Summer break Task SSC-Section Class 9th

Respected parents as you know that students of 9th and 10th will appear in board examination so completion of

summer break task is compulsory. After summer break there will be monthly tests. 10 marks in each subject of home

work task will be added in the result of monthly test.

Sr.

#

Subject Home work task

1 Chemistry Solve the practice book of Unit # 01 and Unit # 02 (Attached to the home work )

2 Physics Prepare 50 MCQs from first two units ( Considering paragraphs , side boxes given in the book ,Values , Formulae , Unit etc) also solve exercise questions and problems of unit #1,2,3 on separate lose sheets

3 Math Note: Solve on narrow lined loose sheets.

Q#1:If A=

and B =

find a- 2A+ 3B b- 3A +2B c -4(A+B) d-

2/3(2A-B)

Q#2: Find X if X+

=

Q#3: If A=

B=

Check whether AB=BA or not also verify

a) = =

Q#4: Simplify

a)

.

÷ 5 b-

x

c-

x

Q#5: If q= +4 Find

a) q+ 1/q b) q-1/q c) + 1/ d) - 1/

Q#6: Find and xy if x+y = 4 and x-y = 2

Q#7: If x= 3+ find a) X+ 1/x b) + 1/

Q#8: Using log table find the value of

Q#8: Show that 7

+ 5

+

= log 2

Q#9: Given that A= if k=3 . what should be the value of d to make A= ?

Q#10: Rationalize the denominator

Q#11: If

find a) X +1/x b) + 1/ c) + 1/

Q#12: Make 50 multiple choice questions from chapter 1,2,3,4,10,11.

(Note: multiple choice questions must be different from the review exercise questions.

Make questions by reading articles given before exercises.)

Q#13: Write all the formulae.(All formulae of squares and cubes.)

4 Biology Solve the first two units of practice book

5 English Prepare objectives from the text book following the directions given below. Bench marks for the objectives from the text book (lesson 1-5)

MCQS from the text book=10from each lesson

Synonyms=5 from each lesson

Antonyms=5 from each lesson

Spellings= 5 from each lesson

Translation 0f 10 sentences daily from Grammar book(present ,past and future) Pg70- 98 pg 100-110

Practice of five voices daily from grammar and composition. Pg74=77, pg 80-83, pg 167-18

6 Urdu

7 Islamiyat

8 Pak.

Studies Fill in the blanks

1. Hindi Urdu Controversy in ----------- was held in 1867.

2. Quaid e Azam was a firm advocate of --------------- theory.

3. Chaudhry Rehmat Ali published a pamphlete named `` -----------------‘’.

4. Quaid e Azam addressed the officers of the government of Pakistan at Karachi on ---

5. On--------------- Quaid e Azam inaugurated the State Bank of Pakistan.

6. War of -------------- was fought in 1857.

7. The fifth pillar of Islam is---------------.

8. Fraternity teaches us to develop------------------- relations with one another.

9. Gandhi Jinnah talks were started in-------------1944.

10. C.R formula was expressed by------------.

11. Simla Conference was held in--------------.

12. Hindu leaders began to write the ``Lahore Resolution’’ as ``-----------Resolution’’.

13. In General Elections 1945-46 the muslim league won-------- seats out of 492 seats.

14. In 1946 Mr---------------- was the chief Minister of Bengal

15. In 1945----------- party came into power in Britain.

16. British Prime Minister------------- sent a Cabinet Mission in India.

17. Muslim League sent ---------------Ministers of Muslim League.

18. Muslim Provinces were included in Group-------------- in Cabinet Mission.

19. Congress------------ Cabinet Mission plan and celebrated.

20. Lord------------- convened an All parties conference.

Q:2 Give short answers of the following .

1. Who was Vasco da Gama?

2. Who were Hyder Ali and Tipu Sultan ?

3. Write a note on princely states in India .

4. Write names of Muslim Minister for Interim government in India .

5. What was the reaction of Congress and Muslim League to the Cabinet Mission plan ?

6. What was the manifesto of Muslim League in 1945-46 Elections?

7. Write the formation of provincial groups in Cabinet Mission Plan.

8. What was the reply of Quaid e Azam about Simla Conference ?

9. What proposals were made by Gandhi in Jinnah- Gandhi talks 1944?

10. What was the reply of Quaid e Azam on the Gandhi’s proposals?

Note : Date Sheet Monthly tests and chemistry practice work sheets are given below.

