chemistry 101 0786153719 / ةريمع حيمس / ءايميكلا نع...

Chemistry 101 / 0786153719إسألني عن الكيمياء / سميح عميرة

1) Which of the following bonds would be best categorized as covalent?

I. H-S II. Al-S III. N-F

A) I only B) II only C) III only D) I and III

E) I, II, and III

2) Rank the following bonds from most to least covalent in nature: (C-H, C-O, C-C, Al-O) a. C-H, C-O, Al-O, C-C b. C-O, C-H, C-C, Al-O c. C-C, C-H, Al-O, C-O d. Al-O, C-O, C-H, C-C e. C-C, C-H, C-O, Al-O

3) Which of the following would contain both covalent and ionic bonding?

A) CaO B) NH3 C) C(diamond) D) Ca(NO3)2 E) CO2

4) There are __________ paired and __________ unpaired electrons in the Lewis symbol

for a Nitrogen atom.

A) 4, 2 B) 2, 4 C) 2, 3 D) 4, 3 E) 0, 3

5) In the Lewis symbol for a sulfur atom, there are __________ paired and __________

unpaired electrons.

A) 2, 2 B) 4, 2 C) 2, 4 D) 0, 6 E) 5, 1

6) There are __________ unpaired electrons in the Lewis symbol for an oxygen atom.


A) 0 B) 1 C) 2 D) 4 E) 3

7) The only noble gas without eight valence electrons is __________. A) Ar B) Ne C) He D) Kr E) All noble gases have eight valence electrons.

8) How many single covalent bonds must a silicon atom form to have a complete octet in

its valence shell? A) 3 B) 4 C) 1 D) 2 E) 0

9) How many hydrogen atoms must bond to silicon to give it an octet of valence electrons? A) 1 B) 2 C) 3 D) 4 E) 5

10) The Lewis structure of AsH3 shows __________ nonbonding electron pair(s) on As. A) 0 B) 1 C) 2 D) 3 E) This cannot be determined from the data given.

11) The Lewis structure of PF3 shows that the central phosphorus atom has __________

nonbonding and __________ bonding electron pairs. A) 2, 2 B) 1, 3 C) 3, 1 D) 1, 2 E) 3, 3

12) The Lewis structure of HCN (H – C≡N) shows that __________ has __________

nonbonding electron pairs.

A) C, 1


B) N, 1 C) H, 1 D) N, 2 E) C, 2

13) Which of the following correctly represents the Lewis structure for PH3?

A) B)

C) D)

14) A double bond (1 sigma and 1 pi bond) consists of __________ pairs of electrons shared between two atoms.

A) 1 B) 2 C) 3 D) 4 E) 6

15) A __________ covalent bond between the same two atoms is the longest. A) single B) double C) triple D) they are all the same length. E) strong

16) As the number of covalent bonds between two atoms increases, the distance between the atoms __________ and the strength of the bond between them __________.

A) increases, increases B) decreases, decreases C) increases, decreases D) decreases, increases E) is unpredictable

17) What is the maximum number of double (pi) bonds that a hydrogen atom can form? A) 0 B) 1 C) 2 D) 3


E) 4

18) In which of the molecules below is the carbon-carbon distance the shortest? A) H2C = CH2 B) H -- C ≡ C -- H C) H3C – CH3 D) H2C = C = CH2 E) H3C - CH2 - CH3

19) Of the bonds C – N, C = N, C ≡ N the C – N bond is __________. A) strongest/shortest B) strongest/longest C) weakest/shortest D) weakest/longest E) intermediate in both strength and length

20) How many equivalent resonance forms can be drawn for CO32-- (carbon is the central

atom)? A) 1 B) 2 C) 3 D) 4 E) 0

21) The Lewis structure of the CO32- ion is __________.

A B C D E

22) To convert from one resonance structure to another, __________. A) only atoms can be moved B) electrons and atoms can both be moved C) only electrons can be moved D) neither electrons nor atoms can be moved E) electrons must be added

23) Using Lewis structure drawings, determine which molecule below will have the shortest bond length between atoms:


A) N2 B) O2 C) Cl2 D) Br2 E) S2

24) Resonance structures differ by __________.

