Covalent Bonding & Molecular Compounds Multiple Choice Review


Download Covalent Bonding & Molecular Compounds Multiple Choice Review


Preview text

Covalent Bonding & Molecular Compounds Multiple Choice Review

PSI Chemistry

Name_________________________________

1) Which pair of elements is most apt to form a molecular compound with each other? A) aluminum, oxygen B) magnesium, iodine C) sulfur, fluorine D) potassium, lithium E) barium, bromine

2) 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

3) Which of the following BEST describes the bonding found within solid Al2O3? A) Strong covalent bonds between atoms with similar electronegativities B) Covalently bound atoms arranged in small individual molecules. C) Electrostatic attractions between + and - charged ions D) Positively charged ions covalently bound with many mobile electrons E) None of these

4) Which of the following species below would be considered molecular in nature? A) C(diamond) B) C(graphite) C) Fe D) AlCl3 E) PCl3

5) The substance below BEST characterized as having a high melting point and able to conduct electricity in the liquid state only would be:
A) CH4 B) V2O5 C) CO D) HF E) C(diamond)

6) A material melts at -77 C, is non-conductive, and consists of small individual molecules held

together by inter-molecular forces. Which of the molecules below is this material likely to be?

A) NaCl

www.njctl.org

Chemistry

Covalent Bonding

B) NH3 C) C(diamond) D) MgO E) Cu

7) Which of the following BEST explains the relatively low melting point of covalent molecular substances?
A) Covalent molecular materials rely on weak electrostatic forces holding the ions together.
B) The “sea” of electrons between the atoms creates relatively weak bonding C) The intermolecular forces between the molecules are weak compared to ionic or
covalent bonds. D) The metals involved create uneven bonding with the non-metals E) The similar electronegativity of the atoms cause repulsions between the molecules

8) Which of the following would be characterized as a molecular compound?

I.

CO

II. Zn(OH)2

III. Fe

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

9) Which of the following would contain both covalent and Ionic bonding? A) CaO B) NH3 C) C(diamond) D) Ca(NO3)2 E) CO2

10) 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

11) The correct name for SO is __________. A) sulfur oxide B) sulfur monoxide C) sulfoxide D) sulfate E) sulfite

www.njctl.org

Chemistry

Covalent Bonding

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

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

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

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

16) Which of the following would be nitrogen(I)oxide? A) NO B) NO2 C) N2O D) N2O3 E) N3O2

17) Which of the following is named INCORRECTLY?

I.

CO - carbon(II)oxide

II. OF2 - diflourine oxide

III. H3P - trihydrogen phosphide

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

18) The correct name for H2O is __________. A) hydrogen oxide

www.njctl.org

Chemistry

Covalent Bonding

B) hydrogen(II) oxide C) dihydrogen oxide D) dihydrogen monoxide E) hydrogen dioxide

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

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

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

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

Lewis Dot Structures 23) The type of compound that is most likely to contain a covalent bond is __________.
A) one that is composed of a metal and a nonmetal B) a solid metal C) one that is composed of only nonmetals D) held together by the electrostatic forces between oppositely charged ions E) There is no general rule to predict covalency in bonds.

24) 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

www.njctl.org

Chemistry

Covalent Bonding

E) 0, 3

25) 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

26) In the Lewis symbol for an Iodine atom, there are __________ paired and __________
unpaired electrons.
A) 4, 2 B) 4,1 C) 2, 5 D) 6, 1 E) 0, 5

27) There are __________ unpaired electrons in the Lewis symbol for an oxygen atom. A) 0 B) 1 C) 2 D) 4 E) 3

28) 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.

29) Which of the following would have all of it’s valance electrons paired in it’s lewis structure representation?
A) Al B) P C) S D) F E) Xe

30) 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

www.njctl.org

Chemistry

Covalent Bonding

E) 0

31) 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

32) Which of the following atoms is without lone electrons to be shared? A) Al B) Be C) B D) He E) H

33) 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

34) 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

35) 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

36) 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

37) What is the maximum number of double (pi) bonds that a carbon atom can form?

www.njctl.org

Chemistry

Covalent Bonding

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

38) 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

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

bond is __________.

40) Of the possible bonds between carbon atoms (single, double, and triple), __________. A) a triple (sigma +2pi) bond is longer than a single bond B) a double (sigma + pi)bond is stronger than a triple bond C) a single (sigma) bond is stronger than a triple bond D) a double (sigma + pi) bond is longer than a triple bond E) a single (sigma) bond is stronger than a double bond

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

42) The ion NO-
A) 15 B) 14 C) 16 D) 10 E) 12

has __________ valence electrons.

43) 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.

www.njctl.org

Chemistry

Covalent Bonding

44) 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

45) 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

46) Of the following, __________ cannot accommodate more than an octet of electrons.
A) P B) As C) O D) S E) I

47) A valid Lewis structure of __________ cannot be drawn without violating the octet rule.
A) NH3 B) IF3 C) PF3 D) SbCl3 E) NO31-

48) A valid Lewis structure of __________ cannot be drawn without violating the octet rule.
A) PO43B) PF3 C) CCl4 D) SeF4 E) NF3

49) The central atom in __________ does not violate the octet rule.
A) SF4 B) KrF2 C) CF4 D) XeF4 E) ICl4-

50) The central atom in __________ violates the octet rule.

www.njctl.org

Chemistry

Covalent Bonding

A) NH3 B) SeF2 C) BF3 D) AsF3 E) CH4

51) A valid Lewis structure of __________ cannot be drawn without violating the octet rule.
A) ClF3 B) PCl3 C) SO3 D) CCl4 E) CO2

52) A valid Lewis structure of __________ cannot be drawn without violating the octet rule.
A) NI3 B) SO2 C) ICl5 D) SiF4 E) CO2

53) A valid Lewis structure of __________ cannot be drawn without violating the octet rule.
A) NF3 B) BeH2 C) SO2 D) CF4 E) SO32-

54) The central iodine atom in the ICl4- ion has __________ non-bonded electron pairs and __________ bonded electron pairs in its valence shell.
A) 2, 2 B) 3, 4 C) 1, 3 D) 3, 2 E) 2, 4

55) The central iodine atom in IF5 has __________ non-bonded electron pairs and __________ bonded electron pairs in its valence shell.
A) 1, 5 B) 0, 5 C) 5, 1 D) 4, 1 E) 1, 4

56) The central Xe atom in the XeF4 molecule has __________ non-bonded electron pairs and __________ bonded electron pairs in its valence shell.
A) 1, 4

www.njctl.org

Chemistry

Covalent Bonding

B) 2, 4 C) 4, 0 D) 4, 1 E) 4, 2
57) Which of the following correctly represents the lewis structure for PH3?

A)

B)

C)

D)

58) How many double (pi) bonds would be present in a CS2 molecule? A) 0 B) 1 C) 2 D) 3 E) 4
59) Which of the following would be the correct lewis structure for methyl amine (CH3NH2)?

A)

B)

C)

D)

Resonance 60) Resonance structures differ by __________.
A) number and placement of electrons B) number of electrons only

www.njctl.org

Chemistry

Covalent Bonding

Preparing to load PDF file. please wait...

0 of 0
100%
Covalent Bonding & Molecular Compounds Multiple Choice Review