Electronic configuration. Atomic number and mass number (nucleon number). Relative atomic mass based on C-12 isotope. Isotopy of elements

Subject : Chemistry

 

Topic :

1. Electronic configuration
2. Atomic number and mass number (nucleon number)
3. Relative atomic mass based on C-12 isotope
4. Isotopy of elements

Class :

SS 1

Term :

1st Term / First Term

Week :

Week 3

Instructional Materials :

• Lagos State Scheme of Work
• Textbooks On Social Studies
• Online Materials
• Picture Charts

 

 

Previous Knowledge :

The pupils have been taught

 PARTICULATE NATURE OF MATTER

in their previous lesson

 

Behavioural Objectives :  At the end of the lesson, the pupils should be able to

• Explain electronic configuration
• State atomic number and mass number (nucleon number)
• Describe relative atomic mass based on C-12 isotope
• Explain Isotopy of elements

Content

 

WEEK 3

TOPICS: PARTICULATE NATURE OF MATTER

CONTENTS:

1. Electronic configuration
2. Atomic number and mass number (nucleon number)
3. Relative atomic mass based on C-12 isotope
4. Isotopy of elements

PERIOD 1: ELECTRONIC CONFIGURATION

Electronic configuration

The electronic configuration of an atom is the distribution of electrons of an atom or molecule (or other physical structure) in atomic or molecular orbitals.

For example, the atomic number of sodium is 11. That means that every sodium atom has 11 electrons orbiting the nucleus.

The first shell can hold a maximum of 2 electrons, so the 2 electrons in a sodium atom occupy the first shell.

The second shell can hold a maximum of 8 electrons, so the remaining 9 electrons occupy the second shell.

This gives us the following electronic configuration for sodium: 1s2 2s2 2p6 3s1.

The shells are filled in order of increasing energy, so the lowest energy orbitals are filled first.

This is why the 1s orbital is filled before the 2s orbital, even though the 2s orbital has a lower energy than the 1s orbital.

The electronic configuration of an atom can be used to predict its chemical properties.

For example, elements in the same column of the periodic table tend to have similar chemical properties because they have the same number of valence electrons.

The number of valence electrons is equal to the number of electrons in the outermost shell.

In the case of sodium, the outermost shell is the 3s orbital, so it has one valence electron.

Other elements in the same column as sodium (such as lithium and potassium) also have one valence electron, so they tend to have similar chemical properties.

Electrons are found revolving around the nucleus of an atom in circular paths known as rings, orbits, energy levels or shells. Each shell contains electrons with similar energy.Those with the lowest energies being nearest to the nucleus.

3 (M shell)

2(L shell)

1 (K shell)

Thus, the arrangement of electrons in the atom according to energy is called ELECTRONIC CONFIGURATION. Letters and figures are associated with these orbits or shells as shown above. The maximum possible number of electrons that can be accommodated in a shell is given by the formula:

Nmax= 2n2. Where Nmax = Maximum no of electron. n= no, of shell.

Thus K- shell can contain 2 × 12 = 2 electrons.

1. Shell can contain 2 × 22 = 8 electrons.
2. Shell can contain 2 × 32= 18 electrons etc

The electron structures of the atoms of the first twenty elements are given in the table below.

Element	Symbol	Number    of protons(or atomic number)	Number    of distribution K    L	electrons in M	the	and    their shells. N
Hydrogen	H	1	1
Helium	He	2	2
Lithium	Li	3	2	1
Beryllium	Be	4	2	2
Boron	B	5	2	3
Carbon	C	6	2	4
Nitrogen	N	7	2	5
Oxygen	O	8	2	6
Fluorine	F	9	2	7
Neon	Ne	10	2	8
Sodium	Na	11	2	8	1
Magnesium	Mg	12	2	8	2
Aluminium	Al	13	2	8	3
Silicon	Si	14	2	8	4
Phosphorus	P	15	2	8	5
Sulphur	S	16	2	8	6
Chlorine	Cl	17	2	8	7
Argon	Ar	18	2	8	8
Potassium	K	19	2	8	8	1
Calcium	Ca	20	2	8	8	2

The electronic configurations of some elements are shown below:

Hydrogen, H (atomic number 1)

Electronk1

Nucleus

Helium, He(atomic number 2)

electrons    k2

Lithium, Li (atomic number 3).

K2 L1   

Neon, Ne (atomic number 10)

2,8

Sodium, Na (atomic number 11)

2, 8, 1

Argon, Ar (atomic number 18 )

    K L    M

    2    8    8

2,8,8

Potassium, K (atomic number 19)    K L M N

    2 8 8 1

Calcium, Ca (atomic number 20)

    K    L    M N

    2    8    8    2

2,8,8,2

EVALUATION: Draw the electronic configuration of the following elements.