A) number and placement of electrons B) number of electrons only C) placement of atoms only D) number of atoms only E) placement of electrons only

25) The ion ICl4- has __________ valence electrons. A) 34 B) 35 C) 36 D) 28 E) 8

26) The ion NO- has __________ valence electrons.

A) 15 B) 14 C) 16 D) 10 E) 12

27) Of the following, __________ cannot accommodate more than an octet of electrons.

A) P B) As C) O D) S E) I

28) A valid Lewis structure of __________ cannot be drawn without violating the octet rule.

A) NH3 B) IF3 C) PF3 D) SbCl3 E) NO3

1-

29) The central atom in __________ does not violate the octet rule.

A) SF4 B) KrF2 C) CF4 D) XeF4


E) ICl4-

30) The central atom in __________ violates the octet rule. A) NH3 B) SeF2 C) BF3 D) AsF3 E) CH4

31) According to VSEPR theory, if there are four electron domains in the valence shell of an

atom, they will be arranged in a(n) __________ geometry. A) octahedral B) linear C) tetrahedral D) trigonal planar E) trigonal bipyramidal

32) Using the VSEPR model, the electron-domain geometry of the central atom in BF3 is

_________ while the molecular geometry would be described as ______________. A) linear, bent B) trigonal planar, bent C) trigonal planar, trigonal planar D) trigonal bipyramidal, bent E) octahedral, square pyramidal

33) The electron-domain geometry of the central atom in OF2 is _________ while the molecular geometry would be described as_________________.

A) linear, bent B) trigonal planar, bent C) tetrahedral, bent D) trigonal bipyramidal, linear E) octahedral, square pyramidal

34) The electron-domain geometry of the central atom in NO2- is _______, while the

molecular geometry would be described as____________. A) linear, linear B) trigonal planar, bent C) tetrahedral, triangular pyramidal D) trigonal bipyramidal, T shaped E) octahedral, octahedral

35) Using the VSEPR model, the electron-domain geometry of the central atom in BrF4- is

_______ while the molecular geometry would be described as_______________. A) linear, bent B) trigonal planar, bent C) tetrahedral, bent


D) trigonal bipyramidal, square planar E) octahedral, square planar

36) Which of the following would have an electron-domain geometry that is tetrahedral in

nature?

I. CH4 II. PH3 III. XeF4


A) I only B) II only C) III only D) I and II only E) I and III only

37) PCl5 has __________ electron domains and a __________ molecular arrangement.

A) 6, trigonal bipyramidal B) 6, tetrahedral C) 5, square pyramidal D) 5, trigonal bipyramidal E) 6, seesaw

38) Using the VSEPR model, the molecular geometry of the central atom in XeF2 is

__________. A) linear B) trigonal planar C) tetrahedral D) bent E) trigonal pyramidal

39) Using the VSEPR model, the molecular geometry of the central atom in BCl3 is __________.

A) linear B) trigonal planar C) tetrahedral D) bent E) trigonal pyramidal

40) The molecular geometry of the H3O+ ion is __________. A) linear B) tetrahedral C) bent D) trigonal pyramidal E) octahedral

41) ClF3 has "T-shaped" geometry. There are __________ non-bonding domains in this molecule.

A) 0 B) 1 C) 2 D) 3 E) 4


42) The ability of an atom in a molecule to attract electrons is best quantified by the

__________. A) paramagnetism B) diamagnetism C) electronegativity D) electron change-to-mass ratio E) first ionization potential

43) Electronegativity __________ from left to right within a period and __________

from top to bottom within a group. A) decreases, increases B) increases, increases C) increases, decreases D) stays the same, increases E) increases, stays the same

44) A nonpolar bond will form between two __________ atoms of __________ electronegativity.

