أهم 100 سؤال فى مراجعة مادة كيمياء لغات الجزء الثانى الصف الثالث ثانوي

من طرف **حنين الصمت** الأربعاء 17 أبريل 2013, 7:32 am

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أهم 100 سؤال فى مادة كيمياء لغات - الجزء الثانى

Definitions

1. Element

2. Quantum energy

3. Electron cloud

4. Aufbau (building-up) principle

5. Hund's rule

6. Cathode rays

7. Line spectra

8. Dual nature of the electron

9. Heisenberg uncertainty principle

10. Bond length

11. Atomic radius

12. Ionization energy

13. Electron affinity

14. Electronegativity

15. Acidic oxide

16. Basic oxides

17. Amphoteric oxides

18. Oxidation number

19. Oxidation

20. Reduction

21. Chemical reaction

22. Ionic bond

23. Covalent bond

24. Pure covalent bond

25. Polar covalent bond

26. Octet rule

27. Valence Bond Theory

28. Hybridization

29. Molecular Orbital Theory

30. Coordinate Bond

31. Hydrogen Bond

32. Metallic Bond

33. Photo electric phenomenon

34. Allotropy

35. Passivity

36. Transition element

37. Paramagnetic properties

38. Diamagnetic properties

39. Magnetic moment

40. Sintering process

41. Roasting of iron ore

42. Alloy

Answers

1- A pure simple substance that cannot be changed to simpler forms by the traditional chemical methods

2- The amount of energy absorbed or emitted when the electron jumps from one energy level to another

3- A region of space around the nucleus where the electron most probable exists

4- Electrons occupy the sublevels in the order of increasing their energy æ the lowest energy sublevels are filled first.

5- No electron pairing takes place in a given sublevel until each orbital contains one electron"

6- A stream of invisible rays is emitted from the cathode through
a discharge tube with low pressure(0.01-0.001 mmHg) and high potential
difference(10000 volts)

7- A limited number of colourless lines result from radiation of gases or vapour under reduced pressure and high temperature.

8- The electron is a particle an also has wave motion

9- The determination of both the velocity and the position of an electron at the same time are practically impossible.

10- The distance between the nuclei of two bonded atoms

11- Half the distance between the nuclei of two similar bonded atoms

12- Amount of energy needed to remove the most loosely bound electron from isolated gaseous atom

13- Amount of energy released when an extra electron is added to neutral gaseous atom

14- The tendency of the atom to attract the electron of the chemical bond to itself

15- Nonmetal oxide dissolves in water forming acid and reacts with base gives salt and water

16- Metal oxides dissolve in water forming alkalis and react with acids giving salt and water

17- Oxides react with acids or bases giving salt and water

18- The number of charges(+ve or –ve) the atom would have in a compound

19- The process of losing electrons leads to increase oxidation number

20- The process of gaining electrons leads to decrease oxidation number

21- Bonds are broken in reactants and new bonds are formed in products

22- Attraction force between +ve cation and –ve anion to form neutral compound

23- Sharing by one pair of electrons or more between two atoms

24- Sharing by one pair of electrons or more between two atoms similar in electronegativity

25- Sharing by one pair of electrons or more between two atoms different in electronegativity

26- By the exception of H2, Li and Be atoms of all elements tend to reach octet structure

27- It explains covalent bond as overlapping two orbitals from the two atoms each orbital has single electron

28- Overlap two or more orbitals close in energy to form hybrid orbitals similar in energy

29- All the atomic orbitals of combined atoms are mixed forming molecular orbitals

30- A type of covalent bond where a donor atom has lone pair of electrons donates it to acceptor atom has a vacant orbital

31- Hydrogen acts as a bridge between two atoms of high electronegativity so it binds the two molecules together

32- The valence electrons of a metal forming electron cloud which decrease the repulsion between the +ve ions of the metal

33- Some atoms such as K and Cs when they are exposed to light their free electrons move forming electric current

34- Presence of an element in more than one form different in physical properties but similar in chemical ones

35- Formation of non porous layer of oxide surround the metal and stop further reaction

36- The element which found incompletely filled sublevels (d) or (f) in one of its state.

