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Bonding Brain Check
Chapter 6
62
Chemistry
Not Applicable
03/25/2004

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Term
What is a bond?
Definition
A uniting force or tie; a link.
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Term
What is a chemical bond?
Definition
A mutual attraction between the nuclei and valence electrons of different atoms that binds the atoms together.
Term
What are intramolecular bonds?
Definition
The forces of attraction that hold molecules together.
Term
List the four types of intramolecular bonds.
Definition
1. Non-polar covalent
2. Polar-covalent
3. Ionic
4. Metallic
Term
What is a nonpolar covalent bond?
Definition
A bond in which the bonded atoms have an equal attraction for shared electrons.
Term
What is a polar covalent bond?
Definition
A bond in which the bonded atoms have an unequal attraction for shared electrons.
Term
Differentiate between single, double, and triple bonds.
Definition
1. A single bond is produced by sharing only one pair of electrons.
2. A double bond is produced when two pairs of electrons are shared.
3. A triple bond is produced when three pairs of electrons are shared.
Term
What is bond strength?
Definition
A measure of the energy needed to break the bonds between atoms in molecules of a compound.
Term
How can you determine relative bond strength using ΔE?
Definition
The greater the differences in electronegativities, the greater the bond strength.
Term
How does bond energy (strength) compare to the number of bonds?
Definition
As the number of bonds increases, bond energy increases.
Term
How does bond energy compare to the length of bonds?
Definition
The longer the bond, the smaller the bond energy.
Term
What is an ion?
Definition
An atom or group of atoms with a charge.
Term
Differentiate between a cation and an anion.
Definition
A cation is a positive ion while an anion is a negative ion.
Term
What is an ionic bond?
Definition
The attraction for an anion and a cation after an electronis transferred from a metal to a nonmetal.
Term
Do metals gain or lose electrons?
Definition
Lose
Term
Do nonmetals gain or lose electrons?
Definition
Gain
Term
Which will have a greater electronegativity, a metal or a nonmetal?
Definition
Nonmetal
Term
What are valence electrons?
Definition
Outer-shell electrons
Term
Why are valence electrons important?
Definition
They are the ones involved in chemical reactions.
Term
What is the octet rule?
Definition
The octet rule refers to the tendency of atoms to prefer to have eight electrons in their valence shell.
Term
What is the magic number?
Definition
Eight
Term
Why is eight the magic number?
Definition
Eight is the magic number because most atoms need a full outer s sublevel and a full outer p sublevel. The numebr of electrons require to fill an s sublevel is two and to fill a p sublevel is 6. Two plus six equals eight.
Term
Are atoms with eight valence electrons more or less stable than atoms with less than eight valence electrons?
Definition
More
Term
Do ionic compounds have high or low melting and boiling points?
Definition
High
Term
Are most ionic compounds hard or soft?
Definition
Hard
Term
Are most ionic compounds brittle or not?
Definition
Brittle
Term
Will most ionic compounds conduct electricity?
Definition
No
Term
Do covalent compounds have high or low melting and boiling points?
Definition
Low
Term
Are most covalent compounds hard or soft?
Definition
Soft
Term
Will most covalent compounds conduct electricity?
Definition
No
Term
What is a metallic bond?
Definition
A bond where an atom achieves a more stable configuration by sharing electrons in its outer shell with many other atoms.
Term
Define ductile.
Definition
Easily drawn into wire.
Term
Define malleable.
Definition
Capable of being hammered into a thin sheet.
Term
Why are most metals ductile?
Definition
The distortion of being drawn into a thin wire does not disrupt the metallic bonding.
Term
Why are most metals malleable?
Definition
The distortion of being hammered into a thin sheet does not disrupt the metallic bonding.
Term
Define heat of vaporization.
Definition
The amount of heat required to convert a unit mass of a liquid at its boiling point into vapor without an increase in temperature.
Term
How does heat of vaporization relate to metallic bond strength?
Definition
As bond strength increases, heat of vaporization increases.
Term
Are metals loose or dense?
Definition
Dense
Term
Do metals have high or low melting and boiling points?
Definition
High
Term
Are metals good or poor conductors of heat?
Definition
Good
Term
Are metals good or poor conductors of electricity?
Definition
Good
Term
Are metals dull or lustrous?
Definition
Lustrous
Term
Define electronegativity.
Definition
The ability of an atom to attract the electron density to itself.
Term
What are the units for electronegativity?
Definition
There are no units.
Term
Who created the first scale of electronegativity?
Definition
Linus Pauling
Term
What was the first scale of electronegativity based on?
Definition
Energy required to break bonds and the dipole moments of molecules.
Term
Tell how electronegativity differences are used to predict bond type.
Definition
1. A difference of 1.7 or above is ionic.
2. A difference of 0.5-1.6 is polar covalent.
3. A difference of less than 0.5 is nonpolar covalent.
Term
What are oxidation numbers?
Definition
The charge that atom would have if the compound was composed of ions.
Term
What is the criss-cross method for predicting chemical formulas?
Definition
It is a method where you use the oxidation numbers of any two ions to easily determine the chemical formula.
Term
What are the steps for using the criss-cross method for determining the chemical formula?
Definition
1. Write the symbol for the more metallic element first. Then, write the symbol for the non-metallic element.
2. Write the combining capacities for the elements.
3. Subscripts are used to indicate the number of atoms each element has in that compound. (if the element has only one atom, then no subscript is needed for that element) Then, criss-cross the number of the combining capacity.
Term
Define intermolecular bond.
Definition
The force of attraction between molecules.
Term
List the four types of intermolecular bonds.
Definition
1. Dipole-dipole forces
2. Hydrogen bonding
3. London dispersion forces
4. Ion-dipole forces
Term
Define dipole-dipole forces.
Definition
The forces of attractions between two polar molecules.
Term
Define hydrogen bonding.
Definition
A low-energy attractive force between hydrogen and another element. It plays a major role in determining the properties of water, proteins, and other compounds.
Term
Define London dispersion forces.
Definition
The forces that exist in nonpolar molecules that involve an accidental dipole that induces a momentary dipole in a neighbor.
Term
Define ion-dipole forces.
Definition
An ion-dipole force is an attractive force that results from the electrostatic attraction between an ion and a neutral molecule that has a dipole.
Term
What is the definition of the prefix "intra?"
Definition
Within
Term
What is the definition of the prefix "inter?"
Definition
Between
Term
Arrange the following in order from lowest melting point to highest: ionic, metallic, non-polar covalent, polar covalent.
Definition
non-polar covalent
Term
Arrange the following in order from lowest boiling point to highest: ionic, metallic, non-polar covalent, polar covalent.
Definition
non-polar covalent
Term
Define cation.
Definition
A positive ion.
Term
Define anion.
Definition
A negative ion.
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