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CHM 1040 > Exam 2 > Flashcards

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)
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2
Q

nomenclature

A

naming

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3
Q

naming compounds: binary ionic compounds

A
  • contains (+) cations and (-) anions
  • type 1
  • type 2
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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+

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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
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6
Q

naming type 1 binary ionic compounds

A
  • cation is always named first (element name)

- anion named second (end in -ide)

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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
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8
Q

what is the name of SrB2?

A

strontium bromide

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9
Q

what is the name of K2S?

A

potassium sulfide

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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
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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
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12
Q

name CrO2

A

chromium (IV) oxide

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13
Q

name chromium (II) fluoride

A

CrF2

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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

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15
Q

binary compounds: type 3

A
  • non-metal and non-metal

- greek prefixes to denote the # of atoms of each element

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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
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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*
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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
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19
Q

name SeO2

A

selenium dioxide

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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)
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21
Q

polyatomic ions

A

charged entities composed of several atoms bound together

  • have special names
  • *MUST MEMORIZE**
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22
Q

oxyanions

A

polyatomic anions exist that contain an atom of a given element and diff #s of oxygen atoms

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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
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24
Q

name KClO

A

potassium hypochlorite

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25
Q

give the formula of ammonium acetate

A

NH4C2H3O2

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26
Q

name KClO3

A

potassium chlorate

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27
Q 
which are named correctly?
      Formula    Name
I       P2O5     diphosphorus pentoxide
II      ClO2      chlorine oxide
III     PbI4       lead iodide
IV    CuSO4  copper (I) sulfate
A

I only

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28
Q

acids

A
  • 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
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29
Q

rules for naming acids

A
  • 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
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30
Q

examples of naming acids

A 
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
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31
Q

names of acids without O

A 
ACID    NAME
HF       hydrofluoric acid
HCl      hydrochloric acid
HBr      hydrobromic acid
HI         hydroiodic acid 
HCN     hydrocyanic acid
H2S      hydrosulfuric acid
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32
Q

names of some acids with O

A 
ACID                 NAME
HNO3           nitric acid
HNO2          nitrous acid
H2SO4         sulfuric acid
H2SO3.         sulfurous acid 
H3PO4      phosphoric acid
HC2H3O2    acetic acid
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33
Q

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

A

B

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34
Q

a compound has the formula Xcl3 where X could represent a metal or a non-metal. What could the name of this compound be?

A

phosphorus trichloride

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35
Q

writing formulas from names

A
  • 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
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36
Q

more nomenclature examples

A 
NaOH: sodium hydroxide
potassium carbonate: K2CO3
sulfuric acid: H2SO4
dinitrogen pentoxide: N2O5
cobalt (III) nitrate: Co(NO3)3
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37
Q

NH4 +

A

ammonium

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38
Q

NO2 -

A

nitrite

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39
Q

NO3 -

A

nitrate

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40
Q

SO3 2-

A

sulfite

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41
Q

SO4 2-

A

sulfate

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42
Q

HSO4 -

A

hydrogen sulfate/bisulfate

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43
Q

OH -

A

hydroxide

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44
Q

CN -

A

cyanide

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45
Q

PO4 3-

A

phosphate

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46
Q

HPO4 2-

A

hydrogen phosphate

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47
Q

H2PO4 -

A

dihydrogen phosphate

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48
Q

CO3 2-

A

carbonate

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49
Q

HCO3 -

A

hydrogen carbonate/bicarbonate

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50
Q

ClO -

A

hypochlorite

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51
Q

ClO2 -

A

chlorite

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52
Q

ClO3 -

A

chlorate

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53
Q

ClO4 -

A

perchlorate

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54
Q

C2H3O2 -

A

acetate

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55
Q

MnO4 -

A

permanganate

56
Q

Cr2O7 2-

A

dichromate

57
Q

O2 2-

A

peroxide

58
Q

clues that a chemical rxn has occurred

A

1) the colors change
2) a solid forms
3) bubbles form
4) heat and/or a flame is produced, or heat is absorbed

59
Q

chemical equations

A
  • 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
Q

balancing a chemical equation

A
  • 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
Q

physical states

A
  • physical states of compounds are often given in a chem equation
    states: s, l, g, aq
62
Q

how to write + balance equations

A
  • 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
Q

in the context of balancing a chem eq, which of the following statements is false?