37- Attraction to the outer magnetic field due to presence of unpaired electron in(d)or(f)sublevel

38- Repulsion to the outer magnetic field due to absence of unpaired electron in(d)or(f)sublevel

39- Number of unpaired electrons in (d) or (f) sublevel

40- Treatment fine particles and powder into big particle

41- Strongly heating iron ore in the air.

42- Mixing two or more elements to get certain properties

Give reasons

36. of atmosphere.

37. Coinage metals are transition elements while group 2B are not

38. Iron reacts with dil. acids gives iron(II) salts not iron(III) salts

39. Transition elements have catalytic effects

40. Reducing gases in midrex furnace have a closed cycle

41. Hydrated cobalt (II) chloride is used in secret ink

42. Anhydrous cobalt (II) chloride is used in chimatic prediction

43. Iron (II) is easily oxidized while Manganese (II) is difficult to be oxidized

44. Transition elements have variable oxidation states

45. Titanium is preferred than aluminum in making rockets

46. Oxygen converted is lined with dolomite

Answers

1. Coinage metals are not completely filled sublevel d in one of
their compound while 2B elements are completely filled sublevel d in
all states

2. The evolved hydrogen is reducing agent

3. Due to the presences of unpaired electrons in d sublevel

4. The result gases CO2+H2O react with methan to form reducing gases inter the furnace

5. Dilute solution has pale pink can't seen by written and turns dark blue by heating

CoCl2 .6H2O CoCl2 + 6H2O

Pale pink dark blue

6. It has dark blue turns pale pink when it absorbs hymidity

CoCl2 + 6H2O CoCl2 .6H2O

dark blue Pale pink

7. It gives Iron (III) half filled more stable while Mn2+ half filled more stable

8. They lose electrons from 4s the 3d as they are close in energy

9. It keeps hardness at high temperature

10. Dolomite reacts with basic and acidic oxide forming slag

Compare between

1- Four quantum numbers

2- Electron affinity and electronegativity

3- Covalent bond and hydrogen bond

4- Sigma bond and pi bond

5- Blast furnace – Midrex furnace and oxygen converter

6- Three types of alloys

Comparison

1

Principle q.no. Subsidiary q.no. Magnetic q.no. Spin q.no.

Indicates principle energy level Indicates sublevel in principle
energy level Indicates no. shape of orbitals in sublevels Indicates spin
motion of electron around its axis

Its symbol n Its symbol l Its symbol m Its symbol ms

Bohr Sommerfield

K,L,M,N,O,P,Q s

2

Electron affinity Elctronegativity

Energy released when gaining electron Attraction of electron of the bond

In single atom In combine atom

Its unit joule or calorie Unitless number

3

Covalent bond Hydrogen bond

Occurs between two nonmetals Occurs between two molecules

Strong Weak

Short Long

4

Sigma bond Pi bond

Overlapping head by head Overlapping side by side

Collinear Collateral

Strong Weak

5

Comparison Blast furnace Midrex furnace Oxygen converter

Charge Ore+coke + lime stone Ore + methane Molten pig iron

Reducing agent CO CO + H2 Impurities

Oxidizing agent Ore Ore Oxygen

Result Pig iron Spongy iron Steel

6

Interstitial Substitution Intermetallic

Mixture of two or more different elements without chemical bonds
Some atoms are replaced by atoms similar in crystal form,diameteror
chemical properties Mixture of two or more different elements with
chemical bonds

the introduced atoms are larger or smaller They are solids They have chemical bond, out of valence rule.

This change their properties Such as : Copper and gold

Iron and nickel Such as : cementite

Fe3C

Equations

How can you prepare:

1- Fr

2- Na2CO3

3- Ammonia

4- Nitric acid

5- Iron in medrix furnace

Answer

1- Ac Fr + He

2- NH3 + CO2 + NaCl + H2O NaHCO3 + NH4Cl

2NaHCO3 Δ Na2CO3 + H2O + CO2

3- 2NH4Cl + Ca(OH)2 Δ CaCl2 + 2H2O + 2NH3

4- 2KNO3 + H2SO4 Δ K2SO4 + 2HNO3

5- 2Fe2O3 + 3CO + 3H2 4Fe + 3CO2 + 3H2O

What is the effect of oxygen on?

