Covalent Bonding & Molecular Compounds Multiple Choice Review - PDF document

Slide 1 / 109 Covalent Bonding & Molecular Compounds Multiple Choice Review Slide 2 / 109 1 Which pair of elements is most apt to form a molecular compound with each other? A aluminum, oxygen B magnesium, iodine sulfur, fluorine C potassium, lithium D barium, bromine E Slide 3 / 109 2 The correct name for SO is __________. A sulfur oxide sulfur monoxide B sulfoxide C sulfate D sulfite E

Slide 4 / 109 3 The correct name for CCl 4 is __________. A carbon chloride B carbon tetrachlorate carbon perchlorate C carbon tetrachloride D carbon chlorate E Slide 5 / 109 4 The correct name for N 2 O 5 is __________. A nitrous oxide nitrogen pentoxide B dinitrogen pentoxide C nitric oxide D nitrogen oxide E Slide 6 / 109 5 The name of PCl 3 is __________. A potassium chloride phosphorus trichloride B phosphorous(III) chloride C monophosphorous trichloride D trichloro potassium E

Slide 7 / 109 6 The name of the binary compound N 2 O 4 is __________. A nitrogen oxide nitrous oxide B nitrogen(IV) oxide C D dinitrogen tetroxide oxygen nitride E Slide 8 / 109 7 The correct name for H 2 O is __________. A hydrogen oxide hydrogen(II) oxide B dihydrogen oxide C dihydrogen monoxide D hydrogen dioxide E Slide 9 / 109 8 The correct name for XeF 4 is __________. A monoxenon pentafluoride xenon pentafluoride B xenon tetrafluoride C monoxenon tetrafluoride D xenon fluorate E

Slide 10 / 109 9 The correct name for P 2 O 5 is __________. A phosphorus oxide B phosphorus pentoxide diphosphorus oxide C phosphate D diphosphorus pentoxide E Slide 11 / 109 10 The name of BCl 3 is __________. A boron chloride boron trichloride B monoboron chloride C trichloro boron D monoboron trichloride E Slide 12 / 109 11 The name of the binary compound CS 2 is __________. A carbon sulfide monocarbon disulfide B carbon disulfide C carbon sulfate D E carbon disulfate

Slide 13 / 109 12 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 a solid metal B one that is composed of only nonmetals C held together by the electrostatic forces between D oppositely charged ions There is no general rule to predict covalency in bonds. E Slide 14 / 109 13 There are __________ paired and __________ unpaired electrons in the Lewis symbol for a Nitrogen atom. A 4, 2 2, 4 B 2, 3 C 4, 3 D 0, 3 E Slide 15 / 109 14 In the Lewis symbol for a sulfur atom, there are __________ paired and __________ unpaired electrons. A 2, 2 4, 2 B 2, 4 C 0, 6 D 5, 1 E

Slide 16 / 109 15 In the Lewis symbol for an Iodine atom, there are __________ paired and __________ unpaired electrons. A 4, 2 4,1 B 2, 5 C 6, 1 D 0, 5 E Slide 17 / 109 16 There are __________ unpaired electrons in the Lewis symbol for an oxygen atom. A 0 B 1 2 C 4 D 3 E Slide 18 / 109 17 The only noble gas without eight valence electrons is __________. A Ar Ne B He C Kr D E All noble gases have eight valence electrons.

Slide 19 / 109 18 How many single covalent bonds must a silicon atom form to have a complete octet in its valence shell? A 3 4 B 1 C 2 D 0 E Slide 20 / 109 19 How many hydrogen atoms must bond to silicon to give it an octet of valence electrons? A 1 B 2 3 C 4 D 5 E Slide 21 / 109 20 A double bond consists of __________ pairs of electrons shared between two atoms. A 1 2 B 3 C 4 D E 6

Slide 22 / 109 21 A __________ covalent bond between the same two atoms is the longest. A single double B triple C D they are all the same length. strong E Slide 23 / 109 22 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 decreases, decreases B increases, decreases C decreases, increases D E is unpredictable Slide 24 / 109 23 What is the maximum number of double bonds that a hydrogen atom can form? A 0 1 B 2 C 3 D E 4

Slide 25 / 109 24 What is the maximum number of double bonds that a carbon atom can form? A 4 1 B 0 C D 2 3 E Slide 26 / 109 25 In which of the molecules below is the carbon- carbon distance the shortest? A H 2 C = CH 2 B H -- C ≡ C -- H C H 3 C – CH 3 D H 2 C = C = CH 2 H 3 C - CH 2 - CH 3 E Slide 27 / 109 26 Of the bonds C – N, C = N, C ≡ N the C – N bond is __________. A strongest/shortest strongest/longest B weakest/shortest C weakest/longest D E intermediate in both strength and length

