gas contains 75% and 25% of the Isotopes with it's relative abundance of 35 and 25 respectively. What is the relative atomic mass (R.A.M) of chlorine?

RAM =( Relative abundance x Atomic mass ) + ( Relative abundance x Atomic mass)

100

35cl of the Isotopes 37CL and 25% of the Isotopes.

To get the answer multiply the mass number of each Isotopes with the abundance.

To get the answer multiply the mass number of each Isotopes with the abundance.

Solution

Goox35)

+

600 x 37)

75 x 35 + 25 x 37

R.A.M of chlorine

= 35.5

• The relative atomic mass of chlorine is 35.5. The word symbol of relative atomic mass is (RAM).

2. A sample of chlorine is a mixture of two Isotopes in the ratio of 3:1. What is the relative atomic mass of chlorine atom?

Solution

R.A.M of chlorine= 35.5

3. A sample of Oxygen is mixture of 3 Isotopes in the ratio of 3:2:1. What is relative atomic mass (R.A.M).

Solution

R.A.M of Oxygen = 16.6

REVIEW QUESTION

1. Define the following

(1) Atomic

(11) Electronic configuration

(111) Atomic number

(iv) Mass number

(V) Isotope

2. Calculate the relative atomic mass of the chlorine of ³⁵₁₇Cl and ³⁷₁₇Cl  have the relative abidance of 75% and 25% respectively

3. Copy and complete the following table of atomic/ electron structure of same element.

a.

(b) Silver is an element which exists naturally and mixture of two isotopic form A and B representation of two isotopes occur in equal number.

A is ¹⁰⁷₄₇Ag , B is ¹⁰⁹₄₇Ag

In each case the upper figure is the mass number and the lower figure is the atomic number, state is the atomic number of

(a)  Proton in atom A

(b)  Electron in atomic B

(c)   (c) Neutrons in atomic A

(d)  (d) Electron in atomic B

(e)   (e) What is the relative atomic mass of naturally occurring silver?

4. Taking the symbol ¹⁶₈x to represent an atom of the element x, state

(a) The atomic number of x

(b) The number of neutron is an atom of x

(c) The number of element in an atom of x

(d) The mass of number of x

If another atom is represented as ¹⁸₈x, what form could be used to state its relation to ¹⁶₈x and what's the difference between them in term of the number and situation of particles present? If a sample of x contained 90% of ¹⁶₈x and 10% of ¹⁸₈x, show that the relative atomic mass of x would be 16.2