Term
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Definition
A uniting force or tie; a link.
(www.dictionary.com) |
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Term
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Definition
| A mutual attraction between the nuclei and valence electrons of different atoms that binds the atoms together. |
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Term
| What are intramolecular bonds? |
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Definition
| The forces of attraction that hold molecules together. |
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Term
| List the four types of intramolecular bonds. |
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Definition
1. Non-polar covalent
2. Polar-covalent
3. Ionic
4. Metallic |
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Term
| What is a nonpolar covalent bond? |
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Definition
| A bond in which the bonded atoms have an equal attraction for shared electrons. |
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Term
| What is a polar covalent bond? |
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Definition
| A bond in which the bonded atoms have an unequal attraction for shared electrons. |
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Term
| Differentiate between single, double, and triple bonds. |
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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. |
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Term
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Definition
| A measure of the energy needed to break the bonds between atoms in molecules of a compound. |
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Term
| How can you determine relative bond strength using ΔE? |
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Definition
| The greater the differences in electronegativities, the greater the bond strength. |
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Term
| How does bond energy (strength) compare to the number of bonds? |
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Definition
| As the number of bonds increases, bond energy increases. |
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Term
| How does bond energy compare to the length of bonds? |
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Definition
| The longer the bond, the smaller the bond energy. |
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Term
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Definition
| An atom or group of atoms with a charge. |
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Term
| Differentiate between a cation and an anion. |
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Definition
| A cation is a positive ion while an anion is a negative ion. |
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Term
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Definition
| The attraction for an anion and a cation after an electronis transferred from a metal to a nonmetal. |
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Term
| Do metals gain or lose electrons? |
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Definition
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Term
| Do nonmetals gain or lose electrons? |
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Definition
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Term
| Which will have a greater electronegativity, a metal or a nonmetal? |
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Definition
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Term
| What are valence electrons? |
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Definition
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Term
| Why are valence electrons important? |
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Definition
| They are the ones involved in chemical reactions. |
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Term
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Definition
| The octet rule refers to the tendency of atoms to prefer to have eight electrons in their valence shell. |
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Term
| What is the magic number? |
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Definition
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Term
| Why is eight the magic number? |
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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. |
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Term
| Are atoms with eight valence electrons more or less stable than atoms with less than eight valence electrons? |
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Definition
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Term
| Do ionic compounds have high or low melting and boiling points? |
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Definition
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Term
| Are most ionic compounds hard or soft? |
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Definition
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Term
| Are most ionic compounds brittle or not? |
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Definition
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Term
| Will most ionic compounds conduct electricity? |
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Definition
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Term
| Do covalent compounds have high or low melting and boiling points? |
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Definition
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Term
| Are most covalent compounds hard or soft? |
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Definition
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Term
| Will most covalent compounds conduct electricity? |
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Definition
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Term
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Definition
| A bond where an atom achieves a more stable configuration by sharing electrons in its outer shell with many other atoms. |
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Term
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Definition
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Term
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Definition
| Capable of being hammered into a thin sheet. |
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Term
| Why are most metals ductile? |
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Definition
| The distortion of being drawn into a thin wire does not disrupt the metallic bonding. |
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Term
| Why are most metals malleable? |
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Definition
| The distortion of being hammered into a thin sheet does not disrupt the metallic bonding. |
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Term
| Define heat of vaporization. |
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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. |
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Term
| How does heat of vaporization relate to metallic bond strength? |
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Definition
| As bond strength increases, heat of vaporization increases. |
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Term
| Are metals loose or dense? |
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Definition
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Term
| Do metals have high or low melting and boiling points? |
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Definition
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Term
| Are metals good or poor conductors of heat? |
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Definition
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Term
| Are metals good or poor conductors of electricity? |
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Definition
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Term
| Are metals dull or lustrous? |
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Definition
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Term
| Define electronegativity. |
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Definition
| The ability of an atom to attract the electron density to itself. |
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Term
| What are the units for electronegativity? |
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Definition
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Term
| Who created the first scale of electronegativity? |
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Definition
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Term
| What was the first scale of electronegativity based on? |
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Definition
| Energy required to break bonds and the dipole moments of molecules. |
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Term
| Tell how electronegativity differences are used to predict bond type. |
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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. |
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Term
| What are oxidation numbers? |
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Definition
| The charge that atom would have if the compound was composed of ions. |
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Term
| What is the criss-cross method for predicting chemical formulas? |
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Definition
| It is a method where you use the oxidation numbers of any two ions to easily determine the chemical formula. |
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Term
| What are the steps for using the criss-cross method for determining the chemical formula? |
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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. |
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Term
| Define intermolecular bond. |
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Definition
| The force of attraction between molecules. |
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Term
| List the four types of intermolecular bonds. |
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Definition
1. Dipole-dipole forces
2. Hydrogen bonding
3. London dispersion forces
4. Ion-dipole forces |
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Term
| Define dipole-dipole forces. |
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Definition
| The forces of attractions between two polar molecules. |
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Term
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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. |
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Term
| Define London dispersion forces. |
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Definition
| The forces that exist in nonpolar molecules that involve an accidental dipole that induces a momentary dipole in a neighbor. |
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Term
| Define ion-dipole forces. |
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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. |
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Term
| What is the definition of the prefix "intra?" |
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Definition
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Term
| What is the definition of the prefix "inter?" |
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Definition
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| Arrange the following in order from lowest melting point to highest: ionic, metallic, non-polar covalent, polar covalent. |
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Definition
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Term
| Arrange the following in order from lowest boiling point to highest: ionic, metallic, non-polar covalent, polar covalent. |
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