Test 1 Study Guide Flashcards
(219 cards)
1
Q
What is a measurement?
A
A comparison against an exact invariable standard.
1. Size and magnitude (number)
2. Standard of comparison (unit)
3. Indication of uncertainty
2
Q
SI/Base Unit: Length
A
meter; meter
3
Q
SI/Base Unit: Volume
A
cubic meter (m^3); Liter
4
Q
SI/Base Unit: Time
A
seconds; seconds
5
Q
SI/Base Unit: temperature
A
Kelvin; K,C,F
6
Q
How do you estimate digits on an analog instrument?
A
Estimate the last digit
7
Q
How do you estimate digits on a digital instrument?
A
The last digit is already an estimated digit
8
Q
What is the difference between precision and accuracy?
A
Precision: The reproducibility of a measurement (how close your measurements are to each other).
Accuracy: How close you are to the true value.
9
Q
What do precision and accuracy depend on?
A
Precision: depends on how good you are at using the instrument.
Accuracy: Depends on the instrument you are using. The smaller the divisions, the more accurate.
10
Q
What is an exact number?
A
Numbers arrived at by direct count or are a defined relationship.
1. $12.52 / 2 dozen
2. 1000g = 1kg
11
Q
Rules of significant figures.
A
- Start counting with the first non-zero digit
- All non-zero numbers are significant
- Captive zeroes: always significant
- Leading zeroes: never significant
- Trailing zeroes: significant after decimal, not significant if no decimal
12
Q
Rules of addition/subtraction with significant figures.
A
Least number of decimal places
13
Q
Rules of multiplication/division with significant figures.
A
Least number of significant figures
14
Q
Metric Prefix: Tera
A
T; 10^12
15
Q
Metric Prefix: Giga
A
G; 10^9
16
Q
Metric Prefix: Mega
A
M; 10^6
17
Q
Metric Prefix: kilo
A
k; 10^3
18
Q
Metric Prefix: hecto
A
h; 10^2
19
Q
Metric Prefix: deca
A
da; 10^1
20
Q
Metric Prefix: deci
A
d; 10^-1
21
Q
Metric Prefix: centi
A
c; 10^-2
22
Q
Metric Prefix: milli
A
m; 10^-3
23
Q
Metric Prefix: micro
A
µ; 10^-6
24
Q
Metric Prefix: nano
A
n; 10^-9
25
Metric Prefix: pico
p; 10^-12
26
SI/Base Unit: mass
kilogram; gram
27
1 mL = ___ cm^3
1
28
The formula for density?
density = mass / volume
29
SI/Base Unit: Density
kg/m^3
Liquids/solids: g/cm^3 or g/mL
gas: g/L
30
What is temperature?
A measurement of the average kinetic energy of particles
31
The formula for Celsius to Kelvin?
K = C + 273.15
32
The formula for Celsius to Fahrenheit?
F = (1.8*C) + 32
33
The formula for Fahrenheit to Celsius?
C = (F - 32) / 1.8
34
What is energy?
The capacity to do work (the process of causing matter to move against a force).
35
What is potential energy?
The energy that an object possesses because of its position, composition, or condition. Ex. water at the top of a hill
36
What is kinetic energy?
The energy of motion. Ex. water rushing down a hill
37
What is chemistry?
The study of matter, its composition, structure, states, properties, and the changes it undergoes.
38
What is matter?
Anything that has mass and takes up space.
39
What are the three states of matter?
Solid, Liquid, Gas
40
What is a solid?
A state of matter with definite shape and definite volume. The particles are close together (fixed) and move very slowly. The interactions between atoms are very strong.
41
What is a liquid?
A state of matter with its shape being the same as the container it is in and its volume being definite. The particles are close together (random) and move at a moderate pace. The interactions between atoms are strong.
42
What is a gas?
A state of matter with its shape being the same as the container it is in and its volume being the same as the container it is in. The particles are far apart (random) and move at a very fast pace. The interactions between atoms are almost none.
43
What is an atom?
