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Chemistry 111 Flashcards

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1
Q

chemistry

A

study of matter and its properties, the changes that matter undergoes, and the energy associated with those changes

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2
Q

matter

A

anything that has mass and volume

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3
Q

composition

A

types and amounts of simpler substances that makes it up

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4
Q

properties

A

characteristics that give each substance it unique identity

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5
Q

physical properties

A

characteristics a substance shows by itself, without changing into or interacting with another substance

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6
Q

chemical properties

A

characteristics a substance shows as it changes into or interacts with another substance(s)

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7
Q

physical change

A

occurs when a substance alters its physical properties and not its composition

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8
Q

chemical change

A

occurs when a substance(s) is converted into a different substance(s)

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9
Q

solid

A

fixed shape that conforms to container; particles lie next to each other in a regular, 3D array

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10
Q

liquid

A

varying shape that conforms to container, has an upper surface; particles lie close together but move randomly around each other

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11
Q

gas

A

varying shape that conforms to container, no upper surface; particles have large distances between them and move randomly throughout container

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12
Q

energy

A

ability to do work

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13
Q

potential energy

A

energy is due to the position of the object relative to other objects

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14
Q

kinetic energy

A

energy due to the motion of the object

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15
Q

conversion factors

A

ratios used to express a quantity in different units

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16
Q

SI units

A

french “syteme internaional d’unites”, seven fundamental units from which other units are derived from

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17
Q

meter

A

1m is distance light travels in a vacuum in 1/299792458 second

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18
Q

volume

A

amount of space any sample matter occupies

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19
Q

cubic meter

A

m^3–SI unit; (1L=1dm^3=10^-3m^3)

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20
Q

mass

A

quantity of matter an object contains

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21
Q

kilograms

A

(kg) SI unit

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22
Q

density

A

(d) density equals mass divided by volume (kg/m^3 SI)

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23
Q

temperature

A

(t) a measure of how hot or cold one object is relative to another

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24
Q

heat

A

the energy that flows from the object with the higher temperature to the object with the lower temperature

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25
Q

thermometer

A

a narrow tube containing a fluid that expands when heated

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26
Q

kelvin

A

SI unit for temperature

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27
Q

Kelvin (absolute scale)

A

same size degree as celsius scale, 1/100 of the difference between freezing and boiling points of water–but has a different zero point (0K=Absolute zero=-273.15degrees Celsius)

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28
Q

celsius scale

A

sets water’s freezing point at 0 degrees and boiling point at 100 degrees

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29
Q

second

A

(s) SI unit, atomic standard (1 second = 9192631770 oscillations of microwave radiation absorbed by gaseous cesium atoms cooled to around 10^-6 K)

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30
Q

extensive properties

A

some variables dependent on the amount of substance present

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31
Q

intensive properties

A

independent of the amount of substance

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32
Q

uncertainty

A

+/- amount that is unknown/not exact, device used depends on how much uncertainty is acceptable

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33
Q

significant figures

A

the digits we record, both certain and the uncertain ones

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34
Q

exact numbers

A

have no uncertainty associated with; do not limit the number of sig figs in a calculation

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35
Q

precision

A

reproducibility, refers to how close the measurements in a series are to each other

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36
Q

accuracy

A

refers to hoe close each measurement is to the actual value

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37
Q

systemic error

A

produces values that are either all higher or all lower than the actual value; part of the experimental system (faulty device or consistent reading mistake)

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38
Q

random error

A

in the absence of systemic error, produces values that are higher and lower than the actual vaule

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39
Q

calibration

A

comparing the measuring device with a known standard

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40
Q

proton

A

positive charge

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41
Q

neutron

A

neutral charge/no charge

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42
Q

electron

A

negative charge

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43
Q

atomic number

A

(z) number of protons in the nucleus of each an elements’ atoms

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44
Q

mass number

A

(A) total number of protons and neutrons in the nucleus of an atom–each proton and each neutron contributes to one unit to the mass number

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45
Q

atomic symbol

A

(element symbol) of an element is based on its english, latin, or greek name

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46
Q

isotopes

A

of an element are atoms that have different number of neutrons and therefore different mass numbers

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47
Q

atomic mass unit (amu)

A

1/12 of the mass of a 12carbon atom

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48
Q

dalton

A

(Da) same as atomic mass unit (amu)