A

subscripts in the reactants must be conserved in the products

64
Q

of the 3 that are correct, which one is preferred most?

CaO + C -> CaC2 + CO2

A

II is preferred

65
Q

balance the following eq & find the sum of the coefficients:
FeO (s) + O2 (g) -> Fe2O3 (s)

A 
4 FeO (s) + 1 O2 (g) -> 2 Fe2O3 (s) 
sum: 7
66
Q

balance & find the sum of the coefficients:

NH3 (g) + HCl (g) -> NH4Cl (s)

A 
1 NH3 (g) + 1 HCl (g) -> 1 NH4Cl (s)
sum: 3
67
Q

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?

A

H2(g) + Cl2(g) -> HCl(g)

68
Q

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

a solid forms

69
Q

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”

A

color changes

70
Q

what does a balanced chemical equation tell us?

A

the ratio of the # of molecules that react & are produced in a chemical rxn

71
Q

4 driving forces favor chm change

A
  • formation of a solid
  • formation of water
  • transfer of e-
  • formation of a gas
72
Q

precipitation

A

the process of formation of a solid during a chm rxn

  • the solid formed is a precipitate
  • rxn known as precipitation rxn
73
Q

precipitate

A

the solid formed during a precipitation rxn

*exchange cations & anions

74
Q

what happens when an ionic compound dissolves in water?

A
  • ions separate & move around independently

- ions separate when the solid dissolves

75
Q

strong electrolyte

A

substance whose each unit produces separated ions when dissolved in water

76
Q

how to decide what products form

A

exchange of cations binding to anions

*switch

77
Q

soluble

A

can dissolve in water

aq

78
Q

slightly soluble/moderately soluble basically means __

A

insoluble

79
Q

how to predict precipitates when solutions of 2 ionic compounds are mixed

A
  • 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
Q

which ion reacts with Pb2+ to form compounds generally soluble in water?

A

NO3-

81
Q

A solution of sodium phosphate reacts with a solution of lead(II) nitrate. What precipitate, if any, will form?

A

Pb3(PO4)2

82
Q

what are the 3 types of equations for rxns in aqueous solutions?

A
  • molecular
  • complete ionic
  • net ionic
83
Q

molecular equation

A
  • 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
Q

complete ionic equation

A
  • all substances that are strong electrolytes are represented as ions
  • spectator ions
85
Q

spectator ions

A

ions that don’t participate directly in a rxn in sol

* the ions that cancel out

86
Q

net ionic equation

A
  • includes only those components that are directly involved in the rxn
  • spectator ions not included
  • order doesn’t matter
  • should always be balanced
87
Q

Write the correct molecular equation, the complete ionic equation, and the net ionic equation for the reaction between cobalt(II) chloride and sodium hydroxide

A

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
Q

what are the 7 strong acids?

A

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
Q

soluble compounds

A

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
Q

insoluble compounds

A

1) S2-, CO3 2-, PO4 3- salts

2) OH- salts except for those w/ Na+, K+, Ba2+, Ca2+

91
Q

strong acid

A

a strong electrolyte that produces H+ ions (protons) when it is dissolved in water

92
Q

acids give __ to bases; bases accept __ and give __ to acids

A

H+; H+; OH-

93
Q

is an acid and base is a good relationship?

A

yes

94
Q

an acid and base always make __ and __

A

water; a salt

95
Q

strong base

A

a substance that produces hydroxide ions (OH-) in water

96
Q

examples of strong bases

A

NaOH and KOH

97
Q

when writing equations, you can never break apart __ and __

A

solids; liquids

98
Q

what are the strong bases?

