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Example Questions
Example Question #1 : Types Of Chemical Bonds
What type of bond is present between the atoms of carbon dioxide?
Nonpolar covalent
Ionic
Coordinate covalent
Polar covalent
Polar covalent
Carbon dioxide has a double bond between the carbon and oxygen molecules. Since there is a moderately large electronegativitiy difference between C and O, the bond can be described as polar covalent.
Though the bonds themselves are polar, the overall symmetry of the molecule means that carbon dioxide has a net zero dipole and is a nonpolar compound.
Example Question #6 : Types Of Chemical Bonds
Which of the following describe a covalent bond?
The metal accepts an electron
The nonmetal gives up an electron
Electrons are being shared
None of these
Both metals give up an electron
Electrons are being shared
In a covalent bond, electrons are shared between two nonmetals. If there is a metal in the compound, that is called an ionic compound, not a covalent compound. Ionic bonds involve the complete transfer of an electron from one species to another.
Example Question #7 : Types Of Chemical Bonds
What type(s) of bond(s) is/are present in the following molecule?
RbCl
ionic
covalent
network covalent
network ionic
complex ionic
ionic
An ionic bond is a bond between a metal (Rb) and a nonmetal(Cl)
Example Question #4 : Types Of Chemical Bonds
What type of compound is ?
Metallic
Covalent
Polyatomic ion
Ionic
Ionic
Ionic compounds are formed between metals, which want to loose electrons, and nonmetals, which want to gain electrons. The sodium (Na) will completely transfer an electron to the chlorine (Cl), giving both atoms a complete octet without sharing electrons.
Covalent compounds generally form between two nonmetals that will both share electrons to complete their octets. Metallic compounds are built from only metals. Polyatomic ions will have a formal charge.
Example Question #1 : Bonds And Forces
Which of the following compounds is not held together by ionic bonds?
Covalent bonds are formed when two nonmetals are bonded together. This covalent bond means that the electrons are shared by the two atoms in order to satisfy each atom's octet. There is very little difference in the electronegativities of the two atoms involved in the bond, so neither atom pulls the electrons closer to its nucleus.
Ionic bonds are formed between a metal and a nonmetal. Due to the dramatic difference between the electronegativities of metals and nonmetals, the electrons are pulled tightly to the nonmetal, and away from the metal nucleus. This results in each atom having a full octet, even though the electrons are not shared.
Carbon and oxygen are both nonmetals, so we would expect only covalent bonds in carbon dioxide.
Example Question #11 : Types Of Chemical Bonds
Which of the following is not a characteristic of ionic compounds?
Good conductors of electricity in the aqueous state
High melting point
High boiling point
Comprised of atoms sharing electrons
Comprised of atoms sharing electrons
Atoms share electrons in covalent bonds, not ionic. In ionic bonding, one or more electrons from an atom with a lower ionization energy are transferred to an atom with greater electron affinity.
Example Question #12 : Types Of Chemical Bonds
Which of the following statements best describes ionic compounds?
Formed when molecules share electrons
3-D arrays of charged particles
Malleable compounds that lack structural stability
Neutral particles that donate electrons
3-D arrays of charged particles
The definition of ionic compounds are three-dimensional arrays of atoms held together by strong ionic bonds. Ions are charged particles that have either gained or lost a certain number of electrons. They have great crystalline strength because of the strong electrostatic forces between the ions.
Example Question #81 : Compounds And Molecules
Which of the following contain(s) intramolecular hydrogen bonding?
I. NH3
II. HF
III. HCOH
IV. CH3CH2CH2OH
I only
I, II, IV
II and I
II and IV
I, II, III, IV
I, II, IV
H bonding is when a H is bonded to either N, O, or F. In the third molecule, the O is only double-bonded to the C; it is not bonded to a single H. All other choices have a N, O, or F bonded to a H
Example Question #82 : Compounds And Molecules
Which of the following best explains hydrogen bonding?
There are too many electrons in a solution, so H atoms interact with them
Electronegative atoms carry most of the electrons in the shared pairs when they are bonded to hydrogen
Hydrogen does not have any electrons
The covalent bonds between other atoms are hydrogen are called hydrogen bonds
Electronegative atoms carry most of the electrons in the shared pairs when they are bonded to hydrogen
Electronegative atoms disproportionately pull covalently bonded electrons toward themselves, which leaves hydrogen with partial positive character.
Example Question #83 : Compounds And Molecules
Hydrogen bonding can occur between which two molecules?
Methanol and methane
Methane and water
Water and hydrogen gas
Methanol and water
Hydrogen bonding can not occur between any of these combinations
Methanol and water
For hydrogen bonding to occur there must be a molecule with a hydrogen bonded to either F,O,N. This is present in water and methanol which both have O-H bonds. There can be hydrogen bonding between two water molecules, and there can be hydrogen bonding between two methanol molecules. The key to this problem is recognizing that it is asking for a situation in which hydrogen bonding is occuring between two separate molecules.
Hydrogen bonding is the association of a hydrogen and one of the three most electronegative elements F,O,N of neighboring molecules. The hydrogen, because it is bonded to one of these elements, aquires a partially positive charge, F,O, or N develops a partially negative charge. The partially positive hydrogen will associate, not bond, with the F,O, or N of a seperate molecule. Remeber that hydrogen bonding is an intermolecular property, so it is occuring between separate molecules.
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