Date Sheet Monthly tests, SSC-Section July 2016

Time: 1 hour Total Marks: 50= (40 test + 10 summer break task)

Outline of test: Section A (6 Marks + Section B 24 Marks + Section C =10 Marks)

SSC-I SSC-II

Sr.

#

Date Subject Syllabus Subject Syllabus

1 Wednesday

July 20,

2016

Chemistry 9th

A & 9th

B : Unit # 1,2,3

9th

C : Unit # 1,2

Math Unit # 1, 2( till 2.5) + theorems

Unit # 9,10

2 Thursday

July 21,

2016

Urdu Lessons 1 till 3 + Letters

1 till 8

English Lessons 1 till 4

3 Monday

July 25,

2016

Math 9th

A & B Units : 1,2,3,4 +

theorems Unit # 10 ,11

9th

C : 1,2,3 + theorems Unit

# 11, 12

Biology Unit # 10 , 11, 13

4 Tuesday

July 26,

2016

English Lessons 1 till 4 + translation Pak.

Studies

Unit # 1& 2

5 Wednesday

July 27,

2016

Physics 9th

A & 9th

B : Unit # 2,3

9th

C : Unit # 2,3

Urdu Lesson 1,2 + Stories 1 till 6

6 Thursday

July 28,

2016

Pak.

Studies

Unit # 1& 2 T.Q Sura Al-Imran Till Verses 82

7 Monday

August 1st

2016

Biology Unit # 1 , 2, 6 Physics Unit # 10,11 ( till intensity of

sound )

8 Tuesday

August 2,

2016

Islamic

Studies

Sura Al-Anfal Raku # 1 till 4

+ Ahadith : first 4

Chemistry Unit # 11 , 12

Practice Book Unit # 01 Fundamentals of chemistry Chemistry 9th

Topic: 1.1 Branches of Chemistry

i- The methods and use of technology in the large scale production of useful substances is called_______

a- Inorganic chemistry b- Biochemistry c- Industrial chemistry d- Physical chemistry

ii- The branch of Chemistry that deals with the changes that occur in atomic nuclei is called ____________.

a- Inorganic chemistry b- Biochemistry c- Nuclear chemistry d- Physical chemistry

Topic: 1.1.1 Differentiation between branches of chemistry

i- Vinegar contains ______ % acetic acid.

a- 10% b- 20% c- 3% d- 5%

ii-Some carbon compounds such as CO2, CO, metal carbonates, hydrogen carbonates and carbides are studied in

________ chemistry.

a- Inorganic b- Organic c- Physical d- Environmental

iii- In _____ , the British chemist John Dalton presented a scientific theory on the existence and nature of matter.

a- 1803 b- 1815 c- 1823 d- 1903

iv- Water a molecular substance cover ___ % of the earth’s crust.

a- 20% b- 50% c- 70% d- 90%

Topic: 1.2 Basic Definitions

i- Any matter that has a particular set of characteristics that differ from the characteristics of another kind of matter

is called a _________ .

a- Compound b- Mixtures c- Substance d- Element

ii- A substance that cannot be converted to other simpler substances is called an _________.

a- Compound b- Mixtures c- Substance d- Element

iii-An impure substance that contains two or more pure substances that retain their individual chemical

characteristics is called a _________.

a- Compound b- Mixtures c- Substance d- Element

Topic: 1.2.2 Atomic Number and Mass Number

i- The number of protons in the nucleus of an atom is known as its _________.

a- Atomic number b- Mass number c- Molecular mass d- Formula mass

ii- The total number of protons and neutrons in an atom is known as its__________.

a- Atomic number b- Mass number c- Molecular mass d- Formula mass

Topic: 1.2.3 Relative Atomic Mass and Atomic Mass Unit

i- One atomic mass unit (amu) is defined as =

mass of one C-12 atom1amu=

12

A hydrogen atom is 8.40% as massive as the standard C-12 atom. Relative atomic mass of hydrogen will be:

a- 1.08amu b- 1.02amu c- 1.07amu d- 1.008amu

Topic: 1.2.4 Empirical Formula, Molecular Formula

i- The chemical formula that gives the simplest whole-number ratio of atoms of each element is called as

