Chapter 1 Flashcards
(267 cards)
1
Q
______ properties ______ depend on sample
A
Intensive; don’t
2
Q
_______ Properties ________ depend on the sample
A
Extensive; do
3
Q
Summarize past experiments; predict future ones
A
Law
4
Q
Speculation, proposed reasoning based on several hypothesis
A
Theories
5
Q
Seven fundamental units
A
SI Units; Mass - kg; length - m; Time - s; Temp - K; Substance - mol; volume - m^3
6
Q
Constant because quantity of matter cannot change
A
Mass
7
Q
Variable, dependent on gravity
A
Weight
8
Q
Ratios used to express a quantity of dif units
A
Conversion factors
9
Q
Conversion factor chosen must _______ all units except the unit in the _______
A
Cancel out; answer
10
Q
Measure of how hot or cold an object is relative to another
A
Temperature
11
Q
Energy that flows from object with higher temp to lower temp
A
Heat
12
Q
T(inC) + 273.15 = __
A
Celsius to Kelvin
13
Q
[T(inF) - 32]x5/9 = ____
A
Fahrenheit to Celcius
14
Q
A characteristic & physical property, ratio of ______ & _______
A
Density;Mass/Volume
15
Q
Mass, volume, energy, ______ on amount of substance
A
Extensive property; dependent
16
Q
Density, temp, _______ on amount of substance
A
Intensive property; does not
17
Q
How close measurements in series are to eachother
A
Precision
18
Q
How close each measurement is to the actual value
A
Accuracy
19
Q
Either ALL higher OR lower than actual value
A
Systematic
20
Q
Higher AND lower than actual value
A
Random
21
Q
Peta (P)
A
10^15
22
Q
Tera (T)
A
10^12
23
Q
Giga(G)
A
10^9
24
Q
Mega(M)
A
10^6
25
Kilo(k)
10^3
26
Hecto(h)
10^2
27
Deka(da)
10^1
28
Deci(d)
10^-1
29
Centi(c)
10^-2 (0.01)
30
Milli(m)
10^-3
31
Micro(u)
10^-6
32
Nano(n)
10^-9
33
Pico(p)
10^-12
34
Femto(f)
10^-15
35
Pure substance
- Made up of only one distinct chemical component
- composition is homogenous and uniform throughout.
36
Mixture
- Composed of two or more chemical components
- Proportions can vary from one sample to another
37
Element
- Substance that cannot be chemically broken down into simpler substances
- Only one atom “type” is present
38
Compound
Substance composed of two or more elements in fixed definitive proportions
39
Law of definite/constant composition
Elemental composition of a compound is always the same
40
Compounds can be represented by 3 formulas. What are they?
Molecular, Empirical, Structural
41
Empirical Formula
Relative number of atoms of each element in a compound
Simplest whole number (ratio) representation of the type & number of elements in the molecule
42
Molecular Formula
Gives the actual number of atoms of each element in a molecule of a compound
43
Because ________ are held together by defined chemical bonds, they are referenced using __________
Molecular compounds;molecular formula
44
Because ________ are not held together by defined chemical bonds, they are referenced using ________
Ionic compounds; empirical formula
45
Cations
Positive ions; number of electrons decreases
46
Anions
Negative ions; number of electrons increases
47
__________ atoms lose electrons and become ___________
Metal; cations
48
____________ gain electrons and become ________
Nonmetals; anions
49
Homogeneous mixture
Mixture made of multiple compounds, appears as one substance
Uniform compositions, mix uniformly
Each component retains some or all of its own unique identity/properties
Ex. Sea water, tea
50
Heterogenous Mixture
