Unit 3 Molecular Geometry, Bonding, and Polarity

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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


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