    (a) Carbon    (b) Fluorine    (c) Aluminium    (d) Nitrogen

PERIOD 2:

ATOMIC NUMBER AND MASS NUMBER (NUCLEON NUMBER) ATOMIC NUMBER:

DEFINITION: Atomic number is the number of protons in an atom of an element.

The atomic number of an element is a whole number and is designated z. In a neutral atom the number of protons must be equal to the number of electrons(since protons are positively charged and electron are negatively charged).

All the atoms of a particular element have the same number of protons in their nuclei (i.e. they have the same atomic number). NO two elements have the same number of protons in their atoms.

 

ATOMIC NUMBER AND MASS NUMBER (NUCLEON NUMBER) ATOMIC NUMBER. The atomic number of an element is equal to the number of protons (positively charged particles) in the nucleus. The symbol Z is used to denote atomic number. The periodic table lists elements in order of increasing atomic number, from left to right and top to bottom. MASS NUMBER. The mass number (A) of an element is equal to the total number of protons and neutrons in the nucleus. The sum of the atomic number (Z) and mass number (A) is equal to the atomic mass, which is listed on the periodic table. The average atomic mass takes into account the natural abundance of each isotope. ISOTOPES. Isotopes are atoms of the same element with different atomic numbers. They have different numbers of neutrons in their nuclei, but the same number of protons. Most elements occur as more than one isotope. For example, carbon has two common isotopes: Carbon-12 (6 protons and 6 neutrons) and Carbon-14 (6 protons and 8 neutrons). The number following the element name is the mass number.

The atomic number of an element is equal to the number of protons in the nucleus. The symbol Z is used to denote atomic number. The periodic table lists elements in order of increasing atomic number, from left to right and top to bottom.

DEFINITION:

MASS NUMBER (NUCLEON NUMBER): The mass number is the sum of the protons and neutrons in an atom of an element.

Mass number is represented by the letter A.

Mass number A = Number of protons + number of neutrons.

i.e. A =p + n. Where p=protons, n= neutrons.

Or number of neutrons n =A – Z.

An atom of an element can be described by writing its symbol together with its atomic number and mass number.

Examples: The atom of carbon, oxygen and sodium can be written as 126C, 168O and2311Na respectively.

EVALUATION:

1. Define the following: (a) Atomic number    (b) Mass number.
2. Describe the atoms of the following elements using their symbol, atomic number and mass number: (a) Phosphorus (b) Silicon (c) Calcium

PERIODS 3 AND 4: ISOTOPY AND RELATIVE ATOMIC MASS

Definition: Isotopy is a phenomenon whereby atoms of an element exhibit different mass number but have the same atomic number.

Mass spectrometric studies show that the atoms of most elements exist in more than one form. This is due to the difference in number of neutrons present in these atoms. Such atoms are known as isotopes. Isotope of an element is represented by the original symbol of the element with the mass number and atomic numbers. For example 126C, 136C, 146C represent atoms of the isotopes of carbon. For each atom, the number of neutrons can be obtained by finding the difference between the mass number A and the atomic number Z i.e. A – Z. Each isotope of an element has its own mass known as isotopic mass.

Isotopes of an element have slightly different physical properties because neutrons contribute only to the mass of an atom and not its chemical behaviour. But isotopes of an element exhibit the same chemical properties because the number of valence electrons in an atom of an element determines its chemical behaviour (properties) and since isotopes have the same number of valence electrons they will be chemically alike.

NOTE:

1. An analysis of the chlorine isotopes.

    Isotope 3517Cl    Isotope 3717Cl

Mass number, A    35    37

Atomic number,Z    17    17

Number of protons    17    17

Number of electrons    17    17

Number of neutrons (A-Z)    35 – 17=18    37 – 17=20

Abundance in nature (%)    75    25

ISOTOPES OF THE SAME ELEMENTS.

Element	Carbon	Oxygen
ISOTOPES	12 C 136C 6	16 O 178O 188O 8
ABUNDANCE IN    NATURE (%)	98.9 1.1	99.76    0.04    0.20

1. The names of the isotopic forms of hydrogen

11H — Protium (or hydrogen)

21H— Deuterium (or heavy hydrogen or D)

31H— Tritium or T

1. The relative atomic mass, RAM of an element which exhibits isotopy is the average mass of its various isotopes as they occur naturally in any quantity of the element and they are not usually in whole numbers.

CALCULATION INVOLVING ISOTOPY.

WORKED EXAMPLE:

1. Determine the relative atomic mass of element X from the data below

    ISOTOPE    MASS    %ABUNDANCE

    24X    24    78.70

    25x    25    10.13

    26x    26    11.7

1. An element X has two isotopes of 2010X and 2210X in the ratio 1:3.

What is the relative atomic mass?