The smallest particle of an element that still has properties of that element.
44
What is a molecule?
2 or more atoms joined together by a chemical bond.
45
What is a pure substance?
A substance made up of only one type of component.
46
What is a mixture?
Two or more particles that are combined, but not chemically.
47
What is the difference between an element and a compound?
An element is only one type of atom and cannot be chemically broken down. A compound is 2 or more elements that are chemically bound together in a definite proportion.
48
What is the difference between a homogeneous and heterogeneous mixture?
A homogeneous solution is uniform throughout and a heterogeneous solution is not uniform throughout.
49
What is the difference between a physical and chemical change?
A physical change can be observed without changing the identity of the substance; whereas, a chemical change can only be observed by changing the identity of the substance.
50
What are examples of physical changes?
Luster, Melting/boiling point, phase of matter, density, solubility, odor, shape
51
What are examples of chemical changes?
Flammability, pH, combustibility, reactivity, ability to oxidize (rust)
52
What laws did Dalton know?
1. Law of Conservation of Mass
2. Law of Definite Proportions
3. Law of Multiple Proportions
53
What is the law of conservation of matter?
Matter cannot be created or destroyed.
54
What is the law of definite proportions?
(law of constant composition) All samples contain the same elements in the same proportion by mass. H_2O: 11% H and 89% O.
55
What is the law of multiple proportions?
When 2+ elements react to form more than one compound, a fixed mass of 1 element will react with the other element. CO: 12g C, 16g O. CO_2: 12g C, 32g O.
56
What is Dalton's Atomic Theory?
1. Matter is composed of atoms
2. Elements are only one type of atom
3. Each element has different properties
4. A compound is 2 or more atoms
5. Atoms are not created or destroyed
57
What did JJ Thomson discover?
The electron, plum pudding model of the atom
58
Who discovered the electron?
JJ Thomson
59
What did Robert Millikan discover?
Charge of the electron; -1.6 x 10^-19 C
60
Who discovered the charge of the electron?
Robert Millikan
61
What did Ernest Rutherford discover?
Proton; modern nuclear atom
62
Who discovered the proton?
Ernest Rutherford
63
What did James Chadwick discover?
Neutron
64
Who discovered the neutron?
James Chadwick
65
What is the mass number?
(A) number of protons + neutrons
66
What is the atomic number?
(Z) number of protons (electrons in a neutral atom)
67
What is an isotope?
Atoms with the same atomic number (Z), but different mass numbers (A).
68
What is the difference between atomic mass and atomic weight?
Atomic mass is the mass of a single atom; whereas, atomic weight is the average mass of all isotopes.
69
What is the atomic weight of an element closest to?
The mass of the most abundant isotope.
70
The formula for atomic weight?
Σ (fractional abundance) x (isotope mass)
71
What is a mole? What number defines it?
The number of carbon atoms in exactly 12 grams of carbon-12. Avogadro's number: 6.022 x 10^23 particles = 1 mol
72
What is the molar mass?
The mass of 1 mole of an element. It is the atomic mass expressed in grams. Also called formula weight and molecular weight.
73
What do the subscripts in a formula show?
The moles of each element in 1 mole of compound
74
What are the parts of a wave?
1. Amplitude
2. Wavelength (λ)
3. Frequency (ν)
75
What is amplitude?
The vertical height (center point to crest or trough) of a wave and is related to the energy the wave is carrying (light intensity).
76
What is wavelength (λ)?
The distance between successive crests on the wave (or any two analogous points)
77
What is frequency (v)?
The number of crests that pass a given location per second, usually reported in Hz.
78
What is the order from lowest energy to highest energy on the electromagnetic spectrum?
Radio, Microwave, Infrared, Visible (ROYGBIV), Ultraviolet, X-ray, Gamma-ray
79
What is the order from lowest frequency to highest frequency on the electromagnetic spectrum?
Radio, Microwave, Infrared, Visible (ROYGBIV), Ultraviolet, X-ray, Gamma-ray
80
What is the order from longest wavelength to shortest wavelength on the electromagnetic spectrum?
