chapter 1 - 3 Flashcards
1
Q
acetate
A
C2H3O2(-)
2
Q
BrO2(-)
A
bromite
3
Q
ClO4(-)
A
perchlorate
4
Q
hypochlorite
A
ClO(-)
5
Q
BrO3(-)
A
bromate
6
Q
bromite
A
BrO2(-)
7
Q
C2H3O2(-)
A
acetate
8
Q
BrO4(-)
A
perbromate
9
Q
C2O4(2-)
A
oxalate
10
Q
bisulfite
A
HSO3(-)
11
Q
bisulfate
A
HSO4(-)
12
Q
bicarbonate
A
HCO3(-)
13
Q
bisulfide
A
HS(-)
14
Q
bromate
A
BrO3(-)
15
Q
ammonium
A
NH4(+)
16
Q
BrO(-)
A
hypobromite
17
Q
accuracy
A
how close to accepted value
18
Q
alkali metals
A
1+ charge (hydrogen is not alkali)
19
Q
alkaline earth metals
A
2+ charge
20
Q
anion
A
negatively charged ion
21
Q
atomic mass
A
average of all isotopes; mass of atom in amu; addition of protons and neutrons
22
Q
atomic number
A
(Z) number of protons
23
Q
avogadro’s number
A
6.022*10^23atoms/1mol
24
Q
ball and stick model
A
the kind that you use in a lab with a ball and then a long stick showing a bond
25
binary compounds
a compound containing two elements
26
carbonate
CO3(2-)
27
j.j thomson
cathode ray tubes which emanated from the negative electrode and was repelled by the negative pole. He postulated that it was a stream of negatively charged particles (electrons). He measured the charge to mass ratio; plum pudding model - electrons are like raisins dispersed in a pudding of positive charge
28
cation
positively charged ions
29
chlorate
ClO3(-)
30
chemical change
can only be observed when a substance is changed into another substance. ex: flammability, corrosiveness, reactivity
31
chemical formula
shows the number of each element in the molecule.
32
chlorite
ClO2(-)
33
chromate
CrO4(2-)
34
chromatography
physical process; separates substances on the bases of differences in the ability of substances to adhere to the solid surface; ink chromatography - dyes to a paper
35
chromium ion
Cr3+
36
ClO(-)
hypochlorite
37
ClO2(-)
chlorite
38
ClO3(-)
chlorate
39
CO3(2-)
carbonate
40
compounds
made up of two or more different kind of elements
41
Copper ion charges
2+, 1+
42
covalent bonds
bonds between atoms by sharing electrons; result is called a molecule; occurs between two nonmetals
43
Cr2O7(2-)
dichromate
44
CrO4(2-)
chromate
45
dalton
created law of multiple proportions; dalton's atomic theory: each element is made up of atoms, atoms of an element are identical, chemical compounds are formed when different elements combine with on another, chemical reaction involve the reorganization of elements
46
density
mass per unit volume; D=m/V; common unites are g/mL, g/cm^3
47
determinate error
systematic error; all results are skewed in one direction
48
dichromate
Cr2O7(2-)
49
distillation
physical process; uses the differences in volatility of substances to separate a homogeneous mixture into its components; heat the substance and as one component boils it rises and goes through cooling chamber which then returns it into liquid into another container.
50
electrolysis of water
chemical process; using electricity to decompose water into oxygen and hydrogen gas
51
empirical formula
when the ratio of molecules is most simplified
52
ending for monatomic anions
-ide
53
fahrenheit to celsius
F=9/5(C)+32
54
filtration
physical process; pour mixture through a filter which separates liquids from solids
55
elements
made up of a unique kind of atom
56
gas
spread very far apart; a lot of mobility
57
H3O(+)
hydronium
58
halogens
1- charge; form diatomic molecules
59
HCO3(-)
bicarbonate
60
heterogeneous
the mixture is not uniform throughout
61
homogeneous
is uniform throughout; if it has a variable composition it will be a homogenous mixture
62
how do you name an acid if the anion does contain oxygen?
if the anion ends in -ate you change it to the suffix -ic; if the anion ends in -ite you change it to the suffix -ous.
63
how do you name an acid if the anion does not contain oxygen?
add the prefix hydro- and the suffix -ic
64
HS(-)
bisulfide
65
HSO3(-)
bisulfite
66
HSO4(-)
bisulfate
67
hydronium
H3O(+)
68
hydroxide
OH(-)
69
hypobromite
BrO(-)
70
hypoiodite
IO(-)
71
indeterminate error
random error; can never be perfect!
