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Chemistry 111 > Test 1 Study Guide > Flashcards

Test 1 Study Guide Flashcards

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

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2
Q

SI/Base Unit: Length

A

meter; meter

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3
Q

SI/Base Unit: Volume

A

cubic meter (m^3); Liter

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4
Q

SI/Base Unit: Time

A

seconds; seconds

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5
Q

SI/Base Unit: temperature

A

Kelvin; K,C,F

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6
Q

How do you estimate digits on an analog instrument?

A

Estimate the last digit

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7
Q

How do you estimate digits on a digital instrument?

A

The last digit is already an estimated digit

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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.

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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.

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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

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11
Q

Rules of significant figures.

A
  1. Start counting with the first non-zero digit
  2. All non-zero numbers are significant
  3. Captive zeroes: always significant
  4. Leading zeroes: never significant
  5. Trailing zeroes: significant after decimal, not significant if no decimal
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12
Q

Rules of addition/subtraction with significant figures.

A

Least number of decimal places

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13
Q

Rules of multiplication/division with significant figures.

A

Least number of significant figures

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14
Q

Metric Prefix: Tera

A

T; 10^12

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15
Q

Metric Prefix: Giga

A

G; 10^9

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16
Q

Metric Prefix: Mega

A

M; 10^6

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17
Q

Metric Prefix: kilo

A

k; 10^3

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18
Q

Metric Prefix: hecto

A

h; 10^2

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19
Q

Metric Prefix: deca

A

da; 10^1

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20
Q

Metric Prefix: deci

A

d; 10^-1

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21
Q

Metric Prefix: centi

A

c; 10^-2

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22
Q

Metric Prefix: milli

A

m; 10^-3

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23
Q

Metric Prefix: micro

A

µ; 10^-6

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24
Q

Metric Prefix: nano

A

n; 10^-9

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25
Q

Metric Prefix: pico

A

p; 10^-12

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26
Q

SI/Base Unit: mass

A

kilogram; gram

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27
Q

1 mL = ___ cm^3

A

1

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28
Q

The formula for density?

A

density = mass / volume

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29
Q

SI/Base Unit: Density

A

kg/m^3
Liquids/solids: g/cm^3 or g/mL
gas: g/L

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30
Q

What is temperature?

A

A measurement of the average kinetic energy of particles

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31
Q

The formula for Celsius to Kelvin?

A

K = C + 273.15

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32
Q

The formula for Celsius to Fahrenheit?

A

F = (1.8*C) + 32

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33
Q

The formula for Fahrenheit to Celsius?

A

C = (F - 32) / 1.8

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34
Q

What is energy?

A

The capacity to do work (the process of causing matter to move against a force).

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35
Q

What is potential energy?

A

The energy that an object possesses because of its position, composition, or condition. Ex. water at the top of a hill

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36
Q

What is kinetic energy?

A

The energy of motion. Ex. water rushing down a hill

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37
Q

What is chemistry?

A

The study of matter, its composition, structure, states, properties, and the changes it undergoes.

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38
Q

What is matter?

A

Anything that has mass and takes up space.

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39
Q

What are the three states of matter?

A

Solid, Liquid, Gas

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40
Q

What is a solid?

A

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.

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41
Q

What is a liquid?

A

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.

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42
Q

What is a gas?

A

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.

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43
Q

What is an atom?

A

The smallest particle of an element that still has properties of that element.

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44
Q

What is a molecule?

A

2 or more atoms joined together by a chemical bond.

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45
Q

What is a pure substance?

A

A substance made up of only one type of component.

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46
Q

What is a mixture?

A

Two or more particles that are combined, but not chemically.

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47
Q

What is the difference between an element and a compound?

A

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.

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48
Q

What is the difference between a homogeneous and heterogeneous mixture?

A

A homogeneous solution is uniform throughout and a heterogeneous solution is not uniform throughout.

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49
Q

What is the difference between a physical and chemical change?

A

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.

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50
Q

What are examples of physical changes?

A

Luster, Melting/boiling point, phase of matter, density, solubility, odor, shape

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51
Q

What are examples of chemical changes?

A

Flammability, pH, combustibility, reactivity, ability to oxidize (rust)

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52
Q

What laws did Dalton know?

A
  1. Law of Conservation of Mass
  2. Law of Definite Proportions
  3. Law of Multiple Proportions
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53
Q

What is the law of conservation of matter?

A

Matter cannot be created or destroyed.

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54
Q

What is the law of definite proportions?

A

(law of constant composition) All samples contain the same elements in the same proportion by mass. H_2O: 11% H and 89% O.

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55
Q

What is the law of multiple proportions?

A

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.

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56
Q

What is Dalton’s Atomic Theory?

A
  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
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57
Q

What did JJ Thomson discover?

A

The electron, plum pudding model of the atom

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58
Q

Who discovered the electron?

A

JJ Thomson

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59
Q

What did Robert Millikan discover?