__________.

a- Atomic number b- Mass number c- Molecular Formula d- Empirical Formula

ii- The actual whole number ratio of atoms of each element present in a compound is called ___________.

a- Atomic number b- Mass number c- Molecular Formula d- Empirical Formula

iii- Following Which Compound have same Molecular as well as same Empirical Formula?

a- H2O b- NH3 c- SO2 d- All above

Topic: 1.2.5 Molecular Mass, Formula Mass

i- The sum of atomic masses of all the atoms present in the molecule is called as __________.

a- Atomic number b- Mass number c- Molecular Mass d- Empirical Mass

ii- The sum of the atomic masses of all the atoms in the formula unit of a substance is called ____________.

a- Atomic number b- Mass number c- Molecular Mass d- Formula Mass

Topic: 1.3 Chemical Species

i- An ______ is a charged species formed from an atom or chemically bonded groups of atoms by adding or removing

electrons.

a- Molecule b- Ion c- Atom d- Compound

Topic: 1.3.1. Ions, Molecular ions and Free Radicals

i- Positively charged ions are called _________. Whereas, the negatively charged ions are called _________.

a- Molecule, Ion b- Molecule, Compound c- Cation, Anion d- Anion, Cation.

ii- When a molecule loses or gains electrons, the resulting species is called a ________ ion.

a- Element b- Atomic c- Ionic d- Molecular

iii- An atom which has an unpaired electron and bears no electrical charge is called________.

a- Element b- Atomic c- Ion d- Free Radical.

Topic: 1.3.2 Representative Particles of Elements and Compounds

i- A molecule that contains only one atom is called_________. Whereas, molecules that contain two or more similar

or different atoms are called __________molecules.

a- Monoatomic, Diatomic b- Monoatomic, Triatomic

c- Monoatomic, Polyatomic d- None of these

Topic: 1.4 Avogadro’s Number and Mole

i- A mole is an amount of a substance that contains _________ particles of that substance.

a- 6.022 x 1010 b- 6.022 x 1012 c- 6.022 x 1023 d- 6.022 x 1043

ii- Mole is experimentally determined number which is also known as Avogadro’s number and it representated as:

a- AN b- Na c- NA d- aN

Topic: 1.5 Chemical Calculations

1.5.1 (Molar Mass Calculations)

i- The molar mass of Sucrose (C12H22O11) is _________.

a- 342g b- 330g c- 325g d- 320g

ii- The mass of 9.05 moles of ozone (O3) is ________.

a- 433g b- 433.34g c- 434.4g d- 420g

iii- How many number of moles are present in 5g of hydrogen filled in ballon?

a- 1.08 moles b- 1.008 moles c- 2.08 moles d- 2.008 moles

Topic: 1.5.2 (Mole Particles Calculations)

i- 0.2 moles of Aluminium contains how many number of atoms?

a- 1.2044x1023 b- 1.2033x1024 c- 0.2244x1023 d- 2.005x1023

ii- 1 Mole of CH4 contains __________ molecules.

a- 3.111x1023 b- 3.011x1024 c- 3.011x1023 d- 3.112x1022

iii- __________ number of moles that would contain 3.011 x 1022 molecules of Formaldehyde compound.

a- 0.09 moles b- 0.05 moles c- 0.06 moles d- 0.08 moles

Short questions

Topic: 1.1 Branches of Chemistry

i- Identify the branch of chemistry in each of the following examples:

a- Haber’s process converts large quantities of hydrogen and nitrogen into ammonia (NH3)._____________________

b- Chlorofluorocarbon compounds are responsible for the depletion of ozone layer. ___________________________

c- α-particles (He++) when bombard on nitrogen atom, a proton is emitted. __________________________________

d- Calorimeter is a device that measures the amount of heat, a substance absorbs on heating or emits on cooling.

_________________________________________________________________________.

iv- Identify the branch of chemistry that deals with the following examples: _________________________________

v- A cornstalk grows from a seed. _______________________________

vi- Dynamite (C3H5N3O9) explodes to form a mixture of gases. _______________________

vii- Purple iodine vapour appears when solid iodine is warmed. ____________________________.

viii- Gasoline ( a mixture of hydrocarbons) fumes are ignited in an auto mobile engine. __________________.

ix-A silver article tarnishes in air. ___________________________x- Ice floats on water. ______________________

xi- Sulphur dioxide is the major source of acid rain. _______________________.

xii-Many other light chlorinated hydrocarbons in drinking water are carcinogens. _________________________.

