| Term | Definition |
|---|
| chemical bond | the force of attraction between any two atoms in a compound |
| lewis symbol or structure | a way to represent atoms using the element symbol and valence electrons as dots |
| ionic bond | a transfer of one or more electrons from one atom to another |
| why does an ionic bond work as a bond? | the opposite charges of the atoms and eagerness to either give up or gain an electron |
| covalent bond | attractive force due to the sharing of electrons between atoms |
| metals tend to form ionic bonds with ______, and vice versa | nonmetals |
| atoms with low ie and low ea tend to form | positive ions |
| atoms with high ie and high ea tend to form | negative ions |
| metals tend to have ____ i.e. and e.a. | low |
| nonmetals tend to have ____ i.e. and e.a. | high |
| ionic substances form | crystallized solids |
| overlapping orbitals in covalent bonds _____________, making the density and probability of finding the electrons there _____ | reinforce each other, greater |
| what effect do nonbonded electron pairs have on the molecule? | they distort the shape slightly |
| pure covalent bond | the sharing of electrons is equal |
| what types of molecules have pure covalent bonds? | homonuclear diatomic molecules |
| polar covalent bond | bonds made up of unequally shared electron pairs |
| in a polar covalent bond, the electrons are pulled a little more towards | the atom with more electrons originally |
| delta(-) | partial negative charge |
| delta(+) | partial positive charge |
| electronegativity | a measure of the ability of an atom to attract electrons in a chemical bond |
| the most electronegative element | F |
| the two naming systems | ionic compounds and covalent compounds |
| short cut for ionic compound formulas | swap one charge for the other and place in subscript |
| what is the one thing to watch out for with the ionic compound formula short cut? | simplify |
| which element goes first, typically? | the metal/cation |
| the ionic compound formula for naming | the name of the positive ion + the anion suffix+ide |
| stock notation is used for | transition metals |
| oxidation state | charge |
| common nomenclature is used for | transition metals |
| common nomenclature -ic describes | the higher of the charges that an ion might have |
| common nomenclature -ous describes | the lower of the charges that an ion might have |
| monatomic ions | ions consisting of a single charged atom |
| hydrogen ion | H+ |
| hydride ion | H- |
| ions from atoms in group 1a will all have a charge of: | 1+ |
| ions from atoms in group 2a will all have a charge of: | 2+ |
| aluminom ion | Al3+ |
| silver ion | Ag+ |
| ions from atoms in group 7a will all have a charge of: | 1- |
| ions from atoms in group 6a will all have a charge of: | 2- |
| charge of the Nitride ion | 3- |
| charge of the Phosphide ion | 3- |
| for monatomic ions, naming it the same as its elemental name means that it has a _____ charge | positive |
| for monatomic ions, giving it the suffix -ide means that it has a _____ charge | negative |
| polyatomic ions | ions composed of 2 or more atoms bonded together with an overall positive or negative charge |
| within a polyatomic ion, there are _____ bonds | covalent |
| the positive and negative ions of polyatomic ions bond with ______ bonds | ionic |
| the only polyatomic ion with a positive charge | NH(4)+ |
| the suffix of -ate in a polyatomic ion | the one with more oxygens |
| the suffix of -ite in a polyatomic ion | the one with fewer oxygens |
| the prefix hypo- in a polyatomic ion | the one with the fewest oxygens |
| the prefix of per- in a polyatomic ion | the one with the most oxygens |
| the charges of polyatomic ions of the same atom ___________ | never change |
| ammonium | NH(4)+ |
| Nitrite | NO(2)- |
| Nitrate | NO(3)- |
| Sulfite | SO(3)2- |
| Sulfate | SO(4)2- |
| Hydroxide | OH- |
| Cyanide | CN- |
| Phosphate | PO(4)3- |
| Carbonate | CO(3)2- |
| Bicarbonate | HCO(3)- |
| Hypochlorite | ClO- |
| Chlorite | ClO(2)- |
| Chlorate | ClO(3)- |
| Perchlorate | ClO(4)- |
| Acetate | CH(3)COO- [aka CH(3)CO(2)-] |
| Permanganate | MnO(4)- |
| Dichromate | Cr(2)O(7)2- |
| Chromate | CrO(4)2- |
| covalent compounds are typically formed from | nonmetals |
| molecules | compounds characterized by covalent bonding |
| are molecules part of a massive 3-D crystal structure? | no |
| covalent compound prefix for 1 atom | mono |
| covalent compound prefix for 2 atoms | di |
| covalent compound prefix for 3 atoms | tri |
| covalent compound prefix for 4 atoms | tetra |
| covalent compound prefix for 5 atoms | penta |
| covalent compound prefix for 6 atoms | hexa |
| covalent compound prefix for 7 atoms | hepta |
| covalent compound prefix for 8 atoms | octa |
| covalent compound prefix for 9 atoms | nona |
| covalent compound prefix for 10 atoms | deca |
| H(2)O | water |
| NH(3) | ammonia |
| C(2)H(5)OH | ethanol |
| C(6)H(12)O(6) | glucose |
| carbon almost always makes ___ bonds in a compound | 4 |
| ionic compounds are usually ____ at room temperature, and why? | solids, high attraction keeps them together |
| covalent compounds are usually ____ at room temperature, and why? | any of the three states, it varies depending on the level of attraction |
| melting point | the temperature at which a solid is converted to a liquid |
