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CHEM > Chem CSET > Flashcards

Chem CSET Flashcards

1
Q

Freon

A

dichlorodifluoromethane

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2
Q

isolated system

A

there is no exchange of matter or energy

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3
Q

Closed system

A

allows for change in energy but not matter

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4
Q

What are the adverse effects of photochemical smog

A

Human health
damage to materials
toxic to plants
atmosphere

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5
Q

what substance can be found at the highest point of a fractionating column during fractional distillation of crude oil

A

propane

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6
Q

Which molecules require description with resonance structures

A

we can write two are more lewis structures that differ only in the position of electrons.

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7
Q

What type of EM spectrum is strong evidence for the big band theory

A

microwave

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8
Q

isotopes

A

atoms of the same number of protons but different number of neutrons
Same atomic number

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9
Q

atomc mass number

A

number or protons and neutrons

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10
Q

Principal quantum number

A

n
energy level or size of an orbital.
larger moving down a group

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11
Q

Ground state

A

lowest energy possible

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12
Q

Electron energy level

spdf

A

s = 1 -2
p =1-6
d = 1-10
f = 1-14

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13
Q

photon

A

electron transition from high to low energy orbital.
the difference in energy released.
weightless particle of electromagnetic radiation

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14
Q

types electromagnetic radiation

A 
heat
light
UV light
x rays
transverse wave
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15
Q

atomic spectrum

A

each transition H electrons make correspond to a different amount of energy and different color is released

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16
Q

Bohr model

A

a small positive nucleus surrounded by electrons located in a specific energy level

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17
Q

electron configuration

A

arrangement of electrons.

1s2

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18
Q

Group 1

A

alkali metals
soft
silvery
react violently with water

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19
Q

group 17

A

halogens

extremely reactive and poisonous

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20
Q

metals

A

shiny
conductive of heat and electricity
malleable
ductile

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21
Q

nonmetals

A

brittle,
dull
poor conductors
have low melting and boiling points

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22
Q

metalloids

A

has properties of metals and nonmetals

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23
Q

when determining molecular mass by osmotic measurement the molar mass will

A

be less

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24
Q

atomic radius

A

1/2 the distance between the nuclei of two bonded atoms

increase moving down and left

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25
Q

electromagnetic radiation

A

a form of energy that travels through space

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26
Q

ionization energy

A

the amount of energy required to remove an electron.

Increases moving up and right.

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27
Q

ionized

A

losing one or more outer electrons

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28
Q

electronegative

A

ability to attract other electrons.
increasing moving up and right.
cannot be measured directly.
has no unit of measurement

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29
Q

boiling point

A

increases then decreases across a period

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30
Q

metallic character along the periodic table

A

increases moving left and down

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31
Q

chemical reactivity

A

substances change chemically

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32
Q

photoelectric effect

A

when electrons are released after light is shone onto a metal

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33
Q

maxwell’s wave theory of light

A

brighter (high intensity) light would lead to higher energy electrons

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34
Q

quanta

A

quantities

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35
Q

E = hf

A

h = 6.63 x 10 ^-34
Quantum theory
F= frequency of radiation

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36
Q

quantum number

A

describe a specific aspect of an electron

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37
Q

angular/azimuthal momentum quantum number

A 
shape of the orbital
l
S= o
p=8
d=88
f = flower
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38
Q

magnetic quantum number

A 
position of the electron
m1
S=0
p= -1 to 1
d = -2 to 2
f = -3 to 3
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39
Q

spin quantum number

A

s
spin of the electron determines properties of the atom
+/- 1/2

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40
Q

properties of gas

A

expand to fill container
v of gas = v of container
can be compressed

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41
Q

ideal gas

A

theoretical that follows a set of principles.
KMT
no volume, attractive or repulsive forces
all collisions are elastic
KE is proportional to temperature

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42
Q

kinetic molecular theory

A

model used to explain behavior of matter.
particles are constantly in motion.
KE is related to temperature.
space between particles is related to the state of matter.
phase change happens when temperature changes significantly.
intermolecular forces

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43
Q

properties of liquid

A

fluid and can flow
definite volume but not shape
low compressibility

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44
Q

properties of solids

A

definite volume and shape
little KE
arranged in a packed crystalline structuer.