Xiii -In Pakistan most of the factories use wet process for the production of cement. ___________________________

Carbon-14 is continuously produced in the atmosphere when high energy neutrons from space collide with nitrogen-

14. _____________________________.

Topic: 1.2 Basic Definitions

Define:

ion,

_______________________________________________________________________________________________

molecular ion,

_______________________________________________________________________________________________

formula unit,

_______________________________________________________________________________________________

free radical,

_______________________________________________________________________________________________

atomic number,

_______________________________________________________________________________________________

mass number,

_______________________________________________________________________________________________

atomic mass unit,

_______________________________________________________________________________________________

Empirical and molecular formula mass

_______________________________________________________________________________________________

_______________________________________________________________________________________________

_______________________________________________________________________________________________

Topic: 1.3 Chemical Calculations

i- What are the molar masses of uranium -238 and uranium -235?

_______________________________________________________________________________________________

_______________________________________________________________________________________________

ii- Why one mole of hydrogen molecules and one mole of H-atoms have different masses?

_______________________________________________________________________________________________

_______________________________________________________________________________________________

_______________________________________________________________________________________________

iii- Write the empirical formulas for the compound containing carbon to hydrogen in the following ratios:

(a) 1:4 ________________________________ (b) 2:6 _____________________________

(c) 2:2 ________________________________ (d) 6:6 _____________________________

iv- Aspirin is used as a mild pain killer. There are nine carbon atoms, eight hydrogen atoms and four oxygen atoms,

in this compound. Write its empirical and molecular formulas.

_______________________________________________________________________________________________

_______________________________________________________________________________________________

_______________________________________________________________________________________________

v- Vinegar is 5% acetic acid. This contains 2 carbon atoms, four hydrogen atoms and 2 oxygen atoms. Write its

empirical and molecular formulas.

_______________________________________________________________________________________________

_______________________________________________________________________________________________

_______________________________________________________________________________________________

vi- Caffeine (C8H10N4O2) is found in tea and coffee. Write the empirical formula for caffeine.

_______________________________________________________________________________________________

_______________________________________________________________________________________________

vii- Potassium Chlorate (KClO3) is used commonly for the laboratory preparation of oxygen gas. Calculate its formula

mass.

_______________________________________________________________________________________________

_______________________________________________________________________________________________

viii- When baking soda, NaHCO3 is heated it releases carbon dioxide, which is responsible for the rising of cookies

and bread. Determine the formula masses of baking soda and carbon dioxide.

_______________________________________________________________________________________________

_______________________________________________________________________________________________

ix- Following compounds are used as fertilizers. Determine their formula masses.

Urea, (NH2)2CO

_______________________________________________________________________________________________

Ammonium nitrate, NH4NO3.

_______________________________________________________________________________________________

x- TNT or trinitrotoluene is an explosive compound used in bombs. It contains 7 C-atoms, 6 H-atoms, 5 N-

atoms and 6 O-atoms. Write its empirical formula.

_______________________________________________________________________________________________

_______________________________________________________________________________________________

_______________________________________________________________________________________________

xi- A molecule contains four phosphorus atoms and ten oxygen atoms. Write the empirical formula of this

compound. Also determine the molar mass of this molecule.

_______________________________________________________________________________________________

_______________________________________________________________________________________________

_______________________________________________________________________________________________

xii- Indigo(C16H10N2O2), the dye used to colour blue jeans is derived from a compound known as indoxyl

(C8H7ON). Calculate the molar masses of these compounds. Also write their empirical formulas.

_______________________________________________________________________________________________

_______________________________________________________________________________________________

_______________________________________________________________________________________________

xiii- Explain Why?

An oxide ion has –2 charge.

_______________________________________________________________________________________________

_______________________________________________________________________________________________

_______________________________________________________________________________________________

Magnesium ion, Mg+2has +2 charge.

_______________________________________________________________________________________________

_______________________________________________________________________________________________

_______________________________________________________________________________________________

Sulphide ion, S-2has–2 charge.

_______________________________________________________________________________________________

_______________________________________________________________________________________________

_______________________________________________________________________________________________

xiv- Identify ions, molecular ions and free radicals from the following species.

