Exam 2 Flashcards
1
Q
naming compounds: binary compounds
A
- composed of 2 elements
- divided into broad classes
- compounds that contain a metal & non-metal (ionic)
- compounds that contain 2 non-metals (covalent)
2
Q
nomenclature
A
naming
3
Q
naming compounds: binary ionic compounds
A
- contains (+) cations and (-) anions
- type 1
- type 2
4
Q
binary ionic compounds: type 1
A
-metal and non-metal
-compounds
-fixed charges
-metal present forms only 1 cation
consists of:
-alkali metals
-alkaline earth metals
-Al3+
-Ga3+
-In3+
-Zn2+
-Ag+
5
Q
binary ionic compounds: type 2
A
- metal and non-metal
- compounds
- no fixed charge
- need roman numerals (indicates charge of metal cation)
- charge of metal ion must be specified
- metal present can form 2 or more cations w diff charges
- consists of: transitional metals
6
Q
naming type 1 binary ionic compounds
A
- cation is always named first (element name)
- anion named second (end in -ide)
7
Q
examples of type 1 binary ionic compounds
A
NaCl: sodium chloride CaS: calcium sulfide Kl: potassium iodide SrI2: strontium iodide ZnS: zinc sulfide CaBr2: calcium bromide aluminum sulfide: Al2S3 Rb2O: rubidium oxide
8
Q
what is the name of SrB2?
A
strontium bromide
9
Q
what is the name of K2S?
A
potassium sulfide
10
Q
naming type 2 binary ionic compounds
A
- cation always named 1st
- anion named 2nd (-ide)
- charge of cation is specified by roman numeral
11
Q
examples of type 2 binary ionic compounds
A
CuBr: copper (I) bromide FeS: iron (II) sulfide PbO2: lead (IV) oxide MnI2: manganese (II) iodide CoCl3: cobalt (III) chloride CuI: copper (I) iodide tin (IV) bromide: SnBr4
12
Q
name CrO2
A
chromium (IV) oxide
13
Q
name chromium (II) fluoride
A
CrF2
14
Q
what is the correct name of the compound that results from the most stable ion for sulfur & the metal ion that contains 24 e-?
A
iron (II) sulfide
15
Q
binary compounds: type 3
A
- non-metal and non-metal
- greek prefixes to denote the # of atoms of each element
16
Q
naming type 3 binary compounds
A
- 1st element named first & full element name is used
- 2nd element is named as though it were an anion
- prefixes are used to denote # of atoms present
- prefix mono- is never used for naming the 1st element
17
Q
prefixes used to indicate numbers in chemical names
A
prefix number mono- 1 di- 2 tri- 3 tetra- 4 penta- 5 hexa- 6 hepta- 7 octa- 8 nona- 9* deca- 10*
18
Q
examples of type 3 binary covalent compounds
A
CO2: carbon dioxide SF6: sulfur hexafluoride N2O4: dinitrogen tetroxide CO: carbon monoxide NO2: nitrogen dioxide selenium hexafluoride: SeF6 PCl5: phosphorus pentachloride dinitrogen monoxide: N2O
19
Q
name SeO2
A
selenium dioxide
20
Q
common type 2 cations
A
ion systemic name Fe3+ iron (III) Fe2+ iron (II) Cu2+ copper (II) Cu+ copper (I) Co3+ cobalt (III) Co2+ cobalt (II) Sn4+ tin (IV) Sn2+ tin (II) Pb4+ lead (IV) Pb2+ lead (II) Hg2+ mercury (II) Hg2 2+ mercury (I)
21
Q
polyatomic ions
A
charged entities composed of several atoms bound together
- have special names
- *MUST MEMORIZE**
22
Q
oxyanions
A
polyatomic anions exist that contain an atom of a given element and diff #s of oxygen atoms
23
Q
examples of polyatomic ions
A
NaOH: sodium hydroxide Mg(NO3)2: magnesium nitrate (NH4)2SO4: ammonium sulfate Fe3(PO4)2: iron (II) phosphate Ca(HCO3)2: calcium bicarbonate potassium permanganate: KMnO4 Fe(OH)2: iron (II) hydroxide antimony (III) oxide: Sb2O3
24
Q
name KClO
A
potassium hypochlorite
25
give the formula of ammonium acetate
NH4C2H3O2
26
name KClO3
potassium chlorate
27
```
which are named correctly?