Slide 28 / 109 27 Of the possible bonds between carbon atoms (single, double, and triple), __________. A a triple bond is longer than a single bond a double bond is stronger than a triple bond B a single bond is stronger than a triple bond C D a double bond is longer than a triple bond E a single bond is stronger than a double bond Slide 29 / 109 - has __________ valence electrons. 28 The ion ICl 4 A 34 35 B 36 C 28 D 8 E Slide 30 / 109 The ion NO - has __________ valence electrons. 29 A 15 14 B 16 C 10 D 12 E

Slide 31 / 109 30 The Lewis structure of AsH 3 shows __________ nonbonding electron pair(s) on As. A 0 1 B 2 C D 3 E This cannot be determined from the data given. Slide 32 / 109 31 The Lewis structure of PF 3 shows that the central phosphorus atom has __________ nonbonding and __________ bonding electron pairs. A 2, 2 1, 3 B 3, 1 C 1, 2 D 3, 3 E Slide 33 / 109 32 The Lewis structure of HCN (H – C≡N) shows that __________ has __________ nonbonding electron pairs. A C, 1 N, 1 B H, 1 C N, 2 D C, 2 E

Slide 34 / 109 33 Of the following, __________ cannot accommodate more than an octet of electrons. A P B As O C D S I E Slide 35 / 109 34 A valid Lewis structure of __________ cannot be drawn without violating the octet rule. A NH 3 B IF 3 C PF 3 D SbCl 3 -1 NO 3 E Slide 36 / 109 35 A valid Lewis structure of __________ cannot be drawn without violating the octet rule. 3- A PO 4 B PF 3 CCl 4 C SeF 4 D E NF 3

Slide 37 / 109 36 The central atom in __________ does not violate the octet rule. * A SF 4 KrF 2 B CF 4 C D XeF 4 - ICl 4 E Slide 38 / 109 37 The central atom in __________ violates the octet rule. A NH 3 B SeF 2 C BF 3 D AsF 3 CH 4 E Slide 39 / 109 38 A valid Lewis structure of __________ cannot be drawn without violating the octet rule. A ClF 3 PCl 3 B SO 3 C CCl 4 D E CO 2

Slide 40 / 109 39 A valid Lewis structure of __________ cannot be drawn without violating the octet rule. A NI 3 SO 2 B ICl 5 C D SiF 4 CO 2 E Slide 41 / 109 40 A valid Lewis structure of __________ cannot be drawn without violating the octet rule. A NF 3 B BeH 2 C SO 2 D CF 4 2- SO 3 E Slide 42 / 109 - ion has 41 The central iodine atom in the ICl 4 __________ non-bonded electron pairs and __________ bonded electron pairs in its valence shell. A 2, 2 3, 4 B C 1, 3 3, 2 D 2, 4 E

Slide 43 / 109 42 The central iodine atom in IF 5 has __________ non- bonded electron pairs and __________ bonded electron pairs in its valence shell. A 1, 5 0, 5 B 5, 1 C 4, 1 D 1, 4 E Slide 44 / 109 43 The central Xe atom in the XeF 4 molecule has __________ non-bonded electron pairs and __________ bonded electron pairs in its valence shell. A 1, 4 2, 4 B 4, 0 C 4, 1 D E 4, 2 Slide 45 / 109 44 Resonance structures differ by __________. A number and placement of electrons number of electrons only B placement of atoms only C number of atoms only D placement of electrons only E

Slide 46 / 109 45 How many equivalent resonance forms can be -2 (carbon is the central atom)? drawn for CO 3 A 1 2 B 3 C D 4 0 E Slide 47 / 109 46 How many equivalent resonance forms can be drawn for SO 2 without expanding octet on the sulfur atom (sulfur is the central atom)? A 0 2 B 3 C 4 D 1 E Slide 48 / 109 47 How many equivalent resonance structures can be drawn for the molecule of SO 3 without having to violate the octet rule on the sulfur atom? A 5 2 B 1 C 4 D 3 E

Slide 49 / 109 48 How many different types of resonance structures -2 where all atoms can be drawn for the ion SO 3 satisfy the octet rule? A 1 2 B 3 C 4 D 5 E Slide 50 / 109 - , __________. 49 In the nitrite ion NO 2 A both bonds are single bonds B both bonds are double bonds one bond is a double bond and the other is a single bond C both bonds are the same D there are 20 valence electrons E Slide 51 / 109 -2 ion is __________. 50 The Lewis structure of the CO 3 A B C D E