The composition varies from one part of the mixture to the other
Portions have different composition and properties
Ex. Concrete
51
Physical Mixtures can/can’t be separated by physical means
Can be separated by physical means
52
Chemically reacted compounds can/can’t be separated using physical means
Can’t be separated by way of physical means
53
Filtration
Separates based upon differences in particle size
54
Crystallization
Separates based upon differences in solubility
55
Distillation
Separates based upon differences in volatility
56
Chromatography
Separates based upon differences in solubility
57
Law of Conservation of Mass
Mass is neither created nor destroyed through chemical reactions
58
Formula for law of conservation of mass
SUM (mReactants) = SUMmProducts + SUMmexcess reactants
59
Law of Conservation of Mass-Energy
The amount of mass-energy must be conserved in a closed system
60
Law of Multiple Proportions
When two or more elements form a series of compounds, the ratios of the masses can always be reduced to a small whole number
61
Avogadros Hypothesis
At the same temperature and pressure, equal volumes of different gases contain the same number of particles
62
Cathode Rays Experiments
JJ Thomson, atom must be composed of negatively charged particles
Particles must come from something that all atoms have in common
Atoms are not indivisible as Dalton thought
63
Millikan Oil-Drop Experiment
X-rays used to number electrons
Determined charge of electron
1.602 x 10^-19
Combining results gave mass of electron 9.10 x 10^-28
64
Particles with the ______ charge repel eachother, whereas particles with _____ charges attract one another
Same;unlike
65
Radioactivity
The spontaneous emission of radiation by an atom
66
Three types of radiation
A particles, b particles, y rays, Rutherford
67
B rays are _______ charged (_e) and have mass, consist of ________
negatively;-1;electrons
68
A rays are _______ charged (_e)
Positively; +2
69
Electrons want to
Minimize their distance from protons; maximize separation from other negatively charged particles
70
Rutherford Gold Foil
Proved existence of both positive and neutrally charged particles in the nucleus
71
Modern atomic theory
Atoms are divisible into protons, neutrons, electrons.
All the atoms of an element contain the same number of protons and electrons
Number of protons defines the element & is called the atomic number
Atoms of the same element can have different properties
72
Isotopes
Atoms with identical #’s of protons and electrons, differ # of neutrons
73
Mass number, A
The total number of protons and neutrons in an atom
Used to differentiate between isotopes of an atomic element
74
Masses of atoms and percent abundances of isotopes are measured using ________ - a technique that separates particles according to their mass
Mass spectrometry
75
Statistical average mass
MAtomic = SUMisotopes Misotope x NAfractional
76
Avogadros #
6.022 x 10^23 amu
77
Periods
Rows of the periodic table
78
Groups
Columns of the period table, similar properties
79
Ionic Compounds
Electrostatic attraction between ions
Metal and Nonmetal
Polyatomic ions
80
Covalent (Molecular) Compounds
Sharing of electrons between atoms
Multiple nonmetals
Represented with molecular formula
81
Removing electrons results in a positively charged _______
Cation
82
Adding electrons results in a negatively charged ______