Formula Name
I P2O5 diphosphorus pentoxide
II ClO2 chlorine oxide
III PbI4 lead iodide
IV CuSO4 copper (I) sulfate
```
I only
28
acids
- certain mols. produce H+ ions when dissolved in H2O
- can be recognized by the H that appears 1st in formula
- mol. w/1 or more H+ ions attached to an anion
29
rules for naming acids
- if the anion DOESN'T HAVE an oxygen, the acid is named w/ the prefix hydro- and the suffix -ic attached to root of element name
- if anion DOES HAVE an oxygen, the acid name is formed from the root element name w/ the suffix -ic or -ous after it
* *ALL END IN "acid"**
- ate = -ic
- ite = -ous
30
examples of naming acids
```
HCl: hydrochloric acid
HCN: hydrocyanic acid
H2S: hydrosulfuric acid
HF: hydrofluoric acid
H3PO4: phosphoric acid
H2S: hydrosulfuric acid
nitric acid: HNO3
H2SO4: sulfuric acid
HC2H3O2: acetic acid
```
31
names of acids without O
```
ACID NAME
HF hydrofluoric acid
HCl hydrochloric acid
HBr hydrobromic acid
HI hydroiodic acid
HCN hydrocyanic acid
H2S hydrosulfuric acid
```
32
names of some acids with O
```
ACID NAME
HNO3 nitric acid
HNO2 nitrous acid
H2SO4 sulfuric acid
H2SO3. sulfurous acid
H3PO4 phosphoric acid
HC2H3O2 acetic acid
```
33
which of the following is named incorrectly?
a) KNO3 = potassium nitrate
b) TiO2 = titanium (II) oxide
c) Sn(OH)4 = tin (IV) hydroxide
d) PBr5 = phosphorous pentabromide
e) H2SO3 = sulfurous acid
B
34
a compound has the formula Xcl3 where X could represent a metal or a non-metal. What could the name of this compound be?
phosphorus trichloride
35
writing formulas from names
- essential to know formula of a compound from its name
- important to learn name, composition, and charge of each common polyatomic anions (and the NH4+ cation)
- must learn names of common acids
36
more nomenclature examples
```
NaOH: sodium hydroxide
potassium carbonate: K2CO3
sulfuric acid: H2SO4
dinitrogen pentoxide: N2O5
cobalt (III) nitrate: Co(NO3)3
```
37
NH4 +
ammonium
38
NO2 -
nitrite
39
NO3 -
nitrate
40
SO3 2-
sulfite
41
SO4 2-
sulfate
42
HSO4 -
hydrogen sulfate/bisulfate
43
OH -
hydroxide
44
CN -
cyanide
45
PO4 3-
phosphate
46
HPO4 2-
hydrogen phosphate
47
H2PO4 -
dihydrogen phosphate
48
CO3 2-
carbonate
49
HCO3 -
hydrogen carbonate/bicarbonate
50
ClO -
hypochlorite
51
ClO2 -
chlorite
52
ClO3 -
chlorate
53
ClO4 -
perchlorate
54
C2H3O2 -
acetate
55
MnO4 -
permanganate
56
Cr2O7 2-
dichromate
57
O2 2-
peroxide
58
clues that a chemical rxn has occurred
1) the colors change
2) a solid forms
3) bubbles form
4) heat and/or a flame is produced, or heat is absorbed
59
chemical equations
- represents a chemical rxn
- reactants on left of arrow, products on right
- arrow means yield
- atoms are neither created nor destroyed
- all atoms present in the reactants must be accounted for among the products
- there must be the same # of each type of atoms on both sides of arrow
60
balancing a chemical equation
- coefficients balance rxn
- sum of coefficients
* diatomic mols ∆ eq
1) atoms are neither created nor destroyed
2) can never ∆ subscripts in a complete rxn
3) reactants -> products
61
physical states
- physical states of compounds are often given in a chem equation
states: s, l, g, aq
62
how to write + balance equations
- read description of chm rxn
- identify reactants, products, and their states
- write apprp formulas
- write unbalanced eq that summarizes the info from previous step
- balance the equation by inspection, starting w/ most complicated mol
- should finish w/ the same # of molecules on both sides of arrow
63
in the context of balancing a chem eq, which of the following statements is false?