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49
Q

mass spectrometry

A

a method for measuring the relative masses and abundances of atomic scale particles very precisely

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50
Q

isotopic mass

A

relative mass of a isotope

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51
Q

atomic mass/atomic mass weight

A

of an element, the average of the masses of its naturally occurring isotope weighted according to their abundances

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52
Q

(modern) periodic table of the elements

A

based on Mendelev’s version but arranged by the atomic number (not mass)

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53
Q

period

A

horizontal rows; each period has number 1-7

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54
Q

groups

A

vertical column; each group has a number 1-8 and either A or B (newer system has only number 1-18 but no letters)

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55
Q

metals

A

large lower-left portion, 3/4 of the elements. (Many main group elements, and all transition and inner transition elements) Generally shiny solids at room temperature (mercury excluded) that conduct heat and electricity well; malleable and ductile

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56
Q

nonmetals

A

lie in small upper-right portion, generally gases or dull, brittle solids at room temperature (bromine excluded) and conduct heat/electricity poorly

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57
Q

metalloids (semimetals)

A

lie along the staircase line, have properties between those of metals and nonmetals

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58
Q

organic chemistry

A

studies the compounds of carbon, specifically those that contain hydrogen, oxygen, nitrogen, and a few others

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59
Q

inorganic chemistry

A

studies compounds of all the other elements and is concerned with catalysts, electronic materials, metal alloys, mineral salts, and etc.

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60
Q

electromagnetic radiation

A

(electromagnetic energy or radiant energy) consists of energy propagated by electric and magnetic fields that increase and decrease in intesity as they move through space

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61
Q

frequency

A

(v) of a wave is the number of cycles it undergoes per second; unit=1second or 1/s^-1 (also called hertz)

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62
Q

wavelength

A

(^ or lambda) distance between any point on a wave and the corresponding point on the next crest (or trough) of the wave… distance the wave travels during one cycle; unit=nm(10^-9), pm(10^-12), or A{with circle on top} (10^-10)

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63
Q

speed

A

distance of a wave is the distance it moves per unit time (m/s)

64
Q

speed of light

A

(c) physical constant; 3.0x10^8m/s

65
Q

amplitude

A

the height of a crest (or depth of a trough) of a wave

66
Q

electromagnetic spectrum

A

all waves in the spectrum travel at the same speed through a vacuum but differ in frequency and, therefore, wavelength

67
Q

infrared

A

(IR) region meets the microwave region on one end and the visible region on the other

68
Q

monochromatic

A

single wavelength (light of….)

69
Q

polychromatic

A

light of many wavelengths

70
Q

ultraviolet

A

(UV) region adjacent to visible light on short wavelengths end… UV radiation/UV light

71
Q

refraction

A

when a light wave passes from one medium into another, the speed of the wave changes; change in speed cause change in direction

72
Q

dispersion

A

[white] light separates into component colors when it passes through a prism (or other refracting object)… each incoming wave is refracted at a different angle

73
Q

diffraction

A

when a wave strikes the edge of an object, it bends around it in a phenomenon called diffraction; if slit= wavelength, forms semicircular wave

74
Q

interference

A

when waves of light pass through two adjacent slits, the nearby emerging circular waves interact

75
Q

black body

A

an idealized object that absorbs all the radiation incident on it, a hollow cube with a small hole in one wall that would absorb all energy approximates a blackbody

76
Q

blackbody radiation

A

changer in intensity and wavelength of emitted light as an object is heated

77
Q

quantum number

A

a positive integer

78
Q

Planck’s constant

A

(h) energy in joules and frequency in s^-1, h=JxS;

h=6.62606876x10^-34J{dot}s

79
Q

quantum

A

each energy packet, a quantum of energy=HxV; each change in an atom’s energy occurs when it absorbs or emits one quantum

80
Q

photoelectric effect

A

when monochromatic light of sufficient frequency shines on a metal plate, a current flows

81
Q

photon theory

A

Eistein’s; light itself is particulate, quantized into tiny “bundles” of energy

82
Q

photon

A

tiny “bundles” of light energy

83
Q

line spectra

A

a series of fine lines at specific frequencies separated by black spaces

84
Q

stationary states

A

certain energy levels; each state is associated with a fixed circular orbit of the electron around the nucleus (higher energy, farther orbit)