A) different, opposite B) identical, different C) different, different D) similar, different E) identical, equal

45) Of the molecules below, the bond in __________ is the most polar. A) HBr B) HI C) HCl D) HF E) H2

46) Of the bonds below, __________ is the least polar. A) Na, S B) P, S C) C, F D) Si, Cl E) Na, Cl 47) Which of the following has the bonds correctly arranged in order of increasing

polarity? A) Be — F, Mg — F, N — F, O — F B) O— F, N — F, Be — F, Mg — F C) O— F, Be — F, Mg — F, N — F


D) N — F, Be — F, Mg — F, O — F E) Mg — F, Be — F, N — F, O — F

48) The molecular geometry of the PF3 molecule is __________, and this molecule is __________.

A) trigonal planar, polar B) trigonal planar, nonpolar C) trigonal pyramidal, polar D) trigonal pyramidal, nonpolar

E) tetrahedral, unipolar

49) The correct name for CCl4 is __________. A) carbon chloride B) carbon tetrachlorate C) carbon perchlorate D) carbon tetrachloride E) carbon chlorate

50) The correct name for N2O5 is __________. A) nitrous oxide B) nitrogen pentoxide C) dinitrogen pentoxide D) nitric oxide E) nitrogen oxide

51) The name of PCl3 is __________. A) potassium chloride B) phosphorus trichloride C) phosphorous(III) chloride D) monophosphorous trichloride E) trichloro potassium

52) The name of the binary compound N2O4 is __________. A) nitrogen oxide B) nitrous oxide C) nitrogen(IV) oxide D) dinitrogen tetroxide

E) oxygen nitride

53) Which of the following would be nitrogen monoxide? A) NO B) NO2 C) N2O D) N2O3


E) N3O2

54) Which of the following is named INCORRECTLY?

I. CO - carbon(II)oxide II. OF2 - difluorine oxide III. H3P - trihydrogen phosphide

A) I only B) II only C) III only D) I and II E) I, II, and III

55) The correct name for H2O is __________. A) hydrogen oxide B) hydrogen(II) oxide C) dihydrogen oxide D) dihydrogen monoxide E) hydrogen dioxide

56) The correct name for XeF4 is __________. A) monoxenon pentafluoride B) xenon pentafluoride C) xenon tetrafluoride D) monoxenon tetrafluoride E) xenon fluorate

57) The correct name for P2O5 is __________. A) phosphorus oxide B) phosphorus pentoxide C) diphosphorus oxide D) phosphate E) diphosphorus pentoxide

58) The name of BCl3 is __________. A) boron chloride B) boron trichloride C) monoboron chloride D) trichloro boron E) monoboron trichloride

59) The name of the binary compound CS2 is __________. A) carbon sulfide B) monocarbon disulfide C) carbon disulfide D) carbon sulfate E) carbon disulfate


60) The __________ quantum number defines the shape of an orbital a)n b) l c) ml d)ms

61) The n = 1 shell contains __________ p orbitals.

a) 0 b) 1 c) 2 d) 3

62) The lowest energy shell that contains f orbitals is the shell with n = _______ a) 1 b) 2 c) 3 d) 4

63) Each p-subshell can accommodate a maximum of __________ electrons. a) 2 b) 6 c) 10 d) 4

64) An electron cannot have the quantum numbers n = __________, l = __________, ml = __________. A) 2, 0, 0 B) 2, 1, -1 C) 3, 1, -1 D) 1, 1, 1 E) 3, 2, 1

65) Which one of the following is an impossible subshell notation? A) 4f B) 2d C) 3s D) 2p E) 3d

66) Which one of the following represents an acceptable possible set of quantum numbers (in the order n, l, ml, and ms) for an electron in an atom?

A) 2, 1, -1, 1/2 B) 2, 1, 0, 0 C) 2, 2, 0, 1/2 D) 2, 0, 1, -1/2 E) 2, 0, 2, +1/2

67) Which electron configuration represents a violation of the Pauli exclusion principle?

A) B)

C) D)


68) Which one of the following is the correct electron configuration for a nitrogen atom?