subscripts in the reactants must be conserved in the products
64
of the 3 that are correct, which one is preferred most?
| CaO + C -> CaC2 + CO2
II is preferred
65
balance the following eq & find the sum of the coefficients:
FeO (s) + O2 (g) -> Fe2O3 (s)
```
4 FeO (s) + 1 O2 (g) -> 2 Fe2O3 (s)
sum: 7
```
66
balance & find the sum of the coefficients:
| NH3 (g) + HCl (g) -> NH4Cl (s)
```
1 NH3 (g) + 1 HCl (g) -> 1 NH4Cl (s)
sum: 3
```
67
When blue light shines on a mixture of hydrogen gas and chlorine gas, the elements react explosively to form gaseous hydrochloric acid. What is the unbalanced equation for this process?
H2(g) + Cl2(g) -> HCl(g)
68
identify a clue that indicates a reaction has occurred in the statement and in the given image “A solid forms when a solution of sodium dichromate is added to a solution of lead nitrate”
a solid forms
69
Identify a clue that indicates a reaction has occurred in the statement and in the given image “Colorless hydrochloric acid is added to a red solution of cobalt(II) nitrate, turning the solution blue”
color changes
70
what does a balanced chemical equation tell us?
the ratio of the # of molecules that react & are produced in a chemical rxn
71
4 driving forces favor chm change
- formation of a solid
- formation of water
- transfer of e-
- formation of a gas
72
precipitation
the process of formation of a solid during a chm rxn
- the solid formed is a precipitate
- rxn known as precipitation rxn
73
precipitate
the solid formed during a precipitation rxn
| *exchange cations & anions
74
what happens when an ionic compound dissolves in water?
- ions separate & move around independently
| - ions separate when the solid dissolves
75
strong electrolyte
substance whose each unit produces separated ions when dissolved in water
76
how to decide what products form
exchange of cations binding to anions
| *switch
77
soluble
can dissolve in water
| aq
78
slightly soluble/moderately soluble basically means __
insoluble
79
how to predict precipitates when solutions of 2 ionic compounds are mixed
- write reactants as they exist b4 any rxn occurs
- remember when a salt dissolves, its ions separate
- consider various solids that could form from this collection of ions in sol
a) simply exchange anions of added salts
80
which ion reacts with Pb2+ to form compounds generally soluble in water?
NO3-
81
A solution of sodium phosphate reacts with a solution of lead(II) nitrate. What precipitate, if any, will form?
Pb3(PO4)2
82
what are the 3 types of equations for rxns in aqueous solutions?
- molecular
- complete ionic
- net ionic
83
molecular equation
- shows complete formulas of all reactants and products
- doesn't give a very clear picture of what actually occurs in solution
- consists of mols are a whole
84
complete ionic equation
- all substances that are strong electrolytes are represented as ions
- spectator ions
85
spectator ions
ions that don't participate directly in a rxn in sol
| * the ions that cancel out
86
net ionic equation
- includes only those components that are directly involved in the rxn
- spectator ions not included
- order doesn't matter
- should always be balanced
87
Write the correct molecular equation, the complete ionic equation, and the net ionic equation for the reaction between cobalt(II) chloride and sodium hydroxide
molecular: CoCl2 (aq) + 2 NaOH (aq) -> Co(OH)2 (s) +2 NaCl (aq)
complete ionic: Co2+ (aq) + 2 Cl- (aq) + 2 Na+ (aq) + 2 OH- (aq) -> Co(OH)2 (s) + 2 Na+ (aq) + 2 Cl- (aq)
net ionic: Co2+ (aq) + 2 OH- (aq) -> Co(OH)2 (s)
88
what are the 7 strong acids?
