chapter 2: atoms, molecules,, and ions Flashcards
1
Q
question of whether matter is or isn’t … led to many ….
A
continuous; experiments
2
Q
antoine Lavoisier’s experiments resulted in the
A
law of conservation of mass
3
Q
law of conservation of mass: mass is neither … nor .. during
A
gained; destroyed; chemical reactions
4
Q
law of constant composition: all samples of pure substance have the
A
same elements in the same proportions by mass
5
Q
law of multiple proportions: for compounds that are formed by the same elements, the masses of the first element that combine with a certain mass of the second element is always
A
a ratio of small whole numbers
6
Q
Democritus proposes matter is … and called the smallest particles of matter…
A
discontinuous; atoms
7
Q
(Dalton’s theory) all matter is made up of
A
atoms
8
Q
(Dalton’s theory) atom: smallest unit of an element that
A
retains the properties of the element
9
Q
(Dalton’s theory) element is made up of one type of …, and the properties of the atoms of an element are ..
A
atom; identical
10
Q
(Dalton’s theory) compounds have atoms of
A
2 or more elements
11
Q
(Dalton’s theory) the number of atoms in a compound is
A
the same
12
Q
(Dalton’s theory) atoms merely…during chemical reactions
A
rearrange
13
Q
(Dalton’s theory) explanation of law of constant composition: compounds are always composed of the same
A
atoms in the same ratios
14
Q
(Dalton’s theory) explanation of the law of multiple proportions: compounds can be made from the same elements in different ratios in which the ratio of atoms will be
A
whole numbers
15
Q
(Dalton’s theory) explanation of law of conservation of mass: in chemical reactions, atoms are merely …., …., and ….; since the number of atoms and the atoms themselves aren’t changing, the mass
A
rearranged; combined; separated; doesn’t change either
16
Q
atoms can be … into several different ..
A
subdivided; subatomic particles
17
Q
the three major subatomic particles comprising atoms include:
A
protons, neutrons, and electrons
18
Q
the manner in which atoms combine and behave is determined by the … and .. of each subatomic particle
A
number; type
19
Q
JJ Thomson used a gas discharge tube to show that cathode rays were
A
electrically charged particles
20
Q
cathode rays traveled in …. and were deflected by … and …
A
straight lines; electric and magnetic fields
21
Q
Thomson determined by the direction of the rays’ deflection that the particles were
A
negatively charged
22
Q
electrons:
A
negatively charged particles
23
Q
Robert A. Milikan measured the
A
charge of the electron
24
Q
(Milikan’s experiment) exposed tiny oil drops to
A
high-energy radiation
25
(Milikan's experiment) measured the rate that the electrically charged oil droplets fell in the
presence/absence of an electric field
26
(Milikan's experiment) calculated the ... on the oil drop
charge
27
(Milikan's experiment) noted that the charge was a multiple of a
single quantity
28
(Milikan's experiment) this quantity is the charge of an
electron (e)
29
with the knowledge of the charge, the ... of the electron was measured
mass
30
in a study meant to analyze deflection of alpha particles as they passed through gold foil, Rutherford recognized that some of the alpha particles were
deflected back toward the source
31
Rutherford proposed a nuclear model of the atom, which suggested that atoms contain
nuclei of positive charge
32
nucleus contains most of an atom's
mass
33
electrons comprise most of the atom's
volume
34
Rutherford found that every element has a different
positive charge
35
Rutherford suggested the existence of a
proton
36
the mass of the proton is ... times that of the electron
1836
37
Rutherford was unable to explain why protons were,....., considering that .... between like charges typically exists
close together; repulsion
38
the existence of a neutral particle was proposed because the proton didn't account for
the entire nuclear mass
39
james chadwick discovers
neutrons
40
neutron's mass is close to that of a
proton
41
strong nuclear binding forces hold the particles of nuclei
together
42
ratio of neutrons to protons is around:
1.0 to 1.6
43
charges of the electron and proton are equal in
magnitude.