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45
Q

amorphous solid

A

doesnt have crystalline structure

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46
Q

hydrogen bonds

A

occur between polar molecules that contain an O F N atom covalently bonded to a H atom

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47
Q

dipole induced dipole

A

occur when a polar molecule induces a temporary dipole moment in a neighboring non polar molecule

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48
Q

dipole

A

separation of charges between two covalently bonded atoms.

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49
Q

dipole dipole

A

intermolecular forces between polar molecule.

positive side of a polar molecule attracts negative or another

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50
Q

london dispersion forces

A

noble gases and non polar molecule

creates temporary dipoles

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51
Q

ion dipole force

A

force between an ion and dipole molecule

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52
Q

intermolecular forces

A

positive charged poles attracted to the negative charged poles

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53
Q

phase change

A

transition from one state of matter to another

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54
Q

sublimination

A

solid to gas

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55
Q

deposition

A

gas to solid

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56
Q

phase diagram

A

graph of the physical state of a substance and the temperature and pressure of the substance

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57
Q

phase equalibium lines

A

where two phases are in equalibrium

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58
Q

triple point

A

point where the temperature and pressure conditions are right for all three states to exist together at equilibrium

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59
Q

critical point

A

gas and liquid states are identical and the substance is in one phase

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60
Q

supercritical fluid

A

state where the gas and liquid phase of a substance are indistinguishable

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61
Q

dipole moment

A

overall unequal distribution of electrons across the entire molecule

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62
Q

non polar molecule

A

even charge distribution and no dipole moment

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63
Q

polar molecule

A

uneven distribution charge and dipole moment

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64
Q

macromolecule

A

huge molecules made up of smaller subunits called monomers.

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65
Q

organic macrmolecules

A

huge molecules that included C and found in living things

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66
Q

inorganic macromolecule

A

huge molecule not found in living things.

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67
Q

C to F

A

5/9 (F-32)

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68
Q

Kelvin scale

A

absolut scale
K
0 is the absolute lowest
K = C + 273

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69
Q

pressure

A

psi
atm
mmHg
1 atm = 14.7 psi = 760 mmHg

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70
Q

daltons law of partial presures

A

total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of each individual gas
Pn + Po = Ptotal

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71
Q

diffustion

A

movement of 1 substance through another

high to low concentration

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72
Q

effustion

A

gas particles exit through tiny holes in a container

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73
Q

graham’s law

A

effusion rate of a gas is inversely proportional to the sqr root of its molecular mass.
used to compare the rate of two different gasses at equilibrium.
speed A / speed B = sqr root (mass B/massA)

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74
Q

standard pressure

A

1 atm = 760 mmHg = 14.7 psi

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75
Q

standard temperature

A

0 C = 273 K

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76
Q

Avogadro’s number

A
  1. 02 x 10 23 amu = 1 mole

1. 2 x 10 ^-7 XRCD

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77
Q

mole

A

you have 6.02 x 10 ^23 of something

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78
Q

avogadros law

A

relationship between the number of particles (n) and the volume of a a gas.
V1/ n1 = V2/ne

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79
Q

1 mole of an ideal gas at STP takes up

A

22.4 L

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80
Q

Boyles law

A

temperature is held constant the pressure of a gas increases as volume decreases

P1(V1) = P2(V2)

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81
Q

charles law

A

if pressure is held constant. as the gas is heated its volume will increase
v1/T1 = V2/T2
T must be Kelvin

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82
Q

Gay-lussac’s law

A

volume of a container is held constant as the temperature increase, the pressure inside the container increases
P1/T1 = P2/T2
T must be kelvin

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83
Q

ideal gas law

A

relates the temperature, pressure, number of moles and volume of any gas,
PV = nRT

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84
Q

PV = nRT

A 
P = pressure
V = volume
n = number of moles
R = .08216 atm/molK
T = Temperature
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85
Q

solvent

A

dissolves solutes

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86
Q

miscible

A

liquid dissovles easily in another

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87
Q

immiscible

A

liquid doesnt dissolve easily in another

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88
Q

ionic compound

A

compound held together by ionic bonds

formed by transfer of electrons

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89
Q

polar covalent

A

atoms held together by valence electrons shared between them

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90
Q

nonpolar covalent

A

valence electrons are shared equally and are no changes in the molecule

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91
Q

Molarity

A

moles of solute / L of solution

M

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92
Q

molality

A

mole solute / kg solvent

m

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93
Q

mass percentage

A

percent by mass of the solute in the solution

{mass solute / mass solution) x 100%

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94
Q

concentration

A

amount of a substance in a given quantity in a solution
M1V1 = M2V2
Stoichiometry given to unknown

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95
Q

SOLUBILITY

A

AMOUNT OF SOLUTE NEEDED TO FORM A SATURATED SOLUTION AT A SPECIFIC TEMPERATURE AND SOLVENT AMOUNT.