Anion
83
Metals tend to ______ e- to form ______
Lose;cations
84
Nonmetals tend to _____ e- to form _____
Gain, anions
85
Ionic Charge Trend
Group 1: +1, Group 2: +2, Group 13: +3, Group 14: +-4, Group 15: -3, Group 16: -2, Group 17: -1, Group 18: 0
86
H(+)
Hydrogen Ion
87
Li(+)
Lithium ion
88
Na(+)
Sodium ion
89
K(+)
Potassium Ion
90
Rb(+)
Rubidium ion
91
Cs(+)
Cesium ion
92
Fr(+)
Francium ion
93
Be(2+)
Beryllium ion
94
Mg(2+)
Magnesium ion
95
Ca(2+)
Calcium ion
96
Sr(2+)
Strontium ion
97
Ba(2+)
Barium ion
98
Ra(2+)
Radium ion
99
Sc(3+)
Scandium ion
100
V(2+)
Vanadium(II) ion
101
V(4+)
Vanadium(IV) ion
102
Cr(2+)
Chromium(II) ion
103
Cr(3+)
Chromium(III) ion
104
Mn(2+)
Manganese(II) ion
105
Mn(3+)
Manganese(III) ion
106
Fe(3+)
Iron(III) ion
107
Fe(2+)
Iron(II) ion
108
Co(3+)
Cobalt(III) ion
109
Co(2+)
Cobalt(II) ion
110
Ni(2+)
Nickel(II) ion
111
Ni(3+)
Nickel(III) ion
112
Cu(+)
Copper(I) ion
113
Cu(2+)
Copper(II) ion
114
Zn(2+)
Zinc ion
115
Ag(1+)
Silver ion
116
Cd(2+)
Cadmium ion
117
Sn(2+)
Tin(II) ion
118
Sn(4+)
Tin(IV) ion
119
Al(3+)
Aluminum ion
120
Pb(2+)
Lead(II) ion
121
Pb(4+)
Lead(IV) ion
122
Ga(3+)
Gallium ion
123
N(3-)
Nitride ion
124
P(3-)
Phosphide ion
125
O(2-)
Oxide ion
126
S(2-)
Sulfide ion
127
Se(2-)
Selenide ion/selenium
128
F(-)
Fluoride ion
129
Cl(-)
Chloride ion
130
Br(-)
Bromide ion
131
I(-)
Iodide ion
132
H(1-)
Hydride ion
133
Ionic compound - a molecule generally formed between the ions of ______ and _______ atoms
Metal;nonmetal
134
Cations, if the neutral atom forms multiple charged species upon ionization… Add the ________ of the charge in ________ and the word ____ after the neutral atoms name
Roman numeral;parenthesis;ion
135
Cr(2+)
Chromium(II) ion
136
Cr(3+)
Chromium(III) ion
137
Fe(2+)
Iron(II) ion
138
Fe(3+)
Iron(III) ion
139
Roman numerals are used in naming _______
Cations that form multiple charged species upon ionization
140
Co(2+)
Cobalt (II) ion
141
Co(3+)
Cobalt(III) ion
142
Cu(+)
Copper(I) ion
143
Cu(2+)
Copper(II) ion
144
Sn(2+)
Tin(II) ion
145
Sn(4+)
Tin(IV) ion
146
Pb(2+)
Lead(II) ion
147
Pb(4+)
Lead(IV) ion
148
H(+)
Hydrogen ion
149
Li(+)
Lithium ion
150
Na(+)
Sodium ion
151
K(+)
Potassium ion
152
Cs(+)
Cesium ion
153
Ag(+)
Silver ion
154
Mg(2+)
Magnesium ion
155
Ca(2+)
Calcium ion
156
Sr(2+)
Strontium ion
157
Ba(2+)
Barium ion
158
Zn(2+)
Zinc ion
159
Cd(2+)
Cadmium ion
160
Anions, replace the end of the neutral atoms name with ____ and add the word _____
-ide;ion
161
F(-)
Fluoride
162
Cl(-)
Chloride
163
Br(-)
Bromide
164
I(-)
Iodide
165
O(2-)
Oxide
166
S(2-)
Sulfide
167
N(3-)
Nitride
168
P(3-)
Phosphide
169
Naming ionic compound, first write the ________ name (minus the word ____) second write the ______ name (minus the word ____)
Cation;ion;anion;ion
170
Name of ______ (metal) + base name of ______ (nonmetal) + ide
Cation;anion;ide
171
Tl(+)
Thallium ion
172
Tl(3+)
Thallium(III) ion
173
__________ - the ion has the resulting negative (-) charge over the entire molecules system - very ________
Polyatomic anion; common
174
__________ - the ion has the resulting positive (+) charge spread over the entire Polyatomic system, _______ common
Polyatomic cation; less
175
A group of atoms that has a charge
Polyatomic ions
176
NH4(+)
Ammonium
177
Ammonium
NH4(+)
178
Hydronium
H3O(+)
179
H3O(+)
Hydronium
180
OH-
Hydroxide ion
181
CN-
Cyanide ion
182
O2(-2)