44
atoms contain equal numbers of
electrons and protons
45
mass of protons and neutrons are almost equal, while the mass of an electron is
very small
46
atomic number (Z): amount of .. in an atomic nucleus; ... an element
protons; identifies
47
number of neutrons in atoms of the same element are not always the same:
isotopes
48
mass number (A): amount of
protons and neutrons in an atom
49
isotopes have the same ... but different ..
atomic number; mass numbers
50
most elements occur in nature as mixtures of
stable isotopes
51
about 75% of naturally occurring elements have
2 or more stable isotopes
52
isotopes disproves one aspect of
Dalton's atomic theory
53
to portray specific isotopes, the following notation is used:
a X
| z
54
X→
element's symbol
55
a→
mass number
56
z→
atomic number
57
the atomic number and element's symbol do not both have to be included, because either one can
identify the element
58
ions: charged atoms that are formed when atoms
lose/gain electrons
59
cation: ... formed when an atom ... one or more electrons
positive ion; loses
60
anion: ....; formed when an atom ... one or more electrons
negative anion; gains
61
notation used to identify ions, and notation used to identify isotopes can be
combined
62
atomic mass unit (u):
1/12 mass of Carbon-12 atom
63
atomic mass unit is the standard unit to measure
atomic mass
64
all other atomic masses are compared with the
Carbon-12 standard
65
1 u =
1.66 x 10-27 kg
66
masses of neutrons and protons are approximately
1 u
67
atomic masses of all the elements found with
mass spectrometers
68
(mass spectrometer) a sample of an element in gaseous form is exposed to a beam of high energy electrons which convert the atoms of the element to
cations
69
(mass spectrometer) a magnetic field deflects the cations into a
curved path
70
(mass spectrometer) the degree of curvature determines the
mass and charge of the ion
71
(mass spectrometer) the charge to mass ratio of the ions is then
calculated
72
mass spectrometer measures .. and .... of isotopes in a sample of an element
masses; relative abundance
73
isotopic compositions of most naturally occurring elements are ... and aren't influenced by the ... of the sample
constant; origin
74
isotopic mass: mass of an
isotope of a given element
75
a weighted average mass can be calculated that considers the
abundance of isotopes
76
atomic mass: weighted ... of the naturally occurring element
average mass
77
atomic mass is an average: portrays natural isotopic
distribution of an element
78
classification of elements enables comprehension of
elements' properties
79
periodic table arranges the elements into ..., with elements of similar properties falling in the same ...
rows; column
80
Mendeleev initially arranged elements by increasing ...., although he deviated from this to place elements with similar ... together
atomic mass; properties
81
Mendeleev predicted the existence of other
elements
82
Moseley ordered the elements based on their
atomic numbers
83
period: ... of the periodic table
horizontal row
84
properties of elements vary across
periods
85
groups: .... of the periodic table
columns
86
properties of elements in the same groups are
similar
87
numbers associated with rows refer to the outermost ... in which electrons can be found in their ground state
energy level
88
numbers associated with groups can provide insight into the .... in the outermost energy level of an atom
electron configuration
89
classification of elements also involves indicating whether the elements are
metals, nonmetals, or metalloids
90
metal:
shiny, good electrical conductor
91
nonmetals: elements that don't ..., elements in ... part of the periodic table
conduct electricity; top right
92
metalloids: have properties of ... and ....; .... of electricity; elements along the line that divides ... and ....
metals nonmetals; semiconductors; metals; nonmetals
93
representative/ main-group elements: elements in groups
1,2, 13-18
94
transition metals: ... block elements from group ..