_______________________________________________________________________________________________

_______________________________________________________________________________________________

_______________________________________________________________________________________________

_______________________________________________________________________________________________

xv- Calculate the number of moles of each substance in samples with the following masses:

.4 g of He

250mg of carbon

15g of sodium chloride

40g of sulphur

1.5kg of MgO

xvi- Calculate the mass in grams of each of the following samples:

1.2 moles of K

75moles of H2

0.25 moles of steam

1.05 moles of

CuSO4.5H2O

0.15moles of H2SO4

i- Calculate the number of molecules present in each of the following samples:

2.5 moles of carbon

dioxide

3.4 moles of ammonia,

NH3

1.09 moles of benzene,

C6H6

0.01 moles of acetic acid,

CH3COOH

ii- Calculate the mass of following:

3.24 x 1018 atoms of iron

2 x 1010 molecules of

nitrogen gas

1 x 1025 molecules of

water

3 x 106 atoms of Al

xix- Calculate the number of atoms in each of the following samples:

3.4 moles of nitrogen

atoms

3.4 moles of nitrogen

atoms

23g of Na

5g of H atoms

xx- Calculate the mass of one mole of:

(a) Copper

_______________________________________________________________________________________________

(b)

Iodine_________________________________________________________________________________________

(c) Potassium

_______________________________________________________________________________________________

(d) Oxygen

_______________________________________________________________________________________________

xxi- The molecular formula of a compound used for bleaching hair is H2O2. Calculate (a) Mass of this compound that

would contain 2.5 moles. (b) No. of moles of this compound that would exactly weigh 30g.

xxii- A spoon of table salt, NaCl contains 12.5grams of this salt. Calculate the number of moles it contains.

xxiii- Before the digestive systems X-rayed, people are required to swallow suspensions of barium sulphate (BaSO4).

Calculate mass of one mole of BaSO4.

xxiv- Aspirin is a compound that contains carbon, hydrogen and oxygen. It is used as a painkiller. An aspirin tablet

contains 1.25 x 1030molecules. How many moles of this compound are present in the tablet?

xxv- A method used to prevent rusting in ships and underground pipelines involves connecting the iron to a block of

a more active metal such as magnesium. This method is called cathodic protection. How many moles of magnesium

are present in 1 billion (1 x 109) atoms of magnesium.

xxvi- What mass of sodium metal contains the same number of atoms as 12.00g of carbon.

xxvii- What mass of oxygen contains the same number of molecules as 42g of nitrogen.

xxviii- Calculate the mass of one hydrogen atom in grams.

1. xxix- Observe the given figure and identify the diagrams that represents the particles of :

a) An element whose particles are atoms.

b) An element whose particles are molecules.

c) A compound.

d) A mixture of an element and a compound.

e) A mixture of two elements.

f) A mixture of two compounds.

2-Observe the given figure and decide which diagram represents particles in an element, a compound or a mixture.

Practice Book Unit # 02 Structures of Atoms Chemistry 9th

Practice Book Unit # 02 Structures of Atoms Chemistry 9th

Topic: 2.1 Theories and experiments related to atomic structure

i- The distribution of electrons in shells (KLM only) using ____ formula.

a- 2n1 b- 2n2 c- 2n3 d- 2n4

Topic: 2.1.1 Rutherford’s atomic model

ii- In ______ Rutherford performed an experiment in order to know the arrangement of electrons and protons in

atoms.

a- 1911 b- 1912 c- 1915 d- 1920

Topic: 2.1.2 Rutherford’s experiment

iii- Rutherford bombarded a very thin gold foil about ________cm thickness with α-particles.

a- 0.0001cm b- 0.0002cm c- 0.0003cm d- 0.0004cm

iv- The distribution of electrons in shells (KLM only) using ____ formula.

a- 2n1 b- 2n2 c- 2n3 d- 2n4

v- The distribution of electrons in shells (KLM only) using ____ formula.

a- 2n1 b- 2n2 c- 2n3 d- 2n4

vi- The distribution of electrons in shells (KLM only) using ____ formula.

a- 2n1 b- 2n2 c- 2n3 d- 2n4

Topic: 2.1.1 Rutherford’s atomic model

i- In ______ Rutherford performed an experiment in order to know the arrangement of electrons and protons in

atoms.

a- 1911 b- 1912 c- 1915 d- 1920

Topic: 2.1.2 Rutherford’s experiment

i- Rutherford bombarded a very thin gold foil about ________cm thickness with α-particles.