A

Group 1
Group 2
+
OH-

99
Q

the net ionic equation for the rxn of a strong acid and a strong base is always the production of __

A

water

100
Q

net ionic equation for HNO3 and LiOH

A

H+ + OH- -> H2O

101
Q

when finding the mass of a compound just look on the __

A

periodic table

102
Q

mole

A

the # equal to the # of C atoms in 12.01 g of C

103
Q

Avogadro’s number

A

6.022 x 10^23

104
Q

1 mole of anything =

A

6.022 x 10^23 atoms of that thing

105
Q

how many atoms are in 1.008g of H?

A

6.022 x 10^23 atoms

106
Q

determine the number of copper atoms in a 63.55g sample of copper

A

6.022 x 10^23 Cu atoms

107
Q

which is closest to the avg mass of 1 atom of copper

A

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
Q

calculate the # of Fe atoms in a 4.48 mole sample of Fe

A
  1. 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
Q

a sample of 26.98 g of Al has the same # of atoms as __ g of Au

A

197.0

110
Q

molar mass

A

mass in grams of a substance

unit: g/mol
- coefficients don’t count, only subscripts

111
Q

find the molar mass of Ba(NO3)2

A
  1. 35 g/mol

137. 33 g + (2 x 14.01g) + (6 x 16.00g)

112
Q

when finding the molar mass and determining sig figs, always use numbers from __

A

periodic table

113
Q

mole of a compound

A

mass of sample (g) / molar mass of compound (g/mol)

114
Q

mass of a sample

A

moles of sample (mol) x molar mass of compound (g/mol)

115
Q

what is the molar mass of nickel (II) carbonate

A

118.7 g/mol
NiCO3
58.69 + 12.01 + 3 x 16.00 = 118.7 g/mol

116
Q

how many grams of fluorine are present in one molecule of boron trifluoride (molecules to grams) ?

A

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
Q

how many grams of chlorine gas are present in 5.65 moles?

A

5.65 moles x 2 (35.45g)/1 mole = 400 g

118
Q

how many moles of KNO3 are present in 17.38 g?

A
  1. 172 moles

17. 38g x 1 mole/101 g/mol = 0.172 moles

119
Q

how many molecules of O2F2 are in 3.44 moles?

A
  1. 072 x 10^24 molecules

3. 44 moles x 6.022 x 10^23 molecules / 1 mole = 2.072 x 10^24 molecules

120
Q

conversions with mass, moles, and atoms

A
  • 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
Q

conversion trick

A 
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
Q

mass percent of an element in a compound

A

mass of element present in 1 mole of compound / mass of 1 mole of compound

123
Q

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

A

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
Q

empirical formula

A

formula of a compound that expresses the smallest whole-number ratio of the atoms present
-simplest whole-number ratio

125
Q

molecular formula

A

the exact formula of the molecules present in a substance
(empirical formula)n
*n is an integer
*always bigger than empirical formula

126
Q

how to find the empirical formula

A

assume 100 g and change % to g
convert g to mol
divide by lowest number
round any decimals

127
Q

how to find the molecular formula

A
  • 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
Q

do diatomics or sig figs matter in empirical/molecular formulas?

A

no

129
Q

Each molecule of ethanol, for instance, contains two carbon atoms, six hydrogen atoms, and one oxygen atom. Find the molar mass

A

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
Q

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.

A

C3H7

131
Q

The composition of adipicacid is 49.3% C, 6.9% H, and 43.8% O (by mass). What is the empirical formula?

A

C3H5O2

132
Q

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?

A

C6H14

molar mass of C3H7 = 43.086 g/mol

86.2 g/mol / 43.086 g/mol = 2

(C3H7) x 2 = C6H14

133
Q

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?

A

C6H10O4

134
Q

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.

A

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
Q

CrO4 2-

A

chromate

CHM 1040 (6 decks)

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