A

Charge of the electron; -1.6 x 10^-19 C

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60
Q

Who discovered the charge of the electron?

A

Robert Millikan

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61
Q

What did Ernest Rutherford discover?

A

Proton; modern nuclear atom

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62
Q

Who discovered the proton?

A

Ernest Rutherford

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63
Q

What did James Chadwick discover?

A

Neutron

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64
Q

Who discovered the neutron?

A

James Chadwick

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65
Q

What is the mass number?

A

(A) number of protons + neutrons

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66
Q

What is the atomic number?

A

(Z) number of protons (electrons in a neutral atom)

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67
Q

What is an isotope?

A

Atoms with the same atomic number (Z), but different mass numbers (A).

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68
Q

What is the difference between atomic mass and atomic weight?

A

Atomic mass is the mass of a single atom; whereas, atomic weight is the average mass of all isotopes.

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69
Q

What is the atomic weight of an element closest to?

A

The mass of the most abundant isotope.

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70
Q

The formula for atomic weight?

A

Σ (fractional abundance) x (isotope mass)

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71
Q

What is a mole? What number defines it?

A

The number of carbon atoms in exactly 12 grams of carbon-12. Avogadro’s number: 6.022 x 10^23 particles = 1 mol

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72
Q

What is the molar mass?

A

The mass of 1 mole of an element. It is the atomic mass expressed in grams. Also called formula weight and molecular weight.

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73
Q

What do the subscripts in a formula show?

A

The moles of each element in 1 mole of compound

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74
Q

What are the parts of a wave?

A
  1. Amplitude
  2. Wavelength (λ)
  3. Frequency (ν)
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75
Q

What is amplitude?

A

The vertical height (center point to crest or trough) of a wave and is related to the energy the wave is carrying (light intensity).

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76
Q

What is wavelength (λ)?

A

The distance between successive crests on the wave (or any two analogous points)

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77
Q

What is frequency (v)?

A

The number of crests that pass a given location per second, usually reported in Hz.

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78
Q

What is the order from lowest energy to highest energy on the electromagnetic spectrum?

A

Radio, Microwave, Infrared, Visible (ROYGBIV), Ultraviolet, X-ray, Gamma-ray

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79
Q

What is the order from lowest frequency to highest frequency on the electromagnetic spectrum?

A

Radio, Microwave, Infrared, Visible (ROYGBIV), Ultraviolet, X-ray, Gamma-ray

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80
Q

What is the order from longest wavelength to shortest wavelength on the electromagnetic spectrum?

A

Radio, Microwave, Infrared, Visible (ROYGBIV), Ultraviolet, X-ray, Gamma-ray

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81
Q

What is the speed of light in a vacuum?

A

(c) 3.00 x 10^8 m/s

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82
Q

The formula that relates wavelength and frequency to speed?

A

c = λ*v

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83
Q

What is constructive interference?

A

When two waves are aligned in such a way as to always add to give increased crest height (amplitude).

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84
Q

What is destructive interference?

A

When two waves are aligned in such a way as to cancel out each other’s effect.

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85
Q

What did Einstein conclude from his photoelectric effect experiment?

A

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.

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86
Q

The formula that relates the energy of a photon to frequency?

A

E = h * v

Energy = J
h = J*s
v = Hz

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87
Q

The formula that relates the energy of a photon to wavelength.

A

E = (h*c) / λ

Energy = J
h = J*s
c = m/s
λ = m

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88
Q

What is Planck’s constant?

A

A proportionality constant with a value of 6.626 x 10^-34 J*s

89
Q

What is the atomic line spectra?

A

The electromagnetic radiation that is either absorbed or emitted by atoms.

90
Q

What is the Bohr model of the hydrogen atom?

A

There are only certain allowable energy states for the electron and these energy states are linked to orbits of a specific radius.

91
Q

What happens when an electron changes energy states?

A
  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
Q

The formula for DeBroglie’s equation?

A

λ = h / (m*v)

93
Q

What did Louis DeBroglie propose?

A

Proposed that the electron has a wave behavior.

94
Q

What does the uncertainty principle tell you?

A

It is fundamentally impossible to determine simultaneously and exactly both the momentum and position of the particle.

95
Q

Who came up with the uncertainty principle?

A

Werner Heisenberg

96
Q

What did Schrodinger tell us about an electron?

A

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
Q

What are the quantum numbers?

A
  1. primary quantum number (n)
  2. angular quantum number (l)
  3. magnetic quantum number (m_l)
  4. spin quantum number (m_s)
98
Q

What are the valid values for the 4 quantum numbers?

A
  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
Q

What does the primary quantum number tell us?

A

The size of the orbital

100
Q

What does the angular quantum number tell us?

A

The shape of the orbital

101
Q

Subshell name: l = 0

A

”s” subshell

102
Q

Subshell name: l = 1

A

“p” subshell

103
Q

Subshell name: l = 2

A

“d” subshell

104
Q

Subshell name: l = 3

A

“f” subshell

105
Q

Shape of “s” subshell?