a- 0.0001cm b- 0.0002cm c- 0.0003cm d- 0.0004cm

ii- In this experiment only _______ million particles was deflected through an angle greater than 90o from their

straight paths.

a- 0.001 million b- 0.1 million c- 01 million d- None of these

iii- The mass of an atom is concentrated in a very small dense positively charged region called ___________.

a- Electron b- Proton c- Nucleus d- All of these

iv- The __________ force due to the revolution of electrons balances the electrostatic force of attraction between

the nucleus and electron.

a- Centripetal b- Centrifugal c- Both a and b d- None of these

Topic: 2.1.1.2 Defects in Rutherford’s atomic model

i- If revolving electron emits energy continuously it should form a ________ spectrum for an atom but a ______

spectrum is obtained.

a- Line, Continious b- Line, Line c- Continious, Continious d- Continious, Line

Topic: 2.1.2 Bohr’s Atomic theory

i- In ______ Neil Bohr proposed a model for an atom that was consistent with Rutherford’s model.

a- 1910 b- 1912 c- 1913 d- 1914

ii- The electron revolves only in those orbits for which the angular momentum of the electron is an integral multiple

of:

a- 2π/h b- 4π/2h c- π/2h d- h/2π

iii- The value of Plank’s Constant is:

a- 6.022x1023J.s b- 6.02x1012J.s c- 6.626x10-34J.s d- None of these

Topic: 2.2 Isotopes

iv- _________ are atoms of an element whose nuclei have the same atomic number but different mass number.

a- Chemical Specie b- Molecular specie c- Isotopes d- None of these

v- In isotope of hydrogen __________ has 1 neutron and 1 proton.

a- Protium b- deuterium c- Tritium d- None of these

vi- Carbon has ________ isotopes.

a- 1 b- 2 c- 3 d- 4

vii- An atom of chlorine–37 has ____ protons and _____ neutrons.

a- 17 protons and 20 neutrons b- 18 protons and 20 neutrons

c- 17 protons and 18 neutrons d- 18 protons and 18 neutrons

viii- The ________isotope of uranium is used in nuclear reactors and atomic bombs.

a- 92U233 b- 92U

234 c- 92 U235 d- 92U

236

ix- The ________ of uranium–235 yields smaller nuclei, neutron and energy.

a- Fusion b- Fission c- Both a and b d- none of these

Topic: 2.2.2 Uses of isotopes

i- Radioactive iodine ______ is used as a tracer in diagnosing thyroid problem.

a- 130 b- 131 c- 132 d- all of these

ii- ______-24 is used to trace the flow of blood and detect possible constrictions or obstructions in the circulatory

system.

a- Sodium (Na) b- Magnesium (Mg) c- Chlorine (Cl) d- Hydrogen (H)

iii- Iodine_______is used to image the brain and Cobalt _____ is commonly used to irradiate cancer cells in the

hope of killing or shrinking the tumors.

a- I- 123 and Co- 60 b- I-124 and Co- 62

c- I- 125 and Co- 63 b- I-123 and Co- 64

iv- ________35 has been used in the structure determination of thiosulphate.

a- Sulphur b- Phosphorous c- Calcium d- Nitrogen

Topic: 2.3 Electronic Configuration 2.3.1 Shells

i- According to _______ atomic theory, the electron in an atom revolves around the nucleus in one of the

circular

ii- paths called shells or orbits.

iii- a- Rutherford’s b- Bohr’s c- Mandeleev d- All of these

iv- 2.3.2 Sub- shells

v- i- The arrangement of electrons in ________ is called as the electronic configuration.

vi- a- Shells b- sub- shells c- Both a and b d- None of these

vii- ii- According to _____ principle, electrons fill the lowest energy sub-shell that is available first.

viii- a- Bohr’s b- Rutherford’s c- Auf-Bau d- None of These

ix- iii- Filling of electrons in the lowest energy sub-shell, the sequence like;

x- a- 1s,2s,3s,--------- b- 2s,3s,---------- c- 1s,3s,2s,--------- d- 1s,2s,4s----------

xi- 2.3.3 Electronic configuration of First 18 elements.

xii- i- Electronic configuration is the distribution of ______ among the different sub-shells of an atom.

xiii- a- Atoms b- Ions c- Molecules d- Electrons

xiv- ii- Maximum how many electrons can accommodate in ‘f’sub- shell?

xv- a- 2 b- 8 c- 10 d- 14

xvi- iii- Valance shell electronic configuration of Neon (10Ne) is;

a- 1s2,2s2,2p5 b- 1s2,2s2,2p6 c- 1s2,2s2,2p8 d- 1s2,2s2,2p4

Topic: 2.1.1 Rutherford’s atomic model (topic 2.1.1, 2.1.2 solve on separate sheets )

i- Describe the contribution that Rutherford made to the development of the atomic theory.

