Exam 1 Flashcards
1
Q
Define chemistry
A
study of matter & how the properties are related to its composition
2
Q
Define matter
A
has mass & occupies space
3
Q
Define mass
A
amount of matter
4
Q
Formula for mass in outer space
A
F=ma or m=f/a
5
Q
4 fundamental forces
A
Gravitational, electromagnetic, strong & weak nucles
6
Q
Define weight
A
m*a due to g
7
Q
Force of attraction by the earth
A
F=(m)(a) or W=(m)(g)
8
Q
Examples of why chemistry is critical in modern society
A
Electronics, materials, medical, personal & home care products, energy
9
Q
Force of gravity on earth
A
9.8 m/s^2 at sea level
10
Q
Force of gravity on the moon
A
1.7 m/s^2
11
Q
Consequences of chemistry
A
Pollution, global warming, warfare, accidents
12
Q
How much has the earth’s temp risen in the past century
A
1.5 degrees F
13
Q
How many tons of CO2 per person from fossil fuel consumption
A
10 tons
14
Q
Average temp of earth’s atmosphere with greenhouse gases vs without
A
With: 57 degrees F
Without: 0 degrees F
15
Q
Sources of CO2 emission from largest to smallest percentage
A
Electricity production, cars & trucks, industry, residential heating
16
Q
Gases contributing to global warming from largest to smalles
A
CO2, CFCs, CH4, N2O
17
Q
Protocol that did not get put in place but would have lowered CO2 emissions dramatically
A
Kiota protocol
18
Q
Regions of earth’s atmosphere lowest to highest
A
Troposphere, stratosphere, mesosphere, thermosphere
19
Q
CO2 absorbs what
A
infrared radiation
20
Q
Concentration of CO2 has risen by what percent in the past century
A
43%
21
Q
Scientists predict the earth temperature will rise by how much in 2100
A
4-9 degrees F
22
Q
1 CFC molecule can destroy how many ozone molecules
A
1,000s
23
Q
Define ozone
A
elemental oxygen (O3)
24
Q
Ozone shields us from what
A
harmful ultraviolet radiation
25
Consequences of ozone depletion
increased skin cancers, crop damage, cataracts
26
Define law
verbal statement or mathematical equation that summarizes observations & experiments (shows physical relationship, not explanation of nature)
27
Newton's universal law of gravity
Gravitational force=F=(Gm1m2)/(r^2)
28
Universal gravitational force constant
6.670*10^-11N*m^2/kg^2
29
Earth's mass is
6*10^24 kg
30
Define theory
Hypothesis that repeatedly withstands the test of experiments & has overwhelming supportive evidence
31
Define substance
Matter with a definite/constant composition & distinct properties
32
Examples of physical properties
Melting/boiling points, density, mass, volume, color, shape
33
Examples of chemical properties
All chemical reactions (composition/decomposition)
34
Define extensive properties
Value depends on quantity of matter
35
Examples of extensive properties
Mass, volume, heat
36
Define intensive properties
Value does not depend on the quantity of matter
37
Examples of intensive properties
Melting/boiling point, density, temp
38
Combination reaction to form table salt is surprisingly a very
Violent reaction
39
Examples of quantitative measurements
Length, mass, time, temp
40
SI base unit for length
meter, m
41
SI base unit for mass
kilogram, kg
42
SI base unit for time
second, s
43
SI base unit for temp
kelvin, K
44
SI base unit for amount of a substance
mole, mol
45
Metric system first started by who
France
46
giga
G, 10^9
47
mega
M, 10^6
48
kilo
k, 10^3
49
deci
d, 10^-1
50
centi
c, 10^-2
51
milli
m, 10^-3
52
micro
μ, 10^-6
53
nano
n, 10^-9
54
pico
p, 10^-12
55
femto
f, 10^-15
56
Greek prefixes used when
value is larger than the base (kilo, mega, giga)
57
Latin prefixes used when
value is smaller than the base (centi, milli, micro)
58
Derived unit examples
Volume (length)^3, area (length)^2, speed (distance/time), acceleration (distance/time^2), energy, force
59
Volume unit 1m^3=
1*10^6cm^3 or 1*10^3dm^3
60
Volume unit 1dm^3=
1 liter
61
Volume 1L=
1000mL or 1000cm^3
62
Volume 1mL=
1cm^3
63
Dimensional analysis involves
Conversion factors
64
Celsius scale based on
Water boils at 100 degrees C & freezes at 0 degrees C (Anders Celsius)
65
Define temp
Direction of heat flow, average kinetic energy
66
Fahrenheit scale based on
Salt saturated water freezes at 0 degrees F & 100 degrees F was normal body temp (Gabriel Fahrenheit)
67
Pure water boils & freezes at what degree F
Boils 212 degrees F, freezes 32 degrees F
68
Convert degrees C to degrees F
(9F/5C)tC+32F
69
Convert degrees F to degrees C
(tF-32F)(5C/9F)
70
Define heat
total kinetic energy
71
Convert C to K
Tk=tC+273.15
72
Substances can be either
elements or compounds
73
Define element
Substance that cannot be decomposed into simpler substances by chemical means
74
How man elements
Roughly 115, 82 natural
75
Sodium latin name
Natrium (Na)
76
Potassium latin name
Kalium (K)
77
Iron latin name
Ferrum (Fe)
78
Tin latin name
Stannum (Sn)
79
Lead latin name
Plumbum (Pb)
80
Silver latin name
Argentum (Ag)
81
Copper latin name
Cuprum (Cu)
82
Define mixture
Combination of 2 or more substances in which the substances retain their distinct identities