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96
Q

polarity

A

unequal sharing of electrons

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97
Q

factors that influence the rate of solution

A

amount of solute already dissolved.
temperature
pressure and nature

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98
Q

empirical formula

A

shows the kind and proportions of atoms in substance in simplest form

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99
Q

chemical formula

A

shorthand of writing a substance by using chemical symbols and number subscripts with the exact numbers of atoms.

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100
Q

Determine percent composition of compounds

A

write formula.
use formula to determine molar mass.
use molar mass to determine mass percentage of each element.

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101
Q

determine the empirical formula

A
  1. find percent composition.
  2. determine mass composition.
  3. determine composition in moles.
  4. find smallest whole number ratio of atoms.
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102
Q

dissolution

A

dissolving a substance

like dissolves like

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103
Q

calculate frequency

A

speed of light = frequency x wavelength

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104
Q

pure substance

A

cannot be separated

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105
Q

homogeneous mixture

A

unform throughout
solution
alloy

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106
Q

heterogeneous mixture

A

not uniform throughout

different components can be seen

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107
Q

separating mixtures

A 
manually,
dissolving
evaporation
distillation
magnetism
filtration
crystallization
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108
Q

chromatography

A

capillary action

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109
Q

retention factor

A

Rf

distance dye traveled compared to the total distance the solvent traveled

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110
Q

conjugate acid

A

acid forms when a base gains a proton

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111
Q

conjugate base

A

formed when an acid loses protons

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112
Q

Acidity Constant

A

Ka = [H+] [A-] / [HA]

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113
Q

calculating pH of a solution

A

-log[H3O+]
Must be in molarity
logarithmic

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114
Q

buffer

A

solution whose pH will not change much when small amounts of acid or base are added to it.

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115
Q

titration

A

a solution of known properties is used to analyze the properties of an unknown solution

  1. balanced equation
  2. V1M1/n1 =V2M2/n2
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116
Q

equivalence point

A

the amount of H ions and OH ions are equal and pH = 7

where titration stops

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117
Q

indicator solution

A

chemical that changes color when a specific pH range

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118
Q

Heat transfer

A

Delta heat = specific heat (m) (delta T)

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119
Q

titration curve

A

graph of PH vs volume of titration added

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120
Q

determine the unknown substance concentration

A

[H+][VH+] = [OH-][VOH-]

  1. gather information
  2. set up and fill in equation
  3. calculate
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121
Q

determine pH during titration

A
  1. determine mol of each reactant
  2. determine which reactant is in excess
  3. calculate pH based on concentration of the excess reactants
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122
Q

titrant

A

solution of known properties

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123
Q

pH during weak acid and strong base titration

A
  1. determine number of moles of each reactant
  2. determine reactant excess
  3. use stoichiometry and Ka/b values to determine acid concentration and pH
  4. rice table
    b. write equilibrium expression for dissociation of acid.
    c. plug and solve
124
Q

Arrhenius equation

A 
K = A e ^(-Ea/RT)
A= frequency factor
e = exponential factor
Ea= activation energy J/mol
R = 8.314

ln K = -EA/RT + Ln A

125
Q

Arrhenius acid

A

produce hydrogen ions

126
Q

Arrhenius bases

A

produces hydroxide ions in water

127
Q

Bronsted Lowry acid

A

only substance that can donate a proton

128
Q

bronsted lowry base

A

substance that accepts protons

129
Q

Kw

A

self ionization of H2O

[H3O+][OH-] = 1 x 10 -14

130
Q

lewis acid

A

substance accepts an electron pair to form a covalent bond

131
Q

lewis base

A

substance donates an elections pair to form a covalent bond

132
Q

lewis acid-base reaction

A

covalent bond is formed between an electron pair bond donor and acceptor

133
Q

E = mc2

A

E=energy
m= mass
c = speed of light = 3 x 10 8

134
Q

nuclear binding energy

A

energy required to separate the nucleus into its individual pieces

135
Q

mass defect

A

difference in mass between a nucleus and its pieces

products weight less

136
Q

disintegration energy

A

energy released during radioactive decay.