A) B)

C) D)

69) Which electron configuration represents a violation of Hund's rule for an atom in its ground

state?

A) B)

C) D)

70) Which of the following is an extensive property?

a) Mass b) Temperature c) Color d) Density e) Boiling point

71) Convert 77 oF to Kelvin scale.

a) 245 K b) 452 K c) 298 K d) 195 K e) 373 K

72) Answer to the expression: (87.90 – 13.0) /4.90 rounded to the proper number

of significant figures is:

a. 19 b. 19.2 c. 19.20 d. 15 e. 15.3


73) Photon is moving at a speed of 3*10^8 m/s , what is its speed in km/min :

a)1.08 x 107 b)18 x 109 c)30 x 105 d)1.8 x 107 e)3.0 x 108

74) How many protons (p) , neutrons (n), and electron (e) dose 2555Mn2+ ion have?

30p, 30n , 23e c)25p, 25n , 55e )b e23n , a) 25p, 30

d) 25p, 30n , 55e e) ) 25p, 30n , 25e

75) The name of HCIO2is :

a)Hydrochloric acid b)chlorous acid c)chioric acid

d)perchloric acid e)Hypochlorous acid

76) Bromine (Br) has two isotopes, with masses of 78.92 and 80.92 . What is the

natural abundance of the Lightest isotope, if the average atomic mass of bromine is

79.90 amu?

a) 13% b) 49% c) 68% d) 51% e) 87%

77) What is the mass of Calcium in 14.6 g CaCl2 ?

(atomic mass Cl = 35.45 g/mol & Ca = 40.08 g/mol )

a. 5.27 g b. 6.77 g c. 4.24 g d. 8.05 g e. 10.6 g

78) What is the empirical formula of a compound with the following composition

by mass:

C = 54.5% , H = 9.09% and O = 36.4%

(Atomic masses: C =12.01 , H = 1.008 , O = 16.00)

a. C2H3O b. C2H6O c. C3H5O2 d. C2H4O e. C2H5O

79) Balance the following equation:

a Be2C + b H2O c Be(OH)2 + d CH4


The ratio of coefficient d/b in the balanced equation is:

a. 1/2 b. 2/1 c. 1/4 d. 3/1 e. 4/1

80) Aluminum metal react with chlorine gas to form solid Aluminum chloride .

What mass of chlorine gas(M.w Cl2=70.9 g/mol is needed to react completely with

163 g of aluminum (M.w Al=26.9g/mol)

s) (32 AlCl(g) 22 Al(s) + 3 Cl

a)324 g b)489g c)214g d)644g e)245

81) Which of the following compound is insoluble in water?

a) Na2CO3 b) FeCO3 c) (NH4)2CO3 d) Na2S e) AgNO3

82) Which of the following is a weak acid?

a) H2SO4 b) HNO3 c) HCl d) HNO2 e) HBr

83) Whice of the following solutions has the least electrical conductance ?

a)KNO(aq) b)(NH2)2CO c)NaCl(aq)

d)LiOH(aq) e)H2SO4(aq)

84) What is the oxidation number for iodine in (H3IO6)-2 ?

a) -2 b) +7 c) -4 d) +1 e) +6

85) Calculate the oxidation number of sulfur , S , in the formula : (S2O3)-2.

a)-2 b)+2 c)+4 d)+5 e)+6

86) How many milliliters of 10.0M HCl must be diluted to obtain 1.0 liter

of 6.0M HCl ?

a. 375 ml b. 300 ml c. 260 ml d. 600 ml e. 1100 ml


87) How much of 1.20 M NaOH will be needed to neutralize 168 ml of 3.0 M

H2SO4?

a)1.8 L b) 0.042 L c) 0.84 L d)0.090 L e) 1.1 L

88) Calculate the density (in g/L) of N2 gas (molar mass = 28.0 g/mol) at STP

conditions.

a) 4.11 b) 3.31 c) 2.05 d) 1.25 e) 2.86

89) Determine the molar mass of a gas if 0.555 L weighs 1.55 g at STP ?