1) H2SO4 = sulfuric acid
2) HCl = hydrochloric acid
3) HBr = hydrobromic acid
4) HI = hydroiodic acid
5) HNO3 = nitric acid
6) HClO4 = perchloric acid
7) HClO3 = chloric acid
89
soluble compounds
1) NO3- salts
2) Na+, K+, NH4+ salts
3) Cl-, Br-, I- salts except for those w/ Ag+, Hg2 2+, Pb2+
4) SO4 2- salts except for those w/ Ba2+, Pb2+, Ca2+
90
insoluble compounds
1) S2-, CO3 2-, PO4 3- salts
| 2) OH- salts except for those w/ Na+, K+, Ba2+, Ca2+
91
strong acid
a strong electrolyte that produces H+ ions (protons) when it is dissolved in water
92
acids give __ to bases; bases accept __ and give __ to acids
H+; H+; OH-
93
is an acid and base is a good relationship?
yes
94
an acid and base always make __ and __
water; a salt
95
strong base
a substance that produces hydroxide ions (OH-) in water
96
examples of strong bases
NaOH and KOH
97
when writing equations, you can never break apart __ and __
solids; liquids
98
what are the strong bases?
Group 1
Group 2
+
OH-
99
the net ionic equation for the rxn of a strong acid and a strong base is always the production of __
water
100
net ionic equation for HNO3 and LiOH
H+ + OH- -> H2O
101
when finding the mass of a compound just look on the __
periodic table
102
mole
the # equal to the # of C atoms in 12.01 g of C
103
Avogadro's number
6.022 x 10^23
104
1 mole of anything =
6.022 x 10^23 atoms of that thing
105
how many atoms are in 1.008g of H?
6.022 x 10^23 atoms
106
determine the number of copper atoms in a 63.55g sample of copper
6.022 x 10^23 Cu atoms
107
which is closest to the avg mass of 1 atom of copper
1.055 x 10^-22 g Cu
1 Cu atom x 1 mol Cu/6.022 x 10^23 Cu atoms x 63.55g Cu/1 mol Cu = 1.055 x 10^-22 g Cu
108
calculate the # of Fe atoms in a 4.48 mole sample of Fe
2. 70 x 10^24 Fe atoms
| 4. 48 mol Fe x 6.022 x 10^23 atoms Fe/1 mol Fe = 2.70 x 10^24 Fe atoms
109
a sample of 26.98 g of Al has the same # of atoms as __ g of Au
197.0
110
molar mass
mass in grams of a substance
unit: g/mol
- coefficients don't count, only subscripts
111
find the molar mass of Ba(NO3)2
261. 35 g/mol
| 137. 33 g + (2 x 14.01g) + (6 x 16.00g)
112
when finding the molar mass and determining sig figs, always use numbers from __
periodic table
113
mole of a compound
mass of sample (g) / molar mass of compound (g/mol)
114
mass of a sample
moles of sample (mol) x molar mass of compound (g/mol)
115
what is the molar mass of nickel (II) carbonate
118.7 g/mol
NiCO3
58.69 + 12.01 + 3 x 16.00 = 118.7 g/mol
116
how many grams of fluorine are present in one molecule of boron trifluoride (molecules to grams) ?
9.465 x 10^-23 g
1 molecule BF3 x 3 atoms F/1 molecule BF3 x 1 mol F/6.022 x 10^23 atoms F x 19.00g F/1 mol F= 9.465 x 10^23 g
117
how many grams of chlorine gas are present in 5.65 moles?