  1. find the difference of products and reactants
  2. multiply 1 u = 1.66 x 10 -27
  3. plug into E = mc2
137
Q

radioactive decay

A

unstable atomic nucleus decays or turns into a more stable nucleus, relating energy in the form of ionizing particles and radiation

138
Q

alpha decay

A 
nucleus emits an alpha particle.
one with four less particles
4
2
blocked by paper
cause cancer
139
Q

alpha particle

A

containing two protons and two neutrons

140
Q

beta decay

A 
when a neutron turns into a proton and an electron is emitted
0
-1
stopped by wood
penetrate skin
used to date living things
141
Q

gamma decay

A 
occurs when the nucleus of an atom is very high energy
0
0
contains no mass
stopped by lead
dangerous
142
Q

what a change in the chemical structure of a hydrocarbon chain isomers that have a shorter chain are

A

more volatile

have a lower boiling point

143
Q

radiocarbon dating

A

carbon dating

method used to determine the age of organic material by measuring the radioactivity of its carbon content

144
Q

uranium lead dating

A

used to find the age of a uranium-containing mineral

145
Q

1 p

1

A

atomic number of a proton is 1
1 = mass number
1 = atomic number

146
Q

nuclear chemistry

A

field of chemistry that deals with the use of radioactive isotopes and other nuclear reactions

147
Q

nuclear fusion

A

two or more atoms fuse together to form a single heavier atom
mass and energy is lost

148
Q

nuclear fission

A

a heavier atom splits into smaller pieces

149
Q

chain reaction

A

domino effect

nuclear fission

150
Q

chemical reaction

A

process where the arrangement of atoms, the way they are connected together, is changed

  1. particles must come into contact with one another
  2. particles must be lined up correctly
  3. particles must collide enough to break their bonds
151
Q

synthesis reaction

A

joining together of two reactants, to produce a complex product

152
Q

decomposition reaction

A

chemical reaction in which a single compound breaks down into two or more compounds or atoms

153
Q

single displacement reaction

A 
type of chemical reaction where an element reacts with a compound and takes the place of another element in that compound
more reactive replaces a less reactive 
1. determine if the reaction will occur
2. determine the products
3. balance the equation
154
Q

Double displacement reaction

A

a chemical reaction where two compounds react and the positive ions and the negative ions of the two reactants switch place forming two new compounds

  1. identify individual ions from the reactants and their charges
  2. switch the cations and anions
  3. balance the equation
155
Q

neutralization reaction

A

occurs between an acid and a base that forms salt and water

156
Q

gas formation

A

two compounds react to form a gaseous product

157
Q

synthesis reaction

A

reactants combine to form a new compound
two elements
two compounds
compound and element

158
Q

aqueous

A

dissolved in water

159
Q

diatomic molecules

A

molecules that are composed of two atoms of the same element

H, N, O, F, Cl, Br, I

160
Q

law of conservation of energy

A

energy is neither created nor destroyed

161
Q

exothermic reaction

A

system releases heat and the surroundings heat up

-

162
Q

endothermic reaction

A

system gains heat as the surrounding cool down.
energy is absorbed
(+)
vaporization

163
Q

enthalpy change

A

amount of energy as heat that is lost or gained by a system

Delta H = (sum of enthalpies of products) - (sum of enthalpies of reactants)

164
Q

reaction rate

A

change in concentration of reactants or products over time

  1. number of particles
  2. temperature
  3. pressure
  4. catalyst
  5. size
165
Q

reaction rate of disappearance

A

-delta(element) / time

166
Q

reaction rate of appearance

A

delta(element) / time

167
Q

effective collision

A
  1. molecules collide with enough energy to break bonds.

2. collide with a favorable orientation

168
Q

activation energy

A

minimum amount of energy it takes to start a chemical reaction

169
Q

activated complex

A

unstable state what is between the reactants and the products in a chemical reaction

170
Q

collision theory

A

helps scientists make predictions about how fast chemical reactions occur
related to the number of successful collisions.
only for gases

171
Q

chemical equilibrium

A

when the rate of the forward reaction equals the rate of the reverse reaction and the concentrations of the products and reactants are unchanged

172
Q

Equilibrium constant

A

K = [Cx x Dy] / [An x Bm]

only gas and aqueous elements

173
Q

lechatelier’s principle

A

any change in a substance on one side of the equation in concentration, temperature or pressure results in an equilibrium shift to oppose the change until a new equilibrium is reached

