Covalent Bonding & A aluminum, oxygen Molecular Compounds B - PDF document

Slide 1 / 109 Slide 2 / 109 1 Which pair of elements is most apt to form a molecular compound with each other? Covalent Bonding & A aluminum, oxygen Molecular Compounds B magnesium, iodine sulfur, fluorine C Multiple Choice Review potassium, lithium D barium, bromine E Slide 3 / 109 Slide 4 / 109 2 The correct name for SO is __________. 3 The correct name for CCl 4 is __________. A sulfur oxide A carbon chloride sulfur monoxide carbon tetrachlorate B B sulfoxide carbon perchlorate C C sulfate carbon tetrachloride D D sulfite carbon chlorate E E Slide 5 / 109 Slide 6 / 109 4 The correct name for N 2 O 5 is __________. 5 The name of PCl 3 is __________. A nitrous oxide A potassium chloride nitrogen pentoxide phosphorus trichloride B B dinitrogen pentoxide phosphorous(III) chloride C C nitric oxide monophosphorous trichloride D D nitrogen oxide trichloro potassium E E

Slide 7 / 109 Slide 8 / 109 6 The name of the binary compound N 2 O 4 is 7 The correct name for H 2 O is __________. __________. A hydrogen oxide A nitrogen oxide hydrogen(II) oxide B B nitrous oxide dihydrogen oxide C nitrogen(IV) oxide C dihydrogen monoxide D dinitrogen tetroxide D E hydrogen dioxide oxygen nitride E Slide 9 / 109 Slide 10 / 109 8 The correct name for XeF 4 is __________. 9 The correct name for P 2 O 5 is __________. A monoxenon pentafluoride A phosphorus oxide xenon pentafluoride phosphorus pentoxide B B xenon tetrafluoride diphosphorus oxide C C monoxenon tetrafluoride phosphate D D xenon fluorate diphosphorus pentoxide E E Slide 11 / 109 Slide 12 / 109 10 The name of BCl 3 is __________. 11 The name of the binary compound CS 2 is __________. A boron chloride A carbon sulfide boron trichloride B monocarbon disulfide B monoboron chloride C carbon disulfide C trichloro boron D carbon sulfate D monoboron trichloride E carbon disulfate E

Slide 13 / 109 Slide 14 / 109 12 The type of compound that is most likely to 13 There are __________ paired and __________ contain a covalent bond is __________. unpaired electrons in the Lewis symbol for a Nitrogen atom. A one that is composed of a metal and a nonmetal A 4, 2 B a solid metal 2, 4 B C one that is composed of only nonmetals 2, 3 C held together by the electrostatic forces between D oppositely charged ions 4, 3 D E There is no general rule to predict covalency in bonds. 0, 3 E Slide 15 / 109 Slide 16 / 109 14 In the Lewis symbol for a sulfur atom, there are 15 In the Lewis symbol for an Iodine atom, there are __________ paired and __________ unpaired __________ paired and __________ unpaired electrons. electrons. A 2, 2 A 4, 2 4, 2 4,1 B B 2, 4 2, 5 C C 0, 6 6, 1 D D 5, 1 0, 5 E E Slide 17 / 109 Slide 18 / 109 16 There are __________ unpaired electrons in the 17 The only noble gas without eight valence Lewis symbol for an oxygen atom. electrons is __________. A 0 A Ar 1 B Ne B 2 He C C 4 Kr D D 3 All noble gases have eight valence electrons. E E

Slide 19 / 109 Slide 20 / 109 18 How many single covalent bonds must a silicon 19 How many hydrogen atoms must bond to silicon atom form to have a complete octet in its valence to give it an octet of valence electrons? shell? A 1 A 3 B 2 4 B 3 C 1 C 4 D 2 D 5 E 0 E Slide 21 / 109 Slide 22 / 109 20 A double bond consists of __________ pairs of 21 A __________ covalent bond between the same electrons shared between two atoms. two atoms is the longest. A 1 A single 2 double B B 3 triple C C D 4 D they are all the same length. 6 strong E E Slide 23 / 109 Slide 24 / 109 22 As the number of covalent bonds between two 23 What is the maximum number of double bonds atoms increases, the distance between the atoms that a hydrogen atom can form? __________ and the strength of the bond between them __________. A 0 1 B A increases, increases 2 C decreases, decreases B 3 D increases, decreases C 4 E D decreases, increases is unpredictable E

