Unit 3 Molecular Geometry, Bonding, and Polarity
Covalent bond
sharing of electrons between two atoms
a line or two dots on the side of an element (by their self)
How is a lone (non bonding) pair of electrons represented?
a line or two dots between element symbols
How is a shared pair of electrons often represented?
2 1
Hydrogen can only share ____ electrons and form ____ bond
D
Which among the following bonds is not possible? A. C and C triple bond B. C and O double bond C. C and C double bond D. C and H double bond
A
Which among the following compound's Lewis Structure contains one lone pair of electrons? A. NH3 B. CH4 C. H2O D. BH3
a
only 2 bonding pairs of electrons on the central atom a. 180 b. 120 c. 114 d. 109.5 e. 107 f. 104
C
Which central atom among the following does not have an eight electron configuration in its outermost orbit? A. PH3 B. CO2 C. BH3 D. H2S
D
Which has the least ionic character? A. Mg-O B. Si-CL c. C-F D. N-O
B
Which molecule among the following contains two lone pairs of electrons? A. PH3 B. H2S C. HCl D. BH3
C
Which molecule among the following is linear? A. NO2 B. SO2 C. CO2 D. H2O
D
Which molecule among the following is linear? A. NO2 B. SO2 C. H2O D. CO2
A
Which molecule among the following is not polar? A. H2 B. CO C. HCl D. NO2
d
only 4 bonding pairs of electrons on the central atom a. 180 b. 120 c. 114 d. 109.5 e. 107 f. 104C
high high
Substancers with ________ melting points have ________ boiling points
tetrahedral
109.5 degrees
(tetrahedral) bent
104 degrees
(tetrahedral) trigonal pyramidal
107 degrees
(trigonal planar) bent
114 degrees
trigonal planar
120 degrees
linear
180 degrees
metals
2 ___________ form a metallic bond
nonmetals
2 _____________ from a covalent bond
f
2 bonding pairs and 2 non bonding pair of electrons on the central atom
e
3 bonding pairs and 1 non bonding pairs of electrons on the central atom
Ionic
All have very high melting points Ionic Covalent Metallic
Metallic
Are shiny because valence electrons are not attached to any particular atom Ionic Covalent Metallic
D
BCI A. Bent B. Linear C. Tetrahedral D. Trigonal planar E. Trigonal pyramidal
B
BCI3 A. Polar B. Nonpolar
b
BCI3 a. 180 b. 120 c. 114 d. 109.5 e. 107 f. 104
C
Based on Lewis structures, predict the ordering of N-O bond lengths in NO+, NO2-, and NO3-. A. NO2- > NO3- > NO+ B. NO+ > NO3- > NO2- C. NO3- > NO2- > NO+ D. NO2- > NO+ > NO3- E. NO3- > NO+ > NO2- F. NO+ > NO2- > NO3-
25
Boiling point occurs at _______ degrees celsius
C
CH2Br2 A. Bent B. Linear C. Tetrahedral D. Trigonal planar E. Trigonal pyramidal
A
CH2Br2 A. Polar B. Nonpolar
C
CH4 A. Bent B. Linear C. Tetrahedral D. Trigonal planar E. Trigonal pyramidal
B
CH4 A. Polar B. Nonpolar
B
CO2 A. Bent B. Linear C. Tetrahedral D. Trigonal planar E. Trigonal pyramidal
B
CO2 A. Polar B. Nonpolar
Covalent
CO2 Ionic Covalent Metallic
Ionic
Ca-Cl Ionic Covalent Metallic
Covalent
Can be solid, liquid or gas 25C Ionic Covalent Metallic
C
Cl-Cl A. Ionic B. Polar Covalent C. Nonpolar Covalent
Covalent
Cl-Cl Ionic Covalent Metallic
C
Consider the compound C2H6. The C-H is _______ and the C-C bond is __________ A. polar, polar B. nonpolar, polar C. polar, nonpolar D. nonpolar, nonpolar E. Ionic, nonpolar
D
Diamond is classified as a ______. A. metallic B. molecular C. Ionic D. network covalent
Covalent
H-F Ionic Covalent Metallic
Covalent
H-H Ionic Covalent Metallic
Covalent
H20 Ionic Covalent Metallic
A
H2O A. Bent B. Linear C. Tetrahedral D. Trigonal planar E. Trigonal pyramidal
A
H2O A. Polar B. Nonpolar
f
H2O a. 180 b. 120 c. 114 d. 109.5 e. 107 f. 104
D
In what state of matter are most molecular compounds that have a high molecular mass at room temperature? A.liquid B. gas C. solution D. solid
C
In what state of matter do molecular compounds of very low molecular mass exist at room temperature? A. liquid B. solution C. gas D. solid
KCI
Ionic Ionic Covalent Metallic
A
K-Cl A. Ionic B. Polar Covalent C. Nonpolar Covalent
Metallic
Mg-K Ionic Covalent Metallic
E
NH3 A. Bent B. Linear C. Tetrahedral D. Trigonal planar E. Trigonal pyramidal
A
NH3 A. Polar B. Nonpolar
Covalent
NH3 Ionic Covalent Metallic
e
NH3 a. 180 b. 120 c. 114 d. 109.5 e. 107 f. 104
Ionic
Na-Cl Ionic Covalent Metallic
B
P-Cl A. Ionic B. Polar Covalent C. Nonpolar Covalent
NP P NP P NP NP
Predict whether the following molecules are polar or nonpolar. Type P for Polar and NP for Nonpolar. BF3 ________ NCl3 ________ SO3 ____________ CO __________ CF4 _______ CS2 ________
B
S-Cl A. Ionic B. Polar Covalent C. Nonpolar Covalent
D
Salts are ionic compounds and have which of the following properties? A. low boiling point B. Conduct as a solid C. Always water soluble D. high melting points
Covalent
The sharing of electrons Ionic Covalent Metallic
6
There are ______ lone pairs of electrons in a molecule of SO2.