Peroxide ion
183
N3(-)
Azide ion
184
Oxyanions
Polyatomic anions composed of oxygen atoms with a fixed composition of atoms from other elements
185
Most oxygenated oxyanion/Most common oxyanion gets the ending of ______
-ate
186
Less oxygenated/less common gets the ending ____
Ite
187
If there are 4 oxyanions in the series, the most gets the prefix _____ and the least gets the prefix _______
Per;hypo
188
Period 2 has a maximum of ____ O atoms
3
189
Period 3 and below has a maximum of ___ O atoms
4
190
CO3(2-)
Carbonate ion
191
NO3(-)
Nitrate ion
192
PO4(3-)
Phosphate ion
193
SO4(2-)
Sulfate ion
194
ClO4(-)
Perchlorate ion
195
Acetate
C2H3O2(-)
196
Carbonate
CO3(2-)
197
Bicarbonate
HCO3(-)
198
Hydroxide
OH-
199
Nitrite
NO2(-)
200
Nitrate
NO3(-)
201
Chromate
CrO4(2-)
202
Dichromate
Cr2O7(2-)
203
Phosphate
PO4(3-)
204
Hydrogen phosphate
HPO4(2-)
205
Dihydrogen phosphate
H2PO4(-)
206
Ammonium
NH4(+)
207
Hypochlorite
ClO(-)
208
Chlorite
ClO2(-)
209
Chlorate
ClO3(-)
210
Perchlorate
ClO4(-)
211
Permanganate
MnO4(-)
212
Sulfite
SO3(2-)
213
Bisulfite
HSO3(-)
214
Sulfate
SO4(2-)
215
Bisulfate
HSO4(-)
216
Cyanide
CN(-)
217
Peroxide
O2(2-)
218
You can make complex oxyanions through the addition of the _______ ion
Hydrogen
219
When adding hydrogen, adding _________ or ____ at the beginning of the anion name
Hydrogen, bi (1), di(2)
220
Ionic compounds containing a specific number of water molecules associated with each formula unit
Hydrates
221
Mono
1
222
Di
2
223
Tri
3
224
Tetra
4
225
Penta
5
226
Hexa
6
227
Hepta
7
228
Octa
8
229
Nona
9
230
Deca
10
231
_________ is not used on the first element listed when naming covalent molecules/hydrates
Mono
232
An ionic compound composed of a ________ ion and an ______ is an Arrhenius acid
Hydronium (H+); anion
233
Hydrochloric acid
HCl
234
Sulfuric acid
H2SO4
235
Nitric acid
HNO3
236
Acetic Acic
HC2H3O2
237
Citric Acid
H3C6H5O7
238
Carbonic Acid
H2CO3
239
Hydrofluoric acid
HF
240
Phosphoric acid
H3PO4
241
If the anion in the end ends in -ide, change the ending to ________ and add the prefix _____
-ic acid; hydro
242
If the anion in the acid ends in ate, change the ending to ______
-ic acid; no hydro
243
If the anion in the acid ends in -ite, change the ending to ______
-ous acid; no hydro
244
The ____________ atom (element on the lower left hand side of the table) is listed _________
Less electronegative; first
245
The _________ atom (element on the upper right hand side of the table) is listed _________
More electronegative;second
246
The ending on the more electronegative element is changed to _____
Ide
247
A prefix is used to denote the number of atoms of each element in the compound
USED IN COVALENT BONDING, 2 NONMETALS
248
In ______ naming, prefixes are used to indicate the number of carbon atoms
Prefixes
249
Meth
1
250
Eth
2
251
Prop
3
252
But
4
253
Add the suffix ______ when the carbon has all four single bonds
-ane
254
When hydrogen atoms are removed to form multiple bonds, add the suffix _____
-ene
255
Removal of hydrogen bonds to form multiple bonds, triple bonds between carbons, use the suffix ______
-Yne
256
Ane
M = 2n+2
257
Ene = _______
M = 2n
258
Yne = m = 2n-2
259
Methane
CH4
260
Propane
C3H8
261
Butane
C4H10
262
Pentane
C5H12
263
Ethene
C2H4
264
Ethane
C2H6
265
-OH is added indicates a ______ change, change -ane to _____
Alcohol; -ol
266
Ammonia
NH3
267
Oxelate
C2O4(2-)
