أهم 100 سؤال فى مراجعة مادة كيمياء لغات الجزء الثانى الصف الثالث ثانوي
منتديات الأجيال التعليمية :: الملتقى الدراسي العام :: منتدى الامتحانات :: امتحانات الصف الثالث الثانوي
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أهم 100 سؤال فى مراجعة مادة كيمياء لغات الجزء الثانى الصف الثالث ثانوي
الدرس في شكل نص مقروء
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
حنين الصمت- مدير عام المنتدى
- عدد المساهمات : 5102
نقاط : 29201
تاريخ التسجيل : 08/09/2011
مواضيع مماثلة
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