85
Q

ground state

A

lowest energy level (1st)

86
Q

excited state

A

when the electron is in any orbit farther from the nucleus, the atom is in an excited state

87
Q

ionization energy

A

energy required to form 1 mole of gaseous ions form 1 mole of gaseous atoms

88
Q

spectrometry/spectroscopy

A

refers to a large group of instrumental techniques that obtain spectra to gather data on a substance’s atomic and molecular energy levels

89
Q

emission spectra

A

occurs when atoms in an excited state emit photon as they return to a lower energy state

90
Q

flame tests

A

performed by placing a granule of ionic compound or a drop of it solution in a flame, rely on these intense emissions to determine elemental composition

91
Q

absorption spectrum

A

produced when atoms absorb photons of certain wavelengths and become excited

92
Q

de Broglie wavelength

A

matter behaves as though it moves in a wave; an object’s wavelength is inversely proportional to its mass

93
Q

wave-particle duality

A

dual character of matter and energy, both matter and energy show booth behaviors

94
Q

uncertainty principle

A

states that it is impossible to know simultaneously the position and momentum (mass times speed) of a particle

95
Q

quantum mechanics

A

which examines the wave nature of the objects on the atomic scale

96
Q

atomic orbital

A

(wave functions) Ψ, a mathematical description of the electron’s matter-wave in 3D

97
Q

hamiltonian operator

A

represents a set of mathematical operations that, when carried out with a particular Ψ, yields one of the allowed energy states of the atom

98
Q

electron density diagram

A

(electron probability density diagram) the pictorial representation for a given energy sublevel of the quantity Ψsquared as a function of r

99
Q

electron cloud depictions

A

imaginary picture, as if taking a time lapse picture of wave-like motion of the electrons

100
Q

radical probability distribution plot

A

number of electrons in energy ring vs the distance from the center

101
Q

probability contour

A

the electron is somewhere within that volume 90% of the time

102
Q

principal quantum number

A

is a positive integer; indicates the relative size of the orbital and therefore the relative distance from the nucleus of the peak int he radial probability distribution plot

103
Q

angular momentum quantum number

A

(l) is an integer from o to (n-1); related to the shape of the orbital

104
Q

magnetic quantum number

A

is an integer from -1 through 0 to +1; prescribes the 3D orientation of the orbital int he space around the nucleus

105
Q

atom’s energy levels

A

(shells), given by the n-value

106
Q

sublevels

A 
(subshells) l-value; divided energy levels 
l=0-->s
l=1-->p
l=2-->d
l=3-->f
107
Q

s orbital

A

spherical shape, one orientation (ml=0), one node

108
Q

p orbital

A

l=1, has 2 regions/lobes of high probability, are on either side of the nucleus

109
Q

d orbital

A

five possible ml values, any one of five orientation, l=2

110
Q

Spin quantum number

A

corresponding to the two directions of the electron’s field, has two possible values (+1/2,-1/2)

111
Q

exclusion principle

A

no two electrons in the same atom can have the same four quantum numbers

112
Q

the effect of nuclear charge (Z) on sublevel energy

A

a higher nuclear charge increases nucleus-electron attractions and, thus, lowers sublevel energies (stabilizes the atom)

113
Q

shielding

A

(“screening”) reduces the full nuclear charge to an effective nuclear charge

114
Q

effective nuclear charge (Zeff)

A

the nuclear charge an electron actually experiences, and this lowers nuclear charge makes the electron easier to remove

115
Q

penetration (has Z effects)

A

~it increases the nuclear attraction for a 2s electron over that for a 2p electron
~ it decreases the shielding of a 2s electron by the 1s electrons

116
Q

splitting of levels into sublevels

A

penetration and the resulting effects on shielding cause an energy level to split into sublevels of differing energy

117
Q

Aufbau principle

A

start at beginning of periodic table and add one proton to the nucleus and one electron to the lowest energy sublevel available

118
Q

orbital diagram

A

a box for each orbital in a given energy level, grouped by sublevel, with arrow representing an electron and its spin

119
Q

Hund’s rule

A

when orbitals of equal energy are available, the electron configuration of lowest energy has the maximum numbers of unpaired electrons with parallel spins