83
Mixtures have variable elemental composition while a pure substance has a
Definite composition
84
Define compound
Substance composed of 2 or more elements combined in a fixed proportion
85
Homogeneous mixture also called a
Solution
86
Ways to separate mixtures
Distillation, filtration, chromatagrophy
87
Law of definite proportions
(Proust) Compound always contains elements combined in the same proportion by mass
88
Dalton's atomic theory, 5 parts
1) matter composed of tiny particles (atoms) 2) all atoms of an element are identical in mass & their properties 3) Atoms of different elements differ in mass & other properties 4) compounds are composed of different elements combined in fixed proportions by mass 5) atoms are indestructable
89
Who created the atomic theory
John Dalton
90
Most renowned scientist of his time, late 1700s, early 1800s
Sir Humphrey Davy
91
Why wasn't Dalton's atomic theory accepted at first
Cocky Sir Humphrey Davy didn't agree with it
92
Law of multiple proportions
2 elements combine to form 1+ compounds, masses of 1 element that combine with a fixed mass of the other element are in ratios of small whole numbers (predicted by Dalton's atomic theory)
93
Define atom
smallest particle of an element which retains the chemical properties of that element
94
Discovery of the first subatomic particle was made by using what
Crookes tube
95
Tool that causes gases to glow & yield a bright spot when it strikes a fluorescent screen
Cathode ray tube
96
Scientist that found out that magnetic & electrical fields bend cathode rays
JJ ThOmpson
97
Cathode ray experiments suggested that Cathode rays are a basic component of all matter. Why?
Same properties regardless of metal used
98
What are cathode rays really
Beam of electrons
99
Whats a coulumb
Unit of electric charge
100
Robert Millikan designed what experiment which determined the charge of an electron
Oil drop experiment
101
Rontgen used cathode rays and discovered that some rays could pass through matter, he dubbed them what
X rays
102
Becquerel found that some compounds emitted rays spontaneously without cathode ray stimulation. This suggested what
Radioactivity
103
Women who was unable to speak after winning a Nobel Prize in physics for helping to discover radioactivity
Marie Curie
104
Three types of radioactivity named by Ernest Rutherford
Alpha, beta, & gamma rays
105
Beam of positively charged particles, helium nuclei
Alpha rays
106
Beam of negatively charged particles, electrons
Beta rays
107
High energy radiation, no charge, does not consist of particles, similar to x rays
Gamma rays
108
JJ ThOmpson created what model for the atom where the atom is mainly composed of protons with some electrons embedded randomly throughout
Plum Pudding model
109
Ernest Rutherford with Geiger & Marsden studied scattering a beam of alpha particles by a thin gold foil, what were they surprised about
Some alpha particles had large scattering angles, a few even bounced back
110
Rutherford's new model of the atom, 2 distinct parts. Called the nuclear model for the atom
1) dense central core (nucleus), + charge 2) negatively charged electrons surround the nucleus & are far removed from the nucleus
111
Protons discovered by who
Rutherford
112
Neutrons discovered by who
James Chadwick
113
Magnitude charge of protons & electrons
P: +1.60*10^-19C E: same, but -
114
Mass of an atom
1*10^-23g
115
Diameter of an atom
1*10^-10m
116
Diameter of the nucleus
1*10^-14m
117
Henry Moseley discovered that the number of what characterizes an element
Protons
118
Letter representing atomic number (# of protons)
Z
119
Letter representing mass number (# of protons + neutrons)
A
120
Define isotope
Same element with different mass #'s
121
Nucleus of a specific isotope called a
nuclide
122
Cobalt 60 used for
Cancer radiation therapy
123
Cesium 137 used for
Food sterilization
124
Iodine 129 used for
Thyroid radiation therapy
125
Technetium 99 used for
Medical imaging of internal organs
126
Scientist who discovered isotopes
JJ ThOmpson
127
#2 in Dalton's theory changed to what after isotopes were discovered
2) All atoms of a given element have the same number of protons & chemical properties
128
Mendeleev & Meyer arranged elements by increasing atomic number in what kinds of a row
horizantal
129
Elements with similar chemical properties are arranged in columns called
groups
130
Metals are located left & center of the periodic table, they have what properties
good conductors of heat & electricity, luster, ductile, malleable, solid at room temp (except mercury)
131
Nonmetals are located to right of the periodic table, they have what properties
poor conductors of heat & electricity, solids are brittle, dull surface
132
Metalloids located to the right & center of the periodic table, divide nonmetals & metals, properties are
intermediate between metals & nonmetals
133
Group A elements are called main group elements or
representative elements
134