106
Q

Shape of “p” subshell?

107
Q

Shape of “d” subshell?

A

4 clover leafs, 1 dumbbell w/ donut

108
Q

What does the magnetic quantum number tell us?

A

The specific orientation of the orbital in 3D space.

109
Q

What is the Pauli exclusion principle?

A
  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
Q

Who is credited with discovering the periodic table?

A

Dimitri Mendeleev

111
Q

Al

112
Q

aluminum

113
Q

Mn

114
Q

manganese

115
Q

Ar

116
Q

argon

117
Q

Hg

118
Q

mercury

119
Q

B

120
Q

boron

121
Q

Ne

122
Q

neon

123
Q

Ba

124
Q

barium

125
Q

Ni

126
Q

nickel

127
Q

Br

128
Q

bromine

129
Q

N

130
Q

nitrogen

131
Q

Ca

132
Q

calcium

133
Q

O

134
Q

oxygen

135
Q

C

136
Q

carbon

137
Q

P

A

phosphorus

138
Q

phosphorus

139
Q

Cl

140
Q

chlorine

141
Q

Pt

142
Q

platinum

143
Q

Cr

144
Q

chromium

145
Q

K

146
Q

potassium

147
Q

Co

148
Q

cobalt

149
Q

Si

150
Q

silicon

151
Q

Cu

152
Q

copper

153
Q

Ag

154
Q

silver

155
Q

F

156
Q

fluorine

157
Q

Na

158
Q

sodium

159
Q

Au

160
Q

gold

161
Q

S

162
Q

sulfur

163
Q

He

164
Q

helium

165
Q

Sn

166
Q

tin

167
Q

H

168
Q

hydrogen

169
Q

Ti

170
Q

titanium

171
Q

I

172
Q

iodine

173
Q

W

174
Q

tungsten

175
Q

Fe

176
Q

iron

177
Q

U

178
Q

uranium

179
Q

Pb

180
Q

lead

181
Q

V

182
Q

vanadium

183
Q

Li

184
Q

lithium

185
Q

Xe

186
Q

xenon

187
Q

Mg

188
Q

magnesium

189
Q

Zn

190
Q

zinc

191
Q

Where are metals located on the periodic table?

192
Q

Where are nonmetals located on the periodic table?

A

Upper right side

193
Q

What are the metalloids on the periodic table?

A

Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium

194
Q

What are the properties of metals?

A

Luster (shiny), good conductor of heat, malleable

195
Q

What are the properties of non-metals?

A

Brittle, dull, good insulator

196
Q

What are the properties of metalloids?

A

Contain properties of both metals and non-metals

197
Q

What is the Aufbau Principle?

A

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
Q

Where are alkali metals on the periodic table?

199
Q

Where are alkaline earth metals on the periodic table?

200
Q

Where are the halogens on the periodic table?

201
Q

Where are the noble gases on the periodic table?

202
Q

What is the difference between a group and a series on the periodic table?

A

A group is a column and a series is a row

203
Q

What is Hund’s rule?

A

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
Q

What is the order of energy for electron configuration?

A

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p

205
Q

What are the valence electrons for main-group elements?

A

The outer electrons, which are those found in the largest shell for the atom having the highest “n” value.

206
Q

What are the valence electrons for the transition metals?

A

The outer electrons, electrons in highest “n” value, + electrons in uncompleted d and f subshells.

207
Q

What is paramagnetic?

A

When an atom has unpaired electrons (attracted to magnetic field)

208
Q

What is diamagnetic?

A

When an atom has no unpaired electrons (repelled by a magnetic field).

209
Q

What is atomic radii?

A

The atomic size or radius of the atom.

210
Q

Trend for atomic radii?

A
  1. Increases down a family (n increases)
  2. Increases right to left (effective nuclear charge decreases)
211
Q

What does Coulomb’s law tell us?

A

Like charges repel and opposite charges attract

212
Q

What is ionization energy?

A

Energy (in kJ) required to completely remove one mole of electrons from one mole of gaseous atoms or ions.

213
Q

Trend for ionization energy?

A
  1. Increases up a family
  2. Increases right to left
214
Q

What is metallic character?

A

A element that loses valence electrons easily.

215
Q

Trend for metallic character?

A
  1. Increases down a group (n increases)
  2. Increases right to left
216
Q

What is electron affinity?

A

Energy change in kJ accompanying the addition of one mole of electrons to one mole of gaseous atoms or ions.

217
Q

Trend for electron affinity?

A
  1. Increases left to right
  2. Only Group 1A really increases up a group
218
Q

Is ionization energy exothermic or endothermic?

A

Endothermic, requires energy (+magnitude)

219
Q

Is electron affinity exothermic or endothermic?

A

Exothermic, releases energy (-magnitude)

Chemistry 111 (5 decks)

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