Radio, Microwave, Infrared, Visible (ROYGBIV), Ultraviolet, X-ray, Gamma-ray
81
What is the speed of light in a vacuum?
(c) 3.00 x 10^8 m/s
82
The formula that relates wavelength and frequency to speed?
c = λ*v
83
What is constructive interference?
When two waves are aligned in such a way as to always add to give increased crest height (amplitude).
84
What is destructive interference?
When two waves are aligned in such a way as to cancel out each other's effect.
85
What did Einstein conclude from his photoelectric effect experiment?
Einstein concluded that light energy is delivered to the atoms in packets called quanta or photons and that the energy of a photon of light is directly proportional to its frequency, or inversely to its wavelength.
86
The formula that relates the energy of a photon to frequency?
E = h * v
Energy = J
h = J*s
v = Hz
87
The formula that relates the energy of a photon to wavelength.
E = (h*c) / λ
Energy = J
h = J*s
c = m/s
λ = m
88
What is Planck's constant?
A proportionality constant with a value of 6.626 x 10^-34 J*s
89
What is the atomic line spectra?
The electromagnetic radiation that is either absorbed or emitted by atoms.
90
What is the Bohr model of the hydrogen atom?
There are only certain allowable energy states for the electron and these energy states are linked to orbits of a specific radius.
91
What happens when an electron changes energy states?
1. Electron jumps up: moves to larger radii orbit if the energy absorbed matches the gap between the orbits.
2. Electron falls down: photon of light corresponding to the energy difference is released
92
The formula for DeBroglie's equation?
λ = h / (m*v)
93
What did Louis DeBroglie propose?
Proposed that the electron has a wave behavior.
94
What does the uncertainty principle tell you?
It is fundamentally impossible to determine simultaneously and exactly both the momentum and position of the particle.
95
Who came up with the uncertainty principle?
Werner Heisenberg
96
What did Schrodinger tell us about an electron?
Created a model to describe the regions in space, or orbitals, where electrons are most likely to be found (90% of the time). His equation gives us 4 quantum numbers that tell us about the energy state of the electron and its probability distribution.
97
What are the quantum numbers?
1. primary quantum number (n)
2. angular quantum number (l)
3. magnetic quantum number (m_l)
4. spin quantum number (m_s)
98
What are the valid values for the 4 quantum numbers?
1. n = 1, 2, 3, 4, ....
2. l = 0, 1, 2, ..., n-1
3. m_l = -l, ...., 0, ..., +l
4. m_s = -1/2, +1/2
99
What does the primary quantum number tell us?
The size of the orbital
100
What does the angular quantum number tell us?
The shape of the orbital
101
Subshell name: l = 0
"s" subshell
102
Subshell name: l = 1
"p" subshell
103
Subshell name: l = 2
"d" subshell
104
Subshell name: l = 3
"f" subshell
105
Shape of "s" subshell?
sphere
106
Shape of "p" subshell?
dumbbell
107
Shape of "d" subshell?
4 clover leafs, 1 dumbbell w/ donut
108
What does the magnetic quantum number tell us?
The specific orientation of the orbital in 3D space.
109
What is the Pauli exclusion principle?
1. Each orbital can hold a maximum of 2 electrons.
2. Electrons in the same orbital repel each other.
3. Electrons in the same orbital must have magnetic spins cancel (spin in the opposite direction)(up, down).
110
Who is credited with discovering the periodic table?