| boiling point | the temperature at which a liquid is converted to a gas |
| which type of compound has the higher melting and boiling points on average? | ionic |
| the two structures that covalent compounds can take as solids | crystalline and amorphous |
| ionic compounds _______ in water | dissociate |
| dissociation | the process by which ionic compounds dissolve in water to form positive and negative ions |
| electrolytes | ions present in a solution, allowing the solution to conduct electricity |
| nonelectrolytes | dissolved substances from covalent compounds that do not conduct electricity |
| aqueous solution | in water |
| trends in drawing structures of molecules and polyatomic ions | least electronegative atom is in the center, hydrogen and halogens occupy terminal positions, and carbon often forms chains of carbon-carbon covalent bonds |
| steps for drawing the structure of molecules and polyatomic ions | 1. Determine the number of electrons that each atom needs in order to reach a full octet (H=2, others=8) 2. Determine the total number of electrons that each atom already has. 3. Subtract the sum of 2 from the sum of 1 to find the total number of electrons that must be shared. 4. Divide the shared electrons by 2 to determine how many bonds will be involved |
| what is the difference between drawing the structure of a neutral compound vs. a polyatomic ion? | you must account for the charge in the polyatomic |
| is the charge of the polyatomic ion attached to any one atom? | no |
| what step is adding to the process of drawing the structure of a polyatomic ion? | you must add or subtract electrons from the total number available to account for the charge |
| what is the most stable bond? | triple |
| bond energy | the amount of energy required to break a bond holding two atoms together |
| what type of bond has the most bond energy? | triple |
| bond length | the distance separating the nuclei of two adjacent atoms |
| what type of bond has the longest bond length? | single |
| what happens to the p orbital shape with double and triple bonds? | it distorts as the atoms/nuclei move closer together |
| with a molecule/compound liek CO(3)2-, where is the double bond? | stretched out over the entire molecule |
| resonance | two or more lewis structures that contribute to the real structure |
| incomplete octet | less than eight electrons around an atom other than H |
| odd electron | if there is an odd number of valence electrons it is not possible to give every atom eight eectrons |
| what is another name for odd electrons? | free radicals |
| expanded octet | an element in the third period or below that may have 10 or 12 electrons around it |
| VSEPR Theory | all electrons around the central atom arrange themselves so they can be as far away from each other as possible to minimize electron |
| VSEPR Theory: in the covalent bond, bonding electrons are localized: | around the nucleus |
| VSEPR Theory: the covalent bond is ________ | directional, having a specific orientation in space between the bonded atoms |
| ionic bonds have _________, which ______ | electrostatic forces, have no specific orientation in space |
| are ionic solids always nonpolar or polar? | polar |
| linear structure | straight line, planar, 180 degrees |
| trigonal planar structure | triangle, planar, 120 degrees |
| tetrahedron is the ____________ | primary structure of a full octet |
| tetrahedron structure | forming a pyramid with a bonded pair at each corner, 109.5 degrees |
| is a lone pair more or less electronegative than a bonded pair? | more |
| trigonal pyramidal structure | exactly like a tetrahedron, but with an unbonded pair at the top, 107 degrees |
| bent/angular structure | exactly like a tetrahedron but with only two bonded pairs, 104.5 degrees |
| lone pairs only matter when they're | on the central atom |
| if no lone pairs are present and there are 2 shared pairs, the shape is | linear |
| if no lone pairs are present and there are 3 shared pairs, the shape is | trigonal planar |
| if no lone pairs are present and there are 4 shared pairs, the shape is | tetrahedral |
| when is a molecule polar? | when its centers of positive and negative charges do not coincide |
| if a compound is a gas under normal conditions then it is (polar/nonpolar) | nonpolar |
| intramolecular force | an attractive force within a molecule |
| intermolecular force | an attractive force between molecules |
| ________ forces are a direct consequence of the ______ forces of the molecules | intermolecular, intramolecular |
| solubility | the maximum amount of solute that dissolves in a given amount of solvent at a specfiic temperature |
| what is the rule of solubility? | like dissolves like |
| what exactly is a hydrogen bond? | when bonds are so polar that the hydrogen can start to share with another atom/pair |
| the more attraction, the _____ the energy needed to break it apart | higher |
| how does molecular mass impact m.p and b.p? | the higher the mass, the higher the m.p. and b.p. because it's more difficult to convert a larger mass to another phase |
| how does polarity impact mp and bp? | polar molecules have higher mp and bp than nonpolar molecules of similar molecular mass because the polar molecules have stronger attractive forces |
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