Group B elements are called
transition elements
135
Two rows below table are called what, broken down into lanthanide & actinide elements
inner transition elements
136
Group 1A called
alkali metals (except hydrogen)
137
Group 2A called
alkaline earth metals
138
Group 6A called
chalcogens
139
Group 7A called
halogens
140
Group 8A called
noble (rare) gases
141
What are the only elements that exist in nature as free, single atoms
Group 8A, the noble gases
142
Atoms combine in what two ways
1) sharing electrons- forms molecules, 2) transferring electrons- forms ionic compounds
143
When nonmetals form with nonmetals or metalloids, this forms. Definite shape, constant composition applies, all are neutral
molecules
144
Different forms of an element are called
allotropes
145
Composed of two or more different nonmetals or metalloids
molecular compounds
146
Chemical formula denoting the exact number of atoms of each element in a molecule
molecular formula
147
Gives the simplest whole number ratio of atoms of each element in the compound
empirical formula (C6H6 becomes CH, C2H4 becomes CH2, CH4 stays the same)
148
Shows which atoms are connected together
structural formulas
149
Species containing a net charge either by gaining electrons or losing electrons
ions
150
A cation is a positively charged ion that is attracted to a negative what in an electrolyte cell
cathode
151
An anion is a negatively charged ion that is attracted to a positive what in an electrolyte cell
anode
152
Metals tend to what
lose electrons- cations
153
Nonmetals tend to what
gain electrons- anions
154
Ions with only one atom are called what
monatomic ions
155
Are monatomic metal ions formed by losing or gaining electrons
losing
156
Are monatomic nonmetal ions formed by losing or gaining electrons
gaining
157
Predicting charges for stable monatomic ions in Group 1A or 2A
of electrons the metal atoms lose is equal to the group #
158
Predicting charges for the number of electrons that a nonmetal atom gains is
Group 7A: gain 1 electron to form X- ions, Group 6A: gain 2 electrons to form X2- ions, Group 5A: gain 3 electrons to form X3- ions
159
Ions that consist of atoms chemically bonded together in a molecular sense & carry a net charge
polyatomic ions
160
These are composed of cations & anions interacting in appropriate proportions to yield an overall neutral compound, forms a crystal lattice structure
ionic compounds
161
Chemical formulas of ionic compounds are always represented in which fashion
empirical formula
162
Formulas for ionic compounds
1) always neutral, 2) cation written first, then anion, 3) subscripts denote # of ions in each type required to yield a neutral compound (formula unit)
163
For charge balance of ionic compounds, the subscript of the cation is equal to the charge on the anion, the subscript of the anion is equal to the charge of the
Cation (Na+ + CO3^2- turns into Na2CO3)
164
How do you name ionic compounds
Cation first, anion second
165
Transition metal ions can form stable ions with variable changes, you use what to name them
stock system, written as element name (charge) ion
166
Naming polyatomic cations
name ends in -ium, + cation (ex: ammonium ion)
167
Naming monatomic nonmetal anions
name derived from stem of element followed by -ide plus ion
168
Naming polyatomic anions
many contain O2 & have suffixes ate & ite
169
OH-
hydroxide ion
170
CN-
cyanide ion
171
O2^2-
peroxide ion
172
CO3^2-
carbonate ion
173
HcO3^-
hydrogen carbonate ion
174
MnO4^-
permanganate ion
175
CrO4^2-
chromate ion
176
Cr2O7^2-
dichromate ion
177
PO4^3-
phosphate ion
178
SCN-
thiocyanate ion
179
C2H3O2-
acetate ion
180
NO2-
nitrite ion
181
NO3-
nitrate ion
182
SO3^2-
sulfite ion
183
SO4^2-
sulfate ion
184
ClO2-
chlorite ion
185
ClO3-
chlorate ion
186
Oxoanions are used for a homologous series with the same central atom w/ a variable number of oxygen atoms, when do you use what suffix
ite suffix (less oxygen), ate suffix (more oxygen). If more than two in series, hypo prefix (even less oxygen than ite) or per (even more oxygen than ate)
187
Naming ionic compounds
Cation named first, then anion, anion not used in name
188
Transition metal ionic compounds specify the charge by using what
stock system
189
Acids are compounds that yield hydronium ions when dissolved in water, named how
acids based on anions whose name ends in -ide, add hydro and change -ide to -ic acid. acids from oxoanions, change the suffix...-ate suffix to -ic acid, for -ite suffix change to -ous acid
190
Binary molecular compounds contain only 2 elements, name them how
name first as the element & second as an anion, use greek prefixes to specify the # of each element, when prefix ends in a or o & the anion name begins with a vowel, then a or o of prefix is often omitted. Acids whose anion ends in ide, if they aren't in water they are named as molecular compounds
191
Hydrates are compounds with a specific number of water molecules that are what
strongly adhered