Slide 25 / 109 Slide 26 / 109 24 What is the maximum number of double bonds 25 In which of the molecules below is the carbon- that a carbon atom can form? carbon distance the shortest? A 4 A H 2 C = CH 2 B 1 B H -- C ≡ C -- H 0 C H 3 C – CH 3 C 2 H 2 C = C = CH 2 D D 3 H 3 C - CH 2 - CH 3 E E Slide 27 / 109 Slide 28 / 109 26 Of the bonds C – N, C = N, C ≡ N the C – N bond 27 Of the possible bonds between carbon atoms is __________. (single, double, and triple), __________. A a triple bond is longer than a single bond A strongest/shortest strongest/longest a double bond is stronger than a triple bond B B weakest/shortest a single bond is stronger than a triple bond C C D weakest/longest D a double bond is longer than a triple bond intermediate in both strength and length E a single bond is stronger than a double bond E Slide 29 / 109 Slide 30 / 109 - has __________ valence electrons. The ion NO - has __________ valence electrons. 28 The ion ICl 4 29 A 34 A 15 35 14 B B 36 16 C C 28 10 D D 8 12 E E

Slide 31 / 109 Slide 32 / 109 30 The Lewis structure of AsH 3 shows __________ 31 The Lewis structure of PF 3 shows that the central nonbonding electron pair(s) on As. phosphorus atom has __________ nonbonding and __________ bonding electron pairs. A 0 A 2, 2 B 1 1, 3 B C 2 3, 1 C 3 D 1, 2 D This cannot be determined from the data given. E 3, 3 E Slide 33 / 109 Slide 34 / 109 32 The Lewis structure of HCN (H – C≡N) shows that 33 Of the following, __________ cannot __________ has __________ nonbonding electron accommodate more than an octet of electrons. pairs. A P A C, 1 B As N, 1 B O C H, 1 C D S N, 2 D I E C, 2 E Slide 35 / 109 Slide 36 / 109 34 A valid Lewis structure of __________ cannot be 35 A valid Lewis structure of __________ cannot be drawn without violating the octet rule. drawn without violating the octet rule. 3- A NH 3 A PO 4 B IF 3 B PF 3 C PF 3 C CCl 4 SbCl 3 SeF 4 D D -1 NO 3 NF 3 E E

Slide 37 / 109 Slide 38 / 109 36 The central atom in __________ does not violate 37 The central atom in __________ violates the octet the octet rule. * rule. A SF 4 A NH 3 B KrF 2 B SeF 2 C CF 4 C BF 3 XeF 4 AsF 3 D D - ICl 4 CH 4 E E Slide 39 / 109 Slide 40 / 109 38 A valid Lewis structure of __________ cannot be 39 A valid Lewis structure of __________ cannot be drawn without violating the octet rule. drawn without violating the octet rule. A ClF 3 A NI 3 PCl 3 SO 2 B B SO 3 ICl 5 C C D CCl 4 D SiF 4 CO 2 CO 2 E E Slide 41 / 109 Slide 42 / 109 - ion has 40 A valid Lewis structure of __________ cannot be 41 The central iodine atom in the ICl 4 drawn without violating the octet rule. __________ non-bonded electron pairs and __________ bonded electron pairs in its valence shell. A NF 3 B BeH 2 A 2, 2 C SO 2 3, 4 B CF 4 D 1, 3 C 2- SO 3 E D 3, 2 2, 4 E

Slide 43 / 109 Slide 44 / 109 42 The central iodine atom in IF 5 has __________ non- 43 The central Xe atom in the XeF 4 molecule has bonded electron pairs and __________ bonded __________ non-bonded electron pairs and electron pairs in its valence shell. __________ bonded electron pairs in its valence shell. A 1, 5 A 1, 4 0, 5 B 2, 4 B 5, 1 C 4, 0 C 4, 1 D 4, 1 D 1, 4 E E 4, 2 Slide 45 / 109 Slide 46 / 109 44 Resonance structures differ by __________. 45 How many equivalent resonance forms can be -2 (carbon is the central atom)? drawn for CO 3 A number and placement of electrons A 1 number of electrons only B 2 B placement of atoms only C 3 C number of atoms only D D 4 placement of electrons only E 0 E Slide 47 / 109 Slide 48 / 109 46 How many equivalent resonance forms can be 47 How many equivalent resonance structures can be drawn for SO 2 without expanding octet on the sulfur drawn for the molecule of SO 3 without having to atom (sulfur is the central atom)? violate the octet rule on the sulfur atom? A 0 A 5 2 2 B B C 3 C 1 4 4 D D 1 3 E E