174
Q

increase in concentration of reactants will make the reaction shift

A

right

175
Q

an exothermic reaction the reactants have an increased temperature the reaction will shift

A

left

176
Q

if there is an increase of pressure on the reactants then the reaction will shift

A

right

177
Q

reaction quotient

A 
Q = [C]c [D]d / [A]a [B]b
determines the direction in which the reaction is moving 
Q>K right
Q=K equilibrium
Q < K left
178
Q

Gibbs free energy

A

G = H - TS
H= enthalpy
S= entropy
predicts whether a chemical reaction will occur spontaneously
the energy available to do work in chemical reactions.
chemical is measure in reference to another chemical state that is assigned a gibbs free energy of 1

179
Q

spontaneous reactions

A

happen without the need of any input of energy

180
Q

gibbs free energy and spontaneous reactions

A

delta G = Gf -Gi = Delta H - T(delta S)

181
Q

Entropy

A

S
particles spread out more
THird law of thermodynamics

182
Q

covalent bonds

A

atoms share elections

strongest

183
Q

ionic bond

A

electrons are transferred between atoms of opposite charge

184
Q

electron sea model

A

metallic bonding where electrons float free in a sea of electrons around metal atoms

185
Q

metallic bonding

A

chemical bonding that takes place from the attraction of metal atoms and the surrounding sea of electrons

186
Q

structural formula

A

shows the location of atoms relative to one another.

  1. determine type and number of atoms.
  2. write lewis dot structure for each
  3. connect the atoms by electron pair bonds
187
Q

polyatomic ion lewis dot structure

A
  1. sum the number of valence electrons from each atom
  2. make a skeleton structure by connecting atoms with single bonds
  3. determine the remaining electrons
  4. place remaining electrons to satisfy octet
  5. double bonds if needed
188
Q

VSEPR theory

A

shape of the molecule is related to the organization of the central atom’s valence electrons

189
Q

molecular geometry

A

linear
trigonal planar
tetrahedral
bent
trigonal pyramidal
1. find lewis dot structure of the molecule
2. locate of central atom, count the number of electron domains
3. identity the number of nonbonding and bonding domains
4. compare to chart

190
Q

molar mass

A

the sum of the total mass in grams of all the atoms that make up a mole of a particular molecule
grams / mole

191
Q

finding molar mass of a compound

A
  1. find the atomic masses of each element
  2. count how many atoms there are for each element
  3. find molar mass
192
Q

calculating number of grams using molar mass

A

number of moles x molar mass

193
Q

stoichiometry

A

study of chemical quantities consumed or produced in a chemical reaction

194
Q

mole ratio

A

ratio of moles of one substance to the moles of another substance in a balanced equation

195
Q

mole to mole calculation

A

moles of given (moles desired/ moles given ratio) =moles desiered

196
Q

moles to mass calculations

A

moles A (mole ration of B / A) (molar mass B) = mass B

197
Q

mass to moles calculations

A

mass A (1 / molar mass A)(mole ration B /A) = moles B

198
Q

mass to mass calculation

A

mass A (1/molar mass A)(mole ration B/A)(mass B/1) = mass B

199
Q

molar volume

A

at STP one more of any gas will fill t 22.4 liters

200
Q

stoichiometry of gases

A
  1. balance the equation
  2. find the moles of the reactants
  3. use mole ration to find products made
  4. convert to desired units
201
Q

limiting reactant

A

used up first

202
Q

excess reactant

A

substance that is in excess

203
Q

finding the limiting reactant

A
  1. layout givens
  2. change mass to moles
  3. multiply a reactant with the mole ratio
204
Q

determine the amount of product made from the limiting reactant

A

limiting reactant (mole ration product / limiting reactant)(molar mass product)

205
Q

theoretical yield

A

maximum amount of product that can be made from the amount of reactant

  1. changes to moles
  2. mole ratio product /reactant
  3. change product to mass
206
Q

percent yield

A

actual yield / theoretical yield (100%)

207
Q

oxidation number

A

number assigned to atoms in molecules to show the general distribution of electrons

  1. if electrons are shared, they belong to the more electronegative atom
  2. pure elements = 0
  3. a binary compound the more electronegative element receive oxidation number equal to the negative charge it would have if it were an anion. the less electronegative element receives an oxidation number if it were a cation
  4. fluorine = -1
  5. oxygen = - 2 except H2O -1, OF2 is + 2
  6. Hydrogen = +1 or -1 when combined with metals
  7. the sum in neutral compound is 0
  8. sum of polyatomic ions is equal to the charge on the ion
  9. monatomic ion is equal to the charge of the ion
208
Q

oxidizing agent

A

substance that causes the oxidation in another substance

209
Q

reducing agent

A

substance that causes another substance to reduce
loses electrons
BIH3 is the strongest
increase down a group

