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Chemistry > midterm > Flashcards

midterm Flashcards

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1
Q

5 traditional areas of chemistry

A

organic
inorganic
biochem
analytical (quantitative and qualitative)
physical

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2
Q

crystalline solid

A

long-range, repeating order

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3
Q

amorphous solid

A

no order

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4
Q

decanting

A

gradually pouring a liquid from one container to another without disturbing the sediment

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5
Q

distillation

A

mixture is heated to boil off the more volatile (easily vaporable) liquid, then the liquid is re-condensed in a condenser and collected in a separate flask

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6
Q

filtration

A

used to separate a mixture of an insoluble solid and liquid

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7
Q

physical property

A

property that a substance displays without changing its composition
ex. taste, color, melting point, density

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8
Q

chemical property

A

property that substance displays only by changing its composition via a chemical change
-often indicated by temperature, color change, gas production
ex. flammability, corrosiveness, flammability

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9
Q

physical change

A

alters physical state/appearance of matter (no change in composition)
ex. water boiling

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10
Q

chemical change

A

alters the composition of matter
ex. iron rusting

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11
Q

Kelvin calculations:

A

K = C + 273
C = K - 273

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12
Q

Fahrenheit calculations:

A

F = 1.8 (C) + 32
C = (F - 32) / 1.8

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13
Q

error =

A

experimental value - accepter value

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14
Q

percent error =

A

|error|/accepted value x100

error| / accepted value x 100%

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15
Q

density =

A

mass/volume

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16
Q

volume =

A

mass/density
length x width x height

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17
Q

mass =

A

density x volume

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18
Q

density _ as temperature _

A

decreases, increases

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19
Q

democritus contributed:

A

atoms were indivisible and indestructible

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20
Q

democritus limited:

A

didn’t explain chemical behavior
lacked experimental support

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21
Q

dalton contributed:

A

all elements are composed of atoms
atoms of the same element are identical
atoms of one element are different than atoms of another element
Law of Definite Proportions
chemical reactions occur when atoms are separated, joined, or rearranged
atoms of one element are never changed into atoms of another element in a chemical reaction

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22
Q

Law of Definite Proportions

A

atoms of different elements can physically mix together/combine in simple whole-number ratios to form compound

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23
Q

thomson contributed:

A

cathode ray tube experiment
electrons
plum pudding model

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24
Q

cathode ray tube experiment

A

electric currents passed through gases in a cathode ray tube
cathode ray traveled from the cathode to the anode
cathode ray deflected by a magnet
cathode ray deflected by charged plates

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25
plum pudding model
showed an atom has electrons evenly dispersed throughout
26
rutherford contributed:
gold foil experiment the atom is mostly empty space and all the positive charge and almost all of the mass comes from the nucleus
27
gold foil experiment
directed a narrow beam of alpha particles at a very thin sheet of gold foil alpha particles scattered from the gold foil
28
rutherford was limited:
didn't explain chemical properties of elements why negatively charged electrons were not pulled into the positively-charged nucleus why atoms don't glow
29
law of conservation of mass
in a chemical reaction, matter is neither created nor destroyed
30
law of definite proportions
all samples of a given compound have the same proportions of their constituent elements
31
law of multiple proportions
when two elements (A and B) form two different compounds, the masses of element B that combine with element A can be expressed as a ratio of small whole numbers
32
of neutrons =
mass # - atomic #
33
avg. atomic mass =
calculate mass contributions add products
34
mass contributions =
isotope mass x natural abundance
35
atomic mass unit
1/12 the mass of a Carbon-12 atom
36
Mendeleev
arranged elements by increasing atomic mass
37
Moseley
determined atomic numbers for known elements
38
periods
rows
39
groups
columns
40
periodic law
elements arranged by increasing atomic number
41
electromagnetic radiation
light acting as a wave
42
amplitude determines
lights intensity/brightness
43
electromagnetic spectrum:
radio waves microwaves infrared visible light UV light x-ray gamma
44
constructive interference
interaction between 2 in-phase waves to make one large wave
45
destructive interference
interaction between 2 out-of-phase waves to make a line
46
diffraction
when traveling waves encounter an obstacle or opening in a barrier that is about the same size as the wavelength, they bend around it
47
interference pattern
diffraction of light through 2 slits separated by a distance comparable to the wavelength destructive interference: dark areas constructive interference: light areas
48
photoelectric effect
many metals emit electrons when light shines on its surface energy that exceeds that threshold frequency becomes kinetic energy
49
atomic spectroscopy
wave nature of particles
50
emission spectrum
emitted light is passed through a prism pattern of wavelengths of light is seen
51
flame test of mercury
blue
52
flame test of helium
violet
53
flame test of hydrogen
red
54
quantized states
electron should only give off specific amounts of energy
55
stationary states
electrons travel in orbits that are at a fixed distance from the nucleus
56
bohr's model limitations:
only explained hydrogen's emission spectrum didn't explain why electrons don't fall into the nucleus
57
bohr's model contributions:
electrons exist only in certain energy levels energy is involved in the transition of an electron from one energy level to another
58
de broglie's contributions:
electrons exhibit wave-like properties electrons have wavelengths electrons have wave-particle duality
59
heisenberg's contributions:
an electron's position is an atom is not precisely defined Heisenberg's Uncertainty Principle
60
Heisenberg's Uncertainty Principle
impossible to determine the location and speed of an electron
61
quantum mechanical model
precisely defines the energy of the electron described its location in terms of probabilities
62
orbital
region of space around a nucleus where there is a high probability of finding an electron
63
n:
energy level
64
l:
sublevel
65
m:
orbital
66
s:
spin
67
Aufbau principle
electron enter low-energy orbitals first orbitals on the same sublevel have the same energy s sublevel has the lowest energy
68
Pauli Exclusion principle
an orbital can contain up to 2 electrons electrons spin up/down electrons behave like magnets electrons in the same orbital have opposite spins
69
Hund's rule
one electron enters each orbital when all orbitals have one electron, they begin to pair up
70
quantum mechanics
explains why periodic trends in properties exist
71
coulomb's law
describes attraction and repulsion between charged particles
72
shielding
repulsions cause the electron to have a net reduced attraction to the nucleus
73
Zeff =
atomic # - core electrons
74
atomic radius =
1/2 the distance between 2 bonded atoms
75
down a group, radius:
# energy levels increases increases energy levels increases shielding increases nuclear charge increases
76
across a period, radius:
# energy levels constant decreases energy levels constant shielding constant nuclear charge increases
77
nuclear attraction
attraction between negative electrons in their orbitals and the positive protons in the nucleus
78
ionization energy
energy required to remove the an electron from an atom
79
electronegativity
the ability of an atom of an element to attract electrons
80
across a period, ionization energy/electronegativity
increases distance from nucleus constant shielding constant nuclear charge increases
81
down a group, ionization energy/electronegativity
decreases distance from nucleus increases shielding increases nuclear charge increases
82
cation
positive ion
83
anion
negative ion

Chemistry (13 decks)

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