1-Lithium

2-sodium

3-potassium

4-iron

Answer

1- 4Li + O2 Δ 2Li2O

2- 2Na + O2 Δ Na2O2

3- K + O2 Δ KO2

4- 3Fe + 2O2 Δ Fe3O4

From iron,How can you get tree oxides of iron?

Answer

Fe + + 4H2O Δ Fe3O4 + 4H2

2FeO + [O] Δ Fe2O3

Fe2O3 + H2 Δ 2FeO + H2O

Fe3O4 + H2 Δ 3FeO + H2O

What is the effect of heat on?

1- Lithium carbonate

2- IironII carbonate

3- Calcium carbonate

4- Sodium nitrate

5- Potassium nitrate

6- Hydroxide of copper

7- Iron III

8- Nitric acid

9- Iron II oxalate

10- Iron II sulphate

Answer

1- Li2CO3 Δ Li2O + CO2

2- FeCO3 Δ FeO + CO2

3- CaCO3 Δ CaO + CO2

4- 2NaNO3 Δ 2NaNO2 + O2

5- 2KNO3 Δ 2KNO2 + O2

6- Cu(OH)2 Δ CuO + H2O

Black ppt.

7- 2Fe(OH)3 Δ Fe2O3 + 3H2O

8- 4HNO3 Δ 2H2O + 4NO2 + O2

COO Δ

9- Fe vacuume FeO + CO2 + CO

COO iron II oxalate

10- 2FeSO4 Δ Fe2O3 + SO2 + SO3

How can you differentiate between:

1- Copper sulphate and iron II sulphate

2- Aluminum chloride and iron III chloride

3- Potassium nitrite and potassium nitrate

4- LiCl – NaCl – KCl – CsCl

5- Dilute nitric acid and conc. Nitric acid

Answer

1-

Expermint Cu2+ Al3+ Fe2+ Fe3+

Salt solution + NaOH Cu(OH)2 Al(OH)3 Fe(OH)2 Fe(OH)3

Blue ppt. White ppt. Green-white ppt Red-brown ppt

2-

CuSO4 + 2NaOH Na2SO4 + Cu(OH)2

Blue ppt.

AlCl3 + 3NaOH 3NaCl + Al(OH)3

White ppt.

FeSO4 + 2NaOH Na2SO4 + Fe(OH)2

greenish white ppt.

FeCl3 + 3NH4OH 3NH4Cl + Fe(OH)3

Reddish brown ppt.

3-

Experiment Nitrite(NO2)- Nitrate(NO3)-

Salt sol. + KMnO4 + H2SO4 The violt colour dissappear No change

5KNO2 + 2KMnO4 + 3H2SO4 5KNO3 + K2SO4 + 2MnSO4 + 3H2O

4-

Flame test Li+ Na+ K+ Cs+

1- Dip a clean wire in dry salt

2- Expose the wire to flame Crimson flame Golden yellow flame Pale violet flame Bluish violet flame

5-

experiment Dilute HNO3 Conc. HNO3

Add iron to both of them Fe + 4HNO3 Fe(NO3)3 + H2O +NO

NO colourless gas turns reddish broen in the air No reaction due to passivity

What are

1- The role of :

Boyle - Dalton – Thomson – Bohr – Schrodinger – Berzelius – Lewis and Kosel – Davy - Solvay – Haber

Answers

Scientist Role

Boyle He put the first definition of element

Dalton He put the first atomic theory

Thomson He discovered the electron

Bohr He put atomic theory – explain spectrum of H2 – put principle q.n.

Schrodinger Modern theory of the atom – quantum no. – wave equation

Berzilus Chassified elements (metal-non metal) – compounds(organic-inorganic)

Lewis and Kosel They put octet rule

Davy He prepared Na-K by electrolysis of their molten halides

Solvay He prepared Na2CO3 by passing CO2+NH3+NaCl+H2O

Haber He prepared NH3 fom N2 and H2 in presence of cat.+500 degree+200 atm