210
Q

balancing a redox reaction

A
  1. write unbalanced equation in ionic form excluding spectator ions.
  2. give each atom an oxidation number
  3. write and balance the half reactions
  4. balance oxygen by adding water
  5. balance hydrogen by adding hydronium
  6. make electrons equal and combine the half reactions q
211
Q

oxidation reaction

A

reactions that takes an electron

212
Q

when an element is reduced it

A

gains electrons

213
Q

single bonds

A

type of covalent bond formed from the sharing of two electrons between two atoms

214
Q

double bonds

A

type of covalent bond where four electrons are shared between two atoms

215
Q

triple bond

A

type of covalent bond where six electrons are shared between two atoms

216
Q

functional group

A

an atom or group of atoms that is responsible for a particular chemical property of an organic compound

217
Q

alcohol

A

contains one or more hydroxyl groups
R - OH
Higher boiling point due to H bonds between molecules

218
Q

hydrocarbon

A

compound made of only carbon and hydrogen

219
Q

alkyl halide

A

compound with a halogen atom
takes place of one or more hydrogens in a hydrocarbon
R-X

220
Q

ketone

A

the carbon of a carbonyl group share bonds with two other carbons
R - CO -R

221
Q

aldehyde

A

carbon of the carbonyl group share a bond with at least one hydrogen
R - CHO

222
Q

ether

A

oxygen is bonded to two carbons

R - O - R

223
Q

carboxylic acid

A

carboxyl group

R - COOH

224
Q

hydroxyl group

A

OH

225
Q

amine group

A

NH4

R - N

226
Q

carbonyl group

A

C=O

227
Q

carboxylic acid

A

OH-C=O

228
Q

ester group

A

OR - C =O

229
Q

polymerization

A

product is produced with repeating units

230
Q

addition reaction

A

two molecules combine together

231
Q

cracking

A

breaking up of big hydrocarbons into smaller pieces

232
Q

redox reaction

A

where a reduction and oxidation occur

233
Q

esterification reaction

A

alcohol combines with carboxylic acid to form an ester and water

234
Q

fermentation

A

process of turning a sugar into alcohols, gases or acids

235
Q

saturated hydrocarbons

A

have as many hydrogen atoms as possible attached to every carbon

236
Q

aliphatic hydrocarbons

A

compounds of hydrogen and carbon that do not contain benzene rings

237
Q

alkanes

A

linear

compounds that are made of varying numbers of carbon atoms that are all saturated with hydrogen atoms

238
Q

cycloalkanes

A

alkane that contain a carbon ring

239
Q

alkenes

A

have at least one double bond between carbon atoms

Eth–

240
Q

alkynes

A

have at least one triple bond between carbon atoms

241
Q

alkenynes

A

have both double and triple bonds

242
Q

arenes

A

aromatic hydrocarbons

have at least one benzene ring

243
Q

benzene ring

A

a ring of 6 carbon atoms with three double bonds

244
Q

aromatic compound

A

any compound with a benzene ring

245
Q

isomers

A

different forms of the same compound.

functional group is placed at a different location.

246
Q

carbohydrates

A

sugars

contain ether, hydroxyl groups

247
Q

polysaccharide

A

large sugar

248
Q

when counting carbons in a carbohydrate

A
  1. find carbon attached to 2 oxygen atoms

2. then count carbons it is attached to

249
Q

monosaccharide

A

single sugar

250
Q

disaccharide

A

sugar molecule containing two monosaccharides

251
Q

glycosidic linkage

A

bond between sugars

252
Q

lipids

A

biological molecules that are insoluble in water but soluble in nonpolar solvents