a) 62.6 g/mol b) 94.5 g/mol c) 86.9 g/mol

d) 53.3 g/mol e) 43.3 g/mol

90) In a reaction of (Ca) metal with water, the volume of Hydrogen gas

collected at 50ºC and pressure of 988 mmHg is 441 ml. What is the mass (in

grams) of the hydrogen gas obtained? The vapor pressure of water at 50ºC is 118

mmHg. (Molar mass of H2=2.016 g/mol) :

a) 0.0436g b) 0.0384g c) 0.0190g d) 0.0242g e) 0.0488g

91) Calculate the root mean square velocity (urms) in (m/s) of O2 molecules in a

sample of O2 gas at 1.0ºC [molar mass of O2 = 32.0 g/mol]

a) 462 b) 44.0 c) 1.24 d) 39.2 e) 12.5

92) For the following gases ( given molar masses ) :

F2(38) , CL2(71) , O2(32) , ana CO2(44)

The order of increasing rate of effusion is :

A ) F2 < Cl2 < CO2 < O2 b) Cl2 < F2< CO2 < O2

C ) Cl2 < O2 < F2 < CO2 d) CO2 < O2 < F2 < Cl2

E ) Cl2 < CO2 < F2 < O2

93) Which of the following is not a state function?

a. internal energy b. volume c. enthalpy d. pressure e. work


94) A gas is allowed to expand, at constant temperature, from a volume of 2.0 L to

9.0 L against external pressure of 1.50 atm. If the gas absorbs 600 J of heat from

the surroundings, then ∆E in J :

a) -85 b) +207 c) -464 d) +85 e) -20

95) How many heat absorbs in kj if temperature rise from 1 oC to 21.7 oC. will

occur when a 30.0 g block of aluminum The specific heat of Al is 0.900 J/g. oC.

a) 0.559 b) 0.360 c) 0.370 d) 0.575 e) 0.114

96) In which one of the following reactions would you expect the value of ∆H to

be significantly lower than that of ∆U ?

a) H2(g) + Br2(g) → 2HBr(g)

b) CO2(s) → CO2(g)

c)C2H2(g) + H2(g) → C2H4(g)

d)H2O(s) → H2O(l)

e)HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)

97) Which one of the following reaction has change H equals to change E ?

a) CaCO3(s) → Cao(s) + CO2(g)

b) H2(g) + 1/2O2(g) → H20(l)

c) CH4(g) + 2O2(g) → CO2(g) + 2H2O (l)

d) H2(g) + CL2(g) → 2Hcl(g)

e) H2O(l) → H2O(g)

98) Use Hess's Law to calculate the enthalpy change for the reaction in KJ/mol :

WO3(s) + 3H2(g) W(s) + 3H2O(g)

From the following data :

2W(s) + 3O2(g) 2WO3(s) ΔH = -1710.8 KJ

2H2(g) + O2(g) 2H2O(g) ΔH = -477.84 KJ

a) 125.9 b) 252.9 c) 364.9 d) 127.6 e) 138.6


99) Using the information below, calculate ∆Hfº for PbO(s) in kJ/mol.

PbO(s) + CO(g) → Pb(s) + CO2(g) ∆Hrxnº = -131.4 kJ/mol

Molecules ∆Hºr(kJ/mol)

CO(g) -110.5

CO2(g) -393.5

a) -413.9 kJ b) -151.6 kJ c) +372.1 kJ d) +413.9 kJ e) -372.1 kJ

100) Use bond energies to estimate the bond enthalpy of reaction

CH4(g) + 2O2(g) CO2(g) + 2H2O(g)

Bond Bond Energy (kJ/mol)

H—H 436

C—H 414

N—H 392

O O 499

C O 802

O—H 460

a) +262 kJ/mol

b) –790 kJ/mol

c) -104 kJ/mol

d) +104 kJ/mol

e) +790 kJ/mol

chemistry 101 0786153719 / ةريمع حيمس / ءايميكلا نع...

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