Dimitri Mendeleev
111
Al
aluminum
112
aluminum
Al
113
Mn
manganese
114
manganese
Mn
115
Ar
argon
116
argon
Ar
117
Hg
mercury
118
mercury
Hg
119
B
boron
120
boron
B
121
Ne
neon
122
neon
Ne
123
Ba
barium
124
barium
Ba
125
Ni
nickel
126
nickel
Ni
127
Br
bromine
128
bromine
Br
129
N
nitrogen
130
nitrogen
N
131
Ca
calcium
132
calcium
Ca
133
O
oxygen
134
oxygen
O
135
C
carbon
136
carbon
C
137
P
phosphorus
138
phosphorus
P
139
Cl
chlorine
140
chlorine
Cl
141
Pt
platinum
142
platinum
Pt
143
Cr
chromium
144
chromium
Cr
145
K
potassium
146
potassium
K
147
Co
cobalt
148
cobalt
Co
149
Si
silicon
150
silicon
Si
151
Cu
copper
152
copper
Cu
153
Ag
silver
154
silver
Ag
155
F
fluorine
156
fluorine
F
157
Na
sodium
158
sodium
Na
159
Au
gold
160
gold
Au
161
S
sulfur
162
sulfur
S
163
He
helium
164
helium
He
165
Sn
tin
166
tin
Sn
167
H
hydrogen
168
hydrogen
H
169
Ti
titanium
170
titanium
Ti
171
I
iodine
172
iodine
I
173
W
tungsten
174
tungsten
W
175
Fe
iron
176
iron
Fe
177
U
uranium
178
uranium
U
179
Pb
lead
180
lead
Pb
181
V
vanadium
182
vanadium
V
183
Li
lithium
184
lithium
Li
185
Xe
xenon
186
xenon
Xe
187
Mg
magnesium
188
magnesium
Mg
189
Zn
zinc
190
zinc
Zn
191
Where are metals located on the periodic table?
Left Side
192
Where are nonmetals located on the periodic table?
Upper right side
193
What are the metalloids on the periodic table?
Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium
194
What are the properties of metals?
Luster (shiny), good conductor of heat, malleable
195
What are the properties of non-metals?
Brittle, dull, good insulator
196
What are the properties of metalloids?
Contain properties of both metals and non-metals
197
What is the Aufbau Principle?
The electron configuration with the lowest energy is one that fills in electrons from lowest energy position orbital in the atom outward to higher energy positions.
198
Where are alkali metals on the periodic table?
Group 1A
199
Where are alkaline earth metals on the periodic table?
Group 2A
200
Where are the halogens on the periodic table?
Group 7A
201
Where are the noble gases on the periodic table?
Group 8A
202
What is the difference between a group and a series on the periodic table?
A group is a column and a series is a row
203
What is Hund's rule?
When orbitals of equal energy are available, the electron configuration of lowest energy has the maximum number of unpaired electrons of parallel spin (up is best).
204
What is the order of energy for electron configuration?
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p
205
What are the valence electrons for main-group elements?
The outer electrons, which are those found in the largest shell for the atom having the highest "n" value.
206
What are the valence electrons for the transition metals?
The outer electrons, electrons in highest "n" value, + electrons in uncompleted d and f subshells.
207
What is paramagnetic?
When an atom has unpaired electrons (attracted to magnetic field)
208
What is diamagnetic?
When an atom has no unpaired electrons (repelled by a magnetic field).
209
What is atomic radii?
The atomic size or radius of the atom.
210
Trend for atomic radii?
1. Increases down a family (n increases)
2. Increases right to left (effective nuclear charge decreases)
211
What does Coulomb's law tell us?
Like charges repel and opposite charges attract
212
What is ionization energy?
Energy (in kJ) required to completely remove one mole of electrons from one mole of gaseous atoms or ions.
213
Trend for ionization energy?
1. Increases up a family
2. Increases right to left
214
What is metallic character?
A element that loses valence electrons easily.
215
Trend for metallic character?
1. Increases down a group (n increases)
2. Increases right to left
216
What is electron affinity?
Energy change in kJ accompanying the addition of one mole of electrons to one mole of gaseous atoms or ions.
217
Trend for electron affinity?
1. Increases left to right
2. Only Group 1A really increases up a group
218
Is ionization energy exothermic or endothermic?
Endothermic, requires energy (+magnitude)
219
Is electron affinity exothermic or endothermic?
Exothermic, releases energy (-magnitude)