120
Q

transition elements

A

those in which d orbitals are being filled

121
Q

inner (core) electrons

A

those an atom has in common with the previous noble gas and any completed transition series… they fill in all the lower energy levels of an atom

122
Q

outer electrons

A

those in the highest energy level (highest n value)… they mostly spend time farthest from the nucleus

123
Q

valence electrons

A

those involved in forming compounds
~for main-group elements, the valence electrons are the outer electrons
~for transition elements, in addition to the outer ns electrons;
the (n-1)d electrons=valence, though metals Fe–>Zn may only use a few, if any, of their d electrons in bonding

124
Q

inner transition elements

A

those which f orbitals are being filled

125
Q

lanthanides

A

(rare earths) period 6, 4f orbitals are filled, after La

126
Q

actinides

A

period 7, 5f orbitals are filled.. after Ac

127
Q

atomic size

A

(the extent of the contour) in terms of how closely one atom lies next to another

128
Q

metallic radius

A

used mostly for metals, it is 1/2 the shortest distance between nuclei of adjacent, individual atoms in a crystal of the element

129
Q

covalent radius

A

used for elements occurring as molecules, mostly nonmetals, it is 1/2 the shortest distance between nuclei of bonded atoms

130
Q

ionization energy

A

(IE) the energy required for complete removal of 1 mol of electrons from 1 mol of gaseous atoms or ions

131
Q

electron affinity

A

(EA) the energy change (kJ/mol) accompanying the addition of 1 mol of electrons to 1 mol of gaseous atoms or ions

132
Q

redox behavior

A

whether it behaves as an oxidizing or reducing agent and the associated charges in its oxidations number

133
Q

amphoteric

A

can act as acids or bases in water

134
Q

isoelectric

A

“iso=same”– ions= “isoelectric” as nearest noble gas; having the same number of electrons or valence electrons

135
Q

pseudo-noble gas configuration

A

(n-1)d configuration attains stability of empty ns and np sublevels filled inner (n-1)d sublevels

136
Q

pragmagnetism

A

attracted by an external field [being or relating to a magnetizing substance that has small but positive susceptibility which varies little with magnetizing force]

137
Q

diamagnetism

A

it is not attracted (an is slightly repelled) by the field

138
Q

ionic radius

A

a measure of the size of the ion and is obtained from the distance between the nuclei of adjacent ions in a crystalline ionic compound

139
Q

ionic compounds

A

transferring electrons from one element to another

140
Q

covalent compounds

A

sharing electrons between atoms of different elements

141
Q

chemical bonds

A

the forces that hold the atoms together in a compound

142
Q

ions

A

charged particles that form when an atom (or small group of atoms) gains/loses one or more electrons

143
Q

binary ionic compounds

A

simplest type of ionic compound, one composed of 2 elements (typically when a metal reacts with a nonmetal)

144
Q

cation

A

positively charged ion

145
Q

anion

A

negatively charged ion

146
Q

monatomic ion

A

a cation or anion derived from a single atom

147
Q

coulomb’s law

A

the energy of attraction (or repulsion) between two particles is directly proportional to the product of the charges and inversely proportional to the distance between them

148
Q

covalent bond

A

a pair of electrons mutually attracted by two nuclei

149
Q

polyatomic ions

A

consist of two or more atoms bonded covalently and have a net positive or negative charge

150
Q

ionic bonding

A

between atoms with large differences in their tendencies to lose or gain electrons

151
Q

metallic bonding

A

the enormous number of atoms in a sample of a metal “pool”their valence electrons into a “sea” of electrons the “flow” between and around each metal-ion core (nucleus plus inner electrons) –>attracting them together

152
Q

lewis electron dot symbol

A

the element symbol represents the nucleus and inner electrons, and dots around the symbol represent the valence electrons

153
Q

octet rule

A

when atoms bond, they lose, gain, or share electrons to attain a filled outer level of eight electrons (or two for H and Li?)

154
Q

Lattice energy

A

the enthalpy change that accompanies the reverse of this equation- 1 mol of ionic solid separating into gaseous ions

155
Q

Born-Haber cycle

A

a series of steps from elements to ionic solid for which all the enthalpies are known except the lattice energy

156
Q

ion pairs

A

gaseous ionic molecules, rather than individual ions

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