Ch 13 Section 1 Flashcards

1
Q

solid compounds can be

A

ionic or molecular

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2
Q

in an ionic solid, a crystal structure is made up of .. held together by …

A

charged particles; ionic attractions

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3
Q

in a molecular solid, molecules are composed of

A

covalently bonded atoms

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4
Q

the solid is held togher by …, … forces

A

noncovalent; intermolecular

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5
Q

when they dissolve in water, ionic compounds and molecular compounds behave

A

differently

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6
Q

when a compound that is made of ions dissolves in water, the

A

ions separate from one another

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7
Q

this separation of ions that occurs when an ionic compound dissolves is called

A

dissociation

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8
Q

assuming 100% dissociation, a solution that contains 1 mol of sodium chloride contains .. of Na+ ions and … of Cl- ions

A

1 mol; 1 mol

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9
Q

a solution that contains 1 mol of calcium chloride contains .. of Ca2+ ions and … of Cl- ions

A

1 mol; 2 mol

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10
Q

although no ionic compound is completely insoluble, compounds of very low solubility can be considered … for most …

A

insoluble; practical purposes

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11
Q

it is difficult to write solubility rules that cover all

A

possible conditions

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12
Q

most sodium compounds are

A

soluble

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13
Q

most phosphates are

A

insoluble

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14
Q

dissociation equations cannot be written for

A

insoluble compounds

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15
Q

if the mixing results in a combination of ions that forms an insoluble compound, a … reaction and … will occur

A

double-displacement; precipitation

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16
Q

precipitation occurs when the attraction between the ions is greater than the attraction between the

A

ions and surrounding water molecules

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17
Q

to decide whether a precipitate can form, you must know the

A

solubilities of these two compounds

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18
Q

reactions of ions in aqueous solution are usually represented by … rather than…

A

net ionic equations; formula equations

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19
Q

a net ionic equation includes only those compounds and ions that undergo a

A

chemical change in a reaction in an aqueous solution

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20
Q

to write a net ionic equation, you first convert the chemical equation into an

A

overall ionic equation

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21
Q

all soluble ionic compounds are shown as

A

dissociated ions in solution

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22
Q

the precipitates are shown as

A

solids

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23
Q

ions that do not take part in a chemical reaction and are found in solution both before and after the reaction are

A

spectator ions

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24
Q

to convert an ionic equation into a net ionic equation, the … are … on both sides of the equation

A

spectator ions; canceled

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25
some molecular compounds can also form
ions in solution (polar compounds)
26
ions are formed from solute molecules by the action of the solvent in a process called
ionization
27
the more general meaning of ionization is the creation of
ions where there were none
28
when n ionic compound dissolves, the ions that were already present
separate from one another
29
when a molecular compound dissolves and ionizes in a polar solvent, ions are formed where
non existed in the undissolved compound
30
like all ions in aqueous solution, the ions formed by such a molecular solute are
hydrated
31
the energy released as heat during the hydration of the ions provides the energy needed to
break the covalent bonds
32
the extent to which a solute ionizes in solution depends on the strength of the bonds within the .. and the strength of attraction between the ...
molecules of the solute; solute and solvent molecules
33
if the strength of a bond within the solute molecule is weaker than the attractive forces of the solvent molecules, then the covalent bond of the solute ... and the ...
breaks; molecule is separated into ions
34
HCl is a molecular compound that
ionizes in aqueous solution
35
the attraction between a polar HCL molecule and the mpolar water molecules is strong enough to break the HCL bond, forming
hydrogen and chloride ions
36
many molecular compounds contain a hydrogen atom bonded by a
polar covalent bon d
37
some of these compounds ionize in an aqueous solution to release
H+
38
the H+ ion attracts other molecules or ions so strongly that it does not normally
exist alone
39
the ionization of hydrgoen chloride in water is better described a a chemical reaction in which a proton is transferred directly from HCl to awater molecule, where it becomes
covalently bonded to oxygen and forms H3O+
40
the H3O+ ion is known as the
hydronium ion
41
the reaction of the H+ ion to form the hydronium ion produces much of the energy needed to
ionize a molecular solute
42
substances that yield ions and conduct an electric current in solution are
electroylytes
43
substances that do not yield ions and do not conduct an electric current in solution are
nonelectrolytes
44
the hydrogen halides are all molecular compounds with single
polar-covalent bonds
45
all hydrogen halides are gases, all are very solubler in water, and all are
electrolytes
46
HCl, hydrogen bromide, and HI strongly conduct an
electric current in an aqueous solution
47
however, hydrogen fluoride only weakly conducts an electric current at the
same concentration
48
the strength with which substances conduct an electric current is related to their
ability to form ions in solution
49
HCL, hydrogen bromide, and hydrogen iodide are 100% ionized in
dilute aqueous solution
50
a strong electrolyte is any compound whose dilute aqueous solutions
conduct electricity well
51
the conductivity of strong electrolytes is due to the presence of all or almost all of the dissolved
compound in the form of ions
52
HCL, hydrogen bromide, and HI are all
acids in aqueous solution
53
these acids, several other acids, and all soluble ionic compounds are
strong electrolytes
54
the distinguishing feature of strong electrolytes is that to whatever extent they dissolve in water, they
yield only ions
55
for example, some strong electrolytes, such as NaCL, may be highly soluble in water and form
ions in solution
56
others may not dissolve much, but the amount that does dissolve exists solely as
ions in solution
57
some molecular compounds form aqueous solutions that contain not only dissolved ions but also some dissolved molecules that are not
ionized
58
HF dissolves in water to give an acidic solution known as
hydrofluoric acid
59
However, the HF bond is much stronger than the bonds between
hydrogen and other halogens
60
when HF dissolves, some molecules
ionize
61
but the reverse reaction--the transfer of H+ ions back to F- ions to form hydrogen fluoride molecules--
also takes place
62
hydrogen fluoride is an example of a
weak electrolyte
63
a weak electrolyte is any compound whose dilute aquous solutions conduct
electricity poorly
64
the poor conductivity of weak electrolytes is due to the presence of a small amount of the
dissolved compound in the form of ions
65
this is in contrast to a nonelectrolyte which dissolves but does not produce any
ions in solution
66
another example of a weak electolyte is CH3COOH,
acetic acid
67
the description of an electrolyte as strong or weak must not be confused with the description of a solution as
concentrated or dilute
68
strong and weak electolytes differ in the degree of
ionization or dissociation
69
concentrated and dilute solutions differ in the amount of
solute dissolved in a given quantity of a solvent
70
hydrochloric acid is always a
strong electrolyte
71
acetic acid is always considered a
weak electrolyte