5.65 moles x 2 (35.45g)/1 mole = 400 g
118
how many moles of KNO3 are present in 17.38 g?
0. 172 moles
| 17. 38g x 1 mole/101 g/mol = 0.172 moles
119
how many molecules of O2F2 are in 3.44 moles?
2. 072 x 10^24 molecules
| 3. 44 moles x 6.022 x 10^23 molecules / 1 mole = 2.072 x 10^24 molecules
120
conversions with mass, moles, and atoms
* atoms or molecules -> moles = MULTIPLY avogadro's #
* moles -> atoms or molecules = DIVIDE avogadro's #
* moles -> grams = MULTIPLY molar mass
* grams -> moles = DIVIDE molar mass
121
conversion trick
```
K H D b D C M
king henry died by drinking chocolate milk
km, hm, Dm, base unit (m, L, g), cm, mm
kilo: 1000
hecto: 100
deca: 10
U: unit
deci: 0.1
centi: 0.01
milli: 0.001
*micro: 0.000001 or 10^-6
*nano: 0.000000001 or 10^-9
```
122
mass percent of an element in a compound
mass of element present in 1 mole of compound / mass of 1 mole of compound
123
morphine, derived from opium plants, has the potential for use and abuse. Its formula is C17H19NO3. Determine the percent of mass for carbon in this compound
71.6% C
(17 x 12.01) / [(17 x 12.01) + (19 x 1.01) + (1 x 14.01) + (3 x 16.00)] = 0.716 x 100 = 71.6%
124
empirical formula
formula of a compound that expresses the smallest whole-number ratio of the atoms present
-simplest whole-number ratio
125
molecular formula
the exact formula of the molecules present in a substance
(empirical formula)n
*n is an integer
*always bigger than empirical formula
126
how to find the empirical formula
assume 100 g and change % to g
convert g to mol
divide by lowest number
round any decimals
127
how to find the molecular formula
- use the molar mass given and divide by the molar mass from ur new empirical formula
- use the number to multiply the empirical formula
128
do diatomics or sig figs matter in empirical/molecular formulas?
no
129
Each molecule of ethanol, for instance, contains two carbon atoms, six hydrogen atoms, and one oxygen atom. Find the molar mass
C2H5OH
mass of C: 2 mol x 12.01 g/mol = 24.02 g
mass of H: 6 mol x 1.008 g/mol = 6.048 g
mass of O: 1 mol x 16.00 g/mol = 16.00 g
mass of 1 mole of C2H5OH = 46.07g = molar mass
130
A gaseous compound containing carbon and hydrogen was analyzed and found to consist of 83.65% carbon by mass. Determine the empirical formula of the compound.
C3H7
131
The composition of adipicacid is 49.3% C, 6.9% H, and 43.8% O (by mass). What is the empirical formula?
C3H5O2
132
A gaseous compound containing carbon and hydrogen was analyzed and found to consist of 83.65% carbon by mass. The molar mass of the compound is 86.2 g/mol. The empirical formula was determined to be C3H7. What is the molecular formula of the compound?
C6H14
molar mass of C3H7 = 43.086 g/mol
86.2 g/mol / 43.086 g/mol = 2
(C3H7) x 2 = C6H14
133
The composition of adipicacid is 49.3% C, 6.9% H, and 43.8% O (by mass). The molar mass of the compound is about 146 g/mol. The empirical formula is C3H5O2. What is the molecular formula?
C6H10O4
134
When 1.00 g of metallic chromium is heated with elemental chlorine gas, 3.045 g of a chromium chloride salt results. Calculate the empirical formula of the compound.
CrCl3
1.00g Cr
3.045 g CrCl
3.045 - 1.00 = 2.045 Cl
Cr 1.00/51.996 = 0.0192 / 0.0192 = 1
Cl 2.045/35.45 = 0.0577 / 0.0192 = 3
CrCl3
135
CrO4 2-
chromate