Topic: 2.1.2 Bohr’s Atomic theory

i- Explain how Bohr’s atomic theory differed from Rutherford’s atomic theory.

ii- Draw Bohr’s Model for the following atoms indicating the location for electrons, protons and neutrons.

a- Carbon (Atomic No. 6, Mass No. 12) b- Chlorine (Atomic No. 17, Mass No. 35)

c. Potassium (Atomic No 19, Mass No. 39) d-Silicon (Atomic No. 14 Mass No. 28 )

e- Argon (Atomic No. 18 Mass No. 39)

iii- State the importance and uses of isotopes in various fields of life.

Topic: 2.2 Isotopes

i- Chlorine is a reactive element used to disinfect swimming pools. It is made up of two isotopes Cl-35 and Cl-37.

Because Cl-35 is more than Cl-37, the atomic mass of chlorine is 35.5amu. is closer to 35 than 37. Write electronic

configuration of each isotope of chlorine. Also write symbol for these isotopes (atomic number for chlorine is 17).

_______________________________________________________________________________________________

_______________________________________________________________________________________________

ii- The atomic number of an element is 23 and its mass number is 56.

a- How many protons and electrons does an atom of this element have?

_______________________________________________________________________________________________

_______________________________________________________________________________________________

_______________________________________________________________________________________________

b- How many neutrons does this atom have?

_______________________________________________________________________________________________

_______________________________________________________________________________________________

_______________________________________________________________________________________________

iv- M-24 is a radioactive isotope used to diagnose restricted blood circulation, for example in legs. How many

electrons, protons and neutrons are there in this isotope? Valence shell electronic configuration of M is 3s1.

_______________________________________________________________________________________________

_______________________________________________________________________________________________

_______________________________________________________________________________________________

_______________________________________________________________________________________________

v- Two isotopes of chlorine are 35

17 Cland

37

17 Cl. How do these isotopes differ? How are they alike?

_______________________________________________________________________________________________

_______________________________________________________________________________________________

_______________________________________________________________________________________________

_______________________________________________________________________________________________

_______________________________________________________________________________________________

Topic: 2.3 Electronic Shells

i- How many sub-shells are there in N shell?

_______________________________________________________________________________________________

ii- Give notation for sub-shells of M shell.

_______________________________________________________________________________________________

iii- List the sub-shells of M Shell in order of increasing energy

_______________________________________________________________________________________________

_______________________________________________________________________________________________

_______________________________________________________________________________________________

vi- The table shows the nuclei of five different atoms.

Name of atom Number of Protons Number of neutrons

A 5 6

B 6 6

C 6 7

D 7 7

E 8 8

a. Which atom has highest mass number? ____________________________________.

b. Which two atoms are isotopes? ______________________________________.

c. Which atom has least number of electrons? ______________________________________.

d. Which atom will have electronic configuration 1s22s22p3. ______________________________.

e. Which of the atom contains the most number of electrons? _____________________________.

vii- Naturally occurring nitrogen has two isotopes N-14 and N-15 which isotope has greater number of electrons.

_______________________________________________________________________________________________

_______________________________________________________________________________________________

v- Write the complete electronic configuration for the following elements;

Al (atomic number 13)

_______________________________________________________________________________.

Si (atomic number 14)

________________________________________________________________________________.

P (atomic number 15)

________________________________________________________________________________.

S (atomic number 16)

________________________________________________________________________________.

Cl (atomic number 17)

_______________________________________________________________________________.

Ar (atomic number 18)

_______________________________________________________________________________.

vi- Write the electronic configuration for the following isotopes

(a) 14

6 C

_________________________________________________________________________________.

(b) 35

17 Cl

_______________________________________________________________________________.

(c) 37

17 Cl

________________________________________________________________________________.