d; 3-12
95
lanthanides: elements that follow
lanthanum
96
actinides: elements that follow
actinium
97
inner transition metals:
lanthanides and actinides
98
alkali metals (group 1):
soft, low melting metals, reactive, abundant
99
alkali metal reactivity increases
down the group
100
alkali metals occur in compounds rather than as
free elements
101
alkaline earth metals (group 2) less reactive than
alkali metals
102
Mg and Ca are
abundant
103
halogens (group 17): term means
salt formers
104
halogens (group 17): among most reactive
nonmetals
105
halogens (group 17): reactivity decreases down the
group
106
halogens (group 17): fluorine is the most ... of all the elements
reactive
107
chlorine is the most ... of the halogens
abundant
108
noble gases (group 18): generally
unreactive
109
molecule: combination of atoms that acts as a single particle due to the strong
attraction between the atoms
110
molecules are electrically
neutral
111
molecules of different atoms form
molecular compounds
112
diatomic molecules consist of
2 atoms
113
if all the atoms in a molecule are the same, the substance is
an element
114
if atoms of two or more elements are present, the substance is a
molecular compound
115
molecular formula: shows the ... of a molecule and indicates the number of each
composition; type of atom in a molecule
116
subscripts give the number of
atoms of an element
117
structural formula: shows how atoms are c
connected in a molecule
118
molecular mass: sum of the masses of a molecule's
atoms
119
molecular mass is expressed in
atomic mass units
120
the number of sig figs when calculating atomic mass is sometimes
random
121
(atomic mass) use either one or two digits after the decimal point, whichever corresponds with the
precision that is wanted
122
some compounds contain elements in the form of
ions
123
ionic compound: compound do
cations and anions that are joined together
124
ionic compounds are held together by
electrostatic forces
125
all ionic compounds are electrically neutral because the sum of the charges of the cations and anions equal
zero
126
the exact number of ions in an ionic crystal varies with the
size of the sample
127
empirical formula: gives the relative numbers of atoms in a substance with the smallest possible
whole-number subscripts
128
empirical formulas of ionic compounds indicate
electrical neutrality
129
empirical formulas of ionic compounds indicate
electrical neutrality
130
metals form
cations
131
nonmetals form
anions
132
for groups 1-3, the metals form cations that have charges that are equal to their
group numbers
133
main group nonmetals form anions that have charges based on their distance from the
noble gases
134
when charges of ions in an ionic compound are known, the formula is written by adjusting the ... on the ions so that the sum of charges is ...
ions; zero
135
monatomic ions: ions that are formed from
single atoms
136
polyatomic ion: group of atoms with a
charge
137
polyatomic ions behave like a .... because of the
single particle; strong attractive forces
138
ammonium is the most common
polyatomic cation
139
empirical formula of an ionic compound with polyatomic ions is also dependent on
charges
140
formula mass: sum of atomic masses of all atoms in an ionic compound's
empirical formula
141
formulas for ionic compounds give the relative numbers of
cations and anions
142
for monatomic ions: cation is named by the element's ...; anion is the root of the element name with suffix ...
name; -ide
143
binary compounds: comprised of
2 elements
144
name of binary compounds doesn't include
numerical prefixes
145
name of polyatomic ions are used in the
compound name
146
metals from other groups can have more than one
cation
147
.... used to specify the charges of metals that have more than one cation
roman numerals
148
older system with suffixes ... and ... to indicate charges
-ous; -ic
149
acids: produce ... in aqueous solution
hydrogen ions
150
when the name of the anion ends in -ide (exception: hydroxide), acid name is found by adding prefix ... and changing the ending to ..; followed by the word ..
hydro-; -ic; acid
151
anions found in acids combine with a sufficient number of hydrogen ions to give
electrical neutrality
152
if polyatomic anion ends in -ate, the name of the acid will end in ... followed by ..
-ic; acid
153
if polyatomic anion ends in -ite, the name of the acid will end in ... followed by ...