Add ratio of occurrence together.

1 + 3= 4

X = 21.5

1. Isotopes of an element X have isotopic masses 65 and 63 respectively. If the relative atomic mass of X is 63.60. Find the relative abundance of each isotope of the element.

Let the relative abundance of element X be y and Z respectively.

Z +Y =100

Z = 100 – y……. (i)

65y + 63z = 63.60 × 100

65y + 63z = 6360 ……(ii) 65y +63(100 – y) = 6360

65y – 63y + 6300 = 6360 2y = 60

1. = = 30

Y= 30

1. = 100 – y= 100 – 30 = 70

Y = 30, Z = 70

The relative abundance of X = 30% 0f 65X and 70% of 63X

EVALUATION:

(a) How many neutrons are present on the isotopes of 4119X (45%) and

4019x(55%)

(b)Calculate the relative atomic mass of X.

Questions

1. What is isotopy?

 

2. What are the three naturally occurring isotopes of carbon?

 

3. How do we determine the relative atomic mass of an element?

 

4. Why is carbon-12 used as the standard against which other isotopes are measured?

 

5. How do we calculate the average atomic mass of an element from its isotopic abundances?

RELATIVE ATOMIC MASSES BASED ON C-12 ISOTOPE

Definition: The Relative Atomic Mass of an element is the number of times the average mass of an atom of the element is heavier than one-twelfth of the mass of one atom of carbon -12

RAM of an element=

Thus the atom of carbon -12 is adopted as the standard for defining the relative atomic mass of the other elements and is given a basic mass value of 12units.

The relative atomic mass of each element has been determined accurately with the aid of the mass spectrometer. This instrument measures the masses of the isotopes of the elements and their abundance and the relative atomic mass is calculated from the data.

Relative atomic masses of the first twenty elements in the periodic

table

Element	Atomic number	Relative atomic mass
Hydrogen	1	1.008
Helium	2	4.0026
Lithium	3	6.939
Beryllium	4	9.0122
Boron	5	10.81
Carbon	6	12.011
Nitrogen	7	14.0067

20|Page

Oxygen	8	15.9994
Fluorine	9	18.9884
Neon	10	20.183
Sodium	11	22.9898
Magnesium	12	24.312
Aluminum	13	26.9812
Silicon	14	28.086
phosphorus	15	30.9738
Sulphur	16	32.06
Chlorine	17	35.453
Argon	18	39.948
Potassium	19	39.102
Calcium	20	40.08

The relative atomic masses of the first twenty elements in the periodic table are given in the table below.

Explain briefly why the chemical properties of isotopes of an element are similar.

 

 

 

Chemical properties of isotopes are similar because the number of protons in the nucleus is what determines an element, and isotopes have the same number of protons. The number of neutrons in the nucleus can vary, however, which gives isotopes different masses. The different number of neutrons does not affect chemical properties because they do not contribute to the nucleus’s charge. The electrons surround the nucleus, so they are most important in chemical reactions. Because isotopes have the same number of protons in their nuclei, they will have the same number of electrons and will thus exhibit similar chemical properties.

 

 

 

 

EVALUATION: From the complete periodic table of elements write out the relative atomic masses of (A) Magnesium (b) Oxygen (c) Chlorine (d) Carbon

GENERAL EVALAUATION

OBJECTIVES TEST :

1. The maximum number of electrons that can be accommodated in the Mshell is. (a) 18 (b) 8 (c) 2 (d) 32
2. The atomic number of chlorine is (a) 17 (b) 18 (c) 20 (d) 7
3. Which of the following is an isotope of hydrogen?

(a)41H (b) 51H (c) 31H (d) 01H

ESSAY QUESTIONS

(1) Chlorine exists in two isotopic mixtures. The first has 17protons and 18 neutrons while the second isotope has 17 protons and 20 neutrons. If the two isotopes are present in ratio 3:1 respectively, calculate the relative atomic mass of chlorine.

(2)Show the electron structure of the following.

(a) Calcium (b) Magnesium (c) Sodium (d) Oxygen

1. If the numbers of charged and unchanged particles in the centre of an atom are 6 and 7 respectively, what is the mass number of the atom?
2. Calculate the number of neutrons in

(a) 2311Na (b) 3717Cl

(5) (a)What is an ‘isotopy’?

(b) Explain briefly why the chemical properties of isotopes of an element are similar.

WEEKEND ASSIGNMENT: Read about the topic ‘’mass spectrometer’’

WEEK ACTIVITY:

(a) Draw a labelled structure of a mass spectrometer showing its basic features. (b) Write two features of a mass spectrometer.

ASSIGNMENT:

Read the topic ‘’symbols of elements’’ page 26 of New school Chemistry. By Osei Yaw Ababio.