72
IO(-)
hypoiodite
73
IO2(-)
iodite
74
IO3(-)
iodate
75
IO4(-)
periodate
76
iodate
IO3(-)
77
iodite
IO2(-)
78
ion
atoms or group of atoms that has a net positive or negative charge
79
ionic bonding
bonds form due to force of attraction between oppositely charged ions
80
ionic solid
A solid consisting of oppositely charged ions
81
iron ion charges
3+, 2+
82
isotopes
atoms with same number of protons but different number of neutrons; same chemical properties
83
kelvin to celsius
K=C+273.15
84
law of conservation of mass
total mass is not changed by a chemical change
85
law of definite porportion
if you combine H and O in the ratio 2:1 you will get water. water will always have that ratio. the ratio of compounds will always be the same.
86
law of multiple proportions
if two elements form more than one compound, then the ratios of the masses of the second element which combine with a fixed mass of the first element will always be ratios of small whole numbers.
87
lead ion charge
2+
88
electron
found outside the nucleus; negatively charged; determines chemical properties
89
length
base unit is the meter; measure of distance
90
liquid
molecules spread farther apart, more mobility
91
manganese ion charge
2+
92
mass
measured in kg; a measure of the amount of material n an object
93
mass percent of an element
(mass of element in a compound/mass of compound)*100%
94
matter
anything that has mass and takes up space
95
mercury ion charge
Hg(2+); Hg2(2+)
96
metals
Metals have characteristic physical properties such as efficient conduction of heat and electricity, malleability (they can be hammered into thin sheets), ductility (they can be pulled into wires), and (often) a lustrous appearance. Chemically, metals tend to lose electrons to form positive ions.
97
metals that form more than one cation
observed for most transition metals, many actinides, and the heaviest elements of groups 13–15
98
metals that form only one cation
usually in groups 1-3,12,13
99
milikan
performed experiments including charged oil drops, allowed him to determine the magnitude of the electron charge and the mass of the electron from thomson's charge to mass ratio.
100
mixture
a material made up of two or more different chemical substances which are not chemically bonded; can be separated using physical methods
101
MnO4(-)
permanganate
102
naming oxyanions
In cases where only two oxyanions are known for an element, the name of the oxyanion with more oxygen atoms ends in -ate, and the name of the oxyanion with fewer oxygen atoms ends in -ite; The halogens and some of the transition metals form more extensive series of oxyanions with as many as four members. In the names of these oxyanions, the prefix per- is used to identify the oxyanion with the most oxygen (so that ClO4− is perchlorate and ClO3− is chlorate), and the prefix hypo- is used to identify the anion with the fewest oxygen (ClO2− is chlorite and ClO− is hypochlorite).
103
neutron
neutral charge
104
NH4(+)
ammonium
105
Nickel ion charge
2+
106
nitrate
NO3(-)
107
nitrite
NO2(-)
108
NO2(-)
nitrite
109
NO3(-)
nitrate
110
noble gases
0 charge
111
nonmetals
they tend to gain electrons in reactions with metals to form
negative ions. Nonmetals often bond to each other by forming covalent bonds.
112
rutherford
directed alpha particles (positively charged particles) to thin sheet of metal foil; most of the particles passed through but some were deflected at large angles; created the model of the nuclear atom - dense center of positive charge (the nucleus)
113
nucleus
small compared to the overall size of the atom; extremely dense - most of the atom's mass; contains protons and neutrons
114
O2(2-)
peroxide
115
OH(-)
hydroxide
116
order for naming ionic compounds
cation first, then anion
117
oxalate
C2O4(2-)
118
oxyanions
Polyatomic anions that contain a single metal or nonmetal atom plus one or more oxygen atoms
119
perbromate
BrO4(-)
120
percent yield
(actual yield/theoretical yield)*100%
121
percent yield
(actual yield/theoretical yield)*100%
122
perchlorate
ClO4(-)
123
period
horizontal rows of elements
124
periodate
IO4(-)
125
permanganate
MnO4(-)
126
peroxide
O2(2-)
127
phosphate
PO4(3-)
128
phosphite
PO3(3-)
129
physical change
can be observed without changing a substance into another substance. ex: boiling point, density, mass ,volume
130
PO3(3-)
phosphite
131
PO4(3-)
phosphate
132
proton
determines that atoms identity; found in the nucleus; always the same number as electrons for neutral atom.
133
pure substance
it is homogenous and it has only one variable composition; has constant composition
134
precision
proximity of several measurements to each other
135
groups/families
elements in the same vertical columns; have similar chemical properties
136
S2O3(2-)
thiosulfate
137
SCN(-)
thiocyanate
138
silver ion charge
+
139
SO3(2-)
sulfite
140
SO4(2-)
sulfate
141
solid
typically most dense (not true of water)
142
solution
a homogenous mixture
143
space filling model
is when atoms are shown as round balls and they are all kinds touching.
144
structural formula
the diagram showing how the molecule is bonded.
145
sulfate
SO4(2-)
146
sulfite
SO3(2-)
147
thiocyanate
SCN(-)
148
thiosulfate
S2O3(2-)
149
tin ion charge
2+; 4+
150
volatility
how readily substances become gasses; used in distillation
151
weight
the force acting on the object due to gravity
152
zinc ion charge
2+