-ous; acid
154
(molecular compounds) element father to the left in the periodic table is given
first
155
(molecular compounds) element closer to the bottom in any group is given
first
156
(molecular compounds) We name the 1st element in the compound followed by the name of the 2nd element with its ending changed to
ide
157
prefixes indicate the number of atoms of each element in
a molecule
158
(molecular compounds) hydrogen is given second when it combines with elements from groups
1A to 5A
159
(molecular compounds) hydrogen is first when it combines with group
6A and 7A
160
oxygen is always last, except when it combines with
fluorine
161
general order in which elements are given in a molecular compounds formula:
B, Si, C, As, P, N, H, Se, S, I, Br, Cl, O, F
162
organic compounds: compounds that have
carbon
163
hydrocarbons: organic compounds that only have
hydrogen and carbon
164
alkanes: simplest class of
hydrocarbons
165
general formula for alkanes is:
CnH2n+2
166
alkanes have an ... ending
-ane
167
(alkanes) linear chains of carbon with enough hydrogen sot that each carbon is connected to
4 other atoms
168
alkanes with more than three carbon atoms may have different arrangements of carbon chain that have
branching
169
for those that are branched, the substituent attached to the longest chain is the
alkyl group
170
names of alkanes are based on the length of the
hydrocarbon chain
171
n-alkanes are
straight, unbranched chains
172
(names of alkanes) methane
CH4
173
(names of alkanes) ethane
C2H6
174
(names of alkanes) propane
C3H8
175
(names of alkanes) n-Butane
C4H10
176
(names of alkanes) n-Pentane
C5H12
177
(names of alkanes) n-Hexane
C6H14
178
(names of alkanes) n-Heptane
C7H16
179
(names of alkanes) n-Octane
C8H18
180
(names of alkanes) n-Nonane
C9H20
181
(names of alkanes) n-Decane
C10H22
182
(names of alkanes) methyl
CH3 -
183
(names of alkanes) ethyl
C2H5 -
184
(names of alkanes) propyl
C3H7 -
185
(names of alkanes) butyl
C4H9 -
186
(names of alkanes) pentyl
C5H11 -
187
(names of alkanes) hexyl
C6H13 -
188
(names of alkanes) Heptyl
C7H15 -
189
(names of alkanes) Octyl
C8H17 -
190
(names of alkanes) Nonyl
C9H19-
191
(names of alkanes) decyl
C10H21 -
192
cycloalkanes: hydrocarbons that contain a
ring of carbon atoms
193
cycloalkanes formula
CnH2n
194
substituents of cylcoalkanes are named in the same manner as alkanes, except they have the prefix
cyclo-
195
When branching occurs in alkanes, branched hydrocarbon substituents are referred to as ... and the ane ending is removed and a ... ending is added
alkyl groups; -yl
196
(naming alkanes) locate the longest .. or biggest ..
chain; ring
197
(naming alkanes) locate substituents and number the chain to minimize the number of the
substituent
198
(naming alkanes) name the substituent, properly located on the chain by a number followed by a
dash
199
(naming alkanes) add the base alkane name of the longest
carbon chain
200
more complex organic compounds have
functional groups
201
functional groups: atoms/ small groups of atoms that undergo
reactions
202
halogesn are
functional groups
203
molecular compounds form when two or more
nonmetals combine
204
(ionic solids) 3d structure held by strong
electrostatic orces
205
(ionic solids) hard, brittle
crystalline solids
206
(ionic solids) high melting
points
207
(ionic solids) must be heated to very high temperatures to be
vaporized
208
(ionic solids) when ionic substances dissolve they separate into
cations and anions (dissociation)
209
(ionic solids) when ionic substances that have polyatomic ions dissolve, the polyatomic ions do not
separate
210
(ionic solids) measuring electrical conductivity distinguishes ionic compounds from most
molecular compounds
211
(ionic solids) solid ionic compounds don't
conduct electricity
212
(ionic solids) electrolyte: substance that produces ions when
dissolved in water; conduts electricitiy
213
(ionic solids) pure water and solutions of most other molecular compounds are poor electrical conductors→
nonelectrolyte
214
(small molecular compounds) typically exist as .., ..., or ...
gases; liquids; low-melting solids
215
(small molecular compounds) forces that hold one molecule to another are
weak
216
(small molecular compounds) low melting
points
217
(small molecular compounds) in liquid phase: molecules are close but can
move
218
(small molecular compounds) in gas phase: molecules are moving and
far apart
219
(small molecular compounds) no phase conducts
electricity