Metallic
W-W Ionic Covalent Metallic
A
What is the molecular geometry of NCS-? A. linear B. trigonal pyramidal C. tetrahedral D. trigonal planar E. bent
C
What type of substance is Al(OH)3? A. Covalent B. Network Solid C. Ionic D. Metallic E. Macromolecular
C
What type of substance is C2H5OH? A. Metallic B. Network Solid C. Covalent D. Macromolecular E. Ionic
A
What type of substance is H2O2 A. Molecular B. Covalent Network C. Metallic D. Macromolecular E. Ionic
C
What type of substance is HCl? A. Covalent Network B. Ionic C. Molecular D. Macromolecular E. Metallic
D
What type of substance is graphite? A. Macromolecular B. Ionic C. Covalent D. Covalent Network E. Metallic
A C D E
Which of the following are characteristics of most ionic solids? (Select all that apply.) A. They are brittle. B. They have low melting points. C. They tend to be crystalline solids. D. They conduct electricity in the molten state. E. They conduct electricity when dissolved in water. F. They conduct electricity in the solid state
B C F H
Which of the following are properties of a metal? (Select all that apply.) A. soluble in a polar solvent B. good heat conductor C. shiny D. poor electrical conductor E. malleable F. brittle G. poor heat conductor H. good electrical conductor
A C F
Which of the following are properties of a nonmetal? (Select all that apply.) A. poor electrical conductor B. malleable C. soft or brittle D. good electrical conductor E. good heat conductor F. poor heat conductor
C
Which of the following bonds is least polar? A. S - P B. Te - I C. C - F D. Si - F
A
Which of the following bonds is the most Polar? A. H - F B. O - F C. C - F D. N - F E. S - F
B
Which of the following compounds contain both ionic and covalent bonds? (select all that apply.) A. CO2 B. NH4Br C. LiCl D. CF4
D
Which of the following forms an ionic crystalline solid at room temperature? A. iodine solid B. methane (CH4) C. carbon dioxide solid D. copper(II) chloride
C
Which of the following has the bonds arranged in order of increasing polarity? A. O-F, B-F, N-F B. N-F, O-F, B-F C. O-F, N-F, B-F D. B-F, N-F, O-F
D
Which of the following is the most polar? A. S-O B. N-O C. C-O D. Si-O
A D
Which of the following molecules or ions contain polar bonds? (Select all that apply.) A. H2S B. S2 2- C. P4 D. NO 2-
C
Which of the following pairs would have the strongest electrostatic attractive force? A. Rb - F B. Rb - I C. Cs - F D. Cs - I
E
Which of the following substances have both ionic and covalent bonds? (Select all that apply.) A. CaCO3 B. CH4 C. diamond D. Mg E. CH3COONa
D
Which substance contains bonds with the greatest ionic character? A. Cl2 B. OF2 C. PI3 D. KBr
Boron
_______ will not form a double or triple bond it is okay with 6 electrons
Electricity
___________ is conducted by moving chargers
Metals Nonmetals
______________ and ___________ for ionic bonds
Chemical bond
a strong attachment between two atoms or ions
Covalent Compounds
are compounds that are composed of atoms that are held together by covalent bonds
Ionic Compounds
are compounds that are composed of cations and anions that are held together by an electrostatic force of attraction
Metallic bond
each atom in a metal is bonded to several neighboring atoms; bonding electrons are relatively free to move throughout the three- dimensional structure of of the metal
Ionic bond
electrostatic force that exist between ions of opposite charge; formed from atoms by the transfer of one or more electrons from one atom to another
