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Chemistry > midterm > Flashcards

midterm Flashcards

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
Q

plum pudding model

A

showed an atom has electrons evenly dispersed throughout

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26
Q

rutherford contributed:

A

gold foil experiment
the atom is mostly empty space and all the positive charge and almost all of the mass comes from the nucleus

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27
Q

gold foil experiment

A

directed a narrow beam of alpha particles at a very thin sheet of gold foil
alpha particles scattered from the gold foil

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28
Q

rutherford was limited:

A

didn’t explain chemical properties of elements
why negatively charged electrons were not pulled into the positively-charged nucleus
why atoms don’t glow

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29
Q

law of conservation of mass

A

in a chemical reaction, matter is neither created nor destroyed

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30
Q

law of definite proportions

A

all samples of a given compound have the same proportions of their constituent elements

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31
Q

law of multiple proportions

A

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

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32
Q

of neutrons =

A

mass # - atomic #

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33
Q

avg. atomic mass =

A

calculate mass contributions
add products

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34
Q

mass contributions =

A

isotope mass x natural abundance

35
Q

atomic mass unit

A

1/12 the mass of a Carbon-12 atom

36
Q

Mendeleev

A

arranged elements by increasing atomic mass

37
Q

Moseley

A

determined atomic numbers for known elements

38
Q

periods

A

rows

39
Q

groups

A

columns

40
Q

periodic law

A

elements arranged by increasing atomic number

41
Q

electromagnetic radiation

A

light acting as a wave

42
Q

amplitude determines

A

lights intensity/brightness

43
Q

electromagnetic spectrum:

A

radio waves
microwaves
infrared
visible light
UV light
x-ray
gamma

44
Q

constructive interference

A

interaction between 2 in-phase waves to make one large wave

45
Q

destructive interference

A

interaction between 2 out-of-phase waves to make a line

46
Q

diffraction

A

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
Q

interference pattern

A

diffraction of light through 2 slits separated by a distance comparable to the wavelength
destructive interference: dark areas
constructive interference: light areas

48
Q

photoelectric effect

A

many metals emit electrons when light shines on its surface
energy that exceeds that threshold frequency becomes kinetic energy

49
Q

atomic spectroscopy

A

wave nature of particles

50
Q

emission spectrum

A

emitted light is passed through a prism
pattern of wavelengths of light is seen

51
Q

flame test of mercury

A

blue

52
Q

flame test of helium

A

violet

53
Q

flame test of hydrogen

A

red

54
Q

quantized states

A

electron should only give off specific amounts of energy

55
Q

stationary states

A

electrons travel in orbits that are at a fixed distance from the nucleus

56
Q

bohr’s model limitations:

A

only explained hydrogen’s emission spectrum
didn’t explain why electrons don’t fall into the nucleus

57
Q

bohr’s model contributions:

A

electrons exist only in certain energy levels
energy is involved in the transition of an electron from one energy level to another

58
Q

de broglie’s contributions:

A

electrons exhibit wave-like properties
electrons have wavelengths
electrons have wave-particle duality

59
Q

heisenberg’s contributions:

A

an electron’s position is an atom is not precisely defined
Heisenberg’s Uncertainty Principle

60
Q

Heisenberg’s Uncertainty Principle

A

impossible to determine the location and speed of an electron

61
Q

quantum mechanical model

A

precisely defines the energy of the electron
described its location in terms of probabilities

62
Q

orbital

A

region of space around a nucleus where there is a high probability of finding an electron

63
Q

n:

A

energy level

64
Q

l:

A

sublevel

65
Q

m:

A

orbital

66
Q

s:

A

spin

67
Q

Aufbau principle

A

electron enter low-energy orbitals first
orbitals on the same sublevel have the same energy
s sublevel has the lowest energy

68
Q

Pauli Exclusion principle

A

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
Q

Hund’s rule

A

one electron enters each orbital
when all orbitals have one electron, they begin to pair up

70
Q

quantum mechanics

A

explains why periodic trends in properties exist

71
Q

coulomb’s law

A

describes attraction and repulsion between charged particles

72
Q

shielding

A

repulsions cause the electron to have a net reduced attraction to the nucleus

73
Q

Zeff =

A

atomic # - core electrons

74
Q

atomic radius =

A

1/2 the distance between 2 bonded atoms

75
Q

down a group, radius:

A

energy levels increases

increases
energy levels increases
shielding increases
nuclear charge increases

76
Q

across a period, radius:

A

energy levels constant

decreases
energy levels constant
shielding constant
nuclear charge increases

77
Q

nuclear attraction

A

attraction between negative electrons in their orbitals and the positive protons in the nucleus

78
Q

ionization energy

A

energy required to remove the an electron from an atom

79
Q

electronegativity

A

the ability of an atom of an element to attract electrons

80
Q

across a period, ionization energy/electronegativity

A

increases
distance from nucleus constant
shielding constant
nuclear charge increases

81
Q

down a group, ionization energy/electronegativity

A

decreases
distance from nucleus increases
shielding increases
nuclear charge increases

82
Q

cation

A

positive ion

83
Q

anion

A

negative ion

Chemistry (13 decks)

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