253
Q

saturated fats

A

triglycerides that have no double bonds in their carboxylic acid chains

254
Q

unsaturated fats

A

triglycerides that have double bonds in their carboxylic acid chains

255
Q

trans fats

A

synthetic

triglycerides that have trans double bonds in their carboxylic acid chains

256
Q

peptide body

A

covalent bond that holds amino acids together

carbonyl and amino nitrogen group

257
Q

enzymes

A

proteins that enable chemical reactions in our bodies

decrease activation barrier

258
Q

the amount of kinetic energy of an object is dependent on

A

mass

speed

259
Q

Kinetic energy

A

KE = 1/2 mas (velocity)sqr

260
Q

energy transformation

A

process of changing energy from one form to another

261
Q

chemical energy

A

from chemical reaction

262
Q

heat energy

A

from thermal reactions

263
Q

electrical energy

A

from charged particles

264
Q

gravitational potential energy

A

energy stored by an object because of its location above the ground

265
Q

elastic potential energy

A

energy stored by an object that can be stretched or compressed

266
Q

nuclear energy

A

energy stored in the nucleus of an atom
fission
fusion

267
Q

internal energy of the system

A

total kinetic energy of the particles and the potential energy of the particles

268
Q

potential energy is measured by

A

the phase of an object

269
Q

1 food calories =

A

1,000 calories

4.184 J

270
Q

heat of fusion

A

heat energy/mass

Hf = m/q

271
Q

heat of vaporization

A

amount of energy required to turn a liquid into a gas at its boiling point
Hv = q/m

272
Q

hess’s law

A

measure enthalpy change of a chemical reaction
adding or subtracting chemical reactions with the same products or reactants.
what ever happens to one side you must do to the other

273
Q

thermochecmical equations

A

shows the enthalpy change going from reactants to products

274
Q

calorie

A

amount of energy required to raise the temperature of one gram of water by 1 C

275
Q

specific heat capacity

A 
amount of energy required to change the temperature of one gram of a substance by 1 C
Q = sm deltaT
Q= energy
s= specific heat capacity 
T = Celcius

S = q/m delta T

276
Q

heating and cooling curves

A

line graph that shows the phase changes a given substance undergoes with increasing or decreasing temperature

277
Q

bond enthalpy

A

energy needed to break a particular bond in a gaseous compound
kJ/mol

278
Q

bond enthalpy values

A

value of energy required to break a particular chemical bond at 298K (25 C)

279
Q

radiation

A

transmission of energy from a body in the form of waves or particles

280
Q

nonionizing radiation

A

encompasses the electromagnetic spectrum from low energy ultraviolet light
nuclear fusion

281
Q

ionization radiation

A

higher frequencies of the electromagnetic spectrum
nuclear fission
radioactive decay

282
Q

Electronegativity

A

increased up and right

283
Q

During titration of adding acid to a base, a few drops of acid are added into the solution after the endpoint. How will this affect calculations for the concentration of the base?

A

It will make the calculations too high. Making the base look stronger than it is.

284
Q

Few drops of water left in a buret that is used to titrate a base into an acid. Will the small amount of water have any effect on the determined value for the concentration of the acid?

A

Yes, because the water will dilute the base, creating an error.

285
Q

Calculating pOH

A

pH =-log [H]
pOH = 14 -pH
Must be molarity

286
Q

pKa

A

-logKa

287
Q

Find pKb from pKa

A

14 - pKa

288
Q

to find concentration from pH

A

10 ^ concentration

289
Q

parts per million

A

(g solute / g solution) x 10^6

290
Q

Erg =

A

visible waves

291
Q

Magnetic moment

A

sqrt (n(n+2))

n= unpared eletrons

292
Q

Density

A

g/cm3

293
Q

What gas is mostly responsible for the greenhouse effect

A

carbon dioxide

294
Q

calculate percentage error

A

actual - measured / acual ) x 100

295
Q

How do energies of similar bonds compare

A

consistent

296
Q

x rays are in the wavelength range of

A

.01 - 10 nm

297
Q

Bohr’s atomic model

A 
mvr = nh/2pi
N = number of orbits
298
Q

Coulombs law

A

ionization energy increases proportionally with the atomic number

299
Q

Faraday

A

1 mole of electrons

300
Q

How does dialysis work

A

allows the electrolytes to pass through and not solution particles

301
Q

types of statistical series

A 
Spatial
conditional
times
qualitative
quantitative
302
Q

calculate the molecular mass from vapor pressure

A

2 (vapor density)

303
Q

Solubility of alkaline earth metal hydroxides/ oxides

A

increase down a group

304
Q

solubility of alkaline earth metal sulfates

A

increase up a group

305
Q

Amu of an electron

A

1/2000

306
Q

accuracy

A

how close a measurement is to the true value

307
Q

precision

A

how close repeated measurements are to each other

CHEM (1 decks)

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